TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

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TN State Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Answer the following questions.

Question 1.
Classify the following aliphatic or aromatic nitro compounds.
(i) 1, 2, dimethyl-1-nitropropane
(ii) 2-nitro-1 -methyl benzene
(iii) 1, 3, 5 trinitro benzene
(iv) 2-phenyl-1-nitro ethane
(v) 2-methyl-2-nitro propane
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 1
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 2

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 2.
What are nitro compounds? How are they classified? Give one example for each type.
Answer:
(i) Nitro compounds are considered as the derivaties of hydrocarbons. If one of the hydrogen atom of hydrocarbon is replaced by the —NO2 group, the resultant organic compound is called a nitrocompound.
(ii) Examples for primary nitro compound.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 3
(iii) Example for secondary nitro compound.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 4
(iv) Example for a tertiary nitro compound.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 5

Question 3.
Write the structural formula of the isomers of the following compound and indicate the type of isomerism involved, (i) 1-nitrobutane,
(ii) nitroethane.
Answer:
(i) (a) 1-nitrobutane and 2-methyl-1-nitropropane are- chain isomers. These two isomers differ in the length of carbon chain and hence exhibit chain isomerism.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 6
(b) 1-nitrobutane, 2-nitrobutane and 2-methyl 2-nitropropane are position isomers. They differ in the position of the functional group and hence exhibit positfon isomerism.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 7
(c) 1-nitrobutane and butyl nitrite are functional isomers. They differ in the nature of the functional group and hence functional isomerism.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 8
(ii) Nitromethane and methyl nitrite exhibit tautomerism.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 9

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 4.
Methyl nitrite and nitro methane exhibits tautomerism. How will you distinguish between these form?
Answer:

Nitro formAci-form
Less acidicMore acidic and also called pseudoacids (or) nitronic acids.
Dissolves in NaOH slowly.Dissolves in NaOH instantly.
Decolourises FeCl3 solution.With FeCl3 gives reddish-brown colour
Electrical conductivity is low.Electrical conductivity is high.

Question 5.
Between 2-nitrobenzene, and 2-methyl – 2- nitro propane which does not exhibit tautomerism? Why?
Answer:
Tautomerism is exhibited by nitro alkanes which contain one or more ‘α’ hydrogen atoms. Then 1° and 2° nitro alkanes exhibit tautomerism while 3° nitro alkanes which do not have a ‘α’ hydrogen atom does not exhibit tautomerism.
2-nitrobutane has a hydrogen atom and hence exhibit tautomerism. While 2-methyl -2- nitropropane does not contain an a hydrogen atom and hence does not exhibit tautomerism.

Question 6.
Explain the acidic nature of nitroalkanes.
Answer:
Primary and secondary nitro alkanes show acidic nature because of the presence of a hydrogen atom.
Because of the presence of electron withdrawing nitro group, the ‘α’ hydrogen atom is abstracted by a base.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 10
Hence, they are acidic. When the number of alkyl groups attached to α- carbon acidity decreases because of +1 effect of alkyl groups.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 11

Question 7.
How will you prepare nitro benzene from (i) ethyl bromide (ii) methane, (iii) α – chloroacetic acid (iv) tert-butyl amine, (v) acetaldoxine.
Answer:
(i) Alkyl bromides (or) iodides on heating with ethanolic solution of potassium nitrite gives nitroethane.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 12
(ii) Gaseous mixture of methane and nitric acid passed through a red hot metal tube to give nitromethane.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 13
(iii) α – chloroacetic acid when boiled with aqueous solution of sodium nitrite gives nitromethane.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 14TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 15
(iv) tert-butyl amine is oxidised with aqueous KMnO4 to give tert – nitro alkanes.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 16
(v) Oxidation of acetaldoxime and acetoneoxime with trifluoroperoxy acetic acid gives nitroethane (1°) and 2- nitropropane (2°) respectively.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 17

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 8.
Give the equation for the reduction of nitromethane in (a) acid medium and (b) neutral medium.
Answer:
(a) Nitromethane on reduction in acid medium gives methylamine.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 18
(b) Reduction under neutral condition using Zn / NH4OH or Zn /CaCl2, hydroxylamine is formed.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 19

Question 9.
Complete the following equation. Identify A, B, and C.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 20
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 21
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 22
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 23

Question 10.
How does ethyl nitrite react with (i) Sn / HCl and (ii) HCl / H2O.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 24

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 11.
What is Nef carbonyl synthesis? Give equation.
Answer:
The formation of an aldehyde by the alkaline hydrolysis of a nitro alkane is known as Nef carbonyl synthesis.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 25

Question 12.
How are the following conversion made?
(i) Benzene to mcta dinitro benzene, (ii) Nitro benzene to nitroso benzene, (iii) Nitro benzene to azo benzene, (iv) Nitro benzene to hydrazo benzene.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 26
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 27

Question 13.
Identify the reagents used in the following conversions. Write complete equations.
(i) nitrobenzene to aniline
(ii) metadinitrobenzene to metanitroaniline
(iii) nitrobenzene to 3-nitrobenzene sulphonic acid.
Answer:
(i) Any reducing agent: Ni (or) Pt or LiAlH4
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 28
(ii) Ammonium poly sulphide
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 29
(iii) Conc. H2SO4
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 30

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 14.
Explain why nitro group in nitro benzene is meta directing.
Answer:
The structure of nitro benzene is a resonance hybrid of the following cannonical structures.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 31
As a result of electron withdrawing nature of the NO2 group, the electron density at ortho and para position deefeases compafed to meta position i.e., the meta position is relatively electron rich compound to ortho and para positions. Hence the electrophile attacks the meta position.

Question 15.
How will you effect the following conversions?
(i) Benzene to m-chloro nitro benzene,
(ii) Benzene to 1, 2, 3 tri nitro benzene
(iii) m-chloro nitro benzenetto m-chloro aniline,
(iv) 1, 3, di nitrobenzene to 3- nitro aniline.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 32

Question 16.
Give the IUPAC names of the following:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 33
Answer:
(i) N -phenyl benzenamine
(ii) N, N -diphenyl benzenamine
(iii) N -methyl-N-phenylethanamine
(iv) prop -2- en-1-amine
(v) hexane-1, 6-diamine
(vi) N -methyl-propan-1-amine
(vii) N, N -diethyl-butan-1-amine
(viii) N -ethyl- N-methyl propan-2-amine
(ix) N, N -dimethyl-benzenamine
(x) phenyl-methanamine

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 17.
Write the structures of the chain isomers of Butan-1-amine.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 34

Question 18.
Explain ‘metamerism’ with a suitable example of amines.
Answer:
Aliphatic amines having the same molecular formula but different alkyl groups on either side of the nitrogen atoms show metamerism,
eg: CH3CH2NHCH2CH3 (diethyl amine) and CH3NHCH2CH2CH3 (methyl-n-propyl amine)
CH3NHCH(CH32)2 (Isopropyl methylamine) are metamers.

Question 19.
What are all the possible isomers of an amine having the molecular formula C3H9N and C4H11N.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 35
These amines exhibit functional isomerism.
Amine (C4H11N): CH3CH2CH2CH2NH2 (Butan-1-amine) exhibit chain as well as position isomerism.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 36

Question 20.
Write the structure of the following:
(i) 4N-dimethyl pentan-2-amine
(ii) 2 (N, N-dimethyl) butanamine
(iii) 2-aminoethanol
(iv) 4-aminobutanoicacid
(v) N-methyl-2-nitro pentanamine
(vi) prop-2-en-l -amine.
(vii) N-ethyl-N-methylbenzenamine
(viii) 3-methylbenzenamine
(ix) 2-methoxybenzenamine
(x) N-phenylbenzenamine
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 37
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 38

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 21.
How is ethanamine prepared from (i) nitroethane, (ii) ethanenitrile, (iii) acetamide, (iv) ethyl bromide?
Answer:
(i) Reduction of nitroethane using H2 in the presence of Ni or Sn/HCl or Pd/H2.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 39
(ii) Reduction of ethanenitrile using sodium amalgam in ethanol.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 40
(iii) Reduction of acetamide using LiAlH4.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 41
(iv) By Gabriel’s phthalimide synthesis.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 42

Question 22.
Identify the products:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 43
Answer:
(i) C6H5NH2 (aniline)
(ii) CH3NHCH3 (N-methyl methanamine)
(iii) C6H5NH2 (aniline)
(iv) C6H5CH2NH2 (benzyl amine)

Question 23.
Using sodium azide (NaN3) convert methyl bromide to methylamine.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 44

Question 24.
How will you prepare aniline from (i) chlorobenzene and (ii) phenol?
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 45

Question 25.
What happens when
(i) Vapours of ethanol and ammonia are passed over alumina.
(ii) Ethanamide is treated with LiAlH4. Give equation.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 46

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 26.
Explain Why?
(i) Amines have higher boiling points than hydrocarbons of comparable molecular mass.
(ii) Among isomeric amines 3° amines have the lowest melting point.
(iii) The boiling point of amines are lower than those of alcohols and acids of comparable molecular mass.
(iv) Aliphatic amines with maximum six carbon atoms are soluble in water to some extent, while aromatic amines are insoluble in water.
Answer:
(i) This is due to the reason that amines being polar form inter molecular hydrogen bonding (except tertiary amines which do not have a H atom linked to N atom) and exist as associated molecules.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 47
(ii) The degree of association depends on the extent of hydrogen bonding. Since 1° amines have two, 2° amines have one while 3° amines have no hydrogen linked to nitrogen. Therefore, among isomeric amine 1° amines have highest while 3° amine have the lowest boiling points.
(iii) The electronegativity of nitrogen is lower than oxygen, amines form weaker H—bonding compared to alcohol and carboxylic acids.i.e., The extent of association is less compared to that of alcohols or carboxylic acids. Hence amines will have lower boiling point compared to alcohol or carboxylic acid of comparable molecular mass.
(iv) All the three classes of amines (1°, 2° and 3°) form H bonds with water as a result lower aliphatic amines are soluble in water. As the size of the alkyl group increases (with increase in molecular mass), the solubility decreases due to a corresponding increase in hydrocarbon part of the molecule. The borderline solubility is reached with amines of about six carbon atoms in the molecule. Aromatic amines, on the other hand are insoluble in water. This is due to larger hydrocarbon part which tend to retard the formation of H-bonds.

Question 27.
Account for the fact that among ethyl amines, the decreasing order of basicity in aqueous solution is (CH3CH2)2NH > (CH3CH2)3N > CH3CH2NH2.
Answer:
The basicity of an amine in aqueous solution primarily depends upon the stability of the ammonium cation or the conjugate acid formed by accepting a proton from water. The stability of the ammonium cation in turn depends on the combination of the following factors.
(i) +1 effect of alkyl groups.
(ii) Extent of hydrogen bonding with water molecules.
(iii) Steric effects of the alkyl groups.
In the case of alkyl groups bigger than ‘CH3’ group i.e., ethyl, propyl, etc there will be steric hindrance to hydrogen bonding. As a result, stability due to +1 effect predominates over the stability due to H—bonding and hence 3° amines because more basic than 1° amines. In all overall decreasing basic strength of ethyl amine follows the sequence (CH3CH2)2NH > (CH3CH2)3N > CH3CH2NH2 > NH3.

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 28.
How does nitrous acid (a mixture of sodium nitrite and dil. HCl) react with (i) CH3NH2 (ii) (CH3)2NH and (iii) (CH3)3N? Give equations.
Answer:
Aliphatic primary amines react with nitrous acid give an alcohol and nitrogen gas is produced. Methyl amine is an exception.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 48
Secondary amines will form nitroso alkyl amine.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 49
Tertiary amines react with nitrous acid and form nitrites.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 50

Question 29.
How does nitrous acid react with the following? Give equations.
(i) ethylamine, (ii) di-ethylamine, (iii) triethyl amine, (iv) aniline, (v) N-methyl aniline, (vi) N, N- dimethylaniline.
Answer:
(i) Ethylamine reacts with nitrous acid to give ethyl diazonium chloride, which is unstable and it is converted to ethanol by liberating N2.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 51
(ii) A yellow dye of N-nitrosodiethylamine is formed.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 52
(iii) Triethylammoniumnitrate which is soluble in water formed.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 53
(iv) Aniline reacts with nitrous acid at low temperature (273 – 278 K) to give benzene diazonium chloride which is stable for a short time and slowly decomposes even at low temperatures.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 54
This reaction is known as diazotisation.
(v)
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 55
This reaction is known as Libermann’s nitroso test.
(vi) Aromatic tertiary amine reacts with nitrous acid at 273K to give p-nitroso compound.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 56

Question 30.
Explain why amino group is ortho para directing in electrophilic substitution reactions.
Answer:
The NH2 group is a strong activating group. In aniline the NH2 is directly attached to the benzene ring, the lone pair of electrons on the nitrogen is in conjugation with benzene ring which increases the electron density at ortho and para position, thereby facilitating the electrophilic attack at ortho and para.

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 31.
Aniline gives 2, 4, 6 tribromo aniline when treated with bromine water, but not a mono bromo aniline. Explain why?
Answer:
Aniline is a more powerful activating group. The lone pair of electrons enters into conjugation with the benzene ring, as a result both ortho and para position become rich in electron density. At the same time Br+ is also a strong electrophile. Hence, all the three positions are attacked by the electrophile.

Question 32.
Why is it necessary to acetylate aniline to get a mono bromo aniline?
Answer:
Acetylation of aniline reduces the activity of the amino group. The activity of the acetylated amine is reduced because the lone pair of electron on nitrogen is delocalised by the neighbouring carbonyl group by resonance. Hence, it is not easily available for conjugation.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 57
The acetyl amino group is less activating than amino group.

Question 33.
Explain why direct nitration of aniline gives a mixture of ortho, meta and para isomers.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 58
Nitration of aniline involves acidic medium. So protonation of aniline takes place forming mainly m-nitro aniline. Hence, direct nitration of aniline forms the following products.

Question 34.
How will you convert aniline?
(i) to p-bromo aniline
(ii) to 2,4,6 tribromo aniline
(iii) to para nitro aniline
(iv) to benzene diazonium chloride
(v) to sulphanilic acid
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 59
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 60
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 61

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 35.
What is zwitter ion? Explain with an example.
Answer:
Zwitter ion is a compound in which both acidic and basic groups are present in the same molecule, eg: sulphanilic acid. It has an acidic (SO2OH) and a basic group (NH2). Thus a proton from the acid leaves and protonates the basic group. As a result it exists as a dipolar ion.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 62

Question 36.
How will you distinguish between primary, secondary and tertiary amine?
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 63
Heisenberg reagent: Benzene sulphoanyl chloride in the presence of excess aqueous KOH solution.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 63

Question 37.
Complete the following reactions:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 65
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 66

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 38.
Give examples for (i) Sandmeyer’s reaction (ii) Gattermann reaction.
Answer:
(i) Sandmeyer’s reaction: Benzene diazonium chloride solution on reaction with cuprous chloride in hydrochloric acid (CuCl / HCl) or cuprous bromide in hydrochloric acid (CuBr / HCl) gives corresponding chloro benzene or bromo benzene. This reaction is known as Sandmeyer’s reaction. Aryl cyanides can also be prepared by this method.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 67
(ii) Gattermann reaction: This reaction involves the treatment of benzene diazonium chloride with Cu / HCl or Cu / HBr respectively instead of cuprous halide and hydrogen halide.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 68

Question 39.
How does the following reagents react with benzene diazonium chloride? Give equations.
(i) HBF4 and the product formed is heated.
(ii) HBF4 and die product formed is heated with an aqueous solution of sodium nitrite in the presence of copper.
(iii) HBF4 and the product is heated with CH3COOH.
(iv) Cuprous cyanide in the presence of KCN.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 69

Question 40.
Accomplish die following conversions.
(i) Nitrobenzene to benzene,
(ii) 4-Nitro aniline to 1, 2, 3 -tribromo benzene,
(iii) p-toludine to 2-bromo-4-methyl aniline,
(iv) m-nitro aniline to m-chloroaniline,
(v) p-nitroaniline to p-iodomtro benzene,
(vi) benzyl chloride to 2-phenyl ethanamine.
Answer:
(i) Nitrobenzene to benzene:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 70
(ii) 4 -nitro aniline to 1, 2, 3 – tribromo benzene.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 71
(iii) p-toludine to 2-bromo 4-methyl aniline.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 72
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 73
(vi) Benzyl chloride to 2- phenyl ethylamine.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 74

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 41.
Give equations for the following reactions.
(i) Ethyl bromide is treated with KCN
(ii) Heating acetamide with P2O5
(iii) Heating acetaldoxime with P2O5
(iv) Treating methyl magnesium bromide with cyanogen chloride.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 75
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 76

Question 42.
Write the IUPAC names of the following:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 77
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 78
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 79

Question 43.
What is the reducing agent used in the following reduction reactions? Give equations.
(i) Ethanenitrile to ethanamine
(ii) Benzonitrile to benzylamine
(iii) Ethane nitrile to Acetaldimine hydrochloride which on hydrolysis gives acetaldehyde.
Answer:
(a) Complete reduction or strong reduction when reduced with H2 in the presence of Pt or Ni as catalyst or by using LiAlH4, or sodium and alcohol alkyl or aryl cyanides yield primary amines.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 93
This specific type of reduction of alkyl or aryl cyanides using LiAlH4 or Na/ alcohol is named as mendices reduction.
(b) Partial reduction or mild reduction: When SnCl2 / HCl is used as a reducing agent at room temperature alkyl or aryl cyanides are reduced to amine hydrochloride which on subsequent hydrolysis gives aldehyde. This type of reduction is named as Stephen’s reduction.
SnCl2 + 2HCl → SnCl4 + 2 [H]
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 80

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 44.
Give examples for (i) Thrope nitrile condensation and (ii) Levine and Hauser acetylation.
Answer:
(i) Thrope nitrile condensation: Self condensation of two molecules of alkyl nitrile (containing α—H atom) in the presence of sodium to form iminonitrile.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 81
(ii) Levine and Hauser acetylation: The nitriles containing α-hydrogen also undergo condensation with esters in the presence of sodamide in ether to form ketonitriles. This reaction is known as “Levine and Hauser” acetylation. This reaction involves replacement of ethoxy (OC2H5) group by methylnitrile (-CH2CN) group and is called as cyanomethylation reaction.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 82

Question 45.
Write the electronic structure of alkyl cyanides and isocyanides.
Answer:
The electronic structure of alkyl cyanides is
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 83
The carbon atom of CN group is sp hybridised. CN group contain one σ and two pi bonds.
The electronic structure of isocyanides is
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 84
Structurally isocyanides are represented as a resonance hybrid of the following two forms.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 85
The dipolar form (I) makes higher contribution.

Question 46.
Name the reagents used in the following reactions.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 86
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 87

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 47.
What happens when methyl isocyanide is:
(a) treated with dilute HCl.
(b) treated with sodium and alcohol
(c) heated at 250°C
(d) treated with sulphur in the presence of ozone.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 88

Question 48.
Mention the uses of (a) Nitro alkanes,
(b) Nitrobenzene,
(c) Cyanides and isocyanides
Answer:
(a) Nitroalkanes:

  1. Nitromethane is used as a fuel for cars.
  2. Chloropicrin (CCl3NO2) is used as an insecticide.
  3. Nitroethane is used as a fuel additive and precursor to explosive and they are good solvents for polymers, cellulose ester, synthetic rubber and dyes etc.,
  4. 4% solution of ethylnitrite in alcohol is known as sweet spirit of nitre and in used as diuretic.

(b) Nitrobenzene:

  1. Nitrobenzene is used to produce lubricating oils in motors and machinery.
  2. It is used in the manufacture of dyes, drugs, pesticides, synthetic rubber, aniline and explosives like TNT, TNB.

(c) Cyanides and isocyanides;

  1. Alkyl cyanides are important intermediates in the organic synthesis of larger number of compounds like acids, amides, esters, amines etc.
  2. Nitriles are used in textile industry in the manufacture of nitrile rubber and also as a solvent particularly in perfume industry.

Question 49.
An organic compound (A) having the molecular formula C2H7N is treated with nitrous acid to give (B) of molecular formula C2H6O which answers the iodoform test. Identify A and B and explain the reactions.
Answer:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 89
Since, ‘B’ is an alcohol formed from A by the action of nitrous acid, A should be a primary amine which contains ‘NH2’ group.
C2H5N—NH2=C2H5 i.e. The alkyl group is C2H5 and hence A is C2H5NH2 ethyl amine. B is ethyl alcohol and it is confirmed by the fact that it answer iodo form test.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 90

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

Question 50.
An organic compound (A) with molecular formula C6H7N gives (B) with HNO2 / HCl at 273K. The aqueous solution of (B) on heating gives compound (C) which gives violet colour with neutral FeCl3. Identify the compounds A, B and C. Write the equations.
Answer:
A = C6H5NH2 (aniline);
B = C6H2N2Cl (benzene diazonium chloride)
C = C6H5OH (phenol)
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 91
(i) Since ‘C’ gives a violet colouration with neutral FeCl3 it should be phenol.
(ii) Since phenol is obtained by boiling aqueous solution of (B), it should be benzene diazonium chloride.
(iii) Hence, A should be aniline.
Equation:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 92

Choose the correct answer:

1.1, 2 dimethyl- 1-nitropropane. Choose the
incorrect statement about this compound.
(a) It is a primary nitro compound.
(b) It is also called nitroneopentane.
(c) The ‘NO2’ group is attached to a secondary carbon atom.
(d) It is an aliphatic compound.
Answer:
(c)

2. 1-nitrobutane and 2-methyl-1-nitro propane:
(a) chain isomers
(b) position isomers
(c) functional isomers
(d) metamers
Answer:
(a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 94

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

3. Which of the following nitro compounds does not exhibit tautomerism?
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 95
Answer:
(d)
Hint: Tertiary nitro alkanes do not exhibit tautomerism due to absence of a-H atoms.

4. The incorrect statement between nitroform and acidform of nitromethane is:
(a) nitroform is less acidic whereas aciform is more acidic.
(b) nitroform dissolves in NaOH slowly while aciform dissolves in NaOH instantly.
(c) Both decolorise FeCl3 solution
(d) They are tautomers
Answer:
(c)
Hint: Nitroform decolorises FeCl3 solution while aciform gives a reddish brown colour with FeCl3 solution.

5.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 96
Identify A and B.
(a) A = CH3CH2NO2 ; B = CH3CH2NH2
(b) A- CH3NO2 ; B = CH3NH2
(c) A = CH3CHO ; B = CH3CH2OH
(d) A = CH3CH2NH2 ; B = CH3CH2OH
Answer:
(a)

6.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 97
Identify A and B.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 98
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 99
Answer:
(b)

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

7. The products obtained by the reduction of nitromethane in acid medium and neutral medium are:
(a) methylamine and N-methylhydroxylamine
(b) methylamine and ethanol
(c) N-methylhydroxylamine and methylamine
(d) N-methylhydroxylamine in both cases.
Answer:
(a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 100

8. An amine is boiled with HCl and H2O. Which of the following will give acetone:
(a) CH3NH2
(b) (CH3)2CHNO2
(c) (CH3)3CNO2
(d) both (b) and (c)
Answer:
(b)
Hint: CH3NH2 gives CH3COOH (CH3)2
CHNO2 gives (CH3)2CO
(CH3)3 CNO2 no reaction

9. The correct IUPAC name for CH2=CH—CH2NH—CH3 is:
(a) Allylmethyl amine
(b) 2-amino-4-pentane
(c) 4 amino pent-l-ene
(d) N-methyl prop-2 en-1 amine
Answer:
(d)

10. Amongst the following the strongest base in aqueous medium is:
(a) CH3NH2
(b) NC—CH2NH2
(c) (CH3)2NH
(d) C6H5NH—CH3
Answer:
(c)
Hint: 2° amines are more basic than 1° amines, i. e., (CH3)2NH is more basic than CH3NH2. Due to -I effect of CN group NC—CH2NH2 is less basic than even CH3NH2. C6H5NHCH3 is less basic than both C6H5NH2 and (CH3)2NH due to delocalisation of lone pair of electrons on the N atom into the benzene ring.

11. In order to prepare a 1 ° amine from an alkyl halide with simultaneous addition of one CH2 group in the carbon chain, the reagent used a source of nitrogen is:
(a) Sodium amide, NaNH2
(b) Sodium azide, NaN3
(c) Potassium cyanide, KCN
(d) Potassium phthalimide C6H4(CO2) NK
Answer:
(c)
Hint: Cyanides on reduction gives 1: amines with a CH2 group
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 101

12. The correct increasing order of basic strength for the following compounds is:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 102
(a) II < III < I
(b) III < I < II
(c) III < II < I
(d) II < I < III
Answer:
(b)

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

13. Best method for preparing primary amines from alkyl halides without changing the number of carbon atoms in the chain is:
(a) Hoffmann bromamide reaction
(b) Gabriel’s phthalimide synthesis
(c) Sandmeyer’s reaction
(d) Reaction with NH3
Answer:
(b)

14. Which of the following compounds is the weakest Bronsted base?
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 103
Answer:
(c)
Hint: Amines (a) and (b) have a stronger tendency to accept a proton and hence stronger Bronsted bases than phenol (c) and alcohol (d) since phenol is more acidic than alcohol, phenol (c) has the least tendency to accept a proton and hence the weakest Bronsted base.

15. Which of the following compounds cannot be prepared by Sandmeyer’s reaction?
(I) Chlorobenzene
(II) Bromobenzene
(III) Iodo benzene
(IV) Fluoro benzene
(a) (IV)
(b) (III)
(c) (I) and (II)
(d) (III) and (IV)
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

16. The products of the following reaction are:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 104
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 105
Answer:
(c)
Hint: —NHCOCH3 is an o/p directing group.

17. An organic compound ‘A’ on treatment with NH3 gives ‘B’ which on heating gives ‘C’. ‘C’ when treated with Br2 in the presence of KOH produces ethylamine. The compound ‘A’ is:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 106
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 107

18. In a set of reactions, meta mono benzoic acid gave a product ‘D’. Identify D.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 108
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 109
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 110
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 111

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

19.
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 112
Answer:
(b)
Hint: Diazonium salts of benzylamine is not stable. It decomposes insitu, to form benzyl alcohol.

20. Predict the product:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 113
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 114
Answer:
(d)

21. Aniline in a set of following reactions yielded a coloured product Y. The structure of Y would be:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 115
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds 116

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

22. Butylamine (I), diethyl amine (II) and N, N diethyl amine, (III) have the same molar mass. The increasing order of their boiling points is:
(a) III < II < I
(b) I < II < III
(c) II < III < I
(d) III < I < II
Answer:
(a)
Hint: Extent of H-bonding increases as the number of H-atoms increases and hence boiling point increases in the order 3°<2°< 1°.

23. Assertion: Ammonolysis of alkyl halides is not a suitable method for the preparation of primary amines.
Reason: Ammonolysis of alkyl halides mainly produces 2° amines.
(a) Both assertion and reason are true and reason is the correct explanation of assertion.
(b) Both assertion and reason are true and reason is not the correct explanation of assertion.
(c) Assertion is true but reason is false.
(d) Both assertion and reason are false.
Answer:
(c)

24. Assertion: Gabriel phthalimide reaction can be used to prepare aryl and arylalkyl amines.
Reason: Aryl halides are as reactive as alkyl halides towards nucleophilic substitution reactions.
(a) Both assertion and reason are true and reason is the correct explanation of assertion.
(b) Both assertion and reason are true and reason is not the correct explanation of assertion.
(c) Assertion is true but reason is false.
(d) Both assertion and reason are false.
Answer:
(d)
Hint: Correct assertion: Gabriel phthalimide reaction can be used to prepare alkyl and aryl alkyl primary amines.
Correct reason: Alkyl and aralkyl halides undergo nucleophilic substitution reaction but aryl halides do not.

TN Board 12th Chemistry Important Questions Chapter 13 Organic Nitrogen Compounds

25. Assertion: Aniline does not undergo Friedel Craft’s reaction.
Reason: Friedel crafts reaction is an electrophilic substitution reaction.
(a) Both assertion and reason are true and reason is the correct explanation of assertion.
(b) Both assertion and reason are true and reason is not the correct explanation of assertion.
(c) Assertion is true but reason is false.
(d) Both assertion and reason are false.
Answer:
(b)
Hint: Correct explanation: AlCl3 forms a salt with aniline (C6H5NH2+ AlCl3) which deactivates the benzene ring thereby preventing Friedel craft’s reaction.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Students get through the TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Answer the following questions.

Question 1.
Write the IUPAC names of the following:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 1
Answer:
(i) 3-phenyl prop-2-en-l-al
(ii) cyclohexanecarbaldehyde
(iii) 3-oxopentan-l-al
(iv) But-2-en-l-al

Question 2.
Give the structure of the following compounds.
(i) 4 – Nitropropiophenone
(ii) 2 – Hydroxycyclopentane carbaldehyde
(iii) phenyl acetaldehyde
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 2

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 3.
Write the IUPAC names of
(i) Diacetone alcohol
(ii) Crotonaldehyde
Answer:
(i) 4-Hydroxy-4-methylpentan-2-ol
(ii) But-2-en-l-al

Question 4.
Write the structure of
(i) 3 – oxopentanal
(ii) 1 – phenylpentan – 1 – one
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 3

Question 5.
Name the following compounds according to IUPAC system of nomenclature.
(i) CH3CH(CH3)CH2CH2CHO
(ii) CH3CH2CO(C2H5)CH2CH2Cl
(iii) CH3CH=CHCHO
(iv) CH3COCH2COCH3
(v) CH3CH(CH3)CH2(CH3)2COCH3
(vi) (CH3)3CCH2COOH
(vii) OHCC6H4CHO(P)
Answer:
(i) 4-methyl pentanal
(ii) 6-chloro-4-ethylhexan-3 -one
(iii) But-2-en-l-al
(iv) Pentane 2,4, dione
(v) 3, 3, 5 Trimethylhexan – 2 – one
(vi) 3, 3, Dimethyl butanoic acid
(vii) Benzene 1,4, dicarbaldehyde

Question 6.
Draw the structures of the following compounds.
(i) 3-methyl butanal
(ii) 4-nitro propiophenone
(iii) p-methyl benzaldehyde
(iv) 4-methylpent-3-en-2-one
(v) 4-chloropentan-2-one
(vi) 3-Bromo-4-phenyl pentanoic acid
(vii) p, p’ dihydroxy benzo phenone
(viii) Hex-2-en-4 yonic acid
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 4
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 5

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 7.
Write IUPAC names of the following aldehydes and ketones. Wherever possible give also common names.
(i) CH3CO(CH2)4CH3
(ii) CH3CH2CH(Br)CH2CH(CH3)CHO
(iii) CH3(CH2)4CHO
(iv) Ph—CH=CH.CHO
(v)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 6
(vi) PhCOPh
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 193

Question 8.
Give the product of ozonolysis of the following alkenes.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 7
Answer:
To identify the product of ozonolysis, draw a line in between C=C bond and ‘O’ on either side of the double bond
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 8
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 9

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 9.
Identify the products of hydration of the following:
(i) ethyne
(ii) prop-1-yne
(iii) Hex-1-yne
(iv) Diphenyl acetylene
Answer:
Hydration means addition of water. The reagent used is mercuric sulphate and dilute sulphuric acid at 333K. Ketones are formed on hydration of alkynes. MarkovnikofFs mle is followed in water addition.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 10
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 11

Question 10.
How are the following compounds formed by distillation of calcium salts of their carboxylic acids?
(i) Formaldehyde,
(ii) Acetaldehyde,
(iii) Acetone,
(iv) Butan-2-one,
(v) Cyclopentanone,
(vi) Benzaldehyde
Answer:
(i) Calcium formate alone is heated.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 12
(ii) By dry distillation of calcium acetate and calcium formate.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 13
(iii) Dry distillation of calcium acetate alone.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 14
(iv) Calcium acetate and calcium propionate are distilled together.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 15
(v) Cyclic ketones are formed when calcium salts of dibasic acids are heated.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 16
(vi) By dry distillation of a mixture of calcium benzoate and calcium formate.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 17

Question 11.
Complete the following equations:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 18
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 19
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 20

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 12.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 21
(i) Identify the product.
(ii) Name the reaction.
(iii) What is the intermediate formed in the reaction.
Answer:
(i) CH3CHO (acetaldehyde)
(ii) Stephen’s reaction
(iii) CH3—CH=NH (an imine)
Complete reaction:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 22

Question 13.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 23
(i) Name the reagent i.e., X used for the above reduction.
(ii) Why other reducing agents like H2, in the presence of a catalyst are not used.
(iii) Write the IUPAC name of the product formed.
Answer:
(i) Diisobutyl aluminium hydride (DIBAL – H) is used as a reducing agent.
X = H2O
(ii) It selectively reduces alkyl cyanides to imines, which on hydrolysis gives aldehydes. The double bond in the nitrile is not reduced. The other reducing agents reduce the double bond also.
(iii) hex-4-enal is the IUPAC name of the product.

Question 14.
How is benzaldehyde prepared from (i) methyl benzene, (ii) benzene, (iii) benzyl alcohol. Give equations.
Answer:
(i) Oxidation of methyl benzene, using chromyl chloride as oxidising agent gives benzaldehyde. Acetic anhydride and CrO3 can also be used for reaction.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 24
(ii) Benzene is treated with CO and HCl Benzaldehyde is formed.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 25
This reaction is known as Gattermann- koch reaction.
(iii) Oxidation of benzyl alcohol using PCC (pyridinium chromo chromate) gives benzaldehyde.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 26

Question 15.
Identify the product of the following reactions. Write the complete equation.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 27
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 28
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 29

Question 16.
Give examples for Friedel-crafts acetylation reaction.
Answer:
Refer Question 15 (ii) and (iii). These reaction are called Friedel-crafts reaction. When acetyl chloride is used it is known as acetylation reaction. When benzoyl chloride is used, it is called benzoylation reaction.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 17.
The boiling points of aldehydes and ketones are high compared to hydrocarbons and ethers of comparable molecular mass. Explain why?
Answer:
It is due to the weak molecular association in aldehydes and ketones arising out of the dipole-dipole interactions.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 30

Question 18.
Explain nucleophilic addition reaction with an example.
Answer:
The carbonyl carbon carries a small degree of positive charge. Nucleophile such as CN can attack the carbonyl carbon and uses its lone pair to form a new carbon – nucleophile ‘σ‘ bond, at the same time two electrons from the carbon – oxygen double bond move to the most electronegative oxygen atom. This results in the formation of an alkoxide ion. In this process, the hybridisation of carbon changes from sp2 to sp3.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 31
The tetrahedral intermediate can be protonated by water or an acid to form an alcohol.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 32
eg: Addition of HCN
Attack of CN on carbonyl carbon followed by protonation gives cyanohydrins.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 33

Question 19.
Explain why the carbonyl group in aldehydes and ketones is polar.
Answer:
The carbonyl group of aldehydes and ketones contains a double bond between carbon and oxygen. Oxygen is more electronegative than carbon and it attracts the shared pair of electron which makes the carbonyl group as polar and hence aldehydes and ketones have high dipole moments.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 34

Question 20.
What is meant by the following terms? Give an example in each case.
(i) Cyanohydrin,
(ii) Acetal,
(iii) Semicarbazone,
(iv) Aldol
(v) Hemiacetal,
(vi) Oxime
(vii) Ketal,
(viii) Imine,
(ix) 2,4, DNP derivative
(x) Schiff’s base
Answer:
(i) gem – Hydroxy nitriles i.e., compounds containing hydroxyl and cyano groups on the same carbon atom are called cyano hydrins. These are produced by the addition of HCN to aldehydes and ketones in weakly basic medium.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 35
(ii) gem – dialkoxy alkanes in which two alkoxy groups attached to the terminal carbon atom are called acetals. They are produced by the action of an aldehyde with two equivalent of monohydric alcohol in the presence of dry HCl gas.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 36
(iii) Semi carbazones are derivatives of aldehydes and ketones and are produced by the action of semicarbazides on them in a weakly acidic medium.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 37
(iv) Aldols are β – hydroxy aldehydes or ketones and are produced by the condensation of two molecules of the same or one molecule each of two different aldehydes or ketones (containing an alpha hydrogen atom) in the presence of dilute, aqueous NaOH.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 38
(v) α – alkoxy alcohols are called hemi acetals. They are produced by the addition of one molecule of a mono hydric alcohol to an aldehyde in the presence of dry HCl gas.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 39
(vi) Oximes are produced when aldehydes or ketones react with hydroxyl amine in weakly acidic medium.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 40
(vii) gem-dialkoxy alkanes in which two alkoxy groups present on the same carbon atom are called ketals.
They are produced when a ketone is heated with ethylene glycol in the presence of dry HCl gas.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 41
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 42
(viii) Compounds containing >C=N group are called imines. These are produced when aldehydes and ketones react with ammonia and its derivatives.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 43
When ‘Z’ = H, alkyl, aryl,—NH, —OH, C6H5 etc..,
(ix) 2, 4, dinitro phenyl hydrazones (i.e., 2, 4, DNP derivative) are produced when aldehydes or ketones react with 2,4 dinitro phenyl hydrazine in weakly acidic medium.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 44
(x) Aldehydes and ketones react with primary aliphatic or aromatic amines in the presence of acid form azomethenes or schifTs bases. Schiffs bases may also be regarded as imines.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 45

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 21.
How does acetaldehyde react with (i) hydroxyl amine, (ii) hydrazine, (iii) phenyl hydrazine, (iv) semicarbazide? Give equations.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 46
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 47

Question 22.
Give equations for the reaction between
(i) acetaldehyde and sodium bisulphite
(ii) acetone and sodium bisulphite
Answer:

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 48

Question 23.
Write the structure of the prodcuts formed when acetone reacts with (i) hydrazine, (ii) phenyl hydrazine, (iii) semicarbazide.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 49
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 50

Question 24.
What is urotropine? How it is formed? Write its structure.
Answer:
Hexamethelenetetramine is called urotropine. It is formed when formaldehyde reacts with ammonia.
6HCHO + 4NH3 → (CH2)6N4 + 6H2O
Structure:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 51

Question 25.
Mention the uses of urotropine.
Answer:

  1. Urotropine is used as a medicine to treat urinary infection.
  2. Nitration of Urotropine under controlled condition gives an explosive RDX (Research and development explosive). It is also called cyclonite or cyclotri methylenetrinitramine.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 26.
What is popoffs rule? How it is used to predict the oxidation products of unsymmetrical ketones.
Answer:
It states that during the oxidation of an unsymmetrical ketone, a (C—CO) bond is cleaved in such a way that the keto group stays with the smaller alkyl group.
Eg:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 52

Question 27.
How will you prepare
(i) diacetone amine from acetone.
(ii) aldimine from acetaldehyde.
(iii) hydrobenzamide from benzaldehyde.
Answer:
(i)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 53
Two molecules of acetone, combine with ammonia to form diacetoneamine.
(ii)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 54
(iii) With ammonia, benzaldehyde forms a complex condensation product called hydrobenzamide.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 55

Question 28.
What is a haloform reaction? Explain with suitable example.
Answer:
Aldehydes and ketones containing CH3CO group (methyl carbonyl group), on treatment with excess halogen in the presence of an alkali produce a haloform (chloro form, bromo form, iodoform). This reaction is known as haloform reaction.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 56

Question 29.
What is iodoform test? Explain.
Answer:
Compounds containing CH3CO (methyl carbonyl) group or compounds on oxidation give compounds containing CH3CO group, when treated with iodine and NaOH gives a yellow precipitate is called iodoform. This is known as iodoform test.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 30.
How will you distinguish between by means of a chemical test.
(i) Propanal and propanone
(ii) acetaldehyde and benzaldehyde
(iii) Ethanal and propanal
Answer:
All these pairs of compounds can be distinguished by iodoform test.
(i) Propanone (CH3 CO CH3) will answer iodoform test. Propanal will not undergo iodo form test.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 57
(ii) Acetaldehyde (CH3CHO) will answer iodoform test, whereas benzaldehyde does not answer iodoform test
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 58
(iii) Ethanal (acetaldehyde) will answer iodoform test, but not propanal acetaldehyde
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 59
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 60

Question 31.
Write a short note an aldol condensation.
Answer:
The carbon attached to carbonyl carbon is called α – carbon and the hydrogen atom attached to α – carbon is called α – hydrogen. In presence of dilute base NaOH, or KOH, two molecules of an aldehyde or ketone having α – hydrogen add together to give β – hydroxyl aldehyde (aldol) or β – hydroxyl ketone (ketol). The reaction is called aldol condensation reaction. The aldol or ketol readily loses water to give α, β – unsaturated compounds which are aldol condensation products.
Acetaldehyde when warmed with dil.NaOH gives β – hydroxyl butraldehyde (acetaldol)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 61

Question 32.
Give the mechanism of aldol condensation.
Answer:
Mechanism: The mechanism of aldol condensation of acetaldehyde takes place in three steps.
Step 1: The carbanion is formed as the α – hydrogen atom is removed as a proton by the base.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 62
Step 2: The carbanion attacks the carbonyl carbon of another unionized aldehyde to form an alkoxide ion.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 63
Step 3: The alkoxide ion formed is protonated by water to form aldol.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 64
The aldol rapidly undergoes dehydration on heating with acid to form α – β unsaturated aldehyde.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 65

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 33.
Give the oxidation products obtained when pentan-2-one is oxidised by (conc.HNO3).
Answer:
During these oxidations, rupture of the carbon-carbon bonds occur on either side of the keto group giving a mixture of carboxylic acid, each containing less a number of carbon atom. Than the original ketone.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 66

Question 34.
What is crossed aldol condensation? Give an example.
Answer:
Aldol condensation can also takes place between two different aldehydes or ketones or between one aldehyde and one ketone such an aldol condensation is called crossed or mixed aldol condensation. This reaction is not very useful as the product is usually a mixture of all possible condensation products and cannot be separated easily.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 67

Question 35.
What happens when benzaldehyde reacts with (i) acetaldehyde in the presence of dilute NaOH (ii) acetone in the presence of dilute NaOH.
[OR] Explain with examples Claisen – Schmidt condensation.
Answer:
Benzaldehyde condenses with aliphatic aldehyde or methyl ketone in the presence of dil. alkali at room temperature to form unsaturated aldehyde or ketone. This type of reaction is called Claisen – Schmidt condensation.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 68

Question 36.
Write a short note on Cannizaro reaction.
Answer:
In the presence of concentrated aqueous or alcoholic alkali, aldehydes which do not have α – hydrogen atom under go self oxidation and reduction (disproportionation) to give a mixture of alcohol and a salt of carboxylic acid. This reaction is called Cannizaro reaction.
Benzaldehyde on treatment with concentrated NaOH (50%) gives benzyl alcohol and sodium benzoate.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 69
This reaction is an example of disproportion reaction.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 37.
Write the mechanism of Cannizaro reaction.
Answer:
Cannizaro reaction involves three steps.
Step 1: Attack of OH on the carbonyl carbons.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 70
Step 2: Hydride ion transfer
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 71
Step 3: Acid – base reaction

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 72
Cannizaro reaction is a characteristic of aldehyde having no α – hydrogen.

Question 38.
Give an example for crossed Cannizaro reaction.
Answer:
When Cannizaro reaction takes place between two different aldehyde (neither containing an α hydrogen atom), the reaction is called as cross cannizaro reaction.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 73
In crossed cannizaro reaction more reactive aldehyde is oxidized and less reactive aldehyde is reduced.

Question 39.
Give an example for benzoin condensation.
Answer:
Benzaldehyde reacts with alcoholic KCN to form benzoin
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 74

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 40.
Complete the following equation.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 74
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 76
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 77
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 78
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 79
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 80

Question 41.
How will you convert ethanal into following compounds?
(i) Butane 1, 3 diol
(ii) But -2-enal
(iii) But-2-enoic acid.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 81

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 42.
Give simple chemical tests to distinguish between the following pairs of compounds.
(i) Acetophenone and benzophenone
(ii) Phenol and benzoic acid
(iii) Pentan -2- one and pentan – 3-one
(iv) Benzaldehyde and acetophenone
Answer:
(i) Acetophenone and benzophenone: Acetophenone being a methyl ketone, when treated with I2 / NaOH (NaOI) gives a yellow precipitate of iodoform but benzophenone does not give a yellow precipitate.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 82
(ii) Phenol and benzoic acid: NaHCO3 test: Benzoic acid being a stronger acid than carbonic acid (H2CO3) decomposes NaHCO3 to evolve CO2, but phenol being weaker than carbonic acid does not.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 83
FeCl3 Test: Phenol gives a violet colouration with neutral ferric chloride solution, while benzoic acid gives a buff coloured precipitate of ferric benzoate.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 84
(iii) Pentan-2-one and pentan-3-one:
Sodium bisulphite test: 2-Pentanone being a methyl ketone when treated with a saturated solution of sodium bisulphite gives a white precipitate of 2 – pentanone sodium bisulphite addition compound where as 3 – pentanone does not.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 85
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 86
(Note: Sterically hindered ketones, do not undergo this reaction, eg: acetophenone)
Iodoform Test: 2 – pentanone, being a methyl ketone, when treated NaOI (I2 / NaOH) gives a yellow precipitate of iodoform but 3-pentanone does not.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 87
(iv) Benzaldehyde and acetophenone:
AgNO3 test: Benzaldehye reduces Tollen’s reagent to give a silver mirror (Ag) but acetophenone does not reduce Tollen’s reagent.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 88
Iodoform test: Acetophenone gives a yellow precipitate when treated with I2 / NaOH but benzaldehyde does not.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 89

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 43.
What happens when benzaldehyde is treated with
(i) Br2 in the presence of FeBr3
(ii) a mixture of conc.H2SO4 and conc.HNO3
(iii) conc.H2SO4
(iv) chlorine
(v) chlorine in the presence of FeCl3
(vi) methyl bromide in the presence of anhydrous AlCl3.
Answer:
(i) m-bromobenzaldehyde is formed.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 90
(ii) m-nitrobenzaldehyde is formed.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 91
(iii) m- benzaldehyde sulphonic acid is formed:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 92
(iv) Benzoyl chloride is formed:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 93
(v) m-chloro benzaldehyde is formed:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 94

Question 44.
Mention the uses of (i) formaldehyde (ii) urotropine (iii) acetaldehyde (iv) acetone (v) benzaldehyde (vi) acetophenone and benzophenone.
Answer:
Formaldehyde:

  1. 40% aqueous solution of formaldehyde is called formalin. It is used for preserving biological specimens.
  2. Formalin has hardening effect, hence it is used for tanning.
  3. Formalin is used in the production of thermosetting plastic known as bakelite, which is obtained by heating phenol with formalin.

Urotropine:

  1. Urotropine is used as a medicine to treat urinary infection.
  2. Nitration of Urotropine under controlled condition gives an explosive RDX (Research and development explosive). It is also called cyclonite or cyclotri methylene trinitramine.

Acetaldehye:

  1. Acetaldehyde is used for silvering of mirrors.
  2. Paraldehyde is used in medicine as a hypnotic.
  3. Acetaldehyde is used in the commercial preparation of number of organic compounds like acetic acid, ethyl acetate etc.,

Acetone:

  1. Acetone is used as a solvent, in the manufacture of smokeless powder (cordite).
  2. It is used as a nail polish remover.
  3. It is used in the preparation of sulphonal, a hypnotic.
  4. It is used in the manufacture of thermosoftening plastic Perspex.

Benzaldehyde is used:

  1. as a flavoring agent
  2. in perfumes
  3. in dye intermediates
  4. as starting material for the synthesis of several other organic compounds like cinnamaldehyde, cinnamic acid, benzyl chloride etc.

Aromatic Ketones:

  1. Acetophenone has been used in perfumery and as a hypnotic under the name hyphone.
  2. Benzophenone is used in perfumery and in the preparation of benzhydrol drop.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 45.
Give equation for the following reactions.
(i) Nitration of acetophenone
(ii) Bromination of benzophenone
(iii) Friedel – crafts alkylation of benzo phenone
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 95

Question 46.
Explain the structure of carboxylic acid group.
Answer:
A carboxyl group is made up of a carboxyl group joined to a hydroxyl group.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 96
In the carboxyl group, the carbon atom is attached to two carbon atoms: one by a double bond and the other by a single bond which in turn linked to a hydrogen atom by a single bond. The remaining free valency of the carbon atom of the carboxyl is satisfied by a H atom or an alkyl group. Thus, the structure of carboxylic acids.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 97
where ‘R’ is ‘H’ or alkyl group.
The carbon atom and the two oxygen atoms are sp2 hybridised. The two sp2 hybridesed orbitals of the carboxyl carbon overlap with one sp2 hybridised orbital of each oxygen atom while the third sp2 hybridised orbital of carbon overlaps with either a ‘s’ orbital of H – atom or a sp3 hybridised orbital of ‘C’ atom of the alkyl group to form three a bonds. Each of the two oxygen atoms are left with one unhybridised orbital which is perpendicular to the a bonding skeleton.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 98
All the three ‘p’ orbitals being parallel, overlap to form n bond which is partly delocalised between carbon and oxygen atoms on one side and carbon and oxygen of the ‘OH’group on the other side.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 99
In other words, RCOOH may be represented as a resonance hybrid of the following two canonical structures.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 100
As a result of resonance (i) the C—O single bond length in carboxylic acids is shorter than the normal C—O single bond in alcohols and ethers and (ii) C=O bond length in carboxylic acids is slightly larger than the normal C=O bond length in aldehydes and ketones.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 47.
How is acetic acid prepared from (i) ethanol (ii) methyl cyanide (iii) ethyl acetate (iv) methyl magnesium bromide (v) acetyl chloride (vi) acetic anhydride? Give equation.
Answer:
(i) Oxidation of ethanol by acidified K2Cr2O7.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 101
(ii) Acid hydrolysis of methyl cyanide.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 102
(iii) Acid hydrolysis of ethylacetate
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 103
(iv) Methyl magnesium bromide reacts with carbondioxide and the product formed on hydrolysis gives acetic acid.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 104
(v) Hydrolysis of acetyl chloride
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 105
(vi) Hydrolysis of acetic anhydride
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 106

Question 48.
Identify X and Y
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 107
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 108
Answer:
(i) X = C6H5COOMg Br; Y = C6H5COOH
(ii) X = C6H5COOH; Y = C6H5COCl
(iii) X = C6H5COOH; Y = C6H5COONa

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 49.
Explain why?
(i) Carboxylic acids have higher boiling point than aldehydes, ketones, or even alcohols of comparable molecular mass.
(ii) Lower aliphatic / carboxylic acid are miscible with water while higher carboxylic acids are immiscible with water.
Answer:
(i) Carboxylic acids have higher boiling point ’ than aldehydes, ketones and even alcohols of comparable molecular masses. This is due to more association of carboxylic acid molecules through intermolecular hydrogen bonding.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 109
(ii) Lower aliphatic carboxylic acids (up to four carbon) are miscible with water due to the formation of hydrogen bonds with water. Higher carboxylic acid are insoluble in water due to increased hydrophobic interaction of hydrocarbon part. The simplest aromatic carboxylic acid, benzoic acid is insoluble in water.

Question 50.
How will you convert
(i) Ethyl benzene to benzoic acid
(ii) Isopropyl benzene to benzoic acid
(iii) p-nitro toluene to p-nitrpbenzoic acid
(iv) o-xylene to phthalic acid
(v) But-2-ene to ethanoic acid
(vi) Benzonitrile to benzoic acid
(vii) Ethyl magnesium iodide to propanoic acid
(viii) Ethyl benzoate to benzoic acid
(ix) Benzamide to benzoic acid
(x) Propan – 2 – one to butanoic acid.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 110
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 111
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 112
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 113

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 51.
Which of the following compounds will undergo aldol condensation? Which the Cannizaro reaction, and which neither? Write the structure of the expected products of aldol condensation and Cannizaro reaction.
(i) Methanal
(ii) 2 – methylpentanal
(iii) Benzaldehyde
(iv) Benzophenone
(v) Cyclohexanone
(vii) Phenyl acetaldehyde
(viii) Butan-1-ol
(ix) 2, 2-dimethyl butanal
Answer:
I. 2 – methyl pentanal
Cyclohexanone
1 – phenyl propanone and phenyl acetaldehyde
contain one or more a hydrogen and hence undergo aldol condensation.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 114
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 115
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 116
II. Methanal, benzaldehyde, and 2,2 dimethyl butanal do not contain a hydrogen atoms and hence undergo cannizaro reaction. The reaction and structures are:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 117
III. Benzophenone is a ketone with no a hydrogens while butan-1-ol is an alcohol. Both of these neither undergo aldol condensation nor cannizaro reaction.

Question 52.
Give equations for reactions of acetic acid with the following reagents.
(i) Na (ii) NaOH (iii) Na2CO3 (iv) PCl5 (v) SOCl2 (vi) C2H5OH (vii) LiAlH4 (viii) Red P and HI (ix) Sodalime (x) NH3 followed by heating (xi) Cl2 / Red P.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 118
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 119
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 120
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 121

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 53.
Show how each of the following could be converted to benzoic acid:
(i) Ethyl benzene,
(ii) acetophenone,
(iii) benzophenone,
(iv) phenyl ethene.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 122
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 123
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 124

Question 54.
What is esterification? Give an example.
Answer:
The formation of an ester by the action of carboxylic acid and alcohol in the presence of an acid is called esterification.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 125
In these reaction the C—OH bond in acids is cleaved.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 55.
Give a brief accounts of decarboxylation reaction.
Answer:
Removal of CO2 from carboxyl group in called as decarboxylation. Carboxylic acids lose carbon di oxide to form hydrocarbon when their sodium salts are heated with soda lime (NaOH and CaO in the ratio 3:1)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 126

Question 56.
Suggest a suitable reagent to bring about the following conversions. Give equations.
(i) Acetic acid to acetyl chloride
(ii) Benzoic acid to ethyl benzoate
(iii) m – nitro benzoic acid to m – nitro methyl benzoate
(iv) Ethanoic acid to ethanol
(v) Acetic acid to ethane
Answer:
(i) PCl5 or SOCl2
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 127
(ii) C2H5OH in the presence of dil H2SO4
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 128
(iii) Methyl alcohol in the presence of dil. H2SO4
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 129
(iv) Lithium aluminium hydride
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 130
(v) HI in the presence of Red phosphorus
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 131

Question 57.
Give the products of the following:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 132
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 133
Answer:
All these reactions are decarboxylation reactions. In these reactions the COONa group is replaced by ‘H’.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 134

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 58.
What is HVZ reaction? Give an example.
Answer:
Carboxylic acids having an α – hydrogen are halogenated at the α – position on treatment with chlorine or bromine in the presence of small amount of red phosphorus to form α halo carboxylic acids. This reaction is known as Hell-Volhard-Zelinsky reaction (HVZ reaction) The α-Halogenated acids are convenient starting materials for preparing α – substituted acids, eg:
Substitution reaction in the hydrocarbon part α – Halogenetion:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 135

Question 59.
Explain why the ‘COOH’ group in benzoic acid in meta directing.
Answer:
The structure of benzoic acid is a resonance hybrid of the following canonical structure.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 136
Because of -M effect of carboxylic acid, the ortho and para positions becomes less in electron density relative to the meta position, i.e., meta-position becomes rich in electron density compared to ortho and para positions. Hence, the electrophile attacks the meta position, i.e., the COOH group deactivates the benzene ring and is the meta directing group.

Question 60.
How are the following compounds prepared from benzoic acid?
(i) m- Bromo benzoic acid
(ii) m- nitro benzoic acid
(iii) m-sulpho benzoic acid.
Answer:
(i) Bromination of benzene gives m – bromo benzoic acid.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 137
(ii) Nitration of benzene using nitrating mixture gives m – nitro benzoic acid.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 138
(iii) Sulphonation of benzene, using fuming sulphuric acid gives m – sulpho benzoic acid.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 139

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 61.
Formic acid is a reducing agent. Substantiate this statement with examples.
Answer:
Formic acid contains both an aldehyde as well as an acid group. Hence, like other aldehydes, formic acid can easily be oxidised and therefore acts as a strong reducing agent.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 140
(i) Formic acid reduces Tollens reagent (ammonical silver nitrate solution) to metallic silver.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 141
(ii) Formic acid reduces Fehlings solution. It reduces blue coloured cupric ions to red coloured cuprous ions.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 142

Question 62.
Give the tests for carboxylic acid group in an organic compound.
Answer:

  1. In an aqueous solution, carboxylic acid turns blue litmus red.
  2. Carboxylic acids give brisk effervescence with sodium bicarbonate due to the evolution of carbon dioxide.
  3. When a carboxylic acid is warmed with alcohol and conc.H2SO4 it forms an ester, which is detected by its fruity odour.

Question 63.
Give a brief account of the acidity of carboxylic acids.
Answer:
Carboxylic acids undergo ionization to produce H+ and carboxylate ions in an aqueous solution. The carboxylate anion is stabilized by resonance which makes the carboxylic acid to donate the proton easily.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 143
The resonance structure of carboxylate ion are given below.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 144
The strength of carboxylic acid can be expressed in terms of the dissociation constant(Ka):
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 145
The dissociation constant is generally called acidity constant because it measures the relative strength of an acid. The stronger the acid, the large will be its Ka value.
The dissociation constant of an acid can also be expressed in terms of pKa value.
pKa = log Ka
A stronger acid will have higher Ka value but smaller pKa value, the reverse is true for weaker acids.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 64.
Briefly discuss the effect of substituents on the acidity of carboxylic acids.
Answer:
Effect of substituents on the acidity of carboxylic acid.
(i) Electron releasing alkyl group decreases the acidity: The electron-releasing groups (+1 groups) increase the negative charge on the carboxylate ion and destabilize it and hence the loss of proton becomes difficult. For example, formic acid is more stronger than acetic acid,
eg:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 146
(ii) Electron withdrawing substituents increases the acidity: The electron-withdrawing substituents decrease the negative charge on the carboxylate ion and stabilize it. In such cases, the loss of proton becomes relatively easy.
Acidity increases with increasing electronegativity of the substituents. For example, the acidity of various halo acetic acids follows the order F—CH2—COOH > Cl—CH2—COOH > Br—CH2—COOH > I —CH3—COOH
Acidity increases with increasing number of electron – withdrawing substituents on the a – carbon.
For example
Cl3C—COOH > Cl2CH—COOH > ClCH2COOH > CH3COOH
The effect of various, electron withdrawing groups on the acidity of a carboxylic acid follows the order,
—NO2 > —CN >—F >—Cl >—Br >—I >Ph
The relative acidities of various organic compounds are
RCOOH > ArOH > H2O > ROH >RC ≡ CH

Question 65.
Fluorine is more electronegative than chlorine even their p- fluoro benzoic acid in weaker than p- chloro benzoic aicd. Explain.
Answer:
Since halogens are far more electronegative than carbon and also possess lone pairs of electrons, they exert both -1 and + M effects. Now, the fluorine, the lone pairs of electrons are present in ‘2p’ orbitals and in chlorine, they are present in ‘3p’ orbitals. Since ‘2p’ orbitals of fluorine and chlorine are of almost equal size, the + M effect is more pronounced in p fluoro benzoic acid than in p-chloro benzoic effect.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 147

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 66.
Explain why p – nitrobenzoic acid has a higher Ka value than benzoic acid.
Answer:
Higher the Ka value, the stronger is the acid. Thus, p-nitro benzoic acid is a stronger acid than benzoic acid. This is due to

  1. Because of — I and -M effect of NO2 group the electron density in O—H bond decreases. As a result, the —O—H bond becomes weak and hence, p – nitrobenzoic acid easily loses a proton than benzoic acid.
    TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 148
  2. Due to -1 and -M effect of nitrogroup dispersal of negative charge occurs and hencep -nitro benzoate ion becomes more stable than benzoate ion.
    TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 149

Question 67.
Give the IUPAC names of the following compounds,
(i) PhCH2CH2COOH
(ii) (CH3)2C=CHCOOH CH
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 150
Answer:
(i) 3 -phenyl propanoic acid
(ii) 3 -methyl but – 2-enoic acid
(iii) 2 -methylcyclopentane carboxylic acid
(iv) 2, 4, 6 -trinitro benzoic acid or 2, 4, 6-trinitro benzene carboxylic acid.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 68.
Explain the mechanism for the reaction.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 151
Answer:
Esterification of carboxylic acids with alcohols is a nucleophilic acyl substitution.
In such reactions the nucleophile first adds to a carbonyl group to give a tetrahedral intermediate which then readily loses the leaving group to give the substitution products. The mechanism involves the following steps.
Step 1: Protonation of the carbonyl group:
In the presence of mineral acids (H2SO4 or HCl), the carbonyl group of the carboxylic acid accepts a proton to form protonated carboxylic acid.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 152
Step 2: Nucleophilic attack of the alcohol molecule. As a result of protonation, the carbonyl carbon becomes electrophilic (i.e. more electropositive) and hence readily undergoes nucleophilic attack by lone pairs of electrons on the oxygen atom of the alcohol molecule to form a tetrahedral intermediate (II).

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 153
Step 3: Loss of a molecule of water and a proton. The tetrahedral intermediate (II) undergoes a proton transfer to give another tetrahedral intermediate (III). During this proton transfer, the OH group gets converted to – OH2 group which being a good leaving group is lost as a neutral water molecule. The protonation ester (IV), thus formed, finally loses a proton to give the ester (V).
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 154

Question 69.
Give the uses of (i) formic acid (ii) acetic acid (iii) benzoic acid (iv) acetyl chloride (v) acetic anhydride (vi) ethyl acetate.
Answer:
Formic acid: It is used

  1. for the dehydration of hides
  2. as a coagulating agent for rubber latex
  3. in medicine for the treatment of gout
  4. as an antiseptic in the preservation of fruit juice.

Acetic acid: It is used

  1. as table vinegar
  2. for coagulating rubber latex
  3. for manufacture of cellulose acetate and poly vinylacetate.

Benzoic acid: It is used

  1. as food preservation either in the pure form or in the form of sodium benzoate
  2. in medicine as an urinary antiseptic
  3. for manufacture of dyes.

Acetyl chloride: It is used

  1. as acetylating agent in organic synthesis
  2. in detection and estimation of —OH, — NH2 groups in organic compounds.

Acetic anhydride: It is used

  1. acetylating agent
  2. in the preparation of medicine like asprin and phenacetin
  3. for the manufacture plastics like cellulose acetate and poly vinyl acetate.

Ethyl acetate is used

  1. in the preparation of artificial fruit essences
  2. as a solvent for lacquers
  3. in the preparation of organic synthetic reagent like ethyl acetoacetate.

Uses
Acetamide is used in the preparation of primary amines.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 70.
A compound with molecular formula, C4H10O3 on acetylation with acetic anhydride gives a compound with molecular weight 190. Find out the number of hydroxyl groups present in the compound.
Answer:
During acetylation one ‘H’ atom (at mass = 1 amu) of the OH group is replaced by an acetyl group (CH3CO – molar mass = 43 amu)
—OH + (CH3CO)2O → —O—COCH3 + CH3COOH
In other words acetylation of each OH group increases the molecular mass by 43 – 1 = 42 amu. Now that the molecular mass of the compound C4H10O3 = 106 amu, while that of the acetylated product is 190 amu. Therefore the number of ‘OH’ groups present in the compound is \(\frac{190-106}{42}\) =2.

Question 71.
Explain (i) Perkins’ reaction (ii) Knoevenagal reaction.
Answer:
(i) Perkins’ reaction:
When an aromatic aldehyde is heated with an aliphatic acid anhydride in the presence of the sodium salt of the acid corresponding to the anhydride, condensation takes place and an α, β unsaturated acid is obtained. This reaction is known as Perkin’s reaction.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 155
(ii) Knoevenagal reaction:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 156
Benzaldehyde condenses with malonic acid in presence of pyridine forming cinnamic acid, Pyridine act as the basic catalyst.

Question 72.
Give names of reagents which bring about the following conversions.
(i) Hexan-1-ol to hexanal
(ii) Cyclohexanol to cyclohexanone
(iii) p-fluorotoluene to p-fluorobenzaldehyde,
(iv) Ethanenitrile to ethanal
(v) allyl alcohol to propenal
(vi) But-2-ene to ethanal
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 157
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 158

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 73.
Bring out Che following conversions.
(i) Benzyl alcohol to phenyl ethanoic acids.
(ii) 3 – nitrobromo benzene to – 3 – nitrobromo benzoic acid
(iii) Methyl acetophenone to benzene 1, 4, dicarboxylic acid
(iv) cyclohexene to hexane 1, 6 dicarboxylic acid.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 159

Question 74.
Identify A – E in the following reactions:
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 160

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 75.
Write a short note on the electrophilic substitution reaction of benzaldehyde.
Answer:
The ‘CHO’ group in benzaldehyde deactivates the benzene ring due to its —M effect. As a result the electron densities in ortho and para position are decreased compared to the meta position, i.e, The meta position is electron rich compared to ortho and para position. Hence electrophilic substitution reaction occur at meta position.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 161

Question 76.
Which acid of each pair shown here would you expect to be stronger?
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 162
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 163
Answer:
(i)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 164
(ii) Due to much stronger -1 effect of F over Cl FCH2 COO ion is much more stable than ClCH2COO ion and hence FCH2COOH is a stronger acid than ClCFI2COOH.
(iii)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 165
Inductive effect decreases with increasing distance, therefore, -I effect of is somewhat stronger in 3-fluorobutanoic acid than in 4-fluorobutanoic acid. In other words, CH3CHCH2COCT ion is in more stable than
FCH2CH2CH2COO ion and hence TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 166 is a stronger acid than FCH2CH2CH2COOH.
Therefore due to greater stability of CF3—C6H4—COO (p) ion over CH3—C6H4COOH (p) is a stronger acid than H3CC6H4—COOH (p).
(iv)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 167

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 77.
Identify A to E in the following reactions:
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 168
(Note: NaBH4 reduces COCl to CH2OH, but does not reduce NO2 to NH2 group.)

Question 78.
How will you bring about the following conversions in not more than two steps?
(i) Propanone to propene
(ii) Benzoic acid to benzaldehyde
(iii) Ethanol to 3 – hydroxy butanal
(iv) Benzene to m – nitrobenzene
(v) Benzaldehyde to benzophenone
(vi) bromo benzene to 1-phenyl ethanol
(vii) Benzaldehyde to 3 phenylpropan-1-ol
(viii) Benzaldehyde to a – hydroxy phenyl acetic acid
(ix) Benzoic acid to p-nitrobenzyl alcohol.
Answer:
(i) Propanone to propene:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 169
(ii) Benzoic acid to benzaldehyde
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 170
(iii) Ethanol to 3 – hydroxy butanal:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 171
(iv) Benzene to m – dinitrobenzene:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 172
(v) Benzaldehyde to benzophenone:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 173
(vi) Bromobenzene to 1 – phenyl ethanol:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 174
(vii) Benzaldehyde to 3 – phenylpropan – 1 – ol:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 175
(viii) Benzaldehyde to a – hydroxyphenyl acetic acid:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 176
(ix) Benzoic acid to m-nitrobenzyl alcohol:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 177

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 79.
What is transesterification? Give an example.
Answer:
Esters of an alcohol can react with another alcohol in the presence of a mineral acid to give the ester of second alcohol. The interchange of alcohol portions of the esters is termed transesterification.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 178

Question 80.
Give an example for Claisen condensation.
Answer:
Esters containing at least one α – hydrogen atom undergo self-condensation in the presence of a strong base such as sodium ethoxide to form β – keto ester. This reaction is known as Claisen condensation.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 179

Question 81.
How are the following compounds prepared?
(i) acetyl chloride and ethyl chloride from ethyl acetate
(ii) acetamide from acetyl chloride
(iii) Acetamide from acetic anhydride.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 180

Question 82.
Complete the following equation:
(i) CH3COCl + CH3NH2
(ii) CH3COCl + (CH3)2 NH →
(iii) (CH3CO)2O + PCl5
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 181

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 83.
How are the following compounds prepared from acetamide?
(i) acetic acid (ii) sodium acetate (iii) methyl cyanide (iv) methyl amine (v) ethyl amine
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 182

Question 84.
Write the structure and IUPAC names of the following acid derivatives.
(i) acetyl chloride (ii) propionyl chloride (iii) Benzoyl chloride (iv) acetic anhydride (v) propionic anhydride (vi) benzoic anhydride (vii) methyl acetate (viii) Ethyl acetate (ix) phenyl acetate (x) acetamide (xi) propionamide (xii) Benzamide.
Answer:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 183
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 184

Question 85.
Briefly explain amphoteric nature of acid amide.
Answer:
Amides behave both as weak acid as well as weak base and thus show amphoteric character. This can be proved by the following reactions.
Acetamide (as base) reacts with hydrochloric acid to form salt.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 185
Acetamide (as acid) reacts with sodium to form sodium salt and hydrogen gas is liberated.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 186

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

Question 86.
An unknown aldehyde (A) on reaction with alkali gives a β – hydroxy aldehyde which loses water to form an unsaturated aldehyde, 2-butanal. Another aldehyde (B) undergoes a disproportionation reaction in the presence of conc.alkali to form products (C) and (D). (C) is an aryl alcohol with formula C7H8O. Identify (A) and (B).
(ii) Write the sequence of chemical reaction involved.
(iii) Name the product, when (B) reacts with zinc amalgam and hydrochloric acid.
Answer:
Since the aldehyde (A) oft reaction With alkali gives a β – hydroxy aldehyde (i.e, an aldol), which loses water to form 2 – butanal (an unsaturated aldehyde) ‘A’ must be acetaldehyde.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 187
Since aldehyde (B) on treatment with conc.alkali undergo disproportionation (i.e., Cannizaro reaction) to give two products (C) and (D). One of these products must be an alcohol and the other must be the corresponding acid. Further, since, the product (C) is an aryl alcohol with molecular C7H5O, (C) must be benzyl alcohol, (i.e, C6H5 aryl group) OH is alcoholic group C6H5O. C7H8O—C6H6O = CH2. i.e, C6H5CH2OH. (D) must be sodium benzoate and aldehyde (B) must be benzaldehyde.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 188
Thus aldehyde (A) is acetaldehyde, (B) is benzaldehyde.
(ii) The sequence of reaction is already explained above.
(iii) When (B) reacts with Zn—Hg / HCl, toluene obtained.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 189

Question 87.
A compound ‘X’ (C2H4O) on oxidation gives ‘Y’ (C2H4O2). X undergoes a haloform reaction. On treatment with HCN, (X) forms (Z) which on hydrolysis gives 2 – hydroxy propanoic acid.
(i) Write down the structures of ‘X’ and ‘Z’.
(ii) Name the product when ‘X’ is treated with dilute NaOH.
(iii) Write down the equation for the reaction involved.
Answer:
(a) Since the MF C2H4O of X corresponds to the general formula CnH2nO, characteristic of aldehydes or ketones. (X) may either be an aldehyde or ketone. Since ketone must have at least ‘3’ carbon atoms but X (C2H4O) has only ‘2’ two. Therefore (X) must be an aldehyde. The only possible aldehyde is CH3CHO (MF C2H4O) (acetaldehyde).
If (X) is acetaldehyde, than the compound (Z) is acetic acid (CH3COOH).
(b) (X) is acetaldehyde is confirmed by the following reaction.
(i) It undergoes haloform reaction
(i.e.,)
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 190
(ii) On treatment with KCN, acetaldehyde forms a cyanohydrin (Z) which on hydrolysis gives 2 – hydroxy propanoic acid.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 191
(iii) In the presence of dilute NaOH, acetaldehyde undergoes aldol condensation to form 3- hydroxy butanal commonly called aldol.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 192

Choose the correct answer:

1. The IUPAC name of the compound is
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 194
(a) Mesityl oxide
(b) 4- methyl pent – 3 – en – 2 – one
(c) 4 – methyl pent – 2 – en – 4 – one
(d) 2 – methyl pent – 4 – one
Answer:
(b)

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

2. Ozonolysis of 2-methyl but-2-ene followed by treatment with Zn/H2O gives:
(a) ethanal
(b) propanone
(c) propanal and prop – 2 – one
(d) ethanal and propan – 2 – one
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 195

3. Identify the product ‘Y’ in the following reaction sequence.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 196
(a) pentane
(b) cyclobutane
(c) cyclopentane
(d) cyclopentanone
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 197

4. One mole of a symmetrical alkene on ozonolysis gives two moles of an aldehyde having molecular mass 44 u. The alkene is:
(a) 2 – butene
(b) ethene
(c) propene
(d) 1 – butene
Answer:
(a)
Hint: The aldehyde with molecular mass 44 u is CH3CHO (acetaldehyde). Therefore the symmetrical alkene is 2 – butene.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 198

5. Ozonolysis of an organic compound gives formaldehyde as one of the products. This confirms the presence of:
(a) a vinyl group
(b) an isopropyl group
(c) an acetylene triple bond
(d) two ethylenic double bonds
Answer:
(a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 199

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

6. Identify the compound ‘X’ in the following reaction:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 200
Answer: (a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 201

7. The order of reactivity of phenyl magnesium bromide (PhMgBr) with the following compounds.
I. CH3CHO,
II. (CH3)2CO and
III. PhCOPh is:
(a) III > II > I (b) II > I > III
(c) I > III > II (d) I > II > III
Answer:
(d)
Hint: Reaction between RMgX with carbonyl compound is nucleophilic addition. The greater the positive charge on the carbonyl carbon, the faster is the rate of nucleophilic addition.

8. A carbonyl compound reacts with hydrogen cyanide to form a cyanohydrin which on hydrolysis forms a racemic mixture of a – hydroxy acids. The carbonyl compound is:
(a) formaldehyde
(b) acetaldehyde
(c) acetone
(d) diethyl ketone
Answer:
(b)
Hint: Acetaldehyde cyanohydrin TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 202 on hydrolysis gives lactic acid TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 203
This contains a chiral carbon and exists as a racemic mixture. All other compounds are symmetrical and hence, their cyanohydrins and their corresponding α – hydroxy acids are not optically active because they do not contain chiral carbon.

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

9. In a set of reactions, acetic acid yielded the product D
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 204
The structure of ‘D’ would be:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 205
Answer:
(a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 206

10. (CH3)2C=CHCOCH3 can be oxidised to (CH3)2C=CHCOOH by:
(a) Chormic acid
(b) NaOI
(c) Cu at 300°C
(d) KMnO4
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 207

11. A compound ‘A’ (C5H10C312) on hydrolysis gives C5H10O which reacts with NH2OH, forms iodoform but does not give Fehling’s test A is:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 208
Answer:
(a)
Hint: Since the compound ‘A’ on hydrolysis gives C5H10O does i ot reduce Fehlings solution but reacts with NH2OH, forms iodoform, it must be methyl ketone.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 209

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

12. Acetophenone, when reacted with a base, C2H5ONa, yields a stable compound that has the structure:

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 210
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 211
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 212

13.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 213
The structure of ‘B’ is:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 214
Answer: (a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 215

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 216

14. Self-condensation of two moles of ethyl acetate in presence of sodium ethoxide yields:
(a) ethyl propionate
(b) ethyl butyrate
(c) acetoacetic ester
(d) methyl acetoacetate
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 217

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

15. m- chlorobenzaldehyde on reaction with conc. KOH at room temperature gives:
(a) potassium-m-chloro benzoic acid and m-hydroxy benzaldehyde.
(b) m-hydroxy benzaldehyde and m-chloro benzyl alcohol.
(c) m-chloro benzyl alcohol and m-hydroxy benzyl alcohol.
(d) potassium-m-chloro benzoate and m-chloro benzyl alcohol.
Answer: (d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 218

16. Consider the following compounds:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 219
Which will give the iodoform test?
(a) only I
(b) both I and II
(c) only II
(d) all
Answer:
(c)
Hint: Although TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 220 contains a CH3CO group linked to carbon, it does not undergo iodoform test. This is because iodination occurs at the more reactive CH2 group rather than terminal CH3 which is essential for iodoform test to occur
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 221

17. Fehling solution will oxidise:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 222
(a) All
(b) only I and IV
(c) only II and IV
(d) only III and IV
Answer:
(d)
Hint: Fehling solution oxidises only aliphatic aldehydes

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

18.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 223
The product ‘Z’ is:
(a) benzaldehyde
(b) benzoic acid
(c) benzene
(d) toluene
Answer:
(b)
Hint:
X = Benzene
Y = Toluene
Z = Benzoic acid

19. Match entries of column I with appropriate entries of column II.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 224
(a) (A) – (p)- (B) – (s)- (C) – (q); (D) – (r)
(b) (A) – (q); (B) – (s); (C) – (p); (D) – (r)
(c) (A) – (r); (B) – (s); (C) – (p); (D) – (q)
(d) (A) – (r); (B) – (p); (C) – (q); (D) – (s)
Answer:
(c)

20. Assertion: Fehling solution oxidizes acetaldehyde to acetic acid but not benzaldehyde to benzoic acid.
Reason: The C—H bond in benzaldehyde is stronger than acetaldehyde.
(a) Both assertion and reason are correct and the reason is the correct explanation of assertion.
(b) Both assertion and reason are correct but the reason is not the correct explanation of assertion.
(c) Assertion is true but reason is wrong.
(d) Both assertion and reason are wrong.
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

21. Assertion: Carboxylic acids contain a carbonyl group but do not give characteristic reactions of the carbonyl group.
Reason: Due to resonance, the electrophilic nature of the carboxyl cation is greatly reduced as compared to carbonyl carbon in aldehydes and ketones.
(a) Both assertion and reason are correct and the reason is the correct explanation of assertion.
(b) Both assertion and reason are correct but the reason is not the correct explanation of assertion.
(c) Assertion is true but the reason is wrong.
(d) Both assertion and reason are wrong.
Answer:
(a)

22. Among the following acids which has the lowest pKa value?
(a) CH3COOH
(b) HCOOH
(c) (CH3)2CHCOOH
(d) CH3CH2COOH
Answer:
(b)
Hint: HCOOH is the strongest acid and hence the lowest pKa value.

23. Which of the following presents the correct order of the acidity in the given compounds?
(a) FCH2COOH > ClCH2COOH > BrCH2COOH > CH3COOH
(b) CH3COOH > BrCH2COOH > ClCH2COOH > FCH2COOH
(c) FCH2COOH > CH3COOH > BrCH2COOH > ClCH2COOH
(d) BrCH2COOH > ClCH2COOH > FCH2COOH > CH3COOH
Answer:
(a)

24. The correct acidity order of the following is
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 225
(a) III > IV > II > I
(b) IV > III > I > II
(c) III > II > I > IV
(d) II > III > IV > I
Answer: (a)
Hint: Carboxylic acids are stronger than phenols. Further, electrons donating groups decrease the acidity of phenol/carboxylic acid while electron-withdrawing groups increase the acidity of phenol/carboxylic acid. Thus, the over all order.
III > IV > II > I

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

25. Which one of the following pairs gives effervescence with aq.NaHCO3
I. CH3COCI
II. CH3COCH3
III. CH3COOCH3
IV. CH3COOCOCH3
(a) I and II
(b) I and IV
(c) II and III
(d) I and III
Answer:
(b)
Hint: Both CH3COCl and CH3COOCOCH3 react with water to produce acids and hence give effervescence with NaHCO3.

26. Propionic acid with Br2/P yields a dibromo product. Its structure would be:
(a) CH(Br)2—CH2COOH
(b) CH2(Br)CH2COBr
(c) CH3C(Br)2COOH
(d) CH2(Br)CH(Br)COOH
Answer:
(c)
Hint:Bromination occurs at a position.

27. When benzoic acid is treated with LiAlH4, it forms:
(a) benzaldehyde
(b) benzyl alcohol
(c) benzene
(d) toluene
Answer:
(b)

28. Sodium ethoxide reacts with ethanoyl chloride. The compound that is produced in the above reaction is:
(a) 2-butanone
(b) ethyl chloride
(c) ethyl ethanoate
(d) diethyl ether
Answer:
(c)
Hint: CH3COCl + C2H5ONa → CH3COOC2H5 + NaCl

TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids

29. Consider the following:
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 226
The correct decreasing order of their reactivity towards hydrolysis is:
(a) II > IV > I > III
(b) II > IV > III > I
(c) I > II > III > IV
(d) IV > II > I > III
Answer:
(a)
Hint: Electron donating groups decrease while electron-withdrawing groups increase the reactivity of acid chlorides towards hydrolysis.
TN Board 12th Chemistry Important Questions Chapter 12 Carbonyl Compounds and Carboxylic Acids 227
The reactivity depends on the positive charge on the cabonyl carbon.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Students get through the TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Answer the following questions.

Question 1.
Classify the following as primary, secondary and tertiary alcohols.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 1
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 2
Answer:
Primary alcohols: (i), (ii), (iii)
Secondary alcohols: (iv), (v)
Tertiary alcohol: (vi)

Question 2.
Identify allyl alcohols in the above (Q.No. 1) examples.
Answer:
(ii) and (vi).

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 3.
Name the following compounds according to IUPAC system:
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 3

Question 4.
Write IUPAC names of the following:
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 4
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 5

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 5.
Write the structures of the compounds whose IUPAC names are as follows:
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 6
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 7

Question 6.
Complete the following reactions:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 8
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 9
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 10

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 7.
Using suitable Grignard reagent and a carbonyl compound, how will you prepare
(i) phenyl methanol,
(ii) butan-2-ol,
(iii) 2-methylhexan-2-ol,
(iv) propan-2-ol.
Answer:
(i) phenyl methanol:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 11
(ii) butan-2-ol:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 12
(iii) 2-methylhexan-2-ol:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 13
(iv) propan-2-ol:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 14

Question 8.
Give equation for the preparation of 2-methyl-2-propanol using a suitbale Grignard reagent and a carbonyl compound.
Answer:
Tertiary containing at least two identical groups can be prepared by the addition of a Grignard reagent to an ester other the formic ester followed by acid hydrolysis.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 15

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 9.
Name the reducing agents that will convert a carbonyl compound to an alcohol. Give an example for each.
Answer:
Raney Ni, / Sodium analgen in H2O (Na—Hg/H2O), H2 in the presence of Pt.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 16
where ‘R’ is an alkyl group.

Question 10.
Why is LiAlH4 is used to reduce crotonaldehyde?
Answer:
Li crotonaldehyde is an unsaturated aldehyde (CH3CH=CHCHO). Lithium aluminium hydride selectively reduces ‘CHO’ group to ‘CH2OH’ group without affecting the C=C.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 17

Question 11.
Name the product formed when sodium borohydride is used as a reducing agent for the reduction of a compound containing both carbonyl and carboxyl group, (or) Identify the product:
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 18

Question 12.
Complete the following reactions:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 19
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 20
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 21

Question 13.
How is glycerol prepared from triglycerides or fats?
Answer:
The alkaline hydrolysis of these fats gives glycerol and the reaction is known as saponification.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 22

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 14.
Complete the following equations:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 23
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 24
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 25

Question 15.
Give mechanism of reaction between alcohols and halogen acids.
Answer:
Primary alcohols react by SN2 mechanism while secondary and tertiary alcohol react by SN1 mechanism.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 26

Question 16.
How will you distinguish between
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 27
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 28
(ii) Secondary alcohol will give a blue colour as shown above whereas a tertiary alcohol will not produce any colour.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 29

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 17.
Give the structures of the products you would expect when each of the following alcohol reacts with (a) HCl-ZnCl2, (b) HBr, (c) SOCl2 (i) Butan-l-ol and (ii) 2-methylbutan-2-ol.
Answer:
(a) with HCl-ZnCl2 (Lucas reagent):
[2-methylbutan-2-ol being a tertiary alcohol reacts with Lucas reagent to produce turbidity immediately due to formation of insoluble tert-alkyl-halide, while butan-l-ol being a primary alcohol does not react with Lucas reagent at room temperature.]
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 30
(b) with HBr: Both alcohols produce the corresponding alkyl bromides.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 31
(c) with SOCl2: Both alcohols react to form their corresponding alkyl chlorides.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 32

Question 18.
Arrange the following compounds in increasing order of boiling points, pentan-1 -ol, butan-1-ol, butan-2-ol, ethanol, propan-1-ol, methanol. Give reason for your answer.
Methanol < ethanol < propan-1-ol < butan-2- ol < butan-1-ol < pentan-1-ol.
Answer:
Boiling point increases regularly as the molecular mass increases due to the corresponding increase in their vander waals forces of attraction. The boiling point increases in the order.
methanol, ethanol, propan-1-ol, butan-1-ol and pentan-1-ol.
Among isomeric alcohol, 2° alcohols have lower boiling point than 1° alcohols due to corresponding decrease in the extent of hydrogen bonding because of steric hindrance. Thus the boiling point of butan-2-ol is lower than butan-1-ol.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 19.
Explain why propanol has higher boiling point than that of hydrocarbon butane?
Answer:
The molecuels of butane are held together by weak vander waals forces of attraction while these of propanol are held together by stronger hydrogen bonding.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 33
Therefore boiling point of propanol is higher than that of butane.

Question 20.
Write the mechanism for the reaction
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 34
Answer:
The reaction follows SN1 mechanism.
Step 1: Formation of protonated alcohol.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 35
Step 2: Protonated alcohols forms carbocation.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 36
Step 3: Elimination of a proton to form alkane.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 37

Question 21.
Give mechanism for the formation of prop-1 – ene from propan-1-ol.
Answer:
The reaction is
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 38
Mechanism:
Step 1: Formation of protonated alcohol.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 39
Step 2: Formation of carbocation.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 40
Step 3: Elimination of a proton.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 41

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 22.
State Saytzeff rule.
Answer:
During intramolecular dehydration, if there is a possibility to form a carbon-carbon double bond at different locations, the preferred location is the one that gives the more (highly) substituted alkene i.e., the stable alkene.

Question 23.
Name the reagents in the following reactions:
(i) oxidation of a primary alcohol to a carboxylic acid.
(ii) oxidation of a primary alcohol to an aldehyde.
(iii) benzyl alcohol to benzoic acid.
(iv) butan-2-one to butan-2-ol.
Answer:
(i) Acidified potassium dichromate or neutral or acidic or alkaline potassium permanganate (followed by hydrolysis with dilute H2SO4).
(ii) Pyridinium chloro chromate(PCC) in CH2Cl2 or pyridinium dichromate (PDC) in CH2Cl2.
(iii) Acidified or alkaline KMnO4 (followed by hydrolysis with dil H2SO4).
(iv) Ni/H2 or NaBH4 or LiAlH4.

Question 24.
What happen when,
(i) vapours of ethanol is passed over heated copper at 573 K.
(ii) vapours of propan-2-ol is passed over heated copper at 573 K.
(iii) vapours of 2-methyl propan-2-ol is passed over heated copper at 573 K. Give equation.
Answer:
(i) Ethanal is formed.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 42
(ii) Propanone is formed.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 43
(iii) 2-methyl prop-1-ene is formed.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 44

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 25.
What is nitroglycerine? How it is formed? Give equation.
Answer:
Glycerotrinitrate (1,2,3, trinitroxy propane) is nitroglycerine. It is formed by nitration of glycerine in the presence of conc. H2SO4.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 45

Question 26.
How is acrolein formed from glycerol?
Answer:
When glycerol is heated with dehydrating agents like conc. H2SO4, KHSO4, or P2O5 acrolein is formed.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 45

Question 27.
Mention the cause for the acidic nature of alcohols.
Answer:
The acidic character of alcohols is due to the electronegative oxygen atom which withdraws electrons of the O—H bond towards itself. As a result, the O—H bond becomes weak and hence a proton can be easily abstracted by a base, i.e., ionization of alcohol to yield alkoxide ion and H+ ions are facilitated.
ROH ⇌ RO + H+

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 28.
Mention the uses of (i) methanol, (ii) ethanol, (iii) ethylene glycol, (iv) glycerol.
Answer:
(i) Uses of methanol:
(a) Methanol is used as a solvent for paints, varnishes, shellac, gums, cement, etc.
(b) In the manufacture of dyes, drugs, perfumes, and formaldehyde.

(ii) Uses of ethanol:
(a) Ethanol is used as an important beverage.
(b) It is also used in the preparation of

  • Paints and varnishes.
  • Organic compounds like ether, chloroform, iodoform, etc.,
  • Dyes, transparent soaps.

(c) As a substitute for petrol under the name power alcohol used as fuel for airplane.
(d) It is used as a preservative for biological specimens.

(iii) Uses of ethylene glycol:
(a) Ethylene glycol is used as an antifreeze in an automobile radiators.
(b) Its dinitrate is used as an explosive with DNG.

(iv) Uses of glycerol:
(a) Glycerol is used as a sweetening agent in confectionery and beverages.
(b) It is used in the manufacture of cosmetics and transparent soaps.
(c) It is used in making printing inks and stamp pad ink and lubricant for watches and clocks.
(d) It is used in the manufacture of explosives like dynamite and cordite by mixing it with china clay.

Question 29.
Alcohols are easily protonated in comparison to phenols. Explain why.
Answer:
In phenols, the lone pair of electrons on the oxygen atom is delocalized over the benzene ring due to resonance and hence, not easily available for protonation. In contrast, in alcohols, the lone pair of electrons on the oxygen atom is localized due to the absence of resonance and hence are easily available for protonation.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 30.
Identify the major product obtained in the following reaction:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 47
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 48

Question 31.
Identify the product of the reaction:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 49
Answer:
In the presence of a weak nucleophile such as ethanol, neopentyl bromide ionizes to form first a 1° carbocation which rearranges to form a more stable 3° carbocation. This is then attacked by the weak nucleophile ethanol followed by a less proton to yield ethyl neopentyl ether.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 50

Question 32.
Show how 2-methyl propan-1-ol is prepared by the reaction of a suitable Grignard reagent.
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 51
This part that has been enclosed in the box comes from methanal while the remaining part comes from the Grignard reagent. Therefore the Grignard reagent should be isopropyl magnesium bromide. Thus,
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 52

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 33.
Write the structure of the products of the following reactions.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 53
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 54
(ii) NaBH4 (sodium bromohydride) is a reducing agent. It reduces aldehydes and ketones but not esters.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 55
(ii) NaBH4 reduces, -CHO group to CH2OH group. Thus,
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 56

Question 34.
What is esterification? Give an example.
Answer:
Formation of an ester TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 57 from an alcohol and an organic acid in the presence of a catalyst is known as esterification. In the reaction, the ‘OH’ of the carboxylic acid and ‘H’ of the alcoholic group are removed as water.
Eg:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 58

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 35.
Why are alcohols are weaker acids than water?
Answer:
In water, ‘O’ atom is attached to two ‘H’ atom, but in alcohols, ‘O’ atom is attached to one ‘H’ atom and one ‘R’ group (alkyl group). Since ‘R’ group has an electron-donating inductive effect (+I), it increases the electron density in the O—H bond compared to that O—H bond in water. In other words, —O—H bond in alcohols is stronger than the —O—H bond in water. As a result, proton removal from alcohol is more difficult than in water. Hence, alcohols are weaker acids than water.

Question 36.
The acidic nature of alcohols is in the order 1° alcohol > 2° alcohol > 3° alcohol. Explain.
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 59
Alkyl (R) groups are electron releasing (i.e., +I effect) the electron density in the O—H bond in tertiary alcohols is maximum followed by secondary alcohol, while in primary alcohols, it is minimum. This means that O—H bond in tertiary alcohol is the strongest and hence most difficult to break followed by O—H bond in the secondary alcohols, while the O—H bond in primary alcohols is the weakest and hence most easy to break. Thus the acidic strength is in the order.
Primary > Secondary > Tertiary

Question 37.
Arrange the following compounds in increasing order against each.
(i) CH3CH2OH, CF3CH2OH. CCl3CH2OH (acid strength)
(ii) 2-methyl-2-propanol, 1-butanol, 2-butanol (reactivity towards sodium)
Answer:
(i) Due to -I effect of halogens, the electron density in the O—H bond decreases. As a result, the O—H bond strength becomes weak and proton removal is easier compared to CH3CH2OH. Further, since fluorine has a stronger -I effect, than chlorine, CF3CH2COOH is a stronger acid than CCl3CH2COOH. Hence, CF3CH2OH is the strongest acid while CH2CH2OH is the weakest acid. Hence increasing order of acid strength is
CH3CH2OH < CCl3CH2OH < CF3CH2OH.
(ii) It is an acid-base reaction since alcohols are acidic and sodium is a strong base. As such, the reactivity of these alcohols towards sodium increases as the acidic character of alcohols increases. Since the acidic character increases in the order 3° < 2° < 1°. Therefore the reactivity towards alcohol increases in the same order.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 60

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 38.
How will you convert phenol to (i) benzene, (ii) aniline, (iii) phenylacetate, (iv) phenyl benzoate, (v) anisole?
Answer:
(i) Benzene: Phenol is converted to benzene on heating with zinc dust. In this reaction, the hydroxyl group which is attached to the aromatic ring is eliminated.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 61
(ii) Aniline: Phenol on heating with ammonia in presence of anhydrous ZnCl2 gives aniline.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 62
(iii) Phenyl acetate:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 63
(iv) Phenyl benzoate:

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 64
(v) Anisole:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 65

Question 39.
Identify A and B in the following:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 66
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 67
(ii) A= HNO2 (273 -278) K
B = H2O
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 68
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 69

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 40.
What is picric acid? How it is prepared? 2,4,6 trinitrophenol is called picric acid.
Answer:
Nitration with cone. HNO3 and conc.H2SO4 gives picric acid.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 70

Question 41.
Give equation for the following:
(i) nitration of phenol,
(ii) sulphonation of phenol,
(iii) nitrosation of phenol.
Answer:
(i) Nitration of phenol: Phenol can be nitrated using 20% nitric acid even at room temperature, a mixture of ortho and para nitro phenols are formed.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 71
(ii) Sulphonation of phenol: Phenol reacts with cone. H2SO4 at 280 K to form o-phenol sulphonic acid as the major product. When the reaction is carried out at 373 K the major product is p-phenol sulphonic acid.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 72
(iii) Nitrosation of phenol: phenol can be readily nitrosated at low temperature with HNO2.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 73

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 42.
What happens when phenol is treated with
(i) acidified potassium dichromate,
(ii) hydrogen in the presence of nickel as a catalyst,
(iii) bromine water,
(iv) bromine in the presence of CCl4.
Answer:
Phenol treated with
(i) acidified potassium dichromate (oxidation):
Phenol undergoes oxidation with air or acidified K2CrO7 with conc. H2SO4 to form 1, 4-benzoquinone.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 74
(ii) hydrogen in the presence of nickel as catalyst (reduction): Phenol on catalytic hydrogenation gives cyclohexanol.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 75
(iii) bromine water (halogenation): phenol reacts with bromine water to give a white precipitate of 2,4,6-tribromo phenol.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 76
(iv) bromine in the presence of CCl4: If the reaction is carried out in CS2 or CCl4 at 278 K, a mixture of ortho and para bromo phenols are formed.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 77

Question 43.
Explain why the phenolic group is ortho para directing.
Answer:
The lone pair of electrons on the oxygen atom of the phenolic group enter into conjugation with the benzene ring due +M effect of the phenolic group. As a result, the ortho and para position become electron-rich compounds to the meta position. Hence the electrophilic attack the ortho and para position.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 78

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 44.
Write a short note on Reimer-Tiemann reaction.
Answer:
On treating phenol with CHCl3 / NaOH, a -CHO group is introduced at the ortho position.
This reaction proceeds through the formation of substituted benzal chloride intermediate.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 79

Question 45.
How will you distinguish between alcohol and phenol?
Answer:

  1. Phenol reacts with benzene diazonium chloride to form a red-orange dye, but ethanol has no reaction with it.
  2. Phenol gives purple coloration with neutral ferric chloride solution, alcohols do not give such coloration with FeCl3.
  3. Phenol reacts with NaOH to give sodium phenoxide. Ethyl alcohol does not react with NaOH.

Question 46.
Mention the uses of phenol.
Answer:

  1. About half of the world production of phenol is used for making phenol-formaldehyde resin. (Bakelite).
  2. Phenol is a starting material for the preparation of
    (a) drugs such as phenacetin, salol, aspirin, etc.
    (b) phenolphthalein indicator.
    (c) explosive like picric acid.
  3. It is used as an antiseptic-carbolic lotion and carbolic soaps.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 47.
Give the IUPAC names of the following ethers.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 80
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 81
Answer:
(i) 1-ethoxy-2-methyl propane
(ii) 2-chloro-l-methoxy ethane
(iii) 4-nitroanisole
(iv) 1-methoxy propane
(v) 4-ethoxy-1, 1, dimethyl cyclohexane
(vi) ethoxy benzene

Question 48.
Ethers are soluble in water. Give reason.
Answer:
The oxygen of ether can also form hydrogen bonds with water and hence they are miscible with water. Ethers dissolve a wide range of polar and non-polar substances.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 82

Question 49.
Write the names of reagents and equations for the preparation of the following ethers by Williamson’s synthesis.
(i) 1 -propoxypropane
(ii) Ethoxy benzene
(iii) 2-methyl-2-methoxy propane
(iv) 1-methoxyethane
Answer:
(i)
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 83
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 84
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 85

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 50.
Give the mechanism for the conversion of (i) ethanol to ethoxyethane, (ii) dehydration of 1-propanol to 1-proproxy propane.
Answer:
(i)
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 86
[Acid catalyzed 1° alcohol to ethers occurs via SN2 reaction, involving a nucleophilic attack by the alcohol molecule on the protonated alcohol molecule.]
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 87

Question 51.
Explain why the boiling point of ethers is slightly higher than that of alkanes and lower than that of alcohols of comparable molecular mass.
Answer:
Due to weak dipole-dipole interactions, the boiling point of ethers is only slightly higher than those of u-alkanes having comparable molecular masses.
The boiling points of ethers are less than that of alcohols is that ethers do not form hydrogen bonds.

Question 52.
Mention the uses of (i) Diethyl ether and (ii) Anisole.
Answer:
Uses of Diethyl ether:

  1. Diethyl ether is used as a surgical anesthetic agent in surgery.
  2. It is a good solvent for organic reactions and extraction.
  3. It is used as a volatile starting fluid for diesel and gasoline engines.
  4. It is used as a refrigerant.

Uses of anisole:

  1. Anisole is a precursor to the synthesis of perfumes and insecticide pheromones
  2. It is used as a pharmaceutical agent.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 53.
Discuss the mechanism of the reaction
CH3OCH2CH3 + HI → CH3I + CH3CH2OH.
Answer:
This reaction is an SN2 reaction. The cleavage of ethers by halogen acids occurs by the following mechanism.
Step 1: Ethers being Lewis acids, undergo protonation to form oxonium ions.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 88
This reaction takes place with HBr or HI because they are sufficiently acidic.
Step 2: Iodide ion is a good nucleophile. Due to steric hindrance, it attacks the smaller alkyl group of oxonium ion formed in step 1 and displaces the alcohol molecule by SN2 mechanism as shown below:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 89
Step 3: when excess HI is used, ethanol formed reacts with another molecule of HI to form ethyl iodide.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 90

Question 54.
Explain why ‘OCH3’ in the anisole group is ortho-para directing.
Answer:
The lone pair of electrons on the oxygen atom of the alkoxy group enters into the conjugation with the benzene ring due to its +M effect.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 91
As a result, the ortho and para position become rich in electron density compared to the meta position. Hence, the electrophile attacks ortho and para position.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

Question 55.
Briefly account of dipolar nature of C—O bonds in ethers.
Answer:
Because of the greater electronegativity of oxygen and carbon, the C—O bond is slightly polar thus have a dipole moment. Since the two C—O bonds in ethers are inclined to each other at an angle of 110°, the two dipoles do not cancel each other. As a result, ethers have a dipole moment of 1.15 to 1.3D
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 92

Question 56.
Give the equation for the reaction between diethyl ether with an excess of oxygen.
Answer:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 93

Question 57.
Give examples for (i) phthalein fusion and (ii) coupling reaction.
Answer:
(i) Phthalein fusion: On heating phenol with phthalic anhydride in presence of conc. H2SO4, phenolphthalein is obtained.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 94
(ii) Coupling reaction: Phenol couples with benzene diazonium chloride in an alkaline solution to form p-hydroxy azobenzene (a red-orange dye).
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 95

Choose the correct answer:

1. The IUPAC name of the compound is:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 96
(a) 2-chloro-5- hydroxyhexane
(b) 2-hydroxy-5-chlorohexane
(c) 5-chlorohexan-2-ol
(d) 2-chlorohexan-5-ol
Answer:
(c)

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

2. The IUPAC name of the compound is:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 97
(a) 1-methoxy-1-methyl ethane
(b) 2-methoxy-2-methyl ethane
(c) 2-methoxypropane
(d) isopropyl-methyl ether
Answer:
(c)

3. Arrange the following compounds in increasing order of boiling point:
I – propan-1-ol
II – butan-1-ol
III – butan-2-ol
IV – pentan-1-ol
(a) I, III, II, IV
(b) I, II, III, IV
(c) IV, III, II, I
(d) IV, II, III, I
Answer:
(a)
Hint: The boiling point increases as the molecular mass increases. Further among isomeric alcohols 1° alcohols have higher boiling points than 2° alcohols.

4. Acid catalysed hydration of alkenes except ethene, leads to the formation of:
(a) primary alcohol.
(b) secondary or tertiary alcohol.
(c) a mixture of primary and secondary alcohol.
(d) a mixture of secondary and tertiary alcohol.
Answer:
(b)
Hint: Hydration of ethene gives a 1° alcohol while all others give a either a 2° alcohol or 3° alcohol.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 98

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

5. Which of the following Grignard reagent is suitable for the preparation of 3-methyl-2- butanol?
(a) 2-butanone + methyl magnesium bromide
(b) Acetone + ethyl magnesium bromide
(c) Acetaldehyde + isopropyl magnesium bromide
(d) Ethyl propionate + methyl magnesium bromide
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 99

6. Which of the following esters shown, after reduction with LiAlH4 and aqueous workup, will yield two molecules of only a single alcohol?
(a) C6H5COOC6H5
(b) CH3CH2COOCH2CH3
(c) CH3COOCH3
(d) C6H5COOCH2C6H5
Answer:
(d)
Hint: Acyl and arylalkyl groups contain the same number of carbon atoms.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 100

7. Which of the following will exhibit highest boiling point?
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 101
Answer:
(b)
Hint: Among isomeric alcohols, the alcohol with no branching has the highest boiling point.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

8. Consider the reactions:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 102
The mechanisms of reactions (i) and (ii) are respectively:
(a) SN1 and SN2
(b) SN1 and SN1
(c) SN2 and SN2
(d) SN2 and SN1
Answer:
(c)

9.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 103
which of the following compounds will be formed?
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 104
Answer:
(a)
Hint: Nucleophilic attack occurs on the smaller alkyl group.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 105

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

10. The reaction of TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 106with RMgX leads to the formation of:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 107
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 108

11.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 109
X is:
(a) bromine in benzene
(b) bromine in water
(c) potassium bromide solution
(d) bromine in CCl4 at 0° C
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 110

12. Phenol can be distinguished from ethanol by the following reagent except.
(a) sodium
(b) I2 / NaOH
(c) neutral FeCl3
(d) Br2 / H2O
Answer:
(a)
Hint: Na reacts with both ethapol and phenol.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

13. An ether is more volatile than an alcohol having the same molecular formula. This is due to:
(a) intermolecular hydrogen bonding in alcohols
(b) dipolar character of ethers
(c) alcohols having resonance structures
(d) intermolecular hydrogen bonding in ethers
Answer:
(a)

14. Mark the correct increasing order of reactivity of the following compounds with HBr / HI.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 111
(a) I < II < III
(b) II < I < III
(c) II < III < I
(d) III < II < I
Answer:
(c)
Hint: All the three benzyl alcohols react with HBr or HI through the formation of intermediate carbocation. Obviously more stable the carbocation, more reactive is the alcohol. Now, electron withdrawing group i.e, NO2, Cl, etc., decrease the stability of carbocations. Since, NO2 is a stronger, electron withdrawing group, then Cl, stability of carbocation increases in the order.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 112
Therefore, the reactivity of the benzyl alcohols increases in the same orders, i.e., II < III < I.

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

15. Which of the following reagents can be used to oxidize primary alcohols to aldehydes?
1. CrO3 in acidic medium,
2. KMnO4 in acidic medium,
3. Pyridinium chlorochromate,
4. Heat in the presence of Cu at 573 K.
(a) 1, 3, 4
(b) 1, 3
(c) 1, 4
(d) none of the above
Answer:
(a)
Hint: KMnO4 will oxidise the aldehyde formed to carboxylic acid.

16. Assertion: Bond angles in ethers is slightly more than the tetrahedral angle.
Reason: There are repulsions between two bulky ‘R’ groups.
(a) Assertion and reason both are correct, and reason is the correct explanation of assertion.
(b) Assertion and reason both are correct, but reason is not the correct explanation of assertion.
(c) Assertion is wrong, but reason is correct.
(d) Both assertion and reason are wrong.
Answer:
(c)
Hint: Correct assertion: Bond angles in ethers are slightly more than the tetrahedral bond angle.

17. Assertion: Bromination of benzene does not require Lewis acid is catalyst.
Reason: Lewis acid polarises the bromine molecule in Friedel craft’s reaction.
(a) Assertion and reason both are correct, and reason is the correct explanation of assertion.
(b) Assertion and reason both are correct, but reason is not the correct explanation of assertion.
(c) Assertion is true, but reason is wrong.
(d) Both assertion and reason are wrong.
Answer:
(b)

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

18. Match the entries in column I with appropriate entries in column II and choose the correct option using the codes given:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 113
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 114
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 115
Answer:
(b)

19. Match the entries in column I with appropriate entries in column II and choose the correct option using the codes given:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 116
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 117
Answer:
(d)

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

20. In the following sequence of reactions,
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 118
(a) CH3CH2CH2OH
(b) CH3CH(OH)CH3
(c) CH3CH2CH2CH2OH
(d) (CH3)3CCH2OH
Answer:
(b)
Hint: Since alkenes give Markovnikoff addition products, therefore 1° alcohols (a), (c) and (d) cannot be obtained by hydration. Thus, ‘Z’ is 2-propanol.
i.e.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 119

21. Consider the following reaction:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 120
The compound ‘Z’ is:
(a) CH3CH2OCH2CH3
(b) CH3CH2OSO3H
(c) CH3CH2OH
(d) CH2=CH2
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 121

22. Formation of tert-butyl ether by reaction of sodium tert-butoxide and methyl bromide involves:
(a) elimination reaction
(b) electrophilic addition reaction
(c) nucleophilic addition reaction
(d) nucleophilic substitution reaction
Answer:
(d)

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

23.
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 122
Answer:
(a)

24. The red coloured compound formed during Victor-Meyer’s test is:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 123
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers 124

TN Board 12th Chemistry Important Questions Chapter 11 Hydroxy Compounds and Ethers

25. Following compounds are given:
(i) CH3CH2OH
(ii) CH3COCH3
(iii) CH3CH(OH)CH3
(iv) CH3OH
Which of the above compounds on being warmed with iodine solution andNaOH, will give iodoform?
(a) (i), (iii) and (iv)
(b) only (i)
(c) (i), (ii) and (iii)
(d) (i) and (ii)
Answer:
(c)
Hint: Compounds containing CH3CO group or CH3CH(OH) group on warming with I2 and NaOH will form iodoform. Hence, (i), (ii) and (iii) will give iodoform.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Students get through the TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Answer the following questions.

Question 1.
Give three examples of adsorption.
Answer:

  1. Charcoal adsorbs ammonia.
  2. Silica gel adsorbs water.
  3. Charcoal adsorbs colorants from sugar.

Question 2.
Distinguish between adsorption and absorption.
Answer:
Adsorption is a surface phenomenon while absorption is a bulk phenomenon, i.e., the adsorbate molecules are distributed throughout the adsorbent.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 3.
What are adsorbent and adsorbates? Give examples.
Answer:
Adsorbent is the material on which adsorption take place. Adsorbed substance is called adsorbate.
Examples for adsorbates: The gaseous molecules like He, Ne, O2, N2, SO2 and NH3 and solutions of NaCl or KCl.
Examples for adsorbents: Silica gel, metals like Ni, Cu, Pt, Ag and Pd and certain colloids.

Question 4.
What is an interface?
Answer:
The surface of separation of two phases where the concentration of adsorbed molecules is high is known as interface.

Question 5.
Mention the characteristics of adsorption.
Answer:

  1. Adsorption can occur in all interfacial surfaces i.e., the adsorption can occur in between gas-solid, liquid solid, liquid- liquid, solid- solid and gas-liquid.
  2. Adsorption is always accompanied by decrease in free energy. When ΔG reaches zero, the equilibrium is attained.
  3. Adsorption is a spontaneous process.
  4. When molecules are adsorbed, there is always a decrease in randomness of the molecules.
    We know, ΔG = ΔH – T ΔS where ΔG is change in free energy.
    ΔH is change in enthalpy and ΔS is change in entropy.
    Hence, ΔH = ΔG + TΔS Adsorption is exothermic as there is an interaction between adsorbate and adsorbent.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 6.
What do you understand by the term ‘sorption’?
Answer:
The term represents simultaneous adsorption and absorption.

Question 7.
What is the term used for sorption of gases on metal surfaces?
Answer:
Occlusion.

Question 8.
Give three examples for chemical adsorption or chemisorption.
Answer:

  1. Adsorption of O2 on tungsten.
  2. Adsorption of H2 on nickel.
  3. Adsorption of ethyl alcohol vapours on nickel.

Question 9.
Give two examples for physical adsorption.
Answer:

  1. Adsorption of N2 on mica.
  2. Adsorption of gases on charcol.

Question 10.
Explain the nature of the force of attraction that exists between an adsorbent and an adsorbate in (i) physical adsorption and (ii) chemical adsorption.
Answer:
The forces of attraction that exists between adsorbate and adsorbent in
(i) Physical adsorption are (a) vander waals force of attraction, (b) dipole-dipole interaction and (c) dispersion forces.
(ii) In chemisorption gas molecules are held to the surface by formation of chemical bonds. Since strong bonds are formed, nearly 400 kJ mole is given out as heat of adsorption.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 11.
Why is adsorption exothermic?
Answer:
When adsorption occurs, entropy decreases, i.e., ΔS = negative. As ΔG = ΔH – TΔS, for a spontaneous process, AG must be negative. This can only be so, if ΔH is negative, i.e., the process is exothermic.

Question 12.
How do size of particles of adsorbent, pressure of gas and prevailing temperature influence the extent of adsorption of a gas on a solid?
Answer:

  1. The smaller the size of the particles of the adsorbent, greater is the surface area, greater is the adsorption.
  2. At constant temperature, adsorption first increases with increase in pressure and then attains equilibrium at high pressures.
  3. In physical adsorption, it decreases with increase in temperatures, but in chemisorption first, it increases and then decreases.

Question 13.
What are adsorption isotherms and isobars? Explain.
Answer:
A plot between the amount of adsorbate adsorbed and pressure or concentration of adsorbate at constant temperature is called adsoiption isotherm.
The plot of the amount of adsorption verses temperature at constant pressure is called adsorption isobar. The adsorption isobars of physisorption and chemisorption as shown in figure.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 1
In physical adsorption, \(\frac{x}{m}\) decreases with increases in T, But in chemical adsorption, \(\frac{x}{m}\) increases with rise in temperature and then decreases. The increase illustrates the requirement of activation of the surface for adsorption is due to fact that the formation of activated complex requires certain energy.
The decrease at high temperature is due to desorption, as the kinetic energy of the adsorbate increases.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 14.
Derive Freundlich adsorption isotherm.
Answer:
A plot between the amount of adsorbate adsorbed and the pressure or concentration of adsorbate at constant temperature is called adsorption isotherms.
In order to explain these isotherms, various equations were suggested as follows: Freundlich adsorption isotherm.
According to Freundlinch,
\(\frac{x}{m}\) = Kp\(\frac{1}{n}\)
where V is the amount of adsorbate or adsorbed on ‘m’ gm of adsorbent at a pressure of p. K and n are constants.
Value n is always less than unity.
This equation is applicable for adsoiption of gases on solid surfaces. The same equation becomes \(\frac{x}{m}\) = Kc\(\frac{1}{n}\) when used for adsorption in solutions with c as concentration.
This equation quantitively predict the effect of pressure (or concentration) on the adsorption of gases (or adsorbates) at a constant temperature.
Taking log on both sides of the equation
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 2
Hence the intercept represents the value of log K and the slope \(\frac{b}{q}\) gives \(\frac{1}{n}\).
This equation explains the increase of \(\frac{x}{m}\) with an increase in pressure. But experimental values show the deviation at low pressure.

Question 15.
Explain the application of adsorption (i) in the use of gas masks, (ii) in the use of softening hard water, (iii) in decolourisation of sugar.
Answer:
(i) Gas masks are devices containing suitable adsorbents so that poisonous gases present in the atmosphere are preferentially adsorbed and the air for breathing is purified.
Activated charcoal is one of the best adsorbents.
(ii) Permutit is employed for this process which adsorbs Ca2+ and Mg2+ ions in its surface, there is an ion exchange as shown below it occurs on the surface.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 3
Exhausted permutit is regenerated by adding a solution of common salt.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 4
(iii) Sugar prepared from molasses is decolourised to remove coloured impurities by adding animal charcoal which acts as decolourising material.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 16.
What are adsorption indicators?
Answer:
In the precipitation titrations, the endpoint is indicated by an external indicator that changes its colour after getting adsorbed on precipitate. It is used to indicate the endpoint of the titration.

Question 17.
Distinguish between homogeneous catalysis and heterogeneous catalysis with suitable examples.
Answer:
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 5

Question 18.
Name the catalysts used in the following:
(i) Haber’s process in the manufacture of ammonia.
(ii) Oxidation of ammonia.
(iii) Hydrogenation of alkenes.
(iv) Decomposition of H2O2.
(v) Formation of acetophenone from benzene and ethanoyl chloride. Also, give equations for the reactions.
Answer:
(i) The catalyst used is Iron,
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 6
(ii) The catalyst is platinum gauze.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 7
(iii) The catalyst is finely divided nickel.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 8
(iv) The catalyst is platinum
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 9
(v) The catalyst is anhydrous aluminium chloride
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 10

Question 19.
Mention the characteristics of catalysts.
Answer:

  1. For a chemical reaction, the catalyst is needed in very small quantities. Generally, a pinch of catalyst is enough for a reaction in bulk.
  2. There may be some physical changes, but the catalyst remains unchanged in mass and chemical composition in a chemical reaction.
  3. A catalyst itself can not initiate a reaction. It means it can not start a reaction that is not taking place. But, if the reaction is taking place at a slow rate it can increase its rate.
  4. A solid catalyst will be more effective if it is taken in a finely divided form.
  5. A catalyst can catalyse a particular type of reaction, hence they are said to be specific in nature.
  6. In an equilibrium reaction, the presence of catalyst reduces the time for attainment of equilibrium and here it does not affect the position of equilibrium and the value of the equilibrium constant.
  7. A catalyst is highly effective at a particular temperature called as optimum temperature.
  8. The presence of a catalyst generally does not change the nature of products
    eg: 2SO2 + O2 → 2SO3
    This reaction is slow in the absence of a catalyst, but fast in the presence if Pt catalyst.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 20.
What are promoters? Explain with an example.
Answer:
In a catalysed reaction the presence of a certain substance increases the activity of a catalyst. Such a substance is called a promoter. For example in the Haber’s process of manufacture ammonia, the activity of the iron catalyst is increased by the presence of molybdenum. Hence molybdenum is called a promoter. In the same way, Al2O3 can also be used as a promoter to increase the activity of the iron catalyst.

Question 21.
Explain the action of anhydrous aluminium chloride in Friedel-Crafts reaction.
Answer:
The mechanism of Friedel crafts reaction is given below
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 11
The action of catalyst is explained as follows:
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 12
It is an intermediate.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 13

Question 22.
Give the mechanism of the following reactions based on intermediate formation theory.
Answer:

  1. Thermal decomposition of KClO3 in the presence of MnO2.
    Steps in the reaction
    2KClO3 → 2KCl + 3O2
    can be given as
    2KClO3 + 6MnO2 → 6MnO3 + 2KCl
    It is an intermediate,
    6MnO3 → 6MnO2 + 3O2
  2. The reaction between H2 and O2 in the presence of copper.
    2Cu + \(\frac{1}{2}\) O2 → Cu2O It is an intermediate.
    Cu2O + H2 → H2O + 2Cu
  3. Oxidation of HCl by air in the presence of CuCl2.
    2CuCl2 → Cl2 + Cu2Cl2
    2Cu2Cl2 + O2 → 2Cu2OCl2
    It is an intermediate.
    2Cu2OCl2 + 4HCl → 2H2O + 4CuCl2
    This theory describes
    (a) the specificity of a catalyst and
    (b) the increase in the rate of the reaction with an increase in the concentration of a catalyst.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 23.
Mention the limitations of the intermediate compound formation theory of catalysis.
Answer:

  1. The intermediate compound theory fails to explain the action of catalytic poison and activators (promotors).
  2. This theory is unable to explain the mechanism of heterogeneous catalysed reactions.

Question 24.
Explain the salient features of the adsorption theory of catalysis.
Answer:
According to this theory, the reactants are adsorbed on the catalyst surface to form an activated complex which subsequently decomposes and gives the product.
The various steps involved in a heterogeneous catalysed reaction are given as follows:

  1. Reactant molecules diffuse from bulk to the catalyst surface.
  2. The reactant molecules are adsorbed on the surface of the catalyst.
  3. The adsorbed reactant molecules are activated and form an activated complex which is decomposed to form the products.
  4. The product molecules are desorbed.
  5. The product diffuses away from the surface of the catalyst.

Question 25.
What are active centres? How does the presence of active centres influence the rate of catalysed reaction?
Answer:
The surface of a catalyst is not smooth. It bears steps, cracks and comers. Hence the atoms on such locations of the surface are coordinatively unsaturated. So, they have much residual force of attraction. Such sites are called active centres. So, the surface carries high surface free energy.
The presence of such active centres increases the rate of reaction by adsorbing and activating the reactants.
The adsorption theory explains the following

  1. Increase in the activity of a catalyst by increasing the surface area. An increase in the surface area of metals and metal oxides by reducing the particle size increases the rate of the reaction.
  2. The action of catalytic poison occurs when the poison blocks the active centres of the catalyst.
  3. A promoter or activator increases the number of active centres on the surfaces.

Question 26.
What is the role of a promoter in heterogeneous catalysis?
Answer:
A promoter increases the number of active centres on the surfaces.

Question 27.
What are catalytic poisons? How do they affect a catalysed reaction?
Answer:
Substances that destroy the activity of catalysts are known as catalytic poisons. They affect the catalytic reaction by occupying the active centres of the catalyst as a result active centres will not available for adsorption by reactants.

Question 28.
Give some examples of enzyme catalyses. Some common examples for enzyme catalysis.
Answer:

  1. The peptide glycyl L-glutamyl L-lyrosin is hydrolysed by an enzyme called pepsin.
  2. The enzyme diastase hydrolyses starch into maltose.
    2(C6H10O5)n + nH2O → nC2H22O11
  3. The yeast contains the enzyme zymase which converts glucose into ethanol.
    C6H12O6 + H2O → 2C2H5OH + 2CO2
  4. The enzyme micoderma aceti oxidises alcohol into acetic acid.
    C2H5OH + O2 → CH3COOH + H2O
  5. The enzyme urease present in soya beens hydrolyses the urea.
    TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 14

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 29.
Briefly outline the characteristics of enzyme catalysed reaction.
Answer:

  1. An enzyme catalyst is specific in nature, i.e., one catalyst cannot catalyse more than one reaction.
  2. The enzyme catalysed reactions are very fast compared to other catalysed reactions.
  3. The rate of an enzyme-catalysed reaction depends on temperature. At an optimum temperature, the rate of the reaction becomes maximum. Beyond the optimum temperate, the rate decrease.
  4. The enzyme activity is maximum at a particular pH called optimum pH. The favourable pH range for enzymatic reactions is 5-7.
  5. The enzymatic activity is increased by the presence of containing substances, known as coenzymes.
  6. The activity of enzymes can also be inhibited or poisoned due to the presence of certain substances.

Question 30.
Explain phase transfer catalysis with an example.
Answer:
Substitution of Cl and CN in the following reaction.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 15
R-Cl = 1-chlorooctane
R-CN = 1-cyanooctane
By direct heating of two-phase mixture of organic 1 -chlorooctane with aqueous sodium cyanide for several days, 1-cyanooctane is not obtained. However, if a small amount of quaternary ammonium salt like tetraalkyl ammonium chloride is added, a rapid transition of 1 -cyanooctane occurs in about 100% yield after 1 or 2 hours. In this reaction, the tetraalkyl ammonium cation, which has hydrophobic and hydrophilic ends, transports CN from the aqueous phase to the organic phase using its hydrophilic end and facilitates the reaction with 1-chloroocatne as shown below:
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 16
So phase transfer catalyst speeds up the reaction by transporting one reactant from one phase to another.

Question 31.
Name the dispersed phase and dispersed medium in the following: fog, dust, sharing cream, milk, paints.
Answer:

ExampleDispersed phaseDispersion medium
FogLiquidGas
DustSolidGas
Sharing creamGasLiquid
MilkLiquidLiquid
PaintSolidLiquid

Question 32.
Give the name of the colloid and one example for (i) a gas dispersed in solid, (ii) a liquid dispersed in a solid, (iii) a solid dispersed in a solid.
Answer:
(i) A gas dispersed in a solid is known as a solid foam. Pumice stone, rubber, bread are examples.
(ii) A liquid dispersed in a solid is known as a gel. Butter and cheese are examples.
(iii) A solid dispersed in another solid is known as a solid sol. Pearls, coloured glass, alloys are examples of solid sols.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 33.
Briefly outline the principle involved in the preparation of colloidal solution by dispersion methods.
Answer:
In the dispersion method, the particles whose size is higher than that of colloidal particles are disintegrated to that of the colloidal particles subjecting it to a mechanical disintegration in a colloid mill or by electro-dispersion.

Question 34.
Explain how colloidal particles of metals are prepared by electro dispersion method.
Answer:
An electrical arc is struck between electrodes dispersed in the water surrounded by ice. When a current of 1 amp /100V is passed an arc produced forms vapours of metal which immediately condense to form a colloidal solution. By this method colloidal solution of many metals like copper, silver, gold, platinum, etc. can be prepared Alkali hydroxide is added as a stabilising agent for the colloidal solution.

Question 35.
Explain peptisation with an example.
Answer:
The conversion of a freshly precipitated substance into a colloid by the addition of an electrolyte (peptising agent) is known as peptisation. For example, freshly precipitated silver chloride is converted into a colloidal solution by the addition of HCl.

Question 36.
Explain the principle involved in the preparation of colloids by the condensation method.
Answer:
Particles whose size are lesser than the colloidal particles are brought together to the size of colloidal particles.

Question 37.
What is the principle involved in the purification of a colloidal solution by dialysis?
Answer:
The separation of crystalloids (electrolytes) from colloids is based upon the principle that particles of crystalloid pass through the animal membrane (bladder) or parchment paper, or cellophane sheet whereas those of colloid do not.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 38.
Explain why? (i) colloidal particles are not visible to the naked eye, (ii) colloidal particles pass through ordinary filter paper, (iii) the sky appears blue, (iv) finest gold sol is red in colour.
Answer:
(i) No particle is visible to the naked eye if its diameter is less than half the wavelength of light used. The shortest wavelength of light is about 4000Å or 400 mμ. Hence no particle of diameter less than 200 mμ can be seen. The size of the colloidal particles is less than 200 mμ.
(ii) The size of the colloidal particles are smaller than the pores in the filter paper and hence, they pass through the filter paper.
(iii) This is due to the Tyndall effect. The colloidal particles absorb light energy and then scatter in all directions.
(iv) The colour of the colloidal solution depends as the wavelength of scattered radiation by dispersed particles. The wavelength of light further depends on the size and nature of particles. The finest gold sol is red in colour. As the size of particles increase, it becomes purple, then blue and finally golden yellow.

Question 39.
Explain the Tyndall effect.
Answer:
Colloids have optical properties. When a homogeneous solution is seen in the direction of light, it appears clear but it appears dark, in a perpendicular direction.
But when light passes through a colloidal solution, it is scattered in all directions. The colloidal particles absorb a portion of light and the remaining portion is scattered from the surface of the colloid. Hence the path of light is made clear. This phenomenon is known as the Tyndall effect.

Question 40.
Give an account of the Brownian movement.
Answer:
The zig-zag random motion of colloidal particles, when viewed through ultramicroscope, is known as Brownian movement. The reason for Brownian movement is that the colloidal sol particles are continuously bombarded with the molecules of the dispersion medium and hence they follow a zigzag, random, continuous movement.
Brownian movement enables us,
I. to calculate Avogadro number.
II. to confirm kinetic theory which considers the ceaseless rapid movement of molecules that increases with an increase in temperature.
III. to understand the stability of colloids: As the particles are in continuous rapid movement they do not come close and hence not get condensed. That is Brownian movement does not allow the particles to be acted on by force of gravity.

Question 41.
Explain the term electrophorosis.
Answer:
The movement of colloidal particles towards cathode or anode depending on the charge of the particles under the influence of electric current is known as electrophorosis.
This experiment is used to detect the charge on the colloidal particles. If the colloidal particles move towards the cathode, it is negatively charged. If they are positively charged, they migrate towards anode.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 42.
Give examples for positively charged and negatively charged colloids.
Answer:

Positively charge colloidsNegatively charge colloids
Ferric hydroxideAg, Au & Pt
Aluminium hydroxideArsenic sulphide
Basic dyesClay
HaemoglobinStarch

Question 43.
Account for the charge on colloidal particles.
Answer:
The colloidal particles, in whichever method is prepared, contain traces of electrolytes. It preferentially adsorbs either positive or negative ions from the solution. If the particles adsorb positive ions from the solution, it becomes a positively charged colloid. If it adsorbs a negative ion from the solution, it becomes a negatively charged colloid.

Question 44.
Account for the stability of a colloid.
Answer:
Since the colloidal particles are either positive or negatively charged, they do not come close together. They repel each other. Thus, the charge on the colloidal particles is responsible for its stability.

Question 45.
Explain the term coagulation or flocculation.
Answer:
The conversion of a colloid to a precipitate is known as coagulation or precipitation. Coagulation results in the removal of charges on the colloid by any one of the following:

  1. Addition of electrolytes
  2. electrophoresis
  3. mixing oppositely charged sols
  4. boiling.

These methods help remove charges from the particles. Thus, the particles come closer, form an aggregate of particles and finally settles down as a precipitate due to gravity.

Question 46.
The peptising agent is added to convert a precipitate into a colloidal solution. Give reason.
Answer:
Ions (either positive or negative) of the peptising agent (electrolyte) are adsorbed on the particles of the precipitate. They repel and hit each other breaking the particles of the precipitate into colloidal size.

Question 47.
Explain what is observed (i) when a beam of light is passed through a colloidal solution.
(ii) an electrolyte, NaCl is added to ferric hydroxide solution,
(iii) electric current is passed through a colloidal solution.
Answer:
(i) Scattering of light by colloidal particles take place and the path of light becomes visible.
(ii) The positively charged colloidal particles of Fe(OH)3 gets coagulated by the oppositely charged Cl ions provided by NaCl.
(iii) On passing electric current, colloidal particles move towards the oppositely charged electrode where they lose their charge Cl get coagulated.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 48.
What happens when gelatin is mixed with gold sol?
Answer:
Gold sol is lyophobic. Gelatin forms lyophilic sol and acts as a protective colloid. On adding gelatin to gold sol, the latter becomes more stable.

Question 49.
A colloid is formed by adding FeCl3 in excess of hot water. What will happen if an excess ferric chloride is added to this colloid?
Answer:
On adding FeCl3 to water, a colloidal sol of hydrated ferric oxide is formed. This is a positively charged colloid as it adsorbs Fe+3 ions on its surface. On adding NaCl, Cl ions bring about coagulation.

Question 50.
How does the boiling of a colloid, help the coagulation of a colloidal solution?
Answer:
Boiling vessels in increased collisions between the colloidal particles. The sol particles combine and settle down as a precipitate.

Question 51.
Explain the protective action of lyophilic colloids.
Answer:
The addition of a lyophobic colloid into lyophilic colloid protects the latter from coagulation. Hence, lyophilic colloids act as protective colloids.

Question 52.
Define gold number. Mention its use.
Answer:
‘Gold number’ as a measure of protecting the power of a colloid. The gold number is defined as the number of milligrams of hydrophilic colloid that will just prevent the precipitation of 10ml of gold sol on the addition of 1ml of 10% NaCl solution. Smaller the gold number greater the protective power.

Question 53.
What are emulsions? Mention various types of emulsions.
Answer:
Emulsions are a colloidal solutions in which a liquid is dispersed in another liquid.
Generally, there are two types of emulsions.

  1. Oil in Water (O/W)
  2. Water in Oil (W/O)

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

Question 54.
Give one example each for (i) oil in water and (ii) water in oil emulsions.
Answer:
(i) In Oil in Water (O/W) emulsions, the dispersed phase is oil and the dispersion medium is water.
eg: Milk is an emulsion of liquid fat dispersed in water and vanishing cream.
(ii) Emulsion of Water in Oil (W/O) in which water is the dispersed phase and oil is the dispersion medium.
eg: Cod liver oil, butter and cold cream.

Question 55.
What is emulsification?
Answer:
The process of preparation of emulsion by the dispersal of one liquid in another liquid is called Emulsification.

Question 56.
What is an emulsifier or emulsification agent?
Answer:
It is a substance added to have a stable emulsion. The type of emulsion formed depends upon the nature of the emulsifying agent. For example, the presence of soluble soaps as an emulsifying agent favours the formation of oil in water type of emulsions, whereas insoluble soaps (containing non alkali metal atoms) favours the formation of water in oil emulsions.

Question 57.
Mention the properties of the emulsion.
Answer:

  1. Emulsions exhibit all the properties like the Tyndall effect, Brownian movement, Electrophoresis, Coagulation on the addition of electrolytes.
  2. Emulsions can be separated into their constituent liquids by boiling, freezing, centrifuging, electrostatic precipitation by adding large amounts of the electrolytes to precipitate out the dispersed phase or by chemical destruction of emulsifying agent.
  3. Emulsions can be diluted by adding any amount of dispersion medium.

Choose the correct answer:

1. Which of the following is true with respect of adsorption?
(a) ΔG < 0, ΔS > 0, ΔH < 0
(b) ΔG < 0, ΔS < 0, ΔH < 0
(c) ΔG > 0, ΔS > 0, ΔH < 0
(d) ΔG < 0, ΔS < 0, ΔH > 0
Answer:
(b)

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

2. Which of the following statements is incorrect regarding physisorption?
(a) It occurs because of vander Waals forces.
(b) More easily liquefiable gases are adsorbed readily.
(c) Under high pressure, it results in multimolecular layer on the adsorbent surface.
(d) Enthalpy of adsorption in low and positive.
Answer:
(d)
Hint: Enthalpy of adsorption is always negative.

3. Physical adsorption of a gaseous species may change to chemical adsorption with
(a) decrease in temperature
(b) increase in temperature
(c) increase in surface area of the adsorbent
(d) decrease in surface area of the adsorbent
Answer:
(b)
Hint: At high temperatures, gaseous species may dissociate into atoms that are chemisorbed, eg: N2 an iron surface at ≥ 773 K.

4. In physisorption, adsorbent does not show specificity for any particular gas because:
(a) involved van der Waals forces are universal
(b) gases involved behave like ideal gases
(c) enthalpy of adsorption is low
(d) it is a reversible gas
Answer:
(a)

5. Which of the following is an example of adsorption?
(a) water on silica gel
(b) water on calcium carbide
(c) hydrogen on finely divided nickel
(d) oxygen on the metal surface
Answer:
(c)

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

6. On the basis of data given below predict which of the following gases show least adsorption on a definite amount of charcoal
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 17
(a) CO2
(b) SO2
(c) CH4
(d) H2
Answer:
(d)
Hint: Higher the critical temperature, the greater is the adsorption. H2 has the least critical temperature and hence least adsorbed.

7. Which of the following are the characteristics of chemisorption?
(i) High heat of adsorption
(ii) Irreversibility
(iii) Low activation energy
(a) (i) and (ii) only
(b) (i) and (iii) only
(c) (ii) and (iii) only
(d) (i), (ii) and (iii)
Answer:
(a)

8. The plot of \(\frac{x}{m}\) (along Y-axis) versus log C (along X-axis) in the Freundlich adsorption isotherm is a horizontal line parallel to X-axis when,
(a) n = 0
(b) n = 1
(c) n = ∞
(d) such a plot is impossible
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 18
i.e., constant parallel to log C axis.
[Note: This is the equation for adsorption of solids in solution.]

9. Match the following:

AFog1Gel
BMilk2Foam
CCheese3Emulsion
DSoap lather4Aerosol

Which of the following is the correct option?
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 19
Answer:
(b)

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

10. Which of the following will show the Tyndall effect?
(a) Aqueous solution of soap below critical miscelle concentration.
(b) Aqueous solution of soap above critical miscelle concentration.
(c) Aqueous solution of sodium chloride
(d) Aqueous solution of sugar
Answer:
(b)

11. Method by which lyophobic sol can be protected:
(a) addition of oppositely charged sol
(b) addition of an electrolyte
(c) addition of lyophilic sol
(d) by boiling
Answer:
(c)

12. Freshly prepared precipitate sometimes gets converted to colloidal solution by:
(a) coagulation
(b) electrolysis
(c) diffusion
(d) peptisation
Answer:
(d)

13. Which of the following electrolytes will have maximum coagulating value for AgI / Ag+ Sol?
(a) Na2S
(b) Na3PO4
(c) Na2SO4
(d) NaCl
Answer:
(b)
Hint: AgI / Ag+ is a positively charged sol. Electrolytes whose negative ion (anion) has the least negative charge will require the maximum amount and will have the maximum coagulating value. Hence, Cl in NaCl.

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

14. A colloidal system having a solid substance as a dispersed phase and liquid as dispersion medium is classified as:
(a) solid sol
(b) gel
(c) emulsion
(d) sol
Answer:
(d)

15. Which of the following process is responsible for the formation of the delta at places where the river meets the sea?
(a) Emulsification
(b) Colloid formation
(c) Coagulation
(d) Peptisation
Answer:
(c)
Hint: Formation of the delta-shaped heap of sand clay etc where the river falls into the sea due to coagulation of sand/clay by NaCl present in seawater.

16. When an excess of a very dilute aqueous solution of KI is added to a very dilute aqueous solution of silver nitrate, the colloidal particles of silver iodide are associated with which of the following Helmholtz double layer?
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 20
Answer:
(d)
Hint:
As excess KI has been added, I ions are adsorbed on AgI forming a fixed layer (giving negative charge). It then attracts the counter ion (K+) from the medium forming a second layer, (diffused layer).

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

17. The ratio of a number of moles of AgNO3, Pb(NO3)2 and Fe(NO3)3 required for coagulation of a definite amount of colloidal sol of silver iodide prepared by mixing AgNO3 with an excess of KI will be:
(a) 1:2:3
(b) 3:2:1
(c) 6:3:2
(d) 2:3:6
Answer:
(c)
Hint:
With excess KI, colloidal particles will be [AgI]I.
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 21
Molar ratio required for coagulation of same amount of [AgI]I is 1 : \(\frac{1}{2}\) : \(\frac{1}{3}\) = 6 : 3 : 2.

18. Gelatin is mostly used in making ice creams in order to:
(a) prevent the formation of colloidal sol.
(b) enrich fragrance.
(c) prevent crystallisation and stabilise the mix.
(d) modify the taste.
Answer:
(c)
Hint: Gelatin is a protective colloid. It stabilises the mix and prevents crystallisation.

19. Which of the following has a minimum gold number?
(a) Starch
(b) Sodium oleate
(c) Gum arabic
(d) Gelatin
Answer:
(d)

TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry

20. Match the following:
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 22
Which of the following is the correct option?
TN Board 12th Chemistry Important Questions Chapter 10 Surface Chemistry 23
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Students get through the TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Answer the following questions.

Question 1.
Define the following terms:
(i) Resistivity,
(ii) conductivity,
(iii) cell constant,
(iv) specific conductance,
(iv) molar conductivity,
(vi) equivalent conductance.
Answer:
(i) Resistivity is defined as the resistance of an electrolyte confined between two electrodes having unit cross-sectional area and are separated by unit distance.
(ii) The reciprocal of specific resistance \(\left(\frac{1}{\rho}\right)\) is called specific conductance or conductivity.
(iii) The ratio between the distance between the two electrodes in a conductivity cell to their area of cross-section is called cell constant.
(iv) The specific conductance is defined as the conductance of a cube of an electrolytic solution of unit dimension.
(v) Molar conductance is defined by the conducting power of all the ions produced by 1 mole of the electrolyte.
(vi) Equivalent conductance is defined as the conductance of ‘V’ m3 of the electrolyte solution containing one gram equivalent of electrolyte in a conductivity cell in which the electrodes are 1 meter apart.

Question 2.
Give the relationship between resistance and specific resistance of an electrolytic conductor.
Answer:
R = ρ × \(\frac{l}{a}\)
where ‘R’ is the resistance, ρ is the specific resistance or resistivity, ‘l’ is the distance between the electrodes in a conductivity cell, and ‘a’ is the area of cross-section of electrodes.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 3.
Mention the units of (i) resistance, (ii) specific resistance, (iii) conductance, (iv) specific conductance, (v) molar conductance and (vi) equivalent conductance.
Answer:

PropertyUnit
Resistanceohm
Specific resistanceohm metre (Dm)
ConductanceSiemens (s)
Specific conductanceohm-1m-1 or mhom-1 (Sm-1)
Molar conductanceSm2mol-1
Equivalent conductanceSm-1

Question 4.
Give the relationship between molar conductance and specific conductance of an electrolyte.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 1

Question 5.
Give the relationship between equivalent conductance and specific conductance of an electrolyte.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 2

Question 6.
Mention the factors which influence electrolytic conductance.
Answer:

  1. A solvent of a higher dielectric constant shows high conductance in solution.
  2. Conductance is inversely proportional to the viscosity of the medium, i.e., conductivity increases with the decrease in viscosity.
  3. If the temperature of the electrolytic solution increases, conductance also increases. An increase in temperature increases the kinetic energy of the ions and decreases the attractive force between the oppositely charged ions and hence conductivity increases.
  4. Molar conductance of a solution increases with an increase in dilution. This is because, for a strong electrolyte, interionic forces of attraction decrease with dilution. For a weak electrolyte, the degree of dissociation increases with dilution.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 7.
Explain how does the molar conductance of the electrolytes varies with the concentration of the electrolyte.
Answer:
The molar conductance of a strong electrolyte increases on dilution. The variation of molar conductance with dilution is given by an empirical formula
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 3
where Λm0 is called limiting molar conductivity and C is the concentration of the electrolyte.
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 4
For strong electrolytes such as KCl, NaCl, etc., the plot, Λm vs √C, gives a straight line as shown in the graph. It is also observed that the plot is not a linear one for weak electrolytes.
For strong electrolyte, at a high concentration, the number of constituent ions of the electrolyte in a given volume is high and hence the attractive force between the oppositely charged ions is also high. Moreover, the ions also experienced a viscous drag due to greater solvation. These factors attribute to the low molar conductivity at high concentrations. When the dilution increases, the ions are far apart and the attractive forces decrease. At infinite dilution the ions are so far apart, the interaction between them becomes insignificant, and hence, the molar conductivity increases and reaches a maximum value at infinite dilution.
For a weak electrolyte, at high concentration, the plot is almost parallel to the concentration axis with a slight increase in conductivity as the dilution increases. When the concentration approaches zero, there is a sudden increase in the molar conductance and the curve is almost parallel to Λm0 axis. This is due to the fact that the dissociation of the weak electrolyte increases with the increase in dilution (Ostwald dilution law). Λm0 values for strong electrolytes can be obtained by extrapolating the straight line. But the same procedure is not applicable for weak electrolytes, as the plot is not a linear one, A°m values of the weak electrolytes can be determined using Kohlraush’s law.

Question 8.
Flow much charge is required for the following reactions?
(i) 1 mole of Al3+ to Al
(ii) 1 mole of Cu2+ to Cu
(iii) 1 mole of MnO4 to Mn2+
Answer:
(i) Al3+ +3e → Al
Reduction of 1 mole of Al3+ requires 3 moles of electrons.
∴ Charge on 3 moles of electrons
= 3 × 96500 C
= 289500 coulomb
(ii) Cu2+ + 2e → Cu
Reduction of 1 mole of Cu2+ requires 2 mole of electrons
= 2 × 96500 C
= 193000 coulomb
(iii) MnO4 + 8H+ + 5e → Mn2+ + 4H2O
Reduction of MnO4 ions require 5 mole of electrons
= 5 × 96500 C
= 482500 Coulomb

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 9.
A solution of CuSO4 is electrolyzed for 10 minutes with a current of 1.5 amperes. What mass of copper deposited at the cathode?
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 5
∴ Mass of copper deposited at the cathode = 0.296 g

Question 10.
How many hours does it take to reduce 3 mole of Fe3+ to Fe2+. With 2 ampere of current? (F = 96500 coulomb)
Answer:
The required equation is Fe3+ + e → Fe2+
3 mole of Fe3+ requires 3 mole of electrons.
∴ Required charge = 3 × 96500 coloumbs
= 289500 coloumbs
charge = current × time
289500 = 2 × t
t = \(\frac{289500}{2}\)
= 1.475 × 105 sec
= 40 hour.

Question 11.
In an electrolysis experiment, a current was passed for 5 hours through two cells connected in series. The first cell contains a solution of gold salt and the second cell contains copper sulfate solution.
If the oxidation number of gold is +3, find the amount of copper deposited on the cathode in the second cell. Also, calculate the magnitude of the current in amperes.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 6
Let Z be the electrochemical equivalent of copper
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 7

Question 12.
The specific conductance of a decinormal solution of KCl is 0.00112 ohm-1 cm-1. The resistance of a cell containing the solution was found to be 56 ohms. What is the value of the cell constant?
Answer:
Specific conductance = \(\frac{Cell constant}{Resistance}\)
Cell constant = Specific conductance × Resistance
= 0.0112 × 56
= 0.6272 cm-1

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 13.
1.0 N solution of salt surrounding two platinum electrodes 2.1 cm apart and 4.2 sq.cm in area was found to offer a resistance of 50 ohms. Calculate the equivalent conductivity of the solution.
Answer:
Given: l = 2.1 cm; a = 4.2 sq.cm; R = 50 ohm
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 8
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 9

Question 14.
The specific conductivity of 0.02 M KCl solution at 25° C is 2.768 × 10-3 ohm-1 cm-1. The resistance of this solution at 25° C, when measured with a particular cell, was 250.2 ohm. The resistance of 0.01 M CuSO4 solution at 25° C measured with the same cell was 8331 ohm. Calculate the molar conductivity of the copper sulfate solution.
Answer:
Cell constant = Specific conductivity of KCl × Resistance = 2.768 × 10-3 × 250.2
For 0.01 M CuSO4
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 10

Question 15.
At 291 K, the molar conductivities at infinite dilution of NH4Cl, NH4OH, and NaCl are 129.8, 217.8, and 108.9 S cm2 respectively. If the molar conductivity of a cent normal solution of NH4OH is 9.33 S cm2, what is the percentage dissociation of NH4OH at this dilution? Also, calculate the dissociation constant of NH4OH.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 11
∴ degree of dissociation (α)
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 12
Calculation of dissociation constant
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 13

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 16.
The conductivity of a saturated solution of AgCl at 288 K. is found to be 1.382 × 10-6 Scm-1. Find its solubility. Given ionic conductances of Ag+ and Cl ion at infinite dilution are 61.9 S cm2 mol-1 and 76.3 S cm2 mol-1 respectively.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 14

Question 17.
Define (i) electrode potential and (ii) emf of a cell.
Answer:
(i) Electrode potential: The potential difference set up between the metal and its ions in the solution is called the electrode potential, (or) electrode potential may be defined as the tendency of an electrode to lose or gain electrons when it is in contact with a solution of its own ions.
(ii) emf of a cell; The difference between the electrode potentials of the two half cells in a galvanic cell is known as the cell potential (or) It is the driving forces that permit the flow of electrons from anode to cathode.

Question 18.
Explain the terms (i) oxidation potential and (ii) reduction potential of an electrode.
Answer:
(i) Oxidation potential: when an electrode is negatively charged with respect to the solution, i.e., it acts as an anode, the potential difference is called oxidation potential.
M ⇌ Mn+ + ne
It refers to the tendency for oxidation to occur at the electrode.
(ii) Reduction potential: When an electrode is positively charged with respect to solution, i.e., it acts as the cathode, the potential difference developed is called reduction potential
Mn+ + ne ⇌ M
It refers to the tendency for reduction to occur at the electrode.

Question 19.
What is a reference electrode? Mention its use.
Answer:
A reference electrode is an electrode whose electrode potential value is known. It is used to determine, electrode potentials of various electrodes.

Question 20.
Mention the characteristics of electrode chemical series.
Answer:

  1. The negative sign of the standard reduction potential indicates that the electrode when joined with SHE, acts as an anode and oxidation occurs at this electrode. Similarly, the sign of standard reduction potential indicates that the electrode when joined with SHE acts as and reduction occurs on this electrode.
  2. Greater the value of standard reduction potential move easily the substance (element or ions) is reduced or in other words, stronger oxidizing agent it is. Similarly, the lower the value of standard reduction potential of the substance greater is the extent of oxidation half-reaction and the substance acts as a reducing agent.
  3. Reactivity of metals: A metal that has a high negative value (or small positive value) of standard reduction potential loses electrons is said to be chemically active. The chemical reactivity decreases from top to bottom of the series.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 21.
Given the standard reduction potentials
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 15
Arrange these metals in their increasing order of reducing character.
Answer:
Ag < Hg < Cr < Mg < K.
The lesser the reduction potentials greater is their reducing character.

Question 22.
Write down the electrode reactions and the net cell reaction for the following cells. Which electrode would be the positive terminal in each cell.
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 16
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 17
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 18

Question 23.
The standard EMF of the cell:
Ni | N12+ || Cu2+ | Cu is 0.59 V. The standard reduction potential of the copper electrode is 0.34 V. Calculate the standard reduction potential of the nickel electrode.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 19

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 24.
A cell is set up between copper and silver electrodes as Cu | Cu2+ || Ag+ | Ag.
Given: TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 41. Calculate the emf of the cell.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 20

Question 25.
Two half cells are Al3+ | Al and Mg2+ | Mg. The reduction potentials of these half cells are -1.66 and -2.36 V. Construct the galvanic cell, write the cell reaction and calculate the emf of the cell.
Answer:
For the construction of a galvanic cell,
= (Electrode with lesser value of reduction potential – Electrode with higher value of reduction potential )
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 21
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 22

Question 26.
A cell is prepared by dipping a copper rod in 1M CuSO4 solution and a nickel rod in 1M NiSO4 solution. The standard reduction potentials of copper and nickel electrodes are 0.34 V and – 0.25 V respectively.
(a) How will you represent the cell?
(b) What will be the cell reaction?
(c) What will be the standard emf of the cell?
(d) Which electrode will be positive?
Answer:
The cell is represented as
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 23
(d) The cathode is a copper electrode. Because reduction occurs at this electrode.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 27.
Predict whether zinc and silver react with 1M H2SO4 to give hydrogen gas or not. Given the standard reduction potentials of zinc and silver electrodes are -0.76 and 0.80 V respectively.
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 24
Answer:
The cell is
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 25
The emf of the cell is positive. Hence the cell reaction is spontaneous. Thus, zinc will liberate hydrogen gas from 1M H2SO4.
Similarly,
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 26
The cell is
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 27
The emf of the cell is negative. Hence the reaction will not occur, i.e., Ag will not displace hydrogen from 1M H2SO4.

Question 28.
Can a nickel sulphate be used to stir a solution of copper sulphate. Support your answer with a reason.
[OR]
Can a solution of 1M copper sulphate be stored in a vessel made of nickel.
Given:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 28
Answer:
The reaction,
Ni + CuSO4 → NiSO4 + Cu
should not occur, if CuSO4 solution to be stored in a nickel vessel.
The cell would be Ni | Ni2+ || Cu2+ | Cu
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 29
The emf is positive. This means copper sulfate reacts with nickel, Hence CuSO4 cannot be stored in a nickel vessel.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 29.
Give the relationship between the electrode potential and the concentration of the electrode.
Answer:
This relationship is given by Nernst equation. For an electrode reaction,
Mn+ + ne → M
the electrode potential is given by the relationship,
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 30

Question 30.
For general cell reactions
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 31
Write the Nernst equation.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 32
where is the number of electrons involved in the cell reaction?

Question 31.
Calculate the electrode potential of copper electrode, when a copper wire is dipped in 0.1 M CuSO4 solution ECu2+/Cu0 = 0.34.
Answer:
The electrode reaction is Cu2+ + 2e → Cu
Applying Nernst equation
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 33
[Note: Decreasing concentration of the electrolyte decreases the electrode potential]

Question 32.
The following reaction takes place in a galvanic cell.
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 34
Calculate the emf of the cell.
Answer:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 35
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 36

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 33.
Give the relationship between the free energy charge of the cell reaction and the emf of the cell.
Answer:
ΔG° = -n FEcell

Question 34.
Give the relationship between the free energy change for the cell reaction and the equilibrium constant.
Answer:
ΔG° = – 2.303 RT log Kc

Question 35.
(a) Calculate the standard free energy change and maximum work obtainable by a galvanic cell, where the cell reaction
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 37
(b) Also calculate the equilibrium constant for the reaction.
Answer:
(a) The cell is
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 38
Thus the maximum work that can be obtainable from the cell = 212.3 kJ mol-1
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 39

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 36.
Describe the nature of anode, cathode, the cell reaction, and salient features of the Leclanche cell.
Answer:
Anode: Zinc container
Cathode: Graphite rod in contact with Mn02
Electrolyte: ammonium chloride and zinc chloride in water.
Emf of the cell is about 1.5 V.
Cell reaction:
Oxidation at anode:
Zn(s) → Zn2+(aq) + 2e … (1)
Reduction at cathode:
2NH4+(aq) + 2e → 2NH3(aq) + H2(g) … (2)
The hydrogen gas is oxidised to water by MnO2
H2(g) + 2MnO2(s) → Mn2O3(s) + H2O (l) …(3)
Equation (1) + (2) + (3) gives the overall redox reaction
Zn(s) + 2NH4+ (aq) + 2MnO2(s) → Zn2+(aq) + Mn2O3(s) + H2O (l) + 2NH3 ….. (4)
The ammonia produced at the cathode combines with Zn2+ to form a complex ion [Zn(NH3)4]2+(aq). As the reaction proceeds, the concentration of NH4+ will decrease and the aqueous NH3 will increase which lead to the decrease in the emf of cell.

Question 37.
Describe the nature of anode, cathode the cell reaction, and salient features of the mercury button cell.
Answer:
Anode: Zinc amalgamated with mercury.
Cathode: HgO mixed with graphite.
Electrolyte: Paste of KOH and ZnO.
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 40
Cell emf: about 1.35V.
Uses: It has a higher capacity and longer life. Used in pacemakers, electronic watches, cameras etc…

Question 38.
Explain the functioning of lead storage batteries.
[OR]
Explain the chemical reaction involved in the process of charging and recharging in a lead storage battery.
Answer:
Anode: Spongy lead
Cathode: Lead plate bearing PbO2
Electrolyte: 38% by mass of H2SO4 with density 1.2g / mL.
Oxidation occurs at the anode:
Pb(s) → Pb2+(aq) + 2e … (1)
The Pb2+ ions combine with SO4-2 to from PbSO4 precipitate.
Pb2+(aq) + SO42 (aq) → PbSO4(s) …….. (2)
Reduction occurs at the cathode:
PbO2(s) + 4H+(aq) + 2e → Pb2+(aq) + 2H2O (l) ……. (3)
The Pb2+ ions also combine with SO42- ions from sulphuric acid to form PbS04 precipitate.
Pb2+(aq) + SO42-(aq) → PbSO …… (4)
Overall reaction:
Equation (1) + (2) + (3) + (4) ⇒
Pb(s) + PbO2 (s) + 4H+(aq) + 2SO42-(aq) → 2PbSO4(s) + 2H2O (l)
The emf of a single cell is about 2 V. Usually six such cells are combined in series to produced 12 volt.
The emf of the cell depends on the concentration of H2SO4. AS the cell reaction uses SO22 ions, the concentration H2SO4 decreases. When the cell potential falls to about 1.8V, the cell has to be recharged.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Question 39.
Discuss the nature of the anode, cathode, and the cell reaction of the Lithium-ion battery. How does it act as a secondary cell?
Answer:
Anode: Porus graphite.
Cathode: transition metal oxide such as CoO2. Electrolyte: Lithium salt in an organic solvent At the anode oxidation occurs:
Li(s) → Li+(aq) + e
At the cathode reduction occurs:
Li+ + CoO2 (s) + e → Li CoO2 (s)
Overall reactions:
Li(s) + CoO2 → Li CoO2 (s)
Both electrodes allow Li+ ions to move in and out of their structures.
During discharge, the Li+ ions produced at the anode move towards the cathode through the non-aqueous electrolyte. When a potential greater than the emf produced by the cell is applied across the electrode, the cell reaction is reversed and now the Li+ ions move from cathode to anode where they become embedded on the porous electrode. This is known as intercalation.
Uses: Used in cellular phones, laptop computer digital camera, etc…

Question 40.
Mention the various methods of protecting metals from corrosion.
Answer:
This can be achieved by the following methods.

  1. Coating metal surface by paint.
  2. Galvanizing by coating with another metal such as zinc, zinc is a stronger oxidizing agent than iron and hence it can be more easily corroded than iron, i.e., instead of iron, the zinc is oxidized.
  3. Catholic protection: In this technique, unlike galvanizing the entire surface of the metal to be protected need not be covered with a protecting metal instead, metals such as Mg or zinc which is corroded more easily than iron can be used as a sacrificial anode and the iron material acts as a cathode. So iron is protected, but Mg or Zn is corroded.

Passivation: The metal is treated with strong oxidizing agents such as concentrated HNO3. As a result, a protective oxide layer is formed on the surface of the metal.
Alloy formation: The oxidizing tendency of iron can be reduced by forming its alloy with other more anodic metals.
eg: stainless steel – an alloy of Fe and Cr.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

Choose the correct answer:

1. In the electrolytic cell, the flow of electrons is from:
(a) cathode to anode in the solution
(b) cathode to the anode through external supply
(c) cathode to the anode through the internal supply
(d) anode to the cathode through the internal supply
Answer:
(b)
Hint: In electrolytic cells, electrons enter the cathode and leave at the anode. Thus in the external supply, electrons flow from cathode to anode. In the solution, only ions flow and not the electrons.

2. Which of the statements about solutions of electrolytes is not correct?
(a) the conductivity of the solution depends upon the size of the ions.
(b) conductivity depends upon the viscosity of the solution.
(c) conductivity does not depend upon the solvation of ions present in the solution.
(d) the conductivity of the solution increases with temperature.
Answer:
(c)
Hint: Greater the solvation of ions, lesser is the conductivity. Hence, (c) is an incorrect statement.

3. A dilute solution of Na2SO4 is electrolyzed using platinum electrodes. The products at the cathode and anode are:
(a) O2 and H2
(b) SO2, Na
(c) O2, Na
(d) S2O82-, H2
Answer:
(a)
Hint: H20 is more readily reduced than Na+. It is more readily oxidised than S04 2. Hence, the electrode reactions are:
at cathode: 2H2O + 2e → H2 + 2OH
at anode: 2H2O → O2 + 4H+ + 4e.

4. The quantity of charge required to obtain one mole of aluminum from Al2O3 is:
(a) 1F
(b) 6F
(c) 3F
(d) 2F
Answer:
(c)
Hint: Al2O3 → 2Al.
i.e., 2Al2O3 + 6e → 2Al or
Al2O3 + 3e → Al.
Hence, to obtain one mol of Al, the charge required is 3F.

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

5. Electrolysis of dilute aqueous solution of NaCl solution was carried out by passing 10 milliampere current. The time required to liberate 0.01 mole of H2 gas at the cathode is (1 Faraday = 96500 C mol-1):
(a) 9.65 × 104 sec
(b) 19.3 × 104 sec
(c) 28.95 × 104 sec
(d) 38.6 × 104 sec
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 42
Thus,
0.5 mol of H2 is liberated by IF = 96500 C 0.01 mol of H2 will be liberated by charge
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 43

6. Al2O3 is reduced by electrolysis at low potentials and high currents. If 4.0 × 104 amperes of current is passed through molten Al2O3 for 6 hours, what mass of aluminium is produced? (Assume 100% current efficiency. At mass of Al = 27 g mol-1):
(a) 8.1 × 104 g
(b) 2.4 × 105 g
(c) 1.3 × 104 g
(d) 9.0 × 103 g
Answer:
(a)
Hint: Al3+ + 3e → Al
1 mol of Al = 27 g of Al is deposited by 3F or 3 × 96500 C of electricity.
Quantity of electricity passed
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 44

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

7. What current is to be passed for 0.02 A for deposition of a certain weight of metal which is equal to electrochemical equivalent?
(a) 4 A
(b) 100 A
(c) 200 A
(d) 2 A
Answer:
(a)
Hint: Electrochemical equivalent is the weight deposited by 1 coulomb.
Q = I × t
1 = I × 0.25 or I = 4A

8. Acertain current liberates 0.504 g of hydrogen in 2 hours. How many grams of oxygen can be liberated by the same current in the same time?
(a) 2.0 g
(b) 0.4 g
(c) 4.0 g
(d) 8.0 g
Answer:
(c)
Hint: H2O → H2 + \(\frac{1}{2}\) O2
Thus if one mole of H2 is liberated, O2 liberated = \(\frac{1}{2}\) mole
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 45

9. Resistance of 0.2 M solution of an electrolyte is 50Ω. The specific conductance of the solution is 1.3 Sm-1. If the resistance of 0.4M solution of the same electrolyte is 260Ω the molar conductivity is:
(a) 6250 Sm2 mol-1
(b) 6.25 × 10-4 Sm2 mol-1
(c) 625 × 10-4 Sm2 mol-1
(d) 62.5 Sm2 mol-1
Answer:
(b)
Hint:
specific conductance = observed conductance × cell constant
K = \(\frac{1}{R}\) × cell constant
or cell constant = K × R
= 1.3 Sm-1 × 50Ω
= 65 m-1
For 0.4 M solution, specific conductance
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 46

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

10. An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to:
(a) increase in the number of ions
(b) increase in ionic mobility
(c) 100% dissociation of electrolyte at normal dilution
(d) increase in both i.e., number of ions and ionic mobility of ion.
Answer:
(b)
Hint: A strong electrolyte is completely ionized at all concentrations. Hence, the number of ions remains the same. However, on dilution, interionic forces decrease, and hence ionic mobility increases. Therefore, equivalent conductance increases.

11. In the electrolysis of which solution, OH ions are discharged in preference to Cl ions?
(a) dilute NaCl
(b) very dilute NaCl
(c) fused NaCl
(d) solid NaCl
Answer:
(b)
Hint: In very dilute NaCl solution, the following reactions take place on electrolysis.
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 47

12. The charge in coulombs on lg ion of N-3 is:
(a) 28.9 × 105 C
(b) 2.89 × 105 C
(c) 2890 C
(d) 28900 C
Answer:
(b)
Hint: Charge on 1 gm ion of N-3
= 3 × 1.6 × 10-19 C
One g ion = 6.023 × 1023 ion
Charge on 1 gm ion of N-3
= 3 × 1.6 × 10-19 × 6.023 × 1023
= 2.89 × 105 C

13. A solution of copper sulfate is electrolyzed for 10 minutes with a current of 1.5 amperes. The mass of copper deposited at the cathode is: (atomic mass of Cu = 63.5 g mol-1)
(a) 29.6 g
(b) 0.296 g
(c) 2.96 g
(d) 1.564 g
Answer:
(b)
Hint: Current = 1.5 amperes
Time = 10 minutes
= 10 × 60 = 600 s
Quantity of electricity passed = i × t
= 1.5 × 600 = 900 C
The reaction occurring at cathode is
Cu2+ + 2e → Cu
i.e., 2F or 2 × 96500 C deposit
= 1 mol = 63.5 g of Cu
900 C will deposit = \(\frac{63.5}{2 \times 96500}\) × 900 = 0.296 g

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

14. The limiting molar conductance of HCl, CH3COONa, and NaCl are respectively 425, 90, and 125 mho cm2 mol-1 at 25° C. The molar conductivity of 0.1 M CH3COOH solution is 7.8 mho cm2 mol-1 at the same temperature. The degree of dissociation of 0.1 M acetic acid at this temperature is:
(a) 0.1
(b) 0.02
(c) 0.15
(d) 0.03
Answer:
(b)
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 48

15. Degree of dissociation of pure water is 1.9 × 10-9. Molar conductances of H+ and OH ions at infinite dilution are 200 S cm2 mol-1 and 350 Scm2 mol-1 respectively.
(a) 3.8 × 10-7 Scm2 mol-1
(b) 5.7 × 10-7 Scm2 mol-1
(c) 9.5 × 10-7 Scm2 mol-1
(d) 1.045 × 10-6 Scm2 mol-1
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 49

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

16. When measured against a standard calomel electrode, an electrode is found to have a standard reduction potential of 0.100 V. If the standard reduction potential of the calomel electrode is 0.244 V, the standard reduction potential of the same electrode against the standard hydrogen electrode will be:
(a) – 0.144 V
(b) + 0.100 V
(c) – 0.344 V
(d) – 0.100 V
Answer:
(b)
Hint: Standard electrode potential is a fixed quantity for a given electrode. Hence, its standard electrode potential against SHE will remain the same. Viz., (0.100 V). (emf of the cell formed will change)

17. On the basis of the following E° values, the strongest oxidising agent is:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 50
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 51
Answer:
(c)
Hint: The strongest oxidizing agent is a substance that is reduced move easily, i.e., it has the highest reduction potential. Reduction potentials of [Fe(CN)6]-3 and Fe3+ are 0.355 V and 0.77 V. Hence, Fe3+ is reduced more easily and hence is the strongest oxidizing agent.

18. Standard electrode potentials for Sn4+ / Sn2+ couple is +0.15 V and that for Cr3+/Cr couple is – 0.74 V. These two couples in their standard states are connected to make a cell. The cell potential will be:
(a) +1.83 V
(b) +1.19 V
(c) +0.89 V
(d) +0.18 V
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 52

19. Cr2O72- + I → I2 + Cr3+;
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 53
(a) 0.54 V
(b) – 0.54 V
(c) +0.18 V
(d) -0.18 V
Answer:
(a)
Hint: In the given reaction, I is oxidized to I2 and Cr2O72+ ions have been reduced to Cr3+. The cell is
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 54

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

20. Given the standard electrode potentials K+/K = -2.93 V; Ag+ / Ag = 0.80 V; Mg22+ / Hg = 0.79; Mg2+/Mg = -2.37 V; Cr2+/Cr = -0.74 V.
Arrange these metals in their increasing order of reducing power.
(a) Ag < Hg < Cr < Mg < K
(b) K < Mg < Cr < Hg < Ag
(c) Hg < Cr < Mg < K < Ag
(d) Mg < Cr < Hg < Ag < K
Answer:
(a)
Hint: Lower the reduction potential, more easily it is oxidized and hence greater is its reducing power.

21. The reduction potential of hydrogen half cell will be negative if:
(a) pH2 = 1 atm and [H+] = 1.0 M
(b) pH2 = 2 atm and [H+] = 1.0 M
(c) pH2 = 2 atm and [H+] = 2.0 M
(d) pH2 = 1 atm and [H+] = 2.0 M
Answer:
(b)
Hint: For hydrogen electrode,
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 55

22. 2Hg → Hg2+; E° = 0.855 V
Hg → Hg2+; E° = 0.799 V
Equilibrium constant for the reaction
Hg + Hg2+ ⇌ Hg22+ at 27° C is:
(a) 89
(b) 82.3
(c) 79
(d) none of these
Answer:
(c)
Hint:
E° for the reaction = 0.855 – 0.799 = 0.056 V
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 56

TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry

23. Standard free energies of formation of (in kJ mol-1) at 298 K are -237.3, -394.2, and -8.2 for H2O(l), CO2(g), and pentane (g) respectively. The value of E°ell for the pentane-oxygen fuel cell is:
(a) 1.968 V
(b) 2.0968 V
(c) 1.0968 V
(d) 0.968 V
Answer:
(c)
Hint: The balanced equation for pentane oxygen cell reaction will be:
TN Board 12th Chemistry Important Questions Chapter 9 Electro Chemistry 57

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Students get through the TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Answer the following questions.

Question 1.
State the formula and the name of the conjugate base of each of the following acids.
(a) H3O+,
(b) HSO4,
(c) HF,
(d) NH4+,
(e) CH3NH3+,
(f) CH3PO4,
(g) CH3COOH,
(h) H2PO4,
(i) HS,
(j) HCO3.
Answer:
(a) H2O – water
(b) SO4-2 – sulphate ion
(c) F – fluoride ion
(d) NH3 – ammonia
(e) CH3NH2 – methyl amine
(f) H2PO4 – dihydrogen phosphate ion
(g) CH3COO – acetate ion
(h) HPO4-2 – hydrogen phosphate ion
(i) S-2 – sulphide ion
(j) CO3-2 – carbonate ion

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 2.
State the formula and name of the conjugate acid of each of the following:
(a) OH,
(b) CH3COOH,
(c) HPO4-2,
(d) CO3-2,
(e) NH3,
(f) CH3NH2,
(g) HS,
(h) CH3COO
(i) H2PO4,
(j) Cl.
Answer:
(a) H3O – water
(b) CH3COOH2+ – protonated acetic acid
(c) H2PO4 – dihydrogen phosphate ion
(d) HCO3 – bicarbonate ion
(e) NH4+ – ammonium ion
(f) CH3NH3+ – protonated methyl amine
(g) H2S – hydrogen sulphide
(h) CH3COO – acetic acid
(i) H3PO4 – phosphoric acid
(j) HCl – hydrochloric acid

Question 3.
Which of the following behave both as Bronsted acids as well as Bronsted bases?
NH3, HSO4, H2SO4, HCO3; H3PO4, HS, H2O.
Answer:
NH3, HSO4 , HCO3 ; HS and H2O behave both as Bronsted acids and Bronsted bases.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 1

Question 4.
Classify Lewis acids and bases from the following:
H3O+, CH3NH2, BF3, OH, Cu2+, S2-, CH3COO.
Answer:
Lewis acids: H3O+, BF3, Cu2+.
Lewis bases: CH3NH2, OH, S2-, CH3COO.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 5.
Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base.
(a) OH, (b) F, (c) H+, (d) BCl3
Answer:
(a) OH is a Lewis base because it acts as an electron-pair donor.
(b) F is also a Lewis base.
(c) H+ is a Lewis acid because it acts as an electron pair acceptor.
(d) BCl3 is an electron-deficient compound electron pair acceptor, hence Lewis acid.

Question 6.
Explain how the [H+] concentration or [OH] concentration, decides a solution as acidic, neutral, or alkaline.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 2

Question 7.
Calculate the hydrogen and hydroxyl ion concentrations in (i) 0.01M HNO3, (ii) 0.001M KOH solution at 298 K.
Answer:
(i) HNO3 is a strong acid. It ionizes as
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 3
(ii) KOH is a strong base. It ionizes as
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 4

Question 8.
Assuming complete dissociation, calculate the pH of the following solutions:
(i) 0.003M HCl,
(ii) 0.005M NaOH,
(iii) 0.002M HBr,
(iv) 0.002M KOH.
Answer:
(i) HCl → H+ + Cl
[H+] = [HCl] = 0.003M
pH = – log [H+]
= – log [0.003] = 2.52

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

(ii) NaOH → Na+ + OH
[OH] = [NaOH] = 0.005M
pOH = – log[OH]
= – log [0.005] = 2.301
pH = 14 – pOH
= 14 – 2.301 = 11.699

(iii) HBr → H+ + Br
[H+] = [HBr]
= 0.002M
pH = – log [H+] (or)
pH = – log [0.002] = 2.6989

(iv) KOH → K+ + OH
[OH] = [KOH]
= 0.002M
pOH = – log [OH ]
pH = – log (0.002) = 2.6929
pH = 14 – pOH (or)
= 14 – 2.6929 = 11.3011

Question 9.
Calculate the pH of the resulting mixtures: 10 ml of 0.02M Ca(OH)2 + 25 ml of 0.1M HCl.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 5
Number of moles of OH ion = 2 x 0.002 = 0.004
Number of moles of H+ ion = 0.0025
Number of moles of OH remaining after neutralisation = 0.004 – 0.0023 = 0.0015
Molarity of OH ions
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 6

Question 10.
The concentration of H+ ions in 0.1 M solution of a weak acid is 1.0 x 10-5 mol L-1. Calculate the dissociation constant of the acid.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 7
[HA] can be taken as 0.1 as 1 x 10-5 is very small. Hence,
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 8

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 11.
Find whether the resulting solution is acidic, neutral, or basic when
(i) a strong acid is mixed with a strong base
(ii) a strong acid is mixed with a weak base
(iii) a weak acid is mixed with a strong base
(iv) a weak acid is mixed with a weak base.
Answer:
(i) A strong acid and a strong base give a neutral solution because both are completely ionized and the reaction goes on completion.
eg:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 9
(ii) A strong acid and a weak base give an acidic solution, as the weak acid is hot completely ionized. The reaction does not go for completion and there is an excess of hydrogen ions in the solution.
eg:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 10
The solution is therefore is acidic.
(iii) A weak acid and a strong base give a basic solution, as the weak acid is not completely ionized. The reaction does not go for completion and there is an excess of hydroxyl ions in the solution.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 11
Hence the solution is basic.
(iv) A weak acid and a weak base give an acidic, neutral, or basic depending on the relative strength of acid or base. If both weak acid and weak base have equal strength, the resulting solution is neutral.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 12

Question 12.
State Ostwald’s dilution law.
Answer:
When dilution increases, the degree of dissociation of weak electrolytes also increases.
The mathematical form is
α = \(\sqrt{\frac{\mathrm{K}_{a}}{\mathrm{C}}}\)
where ‘α’ is the degree of dissociation, Ka is the dissociation constant of the acid and ‘C’ is its concentration.

Question 13.
Explain the term ‘common ion effect’ with an example.
Answer:
The suppression of the dissociation of a weak electrolyte by the addition of an ion in common with that of the weak electrolyte is known as the common ion effect.
Consider the dissociation of acetic acid in the presence of sodium acetate or HCl.
In the absence of any added salt, the dissociation of acetic acid is represented as
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 13
The addition of acetate ions in the form of sodium acetate increases the concentration of acetate ions. This increases the value of Ka. But Ka is a constant at a given temperature. Thus to maintain the Ka value constant, H+ ions combine with acetate ion to form undissociated acetic acid. i.e., The degree of dissociation of acetic acid in the presence of acetate ion is less than in the absence of sodium acetate. The same happens in the presence of HCl.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 14.
What are buffer solutions? Give example.
Answer:

  1. Buffer solutions resist changes in pH by the addition of small quantities of an acid or a base. This ability is known as buffer action.
  2. Buffer solutions consist of a mixture of a weak acid and a salt of a weak acid and a strong base.
    eg: CH3COOH + CH3COONa. This type of buffer is known as an acid buffer.
  3. Buffer solution which consists of a mixture of a weak base and a salt of a weak base and strong acid is known as a basic buffer.
    eg: NH4OH and NH4Cl.

Question 15.
Give the characteristics of a buffer solution.
Answer:

  1. It should have a definite pH. i.e., it has reserve acidity or alkalinity.
  2. Its pH does not change on standing.
  3. Its pH does not change on dilution.
  4. Its pH is only slightly changed by the addition of a small quantity of acid or base.

Question 16.
Give examples of acidic and basic buffers.
Answer:
Acidic buffer:

  1. CH3COOH + CH3COONa
  2. Boric acid and borax.
  3. Pthalic acid and potassium acid pthalate.

Basic buffer:

  1. NH4OH + NH4Cl
  2. Glycine and glycine hydrochloride.
  3. Aniline and aniline hydrochloride.

Question 17.
Explain buffer action with a suitable example.
Answer:
The buffer action in a solution containing CH3COOH and CH3COONa is explained as follows:
The dissociation of the buffer components occurs as below.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 14
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 15
If an acid is added to this mixture, it will be consumed by the conjugate base CH3COO to form the undissociated weak acid i.e., the increase in the concentration of H+ does not reduce the pH significantly.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 16
If a base is added, it will be neutralized by H3O+, and the acetic acid is dissociated to maintain the equilibrium. Hence the pH is not significantly altered.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 17

Question 18.
Explain the terms ‘buffer capacity” and ‘buffer index”.
Answer:
The buffer capacity is the ability of the buffer to resist changes in pH by the addition of small quantities of acid or base. It is measured in terms of buffer capacity. The quantitative measure of buffer capacity is the buffer index. It is defined as the number of equivalents of acid or base to one liter of the buffer solution to change its pH by unity.
β = \(\frac{d \mathrm{~B}}{d(\mathrm{pH})}\)
where P = buffer index, dB = number of gram equivalent of acid/base added to one liter of buffer solution, d(pH) = The change in pH after the addition of an acid or base.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 19.
Derive Henderson equation for the determination of pH of an acid buffer.
Answer:
An acid buffer consists of a mixture of a weak acid and salt with strong acid. The ionization of weak acid, HA is given by
HA ⇌ H+ + A
The dissociation constant of the weak acid is given by,
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 18
It can be assumed that the concentration of [A] ions from the complete ionization of the salt compared to the ionization of the weak acid. Hence, [A] concentration may be considered as the concentration of the salt.
So,
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 19
Taking logarithms on both sides and reversing the sign,
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 20
This is known as Henderson’s equation.

Question 20.
Write Henderson’s equation for a basic buffer.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 21

Question 21.
Suppose it is required to make a buffer solution of pH = 4. Using acetic acid and sodium acetate. How much sodium acetate to be added to 1 liter of N/10 acetic acid? The dissociation constant of acetic acid is 1.8 × 10-5.
Answer:
Applying Henderson’s equation,
The molecular mass of CH3COONa = 82
Amount of salt = 0.018 × 82 = 1.476 g.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 22

Question 22.
Calculate the pH of a buffer solution containing 0.15 moles of NH4OH and 0.25 moles of NH4Cl. (Kb for NH4OH = 1.8 × 10-5)
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 23
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 24

Question 23.
Calculate the pH of 0.1M ammonia solution. Calculate the pH after 50 ml of this solution is treated with 25 ml of 0.1M HCl. The dissociation constant of ammonia, Kb = 1.77 × 10-5.
Answer:
For NH4OH
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 25
When NH3 is added, neutralization occurs
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 26
(MNH4Cl) number of mole of NH4Cl = 0.0025
(MNH4OH) Remaining mole of NH4OH = 0.005 – 0.0025 = 0.0025
According to Henderson’s equation,
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 27

Question 24.
Define hydrolysis.
Answer:
The reaction between cation or anion of the salt with water to produce the acid and base from which the salt formed is known as hydrolysis.
salt + H2O = acid + base

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 25.
Define the term degree of hydrolysis.
Answer:
It is the fraction of one mole of the salt that undergoes hydrolysis is known as the degree of hydrolysis.

Question 26.
Define the term hydrolysis constant (Kh), with an example.
Answer:
The equilibrium constant for the reaction, salt + H2O ⇌ acid + base, is known as the hydrolysis constant (Kh). Consider the hydrolysis of acetate ion.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 28

Question 27.
The pKa of acetic acid and pKb of ammonium hydroxide are 4.76 and 4.75 respectively. Calculate the pH of the ammonium acetate solution.
Answer:
Ammonium acetate is the salt of a weak acid and weak base.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 29

Question 28.
The ionization constant of nitrous acid is 4.5 × 10-4. Calculate the pH of 0.04 M sodium nitrite solution and its degree of hydrolysis.
Answer:
Sodium nitrite is a salt of a weak acid and a strong base.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 30
Substituting these values in equation (1)
pH = \(\frac{1}{2}\) [14 + 3.346 – 1.3979]
= 7.974
Degree of hydrolysis (h)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 31

Question 29.
Calculate the degree of hydrolysis and pH of a 0.1M sodium acetate solution. The hydrolysis constant of sodium acetate is 5.6 × 10-10.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 32

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 30.
Calculate the pH of an aqueous solution of 1.0M ammonium formate assuming complete dissociation. pKa for formic acid is 3.8 and pKb of ammonia = 4.8.
Answer:
Ammonium formate is a salt of a weak acid and weak base.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 33

Question 31.
A 0.02 M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization constant of pyridine.
Answer:
Pyridinium hydrochloride is a salt of a weak base and strong acid.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 34

Question 32.
Define solubility product.
Answer:
It is defined as the product of the concentration of ions in a saturated solution of an electrolyte at a given temperature.

Question 33.
Give expressions for the solubility product of the following: (i) BaSO4, (ii) H2S, (iii) Sb2S3, (iv) AlI3.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 35

Question 34.
Mention the criteria of precipitation of an electrolyte.
Answer:
The ionic product should exceed the value of the solubility product, for precipitation to occur.

Question 35.
How will you decide whether a solution is saturated or unsaturated, from the ionic product values?
Answer:

  1. When the ionic product is less than the solubility product, the solution is unsaturated.
  2. When an ionic product is equal to the solubility product, the solution is saturated.

Question 36.
Obtain a relationship between solubility and solubility product of the following: (i) AgCl, (ii) Ag2CO3, (iii) CaF2, (iv) Cr(OH)3.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 36
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 37

Question 37.
Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to the precipitation of copper iodate? Ks for cupric iodate = 7.4 x 10-8.
Answer:
Given, [NaIO3] = 0.002 M
[Cu(ClO3)2] = 0.002 M
∴ [IO3] = 0.002 M
[Cu+2] = 0.002 M
When equal volumes of these solutions are mixed, their concentrations will be halved.
i.e., [IO3] = 0.001 M
[Cu+2] = 0.001 M
Cu(IO3)2 ⇌ Cu+2 + 2IO3
Ks = [Cu+2][IO3]2
= 0.001 x (0.001)2 = 10-9
Since IP is less than solubility products precipitation will not occur.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

Question 38.
What is the minimum volume of water required to dissolve 1 gm of calcium sulfate at 298 K. The Ks for calcium sulfate is 9.1 x 10-6.
Answer:
Let the solubility of CaSO4 at 298 K be ‘s’ mol L-1.
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 39
Minimum volume of water required to dissolve
1 g of CaSO4 = \(\frac{1000}{0.41}\)
= 2439 mL = 2.439 L

Question 39.
The solubility product of BaS04 is 1.5 x 10-9 Find its solubility (i) in pure water and (ii) in 0.1M BaCl2, solution.
Answer:
(i)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 40
Let ‘s’ be the solubility in mol L-1. Then
Ks = s2
(or) 1.5 x 107 = s2
s = \(\sqrt{1.5 \times 10^{-9}}\)
= 3.87 x 10-5 mol L7

(ii) Let (s’) be the solubility of BaSO4 in 0.1M BaCl2 solution.
Total [Ba2+] = [Ba2+] from BaSO4 from [Ba2+] from BaCl2.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 41

Question 40.
Calculate the pH at which Mg(OH)2 begins to precipitate from a solution containing 0.10 Mg2+ ions.
Answer:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 42

Choose the correct answer:

1. What is the conjugate base of OH?
(a) O2
(b) H2O
(c) O
(d) O2-
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 43

2. C2H5ONa is …………. of C2H5OH.
(a) strong acid
(b) weak acid
(c) strong base
(d) weak base
Answer:
(c)
Hint: C2H5OH is a strong base. a weak acid, C2H5O is a strong base

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

3. Among the following, the one which can act as Bronsted acid as well as Bronsted base is:
(a) H3PO4
(b) AlCl3
(c) CH3COO
(d) H2O
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 44

4. At 25° C, the dissociation constant of a base, BOH is 1.0 x 10-12. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:
(a) 1.0 x 10-6 mol lit-1
(b) 1.0 x 10-7 mol lit-1
(c) 2.0 x 10-6 mol lit-1
(d) 1.0 x 10-5 mol lit-1
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 45

5. Which of the following is the correct statement?
(a) HCO3 is the conjugate base of CO32-
(b) NH2 is the conjugate acid of NH3
(c) H2SO4 is the conjugate acid of HSO4
(d) NH3 is the conjugate base of NH2
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 46

6. Three reactions involving H2PO4 are given below:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 47
In which of the above H2PO4 act as an acid?
(a) (iii) only
(b) (i) only
(c) (ii) only
(d) (i) and (ii)
Answer:
(c)

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

7. Which one of the following will decrease the pH of 50 ml of 0.01M hydrochloric acid?
(a) Addition of 50 ml of 0.01 M HCl
(b) Addition of 50 ml of 0.002 M HCl
(c) Addition of 150 ml of 0.002 M HCl
(d) Addition of 5 ml of 1 M HCl
Answer:
(d)
Hint: For 0.001 M HCl, [H+] = 10-2M; pH = 2
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 48
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 49

8. If pKa for fluoride ion at 25° C, is 10.83, the ionisation constant of hydrofluoric acid at this temperature is:
(a) 1.74 x 10-5
(b) 3.52 x 10-3
(c) 6.75 x 10-4
(d) 5.38 x 10-2
Answer:
(c)
Hint:
pKa + pKb = 14
pKa = 14 – 10.83 = 3.17
pKa= – log Ka = – log 3.17
log Ka= -3.17 = 4.83
(or) Ka= 6.76 x 10-4

9. The pH of a solution obtained by mixing 100 ml of a solution of pH = 3 with 400 ml of a solution of pH = 4 is:
(a) 3 – log 2.8
(b) 1 – log 2.8
(c) 4 – log 2.8
(d) 5 – log 2.8
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 50

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

10. The pH of 0.1M aqueous solution of a weak acid, HA is 3. What is its degree of dissociation?
(a) 1%
(b) 10%
(c) 50%
(d) 25%
Answer:
(a)
Hint: HA ⇌ H+ + A
[H+] = Cα
0.1 x α = 10-3
α = 10-2 i.e., 1%

11. The pKa of acetic acid is 4.74. The concentration of acetic acid is 0.01 M. The pH of acetic acid is:
(a) 3.37
(b) 4.37
(c) 4.74
(d) 0.474
Answer:
(a)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 51

12. How many times 1M CH3COOH solution should be diluted so that pH of the solution is doubled?
(a) 20 times
(b) 200 times
(c) 5.55 x 102 times
(d) 5.55 x 104 times
Answer:
(d)
Hint: pH of a weak acid
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 52

13. 40 ml of 0.1M ammonia is mixed with 20 ml 0.1M HCl. What is the pH of the mixture? (pKb for ammonia is 4.74).
(a) 4.74
(b) 2.26
(c) 9.26
(d) 5.00
Answer:
(c)
Hint: 40 ml of 0.1M NH3 solution
= 40 x 0.1 milli = 4 millimol
20 ml of 0.1 M HCl = 20 x 0.1 = 2 millimol
2 millimol of HCl neutralise 2 millimol of NH4OH, to form 2 millimol of NH4OH.
NH4OH left = 2 millimol
Total volume = 60 ml
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 53

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

14. The pH of a solution formed on mixing 20 ml of 0.05M H2SO4 with 5 ml of 0.45 M NaOH at 298 K is:
(a) 6
(b) 2
(c) 12
(d) 1
Answer:
(c)
Hint:
2NaOH + H2SO4 → Na2SO4 + 2H2O
20 ml of 0.05M H2SO4
= 20 ml of 0.05 millimol
= 1.0 millimol

5 ml of 0.45M NaOH
= 5 x 0.45 millimol
= 2.25 millimol

2 millimol of NaOH will react with 1 millimol of H2SO4.
∴ NaOH left in solution = 0.5 millimol Volume of the solution = 25 ml
∴ [OH] = \(\frac{0.5}{25}\) = 0.01 M = 10-2 M
[H+] = 10-12;
pH = 12

15. Which of the following salts will have the highest pH in water?
(a) KCl
(b) NaCl
(c) Na2CO3
(d) CuSO4
Answer:
(c)
Hint: KCl and NaCl, being salts of strong acid and strong base do not get hydrolysed. Their aqueous solutions are neutral and hence their pH = 7.
Na2CO3 being a salt of weak acid and a strong base, gives NaOH as a product of hydrolysis. Hence, its aqueous solution is alkaline and has pH >7.
CuSO4 being a salt of strong acid and weak base, gives H2SO4, as a product of hydrolysis H2SO4 is a strong acid and its pH < 7.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

16. The H3O+ ion concentration of a solution of pH 6.58 is:
(a) antilog (- 6.58)
(c) antilog (- 5.58)
Answer:
(a)
Hint: pH = – log [H3O+];
log [H3O+] = -pH = – 6.58
[H3O+] = antilog (-6.58)
= 2.63 x 10-7 g ion/lit

17. 30 CC of \(\frac{M}{4}\) HCl, 20 CC of \(\frac{M}{2}\) HNO3, and 40 CC of \(\frac{M}{4}\) NaOH solutions are mixed and the volume is made upto 1 dm3. The pH of the resulting solution is:
(a) 2
(b) 1
(c) 3
(d) 8
Answer:
(a)
Hint:
Total millimoles of H
= (30 x \(\frac{1}{3}\)) + (20 x \(\frac{1}{2}\))
= 10 + 10 = 20
Total millimol of OH
= 40 x \(\frac{1}{4}\) = 10
∴ H+ ions left after the neutralisation = 10 millimoles Volume of the solution
= 1 dm3
∴ Molarity of H+ ions
= \(\frac{10}{1000}\) = 10-2M
pH = – log [H+]
= – log [10-2] = 2

18. The pH of 0.1 M solutions of the following salts increases in the order:
(a) NaCl < NH4Cl < NaCN < HCl
(b) HCl < NH4Cl < NaCl < NaCN
(c) NaCN < NH4Cl < NaCl < HCl
(d) HCl < NaCl < NaCN < NH4Cl
Answer:
(b)
Hint: NaCl = neutral (pH = 7); NH4Cl = slightly acidic (pH < 7); NaCN = basic (pH > 7); HCl = strongly acidic (pH << 7).

19. A weak acid HX has the dissociation constant 1 x 10-5. It forms NaX on reaction with alkali. The degree of hydrolysis of 0.1 M solution of NaX is:
(a) 0.0001%
(b) 0.01 %
(c) 0.1%
(d) 0.15 %
Answer:
(b)
Hint: Hydrolysis reaction is
X + H2O ⇌ HX + OH.
For a salt of weak acid with strong base,
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 54

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

20. Among the following hydroxides, the one which has the lowest value of Ks (solubility product) at ordinary temperature is:
(a) Mg(OH)2
(b) Ca(OH)2
(c) Ba(OH)2
(d) Be(OH)2
Answer:
(d)
Hint: The solubility increases down the group due to an increase in the size of the ion and a decrease in lattice energy. Lower the solubility, lower is the Ks.

21. On adding 0.1M solution each of Ag+, Ba2+, Ca2+ ions in a Na2SO4 solution, the species first precipitated is (Ks(CaSO4) = 10-6, Ks(BaSO4) = 10-11, Ks(Ag2SO4) = 10-5:
(a) Ag2SO4
(b) BaSO4
(c) CaSO4
(d) All of these
Answer:
(b)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 55
The minimum [SO42-] concentration required for precipitation in for BaSO4.

22. The Ks of Ag2CrO4, AgCl, AgBr, and AgI are respectively 1.1 x 10-12, 1.8 x 10-6, 5.0 x 10-13 and 8.3 x 10-17. Which of the following salts will precipitate last of AgNO3 solution containing equal moles of NaCl, NaBr, Nal and Na2CrO4.
(a) AgBr
(b) Ag2CrO4
(c) AgI
(d) AgCl
Answer:
(b)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 56
As the solubility of Ag2CrO4 is highest, it will be precipitated last at all.

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

23. The Ks of Ag2CrO4 is 1.1 x 10 12 at 298 K.
The solubility in mol per litre of Ag2CrO4 in 0.1M. AgNO3 solution is:
(a) 1.1 x 10-11
(b) 1.1 x 10-10
(c) 1.1 x 10-12
(d) 1.1 x 10-9
Answer:
(b)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 57

24. Using Gibb’s free energy change, AG° = +63.3 kJ for the following reaction:
Ag2CO3 (s) ⇌ 2Ag+(aq) + CO32-(aq)
the Ks for Ag2CO3 in water at 25° C is (R = 8.314 JK-1 mol-1)
(a) 3.2 x 10-26
(b) 8.0 x 10-12
(c) 2.9 x 10-3
(d) 7.9 x 10-2
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 58

25. A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20M. If the equilibrium constant, Kb for NH3 equals 1.8 x 10-5, what is the pH of the solution?
(a) 8.73
(b) 9.08
(c) 9.43
(d) 11.72
Answer:
(b)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 59
= 4.74 – 0.176 = 4.56
pH = 14 – pOH = 14 – 4.56 = 9.44

26. What is the [H+] in mol/L of a solution that is 0.20M in CH3COONa and 0.10M in CH3COOH? Kb for CH3COOH = 1.8 x 10-5:
(a) 9.0 x 106
(b) 3.5 x 10-6
(b) 1.1 x 10-5
(d) 1.8 x 10-5
Answer:
(a)
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 60

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

27. In what volume ratio of NH4Cl and NH4OH solution (each 1M) should be mixed to get a buffer solution of pH, 9.80 (pKb for NH4OH is 4.74):
(a) 1 : 2.5
(b) 2.5 : 1
(c) 1 : 3.5
(d) 3.5 : 1
Answer:
(c)
Hint:
Suppose ‘V1’ ml of 1M NH4Cl is mixed with ‘V2’ ml of 1M NH4OH solution:
V1 ml of 1M NH4Cl = V1 millimole
V2 ml of 1M NH4OH = V2 millimole
pH = 9.80, Hence pOH = 14 – 9.80 = 4.20
TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium 61

TN Board 12th Chemistry Important Questions Chapter 8 Ionic Equilibrium

28. Which one of the following pairs of solutions is not an acidic buffer?
(a) H2CO3 + Na2CO3
(b) H3PO4 + Na3PO4
(c) HClO4 + NaClO4
(d) CH3COOH + CH3COONa
Answer:
(c)
Hint: HClO4 is a strong acid. Hence, it cannot be used to make an acidic buffer.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Students get through the TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Answer the following questions.
Question 1.
Express the rate of the following reaction in terms of disappearance of the reactant and appearance or formation of the product: A → B
Answer:
Rate of disappearance of the reactant = \(-\frac{\Delta[\mathrm{A}]}{\Delta t}\)
where the negative sign indicates the concentration of the reactant decreases with time.
Rate of formation of the product = \(+\frac{d[\mathrm{B}]}{d t}\)
The positive sign indicates that the concentration of the product increases with time.

Question 2.
Mention the unit of rate of reaction.
Answer:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 1
For a gaseous reaction, a unit of rate = atm sec-1 since concentration is expressed in partial pressures.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 3.
Explain how will you determine experimentally determine
(i) average rate of reaction
(ii) instantaneous rate of reaction and
(iii) initial rate of reaction.
Answer:
The changes in concentration of the reactants or products are experimentally determined by withdrawing a small portion of the reaction mixture (usually 2 or 5 ml) at suitable intervals of time and then freeze to about 0°C to stop the reaction. The concentration of the reactant or product is measured by a suitable method. A plot of concentration-time is made from the graph, the average rate, instantaneous and initial rates can be determined.
(i) Average rate: Two equivalent points are taken with respect to the time at which the average rate is to be determined. The concentrations corresponding to these points are noted from the graph. The difference in concentration is divided by the time interval between equidistant points. Two equidistant points with respect to T is selected. Let these be ‘t1,’ and ‘t2’ respectively. The corresponding concentrations are x1, and x2 respectively.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 1
(ii) Instantaneous rate of reaction: For the determination of the instantaneous rate of reaction at any time ‘t’, a tangent is the direction to the curve at the point ‘P’ corresponding to that time. The slope of this tangent gives the instantaneous rate of reaction.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 3
Where Q is the angle of a tangent with the time axis. In a similar manner, the rate of formation of the product can be determined by measuring the slope of the tangent at a particular instant in concentration to the time curve.
(iii) Initial rate of reaction:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 4
The rate of reaction is maximum at the time of mixing the concentration. This cannot be determined experimentally. This is determined from the concentration is time curve. The curve is extrapolated to zero time and the slope of this curve at zero time gives the initial rate of the reaction.
\(\frac{\Delta x}{\Delta t}\) = initial rate.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 4.
In the reaction 2A → products the concentration of A decreases from 0.5 mol L1 to 0.4 mol L-1 in 10 minutes. Calculate the rate during this period.
Answer:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 5

Question 5.
The concentration of reactant changes from 0.03 M to 0.02 M in 25 minutes. Calculate the average rate using units of time both in minutes and in seconds.
Answer:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 6

Question 6.
The decomposition of N2O5 is expressed by the equation.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 7
If during a certain interval of time the rate of decomposition of N2O5 is 1.8 x 10-3 mol liter 1 min-1, what will be the rates of formation of NO2 and O2 during the same interval.
Answer:
The rate expression for the decomposition of N2O5 is
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 8
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 9

Question 7.
For each of the following reactions, express the given rate of change of concentration of the product or reactant in terms of rate of change of concentration of other reactants or products in that reaction.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 10
Answer:
(a)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 11
(b) The equality in this case is,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 12
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 13
(c) The equality in this case is,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 14

Question 8.
From the concentration of R at different times given below, calculate the average rate of the reaction.
Answer:
R → P during different intervals of time
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 15
Average rate of reaction between 0 → 5 sec
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 16
Average-rate of reaction between 5-10 sec
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 17
Similarly, average rate between 10 → 20 and 20 → 30 see can be calculated.
Note: What we understand from the above problem is that the rate of reaction is not a constant quantity. It decreases with time.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 9.
The decomposition of N2O5 is CCl4 solution at 318K has been studied by monitoring the concentration of the N2O5 in the solution. Initially, the concentration of N2O5 in the solution is 2.33 M and after 184 minutes it is reduced to 2.08 M. The reaction takes place according to the equation
2N2O5 → 4NO2 + O2.
Calculate the average rate of the reaction in terms of hours, minutes and seconds. What is the rate of production during this period?
Answer:
Average rate of reaction (mol L-1 min-1)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 18
For the given reaction
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 19

Question 10.
In hydrogenation reaction at 25°C it is observed that hydrogen gas pressure falls from 2 atm to 1.2 atm in 50 min. Calculate the rate of reaction in molarity per sec.
Answer:
R = 0.0821 lit mol-1 deg-1
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 20
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 21

Question 11.
Explain why the average rate cannot be used to produce the rate of reaction at any instant.
Answer:
Because the rate decreases with time as the reaction proceeds. It is not constant.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 12.
Bring out the difference between the rate and rate constant of a reaction?
Answer:

Rate of a reactionThe rate constant of a reaction
It represents the speed at which the reactants are converted into products at any instant.It is a proportionality constant.
It is measured as a decrease in the concentration of the reactants or an increase in the concentration of products.It is equal to the rate of reaction when the concentration of each of the reactants in unity.
It depends on the initial concentration of reactants.It does not depend on the initial concentration of reactants.

Question 13.
The decomposition of dimethyl ether leads to the formation of CH4, H2, and Co and the reaction rate in given by
rate = R [CH3OCH3]3/2
The rate is followed by an increase in pressure in a closed vessel so that the rate is expressed in terms of partial pressure of dimethyl ether.
rate = R[PCH3OCH3]3/2
If the pressure is measured in the bar and the time in seconds then what are theTxmts of rate and rate constant?
Answer:
The rate law of the reaction
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 22

Question 14.
State the order with respect to each reactant, overall reaction, and the units of the rate constant in each of the following reactions.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 23
Answer:
(a) Order with respect to NO and Br2 are 2 and 1 respectively, over all order is 3.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 24
(b) Order \(\frac{3}{2}\)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 25
(c) Order with respect to H2 and NO are 1 and 2 respectively.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 26
= mol-2 litre2 sec-1
(d) Order with respect to CO and Cl2 are 2 and \(\frac{1}{2}\) respectively.
Over all order = 2\(\frac{1}{2}\) = \(\frac{5}{2}\)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 27
(e) Order with respect to H2O2 and I are one respectively. Over all order 1 + 1 = 2
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 28

Question 15.
Identify the reaction order from the following rate constants.
(a) k = 3.1 × 10-4 sec-1
(b) k = 1.12 × 10-2
(c) k = 1.35 × 10-2 mol-2 let2 s-1
(d) k = 3.4 × 10-3 mol let s-1
Answer:
(a) Let the reaction be of nth order
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 29
i.e., reaction is of first order.
(b) (atm)1-n × s-1 = atm-1 s-1
1 – n = -1 : or n = 2
i.e., reaction is of second order.
(c)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 30
i.e., reaction is of third order.
(d)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 31
i.e., reaction is of second order.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 16.
Derive an expression for the rate constant for the first-order reaction.
Answer:
A reaction whose fate depends on the reactant concentration raised to the first power is called a first order reaction. Let us consider the following Cl2 first-order reaction,
A → product
Rate law can be expressed as Rate = k [A]1
Where, k is the first order rate constant.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 32
Integrate the above equation between the limits of time t = 0 and time equal to t, while the concentration varies from the initial concentration [A0] to [A] at the later time.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 33
This equation is in a natural logarithm. To convert it into the usual logarithm with base 10, we have to multiply the term by 2.303.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 34

Question 17.
How will you determine the first-order rate constant graphically?
Answer:
For a first order reaction, the rate constant k is given by
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 35
where [A0] is the initial concentration of the reactant and [A] is the concentration of the reactant at time it\
Rearranging this equation in the form . y = mx + c, we get
log [A0] – log [A] = \(\frac{kt}{2.303}\)
2.303 [log [A] – log [A]] = kt
log [A0] – log [A] = \(\frac{k}{2.303}\) t.
Hence a plot of log [A] vs t gives a straight line with a negative slope having the volume of \(\frac{-k}{2.303}\)

Question 18.
Give example for first order reaction.
Answer:
(i) Decomposition of dinitrogen pentoxide
N2O5 → (g) 2NO2 (g) + \(\frac{1}{2}\) O2 (g)
(ii) Decomposition of thionylchloride;
SO2Cl2(l) → SO2 (g) + Cl2 (g)
(iii) Decomposition of the H2O2 in aqueous solution;
H2O2 (aq) → H2O (l) + \(\frac{1}{2}\) O2 (g)
(iv) Isomerisation of cyclopropane to propene.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 19.
Show that acid hydrolysis of an ester is a pseudo first order reaction.
Answer:
A second order reaction can be altered to a first order reaction by taking one of the reactant in large excess, such reaction is called pseudo first order reaction. Let us consider the acid hydrolysis of an ester,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 36
If the reaction is carried out with the large excess of water, there is no significant change in the concentration of water during hydrolysis, i.e., the concentration of water remains almost constant.
Now, we can define k [H2O] = k’ ; Therefore the above rate equation becomes
Rate = k’ [CH3COOCH3]
Thus it follows first-order kinetics.

Question 20.
Give examples of zero-order reactions.
Answer:
(i) Photochemical reaction between H2 and I2
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 37
(ii) Decomposition of N2O on a hot platinum surface
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 38
(iii) Iodination of acetone in an acid medium is zero-order with respect to iodine.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 39

Question 21.
Give the general rate equation for nth-order reaction involving one reactant A.
Answer:
The general rate equation for an nth order reaction involving one reactant [A],
A → product
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 40
Consider the case in which n ≠ 1, integration of above equation between [A0] and [A] at time t = 0 and t = t respectively gives
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 41

Question 22.
Derive an expression to calculate t1/2 for a zero-order reaction.
Answer:
Let us calculate the half life period for a zero-order reaction.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 42
The half-life of a zero-order reaction is directly proportional to the initial concentration of the reactant.

Question 23.
Give the general expression for t1/2 of the nth order (n ≠ 1) reaction.
Answer:
Half-life for an nth order reaction involving reactant A and n ≠ 1
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 43

Question 24.
Give the characteristics of first order reaction.
Answer:

  1. A change in concentration unit will not change the numerical value of ‘k’
    k = \(\frac{2.303}{t}\) log \(\frac{a}{a-x}\)
    Where ‘a’ and (a – x) are the initial concentration of the reactant and concentration of the reactant at time Y respectively. Thus for the first-order reaction, any quantity which is proportional to the concentration can be used in place of concentration to calculate ‘k’.
  2. The time taken for the completion of the same fraction of change is independent of the initial concentration.
  3. Time required to calculate nth fraction of reaction t1/2 can be calculated as When x = \(\frac{a}{n}\) ; t = t1/n
    Substituting these values in,
    TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 44
    The above equation can be used to calculate t3/4 of a reaction.
    TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 45
  4. In a first-order reaction, the amount of reactant remaining after V half-lives can be calculated as follows:TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 46
    where [A0] – initial concentration of the reactant, [A] = concentration of the reactant remaining after ‘n’ half-lives.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 25.
Calculate the half life of a first order reaction from their rate constant given below:
(a) 200 sec-1 (b) 2 min-1 (c) 4 year-1
Answer:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 47
= 3.465 x 10~3 sec
= 0.1732 year.

Question 26.
The rate constant for a first-order reaction is 60 sec. How much time will it take to reduce the initial concentration to its 1/16th value?
Answer:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 48

Question 27.
The thermal decomposition of a compound is of the first order. If 50% of the sample is decomposed in 120 minutes, how long will it take for 90% of the compound to decompose?
Answer:
Half life of the reaction = 120 min.
We know that
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 49
If a= 100, x = 90, a-x = 10
= 5.77 x 10-3 min-1
Applying first order rate equation.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 50

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 28.
Sucrose decomposes in acid solution into glucose and fructose according to the first-order rate law. With t1/2 = 3.00 hrs. What fraction of sucrose remains after 8 hours?
Answer:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 51
Therefore fraction of reactant remaining = 0.1576

Question 29.
Explain the pressure change method in determining a first-order reaction.
Answer:
If pressure is given in gaseous reactions then we use the following kinetic equation.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 52
where p0 is the pressure at the initial stage p0-x is the pressure at time ‘t’ values of p0 and x can be calculated using the following examples.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 53
Case I: If total pressure of the reaction mixture is given in place of pressure of reactants.
pt = (p0 – x + x + x + x)
Where pt is the pressure of reaction vessel at time ‘t’.
Case II: If the pressure of the reaction vessel after a long time or infinite time is given
pt = p0 + p0 +p0

Question 30.
The decomposition of Cl2O7 at 400K in the gas phase to Cl2 and O2 is a first order reaction.
(i) After 55 seconds at 400K, the pressure of Cl2O7 falls from 0.062 to 0.044 atm. Calculate the rate constant.
(ii) Calculate the pressure of Cl2O7 after 100 seconds of decomposition at this temperature.
Answer:
(i) As pressure ∝ concentration.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 54
(ii) Applying the first-order rate equation.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 55

Question 31.
For the decomposition of azo isopropanol to hexane and nitrogen at 543K, the following data are obtained.

t(sec)p (mm of Hr)
035.0
36054.0
72063.0

Calculate the rate constant for the reaction.
Answer:
The reaction is
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 56
Total pressure – p0 – x + x + x
pt = p0 + x
or x = pt – p0
a ∝ p0
∴ (a – x) ∝ p0 – (pt – p0)
= 2p0 – pt
For the first order reaction
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 57

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 32.
Explain Oswald dilution method for determining the order of the reaction.
Answer:
It is applied for these reactions which involve more than one reactant. In this method, the concentration of all reactants are taken in large excess than one. The changes in the concentration of the reactant that is not taken in excess will influence the rate of reaction.
The concentrations of all other reactants practically remain same during the course of reaction. Consider the reaction.
m1A + m2B + m3C → product
Rate = k[A]α [B]β [C]γ
When B and C are taken in excess, the rate law will reduce to
rate = k’ [A]α
where k’ = k[B]β [C]γ
Two sets are taken in which the concentration of A is [A1] and [A2] while B and C are present in large excess,
r1 = [A1]α
r2 = [A2]α
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 58
From this, the value of α, i.e., the order with respect to A is obtained. The process is repeated one by one and order with respect to others is determined.
Total order of reaction = α + β + γ

Question 33.
Show that if the concentration of a reactant is doubled, the rate of the reaction is also doubled for a first-order reaction, increases four times for a second-order reaction, increases by eight times for a third-order reaction, i.e., A → product.
Answer:
(i) If the concentration of A is doubled.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 59
Hence, for the first-order reaction, if the concentration is doubled, the rate is also doubled.
(ii) For a second-order reaction.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 60
i.e., for a second-order reaction, if the concentration of A is doubled, the rate of the reaction increases by 4 times.
(iii) For a third-order reaction,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 61
Hence, for a third-order reaction, if the concentration of the reactant is doubled the rate increases 8 times.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 34.
Compounds A and B react according to the following chemical equation
A (g) +2B(g) → 2C(g)
Answer:
The concentration of either ‘A’ or ‘B’ was changed keeping the concentration of one of the reactants constant and rates were measured as a function of initial concentration following results were obtained. Find the order with respect to A and B and write the rate law for the reaction
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 62
From experiments 1 and 3,
[B] = constant; [A] = doubled
rate is doubled.
Hence rate ∝ [A] i.e., the order with respect to A is 1.
From experiments 1, and 2,
[A] = constant; [B] doubled rate is quadrupled.
Hence, rate ∝ [B]2
i.e., order with respect by B is 2.
Combining rate = k [A] [B]2.

Question 35.
The initial rate of reactions
3A + 2B + C → products at different initial concentrations are given below.

Initial rate ms-1[A0] M[B0] M[C0] M
1) 5.0 x 10-30.0100.0050.010
2) 5.0 x 10-30.0100.0050.015
3) 1.0 x 10-20.0100.0100.010
4) 1.25 x 10-30.0050.0050.010

Answer:
(i) Consider equation (1) and (2)
The concentration of A and B are constant. The rate remains the same for different concentrations of C. Hence, the order with respect to C is zero.
(ii) Consider equations (3) and (1)
The concentration of A and C are constant. The concentration of B is doubled, rate increases by 2 times. Hence order with respect to B is 1.
(iii) Consider equations (4) and (1), The concentration of B and C remain constant. When the concentration of A is doubled, the rate increases by 4 times. Hence order with respect to A is 2.
Alternate method:
Suppose order with respect to A, B and C are α, β and γ respectively. Then the rate law at different concentration of A, B and C are
5.0 × 10-3 = k [0.010]α [0.005]β [0.010]γ …(1)
5.0 × 10-3 = k [0.010]α [0.005]β [0.015]γ …(2)
1.0 × 10-3 = k [0.010]α [0.010]β [0.010]γ …(3)
1.25 × 10-3 = k [0.005]α [0.005]β [0.010]γ …(4)
Dividing (1) by (2)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 63
i.e., order with respect to C is zero.
Dividing (3) by (2)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 64
Dividing (1) by (4) ⇒ 4 = 2α or α = 2
Order with respect to A, B, C are 2, 1 and 0.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 36.
A reaction is first order in A and second order in B.
(i) Write the differential rate equation.
(ii) How is the rate affected by increasing the concentration of B, three times, keeping the concentration of A constant?
(iii) How is the rate affected by when the concentration of both A and B are doubled?
Answer:
(i) A + B → product
rate = k [A] [B]2
(ii) If the concentration of B is tripled, the rate increases by 9 times i.e.,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 65
(iii) If the concentration of both A and B are doubled, the rate increases by 8 times.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 66

Question 37.
The following rate data were obtained at 303K for the following reaction.
2A + B → C + D.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 67
What is the order with respect to each reactant and the overall order of the reaction? write the rate law. Also, calculate the rate constant for the reaction and the units of the rate constant.
Answer:
From experiments 1 and 4, it is seen that [B] the concentration of B is the same but [A] has been made 4 times, the rate of the reaction has also become 4 times. Hence the order with respect to A is 1. i.e., rate ∝ [A],
From experiments 2 and 3, it may be noted that [A] is kept the same but [B] is doubled. The rate of reaction increases by 4 times, i.e., the order with respect to B is 2 combining both,
rate = k[A] [B]2. This is the rate law for the reaction.
Alternatively, suppose the order with respect to A is α and the order with respect to B is β, the general rate law for the reaction is
rate = k [A]α [B]β
From the data given
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 68
Now,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 69
Unit of rate constant (k)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 70
Calculation of rate constant: Substitute the values of α and β in any of the equations.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 71
Hence k = 6.0 mol-1 L2 min-1.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 38.
In a reaction between A and B, the initial rate of reaction was measured at a different initial concentration of A and B as given below.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 72
What is the order with respect to A and B?
Answer:
The general rate law is rate = k [A]α [B]β where α, β are ordered with respect to A and B respectively.
The given data is
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 73
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 74
Thus order with respect to A is 0.5 and that of B is 0.

Question 39.
The decomposition of ammonium nitrate in an aqueous solution was studied by placing the apparatus in a thermostat maintained at a particular temperature. The volume of nitrogen gas collected at different intervals of time was as follows:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 75
The above data prove that the reaction is of the first order.
Answer:
For a first-order reaction,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 76
In the present case, V = 35.05 cm3. The value of R at each instant of time can be calculated as follows:
Values of ‘k’ come nearly constant and hence the reaction is first order.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 77

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 40.
What do understand by a fraction of effective collisions? Mention its significances.
Answer:
Fraction of effective collisions (f) is given by the following expression
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 78
To understand the magnitude of collision factor (f), Let us calculate the collision factor (f ) for a reaction having an activation energy of 100 kJ mol-1 at 300K.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 79
Thus, out of 1018 collisions, only four collisions are sufficiently energetic to convert reactants to products.

Question 41.
Explain the importance of the proper orientation of molecules in the collision theory.
Answer:
Even if the reactant possesses sufficient activation energy, their collisions need not result in the formation of products. The molecules should orient themselves in such a way that their collision becomes fruit fill. The fraction of effective collisions (f) having orientation is given by steric factor (p). Thus, the rate of reaction is given by
rate = p x f x collision rate
(or) rate = pz\(e^{-\mathrm{E}_{a} / \mathrm{RT}}\)

Question 42.
Define activation energy of a reaction.
Answer:
Activation energy is the extra amount of energy that is supplied from outside so that colloiding molecules must produce effective collisions.

Question 43.
Arrhenius equation is given by k = A\(e^{-\mathrm{E}_{a} / \mathrm{RT}}\). Based on this equation answer the following questions.
(i) Can reactions have zero activation energy?
(ii) Can a reaction have negative activation energy?
Answer:
(i) k = A\(e^{-\mathrm{E}_{a} / \mathrm{RT}}\), when the expression becomes k = e° = A.
The rate constant k = collision frequency. This implies that every collision is an effective collision and leads to product formation which is not possible. Thus activation energy can not be zero.
(ii) When Ea is negative, the above equation
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 80
Rate constant having a higher value than collision frequency which is not possible.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 44.
Explain the effect of temperature on reaction rate based on Arrhenius’s theory.
Answer:
An increase in temperature increases the fraction of the total number of molecules having the necessary energy of activation which in terms increases the number of effective collisions and hence the rate.

Question 45.
Write Arrhenius equation and explain the terms? What is the significance of frequency factor A in the equation?
Answer:
The Arrhenius equation is k = A\(e^{-\mathrm{E}_{a} / \mathrm{RT}}\) Where ‘k’ is the rate constant for the reaction, A is called the pre-exponential factor, Ea is the energy of activation and R is the gas constant and T is the absolute temperature. The two quantities A and Ea are called the Arrhenius parameters.
The frequency factor gives the frequency of binary collision of the reacting molecules per liter per second. It practically remains constant and does not vary with temperature.

Question 46.
Explain how the energy of activation for a reaction is determined.
Answer:
The rate constant of a reaction is determined at two different temperatures. If R1 is the rate constant at temperature T1 arid R2 is the rate constant at temperature T2 thereby using a logarithmic form of Arrhenius equation
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 80
Ea can be calculated.

Question 47.
Describe how the energy of activation of a reaction is determined graphically.
Answer:
The Arrhenius equation is written in the form,

This equation is of the form y = mx + C i.e., equation for a straight line. Thus, if a plot of log k is \(\frac{1}{T}\) is a straight line, the validity of the equation is confirmed.
Thus the values of k at different temperatures are found and a plot of log k vs \(\frac{1}{T}\) is made.
A straight line with a negative slope is obtained from the value of the slope, Ea can be calculated.
Slope = \(\frac{-\mathrm{E}_{a}}{2.303 \mathrm{R}}\)

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 48.
The rate constant for a reaction is 1.2 x 10-3 sec at 30°C and 2.1 x 10-3 sec-1 at 40°C. Calculate the energy of activation.
Answer:
Given that k1 = 1.2 x 10-3 sec-1
T1 = 30 + 273 = 303K
k2 = 2.1 x 10-3 sec
T2 = 40 + 273 = 313K
Substituting these values in the equation
Solving Ea = 44126.3J = 44.13kJ

Question 49.
The rate of particular reaction doubles when temperature changes from 27°C to 37°C. Calculate the energy of activation.
Answer:
Given that T1 = 27°C = 273 +21 = 300K
T2 = 37°C = 273 + 37 = 310K
k2 = 2k1
Substituting these values in the equation.
This as solving for Ea
Ea = 53598.6 J mol-1 or 53.6 kJ mol-1

Question 50.
The activation energy of a reaction is 94.14 kJ mol-1 and the value of the rate constant at 313K. is 1.8 x 10-1 sec-1 . Calculate the frequency factor (A).
Answer:
Given that, Ea = 94.14 kJ mol-1 = 9414 J mol-1
T = 313K,
k = 1.8 x 10-1 sec-1 Substituting these values in
= (log 1.8 – 5)+ 15.7082
= (0.2553 – 5)+ 15.708
= 10.963J
A = Anti log (10.963 J)
= 9.194 x 10-10 sec

Question 51.
The first order rate constant for the decomposition of ethyl iodide by the reaction
C2H5I (g) → C2H4 (g) + HI (g)
at 600 K is 1.60 x 10-1 s-1. Its energy of activation is 209 kJ / mol. Calculate the rate constant of the reaction at 700K.
Answer:
Given T1 = 600 K
k1 = 1.60 x 10-5 sec-1
T2 = 700K
k2 = ?
Ea = 299 kJ mol-1 = 299000 J mol-1
Substituting these values in the equation.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

Question 52.
Rate constant ‘k’ of a reaction varies with temperature according to the equation
where Ea is the energy of activation for the reaction. When a graph is plotted for log k vs \(\frac{1}{T}\) a straight line with slope – 6670 K is obtained.
Calculate the energy of activation for the reaction and mention is units.
(R = 8.314 J k-1 mol-1)
Answer:
Slope of the line = \(\frac{-\mathrm{E}_{a}}{2.303 \mathrm{R}}\) = -6670K
Ea = 2.303 x 8.314 x 6670 = 127711.4 J mol-1

Choose the correct answers:

1. Which of the following statements is not correct about the order of reaction?
(a) The order of a reaction can be fractional.
(b) Order of reaction is an experimental quantity.
(c) The order of the reaction is always equal to the sum of the stoichiometric coefficients of reactants in a balanced chemical equation for the reaction.
(d) The order of a reaction is the sum of the powers of molar concentrations of the reactants in the rate law expression.
Answer:
(c)

2. Which of the following statements is correct?
(a) The rate of reaction decreases with the passage of time as the concentration of the reactant decreases.
(b) The rate of reaction is the same at any time during the reaction.
(c) The rate of reaction is independent of temperature change.
(d) The rate of reaction decreases with an increase in the concentration of reactants.
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

3. Which of the following expression is correct for the rate of reaction given below:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 92
Answer:
(c)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 93

4. Time required for 100 percent completion of a zero-order reaction is:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 110
Answer:
(c)

5. For the reaction aA+ bB → cC,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 94
if , then a, b and c respectively are:
(a) 3,1,2
(b) 2,1,3
(c) 1,3,2
(d) 6, 2, 3
Answer:
(c)
Hint: Dividing throughout by 3, we get
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 95
This is so for the reacting A + 3B → 2C

6. The rate of a gaseous reaction is given by the expression k [A] [B]. If the volume of the reaction vessel is suddenly reduced to 1/4th of the initial volume, the reaction rate relating to the original rate will be:
(a) 1/10
(b) 1/8
(c) 8
(d) 16
Answer:
(d)
Hint: Rate = k ab. When volume is reduced to 1/4th, concentrations will become = 4 times.
New rate = k (4a) (4b) = 16 kab = 16 times.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

7. In a reaction A → B, the rate of reaction increases two times on increasing the concentration of the reactant four times, then order of reaction is:
(a) 0
(b) 2
(c) 1/2
(d) 4
Answer:
(c)
Hint: (i) r = kaα, (ii) 2r = k(4a)α
Dividing (ii) by (i),
4α = 2 or 2 = 2 or 2α = 1 or α = 1/2.

8. The rate of the reaction 2 NO + Cl2 → 2 NOCl is given by the rate equation: rate = k[NO]2[Cl2]. The value of the rate constant can be increased by:
(a) increasing the temperature
(b) increasing the concentration of NO
(c) increasing the concentration of Cl2
(d) doing all of these
Answer:
(a)
Hint: The rate constant of a reaction depends only on temperature and does not depend upon concentrations of the reactants.

9. The unit of rate constant for a zero-order reaction is:
(a) mol L-1 s-1
(b) L mol-1 s-1
(c) L2 mol-2 s-1
(d) s-1
Answer:
(a)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 96

10. Rate constant of a reaction (k) is 175 litre2 mol-2 sec-1. What is the order of reaction?
(a) first
(b) second
(c) third
(d) zero
Answer:
(c)
Hint: On the basis of given units of k, the reaction is of 3rd order.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

11. The reaction A → B follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B?
(a) 1 hour
(b) 0.5 hour
(c) 0.25 hour
(d) 2 hours
Answer:
(a)
Hint: The fraction of A reacted in each case is same (0.2 / 0.8 = 1/4),
(0.9 – 0.675)/ 0.90 = 0.225 / 0.90 = 1/4. Hence, time taken is same.

12. 75% of the first-order reaction was completed in 32 min. 50% of the reaction was completed in:
(a) 24 min
(b) 8 min
(c) 16 min
(d) 4 min
Answer:
(c)
Hint: 75 % of reaction is completed in two half-lives, i.e., 2 x t1/2 = 32 min or t1/2 = 16 min.

13. 1/[A] vs time is a straight line. The order of the reaction is:
(a) 1
(b) 2
(c) 3
(d) 0
Answer:
(b)
Hint: log [A] vs time is linear for 1st order reactions, 1/[A] vs time is linear for 2nd order reactions; 1/[A]2 vs time is linear for 3rd order reactions.

14. If a graph is plotted between in k and 1/T for the first-order reaction, the slope of the straight line so obtained is given by:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 97
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

15. 10g of a radioactive isotope is reduced to 1.25g in 12 years. Therefore, half-life period of the isotope is:
(a) 24 years
(b) 4 years
(c) 3 years
(d) 8 years
Answer:
(b)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 98

16. The half-life period of a radioactive element is 20 days. What will be the remaining mass of 100 g of it after 60 days?
(a) 25 g
(b) 50 g
(c) 125 g
(d) 20 g
Answer:
(c)
Hint: 60 days = 3 half-lives, i.e, n = 3;
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 99

17. Activation energy of a chemical reaction can be determined by:
(a) determining the rate constant at standard temperature.
(b) determining the rate constants at two temperatures.
(c) determining the probability of collision.
(d) using catalyst.
Answer:
(b)
Hint:
Knowing k1 and k2 at T1 and T2, Ea can be determined. (Arrhenius equation)

18. According to Arrhenius equation, rate constant k is equal to A\(e^{-\mathrm{E}_{a} / \mathrm{RT}}\). Which of the following options represents the graph of k vs \(\frac{1}{T}\)?
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 100
Answer:
(a)
Hint:
k = A\(e^{-\mathrm{E}_{a} / \mathrm{RT}}\). In k = ln A – \(\frac{\mathrm{E}_{a}}{\mathrm{RT}}\). Hence, graph of In k vs \(\frac{1}{T}\) will be linear with negative slope and intercept = ln A.

19. Which of the following statement is incorrect about the collison theory of chemical reaction?
(a) It considers reacting molecules or atoms to be hard spheres and ignores their structural features.
(b) Number of effective collisions determines the rate of reaction.
(c) Collision of atoms or molecules possessing sufficient threshold energy results into the product formation.
(d) Molecules should collide with sufficient threshold energy and proper orientation for the collision to be effective.
Answer:
(c)
Hint: (c) is incorrect because the formation of the product depends not only on energy but also on proper orientation at the time or collision.

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

20. A first-order reaction is 50% completed in 1.26 x 1014 s. How much time would it take for 100% completion?
(a) 1.26 x 1015 s
(b) 2.52 x 1014 s
(c) 2.52 x 1028 s
(d) infinite
Answer:
(d)
Hint: The whole of the substance never reacts because in every half-life, 50% of the substance reacts. Hence, the time taken for 100% completion of a reaction is infinite.

21. Compounds ‘A’ and ‘B’ react according to the following chemical equation:
A (g) + 2 B(g) → 2C (g)
The concentration of either ‘A’ or ‘B’ was changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 101
(a) Rate = k [A]2 [B]
(b) Rate = k [A] [B]2
(c) Rate = k [A] [B]
(d) Rate = k [A]2 [B]0
Answer:
(b)
Hint: From expts.l and 3, [B] = constant, [A] = doubled, rate is doubled. Hence, Rate ∝ [A].
From expts. 1 and 2, [A] = constant, [B] = doubled, rate quadrupled. Hence, Rate ∝ [B]2.
Combining, Rate = k [A][B]2.

22. The rate constant of reaction A → B is 0.6 x 103 mole per liter per second. If the concentration of A is 5 M, then the concentration of B after 20 minutes is:
(a) 0.36 M
(b) 0.72 M
(c) 1.08M
(d) 3.60 M
Answer:
(b)
Hint: The unit mol L-1 s-1 of the rate constant show that it is a reaction of zero order. For a zero order reaction, x = kt. Amount of A reached (x) = (0.6 x 10-3 mol L-1 s-1 ) (20 x 60 s) = 0.72 mol L-1 [B] formed = [A] reacted = 0.72 mol L-1

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

23. The half-life of a substance in a certain enzyme-catalyzed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg L-1 to 0.04 mg L-1, is:
(a) 414 s
(b) 552 s
(c) 690 s
(d) 276 s
Answer:
(c)
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 102

24. The following data is obtained during the first-order thermal decomposition of A (g) → B (g) + C (s) at constant volume and temperature.

S. No.TimeThe total pressure in pascals
1.At the end of 10 minutes300
2.After completion200

The rate constant in min-1 is
(a) 0.0693
(b) 6.93
(c) 0.00693
(d) 69.3
Answer:
(a)

25. t1/4 can be taken as the time taken for the A concentration of a reactant to drop to its initial value. If the rate constant for a first-order reaction is k, then t1/4 can be written as:
(a) 0.10/k
(b) 029/k
(c) 0.69/k
(d) 0.75/k
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 103

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

26. A plot of log t1/2, versus log C0 is given in the adjoining fig. The conclusion that can be drawn from this graph is:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 104
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 105
Answer:
(b)

27. In the catalysed decomposition of benzene diazonium chloride,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 106
the half-life period is found to be independent of the initial concentration of the reactant. After 10 minutes, the volume of N2 gas collected is 10 L and after the reaction is complete, it is 50 L. Hence rate constant of the reaction (in min-1) is:
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 107
Answer:
(b)

28. The activation energy of a reaction can be determined from the slope of which of the following graph?
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 108
Answer:
(a)
Hint: From the Arrhenius equation,
TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics 109

29. The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:
(a) 60.5 kJ mol-1
(b) 53.6 kJ mol-1
(c) 48.6 kJ mol-1
(d) 58.5 kJ mol-1
Answer:
(b)

30. In the presence of a catalyst, the activation energy of a reaction is lowered by 2 kcal at 27°C. The rate of reaction will increase by:
(a) 2 times
(b) 14 times
(c) 28 times
(d) 20 times
Answer:
(c)

TN Board 12th Chemistry Important Questions Chapter 7 Chemical Kinetics

31. Which one of the following is not correct?
(a) Every bimolecular collision does not result into a chemical reaction.
(b) Collision theory is not applicable to unimolecular reaction.
(c) According to collision frequency, k = PZAB \(e^{-\mathrm{E}_{a} / \mathrm{RT}}\) where ZAB is collision frequency and P is steric factor.
(d) Collision theory assumes molecules to be hard spheres.
Answer:
(b)
Hint: Collision theory is applicable to unimolecular reactions also.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Students get through the TN Board 12th Chemistry Important Questions Chapter 6 Solid State which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 6 Solid State

Answer the following questions.

Question 1.
Why are solids rigid?
Answer:
In solids, the constituent particles (atoms, molecules, or ions) are not free to move but can only oscillate about their mean position due to strong interatomic or intermolecular forces. This imparts rigidity.

Question 2.
Classify the following as amorphous or crystalline solids.
Answer:
Polyurethane, naphthalene, benzoic acid Teflon, potassium nitrate, cellophane, polyvinyl chloride fiberglass, copper.
Amorphous solids: Polyurethane, Teflon, cellophane, polyvinyl chloride, and fiberglass. Crystalline solids: Naphthalene, benzoic acid, potassium nitrate, and copper.

Question 3.
Explain why glass is considered an amorphous solid.
Answer:
Like liquids, it has a tendency to flow, though very slowly. It does not have a sharp melting point. It is isotropic.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 4.
Classify the following solids in different categories based on the nature of intermolecular forces operating in potassium sulfate, tin, benzene, urea, ammonia water, zinc sulfide, graphite, rubidium, argon, silicon carbide.
Answer:
Ionic solids: potassium sulfate, zinc sulfide. Covalent solids: graphite, silicon carbide. Molecular solids: benzene, urea, ammonia water, argon.
Metallic solids: rubidium, tin.

Question 5.
Ionic solids conduct electricity in the molten state but not in the solid state. Explain.
Answer:
In ionic solids, free ions are present in a molten state and they move towards the oppositely charged electrode under the influence of electric current. In a solid state, these ions are fixed in their lattice position and cannot move under the influence of electric current.

Question 6.
Briefly outline the properties of covalent solids.
Answer:

  1. They have a high melting point.
  2. They are poor thermal and electrical conductors.

Question 7.
What are covalent solids? Give example.
Answer:
In covalent solids, the constituents (atoms) are bound together in a three-dimensional network entirely by covalent bonds. eg; Diamond, silicon carbide, etc.

Question 8.
What are molecular solids? Give examples.
Answer:
In molecular solids, the constituents are neutral molecules. They are held together by weak Van der Waals forces. Generally, molecular solids are soft and they do not conduct electricity, eg: I2, graphite.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 9.
Explain various types of molecular solids for example.
Answer:
Molecular solids are classified into (i) non-polar molecular solids, (ii) polar molecular solids, (iii) hydrogen-bonded molecular solids.

  1. In nonpolar molecular solids, the constituent molecules are held together by weak dispersion or London forces, eg: naphthalene, anthracene.
  2. In polar molecular solids, the constituent molecules are formed by polar covalent bonds, eg solid CO2, solid NH3.
  3. In hydrogen-bonded molecular solids, the constituent molecules are held together by hydrogen bonds, eg: ice (H2O), glucose, urea, etc.

Question 10.
Explain the types of the force of attraction that exist (i) nonpolar molecular solids, (ii) polar molecular solids, (iii) hydrogen-bonded molecular solids.
Answer:

  1. In non-polar molecular solids, the constituent particles are held together by weak dispersion or London forces.
  2. In polar molecular solids, the constituent molecules are held by covalent bonds. They are attracted to each other by relatively strong dipole-dipole attraction.
  3. In hydrogen-bonded molecular solids, the molecules are held together by hydrogen bonds.

Question 11.
What are the characteristics of metallic solids? What type of attractive forces exists among the constituent particles?
Answer:
The constituents of a metallic solid are held together by a metallic bonding. The lattice points are occupied by metals ion and the electron’s charge bond encloses the metal ion.
They are hard, possess a high melting point, They conduct heat and electricity. They possess metallic luster.

Question 12
Give examples for metallic solids.
Answer:
Metal and metal alloys, eg: Cu, Fe, Zn, Ag, Au, Cu, Zn, etc.

Question 13.
Define the following: (i) Lattice point, (ii) Crystal lattice, (iii) Unit cell.
Answer:

  1. Lattice point: Each lattice point represents one constituent particle of a solid. This may be an atom, molecule, or ion.
  2. The crystal lattice is a three-dimensional arrangement of identical points in the space which represents how the constituent particles (atoms, molecules, or ions) are arranged in a crystal.
  3. Unit cell A unit cell is the smallest portion of a space lattice which when repeated in different directions generates the entire lattice.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 14.
What are the characteristics of a unit cell?
Answer:
A unit cell is characterized by the three edge lengths or lattice constants a, b, and c and the angle between the edges α, β, and γ.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 1

Question 15.
Briefly explain how constituent particles are arranged in (i) simple cubic, (ii) body-centered cubic, and (iii) face-centered cubic unit cells.
Answer:

  1. In the simple cubic unit cell, each comer is occupied by identical atoms or ions or molecules. And they touch along the edges of the cube, do not touch diagonally. The coordination number of each atom is 6.
  2. In a body-centered cubic unit cell, each comer is occupied by an identical particle, and in addition to that one atom occupies the body center. Those atoms which occupy the comers do not touch each other, however, they all touch the one that occupies the body center. Hence, each atom is surrounded by eight nearest neighbors and the coordination number is 8.
  3. In a face-centered cubic unit cell, identical atoms lie at each comer as well as in the center of each face. Those atoms in the comers touch those in the faces but not each other. The coordination number is 2.

Question 16.
Distinguish between primitive and nonprimitive unit cells.
Answer:

Primitive unit cellsNonprimitive unit cells
A unit cell that contains one lattice point is called a primitive unit cell. In a primitive unit cell, constituent particles are present only at the comers of a unit cell.In the nonprimitive unit cells, the constituent particles are present not only at the comer but also in the centers of the face and body of the unit cell.

Question 17.
Define coordination number? What is the coordination number of each constituent particle present at (i) simple cubic, (ii) body-centered cubic, and (iii) face-centered cubic unit cells?
Answer:
The number of constituent particles that surround an atom/ion in a crystal lattice is called the coordination number.

  1. The coordination number of each atom in a simple cubic unit cell is 6.
  2. The coordination number of each atom in a body-centered cubic unit cell is 8.
  3. The coordination number of an atom is a face-centered cubic unit cell is 2.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 18.
Explain how will you calculate the number of particles in a unit cell.
Answer:

  1. A point that lies at the comer of a unit cell is shared among the eight-unit cells and therefore, only one eight (\(\frac{1}{8}\)th) of each point lies within the unit cell.
  2. A point along the edge is shared by 4 unit cells and only \(\frac{1}{4}\)th of it lies within any one cell.
  3. A face-centered point is shared by 2 unit cells and only \(\frac{1}{2}\) of it is present in a given unit cell.
  4. A body-centered point lies entirely within the unit cell and contributes one complete point to the cell.
    TN Board 12th Chemistry Important Questions Chapter 6 Solid State 2
    Total number of particles in an unit cell (z) = (\(\frac{1}{8}\) × occupied by corners) + \(\frac{1}{4}\) × (occupied by edge centres) + \(\frac{1}{2}\) × (occupied by 24 face centres) + one occupied by body centre.

Question 19.
Calculate the number of particles present in (i) simple cubic (ii) body-centered and (iii) face-centered unit cells.
Answer:

  1. In simple cubic unit cell particles are present only at the comers of the cube and this is shared by 8 other unit cells. Hence, the contribution of the point at the comers to the given unit cell is
    ∴ Z = 8 × \(\frac{1}{8}\) = 1
    i.e, A simple cubic unit cell has a single constituent (atom/molecule/ion) unit per unit cell.
  2. In the body-centered cubic unit cell, comers, as well as the center of the unit cell, are occupied.
    ∴ Z = 8 × \(\frac{1}{8}\) + 1 = 2
    Hence body-centered cubic (bcc) has 2 constituent units per unit cell.
  3. In face-centered cubic unit cell (fee) comers as well as face centers are occupied.
    ∴ Z = 8 × \(\frac{1}{8}\) + 6 + 2 = 4
    Hence, the face-centered cubic unit cell has four constituent units per unit cell.
    [Note: Remember that the number of atoms per unit cell is in the same ratio as the stoichiometry of the compound. Hence, it helps to predict the formula of the compound.]

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 20.
A compound formed by elements A and B has a cubic structure in which A atoms are at the comers and B atoms are at face centers. Derive the formula of the compound.
Answer:
As ‘A’ atoms are present at the 8 comers of the cube, therefore a number of atoms of A in the unit cell = 8 × \(\frac{1}{8}\) = 1.
As ‘B’ atoms are present at the face centers of the 6 faces of the cube, therefore, the number
of atoms of B in the unit cell = \(\frac{1}{2}\) × 6 = 3.
∴ Ratio of atoms A : B = 1 : 3
∴ The formula of the compound is AB3.

Question 21.
A cubic solid is made up of two elements X and Y. Atoms ‘Y’ are present at the comers of the cube and atoms X at the body center. What is the formula of the compound? What are the coordination numbers of X and Y?
Answer:
As Y atoms are present at 8 comers, of the cube, the number of atoms of Y in the unit cell
= \(\frac{1}{8}\) × 8 = 1
As atoms X are present at the body center, therefore, the number of atoms of X in the unit cell = 1.
∴ Ratio of atoms X : Y = 1 : 1
Hence the formula of the compound is XY.
The coordination number of each X and Y = 8.

Question 22.
A compound formed by elements X and Y crystallizes in the cubic structure where Y atoms are at the comers of the cube and X atoms are at alternate faces. What is the formula of the compound?
Answer:
As there are 8 Y atoms are at the comers of the cube and the contribution of each
= \(\frac{1}{8}\) therefore no. of Y atoms per unit cell
= 8 × \(\frac{1}{8}\) = 1
These can only be 2 × atoms an alternate forces.
As contribution of each of them = \(\frac{1}{2}\).
Therefore number of X atom per unit cell
= 2 × \(\frac{1}{2}\) = 1
Ratio of atom X : Y = 1 : 1
Hence the formula of the compound is 1 : 1

Question 23.
Give the expression to find out the inter planar distance (d) between two successive planes of atoms.
Answer:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 3
Where n is the number of planes,
λ is the wavelength of X-ray used,
θ is the angle of diffraction.
Using these values, the edge of the unit cell can be calculated.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 24.
X-rays of wavelength 1.54Å strike a crystal and are observed to be deflected at an angle of 22.5°. Assuming that n = 1, calculate the spacing between the planes of atoms that are responsible for this reflection.
Answer:
Applying Bragg equation,
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 4

Question 25.
Derive an expression to find the density of a crystal from lattice parameters.
Answer:
Using the edge length of a unit cell, we can calculate the density (ρ) of the crystal by considering a cubic unit cell as follows.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 5
substitute (3) in (2)
mass of the unit cell = n × \(\frac{\mathrm{M}}{\mathrm{N}_{\mathrm{A}}}\) …(4)
For a cubic unit cell, all the edge lengths are equal i.e, a = b = c
Volume of the unit cell = a × a × a = a3 …(5)
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 6
Equation (6) contains four variables namely ρ, n, M, and a. If any three variables are known, the fourth one can be calculated.

Question 26.
The edge length of a unit cell is 408 pm. Its density is 10.6 g cm-3. Predict whether the metal is body-centered, or face-centered, or simple cubic.
Answer:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 7
The value of Z indicates that the metal has a fee structure.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 27.
An element crystallizes in bcc structure the edge length of its unit cell is 288 pm. The density of the crystal is 7.2g cm-3. What is the atomic mass of the element?
Answer:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 8

Question 28.
A metallic element exists as a body-centered cubic lattice. Each edge of the unit cell is 2.88 pm. The density of the metal is 7.2g cm-3. How many atoms and unit cells are there in 100 g of the atom?
Answer:
Let the atomic mass of the element be M.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 9

Question 29.
The density of a face-centered cubic clement is 6.25 g cm-3. Calculate the length of the unit cell. (Atomic mass of the element = 60.2 AMU).
Answer:
Given Z = 4; M = 60.2 amu; ρ = 625 g cm-3
NA = 6.023 × 1023
Applying the formula:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 10

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 30.
KBr has NaCl type structure. What is the distance between K+ and Br in KBr, if the density is 2.75 g cm-3?
Answer:
Edge length ‘a’ of the unit cell is calculated as
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 11

Question 31.
Derive an expression to calculate the packing efficiency in a simple cubic arrangement.
Answer:
Let us calculate the packing efficiency in simple cubic arrangement,
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 12
Let us consider a cube with an edge length ‘a’ as shown in fig.
Volume of the cube with edge length a is = a × a × a = a3
Let V is the radius of the sphere. From the figure, a = 2r ⇒ r = \(\frac{a}{2}\)
∴ Volume of the sphere with radius ‘r’
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 13
In a simple cubic arrangement, the number of spheres that belongs to a unit cell is equal to one
∴ Total volume occupied by the spheres in sc unit cell = 1 × \(\left(\frac{\pi a^{3}}{6}\right)\) ……(2)
Dividing (2) by (3)
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 14
i.e., only 52.31% of the available volume is occupied by the spheres in simple cubic packing, making inefficient use of available space and hence minimizing the attractive forces.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 32.
Show that the packing efficiency in the face-centered cubic unit cells is 74%.
Answer:
The cubic close packing is based on the face-centered cubic unit cell. Let us calculate the packing efficiency in the fcc unit cell.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 15
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 16
The total number of spheres belongs to a single fcc unit cell is 4
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 17

Question 33.
Give the relationship between the nearest neighbor distance (d) and the edge (a) of the unit cell of a cubic crystal.
Answer:
For simple cubic: d = a
For face centered cubic: d = \(\frac{a}{\sqrt{2}}\) = 0.707a
For body centered cubic:
d = \(\frac{\sqrt{3}}{2} a\)

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 34.
Give the relationship between atomic radius (r), (which is d/2 for crystals of pure substances) and edge (a) of the unit cell of a cubic crystal.
Answer:
For simple cubic: r = \(\frac{a}{2}\)
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 18

Question 35.
Xenon crystallizes in face-centered cubic lattice and the edge of the unit cell is 620 pm. What is the nearest neighbor distance and what is the radius of the xenon atom?
Answer:
Here, a = 620 pm; d = 2 ; r = ?
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 19

Question 36.
CsCl has bcc arrangement and its unit cell edge length is 400 pm. Calculate the interionic distance in CsCl.
Answer:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 20
The bcc arrangement of CsCl is shown in fig. Where black circle is Cs+ ion and colored circles are Cl ions. The aim is to find half of the body diagonal AE. If the edge of the unit cell is ‘a’.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 21

Question 37.
If the radius of the atom is 75 pm and the lattice type is body-centered cubic, what is the edge of the unit cell?
Answer:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 22

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 38.
The radius of an atom of an element is 500 pm. If it crystallizes as fee lattice, what is the length of the side of the unit cell?
Answer:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 23

Question 39.
A solid AB has a CsCl type structure. The edge length of the unit cell is 404 pm. Calculate the distance of the closest approach between A+ / B ions.
Answer:
The distance of the closest approach is equal to the distance between nearest neighbors (d). As CsCl has a bcc lattice.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 24

Question 40.
What is the radius ratio? Mention its importance.
Answer:
In ionic solids, the ratio of the radius of the cation to the radius of an anion is known as the radius ratio.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 25
The radius ratio of an ionic solid gives the structural arrangement of ionic solids.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 26

Question 41.
What is the meaning of the term imperfection in solids?
Answer:
Imperfection refers to the departure from the perfect periodic arrangement of atoms, ions, or molecules in the structure of crystalline solids.

Question 42.
What are the types of lattice imperfections found in crystals?
Answer:

  1. Stoichiometric defect i.e., Schottky defect and Frenkel defect.
  2. Nonstoichiometric defect viz metal excess, metal deficiency, and impurity defects.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 43.
What are interstitials in a crystal?
Answer:
Atoms or ions that fill the normal vacant interstitial voids in a crystal are known as interstitials.

Question 44.
What is the Schottky defect?
Answer:
If an equal number of cations and anions are missing from their lattice sites, the defect is known as the Schottky defect.

Question 45.
What is Frenkel’s defect?
Answer:
When some ions (usual cation) are missing from the lattice sites and they occupy the interstitial sites. So that, the electro-neutrality, as well as stoichiometry are maintained, it is called Frenkel defect.

Question 46.
Which crystal defect lowers the density of the solid?
Answer:
Schottky defect.

Question 47.
Which crystal defect in crystals does not alter the density of a relevant solid?
Answer:
Frenkel defect.

Question 48.
Which point does defect increase the density of the solid?
Answer:
Schottky defect.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 49.
Which point defect in the crystal increases the density of the solid?
Answer:
Interstitial defect.

Question 50.
Name one solid in which both Frenkel and Schottky defects occur.
Answer:
Silver Bromide.

Question 51.
Why does the Frenkel defect does not change the density of AgCl crystal?
Answer:
Because in Frenkel defect, no ion is missing from the lattice sites. Therefore, no change in density occurs.

Question 52.
What are F. Centres?
Answer:
The free-electron trapped in the anion vacancy is called F.Centres.

Question 53.
What are non-stoichiometric defects?
Answer:
If as a result of imperfections in the crystal, the ratio of the cation to the anions becomes different from that indicated by their ideal chemical formula, then the defect is termed a non-stoichiometric defect.

Question 54.
Why does table salt, NaCl appear yellow in color?
Answer:
Yellow color in sodium chloride is due to metal excess defect due to which unpaired electrons occupy anionic sites. These sites are called F. Centres. These electrons absorb energy from the visible region for excitation which makes the crystal yellow.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 55.
Why is FeO (s) not formed in stoichiometric composition?
Answer:
In the crystal of FeO, some of Fe+2 cations are replaced by Fe+3 cations. Three Fe+2 cations are replaced by two Fe+3 cations to make up for the loss of positive charge. Eventually, there would be fewer atoms of the metal as compared to stoichiometric proportion.

Question 56.
How would you account for the following?

  1. Frenkel defects are not found in alkali metal halides.
  2. Schottky defects lower the density of the solid.
  3. Impurity doped silicon is a semiconductor.

Answer:

  1. This is because alkali metal ions have larger sizes that cannot fit into interstitial sites.
  2. As the number of ions decreases as a result of the Schottky defect, the mass decreases whereas the volume remains the same.
  3. This is due to additional electrons or the creation of holes and doping with impurity. Creation of hole results in p-type semiconductor and creation of electron results in the n-type semiconductor.

Question 57.
Briefly explain the metal excess defect.
Answer:
The metal excess defect arises due to the presence of more metal ions as compared to anions. Alkali metal halides NaCl, KCl show this type of defect. The electrical neutrality of the crystal can be maintained by the presence of anionic vacancies equal to the excess metal ions (or) by the presence of extra cation and electrons present in the interstitial position.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

Question 58.
Briefly explain metal deficiency defects.
Answer:
Metal deficiency defect arises due to the presence of fewer cations than the anions. This defect is observed in a crystal in which, the cations have variable oxidation states.

Question 59.
Briefly explain the impurity defect.
Answer:
A general method of introducing defects in ionic solids is by adding impurity ions. If the impurity ions are in a different valance states from that of the host, vacancies are created in the crystal lattice of the host. For example, the addition of CdCl2 to silver chloride yields solid solutions where the divalent cation Cd2+ occupies the position of Ag+. This will disturb the electrical neutrality of the crystal. In order to maintain the same, a proportional number of Ag+ ions leaves the lattice. This produces a cation vacancy in the lattice, such kinds of crystal defects are called impurity defects.

Choose the correct answer.

1. Which one of the following is a covalent crystal?
(a) Rock salt
(b) Ice
(c) Quartz
(d) Dry ice
Answer: (c)
Hint: Rock salt is an ionic solid, while dry ice and ice are molecular solids.

2. Total volume of atoms present in a face centered cubic unit cell of a metal is:
(r = atomic radius)
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 29
Answer: (b)
Hint: Total no. of atoms in fee unit cell = 4
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 30

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

3. The fraction of the total volume occupied by the atoms present in a simple cube is:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 31
Answer: (b)
In a simple cube, no. of atoms / unit cell = 8 × \(\frac{1}{8}\) = 1
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 32

4. Three elements A, B and C crystallise into a cubic solid lattice. Atoms A occupies the comers, B atoms, the cubic centres, and atoms C, the edges. The formula of the compound is:
(a) ABC
(b) ABC2
(c) ABC3
(d) ABC4
Answer: (c)
Hint:
Atoms A per unit cell = 8 × \(\frac{1}{8}\) = 1
Atom B per unit cell = 1
Atoms C per unit cell = 12 × \(\frac{1}{4}\) = 3
Ratio A : B : C = 1 : 1 : 3.
Hence the formula is ABC3.

5. An alloy of copper, silver and gold is found to have copper forming the simple cubic close packed lattice. If silver atoms occupy the comers and gold atoms are present at the body centres, the formula of the alloy will be:
(a) Cu3 Ag Au
(b) Cu Ag3 Au
(c) Cu4 Ag2 Au
(d) Cu Ag Au.
Answer: (b)
Hint:
Cu atoms per unit cell (present at the comer) = 8 × \(\frac{1}{8}\) = 1
Ag atoms per unit cell (present at the face centres) = 6 × \(\frac{1}{2}\) = 3
Au atoms per unit cell (present at body centre) = 1
Hence the formula is Cu Ag3 Au.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

6. A solid compound XY has NaCl structure. If the radius of the cation is 100 pm, the radius of the anion (Y) will be:
(a) 275.1 pm
(b) 322.5 pm
(c) 241.5 pm
(d) 165.7 pm
Answer: (c)
Hint: NaCl has a face centered cubic structure. Cl ions and Na+ ions are present in the octahedral voids. Hence for such a solid, radius of the cation is = 0.414 × radius of the anion.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 33

7. The number of atoms in 100g of the fcc crystal with density = 10 g/cm3, and the cell edge equal to 200 pm is equal to:
(a) 5 × 1024
(b) 5 × 1025
(c) 6 × 1023
(d) 2 × 1025
Answer:
(a)
Hint:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 34
Thus 12g of the atom contain = 6.023 × 1023 atom.
∴ 100g of the atom will contain
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 35

8. Which of the following statements is not true about amorphous solids?
(a) On heating they may become crystalline at certain temperature.
(b) They may become crystalline or keeping for long time.
(c) Amorphous solids can be moulded by heating.
(d) They are anisotropic in nature.
Answer:
(d)

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

9. The sharp melting point of crystalline solids is due to:
(a) a regular arrangement of constituent particles observed over a short distance in the crystal lattice.
(b) a regular arrangement of constituent particles observed over a long distance in the crystal lattice.
(c) same arrangement of constituent particles in different directions.
(d) different arrangement of constituent particles in different directions.
Answer:
(b)

10. Iodine molecules are held in the crystal lattice by:
(a) London forces
(b) dipole – dipole interaction
(c) covalent bonds
(d) columbic forces
Answer:
(a)

11. Which of the following is a network solid?
(a) SO2 (solid)
(b) I2
(c) diamond
(d) H2O (ice)
Answer:
(c)

12. Which of the following solids is not an electrical conductor?
(i) Mg(s)
(ii) TiO(s)
(iii) I2 (s)
(iv) H2O (ice)
(a) (i) only
(b) (ii) only
(c) (iii) and (iv)
(d) (ii), (iii) and (iv)
Answer:
(c)

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

13. The lattice sites in a pure crystal cannot be occupied by:
(a) molecule
(b) ion
(c) electron
(d) atom
Answer:
(c)
Hint: Electrons can occupy only in the interstitial sites.

14. Cations are present in interstitial sites in:
(a) Frankel defect
(b) Schottky defect
(c) Valency defect
(d) Metal deficiency defect
Answer:
(a)

15. Schottky defect is obtained in crystal when:
(a) Some cations move from their lattice sites to interstitial sites.
(b) equal number of cations and anions are missing from the lattice.
(c) Some lattice sites are occupied by electrons.
(d) Some impurity is present in the lattice.
Answer:
(b)

16. The total number of tetrahedral void in the face centered unit cell is:
(a) 6
(b) 8
(c) 10
(d) 12
Answer:
(b)
Hint: No. of atoms per unit cell in fee = 4
No. of tetrahedral void: 2 × 4 = 8.

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

17. Which of the following statements is not true about hexagonal close packing?
(a) The coordination number is 12.
(b) It has 74% packing efficiency.
(c) Tetrahedral voids of the second layer are covered by spheres of the third layer.
(d) In this arrangement spheres of the fourth layer are exactly aligned with those of the first.
Answer: (d)
Hint: In hcp arrangement ABAB type and not ABC ABC type. Hence (d) is not true.

18. What is the coordination number in square close packed structure in two dimensions?
(a) 2
(b) 3
(c) 4
(d) 6
Answer:
(c)
Hint: The arrangement is AA AA type. In this arrangement each sphere is touching four other spheres touching the particular sphere, a square is formed. Hence, the coordination number is 4.

19. The correct order to packing efficiency in different type of unit cells is:
(a) fee < bee < simple cubic
(b) fee > bcc > simple cubic
(c) fee < bcc > simple cubic
(d) bcc < fee > simple cubic
Answer:
(b)
Hint: fcc = 74%, bcc = 68%; simple cubic = 52.4%

20. In cubic close packing, the unit cell has:
(a) 4 tetrahedral voids each of which is shared by adjacent unit cells. .
(b) 4 tetrahedral voids within the unit cell.
(c) 8 tetrahedral voids each of which is shared by four adjacent unit cells.
(d) 8 tetrahedral voids within the unit cells.
Answer:
(d)
Hint: ccp = hcp
No. of atoms per unit cell in fcc unit cell = 4.
∴ No. of tetrahedral voids = 2 × 4 = 8

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

21. KCl crystallises in the same type of lattice as does NaCl.
Given that \(r_{\mathrm{Na}^{+}} / r_{\mathrm{Cl}^{-}}\) is 0.55 and \(r_{\mathrm{K}^{+}} / r_{\mathrm{Cl}^{-}}\) is 0.74, Calculate the ratio of the side of the unit cell of KCl and NaCl.
(a) 1.123
(b) 0.891
(c) 1.414
(d) 0.414
Answer:
(a)
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 36

22. Ice crystallises in a hexagonal lattice having a volume of the unit cell is 132 × 10 cm3. It density of ice at the given temperature is 0.92 g cm-3, then number of H2O molecules per unit cell is:
(a) 1
(b) 2
(c) 3
(d) 4
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 37

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

24. The edge length of the face-centered cubic unit cell is 508 pm. If the radius of the cation is 110 pm, the radius of the anion will be:
(a) 144 pm
(b) 288 pm
(c) 618 pm
(d) 398 pm
Answer:
(a)
Hint: For the face-centered cubic unit cell (eg: NaCl),
the edge length = 2 × distance between cation and anion
= 2 (r+ + r)
2(r+ + r) = 508 pm
given r+ = 110 pm
2(110 + r) = 508 pm
r = 144 pm

25. Which of the following statements is not correct?
(a) The fraction of the total volume occupied by the atoms in a primitive cell is 0.48
(b) Molecular solids are generally volatile.
(c) The number of carbon atoms in a unit cell of a diamond is 4.
(d) The number of brave lattices in which a crystal can be categorized it.
Answer:
(c)

26. Match the entities with a column I with appropriate entities in column II and choose the correct option using the code given.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 38
(a) (A) – r; (B) – p, r, s; (C) – r, (D) – q
(b) (A) – p,r; (B) – s; (C) – r; (D) – q
(c) (A) – r; (B) – p,s; (C) – q; (D) – r
(d) (A) – r, (B) – s; (C) – r; (D) – p
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

27. Match the entities with column I with appropriate entities in column II and choose the correct option using the code given.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 39
a = cell edge
d = nearest neighbour distance
r = radius
(a) (A) – q; (B) – r; (C) – p; (D) – s
(b) (A) – q; (B) – p; (C) – r; (D) – 5
(c) (A) – q; (B) – s; (C) – q; (D) – p
(d) (A) – q; (B) – s; (C) – r; (D) – p
Answer:
(c)

28. Match the entities with column I with appropriate entities in column II and choose the correct option using the code given.
TN Board 12th Chemistry Important Questions Chapter 6 Solid State 40
(a) (A) – s; (B) – q; (C) – r; (D)-p
(b) (A) – q; (B) – p; (C) – r; (D) – s
(c) (A) – r; (B) – s; (C) – q; (D) – p
(d) (A) – s; (B) – r; (C) – p; (D) – q
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 6 Solid State

29. Assertion (A): Hexagonal close packing is more closely packed than cubic close packing.
Reason (R): Hexagonal close-packing has a coordination number 12 whereas the cubic close packing has a coordination number 8.
(a) If both assertion and reason are true and the reason is the correct explanation of assertion.
(b) If both assertion and reason are true, and the reason is not the correct explanation of assertion.
(c) If the assertion is true but the reason is false.
(d) If both assertion and reason are false.
Answer:
(d)
Hint:
Correct assertion: Hexagonal close packing and cubic close packing are equally close-packed with a packing efficiency of 74%.
Correct reason: Both have the coordination number 12.

30. Assertion (A): Frankel defects are shown by silver halides.
Reason (R): Ag+ ion is smaller in size.
(a) If both assertion and reason are true and the reason is the correct explanation of assertion.
(b) If both assertion and reason are true, and reason is not the correct explanation of assertion.
(c) If the assertion is true but the reason is false.
(d) If both assertion and reason are false.
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Students get through the TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Answer the following questions.

Question 1.
What is the coordination number of the central metal ions in the following complexes?
(i) [Cu(NH3)4]+2
(ii) [Fe(C2O4)3]-3
(iii) [Pt (en)2Cl2]
(iv) [Mo(CN)8]-4
(v) Fe[EDTA]]
(vi) [Pd(H2O)2(ONO)2I2]
Answer:
(i) NH3 is a monodentate ligand.
Point of attachment with Cu+2 = 4 x 1 = 4
C.N of Cu+2 = 4
(ii) C2O4-2 is bidentate ligand.
Point of attachment with Fe+3 = 3 x 2 = 6
C.N of Fe+3 = 6
(iii) ‘en’ is a bidentate ligand and Cl is a monodentate ligand.
Point of attachment with
Pt+2 = 2 x 2 + 2 x 1 = 6
C.N of Pt+2 = 6
(iv) CN is a monodentate ligand.
Point of attachment with Mo+4 = 8 x 1 = 8
C.N of Mo+4 = 8
(v) EDTA is a hexadentate ligand.
Point of attachment with Fe+2 = 6 x 1 = 6
C.N of Fe+2 = 6
(vi) Point of attachment with
Pd+4 = 2 x 1 + 2 x 1 + 2 x 1 = 6
C.N of Pd+2 = 6

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 2.
Calculate the oxidation state, of the central metal atom, in the following:
(i) [CO(NH3)5Cl]+2
(ii) K4[Fe(CN)6]
(iii) [Co(NO2)2(Py)2(NH3)2] NO3
(iv) Ni[CO]4/
(v) [Fe(EDTA)]
Answer:
(i) x + 5 × (0) – 1 = + 2
x = 2 + 1 = 3
oxidation state of cobalt = +3
(ii) 4 × (+1) + x + 6 (-1) = 0
x = +6 – 4 = +2
oxidation state of Iron = + 2.
(iii) x + 2 (-1) + 2(1) + 2(0) – 1 = 0
x = 2 + 1 = 3
oxidation state of cobalt = +3
(iv) x + 4 (0) = 0 or x = 0:
oxidation State of nickel = 0
(v) x + 1 × x (-4) = -1
x = 4 – 1 = +3
oxidation state of Iron = +3

Question 3.
Give the IUPAC names of the following compounds:
(i) K3[Al(C2O4)3]
(ii) [Pt(NH3)4(NO2)Cl] SO4
(iii) K3[Cr(CN)6]
(iv) [CO(NH3)5ONO]Cl2
(v) [Cr(NH3)5CO3]Cl
(vi) [Cr(NH3)5 (NCS)][ZnCl4]
(vii) K[Au(CN)2]
Answer:
(i) Pottasium trioxalatoalurhinate (III)
(ii) Tetraamminechloridonitroplatinum (IV) sulphate.
(iii) Potassiumhexacyanochromate (III)
(iv) Pentaammine nitritocobalt (III) chloride.
(v) Pentaammine carbonate chromium (III) chloride.
(vi) Pentaammine isothiocyanato chromium (III) chloride.
(vii) Potassium dicyanoaurate (I).

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 4.
Write the formula of the following co-ordination compounds.
(i) Tetraammine diaqua cobalt (III) chloride.
(ii) Potassium tetracyano nickelate (II).
(iii) Tris (ethane 1,2, diamine) chromium (III) chloride.
(iv) Amminebromidochloridonitrito-N- platinate (III).
(v) Dichlorido bis (ethane 1, 2, diamine) platinum (IV) nitrate.
(vi) Iron (III) hexacyanoferrate (III).
Answer:
(i) [Co(NH3)4(H2O)2]Cl3
(ii) K2[Ni(CN)4]
(iii) (Cr (en)3]Cl3
(iv) [Pt(NH3)Br Cl (NO2)]‘-
(v) [Pt Cl2 (en)2] (NO2)2
(vi) Fe4(Fe(CN)2]3

Question 5.
Write the IUPAC names of the following
co-ordination compounds:
(i) [Co(NH3)6]Cl3
(ii) [Co(NH3)5Cl]Cl2
(iii) K3[Fe(CN)6]
(iv) K3[Fe (C2O4)3]
(v) K2[Pd Cl4]
(vi) Pt [(NH3)2 Cl (NH2CH3)]Cl.
Answer:
(i) Hexaammine cobalt (III) chloride.
(ii) Pentaammine chloridocobalt (III) chloride.
(iii) Potassium hexacyano ferrate (III).
(iv) Potassium trioxalato ferrate (III).
(v) Potassium tetrachlorido palladate (II).
(vi) Diammine chlorido (methylamine) platinum (II) chloride.

Question 6.
Using IUPAC names, write the formula of the following:
(i) Tetra hydrazozincate (II)
(ii) Hexaammine cobalt (III) sulphate.
(iii) Potassium trioxalato chromate (III)
(iv) Diammine dichlorido platinum (II)
(v) Tetra bromido cuprate (II)
(vi) Pentaamine nitrito-O-cobalt (III)
(vii) Pentaamine nitrito-N-cobalt (III)
Answer:
(i) [Zn(OH)4]-2
(ii) [CO(NH3)6]2SO4
(iii) K3[Cr (C2O4)3]
(iv) [Pt(NH3)2Cl2]
(v) [Cu Br4]-2
(vi) [CO(NH3)5 (ONO)]+2
(vii) [CO(NH3)5NO2]+2

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 7.
Specify the oxidation numbers of the metal ions in the following coordination entities.
(i) [CO(H2O) (CN) (en)2]+2
(ii) [Pt Cl4]-2
(iii) [Cr(NH3)3 Cl3]
(iv) [Co Br2 (en)2]+
(v) K3[Fe(CN)6]
Answer:
(i) x + 0 + (-1) + 0 = + 2; x = +3
(ii) x – 4 = – 2 ; or x = +2
(iii) x + 0 + 3(-1) = 0; x = +3
(iv) x – 4 = -2 or x = +2
(v) 3(1) + x + 6(-1) = 0; or x = +3

Question 8.
Aqueous copper sulphate (blue in colour) gives (i) a green precipitate with aqueous potassium fluoride and (ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.
Answer:
Aqueous copper sulphate exists as [Cu(H2O)4] SO4. It is a labile complex. The blue colour is due to [Cu(H2O)4]+2 ions.
(i) When KF is added, weak H2O ligands are replaced by F ligands forming [CuF4]-2 ions which is a green precipitate.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 1
(ii) When KCl is added, Cl ligands replaced by weak H2O ligands forming [CuCl4]-2 ion which has a bright green colour.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 2

Question 9.
Give two examples for each of the following:
(i) Cationic complex
(ii) Anionic complex
(iii) Neutral complex
Answer:
(i) [Ag(NH3)2]+, [Co(NH3)6]+3
(ii) [Co (CN)6]-3, [Fe(CN)6]-4
(iii) [Ni(CO)4], [CO(NH3)3 Cl3]

Question 10.
What are homoleptic and heteroleptic complexes? Give one example for each.
Answer:
A coordination compound in which the central metal atom / ion is co-ordinated to only one kind of ligand is called homoleptic complex. Examples (Co(NH3)6]+3, [Fe(H2O)6]+3.
A coordination compound in which the central metal atom / ion is coordinated to more than 6ne kind of ligand is called heteroleptic complex. Example [CO(NH3)5Cl]+2, [Pt(NH3)2Cl2].

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 11.
Identify the following complexes as homoleptic or heteroleptic complexes.
(i) [Fe(CN)6]-4
(ii) [CO(NH3)4Cl2]+
(iii) [Cr(en)3]+3
(iv) [Ag(NH2)2]+
(v) [Fe(CN)5NO]-3
Answer:
(i) Homoleptic complex ion.
(ii) Heteroleptic complexion.
(iii) Homoleptic complexion.
(iv) Homoleptic complexion.
(v) Heteroleptic complex ion.

Question 12.
Explain the following giving an example in each case: (i) Linkage isomerism, (ii) Coordination isomerism, (iii) Ionisation isomerism, (iv) Solvate or hydrate isomerism.
Answer:
(i) Linkage isomerism This type of isomers arises when an ambidentate ligand is bonded to the central metal atom/ion through either of its two different donor atoms, eg: In the nitrite ion is bound to the central metal ion Co3+ through a nitrogen atom in one complex,and through oxygen atom in other complex.
[CO(NH3)5(NO2)]2-
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 3
(ii) Coordination isomerism: This type of isomerism arises in coordination compounds having both complex cations and complex anions. The interchange of one or more ligands between the cationic and the anionic coordination entities gives different isomers, eg:
[CO(NH3)6] [Cr(CN)6] and [Cr(NH3)6] [CO(CN)6]
[Cr(NH3)6] [Co(C2O4)3] and [Co(NH3)6]
[Cr(C2O4)3]
[Co(en)3] [Cr(CN)6] and [Cr(en)3] [CO(CN)6]
(iii) Ionisation isomerism: This type of isomerism arises when the coordination compounds give different ions in solution. For example, the complex having the formula [Co(NH3)5 BrSO4] exists in two isomeric forms.
[CO(NH3)3 Br]SO4 and [Co(NH3)5SO4] Br. They give different ions in an aqueous solution.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 4
(iv) Solvate or hydrate isomerism: This isomerism arises when free solvent molecules like H20, ammonia or alcohol present in the coordination entity are exchanged with the ligands outside the coordination entity.
eg: [Cr(H2O)6]Cl3, [Cr(H2O)5Cl]Cl2 H2O [Cr(H2O)4Cl2] Cl2H2O.

Question 13.
Give the ionisation isomer of the following and write their IUPAC names.
(i) [Pt(NH3)4 Cl2] Br2
(ii) [CO(NH3)4Cl2] NO2
Answer:
(i) The ionisation isomer of [Pt(NH3)4 Cl2] Br2 is [Pt(NH3)4 Br2] Cl2. Its IUPAC name is tetraammine dibromido platinum (IV) chloride.
(ii) The ionisation isomer of [CO(NH3)4 Cl2] NO2 is [CO(NH3)4Cl.NO2]Cl. Its IUPAC name is tetraammine chlorido nitro cobalt (III) chloride.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 14.
Briefly outline the geometrical isomerism exhibited by square planar and with an example.
Answer:
Square planar complexes: In square planar complexes of the form [MA2B2] and [MA2BC] (where A, B and C are mono dentate ligands and M is the central metal ion/ atom), Similar groups (A or B) present either on same side or on the opposite side of the central metal atom (M) give rise to two different geometrical isomers and they are called, cis and trans isomers respectively. The square planar complex of the type [M(xy)2] where xy is a bidentate ligand with two different coordinating atoms also shows cis-trans isomerism. Square planar complex of the form [MABCD] also shows geometrical isomerism. In this case, by considering any one of the ligands (A, B, C or D) as a reference, the rest of the ligands can be arranged in three different ways leading to three geometrical isomers.
eg:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 5

Question 15.
Write the structure of geometrical isomers in octahedral complexes of the type Ma4b2, Ma2b4, Ma4bc, Ma3b3 where a + b are monodentate ligands. Give example for each type.
Answer:
(i) Ma4b2 type:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 6
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 7
(ii) Ma3b3 type:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 8
(iii) M(aa3)2b2 or M(aa)2 bc type:
where aa is a symmetrical bidentate ligand, b and c are monodentate ligands, eg: [Co(en)2Cl2]+
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 9

Question 16.
Mention the types of stereoisomerism exhibited by coordination compounds.
Answer:
Coordination compounds exhibit geometrical and is optical isomerism.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 17.
Explain the geometrical isomerism exhibited by the [MA3B3]±n where A and B are monodentate ligands. [OR]
Explain the terms facial and meritorial isomers.
Answer:
Octahedral complex of the type [MA3B3] also shows geometrical isomerism. If the three similar ligands (A) are present in the comers of one triangular face of the octahedron and the other three ligands (B) are present in the opposing triangular face, then the isomer is referred as a facial isomer (fac isomer). If the three similar ligands are present around the meridian which is an imaginary semicircle from one apex of the octahedral to the opposite apex as shown in the figure, the isomer is called as a meridional isomer (mer isomer). This is called meridional because each set of ligands can be regarded as lying on a meridian of an octahedron.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 10

Question 18.
Write the formula of coordination isomers of the following. Write their IUPAC names.
(i) [Pt(NH3)4] [CuCl4]
(ii) [Cr(NH3)6] [Co(C2O4)3]
(iii) [Cr(NH3)6] [Cr(SCN)6]
(iv) Co(en)3[Cr(CN)6]
Answer:
(i) The coordination isomer of [Pt(NH3)4] [CuCl4] is [Cu(NH3)4] [PtCl]4. Its IUPAC name is Tetraammine copper (II) tetrachlorido platinate (II).
(ii) The coordination isomer of [Cr(NH3)6] [Co(C2O4)3] is [CO(NH3)6] [Cr(C2O4)3]. Its IUPAC name is Hexaammine cobalt (III) trioxalato chromate (III).
(iii) The coordination isomer of [Cr(NH3)6] [Cr(SCN)6] is [Cr(NH3)4(SCN)2] [Cr(NH3)2(SCN)4] Tetraammine dithiocyanatochromium (III) diammine tetrathiocyanatochromate (III).
(iv) The coordination isomer of [Co(en)3] [Cr(CN)6] is [Cr(en)3]4 [Co(CN)6], Its ionisation isomer is Tri (ethane 1, 2, diamine) chromium (III) hexacyano cobaltate (III).

Question 19.
Discuss the bonding in metal carbonyls.
Answer:
The metal-carbon bond in metal carbonyls have both σ and π bond character. The metal – carbon sigma bond is formed by the donation of lone pair of electrons from the carbonyl carbon into a vacant orbital of the metal. The metal- carbon pi bond is formed by the donation of a pair of electrons from a filled d orbital of the metal to the vacant antibonding pi molecular orbital of carbon monoxide. The metal ligand bonding causes a synergic effect which strengthens the bond between Co and the metal.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 20.
Indicate the type of isomerism exhibited by the following complexes and draw structures for these isomers.
(i) KCr (H2O)2(C2O4)3
(ii) [Co(en)3]Cl3
(iii) [ CO(NH3)5(NO2)(NO3)2]
(iv) [Pt (NH3) (H2O)Cl2]
Answer:
(i) Both show geometrical (cis-trans) isomerism. Optical isomerism is shown by cis form.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 11
(ii) Two optical isomers can exist. [Co(en)3]+
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 12
(iii) There are 10 possible (geometrically ionisation and linkage) isomers.
Ionisation isomers:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 13
(iv) Geometrical (cis-trans) isomerism can exist.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 14

Question 21.
Give evidence to show that [CO(NH3)5Cl]SO4 and [Co(NH3)5 SO4]Cl are ionisation isomers.
Answer:
The ionisation isomers dissolve in water to yield different ions and thus react differently with different reagents.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 15
A white precipitate is than obtained.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 16

Question 22.
Draw the structure of optical isomers of (i) PtCl2 (en)2, (ii) [Cr(NH3)2 Cl2 (en)2]+
Answer:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 17

Question 23.
Write all the geometrical isomers of [Pt (NH3) BrCl Py] and how many of these exhibit optical isomerism?
Answer:
Three isomers are possible.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 18
Isomers of this type do not show optical isomerism. Optical isomerism rarely occurs in square planar or tetrahedral complexes and that too when they contain asymmetrical chelating ligand.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 24.
Draw the structure of all the isomers (geometrical and optical) of (i) [CO(NH3)Cl (en)2]+2 (ii) [Co(NH3)2Cl2(en)]+
Answer:
(i)
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 19
I and II are optical isomers.
II and III are geometrical isomers.
(ii)
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 20
I and II are geometrical isomers.
II and III are optical isomers.

Question 25.
Draw the structure of geometrical isomers of [Fe(NH3)2(CN)4].
Answer:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 21

Question 26.
Out of the following two coordination entities which is optically active? (i) cis [CrCl3(oX)2]-3(ii) trans [Cr Cl2 (oX)2]-3 The two entities are represented as follows:
Answer:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 22
Of these cis form is optically active.

Question 27.
Write the structures of isomers, if any and write the names of the following complexes. (i) [Cr (NH3)4 Cl2]+, (ii) [Co(en)3]+
Answer:
(i) Geometrical isomers of [Cr(NH3)4Cl2]+
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 23
(ii) Optical isomers of OX [Co(en)3]+3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 24

Question 28.
Platinum (II) forms’square planar complexes and platinum (IV) gives octahedral complexes.. How many geometrical isomers are possible for each of the following. Draw their structures. (a) [Pt(NH3)3Cl]+, (b) [Pt(NH3)Cl5], (c) [Pt(NH3)2ClNO2], (d) [Pt(NH3)4Cl Br]+2.
Answer:
(a) No isomer is possible for a square planar complex MA3B.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 25
(b) No isomer is possible for an octahedral complex of the type MAB5.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 26
(c) cis-trans isomers are possible for a square planar complex MA2BC.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 27
(d) cis-trans isomers are possible for an octahedral complex of the type MA2BC.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 28

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 29.
Explain the term (i) inner orbital complex and (ii) outer orbital complex with an example for each.
Answer:
(i) Bonding in complexes are explained in terms of hybridisation. If the hybridisation of central metal atom/ion involves the use of (n-1) d, ns and np orbitals, then d2sp3 hybridisation is possible for octahedral complexes. Complexes formed by d2sp3 hybridisation of the central metal atom or ion is known as inner orbital complex. [Fe(CN)6]-4, [Fe(CN)6]-3, [Cr(NH3)6]+3 are examples of inner orbital complexes.
(ii) If the hybridisation of the metal ion involved the ns, np and nd orbitals and for octahedral complexes sp3d2 hybridisation involved, the complex formed is known as outer orbital complex. [CoF6]-3 is an example for outer orbital complex.

Question 30.
[Co(CN)6]-3 and [CoF6]-3 are both octahedral complexes. Then what is the difference between the two?
Answer:
In both complexes, Co is in +3 oxidation state. It has 6 electrons in the ‘d’ subshell (d6).
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 29
In the formation of [Co(CN)6], the ‘d’ electrons in 3d level gets paired leaving behind two 3d orbital vacant.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 30
The Co+3 ion makes use of two 3d orbitals, one 4s and two 4p orbitals for hybridisation. d2 sp3 hybridisation and two 4p orbitals for hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 31
The CN ion donates the electron pairs to the d2spi hybrid orbitals and form six covalent bond. Thus [(CO(CN)6]-3 is an inner orbital or low spin complex.
On the other hand, in the formation of [CoF6]-3 the Co+3 ion makes use of outer 4s, 4p and 4d orbitals for hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 32
In the presence of F ion, electron pairing does not occur in 3d orbitals, and Co+3 ion makes use of one 4s, three 4p and two 4d orbitals for hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 33
The six fluoride ion donates a pair of electrons to the six sp3d2 hybrid orbitals and form six-coordinate covalent bonds.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 34
Since outer orbitals are used in the formation it is an outer orbital complex. Since more unpaired electrons are present it is also known as high spin complex.

Question 31.
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory.
(i) [Fe(CN)6]-4
(ii) [FeF6]-3
(iii) [Co(C2O4)3]-3
(iv) [NiCl4]-2
Answer:
(i) [Fe(CN)6]-4: d2sp3 hybridisation octahedral: diamagnetic.
In this complex, the oxidation state of iron is +2.
Electronic configuration of Fe = [Ar]3d46s2
Electronic configuration of Fe+2 = [Ar]3d6
To accommodate six pairs of electrons from six cyanide ions, the iron (II) must make available six empty orbitals. This can be achieved by the d2sp3 hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 35
In the presence of CN ion, a strong ligand, the electrons in 3d subshell gets paired and two of the 3d one 4s and three 4p orbitals hybridise to produce six d2sp3 hybrid orbitals.
Fe+3 (d6) excited state.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 36
Thus, the six pairs of electrons from six cyanide ion occupy the six hybridised orbitals of iron (II) ion. [Fe(CN)6]-4
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 37
Since, there are no unpaired electron present, it is diamagnetic and its geometry is octahedral.

(ii) [FeF6]-3: This complex is high spin or octahedral, since the central atom Fe(II) utilises nd orbitals for hybridisation. It is an octahedral complex involving sp3d2 hybridisation. Each orbital accommodates a lone pair of electrons from six fluoride ions as shown below. [Fe+3(d5) ground state]
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 38
In the presence of F ions (weak ligand) the electrons in 3d orbitals do not get paired and the iron (II) utilises ns, np and nd orbitals for hybridisation. Thus six sp3d2 hybrid orbitals are formed.
[Fe+3 excited state]
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 38
The six pairs of electrons from F ions accommodate the six vacant spid1 hybrid orbitals
[FeF6]-3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 40
Thus, the complex is outer orbital complex, octahedral and paramagnetic.

(iii) [Co(C2O4)3]-3: d2sp3 hybridisation diamagnetic.
The cobalt ion is in +3 oxidation state. It has six electrons in d subshell (d6).
[Co+3(d6)]
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 41
Oxalate ion being a relatively strong ligand pairs of the electrons in ‘d’ subshell, learning two of the ‘d’ orbital for hybridisation. Thus Co+3 ion under goes d2sp3 hybridisation.
Co+3(ground state)
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 42

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 43
The three oxalate anions (bidentate) donate two pairs of electrons to two of the hybrid orbitals.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 44
Thus [Co(C2O4)3]-3 is an inner orbital, octahedral, complex and diamagnetic.

(iv) [NiCl4]-2: In this complex Ni is in +2 oxidation state and has d8 configuration.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 45
The chloride ions donate pair of electrons to each of the four sp3 hybrid orbitals.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 46
Thus, the complex is tetrahedral and paramagnetic.

Question 32.
[NiCl4]-2 is paramagnetic while Ni(CO)4 is diamagnetic though both are tetrahedral why?
Answer:
In Ni(Co)4, Ni is in the zero oxidation state whereas in [NiCl4]-2, it is in +2 oxidation state. In the presence of a CO being a strong ligand, the unpaired ‘d’ electrons of Ni pair up but Cl being a weak ligand it is unable to pair up the unpaired electrons. Hence [NiCl4]-2 is paramagnetic where as Ni(CO)4 is diamagnetic.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 33.
Explain [Co(NH3)6]+3 is an inner orbital complex whereas [Ni(NH3)6]+2 is an outer orbital complex.
Answer:
In the presence of NH3, the 3d electrons pair up learning two ‘d’ orbitals empty to be involved in d2sp3 hybridisation forming inner orbital complex.
In [Ni(NH3)6]+2, Ni is in +2 oxidation state and has d8 configuration. The hybridisation involved in sp3d2 and hence, it forms an outer orbital complex.

Question 34.
[Cr(NH3)6]+3 is paramagnetic while [Ni(CN)4]-2 is diamagnetic explain why?
Answer:
(i) Formation of [Cr(NH3)6]+3:
The oxidation state of chromium in [Cr(NH3)6]+3 ion is +3. The electronic configuration of chromium is [Ar] 3d5 4s1. The hybridisation scheme is shown below:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 47
Ammonia being a weak ligand is unable to pair of up the electrons of Cr+3 and hence Cr+3 undergoes d2sp3 hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 48
Thus the complex is inner orbital, octahedral complex and paramagnetic because of the presence of three unpaired electrons.

(ii) Formation of [Ni(CN)4]-2: In the square planar complexes, the hybridisation involved is dsp2. In [Ni(CN)4]-2, nickel is in +2 oxidation state and has the electronic configuration of d8.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 49
CN ion being a strong ligand, pairs up the 3d electrons leaving one 3d orbital vacant that is used for dsp2 hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 50
Thus the complex is diamagnetic as there are no impaired electron.

Question 35.
A solution of [Ni(H2O)6]+2 is green but a solution of [Ni(CN)4]-2 is colourless explain.
Answer:
In [Ni(H2O)6]+3, Ni is in +2 oxidation state with configuration d8. i.e., it has 2 unpaired electrons which do not pair in the presence of weak H2O ligand. Hence d-d transition is possible and so it is coloured. The d-d transition absorbs red light and the complimentary light emitted is green.
In case of [Ni(CN)4]+2, Ni is in +2 oxidation state with d8 configuration. But in the presence of strong CN ion as ligand, the two unpaired electrons in 3d orbitals are paired up. Hence there are no unpaired electrdhs present and so it is colourless.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 36.
[Fe(CN)6]-4 and [Fe(H2O)6]+2 are of different colours in dilute solution why?
Answer:
In both complexes, Fe is in +2 oxidation state with d6 configuration. In the presence of a weak ligand, they do not pair up. In the presence of strong CN ion, they paired up learning no unpaired electrons. Due to the difference in the number of unpaired electrons they have different colours.

Question 37.
Write down the IUPAC name of each of the following complexes and indicate the oxidation state, electronic configuration and coordination number of the central metal ion. Also, give the stereochemistry and magnetic moment of each complex.
(i) K4[Cr(H2O)2(C2O4)2]
(ii) [CrCl3(Py3)]
(iii) K2[Mn(CN)4]
(iv) [CO(NH3)5Cl]Cl2
(v) CS[FeCl4]
Answer:
(i) Potassiumdiaquaoxalatochromate (III) hydrate.
Coordination number = 6
Shape: Octahedral
Oxidation state of Cr = x + 0 + 2 (- 2) = -1 or x = +3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 51

(ii) Trischloridopyridinechromium (III)
Coordination number of Cr = 6
Shape: Octahedral
Oxidation state of Cr = x – 3 + 0 + 0 = 0 or x = +3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 52

(iii) Potassiumhexacyanomanganate (II)
Coordination number of Mn = 6.
Shape: Octahedral
Oxidation state of Mn = x – 6 = – 4 (or) x = +2
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 53

(iv) Pentaammine chloridocobalt (III) chloride.
Coordination number of Co = 6.
Shape: Octahedral
Oxidation state of Cr = x + 0 – 1 = +2 or x = +3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 54
Magnetic moment = 0

(v) Caesiumtetrachloridoferrate (III).
Coordination number of Fe = 4.
Shape: Tetrahedral
Oxidation number of Fe = x – 4 = -1 or x = +3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 55

Question 38.
Calculate the magnetic moment of the following coordination entities.
(i) [Cr(H2O)6]+3,
(ii) [Fe(H2O)6]+3,
(iii) [Zn(H2O)6]+2
Answer:
The oxidation states are (i) Cr(III); (ii) Fe(II) and (iii) Zn(II)
(i) E.C of Cr+3 = 3d3:
no ofunpaired electrons = 3
Magnetic moment = \(\sqrt{3(3+2)}\) = √15
(ii) E.C of Fe+2 = 3d6:
no of unpaired electrons = 4
Magnetic moment = \(\sqrt{4(4+2)}\) = √24
(iii) E. C of Zn+2 = 3d10:
no of unpaired electrons = 0
Magnetic moment = 0

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 39.
What will be the correct order for the wavelength of absorption in the visible region of the following:
[Ni(NO2)6]-4, [Ni(NH3)6]+2, [Ni(H2O)6]+2
Answer:
As the metal ion is fixed the increasing field strength (CFSE values) of the ligands from the spectrochemical series are in the order.
H2O<NH3<NO2
Thus the energies absorbed for excitation will be in the same order
[Ni(H2O)6]+2 < [Ni(NH3)6]+2 < [Ni(H2O)6]+2
As, E = \(\frac{h c}{\lambda}\), the wavelength absorbed will be in the opposite order.

Question 40.
Give the number of unpaired electrons in the following complex ions: (i) [FeF6]-4, (ii) [Fe(CN)6]-4
Answer:
(i) In [FeF6]-4, Fe is in +2 oxidation state. It has d6 configuration. As F is a weak ligand, the electrons in 3d orbital are not paired.
i-e., TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 56
Hence, it has 4 unpaired electrons.

(ii) In [Fe(CN)6]-4 also, Fe is in +2 oxidation state and it has d6 configuration. Because CN ion is a strong ligand, the electrons in 3d orbital of Fe+2 are paired and so there are no unpaired electrons.

Question 41.
Explain as how two complexes [Ni(CN)4]-2 and [Ni(CO)4] have different structures but do not differ in their magnetic behaviour. (Ni = 28)
Answer:
(i) In Ni(CO)4, nickel is in zero oxidation state. (Ni+2 = 3d8 4s2)
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 57
E.C of Ni in hybridised state
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 58
It is diamagnetic and has a tetrahedral geometry.

(ii) In [Ni(CN)4]-2, Ni is in +2 oxidation state. Electronic configuration of Ni+2 ion is 3d8.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 59
CN ion being a strong liquid and in its presence, the electrons in 3d orbital gets paired leaving are 3d orbital for hybridisation. Thus, it undergoes dsp2 hybridisation.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 60
The CN ions denote a pair of electrons to the valent dsp2 hybrid orbitals. Thus, four Ni CN bonds are formed.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 61
Thus the geometry is square planar and the complex is diamagnetic.

Question 42.
Using valence bond theory explain [Co(NH3)6]+3 in relation to the complex given below:
(i) type of hybridisation [Co(NH3)6]+3 : Co+3 = d6 configuration
(ii) inner or outer orbital complex
(iii) magnetic behaviour
(iv) spin only magnetic moment value.
Answer:
(i) In the presence of ammonia ligand, the electrons in 3d level gets paired up leaving two of the 3d orbitals for hybridisation. Hence, the type of hybridisation is d 2sp3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 62
(ii) Since inner ‘d’ orbitals are used for hybridisation, it is an inner orbital complex.
(iii) The complex is diamagnetic as there are no unpaired electrons.
(iv) Since, there are no unpaired electrons the magnetic moment is zero.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 43.
Discuss the nature of bonding in the following coordination entities on the basis of valence bond theory.
(i) [FeCN6]-4
(ii) [FeF6]2-
(iii) [Co(C2O4)3]-3
(iv) [COF6]-3
Answer:
(i) Oxidation state of Fe in the complex is +2. Its electronic configuration is [Ar] 3d6. Iron undergoes d2sp3 hybridisation giving octahedral, inner orbital complex.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 63
(ii) Oxidation state of iron in the complex is +3. Its electronic configuration is [Ar] 3d5. In the presence of F (weak ligand), the 3d electrons do not get paired. Hence it undergoes sp3d2 hybridisation and forms an outer orbital, octahedral complex.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 64
(iii) The oxidation state of cobalt in the complex is +3. Its electronic configuration is [Ar] 3d6. Since oxalate ion is relatively a strong ligand, the 3d electrons get paired up leaving two of 3d orbital for hybridisation. Thus, cobalt undergoes d2sp3 hybridisation giving octahedral, inner orbital complex.
(iv) Oxidation state of cobalt in the complex is +3. Its electronic configuration is [Ar] 3d6. The F ion being a weak ligand is unable to pair up the electrons in 3d level. It undergoes sp3d2 hybridisation giving an octahedral, outer orbital complex.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 65

Question 44.
What are crystal fields?
Answer:
The ligands especially anionic (or polar neutral ligands) has around them negatively charged field because of which they are called crystal fields.

Question 45.
What do you understand by the term crystal field splitting?
Answer:
When the ligands approach the central metal ion, the electrons in the ‘d’ orbital of central metal ion will be repelled by the lone pairs of the ligands. Because of these interactions, the degeneracy of ‘d’ orbitals of the metal ion is lost and they split into two sets of orbitals having different energies. This is known as crystal field splitting. The extent of crystal field splitting depends on the nature of the ligand.

Question 46.
Briefly discuss the crystal fieid splitting in octahedral complexes.
Answer:
As a result of repulsive forces between the ‘d’ electrons of the metal ion and that of ligands (negative or polar neutral), the degeneracy of the ‘d’ orbitals is lost. Since the two lobes of two eg{dx2-y2, dz2) orbitals lie in the path of approaching ligands these orbitals experience greater forces of repulsion than those of t2g (dxy, dyz and dxz) orbitals is decreased.
Thus, an energy difference exists between two sets of orbitals. This energy difference is called crystal field splitting energy and is represented by Δo. (the subscript ‘o’ stands for octahedral). It measures the crystal field strength of the ligands. The crystal field splitting occurs in such a way that the average energy of the ‘d’ orbitals do not change.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 66
(a) Five degenerate ‘d’ orbitals of the free metal ion.
(b) Hypothetical degenerate ‘GP orbitals at higher energy levels under spherically symmetrical ligand field.
(c) Splitting of ‘d’ orbitals under the influence of ligands.
Thus, three orbitals lie at an energy i.e., 2/5 Δo below the average ‘d’ orbital energy and two ‘d’ orbitals lie at an energy 3/5 Δo above the average energy. The energy gap between t2g and eg sets also denoted by 10Dq.
The energy of t2g orbitals is 4Dq less than that of hypothetical degenerate ‘d’ orbitals and that of eg orbitals is 6Dq above that of hypothetical degenerate ‘d’ orbitals: Thus, t2g set loses energy equal to 0.4 Δo or 4 Dq white eg sets gain energy equal to 0.6 Δo or 6 Dq.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 47.
For the complex
[Fe(en)2Cl2]Cl (en = ethylene diamine), identify The complex is [Fe(en)2Cl2]Cl.
(i) The oxidation number of Fe.
(ii) The hybrid orbital and shape of the complex.
(iii) The magnetic behaviour of the complex.
(iv) The number of geometrical isomers.
(v) Whether there is an optical isomer also.
(vi) The name of the complex (At. No of Fe 26)
Answer:
(i) Oxidation number of Fe
= x + 2 x 0 + 2(-1)
= +1
x – 2 = +1
⇒ x = 3
(ii) Orbitals in Fe+3(d5)
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 67
In the presence of a strong ligand (en), the electrons in 3d orbital get paired.
Fe+3 excited state
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 67
Thus, Fe+3 ion undergoes d2sp3 hybridisation therefore the shape is octahedral.
(iii) The complex is paramagnetic due to the presence of one unpaired electron.
(iv) It exhibits cis-trans isomerism
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 69
(v) Cis isomer will show optical isomerism.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 70
(vi) Dichlorido bis(ethane 1, 2, diamine) iron, (III) chloride.

Question 48.
Compare the following complexes with respect to their shape, magnetic behaviour and the hybrid orbitals involved.
(i) [CoF4]-2, (ii) [Cr(H2O)2(C2O4)2], (iii) [Ni(Co)4], (At No: Co = 27, Cr = 24, Ni = 28).
Answer:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 71

Question 49.
Briefly discuss the crystal field splitting in tetrahedral complexes.
Answer:
The three orbitals i.e., t2g orbitals are close to approaching ligands. As a result of this, the t2g electrons suffer more repulsions than eg electrons. The energy of t2g orbitals increases more than eg orbitals. The splitting is shown below:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 72
The energy gap between two sets of orbitals is designated as Δt. It is observed that Δt, is considerably less than Δo. It has been found that.
Δt = \(\frac{4}{9}\) Δo

Question 50.
Briefly outline crystal field splitting in square planar complexes.
Answer:
As the lobes of dx2-y2 point towards the ligands, this orbital has the highest energy. The lobes of dxy orbital lie between the ligands but are coplanar with them this orbital is the next highest energy. The lobes of dz2 orbital point out of the plane of the complex but the belt around the centre of the orbital (which contain 1/3 of the electron density) lies in the plane. Therefore dz2 orbital is the next highest in energy. The lobes of dx2 and dy2 orbitals point out of the plane of the complex. Hence, they are least affected by the electrostatic field of the ligands. They are degenerate and lowest in energy.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 73

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 51.
What is crystal field splitting energy? How does the magnitude of Δo decide the actual configuration of ‘d’ orbitals in a coordination entity?
Answer:
When ligands approach a transition metal ion, the ‘rf orbital splits into two sets one with lower energy and the other with higher energy. The difference in energy between two sets (t2g and eg) of orbitals is called crystal field splitting energy Δo for an octahedral field.
If Δo < p (pairing energy), the fourth electron enters one of the eg orbitals giving the configuration t2g3 eg1, thereby forming high spin complexes. Such ligands for which Δo < p are called weak field ligands.
If Δo > p, the fourth electron pair up in one of the t2g orbital giving the configuration t2g4 eg0, thus forming low spin complexes. Such ligands for which Δo > p are called strong field ligands.

Question 52.
What is spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.
Answer:
The arrangement of ligands in order of their increasing field strength i.e increasing crystal field splitting energy (CFSE) values is called spectrochemical series.
The ligand with a small value of Δo CFSE (Δo) is called weak field ligands whereas those with a large value of CFSE(Δo) are called strong field ligands.

Question 53.
How does the oxidation state of a metal ion influence or affect the crystal field splitting energy?
Answer:
Generally higher the oxidation state of the metal, greater is the crystal field splitting. For example most of the cobalt (II) complexes have low value of Δ whereas all cobalt (III) complexes have high value of Δ.

Question 54.
Briefly explain the distribution of ‘d’ electrons in t2g and eg orbitals in octahedral complexes in a weak ligand field.
Answer:
Under the influence of weak ligands the energy difference, Δo between t2g and eg sets is relatively small and hence all the five ‘d’ orbitals may be supposed to be degenerate. The distribution of electrons in t2g and eg sets occurs according to Hund’s rule.
When the ligands are weak, the first three electrons numbered as 1,2,3 go to t2g set those numbered 4, 5 go to eg set, those numbered 6, 7, 8 go to t2g set and the remaining two electrons numbered 9 and 10 will occupy eg set. i.e., TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 74
In complexes of weak ligands, Δo is less than P(P is called pairing energy which is the energy required to pair two electrons in the same orbital). Δo is the octahedral crystal field splitting energy, tends to force as many electrons into t2g set while P tends to prevent the electrons to pair up in the t2g level.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 75

Question 55.
The Hexa aqua manganese (II) ions contain five unpaired electrons while hexacyano ions contain only one unpaired electron. Explain using crystal field theory.
Answer:
Mn is in +2 oxidation state and has 3d5 configuration. H2O is a weak ligand. In the presence of water molecules, the distribution of electrons is t2g3 eg2 i.e., all the electrons are unpaired.
In the other hand CN ion is a strong ligand. The distribution of electrons is t2g5 eg0.
i.e., TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 76 and it has one unpaired electron.

Question 56.
Why do compounds having similar geometry have a different magnetic moment?
Answer:
It is due to the presence of strong and weak ligands in complexes. If GFSE is high, the complex will show a low value of the magnetic moment and vice versa. eS: [CoF6]-3 and [CO(NH3)6]+3, the former is paramagnetic and the latter is diamagnetic.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 57.
Briefly explain how the electrons are distributed between t2g and eg sets in an octahedral complex in the presence of a strong field ligand.
Answer:
Under the influence of strong ligands, the energy difference between t2g and eg sets is relatively high and thus the distribution of ‘d’ electrons in t2g and eg sets does not obey Hund’s rule. The first electrons numbers 1, 2, 3, 4, 5, 6 will go to t2g set remaining four electrons numbered 7, 8, 9, 10 will go to eg set.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 77
For these complexes, Δo is greater than p.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 78

Question 58.
Using crystal field theory, draw an energy level diagram of the central metal atom/ion and determine the magnetic moment value of the following.
(i) [COF6]-3,
(ii) [Co(H2O)6]+2,
(iii) [Cu(CN)6]-3
Answer:
(i) F is a weak field ligand and cobalt is in a +3 oxidation state. It has d6 configuration. The electron distribution is t2g4 eg2.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 79
i.e., Number of unpaired electron = 4
Magnetic moment = \(\sqrt{4(4+2)}\) = √24
= 4.9 BM
(ii) In this complex cobalt is in +2 oxidation state. Its electronic configuration is d1. Since water is a weak ligand, electron filling follows Hund’s rule, i.e., t2g5 eg2.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 80
i.e., Number of unpaired electron = 3 Magnetic moment = \(\sqrt{3(3+2)}\) = √15
= 3.87BM
(iii) In this complex cobalt is in +3(d6) oxidation state and CN ion a strong ligand. Electron filling is not obeyed by Hund’s rule. All the six electrons get paired in t2g set.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 81
Since, there is no unpaired electron the complex is diamagnetic.

Question 59.
In the basis of crystal field theory explain why cobalt (III) forms a paramagnetic octahedral complex with weak field ligands whereas it forms a diamagnetic octahedral complex with strong field ligands.
Answer:
With weak field ligand, Δo < P, the electronic configuration (of cobalt (III)) i.e., d6 will be t2g4 eg2 and it has 4 unpaired electrons and is paramagnetic. With strong field ligands, Δo > P, the electron distribution is t2g6 eg0. It has no unpaired electron and hence diamagnetic.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 60.
Differentiate between weak field and strong field coordination entity.
Answer:

Weak field coordination entityStrong field coordination entity
They are formed when the crystal field stabilisation energy (CFSE) in octahedral complexes is less than the energy required for electron pairing in a single orbital (P).They are formed when crystal field stabilisation energy (CFSE) Δo is greater than pairing energy (P).
They are also called high spin complexes.They are also called low spin complexes.
They are mostly paramagnetic.They are mostly diamagnetic or less paramagnetic than weak field.
Never formed by CN ions.Formed by CN like ligands.

Question 61.
State for a d6 configuration, how the actual configuration of the split ‘d’ orbitals in an octahedral field is decided by relative values of Δo and P.
Answer:
For d6 configuration, three electrons will first enter t2g. Now, if P < Δo electrons will pair up in t2g orbitals giving the configuration t2g6 eg0. If Δo< P, two electrons will first enter into eg orbitals and one will pair up in t2g, giving the configuration t2g4 eg2.

Question 62.
Arrange the following ligands in the increasing order of crystal field splitting power.
Answer:
H2O, OH, Cl, F, CN
Cl < F < OH < H2O < CN

Question 63.
Using crystal field theory, show energy level diagrams, write the electronic configuration of the central metal atom/ion and determine the magnetic moment value in the following. (i) [FeF6]-3, (ii) [Fe(H2O)6]+2,
(iii) [Fe(CN)6]-4
Answer:
(i) In this complex, Fe is +3 oxidation state and Fe+3 has 3d5 configuration. Since F is a weak field ligand, electron filling in t2g and eg sets follow Hund’s rule.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 82
i.e., t2g4 eg2. The number of unpaired electron is 5. The magnetic moment value is \(\sqrt{5(5+2)}\) = √35 = 5.92 BM.
(ii) In [Fe(H2O)6]+2, Fe is in +2 oxidation state and has d6 configuration. Since water is a weak ligand electron distribution in t2g and eg orbitals take place according to Hund’s rule.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 83
i.e., t2g4 eg2. The number of unpaired electrons is 4. Its magnetic moment value is \(\sqrt{4(4+2)}\) = √24 = 4.9 BM.
(iii) In [Fe(CN)6]-4, Fe is in +2 oxidation state and has 3d6 configuration. As CN is a strong ligand, electron distribution between t2g and eg sets take place not in accordance with Hund’s rule. All the t2g orbitals are filled with six electrons.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 84
Since there is no unpaired electron, the complex is diamagnetic.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 64.
Give the oxidation state, ‘d’ orbital occupation and coordination number of the central metal ion in the following complexes.
(i) K3[Co(C2O4)3],
(ii) (NH4)[CoF4],
(iii) Cis – [Cr(en)2Cl2]Cl,
(iv) [Mn(H2O)6]SO4.
Answer:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 85

Question 65.
With the help of crystal field theory, product the number of unpaired electrons in [Fe(CN)6]-4 and [Fe(H6O)2]+2 complexes.
Answer:
In both complexes, Fe is present in +2 oxidation state and has d6 configuration. As CN is a strong field ligand, these electrons will pair up giving the configuration t2g6 eg0. As there are no unpaired electrons, the complex is paramagnetic. But H2O is a weak ligand and electron filling follow Hund’s rule i.e., t2g4 eg2. It has 4 unpaired electron and hence paramagnetic.

Question 66.
CO is stronger ligand than NH3 for many metals. Explain giving appropriate reason.
Answer:
Ligands such as CO, CN, NO+ have empty π orbitals which overlap with the filled d orbitals (t2g) of transition metals forming π bonds (back bonding). These π interactions increase the value of Δo. This account for the position
of these ligands as strong ligand. NH3 cannot form π bonds by back bonding.

Question 67.
What is meant by the stability of a coordination compound in solution?
Answer:
The stability of a complex in a solution refers to the degree of association between two species involved in a state of equilibrium. The magnitude of the equilibrium constant for the association is a quantitative measure of stability.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 86
For the above equilibrium, the larger the stability constant, the higher is the proportion of ML4 that exists in the solution.

Question 68.
The stability constant of some complexes are given below:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 87
Among CN and NH3 which is a stronger ligand? Why?
Answer:
The numerical value of the stability constant is a measure of the stability of the complex. Greater the magnitude of the stability constant more stable the complex. Thus CN ion is a stronger ligand than ammonia.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 69.
The dissociation constants of [Cu(NH3)4]+2 and [CO(NH3)6]+3 are 1.10 x 10-12 and 6.2 x 10-36 respectively. Which complex would be more stable and why?
Answer:
Smaller the values of the dissociation constant more stable the complexion in solution Hence [CO(NH3)6]+3 is more stable than [Cu(NH3)4]+2 ion.

Question 70.
Calculate the overall complex dissociation equilibrium constant for the [Cu(NH3)4]+2 ion given that β4 for this complex is 2.14 x 1013.
Answer:
Overall stability constant (B4)
= 2.1 x 1013. Overall dissociation constant is the reciprocal of overall stability constant. Hence, overall dissociation constant.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 88
= 4.7 x 10-14.

Question 71.
Calculate the ratio of [Ag(S2O3)2]-3 and [Ag+] in 0.1 M S2O3 solution. Given the stability or formation constant of [Ag(S2O3)2]-3 is 1.0 x 1013.
Answer:
The equilibrium is
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 89

Question 72.
Mention the use of coordination compounds in metallurgy.
Answer:

  1. Purification of nickel by Mond’s process involves the formation of nickel carbonyl Ni(CO)4 which yields 99.5% pure nickel and decomposition.
  2. Coordination compounds are used in the extraction of silver and gold from their ores by forming a soluble cyano complex. These cyano complexes are reduced by zinc to yield pure metals.

Question 73.
Mention the use of complexes used as catalysts in organic reactions.
Answer:

  1. Wilkinson’s catalyst [(PPh3)3RhCl] is used for the hydrogenation of alkenes.
  2. Ziegler-Natta catalyst – [TiCl4] + Al[C2H5]3 is used in the polymerization of ethene.
  3. In order to get a fine and uniform deposit of superior metals (Ag, Au, Pt etc.,) over base metals, coordination complexes [Ag(CN)2] and [Au(CN)2] etc., are used in an electrolytic bath.

Question 74.
Mention the use of complexes in photography.
Answer:
In photography, when the developed film is washed with sodium thio sulphatesolution (hypo), the negative film gets fixed. Undecomposed AgBr forms a soluble complex called sodiumdithiosulphatoargentate(I) which can be easily removed by washing the film with water.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 90

Question 75.
Mention the use of metal complexes in biological systems.
Answer:

  1. A red blood corpuscle (RBC) is composed of the heme group, which is Fe2+ – Porphyrin complex. It plays an important role in carrying oxygen from the lungs to tissues and carbon dioxide from tissues to the lungs.
  2. Chlorophyll, a green pigment present in green plants and algae, is a coordination complex containing Mg2+ as a central metal ion surrounded by a modified Porphyrin ligand called a corrin ring. It plays an important role in photosynthesis, by which plants converts CO2 and water into carbohydrates and oxygen.
  3. Vitamin B12 (cyanocobalamine) is the only vitamin consist of the metal ion. It is a coordination complex in which the central metal ion is Co+ surrounded by a Porphyrin ligand.
  4. Many enzymes are known to be metal complexes, they regulate biological processes. For example, Carboxypeptidase is a protease enzyme that hydrolytic enzyme important in digestion contains a zinc ion coordinated to the protein.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

Question 76.
What is Cisplatin? Mention its use.
Answer:
Cisplatin is a square planar coordination complex (cis- [Pt (NH3)2C12]), in which two similar ligands are in adjacent positions. It is a platinum-based anticancer drug. This drug undergoes hydrolysis and reacts with DNA to produce various crosslinks. These crosslinks hinder DNA replication and transcription, which results in cell growth inhibition and ultimately cell death. It also crosslinks with cellular proteins and inhibits mitosis.

Question 77.
What are metal carbonyls? Mention their uses.
Answer:
Metal carbonyls are transition metal complexes of carbon monoxide, containing metal-carbonyl (M ← CO) bonds. They are used as catalysts.

Question 78.
What are mononuclear and polynuclear carbonyls? Give examples.
Answer:
Mono nuclear carbonyls contain only one metal atom.eg: Ni(CO)4, ie(CO)5, Cr(CO)6. Polynuclear carbonyls contain two or more metal atoms. They may be homonuclear or heteronuclear.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 91

Question 79.
What are non-bridged metal carbonyls? Give examples.
Answer:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 92

  1. Non bridged metal carbonyls contain only terminal carbonyls, eg: [Ni (Co)4] [Fe(Co)5] and [Cr(Co)6]
  2. Non bridged metal carbonyl which contains terminal carbonyls as well as metal- metal bonds, eg: Mn2(Co)10. It contains Mn—Mn bonds and also Mn ← 10 bonds.

Question 80.
What are bridged carbonyls? Give example.
Answer:
These metal carbonyls contain one or more bridging carbonyl ligands along with terminal carbonyl ligands and one or more Metal-Metal bonds. For example,
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 93
The structure of Fe2(CO)9, di-ironennea carbonyl molecule consists of three bridging CO ligands, six terminal CO groups and a single Fe-Fe bond formed by the weak coupling of the unpaired electrons present in two 3d orbitals of two Fe atoms. This bond is represented by a dotted line and is called a fractional single bond.

Choose the correct answer.

1. Which of the following complexes formed by Cu+2 ions is the most stable?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 94
Answer:
(b)
Hint: Greater the log k value, more stable the complex.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

2. When 1 mol of CrCl3 6H2O is treated with excess of AgNO3 3 mol of AgCl are obtained. The formula of the complex is:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 95
Answer:
(d)

3. The correct IUPAC name of [Pt (NH3)2Cl2] is:
(a) Diammine dichloridoplatinum (II)
(b) Diammine dichloridoplatinum (IV)
(c) Diammine dichlorido platinum (0)
(d) Dichlorodiammine platinum (IV)
Answer:
(a)

4. The stabilisation of coordination compounds due to chelation is called chelate effect. Which of the following is the most stable complex species?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 96
Answer:
(c)
Hint: C2O4-2 is a bidentate ligand forming chelate.

5. The compounds [Co(SO4)(NH3)5] Br and [Co(SO4)(NH3)5]Cl represent:
(a) linkage isomerism
(b) ionisation isomerism
(c) coordination isomerism
(d) no isomerism
Answer:
(d)

6. Which of the following species is not expected to be a ligand?
(a) NO
(b) NH4+
(c) NH2CH2CH2NH2
(d) Co
Answer:
(b)
Hint: It has no lone pair of electrons.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

7. The oxidation state of Fe in the brown ring complex [Fe(H2O)5NO]SO4 is:
(a) +1
(b) +2
(c) +3
(d) +4
Answer:
(a)
Hint: [Fe(H2O)5NO]+2 : x + 0 + 1 = 2
x = 1.

8. [CO(NH3)4 (NO2)2]Cl exhibits:
(a) ionisation isomerism, geometrical isomerism and optical isomerism.
(b) linkage isomerism, geometrical isomerism and optical isomerism.
(c) linkage isomerism, ionisation isomerism and optical isomerism.
(d) linkage isomerism, ionisation isomerism and geometrical isomerism.
Answer:
(d)
Hint:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 97

9. Which of the following complex ions has geometrical isomers?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 98
Answer:
(c)
Hint: Geometrical isomerism is shown by disubstituted octahedral complexes such as [Co(NH3)2 (en)2]+3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 99

10. The correct statement with respect to the complexes Ni(CO)4 and [Ni(CN)4]-2 is:
(a) nickel is in the same oxidation state in both.
(b) both have tetrahedral geometry
(c) both have square planar geometry
(d) have tetrahedral and square planar geometry respectively.
Answer:
(d)
Hint: Ni(CO)4: sp3hybridisation: Tetrahedral
[Ni(CN)4]-2: dsp2 hybridisation: square planar.

11. When 0.01 mole of a cobalt complex is treated with excess AgNO3 solution, 4.305g of silver chloride is precipitated. The formula of the complex is:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 100
Answer:
(c)
Hint: 4.305g AgCl = \(\frac{4.305}{143.5}\) mol = 0.03 mol As 0.01 mol of the complex gives 0.03 mol of AgCl this shows that there are 3 ionisable chlorine atoms i.e., c.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

12. Amongst Ni(CO)4, [Ni(CN)4]-2 and [NiCl4]-2
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 101
Answer:
(c)
Hint: Ni(CO)4 and [Ni(CN)4]-2 do not contain any unpaired electrons while [NiCl4]-2 contain two unpaired electrons.

13. Which of the following complexes are not correctly matched with the hybridisation of their central metal ion?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 102
(a) (i) and (ii)
(b) (ii), (iii) and (iv)
(c) (i), (ii) and (iii)
(d) (ii) and (iv)
Answer:
(b)
Hint:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 103
is a weak ligand and cannot force ‘d’ electrons to pair up forming outer orbital complex.

14. Which of the following complexes has a minimum magnitude of ΔO?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 104
Answer:
(c)
Hint:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 105
Hence, the minimum CFSE is for [CoCl6]-3.

15. Hybridisation, shape and magnetic moment of K3 [Co(CO3)3] is:
(a) d2sp3, octahedral, 4.9 BM
(b) sp3d2, octahedral, 4.9 BM
(c) dsp2, square planar, 4.9 BM
(d) sp3, tetrahedral, 4.9 BM
Answer:
(b)
Hint: In each case, the magnetic moment is 4.9 BM, which shows that each of them has 4 unpaired electrons. Further, in the given complex, oxidation state of cobalt is +3. Hence, it will have d6 configuration.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 106
Thus the possible hybridisation in sp3d2. i.e., outer orbital (high spin) octahedral complex.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

16. The spin only magnetic moment value (in Bohr magneton) of Cr(CO)6 is:
(a) 0
(b) 2.84
(c) 4.90
(d) 5.92
Answer:
(d)
Hint.In Cr(CO)6, Cr is in zero oxidation state, [Ar]3d5 4s1. As CO is a strong ligand, all the six electrons will pair up i.e, there will be no unpaired electron. Hence, u = 0.

17. Among the following complexes (K – P)
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 107
the diamagnetic complexes are:
(a) K, L, M, N
(b) K, M, O, P
(c) L, M, O, P
(d) L, M, N, O
Answer: (c)
Hint:
K = K3[Fe(CN)6] : Fe+3 (3d5) d2sp3 hybridisation.
No. of unpaired electron = 1; Paramagnetic
L = [CO(NH3)6Cl3]; CO+3 (3d6): d2sp3 hybridisation.
No. of unpaired electrons = 0; Diamagnetic
M: Na2 [CO(oX)3]: CO+3 (3d6): d2sp3 hybridisation.
No. of unpaired electron = 0; Diamagnetic
N: [Ni(H2O)6] Cl2 ; Ni+3 (3d8): sp3d2 hybridisation.
No. of unpaired electron = 2; paramagnetic
O: K2 [Pt (CN)1]; Pt+2 (3d8): dsp2 hybridisation.
No. of unpaired electron = 0; Diamagnetic.
P: [Zn(H2O)6] (NO3)2; Zn+2 (3d10); sp3d2 hybridisation;
No. of unpaired electron = 0; Diamagnetic.
Hence, diamagnetic complexes are L, M, O and P.

18. Which of the following facts about the complex [Cr(NH3)6] Cl3 is wrong?
(a) The complex is paramagnetic
(b) The complex is an outer orbital complex
(c) The complex gives white precipitate with silver nitrate solution.
(d) The complex involves d2sp3 hybridisation and is octahedral in shape.
Answer:
(b)
Hint: In [Cr(NH3)6]Cl3, Cr+3(3d3): d2sp3 hybridisation. No. of unpaired electron = 3 paramagnetic. The complex is inner orbital complex as it involves (n -1) d orbitals for hybridisation. [Cr(NH3)6]+3
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 108

19. The ‘d’ electron configuration of Cr+2, Mn+2, Fe+2 and Co+2 are d4, d5, d6 and d1 respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 109
Answer:
(d)
Hint:
In [Mn(H2O)6]+2, Mn+2 = 3d5
So, the number of unpaired electron = 5.
In [C(H2O)6]+2, Fe+2 = 3d6
So, the number of unpaired electron = 4.
In [Co(H2O)6]+2, Co+2 = 3d7
So, the number of unpaired electron = 3.
In [Cr(H2O)6]+2, Cr+2 = 3d4
So, the number of unpaired electron = 4.
All these show sp3d2 hybridisation forming outer orbital complexes. Hence, minimum paramagnetic behaviour is shown by [Co(H2O)6]+2

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

20. Crystal field stabilisation energy for high spin d4 octahedral complex is:
(a) -0.6 Δo
(b) -1.8 Δo
(c) -1.66 Δo + P
(d) -1.2 Δo
Answer:
(a)
Hint: d4 octahedral complex has the configuration t2g3 eg1
CFSE = (-0.4x + 0.6y) Δo
x = no. of electron in t2g
y = no. of electron in eg
CFSE = [-0.4 x 3+ 0.6 x 1] Δo
= [-1.2 + 0.6] Δo
= – 0.6 Δo

21. In spectrochemical series, chlorine is above H2O i.e, Cl > H2O. This is due to:
(a) Good π acceptor properties of chlorine
(b) Strong σ donor and good π acceptor properties of chlorine.
(c) Good π donor properties of chlorine.
(d) Larger size of chlorine than H2O.
Answer:
(c)

22. The magnitude of crystal field stabilisation energy (CFSE or Δt) in tetrahedral complexes is considerably less than in the octahedral field. Because
(a) There are only 4 ligands instead of six.
So the ligand field in only 2/3 the size, hence Δt, is only 2/3 the size.
(b) the direction of orbitals does not coincide with the direction of the ligands. This reduces the crystal field stabilisation energy (Δt) by further 2/3.
(c) both (a) and (b) are correct
(d) both (a) and (b) are wrong.
Answer:
(c)

23. Which of the following complex ions is expected to absorb visible light?
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 110
(At. No: Zn = 30, Sc = 21, Ti = 22; Cr = 24) ,
Answer:
(b)
Hint: d0 (Sc+3, Ti+4) and d10 (Zn+2) species will not absorb visible light and are colurless whereas Cr+3 (d3) can undergo d-d transition on absorption of visible light of particular wave length and will be coloured.

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

24. Which of the following is high spin complex?
(a) [CoCl6]-3
(b) [FeF6]-3
(c) [Co(NH3)6]+2
(d) All of these.
Answer:
(d)
Hint: All the given ligands are weak field ligands. Hence they form high spin complexes.

25. Which one of the following ligand is capable of forming a low spin as well as high spin complex?
(a) CO
(b) F
(c) NH3
(d) CN
Answer:
(c)
Hint:CO and CN are strong ligands and F is a weak ligand. NH3 is neither very weak nor very strong ligand.

26. Complexes with halide ions are generally:
(a) low spin complexes
(b) high spin complexes
(c) both (a) and (b)
(d) neither (a) and (b)
Answer:
(b)
Hint: Halide ions have low CFSE (A) values. They cannot pair up the electrons of the metal atom / ion. Hence they form high spin complexes.

27. Which of the following shall form an octahedral complex?
(a) d4 (low spin)
(b) d8 (high spin)
(c) d6 (low spin)
(d) all of these
Answer:
(c)
Hint: In d6 (low spin) electrons pair up thereby making two empty ‘d orbitals of the metal atom / ion and undergo d2sp3 hybridisation.

28. Match the entities of column I with appropriate entities of column II.
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 111
Code:
TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry 112
Answer:
(a)

TN Board 12th Chemistry Important Questions Chapter 5 Coordination Chemistry

29. Assertion (A): The complex [CO(NH3)3Cl3] does not give precipitate with AgNO3.
Reason (R): The complex does not contain counter ions.
(a) If both assertion and reason are true and reason is the correej explanation of assertion.
(b) If both assertion and reason are true, but reason is not the correct explanation of assertion.
(c) If assertion is true but reason is false.
(d) If both assertion and reason are false.
Answer:
(a)

30. Assertion (A): The [Ni(en)3]Cl2 (en = ethylene diamine) has lower stability than (Ni (NH3)6] Cl2.
Reason (R): In [Ni(en)3] Cl2, the geometry of nickel is trigonal bi-pyramidal.
(a) If both assertion and reason are true and the reason is the correct explanation of assertion.
(b) If both assertion and reason are true, but the reason is not the correct explanation of assertion.
(c) If the assertion is true but the reason is false.
(d) If both assertion and reason are false.
Answer:
(d)
Hint:
Correct assertion: [Ni(en)3]Cl2 has greater Stability than [Ni (NH3)6]Cl2.
Correct Reason: [Ni (en)3]Cl2 has a bidentate ligand (en). It forms chelates.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Students get through the TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements which is useful for their exam preparation.

TN State Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Answer the following questions.

Question 1.
Write the electronic configuration of (a) Cr+3, (b) Cu+, (c) CO+2, (d) Mn+2, (e) Pm+3, (f) Ce+4, (g) Lu+2, (h) Th+4.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 1

Question 2.
To what extent do the electronic configuration decide the stability of oxidation states in the first series of transition elements. Illustrate your answer with an example.
Answer:
In a transition, the series the oxidation state which leads to exactly half filled or completely filled ‘d’ orbitals are more stable. For example, the electronic configuration of Fe(z = 96) is [Ar] 3d6 4s2. It shows +2 and +3 oxidation states. The +3 oxidation state is more stable because it has the configuration [Ar] 3d5.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 3.
Explain why transition elements have many irregularities in their electronic configuration.
Answer:
In the transition elements, there is a little difference in the energy of (n – 1 )d and ns orbitals. The incoming electron may occupy either of these orbitals. Hence, there is irregularities in their electronic configurations.

Question 4.
Name the oxometal anoins of the first series of the transition metals in which the metal exhibits the oxidation state equal to its group number.
Answer:
Cr2O7-2 (dichromate) and CrO4-2 (Chromate):
Group number of Cr=Oxidation state of Cr = 6
MnO4 (permanganate):
Group number of Mn=Oxidation state of Mn=7
VO4-3(vanadate ion):
Group number of V = Oxidation state of V = 5.

Question 5.
What are the stable oxidation states of the transition elements with the electronic configuration in their ground states of their atoms 3d3, 3d5, 3d8, and 3d4.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 2

Question 6.
For M+2/M and M+3/M+2 systems, the E° values for some metals are as follows:
Cr+2/Cr = -0.9V; Cr+3/Cr+2 = -0.4V
Mn+2/Mn = -1.2V; Mn+3/Mn+2 = +1.5 V
Fe+2/Fe – -0.4V; Fe+3/Fe+2 = +0.80V
Use this data to comment upon:
(i) the stability of Fe+3 in acid solution as compared to Cr+3 or Mn+3 and
(ii) the case with which iron can be oxidised as compared to a similar process for either chromium or manganese metal.
Answer:
(i) Higher the reduction potential of species, greater is the tendency for its reduction to take place. Therefore, Mn+3, with the highest reduction potential would be readily reduced to Mn+2 (Mn+3 + e → Mn+2) and hence is least stable. Thus, from the values of reductions potential, it is clear that the stability of Fe+3 in acidic solution is more than Mn+3, but less than that of Cr+3.
(ii) Lower the reduction potential or higher the oxidation potential of a species, greater the case with which its oxidation will take place. Thus, the order of tendency to undergo oxidation is Fe < Cr < Mn.
Note: Oxidation and reduction potentials have the same magnitude but opposite in sign.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 7.
How is the variability of oxidation states of transition metals different from that of non-transition metals? Illustrate with examples.
Answer:
In transition elements, the successive oxidation states differ by unity. For example, manganese shows all oxidation states +2 to +7. On the other hand, non-transition metals exhibit variable oxidation states which differs by two units.eg: Pb(II) and Pb (IV); Sn(II) and Sn(IV).

Question 8.
How would you account for the following?
(i) Many of the transition elements and then compounds can act as good catalysts.
(ii) The metallic radii of the third (5d) series of transition elements are literally the same as those of the corresponding members of the second series.
(iii) There is a greater range of oxidation states among actinoids than those of lanthanoids.
Answer:
(i) The catalytic activity of transition elements is attributed to the following reasons:

  • Because of their variable oxidation states transition metals form unstable intermediates and provide a new path of lower activations energy for the reaction.
  • In some cases, the transition metal provides a suitable large surface area with free vacancies, on which reactants are absorbed.

(ii) This is due to filling of 4/orbitals which have poor shielding effect or due to lanthanoid contraction.
(iii) This is due to comparable energies of 5f, 5d and 7s orbitals in actinoids.

Question 9.
Calculate the number of unpaired electrons in the following gaseous ions.
Mn+3, Cr+3, V+3 and Ti+3 Which one of these is the most stable in an aqueous solution?
Answer:
Mn+3 = [Ar] 3d4 – 4 unpaired electrons
Cr+3 = [Ar] 3d3 – 3 unpaired electrons
V+3 = [Ar] 3d2 – 2 unpaired electrons
Ti+3 = [Ar] 3d1 – 1 unpaired electron
Cr+3 is most stable as it is half-filled t2g level.

Question 10.
The electronic configuration of chromium and copper are [Ar] 3d5 4s1 and [Ar] 3d10 4s1 respectively instead of [Ar] 3d4 4s2 and [Ar] 3d9 3s2. Explain.
Answer:
The electronic configuration [Ar] 3d5 4s1 and [Ar] 3d10 4s1 is more stable than the other because of the extra stability of half filled and completely filled ‘d’ orbitals. This extra stability is due to the symmetrical distribution of electron density.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 11.
The melting and boiling points of Zn, Cd and Hg are low why? (or) Why Zn, Cd and Hg are soft and have low melting points?
Answer:
In Zn, Cd and Hg, all the electrons in the ‘d’ orbitals are paired. Hence metallic bonding present in than are weak. Hence, the attraction between the constituent atoms are weak, i.e., they have low melting and boiling points.

Question 12.
Account for the trend in melting points of 3d series.
Answer:
The melting point first increases as the number of unpaired ‘d’ electrons available for metallic bonding increases, reaches a maximum and then decreases, as the ‘d’ electrons pair up and becomes unavailable for metallic bonding. The maximum melting point is in the middle, where the transition metal has d5 configuration. This results in the formation of strong metallic bonding, which results in the maximum melting point in the middle of the series.

Question 13.
Explain why manganese has a lower melting point than chromium.
Answer:
The electronic configuration of chromium is [Ar] 3d5 4s1 and that of manganese is [Ar] 3d5 4s2 i.e., in manganese-all the ‘d’ orbitals are singly filled and the 4s orbital is completely filled. As the ‘d’ electrons are more tightly held by the nucleus, the electrons are not available for bonding resulting in weaker metallic bonding in manganese compared to chromium.

Question 14.
The second and third members of each group of transition elements have similar atomic radii- Explain.
Answer:
This is due to lanthanide contraction by members of 4f series, which occupy a position between lanthanum (at. no. 57) a first member of 3rd transition series and hafnium (Z = 72), the second member of third transition series.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 3
The pairs of elements Zr – Hf, Nb – Ta, Mo – Wo, possess nearby atomic radii and almost have the same properties.

Question 15.
The atomic radii of the elements in a transition series do not vary much while they do vary in case of ‘s’ and ‘p’ block elements explain.
Answer:
In transition elements two effects are operating, viz nuclear charge effect and screening effect which oppose each other. Due to an increase in nuclear charge from member to member in a transition series the atomic radii tend to decrease. At the same time, the addition of extra electrons in (n – 1 )d orbital provides the screening effect. As the number of ‘d’ electrons increases, the screening effect increases and this tends to increase the size. Due to these opposing tendencies, there is a small change in the atomic radii in a transition series.
In ‘s’ and ‘p’ block elements, the extra electron is added to the same ‘s’ or ‘p’ subshell which does not exert a screening effect and hence, the atomic radii considerably in a period due to an increase in nuclear charge.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 16.
How would you account for the following?
(i) The atomic radius of metals of the third (5d) series of elements are virtually the same as those of corresponding members of the second (4d) series.
(ii) Chromium is a typical hard metal while mercury is a liquid.
Answer:
(i) Due to lanthanoid contraction.
(ii) Chromium has five unpaired electrons in the ‘d’ subshell (3d5 5s1). Hence metallic bonds are very strong. In mercury, all the ‘d’ orbitals are fully filled (3d10 4s2). Hence, metallic bonding is weak and thus it exists as a liquid.

Question 17.
How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of transition metals?
Answer:
Reason for irregular variation of first IE: Generally moving from left to right in a period IE increase because of increase in nuclear charge. The irregular trend is observed, when an electron is removed, the relative energies of 3d and 4s orbitals are altered. Thus there is a reorganisation of energy accompanying ionisation. This results in the release of exchange energy which increases as the number of electrons increases in the ‘d’ configuration and also from the transfer of ‘s’ electrons into ‘d’ orbitals. Chromium has the first low IE because of the loss of one electron gives a stable configuration (d5). Zn has high IE because the electron has to be removed from 4s orbital of the stable configuration (3d10 4s2)
Reason for irregular variation of second IE: After the loss of one electron, the removal of the second electron is difficult. Hence, second IE is much higher and in a general increase from left to right. Cr and Cu show much higher values because the second electron has to be removed from the stable configuration. Cr+(3d5) and Cu+(3d10).

Question 18.
Compare the stabilities of Ni+4 and Pt+4 from their ionisation enthalpy values.
Answer:

IENiPt
I737864
II17531791
III33952800
IV52974150

The smaller the magnitude of the ionisation energy, the more stable is the compound in a particular oxidation state. Nickel (II) compounds are more stable than Pt(II) compounds while Pt(IV) compounds are more stable than Ni(IV) compounds. The sum of the first two and first four IE of nickel and platinum are given below.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 45
Since the first two ionisation energies is less for nickel than platinum, Ni(II) compounds are more stable than platinum.
On the other hand, Pt(IV) compounds are more stable than Ni(IV) compounds as the seem of the first four IE values are less than for Pt the Ni.

Question 19.
The silver atom has completely ‘d’ orbitals (4d10) in its ground state. How can you say that it is a transition element?
Answer:
The electronic configuration of Ag (z = 47) to 4d10 5s1. In addition to +1, it shows an oxidation state of +2 (eg: Ag2O, and F2). i.e., d9 configuration i.e., the ‘d’ orbital is incompletely filled. Hence, it is a transition element.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 20.
Which of the 3d transition metals exhibit the largest number of oxidation states? and why?
Answer:
Manganese (z = 25) shows a maximum number of oxidation states. This is because its electronic configuration is 3d5 4s2. As 3d and 4s are close in energy, it has a maximum number of electrons to lose or share (all the 3d electrons are unpaired) Hence, it shows oxidation state +2 to +7.

Question 21.
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Answer:
Oxygen and fluorine have small sizes and high electronegativity. Hence they can oxidise the metal to its highest oxidation state.

Question 22.
What may be the stable oxidation state of the transition element with the following ‘d’ electronic configuration in the ground state of their atoms? 3d3, 3d5, 3d8 and 3d4.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 4
The maximum oxidation state corresponds to the sum of the ‘5’ and ‘cf electrons in Upto Mn. After that there is an abrupt decrease in the stability of the higher oxidation state.

Question 23.
Why are Mn+2 compounds are more stable than Fe+2 compounds towards oxidation to +3 state?
Answer:
The electronic configuration of Mn is 3d5. Which is half-filled and hence stable. So, the third ionisation enthalpy is very high, i.e., 3rd electron cannot be removed easily. In the case of Fe+2, (3d6), it can lose one more electron to attain the stable (d5) configuration.

Question 24.
Explain briefly how +2 oxidation state becomes more and more stable in the first half of first-row transition elements with increasing atomic number.
Answer:
The sum of IE1, and IE2 increases. Thus, the standard reduction potential becomes less and less negative. Therefore, the tendency to form M+2 ion decreases. The greater stability of +2 state, say for Mn, is due to half-filled (d5) configuration and that for Zn is due to completely filled ‘d’ orbitals. That for nickel is due to the highest negative enthalpy of hydration.

Question 25.
To what extent do the electronic configuration decide the stability of oxidation states in the first series of transition elements? Illustrate your answer with an example.
Answer:
The stability of the oxidation state in the first transition elements are related to their electronic configuration.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 5
The first five elements of the first transition series up to Mn in which 3d subshell is not more than half-filled, the minimum oxidation state is given by the number of electrons in the outer s – subshell and the maximum oxidation state is given by the sum of outer ‘s’ and ‘d’ electrons.

Question 26.
Explain why E°(Mn+3/Mn+2) couple is more positive than for E°(Fe+3/Fe+2) (At.no.of Mn = 25; Fe = 26).
Answer:
The electronic configuration of Mn+2 is Mn+2 = [Ar] 3d5; Mn+3 is 3d4 and that of Fe+2 = [Ar] 3d6; Fe+3 is [Ar] 3d5.
Thus Mn+2 has a more stable configuration than Mn+3 while Fe+3 has a more stable configuration than Fe+2. Consequently, large third ionisation enthalpy is required to change Mn+2 to Mn+3. As E° values is the sum of the enthalpy of atomisation, ionisation enthalpy and hydration enthalpy, therefore E° for Mn+3/ Mn+2 couple is more positive than Fe+3/Fe+2.
Note: The large positive E° for Mn+3/ Mn+2 means that Mn+3 can be easily reduced to Mn+2 (Mn+3 + e → Mn+2) i.e., Mn+3 is less stable, i.e., Fe+3 can be reduced to Fe+2 (Fe+3 + e → Fe+2 but ion easily. Thus, Fe+3 is more stable than Mn+3.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 27.
The E°values in respect of the electrodes of chromium (z = 24), manganese (z = 25) and iron (z = 26) are: Cr+3/Cr+2 = – 0.4V, Mn+3/Mn+2 = 1.5V; Fe+3/Fe+2 – 0.80V. On the basis of the above information compare the feasibilities of further oxidation of their +2 oxidation states.
Answer:
Cr+3 + e -> Cr+2: E° value is -0.4V. The negative value means Cr+3 is more stable or Cr+2 is less stable. Mn+3 + e → Mn+2: E° value is 1.5V. Fe+3 + e → Fe+2: E° value is 0.80V. Greater positive value for Mn+3/Mn+2 than that for Fe+3/Fe+2 shows that Mn+2 is more stable than Fe+2. Hence, the stability of +2 oxidation state is in the order Cr+2 < Fe+2 < Mn+2 or oxidation of their +2 state is in the order Cr+2 > Fe+2 > Mn+2.

Question 28.
The E°(M+2/M) value for copper is positive 0.34V. Explain why?
Answer:
E°(M+2/M) for any metal is related to the sum of the enthalpy change taking place in the following steps.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 6
Copper has a high enthalpy of atomisation and low enthalpy of hydration. Thus, high energy required to transform Cu(s) to Cu+2(aq) is not balanced by its hydration enthalpy Hence E°(Cu+2/Cu) is positive.

Question 29.
Which is a stronger reducing agent Cr+2 or Fe+2 and why?
Answer:
E°(Cr+3/Cr+2) = -0.41V and E°(Fe+3/Fe+2) is 0.77V.
In general, for the reduction reaction Mn+ + ne → M,
Larger the value of standard reduction potential, greater the extent to which Mn+ is reduced to M. i.e., Mn+ acts as an oxidising agent. Compare
Cr+3 + e → Cr+2 E° = -0.41V
Fe+3 + e → Fe+2 E° = 0.77V.
The negative value indicates that Cr+2 is readily oxidised to Cr+3 i.e., it is a stronger reducing agent than Fe+2.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 30.
Explain the terms paramagnetism and diamagnetism with suitable examples.
Answer:

  1. A paramagnetic substance is one that is weakly attracted into a magnetic field and a diamagnetic substance is one that is repelled by a magnetic field.
  2. The paramagnetic behaviour arises due to the presence of one or more unpaired electrons, while a diamagnetic substance is due to the presence of paired electrons.
  3. For example Sc+3 has no unpaired electron and hence diamagnetic whereas Ti+3 has one unpaired electron and hence paramagnetic.

Question 31.
Calculate the magnetic moment of the following ions.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 7
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 8

Question 32.
Explain how transition metals and their compounds act as catalysts.
Answer:
Transition metal has energetically available ‘d’ orbitals that can accept electrons from reactant molecule or metal can form a bond with reactant molecule using its ‘d’ electrons. For example, in the catalytic hydrogenation of an alkene, the alkene bonds to an active site by using its π electrons with an empty ‘d’ orbital of the catalyst.
The σ bond in the hydrogen molecule breaks and each hydrogen atom forms a bond with a ‘d’ electron on an atom in the catalyst. The two hydrogen atoms then bond with the partially broken π -bond in the alkene to form an alkane.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 9

Question 33.
Give examples wherein transition metal compounds act as catalysts in various industrial processes.
Answer:

  1. In the manufacture of sulphuric acid from sulphur trioxide, vanadium pentoxide is used as a catalyst.
  2. Hydroformylation of olefins
    TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 10
  3. Preparation of acetic acid from acetaldehyde.
    TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 11
  4. Zeigler – Natta catalyst
    A mixture of TiCl4 and trialkyl aluminium is used for polymerization.
    TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 12

Question 34.
What is an alloy? How are they formed?
Answer:
An alloy is a mixture of two or more metals. They are formed when molten metals are mixed together and allowed to crystallise, eg: ferrous alloys, gold – copper alloy, chrome alloys etc.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 35.
Explain why transition metals have a tendency to form alloys.
Answer:
For the formation of alloy, the following conditions have to be met.

  1. Both the solute and the solvent must have the same crystal structure.
  2. Their valence and their electronegativity difference must be close to zero. Transition metals satisfy these conditions. Their atomic sizes are similar and one metal atom can be easily replaced by another metal atom from its crystal lattice to form an alloy.

Question 36.
What are interstitial compounds? Give examples.
Answer:
An interstitial compound or alloy is a compound that is formed when small atoms like hydrogen, boron, carbon or nitrogen are trapped in the interstitial holes in a metal lattice. They are usually non-stoichiometric compounds. Transition metals form a number of interstitial compounds such as TiC, ZrH1.92, Mn4N etc., The elements that occupy the metal lattice provide them new properties.

Question 37.
Mention the properties of interstitial compounds.
Answer:

  1. They are hard and show electrical and thermal conductivity.
  2. They have high melting points higher than those of pure metals.
  3. Transition metal hydrides are used as powerful reducing agents.
  4. Metallic carbides are chemically inert.

Question 38.
What are complexes or coordination compounds? Give a brief account of complexes formed by transition metals.
Answer:
Complexes or coordination compounds are these in which a transition metal ion accept a pair of electrons, from a fixed number of compounds in which the central atom can denote a pair of electrons and form coordinate covalent bonds.
eg: [Fe(CN)6]4-. In this complex, Fe+2 ion accepts lone pair of electrons from the cyanide ion and form 6 coordinate covalent bonds. Transition metal ions form complexes due to their small size and high charge and have vacant ‘d’ orbitals to accept electron pairs denoted by other groups.

Question 39.
Give a brief account of oxides formed by transition metals.
Answer:

  1. The metals of the first transition series form oxides with oxygen at high temperatures.
  2. The oxidation state of the metal in the oxides vary from +1 to +7.
  3. The highest oxidation state in the oxides of any transition metal is equal to its group number eg: +7 in Mn2O7. Beyond group 7. No higher oxides of iron above Fe2O3 are known.
  4. All the metals except scandium form oxides of the formula MO which are ionic in nature. As the oxidation number of the metal increases, ionic character decreases, eg: Mn2O7 is covalent even CrO3, V2O5 are covalant and have low melting point.
    TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 13
  5. In general, the oxides in the lower oxidation states of the metals are basic and in their higher oxidation states they are acidic. Whereas in the intermediate oxidation states they are amphoteric.
    TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 14

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 40.
Classify the following oxides as acidic, basic and amphoteric
(a) Mn2O7, (b) CrO3, (c) Cr2O3, (d) CrO.
Answer:
(a) Mn2O7 → acidic
(b) CrO3 → acidic
(c) Cr2O3 → amphoteric
(d) CrO → basic.

Question 41.
Give example and suggest the reason for the following:
(i) The lowest oxide of transition metal is basic, the highest is acidic.
(ii) A transition metal exhibits higher oxidation states in oxides and fluorides.
(iii) The highest oxidation state is exhibited in oxo anion of a metal.
Answer:
(i) The lower oxide of a transition metal is basic because the metal atom has a low oxidation state whereas the highest oxide is acidic due to a higher oxidation state for example, MnO is basic while Mn2O7 is acidic.
(ii) A transition metal exhibits a higher oxidation state in oxides and fluorides because oxygen and fluorine are highly electro negative elements, small in size (and strongest oxidising agents). For example, osmium shows an oxidation state of +6 in O5F6 and vanadium shows an oxidation state of +5 in V2O5.
(iii) Oxo metal anion have the highest oxidations state, eg: Cr in Cr2O7-2, has an oxidation state of +6, whereas Mn in MnO4 ion has an oxidation state of +7. This again due to the combination of the metal with oxygen which is a highly electronegative and oxidising element.

Question 42.
Indicate the steps involved in the preparation of (i) K2Cr2O7 from chromite (ii) KMnO4 from pyrolusite
Answer:
(i) K2Cr2O7 from chromite are
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 15
K2Cr2O7 is separated by fractional crystallisation.
(ii) KMnO4 from pyrolusite are
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 16
KMnO4 is prepared from pyrolusite. MnO2 with KOH in the presence of an oxidising agent like KNO3. This produces dark brown potassium manganate which disproportionates in a neutral or acidic solution to give purple permanganets.

Question 43.
Give chemical oxidation and electrolytic oxidation of MnO4-2 to MnO4.
Answer:
Chemical oxidation: In this method potassium manganate is treated with ozone (O3) or chlorine to get potassium permanganate.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 17
Electrolytic oxidation: In this method aqueous solution of potassium manganate is electrolyzed in the presence of little alkali.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 18
Manganate ions are converted into permanganate ions at anode.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 19
H2 is liberated at the cathode.
2H+ + 2e → H2 ↑
The purple coloured solution is concentrated by evaporation and forms crystals of potassium permanganate on cooling.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 44.
What happens when potassium dichromate is heated? Give equation.
Answer:
It decomposes to give green Cr2O3 and oxygen.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 20

Question 45.
Discuss the action of alkali on potassium dichromate.
Answer:
When an alkali is added to an orange-red solution of potassium dichromate, a yellow solution results due to the formation of chromate.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 21

Question 46.
What is the effect of pH on a solution of potassium dichromate?
Answer:
In aqueous solution
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 22
In acidic medium (i.e., decreasing pH), the equilibrium shifts backwards and the colour is orange-red. In a basic medium, (i.e., increasing pH) the equilibrium will shift forward and the solution is yellow.

Question 47.
Draw the structure of the dichromate ion.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 23

Question 48.
Write the ionic equation to show that K2Cr2O7 is an oxidising agent in an acid medium.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 24

Question 49.
Complete and balance the following equation: (all in acid medium)
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 25
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 26

Question 50.
Describe the chromyl chloride test.
Answer:
When potassium dichromate is heated with any chloride salt in the presence of Conc. H2SO4, orange-red vapours of chromyl chloride (CrO2Cl2) is evolved. This reaction is used to confirm the presence of chloride ions in inorganic qualitative analysis.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 27
The chromyl chloride vapours are dissolved in sodium hydroxide solution and then acidified with acetic acid and treated with lead acetate. A yellow precipitate of lead chromate is obtained.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 28

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 51.
Mention the uses of potassium dichromate.
Answer:

  1. It is used as a strong oxidizing agent.
  2. It is used in dyeing and printing.
  3. It used in leather tanneries for chrome tanning.
  4. It is used in quantitative analysis for the estimation of iron compounds and iodides.

Question 52.
Draw the structure of MnO4 ion.
Answer:
Permanganate ion has tetrahedral geometry in which the central Mn7+ is sp3 hybridised.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 29

Question 53.
What happens when:
(i) potassium permanganate is heated.
(ii) is heated with cold conc. H2SO4
(iii) is heated with hot conc. H2SO4?
Answer:
(i) It decomposes to form potassium
manganate and manganese dioxide.
2KMnO4 → 2K2MnO4 + MnO2 + O2
(ii) It decomposes to form manganese heptoxide which subsequently decomposes explosively.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 30
(iii) It gives manganous sulphate
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 31

Question 54.
How does potassium permanganate act as an oxidising agent in the neutral medium? Explain with examples.
Answer:
In neutral medium, KMnO4 is reduced to MnO2.
MnO4 + 2H2O + 3e → MnO2 + 4OH
(i) It oxidises H2S to sulphur
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 32
(ii) It oxidises thiosulphate into sulphate
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 33

Question 55.
Write an ionic equation or the half-reaction for the oxidising action of KMnO4 in an alkaline medium.
Answer:
MnO4 + 2H2O + 3e → MnO2 + 4OH

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 56.
What is Bayer’s reagent? Mention its use.
Answer:
Cold dilute alkaline KMnO4 is known as Bayer’s reagent. It is used to oxidise alkenes into diols. For example, ethylene can be converted into ethylene glycol and this reaction is used as a test for unsaturation.

Question 57.
What is the action of acidified KMnO4 on
(i) ferrous salts,
(ii) Potassium iodide,
(iii) Oxalic acid
(iv) Sulphide ion,
(v) nitrite ion,
(vi) Sulphite ion.
Answer:
(i) It oxidises ferrous salts to ferric salts
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 34
(ii) It oxidises iodide ion to iodine
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 35
(iii) It oxidises oxalic acid to carbon dioxide.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 36
(iv) It oxidises sulphide ion to sulphur.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 37
(v) It oxides nitrite ion to nitrates
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 38
(vi) It oxidises sulphite ion to sulphates.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 39

Question 58.
Mention the uses of potassium permanganate.
Answer:

  1. It is used as a strong oxidizing agent.
  2. It is used for the treatment of various skin infections and fungal infections of the foot.
  3. It is used in water treatment industries to remove iron and hydrogen sulphide from well water.
  4. It is used as a Bayer’s reagent for detecting unsaturation in an organic compound.
  5. It is used in quantitative analysis for the estimation of ferrous salts, oxalates, hydrogen peroxide and iodides.

Question 59.
Find the equivalent weight of KMnO4 is an acidic, basic and neutral medium.
Answer:
The ionic equation is
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 40
In basic medium:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 41
In neutral medium:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 42

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 60.
What are inner transition elements?
Decide which of the given atomic numbers are the numbers of inner transition elements: 29, 59, 74, 95, 102, 104.
Answer:
The ‘f’ block elements i.e., in which the last electron enters the ‘f’ sub shell are called inner transition elements. These include lanthanides (58 – 71) and actinides (90 – 103). Thus, the elements with atomic numbers 59,95 and 102 are inner transition elements.

Question 61.
The chemistry of actinoid elements is not so smooth as that of lanthanoids justify then statement by giving some examples from the oxidation state of these elements.
Answer:
Lanthanoids show a limited number of oxidation states viz +2, +3, +4 out of which +3 is most common. This is because of the energy gap between 4f and 5d sub shells. The dominant oxidation state of actinides is also +3 but they show a number of oxidation states also eg: uranium (Z = 92) and polonium (Z = 92) show +3, +4 and +5 and +6, neptunium (Z = 94) shows +3, +4, +5 and +7 etc., This is due to small energy diffidence between 5f, 6d and7s subshells.

Question 62.
What is the last element in the series f actinoids? Comment on the possible oxidation state of the element.
Answer:
Last actinoid: Lawrencium (Z = 103).
Electronic configuration; [Rn]86 5f14 6d1 7s2. possible oxidation state = +3.

Question 63.
Name of the members of the lanthanoid series which exhibit +4 oxidation state. Try to correlate this type of behaviour with the electronic configuration of these elements.
Answer:
+4: Ce(Z=58), Pr(Z=59), Nd(Z=60), Tb(Z=65), Dy(Z = 66)
+2: Nd(Z = 60); Sm(Z = 62); Eu(Z = 63), Tm(Z = 69); Yb(Z = 70)
+2 Oxidation state is exhibited when lanthanoid has the configuration 5d0 6s2. So that 2 electrons one easily lost. +4 state is exhibited when the electronic configuration left to close to 4f0 (eg: 4f0, 4f1, 4f2) or close to 4f7 (eg: 4f7 or 4f8)

Question 64.
Write the electronic configuration of the elements with atomic numbers 61, 91, 101 and 109.
Answer:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 43

Question 65.
Compare the chemistry of actinoids with that of lanthanoids with special reference to
(i) electronic configuration
(ii) Oxidation state
(iii) Atomic and ionic radii
(iv) Chemical reactivity
Answer:
(i) The general electronic configuration of lanthanoids is [Xe]54 4f1-14 5d0-1 6s2 where as that of actinoids in [Rn]86 5f1-14 6d0-1 7s2. Thus lanthanoids belong to 4f series whereas actinoids belong to 5f series.
(ii) Lanthanoids show limited oxidation states (+2, +3, +4) out of which +3 is most common. This is because of the large energy gap between 4f and 5d subshells. On the other hand, actinoids show a large number of oxidation states because of a small energy gap between 5f, 6d and 7s subshells.
(iii) Both show a decrease in the size of their atoms or ions in the +3 oxidation state. In lanthanoids, this decrease is called lanthanoid contraction, whereas in actinoids it is called actinoid contraction. However, the contraction is greater from element to element in actinoids due to poor shielding of 5f electrons than that by 4f electrons in lanthanoids.
(iv) Chemical reactivity of lanthanoids
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 44
The chemical behaviour of actinoids:

  1. They react with boiling water to give a mixture of hydride and oxide.
  2. They combine with most of the non-metals at high temperatures.
  3. All these metals are attacked by hydro chloric acid, but the effect of nitric acid is very small due to the formation of a protective oxide layer on their surface.
  4. Alkalies have no action on actinoids.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 66.
The +3 oxidation state of lanthanium (Z = 57), gadoliniun (Z = 64) and lutetium (Z = 71) are especially stable. Why?
Answer:
This is because that is the +3 oxidation state, they have empty, half-filled and completely filled 4f sub shell respectively.

Question 67.
The outer electronic configuration of two members of the lanthanoid are as follows:
(i) 4f1 5d1 6s2 and (ii) 4f7 5d0 6s2
What are their atomic numbers predict the oxidation state exhibited by these elements in their compounds?
Answer:
Complete Electronic configuration of the (i) lanthanoid:
[Xe]54 4f1 5d1 6s2: Atomic number = 58
The element is cerium.
Complete Electronic configuration of the (ii) lanthanoid:
[Xe]54 4f7 5d0 6s2: Atomic number = 68.
The element is Europium (Eu).
Oxidation state of 1st lanthanoid +2(4f2) +3(4f1) and +4(4f0)
Oxidation state of the 2nd lanthanoid:
+2(4f7) and +3(4f6)

Question 68.
Give an explanation for each of the following observations.
(i) The gradual decrease in size (actinoid contraction) from element to element is greater among actinides than that among lanthanides.
(ii) The actinoids exhibit a greater range of oxidation states than the lanthanoids.
(iii) Zv and Hf have identical sizes.
(iv) Ionisation enthalpies of Ce, Pr and Nd are higher than Th, Pa and Cl. Why?
(v) Ce+4 is used as an oxidising agent in volumetric analysis.
Answer:
(i) This is due to poor shielding by 5f electrons from element to element in actinoids than by 4f electrons in lanthanoid series.
(ii)This is because there is less energy difference between 5f and 6d orbitals belonging to actinoids than the energy difference between 4f and 5d Orbitals in the case of lanthanoids.
(iii) This is due to lanthanoid contraction.
(iv) It is because at the beginning, where 5f orbitals begin to be occupied they will penetrate less into the inner core of electrons. The 5felectron will therefore be more effectively shielded from the nuclear charge than 4f electrons of the corresponding lanthanoids. Therefore the outer electrons are less firmly held and they are available for bonding in the actinoids.
(v) Ce+4 has a tendency to attain +3 oxidation state and so it is used as an oxidising agent in volumetric analysis.

Question 69.
Account for the following:
(i) Europium (II) is more stable than cerium(II)
(ii) Actinoid ions are generally coloured.
Answer:
(i) Europium has stable configuration i.e., [Xe] 4f7 5d0 6s0.
(ii) Unpaired electrons are present in their ions which undergo f-f transition.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

Question 70.
On the basis of lanthanoid contraction, explain the following:
(i) Nature of bonding in La2O3 and Lu2O3.
(ii) Trends in the stability of oxosaltes of lanthanoids from La to Lu.
(iii) Stability of complexes of lanthanides.
(iv) Radii of 4d and 5d block elements.
(v) Trends in the acidic character of lanthanoid oxides.
Answer:
(i) As the size decreases, the covalent character increases. Therefore La2O3 is more ionic and Lu2O3 is more covalent.
(ii) As the size decreases from La to Lu, the stability of oxo salts also decreases.
(iii) Stability of the complexes increases as the size of the lanthanoid decreases.
(iv) Radii of 4d and 5d block elements are will be almost the same.
(v) Acidic character of the oxides increases from La to Lu.

Question 71.
What is meant by the term Lanthanoid contraction? What is it due to and what consequences does it have on the chemistry of lanthanides in the periodic table.
Answer:
Lanthanide contraction: The steady decrease in atomic and ionic radii with an increase in atomic number is known as lanthanide contraction.
Causes of lanthanide contraction: As we move along the lanthanoid series, for every additional proton in the nucleus, the corresponding electron goes into 4f sub shell, there is poor shielding of one electron by another in the sub shell due to the shapes of these orbitals. This imperfect shielding is not able to counterbalance the effect on the increased nuclear charge. Thus, the net result is a decrease in size, with an increase in atomic number.
Consequences:

  1. 5d series elements have nearly the same radii as that of the 4d series.
  2. The basic strength of hydroxides decrease from La(OH)3 to Lu(OH)3

Choose the correct answer.

1. The correct order of decreasing second ionisation enthalpy of Ti(22), V(23), Cr(24) and Mn(25) is:
(a) Cr > Mn > V > Ti
(b) V > Mn > Cr > Ti
(c) Mn > Cr > Ti > V
(d) Ti > V > Cr > Mn
Answer:
(a) Cr > Mn > V > Ti
Hint: Electronic configuration of the given elements are
Ti = [Ar] 3d2 4s2; V = [Ar] 3d3 4s2 Cr = [Ar] 3d5 4s1; Mn = [Ar] 3d5 4s2
Their effective nuclear charge increases from Ti to Mn. Hence their first IE increases in the same order, i.e., Mn > Cr > V > Ti. However after the removal of first electron, chromium attains the stable configuration [3d5] and hence, it has very high second IE. For the remaining elements the trend remains the same. Thus, the second IE will be in the order.
Cr > Mn > V >Ti

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

2. The electronic configuration of Cu(II) is 3d9 whereas that of Cu(I) is 3d10. Which of the following is correct?
(a) Cu(II) is more stable.
(b) Cu(II) is less stable.
(c) Cu(I) and Cu(II) are equally stable.
(d) Stability of Cu(I) and Cu(II) salts depends on the nature of copper salts.
Answer:
(a) Cu(II) is more stable.
Hint: Though Cu(I) has 3d10 configurations Cu(II) is more stable. This is due to greater effective nuclear charge of Cu(II). i.e., to hold 17 electrons instead of 18 electrons is Cu(I).

3. Although zirconium belongs to 4d transition series and Hafnium belongs to 5d transition series even their they have similar physical and chemical properties because:
(a) both belong to ‘cf block
(b) both have same number of electrons
(c) both have similar atomic radius
(d) both belong to the same group of the periodic table.
Answer:
(c) both have similar atomic radius

4. Why HCl is not used to make the medium acidic in oxidation reactions of KMnO4 in acidic medium?
(a) Both HCl and KMnO4 act as oxidising agents.
(b) KMnO4 oxidises HCl, to Cl2, which is also an oxidising agent.
(c) KMnO4 is a weaker oxidising agent than HCl.
(d) KMnO4 acts as a reducing agent in the presence of HCl.
Answer:
(b) KMnO4 oxidises HCl, to Cl2, which is also an oxidising agent.

5. KMnO4 acts as an oxidising agent in acidic medium. The number of moles of KMnO4 that will be needed to react one mole of sulphide ions in acidic solution is:
(a) \(\frac{2}{5}\)
(b) \(\frac{3}{5}\)
(c) \(\frac{4}{5}\)
(d) \(\frac{1}{5}\)
Answer:
(a) \(\frac{2}{5}\)
Hint:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 46
2 mol of KMnO4 ≡ 5 mol H2S
\(\frac{2}{5}\) mol of KMnO4 ≡ 1 mol of H2S

6. Which one of the following ions is the most stable in aqueous solution:
Note: Atomic No: Ti = 22, V = 23, Cr – 24, Mn = 25.
(a) Mn+2
(b) Cr+3
(c) V+3
(d) Ti+3
Answer:
(b) Cr+3
Hint: Out of the given species, Cr+3 has the highest negative reduction potential. Hence, it cannot be reduced to Cr+2 and therefore is the most stable in aqueous solution.
Alternatively, Mn+3 = [Ar] 3d4, Cr+3 = [Ar] 3d3, V+3 = [Ar] 3d2, Ti+2 = [Ar] 3d1. In Cr+3, all the three electrons enter the lowest energy 3d1(t2g ) orbitals. The lowering of the energy is maximum and hence the stability is maximum.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

7. In acidic medium MnO4-2:
(a) disproportionates to MnO2 and MnO4
(b) is oxidised to MnO4
(c) reduced to MnO2
(d) is reduced to Mn+2
Answer:
(a) disproportionates to MnO2 and MnO4
Hint:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 47

8. Consider the following statements:
(i) La(OH)3 is the least basic among hydroxides of lanthanides
(ii) Zn+4 and Hf+4 possess almost same ionic radii
(iii) Ce+4 can act as oxidising agent. Which of the above is/are true?
(a) All
(b) (ii) and (iii)
(c) (ii) only
(d) (i) and (iii)
Answer:
(b) (ii) and (iii)
Hint: La(OH)5, is most basic, i.e., (i) is wrong.
(ii) is correct due to lanthanide contraction.
(iii) is correct because Ce+4 tends to change to stable Ce+3.

9. Large number of oxidation states are exhibited by actinoids than these by the lanthanoids, the main reason being:
(a) more energy difference between 5f and 6d than between 4f and 5d orbitals.
(b) more reactive nature of the actinoids than the lanthanoids.
(c) 4f orbitals more diffused than 5f orbitals.
(d) less energy difference between 5f and 6d than between 4f and 5d orbitals.
Answer:
(d) less energy difference between 5f and 6d than between 4f and 5d orbitals.

10. Irregular trend in the standard reduction potential value of the first row transition elements is due to:
(a) regular variation of first and second row enthalpies.
(b) irregular variation of sublimation enthalpies.
(c) regular variation of sublimation enthalpies.
(d) increase in number of unpaired electrons.
Answer:
(b) irregular variation of sublimation enthalpies.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

11. Match the property in column I with the metals in column II.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 48
(a) (i) – (C); (ii) – (A); (iii) – (B)
(b) (i) – (C); (ii) – (D); (in) – (A)
(c) (i) – (B); (ii) – (C); (iii) – (D)
(d) (i) – (D); (ii) – (C); (iii) – (A)
Answer:
(a) (i) – (C); (ii) – (A); (iii) – (B)

12. Match statements given in column I with the oxidation states given in column II.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 49
(a) (i) – (C); (ii) – (A); (iii) – (E); (iv) – (B)
(b) (i) – (B); (ii) – (C); (iii) – (D); (iv) – (A)
(c) (i) – (D); (ii) – (B); (iii) – (C); (iv) – (A)
(d) (i) – (E); (ii) – (C); (iii) – (A); (iv) – (B)
Answer:
(a) (i) – (C); (ii) – (A); (iii) – (E); (iv) – (B)

13. Knowing that the chemistry of lanthanoids
(Ln) is determined by its +3 oxidation state, which of the following statement is incorrect?
(a) The ionic size of Ln(III) decrease in general with increasing atomic number.
(b) Ln(III) compounds are generally colourless.
(c) Ln(III) hydroxides are mainly basic in character.
(d) Because of large size of Ln(III) ions the bonding in its compounds is predominantly ionic in character.
Answer:
(b) Ln(III) compounds are generally colourless.
Hint: Ln(III) compounds are generally coloured due to partly filled f orbitals which permit f-f transition.

14. Which of the following statements regarding cerium (atomic no.58) is incorrect?
(a) The common oxidation states of cerium are +3 and +4.
(b) +3 oxidation state of Ce is more stable than +4.
(c) The +4 oxidation state of Ce is not known in solution.
(d) Cerium (IV) acts as an oxidising agent.
Answer:
(c) The +4 oxidation state of Ce is not known in solution.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

15. MnO4 reacts with Br in alkaline pH to give:
(a) BrO3, MnO2
(b) Br2, MnO4-2
(c) Br2, MnO2
(d) BrO, MnO4-2
Answer:
(a) BrO3, MnO2
Hint:
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 50

16. Amount of oxalic acid present in a solution can be determined by titration with KMnO4 solution in the presence of H2SO4. The titration gives unsatisfactory result when carried out in the presence of HCl because HCl:
(a) reduces permanganate to Mn+2.
(b) oxidises oxalic acid to carbondioxide and water.
(c) gets oxidised by oxalic acid to chlorine.
(d) furnishes H+ ions in additional to those from oxalic acid.
Answer:
(a) reduces permanganate to Mn+2.
Hint: In the presence of HCl, KMnO4 not only oxidises oxalic acid but also oxidises HCl to Cl2 and itself reduced to Mn+2.

17. The spin only magnetic moment of Fe+2 (in Bμ) is approximately:
(a) 4
(b) 1
(c) 5
(d) 6
Answer:
(c) 5
Hint: Fe+2 = 3d6 4s0. It has 4 unpaired electron.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 51

18. Electronic configuration 6f a transition element X in +3 oxidation state is [Ar]3d5. What is its atomic number?
(a) 25
(b) 26
(c) 27
(d) 24
Answer:
(b) 26
Hint: X+3 = [Ar]18 3d5 = 23 electrons As X+3 ion is formed by the loss of 3 electrons from X, X will have 26 electrons. Hence its at. no. = 26 V

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

19. Metallic radii of some elements are given below: Which of these elements will have highest density?

ElementFeCoNiCu
Metallic radii/pm126125125128

(a) Fe
(b) Ni
(c) Co
(d) Cu
Answer:
(d) Cu
Hint: \(\text { Density }=\frac{\text { mass }}{\text { volume }}\)
As we move from Fe to Cu mass increases and volume decreases. Hence, density increases. Increase in mass of Cu dominates over small increase in volume.

20. The magnetic nature of elements depends on the presence of unpaired electrons. Identify the configuration of transition element which shows highest magnetic moment:
(a) 3d7
(b) 3d5
(c) 3d8
(d) 3d2
Answer:
(b) 3d5
Hint: 3d5 has maximum number of impaired electron.

21. There are 14 elements in actinoid series which of the following elements does not belong to this series?
(a) Cl
(b) Np
(c) Tm
(d) Fm
Answer:
(c) Tm
Hint: Actinoid series is with atomic numbers 90 to 103. Thulium (Tm) has atomic number 69.

22. Gadolinium belongs to 4/series. Its atomic number is 64. Which of the following is the correct electronic configuration of gadolinium?
(a) [Xe] 4f7 5d1 6s2
(b) [Xe] 4f6 5d2 6s2
(c) [Xe] 4f8 6s2
(d) [Xe] 4f9 5s1
Answer:
(a) [Xe] 4f7 5d1 6s2
Hint: [Xe]54 4f7 5d1 6s2 due to extra stability of half filled 4f sub shell.

23. Highest oxidation state of manganese in fluoride is +4(MnF4) but the highest oxidation state in oxides is +7(Mn2O7) because:
(a) fluorine is more electronegative than oxygen.
(b) fluorine does not possess ‘d’ orbital.
(c) fluorine stabilises lower oxidation state.
(d) in covalent compounds, fluorine can form only single bonds white oxygen can form double bonds.
Answer:
(d) in covalent compounds, fluorine can form only single bonds white oxygen can form double bonds.

24. Assertion: Mercury is not considered as a transition element.
Reason: Mercury is a liquid.
(a) If both assertion and reason are true and the reason is the correct explanation of the assertion.
(b) If both assertion and reason are true but the reason is not the correct explanation of assertion.
(c) If an assertion is true, but the reason is false.
(d) If both assertion and reason are false.
Answer:
(b) If both assertion and reason are true but the reason is not the correct explanation of assertion.
Hint: Mercury has completely filled ‘d’ orbitals.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

25. Assertion: in any transition series the magnetic moment of M+2 ions first increases and then decreases.
Reason: in a transition series, the number of unpaired electrons increases and then decreases.
(a) if both assertion and reason are true and the reason is the correct explanation of the assertion.
(b) if both assertion and reason are true but the reason is not the correct explanation of assertion.
(c) if the assertion is true, but the reason is false.
(d) if both assertion and reason are false.
Answer:
(a) if both assertion and reason are true and reason is the correct explanation of the assertion.

26. Match the ions in list I with their corresponding property in list II.
TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements 52
(a) (i) – (B) & (C); (ii) – (A) & (D); (iii) – (B) & (C); (iv) – (C)
(b) (i) – (C); (ii) – (A) & (B); (iii) – (D); (iv) – (B) & (C)
(c) (i) – (B) & (C); (ii) – (B); (iii) – (A) & (D); (iv) – (B)
(d) (i) – (D); (ii) – (C); (iii) – (B); (iv) – (A), (D)
Answer:
(a) (i) – (B) & (C); (ii) – (A) & (D); (iii) – (B) & (C); (iv) – (C)

27. The complex forming tendency of a transition metal depends upon:
(a) the availability of number of vacant ‘d’ orbitals.
(b) high ionisation energy.
(c) large size of the cation or high charge density.
(d) variable oxidation states.
Answer:
(a) the availability of a number of vacant ‘d’ orbitals.

28. Which lanthanide is most commonly used?
(a) La
(b) No
(c) Th
(d) Ce
Answer:
(a) La

29. In which of the following pairs are both the ions coloured in an aqueous solution?
(a) Ni+2, Ti+3
(b) Ni+2, Cu+
(c) Sc+3, CO+2
(d) Sc+3, Ti+3
Answer:
(a) Ni+2, Ti+3
Hint: Ni+2 = [Ar] 3d8 t2g6 eg2. It has 2 unpaired electron in e level. Hence it is coloured.
Ti+3 = [Ar]3d1 one unpaired electron and hence coloured.

TN Board 12th Chemistry Important Questions Chapter 4 Transition and Inner Transition Elements

30. When manganese dioxide is fused with KOH or K2CO3 in air, it gives:
(a) potassium permanganate
(b) manganese oxide
(c) manganese heptoxide
(d) potassium manganate
Answer:
(d) potassium manganate