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INTERNATIONAL INDIAN SCHOOL, RIYADH

WORKSHEET (2020-2021)

GRADE - XII – CHEMISTRY - PREBOARD

UNIT 1 SOLID STATE

WORKSHEET 1 1. What are Bravais lattices?

2. Why are amorphous solids isotropic in nature?

3. Why glass is regarded as an amorphous solid?

4. Define the term 'crystal lattice.’

5. Name the crystal system for which all four types of unit cells are possible.

6. What is the total number of atoms per unit cell in a fcc crystal structure?

7. What difference in behaviour between the glass and sodium chloride would you expect

to observe, if you break off a piece of either cube?

8. Define the term voids.

9. What type of stochiometric defect is shown by

(i) ZnS and (ii) CsCl?

10.ZnO on heating turns yellow.why?

11. What is the coordination number for

(a) an octahedral void

(b) a tetrahedral void.

12. How many octahedral voids are there in 1 mole of a compound having cubic closed

packed structure?

13. Arrange simple cubic, bcc and fcc lattice in decreasing order of the fraction of the

unoccupied space.

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14. How much space is empty in a hexagonal closed packed

solid?

15. An element crystallises separately both in hcp and ccp structure. Will the two structures

have the same density? Justify your answer.

16. Write dimensions and bond angles of match-box type of unit

cells.?

[Hint : Orthorhombic crystal system].

17. Calculate the packing efficiency of FCC.

18. In NaCl crystal, Cl– ions form the cubic close packing. What sites are occupied by Na+

ions.

19. In Corundum, O2– ions from hcp and Al3+ occupy two third of octahedral voids.

Determine the formula of corundum.

20. Why is Frenkel defect not found in pure alkali metal halides?

Worksheet 2

1. List four distinctions between crystalline and amorphous solids with one

example of each.

2. Give suitable reason for the following–

(a) Ionic solids are hard and brittle. (b)

Copper is malleable and ductile.

3. Define F–centre. Mention its two consequences.

4. What is packing efficiency. Calculate the packing efficiency in body-centered cubic crystal.

5. Explain :

(a) List two differences between metallic and ionic crystals.

(b) Sodium chloride is hard but sodium metal is soft.

6. Account for the following :

(a) Glass objects from ancient civilizations are found to becomes milky in appearance.

(b) Window glass panes of old buildings are thicker at the bottom than at the top.

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7. Why is graphite soft lubricant and good conductor of electricity?

8. What do you understand by the following types of stacking sequences :

(a) AB AB . ............. (b) A B CABC .................

What kind of lattices do these sequences lead to?

9. Derive the formula for the density of a crystal whose length of the edge of the unit cell is

known?

10. Explain how much portion of an atom located at

(a) corner (b) body centre (c) face-centre and (d) edge centre of a

cubic unit cell, is part of its neighbouring unit cells.

11. In a fcc arrangement of A and B atoms. A are present at the corners of the unit cell and B

are present at the face centres. If one atom of A is missing from its position at the

corners, what is the formula of the compound?

12. A compound made up of elements ‘A’ and ‘B’ crystallises in a cubic closepacked structure.

Atom A are present on the corners as well as facecentres, whereas atoms B are present

on the edge-centres as well as body centre. What is the formula of the compound?

13. Explain the terms :

(a) Intrinsic semiconductor

(b) Extrinsic semiconductor.

14. Explain how vacancies are introduced in a solid NaCl crystal when divalent cations are

added to it.

15. What is meant by non-stoichiometric defect? Ionic solids which have anionic

vacancies due to metal excess defect develop colour. Explain with the help of suitable

example.

WORK SHEET -3

1. Sodium crystallises in a bcc unit cell. What is the approximate number of unit cells in 4.6 g

of sodium? Given that the atomic mass of sodium is 23 g mol–1.

2. In a crystalline solid anions ‘C’ are arranged in cubic close packing, cations ‘A’ occupy 50%

of tetrahedral voids and cations ‘B’ occupy 50% of octahedral voids.

What is the formula of the solid?

3. A metal crystalises into two cubic lattices fcc and bcc, whose edge length are 3.5Å and 3.0Å

respectively. Calculate the ratio of the densities of fcc and bcc lattices.

4. An element of atomic mass 98.5 g mol–1 occurs in fcc structure. If its unit cell edge length

is 500 pm and its density is 5.22 g cm–3. Calculate the value of Avogadro constant.

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5. An element crystallises in a cubic close packed structure having a fcc unit cell of an edge

200 pm. Calculate the density if 200 g of this element contain 24 × 1023 atoms.

6. A fcc unit cell containing atoms of element (molar mass 60.4 g mol–1) has cell edge 4 ×

10–8 cm. Calculate the density of unit cell.

7. The metal calcium (atomic mass = 40 gm mol–1] crystallises in a fcc unit cell with a = 0.556

nm. Calculate the density of the metal if (i) It contains 0.2% Frenkel defect. (ii) It contains

0.1% schottky defect.

8. Analysis shows that a metal oxide has a empirical formula

M 0.96 O. Calculate the percentage of M2+ and M3+ ions in this crystal.

9. AgCl is doped with 10–2 mol% of CdCl2, find the concentration of cation

vacancies.

10. A metallic element has a body centered cubic lattice. Edge length of unit cell is

2.88 × 10–8 cm. The density of the metal is 7.20 gcm–3. Calculate

(a) The volume of unit cell.(b) Mass of unit cell.

(c) Number of atoms in 100 g of metal.

11. Molybednum has atomic mass 96 g mol–1 with density 10.3 g/cm3. The edge length

of unit cell is 314 pm. Determine lattice structure whether simple cubic, bcc or fcc.

(Given NA = 6.022 × 1023 mol–1)

12. The density of copper metal is 8.95 g cm–3. If the radius of copper atom is 127 pm, is

the copper unit cell a simple cubic, a body-centred cubic or a face centred cubic structure?

(Given at. mass of Cu = 63.54 g mol–1 and NA = 6.02 × 1023 mol–1]

13. The well known mineral fluorite is chemically calcium fluoride. It is known that in one

unit cell of this mineral there are 4 Ca2+ ions and 8F– ions and that Ca2+ ions are arranged in

a fcc lattice. The F– ions fill all the tetrahedral holes in the fcc lattice of Ca2+ ions. The edge of

the unit cell is 5.46 × 10–8 cm in length. The density of the solid is 3.18 g cm–3 use this

information to calculate Avogadro’s number (Molar mass of CaF2 = 78.08 g mol–1]

UNIT 2 SOLUTIONS

WORKSHEET 1

1. Give an example of ‘liquid in solid’ type solution.

2. State Henrys law.

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3. What will be the mole fraction of water in C2H5OH solution containing equal number

of moles of water and C2H5OH?

4. Which of the following is a dimensionless quantity : molarity, molality or mole

fraction?

5. 10 gm glucose is dissolved in 400 gm. of solution. Calculate percentage concentration

of the solution.

6. Gases tend to be less soluble in liquids as the temperature is raised. Why?

7. State the conditions which must be satisfied if an ideal solution is to be formed.

8. Aquatic species are more comfortable in cold water rather than in warm water .Explain

9. 9. A mixture of chlorobenzene and bromobenzene forms nearly an ideal solution but a

mixture of chloroform and acetone does not. Why?

10. How is the concentration of a solute present in trace amount in a solution expressed?

11. Which aqueous solution has higher concentration 1 molar or 1 molal solution of the

same solute? Give reason.

12. N2 and O2 gases have KH values 76.48 Kbar and 34.86 kbar respectively at

293 K temperature. Which one of these will have more solubility in water?

13. What type of deviation is shown by Chloroform -CHCl3 solution. Explain

14. Addition of HgI2 to KI (aq.) shows decrease in vapour pressure. Why?

15. What will happen to the boiling point of the solution on mixing two miscible liquids

showing negative deviation from Raoult’s law.

16. Liquid ‘Y’ has higher Vapour pressure than liquid ‘X’, which of them will have

higher boiling point?

17. When 50 mL of ethanol and 50 mL of water are mixed, predict whether the volume of

the solution is equal to, greater than or less than 100 mL. Justify.

18. Which type of deviation is shown by the solution formed by mixing aniline and phenol

19. A and B liquids on mixing produce a warm solution. Which type of deviation from

Raoult’s law is there?

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20. Define cryoscopic constant (molal freezing point depression constant.)

21. Mention the unit of ebulioscopic constant (molal boiling point

Elevation constant.)

22. What is reverse osmosis? Give one large scale use of it.

WORKSHEET 2

1. (a) What are ideal solutions? Write two examples.

(b) Calculate the osmoic pressure in pascals exerted by a solution prepared by

dissolving 1.0g of polymer of mol. mass 185000 in 450 ml of water at 37°C.

2. (a) Describe a method of determining molar mass of a non-volatile solute from

3. vapour pressure lowering.

(b) How much urea (mol. mass 60 g mol–1) must be dissolved in 50g of water

so that the vapour pressure at the room temperature is reduced by 25%? Also

calculate the molality of the solution obtained.

4. (a) Why is the freezing point depression considered as a colligative property?

(b) The cryoscopic constant of water is 1.86 Km–1. Comment on this

statement. (c) Calculate the amount of ice that will separate out on cooling

solution containing 50 g of ethylene glycol in 200 g H2O to –9.3°C

.(Kf for water = 1.86 K kg mol–1)

5. (a) Define osmotic pressure.

(b) Why osmotic pressure is preferred over other colligative properties for the

determination of molecular masses of macromolecules?

WORKSHEET 3

1.Spreading of common salts on the icy roads in a practical applications on depression

in freezing point.Can we use CaCl2 in place of NaCl? Why?

2. What type of azeotrope is formed on mixing nitric acid and water?

3. When 30 ml gram ethanol and 30 ml gram of water are mixed,the volume of resulting

solution is more than 60 ml.Give reason.

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4. Aquatic species feel more comfortable during winter then summer season. Why?

5.Vendors selling aerated drinks bottles are adviced to keep them immersed inside cold

water during summer.

6. If 6.023 𝑥 10 mole cubes of urea are present in 100 ml of its solution, then what is

the concentration of urea solution?

7. Why a person suffering from high blood pressure is advised to take minimum

quantity of common salt?

UNIT 3 ELECTROCHEMISTRY

WORKSHEET 1

1. What is a galvanic cell?

2. Give the cell representation for Daniel Cell.

3. Mention the purpose of salt-bridge placed between two half-cells of a galvanic cell?

4. Give the condition for Daniel Cell in which there is no flow of electrons or current or we

can conclude that there is no chemical reaction.

5. How is electrode potential different from cell potential?

6. Can you store zinc sulphate solution in a copper container? Give suitable reason.

7. How does electrochemical series help us in predicting whether a redox reactions is

feasible in a given direction or not?

8 As per electrochemical series and on the basis of E° values, identify the following :

(a) Gas which has highest tendency for reduction.

(b) Weakest oxidising ion.

9. List the two factors that influence the value of cell potential of a galvaniccell.

WORKSHEET 2

1.. Calculate the equilibrium constant for the reaction at 25°C.

Cu(s) + 2Ag+ (aq) ---- Cu2+ (aq) + 2Ag (s)

The standard cell potential for the reaction at 25°C is 0.46V.

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2.Conductivity of two electrolytic solutions of 0.1 M concentration of the substances A and

B are 9.2 × 10–3 and 4.7 × 10–4 S cm–1, which one of these offer less resistance for the

flow of current and which one is a stronger electrolyte?

3.What is the no of electrons in 1 coloumb of charge?

4.Which solution will allow greater conductance of electricity, 1M NaCl at 293k or 1M

NaCl At 323K and why?

5.Why is the equilibrium const. K related to only 𝑥 cell and not to Ecell

6.Can a nickel spatula be used to stir a solution of copper sulphate ?. Justify your answer.

[𝑥 𝑥𝑥 /Ni = -0.25V & 𝑥 𝑥𝑥 /Cu = 0.34V ]

7.Molar conductivity of an electrolyte increases on dilution.Explain

8.Conductivity of an electrolyte decreases on dilution.Explain

UNIT 7 P BLOCK

1.Draw structures of: XeOF4, SF4 ,XeF4 ,

BrF3 , XeF6 XeO3

2.Arrange the hydrides of group 15 in the increasing order of 1.Thermal stability 2.Bond

dissociation enthalpy 3. Basic strength 4.Reducing character

3.Account for the following

1. Thermal stability of water is much higher than that of H2S

2. the acid strength decreases in the order HF˂HCl˂HBr˂ HI

3. Ammonia is a stronger base than phosphine

4. The +5 oxidation state of Bi is less stable than its +3 state.

5. SF6 is not easily hydrolysed whereas SF4 is readily hydrolysed

6. Bond dissociation enthalpy F2 is leser than that of Chlorine.

7. Nitrogen does not form pentahalide

8.Fluorine is a stronger oxidizing agent than chlorine.

9.Study of actinoids is difficult

10.Bleaching action of Chlorine is permanent

11.O3 is a good oxidising agent

12.Noble gases show low boiling point

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UNIT 10

HALOLKANES AND HALOARENES

1.Write the structure of following halogen compounds

(i) 1–Bromo 4-sec-butyl-2-methylbenzene. (ii) p-Bromotoluene.

(iii)Methylene chloride

2.. Arrange the following in the increasing order of property indicated :

(i) Bromomethane, bromoform, chloromethane, dichloromethane.

(Increasing order of boiling points).

(ii) 1-Chloropropane, isopropyl chloride, 1-chlorobutane

(Increasing order of b.pt.)

(iii) Dichloromethane, chloroform, carbon tetrachloride.

(Increasing order of dipole moment).

(iv) CH3F, CH3Cl, CH3Br, CH3I

(Increasing reactivity towards nucleophilic substitution).

(v) o, m, p-dichlorobenzenes (Increasing order of melting points).

3. Write the difference between

(i) enantiomers and diastereomers

(ii) retention and inversion of configuration.

(iii) electrophilic and nucleophilic substitution reactions.

4. Give a chemical test to distinguish between the following pairs of compounds:

(i) Chlorobenzene and cyclohexylchloride.

(ii) Vinyl chloride and Ethyl chloride.

(iii) n-Propyl bromide and Isopropyl bromide.

5. Which compound in each of the following pairs will react faster in SN2

reaction with OH– and why? (i) CH3Br or CH3I

(ii) (CH3)3 CCl or CH3Cl

(iii) C6H5CH2Cl and C6H5C(Cl)C6H5

(iv) CH2 = CH – Cl and CH2 = CH – CH2Cl

6. Give reasons for the following :

(i) The bond length of C–Cl bond is larger in haloalkanes than that in

haloarenes.

(ii) Although alkyl halides are polar in nature but are not soluble in

water.

(iii) t-Butyl bromide has lower boiling point than n-butyl bromide.

(iv) Haloalkanes react with KCN to form alkyl cyanide as main product

while with AgCN alkyl isocyanide is the main product.

(iv) Sulphuric acid is not used in the reaction of alcohol with Kl.

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(vi) Thionyl chloride is the preferred reagent for converting ethanol to

chloroethane.

(vii) Haloalkanes undergo nucleophilic substitution reaction easily but

haloarenes do not undergo nucleophilic substitution under ordinary

conditions.

(viii) Chlorobenzene on reaction with fuming sulphuric acid gives ortho and

para chlorosulphonic acids.

(ix) 2, 4-Dinitro chlorobenzene is much more reactive than chlorobenzene

towards hydrolysis reaction with NaOH.

(x) Grignard reagent should be prepared under anhydrous

UNIT 11

ALCOHOLS,PHENOLS AND ETHERS

1. Write the equations of the following named reactions:a) Hydro boration b) williamson's synthesis c) cumene phenol process d) Kolbe's reaction e) Riemier Tiemann reaction

2. Explain Lucas test with suitable examples

3. Distinguish chemically between the following pairs of organic compounds

a) Phenol and methanol b) methanol and ethanol c) propan-1-ol and propan-2-ol

d) pentan-3-ol and 2-Methyl butan 2-ol

4. Account for the following:

a) COH bond angle in alcohol is less than tetrahedral angle of 109.50

b) COC bond angle in ether is more than tetrahedral angle of 109.50

c) Phenol has lower dipole moment than alcohol.

d) Phenol under goes electrophillic substitution at ortho and para position

e) Phenol is more acidic than alcohol.

f) In Williamson’s synthesis sec and tert halide cannot be used.

g) para nitro phenol is less steam volatile than ortho nitro phenol.

h) Presence of nitro group at ortho and para position makes phenol more acidic.

i) Alcohols and phenols have higher boiling point

j) Boiling point of alcohol is higher than its isomeric ether.

k) Cresol is less acidic than phenol

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l) . In esterification reaction, water is removed as soon as it is formed

m) Nitrophenols are more acidic than phenols.

n) Methyl phenyl ether reacts with HI to give phenol and methyl iodide and not

methanol and iodo benzene.

o) Methoxy ethane reacts with HI to give methyl iodide and ethanol and not ethyl

iodide and methanol.

p) Tert butyl methyl ether reacts with HI to give tert butyl iodide and methanol and not

not methyl iodide and tert butyl alcohol.

q) Boiling point of butan-1-ol is higher than tert butyl alcohol.

r) In the reaction between acid chloride and alcohol a small amount of pyridine is

added. (s)Alcohol behaves as nucleophile as well as electrophile.

5. Carry out the following conversions:

a) Ethanal to ethanol.b) Acetone to propan-2-ol.c) Ethanoic acid to ethanol.

d) Ethene to ethanol.e) Propene to propan-2-ol.f) Methanal to ethanol.

g) Methanal to benzyl alcohol.h) Ethanal to propan-2-ol.

i) Acetone to 2-methyl propan-2-ol.

j) But-1-ene to butan-1-ol.

k) But-2-ene to butan-2-ol

.l) Chloro benzene to phenol.

(m)Aniline to phenol

.n) Benzene to phenol.o) Tert butyl alcohol to 2-methyl prop-1ene.

p) Propan-2-ol to acetone.q) Benzyl chloride to benzyl alcohol

r) Ethyl magnesium chloride to propan-1-ols) Cumene to phenol

6. Explain the mechanism of the following reactions:

a) CH2= CH2 + H2O CH3CH2OH

b) CH3CH2OH CH2=CH2+H2O

c) CH3CH2OH CH3CH2OCH2CH3

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UNIT 12

ALDEHYDES ,KETONES AND CARBOXYLIC ACID

1. Write equations for the following named reactions:

a) Nucleophillic addition reaction.b) clemensen reduction.

c) wolf kishner reduction.d) aldol condensation.e) crossed aldol condensation

f) cannizaro reaction.g) Rosenmund's reduction.h) kolbe's electrolysis

i) Stephen reaction.j) Etard reaction.k) decarboxylation.l) acylation.

m) schotten baumann reaction.n) Friediel craft's acylation.o) esterification.

p) Gattermann- Koch reaction.q) Hell Volhard Zelensky reaction.

2. Explain

a) Fehling's testb) Tollen's reagent test with suitable examples.

3. Distinguish chemically between the following pairs of organic compounds:

a) Methanal and ethanal.b) ethanal and propanone.c) pentan-2-one and pentan3-one.

d) aceto phenone and benzo phenone.e) formic acid and acetic acid.

f) benzoic acid and ethyl benzoate.g) phenol and benzoic acid.h) ethanal and propanal.

i) propanal and diethyl ether.j) benzaldehyde and acetophenone.k) ethanal and

propanone

4. Account for the following:

a) Aldehyde and ketone are polar in nature.

b) Aldehyde and ketones have higher boiling point than hydro carbons of comparable

molar mass.

c) Aldehyde and ketones have lower boiling point than alcohols of comparable molar

mass.

d) Rosenmund's reduction of acid chloride to aldehyde is carried out using quinoline

and sulphur.

e) Aldehyde is more reactive than ketone towards nucleophilic attack.

f) Butanone is less reactive than propanone in nucleophilic addition reaction

g) 2,2,6-Tri methyl cyclo hexanone is less reactive towards nucleophile than cyclo

hexanone.

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h) Para nitro benzaldehyde is more reactive towards nucleophile than benzaldehyde.

i) Para methyl benzaldehyde is less reactive towards nucleophile than benzaldehyde.

m) Reaction of aldehyde with alcohol to give acetal is carried out in the presence of

HCl(g).

n) Formaldehyde and benzaldehyde undergoes cannizaro reaction and not aldol

condensation.

o) Acetaldehyde undergoes aldol condensation and not cannizaro reaction.

p) Aromatic aldehyde and ketones undergoes electrophillic substitution at meta

position.

q) Carboxylic acid do not show the reactions of aldehyde and ketone though it has

>C=O group.

r) Carboxylic acid has higher boilimg point than aldehyde, ketone and alcohol of

comparable molar mass.

s) In semi carbazide, only one NH2 group is involved in the formation of semi

carbazone.

t) Aldehyde, ketone and carboxylic acid are soluble in water.

u) In oxidation of primary alcohol to carboxylic acid is not carried out using acidified

potassium dichromate.

v) Carboxylic acid is more acidic than alcohol.

w) Carboxylic acid is more acidic than phenol.

x) Acidity of CCl3COOH>CHCl2COOH>CH2ClCOOH>CH3COOH. Give reason

y) Acidity of FCH2COOH>ClCH2COOH>BrCH2COOH>I CH2COOH. Give reason

z) α chloro propanoic acid is more acidic than ß chloro propanoic acid.

aa) Acetic acid is less acidic than formic acid.

bb) Pure acid halide is prepared by the reaction of carboxylic acid with thionyl

chloride.

cc) Carbon in carbonyl group of aldehyde and ketone acts as Lewis acid(electrophile)

while oxygen acts as Lewis base ( nucleophile). dd) Benzoic acid does not

undergo Friediel craft alkylation reaction.

Mention two uses of each.

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5. Carry out the following conversions:

a) Ethanol to ethanal.b) Methanol to methanal. c) Propan-2-ol to propanone.

d) Methanal to i) ethanol ii) benzyl alcohol.

e) Ethanal to i) propan-2-olii) acetone.

f) Acetone to i) tert butyl alcohol ii) 2-Methyl prop-1-ene.

g) Benzaldehyde to i) a- hydroxy phenyl acetic acidii) 3-phenyl propan-1-ol

.h) Butan-1-ol to butanal.

i) Cyclo hex-2-en-1-ol to cyclo hex-2-en 1-one.j) Pentan-3-en-2-ol to pent-3-en-2one.

k) But-2-ene to ethanall) Para nitro toluene to para nitro benzaldehyde.

m) Ethanal to butan-2-one. n) Ethanal to butane- 1,3- diol. o) Ethanal to but-2enal

p) Ethanal to but-2-enoic acid. q) Ethanal to butan-1-olr) Ethanal to butanoic acid.

s) Propanone to propene. t) Propanal to butanone.u) Ethanal to 2-hydroxy butanal.

v) Benzaldehyde to benzo phenone. w) Benzoic acid to benzaldehyde.

x) Propanoic acid to propenoic acid.y) Benzene to m-nitro aceto phenone.

z) Bromo benzene to 1-phenyl ethanol.

9. An organic compound A(C8H8O) gives orange red precipitate with 2,4-DNP reagent. It responds to iodoform test. It does not respond to Tollen’s reagent test. It does not

decolorise bromine water. A on oxidation using CrO3 give B. Identify the compounds

and write thw equations of the reactions involved.

10. An organic compound C9H10O forms 2,4-DNP derivative, reduces Tollen’s reagent and Undergoes cannizaro reaction. On vigorous oxidation it gives Benzene-1,2-

dicarboxylic acid. Identify the compound.

11. An organic compound contain 69.77% C and 11.63% H and the remaining O. Molecular mass of the compound is 86 u. It does not reduce Tollen’s reagent, gives

positive iodoform test and respond to sodium bisulphate test. On oxidation it gives

acetic acid and propanoic acid. Give the structure of the organic compound.

12. Arrange the following in the increasing order of property mentioned:

a) Acetaldehyde, Acetone, Di-tert-butyl ketone, Methyl tert-butyl ketone(

reactivity with HCN)

b) 2-Bromo butanoic acid, 3-Bromo butanoic acid, Butanoic acid, 3-Methyl

propanoic acid (acid strength)

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c) Benzoic acid, 4-Nitro benzoic acid, 3,4-Dinitro benzoic acid, 4-Methoxy

benzoic acid (acid strength)

d) Ethanal, Propanal, Propanone, Butanone( increasing order of reactivity

towards nucleophile)

e) Benzaldehyde, p-Tolualdehyde, p-Nitro benzaldehyde,

Acetophenone(increasing order of reactivity towards nucleophile)

f) Butanal, Butanol, Ethoxy ethane and Butane (increasing order of boilimg

point)

13. Complete each synthesis by giving missing starting material, reactant or product.

c) C6H5CHO + NH2CONHNH2

d) C6H5CHO + CH3CH2CHO

14. Which acid of each pair would you expect to be stronger?

a) Ethanoicacid and fluoro ethanoic acid

b) Fluoro ethanoic acid and chloro ethanoic acid

c) 4- Fluoro butanoic acid and 3-Fluoro butanoic acid

d) p-Trifluoro benzoic acid and p- Methyl benzoic acid.

15. Arrange the following in the increasing order of boiling point: Ethanal, Ethanol,

Ethoxy ethane and Propane

16. Predict the product formed when cyclohexanecarbaldehyde reacts with

a) PhMgBr+H3O+

b) Tollens’reagent

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c) Semicarbazide and weak acid

d) excess ethanol and acid.

e) Zinc amalgam and dilute HCl

17. Give the products of the following reactions:

c) RCH=CHO + NH2CONHNH2

d) C6H5COCH3 + C2H55NH2

f) (C6H5CH2)2Cd + 2 CH3COCl

UNIT 8 -D AND F BLOCK ELEMENTS

Worksheet 1

Account for the following:

1. Zn, Cd and Hg are not considered as transition metals.

2. Cu,Ag &Au are considered as transition metal though it has 3d10 configuration.

3. Zn, Cd and Hg are volatile and Hg is a liquid metal.

4. Transition metals have high enthalpy of atomisation.

5. 4d and 5d elements have higher enthalpy of atomisation than 3d elements.

6. Density of 3d elements increases from Sc to Ni.

7. Atomic and ionic radii generally decrease along the period.

8. Zr and Hf have similar size.

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9. Transition metals do not show regular variation of ionisation enthalpies.

10. 5d elements have higher ionisation enthalpy than 3d and 4d elements.

11. Generally first ionisation enthalpy increases along the period.

12. Cr &Cu has higher second ionisation enthalpy (Cr=24,Cu=29)

13. Mn &Zn has higher 3rd ionisation enthalpy (Mn=25 Zn=30) 14. Cu, Ni and Zn normally

do not exhibit oxidation state higher than +2.

15. Transition metals show variable oxidation state.

16. Transition metals do not show regular variation of E0 values.

17. E0 Mn3+/ Mn2+ have higher +ve value than E0 Cr3+ / Cr2+.(Cr=24 Mn=25).

18. E0 Zn2+ / Zn has higher - value. ( Zn=30).

19. Transition metals form complexes easily.

20. Transition metals act as catalysts.

21. Transition metal compounds are paramagnetic.

22. Sc3+,Cu+ and Zn2+ are diamagnetic .Sc=21 Cu=29 Zn=30).

23. Oxidation state of transition metals increases by one unit.

24. E0 Ni2+ / Ni has higher - ve value.

25. Transition metal compounds are coloured.

26. Sc3+,Cu+ and Zn2+ are colourless .[Sc=21 Cu=29 Zn=30].

27. Transition metals form interstitial compounds easily.

28. Transition metals form alloys easily.

29. Higher oxides of transition metals are acidic.

30. Enthalpy of atomization of transition metals reaches a maximum in the middle of each

series

31. Lanthanoid ions are coloured and paramagnetic.

32. La3+ and Lu3+ are colourless and diamagnetic. (La=57 Lu=71).

33. Ln are paramagnetic.

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34. La3+ is diamagnetic.

35. Ce is stable in +4 oxidation state. E0 Ce4+ / Ce3+ has higher positive value.

36. Eu2+ is a good reducing agent.(Eu=63).

37. Ce4+ is a good oxidising agent .

38. Yb2+ is stable. It acts as a reducing agent. (Yb=70).

39. In lanthanoid hydroxide M(OH)3 basic character decreases with increase in atomic

number.

40. Actinoids show greater range of oxidation state than lanthanoids.

41. Actinoid contraction is greater than lanthanoid contraction.

42. Ionisation enthalpies of early actinoids are lesser than that of early lanthanoids.

43. In the d4 species Mn3+ is an oxidising agent where as Cr2+ is a reducing agent

44. Co(II) is stable in aqueous solution but get oxidised in the presence of complexing

agents.

45. d1 configuration is unstable in transition metals.

46. Transition metals exhibit higher oxidation state in oxides and flourides.

47. Zn has lowest enthalpy of atomisation.

48. First ionization enthalpy of Cr is lower while Zn is higher.(Cr=24, Zn=30)

49. Zn has lower second ionization enthalpy.

50. Number of oxidation states at the extreme ends of 3d transition metals are very few.

51. Transition metals in higher oxidation states are more stabilized in oxides than in

fluorides.

52. E0 Cu2+ / Cu is positive.

53. E0 Sc3+ / Sc2+ has lower value (Sc=21)

54. E0 Zn3+ / Zn2+ have higher positive value.

55. E0 Fe3+ / Fe2+ has comparatively lower positive value than E0 Mn3+ / Mn2+ (Mn=25,

Fe=26)

56. E0 V3+ / V2+ have lower negative value (V=23)

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57. Cu2+ (aq) is more stable than Cu+ (aq) despite the d10 configuration of Cu+

58. Highest fluoride of Mn is MnF4 while highest oxide is Mn2O7.

59. Oxidising power of Oxides VO2+< Cr2O72-

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6.What are transition metals? Which three elements are not considered as transition metals

though they are kept in d block? In which way the electronic configuration of transition

element differ from non transition elements?

7.Compare the stability of +2 oxidation state of the elements with electronic configurations 3d64s2, 3d24s5 and 3d34s2.

CHAPTER 3

CHEMICAL KINETICS

1. Define the term chemical kinetics?

2. Define – Rate of reaction?

3. What is average rate of a reaction?

4. What are the units of rate of a reaction?

5. What is instantaneous rate of a reaction?

7. Enlist the factors affecting rate of a reaction?

8. What do you understand by rate law expression?

10. Define the terms – i) Order of a reaction

ii)Molecularity of a reaction.

11. What are elementary and complex reactions?

12. Differentiate between order and molecularity of a

reaction?

13. Determine the overall order of a reaction which

has the rate law

R = K [A]5/2 [B]3/2

14. What are the units of a rate constant of a

a) First order reaction

b) nth order reaction.

15.Identify the reaction order for from each of the

following rate constant –

a) k = 2.3 ×10-5 L mol-1 s-1

b) k = 3.1 × 10-4 s-1 [1]

16. What is the use of integrated rate equation?

17. For first order reaction –

A →B

Write (1) Differential rate law.

(2) Integrated rate law.

18.Give an example of pseudo – first order reaction

19. Write the expression for half – life period of a first

order reaction?

20. A first order reaction is found to have a rate

constant K = 5.5 × 10-14 sec -1.

Find half life of reaction?

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21. The time required to decompose SO2Cl2 to half of its initial amount is 60 min.

If the decomposition is a first order reaction, calculate the rate constant of the reaction?

UNIT -9 COORDINATION COMPOUNDS

1. Write IUPAC names of the following compounds

a) [Co (NH3 )5 Cl ] Cl2

b) [Cr(NH3 )6 ]3+

c) [Ni(NH3 )6 ] Cl2

d) [CoCl(NO2)(NH3)4 ] Cl

e) [Co(en)2(ONO)2] Cl

f) [Cr(NH3 )5(H2O)]3+

g) K3 [Co(C2O4)3 ]

h) Na3 [Cr(OH)2F4 ]

i) [Co(NH3 )6] [Cr(CN)6 ]

j) [Pt(NH3 )2Cl(NH2CH3)] Cl

2. Write the IUPAC name of ionization isomer of [Co(NH3)5Br ]SO4

3. Write the IUPAC name of linkage isomer of [Co(en)2(ONO)2 ]Cl

4. Write the formula of the following coordination compounds:

a) Tris (ethane-1,2-diamine)cobalt(III)sulphate

b) Amminebromidochloridonitrito-N- platinate(II)

c) Pottasiumtetrachloridopalladate(II)

d) Tetrahydroxozincate

5. Explain the following with suitable examples

a) coordination entity

b) ligand

c) coordination number

d) homoleptic f) heteroleptic

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6. What is meant by unidentate, bidentate and ambidentate ligands? Give two examples each.

7. Give an example of hexadentate ligand.

8. Explain chelation with a suitable example.

9. Write the IUPAC name and indicate the oxidation state,electronic configuration and coordination number of the central metal in the complex [Co (NH3)5 Cl ] Cl2 Also give the primary and secondary valency of the metal.

10. Mention the limitations of valence bond theory.

11. Using valence bond theory, predict the structure and the magnetic behavior of the

below given complexes:

a) [Fe(CN)6 ]4-

b) [Fe(CN)6 ]3-

c) [NiCl4]2-

d) [Ni(CN)4]2-

e) [Cr(NH3)6 ]3+

f) [Co(NH3)6 ]3+

g) [Ni(CO)4] h) [Fe(CO)5]

i) [MnCl4]2-

j) [CoF6 ]3-

k) [Co(en)3]3+

m) [Co(C2O4)3]3-

n) [Mn(CN)6 ]3-

o) [Ni(NH3)6 ]3+

p) [Fe(H2O)6 ]3+

q) [Mn(CN)6 ]4-

r) [FeF6]3-

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s) [MnCl6]3-

t) [MnBr4]2-

12. Name two properties of central metal ion which enables it to form stable complex entities.

13. A coordination compound has the formula CoCl3.4NH3. It does not liberate ammonia but gives precipitate of AgCl with AgNO3 solution. Give the structural formula and

IUPAC name of the complex.

14. Account for the following:

a) [Fe(CN)6]4- is diamagnetic while [Fe(CN)6]3- is paramagnetic.

b) [NiCl4]2- is tetrahedral while [Ni(CN)4]2- is square planar.

c) Hydrated copper sulphate is colored while anhydrous copper sulphate is colorless.

d) [Ti(H2O)6]3+ become colorless on heating.

e) [Ni(H2O)6]2+ is green while [Ni(CN)4]2- is colorless.

f) [Fe(CN)6]4- and [Fe(H2O)6]2+ show different colors in aqueous solution..

g) [Cr(NH3)6]3+ is paramagnetic while[Ni(CN)4]2- is diamagnetic.

h) Tetrahedral complex do not exhibit geometrical isomerism.

15. What is the difference between inner orbital and outer orbital complexes?

Illustrate with one example each.

16. How the given factor affect the stability of complex

a) charge on cation b) nature of ligand.

17. Illustrate the following with an example each:

a) linkage isomerism

b) ionization isomerism

c)coordination isomerism

d) hydrate isomerism

18. Draw the geometrical isomers of [Co(NH3)3(NO2)3] and label them.

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19. Give a chemical test to distinguish between

[Co (NH3)5 Cl ] SO4 and [Co (NH3)5 SO4 ] Cl What type

of isomerism does they exhibit?

20. A metal ion Mn+ having d4 configuration combine with three didentate ligand to

form a complex compound. Assuming D0>P

i) Draw the diagram showing d orbital splitting during this complexformation. ii) Write

the electronic configuration of the valence electron of the metal Mn+ ion in terms of

t2g and eg. iii) What type of hybridisation will Mn+ ion

have? iv) Draw the structure of isomers exhibited by this complex.

21.Draw the figure to show the d orbital splitting in tetrahedral complex.

22.Mention the limitations of crystal field theory.

23. What is spectrochemical series? Explain the difference between strong and weak

ligand.

24. The spin only magnetic moment of the complex[MnBr4]2- is 5.9B.M. Predict the

geometry of the complex.

25. Calculate the spin only magnetic moment of the complex a) [Fe(CN)6]4- b) [CoF6]3-

UNIT 5

SURFACE CHEMISTRY

1. Give differences between

a) adsorption and absorption

b) physisorption and chemisorption

c) lyophilic and lyophobic sol.

2. Explain the terms

a) extent of adsorption(x/m) b) enthalpy of adsorption

c) desorption

d) adsorbent e) adsorbate

3. Mention the factors affecting the adsorption of gases on solids.

4. Explain Freundlich adsorption isotherm with suitable graphs.

5. Why is adsorption a) exothermic process b) surface property

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6. Explain the effect of temperature on physisorption and chemisorption with graphs.

7. Mention five applications of adsorption.

8. Mention the disperse phase and dispersion medium in a)Milk b) butter c) cheese d) Fog e) mist f) froth

9. What do you mean by multi molecular and macro molecular colloids? Give two examples each.

10. What are associated colloids? How does it differ from multi molecular and macro molecular colloids? Give two examples of associated colloids.

11. Explain the terms a) kraft temperature b) CMC(critical micelle concentration)

12. Explain the mechanism of cleaning action of soap.

13. Action of soap is due to emulsification and micelle formation. Comment.

14. How is sulphur sol prepared by chemical method?

15. How is gold sol prepared by a) chemical methodb) Bredig’s arc method?

16. Mention the principle of dialysis.

17. What is Tyndall effect? Mention the condition for Tyndall effect to occur. Give two

application of Tyndall effect.

18. What is Brownian movement? Mention the significance of Brownian movement

19. Describe and explain what is observed when beam of light is passed through

a) colloidal solution. b) an electric current is passed through a colloidal solution.

20.Account for the following:

a) lyophillic colloids are more stable than lyophobic colloids.

b) delta formation occurs at the river beds.

c) alum or ferric chloride is added to stop

bleeding.

d) sky appears blue in colour. e) alum is used in water purification.

21.Explain the terms a) zeta potential

b) Helmoltz electrical double layer

c) coagulation

d) Colloidion

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e) peptisation

22.Explain Hardy and Schulze rule with suitable examples.

23.What is coagulation value?

24.Out of ammonia and nitrogen which gas will be absorbed more readily on the surface

of Charcoal and why?

25.How does adsorption of a gas vary with a) temperature b) pressure? .

26.What do you mean by activation of adsorbent? How is it achieved?

27.A colloidal solution of AgI is prepared by two different methods shown below:-

(i) What is the charge of AgI colloidal particles in the two test tubes (A) and (B)?

(ii) Give reasons for the origin of charge.

UNIT 14

BIOMOLECULES

1. Mention the function of carbohydrates in plants.

2. How are carbohydrates classified? Give one example each.

3. Fructose is a ketohexose but it is a reducing sugar. Why?

4. What are monosaccharides? Give two examples.

5. Write the equations of the reactions involved when glucose is reacted with

a)acetic anhydride

b)HI

c)Hydroxylamine

d)HCN

e)Br2(aq)

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f) concentrated HNO3. Write the significance of each reaction.

6. Enumerate the reactions of glucose which cannot be explained by open structures.

7. Draw the Howarth structures of a) α-D-(+) glucopyranose b) β-D-(+) glucopyranose

c) α-D-(-) fructo furanose d) β-D-(-) fruco furanose

8. Explain the terms a) muta rotation b) anomers.

9. What is invert sugar? Why is it called so?

10. What are anomers? Draw the anomers of glucose. Are they enantiomers?

11. Classify the following as monosaccharides and disaccharides:

a) ribose b) 2-Deoxy ribose c) sucrose d) galactose e) lactose f) maltose g) fructose

15. Explain glycosidic linkage with an example.

16. Explain the following with respect to protein

a) primary structure of protein b) secondary Structure of protein

c) tert structure of protein d) quaternary structure of protein e) native state of protein

f) denaturation of protein g) zwitter ion

17. Explain peptide linkage with an example.

18. Mention the type of bonding in

a) α helix structure b) β sheet structure c) cross links of polypeptide chain d) DNA

19. Name the forces which stabilize secondary and tert structure of protein.

20. Distinguish between

a) α helix and β sheet structure b) fibrous and globular protein. c) primary and secondary

structure of protein d) nucleoside and nucleotide

21. Account for the following;

a) Amino acids are more soluble and has higher melting point than halo acids. b) Amino

acids behave like salts rather than amines or carboxylic acids c) Amino acids are

amphoteric d) On electrolysis amino acids migrate towards cathode in acid solution and

anode in alkaline solution. e) Mono amino mono carboxylic acid has two pk values. f)

Amino acids are optically active. g) on boiling egg it becomes hard

22. Name and give the structure of amino acid which is optically inactive.

23. What are essential and non essential amino acids? Give two examples each.

24. What are enzymes? Explain the mechanism of enzyme catalysed reaction.

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25. What are coenzymes? Give two examples.

28. What are nucleic acids? Mention the functions of nucleic acids.

29. Show the formation of a dinucleotide with an example.

30. Mention the differences between DNA and RNA.

31. Two strands of DNA are not identical but complementary. Explain this statement.

32. What are different types of RNA present in the cell.

33. What is the effect of denaturation of protein?

34. Where does the water present in egg go after boiling?

CHAPTER 13

ORGANIC COMPOUNDS CONTAINING NITROGEN

Q.1. Arrange the following in increasing order of their basic strength in aqueous

solution:

𝑪𝑯𝟑. 𝑵𝑯𝟐, (𝑪𝑯𝟑)𝟑𝑵, (𝑪𝑯𝟑)𝟐𝑵𝑯 Q.2. Arrange the following compounds in increasing order of solubility in water:

𝑪𝟔𝑯𝟓𝑵𝑯𝟐, (𝑪𝟐𝑯𝟓)𝟐𝑵𝑯, 𝑪𝟐𝑯𝟓𝑵𝑯𝟐

Q.3. Write IUPAC name of the following compound: (𝐂𝐇𝟑𝐂𝐇𝟐)𝟐𝐍𝐂𝐇𝟑

Q.4. Arrange the following compounds in an increasing order of basic strengths in their

aqueous solutions:

𝑵𝑯𝟑, 𝑪𝑯𝟑𝑵𝑯𝟐, (𝑪𝑯𝟑)𝟐𝑵𝑯, (𝑪𝑯𝟑)𝟑 𝑵

Q. 5 Rearrange the following in an increasing order of their basic strengths:

𝑪𝟔𝑯𝟓𝑵𝑯𝟐, 𝑪𝟔𝑯𝟓𝑵(𝑪𝑯𝟑)𝟐, (𝑪𝟔𝑯𝟓)𝟐 𝐚𝐧𝐝 𝐂𝐇𝟑𝑵𝑯𝟐.

Q.6. Write the structure of N-Methylethanamine.

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4onQ.7. Give the IUPAC name of:

𝑯𝟐𝑵 − 𝑪𝑯𝟐 − 𝑪𝑯𝟐 − 𝑪𝑯 = 𝑪𝑯𝟐.

Q.8. Why is an alkylamine more basic than ammonia?

Q.9. Give the IUPAC name of :

𝑯𝟐𝑵 − 𝑪𝑯𝟐 − 𝑪𝑯𝟐 − 𝑪𝑯 = 𝑪𝑯𝟐

Q.10. Arrange the following in the decreasing order of their strength in aqueous solutions:

𝑪𝑯𝟑𝑵𝑯𝟐, (𝑪𝑯𝟑)𝟐 𝑵𝑯, (𝑪𝑯𝟑)𝟑 𝒂𝒏𝒅 𝑵𝑯𝟑

Q.11. Write one chemical reaction each to illustrate the following:

(i) Hoffmann’s bromamide reaction

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(ii) Gabriel phthalimide synthesis

Q.12. (i) Arrange the following in an increasing order of basic strength in water:

𝑪𝟔𝑯𝟓𝑵𝑯𝟐, (𝑪𝟐𝑯𝟓)𝟐𝑵𝑯, (𝑪𝟐𝑯𝟓)𝟑𝑵 𝐚𝐧𝐝 𝑵𝑯𝟑

(ii) Arrange the following in increasing order of basic strength in gas phase:

𝑪𝟐𝑯𝟓𝑵𝑯𝟐,(𝑪𝟐𝑯𝟓)𝟐𝑵𝑯, (𝑪𝟐𝑯𝟓)𝟑𝑵 𝐚𝐧𝐝 𝑵𝑯𝟑 𝑵𝑯𝟐.

Q.13. Give the chemical tests to distinguish between the following pairs of

compounds:

(i) Ethylamine and Aniline

(ii) Aniline and Benzyl amine

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Q.14. Describe the following giving the relevant chemical equation in each case:

(i) Carbylamines reaction

(ii) Hofmann's bromamide reaction

Q.15. Complete the following reaction equations:

(i) 𝐂𝟔𝐇𝟓𝐍𝟐𝐂𝐥 + 𝐇𝟑𝐏𝐎𝟐 + 𝐇𝟐𝐎 ⟶ (ii) 𝐂𝟔𝐇𝟓𝐍𝐇𝟐 + 𝐁𝐫𝟐(𝐚𝐪. ) ⟶

Q.16. Give reasons for the following:

(i) Aniline does not undergo Friedal-Crafts reactions.

(ii) (𝐶𝐻3)2𝑁𝐻 is more basic than (𝐶𝐻3)3𝑁 in an aqueous solution. (iii). Primary amines have higher boiling point than tertiary amines.

Q.17. Write the chemical equations involved in the following reactions:

(i) Hoffmann-bromoimides degradation reaction

(ii) Carbylamines reaction

Q.18. How will you convert the followings:

(i) Nitrobenzene into aniline,

(ii) Ethanoic acid into methanamine

(iii) Aniline into N-phenylethanamide (write the chemical equations involved).

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Q.19. Give reasons:

(i) Acetylation of aniline reduces its activation effect.

(ii) 𝐂𝐇𝟑𝐍𝐇𝟐 is more basic than 𝐂𝟔𝐇𝟓𝐍𝐇𝟐. (iii) Although – 𝐍𝐇𝟐 is o/p directing group, yet aniline on nitration gives a significant amount of m-nitroaniline.

Q.20. Amino acids may be acidic, alkaline or neutral, how does this happen? What are

essential and nonessential amino acids? Name one of each type.

Q.21. Account for the following:

(i) Primary amines (𝑹 − 𝑵𝑯𝟐) have higher boiling point than tertiary amines (𝑹𝟑𝑵). (ii) Aniline does not undergo Friedel – Crafts reaction.

(iii). (𝑪𝑯𝟑)𝟐𝑵𝑯 is more basic than (𝑪𝑯𝟑)𝟑𝑵 in an aqueous solution.

Q.22. Give reasons for the following:

(a) Acetylation of aniline reduces its activation effect.

(b) 𝑪𝑯𝟑𝑵𝑯𝟐 is more basic than 𝑪𝟔𝑯𝟓𝑵𝑯𝟐. (c) Although –NH2 is o/p directing group, yet aniline on nitration gives a significant

amount of m-nitroaniline.

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Q.23. Account for the following observations:

(i) 𝐩𝐊𝐛 for aniline is more than that for methylamine. (ii) Methylamine solution in water reacts with ferric chloride solution to give a

precipitate of ferric hydroxide.

(iii). Aniline does not undergo Friedel-Crafts reaction.

Q.24. Write chemical equations for the following conversion:

(i) Nitrobenzene to benzoic acid.

(ii) Benzyl chloride to 20phenylethanamine.

(iii) Aniline to benzyl alcohol.

Q.25. Complete the following reactions:

(i) 𝑪𝑯𝟑 𝑪𝑯𝟐 𝑵𝑯𝟐 + 𝑪𝑯𝑪𝒍𝟑+alc. KOH⟶ 4ono.com 4ono.com 4ono.com 4ono.com 4ono.com 4ono.com 4ono.com 4ono.com 4ono.com

Q.26. (a) Write the structure of main products when aniline reacts with the following

reagents:

(i) 𝑩𝒓𝟐 𝐰𝐚𝐭𝐞𝐫, (ii) HCl,

(iii) (𝑪𝑯𝟑𝑪𝑶)𝟐 O/pyridine. (b) Arrange the following in the increasing order of their boiling point:

𝐂𝟐𝐇𝟓𝐍𝐇𝟐, 𝐂𝟐𝐇𝟓𝐎𝐇, (𝐂𝐇𝟑)𝟑𝐍 (c) Give a simple chemical test to distinguish between the following pair of

compounds:

(𝑪𝑯𝟑)𝟐 𝑵𝑯 𝒂𝒏𝒅 (𝑪𝑯𝟑)𝟑𝑵

Q.27. (a) Write the structures of main products when benzene diazonium chloride reacts

with the following reagents:

(i) 𝑯𝟑𝑷𝑶𝟐 + 𝑯𝟐𝑶 (ii) CuCN/KCN

(iii) 𝑯𝟐𝑶 (b) Arrange the following in the increasing order of their basic character in an

aqueous solution:

𝑪𝟐𝑯𝟓𝑵𝑯𝟐, (𝑪𝟐𝑯𝟓)𝟐𝑵𝑯, (𝑪𝟐𝑯𝟓)𝟑𝑵 (c) Give a simple chemical test to distinguish between the following pair of

compounds:

𝑪𝟔𝑯𝟓 − 𝑵𝑯𝟐 𝒂𝒏𝒅 𝑪𝟔𝑯𝟓 − 𝑵𝑯 − 𝑪𝑯𝟑

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XI-XII Boys Section

UNIT 1 SOLID STATEWORKSHEET 1Worksheet 2ALDEHYDES ,KETONES AND CARBOXYLIC ACIDUNIT 8 -D AND F BLOCK ELEMENTSWorksheet 1Worksheet 2

21. The time required to decompose SO2Cl2 to half of its initial amount is 60 min. If the decomposition is a first order reaction, calculate the rate constant of the reaction?UNIT -9 COORDINATION COMPOUNDSSURFACE CHEMISTRYBIOMOLECULES