international indian school, riyadh worksheet (2020 … · 2020. 9. 13. · (ii) although alkyl...

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INTERNATIONAL INDIAN SCHOOL, RIYADH

WORKSHEET (2020-2021)

GRADE - XII – CHEMISTRY - SECOND TERM

UNIT 2 SOLUTIONS

WORKSHEET 1

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

2. State Henrys law.

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.

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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?

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.

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(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.

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.

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(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.

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

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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

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

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(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.

(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.

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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

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

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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

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.

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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.

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.

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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.

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.

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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)

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

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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

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

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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.

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).

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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.

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.

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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)

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- <MnO4-

60. KMnO4 titration is not carried out using HCl as acid medium.

61. Third ionization enthalpy of La, Gd and Lu are abnormally low( La=57, Gd=64, Lu=71)

62. 5f electrons can take part in bonding to a greater extent than 4f electron though both

have similar angular wave function.

63. Highest oxidation state is exhibited by oxoanion in transition metals.

64. Generally negative value of E0 M2+ / M decreases across the series of 3d elements.

65. It is unsatisfactory to review the chemistry of actinoids in terms of oxidation state.

66. Lower oxides of transition metal are basic while higher oxides are acidic.

67. Sc exhibits only one oxidation state.

68. Cr2+ is stronger reducing agent than Fe2+

69. Mo(VI) and W(VI) are more stable than Cr(VI)

70. There is a greater horizontal similarity in the transition metals than in the main group

elements.

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71. Nickel (II) does not form low spin octahedral complexes.

72. Transition elements form pi complexes.

73. There is more frequent metal-metal bonding in 4d and 5d transition elements.

Worksheet 2

1. What is lanthonoid contraction? What is the reason for lanthonoid contraction?

Mention the consequences of lanthonoid contraction.

2. What is mischmetal? Mention two uses of mischmetal.

3.Compare the stability of +2 oxidation state for the elements of the 3d series.

4.Cr2+(aq) is a better reducing agent than Fe2+ despite the half-filled stability of Fe3+

Why?

5.Which transition metal exhibit only one oxidation state. Why?

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.

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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?

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? [2]

Prepared by:

XI-XII Boys Section

international indian school, riyadh worksheet (2020 … · 2020. 9. 13. · (ii) although alkyl...

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