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Part – II 3 Mark Qs  - 31 to 51 
Unit – 1 (Q – 31)

1.      Define hybridisation.

2.      Distinguish between a particle and a wave.

3.      Explain bond order.

4.      State Heisenberg’s uncertainty principle.

5.      What are the conditions for effective hydrogen bonding?

6.      What is the significance of negative electronic energy?

7.      Why is He₂ not formed?

8.   Define orbital

Unit - 2 (Q – 32)

1.      Calculate the effective nuclear charge experienced by the 4s electron in potassium atom. (S =16.8).

2.      Calculate the electronegativity value of fluorine on Mullikan's scale from the following data: Ionisation potential of F = 17.4 eV/atom, Electron affinity of F = 3.62 eV/atom.

3.      Compare the ionisation energy of nitrogen with that of oxygen.

4.      Define electron affinity.

5.      Explain why the first ionisation energy of Be is greater than that of B. Or The ionisation energy of boron is less than beryllium. Why?

6.      If the d(C – Cl) is 1.76 Å and r(Cl) is 0.99 Å, find the radius of carbon atom.

7.      Ionisation energy of Neon is greater than that of Fluorine. Give reason. Or Neon has more ionisation energy than fluorine. Why?

8.      Larger the size of atom lesser is the ionisation energy. Explain.

9.      Mention the disadvantage of Pauling’s and Mulliken’s electronegativity scale.

10.  The electron affinities of beryllium and nitrogen are almost zero. Why?

11.  Why is electron affinity of fluorine less than that of chlorine?

12.  Why is ionisation energy of fluorine greater than that of oxygen?

13.  Why is the first ionisation energy of Beryllium greater than that of Lithium?
14. Compare the first ionisation energy of Aluminium with that of Magnesium. Justify your answer.

15. Compare the ionisation energies of Carbon and Boron

Unit - 3 (Q – 33)

1.      Draw / Give the electronic structure of following i) PCl5 ii) H3PO3

2.      How is phosphoric acid prepared in the laboratory?

3.      How is potash alum prepared?

4.      How is Xenon fluorides prepared?

5.      Prove that P2O5 is a powerful dehydrating agent. Or Illustrate the dehydrating property of phosphorous pentoxide (P2O5) with two examples. Or P2O5 is a dehydrating agent. Why?

6.      Prove that phosphorous acid is a powerful reducing agent.

7.      What are interhalogen compounds? Give the preparation.

8.      What is plumbo solvency? Or Write a note on plumbo solvency. Or Write about Plumbo solvency.

9.      Write about the Holme's signal.

10. Write the uses of Fluorine

11. What is Burnt alum?

12. How Silver nitrate reacts with orthophosphoric acid?

Unit - 3 (Q – 34)

1.      Discuss / Illustrate the oxidising power of fluorine.

2.      Give / Write the uses of Helium.

3.      Give / Write the uses of neon.

4.      H3PO3 is diprotic. Why?

5.      H3PO4 is triprotic. Prove.

6.      What happens when phosphorus acid is heated?

7.      What is inert pair effect?

8.      What is the action of heat on orthophosphoric acid?

9.      Why is HF not stored in silica or glass bottles? Write the equation.

10. Write the uses of Lead

11. Show that Phosphine is a very good reducing agent

12. Mention uses of Potash alum

13. Write the preparation of ClF, ClF3 and IF7

Unit - 4 (Q – 35)

1.      Explain why Mn2+ is more stable than Mn3+

2.      What is the action zinc on hot NaOH solution?

3.      Why are transition metal ions coloured?

4.      Why do d-block elements exhibit variable oxidation states? Or The transition elements show variable oxidation states. Give reason.

5.      Why do transition elements form complexes? Or d-block elements form complexes compounds. Why?

6.      Write a note on chrome plating. Or How is chrome plating done?

7.      Write the action of aqua regia on gold. Or Write the reaction of gold with aqua regia.

8. What is the action of heat on Silver nitrate?

9. Give the percentage composition and use of Nichrome

10. What is the action of heat on heating, K2Cr2O7?

11. Most of the transition metals and their compounds have catalytic activity. Why?
12. Why do transition elements form alloys?

Unit - 4 (Q – 36)

1.      A substance is found to have a magnetic moment of 3.9 BM. How many unpaired electrons does it contain?

2.      Explain Chromyl chloride test with equation.

3.      Explain electrolytic refining of copper.

4.      Give any two evidences for the oxidising nature of potassium dichromate.

5.      How is Purple of Cassius prepared?

6.      What happens when KI solution is added to an aqueous solution of copper sulphate?

7.      What is spitting of silver? How is it prevented?

8.      What is the action of heat on copper sulphate crystals? Write the equation.

9.      What is the reaction of CuSO4 with KCN?

10.  Why are Zn2+ salts colourless while Ni2+ salts are coloured?
11. How is lunar caustic prepared?

12. What is Philosopher’s wool? How is it formed?

13. Write two alloys of copper and their uses

14. What is called Bordeaux mixture? Mention its use

15. Give the reaction of ammoniacal silver nitrate with Formic acid

Unit - 7 (Q – 37)

1.      Calculate Q value of the following nuclear reaction 13Al27 + 2He4 → 14Si30 + 1H1+ Q. The exact mass of 13Al27 is 26.9815 amu, 14Si30 is 29.9738, 2He4 is 4.0026 amu and 1H1 is 1.0078 amu.

2.      Calculate the decay constant for Ag108 if its half life is 2.31 minutes.

3.      Calculate the number of a and b particles emitted when 90Th232 nucleus is converted into 82Pb208

4.      Determine the average life of U238 having t1/2 = 140 days. Or The half-life period of U238 is 140 days. Calculate the average life time.

5.      Explain the principle behind the 'Hydrogen bomb'.

6.      Give any three differences between chemical reactions and nuclear reactions.

7.      Half-life period of 79Au198 nucleus is 150 days. Calculate its average life.

8.      How many α and β   particles will be emitted by an element 82A218 is changing to a stable isotope of 84B206?

9.      In the conversion of 92U238 → 82Pb206. Calculate the number of alpha and beta particles emitted.

10.  In the following radioactive decay: 92X232 → 89Y220 how many α and β particles are ejected?

11.  The atomic masses of U, He and Proton are 7.01823 amu. 4.00387 amu and 1.00715 amu respectively. Calculate the energy evolved in the reaction.  3Li7+ 1H1 → 2 2He4 + Energy (1 amu = 931MeV).

12.  The decay constant for 6C14 is 2.31 x 10-4 year-1. Calculate the half life period.

13.  The half-life period of a radioactive element is 100 seconds. Calculate the disintegration constant.

14.  What is the Q value of a nuclear reaction?

15.  Write the uses of Radio carbon dating.
16. What is binding energy of nucleus?

17. Neutron bombardment fragmentation of U - 235 occurs according to the equation:

92U235 + 0n1 → 42Mo98 + 54Xe136 + x -1e0 + y 0n1. Calculate the values of x and y.

18. What is spallation reaction? Give an example

19. Write the nuclear reation taking place in the sun.

Unit - 8 (Q – 38)

1.      Determine the number of CsCl units per unit cell. CsCl has BCC arrangement.

2.      How are glasses formed?

3.      Sketch the following lattices: a) Simple cubic b) Face-centred cubic c) Body centred cubic.

4.      State Bragg's law.

5.      What are superconductors? Give its applications.

6.      What is a vitreous state?

7.      What is meant by super conducting transition temperature?

8.      What is molecular crystal? Give an example.

9.      Write a note on Frenkel defect.

10.  Write a note on molecular crystals.

11.  Write a note on the assignment of atoms per unit cell in fcc.

12. Give the uses of superconductors

13. Write Bragg’s equation and explain the terms.

14. Write about metal excess defect

15. What is metal deficiency defect? Give an example

Unit - 9 (Q – 39)

1.      ΔH and ΔS values of a reaction at 300K are –10 k.cal mole-1 and 20 cal. deg-1 mole-l respectively. Calculate ΔG value. Or For a chemical reaction the values of ΔH and ΔS at 300 K are –10 k cal mol-1 and 20 cal deg–1 mol–1 respectively. What is the value of ΔG of the reaction? Predict the nature of the reaction.

2.      Calculate the change of entropy for the process, water (liquid) → water (vapour, 373K) involving ΔH(vap), 373K = 40850J mol-1

3.      Calculate the maximum % efficiency possible from a thermal engine operating between 110°C and 25°C.

4.      Calculate the molar heat of vaporisation of the ideal liquid CCl4 (Boiling point of CCl4 is 76.7°C and ΔS = 87864 J).

5.      Give the entropy statement of second law of thermodynamics. Mention the unit of entropy also.

6.      Give the Kelvin-Planck statement of second law of thermodynamics.

7.      How is ΔG related to ΔH and ΔS? What is the meaning of ΔG = 0?

8.      State Clausius statement of second law of thermodynamics.

9.      State Trouton's rule.

10.  What are the substances that deviate from Trouton's rule? Or What types of liquids or substances deviate from Trouton's Rule?

11.  What is entropy? What is its unit?

12.  What is Gibbs' free energy?

13.  What is the entropy change of an engine that operates at 100°C when 453.6 kcal of heat is supplied to it?

14.  What is the nature of the reaction when - i) ΔG > 0? ii) ΔG < 0? iii) ΔG = 0?
15. Calculate the entropy increase in the evaporation of 1 mole of a liquid when it boils at 100°C having heat of vaporisation at 100°C as 540 Cal / gm.

16.  Calculate the entropy change involved in the conversion of 1 mole of ice at 0°C and 1 atm to liquid at 0°C and 1 atm. The enthalpy of fusion per mole of ice is 6008 J mol-l.

Unit - 10 (Q – 40)

1.      Define / What is equilibrium constant?

2.      Define / What is reaction quotient. How is it related to equilibrium constant?

3.      Dissociation equilibrium constant of HI is 2.06 x 10-2 at 458°C. At equilibrium, concentration of HI and I2 are 0.36 M and 0.15 M respectively. What is the equilibrium concentration of H2 at 458°C?

4.      Dissociation of PCl5 decreases in presence of increase in Cl2. Why?

5.      For the reaction A + B ⇄ 3C at 25°C, a 3 litre volume reaction vessel contains 1, 2 and 4 moles of A, B and C respectively at equilibrium, calculate the equilibrium constant Kc of the reaction at 25°C.

6.      In the equilibrium H2 + I2  ⇄ 2HI, the number of moles of H2, I2 and HI are 1, 2, 3 moles respectively. Total pressure of the reaction mixture is 60 atm. Calculate the partial pressures of H2 and HI in the mixture.

7.      State Lechatlier’s principle.

8.      The equilibrium constant Kc for A(g)  ⇄ B(g) is 2.5 x 10-2. The rate constant of the forward reaction is 0.05 sec-1. Calculate the rate constant of the reverse reaction.

9.      What happens when Δn_g = 0, Δn_g = – ve, Δn_g = + ve in a gaseous reaction?

10.  What is the relationship between formation equilibrium constant and dissociation constant? Give one example.

11.  Why is equilibrium reaction referred to as dynamic equilibrium?

12.  Write the equlibrium constants (Kc & Kp) for the following reactions:

i) H2O2(g) ⇄ H2O(g)+ (g) 2O2      ii) CO(g)+H2O(g) ⇄  CO2(g)+H2(g)    iii) N2O4(g) ⇌2NO2(g)
 

Unit - 11 (Q – 41)

1.      Define half life period.

2.      Derive an equation for the half-life period of a first order reaction.

3.      Give any three examples for opposing reactions.

4.      Show that for a first order reaction time required for 99% completion is twice the time required for 90% completion of the reaction.

5.      The initial rate of a first order reaction is 5.2 x 10-6 mol lit-1 s-1 at 298 K, when the initial concentration of the reactant is 2.6 x 10-3 mol lit-1. Calculate the first order rate constant of the reaction at the same temperature.

6.      What are simple and complex reactions?

7.      What is pseudo first order reaction? Give an example.

8.      Write Arrhenius equation and explain the terms.
9. Give any three Characteristics of simple reactions

10. Write any two characteristics of first order reaction.

11. What is threshold energy?

Unit - 11 (Q – 42)

1.      Define order of a reaction.

2.      The half-life period of a first order reaction is 20 mins. Calculate the rate constant.

3.      The rate constant for a first order reaction is 1.54 x 10–3sec–1. Calculate its half-life period.

4.      What are consecutive reactions? Give an example. Or Write a (brief) note on consecutive reactions.

5.      What are opposing reactions? Give an example.

6.      What are parallel reactions? Give an example.

7.      Write a note on 'activation energy’.
8. Give three examples for first order reaction. 

Unit - 12 (Q – 43)

1.      Give any three differences between physical adsorption and chemical adsorption.

2.      What are emulsions?

3.      What are lyophilic sols? Give example.

4.      What are promoters? Give an example.

5.      What is Brownian movement? Give reason.

6.      What is Catalytic Poison? Give an example.

7.      What is electrodialysis?

8.      What is electrophoresis?

9.      What is heterogeneous catalysis? Give an example

10.  What is (meant by) Tyndall effect?

11.  What is peptisation? Give an example.

12.  What is tanning?

13.  Why colloidal system of gas in gas does not exist?

14.  Write a note on auto-catalyst.

15.  Write any three general characteristics of catalytic reaction.
16. Define colloidal solution

17. How is Delta formed?

18. What is catalysis? Give an example

19. What are Active centres?

20. What are Lyophobic colloids? Give an example.

21. Give the dispersed phase and dispersion medium for gel. Give an example for gel

Unit - 13 (Q – 44)

1.      Define electrochemical equivalent. What is its unit?

2.      Define equivalent conductance. Give the equation for it.

3.      State Faraday's first and second laws of electrolysis.

4.      State Kohlrausch's law.

5.      State Ostwald's dilution law.

6.      The mass of the substance deposited by the passage of 10 ampere of current for 2 hours 40 minutes and 50 seconds is 9.65 g. Calculate the electrochemical equivalent.

7.      What do you understand / is meant by Buffer solution? Mention its types. Give an example.

8.      What is common ion effect? Give an example. Or What is meant by common ion effect?

9.      Why does the metallic conduction decrease with increase in temperature?

10. What is ionic product of water? Give its value.

11. What are indicators? Give an example.

12. Define molar conductance. Mention its unit.

Unit - 15 (Q – 45)

1.      Differentiate diastereomer from enantiomer. Or Distinguish enantiomers and diastereomers.

2.      Give the conditions required for a compound to exhibit optical isomerism. Or What are the conditions for a compound to be optically active?

3.      Give the structure of cis-trans isomers of 2-pentene.

4.      Identify cis or trans isomers from the following:

        

 

5.      Label the following as, E, Z isomers.

            

6.      Mesotartaric acid is an optically inactive (compound with asymmetric atoms / chiral carbon atom.) Justify.

7.      Trans-isomer is more stable than cis-isomer. Why?

8.      What are optical isomers? Give example.

9.      What is racemic mixture? Give an example. Or Write briefly on 'Racemic mixture' with an example.

10. Define 'Racemisation'.

11. Give the structure of Z and E forms of Cinnamic acid

12. Draw the structure of S – cis and S – trans form of 1, 3 – butadiene

13. Distinguish Meso form from Racemic mixture

14. Write the formula (configuration) for d, l and meso tartaric acid.

Unit - 16 (Q – 46)

1.      Alcohols cannot be used as a solvent for Grignard reagents. Why?

2.      Give a brief account on coupling reaction of phenol with benzene diazonium chloride.

3.      Give chemical test to distinguish between ethanol and methanol.

4.      How can Terylene / Dacron be prepared? Or How is Terylene / Dacron prepared from glycol?

5.      How can the consumption of alcohol by a person be detected?

6.      How is benzyl alcohol prepared by Grignard's synthesis?

7.      How is phenol identified?

8.      How is phenol prepared by Dow's process? Or Explain Dow's process.

9.      How will you convert C2H5OH to C2H5 O C2H5

10.  Phenols are soluble in alcohols. Why?

11.  Phenol is insoluble in NaHCO3 solution but acetic acid is soluble. Give reason.

12.  What happens when ethylene reacts with cold dilute alkaline KMnO4?

13.  Why is glycol more viscous than ethanol?

14.  Write a note on Kolbe's reaction.

15.  Write the dye test for phenol. Or How Phenol is identified by dye test? Give equation.

16. Give the Victor Meyer's test for tertiary alcohol.
17. Give short notes on Riemer - Tiemann reaction

18. What is the action of oxalic acid on glycerol at 533 K?

19. Write the equation for action of heat on ethylene glycol with conc. Phosphoric acid.

20. Give the oxidation reaction of phenol.

21. Write the Victor Meyer's test for secondary alcohol.

22. How are 1-propanol and 2-propanol distinguished by oxidation method?

Unit - 16 (Q – 47)

1.      Explain the synthesis of glycerol from propylene. Or How is glycerol synthesized from propylene?

2.      Give any three uses of benzyl alcohol.

3.      How is allyl alcohol obtained from glycerol?

4.      How is ethylene glycol converted into 1, 4-dioxan?

5.      How is nitroglycerine prepared from glycerol?

6.      How is phenolphthalein prepared? Or How will you convert phenol to phenolphthalein?

7.      How is tertiary butyl alcohol converted to isobutylene? Or How will you convert 2-methyl-2-propanol into 2-methyl propene?

8.      How is Terylene prepared from ethylene glycol?

9.      Starting from phenol how would you obtain picric acid?

10.  What happens when glycerol reacts with KHSO4? Or How does glycerol react with KHSO4? Or How is acrolein formed?

11.  Write a note on coupling reaction.Or Write the dye test for phenol
12. How is formic acid prepared from glycerol?

13. Give tests to identify phenol.

14. What happens when the vapour tert-butyl alcohol is passed over heated copper at 573 K?

15. What is glycerose? How is it prepared from glycerol?

16. Give the Victor Meyer's test for tertiary alcohol.

17. Explain Schotten - Baumann reaction

Unit – 18 (Q – 48)

1.      Explain haloform reaction with an example.

2.      Formaldehyde and benzaldehyde give Cannizzaro reaction but acetaldehyde does not account for this?

3.      Give the IUPAC names for the following:

i) Crotonaldehyde ii) Methyl n-propyl ketone iii) Phenyl acetaldehyde.

4.      How does formaldehyde react with ammonia?

5.      How is acetophenone prepared by Friedel-Crafts reaction?

6.      What is formalin? Write its use.

7.      What is Rosenmund's reduction? What is the purpose of adding BaSO4 in it?

8.      What is urotropine? How is urotropine prepared? Give / Mention its important use.

9.      Write briefly on Clemmensen’s reduction.

10.  Write two tests to identify aldehydes.
11. What happens when Benzaldehyde is heated with concentrated NaOH?

12. How does acetone react with chloroform in the presence of KOH?

13. Write Perkins reaction

14. How is benzophenone prepared by Friedel Crafts reaction?

15. State Popott’s rule

16. Write Knoevenagal reaction

17. Write the formula of hexa methylene tetramine and draw its structure.
18. Give the IUPAC name of

 

Unit - 19 (Q – 49)

1.      Account the reducing nature of formic acid with suitable illustration.

2.      Formic acid reduces Tollen’s reagent, but acetic acid does not. Give reasons.

3.      Give tests for Salicylic acid.

4.      Give the source and trivial names of i) C3H7COOH  ii) HCOOH and iii) C11H23COOH

5.      How is methyl salicylate prepared?

6.      Mention the uses of benzoic acid.

7.      Mention the uses of oxalic acid.

8.      What is aspirin? How is it prepared?

9.      What is meant by esterification reaction? Write the equation.

10.  What is the reaction of lactic acid with dil. H2SO4?

11.  What is trans-esterification?

12.  Write a note on HVZ reaction.

13.  Write two tests to identify carboxylic acids.
14. Mention the uses of Formic acid

15. Write the uses of Lactic acid

16. Compare the strength of mono, di, trichloro acetic acid

17. Give the IUPAC name of the following

       a) HOOC – COOH                      b) CH3COOH                     c) HOOC – (CH2)4 – COOH

 18. Give the structures of lactyl chloride and lactide 

Unit - 20 (Q – 50)

1.      An aromatic primary amine A with molecular formula C6H7N undergoes diazotisation to give B. B when treated with hypo phosphorous acid gives C. Identify A, B and C.

2.      An aromatic simplest nitro compound A on reduction using Sn and HCl gives B. B undergoes carbylamines reaction. Identify A and B. Give any one use of compound A.

3.      An organic compound (A) having molecular formula C2H7N is treated with nitrous acid to give (B) of molecular formula C2H6O which answers iodoform test. Identify (A) and (B) and explain the reaction.

4.      An organic compound (A) having molecular formula C2H7N is treated with nitrous acid to give (B) of molecular formula C2H6O which on mild oxidation gives compound (C) of molecular formula C2H4O which answers Tollen’s reagent test. Identify A, B, C.

5.      An organic compound (A) with molecular formula C6H7N gives (B) with HNO2/HCl at 273K. The aqueous solution of (B) on heating gives (C) which gives violet colour with neutral FeCl3. Identify the compounds A, B and C.

6.      An organic compound A of molecular formula C2H5NO on treatment with Na/C2H5OH gives B (C2H7N) and with Br2/ KOH gives C (CH5N). Identify A, B. C.

7.      An organic compound A of molecular formula C2H5ON treated with bromine and KOH -gives B of molecular formula CH5N. Identify A and B. Write the equation involved.

8.

 
9.      Compound A is yellow coloured liquid and it is called oil of mirbane. A on reduction with tin and HCl gives B. B answers carbylamine test. Identify A and B.

10.  How will you convert acetamide to methyl amine? Give equation.

11.  What is diazotisation? Give an example.

12.  What is Gabriel phthalimide synthesis? Or Explain / Write Gabriel’s phthalimide synthesis.

13.  When benzamide is treated with bromine and alkali gives compound A. Also when benzamide is reduced by LiAlH4 compound B is formed. Find A and B. Write the equations.
14. An aromatic primary amine A with molecular formula C6H7N undergoes diazotization to give B. When the aqueous solution of B is boiled it gives C. Identify A, B and C.
15. An organic compound ‘A’ C7H7NO when treated with Br2 / alkali gives ‘B’ C6H7N ‘B’ undergoes diazotization reaction. Identify ‘A’ & ‘B’
16. How is chloropicrin prepared? What is its use? 

Unit - 22 (Q – 51)

1.      Give a note on antibiotics.

2.      Give the preparation of Buna-N rubber.

3.      How is Buna-S rubber prepared? Give its use. Or Write a brief note on Buna-S.

4.      How is Dacron prepared? Give any one of its uses.

5.      How is nylon-66 prepared? Give its use.

6.      In what way are antacids important?

7.      What are anaesthetics? Give example. Or Illustrate with suitable examples the term ‘Anaesthetics’.

8.      What are antacids? Give an example.

9.      What are artificial sweetening agents? Give two examples.

10.  What are Chromophores? Give two examples.

11.  Why are iodoform and phenolic solutions called antiseptic?

12.  Write any three characteristics of dyes.

13. What are antipyretics? Give an example.

14. What are food preservatives? Give an example.

15. What are Antioxidants? Give examples

16. Define chemotherapy

17. What are Auxochromes? Give an example

18. What is antiseptic? Give an example. Or Write a brief note on `Antiseptic'. 

 Part – III  5 Mark Qs  – 52 to 63
Section – A

Q – 52 (Unit – 1)

1.      Apply molecular orbital theory to oxygen molecule. Or Explain the formation of O2 / oxygen molecule using molecular orbital theory.

2.      Derive / Define de Broglie's equation.

3.      Discuss Davisson and Germer’s experiment.

4.      Explain the formation of N2 / nitrogen molecule by using molecular orbital theory.

5.      Give any five postulates of molecular orbital theory.

6. Discuss the shapes of d orbital

7. Discuss the shapes of p orbital

8.      Problems

Q – 53 (Unit – 4)

1.      Explain how potassium dichromate is extracted from chromite ore. Or How is potassium dichromate prepared from chrome iron ore?

2.      Explain the extraction of silver from its chief ore. Or How is silver extracted from its ore?

3.      Explain the extraction of Zinc from its chief ore. Or How is zinc extracted from its chief ore?

4.      How is Cr2O3 reduced to chromium by aluminothermic process? Or Explain aluminothermic process involved in the extraction of chromium.

5.      How is gold extracted from its chief ore? Or How is gold extracted?

Q – 54 (Unit – 5)

1.      Compare / List the points of similarities and differences between lanthanides and actinides. Or Compare the properties of lanthanides and actinides.

2.      Describe the extraction of lanthanides from monazite sand. Or How are lanthanides extracted from monazite sand?

3.      Discuss the position of lanthanides in the periodic table

4.      Mention the oxidation state and of uses of lanthanides.

5.      What is lanthanide contraction? Discuss its causes and consequences.

6.      Write the uses of Lanthanides and Actinides

Section – B

Q – 56 (Unit – 9)

1.      Describe / Explain / Mention / Write the characteristics of free energy G.

2.      Give / State / Write the various statements of second law of thermodynamics.

3.      What are the characteristics of entropy?

4.      Define Troutan’s rule. What are the substances that deviate from this rule?

Q – 57 (Unit – 10)

1.      Apply Le Chatelier's principle for the manufacture of SO3 by contact process and find the conditions for getting maximum yield of SO3.

2.      Apply Le Chatelier's principle to Haber's process for the manufacture of Ammonia.

3.      Derive the expression for Kc and Kp for formation of HI.

4.      Derive the expressions for Kc and Kp for decomposition of PCl5.

5.      Derive the relation Kp = Kc(RT)Δng for a general chemical equilibrium reaction. Or Derive a relation between (equilibrium constant) Kp and Kc.

6.      Discuss the effect of temperature and pressure on the following equilibrium:

N2O4(g) ⇄ 2NO2(g) ΔH = +59.0 kJ / mole.

7. Apply Le Chatelier’s principle for the following reaction N2(g) + O2(g) ⇌ 2NO(g) and discuss the effect of pressure and concentration on it.

8.      Problems

Q – 58 (Unit – 11)

1.      Derive rate constant equation for first order reactions.

2.      Discuss the characteristics of a first order reaction.

3.      Explain the experimental determination of rate constant for the decomposition of hydrogen peroxide in aqueous solutions.

4.      Explain the experimental determination of rate constant of acid hydrolysis of methyl acetate

5.      Explain various types of complex reactions and give one example for each. Or Write notes on (i) consecutive reactions, (ii) parallel reactions and (iii) opposing reactions.

6.      Give / State / Write the characteristics of order of a reaction.

7.      State the differences between simple and complex reactions.

8.      Problems

Section – C

Q – 60 (Unit – 17)

1.      Discuss the isomerism in ethers. Or Discuss the isomerism exhibited by ethers.

2.      Distinguish between anisole and diethyl ether. Or Give the differences between anisole and diethyl ether.

3.      Distinguish between aromatic ethers and aliphatic ethers. Or Distinguish aliphatic and aromatic ethers.

4.      Give any three methods of preparation of ethers.

5.      Give any three methods of preparing diethyl ether.

6.      Give any two methods of preparation of anisole and explain the reaction of HI with anisole.

7.      How do ethers react with HI? Give the significance of the reaction.

8.      How does diethyl ether react with PCl5, one equivalent of HI and excess of HI?

9.      How does diethyl ether react with the following reagents? a) O2 / long contact b) dil.H2SO4 c) PCl5.

10.  Mention three methods of preparing anisole.

Q – 61 (Unit – 18)

1.      Discuss the mechanism of aldol condensation.

2.      Explain / Give the mechanism for Claisen or Claisen-Schmidt reaction.

3.      Explain / Write the mechanism of crossed aldol condensation (of acetone).

4.      Explain 'Popott's rule' with an example.

5.      Explain the mechanism of aldol condensation in acetone.

6.      Explain the mechanism of aldol condensation of acetaldehyde. Or Discuss the mechanism involved in aldol condensation of acetaldehyde.

7.      Explain the mechanism of Cannizzaro reaction

8.      How is acetone converted to - i) mesityl oxide ii) mesitylene?

9.      Illustrate the reducing property of acetaldehyde with examples

10.  Write notes on i) Perkin’s reaction and ii) Knoevenagal reaction iii) Stephen’s reaction.

11.  Write the differences between acetaldehyde and acetone.

12. Write the differences between Acetaldehyde and Benzaldehyde Or

       Compare Aliphaticaldehyde and Aromatic aldehyde

13. Write a note on  i) Clemmenson reduction     and         ii) Knoevenagel reaction

Q – 63 (Unit – 22)

1. Explain briefly on (characteristics of) rocket propellants. Or Write a note on Rocket propellants.

2. Explain briefly on colour and structure of dyes. Or

    Explain Otto – Witt chromophore and auxochrome theory about dyes.

3. Give the characteristics of a dye.

4. How are Buna – S and Nylon – 66 prepared?

5. What are chromophores and auxochromes? Give two examples for each.

6. Write a note on anaesthetics.

7. Write briefly on Buna rubbers.

Part – IV   10 Mark Qs     64. a) to 69. b)

 Q – 64.a (Unit – 2)

1.      Explain any three factors which affect the ionisation energy.

2.      Explain how electronegativity values help to find out the percentage of ionic character in polar covalent bond.

3.      Explain Pauling's method to determine / calculate ionic radii. Or How is ionic radius determined by Pauling's method?

4.      Explain the various factors that affect / influence electron affinity.

5.      How do electronegativity values help to find out the nature of bonding between atoms?

6.      Write notes on Pauling’s and Mulliken’s Scale of Electronegativity. Give the disadvantages.
7. Explain the variation of ionisation energy along the group and period

Q – 64.b (Unit – 3)

1.      Describe in detail how noble gases are isolated by Dewar's process. Or How are noble gases separated by Dewar's method?

2.      Describe in detail how noble gases are isolated from air by Ramsay - Rayleigh's method.

3.      Discuss the structure of interhalogen compounds of AX and AX3 type.

4.      Explain the extraction of lead from its ore. Or How is lead extracted from its ore?

5.      Explain the following: i) dehydrating property of P2O5 ii) oxidizing power of fluorine.

6.      How are noble gases isolated from air?

7.      How does Fluorine differ from other halogens? Or Write the anomalous nature of fluorine.

8.      How is fluorine isolated from their fluorides by Dennis method?

9.      Illustrate i) tribasic nature of orthophosphoric acid ii) reducing property of Phosphorus acid.

10.  Mention the uses of silicones.
11. Write a short note on Etching on glass

Q – 65.a & Q – 55 (Unit – 6)

1.      [Ni(CN)4]2– is diamagnetic whereas [Ni(NH3)4]2+ is paramagnetic. Explain using VB theory.

2.      Apply V.B. theory for magnetic properties of [Ni(CN)6]4–and [FeF6]4– and explain the shape.

3.      Explain / Give / Write the postulates of Werner's theory. Or State the postulates of Werner's theory on co-ordination compound.

4.      Explain Co-ordination isomerism and ionisation isomerism with suitable examples.

5.      Explain hydrate and linkage isomerisms with suitable examples.

6.      For the complexes K4[Fe(CN)6], [Cu(NH3)]SO4 mention  a) IUPAC names b) Central metal Ion c) Ligand d) Co-ordination number e) Charge on the complex ion f) Geometry of the complex g) Nature of complex

7.      How is chlorophyll important in environmental chemistry? Mention its function.

8.      In the coordination complex [Co(NH3)6]Cl3 mention the following: a) IUPAC name of the complex b) Ligand c) Central metal ion d) Co-ordination number e) Nature of complex.

9.      Mention the type of hybridisation, magnetic property and geometry of the following complexes using VB theory. Or Write the application of VB theory on the following complexes: i) [FeF6]4– ii) [Fe(CN)6]4– Or In what way does [FeF6]4– differ from [Fe(CN)6]4–?

10.  Mention the function of haemoglobin in natural process.

11.  Apply VB theory to find out the geometry of [Ni(NH3)4]2+ and calculate its magnetic moment.

12.  Explain the following terms: i) Neutral ligand  ii) chelates iii) coordination sphere.

13.  What are the postulates of valence bond theory?

14. Explain the type of hybridisation, magnetic property and geometry for [Ni(CN)4]2– and [Ni(NH3)4]2+  using VB theory

15. For the complex K3[Cr(C2O4)3].3H2O mention    a) Name   b) Central metal ion          c) Ligand       

       d) Co–ordination number e) Geometry

16. Write : a) IUPAC Name        b) Central metal ion          c) Ligand            d) Coordination number

      e) Geometry of the complex [Co(en)3]Cl3

17. For the complex [Co(NH3)3(NO2)3] Write the following a) IUPAC Name  b) Central metal ion

       c) Ligand      d) Coordination number e) Geometry

18. Mention the the following for the complex [Co(NH3)4Cl2]NO2 a) IUPAC Name b) Central metal ion

c) Ligand            d) Charge on the Co-ordination sphere          e) Co-ordination number 

Q – 65.b (Unit – 7)

1.      Differentiate between chemical reaction and nuclear reaction. Or Distinguish chemical reactions from nuclear reactions.

2.      Distinguish between nuclear fusion reactions and nuclear fission reactions.

3.      Explain nuclear fission reaction with an example.

4.      Explain nuclear reactions that take place in sun.

5.      Explain Radio carbon dating. Or Write a note on / briefly about radio carbon dating.

6.      Explain the principle in the function of hydrogen bomb. Or Explain the principle underlying the function of hydrogen bomb.

7.      How are radioactive isotopes useful in medicine? Or List the medicinal uses of radioactive isotopes.

8.      Mention the use of radio isotopes in the field of

a) study of hydrolysis of ester                  b) mechanism of photosynthesis in plants.

Q – 66.a (Unit – 8)

1.      Explain Bragg's spectrometer method (in / for crystal study / the study of crystals).

2.      Explain Schottky defect and Frenkel defect (in crystals).

3.      Explain the nature of glass.

4.      What are superconductors? Write their uses.

5.      Write notes on any two point defects in Crystals.

6.      Write the properties of ionic crystals.

Q – 66.b (Unit – 12)

1.      Discuss the factors affecting adsorption.

2.      Explain the intermediate compound formation theory of catalysis. Or Write briefly on intermediate compound formation theory of catalysis with an example.

3.      Give any 5 main differences between physical adsorption and chemical adsorption.

4.      How are colloids prepared by chemical methods? Or Write any two chemical methods for the preparation of colloids.

5.      How can colloidal solutions be purified by dialysis?

6.      What is electro-osmosis? Explain the experiment.

7.      Write any three methods for the preparation of colloids by dispersion methods.

8.      Write briefly about the adsorption theory of catalysis.

9.      Write notes on i) Ultrafiltration and ii) Helmholtz double layer.

10.  Write notes on a i) Auto catalyst ii) Promoters.

11.  Write the general characteristics of catalytic reactions.

Q – 67.a (Unit – 13)

1. Derive / Derive an expression for / Explain Ostwald's dilution law

2. Derive Henderson Equation.

3. Differentiate between electronic conduction and electrolytic conduction.

4. Explain / Write the postulates of Arrhenius theory of electrolytic dissociation.

5. Explain Ostwald's theory of indicators.

6. Explain Quinonoid theory of indicators.

7. Explain the buffer action of acidic buffer with an example.

8. What are the evidences in favour of Arrhenius theory of electrolytic dissociation?

9. Explain the buffer action of basic buffer with an example

Q –  67.b & Q – 59 (Unit – 14)

1. Derive Nernst equation (of reversible cell.)

2. How is a Standard Hydrogen Electrode (SHE) constructed? Explain its function.

3. Write an account on Cell terminology.

4. Derive the relation between e.m.f and free energy. Or Establish a relation between free energy and e.m.f 

     Or Write a brief account on the relation between EMF and free energy.

5. Describe Daniel cell.

6. How is e.m.f of a half cell determined?

7. Write IUPAC representation of a cell. Or Write notes on IUPAC convention of representation of a cell.

     Or Write the IUPAC conventions for writing cell diagram with examples.

8. Write notes on single electrode potential.

9. With the help of the electrochemical series, how will you predict whether a metal will displace another metal from its salt solution or not.

 Problems

Q – 68.a (Unit – 15)

1. Describe / Write a note on the conformations of cyclohexanol. Comment on their stability.

2. Discuss / Write in detail about the optical isomerisim in tartaric acid. Or

    Discuss / Explain the optical activity of tartaric acid.

3. Discuss cis-trans isomerism with a suitable example. Or Explain geometrical isomerism with example.

4. Distinguish enantiomers from diastereomers. Give an example each.

5. Distinguish racemic mixture from meso-form with suitable example.

6. Explain internal and external compensation with suitable example.

7. Explain the following isomerism with examples.

    i) cis–trans isomerism in organic compounds          ii) optical isomerism in organic compounds

8. Write the possible isomers of dichlorobenzene and their dipole moment order

9. Write a note on the different types of hydrogen in cyclohexane

68.b Q – 62 (Unit – 19)

1. Account for the reducing property of formic acid.

2. How are the following conversions carried out? a. Salicylic acid → Aspirin

     b. Salicylic acid → Methyl salicylate         c. Lactic acid → Lactide     d. Benzoic acid → Benzyl alcohol.

3. Discuss / Give / Write the mechanism of bromination of salicyclic acid.

4.  Distinguish between formic acid and acetic acid

5. Explain the mechanism of Kolbe's reaction.

6. Explain the reactions of CH3CONH2 with i) P2O5 ii) Br2 / NaOH and iii) hydrolysis by an acid.

7. Give the equation for the action of heat on a) Oxalic acid b) Succinic acid c) Formic acid.

8. Give the mechanism involved in the esterification of a carboxylic acid with alcohol. Or

     Write the mechanism of esterification reaction

9. How the following conversions are carried out / take place? i) Methyl acetate → Ethyl acetate

     ii) Lactic acid → Pyruvic acid       iii) Methyl cyanide → Acetamide      iv) Succinic acid → succinimide

     v) Acetamide → Methyl amine?

10. How is benzoic acid obtained from a) C6H5CH2CH3 / Ethyl benzene b) Phenyl cyanide

       c) Carbon dioxide?

11. How is lactic acid manufactured in large scale / fermentation method? How can it be converted into cyclic diester?

12. How is lactic acid synthesised from acetylene? How can it be converted into cyclic diester?

13. How is oxalic acid manufactured from sodium formate?

14. What happens when i) Oxalic acid is treated with NH3 ii) Benzoic acid is treated with PCl5?

15. What happens when benzoic acid reacts with i) conc. HNO3 / Conc. H2SO4 ii) Cl2 / FeCl3 iii) PCl5?

16. What happens when lactic acid is i) treated with dilute H2SO4  ii) added to / treated with PCl5 

        iii) oxidised with alkaline / acidified KMnO4?

17. What happens when lactic acid is      i) treated with dilute H2SO4                 ii) heated alone

       iii) oxidised with Fenton’s reagent?

18. Discuss the isomerism exhibited by carboxylic acid.

19. Explain  i) Decarboxylation              ii) trans-esterification reaction         iii) Kolbe's electrolytic reaction

       iv) Claisen ester condensation         v) Friedel Crafts acetylation

20. How can salicylic acid be converted to i) Aspirin ii) Methyl salicylate iii) 2, 4, 6 tribromophenol? Or

       How do Salicylic acid react with the following? a) CH3OH        b) (CH3CO)2O     c) Br2 / H2O

21. Write the preparation of Salicylic acid with mechanism

22. How do Succinic acid react with the following? i) NaOH ii) NH3 iii) PCl5

Q – 69.a (Unit – 20)

1.      Distinguish between primary, secondary and tertiary amines.

2.      Explain / Write a note on the reduction of nitrobenzene under different conditions.

3.      Explain / Write the following reactions: i) Carbylamine reaction ii) Gabriel's phthalimide synthesis.

4.      Explain the following reactions in aniline:

a) Coupling reaction b) Schotten-Baumann reaction c) Carbylamine reaction

5.      How are i) phenol, ii) chlorobenzene, iii) biphenyl prepared by using benzene diazonium chloride?

6.      How are the following conversions carried out? a) Nitromethane to methylamine b) Methylamine to methyl isocyanide c) Benzene diazonium chloride to biphenyl

7.      How are the following conversions carried out? i) Nitrobenzene to phenyl hydroxylamine ii) Aniline to phenyl isocyanide iii) Benzene diazonium chloride to biphenyl.

8.      How can the following conversions be effected / carried out?

i. Nitrobenzene to Anisole  ii. Chlorobenzene to Phenyl hydrazine iii. Aniline to Benzoic acid

9.      How does nitrous acid react with primary, secondary and tertiary amines?

10.  Write any three methods of preparing benzylamine?

11.  Write notes on the following i) Mustard oil reaction ii) Diazotisation reaction iii) Gomberg reaction.

12. Explain the reduction of Nitrobenzene in alkaline medium

13. Srarting from benzene diazonium chloride how will you obtain the following i) Phenol   ii) Anisol

  iii) p-hydroxy azobenzene 

Q – 69.b (Unit – 21)

1.      Derive / Discuss / Elucidate / Prove the structure of glucose (in detail).

2.      Discuss / Elucidate the structure of fructose in detail. Or How is the structure of fructose determined?

3.      Explain the functions of lipids in Biosystems.

4.      How are carbohydrates classified? Give example for each. Or Outline the classification of carbohydrates giving example for each.

5.      Mention the biological functions of nucleic acids

6.      What is a peptide bond? Explain / Illustrate the formation of a peptide bond in glycyl alanine. Draw the structures of glucose and fructose.
7. Distinguish between glucose and fructose.

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Posted by : Mr. Ravi N, Lecturer in Chemistry, Govt. Girls' Hr. Sec. School, Kathirkamam, Puducherry - 605 009