MOST IMPORTANT 3 MARKS QUESTIONS FROM VOLUME - I CHAPTER -1 ATOMIC STRUCTURE - II

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1 1 MOST IMPORTANT 3 MARKS QUESTIONS FROM VOLUME - I CHAPTER -1 ATOMIC STRUCTURE - II 1. What do you understand by dual character of matter? 2. State Heisenberg s Uncertainty Principle. 3. Distinguish between a particle and a wave. 4. What are molecular orbital? 5. What are the conditions for effective H 2 -bonding? 6. Why is He 2 not formed? (or) Draw the molecular orbital diagram of Helium molecule. 7. What is bond order? 8. What is the significance of negative electronic energy? 9. Define Hybridisation. 10. Give the applications of de Broglie concept. 11. Give any three methods of verifying the particle character of matter. 12. Give the significance of de Broglie concept. 13. Write about the shape of s orbital. 14. Write about the shape of p orbital. 15. Write about the shape of d orbital. 16. Draw the molecular orbital diagram of Hydrogen molecule. 17. Predict the hybridization of (a) BCl 3 (b) NH (c) CO 3 [Any one ] 18. What is hydrogen bonding? 19. Give the three importance of hydrogen bonding. 20. Calculate the momentum of a particle which has a de-broglie wavelength of 1 Å CHAPTER -2 PERIODIC PROPERTIES - II 21. Why is electron affinity of fluorine less than that of chlorine? (B)(M6,8,13,S7,S9,10) 22. Why is the first ionisation energy of Beryllium greater than that of Lithium? (J6,11) 23. Explain why the first ionisation energy of Be is greater than that of B. (S6) 24. Compare the ionisation energy of Nitrogen with that of Oxygen? (M7) 25. Compare the ionisation energy of Boron and Carbon. (J12) 26. The Ionisation energy of Nitrogen is greater than that of Carbon. Give reason. 27. The Ionisation energy of Neon is greater than that of Fluorine.Give reason. (S9,J10) 28. Mention the Disadvantage of Pauling s and Mullikan s electronegativity scale. (B)(S8) 29. Why is the ionization energy of Fluorine greater that of Oxygen? (M9) 30. The electron affinities of Beryllium and Nitrogen are almost zero.why? (M10) 31. The electron affinities of noble gases are zero.why? 32. The electron affinities of group 17 elements are high.why? 33. Calculate the electronegativity of fluorine by Mulliken scale. The ionization energy of fluorine is 17 ev/atom. The electron affinity of fluorine is 3.62 ev/atom. (M11) 34. If the d(c-cl) is 1.76 Å and r (Cl) is 0.99 Å., Find the radius of carbon atom? (B)(J7)

2 2 35. Calculate the effective nuclear charge experienced by the 4s electron in potassium atom. (S=16.8) (S7,12) 36. Define electron affinity. (M8) 37. Define electronegativity. CHAPTER -3 p BLOCK ELEMENTS 38. What is inert pair effect? (M9) 39. What is plumbo solvency? (B) (J6,7,9,S6,M10,13) 40. What is the action of lead with con. HCl? 41. How is potash alum prepared? (M8) 42. Mention the uses of potash alum. (J12) 43. How is phosphoric acid prepared in the laboratory? (J8) 44. H 3 PO 4 is triprotic. Prove. (M6,13) 45. Prove that phosphorous acid is a powerful reducing agent. (J6, M7) 46. How is phosphine prepared in the laboratory? 47. Prove that phosphine is a powerful reducing agent. 48. Illustrate the dehydration property of phosphorous pentoxide (P 2 O 5 ) with two examples. (B) (M7,9,J10,S6,12) 49. What happens when phosphorus acid of heated? (J9) 50. H 3 PO 3 is diprotic. Why? (S9,M10) 51. What is the action of heat on orthophosphoric acid? (M11) 52. Give the electronic structure of (i) H 3 PO 4 (ii) PCl 3 (iii) H 4 P 2 O Give the electronic structure of (i) H 3 PO 3 and (ii) PCl 5. (S8,J11) 54. Give one test for orthophosphoric acid. 55. Give the uses of orthophosphoric acid. 56. Write about the Holme s signal (S7,9) 57. What is etching of glass? 58. How is HF prepared? 59. Write the preparation of ClF, ClF 3 and IF 7. (J12) 60. Write three uses of fluorine. (S12) 61. Why is HF not stored in silica or glass bottles? Write the equation. (M7,11) 62. Illustrate the oxidising power of fluorine. (B)(J7) 63. What are interhalogen compounds? Give the preparation of any one. (B) (S8) 64. Interhalogen compounds are more reactive than halogens. Why? 65. Give three uses of Neon. (B) (J8,10,S10) 66. Write any three uses of Helium. (S7) 67. Give the uses of argon, krypton and xenon. 68. What are d block elements? 69. How are d block elements classified? CHAPTER - 4 d BLOCK ELEMENTS

3 3 70. Why does Mn(II) show maximum paramagnetic character among the bivalent ions of the first transition series? 71. Explain why Mn 2+ is more stable than Mn 3+. (B) (M6,J12) 72. A substance is found to have a magnetic moment of 3.9 BM. How many unpaired electrons does it contain? (B) (M6) 73. Find the magnetic moment of Fe +2 ion. 74. Zn, Cd, Hg do not form colourless compounds. Why? 75. Sc +3 and Zn +2 ions are colourless. Why? 76. Why do transition elements form complexes? (B) (J6,S7) 77. Why do d block elements have variable oxidation state? (B) (S6,J7,M13) 78. Why are Zn 2+ salts colourless while Ni 2+ salts are coloured? (B)(J9,S12) 79. Why are transition metal ions coloured? (S9) 80. Most of the transition metals and their compounds have catalytic activity. Why? 81. Why do transition metals form alloys? 82. How is chrome plating done? (S6,M8) 83. Write two alloys of copper and their uses. 84. Explain electrolytic refining of copper. (J7) 85. What is spitting of silver and how is it prevented? (S7,M13) 86. What is Philosopher s wool? How is it prepared? 87. What is the action of Zinc on hot NaOH solution? (S8) 88. Give any two evidences for the oxidising nature of potassium dichromate. (J6) 89. What happens when K 2 Cr 2 O 7 is heated? 90. Explain Chromyl chloride test with equation. (M9) 91. What is blue vitriol and how is it prepared? 92. What is the action of heat on copper sulphate crystals? Write the equation. 93. What is the reaction of CuSO 4 with NaOH and ammonia? 94. What is the reaction of CuSO 4 with KCN? 95. What happens when KI solution is added to an aqueous solution of copper sulphate? (S9) 96. What is the reaction of CuSO 4 with H 2 S? 97. How is Lunar caustic prepared? (S12) 98. What happens when AgNO 3 is heated? 99. What is aqua regia? Write the action of aqua regia on gold. (M7) 100. What is calamine and how is it prepared? 101. What is purple of cassius and how is it prepared? CHAPTER 8 SOLID STATE - II 102. Define Unit cell What are superconductors? Give any one of its applications.(b,m6,10,13j6,8,s6) 104. What is a Vitreous state? (B) (S6,S7) 105. How are crystals classified? 106. What is imperfection in solids?

4 What is coordination number? 108. Write a note on the assignment of atoms per unit cell in FCC Write a short note on Metallic crystals Write a note on ionic crystals Give any three properties of ionic crystals Write a note on covalent crystals Determine the no.of CsCl units per unit cell. CsCl has BCC arrangement.(b) (M What is meant by superconducting transition temperature? (J7) 115. Write a note on Molecular crystals. (M8) 116. Write a note on Frenkel defect. (J8) 117. Write a note on Schottky defect Sketch the following lattices : (B) (M9,J12) (a) Simple cubic (b) Face centred cubic (c) Body centred cubic 119. How are glasses formed? (B) (S9,12) 120. State the uses of super conductors. (B) (J10,S10) 121. State Bragg s law. (B) (J11) CHAPTER 9 THERMODYNAMICS - II 122. What is entropy? What is its unit? (B) (M6) 123. What is Gibbs free energy? (B) (J6) 124. What types of liquids or substances deviate from Trouton s Rule? (S6,J11) 125. Give the Kelvin-Planck statement of second law of thermodynamics. (B)(M7,S12) 126. State Claucius statement of second law of thermodynamics. (B) (J7) 127. When does entropy increases? 128. Mention the essential condition for spontaneity in a chemical reaction What is the entropy change of an engine that operates at 100 C. When k.cal of heat is supplied to it? (S7,9,J12) 130. Calculate the molar hear of vaporization of the ideal liquid CCl 4 (Boiling point of CCl 4 is 76.7 C and S = J) (M8) 131. H and S values of a reaction of 300K are -10Kcal mol -1 and 20 cal deg -1 mol -1 respectively. Calculate G value. (J8,10) 132. Give entropy statement of second law of thermodynamics. Mention the unit of entropy also. (S8) 133. Calculate the entropy change involved in the conversion of 1 mole of ice at 0 C and 1 atm. The entropy of fusion per mole of ice is 6008 J mol -1 ) (M9) 134. State Trouton s rule. (S9) 135. Give the limitations of Trouton s rule Calculate the change of entropy for the process water (liq) to water (Vapour, 373K) involving Vap = J mol -1 at 373 K (M10) mole Sn (α, 13 0 C) 1 mole Sn (β, 13 0 C) Calculate the entropy change for the following process possessing H (transition) = 2090 J mol -1. (M13) 138. How is G and S? What is the meaning of G=0? (B) (S10)

5 Calculate the maximum % efficiency possible from a thermal engine operating between 110 C and 25 C. (M11) CHAPTER 10 CHEMICAL EQUILIBRIUM - II 140. The equilibrium constant K c for A(g) B(g) is 2.5 x The rate constant of the forward reaction is 0.05 s -1. Calculate the rate constant of the reverse reaction. (M6) 141. In the equilibrium H 2 + I 2 2HI, the number of moles of H 2, I 2 and HI are 1,2,3 moles respectively. Total pressure of the reaction mixture is 60 atm. Calculate the partial pressure of H 2 and HI in the mixture. (J6) 142. Write the equilibrium constants K c for the following reactions (S6) (i) H 2 O 2(g) H 2 O (g) O 2(g) (ii) CO (g) + H 2 O (g) CO 2(g) + H 2(g) 143. State Le Chatelier s principle. (B)(M6,7,10,13) 144. What happens when n g = 0, n g = -ve, n g = +ve in a gaseous reaction? (J7) 145. Define reaction quotient. (S7) 146. What is the relationship between formation equilibrium constant and dissociation constant? (M8) 147. What is the Reaction quotient? How is it related to equilibrium constant? (J8) 148. 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 K c of the reaction at 25 C. (S8) 149. Degree of dissociation of PCl 5 at 1 atm 25 C is 0.2. Calculate the pressure at which PCl 5 is half dissociated at 25 C. (S12) 150. Explain the effect of temperature and pressure on the following equilibrium by using Le Chatlier s principle.n 2 O 4(g) 2NO 2(g) H = kj/mol (J12) 151. Dissociation of PCl 5 decreases in the presence of increase in Cl 2 Why?(B) (M9,J11) 152. Dissociation equilibrium constant of HI is 2.06x10-2 at 458 C. At equilibrium concentration of HI and I 2 are 0.36M and 0.15M respectively. What is the equilibrium concentration of H 2 at 458 C? (J9) 153. What is equilibrium constant? (B) (S9) 154. Why is chemical equilibrium called as dynamic equilibrium? (B) (M11)

6 1 MOST IMPORTANT 3 MARKS QUESTIONS FROM VOLUME - II CHAPTER -11 CHEMICAL KINETICS - II 1. Give the three examples for opposing reactions. (B) (M6,13,J9,S12) 2. Give three examples for first order reaction. (S12) 3. The half life period of a first order reaction is 20 min. calculate the rate constant. (M6) 4. The initial rate of a first order reaction in 5.2x10-6 mol lit -1 at -1 at 298 K. When the initial concentration of the reactant is 2.6x10-3 mol lit -1 calculate the first order rate constant of the reaction at the same temperature. (J6) 5. Show that for a first order reaction time required for 99% completion is twice the time required for 90% completion of the reaction. (S6) 6. What are consecutive reactions? Give an example. (J6,S6,12) 7. Write the Arrhenius equation and explain the terms. (B) (M7,13) 8. What are parallel reactions? Give an example. (M7,J12) 9. Define order of a reaction. (B) (J7) 10. What are opposing reactions? Give an example. (J7) 11. What are the simple and complex reactions? (B) (S7) 12. Define Activation energy. (B)(S7,M8) 13. What is pseudo first order reaction? Give an example. (M8) 14. Derive an equation for the half-life period of a first order reaction. (B) (S8) 15. What are complex reactions? Give an example. (B) (S8) 16. The rate constant of a first order reaction 1.54 x 10-3 s -1. Calculate its half life period (S10) 17. What is half life period? 18. What is zero order reaction? What is the rate constant of such reaction? 19. Define rate law. 20. Give any three characteristics of order of a reaction. 21. Write the first order rate constant equation and explain the terms. 22. Give the characteristics of a first order reaction. 23. Give the factors which affect the rate of a reaction. 24. Give any three differences between simple and complex reactions? CHAPTER -12 SURFACE CHEMISTRY 25. What is Electrophoresis? (B)(M6,13,J10) 26. Define colloidal solution. (B)(S12) 27. What are emulsions? (B) (J6) 28. White a note on Auto-Catalyst? (S6) 29. Why a colloidal system of gas in gas is does not exist? (B) (M7) 30. What is catalytic poison? Give an example. (J7) 31. What is Tanning? (S7) 32. What is heterogeneous catalysis? Give an example. (M8)

7 2 33. What are active centres? (B)(J12) 34. What are promoters? Give an example. (M10,J8,10) 35. What is electrodialysis? (M6,J10) 36. What is peptisation? Give an example. (S8) 37. What is Brownian movement? Give reason. (M9) 38. Give three differences between physical adsorption and chemical absorption. (S9) 39. What is Tyndall effect? (B)(S10,J11) 40. Write any three general characteristics of catalytic reaction. (M11) 41. Define adsorption. 42. Give the factors which affect the adsorption. 43. What is catalysis? 44. What are the types of catalysis? 45. Why are colloids purified? 46. What is Homogenous catalysis? 47. What is positive catalysis? 48. What is negative catalysis? 49. What is induced catalysis? 50. What is meant by Helmholtz double layer? 51. Give the types of emulsion with example. 52. What is an emulsifying agent? 53. How is artificial rain formed? CHAPTER -13 ELECTROCHEMISTRY - I 54. State Faraday s first and second laws of electrolysis. (M6) 55. State Faraday s second laws of electrolysis. (M13) 56. State Kohlrausch s law. (J6,S8,9,12) 57. What is meant by common ion effect? Give an example. (B) (S6,J7,S7,M8) 58. The mass of the substance deposited by the passage of 10ampere of current for 2 hours 40 minutes and 50 seconds is 9.65 g. Calculate the electro -chemical equivalent. (M7) 59. Define equivalent conductance. Give the equation for it. (B)(J8) 60. State Ostwald s dilution law. (B)(M9) 61. Define electrochemical equivalent. What is its Unit? (B)(J9) 62. What is buffer solution? Give example. (J10,11,12,S10) 63. Define Faraday. 64. What are insulators? Give an example. 65. What is buffer action? 66. What are indicators? 67. What is Henderson s equation? 68. Define specific conductance. Give the equation for it. 69. Define Molar conductance. Give the equation for it.

8 3 70. Define PH. 71. What is ionisation constant and ionic product of water? 72. Derive the relation between PH and POH. 73. Give the importance of Henderson s equation. 74. What are PH indicators? 75. What is called indicator range? 76. What is titration curve? Give its use. CHAPTER -15 ISOMERISM IN ORGANIC CHEMISTRY 77. Meso tartaric acid is an optically inactive compound with asymmetric carbon atoms. Justify your answer. (B) (M6,10,13,S6) 78. Differentiate diasteriomer from enantiomer. (B) (J6,12) 79. What are optical isomers? Give example. (J8) 80. Distinguish between racemic and meso forms. (B)(M7,11,J10,S10,12) 81. Label the following as E, Z isomers : (B)(J7) CH 3 CH 2 OH Cl H (i) (ii) CH 2 OH H Br F 82. What are the conditions for a compound to be optically active? (S7) 83. Identify Cis Trans isomer from the following : (S8) (i) H 3 C C C C = C Br (ii) C C H 3 C C = C Br H 3 C H Br CH What is racemic mixture? Give an example. (B)(M8) 85. Trans isomer is more stable than cis isomer Why? (J11) CHAPTER -16 HYDROXY DERIVATIVES 86. How can the consumption of alcohol by a person be detected? (B)(M6) 87. How will you convert phenol to phenolphthalein? (B)(M6,9,13,J6) 88. Why is glycol more viscous than ethanol? (B)(J6) 89. Give a brief account on coupling reaction of phenol with benzene diazonium chloride. (B)(S6,9,12) 90. Give any three uses of benzyl alcohol. (B)(S6) 91. Phenol is insoluble in NaHCO 3 solution but acetic acid is soluble. Give reason. (B)(M7) 92. What happens when glycerol reacts with KHSO 4? (B)(M7,10,J11,S10)

9 4 93. How will you convert C 2 H 5 OH to C 2 H 5 - O - C 2 H 5? (B)(J7) 94. Explain Dow s process. (B)(M10,J7) 95. Write the dye test for phenol. (B)(J11,S7) 96. How is allyl alcohol obtained from glycerol. (B)(S7) 97. Alcohols cannot be used as a solvent for Grignard reagents. Why? (B)(M8) 98. How is ethylene glycol concerted into dioxan? (B) (M8,S8,J12) 99. How is glycerol synthesized from propylene? (B)(J8) 100. Write a note on Kolbe s reaction. (B)(J8) 101. Give a chemical test to distinguish between ethanol and methanol. (B)(S8) 102. How ate 1-propanol and 2-propanol distinguished by oxidation method? (J12) 103. How is Terylene prepared from glycol? (B)(M9,11,J10) 104. How is phenol identified? (B)(M9) 105. How will you convert 2methyl 1-2 propanol into 2-methyl propene? (M11,J9) 106. What is glycerose? How is it prepared from glycerol? (M13) 107. How is formic acid obtained from glycerol? (S12) 108. What happens when ethylene reacts with cold dilute alkaline KMnO 4? (B)(J9) 109. Phenols are soluble in alcohols. Why? (B)(J10) 110. How will you convert phenol into picric acid? (B) (S10) CHAPTER -18 CARBONYL COMPOUNDS 111. Give the IUPAC names for the following. (B)(M6,13) (i) Crotonaledehyde (ii) Methyl n- propyl ketone (iii) Phenylaceteledehyde/ Benzaldehyde 112. How does formaldehyde react with ammonia? (B)(J6) 113. How is urotropine prepared? Mention its use. (B)(M8,10,J9,11,12,S6,9,10) 114. How is acetophenone prepared by Friedel Crafts method? (B)(M7,9,11) 115. What is formalin? Write its use. (B)(J7) 116. What is Rosenmund`s reduction?what is the purpose of adding BaSO 4 in it? (B)(S7) 117. What is urotropine? Give its use. (B)(M8) 118. Write two tests to identify aldehydes. (B)(J8) 119. What happens when benzaldehyde is heated with concentrated NaOH? (S12) 120. Explain haloform reaction with an example. (B)(S8) 121. Write briefly on Clemmensen s reduction. (J10) CHAPTER -19 CARBOXYLIC ACIDS 122. What is trans-esterification? (M6) 123. What is meant by esterification reaction? Write the equation. (B)(J6) 124. Write a note on HVZ reaction. (S6) 125. Mention the uses of oxalic acid. (B)(M7,9,J11) 126. Give the source and trivial name of (i)hcooh (ii)c 3 H 7 COOH(iii)C 11 H 23 COOH (B)(J9)

10 Formic acid reduces Tollen s reagent but acetic acid does not. Give reasons. (B)(S7,9,10,J12) 128. What is the reaction of lactic acid with dil.h 2 SO 4? (B)(M8) 129. How is methyl salicylate prepared? (J8) 130. Account for the reducing nature of formic acid with suitable illustration. (B)(S8) 131. Write two tests to identify carboxylic acids. (B)(M13,J9) 132. Give the identification tests for salicylicacid. (M10) 133. Mention the use of benzonic acid. (J10) 134. What is aspirin? How is it prepared? (M11) CHAPTER -20 ORGANIC NITROGEN COMPOUNDS 135. How will you convert acetamide to methyl amine? Give equation. (B)(M6) 136. An organic Compound (A) having molecular formula C 2 H 7 N is treated with nitrous acid to give (B) of molecular C 2 H 6 O which answers iodoform test. Identify (A) and (B) and explain the reaction (J6) 137. What is Gabriel s Phthalimide synthesis? (B)(M7,J10,11,S6,7,8) 138. Explain diazotisation with a suitable example. (B)(J7,9) 139. When benzamide is treated with bromine and alkali gives compound A. Also when benzamide is reduced by LiAlH 4, Compound B is formed. Find A and B. Write the equations. (M8) HNO 140. C 6 H 5 CH 2 NH 2 2 A (O) Zn/Hg B HCl C Identify A, B and C An aromatic primary amine (A) with molecular formula C 6 H 7 N undergoes diazotization to give (B).B when treated with hypophosphorous acid gives(c). Identify (A), (B) & (C). (M9) 142. An aromatic hydrocarbon a on nitration gives B which is known as oil of mirbane. B on warming with conc.h 2 SO 4 gives compound C. Identify A,B andc. (J12) 143. An organic compound A C 7 H 7 NO when treated with Br 2 /alkaligives B C 6 H 7 N. B undergoes diazotization reaction. Identify A & B. (S12) 144. An aromatic simplest nitro compd (A) on reduction using Sn and HCl gives (B). B undergoes carbylamine reaction. Identify (A) and (B). Give any one use of compound (A). (S9) 145. Compound (A) is yellow coloured liquid and it is called oil of mirbane (A) on reduction using Sn and HCl gives B. Compd B undergoes carbylamine reaction. What are (A) and (B)?(M10) 146. Organic Compound (A) with the molecular formula C 6 H 7 N gives (B) with HNO 2 /HCl at 273K. Aqueous solution of (B) gives (C) which gives violet. Colouration with neutral FeCl 3. What are (A), (B) and (C). (S10) 147. An Organic Compound (A) of molecular formula C 2 H 5 ON treated with bromine and KOH gives (B) of molecular formula CH 5 N. Identity (A) and (B). Write the reaction involved. (M11,13) (J8)

11 6 CHAPTER -22 CHEMISTRY IN ACTION 148. How is Dacron prepared? Give any one of the uses. (M6) 149. Write a brief note on Buna S. (B)(J6,11) 150. Write a brief note on Antiseptic. (S6) 151. What are antipyritics? Give an example. (M13) 152. What are Chromophores? Give two examples. (B)(M7,10,J9) 153. What are Anaethetics? Give example. (B)(J7,8,S10,12) 154. In what way are antacids important? (B)(S7,J12) 155. Why are iodoform and phenolic solutions called antiseptic? (B)(M8) 156. Write one method of preparation of Buna-N (S8) 157. How is nylon-66 prepared? Give one of its uses. (M9) 158. What are artificial sweeting agents? Give two examples. (B)(S9) 159. Write a note on antibiotics. (B)(J10) 160. Write any three characteristics of dyes. (B)(M11) 161. What are drugs? Give an example What is chemotherapy? 163. What are antispasmodics? Give an example What are analgesics? Give an example What are food preservatives? Give an example What are the functions of Antioxidants? 167. How is Polystyrene prepared? 168. How is Polyethene prepared?

MOST IMPORTANT 3 MARKS QUESTIONS FROM VOLUME - II CHAPTER -11 CHEMICAL KINETICS - II

1 MOST IMPORTANT 3 MARKS QUESTIONS FROM VOLUME - II HAPTER -11 HEMIAL KINETIS - II 1. Give the three examples for opposing reactions. (B) (M6,13,J9,S12) 2. Give three examples for first order reaction.