#### +1 Public Exam March 2019 Important Creative Questions and Answers

11th Standard

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Chemistry

Time : 02:30:00 Hrs
Total Marks : 200
70 x 2 = 140
1. Define relative atomic mass.

2. What do you understand by the term oxidation number?

3. Balance the following equations by ion electron method - ${ C }_{ 2 }{ O }_{ 4 }^{ 2- }+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { Cr }^{ 3+ }+{ CO }_{ 2 }$ (in acid medium)

4. Balance the following equations by oxidation number method - ${ KMn }O_{ 4 }+{ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }+{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ MnSO }_{ 4 }+{ CO }_{ 2 }+{ H }_{ 2 }O$

5. Give examples for the following redox reaction "Metal displacement reaction".

6. 3 grams of hydrogen reacts with 29 g of O, to yield H2O. Which is the limiting reagent?

7. What is the equivalence factor (n) for K2Cr2O7

8. Define matter. What are the types of matter?

9. How many orbitals are possible for n =4?

10. How fast must a 54g tennis ball travel in order to have a de Broglie wavelength that is equal to that of a photon of green light 5400$\overset { 0 }{ A }$ ?

11. Consider the following electronic arrangements for the d5 configuration.
(a)

 $\upharpoonleft \downharpoonright$ $\upharpoonleft \downharpoonright$ $​​\upharpoonleft$

(b)

 $​​\upharpoonleft$ $​​\upharpoonleft$ $​​\upharpoonleft$ $\upharpoonleft \downharpoonright$

(c)

 $​​\upharpoonleft$ $​​\upharpoonleft$ $​​\upharpoonleft$ $​​\upharpoonleft$ $​​\upharpoonleft$

(i) which of these represents the ground state
(ii) which configuration has the maximum exchange energy.

12. What are the defects of Rutherford's model?

13. At what distance is the radial probability maximum for 1s orbital? What is this distance called?

14. How many electrons can be accommodated in the main shell I,m and n?

15. What are isoelectronic ions? Give examples.

16. Define electro negativity.

17. Give the general electronic configuration of lanthanides and actinides.

18. Give Mosley's relationship.

19. Mention the characteristics of 'p' block elements

20. Explain why noble gases are inert?

21. Calculate the screening constant in Zinc for (i) 4s electron, (ii) for a 3d electron. The electronic configuration of Zinc (30) is (ls)2 (2s, 2p)(3s,3p)8 (3d10) (4s)2

22. State the Newland's law of octaves.

23. State Mendeleev's periodic law.

24. Define valency. How is it determined?

25. Explain why hydrogen is not placed with the halogen in the periodic table.

26. Predict which of the following hydrides is a gas on a solid (a) BCI (b) NaH. Give your reason.

27. NH3 has exceptionally high melting point and boiling point as compared to those of the hydrides of the remaining element of group 15. Explain.

28. At room temperature, Hydrogen reacts very slowly. Explain

29. Explain what is meant by efflerescence.

30. Beryllium halides are Covalent whereas magnesium halides are ionic why?

31. Why alkaline earth metals are harder than alkali metals.

32. Alkali metals give a characteristics colour for a bunsen flame. Explain why?

33. Mention the uses of sodium hydroxide.

34. Mention the uses of calcium oxide (CaO).

35. Name two items that can serve as a model for Gay Lusaac' law and explain.

36. Distinguish between diffusion and effusion.

37. State the first law of thermodynamics.

38. What is the usual definition of entropy? What is the unit of entropy?

39. Define enthalpy of combustion.

40. What is lattice energy?

41. Explain Zeroth law of thermodynamics.

42. For the equilibrium PCI5(s) ⇌ PCl3(g) + CI2(g) at 25°C kc = 1.8 x 10-7 R = 8.314 Jk-1 mol-Calculate ΔGo for the reaction.

43. What is entropy of Vapourisation?

44. What the relation between KP and KC. Give one example for which KP is equal to KC.

45. Explain how will you predict the direction of a equilibrium reaction.

46. Derive the relation between KP and KC.

47. For the reaction,${ A }_{ \left( g \right) }+{ B }_{ \left( s \right) }\rightleftharpoons { C }_{ \left( g \right) }+{ D }_{ \left( g \right) }$ Kc = 50 mol lit-1at 127°C. Calculate Kp'

48. How much volume of 6 M solution of NaOH is required to prepare 500 mL of 0.250 M NaOH solution.

49. State Raoult law and obtain expression for lowering of vapour pressure when nonvolatile solute is dissolved in solvent.

50. Define the term ‘isotonic solution’.

51. State Raoult's law

52. What is a pi bond?

53. What is dipole moment?

54. Explain the bond formation in BeCl2 and MgCl2.

55. Explain VSEPR theory. Applying this theory to predict the shapes of IF7, and SF6.

56. What are the number of bond pairs and lone pairs of electrons on N-atom in N${ O }_{ 3}^{ - }$?

57. The type of overlap given below do not involve in bond formation - Why?

58. Describe the classification of organic compounds based on their structure.

59. Describe optical isomerism with suitable example.

60. Explain electromeric effect.

61. $C{ H }_{ 2 }=\overset { - }{ C } H$ is more basic than $HC\equiv { C }^{ - }$ . Explain why?

62. What happens when isobutylene is treated with acidified potassium permanganate?

63. Explain Markow nikoff's rule with suitable example.

64. Identify A and B.

65. Classify the following compounds in the form of alkyl, allylic, vinyl, benzylic halides
(i) CH3 – CH = CH – Cl
(ii) C6H5CH2I
(iii) ${ CH }_{ 3 }-\underset { \overset { | }{ Br } }{ CH } -{ CH }_{ 3 }$
(iv) CH2 = CH – Cl

66. Why is it necessary to avoid even traces of moisture during the use of Grignard reagent?

67. Complete the following reactions
i) CH3 - CH = CH2 + HBr $\overset { Peroxide }{ \longrightarrow }$
ii) CH3 - CH2 - Br + NaSH $\overset { alcohol }{ \underset { { H }_{ 2 }O }{ \longrightarrow } }$
iii) C6H5Cl + Mg $\overset { \Delta }{ \longrightarrow }$
v) CCl4 + H2$\overset { \Delta }{ \longrightarrow }$

68. Define Walden inversion

69. Define particulate pollutants.

70. What is the tolerable limit of fluoride ions in drinking water? What happens if it exceeds 10 ppm?

71. 20 x 3 = 60
72. Mass of one atom of an element is 6.645 x 10-23g. How many moles of element are there in 0.320 kg.

73. How would you know whether a redox reaction is taking place in an acidic, alkaline or neutral medium?

74. One million silver atoms weigh 1.79 x 10-16 g. Calculate the atomic mass of silver.

75. Calculate the equivalent mass of potassium dichromate in acid medium
[K2Cr2O7 + 4H2SO4 )$\rightarrow$K2SO4 + Cr2(SO4)3 +4H2O + 3(O) 3 x 16 = 48 294 g]

76. Identify the type of redox reaction taking place in the following
$\overset { +5 }{ { Y }_{ 2 } } \overset { -2 }{ { O }_{ 5(s) } } +5\overset { 0 }{ { Ca }_{ (s) } } \longrightarrow \overset { 0 }{ 2 } { V }_{ (s) }+\overset { +2 }{ 5 } \overset { -2 }{ { CaO }_{ (s) } }$

77. How many moles of hydrogen is required to produce 10 moles of ammonia?

78. Calculate the uncertainty in position of an electron, if Av = 0.1% and $\upsilon$ = 2.2 x 106 ms-1.

79. Explain the shapes of p orbitals

80. In what period and group will an element with Z = 118 will be present?

81. Why is water molecule polar?

82. Why sodium hydroxide is much more water soluble than chloride?

83. Which of the following gases would you expect to deviate from ideal behavior under conditions of low-temperature F2, CI2, or Br2? Explain.

84. What are spontaneous reactions? What are the conditions for the spontaneity of a process

85. For an equilibrium reaction Kp = 0.0260 at 25° C ΔH= 32.4 kJmol-1, calculate Kp at 37° C

86. What volume of 4M HCl and 2M HCl should be mixed to get 500 mL of 2.5 M HCl?

87. What is the mass of glucose (C6 H12O6) in it one litre solution which is isotonic with 6 g L-1 of urea (NH2 CO NH2)?

88. Write all the possible isomers of molecular formula C4H10O and identify the isomerisms found in them.

89. 0.284 g of an organic substance gave 0.287 g AgCl in a carius method for the estimation of halogen. Find the Percentage of Cl in the compound.

90. From where does ozone come in the photo chemical smog?

91. Explain how oxygen deficiency is caused by carbon monoxide in our blood? Give its effect