2 & 3 Marks
1. The elements belong to the Group 1 and 2 in the modern Periodic
table are called s-block elements. Why?
2. List the names of Alkali metals Or List the names of elements belong to the
Group 1.
3. Which Alkali metal is highly radioactive? Give its Half -
life period.
4. Give the Mineral Source of Alkali metals.
5. Where are Alkali metals stored? Why?
6. Give the Electronic configuration of Alkali metals.
7. Alkali metals have only one Oxidation state which is + 1.
Why?
8. Write the Atomic radius / Metallic radius of Alkali metals in increasing
order.
9. Write the Ionic radius of Alkali metals in increasing
order.
10. Write the Ionisation enthalpy of Alkali metals in
increasing order.
11. On moving down the group Atomic radius and Ionic radius of
Alkali metals increases. Why?
12. The Ionisation enthalpy of Alkali metals decreases down
the group. Why?
13. The Second Ionisation enthalpies of Alkali metals are
very high. Why?
14. Lithium salts are more Soluble than the salts of other
metals of Group 1. Why?
15. What is the Periodic trend of Electronegativity of Alkali
metals?
16. Write note on Flame colour and the Spectra of Alkali metals.
17. What are the reasons for the Distinctive behavior of Lithium?
18. What is the reason for the Diagonal relationship between Lithium
and Magnesium?
19.
Explain
the reaction of
Alkali metals with Liquid Ammonia.
20.
Alkali metals dissolve in Liquid Ammonia are Conducting in nature. Why?
21. Alkali metals dissolve in Liquid Ammonia to give deep
blue solution. Why?
22. What will happen when Alkali metals are standing for long
time in Liquid Ammonia?
23. Write balanced chemical equation for reaction of Alkali
metals with Water.
24. Write balanced chemical equation for reaction of Alkali
metals with Alcohol.
25. Write
balanced chemical equation for reaction of Alkali metals with Alkynes.
26.
Alkali metals act as good Reducing agents. Why?
27.
Give the equation for the reaction of Lithium with Carbon.
28.
How will you produce Hydroxides from Alkali metals?
29.
What will happen when Na, K, Rb and Cs upon combustion with excess Air? And then
they are upon reacting with Water.
30.
Give the equations for the reaction of Super oxides of K, Rb and Cs with Water.
31. Substantiate Lithium fluoride has the Lowest solubility among
Group 1 metal fluorides.
32. Give the Uses of
Sodium carbonate, Na2CO3.10H2O /
Washing soda.
33. Give the Uses of
Sodium chloride, NaCl /
Cooking salt / Table
salt.
34. Give the Uses of
Sodium hydroxide, NaOH.
35. Give the Uses of
Sodium bicarbonate, NaHCO3 /
Backing soda / Sodium
hydrogen carbonate.
36. Why Sodium hydroxide is much more water soluble than
chloride?
37. An Alkali metal (X) forms a Hydrated sulphate, X2SO4.10H2O. Is
the metal more likely to be Sodium or Potassium?
38. Write balanced
Chemical equation for heating solid Sodium bicarbonate.
39. Write balanced
Chemical equation for reaction of solid Potassium hydroxide with CO2.
40. Explain what is
meant by Efflorescence.
41. List the names of Alkaline earth metals Or List the names of elements belong to the
Group 2.
42. Give the Mineral Sources
of Alkaline earth metals.
43. Give the Electronic
configuration of Alkaline earth metals.
44. Write the Atomic
radii of Alkaline earth metals in increasing order.
45. Write the Ionic
radii of Alkaline earth metals in increasing order.
46. Write the Ionization
enthalpy of Alkaline earth metals in increasing order.
47. On moving down
the group Atomic radius and Ionic radius of Alkaline earth metals
increases. Why?
48. On moving down the
group the Ionisation enthalpy decreases as Atomic size increases. Why?
49. Alkaline earth metal
elements exhibit + 2 Oxidation state in their compounds. Why?
50. Alkaline earth
metals are Harder than Alkali metals. Why?
51. The Atomic radii and
Ionic radii of Alkaline earth metals are Smaller than the corresponding members
of the Alkali metals. Why?
52. Ionisation enthalpy
of Alkaline earth metals is Higher than the corresponding members of the Alkali metals. Why?
53. Second Ionisation
enthalpy of Alkaline earth metals is much smaller than the corresponding
members of the Alkali metals. Why?
54. Compounds of
Alkaline earth metals are more extensively Hydrated than those of Alkali
metals. Why?
55. What is the Periodic trend of Electronegativity of
Alkaline earth metals?
56. Write a note on Flame colour and the Spectra of
Alkaline earth metals.
57. What are the reasons for the Distinctive behavior of
Beryllium?
58. What is the reason for the Diagonal relationship between
Beryllium and Aluminium?
59. Give
the Uses of Beryllium.
60. Give the Uses of Strontium.
61. Give the Uses of
Radium.
62. Alkaline earth
metal compounds are Less ionic than the corresponding compounds of Alkali
metals. Why?
63. BeO is Covalent. Why?
64. List the General characteristics of Oxides of Alkaline
earth metals.
65. How will you prepare Peroxides from Alkaline earth
metals?
66. Write
balanced Chemical equation for heating Calcium with Oxygen
67. Show /
Prove that Beryllium hydroxide / Be(OH)2 is Amphoteric.
68. How will you produce Hydroxides from Alkaline earth
metals?
69. How will you produce Halides from Alkaline earth metals?
70. Beryllium halides are Covalent whereas Magnesium halides are
Ionic. Why?
71. Draw the Structure of Beryllium chloride.
72. BeSO4 and MgSO4 dissolve readily in Water.
Why?
73. What is the action of Heat on Alkaline metal Carbonates?
74. What is the action of Heat on Alkaline metal Nitrates?
75. How are Alkaline metal Nitrates prepared?
76. Explain the Preparation of Calcium oxide / Quick lime.
77. Give the Uses of Calcium oxide.
78. How is Calcium hydroxide / Lime water prepared?
79. Give the Uses of Calcium hydroxide.
80. How is Plaster of Paris prepared?
81. Mention the Uses of Plaster of Paris.
82. Which would you expect to have a Higher Melting point, Magnesium
oxide or Magnesium fluoride? Explain your reasoning.
5 Marks
1. Give the Characteristics of Alkali metals. Or Give the
Characteristics of Group 1 elements. Or
Explain the Important Common features of
Group 1 elements.
2. Compare the Properties of Lithium with other elements of
the group.
3. Discuss briefly the Similarities between
Lithium and Magnesium.
4. Explain the Important Chemical properties of Alkali
metals.
5. Write
balanced chemical equation for each of the following chemical reactions:
i) Lithium metal with Nitrogen gas ii) Lithium metal
with Oxygen
iii) Sodium metal
with Oxygen iv)
Potassium metal with Oxygen
v)
Rubidium with Oxygen gas vi)
Cesium with Oxygen gas
6. Write
balanced chemical equation for the chemical reaction of Hydrogen with Li, Na,
K, Rb and Cs. Or How is Alkali metals react with Hydrogen?
7.
Write balanced chemical equation for the reaction of F2, Cl2, Br2, and I2 with Li, Na, K, Rb and Cs. Or How is Alkali metals react with the Halogens?
8.
Give the Uses of Alkali metals.
9. Write the Chemical equations for the reactions involved in
Solvay process of Preparation of Sodium carbonate.
10. Give the Systematic names for the following:
i) Milk of Magnesia ii) Lye
iii) Lime iv) Caustic
potash v) Washing soda
vi) Soda ash vii) Trona
11. How is Sodium
hydroxide prepared commercially by Castner - Kellner method?
12. Explain Biological
importance of Sodium and Potassium.
13. Explain the Important Common features of Group 2 elements.
Or Give the
Characteristics of Alkaline metals.
14. Compare the Properties of Beryllium with other elements
of the group.
15. Discuss briefly the Similarities between Beryllium and
Aluminium. Or
Discuss the
Similarities between Beryllium and Aluminium.
16. Explain the Important Chemical properties of
Alkaline earth metals.
17. How is Alkaline earth metals react with the Halogens?
18.
How is Alkaline earth metals react with Hydrogen?
19. Give the Uses of Magnesium.
20. Give the Uses of Calcium.
21. Give the Uses of Barium.
22. Give the equations for the reaction of Alkaline earth metals with
Oxygen.
23. Alkaline earth metal (A), belongs to 3rd period reacts with
Oxygen and Nitrogen to form compound (B) and (C) respectively. It undergo
metal displacement reaction with AgNO3 solution to form compound (D). Identify A, B, C and D.
24. Explain the Chemical properties of Calcium oxide.
25. Explain the Chemical properties of Calcium hydroxide.
26. Give the Properties of Gypsum.
27. Give the Uses of Gypsum.
28. Write balanced Chemical equation for the following processes:
a) heating Calcium in Oxygen
b) heating Calcium carbonate
c) evaporating a solution of Calcium
hydrogen carbonate
d) heating
Calcium oxide with Carbon
29. Describe briefly the Biological importance of Calcium and
Magnesium.
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