2nd Year Chemistry Chapter 2 s Block Elements Notes MCQs

chemistry 12th notes chapter No 2

1. Which of the following on heating above 100 C gives plaster of Paris:


2. The first ionization energy is higher for the:


3. CaMg₃(SiO₃)₄ is the composition of:


4. Point out the ore of potassium:


5. The element necessary for normal “leaf” development is:


6. Which is not an alkali metal?


7. The alkali metal that reacts with nitrogen directly to form Nitride is:


8. Epsom salt is:


9. Ga has most common oxidation state of:


10. Which ion will have the maximum value of heat of hydration:


11. Which of the elements can produce H₂ gas when treated with  sodium hydroxide:


12. Which one  is not an alkali metals:


13. Which of the following is a rare radioactive element:


14. Dolomite is an ore of:


15. Which halide has the highest melting point:


16. Due to inert pair effect ___________ oxidation state is more stable than ___________ for Sn and Pb.


17. Magnetic effect of current is used:


18. Which of the following is a man-made element?


19. Which of the  compound in formed when Na burn in excess of air:


20. The milk of magnesia is used for the treatment of:


21. Beryllium metal is as hard as:


22. One of the  alkali metals is the most reactive which is that:


23. What is deposited at the cathode during the electrolysis of brine:


24. Alkali metals form:


25. On heating quick lime with coke in an electric furnace, we get:


26. Melting point of pure sodium chloride is:


27. Which of the following does not belong to alkaline earth metals:


28. Oxides and hydroxides of Group 1 elements are:


29. Chemical formula of slaked lime is:


30. If a charge Q flows through any cross section of the conductor in time t, the current I is:


31. A rheostat can be used as variable resistor as well as a __________


32. The only alkaline earth metal which forms peroxide is:


33. Which one does not belong to alkaline earth metals?


34. When some water is added to plaster of Paris, it becomes hard and expansion  in volume how much:


35. All the carbonates, sulphates and phosphates of alkaline earth metals are ___________ in water.


36. Dead burnt gypsum is:


37. Nelson’s cell is used to prepare:


38. When sodium burn in air, it forms sodium:


39. Which pair has both members from same period of periodic table?


40. Which of the following compounds has a per oxide linkage:


41. Which one of the following compounds when dissolved in water reacts with CO₂:


42. LI₂O is:


43. The conventional current is due to the flow of:


44. The product of resistance and conductance is:


45. Down’s cell is used to prepare:


46. Washing soda has the formula:


47. Halite is chemical name of:


48. Which of the following sulphates is not soluble in water:


49. Which  is not a function of sulphur:


50. Which carbonate of alkali metals is insoluble in water:


51. During electrolysis process, density of CuSO₄ solution:


52. The sulphate compound insoluble in water is:


53. Which does not belong to alkali metals:


54. CaCl₂ is added to NaCl in Down’s cell to:


55. Cement contains gypsum:


56. CaSO4⋅ 2H₂O has general name:


57. Which of the following alkali metal hydroxide is the strongest base:


58. Chemical formula of Magnesite is:


59. Which one configurations corresponds to an alkaline earth  metals:


60. The alkali metal whose carbonate is relatively less stable to heat and decomposes on heating, giving its oxides is:


61. Terminal potential difference is greater than emf of the cell when:


62. The substance deposited at the cathode during electrolysis of brine in diaphragm cell:


63. Select the correct increasing order of atomic radius?


64. Chile Salt peter has the chemical formula:


65. Which of following oxides amphoteric is nature?


66. If there is no fourth band, tolerance is shows as:


67. Which of the following oxides is amphoteric in nature?


68. The resistivity of___________ decrease with the increase in temp.


69. Which is the strongest reducing agent?


70. The carbonates of alkali metal are not affected by heat except:


71. Oxidizing power of halogen depends upon:


72. Sodium metal cannot be stored in:


73. The formula of its oxide would be :


74. Which one does not give flame test:


75. Group VII-A elements are generally called:


76. Dolomite has the composition


77. Green is characteristic flame colour of:


78. When a pot difference of 4 volt is applied across resistance, 10 J of energy is converted, Find charge flows:


79. Melting points and boiling points of alkali metals:


80. An aqueous solution of sodium carbonate is alkaline because sodium carbonate is a salt of:


81. The chemical formula of Magnesite is:


82. Lime is often used as:


83. Plaster of Paris is a hydrate of:


84. For non-ohmic devices, the graph between V and I is:


85. The substance not likely to contain CaCO₃ is :


86. The operating temp of Down’s cell is:


87. The main product of the reaction of potassium with oxygen is


88. Dolomite is a carbonate of:


89. Sodium metal can be stored in:


90. Highest electron affinity is shown by?


91. Which one of the element has the maximum electron affinity?


92. Dolomite is:


93. Substance boiling at higher temperature among following is?


94. The flame colour of sodium metal or its compounds is:


95. Which is produced at the cathode during the electrolysis of brine in Nelson’s  cell:


96. The condition for the wheatstone bridge to be balanced is given by:


97. The radioactive element in halogen group is:


98. The oxide of Beryllium is:


99. Unit (S.I) of temperature coefficient of resistivity of a material is:


100. Lime (CaO) is obtained by thermal decomposition of:


Short Questions

1. BeO is and amphoteric oxide. Justify it?
2. Give advantages of Down’s Cell.
3. Give formulae of Natron and Halite.
4. Give four points in which lithium differs from its own family members?
5. Give the name and formulas for the common minerals of magnesium?
6. Give the names and formulas for common minerals of beryllium?
7. Give the names and formulas for common minerals of calcium?
8. Give two major problems that may arise in Nelson’s cell.
9. Heat of hydration of alkaline earth metals go on decreasing from upper to the downward direction:Why?
10. How do you compare LiNO₃ with nitrates of other alkali metals?
11. How do you compare the carbide of beryllium with carbide of calcium?
12. How do you compare the carbonate of lithium with the carbonates of other family members?
13. How do you compare the solubilities of hydroxide of alkaline earth metals?
14. How do you compare the solubilities of sulphates of alkaline earth metals?
15. How do you discuss the effects of heat on the carbonates of group I-A and II-A?
16. How does beryllium react with NaOH to give a salt and evolve hydrogen?
17. How gypsum is converted into plaster of Paris?
18. How KO₂ can be used by mountaineers?
19. How lime and sand are used to make glass?
20. How LiNO₃ and NaNO₃ differ in application of heat. Give corresponding equations.
21. How magnesium and calcium react with nitrogen to give nitrides which on hydrolysis give ammonia?
22. In what respects nitrates of Li Mg and Ba are related with each other?
23. Lithium only gives a simple oxide with oxygen but sodium and potassium give peroxide and superoxide.Why?
24. Mention the flame test of II-A group elements?
25. Prove that decomposition of lithium nitrate gives different products than nitrates of other alkali metals?
26. Reaction of alkali metal oxide with water is acid-base reaction and not an oxidation-reduction reaction. Justify.
27. Solution of Na₂O in water is alkaline and oxides of other alkali metals are alkaline. Justify the statement?
28. Solution of Na₂O in water is alkaline. Justify the statement.
29. The compounds of alkali and alkaline earth metals are colorless but some of them are colored. Give reason?
30. What are milk of magnesia and what is its use?
31. What are the advantages of Down’s cell for the preparation of sodium on commerial scale?
32. What are the flame tests of alkali metals?
33. What are the important ores and minerals of potassium?
34. What are the important ores and minerals of sodium?
35. What are the most abundant elements among the alkali metals in earth’s crust?
36. What happens when CO₂ gas is passed through lime water?
37. What happens when excess CO₂ is passed through lime water?
“38. What happens when:
a. LI₂CO₃ is heated
b. Na₂CO₃ is heated “
39. What is difference between soda ash and washing soda?
40. What is lime and lime water?
41. What is lime mortar? How is it formed?
42. What is lime water and milk of magnesia?
43. What is Plaster of Paris?
44. What is Plaster of Paris? Give its two applications.
45. What is the action of litmus with aqueous solution of Na₂CO₃ ?
46. What is the effect of heat on hydroxides of alkali metals?
47. What is the effect of temperature on Na₂CO₃?
48. What is the importance of sulphur for the plants?
49. What is the trend of changing basicity of oxides down the groups in alkali and alkaline earths?
50. What is the trend of the solubilities of oxides of alkaline earth metals?
51. When sodium reacts with water the hydrogen which evolves catches fire:Why?
52. Which element of group I-A reacts with nitrogen and carbon?
53. Which substances are deposited at cathode and anode in the Nelson’s cell?
54. Why 2% gypsum is added into the cement?
55. Why alkali and alkaline earth metals are the most reactive elements of the periodic table?
56. Why CaCI₂ is added in moltan NaCI in Down’s cell?
57. Why does lithium differ from its own family members?
58. Why is the aqueous solution of Na₂CO₃ alkaline in nature?
59. Why KO₂ is used in breathing equipment used by mountaineers and astronauts?
60. Why lime is added to acidic soil?
61. Why lime water turns milky by passing CO₂ gas but becomes clear with excess of CO₂?
62. Why the alkali metals are not found free in nature?
63. Why the alkali metals are strong reducing agents?
64. Why the alkaline earth metals are reducing agents but less reducing than those of group I-A?
65. Why the aqueous solution of Na₂CO₃ is alkaline in nature?
66. Why the elements of group I-A are called alkali metals?
67. Why the elements of group II-A are called alkaline earth metals?
68. Why the ionic hydrides are very good reducing agents?
69. Why the lime water turns white after white wash on the walls?
70. Why the melting and boiling points of group I-A and II-A decrease down the group?
71. Why the plaster of Paris is called half hydrate?
72. Write two points of difference of Beryllium with its family members.

Long Questions

1. Show four chemical reactions in which Li behaves different from elements of its own group.
2. Compare the chemical behavior of lithium with magnesium.
3. Discuss peculiar behavior of Beryllium with respect to other member of II-A group.
“4. Complete and balance the following equations:
KO₂+ CO₂ ——>
Na₂O₂ + H₂O —–>
Mg₃N₂ + H₂O —–>
BeO + NaOH —–>”
5. Give the reaction of sodium with oxygen.
6. Give reaction of Mg with Nz followed by its hydrolysis.
7. Write the reaction of potassium with (i) hydrogen sulphide (ii) ferrous sulphate (iii) oxalic acid (d) potassium hydroxide
8. Describe the commercial preparation of sodium by Down’s cell. What are advantages of this process?
9. Explain the construction of Down’s cell. Give reactions. place at cathode and anode.
10. Describe preparation of sodium hydroxide by Nelson’s cell.
11. Discuss the role of gypsum in industry.
12. Describe eight points to discuss role of lime in industries.
13. Give four application of lime in agriculture and four applications in industry.
14. Give the formula of Sylvite, Borax, Trona, Natron, Dolomite, Alunite, Asbestos and Barite.
15. Describe occurrence of alkali metals and alkaline earth metals in nature.

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