Class 10 Science – Chapter 3 Metals and Non-metals Question Bank

A. Multiple Choice Questions (MCQs)

Choose the correct option.

1. A metal can be converted into a thin sheet because it possesses:

(a) Ductility
(b) Malleability
(c) Sonority
(d) Conductivity

2. Which of the following is an unusual property of graphite?

(a) It is a metal
(b) It conducts electricity despite being a non-metal
(c) It is liquid at room temperature
(d) It reacts violently with water

3. Which pair contains amphoteric oxides?

(a) Na₂O and K₂O
(b) CO₂ and SO₂
(c) Al₂O₃ and ZnO
(d) CuO and MgO

4. Which metal is expected to react most vigorously with cold water?

(a) Copper
(b) Iron
(c) Sodium
(d) Silver

5. A metal that can displace copper from copper sulphate solution must be:

(a) Less reactive than copper
(b) More reactive than copper
(c) A non-metal
(d) Below gold in the activity series

6. Which process is mainly used to convert a sulphide ore into its oxide?

(a) Calcination
(b) Roasting
(c) Electrolysis
(d) Galvanisation

7. Which metal is obtained from its compounds using electrolytic reduction because of its high reactivity?

(a) Gold
(b) Copper
(c) Sodium
(d) Silver

8. During electrolytic refining, the pure metal is deposited on the:

(a) Anode
(b) Cathode
(c) Electrolyte
(d) Anode mud

9. Which combination is necessary for ordinary rusting of iron?

(a) Nitrogen and sunlight
(b) Oxygen and moisture
(c) Carbon dioxide and nitrogen
(d) Hydrogen and oxygen only

10. Brass is an alloy mainly consisting of:

(a) Copper and zinc
(b) Copper and tin
(c) Lead and tin
(d) Iron and chromium

11. Which metal is placed immediately below hydrogen in the given activity series?

(a) Lead
(b) Copper
(c) Mercury
(d) Silver

12. Which statement correctly describes ionic compounds?

(a) They generally have low melting points.
(b) They conduct electricity well in the solid state.
(c) They contain oppositely charged ions held by electrostatic attraction.
(d) They are generally insoluble in water.

13. Which metal is generally stored under oil because of its vigorous reaction with air and water?

(a) Sodium
(b) Copper
(c) Gold
(d) Silver

14. A carbonate ore is strongly heated to convert it into an oxide. This process is:

(a) Roasting
(b) Calcination
(c) Refining
(d) Galvanisation

15. Which reaction represents a displacement reaction?

(a) Cu + O₂ → CuO
(b) Zn + CuSO₄ → ZnSO₄ + Cu
(c) CaCO₃ → CaO + CO₂
(d) Na⁺ + e⁻ → Na

B. Fill in the Blanks

16. The ability of a metal to be drawn into wires is called __________.

17. The shiny appearance of a freshly polished metal is called metallic __________.

18. Oxides that react with both acids and bases are known as __________ oxides.

19. The naturally occurring substances from which metals can be extracted profitably are called __________.

20. The unwanted earthy materials associated with an ore are collectively called __________.

21. Heating sulphide ores strongly in excess air is known as __________.

22. Heating carbonate ores strongly with limited air is known as __________.

23. The gradual deterioration of a metal due to environmental reactions is called __________.

24. Coating iron or steel with zinc to protect it from rusting is called __________.

25. In electrolytic refining, the impure metal is used as the __________.

26. The insoluble impurities collected below the anode during electrolytic refining are called __________.

27. A homogeneous mixture of two or more metals, or a metal and a non-metal, is called an __________.

28. The arrangement of metals in decreasing order of reactivity is called the __________ series.

29. The ions formed by metals after losing electrons are called __________.

30. Non-metals generally form __________ ions by gaining electrons.

C. True or False

Write True or False.

31. All metals are solids at room temperature.

32. Graphite is a non-metal that can conduct electricity.

33. Gold is among the least reactive metals in the given activity series.

34. A less reactive metal can normally displace a more reactive metal from its salt solution.

35. Sodium reacts vigorously with cold water.

36. Ionic compounds conduct electricity easily in their solid state.

37. Roasting is associated with the conversion of sulphide ores into oxides.

38. Calcination is commonly used for carbonate ores.

39. Rusting of iron requires moisture as well as air.

40. Galvanisation protects iron by coating it with zinc.

D. Match the Following

41. Match Column A with Column B.

Column A	Column B
A. Malleability	1. Copper + zinc
B. Ductility	2. Thin sheets
C. Brass	3. Thin wires
D. Bronze	4. Copper + tin

42. Match the process with its description.

Column A	Column B
A. Roasting	1. Zinc coating
B. Calcination	2. Electrolytic purification
C. Galvanisation	3. Sulphide ore heated in excess air
D. Electrolytic refining	4. Carbonate ore heated with limited air

43. Match the substance with its characteristic.

Column A	Column B
A. Sodium	1. Liquid metal at room temperature
B. Mercury	2. Conducting non-metal
C. Graphite	3. Highly reactive metal
D. Gold	4. Very unreactive metal

E. Very Short Answer Questions

44. Define malleability.

45. What is ductility?

46. Why are metals generally called sonorous?

47. Name one liquid metal at room temperature.

48. Name one non-metal that conducts electricity.

49. What is an amphoteric oxide?

50. Give two examples of amphoteric oxides.

51. What is a displacement reaction?

52. What is meant by an ore?

53. Define gangue.

54. What is roasting?

55. What is calcination?

56. What is corrosion?

57. What is galvanisation?

58. What is an alloy?

59. What is anode mud?

60. Name the metal present in the coating used during galvanisation.

F. Short Answer Questions

61. Why are metals suitable for making electrical wires?

62. Explain why graphite is considered an exception among non-metals.

63. Why can physical properties alone not be used to classify every element strictly as a metal or non-metal?

64. Why are sodium and potassium kept under oil?

65. Why does aluminium resist further corrosion even though it is a reactive metal?

66. Explain why a more reactive metal can displace a less reactive metal from its salt solution.

67. Why do ionic compounds generally have high melting points?

68. Why do ionic compounds conduct electricity in molten or aqueous form but generally not in solid form?

69. Differentiate between a mineral and an ore.

70. Distinguish between roasting and calcination.

71. Why are highly reactive metals obtained by electrolytic reduction rather than by reduction with carbon?

72. Explain the role of carbon in the extraction of metals of medium reactivity.

73. Why is rusting considered a form of corrosion?

74. Explain how galvanisation helps prevent rusting.

75. Why are alloys prepared instead of using some metals in their pure form?

G. Long Answer Questions

76. Explain the major physical properties of metals and mention suitable examples or exceptions.

77. Describe the reactions of metals with oxygen, water and dilute acids. Give suitable chemical equations.

78. Explain the reactivity series of metals. How can displacement reactions be used to compare the reactivity of two metals?

79. Explain the formation of an ionic compound using sodium chloride as an example. Describe the transfer of electrons involved.

80. Describe the important physical and electrical properties of ionic compounds.

81. Explain how metals of low, medium and high reactivity are extracted from their ores.

82. Describe roasting, calcination and reduction with suitable examples.

83. Explain electrolytic refining of metals. What are the roles of the anode, cathode, electrolyte and anode mud?

84. Explain the conditions necessary for rusting of iron and describe different methods used to prevent corrosion.

85. What are alloys? Explain why alloying is useful and give examples of common alloys discussed in the chapter.

H. Assertion–Reason Questions

For each question, choose the correct option:

(A) Both Assertion and Reason are true, and Reason correctly explains Assertion.
(B) Both are true, but Reason does not correctly explain Assertion.
(C) Assertion is true, but Reason is false.
(D) Assertion is false, but Reason is true.

86. Assertion: Ionic compounds generally have high melting points.
Reason: Strong electrostatic forces hold oppositely charged ions together.

87. Assertion: Sodium is stored under oil.
Reason: Sodium reacts very vigorously with air and water.

88. Assertion: Copper cannot displace zinc from zinc sulphate solution.
Reason: Copper is less reactive than zinc.

89. Assertion: Graphite conducts electricity.
Reason: Graphite is a metal.

90. Assertion: Aluminium articles can resist corrosion.
Reason: Aluminium can develop a protective oxide layer on its surface.

91. Assertion: Highly reactive metals are extracted by electrolysis.
Reason: Their compounds cannot generally be reduced effectively using carbon.

92. Assertion: Iron rusts in dry air.
Reason: Rusting requires moisture along with air.

I. Case-Based Questions

Case Study 1: Reactivity of Metals

A student places different metals into suitable salt solutions. In one experiment, iron is placed in copper sulphate solution and a reaction occurs. In another experiment, copper is placed in iron sulphate solution and no displacement is observed.

93. Which metal is more reactive: iron or copper?

94. Identify the type of reaction taking place when iron is placed in copper sulphate solution.

95. Write the balanced chemical equation for the reaction.

96. What general rule about metal reactivity can be concluded from this experiment?

Case Study 2: Extraction of Metals

An ore contains a metal in the form of a sulphide. Before the metal can be extracted, the sulphide is converted into an oxide by heating in excess air. The oxide is then reduced to obtain the metal.

97. Name the process used to convert the sulphide into an oxide.

98. Why is the sulphide converted into an oxide before reduction?

99. Write the roasting equation for zinc sulphide.

100. Name one reducing agent that can be used to reduce a metal oxide.

Case Study 3: Rusting

Three iron nails are kept under different conditions. One is exposed to both air and water, another is kept in water from which dissolved air has been removed and protected from further contact with air, and the third is kept in dry air.

101. In which condition is rusting expected?

102. What does this experiment demonstrate about the requirements for rusting?

103. Why does the nail in dry air not rust under these conditions?

104. Name any two methods used to prevent rusting.

J. Higher-Order Thinking Questions

105. A student says, “Every substance that is shiny must be a metal.” Use an exception from the chapter to evaluate this statement.

106. Metal X displaces metal Y from its salt solution, while metal Y cannot displace metal X. What can you conclude about their relative reactivity?

107. A metal reacts vigorously with cold water and produces a hydroxide and hydrogen. Where would you expect this metal to lie in the reactivity series?

108. A substance is hard and brittle, has a high melting point, and conducts electricity when molten but not in its solid state. What type of compound is it likely to be? Explain.

109. Why would carbon be unsuitable for extracting sodium from sodium oxide by ordinary reduction?

110. An iron object is coated with zinc. Explain why this treatment can protect iron from corrosion.

111. A student heats a carbonate ore and observes the formation of a metal oxide and carbon dioxide. Identify the process and explain why it is useful in metallurgy.

112. Copper and silver are both relatively low in the activity series. What does their position suggest about how they may occur in nature?

Answer Key

MCQs

(b)
(b)
(c)
(c)
(b)
(b)
(c)
(b)
(b)
(a)
(b)
(c)
(a)
(b)
(b)

Fill in the Blanks

Ductility
Lustre
Amphoteric
Ores
Gangue
Roasting
Calcination
Corrosion
Galvanisation
Anode
Anode mud
Alloy
Reactivity / activity
Cations
Negative

True/False

False
True
True
False
True
False
True
True
True
True

Match the Following

A–2, B–3, C–1, D–4
A–3, B–4, C–1, D–2
A–3, B–1, C–2, D–4

Very Short Answers

Ability to be beaten into thin sheets.
Ability to be drawn into thin wires.
They generally produce a ringing sound when struck.
Mercury.
Graphite.
An oxide that reacts with both acids and bases.
Al₂O₃ and ZnO.
A reaction in which a more reactive metal displaces a less reactive metal from its compound.
A mineral from which a metal can be extracted profitably.
Unwanted impurities associated with an ore.
Strong heating of a sulphide ore in excess air.
Strong heating of a carbonate ore with limited air.
Gradual deterioration of a metal due to environmental reactions.
Protection of iron or steel by a zinc coating.
A homogeneous mixture of two or more metals, or a metal and a non-metal.
Insoluble impurities deposited below the anode during electrolytic refining.
Zinc.

Assertion–Reason

Case-Based Answers

Iron.
Displacement reaction.
Fe + CuSO₄ → FeSO₄ + Cu
A more reactive metal can displace a less reactive metal from its salt solution.
Roasting.
Metal oxides are generally easier to reduce to the metal than the corresponding sulphides.
2ZnS + 3O₂ → 2ZnO + 2SO₂
Carbon.
The nail exposed to both air and water.
Both air and moisture are required for rusting under these conditions.
It lacks the moisture needed for rusting.
Painting, oiling, greasing, galvanisation, chrome plating, anodising or alloying.