CBSE Class 10 Chemistry Metals and Non-metals MCQs Set 43

Chemistry Objective Questions and Answers: Metals and Non-metals

Review structured MCQ sets for Class 10 Chemistry Metals and Non-metals. Built according to official CBSE guidelines, these downloadable questions support daily revision and core concept reinforcement.

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Multiple Choice Questions

Question 1: If an isotope of hydrogen has two neutrons in its atom, its atomic number and mass number are respectively
(a) 2 and 1
(b) 3 and 1
(c) 1 and 1
(d) 1 and 3
Show Answer & Explanation

Answer: (d) 1 and 3

Explanation:
1. Hydrogen has atomic number 1 (one proton).
2. Mass number = protons + neutrons = 1 + 2 = 3, so the values are 1 and 3 (tritium).

Teacher's Note:
1. The atomic number never changes for an element.
2. Isotopes differ in the number of neutrons.

Question 2: A mineral is known as an ore if
(a) the metal cannot be produced from it
(b) the metal can be produced from it
(c) the metal can be extracted from it profitably
(d) it is very costly
Show Answer & Explanation

Answer: (c) the metal can be extracted from it profitably

Explanation:
1. An ore is a mineral from which the metal can be extracted conveniently and profitably.
2. All ores are minerals but not all minerals are ores.

Teacher's Note:
1. Example: bauxite is an ore of aluminium but clay is only a mineral.
2. Economics decides what is an ore.

Question 3: The earthy impurities associated with the mineral used in metallurgy are called
(a) slag
(b) flux
(c) gangue
(d) ore
Show Answer & Explanation

Answer: (c) gangue

Explanation:
1. Gangue is the unwanted earthy material (sand, rock, soil) present in the ore.
2. A flux combines with it to form slag.

Teacher's Note:
1. Flux + gangue gives slag.
2. Ore + gangue is the raw material.

Question 4: Match the metal with its ore: (A) Zn, (B) Hg, (C) Cu, (D) Mg with (P) cuprite, (Q) carnallite, (R) calamine, (S) cinnabar.
(a) A-R, B-S, C-P, D-Q
(b) A-P, B-Q, C-R, D-S
(c) A-S, B-R, C-Q, D-P
(d) A-Q, B-P, C-S, D-R
Show Answer & Explanation

Answer: (a) A-R, B-S, C-P, D-Q

Explanation:
1. Calamine is ZnCO3, cinnabar is HgS, cuprite is Cu2O and carnallite is KCl·MgCl2·6H2O.
2. So the pairs are Zn-calamine, Hg-cinnabar, Cu-cuprite and Mg-carnallite.

Teacher's Note:
1. Learn ores: haematite Fe2O3, bauxite Al2O3·2H2O, galena PbS, zinc blende ZnS.
2. Carnallite is also a source of potassium.

Question 5: Sulphur readily dissolves in
(a) water
(b) sodium hydroxide
(c) hydrochloric acid
(d) carbon disulphide
Show Answer & Explanation

Answer: (d) carbon disulphide

Explanation:
1. Sulphur is a non-polar molecular solid and dissolves in the non-polar solvent carbon disulphide.
2. It is insoluble in water.

Teacher's Note:
1. Like dissolves like.
2. Rhombic sulphur is the most stable form at room temperature.

Question 6: Which process is used in the extractive metallurgy of magnesium?
(a) fused salt electrolysis
(b) self reduction
(c) aqueous solution electrolysis
(d) thermite reduction
Show Answer & Explanation

Answer: (a) fused salt electrolysis

Explanation:
1. Magnesium is highly reactive and is obtained by electrolysis of fused (molten) magnesium chloride.
2. Aqueous solution electrolysis would give hydrogen instead.

Teacher's Note:
1. The reactive metals Na, K, Ca, Mg and Al are extracted by electrolysis of molten compounds.
2. Carbon cannot reduce their oxides.

Question 7: The methods of extraction of a metal from its oxide ore include
(a) reduction with carbon, reduction with hydrogen, reduction with aluminium and electrolytic reduction (all four)
(b) reduction with carbon only
(c) electrolytic reduction only
(d) reduction with hydrogen only
Show Answer & Explanation

Answer: (a) reduction with carbon, reduction with hydrogen, reduction with aluminium and electrolytic reduction (all four)

Explanation:
1. Oxide ores can be reduced by carbon (zinc, iron, lead), by hydrogen (some less reactive oxides such as CuO), by aluminium (Cr2O3, MnO2) and electrolytically (Al2O3).
2. So all four methods are used.

Teacher's Note:
1. Choice of the method depends on the reactivity of the metal.
2. More reactive metals need stronger methods.

Question 8: Which metal is extracted by electrolytic reduction of its molten compound?
(a) sodium
(b) silver
(c) lead
(d) copper
Show Answer & Explanation

Answer: (a) sodium

Explanation:
1. Sodium is very reactive and is obtained by electrolysis of molten NaCl (Down's process).
2. Silver, lead and copper are obtained by less powerful methods.

Teacher's Note:
1. Cathode: Na+ + e– → Na.
2. Anode: chlorine is liberated.

Question 9: Which metal occurs in nature both in the free state and in the combined state?
(a) aluminium
(b) magnesium
(c) copper
(d) sodium
Show Answer & Explanation

Answer: (c) copper

Explanation:
1. Copper (and silver) occur native as well as in compounds such as copper pyrites and cuprite.
2. Sodium, aluminium and magnesium are found only combined.

Teacher's Note:
1. Medium-reactivity metals occur in both forms.
2. Gold and platinum are mainly free.

Question 10: An element A has the electronic configuration 2, 8, 6. Which statement is correct?
(a) It will lose six electrons
(b) It will lose two electrons
(c) It is a noble gas
(d) It will gain two electrons to form A2–
Show Answer & Explanation

Answer: (d) It will gain two electrons to form A2–

Explanation:
1. Gaining 2 electrons gives a stable octet (2, 8, 8), which is easier than losing 6 electrons.
2. So A gains 2 electrons and is a non-metal (sulphur).

Teacher's Note:
1. Atoms with 5 to 7 valence electrons gain electrons.
2. The ion formed is S2–.

Question 11: An alloy of copper used for making utensils is
(a) stainless steel
(b) brass
(c) solder
(d) duralumin
Show Answer & Explanation

Answer: (b) brass

Explanation:
1. Brass (Cu + Zn) is used for making utensils.
2. Solder is Pb + Sn, duralumin is aluminium based and stainless steel is iron based.

Teacher's Note:
1. Bronze (Cu + Sn) is used for statues and medals.
2. Alloys are harder than pure metals.

Question 12: In the reaction Fe(s) + Cu2+(aq) → Fe2+(aq) + Cu(s), which statement is correct?
(a) Iron is less reactive and copper is oxidised
(b) Iron is more reactive and iron is oxidised
(c) Copper is more reactive and copper is oxidised
(d) Copper is more reactive and iron is oxidised
Show Answer & Explanation

Answer: (b) Iron is more reactive and iron is oxidised

Explanation:
1. Iron displaces copper, so iron is more reactive than copper.
2. Iron loses electrons (0 to +2), which is oxidation.

Teacher's Note:
1. Fe is the reducing agent and Cu2+ the oxidising agent.
2. Brown copper settles on the iron.

Question 13: An element X forms an oxide XO which conducts electricity. How many electrons are in the valence shell of X and what is the formula of its chloride?
(a) 2 electrons; XCl
(b) 2 electrons; XCl2
(c) 1 electron; XCl
(d) 6 electrons; XCl2
Show Answer & Explanation

Answer: (b) 2 electrons; XCl2

Explanation:
1. In XO the element shows a valency of 2 as oxygen has valency 2.
2. X is a metal that loses 2 electrons, so it has 2 valence electrons and forms XCl2 with chlorine.

Teacher's Note:
1. Ionic oxides conduct in the molten state.
2. Valency 2 combines with Cl(1) in the ratio 1 : 2.

Question 14: Calcination differs from roasting in that
(a) calcination is heating in little or no air (carbonate ores), roasting is heating in excess of air (sulphide ores)
(b) calcination is done in excess of air
(c) roasting is done in no air
(d) both are the same
Show Answer & Explanation

Answer: (a) calcination is heating in little or no air (carbonate ores), roasting is heating in excess of air (sulphide ores)

Explanation:
1. Calcination is strong heating of a carbonate or hydrated ore in the absence or a limited supply of air to give an oxide with loss of CO2 or water.
2. Roasting is heating a sulphide ore in excess air to give oxide and SO2.

Teacher's Note:
1. Calcination: ZnCO3 → ZnO + CO2.
2. Roasting: 2ZnS + 3O2 → 2ZnO + 2SO2.

Question 15: Which one of the following is the main difference between electrolytic reduction and reduction with carbon?
(a) there is no difference
(b) electrolytic reduction is used for gold only
(c) electrolytic reduction is used for very reactive metals such as sodium and aluminium, carbon reduction for metals such as zinc and iron
(d) carbon is used for sodium
Show Answer & Explanation

Answer: (c) electrolytic reduction is used for very reactive metals such as sodium and aluminium, carbon reduction for metals such as zinc and iron

Explanation:
1. Highly reactive metals hold on to oxygen strongly and need the strong reducing action of electrolysis (for example molten NaCl or Al2O3).
2. Less reactive metals such as Zn, Fe and Pb can be reduced by carbon.

Teacher's Note:
1. Electrolysis uses electrical energy.
2. Carbon reduction uses heat.

Question 16: For making gold ornaments, 22 carat gold is preferred over 24 carat gold because
(a) 22 carat gold is heavier
(b) 24 carat gold is blue
(c) 24 carat gold is magnetic
(d) pure 24 carat gold is too soft, while 22 carat is alloyed with copper or silver and is harder
Show Answer & Explanation

Answer: (d) pure 24 carat gold is too soft, while 22 carat is alloyed with copper or silver and is harder

Explanation:
1. Pure gold is soft and would bend or wear out.
2. Alloying with about 8% copper or silver makes it harder and suitable for ornaments.

Teacher's Note:
1. Carat measures purity.
2. 24 carat means 100% gold.

Question 17: What is observed when zinc is added to a solution of iron(II) sulphate?
(a) the solution turns blue
(b) the green colour of the solution fades and iron is deposited: Zn + FeSO4 → ZnSO4 + Fe
(c) hydrogen gas is evolved
(d) nothing happens
Show Answer & Explanation

Answer: (b) the green colour of the solution fades and iron is deposited: Zn + FeSO4 → ZnSO4 + Fe

Explanation:
1. Zinc is more reactive than iron and displaces it.
2. The pale green FeSO4 solution becomes colourless ZnSO4 and iron is deposited.

Teacher's Note:
1. Reactivity: Zn > Fe.
2. No gas is evolved.

Question 18: Why is ZnO called an amphoteric oxide?
(a) it is a gas
(b) it dissolves in water to give a base
(c) it is neutral
(d) it reacts with both acids and bases to form salts and water
Show Answer & Explanation

Answer: (d) it reacts with both acids and bases to form salts and water

Explanation:
1. ZnO + 2HCl → ZnCl2 + H2O (as a base) and ZnO + 2NaOH → Na2ZnO2 + H2O (as an acid).
2. Showing both behaviours makes it amphoteric; Al2O3 is another example.

Teacher's Note:
1. Amphoteric oxides: ZnO, Al2O3, PbO, SnO.
2. Ordinary metal oxides are basic.

Question 19: Which of the following is correct about mineral, ore and gangue?
(a) a mineral occurs naturally in the earth; an ore is a mineral from which the metal can be profitably extracted; gangue is the earthy impurity in the ore
(b) all three mean the same
(c) ore is an impurity and gangue is a metal
(d) mineral is man-made
Show Answer & Explanation

Answer: (a) a mineral occurs naturally in the earth; an ore is a mineral from which the metal can be profitably extracted; gangue is the earthy impurity in the ore

Explanation:
1. Minerals are naturally occurring compounds of metals in the earth's crust.
2. An ore is a mineral that can be used to extract the metal profitably, and gangue is the unwanted material in it.

Teacher's Note:
1. All ores are minerals, but not all minerals are ores.
2. Gangue is removed by concentration.

Question 20: Metal oxides generally differ from non-metal oxides because
(a) metal oxides are basic and non-metal oxides are acidic
(b) metal oxides are acidic
(c) both are neutral
(d) both are gases
Show Answer & Explanation

Answer: (a) metal oxides are basic and non-metal oxides are acidic

Explanation:
1. Metal oxides react with acids to form salt and water, so they are basic.
2. Non-metal oxides react with bases, so they are acidic.

Teacher's Note:
1. Exceptions: Al2O3 and ZnO are amphoteric.
2. CO and H2O are neutral.

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