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Class 10 Science Chapter 3: Metals and Non-metals — Important Questions & Sample Paper

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Reviewed by qpaper's CBSE curriculum team · Edited by Mohit · Updated June 2026

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Yes — this page has 44+ original Class 10 Science Chapter 3 (“Metals and Non-metals”) important questions with answers (Multiple Choice (MCQ), Assertion–Reason, Short Answer, Short Answer, Long Answer, Case Study). Practise them free, or generate a full CBSE board-pattern sample paper (80 marks) and export it to PDF or Word — in English & Hindi, for 2026-27.

Chapter 3 'Metals and Non-metals' in Class 10 Science explores the fundamental differences between metals and non-metals based on their physical and chemical properties. It covers the reactivity series, explaining how metals react with water, acids, and other substances to produce characteristic products like hydrogen gas. The chapter dives into the formation of ionic compounds through electron transfer, emphasizing the properties of such compounds, including their electrical conductivity in molten or dissolved states. A significant portion is dedicated to the occurrence of metals in nature as minerals and ores, along with the metallurgical processes used for extraction, such as roasting, calcination, and reduction using carbon or more reactive metals. Students also learn about the corrosion of metals, its detrimental effects, and methods to prevent it through alloying, painting, or galvanization. Exam questions often require students to identify unknown metals or non-metals based on observed reactions, write balanced chemical equations, draw and interpret the bonding in ionic compounds compared to exceptional cases like graphite, and explain stepwise extraction from specific ores. This chapter builds a strong foundation in inorganic chemistry and materials science.

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Science — Metals and Non-metals

Class 10Time: 3 hrsMax Marks: 80

SECTION A

  1. 1.

    Element X forms a basic oxide XO that dissolves in water to give a solution turning red litmus blue. Element Y forms an acidic oxide YO₂ that turns blue litmus red when dissolved. Heating XO with YO₂ produces a white salt. X and Y are respectively:

    (a) Calcium and sulphur(b) Magnesium and carbon(c) Sodium and nitrogen(d) Potassium and phosphorus
    1
  2. 2.

    Metal oxides generally react with water to form solutions that are:

    (a) Acidic(b) Neutral(c) Basic(d) Amphoteric
    1
  3. 3.

    An element X forms an oxide that, when dissolved in water, turns blue litmus red. Element X is most likely:

    (a) A metal(b) A non-metal(c) An alkali metal(d) An alloy
    1

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Marks distribution & blueprint

In a CBSE exam, this chapter typically contributes questions across the following types. The last column shows how many original questions of each type we have ready in our bank for this chapter:

Question typeMarks eachIn our bank
Multiple Choice (MCQ)1 mark13
Assertion–Reason1 mark6
Short Answer2 marks8
Short Answer3 marks6
Long Answer5 marks5
Case Study4 marks6

44 original, exam-style questions in our bank for this chapter — with answers.

Important & sample questions (with answers)

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  1. Q1. Element X forms a basic oxide XO that dissolves in water to give a solution turning red litmus blue. Element Y forms an acidic oxide YO₂ that turns blue litmus red when dissolved. Heating XO with YO₂ produces a white salt. X and Y are respectively:

    1 mark
    Multiple Choice (MCQ)
    (A) Calcium and sulphur(B) Magnesium and carbon(C) Sodium and nitrogen(D) Potassium and phosphorus
    ▸ Answer

    Calcium and sulphur

  2. Q2. Metal oxides generally react with water to form solutions that are:

    1 mark
    Multiple Choice (MCQ)
    (A) Acidic(B) Neutral(C) Basic(D) Amphoteric
    ▸ Answer

    Basic

  3. Q3. An element X forms an oxide that, when dissolved in water, turns blue litmus red. Element X is most likely:

    1 mark
    Multiple Choice (MCQ)
    (A) A metal(B) A non-metal(C) An alkali metal(D) An alloy
    ▸ Answer

    A non-metal

  4. Q4. Which metal reacts with steam to produce hydrogen but does not react appreciably with cold water?

    1 mark
    Multiple Choice (MCQ)
    (A) Potassium(B) Magnesium(C) Calcium(D) Sodium
    ▸ Answer

    Magnesium

  5. Q5. Assertion (A): Mercury can be obtained from its ore cinnabar by simply heating it in air. Reason (R): Mercury has a very low boiling point and escapes as vapour.

    1 mark
    Assertion–Reason
    (A) Both A and R are true and R is the correct explanation of A.(B) Both A and R are true but R is not the correct explanation of A.(C) A is true but R is false.(D) A is false but R is true.
    ▸ Answer

    A is true but R is false.

  6. Q6. Explain why aluminium metal is used for making cooking utensils even though it is reactive with acids and alkalis.

    2 marks
    Short Answer
    ▸ Answer

    Aluminium forms a tough, impervious layer of aluminium oxide (Al₂O₃) on its surface when exposed to air. This protective layer prevents further reaction, making it safe for cooking.

  7. Q7. During the extraction of moderately reactive metals, carbonate ores are first calcined while sulphide ores are first roasted. Why is this done? Write the chemical equation for the roasting of zinc blende (ZnS).

    2 marks
    Short Answer
    ▸ Answer

    Calcination converts carbonates to oxides by heating in limited air, while roasting converts sulphides to oxides by heating in excess air. Oxides are easier to reduce to the metal. Equation: 2ZnS + 3O₂ → 2ZnO + 2SO₂.

  8. Q8. A metal ‘R’ is obtained from its carbonate ore, calamine, by heating the ore in limited air and then reducing the product with coke. The heating step produces a solid ‘S’ and a gas ‘T’. Identify R, S, and T. Write the balanced equations for the two steps. Why is metal R extensively used to coat iron articles? Name the coating process.

    3 marks
    Short Answer
    ▸ Answer

    R = Zinc, S = Zinc oxide (ZnO), T = Carbon dioxide (CO2). Step 1 (calcination): ZnCO3 (s) → ZnO (s) + CO2 (g). Step 2 (reduction): ZnO + C → Zn + CO (or 2ZnO + C → 2Zn + CO2; either accepted). Zinc coating is used because zinc forms a protective layer of basic zinc carbonate that prevents air and moisture from reaching the iron surface. The process is called galvanisation.

  9. Q9. A metal ‘M’ reacts with dilute hydrochloric acid to liberate a gas ‘P’ that burns with a pop sound. When the same metal is treated with concentrated nitric acid, a brown gas ‘Q’ is evolved. Identify M, P, and Q. Write balanced chemical equations for both reactions and explain why different gases are produced.

    3 marks
    Short Answer
    ▸ Answer

    M = Zinc (Zn), P = Hydrogen (H2), Q = Nitrogen dioxide (NO2). Equations: Zn + 2HCl → ZnCl2 + H2 ↑; Zn + 4HNO3 (conc.) → Zn(NO3)2 + 2NO2 ↑ + 2H2O. Reason: Dilute HCl provides H+ ions that are reduced by Zn to H2. Concentrated HNO3 is a strong oxidising agent; it oxidises Zn and itself gets reduced to NO2 (brown fumes).

  10. Q10. You are provided with solutions of copper(II) sulfate, zinc sulfate, and iron(II) sulfate, along with pieces of zinc, iron, and copper metals. Describe a systematic experimental procedure to determine the relative reactivity order of these three metals. State the observations you would make and write the balanced chemical equations for any reactions that occur. Conclude the reactivity series.

    5 marks
    Long Answer
    ▸ Answer

    Procedure: 1. Place a piece of zinc in copper sulfate solution: blue color fades, reddish-brown copper deposits ⟹ Zn displaces Cu. Zn + CuSO4 → ZnSO4 + Cu. 2. Place a piece of iron in copper sulfate solution: similar displacement, Fe + CuSO4 → FeSO4 + Cu. 3. Place a piece of zinc in iron sulfate solution: greenish solution turns colorless, iron deposits ⟹ Zn + FeSO4 → ZnSO4 + Fe. 4. Place a piece of iron in zinc sulfate: no reaction. 5. Place copper in zinc sulfate or iron sulfate: no reaction. Order: Zn > Fe > Cu (most reactive to least).

  11. Q11. List three physical properties that distinguish metals from non-metals. Using the electron sea model, explain why metals are generally excellent conductors of electricity while non-metals are not. Provide one example of a metal and one of a non-metal to illustrate your explanation.

    5 marks
    Long Answer
    ▸ Answer

    Metals are lustrous, malleable, and ductile; non-metals are dull, brittle if solid, and non-ductile. Metals conduct electricity due to mobile delocalized electrons (electron sea), which move freely when a potential is applied. Non-metals lack free electrons, so they are insulators. Example: Copper (metal) has one free electron per atom in its lattice; sulfur (non-metal) forms covalent molecules with no mobile charges.

  12. Q12. In a school laboratory, two students took two unknown metals X and Y in separate test tubes and added dilute hydrochloric acid to them. Metal X reacted vigorously, producing a colorless gas that burnt with a pop sound when a burning splinter was brought near it. Metal Y showed no reaction with the acid at all.

    4 marks
    Case Study
    1. (i) Name the gas evolved when metal X reacts with HCl. Why does this gas burn with a pop sound?1 mark
    2. (ii) Why did metal Y not react with HCl? Suggest a possible metal for Y.1 mark
    3. (iii) Predict two possible metals for X. Explain why they react in this way.2 marks
    ▸ Answer

    Gas is hydrogen; pops due to combustion. Y is less reactive (e.g., Cu). X could be Mg or Zn – they are above hydrogen and displace it.

Frequently asked questions

Why does sodium chloride conduct electricity only when molten or dissolved, while graphite conducts in solid state?

In solid NaCl, ions are locked in a lattice and cannot move, preventing conduction. Upon melting or dissolving, ions become mobile, allowing current flow. Graphite, a carbon allotrope, has a layered structure where each carbon atom bonds to three others, leaving one delocalized electron per atom. These free electrons move within layers, enabling solid-state conductivity.

How do we extract a metal from its carbonate ore, like calamine?

The carbonate ore is first calcined (heated in limited air) to convert it into the metal oxide, releasing CO₂. The oxide is then reduced by heating with a reducing agent like coke (carbon), which removes oxygen, yielding the pure metal. For example, zinc from calamine (ZnCO₃) is obtained via ZnO formation and reduction with carbon.

What causes the green coating on copper vessels, and how can it be prevented?

Copper reacts with moist air containing CO₂, O₂, and water to form a greenish layer of basic copper carbonate (CuCO₃·Cu(OH)₂). This is corrosion. Prevention methods include applying a protective coating like paint or oil, using corrosion-resistant alloys like brass, or employing sacrificial protection like galvanization.

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