NCERT Solutions for Class 10 Science Chapter 3: Metals and Non-metals (NCERT 2026–27)

These Class 10 Science Chapter 3 solutions cover Metals and Non-metals with every in-text question and every end-of-chapter exercise answered step by step. You will learn the physical and chemical properties of metals and non-metals, the reactivity series, how ionic compounds form, the extraction and refining of metals (metallurgy), corrosion and its prevention — all updated for session 2026–27 and written in exam-ready CBSE style.

Class: 10 Subject: Science Chapter: 3 Title: Metals and Non-metals Branch: Chemistry Session: 2026–27
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Class 10 Science Chapter 3 Solutions – Overview

Chapter 3, Metals and Non-metals, builds on the elements you studied in Class IX. It first compares the physical properties of metals (lustre, malleability, ductility, sonority, high melting points, good conductors of heat and electricity) with those of non-metals, and notes the exceptions (mercury is a liquid metal; gallium and caesium melt in the hand; iodine is a lustrous non-metal; graphite conducts electricity). It then explores the chemical properties of metals — reaction with oxygen, water, acids and salt solutions — leading to the reactivity (activity) series. The chapter explains how metals and non-metals combine by the transfer of electrons to form ionic (electrovalent) compounds, their properties, and finally the extraction of metals from ores (roasting, calcination, reduction, electrolytic reduction and refining) and corrosion with its prevention by galvanisation, alloying and other methods.

Key Concepts & Definitions

Metallic lustre: the shining surface of pure metals.

Malleability: the property of metals to be beaten into thin sheets (gold and silver are most malleable).

Ductility: the ability of metals to be drawn into thin wires (gold is the most ductile).

Sonority: metals produce a ringing sound on striking a hard surface.

Amphoteric oxides: metal oxides such as Al2O3 and ZnO that react with both acids and bases to give salt and water.

Ionic (electrovalent) compounds: compounds formed by the transfer of electrons from a metal to a non-metal, e.g. NaCl, MgCl2; they are hard, brittle, high melting solids, soluble in water, and conduct electricity in molten or aqueous state.

Minerals & ores: elements/compounds occurring naturally in the earth’s crust are minerals; minerals from which a metal can be profitably extracted are ores.

Roasting: heating a sulphide ore strongly in excess air to convert it to oxide. Calcination: heating a carbonate ore strongly in limited air to convert it to oxide.

Corrosion: the slow eating up of a metal surface by the action of moist air, acids, etc. (e.g. rusting of iron, tarnishing of silver, green coat on copper).

Alloy: a homogeneous mixture of two or more metals, or a metal and a non-metal (an alloy with mercury is an amalgam).

Important Reactions & Reactivity Series

Metal + Oxygen: 2Cu + O2 → 2CuO;   4Al + 3O2 → 2Al2O3

Amphoteric oxide: Al2O3 + 6HCl → 2AlCl3 + 3H2O;   Al2O3 + 2NaOH → 2NaAlO2 + H2O

Metal + Water: 2Na + 2H2O → 2NaOH + H2 + heat;   3Fe + 4H2O(g) → Fe3O4 + 4H2

Metal + Dilute acid: Metal + Dilute acid → Salt + Hydrogen

Displacement: Fe + CuSO4 → FeSO4 + Cu (a more reactive metal displaces a less reactive one)

Thermit reaction: Fe2O3 + 2Al → 2Fe + Al2O3 + Heat

Activity series (most → least reactive): K > Na > Ca > Mg > Al > Zn > Fe > Pb > (H) > Cu > Hg > Ag > Au

In-text Questions — Answers

Page 40

1. Give an example of a metal which (i) is a liquid at room temperature. (ii) can be easily cut with a knife. (iii) is the best conductor of heat. (iv) is a poor conductor of heat.

ANSWER (i) Mercury (Hg) is a liquid at room temperature. (ii) Sodium (Na) (also potassium/lithium) can be easily cut with a knife. (iii) Silver (Ag) is the best conductor of heat (copper is the next best). (iv) Lead (Pb) and mercury (Hg) are poor conductors of heat.

2. Explain the meanings of malleable and ductile.

ANSWER Malleable: the property of a metal by which it can be beaten (hammered) into thin sheets without breaking. Gold and silver are the most malleable metals; aluminium foil used for wrapping food is another example. Ductile: the property of a metal by which it can be drawn into thin wires. Gold is the most ductile metal — a wire about 2 km long can be drawn from just 1 g of gold.

Page 46

1. Why is sodium kept immersed in kerosene oil?

ANSWER Sodium is a very reactive metal. It reacts vigorously with the oxygen and moisture (water vapour) of air at room temperature, and the reaction is so exothermic that it can catch fire. To prevent this accidental reaction and fire, sodium is stored immersed in kerosene oil, which keeps it away from air and moisture.

2. Write equations for the reactions of (i) iron with steam (ii) calcium and potassium with water

ANSWER (i) 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g) (ii) Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g) 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g) + heat energy

3. Samples of four metals A, B, C and D were taken and added to the following solution one by one. The results obtained have been tabulated as follows.

MetalIron(II) sulphateCopper(II) sulphateZinc sulphateSilver nitrate
ANo reactionDisplacement——
BDisplacement—No reaction—
CNo reactionNo reactionNo reactionDisplacement
DNo reactionNo reactionNo reactionNo reaction

Use the Table above to answer the following questions about metals A, B, C and D. (i) Which is the most reactive metal? (ii) What would you observe if B is added to a solution of Copper(II) sulphate? (iii) Arrange the metals A, B, C and D in the order of decreasing reactivity.

ANSWER (i) B is the most reactive metal. It displaces iron from iron(II) sulphate, so it lies above iron; A only displaces copper (it is below iron but above copper), while C only displaces silver and D displaces nothing. (ii) Since B is more reactive than iron (and hence than copper), B will displace copper from copper(II) sulphate. A reaction takes place: a reddish-brown copper deposit forms and the blue colour of the solution fades. B + CuSO4 → BSO4 + Cu. (iii) Decreasing order of reactivity: B > A > C > D.

4. Which gas is produced when dilute hydrochloric acid is added to a reactive metal? Write the chemical reaction when iron reacts with dilute H2SO4.

ANSWER Hydrogen gas (H2) is produced when dilute hydrochloric acid is added to a reactive metal. Reaction of iron with dilute sulphuric acid: Fe(s) + H2SO4(aq) → FeSO4(aq) + H2(g)

5. What would you observe when zinc is added to a solution of iron(II) sulphate? Write the chemical reaction that takes place.

ANSWER Zinc is more reactive than iron, so zinc displaces iron from iron(II) sulphate. The light green colour of the iron(II) sulphate solution slowly fades (becomes colourless) and a greyish deposit of iron is formed. Zn(s) + FeSO4(aq) → ZnSO4(aq) + Fe(s)

Page 49

1. (i) Write the electron-dot structures for sodium, oxygen and magnesium. (ii) Show the formation of Na2O and MgO by the transfer of electrons. (iii) What are the ions present in these compounds?

ANSWER (i) Electron-dot structures (valence electrons shown as dots): Sodium (Na, 2,8,1) has 1 valence electron → Na· ; Magnesium (Mg, 2,8,2) has 2 valence electrons → ·Mg· ; Oxygen (O, 2,6) has 6 valence electrons shown as six dots around O (two lone pairs and two single electrons). (ii) Formation of Na2O: Each sodium atom loses 1 electron to form Na+; oxygen gains 2 electrons to form O2–. Two Na atoms transfer 2 electrons in total to one O atom: 2Na → 2Na+ + 2e–; O + 2e– → O2–; giving (Na+)2O2–, i.e. Na2O. Formation of MgO: Magnesium loses 2 electrons to form Mg2+ and oxygen gains those 2 electrons to form O2–: Mg → Mg2+ + 2e–; O + 2e– → O2–; giving Mg2+O2–, i.e. MgO. (iii) In Na2O the ions are Na+ and O2–; in MgO the ions are Mg2+ and O2–.

2. Why do ionic compounds have high melting points?

ANSWER Ionic compounds are made of oppositely charged ions held together by strong electrostatic (inter-ionic) forces of attraction. A large amount of heat energy is needed to overcome these strong forces and separate the ions. Therefore ionic compounds have high melting (and boiling) points.

Page 53

1. Define the following terms. (i) Mineral   (ii) Ore   (iii) Gangue

ANSWER (i) Mineral: the elements or compounds that occur naturally in the earth’s crust are called minerals. (ii) Ore: a mineral that contains a very high percentage of a particular metal so that the metal can be profitably (economically) extracted from it is called an ore. (iii) Gangue: the impurities such as soil, sand, etc. present along with the ore that must be removed before extraction are called gangue.

2. Name two metals which are found in nature in the free state.

ANSWER Gold and silver are found in nature in the free (native) state. (Platinum and copper are also found in the free state.)

3. What chemical process is used for obtaining a metal from its oxide?

ANSWER A metal is obtained from its oxide by reduction. Oxides of less reactive metals are reduced by heating alone; oxides of moderately reactive metals are reduced with a suitable reducing agent such as carbon (coke) or a more reactive metal; oxides of highly reactive metals are reduced by electrolytic reduction (electrolysis of molten compound).

Page 55

1. Metallic oxides of zinc, magnesium and copper were heated with the following metals. In which cases will you find displacement reactions taking place?

Metal →
Oxide ↓		ZincMagnesiumCopper
Zinc oxide—DisplacementNo reaction
Magnesium oxideNo reaction—No reaction
Copper oxideDisplacementDisplacement—
ANSWER A more reactive metal displaces a less reactive metal from its oxide. The order of reactivity is Mg > Zn > Cu. Displacement occurs when: magnesium is heated with zinc oxide (Mg + ZnO → MgO + Zn), magnesium is heated with copper oxide (Mg + CuO → MgO + Cu), and zinc is heated with copper oxide (Zn + CuO → ZnO + Cu). The completed table is shown above.

2. Which metals do not corrode easily?

ANSWER The least reactive metals do not corrode easily — gold, silver and platinum (the noble metals). Copper and aluminium also resist corrosion because a protective oxide layer forms on their surface.

3. What are alloys?

ANSWER An alloy is a homogeneous mixture of two or more metals, or of a metal and a non-metal. It is made by melting the main metal and dissolving the other elements in it in fixed proportions, then cooling. For example, brass (Cu + Zn), bronze (Cu + Sn) and steel (Fe + C). An alloy in which one metal is mercury is called an amalgam.

End-of-chapter Exercises — Solutions

1. Which of the following pairs will give displacement reactions? (a) NaCl solution and copper metal (b) MgCl2 solution and aluminium metal (c) FeSO4 solution and silver metal (d) AgNO3 solution and copper metal.

ANSWER (d) AgNO3 solution and copper metal. Copper is more reactive than silver, so it displaces silver: Cu + 2AgNO3 → Cu(NO3)2 + 2Ag. In (a) copper is below sodium, in (b) aluminium is below magnesium, and in (c) silver is below iron, so no displacement occurs.

2. Which of the following methods is suitable for preventing an iron frying pan from rusting? (a) Applying grease (b) Applying paint (c) Applying a coating of zinc (d) All of the above.

ANSWER (c) Applying a coating of zinc. A frying pan is used for cooking and is heated, so grease or paint would burn off and contaminate the food. Coating with zinc (galvanisation) gives lasting protection even at high temperature and protects the iron even if the coating is scratched.

3. An element reacts with oxygen to give a compound with a high melting point. This compound is also soluble in water. The element is likely to be (a) calcium   (b) carbon   (c) silicon   (d) iron.

ANSWER (a) calcium. Calcium is a metal; its oxide (CaO) is ionic, so it has a high melting point and is basic and soluble in water (forming calcium hydroxide). Carbon and silicon give oxides/acidic substances, and iron oxide is not soluble in water.

4. Food cans are coated with tin and not with zinc because (a) zinc is costlier than tin. (b) zinc has a higher melting point than tin. (c) zinc is more reactive than tin. (d) zinc is less reactive than tin.

ANSWER (c) zinc is more reactive than tin. Being more reactive, zinc would react with the slightly acidic food and form poisonous compounds. Tin is less reactive, so it does not react with food and is safe for coating food cans.

5. You are given a hammer, a battery, a bulb, wires and a switch. (a) How could you use them to distinguish between samples of metals and non-metals? (b) Assess the usefulness of these tests in distinguishing between metals and non-metals.

ANSWER (a) Hammer test (malleability): beat the sample with the hammer. Metals are malleable and flatten into a sheet, while non-metals are brittle and break into pieces. Electrical test: make a circuit with the battery, bulb, wires and switch, and place the sample between two ends of the wire. If the bulb glows, the sample conducts electricity and is a metal; if it does not glow, the sample is a non-metal. (b) These tests are useful in general because most metals are malleable and conduct electricity, while most non-metals are brittle and non-conductors. However, the tests are not foolproof: graphite (a non-metal) conducts electricity and would make the bulb glow, and metals like sodium are very soft. So the tests work for most samples but exceptions exist.

6. What are amphoteric oxides? Give two examples of amphoteric oxides.

ANSWER Amphoteric oxides are metal oxides that react with both acids and bases to produce salt and water. Examples: aluminium oxide (Al2O3) and zinc oxide (ZnO). Al2O3 + 6HCl → 2AlCl3 + 3H2O (acidic behaviour); Al2O3 + 2NaOH → 2NaAlO2 + H2O (basic behaviour).

7. Name two metals which will displace hydrogen from dilute acids, and two metals which will not.

ANSWER Metals placed above hydrogen in the activity series displace hydrogen from dilute acids: e.g. magnesium (Mg) and zinc (Zn) (also iron, aluminium). Metals placed below hydrogen do not displace hydrogen from dilute acids: e.g. copper (Cu) and silver (Ag) (also gold).

8. In the electrolytic refining of a metal M, what would you take as the anode, the cathode and the electrolyte?

ANSWER For electrolytic refining of metal M: the anode is a thick block of impure metal M; the cathode is a thin strip of pure metal M; and the electrolyte is a water-soluble salt solution of metal M (for example, the acidified solution of the salt of M). On passing current, pure M dissolves from the anode and deposits on the cathode, while impurities collect as anode mud.

9. Pratyush took sulphur powder on a spatula and heated it. He collected the gas evolved by inverting a test tube over it, as shown in figure. (a) What will be the action of gas on (i) dry litmus paper? (ii) moist litmus paper? (b) Write a balanced chemical equation for the reaction taking place.

ANSWER On burning, sulphur forms sulphur dioxide gas (SO2), which is an acidic oxide. (a)(i) On dry litmus paper there is no change, because dry SO2 gas cannot act as an acid without water. (a)(ii) On moist blue litmus paper, SO2 dissolves in the moisture to form sulphurous acid (H2SO3) and turns moist blue litmus paper red. (b) S(s) + O2(g) → SO2(g). (With water: SO2 + H2O → H2SO3.)

10. State two ways to prevent the rusting of iron.

ANSWER (i) Galvanisation — coating iron with a thin layer of zinc, which protects it even if the coating is scratched. (ii) Painting, oiling or greasing the iron surface to keep out air and moisture. (Other methods: chrome plating, anodising, or making alloys such as stainless steel.)

11. What type of oxides are formed when non-metals combine with oxygen?

ANSWER Non-metals combine with oxygen to form acidic oxides or neutral oxides. For example, sulphur forms acidic SO2 (which gives sulphurous acid in water), and carbon forms acidic CO2; while water (H2O), carbon monoxide (CO) and nitrous oxide (N2O) are neutral oxides.

12. Give reasons (a) Platinum, gold and silver are used to make jewellery. (b) Sodium, potassium and lithium are stored under oil. (c) Aluminium is a highly reactive metal, yet it is used to make utensils for cooking. (d) Carbonate and sulphide ores are usually converted into oxides during the process of extraction.

ANSWER (a) Platinum, gold and silver are the least reactive (noble) metals. They do not react with air, water or most chemicals, so they keep their shine and do not corrode — ideal for long-lasting jewellery. They are also malleable, ductile and lustrous. (b) Sodium, potassium and lithium are extremely reactive. They react vigorously with oxygen and moisture in air and may catch fire. Storing them under oil (kerosene) keeps them away from air and moisture, preventing such reactions and accidental fires. (c) Aluminium quickly forms a thin, hard, unreactive layer of aluminium oxide (Al2O3) on its surface. This protective layer prevents further reaction, so aluminium does not corrode easily. Being a good conductor of heat with a high melting point, it is suitable for cooking utensils. (d) It is easier to obtain a metal by reducing its oxide than its carbonate or sulphide. Therefore, before reduction, carbonate ores are converted to oxides by calcination and sulphide ores by roasting, after which the oxide is reduced to the metal.

13. You must have seen tarnished copper vessels being cleaned with lemon or tamarind juice. Explain why these sour substances are effective in cleaning the vessels.

ANSWER Copper vessels get a dull green/black tarnish because copper reacts with moist air to form a coating of basic copper carbonate (and copper oxide). Lemon and tamarind juice contain acids (citric acid and tartaric acid). These acids react with and dissolve the basic carbonate/oxide layer, leaving the bright, shiny copper surface clean again.

14. Differentiate between metal and non-metal on the basis of their chemical properties.

ANSWER
Chemical propertyMetalsNon-metals
Reaction with oxygenForm basic (or amphoteric) oxides, e.g. Na2O, MgOForm acidic or neutral oxides, e.g. SO2, CO2
Reaction with dilute acidsDisplace hydrogen (if above H in the series) to give salt + H2Do not displace hydrogen from dilute acids
Reaction with waterReactive metals react to give hydroxide/oxide + H2Generally do not react with water
Ion formationLose electrons to form positive ions (cations)Gain electrons to form negative ions (anions)
Reaction with hydrogenGenerally do not react with hydrogenReact with hydrogen to form hydrides
Reducing/oxidising natureAct as reducing agents (electron donors)Act as oxidising agents (electron acceptors)

15. A man went door to door posing as a goldsmith. He promised to bring back the glitter of old and dull gold ornaments. An unsuspecting lady gave a set of gold bangles to him which he dipped in a particular solution. The bangles sparkled like new but their weight was reduced drastically. The lady was upset but after a futile argument the man beat a hasty retreat. Can you play the detective to find out the nature of the solution he had used?

ANSWER The man dipped the bangles in aqua regia — a freshly prepared mixture of concentrated hydrochloric acid and concentrated nitric acid in the ratio 3:1. Aqua regia is one of the few reagents that can dissolve gold. A thin outer layer of gold dissolved, making the bangles bright and shiny but reducing their weight (and the dissolved gold was kept by the cheat). Hence the solution used was aqua regia.

16. Give reasons why copper is used to make hot water tanks and not steel (an alloy of iron).

ANSWER Copper does not react with cold water, hot water or steam, so it is not corroded by hot water in the tank. Iron (and steel), on the other hand, reacts with steam (3Fe + 4H2O → Fe3O4 + 4H2) and rusts in the presence of hot water and air. Therefore copper, being unreactive towards water and a good conductor of heat, is used for hot water tanks instead of steel.

Extra Practice Questions

Short Answer Type Questions

Q1. Why is gold and silver used for making ornaments rather than sodium or potassium?

ANSWERGold and silver are the least reactive metals — they do not corrode and retain their lustre — whereas sodium and potassium are so reactive that they react with air and water (even catching fire), so they cannot be worn as ornaments.

Q2. Why do ionic compounds conduct electricity in the molten or aqueous state but not in the solid state?

ANSWERIn the solid state the ions are held in fixed positions by strong forces and cannot move. In the molten or aqueous state these forces are overcome, so the ions become free to move towards the electrodes and carry current; hence electricity is conducted.

Q3. Define roasting and calcination with one equation each.

ANSWERRoasting: heating a sulphide ore strongly in excess air to form oxide — 2ZnS + 3O2 → 2ZnO + 2SO2. Calcination: heating a carbonate ore strongly in limited air to form oxide — ZnCO3 → ZnO + CO2.

Q4. Why does sodium not occur in nature in the free state?

ANSWERSodium is at the top of the reactivity series and is extremely reactive. It readily combines with other elements (oxygen, water, chlorine, etc.), so it is always found in nature as compounds and never as a free element.

Q5. Why is the galvanised article protected against rusting even if the zinc coating is broken?

ANSWERZinc is more reactive than iron, so it acts as a sacrificial coating — it gets oxidised in preference to iron. Even when the zinc layer is broken, the exposed zinc corrodes first and protects the iron from rusting.

Long Answer Type Questions

Q1. Describe how a metal in the middle of the activity series (e.g. zinc) is extracted from its sulphide ore.

ANSWERMetals of medium reactivity such as zinc occur as sulphides or carbonates. First the ore is enriched to remove gangue. The sulphide ore is then converted to oxide by roasting (heating in excess air): 2ZnS + 3O2 → 2ZnO + 2SO2. (A carbonate ore would be converted to oxide by calcination: ZnCO3 → ZnO + CO2.) The zinc oxide is then reduced to the metal using carbon as the reducing agent: ZnO + C → Zn + CO. The impure zinc obtained is finally purified by electrolytic refining to get pure zinc.

Q2. Explain the formation of magnesium chloride (MgCl2) by the transfer of electrons and state two properties of the compound formed.

ANSWERMagnesium (2,8,2) has two valence electrons and chlorine (2,8,7) needs one electron to complete its octet. Magnesium loses 2 electrons to form Mg2+ (Mg → Mg2+ + 2e–), and each of two chlorine atoms gains one electron to form Cl– (2Cl + 2e– → 2Cl–). The oppositely charged Mg2+ and Cl– ions are held by strong electrostatic forces as MgCl2, an ionic compound. Properties: it is a hard, crystalline solid with a high melting point, soluble in water, and it conducts electricity in molten or aqueous state.

Q3. What is corrosion? Describe the experiment that shows the conditions necessary for the rusting of iron.

ANSWERCorrosion is the slow eating up of the surface of a metal by the action of air, moisture and chemicals; the rusting of iron is an example. In the experiment, clean iron nails are placed in three test tubes A, B and C. Tube A has ordinary water and is corked (nails exposed to both air and water). Tube B has boiled distilled water with a layer of oil on top and is corked (no dissolved air, only water). Tube C has anhydrous calcium chloride to absorb moisture and is corked (only dry air, no moisture). After a few days, the nails rust only in tube A and not in B or C. This proves that both air (oxygen) and water (moisture) are necessary together for the rusting of iron.

MCQs & Assertion–Reason

1. The most ductile metal is:

(a) silver    (b) gold    (c) copper    (d) aluminium

2. Which of the following is an amphoteric oxide?

(a) Na2O    (b) MgO    (c) ZnO    (d) CuO

3. Which metal reacts violently with cold water?

(a) magnesium    (b) iron    (c) zinc    (d) potassium

4. The reaction of iron(III) oxide with aluminium used to join railway tracks is called the:

(a) roasting reaction    (b) thermit reaction    (c) calcination    (d) displacement of hydrogen

5. Aqua regia is a mixture of concentrated HCl and concentrated HNO3 in the ratio:

(a) 1:3    (b) 3:1    (c) 1:1    (d) 2:1

6. Heating a sulphide ore strongly in excess of air is called:

(a) calcination    (b) reduction    (c) roasting    (d) refining

7. Which gas is evolved when zinc reacts with dilute hydrochloric acid?

(a) oxygen    (b) chlorine    (c) carbon dioxide    (d) hydrogen

8. In the electrolytic refining of copper, the anode is made of:

(a) pure copper    (b) impure copper    (c) graphite    (d) iron

9. The non-metal that conducts electricity is:

(a) sulphur    (b) iodine    (c) graphite    (d) diamond

10. Both air and which of the following are necessary for rusting of iron?

(a) nitrogen    (b) water (moisture)    (c) carbon dioxide    (d) oil

Answer key: 1-(b), 2-(c), 3-(d), 4-(b), 5-(b), 6-(c), 7-(d), 8-(b), 9-(c), 10-(b).

For each Assertion–Reason question, choose: (A) Both true and the Reason correctly explains the Assertion; (B) Both true but the Reason is not the correct explanation; (C) Assertion true, Reason false; (D) Assertion false, Reason true.

A-R 1. Assertion: Sodium is stored under kerosene oil.

Reason: Sodium reacts vigorously with oxygen and moisture of air and may catch fire.

A-R 2. Assertion: Ionic compounds have high melting and boiling points.

Reason: A large amount of energy is needed to overcome the strong electrostatic forces between the ions.

A-R 3. Assertion: Copper displaces silver from silver nitrate solution.

Reason: Copper is less reactive than silver.

A-R 4. Assertion: Carbon cannot be used to reduce the oxides of sodium and aluminium.

Reason: These metals have a greater affinity for oxygen than carbon, so they are extracted by electrolytic reduction.

A-R 5. Assertion: All metal oxides are basic in nature.

Reason: Aluminium oxide and zinc oxide are amphoteric oxides.

Answer key: 1-(A), 2-(A), 3-(C), 4-(A), 5-(D).

Common Mistakes to Avoid

Watch out for these

  • Confusing roasting (sulphide ore, excess air) with calcination (carbonate ore, limited air).
  • Forgetting the exceptions: mercury is a liquid metal, iodine is a lustrous non-metal, and graphite (non-metal) conducts electricity.
  • Writing that hydrogen gas is evolved when metals react with nitric acid — generally it is not, because HNO3 is a strong oxidising agent (Mg and Mn with very dilute HNO3 are exceptions).
  • Forgetting to balance equations and to write physical states (s, l, g, aq) where required.
  • Mixing up the position of hydrogen in the activity series — only metals above hydrogen displace it from dilute acids.
  • Saying dry SO2 turns litmus red — it acts on moist litmus only.

How to score full marks in this chapter

Learn the activity series in order (K, Na, Ca, Mg, Al, Zn, Fe, Pb, H, Cu, Hg, Ag, Au) — many questions on displacement, extraction and reactivity depend on it. Always give balanced equations with correct subscripts/superscripts and state symbols. For reasoning questions (jewellery, storing sodium, aluminium utensils) link your answer to reactivity and the protective oxide layer. Practise the extraction flow: enrichment → roasting/calcination → reduction → refining, and remember which method suits each part of the activity series.

Frequently Asked Questions

What is Class 10 Science Chapter 3 Metals and Non-metals about?

It covers the physical and chemical properties of metals and non-metals, the reactivity series, formation and properties of ionic compounds, extraction and refining of metals (metallurgy), and corrosion with its prevention.

What is the reactivity series in Chapter 3?

The reactivity (activity) series lists metals in decreasing order of reactivity: K > Na > Ca > Mg > Al > Zn > Fe > Pb > (H) > Cu > Hg > Ag > Au. A more reactive metal can displace a less reactive metal from its salt solution.

What is the difference between roasting and calcination?

Roasting is heating a sulphide ore strongly in the presence of excess air to convert it to oxide, while calcination is heating a carbonate ore strongly in limited air to convert it to oxide.

Are these Class 10 Science Chapter 3 solutions free?

Yes. All solutions are free and follow the official NCERT Science textbook for session 2026–27, with every in-text and exercise question answered step by step.

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