Metals and Non-metals Class 10 important questions with answers

What comes in the exam

• Metals and Non-metals is part of the Chemical Substances unit, which is worth 25 marks in all.
• MCQs (1 mark) come most, then 3-mark, 2-mark and 4-mark case-study questions, with some Assertion–Reason and 5-mark questions.
• Almost every year you get questions on getting metals from their ores (roasting, calcination, reduction, the thermit reaction, electrolytic refining) and on showing how an ionic compound forms by electron transfer.
• Amphoteric oxides, how metals react with water, acids and salt solutions, corrosion and alloys also come almost every year, mostly as MCQs and 'give reason' parts.

Top 10 Metals and Non-metals questions from board papers

Real CBSE questions, printed as they appeared. Open each answer to see the marking and the steps.

1. Q1 MCQ · 1 mark CBSE · 2025, 2024 Asked in 2025, 2024

   Nature of Al and Zn oxides

   Oxides of aluminium and zinc are:

   • (A) Acidic
   • (B) Amphoteric
   • (C) Basic
   • (D) Neutral
   Answer and marking

   Correct option: (B) Amphoteric

   1. Recall how Al₂O₃ and ZnO behave with acids and with bases. Al₂O₃, ZnO react with both acids and bases → salt + water
   2. An oxide that reacts with both is called amphoteric. (B) Amphoteric 1 mark

   Answer: (B) Amphoteric

   Marks: Correct option 1

   For full marks: Define it in your answer: reacts with both acids and bases to give salt and water.

   Where students lose marks: Picking (C) Basic: most metal oxides are basic, but aluminium and zinc oxides also react with bases.

   CBSE marking scheme

   Al2O3 and ZnO react with both acids and bases: amphoteric oxides.

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2. Q2 Short answer · 3 marks CBSE · 2026

   Soft metal; Mg + O bonding

   (i) Write one example each of one metal that is so soft that it can be cut with a knife, and one non-metal that is a good conductor of electricity. (1) (ii) Using the electronic configuration, explain how Mg atom combines with oxygen to form magnesium oxide by transfer of electrons. [Atomic number: Mg = 12, O = 8] (2)

   Answer and marking

   1. (i) Name a metal soft enough to cut with a knife. Sodium (or lithium/potassium) 0.5 marks
   2. Name the non-metal that conducts electricity. Graphite 0.5 marks
   3. (ii) Mg has 2 outer electrons; it gives them away. Mg (2,8,2) → Mg²⁺ (2,8) + 2e⁻ 0.5 marks
   4. O has 6 outer electrons; it takes 2 to complete its octet. O (2,6) + 2e⁻ → O²⁻ (2,8) 0.5 marks
   5. Show the transfer with electron dots and the ions formed. Mg: + O → [Mg²⁺][O²⁻] ; ionic MgO 1 mark

   Answer: (i) Sodium, graphite ; (ii) Mg → Mg²⁺ + 2e⁻, O + 2e⁻ → O²⁻, forming ionic MgO

   Marks: Examples 1 · Two ion equations 1 · Electron-dot transfer 1

   For full marks: Write both electronic configurations, before and after, and the charges 2+ and 2− on the ions.

   Where students lose marks: Showing electrons shared between Mg and O as in a covalent bond instead of transferred.

   CBSE marking scheme

   (i) Lithium/sodium/potassium (½); graphite (½). (ii) Mg (2,8,2) → Mg2+ (2,8) + 2e− (½); O (2,6) + 2e− → O2− (2,8) (½); electron-dot diagram: Mg: + O → [Mg2+][O2−], forming ionic MgO (1).

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3. Q3 Short answer · 3 marks CBSE · 2025

   Metals reacting with cold water

   (i) Name two metals which react violently with cold water. List any three observations which a student notes when these metals are dropped in a beaker containing water. (ii) Write a test to identify the gas evolved (if any) during the reaction of these metals with water.

   Answer and marking

   1. (i) Name two metals at the top of the reactivity series. Sodium and potassium (any two of sodium, potassium, lithium) 1 mark
   2. First observation: how the reaction goes. The reaction is violent 0.5 marks
   3. Second observation: the temperature. A large amount of heat is evolved 0.5 marks
   4. Third observation: what happens to the gas. The evolved gas may catch fire 0.5 marks
   5. (ii) The gas is hydrogen; give its test. H₂ burns with a pop sound when a burning splinter is brought near 0.5 marks

   Answer: (i) Sodium, potassium ; violent, much heat, gas catches fire ; (ii) pop sound with a burning splinter

   Marks: Two metals 1 · Three observations 1½ · Test ½

   For full marks: List three separate observations — each earns ½.

   Where students lose marks: Naming calcium or magnesium, which do not react violently with cold water.

   CBSE marking scheme

   (i) Any two of sodium, potassium, lithium (½+½); observations: violent reaction, large amount of heat evolved, evolved gas may catch fire (½×3). (ii) Gas (H2) burns with a pop sound when a burning splinter is brought near (½).

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4. Q4 Case study · 4 marks CBSE · 2026

   Case: ores and their reduction

   Read the following passage and answer the questions given below: Most of metals occur in combined state in form of ores. Carbonate ores are converted into oxides by calcination and sulphide ores by roasting. Oxides are reduced with suitable reducing agent like carbon to get free metal. Highly reactive metals like Al, Mg are also used as reducing agents to obtain metal from their oxides. Most reactive metals are obtained by electrolytic reduction of their molten ores. Alloying is a very good method of improving the properties of a metal. We can get desired properties by this method. The electrical conductivity and melting point of an alloy is less than that of pure metals. (i) Why carbonate or sulphide ores are converted to oxides before extraction of metal from it? (1) (ii) Write a reaction in which Aluminium is used as a reducing agent to obtain metal from its oxide. (1) (iii) (a) How is copper obtained from its ore (Cu2S)? Give equations of the reactions. (2) OR (iii) (b) (I) Why highly reactive metals cannot be obtained from their oxides by using carbon as a reducing agent? (1) (II) Why solder, an alloy of lead and tin, is used for welding electrical wires together? (1)

   Answer and marking

   1. (i) Carbon reduces oxides easily, so the ore is first changed into an oxide. It is easier to obtain (reduce) a metal from its oxide than from its carbonate or sulphide. 1 mark
   2. (ii) Aluminium is more reactive than iron, so it takes oxygen away from iron oxide. Fe₂O₃ + 2Al → 2Fe + Al₂O₃ + heat 1 mark
   3. (iii)(a) First roast the copper sulphide in air to make some copper(I) oxide. 2Cu₂S + 3O₂ →(heat) 2Cu₂O + 2SO₂ 1 mark
   4. Then heat this oxide with the rest of the sulphide; copper is set free. 2Cu₂O + Cu₂S →(heat) 6Cu + SO₂ 1 mark
   5. (iii)(b)(I) Compare how strongly the metal and carbon pull on oxygen. Highly reactive metals have more affinity for oxygen than carbon, so carbon cannot reduce their oxides. 1 mark
   6. (II) Joining wires needs an alloy that melts easily without harming the wires. Solder has a low melting point. 1 mark

   Answer: (i) Oxides are easier to reduce (ii) Fe₂O₃ + 2Al → 2Fe + Al₂O₃ + heat (iii) (a) 2Cu₂S + 3O₂ → 2Cu₂O + 2SO₂ ; 2Cu₂O + Cu₂S → 6Cu + SO₂ / (b) more affinity for oxygen than carbon ; solder has a low melting point

   Marks: (i) Reason 1 · (ii) Thermit equation 1 · (iii) Two equations or two reasons 2

   For full marks: In (iii)(a) write BOTH equations — roasting and then the reaction of Cu₂O with Cu₂S; each carries 1 mark.

   Where students lose marks: Writing only Cu₂S + O₂ → Cu + SO₂ in one line, which skips the Cu₂O step the second mark is for.

   CBSE marking scheme

   (i) It is easier to obtain/reduce a metal from its oxide (1). (ii) Fe2O3 + 2Al → 2Fe + Al2O3 + heat, or 3MnO2 + 4Al → 3Mn + 2Al2O3 + heat (1; balancing optional). (iii)(a) 2Cu2S + 3O2 → 2Cu2O + 2SO2 (heat) (1); 2Cu2O + Cu2S → 6Cu + SO2 (heat) (1). OR (iii)(b) (I) Highly reactive metals have more affinity for oxygen than carbon (1). (II) Solder has a low melting point (1).

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5. Q5 Case study · 4 marks CBSE · 2026

   Case: Statue of Liberty colour

   The Statue of Liberty is one of the seven wonders. It is present on Liberty island in New York harbour in U.S.A. It is made up of a metal. Over a period of time, the metal's colour has changed and the statue gives a greenish look. Answer the following questions based on the above information: (i) What is corrosion? (1) (ii) Why do silver articles turn black after some time? (1) (iii) Copper reacts with moist gas 'A' present in the air and slowly loses its shiny surface. It turns green. Identify 'A' and the substance of green coating formed on the surface of copper. (2) OR (iii) What is an alloy? How is an alloy made? (2)

   Answer and marking

   1. (i) Define it as a slow change of the metal caused by the air around it. Corrosion is the slow, gradual eating away of a metal by moisture, acids etc. in the air. 1 mark
   2. (ii) Name what silver reacts with and the black coating formed. Silver reacts with sulphur in the air to form black silver sulphide. 1 mark
   3. (iii)(a) The green coat contains carbonate, so the gas must be carbon dioxide. A = carbon dioxide (moist) 1 mark
   4. Name the green substance. Green coating: basic copper carbonate 1 mark
   5. (iii)(b) Define an alloy first. An alloy is a homogeneous mixture of two or more metals, or of a metal and a non-metal. 1 mark
   6. Then say how it is made. It is made by melting the main metal and mixing the others in, in the molten state. 1 mark

   Answer: (i) Slow eating away of a metal by air and moisture (ii) silver sulphide (iii) (a) A = CO₂ ; basic copper carbonate / (b) homogeneous mixture of metals ; mixed in molten state

   Marks: (i) Definition 1 · (ii) Reason 1 · (iii) Two points 2

   For full marks: Write 'basic copper carbonate', not just 'copper carbonate' — the full name is what earns the mark.

   Where students lose marks: Naming oxygen as gas A; the green coating needs carbon dioxide (with moisture).

   CBSE marking scheme

   (i) Slow, gradual degradation of a metal by reaction with moisture, acids etc. in the atmosphere (1). (ii) Silver reacts with sulphur in the air forming black silver sulphide (1). (iii) A – carbon dioxide (1); green coating – basic copper carbonate (1). OR (iii) Alloy: homogeneous mixture of two or more metals, or a metal and a non-metal (1); made by mixing the metals in the molten state (1).

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6. Q6 Case study · 4 marks CBSE · 2026

   Case: electrolytic refining

   Read the following passage and answer the questions that follow: An electrochemical process is used for refining metals by selectively dissolving and depositing them through electrolysis. Electrolytic refining is used for metals like Copper, Zinc, Tin, Nickel, Silver and Gold. (a) Define anode mud. (1) (b) In electrolytic refining of copper, name the anode and the cathode. (1) (c) (i) With the help of chemical equations, show the extraction of copper from its ore Cu2S. (2) OR (c) (ii) Draw a neat and labelled diagram showing electrolytic refining of copper. (2)

   Answer and marking

   1. (a) Say what anode mud is and where it collects. Anode mud: insoluble impurities that settle at the bottom below the anode during electrolytic refining 1 mark
   2. (b) The impure metal dissolves, so it is the anode. Anode: impure copper 0.5 marks
   3. Pure copper is deposited on the cathode. Cathode: thin strip of pure copper 0.5 marks
   4. (c)(i) First roast copper sulphide in air. 2Cu₂S + 3O₂ →(heat) 2Cu₂O + 2SO₂ 1 mark
   5. Then the oxide reacts with the rest of the sulphide to give copper. 2Cu₂O + Cu₂S →(heat) 6Cu + SO₂ 1 mark
   6. (c)(ii) Draw the tank and both electrodes joined to a battery. Tank of acidified CuSO₄ ; impure Cu anode and pure Cu cathode dipped in it ; both joined to a battery ; anode mud below the anode 1 mark
   7. Label every part of your diagram. Labels: acidified copper sulphate solution, impure copper anode, pure copper cathode, anode mud 1 mark

   Answer: (a) Insoluble impurities settled below the anode (b) anode impure Cu ; cathode pure Cu (c) (i) 2Cu₂S + 3O₂ → 2Cu₂O + 2SO₂ ; 2Cu₂O + Cu₂S → 6Cu + SO₂ / (ii) labelled diagram

   Marks: (a) Definition 1 · (b) Two electrodes 1 · (c) Two equations, or diagram and labels 2

   For full marks: Label the electrolyte as 'acidified copper sulphate' and show anode mud under the anode — the labels mark needs them.

   Where students lose marks: Swapping the electrodes: pure copper is the cathode, impure copper the anode.

   CBSE marking scheme

   (a) Insoluble impurities that settle at the bottom below the anode during electrolytic refining (1). (b) Anode: impure copper (½); cathode: thin strip of pure copper (½). (c)(i) 2Cu2S + 3O2 →(heat) 2Cu2O + 2SO2 (1); 2Cu2O + Cu2S →(heat) 6Cu + SO2 (1). OR (c)(ii) Diagram of tank with acidified CuSO4 electrolyte, impure Cu anode, pure Cu cathode, anode mud (diagram 1, labels 1).

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7. Q7 Case study · 4 marks CBSE · 2024

   Case: Mg, Al, Fe in dilute HCl

   Three metal samples of magnesium, aluminium and iron were taken and rubbed with sand paper. These samples were then put separately in test tubes containing dilute hydrochloric acid. Thermometers were also suspended in each test tube so that their bulbs dipped in the acid. The rate of formation of bubbles was observed. The above activity was repeated with dilute nitric acid and the observations were recorded. (i) When activity was done with dilute hydrochloric acid, then in which one of the test tubes was the rate of formation of bubbles the fastest and the thermometer showed the highest temperature? (1) (ii) Which metal did not react with dilute hydrochloric acid? Give reason. (1) (iii) Why is hydrogen gas not evolved when a metal reacts with dilute nitric acid? Name the ultimate products formed in the reaction. (2) OR (iii) Name the type of reaction on the basis of which reactivity of metals is decided. You have two metals X and Y. How would you decide which is more reactive than the other? (2)

   Answer and marking

   1. (i) The most reactive metal reacts fastest and gives out the most heat. Magnesium 1 mark
   2. (ii) Check where each metal stands compared with hydrogen. None — all three react with dilute HCl because they are more reactive than hydrogen. 1 mark
   3. (iii)(a) Nitric acid is a strong oxidising agent, so it removes the hydrogen formed. HNO₃ oxidises the H₂ produced to water. 1 mark
   4. Name what it ends up as. Products: water and oxides of nitrogen 1 mark
   5. (iii)(b) A more reactive metal pushes a less reactive one out of its salt. Displacement reaction 1 mark
   6. Put X into a salt solution of Y and see if Y comes out. If X displaces Y from its salt solution, X is more reactive than Y ; if not, Y is more reactive. 1 mark

   Answer: (i) Magnesium (ii) all three react — more reactive than hydrogen (iii) (a) HNO₃ oxidises H₂ to water ; water and nitrogen oxides / (b) displacement ; X displaces Y ⇒ X more reactive

   Marks: (i) Metal 1 · (ii) Metal with reason 1 · (iii) Two points 2

   For full marks: In (iii)(a) say nitric acid is an oxidising agent that turns H₂ into water — the reason earns the first mark.

   Where students lose marks: In (ii) naming iron or aluminium as 'not reacting'; all three metals are above hydrogen in the series.

   CBSE marking scheme

   (i) Magnesium (1). (ii) All three react with HCl as they are more reactive than hydrogen (1) (award if a less reactive metal is named with reason). (iii) HNO3 is a strong oxidising agent and oxidises the H2 produced to water (1); products: water and oxides of nitrogen (1). OR (iii) Displacement reaction (1); if X displaces Y from its salt solution, X is more reactive, and vice versa (1).

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8. Q8 Long answer · 5 marks CBSE · 2026

   Extract Hg, Zn, Na; NaCl facts

   (i) Write the balanced chemical equation involved in the extraction of : (I) Hg from HgS (II) Zn from ZnCO3 (III) Na from NaCl (ii) Why does sodium chloride : (I) not conduct electricity in solid state ? (II) have very high melting point ?

   Answer and marking

   1. (i)(I) Roast the sulphide to oxide, then heat the oxide. 2HgS + 3O₂ →(heat) 2HgO + 2SO₂ ; 2HgO →(heat) 2Hg + O₂ 1 mark
   2. (II) Calcine the carbonate, then reduce the oxide with carbon. ZnCO₃ →(heat) ZnO + CO₂ ; ZnO + C → Zn + CO 1 mark
   3. (III) Sodium is too reactive, so molten NaCl is electrolysed. Cathode: Na⁺ + e⁻ → Na ; anode: 2Cl⁻ → Cl₂ + 2e⁻ 1 mark
   4. (ii)(I) Current needs ions that can move. In the solid the ions cannot move because of the rigid structure. 1 mark
   5. (II) Think how strongly the opposite ions hold each other. Much energy is needed to overcome the strong electrostatic attraction between oppositely charged ions. 1 mark

   Answer: (i) HgS → HgO → Hg ; ZnCO₃ → ZnO → Zn ; Na⁺ + e⁻ → Na (ii) ions not free to move ; strong attraction between ions

   Marks: Three extractions 3 · Two reasons 2

   For full marks: For each metal write BOTH stages (or both electrodes) — one equation alone does not earn the mark.

   Where students lose marks: Writing ZnCO₃ + C → Zn directly, skipping calcination, or electrolysing aqueous NaCl instead of molten NaCl.

   CBSE marking scheme

   (i)(I) 2HgS + 3O2 → (heat) 2HgO + 2SO2; 2HgO → (heat) 2Hg + O2 (1). (II) ZnCO3 → (heat) ZnO + CO2; ZnO + C → Zn + CO (1). (III) Electrolysis of molten NaCl: at cathode Na+ + e- → Na; at anode 2Cl- → Cl2 + 2e- (1). (ii)(I) In the solid the ions cannot move because of the rigid structure (1). (II) Much energy is needed to overcome the strong electrostatic attraction between oppositely charged ions (1).

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9. Q9 Long answer · 5 marks CBSE · 2025

   Metals and oxygen; oxide types

   (i) Consider the following metals: K, Ca, Al, Cu, Ag, Fe. Select from the above metals, a metal which I. does not react with oxygen even at high temperature. II. reacts with oxygen at ordinary temperature and forms a protective oxide layer which prevents the metal from further oxidation. III. catches fire when kept in the open. IV. does not burn in oxygen but the hot metal is coated with a black coloured oxide layer. (ii) What are amphoteric oxides? With the help of balanced chemical equations show that aluminium oxide is an amphoteric oxide. (iii) What are alkalis? Give one example.

   Answer and marking

   1. (i) Use the reactivity series; each correct pick earns half a mark. I Ag ; II Al ; III K ; IV Cu 2 marks
   2. (ii) Define the term first. Amphoteric oxides are metal oxides that react with both acids and bases to give salt and water. 1 mark
   3. Show Al₂O₃ acting as a base with an acid. Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O 0.5 marks
   4. Show Al₂O₃ acting as an acid with a base. Al₂O₃ + 2NaOH → 2NaAlO₂ + H₂O 0.5 marks
   5. (iii) Define an alkali. Alkalis are bases that dissolve in water. 0.5 marks
   6. Give one example. e.g. NaOH (or KOH) 0.5 marks

   Answer: (i) Ag, Al, K, Cu (ii) react with acids and bases ; Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O ; Al₂O₃ + 2NaOH → 2NaAlO₂ + H₂O (iii) water-soluble bases, NaOH

   Marks: Four metals 2 · Definition and two equations 2 · Alkali and example 1

   For full marks: Write one equation with an acid AND one with a base — each is half a mark.

   Where students lose marks: In IV picking iron; it is copper that does not burn but gets a black oxide coat.

   CBSE marking scheme

   (i) I Ag, II Al, III K, IV Cu (½×4). (ii) Metal oxides that react with both acids and bases to give salt and water (1); Al2O3 + 6HCl → 2AlCl3 + 3H2O (½); Al2O3 + 2NaOH → 2NaAlO2 + H2O (½) (no deduction if unbalanced). (iii) Water-soluble bases (½); e.g. NaOH/KOH (½).

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10. Q10 Long answer · 5 marks CBSE · 2024

    Ionic bond: X (12) and Y (17)

    Write electronic configurations of two elements X (At. no. 12) and Y (At. no. 17). Show the formation of ionic compound when X and Y combine with each other. Write the name and formula of the compound formed. State what would happen if electric current is passed through the aqueous solution of this compound. Name the ion that will reach at (i) cathode, and (ii) anode.

    Answer and marking

    1. Fill the shells 2, 8, … for 12 electrons. X (12): 2,8,2 0.5 marks
    2. Do the same for 17 electrons. Y (17): 2,8,7 0.5 marks
    3. X gives one electron to each of two Y atoms; draw it with dots. Mg: + 2 Cl → Mg²⁺ + 2Cl⁻ (Mg gives one electron to each Cl) 1 mark
    4. X is magnesium and Y is chlorine; name the compound. Magnesium chloride 0.5 marks
    5. One Mg²⁺ balances two Cl⁻. MgCl₂ (XY₂) 0.5 marks
    6. Say what the current does to the dissolved compound. The compound splits into ions, which move to opposite electrodes — electrolysis takes place. 1 mark
    7. (i) Positive ions go to the negative electrode. Cathode: Mg²⁺ 0.5 marks
    8. (ii) Negative ions go to the positive electrode. Anode: Cl⁻ 0.5 marks

    Answer: X 2,8,2 ; Y 2,8,7 ; magnesium chloride, MgCl₂ ; electrolysis ; Mg²⁺ to cathode, Cl⁻ to anode

    Marks: Configurations 1 · Formation 1 · Name and formula 1 · Electrolysis 1 · Two ions 1

    For full marks: Write the name AND the formula MgCl₂ — they are half a mark each.

    Where students lose marks: Writing the formula as MgCl; Mg loses two electrons, so it needs two chlorine atoms.

    CBSE marking scheme

    X: 2,8,2 (½); Y: 2,8,7 (½). Electron-dot formation: Mg gives two electrons, one to each of two Cl atoms → Mg2+ and 2Cl– (1). Name: magnesium chloride (½); formula MgCl2 / XY2 (½). The compound dissociates into ions which move to opposite electrodes – electrolysis occurs (1). (i) Cathode: Mg2+ (½); (ii) anode: Cl– (½).

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Free 10-question test: Metals and Non-metals

MCQ and Assertion–Reason questions from CBSE papers. About 10 minutes. Your score shows straight away.

Common mistakes in Metals and Non-metals

How to write for full marks

• For extraction, write each step in order with its own equation: first change the ore to an oxide, then reduce the oxide to the metal. Each step earns marks, so do not skip one.
• Write 'heat' over the arrow where the ore is heated, and add '+ heat' on the right of the thermit equation.
• For the refining diagram, draw the tank, both electrodes and the battery, then label the electrolyte, impure anode, pure cathode and anode mud. The drawing and the labels carry separate marks.
• When a question lists parts I, II, III, IV, answer each one on its own line with its label. Each part carries its own ½ or 1 mark.
• For amphoteric oxides, write the definition, then two equations: the oxide with an acid and the same oxide with a base, each giving salt and water.

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