CBSE Class 10 Science Chapter 3 Metals and Non Metals Important Questions

Chapter 3 of Class 10 Science, Metals and Non-Metals, is one of the most important parts of the syllabus for board exam preparation. Every year, questions from this chapter carry significant weight in the paper. To help students prepare well, practising metals and non metals class 10 important questions is highly recommended. These questions cover all the key concepts such as properties, reactions, uses, and extraction of metals and non-metals. A well-structured practice with metals and non metals important questions ensures that you revise systematically and focus on what is most likely to appear in the exam.

In this chapter, students learn to differentiate between metals and non-metals on the basis of their physical and chemical properties. For example, the softness of sodium, the hardness of diamond, and the conductivity of graphite are concepts that frequently appear in metal and non metals class 10 important questions. Along with these, you also need to study the activity series, ionic bonding, corrosion, and alloys. This is why solving class 10 metals and non metals important questions from every topic is necessary.

Apart from direct questions, exams also test conceptual understanding through application-based and reasoning problems. To prepare for these, students must attempt hots questions on metals and non-metals class 10. These questions not only sharpen analytical skills but also help in writing clear and confident answers. 

For effective revision, we provide metals and non metals class 10 important questions with answers. These answers are written in simple steps so that students can easily recall and reproduce them during exams. While going through important questions of metal and nonmetal class 10, you will also notice that many questions repeat in some form every year, which makes practice even more useful.

Do check: CBSE Class 10 Science Chapter 2 Acid, Bases and Salts Important Questions

As you prepare for upcoming exams, especially the board exam cycle, the latest metals and non metals class 10 important questions 2025 have been included to match the current pattern. Even if you are looking for one key metal and non metal important question to revise quickly, you will find examples here for last-minute practice.

Metals and Non Metals Class 10 Important Questions

Ques. Give one example each of

(i) a very soft metal that can be cut with a knife, and the hardest non-metal.
(ii) a metal and a non-metal that are liquids at room temperature.

Ans.

(i) Sodium is a soft metal; diamond (carbon) is the hardest non-metal.
(ii) Mercury is the liquid metal; bromine is the liquid non-metal.

Ques. Name the metals used for:

(i) making stainless steel (alloyed with iron), 
(ii) making jewellery.

Ans.

(i) Chromium and nickel.
(ii) Gold and platinum.

Ques. Give three reasons each to show that:

(i) sulphur is a non-metal, 
(ii) magnesium is a metal. Include one chemical equation.

Ans.

(i) Sulphur (non-metal):

• Dull and brittle (not shiny, breaks easily).
• Poor conductor of heat and electricity.
• Forms acidic oxide: S + O₂ → SO₂; SO₂ in water gives acidic solution.

(ii) Magnesium (metal):

• Shiny, malleable in thin ribbons.
• Good conductor of heat and electricity.
• Forms basic oxide: 2Mg + O₂ → 2MgO; MgO in water gives Mg(OH)₂ (basic).

Ques. What is cinnabar? How do we get the metal from it?

Ans. Cinnabar is mercury(II) sulphide, HgS. On roasting (heating in air):

HgS + O₂ → HgO + SO₂; then HgO → Hg + ½O₂ (on heating). The mercury is finally purified by distillation.

Ques.

(a) Draw electron-dot structures for K and Cl.
(b) Show how KCl forms by electron transfer.
(c) Name the ions present in KCl.

Ans.

(a) K: • (one valence dot); Cl: •• :Cl: •• (seven valence dots).
(b) K → K⁺ + e⁻; Cl + e⁻ → Cl⁻; so K⁺ and Cl⁻ attract to form KCl.
(c) Potassium ion (K⁺) and chloride ion (Cl⁻).

Ques. 

(a) Give electron-dot structures of Ca and S.
(b) Show the formation of CaS by electron transfer.
(c) Name the ions in CaS. (Ca = 20, S = 16)

Ans.

(a) Ca: •• (two valence electrons); S: six valence electrons.
(b) Ca → Ca²⁺ + 2e⁻; S + 2e⁻ → S²⁻; combine to form CaS.
(c) Calcium ion (Ca²⁺) and sulphide ion (S²⁻).

Do check: CBSE Class 10 Science Chapter 4 Carbon and its Compounds Important Questions

Ques.

(a) Give electron-dot diagrams for Cl (17) and Ca (20). Show formation of CaCl₂.
(b) State the nature of the compound and three physical properties.

Ans.

(a) Ca has 2 valence electrons; each Cl has 7. Ca → Ca²⁺ + 2e⁻; two Cl atoms each gain one electron: 2Cl + 2e⁻ → 2Cl⁻. Ions combine to give CaCl₂.
(b) Ionic compound. Properties: hard, high melting/boiling points, soluble in water; molten/aqueous solutions conduct electricity.

Ques. You have sodium, magnesium and copper. Suggest two tests to arrange them in decreasing reactivity.

Ans.

Test 1: Reaction with water – Sodium reacts vigorously with cold water; magnesium reacts only with hot water; copper does not react.
Test 2: Displacement from salt – Mg displaces Cu from CuSO₄; Cu cannot displace Mg from MgSO₄. Order: Na > Mg > Cu.

Ques. Using magnesium ribbon and sulphur powder, show that metal oxides are basic and non-metal oxides are acidic.

Ans.

Burn Mg → MgO; dissolve in water → turns red litmus blue (basic).
Burn S → SO₂; dissolve in water → turns blue litmus red (acidic). Conclusion: most metal oxides are basic, non-metal oxides are acidic.

Ques. 

(a) An ore gives brisk effervescence with dilute HCl. What type is it? Outline steps to get the metal from the enriched ore.
(b) A copper coin is dipped in AgNO₃ solution. What changes occur? Give the equation.

Ans.

(a) Carbonate ore (CO₂ bubbles). Steps: Calcination (MCO₃ → MO + CO₂), then reduction of MO to metal (e.g., with C/CO), followed by refining if needed.
(b) Copper displaces silver: Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s). Coin gets silver coating; solution turns blue (Cu²⁺).

Ques. Why are (a) school bells made of metal, (b) electric wires made of copper?

Ans.

(a) Metals are sonorous—they ring when struck.
(b) Copper is a very good conductor and ductile, so it’s ideal for wires.

Ques. Suggest a reduction method for extracting:

(i) a low-reactivity metal, 
(ii) a very highly reactive metal, (iii) a middle-reactivity metal.

Ans.

(i) Chemical reduction using C/CO.
(ii) Electrolytic reduction (electrolysis of molten salt).
(iii) Aluminothermic/chemical reduction (e.g., with Al/CO).

Do check: CBSE Class 10 Science Important Questions

Ques. 

(a) Define activity series. Arrange Au, Cu, Fe, Mg in increasing reactivity.
(b) What happens when:
(i) Zn pieces are put in CuSO₄, (ii) Ag pieces are put in FeSO₄?

Ans.

(a) The activity series lists metals from most to least reactive. Order: Au < Cu < Fe < Mg.
(b) (i) Zn displaces Cu: Zn + CuSO₄ → ZnSO₄ + Cu; blue solution fades, brown Cu deposits.
(ii) No reaction (Ag is less reactive than Fe).

Ques. A copper plate left in a bathroom for a week turns green. What is the green substance?

Ans. Basic copper carbonate, CuCO₃·Cu(OH)₂, formed by reaction with moist air and CO₂.

Ques. Name: (a) a metal kept under kerosene, (b) a lustrous coloured non-metal, (c) a metal that melts on the palm, (d) a metal that’s a poor heat conductor.

Ans. (a) Sodium, (b) Iodine, (c) Gallium, (d) Lead.

Ques. Why does calcium float on water? Write the equation. Name one more metal that soon floats in water.

Ans. H₂ bubbles stick to calcium, making it float.

Ca + 2H₂O → Ca(OH)₂ + H₂↑

Magnesium (with hot water) also floats due to H₂ bubbles.

Ques.

(a) Why is aluminium oxide amphoteric?
(b) Why do ionic compounds conduct only when molten or in solution?

Ans.

(a) Al₂O₃ reacts with acids and bases to give salts and water.
(b) Ions are free to move only in molten/aqueous states, so they can carry electric current.

Ques.

(a) Show ionic bonding in CaO with dot structures (Ca: 20, O: 8).
(b) Name the metals in bronze.

Ans.

(a) Ca → Ca²⁺ + 2e⁻; O + 2e⁻ → O²⁻; Ca²⁺ and O²⁻ form CaO.
(b) Copper and tin.

Ques. A metal X turns green in air.

(i) Identify X and the process.
(ii) Name and formula of the green layer.
(iii) Two ways to prevent it.

Ans.

(i) Copper; corrosion.
(ii) Basic copper carbonate, CuCO₃·Cu(OH)₂.
(iii) Coating (paint/tin), or alloying (e.g., bronze/brass).

Ques. Write balanced equations for:

(i) Al heated in air—name product.
(ii) Fe with steam—name product.
(iii) Ca with water—why does Ca float?

Ans.

(i) 4Al + 3O₂ → 2Al₂O₃ (aluminium oxide).
(ii) 3Fe + 4H₂O(g) → Fe₃O₄ + 4H₂ (magnetite).
(iii) Ca + 2H₂O → Ca(OH)₂ + H₂; H₂ bubbles stick, so it floats.

Ques. Balanced equations:

(a) Dil. H₂SO₄ with Al powder.
(b) Dil. HCl with Na₂CO₃.
(c) CO₂ through limewater.

Ans.

(a) 2Al + 3H₂SO₄(dil.) → Al₂(SO₄)₃ + 3H₂
(b) 2HCl + Na₂CO₃ → 2NaCl + H₂O + CO₂
(c) CO₂ + Ca(OH)₂ → CaCO₃↓ + H₂O; excess CO₂: CaCO₃ + CO₂ + H₂O → Ca(HCO₃)₂

Do check: CBSE Class 10 Science Syllabus

Ques. What is rusting? Describe an activity to show conditions needed.

Ans. Rusting is formation of hydrated iron(III) oxide on iron in air and moisture.

Activity with three test tubes:

A: iron + air + water → rusts;

B: iron + boiled water + oil layer (no air) → no rust;

C: iron + dry air + desiccant (no water) → no rust. Conclusion: needs both air and water.

Ques. 

(a) Show electron transfer in forming Na₂O.
(b) Why are ionic compounds hard?
(c) Why don’t solids conduct but melts do?

Ans.

(a) 2Na → 2Na⁺ + 2e⁻; O + 2e⁻ → O²⁻; gives Na₂O.
(b) Strong electrostatic forces lock ions in place → hard.
(c) In solids ions are fixed; in molten state ions are free, so they conduct.

Ques. 

(a) Show electron transfer in forming MgO. Write the ions present.
(b) Name a common solvent for ionic compounds.
(c) Why do their aqueous solutions conduct?

Ans.

(a) Mg → Mg²⁺ + 2e⁻; O + 2e⁻ → O²⁻; ions: Mg²⁺, O²⁻.
(b) Water.
(c) Free ions in solution carry charge.

Ques. What are amphoteric oxides? Pick them from: Na₂O, ZnO, Al₂O₃, CO₂, H₂O.

Ans. Oxides that react with both acids and bases. From the list: ZnO and Al₂O₃.

Ques. Define: (i) mineral, (ii) ore, (iii) gangue.

Ans.

(i) Mineral: natural substance containing a metal or its compound.
(ii) Ore: a mineral rich enough to extract the metal profitably.
(iii) Gangue: the unwanted rocky material mixed with the ore.

Ques. 

(a) Name the coatings formed on silver and copper in moist air.
(b) What is galvanisation and why is it done?
(c) Define alloy, how made, and how small amounts of (i) carbon, (ii) Ni + Cr affect iron.

Ans.

(a) Ag₂S (black), and CuCO₃·Cu(OH)₂ (green).(b) Galvanisation: coating zinc on iron to prevent rusting.
(c) Alloy: homogeneous mix of metals (sometimes with a non-metal), made by melting and mixing.
(i) A little carbon increases steel’s hardness/strength.
(ii) Ni + Cr with iron make stainless steel (tough, corrosion-resistant).

Ques. Differentiate roasting and calcination with equations. How is Zn extracted? Name two metals that can reduce metal oxides.

Ans.

Roasting: heating sulphide ores in air: 2ZnS + 3O₂ → 2ZnO + 2SO₂.
Calcination: heating carbonate/hydrated ores without air: ZnCO₃ → ZnO + CO₂.
Zinc: concentrate → roast/calcine to ZnO → reduce (e.g., with C/CO) → refine.
Reducers: Aluminium, magnesium (also carbon/CO).

Do check: CBSE Class 10 Science Notes

Ques.

(a) Atom A loses 2e⁻; atom B gains 1e⁻.
(i) What bond forms? (ii) Formula?
(b) Explain MgCl₂ formation similarly.
(c) Why does NaCl conduct only when molten?
(d) Why is NaCl’s melting point high?

Ans.

(a) (i) Ionic bond. (ii) A²⁺ with two B⁻ → AB₂.
(b) Mg²⁺ + 2Cl⁻ → MgCl₂ by electron transfer.
(c) Ions are mobile only when molten/aqueous.
(d) Strong ionic forces need high energy to break.

Ques.

(a) Why can’t carbon reduce MgO?
(b) How is Na obtained from molten NaCl?
(c) How is copper obtained from sulphide ore?

Ans.

(a) Magnesium is more reactive than carbon; MgO is too stable.
(b) Electrolysis of molten NaCl: Na⁺ + e⁻ → Na (cathode); Cl₂ at anode.
(c) Roast Cu₂S → Cu₂O + SO₂; then reduce (self-reduction): Cu₂O + Cu₂S → 4Cu + SO₂; refine electrolytically.

Ques. Why are highly reactive metals extracted differently from mid-reactive ones? Explain sodium extraction.

Ans.

Highly reactive metals form very stable compounds, so they need electrolysis. Mid-reactive metals can be chemically reduced.

Sodium: electrolysis of molten NaCl → Na (cathode) and Cl₂ (anode).

Ques. Name two most reactive metals. Show with an electron diagram how one reacts with a halogen, and list four properties of the compound.

Ans. Potassium (K) and sodium (Na). Example: Na → Na⁺ + e⁻; Cl + e⁻ → Cl⁻; forms NaCl. Properties: high melting point, water-soluble, conducts when molten/aqueous, hard/solid.

Ques. A very good conductor used for wires occurs as sulphide M₂S.

(i) Identify M.
(ii) How is it extracted? Give equations.
(iii) Outline electrolytic refining.

Ans.

(i) Copper.
(ii) Concentrate Cu₂S by froth flotation; roast: 2Cu₂S + 3O₂ → 2Cu₂O + 2SO₂; then self-reduction: Cu₂O + Cu₂S → 4Cu + SO₂.
(iii) Electrorefining: impure Cu anode, pure Cu cathode, CuSO₄ solution; Cu dissolves at anode and plates on cathode; anode mud remains.

Ques. Explain:

(i) Silver and copper lose shine in air—name the compounds formed.
(ii) Tamarind cleans tarnished copper.
(iii) Al corrodes less than Fe though more reactive.

Ans.

(i) Ag₂S on silver; basic copper carbonate on copper.
(ii) Tamarind’s acids dissolve basic copper carbonate.
(iii) Al forms a thin, protective Al₂O₃ layer (passivation).

Ques.

(a) Electron-dot structures of Na, O, Mg.
(b) Show formation of Na₂O and MgO; name ions.
(c) Give three properties of ionic compounds.

Ans.

(a) Na• , ••O•• with six dots needing two e⁻, Mg••.
(b) 2Na⁺ + O²⁻ → Na₂O; Mg²⁺ + O²⁻ → MgO. Ions: Na⁺, O²⁻, Mg²⁺.
(c) High melting points, water-soluble, conduct when molten/aqueous.

Ques. What are alloys? How are they made? Give make-up and uses of brass, bronze, solder.

Ans. Alloys are uniform mixtures of metals (sometimes with a non-metal), made by melting and mixing.

• Brass: Cu + Zn — decorative items, hardware.
• Bronze: Cu + Sn — statues, medals, bearings.
• Solder: Pb + Sn — joins wires (low melting point).

Do check: CBSE Class 10 Science Sample Papers

Ques. A metal E is stored under kerosene. A small piece catches fire in air; its product in water turns red litmus blue.

(i) Name E.
(ii) Give equations in air and with water.
(iii) How is E obtained from its molten chloride

Ans.

(i) Sodium.
(ii) In air (overall): 4Na + O₂ → 2Na₂O (also forms Na₂O₂); with water: 2Na + 2H₂O → 2NaOH + H₂.
(iii) Electrolysis of molten NaCl.

Ques. Give two differences between calcination and roasting.

Ans.

• Calcination: heat without air; used for carbonates/hydrated ores; e.g., ZnCO₃ → ZnO + CO₂.
• Roasting: heat in air; used for sulphide ores; e.g., 2ZnS + 3O₂ → 2ZnO + 2SO₂.

Ques. A non-metal X has two forms Y and Z. Y is the hardest natural substance; Z conducts electricity. Identify X, Y, Z.

Ans. X = carbon; Y = diamond; Z = graphite.

Ques. Why does calcium float on water?

Ans. Hydrogen bubbles cling to the metal, reducing density so it floats.

Ques. Name a lustrous non-metal and a non-lustrous metal.

Ans. Iodine (lustrous non-metal); lead (dull metal).

Ques. Which gas is released when a metal reacts with an acid? How do you test it?

Ans. Hydrogen. Bring a burning splint near the gas—‘pop’ sound confirms H₂.

Ques. Name a metal that gives hydrogen with very dilute HNO₃.

Ans. Magnesium (nitric acid is usually oxidising, but very dilute can give H₂ with Mg).

Ques. Name two metals found free in nature.

Ans. Gold and silver.

Ques. Do reactions of Na, Mg, Fe with air/water reflect their order in the reactivity series? Explain.

Ans. Yes. Na reacts violently even with cold water (most reactive). Mg needs hot water/steam. Fe reacts only with steam. Thus Na > Mg > Fe.

Ques. X + YSO₄ → XSO₄ + Y; but Y + XSO₄ → no reaction. Which is more reactive?

Ans. X is more reactive—it displaces Y from YSO₄; Y cannot displace X.

Ques. What is an alloy? What is solder made of, and why is it used for electrical wiring?

Ans. Alloy: homogeneous metal mixture. Solder = Pb + Sn; it has a low melting point, so it’s ideal for joining wires.

Ques. Using electronic configurations, explain how Mg combines with O to form MgO.

Ans. Mg (2,8,2) loses 2e⁻ → Mg²⁺; O (2,6) gains 2e⁻ → O²⁻; ions attract → MgO.

Ques. A metal X with cold water gives a base Y of formula XOH (Mᵣ = 40) and gas Z that catches fire. Identify X, Y, Z.

Ans. X = Na (≈23, but XOH Mᵣ=40 fits KOH; however K reacts even more vigorously). Since gas Z burns (H₂), the intended set is: X = K (39), Y = KOH (40), Z = H₂.

Ques. Write equations showing Al₂O₃ reacts with both acid and base.

Ans.

With acid: Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O
With base: Al₂O₃ + 2NaOH + 3H₂O → 2Na[Al(OH)₄]

Ques.

(a) Name the main ore of Hg and its extraction with equation.
(b) What is the thermite reaction? Use in welding.
(c) Name the method for extracting highly reactive metals.

Ans.

(a) Cinnabar (HgS); roast: HgS + O₂ → HgO + SO₂; then HgO → Hg + ½O₂.
(b) Aluminothermy: Fe₂O₃ + 2Al → 2Fe(l) + Al₂O₃ + heat; molten Fe welds rails/parts.
(c) Electrolytic reduction.

Do check: NCERT Solutions for Class 10 Science

Ques.

(a) How are metals at the top of the reactivity series extracted? Example.
(b) One alloy of (i) metal + non-metal, (ii) two metals.

Ans.

(a) By electrolysis; e.g., Al from bauxite (as Al₂O₃) via molten electrolysis.
(b) (i) Steel (Fe + C), (ii) Brass (Cu + Zn).

Ques. 

(a) Two ways to prevent rusting.
(b) Ores of (i) Hg, (ii) Zn.
(c) Explain electrolytic refining of copper with a labeled setup description.

Ans.

(a) Painting/greasing, galvanising (Zn coat).
(b) (i) Cinnabar (HgS), (ii) Zinc blende (ZnS).
(c) Anode: impure Cu; Cathode: pure Cu; Electrolyte: CuSO₄ + H₂SO₄. Pass current: Cu dissolves at anode (Cu → Cu²⁺ + 2e⁻), plates at cathode (Cu²⁺ + 2e⁻ → Cu). Impurities drop as anode mud.

Ques. How do ionic compounds form? State three general properties.

Ans. Electron transfer from metal to non-metal makes ions that attract. Properties: high melting point, water-soluble, conduct when molten/aqueous.

Ques.

(a) Explain extraction by reduction for a low-reactivity metal X and a high-reactivity metal Y.
(b) Show NaCl formation by electron transfer.
(c) Two observations when a very reactive metal is dropped into water.

Ans.

(a) X: chemical reduction (C/CO/Al). Y: electrolysis.
(b) Na → Na⁺ + e⁻; Cl + e⁻ → Cl⁻; → NaCl.
(c) Vigorous reaction/flame, alkaline solution formed (turns red litmus blue), H₂ evolved.

Ques. 

(a) A metal X reduces Fe₂O₃ very exothermically and itself is obtained by electrolysis. Identify X and write the reaction.
(b) Justify that Al₂O₃ is amphoteric; give another amphoteric oxide.
(c) Name the metals in bronze.

Ans.

(a) Aluminium: Fe₂O₃ + 2Al → 2Fe + Al₂O₃ + heat.
(b) Al₂O₃ reacts with acids and bases; another: ZnO.
(c) Copper and tin.

Ques. Valency of silicon (Z = 14)?

Ans. 4.

Ques. Valency of phosphorus (Z = 15)?

Ans. Commonly 3 (also 5 in some compounds).

Ques. Valency of element with Z = 35 (bromine)?

Ans. 1 (forms Br⁻).

Ques. Mg (group 2, Z=12) and O (group 16, Z=8): draw configurations and show ionic bond.

Ans. Mg: 2,8,2 → Mg²⁺; O: 2,6 → O²⁻; attraction gives MgO.

Ques. Solids A and B don’t react cold; on heating, an exothermic reaction gives a liquid metal C and a solid D floating on it; used for on-site welding. Identify and write balanced equation with states and heat mention. Name two reaction types.

Ans. A = Al, B = Fe₂O₃, C = Fe(l), D = Al₂O₃(s).
Equation: Fe₂O₃(s) + 2Al(s) → 2Fe(l) + Al₂O₃(s) + heat (thermite).
Types: Displacement and redox.

Ques. Arrange in decreasing reactivity: Na, K, Cu, Ag.

Ans. K > Na > Cu > Ag.

Ques. An ore gives SO₂ when heated in air. Which concentration method is used? Briefly describe two steps to get the metal.

Ans. It’s a sulphide ore → use froth flotation. Steps: Roasting (MS + O₂ → MO + SO₂) then reduction (MO → M) with C/CO/Al.

Ques. Explain:

(i) Ionic compounds have high melting/boiling points.
(ii) Very reactive metals can’t be reduced by carbon.
(iii) Copper turns green in rainy season.

Ans.

(i) Strong ionic forces need much heat to break.
(ii) Their oxides are too stable; the metals are strong reducers.
(iii) Forms basic copper carbonate in moist CO₂ air.

Ques. Reasons:

(i) Shiny metals become dull in air over time.
(ii) Zn doesn’t give H₂ with dilute HNO₃.
(iii) Metal sulphides are in rocks; metal halides in sea water.

Ans.

(i) Surface compounds form (corrosion/tarnish).
(ii) Dilute HNO₃ is an oxidising agent; it forms NO/NO₂, not H₂.
(iii) Chloride-rich seas favour halides; sulphur occurs in the crust, so sulphides form in rocks.

Ques. Reasons:

(i) Wires are insulated with rubber.
(ii) Zn gives H₂ with dil. HCl but Cu doesn’t.
(iii) Sulphide ores are first converted to oxides.

Ans.

(i) Rubber is an insulator.
(ii) Zn is above H in the series; Cu is below.
(iii) Oxides are easier to reduce than sulphides.

Ques. 

(a) Define corrosion and give two prevention methods.
(b) For a mid-reactivity metal M from a sulphide ore: list extraction steps.

Ans.

(a) Corrosion: slow damage of metals by environment; prevention: galvanising, painting/electroplating, alloying.
(b) Concentration (froth flotation) → Roasting to MO → Reduction (MO + C/CO → M) → Refining (e.g., electrolytic).

Ques. 

(a) Distinguish ionic vs covalent compounds in:
(i) force strength, (ii) water solubility, (iii) electrical conduction.
(b) Reduction methods for:
(i) a mid-reactivity metal M,
(ii) a high-reactivity metal N. Give one example each.

Ans.

(a) Ionic: very strong forces, usually water-soluble, conduct when molten/aqueous. Covalent: weaker intermolecular forces, often water-insoluble, do not conduct (except some like graphite/acids).
(b) (i) Chemical reduction (e.g., MnO₂ + 4Al → 3Mn + 2Al₂O₃ or with C/CO).
(ii) Electrolysis (e.g., Al from Al₂O₃; Na from molten NaCl).