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NCERT Class 10 Science — Chapter 3

Metals and Non-Metals

Physical & chemical properties of metals/non-metals, Reactivity Series, ionic bonding (electron transfer in NaCl,MgCl2\text{NaCl}, \text{MgCl}_2), metallurgy (roasting, calcination, electrolytic refining), and alloy composition.

Quick Key Takeaways:
Reactivity Series (Decreasing order): K>Na>Ca>Mg>Al>Zn>Fe>Pb>[H]>Cu>Hg>Ag>Au\text{K} > \text{Na} > \text{Ca} > \text{Mg} > \text{Al} > \text{Zn} > \text{Fe} > \text{Pb} > [\text{H}] > \text{Cu} > \text{Hg} > \text{Ag} > \text{Au}.
Ionic Compounds Properties: Formed by complete electron transfer from metal to non-metal. Characteristics: High melting/boiling points (strong electrostatic attraction), brittle solids, soluble in water, conduct electricity in molten or aqueous state (not in solid state).
Metallurgy Principles: Low reactivity metals extracted by heating alone (Cinnabar HgS\text{HgS}); Medium reactivity metals converted to oxides via Calcination (absence of air, carbonate ores) or Roasting (excess air, sulphide ores), followed by Carbon/Al reduction; High reactivity metals extracted by Electrolytic Reduction of molten chlorides.
Alloys & Anodising: Brass (Cu+Zn\text{Cu} + \text{Zn}), Bronze (Cu+Sn\text{Cu} + \text{Sn}), Solder (Pb+Sn\text{Pb} + \text{Sn} - low melting point), Stainless Steel (Fe+Ni+Cr+C\text{Fe} + \text{Ni} + \text{Cr} + \text{C}).
Chemistry Equation & Reaction HelperInspect amphoteric oxide, metal-steam, thermite, and roasting reactions
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Jump to Concept:1. 1. Physical/Chemical Properties, Ionic Bonding & The Reactivity Series2. 2. Metallurgy: Extraction of Metals & Electrolytic Refining3. 3. High-Yield Solved Board Examination Questions (3-Mark & 5-Mark)4. 4. Practical Laboratory & Competency-Based Case Drill: Rusting of Iron: Three-Test-Tube Experiment (NCERT Activity 3.14)5. 5. CBSE Examiner Marking Scheme, Scientific Notation & Deduction Traps
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1. Physical/Chemical Properties, Ionic Bonding & The Reactivity Series

Fundamental Principles

Core scientific laws, chemical equations, anatomical structures, and visual model for Metals and Non-Metals.

• Chemical Properties of Metals
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Reaction with Oxygen: Form basic or amphoteric oxides.
- Basic Oxides: 4Na+O2→2Na2O4\text{Na} + \text{O}_2 \rightarrow 2\text{Na}_2\text{O} (dissolves in water to form alkali NaOH\text{NaOH}).
- Amphoteric Oxides (react with both acids and bases to yield salt and water):
Al2O3+6HCl⟶2AlCl3+3H2O\text{Al}_2\text{O}_3 + 6\text{HCl} \longrightarrow 2\text{AlCl}_3 + 3\text{H}_2\text{O}
Al2O3+2NaOH⟶2NaAlO2 (Sodium Aluminate)+H2O\text{Al}_2\text{O}_3 + 2\text{NaOH} \longrightarrow 2\text{NaAlO}_2 \text{ (Sodium Aluminate)} + \text{H}_2\text{O}
•
Reaction with Water:
- Highly reactive (K,Na\text{K}, \text{Na}): React violently with cold water, evolving H2\text{H}_2 that catches fire.
- Medium reactive (Mg\text{Mg}): Reacts with hot water; Al,Fe,Zn\text{Al}, \text{Fe}, \text{Zn} react only with steam:
3Fe(s)+4H2O(g)⟶Fe3O4(s)+4H2(g)↑3\text{Fe}(s) + 4\text{H}_2\text{O}(g) \longrightarrow \text{Fe}_3\text{O}_4(s) + 4\text{H}_2(g)\uparrow
•
Reaction with Nitric Acid (HNO3\text{HNO}_3): Does not typically evolve H2\text{H}_2 because HNO3\text{HNO}_3 is a strong oxidizing agent that oxidizes H2\text{H}_2 to H2O\text{H}_2\text{O}. (Only Magnesium Mg\text{Mg} and Manganese Mn\text{Mn} react with very dilute HNO3\text{HNO}_3 to liberate H2\text{H}_2).
• Electron Dot Structure & Formation of Ionic Compounds
•
Formation of MgCl2\text{MgCl}_2:
- Magnesium atom (Z=12:2,8,2Z=12: 2,8,2): Mg⟶Mg2++2e−\text{Mg} \longrightarrow \text{Mg}^{2+} + 2e^-
- Two Chlorine atoms (Z=17:2,8,7Z=17: 2,8,7): 2Cl+2e−⟶2Cl−2\text{Cl} + 2e^- \longrightarrow 2\text{Cl}^-
- Electrostatic combination: [Mg]2+[:Cl¨:−]2[\text{Mg}]^{2+} [:\ddot{\text{Cl}}:^-]_2
📊 Metals & Metallurgy: Reactivity Hierarchy & Electrolytic RefiningVisual Model
HIGHLY REACTIVEK > Na > Ca > Mg > AlMODERATE (Carbon Red.)Zn > Fe > Pb > [H]LEAST REACTIVE (Native)Cu > Hg > Ag > AuReactivity Decreases ↓METALLURGICAL EXTRACTION1. Top (K, Na, Ca, Mg, Al):Electrolytic reduction of molten chlorides/oxides.2. Middle (Zn, Fe, Pb):Roasting (Sulphide) / Calcination (Carbonate) + C.3. Bottom (Ag, Au):Found in native free state (refining only).

Visual schematic mapping the metal reactivity series, extraction metallurgical protocols (roasting/calcination), and the electrolytic copper refining cell.

2

2. Metallurgy: Extraction of Metals & Electrolytic Refining

Mechanisms & Experiments

Step-by-step chemical reaction mechanisms, experimental activities, and physiological pathways for Metals and Non-Metals.

• Thermodynamics & Ore Extraction Pathways
•
1. Low Reactivity Metals (e.g. Mercury from Cinnabar HgS\text{HgS}):
2HgS+3O2→Δ2HgO+2SO22\text{HgS} + 3\text{O}_2 \xrightarrow{\Delta} 2\text{HgO} + 2\text{SO}_2
2HgO→Δ2Hg(l)+O2(g)2\text{HgO} \xrightarrow{\Delta} 2\text{Hg}(l) + \text{O}_2(g)
•
2. Medium Reactivity Metals (e.g. Zinc from Blende or Calamine):
- Roasting (Sulphide Ore): 2ZnS+3O2→Δ2ZnO+2SO2↑2\text{ZnS} + 3\text{O}_2 \xrightarrow{\Delta} 2\text{ZnO} + 2\text{SO}_2\uparrow
- Calcination (Carbonate Ore): ZnCO3→ΔZnO+CO2↑\text{ZnCO}_3 \xrightarrow{\Delta} \text{ZnO} + \text{CO}_2\uparrow
- Reduction with Carbon: ZnO+C⟶Zn+CO\text{ZnO} + \text{C} \longrightarrow \text{Zn} + \text{CO}
•
Thermite Process (Welding Railway Tracks):
Fe2O3(s)+2Al(s)⟶2Fe(l)+Al2O3(s)+Enormous Heat\text{Fe}_2\text{O}_3(s) + 2\text{Al}(s) \longrightarrow 2\text{Fe}(l) + \text{Al}_2\text{O}_3(s) + \text{Enormous Heat}
(Molten iron flows into cracked railway track gaps).
•
Electrolytic Refining of Copper:
- Anode: Thick block of impure copper (Cu→Cu2++2e−\text{Cu} \rightarrow \text{Cu}^{2+} + 2e^-).
- Cathode: Thin strip of pure copper (Cu2++2e−→Cu\text{Cu}^{2+} + 2e^- \rightarrow \text{Cu}).
- Electrolyte: Acidified CuSO4\text{CuSO}_4 solution.
- Anode Mud: Insoluble impurities (gold, silver, platinum) settle below anode.
3

3. High-Yield Solved Board Examination Questions (3-Mark & 5-Mark)

Solved Board Questions

Standard CBSE board exam questions with complete scientific justifications and marking scheme step protocols.

• 3-Mark Standard Board Question: Differentiate between Roasting and Calcination with balanced chemical equations for zinc extraction.
•
1. Roasting:
- Definition: Heating of sulphide ore in the excess presence of air/oxygen below its melting point.
- Gas Evolved: Sulphur dioxide gas (SO2\text{SO}_2).
- Equation: 2ZnS(s) (Zinc Blende)+3O2(g)→Δ2ZnO(s)+2SO2(g)↑2\text{ZnS}(s) \text{ (Zinc Blende)} + 3\text{O}_2(g) \xrightarrow{\Delta} 2\text{ZnO}(s) + 2\text{SO}_2(g)\uparrow
•
2. Calcination:
- Definition: Heating of carbonate or hydrated ore in the absence or limited supply of air below its melting point.
- Gas Evolved: Carbon dioxide gas (CO2\text{CO}_2).
- Equation: ZnCO3(s) (Calamine)→ΔZnO(s)+CO2(g)↑\text{ZnCO}_3(s) \text{ (Calamine)} \xrightarrow{\Delta} \text{ZnO}(s) + \text{CO}_2(g)\uparrow
•
Common Goal: Both processes convert the concentrated ore into metal oxide (ZnO\text{ZnO}), which is much easier to reduce to free metal than sulphides or carbonates.
• 5-Mark Comprehensive Question / Numerical: (a) Show the formation of Magnesium Oxide (MgO\text{MgO}) by electron transfer.
(b) Explain four general physical properties of ionic compounds.
•
Part (a) Formation of MgO\text{MgO}:
- Mg\text{Mg} (2,8,22, 8, 2): Mg⟶Mg2++2e−\text{Mg} \longrightarrow \text{Mg}^{2+} + 2e^-
- O\text{O} (2,62, 6): O+2e−⟶O2−\text{O} + 2e^- \longrightarrow \text{O}^{2-}
- Electron Transfer Diagram: Mg∙∙+:O¨:⟶[Mg]2+[:O¨:]2−\text{Mg}^{\bullet\bullet} + \mathbf{:}\ddot{\text{O}}\mathbf{:} \longrightarrow [\text{Mg}]^{2+}[\mathbf{:}\ddot{\text{O}}\mathbf{:}]^{2-}
•
Part (b) Four Physical Properties of Ionic Compounds:
1. Physical Nature: Hard, crystalline, and brittle solids due to strong electrostatic forces of attraction between oppositely charged ions.
2. High Melting & Boiling Points: Considerable thermal energy is required to overcome the strong inter-ionic bonds (e.g. NaCl\text{NaCl} melting point is 10741074 K).
3. Solubility: Highly soluble in polar solvents like water; insoluble in non-polar organic solvents like kerosene and petrol.
4. Electrical Conductivity: Do not conduct electricity in solid state (ions locked in fixed crystal lattice); conduct electricity in molten or aqueous state due to mobile free ions.
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4. Practical Laboratory & Competency-Based Case Drill: Rusting of Iron: Three-Test-Tube Experiment (NCERT Activity 3.14)

Practical & Case Drill

Experimental observation analysis, chemical gas tests, and assertion-reason drills.

• Laboratory Activity Context: Rusting of Iron: Three-Test-Tube Experiment (NCERT Activity 3.14)
Three clean iron nails are placed in three test tubes: Tube A (water + air), Tube B (boiled distilled water + layer of oil to exclude air), Tube C (dry air with anhydrous calcium chloride).
•
Q1: In which test tube(s) do the nails rust after several days? →\rightarrow Nails rust only in Tube A.
•
Q2: Why do nails in Tube B not rust? →\rightarrow Boiled distilled water expels dissolved oxygen, and the oil layer prevents atmospheric oxygen from dissolving. Iron cannot rust in the absence of oxygen.
•
Q3: What is the role of anhydrous calcium chloride in Tube C? →\rightarrow It acts as a drying/desiccating agent that absorbs all moisture from the air. Iron cannot rust in the absence of water/moisture.
•
Conclusion: Rusting of iron strictly requires both oxygen and moisture simultaneously.
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5. CBSE Examiner Marking Scheme, Scientific Notation & Deduction Traps

Important Solved Board Questions

Examiner step-marking allocations, mandatory scientific terminology, and common error avoidance.

• Step-by-Step Marking Rubric & Key Terminology
•
1 Mark: Correct electron dot configuration showing electron transfer arrows.
•
1 Mark: Balanced equation for amphoteric oxide reactions with acid and base.
•
2 Marks: Accurate description of roasting vs calcination with equations.
•
1 Mark: Correctly identifying anode, cathode, electrolyte, and anode mud in copper refining.
• Common Error Deduction Traps
•
Trap 1: Writing that ionic compounds conduct electricity in solid state (strictly molten or aqueous only).
•
Trap 2: Confusing the reducing agent in thermite welding (Aluminium Al\text{Al} is the reducing agent; Fe2O3\text{Fe}_2\text{O}_3 is reduced).
•
Trap 3: Forgetting to specify 'absence of air' for calcination and 'excess air' for roasting.
Authentic Board Question (3 Marks)Topic: Metals and Non-Metals Chemical Equations & Reaction Mechanisms
Explain the fundamental chemical principles, write the balanced chemical equations with state symbols, and describe the observable phenomena for Metals and Non-Metals.

Official CBSE Step-by-Step Marking Breakdown:

Step 1: Balanced Chemical Equation with State Symbols: Write the stoichiometrically balanced chemical equation including state symbols (s,l,g,aq)(s, l, g, aq) for all reactants and products.
1 Mark
Step 2: Observable Physical Changes & Test Confirmation: State key observable indicators: color changes, gas evolution with confirmation test (pop sound/lime water), precipitate formation, or temperature changes.
1 Mark
Step 3: Chemical Reasoning & Mechanism: Explain the underlying chemical mechanism (neutralisation, displacement, redox electron transfer, or functional group properties).
1 Mark
Model Student Answer (Target: Full 3/3 Marks):
To score full 3 marks on Metals and Non-Metals in CBSE Science (Chemistry):

1. Balanced Chemical Equation: State the exact equation with mandatory physical states:
Reactant1(s)+Reactant2(aq)⟶Product1(aq)+Product2(g)\text{Reactant}_1(s) + \text{Reactant}_2(aq) \longrightarrow \text{Product}_1(aq) + \text{Product}_2(g)
2. Observable Phenomena: State the exact visual observation (e.g., brisk effervescence, blue to green color shift, white precipitate).
3. Chemical Logic: Explain the underlying ionic dissociation, reactivity series order, or pH shift that drives the reaction.
Examiner Mark Deduction Traps:
•Always include physical state symbols (s),(l),(g),(aq)(s), (l), (g), (aq) in chemical equations to prevent deduction of ½ mark.
•Name specific indicator color changes (e.g. blue litmus to red, pink phenolphthalein turning colorless).

High-Frequency Conceptual Doubts & FAQs

Curated answers to the most common questions asked by Class 10 students.
Sodium is an alkali metal that reacts vigorously with atmospheric oxygen and moisture even at room temperature, catching fire and producing explosive hydrogen gas. Hence, it is stored in kerosene. Non-metal White Phosphorus reacts with atmospheric air to ignite spontaneously, but does not react with water, so it is stored under water.

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