ICSE Chemistry 2026 Prediction Paper — Free Download with Answers & Topic Analysis

Why This Prediction Paper?

At Bright Tutorials, our expert teachers have analyzed 10+ years of ICSE Chemistry board exam patterns to identify the most frequently tested topics, question styles, and mark distributions. This prediction paper is designed to:

• Maximize your score — every question targets high-probability topics
• Build exam confidence — practice under real exam conditions (80 marks, 2 hours)
• Save revision time — focus on what actually matters for 11 March 2026
• Provide complete solutions — detailed answers with step-by-step explanations

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SECTION A (40 Marks) — Attempt All Questions

Question 1 — Multiple Choice Questions [15 Marks]

(i) An element has atomic number 17. It belongs to:

• (a) Group 1, Period 3
• (b) Group 17, Period 3
• (c) Group 7, Period 3
• (d) Group 17, Period 2

(ii) Assertion (A): Carbon tetrachloride (CCl₄) does not conduct electricity.
Reason (R): CCl₄ is a covalent compound and does not form ions in solution.

• (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

(iii) The number of moles in 11.2 litres of nitrogen gas at STP is:

• (a) 1
• (b) 0.5
• (c) 2
• (d) 0.25

(iv) During the electrolysis of acidulated water, hydrogen is collected at the:

• (a) Anode by downward displacement of water
• (b) Cathode by downward displacement of water
• (c) Anode by upward displacement of air
• (d) Cathode by upward displacement of water

(v) The organic compound formed when ethanol reacts with excess concentrated sulphuric acid at 170°C is:

• (a) Ethane
• (b) Ethene
• (c) Ethoxyethane
• (d) Ethanoic acid

(vi) Which of the following is the correct order of increasing ionization potential?

• (a) Na < Mg < Al < Si
• (b) Si < Al < Mg < Na
• (c) Na < Al < Mg < Si
• (d) Al < Na < Mg < Si

(vii) A gas X turns moist lead acetate paper black. The gas X is:

• (a) SO₂
• (b) HCl
• (c) H₂S
• (d) NH₃

(viii) In the Contact Process, the catalyst used for the conversion of SO₂ to SO₃ is:

• (a) Finely divided iron
• (b) Platinum or Vanadium pentoxide (V₂O₅)
• (c) Manganese dioxide
• (d) Concentrated sulphuric acid

(ix) Which of the following compounds has a coordinate (dative) bond?

• (a) NaCl
• (b) H₂O
• (c) NH₄⁺
• (d) CH₄

(x) A solution has a pH of 12. Which of the following statements is correct?

• (a) It is a strong acid
• (b) It is a weak acid
• (c) It is a strong base
• (d) It will turn blue litmus red

(xi) The molecular formula of a compound with empirical formula CH₂O and vapour density 30 is:

• (a) CH₂O
• (b) C₂H₄O₂
• (c) C₃H₆O₃
• (d) C₄H₈O₄

(xii) During electrorefining of copper, the impure copper acts as:

• (a) Cathode
• (b) Anode
• (c) Electrolyte
• (d) External electrode

(xiii) Which of the following is not a property of ionic compounds?

• (a) High melting point
• (b) Conduct electricity in molten state
• (c) Soluble in organic solvents
• (d) Form crystals

(xiv) The next higher homologue of C₂H₅OH is:

• (a) CH₃OH
• (b) C₃H₇OH
• (c) C₃H₅OH
• (d) C₂H₃OH

(xv) An element X forms an oxide X₂O₃. The element X is most likely to be in:

• (a) Group 1
• (b) Group 2
• (c) Group 13
• (d) Group 16

Question 2

(i) The diagram below represents the electrolysis of copper sulphate solution using copper electrodes. Study the diagram and answer the following: [5]

[Diagram: Electrolytic cell with copper electrodes in CuSO₄ solution]

• (a) Write the reaction that takes place at the cathode.
• (b) Write the reaction that takes place at the anode.
• (c) What happens to the colour of the electrolyte during this process? Give a reason.
• (d) Name the ions that migrate towards the anode.
• (e) State one industrial application of this process.

(ii) Give one word or phrase for each of the following: [5]

• (a) The property of elements by which they tend to gain electrons.
• (b) A salt formed when the acid is partially neutralized by a base.
• (c) The process of heating an ore in the absence of air below its melting point.
• (d) A hydrocarbon containing a triple bond between two carbon atoms.
• (e) The tendency of an atom to attract shared pair of electrons towards itself.

(iii) Fill in the blanks: [5]

• (a) Metals generally have __________ ionization potential. (high / low)
• (b) When NaOH is added to FeCl₃ solution, a __________ precipitate is formed. (green / reddish-brown / white)
• (c) Alkenes are __________ hydrocarbons. (saturated / unsaturated)
• (d) In the Haber Process, N₂ and H₂ combine in the ratio __________. (1:2 / 1:3 / 2:3)
• (e) A cation is formed by the __________ of electrons. (gain / loss)

(iv) Match the following: [5]

Column A	Column B
(a) Calcination	(i) Used as a drying agent for HCl gas
(b) Concentrated sulphuric acid	(ii) Heating in absence of air
(c) Cryolite	(iii) Dehydrating agent
(d) Ethyne	(iv) Na₃AlF₆
(e) Silver nitrate	(v) Used to distinguish between dilute HCl and dilute H₂SO₄
	(vi) Contains a triple bond
	(vii) Barium chloride

(v) Write the IUPAC name for each of the following: [5]

• (a) CH₃—CH₂—CH₂—CHO
• (b) CH₃—CH(CH₃)—CH₂—CH₃
• (c) CH₃—CO—CH₃

Draw the structural formula for: (d) But-2-ene   (e) Propan-1-ol

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SECTION B (40 Marks) — Attempt Any Four

Question 3 [10 Marks]

(i) Study the periodic table excerpt and answer: [3]

Group →	1	2	13	14	15	16	17	18
Period 2	Li	Be	B	C	N	O	F	Ne
Period 3	Na	Mg	Al	Si	P	S	Cl	Ar

• (a) Which element in Period 3 has the highest electron affinity? Give a reason.
• (b) Compare the atomic radius of Na and Cl. Explain why.
• (c) Which element will form an ion with a charge of 2−? Write the electronic configuration of this ion.

(ii) Give balanced equations for: [3]

• (a) Laboratory preparation of ammonia gas using an ammonium salt.
• (b) Action of concentrated nitric acid on copper.
• (c) Action of concentrated sulphuric acid on carbon (as an oxidizing agent).

(iii) An element Z has atomic number 12. [4]

• (a) Write the electronic configuration of Z.
• (b) State the group and period to which Z belongs.
• (c) Is Z a metal or a non-metal?
• (d) Write the formula of the chloride of Z.
• (e) What type of bonding will be present in the chloride of Z? Draw the electron dot diagram.

Question 4 [10 Marks]

(i) State your observations when: [3]

• (a) Excess NaOH is added to CuSO₄ solution and the mixture is warmed.
• (b) Ammonium sulphate is heated with NaOH solution.
• (c) Concentrated sulphuric acid is added to sugar crystals.

(ii) Identify the acid from the list: [Dilute HCl, Dilute H₂SO₄, Conc. H₂SO₄, Dilute HNO₃, Conc. HNO₃] [3]

• (a) Produces white ppt with BaCl₂ solution, insoluble in dilute HCl.
• (b) Reacts with Cu to produce a blue solution and a colourless gas that turns brown in air.
• (c) Acts as a dehydrating agent on hydrated CuSO₄ crystals.

(iii) A salt is white, gives yellow residue when hot (white when cold), white ppt with NaOH (soluble in excess), white ppt with dilute HCl. Identify: [4]

• (a) The cation   (b) The anion   (c) The salt   (d) Equation for action of heat

Question 5 [10 Marks]

(i) KClO₃ decomposes: 2KClO₃ → 2KCl + 3O₂ (K=39, Cl=35.5, O=16) [4]

• (a) Mass of KClO₃ required for 6.72L O₂ at STP.
• (b) Moles of KCl produced.
• (c) Mass of residue left behind.

(ii) A compound: C=40%, H=6.67%, O=53.33%. Vapour density = 30. (C=12, H=1, O=16) [3]

• (a) Find the empirical formula.   (b) Find the molecular formula.

(iii) Complete combustion of 1L ethane: 2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O [3]

Calculate volume of O₂ required and CO₂ produced.

Question 6 [10 Marks]

(i) Balanced equations for conversions: [3]

• (a) Ethanol → Ethanoic acid   (b) Ethene → Ethanol   (c) Ethanoic acid → Ethyl ethanoate

(ii) Distinguish between using chemical tests: [4]

• (a) Ethanol and Ethanoic acid   (b) Methane and Ethene

(iii) Write structural formula and IUPAC name of: [3]

• (a) First member of alkynes   (b) Isomer of butane   (c) Alcohol with formula C₃H₈O

Question 7 [10 Marks]

(i) Extraction of aluminium from bauxite: [4]

• (a) Name the concentration process and write the equation.
• (b) Why is cryolite added?
• (c) Equation at the cathode.
• (d) Why must the carbon anode be replaced periodically?

(ii) Name the alloy: (a) Copper + Tin   (b) Aluminium alloy for aircraft. State one property each. [2]

(iii) Can the following pairs be distinguished by the given reagent? [4]

• (a) NaNO₃ and Zn(NO₃)₂ using NaOH
• (b) FeSO₄ and Fe₂(SO₄)₃ using NH₄OH
• (c) Dilute HCl and dilute H₂SO₄ using Pb(NO₃)₂
• (d) MnO₂ and FeCl₃ using conc. HCl

Question 8 [10 Marks]

(i) Draw a labelled diagram for the lab preparation of HCl gas. Write the balanced equation. [3]

(ii) Elements P(8), Q(11), R(13), S(17), T(20): [4]

• (a) Highest electronegativity?   (b) Which two form ionic bond? Formula?
• (c) Largest atomic radius? Why?   (d) Which forms amphoteric oxide?

(iii) Complete and balance: [3]

• (a) Fe₂O₃ + CO → ___ + ___
• (b) NaOH + Cl₂ → ___ + ___ + ___
• (c) C₂H₅OH + Na → ___ + ___

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Complete Answer Key & Explanations

Question 2 — Answers

(i) Electrolysis of CuSO₄ with copper electrodes:

• (a) Cathode: Cu²⁺ + 2e⁻ → Cu (copper deposited)
• (b) Anode: Cu → Cu²⁺ + 2e⁻ (copper dissolves)
• (c) Colour remains unchanged (blue) — Cu²⁺ ions replaced from anode
• (d) SO₄²⁻ ions migrate to anode
• (e) Electrorefining of copper

(ii) Definitions: (a) Electron affinity (b) Acid salt (c) Calcination (d) Alkyne (e) Electronegativity

(iii) Blanks: (a) low (b) reddish-brown (c) unsaturated (d) 1:3 (e) loss

(iv) Matching: (a)→(ii) (b)→(iii) (c)→(iv) (d)→(vi) (e)→(v)

(v) IUPAC: (a) Butanal (b) 2-Methylbutane (c) Propan-2-one (d) CH₃—CH=CH—CH₃ (e) CH₃—CH₂—CH₂—OH

Section B — Complete Answers

Question 3

(i) (a) Chlorine — highest electron affinity (small size, needs 1e⁻ for octet) (b) Na > Cl — nuclear charge increases across period, same shell (c) Oxygen forms O²⁻ (config: 2, 8)

(ii) (a) 2NH₄Cl + Ca(OH)₂ → CaCl₂ + 2H₂O + 2NH₃↑ (b) Cu + 4HNO₃(conc.) → Cu(NO₃)₂ + 2NO₂↑ + 2H₂O (c) C + 2H₂SO₄(conc.) → CO₂↑ + 2SO₂↑ + 2H₂O

(iii) (a) Config: 2, 8, 2 (b) Group 2, Period 3 (c) Metal (Magnesium) (d) MgCl₂ (e) Ionic bonding

Question 4

(i) (a) Pale blue ppt of Cu(OH)₂, on warming turns black (CuO) (b) Pungent gas (NH₃), turns moist red litmus blue (c) Sugar turns black — charring by dehydrating agent

(ii) (a) Dilute sulphuric acid (b) Dilute nitric acid (c) Concentrated sulphuric acid

(iii) Cation: Zn²⁺ | Anion: CO₃²⁻ | Salt: ZnCO₃ | Heat: ZnCO₃ → ZnO + CO₂↑

Question 5

(i) (a) 0.3 mol O₂ → 0.2 mol KClO₃ = 24.5 g (b) 0.2 moles KCl (c) Residue = 14.9 g

(ii) (a) Empirical formula: CH₂O (b) Molecular formula: C₂H₄O₂

(iii) 1L C₂H₆ needs 3.5L O₂, produces 2L CO₂

Question 6

(i) (a) C₂H₅OH + 2[O] → CH₃COOH + H₂O (b) C₂H₄ + H₂O → C₂H₅OH (c) CH₃COOH + C₂H₅OH ⇌ CH₃COOC₂H₅ + H₂O

(ii) (a) Na₂CO₃ test — ethanoic acid gives effervescence (b) Bromine water — ethene decolourises it

(iii) (a) Ethyne: CH≡CH (b) 2-Methylpropane (c) Propan-1-ol: CH₃CH₂CH₂OH

Question 7

(i) (a) Bayer's Process (b) Cryolite lowers melting point to ~950°C (c) Al³⁺ + 3e⁻ → Al (d) Anode reacts with O₂ → CO₂

(ii) (a) Bronze — corrosion resistant (b) Duralumin — light & strong

(iii) All Yes — (a) white ppt with Zn, none with Na (b) green vs brown ppt (c) PbCl₂ vs PbSO₄ (d) MnO₂ produces Cl₂

Question 8

(i) NaCl + H₂SO₄(conc.) → NaHSO₄ + HCl↑

(ii) (a) S (Cl) — highest electronegativity (b) Q (Na) + S (Cl) → NaCl (c) T (Ca) — 4 shells (d) R (Al) — amphoteric oxide

(iii) (a) Fe₂O₃ + 3CO → 2Fe + 3CO₂ (b) 2NaOH + Cl₂ → NaCl + NaOCl + H₂O (c) 2C₂H₅OH + 2Na → 2C₂H₅ONa + H₂↑

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Topic-Wise Probability Analysis

Key Revision Tips for 11 March 2026

1. Mole Concept Numericals — Practice mass-volume-mole conversions, empirical/molecular formula problems
2. Organic Chemistry — Master IUPAC naming, structural formulas, isomers, and distinguishing tests
3. Periodic Table — Know all trends (atomic radius, IP, EA, electronegativity) and element identification
4. Electrolysis — Electroplating setup, cathode/anode reactions, electrorefining of copper
5. Study of Compounds — Lab prep of HCl, NH₃; properties of conc. H₂SO₄ and HNO₃
6. Chemical Bonding — Electron dot diagrams, coordinate bond, ionic vs covalent properties
7. Salt Analysis — Flame tests, precipitate colours, action of heat on salts
8. Metallurgy — Extraction of Al (Bayer's + Hall-Héroult), alloys and their properties

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