ICSE Class 9 Chemistry Syllabus 2026-27 — Complete Guide with 9 Chapters & Tips

What's New in 2026-27?

The ICSE Class 9 Chemistry syllabus for 2026-27 covers 9 chapters that introduce students to fundamental chemical concepts — from writing chemical equations to understanding atomic structure, the periodic table, gas laws, and environmental chemistry. CISCE emphasises practical chemistry skills alongside theoretical knowledge, with questions increasingly testing the ability to write balanced equations, explain observations, and apply concepts to real-world scenarios.

Chemistry carries 80 marks for the theory examination and 20 marks for Internal Assessment (practical work). Duration: 2 hours.

Syllabus Overview

Chapter No.	Chapter Name	Key Topics
1	Language of Chemistry	Symbols, formulae, balancing equations, types of reactions
2	Chemical Changes and Reactions	Types of reactions, endothermic/exothermic, catalysts
3	Water	Hard/soft water, treatment, water of crystallisation
4	Atomic Structure and Chemical Bonding	Sub-atomic particles, electron configuration, Bohr model, bonding
5	The Periodic Table	Dobereiner, Newlands, Mendeleev, Modern periodic table
6	Hydrogen	Preparation, properties, uses, isotopes
7	Study of Gas Laws	Boyle's law, Charles' law, gas equation
8	Atmospheric Pollution	Air pollutants, acid rain, ozone depletion, greenhouse effect
9	Practical Work	Gas identification tests, salt analysis

Chapter-wise Detailed Syllabus

1. Language of Chemistry

Chemical Symbols and Formulae: Symbols of common elements, writing chemical formulae using valency, molecular and empirical formulae.

Chemical Equations: Writing word equations and formula equations. Balancing chemical equations by inspection (trial and error method). Information conveyed by a balanced equation — reactants, products, states, molar ratios.

Types of Chemical Reactions: Combination, decomposition, displacement, double displacement, neutralisation, oxidation-reduction (basic understanding).

2. Chemical Changes and Reactions

Physical vs. chemical changes — differences and examples. Conditions necessary for chemical reactions — heat, light, electricity, catalyst, pressure. Energy changes — exothermic reactions (heat released) and endothermic reactions (heat absorbed). Rate of reaction — factors affecting (concentration, temperature, surface area, catalyst). Catalysts — definition, types (positive and negative), examples.

3. Water

Water as a Solvent: Universal solvent, solutions, suspensions, and colloids.

Hard and Soft Water: Causes of hardness (calcium and magnesium salts). Temporary hardness (bicarbonates) — removal by boiling. Permanent hardness (sulphates, chlorides) — removal by washing soda, ion exchange, distillation. Disadvantages of hard water.

Water Treatment: Municipal water treatment process — sedimentation, filtration, chlorination. Importance of clean water.

Water of Crystallisation: Definition, examples (CuSO₄·5H₂O, Na₂CO₃·10H₂O, FeSO₄·7H₂O). Hydrated and anhydrous salts. Hygroscopic, deliquescent, and efflorescent substances.

4. Atomic Structure and Chemical Bonding

Sub-atomic Particles: Electron (Thomson — cathode ray experiment), proton (Goldstein — anode ray experiment), neutron (Chadwick). Properties — mass, charge, location.

Atomic Models: Thomson's plum pudding model, Rutherford's nuclear model (gold foil experiment), Bohr's model — energy levels/shells (K, L, M, N). Electronic configuration — 2, 8, 8 rule. Atomic number (Z), mass number (A), isotopes, isobars.

Chemical Bonding: Octet rule. Electrovalent (ionic) bonding — transfer of electrons, examples (NaCl, MgO, CaCl₂). Covalent bonding — sharing of electrons, examples (H₂, O₂, H₂O, NH₃, CH₄). Electron dot structures. Comparison of ionic and covalent compounds.

5. The Periodic Table

Historical Development: Dobereiner's Triads — pattern of atomic weights. Newlands' Law of Octaves — every 8th element shows similar properties. Mendeleev's Periodic Table — arrangement by atomic weight, prediction of undiscovered elements (Eka-boron, Eka-silicon), achievements and limitations.

Modern Periodic Table: Arrangement by atomic number (Moseley). Periods (7) and Groups (18). Classification — s-block, p-block, d-block, f-block. Metals, non-metals, metalloids. Periodicity of properties — atomic size, metallic/non-metallic character. Valency from electronic configuration.

6. Hydrogen

Laboratory Preparation: Zinc + dilute HCl/H₂SO₄. Collection by downward displacement of water.

Properties: Physical — colourless, odourless, lightest gas. Chemical — combustion (2H₂ + O₂ → 2H₂O), reducing agent (CuO + H₂ → Cu + H₂O), reaction with chlorine.

Uses: Haber's process (NH₃ manufacture), hydrogenation of oils, fuel (hydrogen fuel cells), rocket fuel.

Isotopes: Protium (¹H), Deuterium (²H), Tritium (³H) — uses of heavy water.

7. Study of Gas Laws

Boyle's Law: At constant temperature, P ∝ 1/V (P₁V₁ = P₂V₂). Graphical representation — P vs V, P vs 1/V, PV vs P.

Charles' Law: At constant pressure, V ∝ T (V₁/T₁ = V₂/T₂). Absolute zero (-273°C = 0 K). Kelvin scale. Graphical representation — V vs T.

Gas Equation: Combining Boyle's and Charles' laws: P₁V₁/T₁ = P₂V₂/T₂. STP conditions (0°C, 1 atm). Numerical problems involving pressure, volume, and temperature changes.

8. Atmospheric Pollution

Air Pollutants: CO, CO₂, SO₂, NO₂, particulate matter, CFCs — sources and effects.

Acid Rain: Formation (SO₂ + H₂O → H₂SO₃, NO₂ + H₂O → HNO₃). Effects on buildings, aquatic life, vegetation. Prevention measures.

Ozone Depletion: Ozone layer — location, importance. CFCs and their role in ozone depletion. Montreal Protocol. UV radiation effects.

Greenhouse Effect: Greenhouse gases (CO₂, CH₄, N₂O). Global warming — causes, effects (sea level rise, climate change), mitigation strategies.

9. Practical Work

Identification of gases in the laboratory — hydrogen (pop test), oxygen (glowing splint), carbon dioxide (lime water test), chlorine (colour, bleaching), ammonia (smell, turns red litmus blue), hydrogen chloride (dense white fumes with NH₃). Action of acids and bases on indicators. Preparation of salts. Safety precautions in the laboratory.

Exam Pattern 2026-27

Component	Details	Marks
Section I	Compulsory short-answer questions from all chapters	40 marks
Section II	Answer 4 out of 6 structured/long-answer questions	40 marks
Internal Assessment	Practical work, project, periodic tests	20 marks
Total		100 marks

Prescribed Textbooks

• Concise Chemistry Class 9 — Selina Publishers
• Dalal ICSE Chemistry Class 9 — Allied Publishers
• ICSE Chemistry for Class 9 — S. Chand Publishers

Preparation Tips

1. Master equation balancing — This is the foundation of all chemistry. Practise balancing 10 equations daily until it becomes automatic. Start with simple combination reactions and progress to complex ones.
2. Learn the periodic table structure — Understand the logic of periods, groups, and blocks. Know the first 20 elements and their electronic configurations by heart.
3. Create gas identification charts — Make a table: gas name, colour, odour, test, result. This is the most scoring practical section.
4. Practise gas law numericals — Boyle's law and Charles' law problems are computational and scoring. Practise 15-20 problems covering all variations (P, V, T changes).
5. Understand bonding with diagrams — Draw electron dot structures for every example compound. Visualising electron transfer (ionic) and sharing (covalent) makes bonding intuitive.
6. Connect pollution topics to current events — Read about Delhi's air quality, Mumbai's water issues, and global warming agreements. Real-world examples strengthen your answers.
7. Practise writing chemical equations — Not just balancing but writing full equations with states (s, l, g, aq) and conditions (heat, catalyst). This is essential for Class 10.