ICSE Class 10 Chemistry Syllabus 2026-27

Chemistry is one of the three core science subjects in the ICSE Class 10 board examination. It is a subject that blends theoretical understanding, chemical equations, and practical application, making it both challenging and highly rewarding for students who prepare with a clear strategy. A solid understanding of the ICSE Class 10 Chemistry syllabus for the 2026-27 session is the first step towards achieving top marks.

This complete guide covers the full chapter-wise ICSE Class 10 Chemistry syllabus, exam pattern, marking scheme, practical syllabus, prescribed textbook, and expert preparation tips. Whether you are beginning your preparation or looking for a structured revision plan, this page gives you everything you need in one place.

Quick Facts: ICSE Class 10 Chemistry 2026-27

ICSE Class 10 Chemistry Exam Pattern 2026-27

The ICSE Class 10 Chemistry written paper carries 80 marks and is divided into two sections. Section I is compulsory for all students and Section II provides internal choice. The practical component of 20 marks is assessed by the school throughout the academic year.

Practical Assessment Details (20 Marks)

The practical component is conducted and assessed by the school teacher throughout the academic year. It includes the following:

•        Practical Work: Performing prescribed Chemistry experiments accurately and safely.

•        Observation and Records: Maintaining a neat practical file with observations, readings, diagrams, and inferences.

•        Viva Voce: Oral questions based on experiments and Chemistry concepts.

•        Project Work: A short Chemistry project or investigative assignment assessed by the teacher.

ICSE Class X — Chemistry

Official CISCE Syllabus 2026-27

Exam Pattern: One paper, 2 hours duration, 80 marks + Internal Assessment of practical work 20 marks Note: All chemical processes/reactions should be studied with reference to the reactants, products, conditions, observations and the (balanced) equations and diagrams.

Section I (40 marks) — Short answer questions, compulsory, entire syllabus Section II (40 marks) — Six questions; answer any four

1. Periodic Properties and Variations of Properties – Physical and Chemical

(i) Periodic properties and their variations in groups and periods

• Definitions and trends of the following periodic properties in groups and periods:

  • Atomic size

  • Metallic character

  • Non-metallic character

  • Ionisation potential

  • Electron affinity

  • Electronegativity

    
    

(ii) Periodicity on the basis of atomic number for elements

• Study of modern periodic table up to Period 3

• Students to be exposed to the complete modern periodic table but no questions will be asked on elements beyond Period 3 – Argon

• Periodicity and other related properties to be explained on the basis of nuclear charge and shells (not orbitals)

• Special reference to the alkali metals and halogen groups

  
  

2. Chemical Bonding

Electrovalent, covalent and co-ordinate bonding, structures of various compounds, Electron dot structure.

Electrovalent Bonding

• Electron dot structure of electrovalent compounds: NaCl, MgCl₂, CaO

• Characteristic properties of electrovalent compounds:

  • State of existence

  • Melting and boiling points

  • Conductivity (heat and electricity)

  • Dissociation in solution and in molten state — to be linked with electrolysis

    
    

Covalent Bonding

• Electron dot structure of covalent molecules on the basis of duplet and octet of electrons (examples: hydrogen, chlorine, nitrogen, ammonia, carbon tetrachloride, methane)

• Polar covalent compounds — based on difference in electronegativity; examples: HCl and H₂O including structures

• Characteristic properties of covalent compounds:

  • State of existence

  • Melting and boiling points

  • Conductivity (heat and electricity)

  • Ionisation in solution

• Comparison of electrovalent and covalent compounds

  
  

Coordinate Bonding

• Definition

• The lone pair effect of the oxygen atom of the water molecule and the nitrogen atom of the ammonia molecule to explain the formation of H₃O⁺ and OH⁻ ions in water and NH₄⁺ ion

• The meaning of lone pair; the formation of hydronium ion and ammonium ion must be explained with the help of electron dot diagrams

  
  

3. Study of Acids, Bases and Salts

(i) Simple definitions in terms of the molecules and their characteristic properties

(ii) Ions present in mineral acids, alkalis and salts and their solutions; use of litmus and pH paper to test for acidity and alkalinity

• Examples with equations for the ionisation/dissociation of ions of acids, bases and salts

• Acids form hydronium ions (only positive ions) which turn blue litmus red; alkalis form hydroxyl ions (only negative ions) with water which turn red litmus blue

• Salts are formed by partial or complete replacement of the hydrogen ion of an acid by a metal

• Introduction to pH scale to test for acidity, neutrality and alkalinity by using pH paper or Universal indicator

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(iii) Definition of salt; types of salts

• Types of salts: normal salts, acid salt, basic salt — definition and examples

  
  

(iv) Action of dilute acids on salts

• Decomposition of hydrogen carbonates, carbonates, sulphites and sulphides by appropriate acids with heating if necessary (relevant laboratory work must be done)

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(v) Methods of preparation of Normal salts with relevant equations (Details of apparatus or procedures not required)

• Direct combination

• Displacement

• Precipitation (double decomposition)

• Neutralisation of insoluble base

• Neutralisation of an alkali (titration)

• Action of dilute acids on carbonates and bicarbonates

  
  

4. Analytical Chemistry

(i) Action of Ammonium Hydroxide and Sodium Hydroxide on solution of salts

• Colour of salt and its solution

• Formation and colour of hydroxide precipitated for solutions of salts of Ca, Fe, Cu, Zn and Pb

• Action on addition of Sodium Hydroxide to solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess — formation and colour of hydroxide precipitated to be highlighted with equations

• Action on addition of Ammonium Hydroxide to solution of Ca, Fe, Cu, Zn, and Pb salts drop by drop in excess — formation and colour of hydroxide precipitated to be highlighted with equations

• Special action of Ammonium Hydroxide on solutions of copper salts

• Special action of Sodium Hydroxide on ammonium salts

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(ii) Action of alkalis (NaOH, KOH) on certain metals, their oxides and hydroxides

• The metals must include aluminium, zinc and lead, their oxides and hydroxides, which react with caustic alkalis (NaOH, KOH), showing the amphoteric nature of these substances

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5. Mole Concept and Stoichiometry

(i) Gay Lussac's Law of Combining Volumes; Avogadro's Law

• Idea of mole — a number just as a dozen, a gross (Avogadro's number)

• Avogadro's Law — statement and explanation

• Gay Lussac's Law of Combining Volumes — statement and explanation

• Understanding molar volume — "the mass of 22.4 litres of any gas at S.T.P. is equal to its molar mass"

• Questions will not be set on formal proof but may be taught for clear understanding

• Simple calculations based on molar volume and Gay Lussac's Law

  
  

(ii) Refer to the atomicity of hydrogen, oxygen, nitrogen and chlorine (proof not required)

• The explanation can be given using equations for the formation of HCl, NH₃, and NO

  
  

(iii) Vapour Density and its relation to relative molecular mass

• Molecular mass = 2 × vapour density (formal proof not required)

• Deduction of simple (empirical) and molecular formula from:

  • The percentage composition of a compound

  • The masses of combining elements

    
    

(iv) Mole and its relation to mass

• Relating mole and atomic mass; arriving at gram atomic mass and then gram atom

• Relating mole and molecular mass; arriving at gram molecular mass and gram molecule

• Simple calculations based on relation of mole to mass, volume and Avogadro's number

  
  

(v) Simple calculations based on chemical equations

• Related to weight and/or volumes of both reactants and products

  
  

6. Electrolysis

(i) Electrolytes and non-electrolytes — definitions and examples

(ii) Substances containing molecules only, ions only, both molecules and ions

• Examples; relating their composition with their behaviour as strong and weak electrolytes as well as non-electrolytes

  
  

(iii) Definition and explanation of:

• Electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation and reduction (on the basis of loss and gain of electrons)

  
  

(iv) An elementary study of the migration of ions, with reference to the factors influencing selective discharge of ions (reference should be made to the activity series as indicating the tendency of metals, e.g. Na, Mg, Fe, Cu, to form ions) — illustrated by the electrolysis of:

• Molten lead bromide

• Acidified water with platinum electrodes

• Aqueous copper (II) sulphate with copper electrodes; electron transfer at the electrodes

• (The above electrolytic processes to be studied in terms of: electrolyte used, electrodes used, ionisation reaction, anode reaction, cathode reaction, and selective discharge theory wherever applicable)

  
  

(v) Applications of electrolysis

• Electroplating with nickel and silver; choice of electrolyte for electroplating

• Electro refining of copper

• (Reasons and conditions for electroplating; names of electrolytes and electrodes used; equations for reactions at electrodes for electroplating and refining of copper)

  
  

7. Metallurgy

(i) Occurrence of metals in nature

• Mineral and ore — meaning only

• Common ores of iron, aluminium and zinc

  
  

(ii) Stages involved in the extraction of metals

• Dressing of the ore — hydrolytic method, magnetic separation, froth flotation method

• Conversion of concentrated ore to its oxide — roasting and calcination (definition, examples with equations)

• Reduction of metallic oxides — some can be reduced by hydrogen, carbon and carbon monoxide (e.g. copper oxide, lead(II) oxide, iron(III) oxide and zinc oxide) and some cannot (e.g. Al₂O₃, MgO) — refer to activity series

• Active metals by electrolysis e.g. sodium, potassium and calcium (reference only)

• Equations with conditions should be given

• Electro refining (reference only)

  
  

(iii) Extraction of Aluminium

• Chemical method for purifying bauxite by using NaOH — Baeyer's Process

• Electrolytic extraction — Hall-Héroult's Process:

  • Structure of electrolytic cell — the various components as part of the electrolyte, electrodes and electrode reactions

  • Description of the changes occurring, purpose of the substances used and the main reactions with their equations

    
    

(iv) Alloys — composition and uses

• Stainless steel, duralumin, brass, bronze, fuse metal/solder

  
  

8. Study of Compounds

A. Hydrogen Chloride

• Preparation of hydrogen chloride from sodium chloride

• The laboratory method of preparation in terms of: reactants, product, condition, equation, diagram, procedure, observation, precaution, collection and identification

• Simple experiment to show the density of the gas — heavier than air

• Solubility of hydrogen chloride — fountain experiment: setting of apparatus, procedure, observation, inference

• Method of preparation of hydrochloric acid by dissolving the gas in water — the special arrangement and mechanism by which back suction is avoided

• Reaction with ammonia

• Acidic properties of its solution — reaction with metals, their oxides, hydroxides and carbonates to give their chlorides; decomposition of carbonates, hydrogen carbonates, sulphides, sulphites

• Precipitation reactions with silver nitrate solution and lead nitrate solution

  
  

B. Ammonia

• Laboratory preparation from ammonium chloride and collection (in terms of: setting of apparatus, diagram, procedure, observation, collection and identification)

• Ammonia from nitrides like Mg₃N₂ and AlN using warm water

• Ammonia from ammonium salts using alkalis

• Manufacture by Haber's Process

• Density and solubility of ammonia — fountain experiment

• The burning of ammonia in oxygen

• The catalytic oxidation of ammonia (with conditions and reaction)

• Its reactions with hydrogen chloride and with hot copper(II) oxide and chlorine (both chlorine in excess and ammonia in excess — in terms of reactants, products, conditions, equations and observations)

• Aqueous solution of ammonia — reaction with sulphuric acid, nitric acid, hydrochloric acid and solutions of iron(III) chloride, iron(II) sulphate, lead nitrate, zinc nitrate and copper sulphate

• Uses of ammonia — manufacture of fertilizers, explosives, nitric acid, refrigerant gas (Chlorofluorocarbon and its suitable alternatives which are non-ozone depleting), and cleansing agents

  
  

C. Nitric Acid

• One laboratory method of preparation from potassium nitrate or sodium nitrate (in terms of: reactants, products, conditions, equations, setting up of apparatus, diagram, precautions, collection and identification)

• Manufacture by Ostwald's Process (only equations with conditions where applicable)

• As an oxidising agent — its reaction with copper, carbon, sulphur

  
  

D. Sulphuric Acid

• Manufacture by Contact Process (equations with conditions where applicable)

• Its behaviour as an acid when dilute — reaction with metal, metal oxide, metal hydroxide, metal carbonate, metal bicarbonate, metal sulphite, metal sulphide

• Concentrated sulphuric acid as an oxidising agent — the oxidation of carbon and sulphur

• Concentrated sulphuric acid as a dehydrating agent — (a) the dehydration of sugar (b) copper(II) sulphate crystals

• Non-volatile nature of sulphuric acid — reaction with sodium or potassium chloride and sodium or potassium nitrate

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9. Organic Chemistry

(i) Introduction to Organic compounds

• Unique nature of Carbon atom — tetravalency, catenation

• Formation of single, double and triple bonds; straight chain, branched chain, cyclic compounds (only benzene)

  
  

(ii) Structure and Isomerism

• Structure of compounds with single, double and triple bonds

• Structural formulae of hydrocarbons; structural formula must be given for alkanes, alkenes, alkynes up to 5 carbon atoms

• Isomerism — structural (chain, position)

  
  

(iii) Homologous series — characteristics with examples

• Alkane, alkene, alkyne series and their gradation in properties and the relationship with molecular mass or molecular formula

  
  

(iv) Simple nomenclature

• Simple nomenclature of hydrocarbons with simple functional groups — double bond, triple bond, alcoholic, aldehydic, carboxylic group

• Longest chain rule and smallest number for functional groups rule

• Trivial and IUPAC names (compounds with only one functional group)

  
  

(v) Hydrocarbons: alkanes, alkenes, alkynes

• Alkanes — general formula; methane (greenhouse gas) and ethane — methods of preparation from sodium ethanoate (sodium acetate), sodium propanoate (sodium propionate), from iodomethane (methyl iodide) and bromoethane (ethyl bromide); complete combustion of methane and ethane; reaction of methane and ethane with chlorine through substitution

• Alkenes — unsaturated hydrocarbons with a double bond; ethene as example; methods of preparation by dehydrohalogenation reaction and dehydration reactions

• Alkynes — unsaturated hydrocarbons with a triple bond; ethyne as example; methods of preparation from calcium carbide and 1,2-dibromoethane (ethylene dibromide)

• Only main properties, particularly addition products with hydrogen and halogen namely Cl₂, Br₂ and I₂ pertaining to alkenes and alkynes

• Uses of methane, ethane, ethene, ethyne

  
  

(vi) Alcohols: ethanol — preparation, properties and uses

• Preparation of ethanol by hydrolysis of alkyl halide

• Properties — Physical: nature, solubility, density, boiling points; Chemical: combustion, action with sodium, ester formation with acetic acid, dehydration with conc. sulphuric acid to prepare ethene

• Denatured and spurious alcohol

• Important uses of ethanol

  
  

(vii) Carboxylic acids (aliphatic — mono carboxylic acid): Acetic acid — properties and uses

• Structure of acetic acid

• Properties — Physical: odour (vinegar), glacial acetic acid (effect of sufficient cooling to produce ice-like crystals); Chemical: action with litmus, alkalis and alcohol (idea of esterification)

• Uses of acetic acid

  
  

Internal Assessment of Practical Work — 20 Marks

Candidates will be asked to observe the effect of reagents and/or of heat on substances supplied to them. Exercises will be simple and may include the recognition and identification of certain gases and ions.

Gases to be identified: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide, Ammonia, Water vapour, Nitrogen dioxide

Ions to be identified: Calcium, Copper, Iron, Lead, Zinc, Ammonium — Carbonate, Chloride, Nitrate, Sulphide, Sulphite, Sulphate

Knowledge of a formal scheme of analysis is not required. Semi-micro techniques are acceptable.

Minimum practical work to be completed:

1. Action of heat on the following substances — make observations, identify products, make deductions (equations not required):

   • Copper carbonate, zinc carbonate

   • Zinc nitrate, copper nitrate, lead nitrate

2. Make a solution of the unknown substance; add sodium hydroxide solution or ammonium hydroxide solution, make observations and give deduction. Warming may be needed. Choose from substances containing Ca²⁺, Cu²⁺, Fe²⁺, Fe³⁺, Pb²⁺, Zn²⁺, NH₄⁺

3. Supply a solution of dilute acid and alkali. Determine which is acidic and which is basic, giving two tests for each.

4. Add concentrated hydrochloric acid to each of the given substances, warm, make observations, identify any product and make deductions:

   • (a) copper oxide

   • (b) manganese dioxide

Evaluation:

• Subject Teacher (Internal Examiner): 10 marks

• External Examiner: 10 marks

• Marks entered online on CISCE's CAREERS portal by Head of school

ICSE Class 10 Chemistry Chapter Overview

ICSE Class 10 Chemistry Practical Syllabus

The practical component carries 20 marks and is evaluated by the school throughout the year. Candidates will be asked to observe the effect of reagents and/or of heat on substances supplied to them. The exercises will be simple and may include the recognition and identification of certain gases and ions. The following are the minimum experiments prescribed by CISCE:

ICSE Class 10 Chemistry Marking Scheme 2026-27

Recommended Books for ICSE Class 10 Chemistry 2026-27

How to Prepare for ICSE Class 10 Chemistry: Expert Tips

1. Understand Rather Than Memorise

Chemistry involves a large number of equations, reactions, and properties. Instead of memorising them blindly, understand the logic behind why reactions occur. When you understand the reactivity series, for example, predicting displacement reactions becomes straightforward rather than something you need to memorise.

2. Write and Balance Equations Daily

Chemical equations are tested heavily in both sections of the paper. Make it a daily habit to write out and balance equations for reactions covered in each chapter. Pay close attention to state symbols and conditions such as heat, catalyst, and pressure.

3. Master the Mole Concept and Stoichiometry

The Mole Concept is one of the most calculation-intensive chapters in the ICSE Chemistry syllabus. Practise a wide variety of numerical problems including percentage composition, empirical formula, molecular formula, and gas volume calculations. This chapter rewards students who practise consistently.

4. Create a Reaction Summary Sheet

For each chapter in Study of Compounds (HCl, Ammonia, Nitric Acid, Sulphuric Acid), create a one-page summary listing all key reactions, conditions, observations, and uses. Revising these summary sheets regularly in the final weeks of preparation will save significant time.

5. Practise Analytical Chemistry Thoroughly

The Identification of Ions chapter is directly tested in both the written paper and the practical examination. Know the confirmatory tests, the reagents used, and the expected observations for every cation and anion in the syllabus. Prepare a table for quick revision.

6. Do Not Skip Organic Chemistry

Organic Chemistry (hydrocarbons, alcohols, and carboxylic acids) is a chapter many students underestimate. It carries significant marks and is relatively straightforward once you understand IUPAC naming, functional groups, and the key reactions for each organic compound.

7. Take Practical Work Seriously Throughout the Year

The 20-mark practical component is spread across the year. Perform every experiment carefully, record observations neatly, and understand the theory behind each experiment. A well-maintained practical file and confident viva answers can secure you full marks in this component.

8. Solve Previous 10 Years of ICSE Chemistry Papers

Past papers are one of the best preparation tools for ICSE Chemistry. They reveal the most frequently tested chapters, the type of questions asked in Section I and Section II, and help you manage your time effectively. After solving each paper, analyse your mistakes and revise accordingly.

Frequently Asked Questions

Q1. Which are the most important chapters in ICSE Class 10 Chemistry?

Mole Concept and Stoichiometry, Study of Compounds (Ammonia, Sulphuric Acid, Nitric Acid, HCl), Electrolysis, Analytical Chemistry (Identification of Ions), and Metallurgy are among the most important and frequently tested chapters in the ICSE Class 10 Chemistry board paper.

Q2. How many marks does the practical carry in ICSE Chemistry?

The practical or internal assessment component carries 20 marks in ICSE Class 10 Chemistry. It includes experiments, practical records, viva voce, and project work, all assessed by the school.

Q3. Is Organic Chemistry difficult in ICSE Class 10?

Organic Chemistry in ICSE Class 10 is manageable if approached systematically. Focus on IUPAC nomenclature, the general properties of alkanes, alkenes, and alkynes, and the key reactions of ethanol and acetic acid. With regular practice it becomes one of the more straightforward units.

Q4. Which textbook is best for ICSE Class 10 Chemistry?

Concise Chemistry Class 10 by Selina Publishers is the most widely recommended textbook for ICSE Chemistry. It covers the complete syllabus with clear explanations, worked examples, and comprehensive exercises for every chapter.

Q5. Where can I find the official ICSE Chemistry syllabus for 2026-27?

The official ICSE Class 10 Chemistry syllabus for 2026-27 is available on the CISCE official website at www.cisce.org. Always refer to the official source to confirm chapter inclusions and any updates or revisions.