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ICSE Class 10 Chemistry Syllabus 2025 PDF, Exam Pattern

ICSE Class 10 Chemistry Syllabus 2025 has been released by CISCE on its official website @cisce.org. Candidates can download the complete syllabus PDF from this website.

Yashasvi Tyagi16 Jun, 2025

ICSE Class 10 Chemistry syllabus for the academic year 2025 has been officially released by the Council for the Indian School Certificate Examinations (CISCE). This syllabus outlines all the essential topics and concepts students are expected to learn during the academic session.

Key areas covered include Periodic Properties, Chemical Bonding, Acids, Bases and Salts, Analytical Chemistry, Mole Concept and Stoichiometry, Electrolysis, Metallurgy, and Organic Chemistry.

The ICSE class 10 syllabus also integrates practical work to reinforce students’ understanding through hands-on experiments and observations. By thoroughly going through the syllabus, students can get a clear picture of what to focus on, structure their study schedule effectively, and prepare with confidence for the upcoming board examinations.

ICSE Class 10 Chemistry Solutions

ICSE Class 10 Chemistry Syllabus 2025 Overview

The Council for the Indian School Certificate Examinations (CISCE) has released the ICSE Class 10 Chemistry syllabus for the academic year 2025. Below is an overview of the key details related to the syllabus and exam pattern.

ICSE Class 10 Chemistry Syllabus 2023-2024 Overview
S.No.	Chapter	Topics
1.	Periodic Properties and Variations of Properties	Periodic properties and variations in groups and periods
		Periodicity on the basis of atomic number for elements
2.	Chemical Bonding	Electrovalent, covalent and coordinate bonding
		Structures of various compounds
		Electron dot structure, characteristic properties
3.	Study of Acids, Bases, and Salts	Simple definitions in terms of molecules and their characteristic properties
		Ions present in mineral acids, alkalis, and salts and their solutions
		Use of litmus and pH paper to test for acidity and alkalinity
		Definition and types of salts
		Action of dilute acids on salts
		Methods of preparation of Normal salts with relevant equations
4.	Analytical Chemistry	Action of Ammonium Hydroxide and Sodium Hydroxide on solution of salts Action of alkalis (NaOH, KOH) on certain metals, their oxides, and hydroxides
5.	Mole Concept and Stoichiometry	Gay Lussac’s Law of Combining Volumes, Avogadro’s Law
		Refer to the atomicity of hydrogen, oxygen, nitrogen, and chlorine
		Vapour Density and its relation to relative molecular mass
		Mole and its relation to mass
		Simple calculations based on chemical equations
6.	Electrolysis	Electrolytes and non-electrolytes
		Definition and explanation of electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation, and reduction.
		An elementary study of the migration of ions, illustrated by the electrolysis of various substances
		Applications of electrolysis
7.	Metallurgy	Occurrence of metals in nature
		Stages involved in the extraction of metals
		Extraction of Aluminium
		Alloys - composition and uses
8.	Study of Compounds	Hydrogen Chloride - preparation, reactions, properties
		Ammonia - preparation, reactions, uses
		Nitric Acid - preparations, reactions
		Sulphuric Acid - preparation and its behaviour as an acid, oxidising agent, dehydrating agent
9.	Organic Chemistry	Introduction to Organic compounds
		Structure and Isomerism
		Homologous series with characteristics and examples
		Simple nomenclature
		Hydrocarbons - alkanes, alkenes, alkynes

ICSE Class 10 Chemistry Syllabus 2025 Chapter-Wise

ICSE Class 10 Chemistry Syllabus for 2025 aims to cover essential Chemistry concepts such as periodic properties, chemical bonding, acids, bases, salts, analytical chemistry, mole concept, stoichiometry, electrolysis, metallurgy, and organic chemistry. The detailed topics for each chapter are provided below:

Chapter 1: Periodic Properties and variations of Properties – Physical and Chemical

(i) Understanding the variations of properties at regular intervals in groups and periods. Examine and grasp the definitions and trends of the subsequent periodic properties in both groups and periods:

Size of atoms
Metallic attributes
Non-metallic attributes
Ionisation potential
Electron affinity
Electronegativity

(ii) The arrangement based on atomic numbers for elements. Explore the modern periodic table, specifically up to period 3 (although students will be familiarised with the entire table, questions will only pertain to elements up to Argon). Explain periodicity and associated properties based on nuclear charge and shells (not orbitals).

Chapter 2: Chemical Bonding

(a) Electrovalent bonding: Electron dot structures for electrovalent compounds like NaCl, MgCl2, and CaO. Distinctive features of electrovalent compounds, such as their form of existence, melting and boiling points, conductivity (heat and electricity), and dissociation in solution and molten state connected to electrolysis.

(b) Covalent Bonding: Electron dot structures for covalent molecules based on duplet and octet electron rules (e.g., hydrogen, chlorine, nitrogen, ammonia, carbon tetrachloride, methane). Polar Covalent compounds explained by differences in electronegativity, with examples like HCl and H2O, including their structures. Characteristic properties of Covalent compounds, considering their state, melting and boiling points, conductivity (heat and electricity), and ionisation in solution. Comparison between Electrovalent and Covalent compounds.

(c) Coordinate Bonding: Definition Explaining the lone pair effect of the oxygen atom in water and the nitrogen atom in ammonia, illustrating the formation of H3O+ and OH- ions in water and NH4+ ions.

Chapter 3: Study of Acids, Bases and Salts

(i) Clear explanations based on the molecules and their characteristic properties.

(ii) Examination of ions found in mineral acids, alkalis, and salts, along with their solutions; application of litmus and pH paper for assessing acidity and alkalinity.

Providing examples with equations for the ionisation/dissociation of acids, bases, and salts. Acids generate hydronium ions (positive ions only), turning blue litmus red

Alkalis produce hydroxyl ions (negative ions only) in water, changing red litmus to blue. Salts result from the partial or complete replacement of the hydrogen ion of an acid by a metal, elucidated through suitable examples. Introduction to the pH scale for testing acidity, neutrality, and alkalinity using pH paper or Universal indicator.

(iii) Explanation of salt and its various types.

Detailing types of salts: normal salts, acid salt, basic salt, with definitions and examples.

(iv) Exploration of the impact of dilute acids on salts.

Breaking down hydrogen carbonates, carbonates, sulphites, and sulphides using appropriate acids, with heating if needed. (Conducting relevant laboratory experiments is essential.)

(v) Presentation of methods for preparing Normal salts with corresponding equations. Included methods are:

Direct combination
Displacement
Precipitation (double decomposition)
Neutralisation of insoluble base
Neutralisation of an alkali (titration)
Action of dilute acids on carbonates and bicarbonates.

Chapter 4: Analytical Chemistry

(i) The effect of Ammonium Hydroxide and Sodium Hydroxide on salt solutions: observing the colour of the salt and its solution; noting the creation and colour of the precipitated hydroxide for Ca, Fe, Cu, Zn, and Pb salts; emphasising the unique impact of ammonium hydroxide on copper salt solutions, as well as the action of sodium hydroxide and ammonium salts.

Regarding salt solutions:

Noting the colour of the salt and its solution.
Adding Sodium Hydroxide gradually to solutions of Ca, Fe, Cu, Zn, and Pb salts, and observing the formation and colour of the resulting hydroxide precipitate, with relevant equations.
Adding Ammonium Hydroxide gradually to solutions of Ca, Fe, Cu, Zn, and Pb salts, and observing the formation and colour of the resulting hydroxide precipitate, with relevant equations.
Highlighting the specific impact of Ammonium Hydroxide on copper salt solutions and the effects of sodium hydroxide and ammonium salts.

(ii) The reaction of alkalis (NaOH, KOH) with certain metals, their oxides, and hydroxides, including aluminium, zinc, and lead. These substances exhibit amphoteric characteristics when interacting with caustic alkalis (NaOH, KOH).

Chapter 5: Mole Concept and Stoichiometry

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

Concept of mole – a quantity like a dozen or a gross (Avogadro's number).
Avogadro's Law - declaration and explanation.
Gay Lussac's Law of Combining Volumes – Explanation and statement.
Understanding molar volume - "the weight of 22.4 litres of any gas at S.T.P. is the same as its molar mass." (Formal proof won't be covered but may be explained for clarity).
Basic computations based on molar volume and Gay Lussac's law.

(ii) Discuss the atomicity of hydrogen, oxygen, nitrogen, and chlorine (proof not necessary).
The explanation can be provided using equations for the creation of HCl, NH3, and NO.

(iii) Vapour Density and its connection to relative molecular mass:
Molecular mass = 2*vapour density (formal proof not needed) Derivation of simple (empirical) and molecular formulas from:

(a) the percentage composition of a compound.
(b) the masses of combining elements.

(iv) Mole and its connection to mass. Relating mole and atomic mass; obtaining gram atomic mass and then gram atom; atomic mass deals with one atom; gram atomic mass is the mass of one mole of atoms. Relating mole and molecular mass, arriving at gram molecular mass and gram molecule – molecular mass relates to a molecule, gram molecular mass is the mass of one mole of molecules. Basic calculations based on the relationship of mole to mass, volume, and Avogadro's number.

Chapter 6: Electrolysis

(i) Electrolytes and non-electrolytes. Definitions and examples.

(ii) Materials with only molecules, only ions, or both molecules and ions.

Substances with molecules exclusively, ions exclusively, or a combination of molecules and ions.
Examples explain how their composition influences their behaviour as strong or weak electrolytes and non-electrolytes.

(iii) Explanation and definition of electrolysis, electrolyte, electrode, anode, cathode, anion, cation, oxidation, and reduction (based on the loss and gain of electrons).

(iv) Basic examination of ion migration, considering factors affecting selective discharge of ions (referring to the activity series, indicating metal tendencies, e.g., Na, Mg, Fe, Cu, to form ions). This is demonstrated through the electrolysis of:

Molten lead bromide
Acidified water with platinum electrodes
Aqueous copper (II) sulphate with copper electrodes; showcasing electron transfer at the electrodes.

(v) Practical uses of electrolysis. Application examples include electroplating with nickel and silver, selection of electrolyte for electroplating, and electrorefining of copper.

Chapter 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.
Electro refining – reference only.

(iii) Extraction of Aluminium.

Chemical method for purifying bauxite by using NaOH – Baeyer’s Process.
Electrolytic extraction – Hall Heroult’s process: Structure of electrolytic cell - the various components as part of the electrolyte, electrodes, and electrode reactions. Description of the changes occurring, the 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

Chapter 8: Study of Compounds

Hydrogen Chloride
Ammonia
Nitric Acid
Sulphuric Acid

Chapter 9: Organic Chemistry

(i) Overview of Organic Substances.

(ii) Construction and Isomeric Forms.

(iii) Homologous Sequences – Features with Instances.

(iv) Basic Naming.

(v) Hydrocarbons: Saturated (alkanes), Unsaturated (alkenes, alkynes).

(vi) Alcohols: Ethanol – Making, Traits, and Applications.

(vii) Carboxylic Acids (aliphatic - single-carboxylic acid): Acetic Acid – Characteristics and Applications of Acetic Acid.

ICSE Class 10 Chemistry Syllabus Practical Work

Candidates will need to observe the impact of reagents or heat on given substances. The exercises will be straightforward, involving the recognition and identification of certain gases and ions. However, examiners may choose substances beyond those with listed ions.

Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide, Ammonia, Water vapour, Nitrogen dioxide.
Ions : Calcium, Copper, Iron, Lead, Zinc, Ammonium, Carbonate, Chloride, Nitrate, Sulphide, Sulphite, Sulphate.

While knowledge of a formal analysis scheme is unnecessary, semi-micro techniques are acceptable. Candidates using such techniques may need to adjust instructions according to the apparatus's size. Candidates should have completed the following minimum practical work:

Observe the action of heat on substances like copper carbonate, zinc carbonate, zinc nitrate, copper nitrate, and lead nitrate. Record observations, identify products, and make deductions (equations not required).
Make a solution of an unknown substance: add sodium hydroxide solution or ammonium hydroxide solution, observe, and deduce. Warming the mixture may be necessary. Choose substances containing Ca2+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+, NH4+.
Provide a solution of dilute acid and alkali. Determine which is acidic and which is basic, providing two tests for each.
Add concentrated hydrochloric acid to given substances, warm, observe, identify any product, and make deductions for copper oxide and manganese dioxide.

ICSE Class 10 Chemistry Exam Pattern 2025

If you're preparing for the ICSE Class 10 Chemistry Board Exam 2025, it's important to understand the exam pattern thoroughly. This will help you manage your time and approach each section strategically.

ICSE Class 10 Chemistry Exam Pattern 2025
Component	Details
Total Duration	2 Hours
Total Marks	100 Marks
Theory Exam	80 Marks
Internal Assessment	20 Marks (Based on Practical Work)
Sections in Theory Exam	Section I (40 Marks) and Section II (40 Marks)
Section I	Compulsory short-answer questions covering the entire syllabus
Section II	Six questions given, attempt any four out of the six

ICSE Class 10 Chemistry Syllabus 2025 PDF Download

Students preparing for the upcoming board exams can download the ICSE Class 10 Chemistry Syllabus 2025 PDF from the direct link provided below.

The PDF includes the complete syllabus with all important topics, units, exam pattern, and practical work guidelines. Accessing the syllabus in PDF format allows students to refer to it anytime, even without internet connectivity, making it easier to plan and manage their study schedule. It is advisable to keep a printed or saved copy of the syllabus for quick and frequent reference during the academic year.

ICSE Class 10 Chemistry Syllabus 2025

Study without using the internet

Preparation Tips for ICSE Class 10 Chemistry 2025

Begin by carefully reviewing the entire ICSE Class 10 Chemistry syllabus. Focus on important chapters like Chemical Reactions, Acids, Bases and Salts, Periodic Table, Metallurgy, and Organic Chemistry.
Understand each concept clearly instead of memorizing reactions. Know why and how reactions occur, and relate them to real-life applications.
Practice balancing chemical equations regularly. It’s a core skill needed for writing reactions accurately in exams.
Make concise notes of important concepts, definitions, reactions, and tests. Use flashcards for quick revision of chemical formulas and valencies.
Learn and revise the periodic table—pay special attention to groups, periods, trends, and properties of elements.
Practice numericals from topics like Mole Concept, Gas Laws, and Stoichiometry. Show all steps clearly and follow unit conversions carefully.
Internal assessment carries 20 marks. Perform all practicals sincerely, maintain an accurate lab record book, and prepare well for viva questions.
Solve past years’ papers and sample questions to understand the question pattern. Aim to complete mock tests within the 2-hour time limit.
Revise the syllabus at least twice before the exam and clarify any doubts early. Focus more on the topics you find difficult.

ICSE Class 10 Chemistry Syllabus 2025 FAQs

What are the main topics covered in the ICSE Class 10 Chemistry Syllabus 2025?

The syllabus covers fundamental concepts like periodic properties, chemical bonding, acids, bases, salts, analytical chemistry, the mole concept, stoichiometry, electrolysis, metallurgy, and organic chemistry.

Where can I find the official ICSE Class 10 Chemistry Syllabus 2025?

You can download the official syllabus PDF from the Council for the Indian School Certificate Examinations (CISCE) website @cisce.org.

What is the exam pattern for ICSE Class 10 Chemistry?

The exam consists of two parts: Part I (Theory) with short answer and long answer questions, and Part II (Practical) with experiments and viva voce.

How can I prepare for the ICSE Class 10 Chemistry practical exam?

Thoroughly understand the theoretical concepts behind the experiments listed in the syllabus, practice drawing diagrams and chemical equations, and be prepared to explain your observations and results to the examiner.

What are some tips for scoring well in ICSE Class 10 Chemistry?

Regularly attend classes and pay attention in lectures, practice solving past year question papers and sample papers, focus on understanding key concepts rather than rote learning, and maintain a good study schedule.

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