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Chemistry Class 8 ICSE CISCE Topics and Syllabus

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CISCE Syllabus For Class 8 Chemistry: Knowing the Syllabus is very important for the students of Class 8. Shaalaa has also provided a list of topics that every student needs to understand.

The CISCE Class 8 Chemistry syllabus for the academic year 2021-2022 is based on the Board's guidelines. Students should read the Class 8 Chemistry Syllabus to learn about the subject's subjects and subtopics.

Students will discover the unit names, chapters under each unit, and subtopics under each chapter in the CISCE Class 8 Chemistry Syllabus pdf 2021-2022. They will also receive a complete practical syllabus for Class 8 Chemistry in addition to this.

Academic year:

CISCE Class 8 Chemistry Revised Syllabus

CISCE Class 8 Chemistry and their Unit wise marks distribution

CISCE Class 8 Chemistry Course Structure 2021-2022 With Marking Scheme

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1 Matter
  • Nature of matter
  • Main postulates of the kinetic molecular theory of matter.
  • Explanation of change of state of the matter on the basis of interparticle space and interparticle attraction and collision.
  • Law of conservation of mass. (statement and explanation with examples)
  • Interconversion of states of matter.
2 Physical and Chemical Changes
  • Physical and Chemical changes
3 Elements, Compounds and Mixtures
  • Revision of Matter taught in earlier classes.
  • Elements, compounds and mixture – a brief explanation.
  • Separation of the components of a mixture.
  • Emphasis on the principle of separation.
4 Atomic Structure
  • Fundamental subatomic particles present in an atom: electrons, protons, neutrons.
  • Nucleus and extra nuclear parts.
  • Atomic number and mass number.
  • The combining capacity of elements
5 Language of Chemistry
  • Symbols of elements.
  • Formulae of compounds.
  • Chemical equations (from word equations).
  • Law of conservation of mass.
  • Balancing simple equations
  • Relate the law to the balancing of simple equations.
  • Information gathered from a chemical equation.
  • Limitations of a chemical equation: Catalyst, conditions for the reaction, state of the reactants and products, nature of the chemical reaction are not gathered from the equation.
6 Chemical Reactions
  • Types of reactions:
    • Combination
    • Decomposition
    • Displacement
    • Double displacement.
  • Reactivity series:
  • In reactivity, series metals are arranged in order of their reactivity.
  • The metal that displaces the metal ion from the solution is more reactive.
  • Predict the reactivity of metals.
  • Endothermic and exothermic processes/reactions.
  • Neutralization reaction.
  • Decomposition reactions to form Oxides.
  • Classification of oxides:
  • Metal oxides are basic; nonmetal oxides are acidic in nature.
  • Acidic oxides react with base and basic oxides react with acids. some oxides such as ZnO, PbO react both with acids and bases. These are amphoteric oxides.
7 Hydrogen
  • Preparation of hydrogen, from water – electrolysis (Introduction to terms electrode, electrolyte, electrolysis – detailed process not required).
  • Preparation of hydrogen in the laboratory.
  • Preference of zinc as the metal to be used ( with reasons).
  • Choice of dilute acids (other than dil. nitric acid).
  • Bosch’s process.
  • Properties and uses of hydrogen.
  • Oxidation and Reduction.
8 Water
  • Dissolution of salts in water – meaning and explanation.
  • Universal solvent – meaning.
  • Solutions, suspensions, colloids.
  • Differentiate unsaturated/saturated and supersaturated solutions.
  • Suspensions and colloids.
  • Water of crystallisation.
  • Hydrated and Anhydrous substances, hygroscopic.
  • Reactivity of metals with cold water, hot water and steam ( with products formed).
  • Hard and soft water and methods of softening of hard water.
  • Disadvantage of using hard water.
  • Removing hardness of water by boiling or by treating with washing soda
9 Carbon and Its Compounds
  • Allotropes of Carbon – definition and explanation.
  • Crystalline and amorphous nature of allotropes of carbon.
  • Uses of diamond, graphite, coke, coal, soot.
  • Laboratory preparation, properties and uses of carbon dioxide
  • Physical properties of Carbon dioxide.
  • Chemical properties of Carbon Dioxide.
  • Acidic nature.
  • Reaction with lime water.
  • Properties and uses of Carbon monoxide.
  • Emphasis on use as reducing agent in the extraction of iron.
  • Emphasize the harmful properties of Carbon monoxide when inhaled – Asphyxia.
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