Chemistry (English Medium) ICSE Class 9 CISCE Syllabus 2024-25


CISCE ICSE Class 9 Chemistry Syllabus - Free PDF Download

CISCE Syllabus 2024-25 ICSE Class 9: The CISCE ICSE Class 9 Chemistry Syllabus for the examination year 2024-25 has been released by the Council for the Indian School Certificate Examinations, CISCE. The board will hold the final examination at the end of the year following the annual assessment scheme, which has led to the release of the syllabus. The 2024-25 CISCE ICSE Class 9 Chemistry Board Exam will entirely be based on the most recent syllabus. Therefore, students must thoroughly understand the new CISCE syllabus to prepare for their annual exam properly.

The detailed CISCE ICSE Class 9 Chemistry Syllabus for 2024-25 is below.

Academic year:

CISCE ICSE Class 9 Chemistry Revised Syllabus

CISCE ICSE Class 9 Chemistry and their Unit wise marks distribution

CISCE ICSE Class 9 Chemistry Course Structure 2024-25 With Marking Scheme



1 The Language of Chemistry
  • Matter (Substance)  
    • Matter
    • Creation of Matter
    • Physical Nature of matter
    1. The matter is made up of particles
    2. How small is this particles of matter
    3. Colour, odour, melting point, boiling point, density
    • Chemical properties: Composition, combustibility, activity with acids and bases
  • Molecules  
    • Molecule
    • Properties of molecule
  • Pure Substances  
    • Pure substance
    • Characteristics of Pure substance
    • Examples of Pure Substance
  • Elements  
    • Element
    • Characteristics of Element
    • Common Element
    1. In the universe
    2. In the Earth's crust
    3. Elements in the human Body
    4. Elements in air
    • Birth of the Element
  • Classification of Molecules  
  • Symbols Used to Represent Atoms of Different Elements  
  • Valency  
  • Variable Valency  
  • Ions (Radicals) and Its Types  
    • Radicals
    • Types of Radicals
    1. Basic radical
    2. Acid radical
  • Chemical Formula or Molecular Formula  
    • Chemical formulae of compounds : A recapitulation
  • Naming Chemical Compounds  
  • To Calculate the Valency from the Formula  
  • Chemical Equation  
    • Chemical Equation
    • Need for Chemical equation
    • Limitation of Chemical equation
  • Balancing Chemical Equation  
    • Steps in writing the skeleton equation
    • Balancing chemical equation
    • Information conveyed by a balanced chemical equation
    • A chemical equation can be made more informative by writing the additional information. 
  • Atomic Mass  
    • Atomic mass
    • Gram atomic mass
    • Average atomic mass
  • Molecular Mass  
    • Molecular mass
    • Characteristics of molecular mass
    • Gram molecular mass
  • Percentage Composition, Empirical and Molecular Formula  
    • Percentage composition
    • Chemical formula
      1) Empirical formula
      2) Molecular formula
    • Steps involved in determining the empirical formula
    • Steps for determination of the molecular formula of a compound
  • Empirical Formula of a Compound  
  • Hydrogen  
    • Hydrogen
    • Discovery of Hydrogen
    • Occurrence of Hydrogen
2 Chemical Changes and Reactions
  • Classification of Change: Chemical Changes  
    • Chemical Change
    • Properties of Chemical Change
    • Importance of Chemical Change
  • Chemical Reaction  
    • Chemical Reaction
    • Reactants
    • Products
    • Word Equation
    • Characteristics of Chemical Reactions
  • Conditions Necessary for Chemical Reactions  
    • How will you know that a chemical change has taken place?
    1. Close contact
    2. Attraction in the physical state of the reactants (through the solution)
    3. Heat energy
    4. Light energy
    5. Electricity
    6. Pressure
    7. Catalysts: Positive catalyst and Negative catalyst
  • Types of Chemical Change or Chemical Reaction  
    • Direct Combination (or Synthesis) Reaction  
    • Decomposition Reactions  
    • Single Displacement Reactions  
    • Double Displacement Reaction  
  • Energy Change in Chemical Reactions  
    • Energy Change in Chemical Reactions:
    1. Exothermic Chemical Changes
    2. Endothermic Chemical Changes
    3. Photochemical Reaction
    4. Electrochemical Reaction
3 Water
  • Water, Our Lifeline  
    • Introduction
    • Water: A Compound
    • Occurrence of water
  • Physical Properties of Water  
    • Physical Properties of Water:
    1. Nature
    2. Boiling point
    3. The freezing point of water or melting point of ice
    4. Density
    5. Anomalous expansion of water
    6. Latent heat of fusion of ice
    7. Latent heat of vaporization of water
    8. Specific heat capacity
  • Chemical Properties of Water  
    • Chemical properties
    1. Dissociation of water
    2. Amphoteric nature
    3. Oxidising and reducing nature
    4. Hydrolytic reactions
    5. Formation of hydrates with metal salts
  • Water - a Universal Solvent  
    • Universal Solvent
    • Experiment: To show that ordinary tap water contains dissolved solids.
    • Importance of dissolved salts in water.
    • Air dissolved in water.
    • Experiment: To show that tap water contains dissolved gases (air). 
    • Importance of air dissolved in water.
  • Solutions as 'Mixtures' of Solids in Water  
    • Homogeneous mixture
    • Solution
    • Solute
    • Solvent
    • Binary solution
    • Ternary solutions
    • Quaternary solutions
    • Homogeneous solution
    • Solid solution
    • True solution
    • Characteristics of a true solution
  • Components of Solutions  
  • Different Types of Solutions  
    • Different Types of Solutions:
    1. Supersaturated solution
    2. Unsaturated solution
    3. Saturated solution
    4. Aqueous solution
    5. Non-aqueous solution
    6. Dilute solution
    7. Concentrated solution
  • Saturated Solutions  
    • What is a Saturated Solution?
    • How to Prepare a Saturated Solution?
    • Factors affecting the Point of Saturation
    • Effect of cooling and heating of Saturation
    • Everyday Examples of Saturated Solution
  • Concentration of a Solution  
    • Reactions in solutions
    1. Mass percentage
    2. Mole fraction
    3. Molarity
    4. Molality
    5. Volume percentage
  • Solubility  
    • Solubility
    • Factors affecting solubility
    1. Nature of the solute and solvent
    2. Effect of Temperature
    3. Effect of Pressure
    • Solubility curves can be used
    • Determination of the solubility of a solute at a particular temperature 
    • Effect of pressure and temperature on solubility of gases in water (liquids) 
  • Crystals and Crystallisation  
    • Crystals
    • Crystallisation
    • Experiment: To prepare large crystals of copper sulphate.
  • Hydrated and Anhydrous Substances  
  • Efflorescence, Hygroscopic, and Deliquescence Substances  
    • Efflorescence
    • Deliquescence
    • Hygroscopy
  • Drying and Dehydrous Substances  
  • Classification of water: Soft and Hard Water  
    • Soft and Hard water
    • Types of Hard water
    1. Temporary Hardness
    2. Permanent Hardness
  • Causes of Hardness  
  • Advantage and Disadvantage of Hard Water  
  • Removal of Hardness of Water  
    • Softening of water
    1. Removal of temporary hardness
      a) By boiling
      b) Clark's method
    2. Removal of permanent hardness
      a) By washing soda method
      b) lon-exchange/Permutit method
      c) Calgon method
      d) Synthetic resins method
      ⇒ Ion exchange resins are of two types
      i) Cation exchange resins
      ii) Anion exchange resins
    • Degree of hardness of water
  • Salts  
    • Salts
    • Family of Salts
    • pH of Salts
  • Prevention of Water Pollution  
4 Atomic Structure and Chemical Bonding
  • Chemical Bond  
    • Bond
    • Chemical bond
    • Kossel – Lewis approach to chemical bonds
    • Lewis dot structure
  • History of Atom  
  • Dalton’s atomic theory  
  • Elements  
    • Element
    • Characteristics of Element
    • Common Element
    1. In the universe
    2. In the Earth's crust
    3. Elements in the human Body
    4. Elements in air
    • Birth of the Element
  • Atoms: Building Blocks of Matter  
    • Atoms: Building Blocks of Matter
    • How big are atoms?
    • How do atoms exist?
  • Discovery of Charged Particles in Matter  
    • Cathode Ray Tube (CRT) experiment
    • Electrons (e)  
      • Electrons
      • Discovery of Electrons
      • Properties of Cathode rays
      • Charge to Mass Ratio of Electron
      • Charge on the Electron
    • Protons (p)  
      • Protons
      • Discovery of Protons
      • Properties of Anode rays
    • Nucleus  
      • Discovery of Nucleus
      • Deflection of α-particle by a gold leaf
    • Neutrons (n)  
      • Neutrons
      • Discovery of Neutrons
      • Properties of Neutrons
  • J. J. Thomson’s Atomic Model  
  • Lord Rutherford’s Atomic model  
    • Biography of Ernest Rutherford
    • Reason behind discovery of Rutherford’s atomic model
    • Rutherford’s α-particle scattering experiment
    • Observations of α-scattering experiment
    • Conclusions of α-scattering experiment
    • Rutherford's model of an atom
    • Some terminologies related to the α- scattering experiment
      1) Number of scattered particles
      2) Distance of closest approach (Nuclear dimension)
      3) Impact parameter (b)
  • Neils Bohr’s Model of an Atom  
    • Bohr's model of an atom
    • Postulates of Bohr's atomic model
    • Merits of Bohr's model
    • Drawbacks of Bohr's model
  • Structure of an Atom  
  • Atomic Number (Z), Mass Number (A), and Number of Neutrons (n)  
    • Atomic number or Nuclear charge
    • Nucleons
    • Mass number
    • Relationship between atomic number and mass number
    • Representation of element
    • Number of Neutrons (n)
  • Atomic Mass  
    • Atomic mass
    • Gram atomic mass
    • Average atomic mass
  • Electronic Configuration of Atom  
  • Valency Electrons  
  • Reason for Chemical Activity of an Atom  
  • Isotopes  
    • Isotopes
    • Examples
    • Properties of Isotopes
    • Mass of Isotopes
  • Isobars  
    • Isobars
    • Example of Isobars
    • Characteristics of Isobars
  • Electrovalent (or Ionic) Bond  
    • Ionic Bond
    • Electrovalent Bond
    • Electronegativity and Ionic Bonding
    • Ionic Bond Properties
    • Characteristics of Ionic compounds
    • Examples of Ionic Bonds
  • Formation of an Electrovalent (or Ionic) Bond  
    • Conditions for the formation of an electrovalent (or ionic) bond
    • Why Are Ionic Compounds Stable?
    • Structures of some electrovalent compounds
    1. Sodium chloride (NaCl) 
    2. Magnesium chloride (MgCl2
    3. Calcium oxide (CaO)
  • The Covalent Bond  
    • Covalent Bond
    • Covalent Bonding can be Achieved in two Ways
    • Covalent Bonding in Carbon Atom
    • Properties of Covalent Bond
    • Polar Covalent Bond
    • Non-polar Covalent Bond
    • Polarization of Covalent Bonds
  • Types of Covalent Bond  
    • Types of Covalent Bond
    1. Single Covalent Bond
    2. Double Covalent Bond
    3. Triple Bond
  • Formation of Covalent Bond  
    • Formation of Covalent Bond:
    1. Hydrogen molecule (Non-polar compound)
    2. Chlorine molecule (Non-polar compound)
    3. Oxygen molecule (non-polar compound)
    4. Nitrogen molecule (Non-polar compound)
    5. Hydrogen chloride (polar compound)
    6. Water molecule (polar compound)
    7. Ammonia molecule (polar compound)
    8. Carbon tetrachloride molecule (Non-polar compound)
    9. Methane molecule (Non-polar compound)
5 The Periodic Table
  • History of Periodic Table: Early Attempts at the Classification of Elements  
    • Reasons for classification of elements
    • Early Attempts at the Classification of Elements
  • Dobereiner’s Triads  
    • Dobereiner’s Triads
    • Limitations of Dobereiner’s Triads
  • Newland's Law of Octaves  
    • Newlands’ Law of Octaves
    • Limitations of Newlands’ Law of Octaves
  • Mendeleev’s Periodic Table  
    • Mendeleev’s Periodic Table
    • Features of Mendeleev’s Periodic Table
  • Merits and Demerits of Mendeleev’s Periodic Table  
  • Modern Periodic Law  
    • Atomic number as the basis for modern periodic law
  • The Modern Periodic Table  
    • Modern Periodic Table
    • Salient features of the modern periodic table
    1. Features of Periods
    2. Features of Groups
    3. Position of hydrogen in the periodic table
    4. Position of Rare Gases
  • Types of Element on the Basis of Periodic Table  
    • Representative elements
    • Transition elements
    • Inner transition elements
    • Inert gases or noble gases
    • s-Block Elements
    • p-Block Elements
    • d-Block Elements
    • f – Block Elements
  • Advantage and Disadvantage of Modern Periodic Table  
  • Periodic Properties  
    • Periodicity
    • Periodicity of elements
    • Cause of periodicity
    • Periodic Properties: Shells (Orbits)  
    • Periodic Properties: Valency  
    • Periodic Properties: Properties of Elements  
    • Periodic Properties: Atomic Radius Or Atomic Size  
    • Periodic Properties: Metallic Character  
  • Study of Specific Groups in Periodic Table  
    • Group I (Alkali Metals)  
    • Group II (Alkaline Earth Metals)  
    • Group VIIA Or Group 17 (The Halogens)  
    • Group Zero or 18 Group (Noble Gases)  
  • Uses of Periodic Table  
  • Types of Elements: Metals  
    • Metals
    • Occurrence of metal
    • Uses of Metals
6 Study of the First Element - Hydrogen
  • Position of Hydrogen in Periodic Table  
  • Similarities Between Hydrogen and Alkali Metals  
  • Similarities Between Hydrogen and Halogens  
  • Hydrogen  
    • Hydrogen
    • Discovery of Hydrogen
    • Occurrence of Hydrogen
  • Preparation of Hydrogen  
  • Application of Activity Series in the Preparation of Hydrogen  
    • Displacement of hydrogen from dilute acids
    • Displacement of hydrogen from alkalis
  • Laboratory Preparation of Hydrogen  
  • Manufacture of Hydrogen  
    • Manufacture of Hydrogen
    1. Bosch process
    2. By electrolysis of water
  • Physical Properties of Hydrogen  
  • Chemical Properties of Hydrogen  
  • Uses of Hydrogen  
  • Oxidation, Reduction and Redox Reactions  
    • Oxidation
    • Reduction
    • Redox Reactions
    • Oxidising agents and Reducing agents
    • Oxidation reactions in daily life
    • Oxidation number
7 Study of Gas Laws
  • Gases and Its Characteristics  
    • Gases
    • Behaviour and characteristic properties of gases
    1. Composition of gases
    2. Gases have neither a fixed volume nor a fixed shape
    3. Gases exert pressure in all directions
    4. Gases are highly compressible
    5. Gases are highly expansible
    6. Gases have low density
    7. Gases have a natural tendency to mix with one another (diffusion)
    8. Gases can be liquefied
  • Molecular Motion : Relationship of Temperature, Pressure and Volume  
  • The Gas Laws  
    • The Gas Laws
    • Standard variables for gas laws
    1. The volume (V)
    2. The pressure (P)
    3. The temperature (T)
  • Fundamental Laws of Gases  
    • Pressure and Volume Relationship or Bolye's Law  
      • Boyle's law
      • Mathematical expression of Boyle's law
      • Graphical verification of Boyle's law
      • Explanation of Boyle's law in terms of molecular motion (kinetic theory).
      • Significance of Boyle's Law
      • Experiment of Pressure and Volume relationship in gases
    • Temperature - Volume Relationship or Charles's Law  
      • Charle's Law
      • Mathematical expression of Charles's Law
      • Graphical representation of Charle's law
      • Significance of Charle's Law
  • Absolute Zero  
  • Temperatures  
    • Temperature
    • Unit of Temperature
  • Scales of Thermometers  
    1. Fahrenheit scale
    2. Celsius temperature scale
    3. Kelvin scale (Absolute scale)
    • Relationship between the three scales of temperature
    • Conversion of Temperature from celsius scale to kelvin scale and vice-versa
  • Gas Equation  
  • Standard Temperature Pressure (S.T.P.)  
  • The Effect of Moisture and Pressure  
8 Atmospheric Pollution
  • Atmospheric Pollution  
  • Air Pollution and Its Causes  
    • Air Pollution
    • Causes of Air pollution
    • Sources of Air Pollution
  • Effects of Air Pollution  
  • Prevention of Air Pollution  
    • Measures to control air pollution
    • Devices to control air pollution
    1. Electrostatic precipitator (ESP)
    2. Scrubbers
    3. Catalytic converters
  • Gaseous Pollutants and Their Effects  
  • Acid Rain  
    • Acid rain
    • Effects of Acid rain
  • Causes of Acid Rain  
  • Green House Effect  
    • Green House Effect
    • Green House gases
  • Advantage of Green House Effect  
  • Global Warming  
    • Global Warming
    • Causes of Global warming
    • Effect of Global Warming
  • Preventive Measures of Global Warming  
  • Ozone  
    • Ozone
    • Function of ozone in the atmosphere
    • Harmful effects of ozone
  • Ozone Layer Depletion  
    • Depletion of Ozone Layer
    • Chemicals responsible for the destruction of the ozone layer
9 Elements, Compounds and Mixtures
  • Differences Between Elements, Compounds, and Mixtures  
  • Types of Mixtures  
  • Mixture  
  • Separation of Mixtures  
  • Use of Solvent and Filtration  
  • Change of State of Matter  
    • Concept of Evaporation  
      • Factors Affecting Evaporation
      • How does Evaporation cause cooling?
  • Methods of Separation  
    • Simple Distillation Method  
    • Simple Distillation Method  
    • Chromatography Method  
      • Chromatography
      • Types of chromatography
      1. Adsorption chromatography
        i) Column chromatography
        ii) Thin layer chromatography (TLC)
      2. Partition chromatography: paper chromatography
    • Centrifugation Method  
    • Solvent Extraction (Using a Separating Funnel Method)  
12 Matter and Its Composition: Law of Conservation of Mass
  • Change of State of Matter  
  • Inter-particle Space and Interparticle Attraction and Collision  
  • Laws of Chemical Combination  
    • Law of Conservation of Mass  
13 Practical Work
  • Laboratory Preparation of Hydrogen  
  • Laboratory Preparation of Oxygen  
  • Laboratory Preparation of Carbon Dioxide  
  • Laboratory Preparation of Chlorine  
  • Laboratory Preparation of Hydrogen Chloride Gas  
    • Preparation of hydrogen chloride gas from common salt.
    • Purification of HCI gas
  • Laboratory Preparation of Sulphur Dioxide  
  • Laboratory Preparation of Hydrogen Sulphide  
  • Laboratory Preparation of Ammonia Gas  
    • Preparation of ammonia from ammonium chloride and calcium hydroxide.
    • Preparation of ammonia from magnesium nitride.
  • Laboratory Preparation of Water Vapour  
  • Laboratory Preparation of Nitrogen Dioxide  
  • Action of Heat on a Given Substance  
    • Action of heat on Copper carbonate (Green solid)
    • Action of heat on Zinc carbonate (White solid)
    • Action of heat on Washing soda (White crystals)
    • Action of heat on Copper sulphate (Blue crystals)
    • Action of heat on Zinc nitrate (White solid)
    • Action of heat on Copper nitrate (Green solid)
    • Action of heat on Lead nitrate (White solid)
    • Action of heat on Ammonium chloride (White solid)
    • Action of heat on Iodine Violet solid
    • Action of heat on Ammonium dichromate (Orange solid)
  • Action of Dilute Sulphuric Acid on a Given Substance  
    • The action of dilute sulphuric acid on magnesium.
    • The action of dilute sulphuric acid on Zinc.
    • The action of dilute sulphuric acid on Sodium carbonate
    • The action of dilute sulphuric acid on Sodium bicarbonate.
    • The action of dilute sulphuric acid on Iron(II) sulfide
    • The action of dilute sulphuric acid on sodium sulfate
    • The action of dilute sulphuric acid on Potassium sulfite
  • Dry Test  
    • Recognition of Substances by Colour  
    • Recognition of Substances by Odour  
    • Recognition of Substances by Physical State  
      • Table of solubility of salts and bases in water
    • Recognition of Substances by Action of Heat  
      • Identification of solids by the action of heat:
      • Ammonium salt 
      • PbO2, Pb3O4, HgO, KNO3, NaNO3
      • Carbonate and bicarbonate (except K2CO3 and Na2CO3
      • Hydrated salt
      • Sulphite or sulphate
      • Lead compounds decompose to give lead monoxide; PbO
      • Zinc compounds decompose on heating to give zinc oxide 
      • Copper compound decomposes to give black copper oxide CuO.
      • Some naturally occurring acids:
      • Acetic acid
      • Citric acid
      • Butyric acid 
      • Hydrochloric acid
      • Formic acid
      • Lactic acid
      • Malic acid
      • Oleic acid
      • Stearic acid
      • Tartaric acid
      • Uric acid
    • Flame Test  
  • Classification of water: Soft and Hard Water  
    • Soft and Hard water
    • Types of Hard water
    1. Temporary Hardness
    2. Permanent Hardness
  • Simple Experiments Based on Hard Water and Soft Water  
    • Differentiating hard water from soft water.
    • Differentiating between temporary and permanent hard water.
    • Soap and detergents
    • Comparing the effects of soaps and detergents on hard water.
  • Water Pollution and Its Causes  
    • Water Pollution
    • Causes of Water Pollution
    • Sources of Water Pollution
  • Water Quality  
  • Strength of Acidic or Basic Solutions  
    • pH Scale
    • Importance of pH in Everyday Life
  • Prevention of Water Pollution  

Textbook SolutionsVIEW ALL [3]


      Forgot password?
Use app×