ICSE Class 9 Syllabus 2028 Chemistry

ICSE
INDIAN CERTIFICATE OF
SECONDARY EDUCATION
EXAMINATION
YEAR 2028

SCIENCE
CHEMISTRY
(52)

Developed by:
Research, Development and Curriculum Division (RDCD)
CISCE

January 2026
____________________________________________________________________________________________

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SCIENCE (52)
CHEMISTRY

SCIENCE Paper - 2

Aims:
1. To acquire the knowledge of terms, concepts, processes, techniques and principles related to the subject.
2. To develop the ability to apply the knowledge of contents and principles of chemistry in unfamiliar situations.
3. To acquire skills in proper handling of apparatus and chemicals.
4. To foster scientific temper, ethical attitude, moral values and problem-solving skills for making informed and
responsible decisions.
5. To establish linkages between scientific knowledge and other curricular areas.
6. To appreciate India’s knowledge traditions and its connection to scientific ideas.
7. To recognise Chemical Science as having an important impact on the environment relating to cycles in nature;
natural resources, pollution.

CLASS IX
There will be one paper of two hours duration of 80 marks, and Internal Assessment of practical work carrying
20 marks.
Note: All chemical processes/reactions should be studied with reference to the reactants, products, conditions,
observations and the (balanced) equations and diagrams.

1. The Language of Chemistry
(i) Symbol of an element; valency; representation of radicals and formulae of compounds. Balancing of
simple chemical equations.
• Symbol – definition; symbols of the elements used often.
• Valency - definition; hydrogen combination and number of valence electrons of the metals and non-
metals; mono, di, tri and tetra valent elements.
• Radicals – definition; formulae formation, reactivity of radicals, and valencies. Existence of radicals
in atmosphere, their effects on living organisms. Reduction or elimination.
• Compounds – name and formulae.
• Chemical equation – definition and examples of chemical equations with one reactant and two or
three products, two reactants and one product, two reactants and two products and two reactants and
three or four products; balancing of equations (by hit and trial method).
(ii) Relative Atomic Masses (atomic weights) and Relative Molecular Masses (molecular weights): either -
standard H atom or 1/12th of carbon 12 atom.
• Definitions.
• Calculation of Relative Molecular Mass and percentage composition of a compound.

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2. Chemical changes and reactions
(i) Types of chemical changes.
• Direct combination
• Decomposition
• Displacement
• Double decomposition/Double displacement
(Double Displacement Reaction of Sodium Sulphate with Barium Chloride; Reaction of Silver Nitrate
with Sodium Chloride; Reaction of Lead Nitrate with Potassium Iodide.)
(The above to be taught with suitable chemical equations as examples followed by demonstration).
(ii) Energy changes in a chemical change.
Exothermic and endothermic reactions with examples – evolution/absorption of heat, light and electricity.

3. Water
(i) Water as a universal solvent.
• Mixtures, solutions, colloids and suspensions.
• Solutions as 'mixtures' of solids in water; saturated, unsaturated and supersaturated solutions.
• Qualitative effect of temperature on solubility along with solubility curve (e.g. solutions of calcium
sulphate, potassium nitrate and sodium chloride in water).
(ii) Water of Crystallisation-Definition only.
(a) Hydrated substances: meaning and examples (CuSO 4 . 5H 2 O, FeSO 4 . 7H 2 O, Na 2 CO 3 . 10H 2 O,
Na 2 SO 4 .10H 2 O).
(b) Anhydrous substances.
Meaning and examples only (NaNO 3 , KCl, PbCl 2 , K 2 SO 4 ).
(c) Properties.
• Efflorescence- definition and examples like Washing soda- Na 2 CO 3 .10H 2 O.
• Deliquescence- definition and examples like Ferric chloride – FeCl 3.
• Hygroscopy – definition and examples like Quick lime - CaO, concentrated Sulphuric acid-
H 2 SO 4.
(iii) Drying Agents- meaning and examples like Quick lime- CaO and Dehydrating Agents- meaning and
examples like concentrated Sulphuric acid- H 2 SO 4 .
(iv) Soft water and Hard water.
• Meaning (in terms of action of soap).
• Advantages and disadvantages of soft water and hard water.
• Types and causes of hardness.
(v) Removal of Temporary and Permanent hardness.
• Removal of hardness
(i) By boiling
(ii) By addition of washing soda
• Making water potable- Filtration, Chlorination, Defluoridation, Role of Alum in purification of
water. Common diseases due to polluted water-diarrhoea, typhoid, cholera, dysentery, hepatitis A,
polio, cancer and organ damage.

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4. Atomic Structure and Chemical bonding
(i) Structure of an Atom, discovery of nucleus, electrons, Rutherford’s and Bohr’s model of an atom, mass
number and atomic number, Isotopes and Octet Rule.
• Definition of an atom.
• Constituents of an atom - nucleus (protons, neutrons) with associated electrons; mass number, atomic
number.
• Rutherford’s experiment (gold foil), the conclusions, merits and demerits.
• Bohr’s model- Simplified form (Mathematical expressions not required).
• Electron distribution in the orbits - 2n2 rule, Octet rule. Reason for chemical activity of an atom.
• Definition and examples of isotopes (hydrogen, carbon, chlorine).
(ii) Electrovalent and covalent bonding, ions and electrons, radicals, structures of various
compounds – orbit structure.
(a) Electrovalent Bond.
• Definition
• Ion formation
• Atomic orbit structure for the formation of Electrovalent compounds (e.g. NaCl, MgCl 2 , CaO)
(b) Covalent Bond.
• Definition
• Atomic orbit structure for the formation of Covalent molecules on the basis of duplet and octet
of electrons (examples: hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water,
ammonia, carbon tetrachloride, methane).
• Radical formation on breaking a covalent bond.

5. The Periodic Table
Dobereiner’s Triads, Newland’s law of Octaves, Mendeleev’s contributions; Modern Periodic Law, the
Modern Periodic Table (Groups and periods).
• General idea of Dobereiner’s triads, Newland’s law of Octaves, Mendeleev’s periodic law-limited to
principles, examples, merits and limitations.
• Discovery of Atomic Number and its use as a basis for Modern Periodic law.
• Modern Periodic Table (Groups 1 to 18 and periods 1 to 7).
(Placement of Transition and Inner transition elements to be mentioned).
• Special reference to Alkali metals (Group 1), Alkaline Earth metals (Group 2), Halogens (Group 17) and
Zero Group (Group 18).

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6. Study of the First Element -Hydrogen
Position of the non-metal (Hydrogen) in the periodic table and general group characteristics with reference to
valency electrons, burning, ion formation applied to the above-mentioned element.
(i) Hydrogen from: water, dilute acids and alkalis.
(a) Hydrogen from water.
• The action of cold water on sodium, potassium and calcium.
• The action of hot water on magnesium.
• The action of steam on aluminium, zinc, and red-hot iron; (reversibility of reaction between iron
and steam).
• The action of steam on non-metal (carbon).
Students can be shown the action of sodium and calcium on water in the laboratory. They must
be asked to make observations and write equations for the above reactions. Application of
activity series for the above-mentioned reactions.
(b) Displacement of hydrogen from dilute acids.
• The action of dilute sulphuric acid or hydrochloric acid on metals: Mg, Al, Zn and Fe.
• Reasons for not using other metals and dilute nitric acid.
(c) Displacement of hydrogen from alkalis.
The action of Alkalis ((NaOH, KOH) on Al, Zn and Pb – unique nature of these elements.
(ii) The preparation and collection of hydrogen by a standard laboratory method other than electrolysis.
The reason for using zinc in the laboratory preparation, the removal of impurities in the hydrogen gas,
the precautions during the collection of the gas.
(iii) Industrial manufacture of hydrogen by Bosch process.
• Main reactions and conditions.
• Separation of CO 2 and CO from hydrogen.
(iv) Oxidation and reduction reactions.
Differences in terms of addition and removal of oxygen / hydrogen.
• Electronic concept (Gain/loss of electrons).
• Oxidizing and Reducing agents.
• Redox reaction.

7. Study of Gas Laws
(i) The behaviour of gases under changes of temperature and pressure; explanation in terms of molecular
motion (particles, atoms, molecules); Boyle’s Law, Charles’s Law and absolute zero; gas equation; simple
relevant calculations.
• The behaviour of gases under changes of temperature and pressure; explanation in terms of
molecular motion (particles, atoms, molecules).
• Mathematical derivation & Graphical representation of Boyle’s Law: statement, mathematical form,
simple calculations.
• Mathematical derivation & Graphical representation of Charles’s Law: statement, mathematical
form, simple calculations.
• Absolute zero on Kelvin scale of temperature.
• Gas equation P 1 V 1 / T 1 = P 2 V 2 / T 2 ; simple relevant calculations based on gas equation.

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(ii) Relationship between Kelvin scale and Celsius Scale of temperature; Standard temperature and pressure.
Conversion of temperature from Celsius Scale to Kelvin scale and vice versa. Standard temperature and
pressure (Simple calculations on conversion of temperature and on standard temperature and pressure).

8. Atmospheric and Environmental Chemistry
Atmospheric Pollution.
(a) Acid Rain- Composition, cause and its impact.
Sulphur in fossil fuels giving oxides of sulphur when burnt. High temperatures in furnaces and internal
combustion engines produce oxides of nitrogen. (Equations to be included.). Effects of acid rain on soil
chemistry and water bodies.
(b) Global warming.
Greenhouse gases-their sources and ways of reducing their presence in the atmosphere.
(Water Vapour, carbon dioxide, methane and oxides of nitrogen.)
(c) Ozone depletion.
• Formation of ozone- relevant equations.
• Functions of ozone in the atmosphere.
• Destruction of the ozone layer- Chemicals responsible for this to be named but reactions not required.
Water Pollution.
Water – composition and substances that are present in it, beneficial and potentially harmful to life.
• Benefits: Dissolved oxygen for aquatic life, essential minerals for life.
• Harmful: Contamination with toxic heavy metals (Special mention to ‘Minamata disease’); plastics;
sewage, pesticides in water bodies.

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INTERNAL ASSESSMENT OF PRACTICAL WORK
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 listed below.
Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide,
Ammonia, Water vapour, Nitrogen dioxide.
Candidates are expected to have completed the following minimum practical work.
Simple experiments on:
1. Action of heat on the following compounds.
(a) copper carbonate, zinc carbonate
(b) washing soda, copper sulphate crystals
(c) zinc nitrate, copper nitrate, lead nitrate
(d) ammonium chloride, iodine, ammonium dichromate
Make observations, identify the products and make deductions where possible.
2. Apply the flame test to identify the metal in the unknown substance.
(a) a sodium salt
(b) a potassium salt
(c) a calcium salt
(d) a copper salt
3. Simple experiments based on hard water and soft water – identification of hardness – simple softening – by
heating the temporary hard water, using washing soda and advantage of using detergents over soap in hard
water.
4. Experiments related to Double Displacement Reaction (examples).
(a) Reaction of Sodium Sulphate with Barium Chloride.
(b) Reaction of Silver Nitrate with Sodium Chloride.
(c) Reaction of Lead Nitrate with Potassium Iodide.
5. Find out the sources of pollution of water bodies in the locality. Suggest preventive steps to control it.

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