ICSE Class 9 Syllabus 2027 Chemistry

ICSE YEAR 2027

INDIAN CERTIFICATE OF
SECONDARY EDUCATION
EXAMINATION

SCIENCE (52)
CHEMISTRY

February 2025
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SCIENCE (52)
CHEMISTRY

SCIENCE Paper - 2
Aims:
3. To acquire skills in proper handling of apparatus
1. To acquire the knowledge of terms, concepts, and chemicals.
processes, techniques and principles related to the
subject. 4. To develop scientific temper, attitude and
problem-solving skills.
2. To develop the ability to apply the knowledge of
contents and principles of chemistry in unfamiliar 5. To recognize Chemical Science as having an
situations. 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 reactants and three or four products;
80 marks and Internal Assessment of practical work balancing of equations. (by hit and trial
carrying 20 marks. method).
Note: All chemical processes/reactions should be
studied with reference to the reactants, products,
(ii) Relative Atomic Masses (atomic weights)
conditions, observations and the (balanced)
and Relative Molecular Masses (molecular
equations and diagrams.
weights): either - standard H atom or 1/12th
of carbon 12 atom.
1. The Language of Chemistry
• Definitions
(i) Symbol of an element; valency; formulae of
radicals and formulae of compounds. • Calculation of Relative Molecular Mass
Balancing of simple chemical equations. and percentage composition of a
compound.
• Symbol – definition; symbols of the
elements used often. 2. Chemical changes and reactions
• Valency - definition; hydrogen (i) Types of chemical changes.
combination and number of valence • Direct combination
electrons of the metals and non-metals; • Decomposition
mono, di, tri and tetra valent elements.
• Displacement;
• Radicals – definition; formulae and • Double decomposition
valencies.
(The above to be taught with suitable
• Compounds – name and formulae. chemical equations as examples).
• Chemical equation – definition and (ii) Energy changes in a chemical change.
examples of chemical equations with
Exothermic and endothermic reactions with
one reactant and two or three products,
examples – evolution/absorption of heat,
two reactants and one product, two
light and electricity.
reactants and two products and two
1
ICSE Examination Year 2027

3. Water electrons; mass number, atomic
number.
(i) Water as a universal solvent.
• Solutions as 'mixtures' of solids in • Electron distribution in the orbits - 2n2
water; saturated solutions. rule, Octet rule. Reason for chemical
activity of an atom.
• Qualitative effect of temperature on
solubility (e.g. solutions of calcium • Definition and examples of isotopes
sulphate, potassium nitrate and (hydrogen, carbon, chlorine).
sodium chloride in water). (ii) Electrovalent and covalent bonding,
(ii) Hydrated and anhydrous substances. structures of various compounds – orbit
structure
(a) Hydrated substances:
(a) Electrovalent Bond
Water of Crystallisation – meaning
and examples. • Definition
(b) Anhydrous substances: • Atomic orbit structure for the
Meaning and examples only formation of Electrovalent
compounds (e.g. NaCl, MgCl 2 ,
(c) Properties: CaO);
• Efflorescence (b) Covalent Bond
• Deliquescence • Definition
• Hygroscopy
• Atomic orbit structure for the
• Removal of hardness formation of Covalent molecules on
(i) By boiling the basis of duplet and octet of
electrons (examples: hydrogen,
(ii) By addition of washing chlorine, oxygen, nitrogen,
soda hydrogen chloride, water,
(Definition and examples of each of the ammonia, carbon tetrachloride,
above). methane.)
(iii) Drying and Dehydrating Agents 5. The Periodic Table
Meaning and examples only. Dobereiner’s Triads, Newland’s law of Octaves,
(iv) Soft water and Hard water Mendeleev’s contributions; Modern Periodic
Law, the Modern Periodic Table. (Groups and
• Meaning, (in terms of action of periods)
soap)
• General idea of Dobereiner’s triads,
• Advantages and disadvantages of Newland’s law of Octaves, Mendeleev’s
soft water and hard water. periodic law.
• Types and causes of hardness. • Discovery of Atomic Number and its use as
4. Atomic Structure and Chemical bonding a basis for Modern Periodic law.
(i) Structure of an Atom, mass number and • Modern Periodic Table (Groups 1 to 18 and
atomic number, Isotopes and Octet Rule. periods 1 to 7).
• Definition of an atom • Special reference to Alkali metals (Group 1),
Alkaline Earth metals (Group 2) Halogens
• Constituents of an atom - nucleus (Group 17) and Zero Group (Group 18).
(protons, neutrons) with associated

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6. Study of the First Element -Hydrogen (iii) Industrial manufacture of hydrogen by
Position of the non-metal (Hydrogen) in the Bosch process.
periodic table and general group characteristics • Main reactions and conditions.
with reference to valency electrons, burning, ion
formation applied to the above-mentioned • Separation of CO 2 and CO from
element. hydrogen.

(i) Hydrogen from: water, dilute acids and (iv) Oxidation and reduction reactions.
alkalis. Differences in terms of addition and
(a) Hydrogen from water: removal of oxygen / hydrogen.

• The action of cold water on sodium 7. Study of Gas Laws
potassium and calcium. (i) The behaviour of gases under changes of
• The action of hot water on temperature and pressure; explanation in
terms of molecular motion (particles, atoms,
magnesium.
molecules); Boyle’s Law and Charles’ Law;
• The action of steam on aluminium, absolute zero; gas equation; simple relevant
zinc, and iron; (reversibility of calculations.
reaction between iron and steam).
• The behaviour of gases under changes
• The action of steam on non-metal of temperature and pressure;
(carbon). explanation in terms of molecular
Students can be shown the action of motion (particles, atoms, molecules).
sodium and calcium on water in the • Boyle’s Law: statement, mathematical
laboratory. They must be asked to form, simple calculations.
make observations and write
• Charles’ Law: statement,
equations for the above reactions. mathematical form, simple
Application of activity series for the calculations.
above-mentioned reactions.
• Absolute zero Kelvin scale of
(b) Displacement of hydrogen from dilute temperature.
acids.
• Gas equation P 1 V 1 / T 1 = P 2 V 2 / T 2 ;
The action of dilute sulphuric acid or simple relevant calculations based on
hydrochloric acid on metals: Mg, Al, Zn gas equation.
and Fe .
(ii) Relationship between Kelvin scale and
(To understand reasons for not using Celsius Scale of temperature; Standard
other metals and dilute nitric acid.) temperature and pressure.
(c) Displacement of hydrogen from alkalis. Conversion of temperature from Celsius
The action of Alkalis (NaOH, KOH) on Scale to Kelvin scale and vice versa.
Al, Zn and Pb – unique nature of these Standard temperature and pressure. (Simple
elements. calculations).
(ii) The preparation and collection of hydrogen 8. Atmospheric pollution
by a standard laboratory method other than (a) Acid rain – composition, cause and its
electrolysis. impact.
In the laboratory preparation, the reason
Sulphur in fossil fuels giving oxides of
for using zinc, the impurities in the gas, sulphur when burnt. High temperatures in
their removal and the precautions in the furnaces and internal combustion engines
collection of the gas must be mentioned.

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produce oxides of nitrogen. (Equations to Simple experiments on:
be included). Acid rain affects soil
1. Action of heat on the following compounds:
chemistry and water bodies.
(a) copper carbonate, zinc carbonate
(b) Global warming:
Greenhouse gases – their sources and ways (b) washing soda, copper sulphate crystals
of reducing their presence in the (c) zinc nitrate, copper nitrate, lead nitrate
atmosphere.
(d) ammonium chloride, iodine, ammonium
(Water vapour, carbon dioxide, methane dichromate
and oxides of nitrogen)
Make observations, identify the products and
(c) Ozone depletion make deductions where possible.
• Formation of ozone – relevant
2. Action of dilute sulphuric acid on the following
equations
substances. (warm if necessary)
• Function in the atmosphere.
(a) a metal
• Destruction of the ozone layer –
chemicals responsible for this to be (b) a carbonate
named but reactions not required. (c) a sulphide
(d) a sulphite
INTERNAL ASSESSMENT OF
PRACTICAL WORK Make observations, identify the gas evolved and
make deductions.
Candidates will be asked to observe the effect of
3. Apply the flame test to identify the metal in the
reagents and/or of heat on substances supplied to
unknown substance.
them. The exercises will be simple and may include
the recognition and identification of certain gases (a) a sodium salt
listed below. (b) a potassium salt
Gases: Hydrogen, Oxygen, Carbon dioxide,
(c) a calcium compound
Chlorine, Hydrogen chloride, Sulphur dioxide,
Hydrogen sulphide, Ammonia, Water vapour, 4. Simple experiments based on hard water and soft
Nitrogen dioxide. water – identification of hardness – simple
softening – by heating the temporary hard water,
Candidates are expected to have completed the using washing soda and advantage of using
following minimum practical work.
detergents over soap in hard water.
5. Find out the sources of pollution of water bodies
in the locality. Suggest preventive steps to
control it.

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