ICSE Class 10 Syllabus 2027 Chemistry

ICSE YEAR 2027

INDIAN CERTIFICATE OF
SECONDARY EDUCATION
EXAMINATION

SCIENCE (52)
CHEMISTRY

February 2025
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children, through high quality educational
endeavours, empowering them to contribute towards
a humane, just and pluralistic society, promoting
introspective living, by creating exciting learning
opportunities, with a commitment to excellence.

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Minimum monitoring.
Allowing schools to evolve their own niche.
Catering to the needs of the children.
Giving freedom to experiment with new ideas
and practices.
Diversity and plurality - the basic strength for
evolution of ideas.
Schools to motivate pupils towards the
cultivation of:
Excellence - The Indian and Global
experience.
Values - Spiritual and cultural - to be the bedrock
of the educational experience.
Schools to have an 'Indian Ethos', strong roots in
the national psyche and be sensitive to national
aspirations.

CLASS X
There will be one paper of two hours duration of • Characteristic properties of electrovalent
80 marks and Internal Assessment of practical work compounds – state of existence, melting
carrying 20 marks. and boiling points, conductivity (heat and
Note: All chemical processes/reactions should be electricity), dissociation in solution and in
studied with reference to the reactants, products, molten state to be linked with electrolysis.
conditions, observations and the (balanced) equations (b) Covalent Bonding:
and diagrams.
• Electron dot structure of covalent
1. Periodic Properties and variations of Properties molecules on the basis of duplet and octet
– Physical and Chemical of electrons

(i) Periodic properties and their variations in • Non-polar covalent compounds (example:
groups and periods. hydrogen, chlorine, oxygen, nitrogen,
carbon tetrachloride, methane.)
Definitions and trends of the following
periodic properties in groups and periods • Polar Covalent compounds – based on
should be studied: difference in electronegativity:
• atomic size Examples – HCl, NH 3 and H 2 O including
• metallic character structures.
• non-metallic character • Characteristic properties of Covalent
• ionisation potential compounds – state of existence, melting
and boiling points, conductivity (heat and
• electron affinity
electricity), ionisation in solution.
• electronegativity
Comparison of Electrovalent and
(ii) Periodicity on the basis of atomic number for Covalent compounds.
elements.
(c) Coordinate Bonding:
• The study of modern periodic table up to
period 4 (students to be exposed to the • Definition
complete modern periodic table but no • The lone pair effect of the oxygen atom of
questions will be asked on elements the water molecule and the nitrogen atom
beyond period 4 – Calcium); of the ammonia molecule to explain the
• Periodicity and other related properties formation of H 3 O+ and OH- ions in water
to be explained on the basis of nuclear and NH 4 + ion.
charge and shells (not orbitals). The meaning of lone pair; the formation of
(Special reference to the alkali metals and halogen hydronium ion and ammonium ion must be
groups). explained with the help of electron dot
diagrams.
2. Chemical Bonding
Electrovalent, covalent and co-ordinate bonding, 3. Study of Acids, Bases and Salts
structures of various compounds, Electron dot (i) Simple definitions in terms of the molecules
structure. and their characteristic properties.
(a) Electrovalent bonding: (ii) Ions present in mineral acids, alkalis and salts
• Electron dot structure of Electrovalent and their solutions; use of common acid-base
compounds NaCl, MgCl 2 , CaO. indicator (litmus, methyl orange and
phenolphthalein) and pH paper to test for
acidity and alkalinity.

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• Examples with equation for the On solution of salts:
ionisation/dissociation of ions of acids, • Colour of salt and its solution.
bases and salts. • Action on addition of Sodium
• Acids form hydronium ions (only positive Hydroxide to solution of Fe, Cu, Zn,
ions) which turn blue litmus red, alkalis and Pb salts drop by drop in excess.
form hydroxyl ions (only negative ions) Formation and colour of hydroxide
with water which turns red litmus blue. precipitated to be highlighted with the
help of equations.
• Salts are formed by partial or complete • Action on addition of Ammonium
replacement of the hydrogen ion of an acid Hydroxide to solution of Fe, Cu, Zn,
by a metal. (To be explained with suitable and Pb salts drop by drop in excess.
examples). Formation and colour of hydroxide
• Introduction to pH scale to test for acidity, precipitated to be highlighted with the
neutrality and alkalinity by using pH paper help of equations.
or Universal indicator. • Special action of Ammonium
(iii) Definition of salt; types of salts. Hydroxide on solutions of copper
salts and sodium hydroxide on
Types of salts: normal salts, acid salt, basic ammonium salts.
salt, complex salts (definition and examples).
(ii) Action of alkalis (NaOH, KOH) on certain
(iv) Action of dilute acids on salts.
metals, their oxides and hydroxides.
Decomposition of hydrogen carbonates,
The metals must include aluminium, zinc
carbonates, hydrogen sulphites, sulphites
and lead, their oxides and hydroxides,
and sulphides by appropriate acids with
which react with caustic alkalis (NaOH,
heating if necessary. (Relevant laboratory
KOH), showing the amphoteric nature of
work must be done).
these substances.
(v) Methods of preparation of Normal salts with
relevant equations. (Details of apparatus or 5. Mole Concept and Stoichiometry
procedures not required). (i) Gay Lussac’s Law of Combining Volumes;
Avogadro’s Law.
Methods included are:
• Idea of mole – a number just as a dozen, a
• Direct combination
gross (Avogadro’s number).
• Displacement
• Avogadro’s Law - statement and
• Precipitation (double decomposition) explanation.
• Neutralization of insoluble base • Gay Lussac’s Law of Combining Volumes.
• Neutralisation of an alkali (titration) – Statement and explanation.
• Action of dilute acids on carbonates and • Understanding molar volume- “the mass
bi-carbonates. of 22.4 litres of any gas at S.T.P. is equal
to its molar mass”. (Questions will not be
4. Analytical Chemistry set on formal proof but may be taught for
(i) Action of Ammonium Hydroxide and clear understanding).
Sodium Hydroxide on solution of salts: • Simple calculations based on the molar
colour of salt and its solution; formation volume and Gay Lussac’s law.
and colour of hydroxide precipitated for
solutions of salts of Fe, Cu, Zn and Pb; (ii) Refer to the atomicity of hydrogen, oxygen,
special action of ammonium hydroxide on nitrogen and chlorine (proof not required).
solutions of copper salt and sodium
hydroxide on ammonium salts. The explanation can be given using equations
for the formation of HCl, NH 3 , and NO.

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(iii) Vapour Density and its relation to relative (iv) An elementary study of the migration of ions,
molecular mass: with reference to the factors with examples
influencing selective discharge of ions
• Molecular mass = 2×vapour density
(reference should be made to the activity
(formal proof not required)
series as indicating the tendency of metals,
• Deduction of simple (empirical) and e.g. Na, Mg, Fe, Cu, to form ions) illustrated
molecular formula from: by the electrolysis of:
(a) the percentage composition of a • Molten lead bromide
compound.
• acidified water with platinum electrodes
(b) the masses of combining elements.
• Aqueous copper (II) sulphate with copper
(iv) Mole and its relation to mass. electrodes and platinum electrodes;
• Relating mole and atomic mass; arriving electron transfer at the electrodes.
at gram atomic mass and then gram The above electrolytic processes can be
atom; atomic mass is a number dealing studied in terms of electrolyte used,
with one atom; gram atomic mass is the electrodes used, ionization reaction, anode
mass of one mole of atoms. reaction, cathode reaction, use of selective
discharge theory, wherever applicable.
• Relating mole and molecular mass
arriving at gram molecular mass and (v) Applications of electrolysis.
gram molecule – molecular mass is a
• Electroplating with nickel and silver,
number dealing with a molecule, gram
choice of electrolyte for electroplating
molecular mass is the mass of one mole
(nickel sulphate solution and sodium
of molecules.
argentocyanide).
• Simple calculations based on relation of
• Electro refining of copper.
mole to mass, volume and Avogadro’s
number. Reasons and conditions for electroplating;
names of the electrolytes and the electrodes
(v) Simple calculations based on chemical
used should be given. Equations for the
equations
reactions at the electrodes should be given
Related to weight and/or volumes of both for electroplating, refining of copper.
reactants and products.
7. Metallurgy
6. Electrolysis
(i) Occurrence of metals in nature:
(i) Electrolytes and non-electrolytes.
• Mineral and ore - Meaning and definition.
Definitions and examples.
• Common ores of iron, aluminium and
(ii) Substances containing molecules only, ions zinc.
only, both molecules and ions.
(ii) Stages involved in the extraction of metals.
• Substances containing molecules only
ions only, both molecules and ions. (a) Pulverization and dressing of the ore –
hydrolytic method, magnetic separation,
• Examples; relating their composition with froth flotation method.
their behaviour as strong and weak
electrolytes as well as non-electrolytes. (b) Conversion of concentrated ore to its
oxide- roasting and calcination
(iii) Definition and explanation of electrolysis, (definition, examples with equations).
electrolyte, electrode, anode, cathode, anion,
cation, oxidation and reduction (on the basis (c) Reduction of metallic oxides- some can be
of loss and gain of electrons). reduced by hydrogen, carbon and carbon

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monoxide (e.g. copper oxide, lead (II) • Solubility of hydrogen chloride (fountain
oxide, iron (III) oxide and zinc oxide) and experiment); setting of the apparatus,
some cannot (e.g. Al 2 O 3 , MgO). Active procedure, observation, inference.
metals by electrolysis e.g. sodium,
potassium and calcium. • Method of preparation of hydrochloric
acid by dissolving the gas in water- the
Equations with conditions should be special arrangement and the mechanism
given. by which the back suction is avoided
(d) Electro refining – reference only. should be learnt.
• Reaction with ammonia
(iii) Extraction of Aluminium.
• Acidic properties of its solution - reaction
(a) Chemical method for purifying bauxite by
with metals, their oxides, hydroxides and
using NaOH – Baeyer’s Process only.
carbonates to give their chlorides;
(b) Electrolytic extraction – Hall Heroult’s decomposition of carbonates, hydrogen
process only: carbonates, sulphides, sulphites.
Structure of electrolytic cell - the • Aqua regia composition and uses.
various components as part of the • Precipitation reactions with silver nitrate
electrolyte, electrodes and electrode solution and lead nitrate solution.
reactions.
• Tests for HCl gas and Hydrochloric acid.
Description of the changes occurring,
purpose of the substances used and the B. Ammonia
main reactions with their equations. Ammonia: its laboratory preparation from
(iv) Alloy and Amalgam – composition and uses. ammonium chloride and collection; ammonia
from nitrides like Mg 3 N 2 and AlN and
Composition and uses of Stainless steel, ammonium salts. Manufacture by Haber’s
magnalium, duralumin, brass, bronze, fuse Process; density and solubility of ammonia
metal / solder. (fountain experiment); aqueous solution of
8. Study of Compounds ammonia; its reactions with hydrogen chloride
and with hot copper (II) oxide, lead (IV) oxide
A. Hydrogen Chloride and chlorine; the burning of ammonia in
Hydrogen chloride: preparation of hydrogen oxygen; uses of ammonia.
chloride from sodium chloride; refer to the • Laboratory preparation from ammonium
density and solubility of hydrogen chloride chloride and collection; (the preparation
(fountain experiment); reaction with to be studied in terms of, setting of the
ammonia; acidic properties of its solution. apparatus and diagram, procedure,
• Preparation of hydrogen chloride from observation, collection and identification)
sodium chloride; the laboratory method • Ammonia from nitrides like Mg 3 N 2 and
of preparation can be learnt in terms of AlN using warm water.
reactants, product, condition, equation,
Ammonia from ammonium salts using
diagram or setting of the apparatus,
alkalies.
procedure, observation, precaution,
collection of the gas and identification. The reactions to be studied in terms of
reactants, products, conditions and
• Simple experiment to show the density of equations.
the gas (Hydrogen Chloride) –heavier
than air. • Manufacture by Haber’s Process.
• Density and solubility of ammonia
(fountain experiment).

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• The burning of ammonia in oxygen. D. Sulphuric Acid
• The catalytic oxidation of ammonia Large scale preparation, its behaviour as an
(with conditions and reaction) acid when dilute, as an oxidizing agent when
• Its reactions with hydrogen chloride and concentrated - oxidation of carbon and
with hot copper (II) oxide, lead (IV) oxide sulphur; as a dehydrating agent - dehydration
and chlorine (both chlorine in excess and of sugar and copper (II) sulphate crystals; its
ammonia in excess). non-volatile nature.

All these reactions may be studied in terms of • Manufacture by Contact Process
reactants, products, conditions, equations Equations with conditions where
and observations. applicable).

• Aqueous solution of ammonia - reaction • Its behaviour as an acid when dilute -
with sulphuric acid, nitric acid, reaction with metal, metal oxide,
hydrochloric acid and solutions of hydroxide, carbonate, hydrogen
iron(III) chloride, iron(II) sulphate, lead carbonate, sulphite, hydrogen sulphite
nitrate, zinc nitrate and copper sulphate. and sulphide.

• Uses of ammonia - manufacture of • Sulphuric acid as dibasic acid.
fertilizers, explosives, nitric acid, • Concentrated sulphuric acid as an
refrigerant gas (Chlorofluro carbon – and oxidizing agent - the oxidation of carbon
its suitable alternatives which are non- and sulphur.
ozone depleting), and cleansing agents.
• Concentrated sulphuric acid as a
• Tests for ammonia. dehydrating agent- (a) the dehydration of
C. Nitric Acid sugar (b) Copper (II) sulphate crystals.
Nitric Acid: one laboratory method of • Non-volatile nature of sulphuric acid -
preparation of nitric acid from potassium reaction with sodium or potassium
nitrate or sodium nitrate. Large scale chloride and sodium or potassium nitrate.
preparation. Nitric acid as an oxidizing agent. • Tests for sulphuric acid.
• Laboratory preparation of nitric acid 9. Organic Chemistry
from potassium nitrate or sodium nitrate;
the laboratory method to be studied in (i) Introduction to Organic compounds.
terms of reactants, products, conditions, • Unique nature of Carbon atom – tetra
equations, setting up of apparatus, valency, catenation.
diagram, precautions, collection and
identification. • Formation of single, double and triple
bonds, straight chain, branched chain,
• Manufacture of Nitric acid by Ostwald’s cyclic compounds (only benzene
process (Only equations with conditions structure).
where applicable).
(ii) Structure and Isomerism.
• As an oxidising agent: its reaction with
copper, carbon, sulphur. • Structure of compounds with single,
double and triple bonds.
• Acidic properties of its solution – reaction
with magnesium and manganese, oxides, • Structural formulae of hydrocarbons.
hydroxides, carbonates, hydrogen Structural formula must be given for:
carbonate, sulphites and hydrogen alkanes, alkenes, alkynes up to 5 carbon
sulphites. atoms.
• Test for nitric acid. • Isomerism – structural (chain, position)

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(iii) Homologous series – characteristics with • Preparation of ethanol by hydrolysis of
examples. alkyl halide.
Alkane, alkene, alkyne series and their • Properties – Physical: Nature, Solubility,
gradation in properties and the relationship Density, Boiling Points. Chemical:
with the molecular mass or molecular Combustion, action with sodium, ester
formula. formation with acetic acid, dehydration
with conc. Sulphuric acid to prepare
ethene.
(iv) Simple nomenclature.
• Denatured, methylated alcohol or spirit
Simple nomenclature of the hydrocarbons and spurious alcohol.
with simple functional groups – (halides,
double bond, triple bond, alcoholic, • Important uses of Ethanol.
aldehydic, carboxylic ketone, ether and ester) (vii) Carboxylic acids (aliphatic - mono carboxylic
longest chain rule and smallest number for acid): Acetic acid – properties and uses of
functional groups rule – trivial and IUPAC acetic acid.
names (compounds with only one functional
group). • Structure of acetic acid.
(v) Hydrocarbons: alkanes, alkenes, alkynes. • Properties of Acetic Acid: Physical
properties – odour (vinegar), glacial acetic
• Alkanes - general formula; methane acid (effect of sufficient cooling to produce
(greenhouse gas) and ethane - methods of ice like crystals). Chemical properties –
preparation from sodium ethanoate action with litmus, alkalis and alcohol (idea
(sodium acetate), sodium propanoate of esterification).
(sodium propionate), from iodomethane
(methyl iodide) and bromoethane (ethyl • Uses of acetic acid.
bromide). Complete and incomplete
combustion of methane and ethane,
reaction of methane and ethane with
INTERNAL ASSESSMENT OF
chlorine through substitution. PRACTICAL WORK
• Alkenes – (unsaturated hydrocarbons Candidates will be asked to observe the effect of
with a double bond); ethene as an ragents and/or of heat on substances supplied to them.
example. Methods of preparation of The exercises will be simple and may include the
ethene by dehydro halogenation reaction recognition and identification of certain gases and ions
and dehydration reactions. listed below. The examiners will not, however, be
• Alkynes - (unsaturated hydrocarbons with restricted in their choice to substances containing the
a triple bond); ethyne as an example of listed ions.
alkyne; Methods of preparation from Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine,
calcium carbide and 1,2 dibromoethane Hydrogen chloride, Sulphur dioxide, Hydrogen
ethylene dibromide). sulphide, Ammonia, Water vapour, Nitrogen dioxide.
Only main properties, particularly addition Ions: Copper, Iron, Lead, Zinc and Ammonium,
products with hydrogen and halogen namely Carbonate, Chloride, Nitrate, Sulphide, Sulphite and
Cl 2 , Br 2 and I 2 pertaining to alkenes and Sulphate.
alkynes.
Knowledge of a formal scheme of analysis is not
• Uses of methane, ethane, ethene, ethyne. required. Semi-micro techniques are acceptable but
(vi) Alcohols: ethanol – preparation, properties candidates using such techniques may need to adapt
and uses. the instructions given to suit the size of the apparatus
being used.

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Candidates are expected to have completed the EVALUATION
following minimum practical work:
The assignments/project work are to be evaluated by
1. Action of heat on the following substances: the subject teacher and by an External Examiner. (The
(a) Copper carbonate, zinc carbonate External Examiner may be a teacher nominated by the
Head of the school, who could be from the faculty, but
(b) zinc nitrate, copper nitrate, lead nitrate
not teaching the subject in the section/class. For
Make observations, identify the products and example, a teacher of Chemistry of Class VIII may be
make deductions where possible (equations not deputed to be an External Examiner for Class X
required). Chemistry projects.)
2. Make a solution of the unknown substance: add The Internal Examiner and the External Examiner will
sodium hydroxide solution or ammonium
assess the assignments independently.
hydroxide solution, make observations and give
your deduction. Warming the mixture may be
Award of Marks (20 Marks)
needed. Choose from substances containing
Cu2+, Fe2+, Fe3+, Pb2+, Zn2+, NH 4 +. Subject Teacher (Internal Examiner) 10 marks
3. Supply a solution of a dilute acid and alkali. External Examiner 10 marks
Determine which is acidic and which is basic, The total marks obtained out of 20 are to be sent to
giving two tests for each. CISCE by the Head of the school.
4. Add concentrated hydrochloric acid to each of The Head of the school will be responsible for the
the given substances, warm, make observations, online entry of marks on CISCE’s CAREERS portal
identify any product and make deductions: (a) by the due date.
copper oxide (b) manganese dioxide.

NOTE: According to the recommendation of International Union of Pure and Applied Chemistry (IUPAC),
the groups are numbered from 1 to 18 replacing the older notation of groups IA …. VIIA, VIII, IB …… VIIB
and 0. However, for the examination both notations will be accepted.
Old IA IIA IIIB IVB VB VIB VIIB VIII IB IIB IIIA IVA VA VIA VIIA 0
notation
New 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
notation

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