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chem 10 ICSE 2010 syllabus
Posted Date: 01 Jul 2008 Resource Type: Articles/Knowledge Sharing Category: Syllabus
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Posted By: hima Member Level: Gold
Rating:  Points: 2
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SCIENCE (52)
PAPER 2: CHEMISTRY
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 develop scientific temper, attitude and
problem solving skills.
CLASS IX
There will be one paper of one and half-hours
duration of 80 marks and Internal Assessment of
practical work carrying 20 marks.
The paper will be divided into two sections,
Section I (40 marks) and Section II (40 marks).
Section I (compulsory) will contain short answer
questions on the entire syllabus.
Section II will contain six questions. Candidates
will be required to answer any four of these six
questions.
Note: All chemical reactions should be studied with
reference to the reactants, products, conditions,
observations and the (balanced) equation.
1. Matter and its Composition
(i) Inter-conversion of states of matter; m.p.,
b.p. (relevant experiments).
(ii) Explanation of change of state of matter on
the basis of Kinetic Theory of Matter.
2. 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 and Charles’ Law;
absolute (Kelvin) zero; gas equation; simple
relevant calculations.
(ii) Relationship between Kelvin Scale and
Celsius Scale of temperature; Standard
temperature and pressure (reduction to
S.T.P. required).
3. Elements, Compounds and Mixtures
(i) General characteristics and differences
between elements, compounds and
mixtures.
(ii) Separation of mixtures involving use of a
solvent, filtration, evaporation and
distillation, fractional distillation, simple
paper chromatography (limited to separation
of colouring matter in ink); immiscible
liquids (separating funnel).
(iii) Types of mixtures: of two solids, a solid and
a liquid, two liquids, liquid and gas, two
gases.
4. The language of Chemistry
Symbol of an element; valency; formulae of
radicals and formulae of compounds. Balancing
of simple chemical equations.
5. Physical and Chemical Changes
(i) Definitions and comparison of Physical and
Chemical changes.
(ii) Conditions for chemical change.
(iii) Types of chemical change.
(iv) Energy changes in a chemical change.
(v) Burning: Definition and conditions of
burning.
68
6. Water
(i) Physical Properties: Water as a compound
and as a universal solvent; its physical states
and chief physical properties; solutions as
'mixtures' of solids in water; saturated
solutions; qualitative effect of temperature
on solubility (e.g. solutions of calcium
sulphate, potassium nitrate, sodium chloride
in water).
(ii) Water of crystallization: removal of water
of crystallization; idea of anhydrous
substances; air dissolved in water and its
biological importance.
(iii) Chemical Properties: The action of cold
water on sodium and calcium; the action of
hot water on magnesium and steam on iron;
reversibility of reaction between iron and
steam; reactivity series.
7. Atomic Structure
(i) Atom consists of a nucleus (protons,
neutrons) with associated electrons, mass
number and atomic number.
(ii) Isotopes of hydrogen, carbon, chlorine.
Reason for chemical activity of an atom
(electronic configuration). Octet Rule.
8. The Periodic Table
(i) Dobereiner’s Triads, Newland’s Octaves,
Mendeleev’s contributions; Modern
Periodic Law, the representative periodic
table for 8 groups up to period 3.
(ii) Uses of Modern Periodic Table.
Study of the First Element -Hydrogen
Position of the non-metal (Hydrogen) in the
periodic table and general group
characteristics applied to the above
mentioned element.
(i) Hydrogen from water.
(ii) Displacement of hydrogen from dilute
sulphuric acid or hydrochloric acid by
zinc or iron (no reaction with copper).
(iii) Displacement of hydrogen from alkalis
(NaOH, KOH) by Zn, Al.
(iv) The preparation and collection of
hydrogen by a standard laboratory
method other than electrolysis.
Study of the Group 14 (Fourth
Group) Element - Carbon
Position of the non-metal (Carbon) in the
periodic table and general group
characteristics applied to the above
mentioned element.
Natural occurrence; Allotropy (definition);
Allotropes of Carbon – diamond, graphite
and fullerene; burning of these in O2 giving
CO2. Other forms of Carbon: wood, bone
charcoal, soot, gas carbon – their uses.
Study of the Group 15 (Fifth Group)
Element - Nitrogen
Position of the non-metal (Nitrogen) in the
periodic table and general group
characteristics applied to the above
mentioned element.
(i) Laboratory preparation and collection
of nitrogen.
(ii) Properties of nitrogen.
Study of the Group 16 (Sixth Group)
Elements – Oxygen, Sulphur
Position of the non-metals (Oxygen,
Sulphur) in the periodic table and general
group characteristics applied to the above
mentioned elements.
(i) Occurrence of oxygen in air, water and
oxides.
(ii) The preparation and collection of
oxygen in the laboratory e.g. from:
(i) hydrogen peroxide (ii) potassium
chlorate with manganese (IV) oxide.
(iii) oxygen from higher oxides like
Pb3O4, PbO2.
(iii) Density of oxygen as compared to air.
(iv) Solubility of oxygen in water.
(v) The burning of common elements in
oxygen (e.g. carbon, sulphur,
phosphorus, sodium, calcium,
magnesium, iron); burning of a candle
in air – products formed: water and
carbon dioxide.
69
(vi) Conditions for and prevention of
rusting.
(vii) Sulphur - extraction by Frasch
process. Structure and process.
(viii) Chemical properties of sulphur.
(ix) Uses of sulphur.
Study of Group 17 (Seventh Group)
Element - Chlorine
Position of the non-metal (Chlorine) in the
periodic table and general group
characteristics applied to the above
mentioned element.
(i) Preparation and collection of chlorine;
refer to the density, solubility and
poisonous nature of chlorine; oxidation
of concentrated hydrochloric acid by
MnO2; NaCl and concentrated sulphuric
acid and MnO2; bleaching powder;
PbO2 and Pb3O4.
(ii) Reaction of chlorine with burning
sodium, hot iron, phosphorus. Sodium
hydroxide solutions, cold and hot,
potassium iodide solution, hydrogen
sulphide and ammonia; uses of
Chlorine: in water purification,
bleaching agent, manufacture of
hydrochloric acid and other important
uses.
9. Study of Carbon Monoxide and Carbon
Dioxide
(i) Carbon monoxide formed by incomplete
combustion of carbon or carbon compounds
(e.g. exhaust fumes from cars); methods of
preparing and collecting carbon monoxide
(preparation of CO from oxalic and formic
acids); conversion of CO2 into CO and viceversa;
separation of CO2 or CO from a
mixture of the two; reducing property of CO
with reference to metallic oxides (refer to
the density, solubility and poisonous nature
of carbon monoxide).
(ii) Carbon dioxide: an oxide of carbon; its
formation when charcoal, wood or other
organic substances (e.g. ethanol) are burned
in air or oxygen; the main concept that
hydrocarbons mostly contain carbon
and hydrogen, which on burning
produce water and carbon dioxide should be
understood (can be demonstrated by burning
of candle).
(iii) Obtaining CO2 from sodium hydrogen
carbonate and carbonates; reaction with
quicklime, slaked lime, lime water and their
important uses.
(iv) The reactions of carbon dioxide with lime
water, sodium hydroxide solution and
magnesium; difference between CO and
CO2 with reference to their densities,
combustibility and action of lime water; use
of carbon dioxide in refrigeration, fire
extinguishers and photosynthesis.
INTERNAL ASSESSMENT OF
PRACTICAL WORK
Candidates will be asked to observe to 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. Heat the given (unknown) substance, make
observations, identify any products and make
deductions where possible.
(a) copper carbonate, zinc carbonate
(b) washing soda, copper sulphate crystals
(c) zinc nitrate, copper nitrate, lead nitrate
(d) ammonium chloride, iodine, ammonium
dichromate
2. Add dilute sulphuric acid to the unknown
substance, warm if necessary, make
observation, identify the product and make
deductions.
(a) a sulphide
(b) a carbonate
(c) a metal
70
3. Apply the flame test to identify the metal in the
unknown substance.
(a) a sodium salt
(b) a potassium salt
(c) a calcium compound
4. The percentage composition of a mixture of
powdered salt and water-washed sand.
The experiment would test techniques in
dissolving, filtering or decanting, washing and
weighing. It may be counted out as taking too
much time. The weakness could be met by
supplying a given weight of the mixture; also by
choosing sand of such grain size that filtering or
decanting will not be slow and yet not so large
that separation of salt and sand cannot be done
simply by sorting out mechanically the sand
from the salt. The experiment should take about
20 minutes using 10g mixture (4g sand, 6g salt).
5. 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.
CLASS X
There will be one paper of one and a half-hours
duration of 80 marks and Internal Assessment of
practical work carrying 20 marks.
The paper will be divided into two sections,
Section I (40 marks) and Section II (40 marks).
Section I (compulsory) will contain short answer
questions on the entire syllabus.
Section II will contain six questions. Candidates
will be required to answer any four of these six
questions.
Note: All chemical reactions should be studied with
reference to the reactants, products, conditions,
observations and the (balanced) equation.
1. Periodic Properties and variations of
Properties – Physical and Chemical
(i) Periodic properties and their variations in
groups and periods.
(ii) Relation between atomic number for light
elements (proton number) and periodicity
and atomic mass for light elements; the
modern periodic table up to period 3
(students to be exposed to the complete
modern periodic table but no questions will
be asked on elements beyond period 3 –
Argon); periodicity and other related
properties to be described in terms of shells
(not orbitals); special reference to the alkali
metals and halogen groups.
2. Chemical Bonding – Covalent and ionic
compounds – structures of various
compounds – orbit structure and electron dot
structure
(i) Types of bonding: electrovalent and
covalent. Compounds: characteristic
properties of electrovalent and covalent
compounds and differences between them;
oxidation and reduction in terms of loss or
gain of electrons by atoms of an element.
(ii) Structure of electrovalent compounds:
NaCl, MgCl2, CaO; covalent molecules like
hydrogen, chlorine, nitrogen, water,
ammonia, carbon tetrachloride, methane.
(iii) Coordinate Bond: Formation of H3O+ and
NH4
+ ion.
3. Study of Acids, Bases and Salts
(i) Simple definitions in terms of the molecules
and their characteristic properties.
(ii) Ions present in mineral acids, alkalis and
salts and their solutions; use of litmus to test
for acidity and alkalinity.
(iii) Definition of salt; types of salts.
(iv) General properties of salts:
Deliquescence, efflorescence, water of
crystallization.
71
Decomposition of bicarbonates,
carbonates, chlorides and nitrates by
appropriate acids with heating if
necessary (relevant laboratory work must
be done).
(v) Preparation: laboratory preparation of salts
(normal and acid salts) – relevant laboratory
work is essential.
4. Analytical Chemistry – Use of Ammonium
Hydroxide and Sodium Hydroxide and
Standard Tests
(i) On solution of salts: colour of salt and its
solution; formation and colour of hydroxide
precipitated for solutions of salts of Mg, Fe,
Cu, Zn and Pb; special action of ammonium
hydroxide on solutions of copper salts.
(ii) On certain metals and their oxides (relevant
laboratory work is essential).
5. Mole Concept and Stoichiometry
(i) Gay Lussac’s Law of Combining Volumes;
Avogadro’s Law.
(ii) Refer to the atomicity of hydrogen, oxygen,
nitrogen and chlorine (proof not required).
(iii) Relative atomic masses (atomic weight) and
relative molecular masses (molecular
weights): either H=1 or 12C=12 will be
accepted; molecular mass = 2×vapour
density (formal proof not required).
Deduction of simple (empirical) and
molecular formula from the percentage
composition of a compound; the molar
volume of a gas at S.T.P.; simple
calculations based on chemical equations;
both reacting weight and volumes.
6. Electrolysis
(i) Electrolytes and non-electrolytes.
(ii) Substances containing molecules only, ions
only, both molecules and ions.
(iii) An elementary study of the migration of
ions, illustrated by the electrolysis of:
molten lead bromide; acidified water with
platinum electrodes and aqueous
copper (II) sulphate with copper electrodes;
electron transfer at the electrodes.
(iv) Application of electrolysis: electroplating
with nickel and silver; purification of
copper.
(v) Acids, bases and salts as electrolytes:
reference should be made to the activity
series as indicating the tendency of metals,
e.g. Na, Mg, Fe, Cu, to form ions; action of
alkalis on certain metals and their oxides;
action of acids on oxides and salts.
7. Metallurgy
(i) Definition of Metal and Non-metals.
(ii) Position of the metals (alkali metals and
alkaline earth metals) in the Periodic table
and general characteristics applied to these
elements.
(iii) Comparison of Metals and Non-metals.
(iv) General properties with special reference to
physical properties: state, lustre, melting
point, density, ductility, malleability,
brittleness, conduction of electricity
(exceptions to be specifically noted - e.g.
graphite, mercury); chemical properties:
a metal forms at least one basic oxide;
non-metal, an acidic or neutral oxide;
discharge of metallic ions at the cathode
from fused metallic chlorides (link with
bonding and ion formation); many metals
liberate hydrogen from dilute HCl and
H2SO4.
(v) Reduction of metallic oxides; some can be
reduced by hydrogen, carbon and carbon
monoxide (e.g. copper oxide, lead oxide,
iron (II) oxide) and some cannot (e.g.
Al2O3, MgO - refer to activity series).
(vi) Extraction of metals based on the activity
series.
(vii) Metals and their alloys: common ores of
iron, aluminium and zinc. Extraction of
Aluminium
(a) Uses of iron, aluminium and zinc and
their alloys.
(b) Other important alloys – bronze, fuse
metal.
72
8. Study of Compounds
Hydrogen Chloride
Hydrogen chloride: preparation of hydrogen
chloride from sodium chloride; refer to the
density and solubility of hydrogen chloride
(fountain experiment); reaction with
ammonia; acidic properties of its solution.
Ammonia
(i) Ammonia: its laboratory preparation
from ammonium chloride and
collection; ammonia from nitrides
like Mg3N2 and AlN and ammonium
salts; preparation from air and from
ammonium nitrite; Manufacture by
Haber’s Process; density and solubility
of ammonia (fountain experiment);
aqueous solution of ammonia; its
reactions with hydrogen chloride and
with hot copper (II) oxide and chlorine;
the burning of ammonia in oxygen; uses
of ammonia.
(ii) The catalytic oxidation of ammonia, as
the source of nitric acid; simple diagram
for a catalytic oxidation of ammonia in
the laboratory (with conditions and
reactions only).
Nitric Acid and Nitrates:
(i) Nitric Acid: one laboratory method of
preparation of nitric acid from
potassium nitrate or sodium nitrate.
Nitric acid as an oxidizing agent.
(ii) Nitrates: salts of nitric acid. Action of
heat on the nitrates of potassium,
sodium, lead, copper and ammonium.
Sulphur Dioxide, Hydrogen Sulphide and
Sulphuric Acid
(i) Formation of sulphur dioxide by
burning sulphur and by the action of
dilute acid on sodium sulphite and other
sulphites; one laboratory method of
preparing and collecting sulphur
dioxide; density and solubility; ease of
liquefaction and poisonous nature of
sulphur dioxide; comparison of
bleaching action of chlorine and sulphur
dioxide; reactions of sulphur dioxide
with water, sodium hydroxide solution
and chlorine. Uses, including:
manufacturing of sulphuric acid by first
converting SO2 to SO3; bleaching and
food preserving.
(ii) Hydrogen sulphide: its peculiar smell
and its tendency to form sulphides and
be converted to sulphur (study of its
preparation not required).
(iii) Sulphuric Acid: its behaviour as an acid
when dilute, as an oxidizing agent when
concentrated - oxidation of carbon
and sulphur; as a dehydrating agent -
dehydration of sugar and copper (II)
sulphate crystals; its non-volatile nature.
9. Organic Chemistry
(i) Introduction to Organic compounds.
(ii) Structure and Isomerism.
(iii) Homologous series.
(iv) Simple nomenclature.
(v) Hydrocarbons: alkanes, alkenes, alkynes.
(vi) Alcohols: methanol, ethanol – preparation
and properties; its uses.
(vii) Carboxylic acids (aliphatic - mono
carboxylic acid): Acetic acid – properties
and uses of acetic acid.
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
and ions listed below. The examiners will not,
however, be restricted in their choice to substances
containing the listed ions.
Gases: Hydrogen, Oxygen, Carbon dioxide,
Chlorine, Hydrogen chloride, Sulphur dioxide,
Hydrogen sulphide, Ammonia, Water vapour,
Nitrogen dioxide.
Ions: Calcium, Copper, Iron, Lead, Zinc and
Ammonium, Carbonate, Chloride, Nitrate, Sulphide,
Sulphite and Sulphate.
73
Knowledge of a formal scheme of analysis is not
required. Semi-micro techniques are acceptable but
candidates using such techniques may need to adapt
the instructions given to suit the size of the
apparatus being used.
Candidates are expected to have completed the
following minimum practical work:
1. Make a solution of the unknown substance: add
sodium hydroxide solution or ammonium
hydroxide solution, make observations and give
your deduction. Warming the mixture may be
needed. Choose from substances containing
Ca2+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+, NH4
+.
2. Supply a solution of a dilute acid and alkali.
Determine which is acidic and which is basic,
giving two tests for each.
3. Add concentrated hydrochloric acid to each of
the given substances, warm, make observations,
identify any product and make deductions:
(a) copper oxide (b) manganese dioxide.
4. Use of pH in soil analysis, water analysis,
medical field – simple identification with
universal indicator.
EVALUATION
The assignments/project work are to be evaluated by
the subject teacher and by an External Examiner.
(The External Examiner may be a teacher
nominated by the Principal, who could be from the
faculty, but not teaching the subject in the
section/class. For example, a teacher of Chemistry
of Class VIII may be deputed to be an External
Examiner for Class X Chemistry projects.)
The Internal Examiner and the External Examiner
will assess the assignments independently.
Award of marks (20 Marks)
Subject Teacher (Internal Examiner) 10 marks
External Examiner 10 marks
The total marks obtained out of 20 are to be sent to
the Council by the Principal of the school.
The Head of the school will be responsible for the
entry of marks on the mark sheets provided by the
Council.
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
notation
IA IIA IIIB IVB VB VIB VIIB VIII IB IIB IIIA IVA VA VIA VIIA 0
New
notation
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
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