Cambridge IGCSE Science Combined 0653 Syllabus 2019-2021
Chemistry Syllabus
The full Cambridge IGCSE Combined Science Syllabus can be found fficial CIE syllabus can be
found
here. It is best to always refer to the
original syllabus.
The Chemistry Syllabus runs from C1-C12
C1.
The particulate nature of matter
· State
the distinguishing properties of solids, liquids and gases
· Describe
the structure of solids, liquids and gases in terms of particle separation,
arrangement and types of motion
· Describe
the changes of state in terms of melting, boiling, evaporation, freezing and
condensation
· Explain changes of state in terms of particle theory and the energy
changes involved*
· Describe
qualitatively the pressure and temperature of a gas in terms of the motion of
its particles
· Demonstrate
understanding of the terms atom,
molecule and ion
C2.
Experimental techniques
2.1Measurement
· Name
and suggest appropriate apparatus for the measurement of time, temperature,
mass and volume, including burettes, pipettes and measuring cylinders
2.2 Criteria of purity
· Interpret
simple chromatograms
· Interpret simple chromatograms, including the use of Rf
values
2.3 Methods of purification
· Describe
and explain methods of separation and purification using a suitable solvent,
filtration, crystallisation, distillation, fractional distillation and paper
chromatography
· Suggest
suitable separation and purification techniques, given information about the
substances involved
C3.
Atoms, elements and compounds
3.1 Physical and
chemical changes
·
Identify physical and chemical
changes, and understand the differences between them.
3.2 Elements,
compounds and mixtures
· Describe
the differences between elements, compounds and mixtures and between metals and
non-metals
· Define
the terms solvent, solute, solution and concentration
3.3 Atomic
structure and the Periodic Table
· Describe
the structure of an atom in terms of a central nucleus, containing protons and
neutrons, and ‘shells’ of electrons
· Describe
the build-up of electrons in ‘shells’ and understand the significance of the
noble gas electronic structures and of the outer shell electrons (The ideas of the distribution of electrons
in s and p orbitals and in d block elements are not required)
· State
the charges and approximate relative masses of protons, neutrons and electrons
· Define
and use proton number (atomic
number) as the number of protons in the nucleus of an atom
· Define
and use nucleon number (mass
number) as the total number of protons and neutrons in the nucleus of an atom
· Use proton number and the simple structure of atoms to explain the
basis of the Periodic Table, with special reference to the elements of proton
numbers 1 to 20*
3.4 Ions and ionic bonds
·
Describe
the formation of ions by electron loss or gain.
·
Using
dot and cross diagrams describe the formation of ionic bonds between elements
from Groups I and VII.
· Describe the formation of ionic bonds between metallic and
non-metallic elements to include the strong attraction between ions because of
their opposite electrical charges *
· Describe the lattice structure of ionic compounds as a regular
arrangement of alternating positive and negative ions, exemplified by the
sodium chloride structure*
3.5 Molecules and
covalent bonds
· State
that non-metallic elements form simple molecules with covalent bonds between
atoms
· Describe
the formation of single covalent bonds in H2, Cl2, H2O, CH4, NH3 and HCl
as the sharing of pairs of electrons leading to the noble gas
configuration including the use of dot-and-cross diagrams
· Use and draw dot-and-cross diagrams to represent the bonding in the
more complex covalent molecules such as N2, C2H4, CH3OH, and CO2*
· Describe
the differences in volatility, solubility and electrical conductivity between
ionic and covalent compounds
· Explain the differences in melting point and boiling point of ionic
and covalent compounds in terms of attractive forces*
·
Use the symbols of the elements to
write the formulae of simple compounds.
· Determine the formula of an ionic compound from the charges on the
ions present*
· Deduce
the formula of a simple compound from the relative numbers of atoms present
· Deduce
the formula of a simple compound from a model or a diagrammatic representation
· Construct
and use word equations
· Interpret
and balance simple symbol equations
· Construct and use symbol equations, with state symbols, including
ionic equations*
C5.
Electricity and chemistry
· Define
electrolysis as the breakdown
of an ionic compound when molten or in aqueous solution by the passage of
electricity
·
Use the terms inert electrode, electrolyte,
anode and cathode
· Describe electrolysis in terms of the ions present and the reactions
at the electrodes, in terms of gain of electrons by cations and loss of
electrons by anions to form atoms*
· Describe
the electrode products and the observations made, using inert electrodes
· (platinum
or carbon), in the electrolysis of:
– molten
lead(II) bromide
– concentrated
aqueous sodium chloride
– dilute
sulfuric acid
· Predict the products of the electrolysis of a specified molten
binary compound*
· C6. Energy changes in chemical
reactions
· Describe
the meaning of exothermic and endothermic reactions
· Describe
bond breaking as an endothermic process and bond forming as an exothermic process
· Draw
and label energy level diagrams for exothermic and endothermic reactions using data
provided
· Interpret energy level diagrams showing exothermic and endothermic
reactions and the activation energy of a reaction
7.1 Rate (speed)
of reaction
· Describe
practical methods for investigating rate of a reaction which produces a gas
· Interpret
data obtained from experiments concerned with rate of reaction
· Suggest suitable apparatus, given information, for experiments,
including collection of gases and measurement of rates of reaction*
· Describe
the effect of concentration, particle size, catalysts and temperature on the
rate of reactions Note: Candidates should be encouraged to use the term rate rather than speed.
· Describe and explain the effect of changing concentration in terms
of frequency of collisions between reacting particles*
· Describe and explain the effect of changing temperature in terms of
the frequency of collisions between reacting particles and more colliding
particles possessing the minimum energy (activation energy) to react*
· 7.2
Redox
· Describe
oxidation and reduction in chemical reactions in terms of oxygen loss / gain
· (Oxidation
state limited to its use to name ions, e.g. iron(II), iron(III), copper(II).)
· Define and identify an oxidising
agent as a substance which oxidises another substance during a redox
reaction and a reducing agent as
a substance which reduces another substance during a redox reaction*
· C8. Acids, bases and salts
· 8.1
The characteristic properties of acids and bases
· Describe
neutrality and relative acidity and alkalinity in terms of pH (whole numbers
only) measured using Universal Indicator
· Describe
the characteristic properties of acids (exemplified by dilute hydrochloric acid
and dilute sulfuric acid) including their effect on litmus paper and their
reactions with metals, bases and carbonates
· Describe
and explain the importance of controlling acidity in soil
8.2 Preparation of salts
· Describe
the preparation, separation and purification of salts using techniques
specified in Section C2 and the reactions specified in Section C8.1
· Suggest a method of making a given salt from suitable starting
material, given appropriate information*
8.3 Identification of ions and gases
· Describe
and use the following tests to identify: aqueous
cations and cations, anions and gases.
9.1 The Periodic Table
· Describe
the Periodic Table as a method of classifying elements and its use to predict properties
of elements
9.2 Periodic trends
· Describe
the change from metallic to non-metallic character across a period
· Describe and explain the relationship between Group number, number
of outer shell electrons and metallic/non-metallic character*
9.3 Group properties
· Describe
lithium, sodium and potassium in Group I as a collection of relatively soft
metals showing a trend in melting point, density and reaction with water
· Predict the properties of other elements in Group I, given data,
where appropriate*
· Describe
the halogens, chlorine, bromine and iodine in Group VII, as a collection of
diatomic non-metals showing a trend in colour and physical state
· State the reaction of chlorine, bromine and iodine with other halide
ions
· Predict the properties of other elements in Group VII, given data
where appropriate
· Identify trends in other groups, given data about the elements
concerned*
9.4 Transition elements
· Describe
the transition elements as a collection of metals having high densities, high
melting points and forming coloured compounds, and which, as elements and
compounds, often act as catalysts
9.5 Noble gases
· Describe
the noble gases, in Group VIII or 0, as being unreactive, monoatomic gases and explain
this in terms of electronic structure
· State the uses of the noble gases in
providing an inert atmosphere, i.e. argon in lamps, helium for filling balloons
10.1 Properties of metals
· Describe
the general physical properties of metals as solids with high melting and
boiling points, malleable and good conductors of heat and electricity
· Describe
alloys, such as brass, as mixtures of a metal with other elements
· Explain
in terms of their properties why alloys are used instead of pure metals
· Identify representations of alloys from diagrams of structure*
10.2 Reactivity series
· Place
in order of reactivity: potassium, sodium, calcium, magnesium, aluminium,
(carbon), zinc, iron, (hydrogen) and copper, by reference to the reactions, if
any, of the elements with: water or steam dilute hydrochloric acid reduction of
their oxides with carbon
· Describe the reactivity series in terms of the tendency of a metal
to form its positive ion, illustrated by its reaction, if any, with the aqueous
ions of other listed metals*
·
Deduce an order of reactivity from a
given set of experimental results
10.3
Extraction of metals from their ores
· Describe
the use of carbon in the extraction of copper from copper oxide
· Describe and explain the essential reactions in the extraction of
iron from hematite in the blast furnace
C + O2 → CO2
C + CO2 → 2CO
Fe2O3 + 3CO → 2Fe + 3CO2*
· Know
that aluminium is extracted from the ore bauxite by electrolysis
· Relate the method of extraction of a metal from its ore to its
position in the reactivity series for the metals listed in section C10.2 and for
other metals, given information*
· Describe
metal ores as a finite resource and hence the need to recycle metals
11.1 Water
· Describe
a chemical test for water using copper(II) sulfate and cobalt(II) chloride
· Describe,
in outline the treatment of the water supply in terms of filtration and
chlorination
11.2 Air
· State
the composition of clean air as being a mixture of 78% nitrogen, 21% oxygen and
small quantities of noble gases, water vapour and carbon dioxide
· Name
the common pollutants in air as being carbon monoxide, sulfur dioxide and
oxides of nitrogen
· State
the adverse effect of these common air pollutants on buildings and on health
· State
the conditions required for the rusting of iron (presence of oxygen and water)
· Describe
and explain barrier methods of rust prevention, including paint and other
coatings
11.3 Carbon dioxide and methane
· State
the formation of carbon dioxide: as a product of complete combustion of carbon-containing
substances as a product of respiration as a product of the reaction between an
acid and a carbonate as a product of thermal decomposition of calcium carbonate
· State
that carbon dioxide and methane are greenhouse gases
· State that increased concentrations of greenhouse gases cause an
enhanced greenhouse effect, which may contribute to climate change*
C12.1 Fuels
· State
that coal, natural gas and petroleum are fossil fuels that produce carbon
dioxide on combustion
· Name
methane as the main constituent of natural gas
· Describe
petroleum as a mixture of hydrocarbons and its separation into useful
· fractions
by fractional distillation
· Describe the properties of molecules within a fraction*
· Name
the uses of the fractions as:
– refinery
gas for bottled gas for heating and cooking
– gasoline
fraction for fuel (petrol) in cars
– naphtha
fraction as a feedstock for makingchemicals
– diesel
oil/gas oil for fuel in diesel engines
– bitumen
for road surfaces
· 12.2
Homologous series
· 1 Describe the homologous series of alkanes and alkenes as families
of compounds with the same general formula and similar chemical properties*
· 12.3
Alkanes
· Describe
alkanes as saturated hydrocarbons whose molecules contain only single covalent bonds
· Describe
the properties of alkanes (exemplified by methane) as being generally
unreactive, except in terms of burning
· Describe
complete combustion of hydrocarbons to give carbon dioxide and water
· 12.4
Alkenes
· Describe
alkenes as unsaturated hydrocarbons whose molecules contain one double covalent
bond
· State
that cracking is a reaction that produces Alkenes
· Describe the formation of smaller alkanes, alkenes and hydrogen by
the cracking of larger alkane molecules and state the conditions required for
cracking*
· Recognise
saturated and unsaturated hydrocarbons:
– from
molecular structures
– by
their reaction with aqueous bromine
· Describe
the formation of poly(ethene) as an example of addition polymerisation of
· monomer
units
*=EXTENDED PAPER
