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Brown's Chemistry IGCSE in CHEMISTRY -
Edexcel syllabus 4335 My
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Syllabus content
sections in bold
are higher only and [reference links
to pages within
this site]
For quizzes: F =
UK Foundation-easier and H = UK Higher-harder!
 1.
Principles of
chemistry
-
1(a) Atoms: Candidates should be able to:
-
recall simple experiments leading to the idea of the smallness of
particles and to their motion including dilution of coloured solutions, diffusion experiments.
-
define an element, and an atom as the particle of which elements are
composed
-
recall that atomic masses are the masses of atoms relative to
12C = 12
and are referred to as relative atomic masses
-
understand a mole of atoms as a number of atoms equal to the Avogadro
constant.
- 1(b) Atomic
Structure: Candidates should be able to:
- recall the structure of an atom in terms of
a central nucleus of protons and neutrons, surrounded by orbiting electrons
- state the relative mass and
relative charge of a proton, neutron and electron
- explain the terms atomic
number, mass number, isotopes and relative
atomic mass (A)
- calculate the relative
atomic mass of an element from the relative abundances of its
isotope
- recall the electron
configuration of the first twenty elements of the Periodic Table
- relate periodicity to electronic
configuration
- relate similarity of electron configuration to similarity of the
chemical properties of the Group 1 elements (2.1; 2.8.1; 2.8.8.1) and the Group 7 elements (2.7;
2.8.7; 2.8.18.7; 2.8.18.18.7)
- link electron configuration and ionic
charge
- appreciate the importance of the noble gas electron configurations
(2;
2.8; 2.8.8; 2.8.18.8; 2.8.18.18.8).
-
1(c) Relative formula masses
and molar volumes: Candidates should be able to:
-
calculate the
relative formula masses (Mr) from relative atomic
masses (Ar)
-
recall that the mole is an amount of substance which can also be
expressed as the Avogadro constant number of particles (atoms, molecules, formulae, ions or
electrons) or as a relative formula mass in grams
-
understand the significance of the molar volume of a
gas
-
use the
molar volume of a gas at stp and rtp
-
1(d) Chemical
formulae and chemical equations: Candidates should be able to:
-
recall
experiments to find the formulae of simple compounds such
as copper(II) oxide and water
-
recall that
the formulae of other compounds have been obtained experimentally
-
apply the idea of a mole of atoms in finding the chemical
formulae
-
calculate
empirical formulae and molecular formulae
-
calculate
percentage yield
-
recall quantitative
experiments, including direct mass
determination, the use of standard solutions and the measurement of volumes in reactions
involving gases, to determine the relative numbers of particles involved in
chemical reactions
-
write word
equations to represent the reactions studied in the syllabus
-
write chemical equations
that do not require balancing to represent the reactions studied
in this syllabus
-
use the state symbols
(l), (s), (g) and (aq) are used in
chemical equations to represent liquids, solids, gases and aqueous solutions respectively.
-
write
balanced chemical equations to represent the reactions studied
in this syllabus
- 1(e) Ionic compounds: Candidates should be able to:
- describe the formation of ions by gain or loss of
electrons
- link electronic
configuration and ionic charge
- use the dot and cross model
to explain the formation of an ionic compound by electron
transfer, limited to combinations of Li+, Na+,
Mg2+, F-, Cl- and O2-
- recall that
- ionic compounds such as
NaCl and MgO have high melting points and high boiling points
because of strong electrostatic forces between ions
- MgO has a much higher
melting/boiling point than NaCl because of the higher charges
on its ions
- recall that there is a
strong electrostatic attraction between oppositely charged ions,
called ionic bonding, and this extends throughout
the ionic structure
-
describe an ionic crystal as a giant three-dimensional ionic
structure held together by attraction between oppositely charged ions.
- 1(f) Covalent compounds: Candidates should be able to:
- describe how covalent bonds
involve the sharing of electron pairs between outer electron
shells of atoms and these bonds are strong
- recall that the covalent bond
is the result of attraction between the
bonding pair of electrons and the nuclei of the atoms involved in the bond
- use dot and cross diagrams
to represent single covalent bonds in hydrogen, water, methane and
hydrogen chloride
- describe the electron
arrangement in more complex covalent molecules such as nitrogen,
ethane and carbon dioxide
- describe the shapes of
carbon dioxide, methane
- describe and explain the
physical properties of a typical simple covalent compound
e.g. appreciate that weak intermolecular forces result in low melting
points and boiling points
- recall that diamond and
graphite are allotropes of carbon
- describe and explain the giant molecular covalent
crystal structures of diamond and
graphite and relate their structures to their use - graphite as a
lubricant and diamond in cutting
- understand that atoms in diamond and graphite are held together by
strong covalent bonds which result in high sublimation points.
- 1(g) Electrolysis: Candidates should be able
to:
- recall simple experiments to distinguish between electrolytes and
non-electrolytes
- understand an electric current as a flow of electrons or
ions
- recall the charges on common ions met in the
syllabus
- recall that one Faraday
represents one mole of
electrons
- calculate the amounts of
the products of the electrolysis of molten salts and aqueous
solutions
- write ionic half-equations representing the reaction at each electrode
during electrolysis
- recognise oxidation and reduction as the loss and gain of electrons
respectively
- 1(h) Metallic crystals: Candidates should be able to:
- describe a metal as a giant structure in which electrons are free to
move throughout the whole structure
- relate the structure of a metal to observable
physical properties such as
conductivity and malleability
2. Chemistry of the elements
- 2(g) Hydrogen: Candidates should be able to:
- recall the effect of dilute hydrochloric and dilute sulphuric acids on
magnesium, aluminium, zinc and iron
- describe the laboratory preparation of
hydrogen
- describe the combustion of
hydrogen to form water
- describe a simple chemical test for
water
- describe the combustion of hydrogen with oxygen to form
water
- describe a physical test to show if water is
pure
- describe the reaction of hydrogen with chlorine.
- 2(h) The transition metals iron
and copper: Candidates should be able to:
- describe the action of steam, hydrogen chloride and chlorine on
iron
-
discuss the formation of
iron(II) and iron(III) hydroxides from salt solutions
- describe the redox reaction of nitric acid on
copper
- describe the simple chemical and physical properties of
copper(II)
oxide, hydroxide, nitrate, sulphate, carbonate, and chloride
- recall the existence of copper(I) compounds such as
copper(I) oxide
- describe the reaction of
copper(II) ions with ammonia to form the
complex ion [Cu(H20)2(NH3)4]2+
- understand that the study of these two metals and their compounds
illustrates typical transition metal properties of variable valency, formation of
coloured compounds and formation of complex ions.
- 2.(i) Reactivity series: Candidates should be able to:
- understand that the reactivity of elements can be used to order
elements
- relate the pattern in the reactions of the elements and their
compounds which are specified elsewhere in the syllabus to a reactivity
series
- recall reactions used to establish the following order of reactivity:
potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, (hydrogen) and
copper
- establish position within a reactivity series using displacement
reactions involving metals and their compounds in aqueous solutions.
- describe the sacrificial
protection of iron and mild steel in terms of the reactivity
series
- 2.(j)
Preparing and analysing:
Candidates should be able to:
3. Organic chemistry
- 3(a) Alkanes: Candidates should be able to:
- recall that alkanes as saturated
hydrocarbons
- explain the terms homologous series and general
formula
- recall that, in alkanes, the four bonds on each carbon atom are
directed to the corners of a tetrahedron
- draw displayed formulae for
alkanes
- explain the term
isomerism
- draw displayed formulae of alkanes containing up to five carbon atoms where they
exist, and name them (including isomers)
- describe the
chlorination of methane
- 3(b) Alkenes: Candidates should be able
to:
- recall that alkenes as unsaturated
hydrocarbons
- recall that, in alkenes, the three bonds on each carbon atom are
directed to the corners of an equilateral triangle
- draw displayed formulae for
alkenes up to 4 carbon atoms in a molecule
- describe the addition of halogens to
alkenes, including the decolorising of bromine water as a test for
alkenes
- (e) recall that e1hane-l,2-diol is made from ethene.
- 3(c) Ethanol: Candidates should be able to:
- recall the industrial preparation
by
- by fermentation of
sugars
- passing ethene and steam
over a heated phosphoric acid catalyst
- evaluate the factors
which are relevant to the choice of method to be used in the
manufacture of ethanol e.g. the relative availability of sugar
cane and crude oil
- describe the reaction of
ethanol with sodium
- describe the oxidation of ethanol to ethanoic
acid
- describe the dehydration of ethanol to
ethene
- describe the reaction of ethanol with carboxylic acids, such as
ethanoic acid, to form esters
- recall that many esters have distinct pleasant
smells
4. Physical chemistry
This section deals with some of the physical aspects of chemistry.
5. Chemistry in society
- 5(a) The
extraction and uses of metals: Candidates should be able to:
- describe and explain the
extraction of aluminium from purified aluminium oxide by
electrolysis , including: use of molten cryolite, need to replace
the positive electrodes and cost of the electricity as a major
consideration
- write ionic
half-equations for the reactions at the electrodes in aluminium
extraction
- describe the reaction of
carbon with metal oxides
- recall how iron is extracted
from iron ore in a blast
furnace using the raw materials: iron oxide ore, coke, limestone
and air
- describe and explain the
main reactions involved in the extraction of iron, including the
role of carbon dioxide and limestone
- describe the extraction of zinc by both electrolysis and reduction by
carbon monoxide
- describe the extraction of chromium by the Thermite
process
- explain how the methods of extraction of the metals in this section to
their positions in the reactivity series
- describe and explain the purification of
copper by electrolysis using impure copper as the positive
electrode, pure copper as the negative electrode in a solution of
copper(II) sulphate
- recall some important uses of the metals in this
section and relate the uses to specified properties
- 5(b) Natural oil and gas:
Candidates should be able to:
- recall that crude oil is a complex mixture of
hydrocarbons
- describe how crude oil is separated into
hydrocarbon fractions by fractional
distillation
- recall that the fractions obtained from crude
oil are refinery gases, gasoline, kerosene, diesel, fuel oil and
bitumen
- describe the physical properties and uses of the different
fractions
- recall that incomplete
combustion of fuels mat produce carbon monoxide
- recall that carbon monoxide
is poisonous because it reduces the capacity of blood to carry
oxygen
- recall that fractional distillation of crude oil produces more
long-chain hydrocarbons and fewer short-chain than required
- describe how long-chain hydrocarbons are cracked to give more
short-chain hydrocarbons
-
discuss the damage to the environment that may arise from
the spillage of crude oil and the release of hydrocarbons into the atmosphere.
- 5(c) Synthetic polymers: Candidates should be able to:
- recall that a polymer is formed by joining up many small molecules of
monomer
- recall that polymers may be made by two different
processes, addition
and condensation
- recall that ethene is used in the manufacture of the addition
polymer poly( ethene) (polyethene)
- describe the formation of poly( ethene ) and draw its
structure, showing the repeating unit
- apply the principles of addition polymerisation to other addition
polymers poly(propene) and poly(chloroethene)
- recall the uses of polymers:
poly(ethene), poly(propene) and poly(chloroethene) and be able to
link the properties to its use
- recall the types of monomers used in the manufacture of the condensation
polymer nylon
- describe the formation of nylon and draw its structure in a block
diagram format
- apply the principles of
condensation polymerisation to other condensation polymers,
including Terylene
- 5(d) The
manufacture of some important chemicals:
Candidates should be able to:
- recall how nitrogen, from
air, and hydrogen, from natural gas or the cracking of
hydrocarbons are used in the manufacture of ammonia
- recall the conditions used
in the Haber process: temperature of about 450oC, a
pressure of about 200 atmospheres, an iron catalyst, and how the
ammonia produced is liquified and any unused hydrogen and nitrogen
gases are recycled through the reactor
- recall the important uses of ammonia, including the manufacture of
nitric acid and NPK
fertilisers
-
describe the industrial manufacture of nitric acid from
ammonia
- recall the sources of
sulphur
- recall the raw materials used in the industrial manufacture
of sulphuric acid
- describe the industrial
manufacture of sulphuric acid by the Contact
Process, including essential conditions
- recall important uses of sulphuric
acid, to illustrate its economic importance
- understand that sulphur dioxide and nitrogen oxides are pollutant
gases which contribute to acid rain
- discuss some of the problems associated with acid
rain
- describe the industrial manufacture of sodium hydroxide and chlorine
by the electrolysis of sodium chloride solution (brine) in a diaphragm
cell
- recall some important uses of sodium hydroxide
(manufacture of soap, paper, ceramics) and
chlorine (in bleach and sterilising water supplies)
Some further
guidance on the specification content
Calculations
Candidates will be expected to perform a range of calculations as part of the
specification. These will include:
•
finding empirical and molecular formulae from experimental data
  5.
Empirical formula and formula mass of a compound from reacting masses
(easy start, not using moles)
8. Using
moles to calculate empirical formula and deduce molecular formula of a compound/molecule
(starting with reacting masses or % composition)
•
calculating percentage purity and percentage yield
14.
Other calculations e.g. % purity, % percentage & theoretical yield,
•
mass/mass and mass/volume calculations i.e. calculating the mass of solid or
volume of gas in a chemical equation, given data about the mass or volume of
another reactant
7.
Introducing moles: The connection between moles, mass and formula mass - the basis of reacting mole ratio calculations
(relating reacting masses and formula mass).
•
using Avogadro’s Law to equate the ratio of the number of moles and the volumes
of reacting gases
10.
Reacting gas volume
ratios, Avogadro's Law
and Gay-Lussac's Law (ratio of gaseous
reactants-products)
•
standard acid / alkali titrations
12. Volumetric titration calculations
e.g. acid-alkali titrations
(and diagrams of apparatus)
•
conversion of gdm-3 to moldm-3
for solutions
11.
Molarity, volumes and solution
concentrations (and diagrams of apparatus)
•
electrolysis calculations involving the expression Q
= It and Faraday constant
13. Electrolysis products calculations
(negative cathode and positive anode products)
•
bond energy calculations
15.
Energy transfers in physical/chemical changes - section on bond energies
“The
simple physical and chemical properties of compounds of Group 1 and Group 2
elements”
Candidates will be expected to know the following information:
• the
solubility of the hydroxides, halides, sulphates, nitrates and carbonates of the
elements of Group 1
•
Group 1 oxides react with water to form solutions containing hydroxide ions
•
Group 1 hydroxides dissolve in water to form alkaline solutions
•
the solubility of the hydroxides, sulphates,
nitrates and carbonates of the elements of Group 2
•
Group 2 oxides react with water to form hydroxides
•
Group 2 hydroxides are slightly soluble in water,
forming alkaline solutions
•
the thermal decomposition of carbonates of Group 2
elements
“The
simple physical and chemical properties of copper(II) compounds”
Candidates will be expected to know the following information:
• the
colour and solubility of copper(II) oxide, hydroxide, chloride,
sulphate, nitrate and carbonate
•
the thermal decomposition of copper(II) carbonate
and nitrate
• the
reduction of copper(II) oxide to copper
“Physical properties and simple chemistry of ammonia and its compounds”
Candidates will be expected to know the following information:
• the
solubility of ammonia in water; and that the solution formed is alkaline
• a
simple test for ammonia (using damp litmus)
•
that ammonia is colourless, less dense than air and has a pungent odour
• the
reaction of ammonium ions with an alkali, such as sodium hydroxide, to produce
ammonia
•
ammonium salts are soluble
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