|
  Doc
Brown's Chemistry Clinic
GCE
O level chemistry - syllabus 7081
EDEXCEL
LONDON INTERNATIONAL CHEMISTRY
My
unofficial support for this syllabus
EDEXCEL AS Chemistry (not Nuffield)
EDEXCEL A2 Chemistry
EMAIL PLEASE
if this page is of ANY USE?? or you have a query or spotted an error
or you can't find any notes on some aspect of the syllabus
Other KS4/GCSE/IGCSE Science-CHEMISTRY syllabus that
might be yours and NOT this one!
Full list of IGCSE-KS4-GCSE Chemistry, Earth
Science & Radioactivity REVISION NOTES
Useful GCSE mini site-map of Doc Brown's
Chemistry Clinic saveable to Desktop and all links work from
Desktop
PLEASE READ THE FOLLOWING VERY CAREFULLY
My
UNOFFICIAL SUPPORT for
this
CHEMISTRY syllabus are outlined below. PLEASE REMEMBER it is
your responsibility to know what to revise, not mine!, BUT I hope my little
contributions help students too.
PLEASE remember the
notes are NOT complete and not just for your particular syllabus, but are
designed to cover, eventually, any Chemistry, Earth Science and Radioactivity of
any GCSE syllabus. When you follow a link you will find some useful information
on the web page about the topic you are researching. Sometimes the link goes
straight to the relevant paragraph but otherwise use the sub-indexes of key
words or headings at the top of each page. All the syllabus-topic-unit titles
are taken from the official GCSE syllabuses.
[Reference links
to pages within
this site] For quizzes: F = UK
Foundation-easier and H = UK Higher-harder!
Syllabus content
 1. Principles of
chemistry
The experimental basis
underlying much of this section, e.g. atomic and ionic theory and the Periodic Table, is to be found in the other sections. The discussion of
atomic and ionic theories should lead to the ability to interpret what is seen in the
laboratory in terms of molecules, atoms, ions and electrons and their movement. Molecular and
ionic equations should be used to contribute to this end.
-
1.1 Atoms: Candidates should be able to:
-
(a) recall simple experiments leading to the idea of the smallness of
particles and to their motion including dilution of coloured solutions, diffusion experiments and
Brownian motion
-
(b) define an element, and an atom as the particle of which elements are
composed
-
(c) recall that atomic masses are the masses of atoms relative to
12C = 12
and are referred to as relative atomic masses
-
(d) understand a mole of atoms as a number of atoms equal to the Avogadro
constant.
-
LINKS: [atomic
structure, calculations,
atoms/elements and
states of matter]
-
1.2 Chemical
formulae: Candidates should be able to:
-
(a) apply the idea of a mole of atoms in finding the chemical
formulae
-
(b) recall investigations to find the formulae of simple compounds such
as copper(II) oxide and water
-
(c) recall that the formulae of other compounds have been obtained
experimentally
-
LINKS: [calculations]
-
1.3 Relative
molecular and formula masses: Candidates should be able to:
-
(a) 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
-
(b) find the molar volumes of some gases from practical data and from
relative formula masses and densities and from them deduce Avogadro's law
-
(c) understand the significance of the molar volume of a gas.
-
LINKS: [calculations]
-
1.4 Chemical
equations: Candidates should be able to:
-
(a) recall quantitative experimental investigations, 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
-
(b) write balance chemical equations to represent the reactions studied
in this syllabus
-
(c) recall that the State symbols
(l), (s), (g) and (aq) are used in
chemical equations to represent liquids, solids, gases and aqueous solutions respectively.
-
LINKS: [calculations,
equation
section and Types
of Chemical Reaction]
-
1.5 The Periodic
Table: Candidates should be able to:
-
(a) appreciate the Periodic Table as the arrangement of elements in a
table according to atomic number
-
(b) classify elements as 'metals' and 'non-metals' on the basis of their
properties and be aware that some elements exhibit a mixture of the properties of metals and
non-metals
-
(c) recall families of elements including the alkali metals (Group 1), the
alkaline earth metals (Group 2) and the halogens (Group 7)
-
(d) discuss the correlation of charges of ions with position in the
Periodic Table
-
(e) discuss the relative reactivity of the elements in groups of metals
and non-metals
-
(f) recall the noble gases (Group 0) as a family of inert
gases
-
(g) discuss sequences in the valencies of the elements across periods such
as CH4, NH3, OH2, ClH
-
LINKS: [Periodic
Table,
Gp1
Alkali Metals,
Gp7 Halogens,
Gp0 Noble Gases,
bonding,
section on
valency]
-
1.6 Structure of the atom in
relation to the Periodic Table: Candidates should be able to:
- (a) recall the structure of an atom in terms of protons, neutrons and
electrons
- (b) explain the terms atomic number. mass number. isotopes and relative
atomic mass
- (c) relate periodicity to electronic
configuration
- (d) 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)
- (e) link electron configuration and ionic
charge
- (t) appreciate the importance of the noble gas electron configurations
(2;
2.8; 2.8.8; 2.8.18.8; 2.8.18.18.8).
- LINKS: [atomic
structure and
periodic table]
-
1.7 Ionic compounds: Candidates should be able to:
- (a) describe the formation of ions by gain or loss of
electrons
- (b) describe the formation of ionic crystals such as sodium
chloride
- (c) appreciate the ionic bond as the result of an attraction between
oppositely charged ions
- (d) describe an ionic crystal as a giant three-dimensional ionic
structure held together by attraction between oppositely charged ions.
- LINKS: [ionic bonding]
-
1.8 Electrolysis: Candidates should be able
to:
- (a) recall simple experiments to distinguish between electrolytes and
non-electrolytes
- (b) understand an electric current as a flow of electrons or
ions
- (c) recall the faraday as a mole of
electrons
- (d) recall quantitative studies of the products of the electrolysis of
molten salts or aqueous solutions
- (e) recall the charges on common ions met in the
syllabus
- (t) write ionic equations representing the reaction at each electrode
during electrolysis
- (g) understand oxidation and reduction as the loss and gain of electrons
respectively
- (h) appreciate that experiments on migration of ions provides some
evidence for the ionic theory
- (i) connect displacement experiments between metals and ions with work on
the reactivity series.
- LINKS: [introduction
+ summary,
reactivity-redox and calculations]
-
1.9 Covalent compounds: Candidates should be able to:
- (a) describe the formation of covalent bonds by sharing of
electrons
- (b) appreciate the covalent bond as the result of attraction between the
bonding pair of electrons and the nuclei of the atoms involved in the bond
- (c) recall the existence of simple molecular crystals of ice, solid carbon
dioxide, solid methane, solid ammonia and iodine at suitable temperatures
- (d) describe the shapes of the above molecules and the weak forces
between the molecules in the crystals
- (e) appreciate that weak intermolecular forces result in low melting
points and boiling points
- (f) describe the giant molecular covalent crystals of diamond and
graphite
- (g) appreciate that atoms in diamond and graphite are held together by
strong covalent bonds which result in high sublimation points.
- LINKS: [covalent bonding]
-
1.10 Metallic crystals: Candidates should be able to:
- (a) describe a metal as a giant structure in which electrons are free to
move throughout the whole structure
- (b) relate the structure of a metal to observable properties such as
conductivity and malleability .
- LINKS:
[metallic
bonding and
uses
of metals]
2. Chemistry of the elements
This section is concerned with the simple inorganic chemistry of metals
and non-metals.
-
2.1 The Group 7 elements
chlorine, bromine and iodine: Candidates should be able to:
- (a) describe the physical characteristics of the
elements
- (b) recall the inter-conversion of halogen and halide
ion
- (c) appreciate the difference between hydrogen chloride and hydrochloric
acid
- (d) describe the properties of solutions of hydrogen chloride in water and
in methylbenzene
- (e) describe the laboratory preparation of chlorine from hydrochloric
acid
- (f) state a simple chemical test for chlorine
- (g) discuss similarities in the chemistry of these elements which
establish them as a family of elements
- (h) discuss reactions in which one halogen displaces
another
- (i) make predictions about the properties of other
halogens
- (j) make appropriate links between this section and the chlorides of the
metals in sections 2. 7, 2.8 and 2.9, and other halides of the Group 1 elements.
- LINKS: [halogens,
gas tests,
periodic table and ionic
bonding-formula]
-
2.2 Oxygen: Candidates should be able to:
- (a) recall the industrial extraction of oxygen, by fractional
distillation, from liquid air
- (b) recall the gases present in air and their approximate percentage by
volume
- (c) understand oxidation and reduction as the addition and removal of
oxygen respectively
- (d) state a simple chemical test for
oxygen
- (e) discuss the reactions with oxygen in air of magnesium, iron, copper,
carbon, sulphur and methane
- (f) recall how to determine the percentage by volume of oxygen in the air
from at least one of the above reaction
- (g) discuss oxides of carbon, nitrogen and sulphur and their reactions
with water
- (h) recall the conditions under which iron
rusts
- (i) describe how rusting of iron may be prevented by grease, oil, paint,
plastic and galvanising
- (j) discuss the reduction of oxides in terms of the reactivity of
elements.
- LINKS: [metal
reactivity-redox-rusting,
metal
extraction,
gas
tests and
note
in Q1 earth science page]
-
2.3 Sulphur: Candidates should be able to:
- (a) recall industrial sources of
sulphur
- (b) describe the physical characteristics of the element including its
allotropes
- (c) recall the nature of sulphur
dioxide
- (d) state a simple chemical test for sulphur
dioxide
- (e) describe the reaction of sulphur dioxide with
alkalis
- (f) describe the reaction of sulphites with dilute
acids
- (g) state a precipitation test for sulphates.
- LINKS: [extra
industrial chemistry and ion
and gas
tests]
-
2.4 Nitrogen: Candidates should be able to:
- (a) recall the industrial extraction of nitrogen, by fractional
distillation, from liquid air
- (b) recall the importance of the inert nature of nitrogen in protecting
food
- (c) describe the laboratory preparation of
ammonia
- (d) recall the physical properties of
ammonia
- (e) state a simple chemical test for
ammonia
- (f) recall the reaction of nitrogen with oxygen to form nitrogen monoxide
and nitrogen dioxide
- (g) discuss the simple chemistry of aqueous ammonia, ammonium chloride,
ammonium nitrate and ammonium sulphate
- (h) recall that nitric acid is made from
ammonia
- (i) make appropriate links between this section and the nitrates of the
metals in section 2.7 and the
reaction of copper with nitric acid in section 2.9.
- LINKS: [ammonia
etc. and ion
and gas
tests]
-
2.5 Carbon: Candidates should be able to:
- (a) describe the physical characteristics of the element including its
allotropes
- (b) discuss the differences in the physical characteristics and
reactivity of diamond and graphite in relation to their structures
- (c) discuss the reaction of carbon with metal
oxides
- (d) describe the laboratory preparation of carbon
dioxide
- (e) recall the physical and chemical properties of carbon
dioxide
- (f) state a simple chemical test for carbon
dioxide
- (g) recall common uses of carbon dioxide including carbonating drinks and
in fire extinguishers
- (h) recall that incomplete combustion of fuels may produce carbon
monoxide
- (i) discuss the toxic nature of carbon monoxide and its effect on the
body
- (g) make appropriate links between this section and the carbonates of the
metals in section 2.7 and copper(II) carbonate in section 2.9.
- LINKS: [bonding,
oil-fuels-combustion,
acid reactions, and gas
tests etc.]
-
2.6 Hydrogen: Candidates should be able to:
- (a) recall the effect of dilute hydrochloric and dilute sulphuric acids on
magnesium, aluminium, zinc and iron
- (b) describe the laboratory preparation of
hydrogen
- (c) state a simple chemical test for
hydrogen
- (d) describe the combustion of hydrogen with oxygen to form
water
- (e) state a simple chemical test to show the presence of
water
- (f) describe a physical test to show if water is
pure
- (g) describe the reaction of hydrogen with chlorine.
- LINKS: [acid reactions,
reactivity of metals with acids,
gas
tests etc.
and
Halogens]
-
2.7 The Group 1 elements
lithium, sodium and potassium: Candidates should be able to:
- (a) describe the action of these elements on
water
- (b) recognise that the reactivities of these elements with water provides
a basis for their recognition as a family of elements
- (c) discuss the simple physical and chemical properties of the hydroxides,
halides, sulphates, nitrates and carbonates of these elements in terms of general
patterns of behaviour
- (d) make predictions about other elements and their compounds in this
group.
- LINKS: [Alkali
Metals and
metal reactivity]
-
2.8 The Group 2 elements
magnesium and calcium: Candidates should be able to:
- (a) describe the action of these elements on
water
- (b) discuss the simple physical and chemical properties of the
oxides,
hydroxides, chlorides and carbonates of these elements in terms of general patterns of
behaviour
- (c) make predictions about other elements and their compounds in this
group.
- LINKS: [metal
reactivity,
acid reactions and
very detailed
chemistry! (written for AS-A2-IB students)]
-
2.9 The transition metals iron
and copper: Candidates should be able to:
- (a) describe the action of steam, hydrogen chloride and chlorine on
iron
- (b) discuss the formation of
iron(II) and iron(III) hydroxides
- (c) describe the action of nitric acid on
copper
- (d) discuss the simple chemical and physical properties of
copper(II)
oxide, hydroxide, nitrate, sulphate, carbonate, and chloride
- (e) recall the existence of copper(I) compounds such as
copper(I) oxide
- (f) describe the reaction of
copper(II) ions with ammonia to form the
complex ion [Cu(H20)2(NH3)4]2+
- (g) appreciate 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.
- LINKS: [transition
metals]
-
2.10 Reactivity series: Candidates should be able to:
- (a) appreciate that the reactivity of elements can be used to order
elements
- (b ) relate the pattern in the reactions of the elements and their
compounds which are specified elsewhere in the syllabus to a reactivity
series
- (c) recall evidence used to establish the following order of reactivity:
potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, (hydrogen) and
copper
- (d) establish position within a reactivity series using displacement
reactions involving metals and their compounds in aqueous solutions.
- LINKS:
[metal reactivity]
-
2.11 Simple tests for ions:
Candidates should be able to:
- (a) recall simple tests for the cations sodium, potassium, calcium,
ammonium, copper(II), iron(II) and iron(III) (flame tests are sufficient for sodium,
potassium and calcium)
- (b) recall simple tests for the anions chloride, bromide and
iodide;
sulphate and carbonate.
- LINKS: [chemical
id tests]
3. Organic chemistry
This section provides a simple introduction to the organic chemistry of
carbon.
-
3.1 Alkanes: Candidates should be able to:
- (a) identify alkanes as saturated
hydrocarbons
- (b ) explain the terms homologous series and general
formula
- (c) recall that, in alkanes, the four bonds on each carbon atom are
directed to the corners of a tetrahedron
- (d) draw displayed formulae for
alkanes
- (e) explain the term
isomerism
- (f) draw isomers of alkanes containing up to five carbon atoms where they
exist, and name them
- (g) describe the halogenation of alkanes.
- LINKS:
[oil
products,
extra
organic and
lots of
examples!]
-
3.2 Alkenes: Candidates should be able
to:
- (a) identify alkenes as unsaturated
hydrocarbons
- (b) recall that, in alkenes, the three bonds on each carbon atom are
directed to the corners of an equilateral triangle
- (c) draw displayed formulae for
alkenes
- (d) describe the addition of halogens to
alkenes
- (e) recall that e1hane-l,2-diol is made from ethene.
- LINKS: [oil
products, extra
organic and lots of
examples!]
-
3.3 Ethanol: Candidates should be able to:
- (a) discuss the industrial preparation of ethanol by fermentation and the
hydrolysis of ethene
- (b) describe the reaction of ethanol with sodium and phosphorus
pentachloride
- (c) describe the oxidation of ethanol to ethanoic
acid
- (d) describe the dehydration of ethanol to
ethene
- (e) describe the reaction of ethanol with carboxylic acids, such as
ethanoic acid, to form esters
- (f) recall that many esters have distinct pleasant
smells
- LINKS:
[oil
products, extra
organic and extra
industrial chemistry]
4. Physical chemistry
This section deals
with some of the physical aspects of chemistry
5. Chemistry in society
It is intended that this aspect of Chemistry should add relevance and
interest to the whole course. The material of this section could be integrated into the course
wherever suitable as soon as the underlying principles have been met. It is important to
present Chemistry as a developing subject and to bring pupils to an appreciation of its nature
and scope. For this reason a fairly wide range of material is covered but detailed treatment
is not expected. In the treatment of industrial processes the emphasis should be on the raw
materials available, the demand for products and the principles underlying the processes. Some
attention should also be give to the environmental problems that may arise as a result of
the processes.
-
5.1 Principles underlying the
extraction of metals: Candidates should be able to:
- (a) recall the raw materials used in the production of
aluminium
- (b) describe the electrolysis of a solution of
alumina (Al2O3, bauxite ore) in
cryolite
- (c) recall the raw materials used in the manufacture of
iron
- (d) describe the extraction of iron in the blast
furnace
- (e) identify carbon monoxide as the reducing agent in the above
process
- (f) describe the extraction of zinc by both electrolysis and reduction by
carbon monoxide
- (g) describe the extraction of chromium by the Thermite
process
- (h) relate the methods of extraction of the metals in this section to
their positions in the reactivity series
- (i) describe the use of electrolysis in the purification of
copper
- (j) recall some important uses of the metals in this
section
- (k) discuss some of the problems of dealing with waste from
metal-extracting
processes.
- LINKS: [metal
extraction, intro-summary-links
on electrolysis, extra
industrial chemistry and
metal reactivity]
-
5.2 Natural oil and gas: Candidates should be able to:
- (a) recall that crude oil is a complex mixture of
hydrocarbons
- (b) describe how crude oil is separated into fractions by fractional
distillation
- (c) identify the fractions obtained from crude
oil
- (d) state the physical properties and uses of the different
fractions
- (e) recall that fractional distillation of crude oil produces more
long-chain hydrocarbons and less of the short-chain than required
- (f) describe how long-chain hydrocarbons are cracked to give more
short-chain hydrocarbons
- (g) discuss the potential damage to the environment that may arise from
the spillage of crude oil and the release of hydrocarbons into the atmosphere.
- LINKS: [oil
products]
-
5.3 Synthetic polymers: Candidates should be able to:
- (a) recall that a polymer is formed by joining up many small molecules of
monomer
- (b) recall that polymers may be made by two different
processes, addition
and condensation
- (c) recall that ethene is used in the manufacture of the addition
polymer poly(ethene) (polyethene)
- (d) describe the formation of poly( ethene ) and draw its
structure
- (e) apply the principles of addition polymerisation to other addition
polymers, including poly(phenylethene) (old name 'polystyrene')
- (t) recall the monomers used in the manufacture of the condensation
polymer nylon
- (g) describe the formation of nylon and draw its structure in a block
diagram format
- (h) apply the principles of condensation polymerisation to other condensation
polymers, including terylene
- LINKS: [oil
products, extra
organic and bonding]
-
5.4 The heavy chemicals industry:
Candidates should be able to:
- (a) recall the raw materials used in the industrial manufacture of
ammonia
- (b) describe the industrial synthesis of ammonia via the Haber
Process
- (c) recall important uses of ammonia including the manufacture of NPK
fertilisers
- (d) describe the industrial manufacture of nitric acid from
ammonia
- (e) recall the raw materials used in the industrial manufacture
of sulphuric acid
- (f) describe the industrial synthesis of sulphuric acid via the Contact
Process
- (g) recall important uses of sulphuric
acid
- (h) appreciate that sulphur dioxide and nitrogen oxides are pollutant
gases which contribute to acid rain
- (i) discuss some of the problems associated with acid
rain
- (j) describe the industrial manufacture of sodium hydroxide and chlorine
by the electrolysis of brine
- (k) recall important uses of sodium hydroxide and
chlorine
- (l) describe the manufacture of soap
- LINKS:[ammonia,
extra industrial
chemistry, extra
organic , oil-fuels
etc. and
brine electrolysis]
This page is designed
to help with the learning-revision for EDEXCEL
LONDON INTERNATIONAL CHEMISTRY GCE
O level chemistry - syllabus 7081 science examinations, concentrating
on revising the chemistry of the syllabus.
*
Copyright © Dr W P Brown 2000-2008 All rights reserved
for the
revision notes pages, quizzes, worksheets etc. *
Doc Brown's Chemistry Clinic *
www.docbrown.info/ *
|
10Q multiple choice test 
10Q short
answer questions
multi-word fill question 
crossword puzzle 
revision notes; 
syllabus/summary
structured question (+ans) 
data, 
useful internal or external link