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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.
describe the states of matter and explain their interconversion in terms of
the kinetic particle theory
describe and explain diffusion.
describe evidence for the movement of particles in gases and liquids
(A treatment of Brownian motion is not required).
describe dependence of rate of diffusion on molecular mass (treated
qualitatively)
States of Matter (gas,
liquid and solid)
2. Experimental Techniques
2.1 Measurement
name appropriate apparatus for the measurement of time, temperature, mass
and volume, including burettes, pipettes and measuring cylinders (some mention
in salt preparations)
2.2(a) Criteria of purity
describe paper chromatography and how interpret simple chromatograms.
outline how chromatography techniques can be applied to colourless
substances by exposing chromatographs to substances called locating agents
(knowledge of specific locating agents is not required)
identify substances and assess their purity from melting point and boiling
point information
understand the importance of purity in substance in everyday life, eg.
foodstuffs and drugs
Elements, Compounds, Mixtures
and their Separation
2.2(b) Methods of purification
describe methods of purification by the use of a suitable solvent,
filtration (see 8.3), crystallisation (see 8.3), distillation (including use of fractionating
column and refer to the fractional distillation of : crude oil (section 14.2), fermented
liquor (section 14.6).
suggest suitable purification techniques, given information about the
substances involved
Elements, Compounds, Mixtures
and their Separation and
Oil Products
3. Atoms, elements and
compounds
3.1 Atomic structure and
the Periodic Table
state the relative charges and approximate relative masses of protons,
neutrons and electrons
define proton (atomic) number and nucleon (mass) number
use proton number and the simple structure of atoms to explain the basis of
the Periodic Table (see section 9), with special reference to the elements of
proton number 1 to 20
define isotopes
state the two types of isotopes as being radioactive and non-radioactive
state one medical and one industrial use of radioactive isotopes
describe the build-up of electrons in ‘shells’ and understand the
significance of the noble gas electronic structures and of valency electrons
(The ideas of the distribution of electrons in s and p orbitals and in d block
elements are not required. Note that a copy of the Periodic Table will be available in the examination).
describe the differences between elements mixtures and compounds, and
between metals and non-metals.
Elements, Compounds, Mixtures etc.
and The
Periodic
Table
describe alloys, such as brass, as a mixture of a metal with other elements.
Structure
and Bonding (ionic, covalent, metallic)
3.2(a) Ions and ionic bonds
describe the formation of ions by electron loss or gain
describe the formation of ionic bonds between metallic and non-metallic
elements
describe the formation of ionic bonds between elements from Groups I and VII
describe the lattice structure of ionic compounds as a regular arrangement
of alternating positive and negative ions
Structure
and Bonding
3.2(b) Molecules and covalent bonds
describe the formation of single covalent bonds in H2, Cl2,
H2O, CH4 and HCl as the sharing of pairs of electrons
leading to the noble gas configuration
describe the electron arrangement in 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
Structure
and Bonding
3.2(c) Macromolecules
describe the giant covalent structures of graphite and diamond
describe the macromolecular structure of silicon (IV) oxide (silicon
dioxide)
relate their structures to the use of graphite as a lubricant and of diamond
in cutting
describe the similarity in properties between diamond and silicon (IV)
oxide, related to their structures
Structure
and Bonding (section on 3D giant covalent)
and Notes on polymer macromolecules
3.2(d) Metallic bonding
describe metallic bonding as a lattice of positive ions in a ‘sea of
electrons’ and use this to describe the electrical conductivity and
malleability of metals
Structure
and Bonding
including alloy structure
4. Stoichiometry
use the symbols of the elements and write the
formulae of simple compounds
deduce the formula of a simple compound from the relative numbers of atoms
present
determine the formula of an ionic compound from the charges on the ions
present
deduce the formula of a simple compound from a model or a diagrammatic
representation
construct word equations and simple balanced chemical equations
construct equations with state symbols, including ionic equations
deduce the balanced equation for a chemical reaction, given relevant
information
define relative atomic mass, Ar.
(A means mass number)
define relative molecular mass, M as the sum of the relative atomic masses
(relative formula mass or M, will be used for ionic compounds)
(Calculations involving reacting masses may be set involving simple
proportions)
Chemical Equations
Chemical CalculationsNotes
and examples with questions built in (14exercises ready)
Atomic
Structure and the
Periodic Table
4.1 The mole concept
define the mole and the Avogadro constant
use the molar gas volume, taken as 24 dm3 at room temperature
and pressure
calculate stoichiometric reacting masses and volumes of gases and
solutions, solution concentrations expressed in g/dm3 and mol/dm3.
(Calculations involving the idea of limiting reactants may be set. Questions
on the gas laws and the conversion of gaseous volumes to different
temperatures and pressures will not be set).
calculate empirical formulae and molecular formulae
calculate % yield and % purity
Chemical CalculationsNotes
and examples
with questions built in (14exercises ready)
5. Electricity and
Chemistry
describe the electrode products in the
electrolysis of: molten lead (II) bromide; concentrated hydrochloric
acid; concentrated aqueous
sodium chloride - between inert electrodes (platinum or carbon)
relate the products of electrolysis to the electrolyte and electrodes used,
exemplified by the specific examples together with aqueous copper (II)
sulphate using carbon electrodes and using copper electrodes (as used in the
refining of copper)
state the general principle that metals or hydrogen are formed at the
negative electrode (cathode), and that non-metals (other than hydrogen) are
formed at the positive electrode (anode)
describe electrolysis in terms of the ions present and reactions at the
electrodes in the examples given
predict the products of the electrolysis of a specified binary compound in
the molten state
predict the products of electrolysis of a specified halide in dilute or
concentrated aqueous solution
describe, in outline, the manufacture of (i) aluminium from pure aluminium
oxide in molten cryolite, (ii) chlorine and sodium hydroxide from concentrated
aqueous sodium chloride (Starting
materials and essential conditions should be given but no technical details or
diagrams).
describe the electroplating of metals and name the uses of electroplating
describe the reasons for the use of copper and (steel-cored) aluminium in
cables, and why plastics and ceramics are used as insulators
Group 7 "The
Halogens"
for the electrolysis of sodium chloride
(task
sheet)
Group 7 "The
Halogens" etc. The
Halogens
and The
Electrolysis of Salt etc.
Extraction & purification of Metals
(Fe, Al, Cu)
Introduction to and summary of electrolysis and
Extra Industrial Chemistry, uses of metals
6. Chemical Changes
6.1 Energetics of a
reaction
describe the meaning of exothermic and endothermic reactions
describe bond breaking as endothermic and bond forming as exothermic
Energy Transfers in Chemical
Reactions (revision of physical/chemical changes)
describe the production of electrical energy from simple cells,
i.e.. two
electrodes in an electrolyte (This should be linked with the reactivity series
in section 10.2 and redox in section 7.3) (see Metal
Reactivity)
state the use of batteries as a convenient portable energy source
describe the effect of concentration, particle size, catalysts (including
enzymes) and temperatures on the speeds of reactions
describe a practical method for investigating the speed of a reaction
involving gas evolution
devise a suitable method for investigating the effect of a given variable
on the speed of a reaction
interpret data obtained from experiments concerned with speed of reaction
describe and explain the effects of temperature and concentration in terms
of collisions between reacting particles
describe the effect of light on the speed of reactions
describe the application of the above factors to the danger of explosive
combustion with fine powders (eg. flour mills) and gases (eg. mines)
describe the use of silver salts in photography as a process of reduction
of silver ions to silver; and photosynthesis as the reaction between carbon
dioxide and water in the presence of chlorophyll and sunlight (energy) to
produce glucose
Rates of Reactions
Energy Transfers in Chemical
Reactions (including activation energy)
7.2 Reversible
reactions
describe the idea that some chemical reactions can be reversed by changing
the reaction condition, limited to the effects of heat on hydrated salts (see
extraction and corrosion of metals)
predict the effect of changing the conditions (temperature and pressure) on
other reversible reactions
understand the concept of equilibrium
Reversible reactions and
Ammonia synthesis and uses
7.3 Redox
define oxidation and reduction in terms of oxygen loss/gain (see
10.3 extraction
and corrosion of metals)
define redox in terms of electron transfer (Oxidation state limited to its use to name ions, eg. iron(II), iron(III),
copper(II), manganate(VII) dichromate (VI).
identify redox reactions by changes in oxidation state and by the colour
changes involved when using acidified potassium manganate(VII), and potassium
iodide. (Recall of equations involving KMnO4 is not required).
Reactivity
of Metals, Corrosion and Redox
Reactivity;
rusting etc.
8. Acids, bases and salts
8.1 The characteristic properties of acids
and bases
describe the characteristic properties of acid as reactions with metals,
bases, carbonates and effect on litmus
define acids and bases in terms of proton transfer, limited to aqueous
solutions
describe the meaning of weak and strong acids and bases
describe the characteristic properties of bases as reactions with acids and
with ammonium salts and effect on litmus
describe neutrally and relative acidity and alkalinity in terms of pH (whole
numbers only) measured using Universal Indicator paper
describe and explain the importance of controlling acidity in soil
describe the preparation, separation and purification of salts as examples
of some of the techniques specified in section 2.2(b) and the reaction
specified in section 8.1
describe the preparation of insoluble salts by precipitation
suggest a method of making a given salt from suitable starting materials,
given appropriate information
more on salt preparations on "extra aqueous chemistry" page
8.4 Identification of
ions and gases
describe the following tests to identify :
aqueous cations: aluminium, ammonium, calcium, copper (II), iron (II), iron (III), and zinc,
(using aqueous sodium hydroxide and aqueous ammonia as appropriate). (Formulae of complex ions are not required).
anions: carbonate (by reaction with dilute acid and then limewater), chloride (by
reaction under acidic conditions with aqueous silver nitrate), iodide (by
reaction under acidic conditions with aqueous lead (II) nitrate), nitrate (by
reduction with aluminium), sulphate (by reaction under acidic conditions with
aqueous barium ions)
describe lithium, sodium and potassium in Group I as a collection of
relatively soft metals showing a trend in melting point, density, in reaction
with water.
predict the properties of other elements in
Group 1, given data, where
appropriate
describe chlorine, bromine and iodine in Group VII as a collection of
diatomic non-metals showing a trend in colour, state and their reaction with
other halide ions
predict the properties of other elements in Group
7 given data, where
appropriate
identify trends in other Groups given information about the elements
concerned
Group 1 "The Alkali Metals"
Group 7 "The
Halogens" etc. The
Halogens The
Electrolysis of Salt etc.
9.3 Transition elements
describe the transition element 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
Transition Metals
General
tests on Metals (in the Periodic
Table - Alkali + Transition)
and
Extra Industrial Chemistry - uses of metals
9.4 Noble gases
describe the noble gases as being unreactive
describe the uses of the noble gases in providing an inert atmosphere,
i.e..
argon in lamps; helium for filling balloons
Group 0 Noble Gases
10 Metals
10.1 Properties of metals
describe the general physics and chemical properties of metals
explain why metals are often used in the form of alloys
identify representations of alloys from diagrams of structures
"Extra Industrial
chemistry" - uses of metals and Bonding - metals-alloys structure
10.2 Reactivity series
place in order of reactivity: calcium, copper, (hydrogen), iron, magnesium,
potassium, sodium and zinc by reference to the reactions, if any, of the
metals with: water or steam, dilute hydrochloric acid and the reduction of their oxides
with carbon
describe the reactivity series as related to the tendency of a metal to
form its positive ion, illustrated by its reaction, if any, with the aqueous
ion or the oxides of the other listed metals
describe the action of heat on the hydroxides and nitrates of the listed
metals (in 1st section, thermal
decomposition)
account for the apparent un-reactivity of aluminium in terms of the oxide
layer which adheres to the metal
deduce an order of reactivity from a given set of experimental results
Metal Reactivity, Corrosion and Redox ;
rusting etc.
see also notes on "Extra Industrial
chemistry" - uses of metals
10.3(a) Extraction of metals
describe the ease in obtaining metals from their ores by relating the
elements to the reactivity series
describe the essential reactions in the extraction of iron from haematite
describe the conversion of iron into steel
describe, in outline, the extraction of zinc from zinc blende
describe, in outline, the extraction of
aluminium from pure aluminium oxide and name the main ore of aluminium
Extraction
and purification of Metals (Fe, Al, Cu)
Metal
Reactivity & Extraction (combination: Reactivity + Extraction tests)
10.3(b) Uses of metals
name the uses of aluminium: in the manufacture of aircraft because of its
strength and low density; in food containers because of its resistance to
corrosion
describe the idea of changing the properties of iron by the controlled use
of additives to form steel alloys
name the uses of mild steel (car bodies and machinery) and stainless steel
(chemical plant and cutlery)
name the uses of zinc for galvanising and for making brass
name the uses of copper related to its properties; electrical wiring and in
cooking utensils
describe the composition of clean air as being approximately 79% nitrogen,
20% oxygen and the remainder as being a mixture of noble gases, water vapour
and carbon dioxide (Earth Science
notes section Q1.)
name the common pollutants in the air as being carbon monoxide, sulphur
oxides of nitrogen and lead compounds (see "Oil"
and "Fuels")
state the source of each of these pollutants:
carbon monoxide from the
incomplete combustion of carbon-containing substance; sulphur dioxide from the combustion of fossil fuels which contain sulphur
compounds (leading to ‘acid rain’); oxides of nitrogen and lead compounds from car exhausts
(Oil -
combustion - pollution)
describe and explain the presence of oxides of nitrogen in car exhausts and
their catalytic removal (Oil - combustion -
pollution
describe methods of rust prevention: paint and other coatings, to exclude
oxygen and galvanising AND describe sacrificial protection in terms of the
reactivity series of metals
(see 10.2 and 10.3 for notes and test links)
describe the need for nitrogen, phosphorus and
potassium containing
fertilisers (see ammonia)
describe the essential conditions for the manufacture of ammonia by the
Haber process including the source of the hydrogen and nitrogen, i.e..
hydrocarbons or steam and air (see ammonia)
Reversible reactions and
Ammonia synthesis and uses
Chemical Tests + reaction notes; and
notes on "Types of Reactions"
12. Sulphur
name some sources of sulphur
name the use of sulphur in the manufacture of sulphuric acid
name the uses of sulphur dioxide as a bleach in the manufacture of wood
pulp for paper; as a food preservative (by killing bacteria)
describe the manufacture of sulphuric acid by the Contact process
describe the properties of dilute sulphuric acid as a typical acid
name the uses of sulphuric acid as in the manufacture of detergents and
fertilisers
see also notes on "Extra Industrial
chemistry" - sulphuric acid
13. Carbonates
describe the manufacture of lime (calcium
oxide) from calcium carbonate (limestone) in terms of the chemical reactions
involved
name some uses of lime and slaked lime as in treating acidic soil and
neutralising acidic industrial waste products
name the uses of calcium carbonate in the manufacture of iron and of cement
see also notes on "Extra Industrial
chemistry" - Limestone
14. Organic Chemistry
14.1 Names of compound
name, and draw the structures of, methane, ethane, ethanol. ethanoic acid
and the products of the reactions stated in sections 14.4 – 14.6
name, and draw the structures of, the unbranched alkanes, alkenes (not
cis-trans), alcohols and acids containing up to four carbon atoms per molecule
state the type of compound present given a chemical name, ending in –ane,
-ene, -ol, or –oic acid or a molecular structure
Oil and useful products
(fuel, plastics)and Extra
Organic Chemistry
14.2 Fuels
name the fuels coal, natural gas and petroleum
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
name the uses of the fractions as; petrol fraction as fuel in cars; paraffin
fraction for oil stoves and aircraft fuel; diesel fraction for fuel in diesel
engines, lubricating fraction for lubricants and making waxes and polishes;
bitumen for main roads
Oil and useful products
(fuel, plastics);
odd notes on "Fuels"
multiple choice tests on "Useful Products of oil"
14.3 Homologous series
describe the concept of homologous series as
a ‘family’ of similar compounds with similar properties due to the
presence of the same functional group
describe the general characteristics of an homologous series
Oil and useful products
(fuel, plastics)and Extra
Organic Chemistry
14.4 Alkanes
describe the properties of alkanes
(exemplified by methane) as being generally unreactive, except in terms of
burning
describe the bonding in alkanes
describe and identify structural isomerism
describe substitution reactions of alkanes with chlorine
Oil and useful products
(fuel, plastics)and Extra
Organic Chemistry
14.5 Alkenes
describe the manufacture of alkenes and of
hydrogen by cracking
distinguish between saturated and unsaturated hydrocarbons from molecular
structures and by simple chemical tests
describe the properties of alkenes in terms of addition reactions with
bromine, hydrogen and steam
describe the formation of poly(ethene) as an example of addition
polymerisation of monomer units
Oil and useful products
(fuel, plastics)and Extra
Organic Chemistry
multiple choice tests on "Useful Products of oil"
14.6 Alcohols
describe the formation of ethanol by
fermentation and by the catalytic addition of steam to ethene
describe the properties of ethanol in terms of burning
name the uses of ethanol; as a solvent; as a fuel; as a constituent of wine
and beer
Extra Organic
Chemistry
14.7 Acids
describe the formation of ethanoic acid by
the oxidation of ethanol with atmospheric oxygen and with acidified potassium
dichromate (VI) (see also redox)
describe ethanoic acid as a typical weak acid
describe the reaction of ethanoic acid with ethanol to give an ester (ethyl
ethanoate)
Extra Organic
Chemistry
14.8 Macromolecules
describe macromolecules in terms of large
molecules built up from small units (monomers), different macromolecules
having different units and/or different linkages
Oil and useful products
(fuel, plastics)
and Extra
Organic Chemistryand bonding
14.8(a) Synthetic
polymers
name some typical uses of plastics and of
man-made fibres
describe the pollution problems caused by non-biodegradable plastics
deduce the structure of the polymer product from a given alkene and vice
versa
describe the formation of nylon (a polyamide)
by condensation polymerisation, the structure of nylon represented as ...
(the rectangles represent the rest of the carbon chains in each unit) (3
units etc.)
describe the formation of Terylene (a polyester) by
condensation polymerisation and the structure of Terylene represented as
(3 units etc.)
(Details of manufacture and mechanisms of these polymerisations are not
required).
Oil and useful products
(fuel, plastics)
and Extra
Organic Chemistryand bonding
14.8(b) Natural
macromolecules
name proteins, fats and carbohydrates as
the main constituents of food
describe proteins as possessing the same (amide) linkages as nylon but with
different units
describe the hydrolysis of proteins to amino acids (structures and names
not required)
describe fats as having the same ester linkages as Terylene but with different units
describe soap a product of hydrolysis of fats
describe complex carbohydrates in terms of a large number of sugar
units joined together by condensation polymerisation eg the diagram shows 4
units of a natural carbohydrate polymer ... ... (the rectangles represent
the rest of the carbon chains in each unit) .....
etc.
describe the acid hydrolysis of complex carbohydrates (eg. starch) to give
simple sugars
describe the fermentation of simple sugars to produce ethanol (and carbon
dioxide) and its importance to brewing and wine making (Candidates will not be expected to give the molecular formulae of sugars).
describe, in outline, the usefulness of chromatography in separating and
identifying the products of hydrolysis of carbohydrates and proteins
Extra
Organic Chemistry
Qualitative
Analysis Tests to know
Tests for anions:
carbonate, chloride, iodide, nitrate, sulphate
Tests for aqueous cations:
aluminium, ammonium, calcium, copper(II), iron (II), iron(III), zinc
Tests for gases:
ammonia, carbon dioxide, chlorine, hydrogen, oxygen
Chemical
tests: methods, observations, equations
and notes on
the preparation and collection of gases
This page is designed
to help with the learning-revision for OCR
IGCSE CHEMISTRY (CIE) International GCSE
Level chemistry OCR code 0620 Cambridge Extended syllabus for
grades A* to C
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