Course Content
1 Solids, liquids and gases
1 State the distinguishing properties of solids, liquids and gases
2 Describe the structures of solids, liquids and gases in terms of particle separation, arrangement and motion
3 Describe and explain changes of state (melting, boiling, evaporating, freezing and condensing) in terms of
kinetic particle theory
4 Interpret and explain heating and cooling curves in terms of kinetic particle theory
5 Describe and explain, in terms of kinetic particle theory, the effects of temperature and pressure on the
volume of a gas
2 Diffusion
1 Describe and explain diffusion in terms of kinetic particle theory
2 Describe and explain the effect of relative molecular mass on the rate of diffusion of gases
3 Elements, compounds and mixtures
1 Describe the differences between elements, compounds and mixtures
4 Atomic structure and the Periodic Table
1 Describe the structure of the atom as a central nucleus containing neutrons and protons surrounded by
electrons in shells
2 State the relative charges and relative masses of a proton, a neutron and an electron
3 Define proton number / atomic number as the number of protons in the nucleus of an atom
4 Define mass number / nucleon number as the total number of protons and neutrons in the nucleus of an atom
5 Determine the electronic configuration of elements and their ions with proton number 1 to 20, e.g. 2,8,3
6 State that:
(a) Group VIII noble gases have a full outer shell
(b) the number of outer shell electrons is equal to the group number in Groups I to VII
(c) the number of occupied electron shells is equal to the period number
5 Isotopes
1 Define isotopes as different atoms of the same element that have the same number of protons but
different numbers of neutrons
2 State that isotopes of the same element have the same chemical properties because they have the same
number of electrons and therefore the same electronic configuration
3 Interpret and use symbols for atoms, e.g. 12/6 C and ions, e.g. 35/17 Cl
4 Calculate the relative atomic mass of an element from the relative masses and abundances of its isotopes
6 Ion and ionic bonds
1 Describe the formation of positive ions, known as cations, and negative ions, known as anions
2 Describe the giant lattice structure of ionic compounds as a regular arrangement of alternating positive and
negative ions
3 State that an ionic bond is a strong electrostatic attraction between oppositely charged ions
4 Describe the formation of ionic bonds between ions of metallic and non-metallic elements, including the
use of dot-and-cross diagrams
5 Describe and explain in terms of structure and bonding the properties of ionic compounds:
(a) high melting points and boiling points
(b) good electrical conductivity when aqueous or molten and poor when solid
7 Simple molecules and covalent bonds
1 State that a covalent bond is formed when a pair of electrons is shared between two atoms leading to
noble gas electronic configurations
2 Describe the formation of covalent bonds in simple molecules, including H2, Cl2, H2O, CH4, NH3, HCl, CH3OH,
C2H4, O2, CO2 and N2. Use dot-and-cross diagrams to show the electronic configurations in these
and similar molecules
3 Describe and explain in terms of structure and bonding the properties of simple molecular compounds:
(a) low melting points and boiling points in terms of weak intermolecular forces (specific types of
intermolecular forces are not required)
(b) poor electrical conductivity
8 Giant covalent structures
1 Describe the giant covalent structures of graphite, diamond and silicon(IV) oxide, SiO2
2 Relate the structures and bonding of graphite and diamond to their uses, limited to:
(a) graphite as a lubricant and as an electrode
(b) diamond in cutting tools
3 Describe the similarity in properties between diamond and silicon(IV) oxide, related to their structures
9 Metallic bonding
1 Describe metallic bonding as the electrostatic attraction between the positive ions in a giant metallic
lattice and a ‘sea’ of delocalised electrons
2 Explain in terms of structure and bonding the properties of metals:
(a) good electrical conductivity
(b) malleability and ductility
10 Formulae
1 State the formulae of the elements and compounds named in the subject content
2 Define the molecular formula of a compound as the number and type of different atoms in one molecule
3 Define the empirical formula of a compound as the simplest whole number ratio of the different atoms or
ions in a compound
4 Deduce the formula of a simple compound from the relative numbers of atoms or ions present in a model
or a diagrammatic representation
5 Deduce the formula of an ionic compound from the charges on the ions
6 Construct word equations, symbol equations and ionic equations to show how reactants form products,
including state symbols
7 Deduce the symbol equation with state symbols for a chemical reaction, given relevant information
11 Relative masses of atoms and molecules
1 Describe relative atomic mass, Ar , as the average mass of the isotopes of an element compared to 1/12th of
the mass of an atom of 12C
2 Define relative molecular mass, Mr, as the sum of the relative atomic masses. Relative formula mass, Mr,
will be used for ionic compounds
12 The mole and the Avogadro constant
1 State that the mole, mol, is the unit of amount of substance and that one mole contains 6.02 × 1023
particles, e.g. atoms, ions, molecules; this number is the Avogadro constant
2 Use the relationship
amount of substance (mol) = mass (g)
molar mass (g / mol)
to calculate:
(a) amount of substance
(b) mass
(c) molar mass
(d) relative atomic mass or relative molecular / formula mass
(e) number of particles, using the value of the Avogadro constant
3 Use the molar gas volume, taken as 24 dm3 at room temperature and pressure, r.t.p., in calculations
involving gases
4 State that concentration can be measured in g / dm3 or mol / dm3
5 Calculate stoichiometric reacting masses, limiting reactants, volumes of gases at r.t.p., volumes of solutions
and concentrations of solutions expressed in g / dm3 and mol / dm3, including conversion between cm3 and dm3
6 Use experimental data to calculate the concentration of a solution in a titration
7 Calculate empirical formulae and molecular formulae, given appropriate data
8 Calculate percentage yield, percentage composition by mass and percentage purity, given appropriate data
13 Electrolysis
1 Define electrolysis as the decomposition of an ionic compound, when molten or in aqueous solution, by the
passage of an electric current
2 Identify in simple electrolytic cells:
(a) the anode as the positive electrode
(b) the cathode as the negative electrode
(c) the electrolyte as the molten or aqueous substance that undergoes electrolysis
3 Describe the transfer of charge during electrolysis to include:
(a) the movement of electrons in the external circuit
(b) the loss or gain of electrons at the electrodes
(c) the movement of ions in the electrolyte
4 Identify the products formed at the electrodes and describe the observations made during the electrolysis of:
(a) molten lead(II) bromide
(b) concentrated aqueous sodium chloride
(c) dilute sulfuric acid
using inert electrodes made of platinum or carbon / graphite
5 Identify the products formed at the electrodes and describe the observations made during the electrolysis
of aqueous copper(II) sulfate using inert carbon / graphite electrodes and when using copper electrodes
6 State that metals or hydrogen are formed at the cathode and that non-metals (other than hydrogen) are
formed at the anode
7 Predict the identity of the products at each electrode for the electrolysis of a binary compound in the
molten state
8 Predict the identity of the products at each electrode for the electrolysis of a halide compound in dilute or
concentrated aqueous solution
9 Construct ionic half-equations for reactions at the anode (to show oxidation) and at the cathode (to show reduction)
10 State that metal objects are electroplated to improve their appearance and resistance to corrosion
11 Describe how metals are electroplated
14 Hydrogen–oxygen fuel cells
1 State that a hydrogen–oxygen fuel cell uses hydrogen and oxygen to produce electricity with water as the
only chemical product
2 Describe the advantages and disadvantages of using hydrogen–oxygen fuel cells in comparison with
gasoline / petrol engines in vehicles
15 Exothermic and endothermic reactions
1 State that an exothermic reaction transfers thermal energy to the surroundings leading to an increase in
the temperature of the surroundings
2 State that an endothermic reaction takes in thermal energy from the surroundings leading to a decrease in
the temperature of the surroundings
3 State that the transfer of thermal energy during a reaction is called the enthalpy change, ΔH, of the
reaction. ΔH is negative for exothermic reactions and positive for endothermic reactions
4 Define activation energy, Ea, as the minimum energy that colliding particles must have to react
5 Draw, label and interpret reaction pathway diagrams for exothermic and endothermic reactions using
information provided, to include:
(a) reactants
(b) products
(c) enthalpy change of the reaction, ΔH
(d) activation energy, Ea
6 State that bond breaking is an endothermic process and bond making is an exothermic process and explain
the enthalpy change of a reaction in terms of bond breaking and bond making
7 Calculate the enthalpy change of a reaction using bond energies
16 Physical and chemical changes
1 Identify physical and chemical changes, and describe the differences between them
17 Rate of reaction
1 Describe collision theory in terms of:
(a) number of particles per unit volume
(b) frequency of collisions between particles
(c) kinetic energy of particles
(d) activation energy, Ea
2 State that a catalyst increases the rate of a reaction, decreases the activation energy, Ea, of a reaction and
is unchanged at the end of a reaction
3 Describe and explain the effect on the rate of reactions of:
(a) changing the concentration of solutions
(b) changing the pressure of gases
(c) changing the surface area of solids
(d) changing the temperature
(e) adding or removing a catalyst, including enzymes using collision theory
4 Describe and evaluate practical methods for investigating the rate of a reaction, including change in mass
of a reactant or a product and the formation of a gas
5 Interpret data, including graphs, from rate of reaction experiments
18 Reversible reactions and equilibrium
1 State that some chemical reactions are reversible as shown by the symbol ⇌
2 Describe how changing the conditions can change the direction of a reversible reaction for:
(a) the effect of heat on hydrated compounds
(b) the addition of water to anhydrous compounds including copper(II) sulfate and cobalt(II) chloride
3 State that a reversible reaction in a closed system is at equilibrium when:
(a) the rate of the forward reaction is equal to the rate of the reverse reaction
(b) the concentrations of reactants and products are no longer changing
4 Predict and explain, for a reversible reaction, how the position of equilibrium is affected by:
(a) changing temperature
(b) changing pressure
(c) changing concentration
(d) using a catalyst
using information provided
5 State the symbol equation for the production of ammonia in the Haber process, N2 (g) + 3H2(g) ⇌ 2NH3(g)
6 State the sources of the hydrogen (methane) and nitrogen (air) in the Haber process
7 State the typical conditions in the Haber process as 450 °C, 20 000 kPa / 200 atm and an iron catalyst
8 State the symbol equation for the conversion of sulfur dioxide to sulfur trioxide in the Contact process,
2SO2(g) + O2(g) ⇌ 2SO3(g)
9 State the sources of the sulfur dioxide (burning sulfur or roasting sulfide ores) and oxygen (air) in the
Contact process
10 State the typical conditions for the conversion of sulfur dioxide to sulfur trioxide in the Contact process as
450 °C, 200 kPa / 2 atm and a vanadium(V) oxide catalyst
11 Explain, in terms of rate of reaction and position of equilibrium, why the typical conditions stated are used
in the Haber process and in the Contact process, including safety considerations and economics
19 Redox
1 Use a Roman numeral to indicate the oxidation number of an element in a compound
2 Define redox reactions as involving simultaneous reduction and oxidation
3 Define oxidation in terms of:
(a) gain of oxygen
(b) loss of electrons
(c) an increase in oxidation number
4 Define reduction in terms of:
(a) loss of oxygen
(b) gain of electrons
(c) a decrease in oxidation number
5 Identify redox reactions as reactions involving gain and loss of oxygen, or gain and loss of electrons
6 Identify redox reactions by changes in oxidation number using:
(a) the oxidation number of elements in their uncombined state is zero
(b) the oxidation number of a monatomic ion is the same as the charge on the ion
(c) the sum of the oxidation numbers in a compound is zero
(d) the sum of the oxidation numbers in an ion is equal to the charge on the ion
7 Identify redox reactions by the colour changes involved when using acidified aqueous potassium
manganate(VII) or aqueous potassium iodide
8 Define an oxidising agent as a substance that oxidises another substance and is itself reduced
9 Define a reducing agent as a substance that reduces another substance and is itself oxidised
10 Identify oxidation, oxidising agents, reduction and reducing agents in redox reactions
20 The characteristic properties of acids and bases
1 State that aqueous solutions of acids contain H+ ions and aqueous solutions of alkalis contain OH– ions
2 Define acids as proton donors and bases as proton acceptors
3 State that bases are oxides or hydroxides of metals and that alkalis are soluble bases
4 Describe the characteristic properties of acids in terms of their reactions with:
(a) metals
(b) bases
(c) carbonates
5 Describe the characteristic properties of bases in terms of their reactions with:
(a) acids
(b) ammonium salts
6 State that a neutralisation reaction occurs between an acid and a base
7 Describe the neutralisation reaction between an acid and an alkali to produce water,
H+(aq) + OH−(aq) → H2O(l )
8 Describe acids and alkalis in terms of their effects on:
(a) litmus
(b) thymolphthalein
(c) methyl orange
9 Define a strong acid as an acid that is completely dissociated in aqueous solution and a weak acid as an acid
that is partially dissociated in aqueous solution
10 State examples of strong acids, including hydrochloric acid, nitric acid and sulfuric acid and construct the
symbol equations to show their complete dissociation, e.g. HCl(aq) → H+(aq) + Cl –(aq)
11 State examples of weak acids, including carboxylic acids and construct the symbol equations to show their
partial dissociation, e.g. for ethanoic acid, CH3COOH(aq) ⇌ H+(aq) + CH3COO–(aq)
12 Describe how to compare hydrogen ion concentration, neutrality, relative acidity and relative alkalinity in
terms of colour and pH using universal indicator paper
21 Oxides
1 Describe amphoteric oxides as oxides that react with acids and bases to produce a salt and water
2 Classify oxides as acidic, including SO2 and CO2, basic, including CuO and CaO, or amphoteric,
limited to Al2O3 and ZnO, related to metallic and non-metallic character
22 Preparation of salts
1 Describe the preparation, separation and purification of soluble salts by reaction of an acid with:
(a) an alkali by titration
(b) excess metal
(c) excess insoluble base
(d) excess insoluble carbonate
2 Describe the preparation of insoluble salts by precipitation
3 Describe the general solubility rule for salts:
(a) sodium, potassium and ammonium salts are soluble
(b) nitrates are soluble
(c) chlorides are soluble, except lead and silver
(d) sulfates are soluble, except barium, calcium and lead
(e) carbonates are insoluble, except sodium, potassium and ammonium
(f) hydroxides are insoluble, except sodium, potassium, ammonium and calcium (partially)
4 Define a hydrated substance as a substance that is chemically combined with water and an anhydrous
substance as a substance containing no water
5 Define the term water of crystallisation as the water molecules present in hydrated crystals, including
CuSO4•5H2O and CoCl 2•6H2O
23 Arrangement of elements
1 Describe the Periodic Table as an arrangement of elements in periods and groups and in order of increasing
proton number / atomic number
2 Describe the change from metallic to non-metallic character across a period
3 Describe the relationship between group number and the charge of the ions formed from elements in that
group
4 Explain similarities in the chemical properties of elements in the same group of the Periodic Table in terms
of their electronic configuration
5 Explain how the position of an element in the Periodic Table can be used to predict its properties
6 Identify trends in groups, given information about the elements
24 Group I properties
1 Describe the Group I alkali metals, lithium, sodium and potassium, as relatively soft metals with general
trends down the group, limited to:
(a) decreasing melting point
(b) increasing density
(c) increasing reactivity
2 Predict the properties of other elements in Group I, given information about the elements
25 Group VII properties
1 Describe the Group VII halogens, chlorine, bromine and iodine, as diatomic non-metals with general trends
down the group, limited to:
(a) increasing density
(b) decreasing reactivity
2 State the appearance of the halogens at r.t.p. as:
(a) chlorine, a pale yellow-green gas
(b) bromine, a red-brown liquid
(c) iodine, a grey-black solid
3 Describe and explain the displacement reactions of halogens with other halide ions
4 Predict the properties of other elements in Group VII, given information about the elements
26 Transition elements
1 Describe the transition elements as metals that:
(a) have high densities
(b) have high melting points
(c) have variable oxidation numbers
(d) form coloured compounds
(e) often act as catalysts as elements and in compounds
27 Noble gases
1 Describe the Group VIII noble gases as unreactive, monatomic gases and explain this in terms of electronic
configuration
28 Properties of metals
1 Compare the general physical properties of metals and non-metals, including:
(a) thermal conductivity
(b) electrical conductivity
(c) malleability and ductility
(d) melting points and boiling points
2 Describe the general chemical properties of metals, limited to their reactions with:
(a) dilute acids
(b) cold water and steam
(c) oxygen
29 Uses of metals
1 Describe the uses of metals in terms of their physical properties, including:
(a) aluminium in the manufacture of aircraft because of its low density
(b) aluminium in the manufacture of overhead electrical cables because of its low density and good
electrical conductivity
(c) aluminium in food containers because of its resistance to corrosion
(d) copper in electrical wiring because of its good electrical conductivity and ductility
30 Alloys and their properties
1 Describe an alloy as a mixture of a metal with other elements, including:
(a) brass as a mixture of copper and zinc
(b) stainless steel as a mixture of iron and other elements such as chromium, nickel and carbon
2 Explain in terms of structure how alloys can be harder and stronger than the pure metals because the
different sized atoms or ions in alloys mean the layers can no longer slide over each other
3 Describe the uses of alloys in terms of their physical properties, including stainless steel in cutlery because
of its hardness and resistance to rusting
4 Identify representations of alloys from diagrams of structure
31 Reactivity series
1 State the order of the reactivity series as: potassium, sodium, calcium, magnesium, aluminium, carbon,
zinc, iron, hydrogen, copper, silver, gold
2 Describe the relative reactivities of metals in terms of their tendency to form positive ions, by displacement
reactions, if any, with the aqueous ions of magnesium, zinc, iron, copper and silver
3 Describe the reactions, if any, of:
(a) potassium, sodium and calcium with cold water
(b) magnesium with steam
(c) magnesium, zinc, iron, copper, silver and gold with dilute hydrochloric acid
and explain these reactions in terms of the position of the metals in the reactivity series
4 Explain the apparent unreactivity of aluminium in terms of its oxide layer
5 Deduce an order of reactivity from a given set of experimental results
32 Corrosion of metals
1 State the conditions required for the rusting of iron and steel to form hydrated iron(III) oxide
2 Describe how barrier methods prevent rusting by excluding oxygen or water
3 State some common barrier methods, including painting, greasing and coating with plastic
4 Explain sacrificial protection in terms of the reactivity series and in terms of electron loss
5 Describe the use of zinc in galvanising as an example of a barrier method and sacrificial protection
33 Extraction of metals
1 Describe the ease of obtaining metals from their ores, related to the position of the metal in the reactivity
series
2 Describe the extraction of iron from hematite in the blast furnace, including symbol equations for each
step, limited to:
(a) the burning of carbon (coke) to provide heat and produce carbon dioxide
(b) the reduction of carbon dioxide to carbon monoxide
(c) the reduction of iron(III) oxide by carbon monoxide
(d) the thermal decomposition of calcium carbonate / limestone to produce calcium oxide
(e) the formation of slag
3 Describe the extraction of aluminium from purified bauxite / aluminium oxide, including:
(a) the role of cryolite
(b) why the carbon anodes need to be regularly replaced
(c) the reactions at the electrodes, including ionic half-equations
Details of the purification of bauxite are not required
34 Water
1 Describe chemical tests for the presence of water using anhydrous cobalt(II) chloride and anhydrous
copper(II) sulfate
2 Describe how to test for the purity of water using melting point and boiling point
3 Explain that distilled water is used in practical chemistry rather than tap water because it contains fewer
chemical impurities
4 State that water from natural sources may contain substances, including:
(a) dissolved oxygen
(b) metal compounds
(c) plastics
(d) sewage
(e) harmful microbes
(f) itrates from fertilisers
(g) phosphates from fertilisers and detergents
5 State that some of these substances are beneficial, including:
(a) dissolved oxygen for aquatic life
(b) some metal compounds provide essential minerals for life
6 State that some of these substances are potentially harmful, including:
(a) some metal compounds are toxic
(b) some plastics harm aquatic life
(c) sewage contains harmful microbes which cause disease
(d) nitrates and phosphates lead to deoxygenation of water and damage to aquatic life
Details of the eutrophication process are not required
7 Describe the treatment of the domestic water supply in terms of:
(a) sedimentation and filtration to remove solids
(b) use of carbon to remove tastes and odours
(c) chlorination to kill microbes
35 Fertilisers
1 State that ammonium salts and nitrates are used as fertilisers
2 Describe the use of NPK fertilisers to provide the elements nitrogen, phosphorus and potassium for
improved plant growth
36 Air quality and climate
1 State the composition of clean, dry air as approximately 78% nitrogen, N2, 21% oxygen, O2
, and the remainder as a mixture of noble gases and carbon dioxide, CO2
2 State the source of each of these air pollutants:
(a) carbon dioxide from the complete combustion of carbon-containing fuels
(b) carbon monoxide and particulates from the incomplete combustion of carbon-containing fuels
(c) methane from the decomposition of vegetation and waste gases from digestion in animals
(d) oxides of nitrogen from car engines
(e) sulfur dioxide from the combustion of fossil fuels which contain sulfur compounds
3 State the adverse effects of these air pollutants:
(a) carbon dioxide: higher levels of carbon dioxide leading to increased global warming, which leads to
climate change
(b) carbon monoxide: toxic gas
(c) particulates: increased risk of respiratory problems and cancer
(d) methane: higher levels of methane leading to increased global warming, which leads to climate change
(e) oxides of nitrogen: acid rain, photochemical smog and respiratory problems
(f) sulfur dioxide: acid rain
4 Describe how the greenhouse gases carbon dioxide and methane cause global warming, limited to:
(a) the absorption, reflection and emission of thermal energy
(b) reducing thermal energy loss to space
5 State and explain strategies to reduce the effects of these environmental issues, limited to:
(a) climate change: planting trees, reduction in livestock farming, decreasing use of fossil fuels, increasing
use of hydrogen and renewable energy, e.g. wind, solar
(b) acid rain: use of catalytic converters in vehicles, reducing emissions of sulfur dioxide by using low
sulfur fuels and flue gas desulfurisation with calcium oxide
6 Explain how oxides of nitrogen form in car engines and describe their removal by catalytic converters, e.g.
2CO + 2NO → 2CO2 + N2
7 Describe photosynthesis as the reaction between carbon dioxide and water to produce glucose and oxygen
in the presence of chlorophyll and using energy from light
8 State the word equation and symbol equation for photosynthesis
37 Formulae, functional groups and terminology
1 State that a structural formula is an unambiguous description of the way the atoms in a molecule are
arranged, including CH2=CH2, CH3CH2OH, CH3COOCH3
2 Draw and interpret the displayed formula of a molecule to show all the atoms and all the bonds
3 Write and interpret general formulae of compounds in the same homologous series, limited to:
(a) alkanes, CnH2n+2
(b) alkenes, CnH2n
(c) alcohols, CnH2n+1OH
(d) carboxylic acids, CnH2n+1COOH
4 Define structural isomers as compounds with the same molecular formula, but different structural
formulae, including C4H10 as CH3CH2CH2CH3 and CH3CH(CH3)CH3 and C4H8 as CH3
CH2CH=CH2 and CH3CH=CHCH3
5 Identify a functional group as an atom or group of atoms that determine the chemical properties of a
homologous series
6 Describe the general characteristics of a homologous series as:
(a) having the same functional group
(b) having the same general formula
(c) differing from one member to the next by a –CH2– unit
(d) displaying a trend in physical properties
(e) sharing similar chemical properties
7 State that a saturated compound has molecules in which all carbon–carbon bonds are single bonds
8 State that an unsaturated compound has molecules in which one or more carbon–carbon bonds are not
single bonds
38 Naming organic compounds
1 Name and draw the structural and displayed formulae of unbranched:
(a) alkanes
(b) alkenes, including but-1-ene and but-2-ene
(c) alcohols, including propan-1-ol, propan-2-ol, butan-1-ol and butan-2-ol
(d) carboxylic acids
(e) the products of the reactions stated in sections 11.4–11.7
containing up to four carbon atoms per molecule
2 State the type of compound present given the chemical name ending in -ane, -ene, -ol, or -oic acid or from
a molecular, structural or displayed formula
3 Name and draw the displayed formulae of the unbranched esters which can be made from unbranched
alcohols and carboxylic acids, each containing up to four carbon atoms
39 Fuels
1 Name the fossil fuels: coal, natural gas and petroleum
2 Name methane as the main constituent of natural gas
3 State that hydrocarbons are compounds that contain hydrogen and carbon only
4 State that petroleum is a mixture of hydrocarbons
5 Describe the separation of petroleum into useful fractions by fractional distillation
6 Describe how the properties of fractions obtained from petroleum change from the bottom to the top of
the fractionating column, limited to:
(a) decreasing chain length
(b) higher volatility
(c) lower boiling points
(d) lower viscosity
7 Name the uses of the fractions as:
(a) refinery gas fraction for gas used in heating and cooking
(b) gasoline / petrol fraction for fuel used in cars
(c) naphtha fraction as a chemical feedstock
(d) kerosene / paraffin fraction for jet fuel
(e) diesel oil / gas oil fraction for fuel used in diesel engines
(f) fuel oil fraction for fuel used in ships and home heating systems
(g) lubricating oil fraction for lubricants, waxes and polishes
(h) bitumen fraction for making roads
40 Alkanes
1 State that the bonding in alkanes is single covalent and that alkanes are saturated hydrocarbons
2 Describe the properties of alkanes as being generally unreactive, except in terms of combustion and
substitution by chlorine
3 State that in a substitution reaction one atom or group of atoms is replaced by another atom or group
of atoms
4 Describe the substitution reaction of alkanes with chlorine as a photochemical reaction, with ultraviolet
light providing the activation energy, Ea, and draw the structural or displayed formulae of the products,
limited to monosubstitution
41 Alkenes
1 State that the bonding in alkenes includes a double carbon–carbon covalent bond and that alkenes are
unsaturated hydrocarbons
2 Describe the manufacture of alkenes and hydrogen by the cracking of larger alkane molecules using a high
temperature and a catalyst
3 Describe the reasons for the cracking of larger alkane molecules
4 Describe the test to distinguish between saturated and unsaturated hydrocarbons by their reaction with
aqueous bromine
5 State that in an addition reaction only one product is formed
6 Describe the properties of alkenes in terms of addition reactions with:
(a) bromine or aqueous bromine
(b) hydrogen in the presence of a nickel catalyst
(c) steam in the presence of an acid catalyst
and draw the structural or displayed formulae of the products
42 Alcohols
1 Describe the manufacture of ethanol by:
(a) fermentation of aqueous glucose at 25–35 °C in the presence of yeast and in the absence of oxygen
(b) catalytic addition of steam to ethene at 300 °C and 6000 kPa / 60 atm in the presence of an
acid catalyst
including a comparison of the advantages and disadvantages of the two methods
2 Describe the combustion of alcohols
3 State the uses of ethanol as:
(a) a solvent
(b) a fuel
43 Carboxylic acids
1 Describe the reactions of carboxylic acids with:
(a) metals
(b) bases
(c) carbonates
including names and formulae of the salts produced
2 Describe the formation of ethanoic acid by the oxidation of ethanol:
(a) with acidified aqueous potassium manganate(VII)
(b) by bacterial oxidation during vinegar production
3 Describe the reaction of a carboxylic acid with an alcohol using an acid catalyst to form an ester
44 Polymers
1 Define polymers as large molecules built up from many smaller molecules called monomers
2 Identify the repeat units and / or linkages in addition polymers and in condensation polymers
3 Deduce the structure or repeat unit of an addition polymer from a given alkene and vice versa
4 Deduce the structure or repeat unit of a condensation polymer from given monomers and vice versa,
limited to:
(a) polyamides from a dicarboxylic acid and a diamine
(b) polyesters from a dicarboxylic acid and a diol
5 Describe the differences between addition and condensation polymerisation
6 State that plastics are made from polymers
7 Describe how the properties of plastics have implications for their disposal
8 Describe the environmental challenges caused by plastics, limited to:
(a) disposal in land fill sites
(b) accumulation in oceans
(c) formation of toxic gases from burning
9 Describe and draw the structure of:
(a) nylon, a polyamide
(b) PET, a polyester
O O O O
|| || || ||
----C----C---O------C---C----O----O
The full name for PET, polyethylene terephthalate, is not required
10 State that PET can be converted back into monomers and re-polymerised
11 Describe proteins as natural polyamides and that they are formed from amino acid monomers with the
general structure:
R
H | O
N---- C----C
H O----H
where R represents different types of side chain
12 Describe and draw the structure of proteins as:
H O
| ||
----N----C----N----C----N----C
| ||
H O
45 Experimental design
1 Name appropriate apparatus for the measurement of time, temperature, mass and volume, including:
(a) stopwatches
(b) thermometers
(c) balances
(d) burettes
(e) volumetric pipettes
(f) measuring cylinders
(g) gas syringes
2 Suggest advantages and disadvantages of experimental methods and apparatus
3 Describe a:
(a) solvent as a substance that dissolves a solute
(b) solute as a substance that is dissolved in a solvent
(c) solution as a mixture of one or more solutes dissolved in a solvent
(d) saturated solution as a solution containing the maximum concentration of a solute dissolved in the
solvent at a specified temperature
(e) residue as a substance that remains after evaporation, distillation, filtration or any similar process
(f) filtrate as a liquid or solution that has passed through a filter
46 Acid–base titrations
1 Describe an acid–base titration to include the use of a:
(a) burette
(b) volumetric pipette
(c) suitable indicator
2 Describe how to identify the end-point of a titration using an indicator
47 Chromatography
1 Describe how paper chromatography is used to separate mixtures of soluble substances, using a suitable
solvent
2 Describe the use of locating agents when separating mixtures containing colourless substances. Knowledge
of specific locating agents is not required
3 Interpret simple chromatograms to identify:
(a) unknown substances by comparison with known substances
(b) pure and impure substances
4 State and use the equation for Rf :
distance travelled by substance
Rf = -----------------------------------------
distance travelled by solvent
48 Separation and purification
1 Describe and explain methods of separation and purification using:
(a) a suitable solvent
(b) filtration
(c) crystallisation
(d) simple distillation
(e) fractional distillation
2 Suggest suitable separation and purification techniques, given information about the substances involved
3 Identify substances and assess their purity using melting point and boiling point information
49 Identification of ions and gases
1 Describe tests to identify the anions:
(a) carbonate, CO32–, by reaction with dilute acid and then testing for carbon dioxide gas
(b) chloride, Cl –, bromide, Br –, and iodide, I–, by acidifying with dilute nitric acid then adding aqueous
silver nitrate
(c) nitrate, NO3–, by reduction with aluminium foil and aqueous sodium hydroxide and then testing for
ammonia gas
(d) sulfate, SO42–, by acidifying with dilute nitric acid then adding aqueous barium nitrate
(e) sulfite, SO32–, by reaction with acidified aqueous potassium manganate(VII)
2 Describe tests using aqueous sodium hydroxide and aqueous ammonia to identify the aqueous cations:
(a) aluminium, Al 3+
(b) ammonium, NH4 +
(c) calcium, Ca2+
(d) chromium(III), Cr3+
(e) copper(II), Cu2+
(f) iron(II), Fe2+
(g) iron(III), Fe3+
(h) zinc, Zn2+
3 Describe tests to identify the gases:
(a) ammonia, NH3, using damp red litmus paper
(b) carbon dioxide, CO2, using limewater
(c) chlorine, Cl 2, using damp litmus paper
(d) hydrogen, H2, using a lighted splint
(e) oxygen, O2, using a glowing splint
(f) sulfur dioxide, SO2, using acidified aqueous potassium manganate(VII)
4 Describe the use of a flame test to identify the cations:
(a) lithium, Li+
(b) sodium, Na+
(c) potassium, K+
(d) calcium, Ca2+
(e) barium, Ba2+
(f) copper(II), Cu2+
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