12 Group 17
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Candidates should be able to:
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12.1 Physical properties of selected Group 17 elements
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(a) state that the colour intensity of Group 17
elements: Cl2, Br2, I2, increase down the group;
(b) explain how the volatility of Group 17
elements decreases down the group
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12.2 Reactions of selected Group 17 elements
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(a) deduce and explain the relative reactivities of
Group 17 elements as oxidising agents from
Eº values;
(b) explain the order of reactivity of F2, Cl2, Br2, I2
with hydrogen, and compare the relative
thermal stabilities of the hydrides;
(c) explain the reactions of chlorine with cold and
hot aqueous sodium hydroxide.
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12.3 Reactions of selected halide ions
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(a) explain and write equations for reactions of
Group 17 ions with aqueous silver ions
followed by aqueous ammonia;
(b) explain and write equations for reactions of
Group 17 ions with concentrated sulphuric
acid.
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12.4 Industrial applications of halogens and their compounds
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(a) describe the industrial uses of the halogens and
their compounds as antiseptic, bleaching agent
and in black-and-white photography;
(b) explain the use of chlorine in water treatment.
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10 Group 2
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Candidates should be able to:
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10.1 Selected Group 2 elements and their compounds
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(a) describe the trends in physical properties of
Group 2 elements: Mg, Ca, Sr, Ba;
(b) describe the reactions of Group 2 elements
with oxygen and water;
(c) describe the behaviour of the oxides of Group
2 elements with water;
(d) explain qualitatively the thermal
decomposition of the nitrates, carbonates and
hydroxides of Group 2 elements in terms of
the charge density and polarisability of large
anions;
(e) explain qualitatively the variation in solubility
of sulphate of Group 2 elements in terms of the
relative magnitudes of the enthalpy change of
hydration for the relevant ions and the
corresponding lattice energy.
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10.2 Anomalous behaviour of beryllium
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(a) explain the anomalous behaviour of beryllium
as exemplified by the formation of covalent
compounds;
(b) describe the diagonal relationships between
beryllium and aluminium;
(c) explain the similarity of aqueous beryllium
salts to aqueous aluminium salts in terms of
their acidic property.
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10.3 Uses of Group 2 compounds
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(a) state the uses of Group 2 compounds in agriculture, industry and medicine.
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11 Group 14
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Candidates should be able to:
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11.1 Physical properties of Group 14 elements
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(a) explain the trends in physical properties (melting points and electrical conductivity) of Group 14 elements: C, Si, Ge, Sn, Pb.
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11.2 Tetrachlorides and oxides of Group 14 elements
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(a) explain the bonding and molecular shapes of the tetrachlorides of group 14 elements; (b) explain the volatility, thermal stability and hydrolysis of tetrachlorides in terms of structure and bonding; (c) explain the bonding, acid-base nature and the thermal stability of the oxides of oxidation states +2 and +4.
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11.3 Relative stability of +2 and +4 oxidation states of Group 14 elements
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(a) explain the relative stability of +2 and +4 oxidation states of the elements in their oxides, chlorides and aqueous cations.
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11.4 Silicon, silicone and silicates
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(a) describe the structures of silicone and silicates (pyroxenes and amphiboles), sheets (mica) and framework structure (quartz) (general formulae are not required);
(b) explain the uses of silicon as a semiconductor
and silicone as a fluid, elastomer and resin;
(c) describe the uses of silicates as basic materials
for cement, glass, ceramics and zeolites.
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11.5 Tin alloys
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(a) describe the uses of tin in solder and pewter.
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8 Electrochemistry
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Candidates should be able to:
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8.1 Half-cell and redox equations
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(a) explain the redox processes and cell diagram
(cell notation) of the Daniell cell;
(b) construct redox equations.
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8.2 Standard electrode potential
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(a) describe the standard hydrogen electrode;
(b) use the standard hydrogen electrode to
determine standard electrode potential
(standard reduction potential), E0;
(c) calculate the standard cell potential using the
Eo values, and write the redox equations;
(d) predict the stability of aqueous ions from Eº
values;
(e) predict the power of oxidising and reducing
agents from Eº values;
(f) predict the feasibility of a reaction from
value and from the combination of various
electrode potentials: spontaneous
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8.3 Non-standard cell potentials
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(a) calculate the non-standard cell potential, Ecell,
of a cell using the Nernst equation.
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8.4 Fuel cells
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(a) describe the importance of the development of more efficient batteries for electric cars in terms of smaller size, lower mass and higher voltage, as exemplified by hydrogen-oxygen fuel cell.
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8.5 Electrolysis
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(a) compare the principles of electrolytic cell to
electrochemical cell;
(b) predict the products formed during
electrolysis;
(c) state the Faraday’s first and second laws of
electrolysis;
(d) state the relationship between the Faraday
constant, the Avogadro constant and the
electronic charge;
(e) calculate the quantity of electricity used, the
mass of material and/o
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8.6 Applications of electrochemistry
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(a) explain the principles of electrochemistry in
the process and prevention of corrosion
(rusting of iron);
(b) describe the extraction of aluminium by
electrolysis, and state the advantages of
recycling aluminium;
(c) describe the process of anodisation of
aluminium to resist corrosion;
(d) describe the diaphragm cell in the manufacture
of chlorine from brine;
(e) describe the treatment of industrial effluent by
electrolysis to remove Ni2+, Cr3+ and Cd2+;
(f) describe the electroplating of coated plastics.
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7 Chemical Energetics
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Candidates should be able to:
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7.1 Enthalpy changes of reaction, ΔH
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(a) Explain that most chemical reactions are accompanied by enthalpy changes (exothermic or endothermic);
(b) Define enthalpy change of reaction, ΔH, and state the standard conditions;
(c) Define enthalpy change of formation, combustion, hydration, solution, neutralisation, atomisation, bond energy, ionisation energy and electron affinity;
(d) Calculate the heat energy change from experimental measurements using the relationship: heat change, q mc T or q = mc ;
(e) Calculate enthalpy changes from experimental results.
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7.2 Hess’ law
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(a) State Hess’ law, and its use to find enthalpy changes that cannot be determined directly, e.g. an enthalpy change of formation from enthalpy changes of combustion;
(b) Construct energy level diagrams relating the enthalpy to reaction path and activation energy;
(c) Calculate enthalpy changes from energy cycles.
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7.3 Born-Haber cycle
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(a) Define lattice energy for simple ionic crystals in terms of the change from gaseous ions to solid lattice;
(b) Explain qualitatively the effects of ionic charge and ionic radius on the numerical magnitude of lattice energy values;
(c) Construct Born-Haber cycle for the formation of simple ionic crystals.
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7.4 The solubility of solids in liquids
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(a) Construct energy cycles for the formation of aqueous solutions of ionic compounds;
(b) Explain qualitatively the influence on solubility of the relationship between enthalpy change of solution, lattice energy of solid and enthalpy change of hydration or other solvent-solute interaction.
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9 Periodic Table: Periodicity
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Candidates should be able to:
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9.1 Physical properties of elements of Period 2 and Period 3
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(a) Interpret and explain the trend and gradation
of atomic radius, melting point, boiling point,
enthalpy change of vaporisation and electrical
conductivity in terms of structure and bonding;
(b) Explain the factors influencing ionisation
energies;
(c) Explain the trend in ionisation energies across
Period 2 and Period 3 and down a group;
(d) Predict the electronic configuration and position of unknown elements in the Periodic Table from successive values of ionisation energies.
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9.2 Reactions of Period 3 elements with oxygen and water
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(a) Describe the reactions of Period 3 elements
with oxygen and water;
(b) Interpret the ability of elements to act as
oxidising and reducing agents.
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9.3 Acidic and basic properties of oxides and hydrolysis of oxides
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(a) Explain the acidic and basic properties of the
oxides of Period 3 elements;
(b) Describe the reactions of the oxides of Period
3 elements with water;
(c) Describe the classification of the oxides of
Period 3 elements as basic, amphoteric or
acidic based on their reactions with water, acid
and alkali;
(d) Describe the use
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