| Content | Depth of Treatment | Activities | Social and Applied Aspects |
1.1 Periodic Table
(Time needed: 4 class periods) | Elements. Symbols of elements 1-36.
The periodic table as a list of elements arranged so as to demonstrate trends in their physical and chemical properties. Brief statement of the principal resemblances of elements within each main group, in particular alkali metals, alkaline earth metals, halogens and noble gases. | Arranging elements in order of relative atomic mass; note differences compared with the modern periodic table. Demonstration of the reaction with water of lithium, sodium and potassium. | History of the idea of elements,
including the contributions of the Greeks, Boyle, Davy and Moseley. History of the periodic table, including the contribution of Mendeleev. Comparison of Mendeleev's table with the modern periodic table. |
1.2 Atomic Structure
(Time needed: 5 class periods) | Matter is composed of particles, which may be atoms, molecules or ions. Atoms. Minute size of atoms. Law of conservation of mass. Properties of electrons, protons and neutrons (relative mass, relative charge, location within atom). Atomic number (Z ), mass number (A), isotopes; hydrogen and carbon as examples of isotopes. Relative atomic mass (Ar). The 12C scale for relative atomic masses. | | Very brief outline of the historical development of atomic theory (outline principles only; mathematical treatment not required): Dalton: atomic theory; Thomson: negative charge of the electron; Rutherford: discovery of the nucleus as shown by the a-particle scattering experiment; and Bohr: model of the atom. Use of the mass spectrometer in determining relative atomic mass. |
1.3 Radioactivity
(Time needed: 3 class periods) | Alpha, beta and gamma radiation (nature and penetrating ability).
One example each of: - an a-emitter, e.g. 241Am
- a ß-emitter, e.g. 14C
- a ?-emitter, e.g. 60Co.
Radioisotopes. Half-life (non- mathematical treatment). | Demonstration of properties - detection and penetrating power (this can be shown using an appropriate videotape, if desired). (Principle of Geiger-Müller tube not required.) | Historical outline of radioactivity: work of Becquerel (discovery of radiation from uranium salts); Marie and Pierre Curie (discovery of polonium and radium). Widespread occurrence of radioactivity. Uses of radioisotopes (three examples). 14C age determination (calculations not required). 60Co for cancer treatment. Food irradiation. |
1.4 Electronic Structure of Atoms
(Time needed: 7 class periods) | Energy levels in atoms. Organisation of particles in atoms of elements nos. 1-20 (numbers of electrons in each main energy level). Classification of the first twenty elements in the periodic table on the basis of the number of outer electrons. Atomic radii (covalent radii only). Explanations for general trends in values:
(i) down a group
(ii) across a period (covalent radii of main group elements only). Dependence of chemical properties of elements on their electronic structure. Explanations in terms of atomic radius, screening effect and nuclear charge for general trends in properties of elements in groups I and VII. | Mandatory experiment 1.1* See mandatory experiment 1.2 below (reactivity of halogens). | Sodium street lights, fireworks. |
1.5 Oxidation and Reduction
(Time needed: 7 class periods) | Introduction to oxidation and reduction: simple examples only, e.g. Na with Cl2, Mg with O2, Zn with Cu2+. Oxidation and reduction in terms of loss and gain of electrons. Oxidising and reducing agents. The electrochemical series as a series of metals arranged in order of their ability to be oxidised (reactions, other than displacement reactions, not required). Electrolysis of (i) copper sulfate solution with copper electrodes and (ii) acidified water with inert electrodes. | Mandatory experiment 1.2 (half equations only required, e.g. 2Br- - 2e- ? Br2). Demonstration of ionic movement. | Rusting of iron. Swimming-pool water treatment. Use of scrap iron to extract copper. Electroplating. Purification of copper. Chrome and nickel plating. Cutlery. |
2.1 Chemical Compounds
(Time needed: 6 class periods) | Compounds. Simple chemical formulas. Stability of noble gas electron configurations. Bonding and valency in terms of the attainment of a stable electronic structure. Octet rule and its limitations. | Using the octet rule to predict the formulas of simple compounds - binary compounds of the first 36 elements (excluding d-block elements) and the hydroxides and carbonates of these elements (where such exist). | Uses of helium and argon related to their chemical unreactivity. |
2.2 Ionic Bonding
(Time needed: 4 class periods) | Positive and negative ions. Minute size of ions. Ionic bonding as electron transfer. Sodium chloride crystal structure. Characteristics of ionic substances. | Representation of ionic bonds using dot and cross diagrams. Examination of a model of the NaC1 crystal. Mandatory experiment 2.1 | Ionic materials in everyday life (two uses, e.g. salt tablets to replace salt lost by sweating). |
2.3 Covalent Bonding
(Time needed: 4 class periods) | Molecules. Minute size of molecules. Covalent bonding as the sharing of pairs of electrons. Single, double and triple covalent bonds. Polar and non-polar covalent bonding. Characteristics of covalent substances. | Representation of covalent bonds using dot and cross diagrams. Polarity test for liquids (use of charged plastic rod). Testing solubility in different solvents of ionic and covalent substances. | Polar and non-polar materials in everyday life (two examples of each). |
2.4 Electronegativity
(Time needed: 2 class periods) | Electronegativity. Periodic variation of electronegativity - explanation for general trends in values:
(i) down a group
(ii) across a period. Electronegativity differences and polarity of bonds. | Prediction of bond type using electronegativity differences. | |
2.5 Shapes of Molecules and Intermolecular Forces
(Time needed: 1 class period) | Shapes of some simple molecules. | Use of models or balloons to illustrate molecular shapes. | |
3.1 States of Matter
(Time needed: 1 class period) | Motion of particles in solids, liquids and gases. Diffusion (Graham's law not required). | NH3 and HCl, ink and water, smoke and air. | |
3.2 Gas Laws
(Time needed: 3 class periods) | Boyle's law. Charles's law. Combined gas law:
(P1V1)/T1=(P2V2)/T2=constant | Calculations not required. Calculations not required. Simple calculations, including correction of gas volumes to s.t.p. (units: Pa, cm3, K). | Boyle's air pump. |
3.3 The Mole
(Time needed: 9 class periods) | Avogadro constant. The mole as the SI unit for amount of substance containing the Avogadro number of particles. Standard temperature and pressure (s.t.p.). Molar volume at s.t.p., molar mass, relative molecular mass (Mr). | Calculation of relative molecular mass from relative atomic masses. Converting moles to grams, litres and number of particles. Converting grams and litres to moles. Mandatory experiment 3.1 | |
3.4 Chemical Formulas
(Time needed: 6 class periods) | Empirical and molecular formulas. Percentage composition by mass. Structural formulas. | Calculations of empirical formulas, given the percentage composition by mass. Calculation of molecular formulas, given the empirical formulas and the relative molecular masses (examples should include simple biological substances, such as glucose and urea). Calculations. Simple examples. | |
3.5 Chemical Equations
(Time needed: 9 class periods) | Chemical equations. Balancing chemical equations. Calculations based on balanced equations using the mole concept (balanced equations will be given for all calculations). | Simple examples. Calculations in g and kg rather than tonnes. Calculations involving masses and volumes. | |
4.1 Concentration of Solutions
(Time needed: 6 class periods) | Solutions.
Expression of solution concentration in mol l-1 (molarity), g l-1 and also in % (v/v). Colour intensity as a function of concentration (simple treatment only). Primary standards.
Standard solutions. | Calculation of molarity from concentration in grams per litre and vice versa. Calculation of number of moles from molarity and volume. Mandatory experiment 4.1 | Use of % (v/v), e.g. wine. |
4.2 Acids and Bases
(Time needed: 3 class periods) | Acids, bases and salts.
Neutralisation - formation of a salt from an acid and a base. Arrhenius theory of acids and bases (for aqueous solutions only). | | Household acids and bases (two examples of each). Everyday examples of neutralisation, e.g. use of lime in agriculture, use of stomach powders for acid indigestion. |
4.3 Volumetric Analysis
(Time needed: 10 class periods) | Apparatus used in volumetric analysis. Correct titrimetric procedure.
Acid-base titrations. | Solving volumetric problems, using the formula method. (Balanced equations will be given in all volumetric problems.) Mandatory experiment 4.2 Mandatory experiment 4.2A | |
5.1 Sources of Hydrocarbons
(Time needed: 1 class period) | Coal, natural gas and petroleum as sources of hydrocarbons. | | Decomposition of animal waste and vegetation as methane sources. Hazards of methane production in slurry pits, coal mines and refuse dumps.
Methane as a contributor to the greenhouse effect. |
5.2 Structure of Aliphatic Hydrocarbons
(Time needed: 5 class periods) | Alkanes, alkenes and alkynes as homologous series. For alkynes, only ethyne to be considered. Systematic names, structural formulas and structural isomers of alkanes to C-5. Structures, but not isomers, of hexane, heptane, octane, cyclohexane and 2,2,4-trimethylpentane (iso-octane) to be considered. Systematic names, structural formulas and structural isomers of alkenes to C-4. Physical properties [physical state, solubility (qualitative only) in water and in non-polar solvents]. | Use of models. Demonstration of the solubility properties of methane, ethene and ethyne. | |
5.3 Aromatic Hydrocarbons
(Time needed: 1 class period) | Structure of benzene, methylbenzene and ethylbenzene as examples of aromatic compounds. Physical properties [physical state, solubility (qualitative only) in water and in non-polar solvents]. | Use of models. Demonstration of the solubility properties of methylbenzene. | See aromatic compounds (page 20). |
5.4 Exothermic and Endothermic Reactions
(Time needed: 5 class periods) | Chemical reactions can result in a change in temperature. Exothermic and endothermic reactions (and changes of state). Combustion of alkanes and other hydrocarbons. Heat of reaction (general term). Sign of ?H. Heat of combustion. Bomb calorimeter as an instrument for accurately measuring heats of combustion. Heats of combustion of different fuels. | Demonstration of an exothermic and an endothermic reaction. Mandatory experiment 5.1 | Use of the bomb calorimeter in determining calorific values of foods.
Kilogram calorific values of fuels, and their uses (calculations not required). |
5.5 Oil Refining and its Products
(Time needed: 4 class periods) | Fractionation of crude oil. Production of the refinery gas, light gasoline, naphtha, kerosene, gas oil and residue fractions. | | Uses of the refinery gas, light gasoline, naphtha, kerosene, gas oil and residue fractions. Composition of natural gas and liquid petroleum gas (LPG). Addition of mercaptans to natural gas for safety reasons. Composition of petrol. Auto-ignition. Octane numbers as a measure of the tendency of a fuel to cause knocking. Lead in petrol. Alternatives to lead: improving octane number by
(i) isomerisation
(ii) dehydrocyclisation
(iii) catalytic cracking. |
5.6 Other Chemical Fuels
(Time needed: 3 class periods) | Ethyne: preparation, combustion, tests for unsaturation. Hydrogen: manufacture by
(i) electrolysis of water
(ii) steam reforming of natural gas (simple treatment only). | Mandatory experiment 5.2 (equations and structures of products not required for the tests for unsaturation). | Oxyacetylene welding and cutting. Industrial uses. Potential as a fuel. |
6.1 Reaction Rates
(Time needed: 3 class periods) | Rate of reaction. | Mandatory experiment 6.1 Plotting and simple interpretation of reaction rate graphs. | |
6.2 Factors Affecting Rates of Reaction
(Time needed: 7 class periods) | Concentration. Particle size. Temperature. Nature of reactants. Catalysts. | Demonstration of the effects on reaction rate of
(i) particle size
(ii) catalysts. Mandatory experiment 6.2 Demonstration of the oxidation of methanol using a hot platinum or nichrome catalyst. Demonstration of the oxidation of potassium sodium tartrate by hydrogen peroxide, catalysed by cobalt(II) salts. | Dust explosions. Enzymes as catalysts produced by living cells (two examples). Catalytic converters:
(i) nature of catalysts
(ii) reactions catalysed
(iii) environmental benefits. Catalyst poisons. |
7.1 Tetrahedral Carbon
(Time needed: 3 class periods) | Saturated organic compounds. Alkanes. Alcohols: structure and nomenclature up to C-4 (primary and secondary alcohols only). Physical properties [physical state, solubility (qualitative only) in water and in non-polar solvents]. | Use of models, as appropriate. Comparison of structure with water. Solubility of (a) methanol and (b) butan-1 -ol in (i) cyclohexane and (ii) water. | Use as fuels. Ethanol as a solvent.
Fermentation as a source of ethanol; use of fermentation in the brewing and distilling industries.
Methanol as a denaturing agent. |
7.2 Planar Carbon
(Time needed: 9 class periods) | Unsaturated organic compounds. Alkenes: non-polar double bond. Structure and nomenclature up to C-4. Carbonyl compounds (aldehydes only): polar double bond. Structure and nomenclature up to C-4. Physical properties [physical state, solubility (qualitative only) in water and in non-polar solvents]. Carboxylic acids: polar double bond. Structure and nomenclature up to C-4. Physical properties [physical state, solubility (qualitative only) in water and in non-polar solvents]. Simple explanation of the use of the circle to represent the identical bonds in benzene, intermediate between double and single. Aromatic compounds. An indication of the range and scope of aromatic chemistry (structures not required). | Use of models, as appropriate. Solubility of ethanal in (i) cyclohexane and (ii) water. Solubility of ethanoic acid in (i) cyclohexane and (ii) water. Mandatory experiment 7.1 Solubility of methylbenzene in (i) cyclohexane and (ii) water. Inspect structural formulas of a range of consumer products to show the presence of benzene rings. | Use in making plastics. Methanoic acid in nettles and ants; ethanoic acid in vinegar. Use of methylbenzene as an industrial solvent. Aromatic compounds form the basis of dyestuffs, detergents, herbicides and many pharmaceutical compounds (one example in each case; structures not required). Aromatic acid-base indicators: phenolphthalein, methyl orange (structures not required). Carcinogenic nature of some aromatic compounds, e.g. benzene. Not all aromatic compounds are carcinogenic, e.g. aspirin (structure of aspirin not required). |
7.3 Organic Chemical Reaction Types
(Time needed: 14 class periods) | Students are not, in general, required to know the conditions (temperature, pressure, catalyst, solvent) for these reactions, except where specified elsewhere in the syllabus. They are required to be able to write balanced equations for the reactions, using structural formulas, unless otherwise indicated. (a) Addition reactions
Alkenes - reactions with hydrogen, chlorine, bromine, water and hydrogen chloride. Polymerisation reaction (of ethene and propene only - reaction mechanism not required). Unreactivity of benzene with regard to addition reactions, relative to ethene. (b) Substitution reactions
Halogenation of alkanes. (c) Elimination reactions
Dehydration of alcohols. (d) Redox reactions
Alcohols:
Oxidation using KMnO4 or Na2Cr2O7 to (i) aldehydes and (ii) acids (half equations only required). Oxidation of aldehydes to acids (half equations only required). Combustion - a reaction common to most organic compounds.
Combustion of alcohols. Non-flammability of fully halogenated alkanes. (e) Reactions as acids
Reactions of alcohols with sodium.
Reactions of carboxylic acids with magnesium, with sodium hydroxide and with sodium carbonate. (f) Organic synthesis: principles and examples
Chemical synthesis involves
(i) bond breaking and
(ii) bond forming.
Example of organic synthesis: PVC from ethene (structures and synthetic route required). | Mandatory experiment 7.2 Mandatory experiment 7.3 (equations and structures of products not required, unless specified elsewhere in the syllabus). Mandatory experiment 7.4 Mandatory experiment 7.5 | Industrial sources.
Industrial importance of (i) products of the addition reactions of ethene with chlorine, bromine, water and hydrogen chloride (ii) hydrogenation of vegetable oils Alkenes as raw materials in the industrial manufacture of plastics. An indication of the range and scope of the petrochemical industry (two examples of synthetic products of this industry; structures not required, unless specified elsewhere in the syllabus).. Soap manufacture. Ethanal formation in the metabolism of ethanol in the human body. Alcohols as motor fuels. Flame retardants, fire extinguishers Useful products of organic synthesis (two examples, e.g. aspirin, paracetamol; structures and synthetic routes not required).. |
7.4 Organic Natural Products
(Time needed: 4 class periods) | Extraction techniques, e.g. solvent extraction, steam distillation. | Mandatory experiment 7.6 | An indication of the range and scope of organic natural product chemistry (two examples of useful organic natural products; structures not required). |
7.5 Chromatography and Instrumentation in Organic Chemistry
(Time needed: 3 class periods) | Chromatography as a separation technique in which a mobile phase carrying a mixture is caused to move in contact with a selectively absorbent stationary phase. Instrumental methods of separation or analysis, or both:
Mass spectrometry (cf.1.2, page 7).
Gas chromatography (GC).
High-performance liquid chromatography (HPLC). Brief reference to the principles of each method. Interpretation of spectra etc. not required. (It should be noted that these techniques are applicable not only to organic chemistry but also to many other areas of chemistry.) | Mandatory experiment 7.7 | Use of thin-layer chromatography (TLC) in the separation of dyes taken from fibres in forensic work. GC and HPLC as more advanced separation techniques. Examples of uses:
Analysis of (i) gases from a waste dump and (ii) trace organic pollutants in water. Drug tests on athletes; blood alcohol tests. Growth-promoters in meat; vitamins in foods. |
8.1 Chemical Equilibrium
(Time needed: 4 class periods) | Reversible reactions - dynamic equilibrium. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. Equilibrium law and constant (Kc only). | | |
8.2 Le Chatelier's Principle
(Time needed: 5 class periods) | Le Chatelier's principle. Effect (if any) on equilibrium position of concentration, pressure, temperature and catalyst. | Mandatory experiment 8.1 | Industrial application of Le Chatelier's principle in the catalytic oxidation of sulfur dioxide to sulfur trioxide and in the Haber process. |
9.1 pH Scale
(Time needed: 4 class periods) | pH scale. Use of universal indicator paper or solution.
Limitations of the pH scale - usefulness confined to dilute aqueous solutions. | Calculation of pH of dilute aqueous solutions of strong acids and bases (calculation of pH of mixtures of strong acids and bases not required). | |
9.2 Hardness in Water
(Time needed: 3 class periods) | Hardness in water. Causes of temporary and permanent hardness. Deionisation. | Tests on scale deposits in a kettle. | Removal of hardness by boiling and ion exchange. |
9.3 Water Treatment
(Time needed: 4 class periods) | Water treatment - sedimentation, flocculation, filtration, chlorination, fluoridation and pH adjustment. Sewage treatment (primary, e.g. settlement, screening; secondary, e.g. bacterial breakdown; tertiary, i.e. reduction of level of phosphates and nitrates).Cost of tertiary treatment. The role of nutrients in the eutrophication of water. | | Awareness that there are EU limits for various chemical species in water (two examples, e.g. nitrates, phosphates, specific metal ions). |
9.4 Water Analysis
(Time needed: 6 class periods) | Instrumental methods of analysis:
pH meter
Colorimetry
Brief reference to principles of each method. Tests for anions (cf. mandatory experiment 2.1). | Mandatory experiment 9.1 Mandatory experiment 9.2 | Examples of uses:
Analysis of river and lake water.
Analysis of (i) lead in water and (ii) fertilisers. Organic chemical pollutants, e.g. sewage, industrial waste, silage, milk. |
1A.1 General Principles
(Time needed: 4 class periods) | Batch, continuous and semicontinuous industrial chemical processes. Characteristics of effective and successful industrial chemical processes, such as
(i) feedstock (raw materials, preparation)
(ii) rate (temperature and pressure variables, catalyst)
(iii) product yield (temperature and pressure variables, catalyst)
(iv) co-products (separation, disposal or sale)
(v) waste disposal and effluent control (waste water treatment, emission control)
(vi) quality control
(vii) safety (location of site, onsite training, monitoring of hazards, safety features)
(viii)costs (fixed costs, variable costs; cost reduction by use of heat exchangers, catalysts, recycling and selling of useful coproducts; costs of waste disposal)
(ix) site location
(x) suitable materials for the construction of chemical plant (unreactive, resistant to corrosion). | See above. | Awareness of the contributions of chemistry to society, e.g. provision of pure water, fuels, metals, medicines, detergents, enzymes, dyes, paints, semiconductors, liquid crystals and alternative materials such as plastics and synthetic fibres; increasing crop yields by the use of fertilisers, herbicides and pesticides; food-processing. |
1A.2 Case Study
(Time needed: 5 class periods) | A case study based on the Irish chemical industry. ONE of the three following processes should be studied, using the principles outlined in 1A.1 as far as they are relevant to the process:
(a) Ammonia manufacture from natural gas, water vapour and air, and its conversion to urea. Equation required for ammonia formation.
(b) Nitric acid manufacture from ammonia, and its use to make fertilisers. Equation required for oxidation of nitrogen monoxide.
(c) Magnesium oxide manufacture from sea water. Equation required for formation of magnesium oxide. | | Awareness of the range and scope of the Irish chemical industry (two examples of products produced by this industry, other than those referred to in the case study chosen). Use of magnesium oxide as a heat-resistant material in the walls of furnaces. |
1B.1 Oxygen
(Time needed: 1 class period) | Manufacture of oxygen using liquefaction and fractional distillation of air. | | Uses of oxygen and of liquid nitrogen (two examples in each case). |
1B.2 Nitrogen
(Time needed: 1 class period) | Structure and inertness. Atmospheric abundance. Natural fixation of nitrogen; nitrogen and oxygen in an electric discharge. Nitrogen cycle. | | Any two uses, e.g. keeping foods fresh, flushing out dangerous vapours from oil tankers. |
1B.3 Carbon Dioxide
(Time needed: 3 class periods) | Combustion of carbon to give carbon monoxide and carbon dioxide. Carbon monoxide as a neutral oxide. Carbon dioxide as an acidic oxide. Fermentation in ethanol production as a source of carbon dioxide. The carbon cycle. | Demonstration of the effect of carbon dioxide on universal indicator solution. | Carbon monoxide as a poison. Carbon monoxide in cigarette smoke and vehicle exhaust fumes. Carbon dioxide in carbonated drinks. The greenhouse effect and the influence of human activity on it.
Greenhouse gases and their relative effects (especially carbon dioxide and water vapour).
Reduction of atmospheric carbon dioxide levels by dissolving in the ocean. Possible implications of the increased greenhouse effect. |
1B.4 Atmospheric Pollution
(Time needed: 2 class periods) | Oxides of nitrogen and sulfur: sources of pollution (natural, domestic, industrial, internal combustion engine).
Dissolving of nitrogen dioxide and sulfur dioxide to form acids. | Demonstration of the effect of sulfur dioxide on universal indicator solution. | Acid rain and its effects on the environment. Scrubbing of waste gases using limestone. |
1B.5 The Ozone Layer
(Time needed: 2 class periods) | Chloroalkanes: preparation from alkanes, e.g. chlorination of methane. | | Chlorofluorocarbons and the ozone layer. Formation of ozone in the stratosphere. Beneficial effect of the ozone layer. CFCs and HCFCs. Uses of CFCs. CFCs are believed to be the main cause of damage to the ozone layer. Effects of damage to the ozone layer. |
2A.1 Crystals
(Time needed: 3 class periods) | Ionic, molecular, metallic and covalent macromolecular crystals - physical properties related to the crystal binding forces.
Crystal structure is determined by scattering of X-rays by the crystal (non-mathematical treatment only). | Use of models. | Contributions of
(i) Braggs: development of the X-ray technique for determining crystal structure;
(ii) Dorothy Hodgkin: determination of the crystal structure of complex organic molecules, e.g. vitamin B12, penicillin (structures not required).
The discovery of buckminsterfullerene (structure not required). |
2A.2 Addition Polymers
(Time needed: 5 class periods) | Addition polymers. Monomers.
Polymerisation of alkenes: poly(ethene) (low-density), poly(chloroethene), poly(phenylethene). | Demonstration of physical properties (density, flexibility, hardness) of poly(ethene), poly(chloroethene) and poly(phenylethene). | The industrial and domestic importance and advantages of these polymers in plastics and fibres (two examples of uses of each polymer).
Brief history of the discovery of low-density poly(ethene).
Recycling of plastics, exemplified by the recycling of polystyrene (stages: sorting, shredding, washing, drying and re-extrusion). |
2A.3 Metals
(Time needed: 1 class period) | Comparison between metals and non-metals (hardness, lustre, malleability, ductility, heat conductivity and electrical conductivity). Alloys. | | Carbon in steel and hardness. |
2B.1 The Electrochemical Series
(Time needed: 1 class period) | Different combinations of metals produce different voltages in a simple cell.
The electrochemical series (reactions of metals with acids, water and oxygen not required). | | Contributions of Galvani, Volta, Davy and Faraday. |
2B.2 Electrolysis of Molten Salts
(Time needed: 1 class period) | Electrolysis of molten lead bromide, using inert electrodes. | | |
2B.3 Corrosion
(Time needed: 1 class period) | Corrosion of metals. Relative corrodibility of metals. | | Corrosion prevention (application of a protective layer on a metal: galvanising and surface coating). |
2B.4 Strongly Electropositive Metals (Na and Al)
(Time needed: 2 class periods) | Extraction by electrochemical methods. | | Uses (two examples in each case). Recycling of aluminium. |
2B.5 d-Block Metals
(Time needed: 4 class periods) | Transition elements: general chemical properties (colour, use as catalysts). Manufacture of iron (blast furnace - chemical aspects) and steel. Steels as alloys of iron. Electric arc process for steel manufacture (outline of main stages). | | Uses of iron and steel (two examples in each case). Environmental aspects of iron and steel production. |
1.1 Flame tests (Li, Na, K, Ba, Sr and Cu only).
1.2 Redox reactions of group VII elements: halogens as oxidising agents (reactions with bromides, iodides, Fe2+ and sulfites).
Displacement reactions of metals (Zn with Cu2+, Mg with Cu2+).
2.1 Tests for anions in aqueous solutions: chloride, carbonate, nitrate, sulfate.
3.1 Determination of the relative molecular mass of a volatile liquid (conical flask or gas syringe may be used).
4.1 Preparation of standard solution of sodium carbonate.
4.2 Standardisation of a hydrochloric acid solution using a standard solution of sodium carbonate.
4.2A A hydrochloric acid/sodium hydroxide titration, and the use of this titration in making the salt sodium chloride.
5.1 Determination of the heat of reaction of hydrochloric acid with sodium hydroxide.
5.2 Preparation and properties of ethyne [combustion, tests for unsaturation using bromine water and acidified potassium manganate(VII) solution].
6.1 Monitoring the rate of production of oxygen from hydrogen peroxide, using manganese dioxide as a catalyst.
6.2 Studying the effects on the reaction rate of (i) concentration and (ii) temperature, using sodium thiosulfate solution and hydrochloric acid.
7.1 Recrystallisation of benzoic acid and determination of its melting point.
7.2 Preparation of soap.
7.3 Preparation and properties of ethene [combustion, tests for unsaturation using acidified potassium manganate(VII) solution and bromine water].
7.4 Preparation and properties of ethanal [properties limited to reactions with (i) acidified potassium manganate(VII) solution, (ii) Fehling's reagent and (iii) ammoniacal silver nitrate].
7.5 Preparation and properties of ethanoic acid (properties limited to reactions with sodium carbonate and magnesium).
7.6 Extraction of clove oil from cloves (or similar alternative) by steam distillation.
7.7 Separation of a mixture of indicators using paper chromatography or thin-layer chromatography or column chromatography.
8.1 Simple experiments to illustrate Le Chatelier's principle.
9.1 Colorimetric experiment to estimate free chlorine in swimming-pool water or bleach (using a colorimeter or a comparator).
9.2 Determination of total suspended and total dissolved solids (expressed as p.p.m.) by filtration and evaporation respectively.
Determination of pH.