PHYSICAL CHEMISTRY
1. ATOMS, MOLECULES AND STOICHIOMETRY
• Relative masses of atoms and molecules
• The mole, the Avogadro constant
• The calculation of empirical and molecular formulae
• Reacting masses and volumes (of solutions and gases)
2. REDOX REACTIONS
• Redox processes: electron transfer and changes in oxidation number (oxidation state)
3. ATOMIC STRUCTURE
• The nucleus of the atom: neutrons and protons, isotopes, proton and nucleon numbers
• Electrons: electronic energy levels, ionisation energies, atomic orbitals, extranuclear structure
4. CHEMICAL BONDING
• Ionic (electrovalent) bonding
• Covalent bonding and co-ordinate (dative covalent) bonding
(i) The shapes of simple molecules
(ii) Bond energies, bond lengths and bond polarities
• Intermolecular forces, including hydrogen bonding
• Metallic bonding
• Bonding and physical properties
• The solid state
5. CHEMICAL ENERGETICS
• Enthalpy changes: ΔH of formation, combustion, and neutralisation; bond energy; lattice energy
• Hess’ Law
6. EQUILIBRIA
• Chemical equilibria: reversible reactions; dynamic equilibrium
(i) Factors affecting chemical equilibria
(ii) Equilibrium constants
(iii) The Haber process
• Ionic equilibria
(i) Brønsted-Lowry theory of acids and bases
(ii) Acid dissociation constants, Ka
(iii) Base dissociation constants, Kb
(iv) The ionic product of water, Kw
(v) pH: choice of indicators
(vi) Buffer solutions
7. REACTION KINETICS
• Simple rate equations; orders of reaction; rate constants
• Concept of activation energy
• Effect of concentration, temperature, and catalysts on reaction rate
• Enzymes as biological catalysts
8. INORGANIC CHEMISTRY
THE PERIODIC TABLE: CHEMICAL PERIODICITY
• Periodicity of physical properties of the elements: variation with proton number across the third period (sodium to argon) of:
(i) Atomic radius and ionic radius
(ii) Melting point
(iii) Electrical conductivity
(iv) Ionisation energy
• Periodicity of chemical properties of the elements in the third period
(i) Reaction of the elements with oxygen and chlorine
(ii) Variation in oxidation number of the oxides (sodium to sulphur only) and of the chlorides (sodium to phosphorus only)
(iii) Reactions of these oxides and chlorides with water
(iv) Acid/base behaviour of these oxides and the corresponding hydroxides
9. ORGANIC CHEMISTRY
9.1 INTRODUCTORY TOPICS
In each of the sections below, 9.1 to 9.6, candidates will be expected to be able to predict the reaction products of a given compound in reactions that are chemically similar to those specified.
Content
• Molecular, structural and empirical formulae
• Functional groups and the naming of organic compounds
• Characteristic organic reactions
• Shapes of organic molecules; σ and π bonds
• Isomerism: structural; geometrical
9.2 HYDROCARBONS
• Alkanes (exemplified by ethane)
(i) Combustion and substitution reactions
• Alkenes (exemplified by ethene)
(i) Addition and oxidation reactions
• Arenes (exemplified by benzene and methylbenzene)
(i) Influence of delocalised π electrons on structure and properties
(ii) Substitution reactions
(iii) Oxidation of side-chain
• Hydrocarbons as fuels
9.3 HALOGEN DERIVATIVES
• Halogenoalkanes
(i) Substitution
(ii) Elimination
• Relative strength of the C-Hal bond
9.4 ALCOHOLS
• Alcohols (exemplified by ethanol)
(i) Formation of halogenoalkanes
(ii) Reaction with sodium; oxidation; dehydration
(iii) The tri-iodomethane test
9.5 CARBONYL COMPOUNDS
• Aldehydes (exemplified by ethanal)
(i) Oxidation to carboxylic acid
(ii) Reaction with hydrogen cyanide
(iii) Characteristic tests for aldehydes
• Ketones (exemplified by propanone)
(i) Reaction with hydrogen cyanide
(ii) Characteristic tests for ketones
9.5 CARBONYL COMPOUNDS
• Aldehydes (exemplified by ethanal)
(i) Oxidation to carboxylic acid
(ii) Reaction with hydrogen cyanide
(iii) Characteristic tests for aldehydes
• Ketones (exemplified by propanone)
(i) Reaction with hydrogen cyanide
(ii) Characteristic tests for ketones
Detailed Syllabus (SEAB) [PDF]
2008 GCE A Level Exam Syllabuses
