SEAB GCE A-Level H1 Chemistry – Scheme of Assessment
Papers Overview
All candidates must sit for both Paper 1 and Paper 2.
| Paper | Type of Paper | Duration | Weightage | Marks |
|---|---|---|---|---|
| 1 | Multiple Choice | 1 hour | 33% | 30 |
| 2 | Structured Questions | 2 hours | 67% | 80 |
CORE IDEA 1 – MATTER
1. 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
CORE IDEA 2 – STRUCTURE AND PROPERTIES
2. CHEMICAL BONDING
- Ionic bonding, metallic bonding, covalent bonding and co-ordinate (dative covalent) bonding
- Shapes of simple molecules and bond angles
- Bond polarities and polarity of molecules
- Intermolecular forces, including hydrogen bonding
- Bond energies and bond lengths
- Lattice structure of solids
- Bonding and physical properties
3. THEORIES OF ACIDS AND BASES
- Arrhenius and Brønsted-Lowry theories of acids and bases
- Acid dissociation constants, Ka
- Base dissociation constants, Kb
- The ionic product of water, Kw
- pH: choice of indicators
- Buffer solutions
4. THE PERIODIC TABLE
- Periodicity of atomic and physical properties of the elements: variation with proton number across the thirdperiod (sodium to chlorine) and down Group 17 of:
- (i) electronic configuration
- (ii) atomic radius and ionic radius
- (iii) ionisation energy
- (iv) electronegativity
- (v) melting point
- (vi) electrical conductivity
- Periodicity of chemical properties of the elements in the third period:
- (i) variation in oxidation number and bonding of the oxides (sodium to sulfur only) and of the chlorides (sodium to phosphorus only)
- (ii) reactions of these oxides and chlorides with water
- (iii) acid/base behaviour of these oxides and the corresponding hydroxides
- Periodicity of chemical properties of the elements down the group (Group 1 and Group 17):
- (i) as reducing agents (Group 1) and oxidising agents (Group 17)
- (ii) thermal stability of Group 17 hydrides
CORE IDEA 3 – TRANSFORMATION
5. THE MOLE CONCEPT 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)
- Redox processes: electron transfer and changes in oxidation number (oxidation state)
6. CHEMICAL ENERGETICS: THERMOCHEMISTRY
- Enthalpy changes: ∆H, of formation; combustion; neutralisation; bond energy; lattice energy
- Hess’ Law
7. REACTION KINETICS
- Simple rate equations; orders of reaction; rate constants
- Concept of activation energy
- Effect of concentration, temperature, and catalysts on reaction rate
- Heterogenous catalysts
- Enzymes as biological catalysts
8. CHEMICAL EQUILIBRIA
- Chemical equilibria: reversible reactions; dynamic equilibrium
- (i) factors affecting chemical equilibria
- (ii) equilibrium constants
- (iii) the Haber process
EXTENSION TOPIC
9. POLYMERS AND ORGANIC CHEMISTRY
- Empirical, molecular and structural formulae
- Functional groups and the naming of organic compounds
- Common terms for organic reactions
- Isomerism: constitutional (structural); cis-trans
- Shapes of organic molecules; σ and π bonds
- Alkanes (as exemplified by ethane)
- (i) combustion and substitution reaction•
- Alkenes (as exemplified by ethene)
- (i) combustion and addition reactions
- Halogenoalkanes (as exemplified by bromoethane)
- (i) substitution
- (ii) elimination
- Alcohols (as exemplified by ethanol)
- (i) combustion
- (ii) oxidation to carboxylic acids
- (iii) elimination
- Aldehydes (as exemplified by ethanal)
- (i) oxidation to carboxylic acid
- (ii) reduction
- Ketones (as exemplified by propanone)
- (i) reduction
- Carboxylic acids (as exemplified by ethanoic acid)
- (i) ester formation
- (ii) amide formation
- Amino acids (as exemplified by aminoethanoic acid)
- Structure and uses of polymers
