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Chemistry (9476)

23 sections available

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

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

THE GASEOUS STATE

Ideal gas behaviour and deviations from it
pV = nRT and its use in determining a value for Mr
Dalton’s Law and its use in determining the partial pressures of gases in a mixture

THEORIES OF ACIDS AND BASES

Arrhenius, Brønsted-Lowry and Lewis theories of acids and bases

THE PERIODIC TABLE

The Periodic Table

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)

CHEMICAL ENERGETICS: THERMOCHEMISTRY AND THERMODYNAMICS (GIBBS FREE ENERGY AND ENTROPY)

Enthalpy changes: ΔH, of formation; combustion; hydration; solution; neutralisation; atomisation; bond energy; lattice energy; electron affinity
Hess’ Law, including Born-Haber cycles
Entropy and Free Energy

REACTION KINETICS

Simple rate equations; orders of reaction; rate constants
Concept of activation energy
Effect of concentration, temperature, and catalysts on reaction rate
Homogeneous and heterogeneous catalysis
Enzymes as biological catalysts

CHEMICAL EQUILIBRIA

Chemical equilibria: reversible reactions; dynamic equilibrium

ACID-BASE EQUILIBRIA

Acid dissociation constants, Ka and the use of pKa
Base dissociation constants, Kb and the use of pKb
The ionic product of water, Kw
pH: choice of pH indicators
Buffer solutions

SOLUBILITY EQUILIBRIA

Solubility product; the common ion effect and complex ion formation

ORGANIC CHEMISTRY INTRODUCTION

Empirical, molecular and structural formulae
Functional groups and the naming of organic compounds
Shapes of organic molecules; σ and π bonds

ISOMERISM

Isomerism: constitutional (structural); cis-trans; enantiomerism

ORGANIC REACTIONS AND MECHANISMS

Common terms for organic reactions and reactivities
Reactivity of some classes of compounds and their characteristic organic reaction mechanisms

HYDROCARBONS

Alkanes (exemplified by ethane)
Alkenes (exemplified by ethene)
Arenes (exemplified by benzene and methylbenzene)
Hydrocarbons as fuels

HALOGEN DERIVATIVES

Halogenoalkanes
Relative strength of the carbon-halogen bond
Unreactivity of halogenoarenes

HYDROXY COMPOUNDS

Alcohols (exemplified by ethanol)
Phenol

CARBONYL COMPOUNDS

Aldehydes (exemplified by ethanal)
Ketones (exemplified by propanone and phenylethanone)

CARBOXYLIC ACIDS AND DERIVATIVES

Carboxylic acids (exemplified by ethanoic acid and benzoic acid)
Acyl chlorides (exemplified by ethanoyl chloride)
Esters (exemplified by ethyl ethanoate and phenyl benzoate)

NITROGEN COMPOUNDS

Amines (exemplified by ethylamine and phenylamine)
Amides (exemplified by ethanamide)
Amino acids (exemplified by aminoethanoic acid)

POLYMERS

Addition and condensation of polymers
Proteins
Biodegradability of poly(alkenes), polyesters and polyamides

ELECTROCHEMISTRY

Redox processes: electron transfer and changes in oxidation number (oxidation state)
Electrode potentials
Electrolysis

AN INTRODUCTION TO THE CHEMISTRY OF TRANSITION ELEMENTS

General physical and characteristic chemical properties of the first set of transition elements, scandium to copper
Colour of complexes

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