Chapter 0: Fundamentals 0.1 Measurement in chemistry and science - SI units 0.2 Expressing large and small numbers using scientific notation 0.3 Using metric prefixes 0.3.1 Units of mass and volume used in chemistry 0.4 Significant figures 0.5 Calculations using scientific notation 0.
5.1 Adding and subtracting 0.5.2 Multiplying and dividing numbers 0.6 Writing chemical formulae and equations 0.6.1 Writing chemical formulae 0.6.
2 Writing and balancing chemical equations 0.6.3 Indicating the physical state of reactants and products in chemical equations Quick-check summary Chapter 1: Atomic Structure 1.1 Atomic Structure 1.1.1 Atomic particles 1.1.2 Mass number (A) and atomic number (Z) 1.
1.3 Isotopes 1.1.4 Radioisotopes 1.2 Electronic Structure 1.2.1 The periodic table 1.2.
2 Electron energy levels 1.2.3 Simple electronic configurations 1.2.4 Sub-shells and atomic orbitals 1.2.5 Describing electronic configurations 1.2.
6 Electronic structures and the periodic table Quick-check summary Chapter 2: Chemical Bonding 2.1 Bonding 2.1.1 Atoms and molecules 2.1.2 Metallic bonding 2.1.3 Ionic bonding 2.
1.4 Covalent bonding 2.2 Valence Shell Electron Pair Repulsion Theory (VSEPR) 2.2.1 Two electron centres around the central atom: linear molecules 2.2.2 Three electron centres around the central atom: trigonal planar molecules 2.2.
3 Four electron centres around the central atom: tetrahedral, pyramidal, bent molecules 2.2.4 Five electron centres around the central atom: trigonal bipyramidal molecules 2.2.5 Six electron centres around the central atom: octahedral molecules 2.3 Polar bonds and polar molecules 2.3.1 Electronegativity 2.
3.2 Polar bonds 2.3.3 Polar molecules 2.4 Intermolecular forces 2.4.1 Permanent dipole-permanent dipole interactions 2.4.
2 London dispersion forces (instantaneous dipole-induced dipole) 2.4.3 Hydrogen bonding 2.4.4 Summary of strengths of intermolecular forces 2.4.5 A special case: ion-dipole intermolecular forces Quick-check summary Chapter 3 Masses of atoms, molecules and reacting substances 3.1 Masses of atoms and molecules 3.
1.1 Relative atomic mass, Ar 3.1.2 Relative molecular mass, Mr 3.1.3 Relative formula mass 3.2 Amount of substance 3.2.
1 The mole 3.2.2 Converting between moles and masses of substances - Molar mass 3.3 Calculations with moles 3.3.1 Reacting masses 3.3.2 Percentage yield 3.
3.3 Percentage composition by mass 3.3.4 Empirical Formula 3.4 Solutions; concentrations and dilutions 3.4.1 Measuring and expressing concentrations 3.4.
2 Solutions and dilutions 3.4.3 Alternative units of concentration 3.5 Titration calculations 3.6 Calculations with gas volumes Quick check summary Chapter 4: States of Matter Introduction 4.1 Solids 4.1.1 Metallic lattices 4.
1.2 Ionic lattices 4.1.3 Simple molecular solids and giant molecular structures 4.2 Liquids 4.2.1 Evaporation and condensation, vapour pressure and boiling 4.2.
2 Effect of intermolecular forces on melting and boiling points 4.3 Gases 4.3.1 Ideal gases 4.3.2 The ideal gas equation 4.3.3 The molar gas volume Quick check summary Chapter 5 Oxidation-reduction (redox) reactions 5.
1 Redox Reactions 5.1.1 Electron transfer in redox reactions 5.1.2 Oxidation numbers 5.1.3 Naming compounds based on the oxidation state of elements in the compound 5.1.
4 Redox half-equations 5.1.5 Oxidising agents and reducing agents 5.2 Disproportionation Reactions 5.3 Redox titrations Quick check summary Chapter 6 Energy, Enthalpy and Entropy 6.1 Enthalpy Changes 6.1.1 Energy and enthalpy 6.
1.2 Exothermic and endothermic reactions 6.1.3 Reaction pathway diagrams 6.1.4 Measuring enthalpy changes 6.1.5 Measuring enthalpy changes using calorimetry 6.
1.6 Hess''s Law 6.1.7 Bond energies and enthalpy changes 6.1.8 Born-Haber cycles 6.1.9 Factors affecting the size of the lattice energy 6.
2 Entropy and Gibbs Free Energy 6.2.1 Entropy 6.2.2 Spontaneous processes and the 2nd law of thermodynamics 6.2.3 Gibbs free energy and spontaneous reactions Quick-check summary Chapter 7 Chemical Equilibrium and Acid-Base Equilibria Introduction 7.1 Equilibria and reversible reactions 7.
1.1 The equilibrium mixture and the equilibrium constant, Kc. 7.1.2 The effects of changing the reaction conditions at equilibrium 7.1.3 Heterogeneous and homogeneous equilibria 7.1.
4 The equilibrium constant, Kp 7.2 Acid - base equilibria 7.2.1 The Brønsted-Lowry theory of acids and bases 7.2.2 The pH scale 7.2.3 Strong and weak acids and bases 7.
2.4 The ionisation of water 7.2.5 Acid-base reactions 7.2.6 Carrying out a titration 7.2.7 Indicators 7.
2.8 Acid-base titrations 7.2.9 Buffers 7.2.10 Calculating the pH of a buffer solution 7.2.11 Lewis acids and bases Quick-check Summary Chapter 8 Chemical Kinetics - The Rates of Chemical Reactions Introduction 8.
1 The rate of reaction 8.1.1 Defining the rate of a chemical reaction 8.1.2 Collision theory 8.1.3 Factors that affect the rate of a reaction 8.2 Determining the rate of a chemical reaction 8.
2.1 Methods of monitoring the rate 8.2.2 The rate of reaction at any instant 8.2.3 An example of measuring rate of reaction at any time 8.3 The rate expression 8.3.
1 Determining the rate expression using instantaneous rates 8.3.2 Determining the rate expression using the initial rates method 8.3.3 Determining the rate expression by inspection 8.3.4 Determining the rate expression using the integrated rate expression. 8.
4 The half-life of a reaction 8.4.1 Half-life of first-order reactions 8.4.2 Half-life of zero-order reactions 8.4.3 Half-life of second-order reactions 8.5 Reaction mechanisms 8.
5.1 Reaction mechanisms and the rate-determining step 8.5.2 Using the rate expression to determine the mechanism of a reaction 8.6 Effect of temperature on reaction rate 8.6.1 The distribution of the energies of molecules with temperature 8.6.
2 The Arrhenius Equation Quick-check Summary Chapter 9 Electrochemistry Introduction 9.1 Redox reactions - a reminder 9.2 Redox reactions and electrochemical cells 9.2.1 Electrochemical cells and half-cells 9.2.2 Standard electrode potentials, E? 9.2.
3 The standard hydrogen electrode 9.2.4 Values of standard reduction potentials 9.2.5 Half-cells involving non-metals and non-metal ions 9.2.6 The cell diagram 9.2.
7 Using E? values to obtain voltages of electrochemical cells 9.2.8 Using standard reduction potentials to predict the outcome of redox reactions 9.2.9 Relation between E? and Gibbs energy 9.2.10 The effect of non-standard conditions on cell potential - the Nernst equation 9.3 Using redox reactions - Galvanic cells 9.
3.1 Galvanic (voltaic) cells 9.3.2 The variety of cells 9.3.3 Disposable batteries 9.3.4 Rechargeable cells 9.
3.5 Fuel cells 9.4 Using redox reactions - Electrolytic cells 9.4.1 Electrolysis 9.4.2 Electrolysis of molten substances 9.4.
3 Electrolysis of aqueous solutions 9.4.4 Calculating the amount of substance deposited during electrolysis Quick-check Summary Chapter 10: Group trends and periodicity 10.1 The Periodic Table: Periods, Groups and Periodicity 10.2 Trends in properties of elements in the same vertical group of the periodic table 10.2.1 Electron configuration 10.2.
2 Effective nuclear charge, Zeff 10.2.3 Atomic radius 10.2.4 Ionisation energies 10.2.5 Electronegativity 10.3 Trends in properties of elements in the same horizontal period 10.
3.1 Electron configuration 10.3.2 Atomic radius 10.3.3 Ionisation Energy 10.3.4 Electronegativity 10.
3.5 Electron affinity , ?EAH? 10.3.6 Ionic radius 10.3.7 Melting Point and Boiling Point 10.3.8 Trends in chemical properties across a period Quick check summary Chapter 11: The Periodic Table - chemistry of Groups 1, 2, 7 and transition elements Introduction 11.
1 Group 1 - The Alkali Metals 11.1.1. Physical properties of Group 1 elements 11.1.2 Chemical properties of Group 1 elements 11.2 Group 2 - The Alkaline Earth Metals 11.2.
1 Physical properties of Group 2 elements 11.2.2 Chemical properties of Group 2 elements 11.2.3 Some s block compounds and their properties 11.3 Group 7 (17) The Halogens 11.3.1 Physical properties of Group 7 (17) elements 11.
3.2 Reactions of Group 7 elements 11.4 The Transition Elements 11.4.1 Physical properties of transition elements 11.4.2 Complexes of transition element.