1-States of matter 1-1 Everythings is made of particles 1-2 Solids, liquids, and gases 1.3 The particles in solids, Liquids, and gases 1.4 Heating and cooling curves 1.5 A closer look at gases

Energy changes in reactions Describing exothermic reactions Describing endothermic reactions A closer look at energy changes Reaction pathway diagram Activation Energy and Enthalpy Calculation Enthalpy changes The hydrogen-oxygen fuel cell

2.1 - Meet the elements 2.2 – More about atoms 2.3 – How electrons are arranged 2.4 –Isotops and Ar

9.1 Introducing reaction rates 9.2 Measuring the rate of reaction 9.3 / 9.4 Changing the rate 9.5 Explaining rate changes 9.6 Catalyst

Chemistry IB _ Grade 11 and 12 Topic 3 : Periodicity

Chemistry IB _ Grade 11 and 12 Topic 9 : Redox processes

Chemistry IB _ Grade 11 and 12 Topic 6 : Chemical kinetics

Chemistry IB _ Grade 11 and 12 Topic 10 : Organic chemistry

Chemistry IB _ Grade 11 and 12 Topic 11 : Measurement and data processing

Chemistry IB _ Grade 11 and 12 Topic 2 : Atomic structure

Chemistry IB _ Grade 11 and 12 Topic 5 : Energetics/thermochemistry

Chemistry IB _ Grade 11 and 12 Topic 8 : Acids and bases

Chemistry IB _ Grade 11 and 12 Topic 4 : Chemical bonding and structure

Chemistry IB _ Grade 11 and 12 Topic 7 : Equilibrium

Chemistry IB _ Grade 11 and 12 Topic 1 : Stoichiometric relationships

Structure 2 / IB Chemistry / Structure 2.2 (lesson / Worksheets / Tests/ Tables / Figures) Structure 2.2—The covalent model Structure 2.2.1—A covalent bond is formed by the electrostatic attraction between a shared pair of electrons and the positively charged nuclei. Structure 2.2.2—Single, double and triple bonds involve one, two and three shared pairs of electrons respectively. Structure 2.2.3—A coordination bond is a covalent bond in which both the electrons of the shared pair originate from the same atom. Structure 2.2.4—The valence shell electron pair repulsion (VSEPR) model enables the shapes of molecules to be predicted from the repulsion of electron domains around a central atom. Structure 2.2.5—Bond polarity results from the difference in electronegativities of the bonded atoms. Structure 2.2.6—Molecular polarity depends on both bond polarity and molecular geometry. Structure 2.2.7—Carbon and silicon form covalent network structures. Structure 2.2.8—The nature of the force that exists between molecules is determined by the size and polarity of the molecules. Intermolecular forces include London (dispersion), dipole-induced dipole, dipole–dipole and hydrogen bonding. Structure 2.2.9—Given comparable molar mass, the relative strengths of intermolecular forces are generally: London (dispersion) forces < dipole–dipole forces < hydrogen bonding. Structure 2.2.10—Chromatography is a technique used to separate the components of a mixture based on their relative attractions involving intermolecular forces to mobile and stationary phases.

Structure 2 / IB Chemistry / Structure 2.1 +worksheets +Formulae of common ions / ionic compounds Structure 2. Models of bonding and structure Structure 2.1.1 — When metal atoms lose electrons, they form positive ions called cations. When non-metal atoms gain electrons, they form negative ions called anions. Structure 2.1.2 — The ionic bond is formed by electrostatic attractions between oppositely charged ions. Structure 2.1.3—Ionic compounds exist as three-dimensional lattice structures, represented by empirical formulas.

11.1 Acids and bases 11.2 A closer look at acids and alkalis 11.3 The reaction of acids and bases 11.4 A closer look at neutralisation 11.5 Oxides 11.6 Making Salts 11.7 Making insoluble salt by precipitation 11.8 Finding the concentration by titration

Compounds, mixtures, and chemical change Why do atoms form bonds? The ionic bond More about ions The covalent bond Covalent compounds Comparing ionic and covalent compounds Giant covalent structures The bonding in metals

Reactivity 2.3—How far? The extent of chemical change Reactivity 2.3.1—A state of dynamic equilibrium is reached in a closed system when the rates of forward and backward reactions are equal. Reactivity 2.3.2—The equilibrium law describes how the equilibrium constant, K, can be determined from the stoichiometry of a reaction. Reactivity 2.3.3—The magnitude of the equilibrium constant indicates the extent of a reaction at equilibrium and is temperature dependent. Reactivity 2.3.4—Le Châtelier’s principle enables the prediction of the qualitative effects of changes in concentration, temperature and pressure to a system at equilibrium. Reactivity 2.3.5—The reaction quotient, Q, is calculated using the equilibrium expression with non- equilibrium concentrations of reactants and products. Reactivity 2.3.6—The equilibrium law is the basis for quantifying the composition of an equilibrium mixture. Reactivity 2.3.7—The equilibrium constant and Gibbs energy change, ΔG, can both be used to measure the position of an equilibrium reaction.