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

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

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

Chemistry IB _ Grade 11 and 12 Topic 7 : Equilibrium

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

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

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

5 - usings moles 5.1 The mole 5.2 Calculations from equations 5.3 Reactions involving gases 5.4 The concentration of a solution 5.5 Finding the empirical formula 5.6 From empirical to final formula 5.7 Finding % yield and % purity

Reactivity 1.2 - Energy cycles in reactions Reactivity 1.2.1 - Bond-breaking absorbs and bond-forming releases energy. Reactivity 1.2.2 - Hess’s law states that the enthalpy change for a reaction is independent of the pathway between the initial and final states. Reactivity 1.2.3 - Standard enthalpy changes of combustion, ΔHc ⦵, and formation, ΔHf ⦵, data are used in thermodynamic calculations. Reactivity 1.2.4 - An application of Hess’s law uses enthalpy of formation data or enthalpy of combustion data to calculate the enthalpy change of a reaction. Reactivity 1.2.5—A Born–Haber cycle is an application of Hess’s law, used to show energy changes in the formation of an ionic compound.

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

Reactivity 2.2—How fast? The rate of chemical change Reactivity 2.2.1—The rate of reaction is expressed as the change in concentration of a particular reactant/product per unit time. Reactivity 2.2.2—Species react as a result of collisions of sufficient energy and proper orientation. Reactivity 2.2.3—Factors that influence the rate of a reaction include pressure, concentration, surface area, temperature and the presence of a catalyst. Reactivity 2.2.4—Activation energy, Ea, is the minimum energy that colliding particles need for a successful collision leading to a reaction. Reactivity 2.2.5—Catalysts increase the rate of reaction by providing an alternative reaction pathway with lower Ea. Reactivity 2.2.6—Many reactions occur in a series of elementary steps. The slowest step determines the rate of the reaction. Reactivity 2.2.7—Energy profiles can be used to show the activation energy and transition state of the rate-determining step in a multistep reaction. Reactivity 2.2.8—The molecularity of an elementary step is the number of reacting particles taking part in that step. Reactivity 2.2.9—Rate equations depend on the mechanism of the reaction and can only be determined experimentally. Reactivity 2.2.10—The order of a reaction with respect to a reactant is the exponent to which the concentration of the reactant is raised in the rate equation. The order with respect to a reactant can describe the number of particles taking part in the rate-determining step. The overall reaction order is the sum of the orders with respect to each reactant. Reactivity 2.2.11—The rate constant, k, is temperature dependent and its units are determined from the overall order of the reaction. Reactivity 2.2.12—The Arrhenius equation uses the temperature dependence of the rate constant to determine the activation energy. Reactivity 2.2.13—The Arrhenius factor, A, takes into account the frequency of collisions with proper orientations.

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