Understand reaction rates: factors like temperature, surface area, concentration, and pressure affect how quickly reactions occur by influencing particle collisions. Catalysts speed up reactions by lowering activation energy without being consumed. Practical examples include changing temperatures, varying concentrations, and using catalysts like manganese oxide to increase reaction rates.

Understand bond energies: energy level diagrams illustrate exothermic and endothermic reactions, showing enthalpy change (ΔH) and activation energy. Breaking bonds requires energy, making it an endothermic process, while forming bonds releases energy, making it exothermic. Calculate ΔH using bond energies: subtract energy released when bonds form from energy required to break bonds.

Learn about energetics: exothermic reactions release heat, increasing temperature, while endothermic reactions absorb heat, lowering temperature. Calorimetry measures enthalpy change (ΔH) by recording temperature changes during reactions, such as combustion or neutralisation. The heat energy transferred is calculated using the formula Q = mcΔT, helping determine the energy change per gram or mole of a substance.

Learn about chemical tests: identify gases like hydrogen, oxygen, and carbon dioxide using specific reactions. Flame tests reveal metal ions by color, while tests with sodium hydroxide identify cations like Cu²⁺ and Fe³⁺. Anions like chlorides, sulphates, and carbonates form distinctive precipitates when reacted with specific reagents. Water can be tested chemically with anhydrous copper sulphate or physically by its melting and boiling points.

Learn about making salts: soluble salts are prepared by reacting acids with alkalis, often using titration to ensure precise neutralization. Insoluble salts form via precipitation reactions between two soluble reactants, with the resulting precipitate filtered, washed, and dried to obtain a pure sample.

Understand acids, bases, and salts: acids are proton donors, and bases are proton acceptors. Acids react with metals, bases, and carbonates to form salts, often releasing gases like hydrogen or carbon dioxide. Solubility rules predict if salts are soluble or form precipitates, aiding in practical salt preparation methods.

Learn about titrations: a technique used to determine the concentration of an acid or alkali by measuring the volume needed to neutralize it. This process involves using indicators like phenolphthalein, which changes color at the endpoint, and calculating moles to find unknown concentrations.

Learn about acids and alkalis: acids release hydrogen ions (H⁺), while alkalis release hydroxide ions (OH⁻). Indicators like litmus, phenolphthalein, and methyl orange help distinguish between them. The pH scale classifies solutions from acidic to alkaline, with neutralization reactions forming water when acids and alkalis mix.

Understand the uses and extraction of metals. Most metals are extracted from ores, with less reactive metals extracted using carbon reduction and more reactive ones via electrolysis. Metals like aluminium, copper, and iron are used widely due to their properties, such as conductivity and malleability. Alloys, mixtures of metals, are stronger and more resistant than pure metals.

Learn about the reactivity of metals and the reactivity series. Metals react with water and acids, with more reactive metals displacing less reactive ones in redox reactions. Rusting of iron, an oxidation process, can be prevented using barriers, galvanizing or sacrificial protection.