Studied by 2 peopleReactivity of Metals
Refers to a metal's tendency to form cations when reacting with other substances, with a higher tendency indicating higher reactivity. The reactivity series lists metals in order of reactivity.
Extraction of Metals and Reduction
Describes the process of extracting metals from compounds, often using carbon for less reactive metals. Reduction involves the gain of electrons, as per the OILRIG principle.
Oxidation and Reduction in Terms of Electrons
OILRIG principle explains oxidation as loss and reduction as gain of electrons. Charges should balance in chemical equations, with cations losing electrons and anions gaining them.
Reactions of Acids with Metals
Involves the reaction of acids with metals to form salt and hydrogen, following the principles of oxidation and reduction.
Neutralisation of Acids and Salt Production
Neutralization reactions between acids and alkalis/bases produce salts and water. The type of salt formed depends on the reactants involved.
Soluble Salts
Form when an acid reacts with a solid insoluble substance, requiring the solid to be added until it no longer dissolves, followed by crystallization.
The pH Scale and Neutralization
pH scale measures acidity/basicity, with lower pH indicating stronger acids. Neutralization involves the reaction of H+ and OH- ions to form water.
Titrations
Used to determine the concentration of an unknown substance in a solution, involving a step-by-step process to calculate concentrations accurately.
Strong and Weak Acids
Strong acids completely ionize in solution, leading to low pH, while weak acids only partially ionize. The strength refers to the concentration of H+ ions in the solution.
Electrolysis
Involves passing a current through a solution to break down compounds into elements, with ions moving to electrodes based on charge. It is used for extracting metals and producing substances like aluminum.
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