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Redox is short for reduction-oxidation. It is the transferring of electrons from one species to another.
OXIDATION: A reaction where an atom or a group of atoms lose electrons.
OXIDISING AGENT: A reagent that oxidises (removes electrons from) another species.
REDUCTION: A reaction in which an atom or group of atoms gain electrons.
REDUCING AGENT: A reagent that reduces (adds electrons to) another species.
OXIDATION STATES: The number of electrons lost or gained from by an atom in a compound
compared to the uncombined atom.
HALF EQUATION: An equation which considers just one of the species involved and shows the
electrons transferred to or from it.
DISPROPORTIONATION: Where one atom is both oxidised and reduced. (Normally group 7)
SPECTATOR ION: Ions that are unchanged during a chemical reaction (take no part in it).
Balancing equations must be balanced for atoms and charge.
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To work out half equations, you need to know the elements that have been oxidised and
ATOM OXIDATION STATE
Metal ions (group 1, 2, 3) Ionic state +1, +2, +3
Hydrogen ions +1 (metal hydrides -1)
Fluoride ions -1
Oxygen ions -2 (except F and peroxides, -1)
Chloride ions -1 (except F or O
4 Point Rule
1. Balance for atoms other than O and H
2. Balance for O using HO
3. Balance for H using H