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Oxidation and Reduction (Redox)

Key Concepts

Oxidation: loss of electrons
Reduction: gain of electrons
Oxidant (oxidising agent): causes another species to be oxidised
Oxidant: gains electrons (oxidant is reduced)
Reductant (Reducing Agent): causes another species to be reduced
Reductant: loses electrons (reductant is oxidised)
Redox Reactions: one species (reductant) provides electrons for another species (oxidant).

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Examples

Oxidation : Na -----> Na⁺ + e

Sodium atom loses an electron to produce a positively charged sodium ion (cation)
Sodium has been oxidised.

Reduction : F + e -----> F^-

Fluorine atom gains an electron to form the negatively charged fluoride ion (anion)
Fluorine has been reduced.

REDOX (electron transfer) Reaction : Na + F -----> Na⁺ + F^-

An electron has been transferred from the sodium atom to the flourine atom.
Sodium has lost an electron, it has been oxidised
Sodium is the reductant as it has caused the fluorine to be reduced to the fluoride ion.
Fluorine has gained an electron, it has been reduced.
Fluorine is the oxidant as it has caused the sodium to be oxidised to the sodium ion.

Uses of REDOX Reactions

Generation of electricity (galvanic cells)
Recharging rechargable batteries
Electrolytic extraction of metals (aluminium, sodium)
Electroplating
Quantitative analysis (REDOX titrations)

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