Transition Metals - Redox Reactions Revisited (A-Level Chemistry)

Redox Reactions Revisited

Redox Reactions

Key Terms

An oxidation reaction is the process of electron loss.

A reduction reaction is the process of electron gain.

An oxidising agent gets reduced by accepting electrons

A reducing agent gets oxidised as it gives up electrons.

Oxidation Numbers

The oxidation state (or number) of an element represents the total number of electrons that the element has either accepted by an element (negative oxidation number) or removed from an element (positive oxidation number), to get to its current form. It shows us the degree of oxidation of an atom or ion in a compound.

Oxidation involves an increase in oxidation state

Reduction involves a decrease in oxidation state

Half-equations to Form Redox Equations

In a redox reaction, a reduction and an oxidation happen simultaneously. We can divide the reaction into two separate equations, one showing oxidation and the other showing reduction. These are called half-equations.

In previous tutorial we have learnt how to form an overall redox equation by combining two half-equations.

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