Redox Reactions

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Chemistry revision on redox reactions for A-Level Chemistry.

Reduction and oxidation are terms used to describe

any reactions in which electrons are transferred.

A substance that is reduced

takes electrons from the substance that is oxidised.

A reaction in which both oxidation and reduction takes place is called a

redox reaction.

Oxidation is

the loss of electrons or an increase in oxidation number.

Reduction is

the gain of electrons or a decrease in oxidation number.

Half equations show

electron transfer, which element is oxidised and which is reduced.

Metals tend to be

oxidised.

Non-Metals tend to be

reduced.

The more electronegative element attracts more

electron(s) and is then reduced.

Oxidising Agent: is

a reagent that oxidises another species by taking electrons from it.

Reducing Agent is

a reagent that reduces another species by adding electrons to it.

Oxidising and reducing agents are always

the whole species (as the chemical appeared in the beginning of the equation).

A disproportionation reaction

is the oxidation and reduction of the same element in a redox reaction, such as Cl2 + H20 --> HCL + HOCl, with chlorine being oxidised and reduced.

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