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14 Cards in this Set

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  • Back

Define 'Oxidation'

The loss of electrons, resulting in an increase of oxidation state

Define 'Reduction'

The gain of electrons, resulting in a decrease of oxidation state

What is a 'Reducing agent'?

A species that reduces another species by donating one or more electrons, thus being itself oxidised.

What is an 'Oxidising agent'?

A species that oxidises another species by removing one or more electrons, thus being itself reduced.

Define 'species'

An atom, molecule or ion

An example of a redox equation is where Mg burns in oxygen:

2Mg + O2 ----> 2MgO

Write reductive and oxidative half equations for this reaction

Oxidative: Mg -----> Mg2+ +2e-

Reductive: O2 + 4e- ----> 2O2-

What are the typical oxidation numbers of Oxygen and Hydrogen?

Oxygen -2

Hydrogen +1

Exceptions: Oxygen is -1 in peroxides

Hydrogen is -1 when combined with a less electronegative element e.g in KH

What is the oxidation number of H2

0 as it is in its elemental form

The sum of all the oxidation numbers in a neutral compound is...?


What is the oxidation number of nitrogen in the following:




-3 in NH3

+3 in (NO2)-

+5 in (NO3)-

Deduce the formula for Iron (III) Sulphate

Fe is 3+, SO4 is 2-

To give a neutral compound they must be in a 2:3 ratio


Most chlorine based bleaches contain the ClO- ion.

State the oxidation state of Cl in this compound and give its systematic name

Cl is +1

Chlorate (1)

Fe (s) -----> Fe2+ (aq) + 2e-

O2 (aq) + 2H2O (l) + 4e- -----> 4OH- (aq)

2Fe (s) + O2 (aq) + 2H2O (l) -----> 4OH- (aq) + 2Fe2+ (aq)

What is the change in oxidation number of Chlorine is this reaction?

KClO3 (S) ------> KCl (s) + 1.5O2 (g)

From +5 to -1