Oxidizing Agent - Example of Oxidation

Example of Oxidation

The formation of iron(III) oxide;

4Fe + 3O₂ → 2Fe₂O₃

In the above equation, the iron (Fe) has an oxidation number of 0 before and 3+ after the reaction. For oxygen (O) the oxidation number began as 0 and decreased to 2−. These changes can be viewed as two "half-reactions" that occur concurrently:

1. Oxidation half reaction: Fe0 → Fe3+ + 3e−
2. Reduction half reaction: O₂ + 4e− → 2 O2−

Iron (Fe) has become oxidized because its oxidation number increased and was the reducing agent because it gave electrons to the oxygen (O). Oxygen (O) has been reduced because the oxidation number has decreased and was the oxidizing agent because it took electrons from iron (Fe).