Example of Redox Reaction
The formation of iron(III) oxide;
- 4Fe + 3O2 → 2Fe23+O36-
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:
- Oxidation half reaction: Fe0 → Fe3+ + 3e−
- Reduction half reaction: O2 + 4e− → 2 O2−
Iron (Fe) has been oxidized because the oxidation number increased. Iron is the reducing agent because it gave electrons to the oxygen (O2). Oxygen (O2) has been reduced because the oxidation number has decreased and is the oxidizing agent because it took electrons from iron (Fe).
Read more about this topic: Reducing Agent
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