Reducing Agent - Example of Redox Reaction

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:

1. Oxidation half reaction: Fe0 → Fe3+ + 3e−
2. 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).