Oxidation

In-depth explanation of Oxidation

Oxidation is the loss of electrons by a species, which corresponds to an increase in its oxidation number. In a half-reaction electrons appear as products, so the oxidized species is the one that gives up electrons. Oxidation always occurs together with reduction, since the electrons released must be taken up by another species. At an electrochemical electrode, oxidation takes place at the anode. Recognizing oxidation is the first step in analyzing redox reactions in corrosion, combustion and biological electron transport.

Going deeper: Oxidation

Key ideas: Oxidation is loss of electrons, equivalent to an increase in oxidation number. Mnemonic OIL RIG. It also appears as gain of oxygen or loss of hydrogen in organic chemistry. In half-reactions, electrons appear on the product side: Fe2+ giving Fe3+ + e-.

Common mistakes and connections: Mistake: calling any reaction that involves oxygen an oxidation without checking oxidation numbers, or thinking oxidation can occur alone. It always couples with reduction, and electrons lost equal electrons gained. Oxidation takes place at the anode in both galvanic and electrolytic cells.

Visualization of Oxidation

Zinc is oxidized at the anode, Zn to Zn2+ + 2e-, sending electrons through the wire and raising its oxidation number from 0 to +2. The interactive lesson shows this as a live animation or chart.

Worked example and use case

Zinc metal is oxidized: Zn -> Zn2+ + 2e-, and its oxidation number rises from 0 to +2.

Where Oxidation fits in Acids, Bases & Electrochemistry

Oxidation is topic 36 of 105 in Acids, Bases & Electrochemistry.

Related topics

• Buffer CapacityAdvanced
• Blood Buffer SystemAdvanced
• Oxidation NumberBeginner
• ReductionBeginner
• Redox ReactionsBeginner
• Oxidizing AgentBeginner

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