Oxidation, Reduction & Redox — GCSE Chemistry Revision
Revise Oxidation, Reduction & Redox for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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Go to Acids & AlkalisWhat is Oxidation, Reduction & Redox?
Oxidation and reduction are chemical processes that always happen together, which is why they are often called redox reactions. Oxidation is the loss of electrons, gain of oxygen, or loss of hydrogen. Reduction is the gain of electrons, loss of oxygen, or gain of hydrogen.
Board notes: Redox is a fundamental concept, particularly for higher-tier students. All boards expect you to be able to define oxidation and reduction in terms of oxygen transfer. For higher tiers, you must also use the concept of electron transfer and be able to write and interpret half-equations.
Step-by-step explanationWorked example
In the reaction Zn + CuSO₄ → ZnSO₄ + Cu, the zinc atom loses two electrons to become a Zn²⁺ ion (oxidation). The Cu²⁺ ion in copper sulfate gains two electrons to become a copper atom (reduction). Zinc is the reducing agent, and the Cu²⁺ ion is the oxidising agent.
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Common mistakes
- 1Forgetting the OILRIG mnemonic: Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons).
- 2Confusing the oxidising agent and the reducing agent. The substance that gets oxidised is the reducing agent, and the substance that gets reduced is the oxidising agent.
- 3Not being able to identify what has been oxidised and what has been reduced in a given reaction, especially in terms of electron transfer.
Oxidation, Reduction & Redox exam questions
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Oxidation, Reduction & Redox
Core concept
Oxidation and reduction are chemical processes that always happen together, which is why they are often called redox reactions. Oxidation is the loss of electrons, gain of oxygen, or loss of hydrogen.…
Frequently asked questions
What is a half-equation?
A half-equation shows either the oxidation or the reduction part of a redox reaction, including the electrons that are lost or gained. For example, Zn → Zn²⁺ + 2e⁻ is an oxidation half-equation.
Can a reaction be just oxidation or just reduction?
No, if one substance loses electrons, another substance must gain them. Oxidation and reduction always occur simultaneously in a redox reaction.