Oxidation & Reduction Using Electrons (WJEC GCSE Science (Double Award)): Revision Note

Oxidation & Reduction Using Electrons

• As well as understanding oxidation and reduction in terms of oxygen, you need to understand these reactions in terms of electrons

• When a substance loses electrons it is oxidised

• When a substance gains electrons it is reduced

• If this occurs in the same reaction, the reaction is a redox reaction

• For example, when iron reacts with a compound of copper such as copper sulfate a displacement reaction occurs

iron + copper sulfate → iron(II) sulfate + copper 

Fe + CuSO₄ → FeSO₄ + Cu

• We can write this as an ionic equation

Fe + Cu²⁺ + SO₄^2– → Fe²⁺ + SO₄^2– + Cu

• We can then remove the spectator ions to see the overall change

Fe + Cu²⁺→ Fe²⁺ + Cu

• The iron has lost electrons to become a positive ion, so has been oxidised

• The positive copper ion has gained electrons to become an atom, so have been reduced

The redox reaction between Fe and Cu²⁺

The Fe atom is oxidised (loses electrons) and the Cu²⁺ ion is reduced (gains electrons)

Electrolysis

• Oxidation and reduction take place during the process of electrolysis at the anode (positive electrode) and the cathode (negative electrode) 

• Positive ions are attracted towards the cathode

  • Reduction (gain of electrons) takes place here

  • E.g. Pb²⁺ + 2e^– → Pb

• Negative ions are attracted towards the anode

  • Oxidation (loss of electrons) takes place here

  • E.g. 2Br^– → Br₂ + 2e^–