Oxidation & Reduction in Terms of Electrons (AQA GCSE Chemistry: Combined Science)

Revision Note

Stewart

Author

Stewart

Last updated

Did this video help you?

Oxidation & reduction in terms of electrons

Higher tier only

  • 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+ + SO42– → Fe2+ + SO42– + Cu

  • The sulfate ions, SO42-, appear on both sides of the equation unchanged
    • This means that they are spectator ions and do not participate in the chemistry of the reaction
    • So, they can be removed from the equation

Fe + Cu2+→ Fe2+ + Cu

  • This balanced ionic equation can be further split into two half equations illustrating oxidation and reduction individually

Fe → Fe2+ + 2e

Cu2+ + 2e→ 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+

oxidation-and-reduction-electrons

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

Examiner Tip

Remember: OIL RIGOxidation ILoss, Reduction IGain of electrons

Worked example

Which change in the following equation is oxidation?

V3+ + Fe3+  → V4+ + Fe2+

Answer:

  • Step 1 - Identify the changes for each species
    • V3+ to V4+ 
      • V3+ has lost 1 electron 
    • Fe3+ to Fe2+
      • Fe3+ has gained 1 electron
  • Step 2 Identify each change as either oxidation and reduction
    • V3+ to V4+ is oxidation
    • Fe3+ to Fe2+ is reduction
    • Therefore, V3+ has been oxidised

Identifying oxidised & reduced species

Higher tier only

  • Using the principles of electron loss and gain it is possible to identify which species undergo oxidation and reduction in redox reactions

Worked example

Zinc displaces copper from a solution of copper(II)sulfate. Using ionic equations, determine which species undergoes oxidation and which species undergoes reduction.

Answer

  1. Write the full equation
    • Zn (s) + CuSO4 (aq) → ZnSO4 (aq) + Cu (s)
  2. Write the ionic equation
    • Zn (s) + Cu2+ (aq) + SO subscript 4 superscript 2 minus end superscript (aq) → Zn2+ (aq) + SO subscript 4 superscript 2 minus end superscript (aq) + Cu (s)
  3. Use the ionic equation to rule out / ignore spectator ions that are present as reactants and products
    • SO subscript 4 superscript 2 minus end superscript is present as a reactant and a product so it can be ignored
  4. Use the ionic equation to identify the species that is oxidised (OIL)
    • Zn (s) → Zn2+ (aq) + 2e 
  5. Use the ionic equation to identify the species that is reduced (RIG)
    • Cu2+ (aq) + 2e → Cu (s)

Examiner Tip

After writing half equations, you can see if they are correct by checking that the number of electrons on either side is the same, which should combine to give 0 charge.

You've read 0 of your 5 free revision notes this week

Sign up now. It’s free!

Join the 100,000+ Students that ❤️ Save My Exams

the (exam) results speak for themselves:

Did this page help you?

Stewart

Author: Stewart

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Exam Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.