GCSE Chemistry Revision — Reactivity Series
Revise Reactivity Series for GCSE Chemistry with a topic explanation, worked example and common mistakes. Check the board notes for specification differences.
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What is Reactivity Series?
The reactivity series is a list of metals arranged in order of their reactivity, from most reactive to least reactive. A metal's position in the series determines how readily it loses electrons to form positive ions. A more reactive metal can displace a less reactive metal from its compound.
Board notes: The reactivity series is a key concept for all exam boards. You need to know the order of reactivity for common metals and be able to predict the products of displacement reactions. Its link to metal extraction is also very important.
Step-by-step explanationWorked examples
Worked example
If you place a piece of iron in a solution of copper(II) sulfate, the iron is more reactive than the copper. The iron will displace the copper, forming iron(II) sulfate and solid copper: Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s).
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Common mistakes
- 1Memorising the series in the wrong order. A common mnemonic is 'Please Stop Calling Me A Cute Zebra, I Like Her Call, Smart Guy!' (Potassium, Sodium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Lead, Hydrogen, Copper, Silver, Gold).
- 2Forgetting that carbon and hydrogen are included in the series for comparison, even though they are non-metals.
- 3Confusing displacement reactions with other reaction types. A displacement reaction is specifically when a more reactive element takes the place of a less reactive element in a compound.
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Frequently asked questions
How can you determine the reactivity of two metals?
You can react each metal with water, acid, or a solution containing the ions of the other metal. The metal that reacts more vigorously or displaces the other is the more reactive one.
What is the connection between reactivity and extraction?
The position of a metal in the reactivity series determines how it is extracted from its ore. Metals more reactive than carbon must be extracted by electrolysis, while less reactive metals can be extracted by reduction with carbon.