GCSE Chemistry Revision — Cells & Batteries
Revise Cells & Batteries 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 Cells & Batteries?
A simple electrochemical cell, or battery, consists of two different metals connected by a wire and dipped in an electrolyte. The difference in reactivity between the two metals creates a potential difference (voltage) that drives a flow of electrons from the more reactive metal to the less reactive metal. A battery is simply two or more cells connected in series.
Board notes: Cells and batteries are covered by all exam boards, often in the context of the reactivity series and electrochemistry. You should be able to explain how a simple cell works, predict the direction of electron flow, and understand the factors affecting the voltage produced.
Step-by-step explanationWorked examples
Worked example
A simple cell can be made with a zinc electrode and a copper electrode in a solution of sulfuric acid. Zinc is more reactive than copper, so it loses electrons more readily (Zn → Zn²⁺ + 2e⁻). These electrons flow through the wire to the copper electrode, where they are taken by hydrogen ions from the acid (2H⁺ + 2e⁻ → H₂).
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Common mistakes
- 1Confusing a cell with a battery. A battery is technically a collection of cells, although the terms are often used interchangeably.
- 2Forgetting that the voltage produced depends on the difference in reactivity of the metals. The further apart the metals are in the reactivity series, the higher the voltage.
- 3Not understanding the direction of electron flow. Electrons always flow from the more reactive metal (which is oxidised) to the less reactive metal (where reduction occurs).
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Frequently asked questions
What is an electrolyte?
An electrolyte is a solution, usually an ionic solution, that can conduct electricity. It contains mobile ions that can move to the electrodes to complete the electrical circuit.
What is the difference between rechargeable and non-rechargeable batteries?
In non-rechargeable batteries, the chemical reactions are irreversible. Once the reactants are used up, the battery is dead. In rechargeable batteries, the reactions can be reversed by applying an external current, regenerating the original reactants.