GCSE · Chemistry · AQA · Spec 8462

Cells and batteries (chem only)

A battery is not one mysterious box: it is chemistry arranged so reactions can push electricity around a circuit.

Build a simple chemical cell

Choose the setup that matches the minimum ingredients in the lesson.

Which arrangement can make a simple chemical cell?

Relationship matrix

Tap any cell to reveal it. Tap a column header to read one property down every item.

What to rememberHow to use it
Electrode pairtwo different metals
Electrolytein contact with both electrodes
Cells in seriestwo or more cells
Reactivity dataevidence supplied in a question

Each cell hides a short answer and the reason behind it. Predict before you tap.

Process · Closed loop

Why a rechargeable cell can be used again

Charging reverses the chemical reactions so the cell can go through another discharge cycle.

1Discharge2Reactants change3External current4Reaction reversed

Stage 01

Discharge

Chemical reactions in the cell produce electricity.

Watch out: This loop describes rechargeable cells. In a non-rechargeable cell, the reaction stops when a reactant is used up.

Core cell and battery terms

Say the meaning before revealing it.

From one cell to a battery

Follow what changes as you move from a single simple cell to several cells in series.

CHEMISTRY · CELLS

Cells and batteries

Two different metals and an electrolyte can turn chemical reactions into electrical energy.

What you need to know

  • A simple cell can be made from two different metals in contact with an electrolyte.
  • The voltage of a cell depends on factors including the electrode materials and the electrolyte.
  • A battery has two or more cells connected in series to provide a greater voltage.
  • Non-rechargeable cells stop when a reactant is used up; alkaline batteries are non-rechargeable.
  • Rechargeable cells can be recharged because an external current reverses the chemical reactions.
  • Use supplied data to compare relative reactivity, voltage and suitability rather than guessing.

The big picture

Chemical cells contain chemicals that react to produce electricity. A simple cell uses two different metal electrodes in contact with an electrolyte, and the voltage depends on factors including the electrode materials and the electrolyte. A battery contains two or more cells connected in series to provide a greater voltage. Non-rechargeable cells stop when a reactant is used up; rechargeable cells can be charged because an external current reverses the reactions.

Key points

1Chemical reactions in a cell produce electricity.
2Two different metals plus an electrolyte make the basic simple-cell setup.
3Electrode choice and electrolyte can affect the voltage produced.
4Connecting cells in series makes a battery with a greater voltage.
5Rechargeable cells rely on reactions that can be reversed by an external current.
6Evaluation should use the evidence provided, including reactivity, voltage and whether recharging is needed.

Worked example

Problem

A device needs a greater voltage than one cell provides and will be used repeatedly. What two design ideas should you consider?

🧠

Memory hook

CELL: Chemicals Energise through two Linked metals in an eLectrolyte; a battery links cells in series.

★ Exam tip

When data are supplied, quote the evidence you are using. Separate metal reactivity, measured voltage and rechargeability instead of treating them as the same property.

⚠ Watch out

Calling a battery a single cell. A battery is two or more cells connected together in series.

✓

Check yourself

What two parts make a simple cell, what can change its voltage, and why can a rechargeable cell be charged again?

Flashcards

(20)
What do chemical cells contain?
Chemicals that react to produce electricity.
What is needed to make a simple cell?
Two different metals in contact with an electrolyte.
Why must the two electrodes in the simple-cell setup be different metals?
The specified simple-cell setup uses two different metals in contact with an electrolyte.
What is an electrode in this topic?
One of the conducting materials in contact with the electrolyte.
What is an electrolyte?
The material in contact with both electrodes; its type can affect the cell voltage.
Name two factors that affect cell voltage.
The type of electrode and the type of electrolyte.
What is a battery?
Two or more cells connected together in series.
Why are cells connected in series in a battery?
To provide a greater voltage.
What eventually stops a non-rechargeable cell?
One of the reactants is used up, so the chemical reactions stop.
Are alkaline batteries rechargeable in this topic?
No. Alkaline batteries are non-rechargeable.
Why can a rechargeable cell be recharged?
An external electrical current reverses the chemical reactions.
What is supplied to a rechargeable cell during charging?
An external electrical current.
Does the word “battery” automatically mean rechargeable?
No. Batteries can be rechargeable or non-rechargeable.
What does relative reactivity data allow you to do?
Compare or rank the metals by how reactive they are, using the supplied data.
If data say X > Y > Z in reactivity, which is most reactive?
X.
Should you infer a cell voltage from reactivity data alone?
No. Use the voltage evidence provided, because voltage depends on factors including electrodes and electrolyte.
What evidence can help evaluate a cell or battery?
Data such as voltage, electrode/electrolyte choice, relative reactivity and whether it can be recharged.
What happens to the reactions while a rechargeable cell is discharged?
They proceed in the direction that produces electricity.
What happens to those reactions during charging?
They are reversed by the supplied external current.
How can a battery provide more voltage than one cell?
By connecting two or more cells together in series.

Tap any card to flip it, or use Study as deck to go through them one at a time. In the full lesson these run as a spaced-repetition deck — you rate each card Hard, Good or Easy and the tricky ones keep coming back until they stick.

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How this lesson was checked. This AQA GCSE Chemistry (specification 8462)lesson was published through Lightbulb Learning's human-designed editorial process — the educational standards, accuracy rules and publication checks it must pass were authored and approved by Philip Halpin. It passed subject-specific assessment, automated educational checks and technical publication verification before going live (publication checks completed 29 August 2026). Published pages are monitored, human spot-checking is ongoing across the lesson library, and anything found wrong is corrected or withdrawn. How our lessons are made and checked. Spotted a mistake? Email hello@lightbulblearning.co and we'll review it.