GCSE Chemistry Revision — Electrolysis
Revise Electrolysis for GCSE Chemistry with a topic explanation, worked example and common mistakes. Check the board notes for specification differences.
At a glance
- What StudyVector is
- An exam-practice platform with board-aligned questions, explanations, and adaptive next steps.
- This topic
- Electrolysis in GCSE Chemistry: explanation, examples, and practice links on this page.
- Who it’s for
- Students revising GCSE Chemistry for UK exams.
- Exam boards
- Check your course page and the topic board notes for supported specifications.
- Free plan
- Sign up free to use tutor paths and feedback on your answers. Free access is Free daily revision · No card required. Pricing
- What makes it different
- Syllabus-shaped practice and progress tracking—not generic AI answers.
This page includes a topic explanation and a worked example. Check your course for current practice coverage.
Next in this topic area
Next step: Electrolysis of Aqueous Solutions
Continue in the same course — structured practice and explanations on StudyVector.
Go to Electrolysis of Aqueous SolutionsTopic explanation
What is Electrolysis?
Electrolysis is the process of breaking down an ionic compound, either molten or in solution, by passing an electric current through it. The substance being broken down is called the electrolyte. The current is passed through via two electrodes: a positive one called the anode, and a negative one called the cathode.
Board notes: Electrolysis is a major topic for all exam boards. You must understand the basic setup, the terminology (electrolyte, electrode, anode, cathode), and be able to predict the products of the electrolysis of simple molten ionic compounds. The electrolysis of aqueous solutions is a more advanced, higher-tier topic.
Step-by-step explanationWorked examples
Worked example
In the electrolysis of molten lead(II) bromide (PbBr₂), the lead ions (Pb²⁺) are attracted to the negative cathode, where they gain two electrons to become lead atoms (Pb). The bromide ions (Br⁻) are attracted to the positive anode, where they each lose one electron to become bromine atoms, which then pair up to form bromine molecules (Br₂).
Practise this topic
Start with low-focus cards for Electrolysis, then move into full exam-style practice when you want the heavier session.
Common mistakes
- 1Confusing the anode and cathode. A useful mnemonic is PANIC: Positive Anode, Negative Is Cathode.
- 2Forgetting that the electrolyte must be molten or in solution for the ions to be free to move and conduct electricity.
- 3Not being able to predict the products of electrolysis. Remember that positive ions (cations) move to the cathode and negative ions (anions) move to the anode.
Electrolysis exam questions
Check the available question sets for Electrolysis. Use your course and exam board to confirm which practice is relevant.
Electrolysis exam questionsGet help with Electrolysis
Get a personalised explanation for Electrolysis from the StudyVector tutor. Ask follow-up questions and work through problems with step-by-step support.
Open tutorSave your progress in Electrolysis
Start a free account for low-focus question cards, feedback and Play routes across available topics. Free daily limits apply; no card required.
Continue your revision
A public question for Electrolysis is still being reviewed. Your course page shows the topics currently available for practice.
Continue with Electrolysis
Create a free account to keep your course choice and save your practice progress.
Start free low-focus cardsAlready have an account? Log in
Frequently asked questions
What happens at the cathode?
At the cathode (negative electrode), positive ions gain electrons. This process is called reduction.
What happens at the anode?
At the anode (positive electrode), negative ions lose electrons. This process is called oxidation.