Electrolysis — GCSE Chemistry Revision
Revise Electrolysis for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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
- Practice is aligned to major specifications (AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP).
- Free plan
- Sign up free to use tutor paths and feedback on your answers. Free access is 3 days uncapped, then 30 min practice/day. Pricing
- What makes it different
- Syllabus-shaped practice and progress tracking—not generic AI answers.
Topic has curated content entry with explanation, mistakes, and worked example. [auto-gate:promote; score=70.6]
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 SolutionsWhat 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 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
Jump into adaptive, exam-style questions for Electrolysis. Free to start; sign in to save progress.
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
Exam-style questions for Electrolysis with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
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 tutorFree full access to Electrolysis
Sign up in 30 seconds to unlock step-by-step explanations, exam-style practice, instant feedback and on-demand coaching — completely free, no card required.
Try a practice question
Unlock Electrolysis practice questions
Get instant feedback, step-by-step help and exam-style practice — free, no card needed.
Start Free — No Card NeededAlready have an account? Log in
Step-by-step method
Step-by-step explanation
4 steps · Worked method for Electrolysis
Core concept
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 …
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.