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ElectrolysisDefinitions

Key Definitions

Part of Electrolysis of Molten Compounds — GCSE Chemistry

This definitions covers Key Definitions within Electrolysis of Molten Compounds for GCSE Chemistry. Revise Electrolysis of Molten Compounds in Electrolysis for GCSE Chemistry with 20 exam-style questions and 0 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 5 of 11 in this topic. Make sure you can use the exact wording confidently, because definition marks are often lost through vague language.

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Section 5 of 11

Practice

20 questions

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📖 Key Definitions

Electrolysis: The decomposition of an ionic compound (when molten or in solution) by passing electricity through it. Electrical energy is used to break down the compound into its elements.

Molten: Melted — a solid that has been heated until it becomes liquid. Molten ionic compounds can conduct electricity because the ions are free to move.

Reduction: Gain of electrons. Occurs at the cathode during electrolysis. Cations gain electrons and become neutral atoms.

Oxidation: Loss of electrons. Occurs at the anode during electrolysis. Anions lose electrons and become neutral atoms or molecules.

Half equation: An equation showing what happens at one electrode during electrolysis, including the electrons gained or lost. E.g., Pb²⁺ + 2e⁻ → Pb

Electrostatic attraction: The force of attraction between oppositely charged particles (e.g., positive cations attracted to negative cathode).

Keep building this topic

Read this section alongside the surrounding pages in Electrolysis of Molten Compounds. That gives you the full topic sequence instead of a single isolated revision point.

Example: Electrolysis of Molten Lead Bromide (PbBr₂)Key Facts to MemoriseBreaking Free — The Prison Break of IonsElectrolysis Cell

Practice Questions for Electrolysis of Molten Compounds

Which condition is required for electrolysis to occur with an ionic compound?

  • A. The ions must be free to move (molten or in solution)
  • B. The compound must be dissolved in organic solvent
  • C. The compound must be heated above 1000 °C
  • D. The compound must contain metallic bonds
1 markfoundation

State the products formed at each electrode when molten lead bromide (PbBr₂) is electrolysed.

2 marksstandard

Quick Recall Flashcards

How do you remember that cations go to the cathode?
CATions → CAThode (both start with CAT) ANions → ANode (both start with AN) Metal at the Minus (cathode is negative), Non-metal at the Plus (anode is positive).
Why does solid lead bromide NOT conduct electricity?
In the solid state, all ions (Pb²⁺ and Br⁻) are held in fixed positions in the ionic lattice by strong electrostatic forces. They cannot move, so they cannot carry electrical charge.

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Example: Electrolysis of Molten Lead Bromide (PbBr₂)

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Key Facts to Memorise