This key facts covers Key Facts to Memorise 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 8 of 13 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 8 of 13
Practice
20 questions
Recall
0 flashcards
📌 Key Facts to Memorise
- Solid ionic compounds DON'T conduct — ions are locked in fixed positions in the lattice and cannot move
- Molten ionic compounds DO conduct — ions are free to move and carry charge to the electrodes
- CATHODE (−): Attracts positive ions → cations GAIN electrons → METAL forms (this is REDUCTION)
- ANODE (+): Attracts negative ions → anions LOSE electrons → NON-METAL forms (this is OXIDATION)
- Molten = simple prediction: Only 2 types of ion present → metal at cathode, non-metal at anode
- PbBr₂ products: Lead metal at cathode (silvery), Bromine gas at anode (orange/brown)
- NaCl products: Sodium metal at cathode (silvery), Chlorine gas at anode (green/yellow)
- MgCl₂ products: Magnesium metal at cathode, Chlorine gas at anode
- Memory trick: CATions → CAThode; Reduction at Cathode (both have C); ANions → ANode
Quick Check: Why must an ionic compound be molten (or in solution) for electrolysis to work?
In the solid state, the ions are held in fixed positions in the ionic lattice by strong electrostatic forces — they cannot move. When molten, the lattice breaks down and the ions become free to move through the liquid towards the electrodes, allowing electrical charge to be carried and electrolysis to occur.