This comparison covers Example: Electrolysis of Molten Lead Bromide (PbBr₂) within Electrolysis of Molten Compounds for GCSE Chemistry. Revise Electrolysis of Molten Compounds in Electrolysis for GCSE Chemistry with 21 exam-style questions and 14 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 4 of 11 in this topic. Use this comparison to connect the idea to the wider topic before moving on to questions and flashcards.

🔬 Example: Electrolysis of Molten Lead Bromide (PbBr₂)

Electrode	Ion arriving	Half equation	Product observed
CATHODE (−)	Pb²⁺ gains 2 electrons (reduction)	`Pb²⁺ + 2e⁻ → Pb`	Lead metal — silvery liquid, sinks to bottom
ANODE (+)	Br⁻ loses electrons (oxidation)	`2Br⁻ → Br₂ + 2e⁻`	Bromine gas — orange/brown fumes

Overall equation: PbBr₂ → Pb + Br₂

The compound is broken down into its elements using electrical energy.

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

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.

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).

Example: Electrolysis of Molten Lead Bromide (PbBr₂)