Electrolysis of Lead (II) Bromide

  • Lead(II) bromide is a binary ionic compound meaning that it is a compound consisting of just two elements joined together by ionic bonding.
  • When these compounds are heated beyond their melting point, they become molten and can conduct electricity as their ions can move freely and carry the charge.
  • These compounds undergo electrolysis and always produce their corresponding element.
  • To predict the products of any binary molten compound first identify the ions present.
  • The positive ion will migrate towards the cathode and the negative ion will migrate towards the anode.
  • Therefore the cathode product will always be the metal and the product formed at the anode will always be the non-metal.

Electrolysis of Lead (II) Bromide

Electrolysis of Lead Bromide, IGCSE & GCSE Chemistry revision notes

Diagram Showing the Electrolysis of Lead (II) Bromide


  • Add lead(II) bromide into a crucible and heat so it will turn molten, allowing ions to be free to move and conduct an electric charge.
  • Add two graphite rods as the electrodes and connect this to a power pack or battery.
  • Turn on the power pack or battery and allow electrolysis to take place.
  • Negative bromide ions move to the positive electrode (anode) and lose two electrons to from bromine molecules. There is bubbling at the anode as brown bromine gas is given off.
  • Positive lead ions move to the negative electrode (cathode) and gain electrons to form grey lead metal which deposits on the surface of the electrode.

Electrode Products:
Anode: Bromine gas
Cathode: Solid lead metal

AQA GCSE Chemistry Notes

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Morgan Curtin Chemistry

Author: Morgan

Morgan’s passion for the Periodic Table begun on his 10th birthday when he received his first Chemistry set. After studying the subject at university he went on to become a fully fledged Chemistry teacher, and now works in an international school in Madrid! In his spare time he helps create our fantastic resources to help you ace your exams.