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Electrolysis of Molten Ionic Compounds | Chemistry for Grade 10 PDF Download

Electrolysis of Simple Ionic Compounds

  • 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

Diagram showing the electrolysis of lead (II) bromideDiagram showing the electrolysis of lead (II) bromide

Method

  • 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 form 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 bottom of the electrode

Electrode Products:
Anode: Bromine gas
Cathode: Lead metal

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