Electrolysis of Molten Compounds (CIE IGCSE Chemistry)

• A binary ionic compound is one consisting of just two elements joined together by ionic bonding
• When these compounds undergo electrolysis they always produce their corresponding elements 
• To predict the products made at each electrode, first identify the ions 
• 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

Example: Electrolysis of molten lead(II) bromide  

Method:

• Add lead(II) bromide into a beaker and heat it 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 each loses one electron 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 a grey lead metal which deposits on the surface of the electrode

Diagram showing the electrolysis of lead(II) bromide

Answer:

• • The ions present are potassium (K⁺) and chloride (Cl^-)
  • The chloride ions are attracted to the anode and form chlorine gas
  • The potassium ions are attracted to the cathode and form potassium metal