Describe competing reactions in the electrolysis of aqueous solutions of ionic compounds in terms of the different ionic species present.
Explain how the relative reactivity of the elements involved dictates which ions are discharged at the electrodes in an aqueous solution.
Recall that at the negative electrode (cathode), hydrogen gas is produced if the metal in the compound is more reactive than hydrogen.
Recall that at the positive electrode (anode), oxygen gas is produced unless the solution contains halide ions, in which case the corresponding halogen is produced.
Understand that aqueous solutions contain hydrogen and hydroxide ions from the breakdown of water molecules, which compete during electrolysis.
Investigate what happens when different aqueous solutions are electrolysed using inert electrodes, involving the development of a hypothesis.
Write half equations for the specific reactions occurring at the electrodes in aqueous electrolysis (Higher Tier only).
