Which ionic equation shows a reaction that actually takes place, with the species oxidised or reduced correctly identified?
I2+2Br−→2I−+Br2\mathrm{I_{2} + 2Br^{-} \rightarrow 2I^{-} + Br_{2}}I2+2Br−→2I−+Br2; bromide ions are oxidised
Cl2+2I−→2Cl−+I2\mathrm{Cl_{2} + 2I^{-} \rightarrow 2Cl^{-} + I_{2}}Cl2+2I−→2Cl−+I2; chlorine molecules are oxidised
Br2+2I−→2Br−+I2\mathrm{Br_{2} + 2I^{-} \rightarrow 2Br^{-} + I_{2}}Br2+2I−→2Br−+I2; iodide ions are oxidised
Br2+2Cl−→2Br−+Cl2\mathrm{Br_{2} + 2Cl^{-} \rightarrow 2Br^{-} + Cl_{2}}Br2+2Cl−→2Br−+Cl2; bromine molecules are reduced
41 exam-style questions on Edexcel GCSE Chemistry 7.2 Group 7, covering 7.2.1 Physical properties of the halogens, 7.2.2 Reactions of the halogens, 7.2.3 Relative reactivity and displacement reactions of the halogens, and 7.2.4 Halogen displacement as a redox reaction. Each one has a worked solution and a mark scheme showing where the marks go.