M2 Halogens F 2 > Cl 2 > Br 2 > I 2 Oxidising agent forces another substance to lose electrons, so it must gain electrons itself. This means that F 2 will become F - more readily than Cl 2 etc. See Module book for why Oxidising power of the Halogens

M2 Halogens Displacement reactions SpeciesColour Cl -, Br -, I - colourless Cl 2 pale yellow/green Br 2 yellow/brown I2I2 brown/black solid

M2 Halogens Br 2 + 2Cl -  no reaction Cl 2 + 2Br -  2Cl - + Br 2 pale green/yellow  yellow/brown Cl 2 + 2I -  2Cl - + I 2 pale green/yellow  brown/black solid Br 2 + 2I -  2Br - + I 2 yellow/brown  brown/black solid Displacement reactions

M2 Halogens I - > Br - > Cl - > F - This makes sense as it is the opposite to the oxidising ability of the halogens A reducing agent will force another substance to gain electrons, so it must lose electrons itself. Chlorine is unlikely to lose electrons, so it is a poor reducing agent. Reducing ability of the halide ions