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\subsubsection{Reactions of halogens with halide ions}  Halogens undergo displacement reactions when reacted with a less reactive halide. This can be shown using full, and ionic equations:  \begin{align*}  Cl_2+2KI\Rightarrow 2KCl + I_2 & &&  \text{Full equation, with state symbols omitted}\\ Cl_2 + 2I^- \Rightarrow 2Cl_- +I_2 & &&  \text{Ionic equation, with state symbols omitted} \end{align*] \end{align*}  Ions not involved are spectator ions. The halogen is an oxidising agent, and is said to have been reduced. For the above reactions, this is shown by the half-equations:  \begin{align*}  Cl_2 + 2e^-\Rightarrow 2Cl^- & &&  \text{Reduction of chlorine}\\ 2I^- \Rightarrow I_2 + 2e^- & &&  \text{Oxidation of iodide} \end{align*}  This is a redox reaction as both reduction and oxidation have occured. Fluorine is the strongest oxidising agent, and will displace any other halogen, whilst iodine is unable to displace any. As the colour changes are difficult to dtect, it is easier to add an organic solvent.