Halogens, elemental oxidation

The standard reduction potentials for the main species formed by the Group 17 elements in aqueous solution are given in Tables 6.16 and 6.17, for pH values 0 and 14, respectively. Irrespective of the pH of the solution, the halogen elements range from the extremely powerful F2 (which has the potential to oxidize water to dioxygen), through the powerful oxidants Cl2 and Br2, to 12, which is a relatively weak oxidant. 

Lithium Arsenide, Li3As, is formed when a mixture of the elements in suitable proportions is heated to redness, or when lithium arsenate is reduced by heating with charcoal in an electric furnace.8 It is a dark brown crystalline substance of great reactivity. It is attacked by the halogen elements at the ordinary temperature with incandescence. It burns vividly when heated in oxygen it reacts violently with nitric acid, and at a comparatively low temperature it reduces many metallic oxides. 

Cl, oxidizes iodide to yield chloride ions and iodine. With the halogens, fluorine is the most powerful oxidizing agent, and each element going down the group becomes less powerful. As a result, a halogen can oxidize the halogens below it in a replacement reaction. 

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