Consider the reaction of water with $F_{2}$ and suggest,in terms of oxidation and reduction,which species are oxidized and which are reduced.

(N/A) The reaction between fluorine and water is represented as:
$2F_{2(g)} + 2H_{2}O_{(l)} \to 4H_{(aq)}^{+} + 4F_{(aq)}^{-} + O_{2(g)}$
In this reaction,the oxidation states change as follows:
$F_{2}$ (oxidation state $0$) is reduced to $F^{-}$ (oxidation state $-1$). Since the oxidation state decreases,$F_{2}$ is reduced.
$H_{2}O$ (oxygen oxidation state $-2$) is oxidized to $O_{2}$ (oxidation state $0$). Since the oxidation state increases,water is oxidized.
Thus,$F_{2}$ acts as the oxidizing agent and is reduced,while $H_{2}O$ acts as the reducing agent and is oxidized.