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

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Solution

The reaction between fluorine and water can be represented as:
$2 F_{2 (g)} + 2 H_{2} O_{(l)} ⟶ 4 H_{(a q)}^{+} + 4 F_{(a q)}^{-} + O_{2 (g)}$
This is an example of a redox reaction as water is getting oxidized to oxygen, while fluorine is being reduced to fluoride ion.
The oxidation numbers of various species can be represented as:

Fluorine is reduced from zero to (-1) oxidation state. A decrease in oxidation state indicates the reduction of fluorine.
Water is oxidized from (- 2) to zero oxidation state. An increase in oxidation state indicates
oxidation of water.

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Similar questions

F_{2} + 2 e^{-} \to 2 F^{-} (a q); E = + 2.87 V

C a^{+} + 2 e^{-} \to C a (s); E = - 2.76 V

Substance which is reduced is reducing agent ....if yes or no why ...

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F_{2} + 2 e^{-} \to 2 F^{-} (a q)

E^{o} = + 2.87 V

{C a}^{2 +} + 2 e^{-} \to C a (s)

E^{o} = - 2.76 V

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