Which of the following is the best description of the behaviour of bromine in the reaction given below?
$H_{2} O + {B r}_{2} ⟶ H O B r + H B r$

Proton acceptor only

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Both oxidised and reduced

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Oxidised only

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Reduced only

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Solution

The correct option is C Both oxidised and reduced
In the reaction
$H_{2} O + {B r}_{2} ⟶ H O B r + H B r$
Both oxidised and reduced.
The oxidation number of bromine changes from 0 (in $B r_{2}$ ) to +1 (in HOBr). Thus, bromine is oxidized.
The oxidation number of bromine changes from 0 (in $B r_{2}$ ) to -1 (in HBr). Hence, bromine is reduced.

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