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Which of the following is the best description for the behavior of bromine in the reaction given below?
$H_{2} O + {Br}_{2} \to HOBr + HBr$

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Proton acceptor only

Both oxidized and reduced

Oxidized only

Reduced only

answer is B.

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Detailed Solution

Oxidation state of Br in Br₂ is zero, the oxidation state of Br in HOBr is +1 and in HBr is -1.

$H_{2} O + \overset{0}{{Br}_{2}} ⟶ \overset{+ 1}{HOBr} + \overset{- 1}{HBr}$

In the above reaction, Br is oxidized from 0 to +1 and reduced from 0 to -1. This concludes that Br is reduced as well as oxidized in the above reaction.

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