Which is the best description of behaviour of bromine in the reaction given below?

\(H_2O  + Br_2 \longrightarrow HBr + HOBr\)

Both oxidized and reduced

The correct answer is option 2. Both oxidized and reduced.

In the given reaction:

\[ H_2O + Br_2 \longrightarrow HBr + HOBr \]

Bromine undergoes both oxidation and reduction. Let's break it down:

Oxidation: Bromine (\(Br_2\)) goes from an oxidation state of 0 to -1 in \(HOBr\). Therefore, bromine is oxidized.

Reduction: Bromine (\(Br_2\)) gains electrons to form \(HBr\), where bromine is in the -1 oxidation state. Therefore, bromine is reduced.

So, the best description of the behavior of bromine in this reaction is: 2. Both oxidized and reduced