Which is the best description of the behaviour of bromine in the reaction given below
`H_(2)O+Br_(2) rarr HOBr+HBr`

Options

A. Proton acceptor only
B. Both oxidised and reduced
C. Oxidised only
D. Reduced only

Explanation

To analyze the behavior of bromine (Br) in the reaction \( H_2O + Br_2 \rightarrow HOBr + HBr \), we need to follow these steps:

### Step 1: Identify the oxidation states
First, we need to determine the oxidation states of bromine in the reactants and products.

- In \( Br_2 \) (bromine molecule), the oxidation state of bromine is 0.
- In \( HOBr \) (hypobromous acid), the oxidation state of bromine is +1.
- In \( HBr \) (hydrobromic acid), the oxidation state of bromine is -1.

### Step 2: Analyze the changes in oxidation states
Now, we can analyze how the oxidation state of bromine changes during the reaction:

- Bromine in \( Br_2 \) (0) is oxidized to \( HOBr \) (+1).
- Bromine in \( Br_2 \) (0) is reduced to \( HBr \) (-1).

### Step 3: Determine the behavior of bromine
Since bromine undergoes both oxidation (to +1) and reduction (to -1) in this reaction, we can conclude that bromine acts as both an oxidizing agent and a reducing agent.

### Conclusion
Thus, the best description of the behavior of bromine in the given reaction is that it is both oxidized and reduced.

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