Which of the following is the best description of the behaviour of bromine in the reaction given below?
H 2 ​ O+Br 2 ​ ⟶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 (Br₂) in the reaction with water (H₂O), we can follow these steps:

### Step 1: Write the Reaction
The given reaction is:
\[ \text{H}_2\text{O} + \text{Br}_2 \rightarrow \text{HOBr} + \text{HBr} \]

### Step 2: Determine the Oxidation States
Next, we need to determine the oxidation states of bromine in the reactants and products.

- In Br₂ (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 3: Analyze the Changes in Oxidation States
Now, let's analyze the changes in oxidation states:
- From Br₂ (0) to HOBr (+1): Bromine is **oxidized** (loss of electrons).
- From Br₂ (0) to HBr (-1): Bromine is **reduced** (gain of electrons).

### Step 4: Conclusion about the Behavior of Bromine
Since bromine undergoes both oxidation and reduction in this reaction, we can conclude that bromine is acting as both an oxidizing agent and a reducing agent.

### Final Answer
The best description of the behavior of bromine in the reaction is that it is **both oxidized and reduced**.