In the conversion `Br_(2) rarr BrO_(3)^(-)` the oxidation state of bromine changes from

Options

A. `– 1 "to" – 1`
B. 0 to – 1
C. 0 to + 5
D. 0 to – 5

Explanation

To determine the change in oxidation state of bromine in the conversion from \( \text{Br}_2 \) to \( \text{BrO}_3^- \), we can follow these steps:

### Step 1: Identify the oxidation state of bromine in \( \text{Br}_2 \)

In the diatomic molecule \( \text{Br}_2 \), bromine is in its elemental form. The oxidation state of any element in its standard state is 0. Therefore, the oxidation state of bromine in \( \text{Br}_2 \) is:

\[ \text{Oxidation state of Br in } \text{Br}_2 = 0 \]

### Step 2: Determine the oxidation state of bromine in \( \text{BrO}_3^- \)

To find the oxidation state of bromine in the bromate ion \( \text{BrO}_3^- \), we can set up an equation based on the known oxidation states of oxygen. Oxygen typically has an oxidation state of -2.

Let \( x \) be the oxidation state of bromine in \( \text{BrO}_3^- \). The ion has a total charge of -1, and there are three oxygen atoms contributing to the charge. Therefore, we can write the equation:

\[ x + 3(-2) = -1 \]

This simplifies to:

\[ x - 6 = -1 \]

### Step 3: Solve for \( x \)

Now, we can solve for \( x \):

\[ x = -1 + 6 \]
\[ x = +5 \]

Thus, the oxidation state of bromine in \( \text{BrO}_3^- \) is:

\[ \text{Oxidation state of Br in } \text{BrO}_3^- = +5 \]

### Step 4: Calculate the change in oxidation state

Now, we can find the change in oxidation state of bromine during the conversion from \( \text{Br}_2 \) to \( \text{BrO}_3^- \):

\[ \text{Change in oxidation state} = +5 - 0 = +5 \]

### Conclusion

The oxidation state of bromine changes from 0 in \( \text{Br}_2 \) to +5 in \( \text{BrO}_3^- \).

### Final Answer

The oxidation state of bromine changes from 0 to +5.

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