In the conversion of `I_2 rarr IO_3^-`the oxidation state of iodine changes from

Options

A. 0 to +6
B. 0 to +5
C. 0 to -1
D. 0 to -3

Answer

To determine the change in oxidation state of iodine in the conversion from \( I_2 \) to \( IO_3^- \), we can follow these steps:

### Step 1: Determine the oxidation state of iodine in \( I_2 \)
In the molecular form \( I_2 \), each iodine atom has an oxidation state of 0 because it is in its elemental form.

### Step 2: Set up the oxidation state equation for \( IO_3^- \)
In the ion \( IO_3^- \), we need to find the oxidation state of iodine (let's denote it as \( x \)). The oxidation states of oxygen are typically -2. Since there are three oxygen atoms, their total contribution to the charge is:
\[ 3 \times (-2) = -6 \]

### Step 3: Write the equation for the total charge
The overall charge of the ion \( IO_3^- \) is -1. Therefore, we can set up the following equation:
\[ x + (-6) = -1 \]

### Step 4: Solve for \( x \)
Now, we can solve for \( x \):
\[ x - 6 = -1 \]
\[ x = -1 + 6 \]
\[ x = +5 \]

### Step 5: Determine the change in oxidation state
Now we can compare the oxidation states:
- The oxidation state of iodine in \( I_2 \) is 0.
- The oxidation state of iodine in \( IO_3^- \) is +5.

### Step 6: Calculate the change
The change in oxidation state is:
\[ 0 \rightarrow +5 \]
This indicates that iodine is oxidized from an oxidation state of 0 to +5.

### Conclusion
Thus, the oxidation state of iodine changes from 0 to +5 in the conversion from \( I_2 \) to \( IO_3^- \).