The oxidation sates of iodine in `HIO_(4), H_(3)IO_(5)` and `H_(5)IO_(6)` are respectively :

Options

A. `+1,+3,+7`
B. `+7,+7,+3`
C. `+7,+7,+7`
D. `+7,+5,+3`

Explanation

To find the oxidation states of iodine in the compounds \( HIO_4 \), \( H_3IO_5 \), and \( H_5IO_6 \), we will follow a systematic approach.

### Step 1: Determine the oxidation state of iodine in \( HIO_4 \)

1. **Assign known oxidation states:**
- Hydrogen (H) = +1
- Oxygen (O) = -2

2. **Set up the equation:**
Let the oxidation state of iodine be \( X \).
\[ 1 + X + (-2) \times 4 = 0 \]

3. **Simplify the equation:**
\[ 1 + X - 8 = 0 \]
\[ X - 7 = 0 \]
\[ X = +7 \]

### Step 2: Determine the oxidation state of iodine in \( H_3IO_5 \)

1. **Assign known oxidation states:**
- Hydrogen (H) = +1
- Oxygen (O) = -2

2. **Set up the equation:**
Let the oxidation state of iodine be \( Y \).
\[ 3 \times 1 + Y + (-2) \times 5 = 0 \]

3. **Simplify the equation:**
\[ 3 + Y - 10 = 0 \]
\[ Y - 7 = 0 \]
\[ Y = +7 \]

### Step 3: Determine the oxidation state of iodine in \( H_5IO_6 \)

1. **Assign known oxidation states:**
- Hydrogen (H) = +1
- Oxygen (O) = -2

2. **Set up the equation:**
Let the oxidation state of iodine be \( Z \).
\[ 5 \times 1 + Z + (-2) \times 6 = 0 \]

3. **Simplify the equation:**
\[ 5 + Z - 12 = 0 \]
\[ Z - 7 = 0 \]
\[ Z = +7 \]

### Conclusion

The oxidation states of iodine in \( HIO_4 \), \( H_3IO_5 \), and \( H_5IO_6 \) are respectively:
- \( HIO_4 \): +7
- \( H_3IO_5 \): +7
- \( H_5IO_6 \): +7

Thus, the final answer is \( +7, +7, +7 \).