The oxidation state of iodine in `HIO_4,H_3IO_5` and `H_5IO_6` are respectively

Options

A. (+1,+3,+7)
B. (+7,+7,+3)
C. (+7,+7,+7)
D. (+7,+5,+3)

Answer

To determine the oxidation state of iodine in the compounds \( HIO_4 \), \( H_3IO_5 \), and \( H_5IO_6 \), we can follow these steps:

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

1. **Identify the known oxidation states**:
- Hydrogen (H) has an oxidation state of \( +1 \).
- Oxygen (O) has an oxidation state of \( -2 \).

2. **Set up the equation**:
- Let the oxidation state of iodine (I) be \( x \).
- The formula for \( HIO_4 \) gives us:
\[ +1 + x + 4(-2) = 0 \]

3. **Solve for \( x \)**:
\[ +1 + x - 8 = 0 \]
\[ x - 7 = 0 \implies x = +7 \]

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

1. **Identify the known oxidation states**:
- Hydrogen (H) has an oxidation state of \( +1 \).
- Oxygen (O) has an oxidation state of \( -2 \).

2. **Set up the equation**:
- Let the oxidation state of iodine (I) be \( x \).
- The formula for \( H_3IO_5 \) gives us:
\[ 3(+1) + x + 5(-2) = 0 \]

3. **Solve for \( x \)**:
\[ +3 + x - 10 = 0 \]
\[ x - 7 = 0 \implies x = +7 \]

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

1. **Identify the known oxidation states**:
- Hydrogen (H) has an oxidation state of \( +1 \).
- Oxygen (O) has an oxidation state of \( -2 \).

2. **Set up the equation**:
- Let the oxidation state of iodine (I) be \( x \).
- The formula for \( H_5IO_6 \) gives us:
\[ 5(+1) + x + 6(-2) = 0 \]

3. **Solve for \( x \)**:
\[ +5 + x - 12 = 0 \]
\[ x - 7 = 0 \implies x = +7 \]

### Conclusion

The oxidation states of iodine in the compounds are:
- \( HIO_4 \): \( +7 \)
- \( H_3IO_5 \): \( +7 \)
- \( H_5IO_6 \): \( +7 \)

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

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