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

Explanation

To determine the oxidation states 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 of iodine in \( HIO_4 \)

1. Write the equation for the oxidation states:
\[ \text{Oxidation state of H} + \text{Oxidation state of I} + \text{Oxidation state of O} = 0 \]
For \( HIO_4 \):
- Oxidation state of H = +1
- Oxidation state of O = -2 (and there are 4 oxygen atoms)

2. Set up the equation:
\[ +1 + x + 4(-2) = 0 \]
Simplifying this gives:
\[ +1 + x - 8 = 0 \implies x - 7 = 0 \implies x = +7 \]

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

1. Write the equation for the oxidation states:
For \( H_3IO_5 \):
- Oxidation state of H = +1 (and there are 3 hydrogen atoms)
- Oxidation state of O = -2 (and there are 5 oxygen atoms)

2. Set up the equation:
\[ 3(+1) + x + 5(-2) = 0 \]
Simplifying this gives:
\[ 3 + x - 10 = 0 \implies x - 7 = 0 \implies x = +7 \]

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

1. Write the equation for the oxidation states:
For \( H_5IO_6 \):
- Oxidation state of H = +1 (and there are 5 hydrogen atoms)
- Oxidation state of O = -2 (and there are 6 oxygen atoms)

2. Set up the equation:
\[ 5(+1) + x + 6(-2) = 0 \]
Simplifying this gives:
\[ 5 + x - 12 = 0 \implies x - 7 = 0 \implies x = +7 \]

### Conclusion

The oxidation states of iodine in \( HIO_4 \), \( H_3IO_5 \), and \( H_5IO_6 \) are all +7.

### Final Answer:
The oxidation states of iodine in \( HIO_4 \), \( H_3IO_5 \), and \( H_5IO_6 \) are respectively: **+7, +7, +7**.

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