Question

Question #2c26e

Answer 1

The oxidation states would be +1, +3 and +5 respectively.

Explanation:

You obtain these by considering that in an oxoacid the `H` always counts for +1 and the `O` for -2. The chlorine has to even this out.

(1) `HClO->Cl` must be +1 `->Cl_2O` (dichlorine monoxide)

(2) `HClO_2->Cl` must be +3`->Cl_2O_3` (dichlorine trioxide)

(3) `HClO_3->Cl` must be +5`->Cl_2O_5` (dichlorine pentoxide)

Note:
Often the 'di' in the name is omitted, as all acid-forming chloro-oxides are 'di'. In case (1) this can lead to confusion with `ClO`, which is a neutral oxide.