The oxidation state of `S` in `H_(2)S_(2)O_(8)` is

Options

A. `+6`
B. `+7`
C. `+8`
D. 0

Answer

A

Explanation

`H_(2)S_(2)O_(8)`
`H-O-underset(O)underset(||)overset(O)overset(||)S-O-O-underset(O)underset(||)overset(O)overset(||)S-O-H`
Two oxygen atoms are involved in peroxide linkage, hence oxidation number will be -1 (each).
`H_(2)S_(2)O_(8)=underset(H)(2(+1))+underset(S)(2(x))+underset(O-O)(2(-1))+underset(O)(6(-2))=0`
`x=+6`