The oxidation states of S-atoms in `S_(4)O_(6)^(2-)` from left to right respectively,, are:

Options

A. `+6, 0, 0, +6`
B. `+3,1, +1, +3`
C. `+5, 0, 0, +5`
D. `+4, +1, +1, +4`

Answer

C

Explanation

The tetrathionae anions, `S_(4)O_(6)^(2-)` is a sulphur oxoacid derived from the compound tetrathionic acid. Anion can be viewed as the product formed from reaction between lewis base, `S_(2)^(2-)` and lewis acid, `SO_(3)`
`S_(2)^(2-) + 2SO_(3) to S_(4)O_(6)^(2-)`
Two of the sulphur atoms are present in the oxidation of zero and two are in oxidation state +5. The structure of `S_(4)O_(6)^(2-)`

Since each of the te wygen atom by a da a single bond, the atoms is +3. Since to each other by a attached to similar forming S-S bond ch of the terminal sulphur atom is connected to two oxygen atom by by a double bond and to one oxygen atom by S bond, the oxidation state of these terminal sulphur +5. Since, two central sulphur atoms are linked other by a single bond, and the sulphur is further to similar species on either side, the electron pair s.s bond remains in the centre and hence, each wo central sulphur atoms has on oxidation state of Thus the average oxidation state of the four sulphur stom is:
`(2 xx 5 + 2 xx 0)//4 = 2.5`