The oxidation states of S atom in `S_(4)O_(6)^(2-)` from left to right respectively are
`O-underset(O)underset(||)overset(O)overset(||)S-S-S-underset(O)underset(||)overset(O)overset(||)S-O`

Options

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

Answer

C

Explanation

Each of the two terminal sulphur atoms is connected to two oxygen atoms by a double bond and one oxygen atom by a single bond. Its oxidation numberis `+5`. Two central sulphur atoms are linked to each other by a single bond and each sulphur is further attached to similar species on either side, the electron pair forming S-S bond remain in the centre and hence each atom has oxidation number zero.