Consider the ions: ${\mathrm{S}}_2{\mathrm{O}}_3^{2-}$ (X) and ${\mathrm{S}}_2{\mathrm{O}}_4^{2-}$ (Y). How many statements are correct regarding (X) and (Y). (d stands for bond length)

(a) $d_{S-S}:X<Y$

(b) $d_{S-O}:X<Y$

(c) Average oxidation state of S in (X) is less than that in (Y)

(d) In both (X) and (Y), the central S atom is sp³ hybridised   

The ions: ${\mathrm{S}}_2{\mathrm{O}}_3^{2-}$ (X) and ${\mathrm{S}}_2{\mathrm{O}}_4^{2-}$ (Y) can be represented as,

Average oxidation state of S in (X) is less than that in (Y)

$\text{ Avg O.S. }=+2\text{ Avg O.S. }=+3$

The bond length of both S-S and S-O is less in X compared to Y.

   $\text{ B.L. }(\mathrm{S}-\mathrm{S}) \mathrm{Y}>\mathrm{X}$

$\text{ B.L. }(\mathrm{S}-\mathrm{O})\mathrm{Y}\left(151\mathrm{pm}\right)>\mathrm{X}\left(147\mathrm{pm}\right)$

Due to l.p. on${ }^{\text{'}\text{'}}{S}^{\mathrm{\prime }}{\text{ in }}^{\text{'}}{Y}^{\text{'}},\mathrm{\%}\text{ in }S-O\text{ bond }\uparrow \text{ and B.L. }\uparrow$

The central S atom is sp³ hybridised in both the molecule.