The correct order of S-S bond length in the f | vedclass

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(A) The $S-S$ bond length depends on the oxidation state of sulfur and the repulsion between lone pairs on the sulfur atoms.In $S_2O_4^{2-}$ (dithioni

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$I > II > III$

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(A) The $S-S$ bond length depends on the oxidation state of sulfur and the repulsion between lone pairs on the sulfur atoms.In $S_2O_4^{2-}$ (dithionite),each sulfur atom has one lone pair,leading to significant $L.P.-L.P.$ repulsion between the two sulfur atoms,which increases the $S-S$ bond length.In $S_2O_5^{2-}$ (disulfite),one sulfur has a lone pair and the other does not,resulting in less repulsion compared to $S_2O_4^{2-}$.In $S_2O_6^{2-}$ (dithionate),both sulfur atoms are in a higher oxidation state and have no lone pairs involved in $S-S$ repulsion,resulting in the shortest $S-S$ bond length.Therefore,the correct order of $S-S$ bond length is $I > II > III$.

The correct order of $S-S$ bond length in the following oxyanions is:
$(I) \, S_2O_4^{2-}$
$(II) \, S_2O_5^{2-}$
$(III) \, S_2O_6^{2-}$

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The correct order of $S-S$ bond length in the following oxyanions is:$(I) \, S_2O_4^{2-}$$(II) \, S_2O_5^{2-}$$(III) \, S_2O_6^{2-}$