I recently came across this sentence in my textbook “the bonds between sulphur and oxygen in oxides of sulphur (SO2 and SO3 ) are much shorter than might be expected for a single bond


SO3 bondingso3

I feel it could be due to partial double bond character due to resonance

And the same textbook gives an explanation “In these molecules, in addition to normal π bond, a π bond is also formed by the sidewise overlap of a filled 2p-orbital of oxygen with a vacant 3d-orbital on the sulphur). This is called pπ - dπ bond and results in bringing the two atoms closer and thus accounts for shorter bond length of S-O bond.

Which is definitely untrue and incorrect

Please provide a reason for the same

  • 4
    $\begingroup$ Well, maybe this is because they are not single bonds? $\endgroup$ – Ivan Neretin Jan 14 at 8:17
  • $\begingroup$ Please cite the sources for the quotes and images you use, even (or especially) it they are from of own network. $\endgroup$ – Martin - マーチン Apr 14 at 19:32
  • $\begingroup$ "Which is definitely untrue and incorrect" Why do you think so? $\endgroup$ – Karl Apr 14 at 19:56
  • $\begingroup$ @Karl “That is thoroughly incorrect. chemistry.stackexchange.com/questions/51168/… chemistry.stackexchange.com/questions/29101/… – Mithoron” $\endgroup$ – Chemist Apr 14 at 21:07
  • $\begingroup$ Please explain this (in one or two scentences) in your question. It's not obvious. $\endgroup$ – Karl Apr 14 at 21:12

If you would consider it more carefully, you would see that the bond order in SO2 and SO3 are, respectively, 1.5 and 4/3. This means that they are shorter than a single bond of sulphur and oxygen.


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