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 '19 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 '19 at 19:32
  • $\begingroup$ "Which is definitely untrue and incorrect" Why do you think so? $\endgroup$ – Karl Apr 14 '19 at 19:56
  • $\begingroup$ @Karl “That is thoroughly incorrect. chemistry.stackexchange.com/questions/51168/… chemistry.stackexchange.com/questions/29101/… – Mithoron” $\endgroup$ – Chemist Apr 14 '19 at 21:07
  • $\begingroup$ Please explain this (in one or two scentences) in your question. It's not obvious. $\endgroup$ – Karl Apr 14 '19 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.


Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.