2
$\begingroup$

I know that the $\ce{S8}$ molecule contains 16 pairs of lone electrons. My teacher always says that we must try to reduce the no of lone pairs, so, had there been double bonds between 8 atoms of sulfur then the no of lone pairs would be reduced. Then why aren't there any double bonds?

$\endgroup$
3
$\begingroup$

An $\ce{S}$ atom in a molecule must have 2 bonds to be neutral and in the $\ce{S8}$ ring it needs both of these bonds to continue the chain/ring. If you introduce some double bonded S atoms into the ring each of these will have 3 bonds and will thus be positively charged. So, while reducing the number of free electron pairs you increase the charge of the compound which would be wrong because $\ce{S8}$ isn't charged. You can only use free electron pairs to form double bonds if you have some electron deficient atoms in the neighborhood which can "receive" them.

$\endgroup$

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.