In the chapter on molecular orbitals, my chemistry book mentions three types of sigma bonds: those formed by s-s ($\ce{H2}$), s-p ($\ce{HCl}$), p-p ($\ce{Cl2}$) hybrid-s ($\ce{CH4}$) and hybrid-hybrid ($\ce{C2H6}$) overlap. How is it possible to predict the type of atomic orbital overlap by which a specific σ bond is formed?


1 Answer 1


The basic answer is go by what is available.

  • Hydrogen does not have any other occupied orbitals than s-orbitals. Hence it must use an s-orbital for bonding. This goes both directions.

  • Carbon requires four bonds. In order to achieve this, it must hybridise in some way, otherwise, an electron pair would be in an s-orbital and an empty p-orbital would be unavailable for bonding. Hence carbon uses hybrid orbitals in both directions.

  • Chlorine could hybridise, but it doesn’t have to fulfill its bonding needs. In general, an electron pair in an s-orbital is more stable than one in a p-orbital because it is ‘closer to the nucleus’. (That layman’s argument is bad but gets us a long way.) So chlorine will happily use its p-orbitals for bonding.

    This goes both ways, by the way, so a carbon-chlorine bond ($\ce{C-Cl}$) is a hybrid-p sigma bond.

  • Finally, let’s consider oxygen and nitrogen. They would love to just bond with their p-orbitals, but even if hydrogen is the bonding partner that leads to too much steric strain. Therefore, they hybridise just enough to alleviate the steric stress while still maintaining a maximum s-character for a/the lone pair. So those would love to form bonds with their p-orbitals but typically can’t (so they must use hybrid orbitals). Phosphorus and sulfur are large enough to generally allow bonding only with p-orbitals.

  • $\begingroup$ This (specifically the carbon example) seems to imply that a bond is really just a combination of one half-filled orbital from each atom. Is that correct? $\endgroup$
    – Marcel
    Sep 22, 2016 at 20:32
  • $\begingroup$ Also: what do you mean by "This goes both directions"? $\endgroup$
    – Marcel
    Sep 22, 2016 at 20:34
  • 1
    $\begingroup$ @Marcel Yeah, the orbitals combine to form a bond. ‘This goes both directions’ is supposed to say that it doesn’t matter if say carbon is ‘on the left’ or ‘on the right’; it’ll use the same orbitals. $\endgroup$
    – Jan
    Sep 22, 2016 at 20:55

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