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I have learnt that for carbocations, electrons are delocalized from the $\ce{C-H}$ $\sigma$-bond to the empty p-orbital of carbon.

Moreover, alkenes are stabilized by the delocalization of electron from $\ce{C-H}$ $\sigma$-bond to the empty anti bonding $\pi$ molecular orbital.

But, don't electrons in anti bonding molecular orbitals lead to instability? So, how does hyper conjugation lead to stability of alkenes?

I believe this question has already been asked before, but I couldn't find any satisfactory and/or relevant answers.

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You are confusing the mixing of orbitals with the promotion of electrons from one orbital to another. You're thinking of this:

$\hspace{50 mm}$Promotion of electron

I don't blame you, because the phrasing "delocalisation into an antibonding orbital" implies that, but that is not actually what happens.

In what actually happens, the two original orbitals are said to mix. They cease to exist. They overlap to give two new MOs, one which is even lower in energy and one which is higher in energy, like in this diagram:

$\hspace{45 mm}$Mixing

The "new MO 1" has characteristics of both the original $\ce{C-H}$ $\sigma$ as well as the original $\ce{C=C}$ $\pi^*$, which is why we loosely say "donation into the $\pi^*$ orbital". However, don't take it too literally. The phrase means that two orbitals are mixed. It does not mean that electrons are promoted from one orbital to another.

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  • $\begingroup$ But still, we are DELOCALIZING electron density into an anti bonding orbital.So, shouldn't that be unstable? $\endgroup$ – Newton Dec 24 '15 at 9:08
  • $\begingroup$ Wait, which orbital is "lower in energy" ? $\endgroup$ – Newton Dec 24 '15 at 9:09

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