[nriggan]

Okay, so N2 has a triple bond and a lone pair on each N atom. This implies that there are two pi bonds and one sigma bond. Now, every website, forum, etc. has said that each N atom hybridizes to form an sp orbital, so the sigma bond formed would be denoted as [σ sp-sp]. However, upon investigating the occupied and shared energy levels of each Nitrogen, I realized that this sigma bond could very well be a [σ 2p-2p] bond, which would actually make more sense as it would leave the 2s orbital as the lone pairs on each Nitrogen as opposed to an sp lone pair which as far as my knowledge goes, does not exist. I have a chemistry exam tomorrow, and I really need to be sure of this ASAP. Thanks for your helps guys.

[Hunter2]

Nitrogen |N=N|  you can compare with the ethyne H-C=C-H. The orbitals are sp hybridizised.

[nriggan]

Ooookay, but why? Wouldn't it make more sense for the 2s orbital to serve as a lone pair than a leftover sp? And could you provide an example of something with a [σ2p-2p] bond?

[Corribus]

There are a lot of reasons this wouldn't work. One is that if the lone pairs were located in unhybridized s-orbitals, they'd be located a lot closer to the electron dense bonding region the molecule, which would entail a large interaction energy. Located into sp-hybridized orbitals directed in the opposite direction, electron-repulsion between the lone pair and the bonding electrons is minimized.

[nriggan]

Thank you!! Oh and about that example of a σ2p-2p bond....I can't seem to find one anywhere. Most places don't even describe the contributing atomic orbitals in the making of a molecular orbital. If anyone could possibly think up one that would be fantastic.

[Irlanur]

I still don't understand why there are any arguments about hybridisation... it's a matter of mathematical convenience and not a matter of physics.