Double Pi Bonds

[Nicole Huang 3F]

If there was a triple bond between two atoms between C and N, where both had a hybridization of 2sp, how would the bonding work? Is it a sigma bond formed between one sp orbital, and a pi bond with the other sp orbital; but then there would still need to be another pi bond because it's triple so I'm not sure which orbitals it would use to bond. I was wondering if anyone could explain how the bondings would work visually. Thanks!

For reference, it would like like:
[some molecule] - C ≡ N :

[505352202]

The triple bond is composed of one σ bond and two π bonds. The sigma bond is formed from head-to-head overlap of the sp hybrid orbitals from the C and N atoms. The two π bonds in the triple bond are formed from overlap of the two unhybridized p atomic orbitals on each C and N atom.

[Annie Tong 2G]

I'm not entirely sure but here's my guess: carbon's hybridization would be 2sp ↑ ↑ and 2p ↑ ↑. Nitrogen is 2sp ↑ ↑ and 2p ↑↓ ↑ ↑. The 2sp overlap forms a sigma bond and the two 2p overlaps form two pi bonds. The ↑↓ in nitrogen's 2p orbital is its lone pair.

[Silvi_Lybbert_3A]

So with CN, there is a triple bond which means there will be one sigma bond and two pi bonds (this is always the case with a triple bond, at least for our purposes I believe). The C and the N both have 2sp hybridization as you said. But there are three p-orbitals (px, py, and pz), and only one of these p-orbitals is brought into hybridization with the 1s orbital. So, both carbon and nitrogen in this molecule have two unhybridized 2p orbitals each. These unhybridized orbitals are perpendicular to the hybridized orbital involved in the sigma bond (C2sp, N2sp). They are perpendicular to the hybridized orbital but also parallel to each other in the directions they point. They will bond with each other side-to-side (C2p, N2p). A really helpful way to figure this out and visualize it is using your fingers as Dr. Lavelle did in lecture.

This image shows triple bond (remember: each unhybridized p-orbital has two lobes).

[Chenning Yang Dis3l]

This is a great question! I was wondering.

[kristinalaudis3e]

So in a triple bond, one is a sigma bond and 2 are pi bonds. For the sigma bonds, they will overlap end to end, but for the pi bonds, they have to overlap side by side. The 2 pi bonds are formed when the unoccupied p orbitals that are not overlapping end to end then overlap side by side with the other unoccupied p orbitals.

[Jaclyn Schwartz 1I]

In a triple bond, there is one sigma bond and two pi bonds. I believe sigma bonds are end to end while pi bonds are side to side bonds.