Pi bonds

[Nina Fukui 2J]

I know Pi bonds appear when there's a double or triple bond but is there a specific way to label which is which? or do we just need to know that pi bonds appear in certain conditions?

[SophiaJenny3I]

I am almost certain that Dr. Lavelle said in lecture we don't need to know which is which, it's just a matter of knowing the different properties and how/when pi bonds exist!

[Xinyu Li 1C]

Pi bond is the lateral or side-by-side overlap of 2 orbitals (4 orbital overlap). It do not allow bound atoms to rotate and have 1 nodal plane. It usually between p- and d- orbitals.

[Jayasree Peri 2J]

If you wanted to label it, you could probably randomly assign which ones are pi-bonds and which ones are sigma-bonds. But, I think that, for the purposes of this class, we don't need to label; we just need to know what they are and when they occur.

[Gwendolyn Hill 2F]

Generally you just know that 1 of them is a pi bond in a double bond, and Lavelle draws the triple bonds with two pi bonds on the outside. It's just a way of thinking about them, since in reality the pi bonds are in a general "space" (lewis structures aren't really super accurate), and the bonds are a combination of pi bonds and sigma... I think it's okay, and as you know where they exist you should be good.

[Lauren Mungo 1K]

I think Dr. Lavelle just wants us to be able to identify the characteristics of each bond (pi= side by side, one nodal plane, inhibits rotation)

[Heidi Buri 2I]

Hi! Yes, pi bonds to appear when there is a double or triple bond. In a double bond, there is one pi bond. In a triple bond, there are two pi bonds. I don't believe we need to know which is which, just when pi bonds exist, where the pi bonds would be in the molecule, and how many pi bonds there are.

[Lisa Wang 3B]

I remember seeing a lot of pi bonds having this hybridization: 2p. In fact, every pi bond I've seen has that hybridization. Does anyone know why that is?