- #1
Hammad Shahid
- 64
- 3
So this question is about the bond molecular orbital diagrams for elements in the 2nd period, before O.
When the diatomic bond forms, the two pi 2p* orbitals are shown lower in energy than the sigma 2p*, uptil we get to O2.
I want to understand why this is?
From what I know, a sigma bond resulting resulting from constructive interference of an end-to-end overlap of a p-orbital forms a stronger bond than the side-by-side overlaps of the pi bond.
So why is it that for certain elements, the pi bonds are formed before the sigma bond? Shouldn't the sigma bond always be lower in energy?
Quick responses would be appreciated. I have a final tomorrow.
Thanks.
When the diatomic bond forms, the two pi 2p* orbitals are shown lower in energy than the sigma 2p*, uptil we get to O2.
I want to understand why this is?
From what I know, a sigma bond resulting resulting from constructive interference of an end-to-end overlap of a p-orbital forms a stronger bond than the side-by-side overlaps of the pi bond.
So why is it that for certain elements, the pi bonds are formed before the sigma bond? Shouldn't the sigma bond always be lower in energy?
Quick responses would be appreciated. I have a final tomorrow.
Thanks.