[Juicebox]

Hello,

I understand that the three carbon 2p orbitals of this compound combine to make three pi orbitals and that one of the pi orbitals is lower in energy than a carbon 2p atomic orbital would be. I do not understand why the other two pi orbitals are higher energy and I also am having trouble visualizing the shapes of the lower and higher energy pi orbitals.

One more question: if you were to substitute one of the carbons for a boron atom, would the compound be stable?

Thanks

Orbital diagram of what I'm asking about:

[Juicebox]

Well I figured out the issue I had with the molecular orbital diagrams and shapes.

I'm still not sure if substituting boron for one of the carbons would create a more stable molecule or not. Any thoughts?

[research]

I understand that the three carbon 2p orbitals of this compound combine to make three pi orbitals and that one of the pi orbitals is lower in energy than a carbon 2p atomic orbital would be.

where did you find it?

[Juicebox]

I understand that the three carbon 2p orbitals of this compound combine to make three pi orbitals and that one of the pi orbitals is lower in energy than a carbon 2p atomic orbital would be.

where did you find it?

Sorry, where did I find what exactly?

[research]

I meant the orbitals level.
 I remembered that according to farest rule (I hope the dictation be right)we could consider annulens in a circle with Mobius and Huckel rule, I think the way which you have mentioned for the cyclopropane orbitals is because of mobius rule in contrast if you use huckel rule you will have one orbital with lower energy and the two remaining orbitals will be in upper level of energy, I 'm sure this rule is applicable for annulenes but in this case

[pacifyer]

Cyclopropenyl cation is aromatic...