p orbital/ hybridization

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p orbital/ hybridization

Postby 104599631 » Fri Oct 23, 2015 4:19 pm

I'm very confused with the unhybridized p orbitals in the example of ethene. 1) Why are the p orbitals unhybridized? 2) why are they there considering carbon only has 3 areas of electron density which consists of the 3 2sp^2 orbitals? 3) How do the pi bonds connect the two orbitals together?

Richmund Tan 1L
Posts: 25
Joined: Fri Sep 25, 2015 3:00 am

Re: p orbital/ hybridization

Postby Richmund Tan 1L » Fri Oct 23, 2015 5:04 pm

Hello there, I believe I can answer your third question. The Pi bonds overlap side by side, and if you recall the diagram Dr. Lavelle drew on the board, these overlapping sides are located on the z axis (if you imagine the board to be the 2-D space that covers x and y, and the 3-D space comes out and sinks into the board being the z axis). Since they overlap side by side, therefore, a Pi bond is formed.
Hope this helps and I'm interested in figuring out the other answers to your questions.

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