white_o
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I was just wondering if someone could explain about the pi bond in an alkene. So do the p-orbitals rotate and just overlap and that's why a bond is formed?
So the blue lines are the p-orbitals which rotate and then they just overlap so it forms a bond that is drawn as the red oval? So does this mean the electrons bond and keep rotating around the sigma bond, if that makes sense? Someone please explain!! Thanks
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interstitial
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let's take ethene for example

the carbon atoms form sp2 hybrid orbitals to form 3 bonds each (ordinarily they can only form 2)

these bond with the hydrogen and carbon to form molecular orbitals

the remaining p orbital overlaps above and below the carbon atoms

afaik every double bond is made of a sigma bond and pi bond

the pi bond is a molecular orbital similar to a regular orbital which shows where the electrons are likely to be found

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charco
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(Original post by Qaiys)
I was just wondering if someone could explain about the pi bond in an alkene. So do the p-orbitals rotate and just overlap and that's why a bond is formed?
So the blue lines are the p-orbitals which rotate and then they just overlap so it forms a bond that is drawn as the red oval? So does this mean the electrons bond and keep rotating around the sigma bond, if that makes sense? Someone please explain!! Thanks
'p' orbitals do not rotate. They represent a region of space in which there is a 0.99 probability of finding an electron of that energy ...
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