sigma vs pi bonds


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Valeria Viera 1B
Posts: 60
Joined: Fri Apr 06, 2018 11:05 am

sigma vs pi bonds

Postby Valeria Viera 1B » Sat Jun 09, 2018 9:04 pm

I get that a single bond has one sigma bond and that a double bond has one sigma and one pi bond but what is the difference between a sigma bond and a pi bond?

Danielle Sumilang - 1F
Posts: 31
Joined: Fri Apr 06, 2018 11:05 am

Re: sigma vs pi bonds

Postby Danielle Sumilang - 1F » Sat Jun 09, 2018 10:46 pm

Hello!

Sigma bonds occur when orbitals overlap from end to end. Pi bonds occur when orbitals overlap from side to side. Sigma bonds also allow bound atoms to rotate. If I'm not mistaken, sigma bonds can form when there is an s-s orbital overlap or an s-p orbital overlap while pi bonds form only when there is a p-p orbital overlap.

Heung Ching Chia 1E
Posts: 25
Joined: Mon Apr 09, 2018 1:38 pm

Re: sigma vs pi bonds

Postby Heung Ching Chia 1E » Sat Jun 09, 2018 11:00 pm

I hope this comparison table helps!
Sigma bonds have a head on overlap compared to pi bonds which overlap sideways. Pi bonds also restrict rotation while sigma bonds allow free rotation around the bond.
Attachments
sigma bond vs pi bond table.PNG

Andre-1H
Posts: 39
Joined: Fri Apr 06, 2018 11:01 am

Re: sigma vs pi bonds

Postby Andre-1H » Sun Jun 10, 2018 11:00 am

Heung Ching Chia 1E wrote:I hope this comparison table helps!
Sigma bonds have a head on overlap compared to pi bonds which overlap sideways. Pi bonds also restrict rotation while sigma bonds allow free rotation around the bond.


Could you talk about how to understand sp2 and sp3 hybridization? I'm still confused on this subject. How do you understand the difference between the hybrid orbitals

Johanna Caprietta 1E
Posts: 30
Joined: Fri Apr 06, 2018 11:02 am

Re: sigma vs pi bonds

Postby Johanna Caprietta 1E » Sun Jun 10, 2018 11:12 am

If a molecule has an sp2 hybridization, the molecule has three bonds. For a molecule with an sp3 hybridization, the molecule would have four bonds. The following consititutes as 1 bond: a lone pair, a single bond, a double bond, and a triple bond.
I hope this answers your question Andre.


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