(Polar molecules, Non-polar molecules, etc.)
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I understand pi and sigma bonds are caused by an overlap in location between electron dense regions. However I’m having trouble conceptualizing the difference between them, specifically when visualizing them. Does anyone have any tips? Thanks!
The sigma bond is more just like your basic head on covalent bond, where the bond is in line with the bonding orbitals. The pi bond is a covalent bond perpendicular to the bond direction, which is usually in p-orbitals never s. This is why you wouldn't be able to rotate a double or triple bond around its axis like you can with a single bond.
I see, that definitely does help. I remember my T.A briefly mentioned that there's a shortcut in identifying which type of bonds exist by memorizing the association between single/double/triple bonds and pi/sigma bonds. Unfortunately, I don't remember exactly what the association was. Does anyone know the association? Thanks!
There is always one sigma bond in any kind of bond, and additional bonds are pi bonds. A single bond is 1 sigma bond. A double bond is 1 sigma bond and 1 pi bond. A triple bond is 1 sigma bond and 2 pi bonds.
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