## Hybridization bonds

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

EllaBerry
Posts: 68
Joined: Fri Sep 28, 2018 12:29 am

### Hybridization bonds

I'm still confused on the topic of hybridization, can someone explain why when there is a single bond it is just a sigma bond but when there is a double bond it is a sigma and pi bond?

Jonas Talandis
Posts: 60
Joined: Fri Sep 28, 2018 12:16 am

### Re: Hybridization bonds

Because sigma bonds overlap head on and pi bonds overlap side by side. It has to do with orbital configuration. In today's lecture, the C2H4 molecule had a pi bond where the double bond was because the left over unhybridized orbital at the 2p level was oriented at 90 degrees outward, resulting in a side by side pi bond. Single bonds are always sigma because the unpaired electrons always overlap head-on. The addition of a double or triple bond is a result of unpaired electrons in these unhybridized orbitals, resulting in side by side overlaps.

005199302
Posts: 108
Joined: Fri Sep 28, 2018 12:15 am

### Re: Hybridization bonds

When two atoms bond head on they create a sigma bond. When there's a double bond, the first bond is a sigma bond, but the second bond of the double bond can't face the other atom head on. Instead, it overlaps side by side as a result of repulsion from the first bond. This is the reason that a single sigma bond is much stronger than a singe pi bond.