(Polar molecules, Non-polar molecules, etc.)

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Tyler Angtuaco 1G
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Postby Tyler Angtuaco 1G » Wed Nov 13, 2019 1:55 pm

Can someone explain the concept of overlapping orbitals and their effect on the strength of bonds?

Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

Re: Hybridization

Postby KNguyen_1I » Wed Nov 13, 2019 4:15 pm

So, there are two types of overlapping orbitals to my understanding: sigma and pi bonds. Sigma bonds are formed when the ends of each electron orbital comes together, while pi bonds are where they overlap side by side (think of the p-orbital lobes-- touching tips is a sigma and side by side is a pi bond).
I think that the second bond in a double bond is a pi bond.
Single bonds are always a sigma bond. Double bonds have one sigma and one pi. Triple bonds have one sigma and two pi.
As for hybridization, this happens when a s and p orbital combine to have more space for electrons (if you draw out the electron configuration). So you get stuff like sp, sp2, sp3. This influences the geometry and possible orientation of bonds, I believe.
Hope this helps!

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