orbital hybridization and polarity

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Jennifer Guzman 4C
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Joined: Wed Feb 14, 2018 3:01 am

orbital hybridization and polarity

Postby Jennifer Guzman 4C » Sun Nov 25, 2018 8:58 pm

Is there a trick for finding out orbital hybridization and polarity if you know the molecular shape?

Posts: 68
Joined: Fri Sep 28, 2018 12:26 am

Re: orbital hybridization and polarity

Postby armintaheri » Sun Nov 25, 2018 10:47 pm

Polarity has to do with asymmetry and difference in electronegativity. If there are polar bonds and the molecule is asymmetrical, then it's polar. Hybridization requires a little bit of thinking. You can think of the central atom having multiple electron "sites". A site can contain a bond or a lone pair. The number of sites determines its hybridization. The carbon in methane has four bonds and no lone pairs. So it has 4 sites. That means it has to be sp3 hybridization. The oxygen in water has two bonds and a lone pair, so it has 3 sites, which means the hybridization has to be sp2. The carbon in carbon dioxide has two double bonds and no lone pairs, so it has 2 sites, which means there has to be sp hybridization. Basically, the number of hybridized orbitals is the same as the number of electron sites.

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