orbital hybridization and polarity


Moderators: Chem_Mod, Chem_Admin

Jennifer Guzman 4C
Posts: 38
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?

armintaheri
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.


Return to “Hybridization”

Who is online

Users browsing this forum: No registered users and 1 guest