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Unformatted text preview: Orbital Hybridization We've learned how constructive and destructive interference of atomic orbitals explains the formation of bonding and anti-bonding orbitals. We also leaned about two types of bonding: and bonding. So you might expect that for polyatomic molecules, all you need to do is put the atoms of the molecule near each other in the right geometry and then see what or bonds form between all the atomic orbitals. Well, it is almost that simple. The only problem is that for most molecular geometries the atomic orbitals on an atom do not point in the right direction for a or bond to form. Let's look at BF 3 as an example. From VSEPR we know the geometry around the Boron atom should be trigonal planar. But for a Boron atom all the valence elelctrons are in the 2s, 2p x , 2p y , 2p z orbitals. Recall their shapes: The problem you'll find is that there's no way you can put three Fluorine atoms around the s and p orbitals of Boron in a trigonal planar configuration and form 3 equivalent...
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- Winter '08