Orbital Hybridization - OrbitalHybridization

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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:  σ  and  π  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  σ  or  π  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  σ  or  π  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 
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This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

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Orbital Hybridization - OrbitalHybridization

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