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From what we briefly learned in my discussion section, hybridization is the combining of atomic orbitals into new hybrid orbitals to pair electrons and form chemical bonds. We did several examples where we would first draw the lewis structure of the compound, for example BeCl2. Then we would determine how many areas of electron density there were when looking at the Lewis structure. for BeCl2 in particular, there are 2 areas of electron density (both Cl's surrounding the Be). This would mean we would hybridize 2 orbitals (combine 2 orbitals together), which in this case would be the 2s orbital (where the highest level electrons were for Be) and the orbital above it, which is the 2p orbital. Therefore, the hybridization of Be would be sp.
Hybridization describes the process where atomic orbitals fuse together in order to form new hybrid orbitals. To determine hybridization, you have to look at the number of atoms attached to the central atom and add it to the number of lone pairs. If the answer is 4, then the atom is sp3, if the answer is 3, then the atom is sp2, and so on.
405404782 Gabriel Rigole 4F wrote:Can someone explain hybridization and how to determine what the hybridization of a molecule is?
Just like what Eileen said, the hybridization of the molecule depends on the number of bonds around the atom in question. Dr. Lavelle will talk about it more after Test #2.
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