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Posted: Sat Jun 09, 2018 9:06 pm
Can someone explain to me how to determine hybridization? What are some key things to remember?
Posted: Sat Jun 09, 2018 10:35 pm
Hybridization is the mixing of orbitals into new orbitals to accommodate electrons to form new chemical bonds of the valence-bond theory. To solve for hybridization, look at the amount of electrons/atoms bonded to the central atom. For linear, there is 2 atomic orbitals as well as two hybrid orbitals, so the hybridization is sp. There’s a full table on page 125 showing all the hybridization of atoms.
Posted: Sun Jun 10, 2018 11:52 am
I would say for the final we need to know how to identify how many electron bonds a molecule has and memorizing what the hybridization would be.
Posted: Sun Jun 10, 2018 12:22 pm
To find hybridization you must determine the number of regions of electron density present.
A region of electron density is either a pair of lone pair electrons or a bond (every single, double and triple bonds just counts as one region). The number of regions correspond to a hybrid orbital (s, sp, sp2 etc.)
1 region - s
2 regions- sp
3 regions- sp2
4 regions- sp3
5 regions- sp3d
Count the number of regions of electron density around the particular atom you are focusing on and then it’s hybridization is shown above which should be memorized.