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Count the number of electron densities that are surrounding the central atom. For example, if there are 4, then the hybridization is sp3. If there are 5, then it is sp3d, since the p orbital can only contain three, and s can only have one, the 5th electron goes to the d orbital.
I usually look at how many other atoms are being attached to the central atom and if it is say 3 other atoms the hybridization is just one less; sp2. For 5 and 6atoms attached to the central atom you just have to remember you are using d orbitals so it will always have an sp3 and then however many d orbitals are being used. If it is 5 it will be dsp3 and 6 is d2sp3
Like other people said before, count the number of areas of electron density. Lone pairs count as one area of electron density. Single, double, and triple bonds also only count as one are of electron density. It might be weird to think that a double and triple bond count only as a single area of electron density since they have four and six electrons involved, respectively, but I guess it kind of makes sense since they attach only 2 atoms together. Once you have the number of areas of electron density, then you should have a corresponding number of orbitals in the hybridized orbital. E.g. 1 area of electron density = s, 2 areas = sp, 3 areas = sp2, 4 areas = sp3, 5 areas = sp3d, 6 areas = sp3d2
Draw the lewis structure, and calculate the steric number which is the number of sigma bonds and number of lone pairs. Based on the steric number we can figure out the hybridization. E.g. steric number 2 = sp, 3= sp2 and so on.
KarlaArevalo4D wrote:Does anyone have an easy way to find the hybridization of the central atom they are able to share? Much appreciated.
The easiest way is to consider the number of regions with electron density. This includes lone pairs.
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