"State the relative orientations of each of the following hybrid orbitals
(a) sp3 ;(b) sp ;(c) sp3d2 ;(d) sp2"
Can someone explain this to me? Is this something we need to know for the final?
Textbook problem 2F1
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Re: Textbook problem 2F1
It's just asking what kind of geometry it creates. So sp3 for example is tetrahedral bc the # of hybrid orbitals corresponds to the number of regions of e- density. sp2 would be trigonal planar and so on.
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Re: Textbook problem 2F1
This refers to the electron geometry that corresponds with the hybridization. And you should probably know this for the final.
sp3d2- octahedral
sp3d- trigonal bipyramidal
sp3- tetrahedral
sp2- trigonal planar
sp-linear
sp3d2- octahedral
sp3d- trigonal bipyramidal
sp3- tetrahedral
sp2- trigonal planar
sp-linear
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Re: Textbook problem 2F1
This question is asking for the molecular shapes that result from each hybridization scheme. The trick I use remember is to count the individual number of orbitals in the hybridization, which is equal to the number of regions of electron density in the molecule. So for sp3, there is one 's' and three 'p's', so the number of regions of electron density is four, and the resulting shape is tetrahedral. You can do this for others like sp3d2, where there is six orbitals involved, meaning six regions and an octahedral shape. Hope this helps
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