2.45 Hybridization

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2.45 Hybridization

Postby ZainAlrawi_1J » Wed Dec 04, 2019 4:39 pm

Can someone explain how the hybridization of the lone pairs in part b of this question are derived? I have never seen a question like this before and I'm not even sure that we have went over it.

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Re: 2.45 Hybridization

Postby nicolely2F » Wed Dec 04, 2019 6:34 pm

It follows the same logic as the bonds. The oxygen has a hybridization of sp2 (two being lone pairs) because it is connected to three areas of electron density; each lone pair will have that hybridization because they are electrons in hybridized orbitals, same as if they were bonded

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Re: 2.45 Hybridization

Postby DTingey_1C » Wed Dec 04, 2019 6:56 pm

If it makes it easier to understand, think of the hybridization as something akin to the shape of the molecule. sp3 means there are 4 regions of e- density, meaning the shape can be AX4, AX3E, AX2E2, ect. This means that you can almost name a molecule as a tetrahedral by knowing that its hybridization is sp3, assuming there are no lone pairs.

Sears 4A
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Re: 2.45 Hybridization

Postby Sears 4A » Wed Dec 04, 2019 7:58 pm

however many regions of electron density an atom has, it will have exactly that many hybrid orbitals, even if they are lone pairs

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