Question from textbook


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Riya Shah 4H
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Question from textbook

Postby Riya Shah 4H » Mon Nov 26, 2018 10:28 pm

Why is BrF3 sp3d hybridized?

Rachel Yoo 1F
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Re: Question from textbook

Postby Rachel Yoo 1F » Mon Nov 26, 2018 10:30 pm

It has 3 bonds and two lone pairs which means its hybridization is sp3d

Elisa Bass 4L
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Re: Question from textbook

Postby Elisa Bass 4L » Mon Nov 26, 2018 10:31 pm

When you draw the Lewis structure, the molecule is shown to have two lone pairs on Br in addition to the three bonds Br forms with the three F. Because each lone pair represents another region of electron density, five hybridized orbitals are needed and there are five sp3d orbitals.

Hanniel U 2B
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Re: Question from textbook

Postby Hanniel U 2B » Mon Nov 26, 2018 10:42 pm

Because it is T-shaped and T-shaped molecules have sp^3d hybridization.

Elena Maneffa 1E
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Re: Question from textbook

Postby Elena Maneffa 1E » Mon Nov 26, 2018 10:55 pm

When we find the lewis dot structure for BrF3 we realize that it is T-shaped. It is bonded to 3 atoms and has 2 lone pairs. The electron density or electron arrangement is 5. The atomic orbitals has to match the number of hybrid orbitals. In sp^3d: there are 5 hybrid orbitals.


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