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Question from textbook

Posted: Mon Nov 26, 2018 10:28 pm
by Riya Shah 4H
Why is BrF3 sp3d hybridized?

Re: Question from textbook

Posted: Mon Nov 26, 2018 10:30 pm
by Rachel Yoo 1F
It has 3 bonds and two lone pairs which means its hybridization is sp3d

Re: Question from textbook

Posted: Mon Nov 26, 2018 10:31 pm
by Elisa Bass 4L
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.

Re: Question from textbook

Posted: Mon Nov 26, 2018 10:42 pm
by Hanniel U 2B
Because it is T-shaped and T-shaped molecules have sp^3d hybridization.

Re: Question from textbook

Posted: Mon Nov 26, 2018 10:55 pm
by Elena Maneffa 1E
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.