4.19 b

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MichelleTran3I
Posts: 25
Joined: Fri Sep 29, 2017 7:06 am

4.19 b

Postby MichelleTran3I » Tue Nov 28, 2017 12:39 pm

Why is the shape of (CH3)2Be tetrahedral? With Be as the central atom, there's only two regions of electron density. Can someone please explain how it ends up being a tetrahedral? Thanks!

Mitch Mologne 1A
Posts: 74
Joined: Fri Sep 29, 2017 7:04 am

Re: 4.19 b

Postby Mitch Mologne 1A » Tue Nov 28, 2017 12:56 pm

I believe that is just a mistake in the book because the hybridization of the molecule is sp, implying that the molecule is linear.

Katie 1E
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Re: 4.19 b

Postby Katie 1E » Tue Nov 28, 2017 12:58 pm

In the answer key they explain that the bond between Be and the Carbons on either side of it are considered sp and linear. However, the CH3 on either side of the Be are considered tetrahedral because it connects to Be on one end and H on the other three. So you were right, the Be of the atom is not tetrahedral, but the C attached to it are.

Brigitte Phung 1F
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Re: 4.19 b

Postby Brigitte Phung 1F » Tue Nov 28, 2017 12:59 pm

The shape of (CH3)2Be is only tetrahedral about the carbon atoms as they both have 4 regions of electron density (3 hydrogens about them and are both bonded to Be). However, Be only has two regions of electron density, so the C-Be-C bond is linear with a bond angle of 180 degrees. Hope this helps!


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