(Polar molecules, Non-polar molecules, etc.)

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Postby Philip » Sun Nov 24, 2019 8:44 pm

So I was wondering why for T shape the two electron pairs are like right next to each other in the trigonal planar part of the trigonal bipyramidal

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Re: T-Shape

Postby madijohnson_4A » Sun Nov 24, 2019 8:48 pm

In the Lewis structure, it looks like the electrons pairs are right next to each other, but in the VSEPR model they are much further apart with the 3D shape. For example with water, it looks like the lone pairs are right next to each other, but they are actually spaced out in the tetrahedral shape for the most energetically favorable structure.

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Re: T-Shape

Postby jvera4b » Sun Nov 24, 2019 8:54 pm

The electron pairs are in the "trigonal planar" part of the molecule because that forms the shape with the least amount of repulsion.

Madeline Phan 1E
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Re: T-Shape

Postby Madeline Phan 1E » Sun Nov 24, 2019 8:55 pm

In the VSEPR model, they are actually significantly far apart because the electrons are trying to get as far apart as possible.

Ashley Wang 4G
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Re: T-Shape

Postby Ashley Wang 4G » Sun Nov 24, 2019 10:37 pm

The two lone pairs are located in two of the three trigonal-planar positions because then they are only interacting with two of the bonded pairs at 90 degrees, and one at 120 degrees. This minimizes repulsion, whereas if they were located in the axial positions they would be interacting with all three bonded pairs at 90 degrees.

Hope this helps!

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Re: T-Shape

Postby emwoodc » Fri Nov 29, 2019 9:26 pm

in the VSEPR model, you can see that it is not the same.

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