Octahedral vs Trigonal Bypyramidal family

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Jade Fosburgh Discussion 2C
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Joined: Fri Sep 29, 2017 7:07 am

Octahedral vs Trigonal Bypyramidal family

Postby Jade Fosburgh Discussion 2C » Sun Nov 19, 2017 5:51 pm

In the trigonal bypyramidal family, I know there are always 5 regions of electron density around the central atom, and there is the axial and equatorial plane. When you start to account for lone pairs, they occupy the regions of electron density in the equatorial plane (see-saw, T-shaped).

But for structures in the octahedral family, is there such thing as an equatorial or axial plane? Or does it not matter which atom you pick when looking at lone pairs. Just having trouble visualizing. Thanks!

StephanieDoan3B
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Re: Octahedral vs Trigonal Bypyramidal family

Postby StephanieDoan3B » Sun Nov 19, 2017 8:00 pm

Every angle in an octahedral structure is 90 degrees. In other words, the orientation of the molecule doesn't matter, so the electron density you choose for the placement of the first lone pair doesn't matter.

Chris Pleman 3E
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Re: Octahedral vs Trigonal Bypyramidal family

Postby Chris Pleman 3E » Sun Nov 19, 2017 11:15 pm

For the Octahedral shape, there will be four atoms on one plane, and two axial atoms bonded to the central atom.

Justin Lai 1C
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Joined: Fri Sep 29, 2017 7:04 am

Re: Octahedral vs Trigonal Bypyramidal family

Postby Justin Lai 1C » Sun Nov 19, 2017 11:28 pm

Yes pretty sure there is axial and equatorial plane. Lone pairs start occupying axial planes to make square pyramidal and square planar.


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