Dipole Moments Cancel in Tetrahedral?

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Sydney Myers 4I
Posts: 100
Joined: Fri Aug 09, 2019 12:17 am

Dipole Moments Cancel in Tetrahedral?

Postby Sydney Myers 4I » Fri Dec 06, 2019 10:45 am

Would two dipole moments cancel if they are on opposite sides of a tetrahedral molecule? Because they're not exactly in line with each other!

Jessica Booth 2F
Posts: 101
Joined: Fri Aug 30, 2019 12:18 am

Re: Dipole Moments Cancel in Tetrahedral?

Postby Jessica Booth 2F » Fri Dec 06, 2019 10:48 am

No, they would not cancel. The only way to have a nonpolar tetrahedral molecule is if all the atoms attached to the central atom are the same.

Justin Quan 4I
Posts: 104
Joined: Sat Sep 14, 2019 12:17 am

Re: Dipole Moments Cancel in Tetrahedral?

Postby Justin Quan 4I » Fri Dec 06, 2019 12:27 pm

To add on, dipole moments would only cancel if all the surrounding atoms are the same, ex: CH4 is non polar.

Brittney Hun 2C
Posts: 104
Joined: Wed Sep 11, 2019 12:15 am

Re: Dipole Moments Cancel in Tetrahedral?

Postby Brittney Hun 2C » Sat Dec 07, 2019 9:08 am

The tetrahedral shape is never non-polar unless all elements surrounding the central atom are identical. It's easies to see the 3-D shape, and how they would not be able to cancel out.

Diana_Diep2I
Posts: 130
Joined: Sat Aug 17, 2019 12:17 am

Re: Dipole Moments Cancel in Tetrahedral?

Postby Diana_Diep2I » Sat Dec 07, 2019 2:09 pm

If you draw the tetrahedral lewis structure in its actual shape, you would see that they would not cancel due to the vectors pointing upwards or downwards. The structure does not have bond angles of 90º. There would be a net dipole going up or down. For example, CH2Cl2 would still be polar and like the posts above me said, the only time a tetrahedral molecule is nonpolar is when all four atoms attached to the central atom are the same, like CCl4.

HuyHa_2H
Posts: 100
Joined: Wed Sep 11, 2019 12:15 am

Re: Dipole Moments Cancel in Tetrahedral?

Postby HuyHa_2H » Sat Dec 07, 2019 2:39 pm

If you draw out the proper shape, then obviously the molecule will be polar because of dipoles that aren't canceling each other out. So, it's only if the molecules are the same where the dipoles would cancel each other out.


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