Dipole Moment

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

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Dipole Moment

Postby Maria1E » Wed Dec 06, 2017 3:03 pm

How do we go about determining if there is a dipole moment when the central atom has lone pairs on it?

For example, why would KrCl4 (which has 2 pairs of lone electrons on the K) have no dipole moment, while IF5 (which has one pair of lone electrons on the I) has a dipole moment?

Yifei Wang 3G
Posts: 19
Joined: Fri Sep 29, 2017 7:07 am

Re: Dipole Moment

Postby Yifei Wang 3G » Wed Dec 06, 2017 3:59 pm

try to look at the geometry of the molecule. From the structure, you can see the lone pair is occupying more space than a bond would, therefore the angle is slightly altered and the dipole moment cannot cancel out.

Kevin Morden 1E
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Re: Dipole Moment

Postby Kevin Morden 1E » Wed Dec 06, 2017 6:15 pm

KrCl4 is square planar, meaning that the dipole of all four chlorines will essentially cancel each other out because there are on the same plane. On the other hand, IF5 is square pyramidal, restricting all of the dipoles from canceling because the octahedral contains one lone pair.

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