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

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Abigail Volk 1F
Posts: 52
Joined: Fri Sep 29, 2017 7:07 am
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Postby Abigail Volk 1F » Tue Dec 05, 2017 11:56 pm

The questions says, "what is the shape of the ClO2+ ion? what is the expected OClO bond angle?" I'm still slightly confused on how to determine bond angles. Can you use the example in the question to explain how to determine the bond angle? thanks

Alexander Peter 1F
Posts: 20
Joined: Wed Jun 28, 2017 3:00 am

Re: 4.5

Postby Alexander Peter 1F » Wed Dec 06, 2017 12:18 am

First off, assuming you had no problem creating the Lewis Structure, you'd see that Cl is the central atom with two double bonds to each O, and one lone e- pair. This shows that there are three e- densities around Cl, and they want to be as far apart as they can from one another. The shape that would be made because of this fact is a trigonal planar, with each angle being 120 degrees. However, the lone e- pair has stronger repulsion and is pushing the other two O away from it, creating a bond angle between the O atoms slightly smaller than 120 degrees. A helpful chart I've used to understand the pattern on how electron densities determine molecule shape can be found here: http://images.tutorvista.com/cms/images ... ecules.png

Camille 4I
Posts: 57
Joined: Sat Aug 24, 2019 12:18 am

Re: 4.5

Postby Camille 4I » Sun Nov 10, 2019 10:32 pm

Do lone pairs have more repulsion than double bonds?

Kaylee Sepulveda 4G
Posts: 100
Joined: Thu Jul 11, 2019 12:16 am

Re: 4.5

Postby Kaylee Sepulveda 4G » Mon Nov 18, 2019 7:04 pm

Camille 4I wrote:Do lone pairs have more repulsion than double bonds?

Yes, the strength of repulsion goes
lone pair-lone pair > lone pair-bonding pair > bonding pair-bonding pair

Shrayes Raman
Posts: 129
Joined: Sat Jul 20, 2019 12:15 am

Re: 4.5

Postby Shrayes Raman » Mon Nov 18, 2019 10:52 pm

Since the lewis dot structure show a lone pair on the Cl there will be a repulsion from the lone pair causing a 120 degree bent shape.

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