Textbook 2E13C

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

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Connie Liang 3L
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Textbook 2E13C

Postby Connie Liang 3L » Sun Dec 06, 2020 9:00 pm

How come in the Lewis Structure for IO3- all the oxygens are single bond instead of double bonded? With double bonds, the Lewis Structure would still have a charge of -1 and have the same molecular shape.

Gwendolyn Hill 2F
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Re: Textbook 2E13C

Postby Gwendolyn Hill 2F » Sun Dec 06, 2020 9:02 pm

Pretty sure that since I is a larger molecule, the single bond representation is more accurate. I'm sure that having resonance structures combining would give us a bond length somewhere in between, but it might be because single bonds are longer and I is a larger molecule, and double bonds are shorter. That might not be correct, but that's how I might think about it.

Sean Phen
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Re: Textbook 2E13C

Postby Sean Phen » Sun Dec 06, 2020 9:04 pm

I am not exactly sure about this problem because I did not do it yet. But, there are sometimes more than one way that you can make the Lewis structure.

Connie Liang 3L
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Re: Textbook 2E13C

Postby Connie Liang 3L » Mon Dec 07, 2020 3:46 pm

Gwendolyn Hill 3G wrote:Pretty sure that since I is a larger molecule, the single bond representation is more accurate. I'm sure that having resonance structures combining would give us a bond length somewhere in between, but it might be because single bonds are longer and I is a larger molecule, and double bonds are shorter. That might not be correct, but that's how I might think about it.

Thanks Gwendolyn! I just read in the textbook that it's difficult for atoms beyond Period 2 to form double bonds because the atoms are so large that their orbital overlaps are pretty weak. Thanks for your clarification :)


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