ClO2 Lewis Structure

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Victoria Ford 4D
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Joined: Fri Sep 25, 2015 3:00 am

ClO2 Lewis Structure

Postby Victoria Ford 4D » Sun Oct 25, 2015 2:17 pm

On 3.67 Part C, the question asks about the Lewis Structure for ClO2. I understand what the actual question is asking and the answer. My question, however, is when drawing the Lewis Structure, the formal charge on either O is -1 and on Chlorine, +2. Why don't we use double bonds here for the formal charge to be better balanced and achieve a more stable molecule? Can't Chlorine have an expanded octet?

Chem_Mod
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Re: ClO2 Lewis Structure

Postby Chem_Mod » Sun Oct 25, 2015 3:53 pm

Would you be able to post a picture so I can see for sure what you are talking about?

Victoria Ford 4D
Posts: 65
Joined: Fri Sep 25, 2015 3:00 am

Re: ClO2 Lewis Structure

Postby Victoria Ford 4D » Sun Oct 25, 2015 4:56 pm

So the double bond lewis structure was how I drew it in order to have the lowest formal charge.

ClO2 LS - Double Bonds.png
My Answer
ClO2 LS - Double Bonds.png (2.54 KiB) Viewed 2749 times


However, the book shows it with single bonds.

Screen Shot 2015-10-25 at 4.53.22 PM.png
Book's Answer

Shrita Pendekanti 4B
Posts: 22
Joined: Fri Sep 25, 2015 3:00 am

Re: ClO2 Lewis Structure

Postby Shrita Pendekanti 4B » Tue Oct 27, 2015 11:38 am

I believe this is the answer because a structure that includes a radical is not supposed to be of the lowest energy possible. But rather, that unpaired electron is there to make bonds with another atom, which is more likely to happen if Cl has only 2 single bonds and thus has not filled its octet.


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