ClO2 Lewis Structure

[Victoria Ford 4D]

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]

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

[Victoria Ford 4D]

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

My Answer

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

However, the book shows it with single bonds.

Book's Answer

[Shrita Pendekanti 4B]

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.