3.67B and Radicals

[Ramya Natarajan 1D]

In each of these compounds, an atom violates the octet rule. Identify the atom and explain the deviation from the octet rule: b) ClO2

I understand that Cl is the atom violating the octet rule, but I'm confused because there's an odd number of atoms. What would this cause the Lewis structure to look like. Having an odd number of electrons means that one will always be unpaired, so how is this possible? Does this automatically make the molecule a radical?

[sandros]

A radical has an odd number of electrons which leads to its unpaired electron. Therefore, anytime you count the electrons and obtain an odd number, then you can conclude that it is a radical. Hope this answers your question.

[Kelly Kiremidjian 1C]

Yes, this molecule has an odd number of electrons(19). So the two oxygens would both have octets. But there are not enough electrons for chlorine to have an octet. Chlorine then has one lone pair, and one single electron.