In Class Example, Re: radicals, NO

[Maria Trujillo 1L]

In class we were given the example of NO and the Lewis structure given the formal charge. Although we were not given the formal charge, we end up with N+ and O-, and because of that we know to fill O and leave N with only five e- dots. However, we are given the counterexample where the reverse is done. O only has 5 e- dots and N is filled which then gives us the charges: N- and O+2. My question is why is the counterexample incorrect?

[Chem_Mod]

No. The most stable structure for radical NO is a double bond between N and O, N having 1 lone pair of electrons and the lone electron while O has 2 lone pairs of electrons

[Emma Leshan 1B]

Remember that O always has an octet because of its high electronegativity, and that should help.