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In Class Example, Re: radicals, NO

Posted: Sun May 13, 2018 10:07 pm
by 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?

Re: In Class Example, Re: radicals, NO

Posted: Sun May 13, 2018 10:09 pm
by 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

Re: In Class Example, Re: radicals, NO

Posted: Wed May 16, 2018 3:14 pm
by Emma Leshan 1B
Remember that O always has an octet because of its high electronegativity, and that should help.