In Class Example, Re: radicals, NO


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Maria Trujillo 1L
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Joined: Fri Apr 06, 2018 11:05 am

In Class Example, Re: radicals, NO

Postby Maria Trujillo 1L » Sun May 13, 2018 10:07 pm

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
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Re: In Class Example, Re: radicals, NO

Postby Chem_Mod » Sun May 13, 2018 10:09 pm

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
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Re: In Class Example, Re: radicals, NO

Postby Emma Leshan 1B » Wed May 16, 2018 3:14 pm

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


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