- #1
Qube
Gold Member
- 468
- 1
Homework Statement
Is N triple bond O with a radical on oxygen a valid LS for the nitric oxide molecule?
Homework Equations
Max number of valence electrons in a shell - 2n2.
Oxygen is in second row of periodic table. Max valence electrons: 2(2)2 = 8.
The Attempt at a Solution
I remember once I got reprimanded by my teacher for drawing some nitrogen-based molecule with five bonds afforded to nitrogen in a vain attempt to make nitrogen's formal charge 0. Unfortunately, nitrogen doesn't form five bonds regularly. Nitrogen isn't a hypervalent molecule. Nitrogen is in the second row of the periodic table and accessing the extra orbitals needed to form more than 4 bonds doesn't happen on a regular basis.
However, my teacher recently drew this depiction of the nitric oxide molecule and says it's a valid LS.
Uh, what?
Your thoughts, please. I understand that oxygen does have empty d-orbitals, and for that matter, empty f-orbitals, but really? Oxygen forming a triple bond on top of having a radical and a lone pair? How legit is the latter LS below?
http://i.minus.com/jHCK0jK0k7uVu.png
Last edited by a moderator: