O
2NONO
2http://en.wikipedia.org/wiki/Dinitrogen_pentoxideApparently the oxidation state of Nitrogen is V. Why is that? It has five electrons circling it, one set is paired. One of the electrons bonds to the oxygen in the middle of the molecule forming a single bond. (now technically there is resonance between the other two but let's ignore it). Another electron goes to a single bond with one of the oxygen atoms on the end.
Ok, so nitrogen has 3 electrons left circling it, 2 are paired, 1 is unpaired. The final bond to the oxygen is a double bond. The sigma bond grabs the first unpaired electron. The pi bond will grab another electron, unless it grabs both paired nitrogen electrons, but that would be a problem because then there would be 3 electrons (2 from Nitrogen 1 from Oxygen) in the pi bond, as well as 2 in the sigma. Can someone explain this to me please?
Also, the oxygen in the middle would have a -2 oxidation state, while the others would technically be -1.5, correct?