All right, guys. So it turns out that there were no neutral structures, so I couldn't use the neutral rule. All of these molecules fulfilled their octets, so I couldn't use the octet rule. But we had differences in electronegativity. It turns out that the O being with a negative charge is going to be more stable. So that would be my major contributor. Why? Because it turns out that O is more electronegative, I'm just going to use "for electronegative," than N. What that means is that oxygen is more comfortable having that lone pair on it than nitrogen is. So this would be less electronegative. Because of that, this is going to be the minor contributor. So when I go ahead and draw my resonance hybrid, we can draw it the same exact way, but we have to acknowledge that, let's say that I'm drawing it like this, NCO, partial bond, partial bond.
One of the ways that we could draw this is we could draw the partial negative on the O bigger. So we draw a bigger partial negative on the O and a smaller partial negative on the N. Why is that? Because remember, we just said that even though both of these could exist, the negative on the O is going to be the most stable. So that means that most of the time it's going to look more like this one—sorry, that kind of got blurry—more like this one and less like the other one. So this means that my hybrid would be a bigger share of the major contributor. Does that kind of make sense?