I've recently entered the wonderful world of O-Chem and seem to have some issues with resonance. I understand that it's just another way of looking at where electrons are, but I have some issues moving them around properly.
For example: N3CH3

CH3-N=N=N
+ -
I look at something like this and am so confused. Where do I move the electrons? Do I take from the nitrogen on the end and move it to the one in the middle to result in no weird charges, or do I do something else?

Any help would be AMAZING!!

Uh, what do you mean by move the electrons? :confused:

I mean the charges, or something... I have no idea. At this point I'm kind of just going with it. Lol

Oh and I just noticed that the positive charge is supposed to be on the middle nitrogen, and the negative on the end one.

(I have never seen that compound, but I'll try)

If I understand your question well...

You will notice that the middle N atom has four bonds, hence it is very unstable.

(I'll talk about outermost electrons only to simplify things)
This nitrogen has initially 5 electrons, then bonding doubly with the adjacent N atoms, it now has got 9 electrons, too much for it to hold and the right N atom has 7 electrons total. The molecule therefore donates that extra electron from the middle N atom to the right N atom, so that both have an octet of electrons (stability). It's some sort of de-localisation I guess. Since the middle N lost an electron, it becomes +ve and the riht electron becomes -ve as it has received an electron.