How do I determine Formal Charge?

[Rogelio Bazan 1D]

So I understand that the equation for the formal charge is the following:
Formal Charge = [# valence electrons on neutral atom] – [(# lone electron pairs) + (½ # bonding electrons)]

What I don't understand is that yes the best formal charge should be the 0 (zero) but there are times in which the octet rule is overruled like the examples in class. I feel like this is what is confusing me the most and I would like some clarification. Thanks. -Roger

[Chem_Mod]

Even for the expanded octet structures and octet exception structures, the equation for the formal charge is still the same.

[Hannah Lee 1B]

Yes, ideally you would try to draw the molecule in such a way that the formal charge of each atom is 0. However, in cases like an odd number of electrons (ex. NO),
incomplete octets (ex. BF3), or expanded valence shells (atoms with 3d and up), the octet rule can be broken and the formal charges can be not zero, as long as they add up to the molecule's charge.