Editing Lewis structure (section)

== Formal charge ==
{{Main article|Formal charge}}
In terms of Lewis structures, [[formal charge]] is used in the description, comparison, and assessment of likely [[topology|topological]] and [[Resonance (chemistry)|resonance]] structures<ref name="miessler_1">Miessler, G. L. and Tarr, D. A., ''Inorganic Chemistry'' (2nd ed., Prentice Hall 1998) {{ISBN|0-13-841891-8}}, pp. 49–53 – Explanation of formal charge usage.</ref> by determining the apparent electronic charge of each atom within, based upon its electron dot structure, assuming exclusive covalency or [[non-polar]] bonding. It has uses in determining possible electron re-configuration when referring to [[reaction mechanism]]s, and often results in the same sign as the [[partial charge]] of the atom, with exceptions. In general, the formal charge of an atom can be calculated using the following formula, assuming non-standard definitions for the markup used:

:<math>C_f = N_v - U_e - \frac {B_n} 2 </math>
where:
* <math>C_f</math> is the formal charge.
* <math>N_v</math> represents the number of valence electrons in a free atom of the element.
* <math>U_e</math> represents the number of unshared electrons on the atom.
* <math>B_n</math> represents the total number of electrons in bonds the atom has with another.

The formal charge of an atom is computed as the difference between the number of valence electrons that a neutral atom would have and the number of electrons that belong to it in the Lewis structure. Electrons in covalent bonds are split equally between the atoms involved in the bond. The total of the formal charges on an ion should be equal to the charge on the ion, and the total of the formal charges on a neutral molecule should be equal to zero.