CHEM 110 Lecture Notes - Lecture 13: Lone Pair, Valence Electron, Lewis Structure
Document Summary
Covalent bond- electrons of two atoms are shared at the orbital level to complete octets. In lewis structures, shared pairs are dashes and lone pairs are dots. Establish connectivity of the atoms with single bonds. Distribute remaining e- (in pairs) to surrounding atoms to complete octets; leftovers are place on central atom. Make multiple bonds if necessary (use lone pairs to make double/triple bonds) Consider formal charge if multiple structures exist. N(v)= # of valence electrons in an isolated atom. N(ls)= # of electrons on the atom in the lewis structure or lone pair electrons + Smallest formal charge = most stable structure (0 + x 8)= 0. Ex: fc (c)= 4 (4 + x 4)= 0. Fc (o)= 6 (6 + x 2)= 0. Fc (o)= 6 (6 + x 2)= -1. Fc (cl)= 7 - (4 + x 2)= +1 smallest fc.
