1) Count the total number of valence electrons for the molecule

2) The first element listed in the central element (UNLESS it's hydrogen or a tri-atom)

3) Draw the central atom and disperse the others around it, connect each with a single bond ( -2 electrons for every bond)

4) Satisfy octets for outer atoms first and disperse remaining electrons as lone pairs on the central atom

5) If there's any unpaired electrons on the central atom and an outer atom, 'push' electrons to the bonding region to create double/triple bonds to make as many octets as possible

6) determine the formal charges of each atom to determine the most stable Lewis structure

- If a molecule has a charge symbol on it, add/subtract 1 electron from the total v.e for every +/- and draw brackets around the entire structure with the charge outside in the upper right corner

Review: Chapter 5 - Electronegativity, bond polarity, and Lewis structures