2.  1. count the total electrons by adding the valence electrons of each atom (if there is a charge add or subtract electrons to account)

3.  2. arrange the peripheral atom symbols around the central atom and place 1 pair of valence e- between each atom

4.  3. place more pairs of valence electrons on all the peripheral atoms to complete their octets (using the remaining electrons)

5.  4. Place any remaining electrons on the central atom as lone pairs

6.  5. if the central atom’s octet is not complete, move a lone pair from a peripheral atom to a new position between that atom and the central (creating double bonds)

7. Valence Shell Electron Pair Repulsion Theory

8.  valence electrons surrounding an atom mutually repel each other and therefore all molecules adopt an arrangement to minimize repulsion

9.  1. only the valence electrons of the central atom are important to molecular shape

10.  2. valence electrons are paired in a molecule of polyatomic ion

11.  3. bonded pairs of electrons and lone pairs of electrons are treated approximately equally

12.  4. valence electron pairs repel each other electrostatically

13.  5. the molecular shape is determined by the positions of the electron pairs when they are a maximum distance apart