
1. count the total
electrons by adding the
valence electrons of
each atom (if there is a
charge add or subtract
electrons to account)

2. arrange the
peripheral atom symbols
around the central atom
and place 1 pair of
valence e- between each
atom

3. place more pairs of
valence electrons on all
the peripheral atoms to
complete their octets
(using the remaining
electrons)

4. Place any remaining
electrons on the central
atom as lone pairs

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)
Valence Shell Electron Pair
Repulsion Theory

valence electrons
surrounding an atom
mutually repel each
other and therefore all
molecules adopt an
arrangement to
minimize repulsion

1. only the valence
electrons of the central
atom are important to
molecular shape
 2.
valence electrons are
paired in a molecule of
polyatomic ion

3. bonded pairs of
electrons and lone pairs
of electrons are treated
approximately equally

4. valence electron
pairs repel each other
electrostatically

5. the molecular shape
is determined by the
positions of the electron
pairs when they are a
maximum distance apart