Looks like no one added any tags here yet for you.
Formal charge
Valence electrons-electrons in lone pairs-# of bonds
why sulfur and phosphorus are exceptions
because they can surpass the octet rule; this is because they have empty d orbitals that can be filled with extra electrons, giving rise to the possibility of an expanded octet
Resonance structures
molecular/ionic compounds with more than 1 possible lewis structure
linear molecular geometry
if there are 2 atoms bonded to the central atom and zero lone pairs
180 degrees
linear molecular geometry
if there are only 2 atoms; can’t make a shape
180 degrees
bent molecular geometry
if there are 2 atoms bonded to the central atom and one lone pair
a little <109.5 degrees
bent molecular geometry
if there are 2 atoms bonded to the central atom and 2 lone pairs
a little <109.5 degrees
trigonal planar molecular geometry
if there are 3 atoms bonded to the central atom and 0 lone pairs
120 degrees
trigonal pyramidal molecular geometry
if there are 3 atoms bonded to the central atom and 1 lone pair
a little <109.5 degrees
tetrahedral molecular geometry
if there are 4 atoms bonded to the central atom and 0 lone pairs
109.5 degrees
london dispersion intermolecular forces
in all molecules
dipole-dipole intermolecular forces
in polar molecules
hydrogen bonding intermolecular forces
in polar molecules with H-F, H-O, H-N bonds
compound is nonpolar if
the central atom has 0 lone pairs
all atoms around central atom are the same
dipole moments
they point toward the most electronegative molecules
bond polarity is toward the more electronative atom
molecular polarity is the overall dipole moment
If the electronegativity is
<0.4, it is
nonpolar
If the electronegativity is
0.4-1.7, it is
polar
If the electronegativity is
>1.7, it is
ionic