TERM 1
Intermolecular Forces
DEFINITION 1
different from bondsattractive forces between
moleculesweaker than chemical bonds (ionic &
covalent)determines properties of matter (viscosity, melting
point, etc)4 types:
dipole-dipole forces
ion-dipole forces
dispersion forces
hydrogen bonding (not actually bond)
TERM 2
Dipole-Dipole Forces
DEFINITION 2
exists between polar molecules (with dipole moment)weaker
than hydrogen bondingstronger than non-polar forcesex:KCl,
BrF, SO2
TERM 3
Ion-Dipole Forces
DEFINITION 3
exists between ion and polar moleculestronger than
hydrogen bonds (strongest IM forces)cations (+) form
stronger force than anions (-)... ions with higher charges form
stronger forces because there's more space
TERM 4
Dispersion Forces
DEFINITION 4
exist in all types of molecules and ato ms, but most significant in
non-polar moleculesweakest o f the IM forces
induced dipole-induced molecule- 2 non-polar molecules form
dispersion forces
ion-induced dipole forces- an ion and a non-polar molecule for m
dispersion forces
dipole-induced dipole forces- a polar molecule and a non-polar
molecule form dispersion forces
TERM 5
Hydrogen Bonding
DEFINITION 5
type of dipole-dipole force (though stronger)different and
weaker than covalent bond, slightly weaker than ion-dipole
forcesforms between hydrogen in a polar bond and an
electronegative atom (only N, O, or F) in another molecule
