C11 - Liquids & IMFs (Gen. Chem 1)

dispersion forces

IMFs between two nonpolar molecules’ temporary dipoles

dipole-dipole forces

IMFs between two dipoles

polarizability

ease of an atom to move its electrons to one side

• increases with more e^- & greater size

Van der Waals forces

dispersion + dipole-dipole

hydrogen bonding

hydrogen atom in a polar bond + lone pair in an electronegative ion/atom (N, O, F)

ion-dipole forces

IMFs between a dipole and an ion

IMF strength (weak → strong)

dispersion → dipole-dipole → hydrogen → ion-dipole → ionic

critical temperature

temperature above which a vapor cannot be liquefied via pressure ↑

critical pressure

pressure required to cause liquefaction @ critical temperature

volatile liquids

liquids which evaporate readily

triple point

three phases in equilibrium