II Exam 1 Flashcards
(31 cards)
phase change: solid to liquid
melting
phase change: liquid to solid
freezing
phase change: liquid to gas
vaporization
phase change: gas to liquid
condensation
phase change: solid to gas
sublimation
phase change: gas to solid
deposition
vaporization
– if you increase temp, what happens to kinetic energy?
KE increases
vaporization
– if you increase intermolecular forces, what happens to kinetic energy?
greater KE needed for molecule to escape surface
if you have stronger cohesion forces, what happens to vapor pressure?
lower vapor pressure
if you have weaker cohesion forces, what happens to vapor pressure?
higher vapor pressure
relationship between temperature and vapor pressure
proportional
relationship between boiling point and vapor pressure
inversely proportional
relationship between boiling point, cohesion forces, and vapor pressure
the higher the boiling point, the stronger cohesion forces will be, and the lower the vapor pressure will be
during a phase change, is there an increase in temperature?
no
phase change diagrams
– at high temp and lower pressure, what is the phase?
gas
phase change diagrams
– at low temp and higher pressure, what is the phase
solid
intermolecular forces
– does a larger charge increase or decrease attraction?
increase
*relative to the bonding forces among atoms
intermolecular forces
– does a longer distance increase or decrease attraction?
decrease
*relative to the bonding forces among atoms
dispersion forces
- weakest intermolecular force
- present in all atoms and all molecules
dipole-dipole
intermolecular force present in polar molecules
- only exist in a picture (not a pure substance)
hydrogen bonding
intermolecular force in molecules containing H bonded to F, O, or N
ion dipole
a full change, either positive or negative
- charge is a greater factor than size when determining the strength
if we increase mass, does intermolecular forces increase or decrease?
increases
body-centered atom in 1 unit cell
1 atom
