Chapter 10 Flashcards
solid
high density
very limited freed om of motion
strong IMFs
liquid
high density
some freed om of motion
moderate strength of IMFs
gas
low density
complete freedom of motion
weak IMFs
intermolecular forcesq
attractive forces that exists between molevules and atoms
four types of intermolecular forces
- dispersion forces
- dipol-dipole forces
- hydrongen bonding
- ion-dipole forces
dispersion forces(london forces)
exhibited by all atoms and molecules that results from rapid flutuating, temporay diples
induced dipole
temporary dipole formed when the electrons of an atom or molecule are distored by the instantaneous dipole of a neighboring atom or molecule
effects of molar mass on dispersion forces
larger the molar mass= stronger the attraction
effects of shape of molecule on dispersion forces
larger surface = stronger attraction
dipersion factors effect boiling point
strong dispersion forces = high boiling point
weak dispersion force= low boiling point
dipole-dipole forces
an IMF presented only in polar molecules
stronger than dispersion forces
polar bonds
electronegativity difference is (0.5-1.7)
for a molecule to be polar it must have
- polar bonds(large electronegativity differnece)
2. asymmetrical shape; polar bonds do not cancel out
nonpolar molecule with identical polar bonds
linear
trigonal planar
tetrahedral
polar molecule with polar bonds
bent
trigonal pyramidal
hydrogen bonding
present when polar molecules containg h atoms bodn directly to small and highly electronegative f, o, or n atoms
(stonger than dipole-dipole and dispersion forces)
ion-dipole forces
occurs when an ionic combound is mixed with a polar compound
stronger than any other Imfs
threee manifestation of imfs
- viscosity
- surface tension
- capillary
viscosity
measure of aliquid resisytance to flow
how imf effects viscosity
stonger imf= higher viscosity
how temperatuire effects viscosity
higher temperature= lower viscosity
surface tension
the energy required to increase the surface area of a liquid by a unit amount
how imfs effect surface tension
higher IMFs=higher surface tension
how temperature effects surface tension
higher temperature = lower surface tension
vaporization
liquid to gas
endothermic process
heat of vaporization
the amount of heat required to vaporize one mole of a liquid to gas; always positive
condensation
gas to liquid
exothermic process
enrgy is released
heat of condensation
the amount of heat released when one mole of a gas condenses to liquid; always negative
the rate of vaporization increases with
increasing temperature
increasing surface area
decreasing strength of intermolecular forces
dynamic equilibriun
state of a system in which reciprocal process are occuring at equal rates
the double arrou indicates a dynamic equilibrium
vapor pressure
pressure exterted bya a vapor in equilbrium witha solid or liquid at a given tenperatur in a clsoed system
how IMFs affect bapor pressure
weaker IMFs= higher vapor pressure
how temperature affects vapor pressure
higher temperature- higher vapor pressure
boiling point
is the temp. at which the vapor pressure of a liquid equals the pressure of a gas above it
how imf effect boiling point
stronger IMFs = higher boiling point
normal boiling point
the temp. at which it vapor pressure equals 1 atm
sublimation
the phase transition from solid to gas
deposition
the phase transition from gas to solids
melting/fusion
solid to liquid
melting point
temp at which the solid and liquid pahses of a substace are in equilibirum
freezing
liquid to solid
phase diuagram
presuure - temperature
y-x
sumeraizing condition under the pahses of a substance can exist
regions
the three main regions- solid, liquid, and gas- represent conditions where that particular state is stable
lines
the substances are in equalibrium between the two states on wither side of the line
both states coestist, and equally stable
triple point
temperature and pressure at which the vapor, liquid, and solid, phases of a substance are in equilibrium
