Solid
FIXED shape and volume
vibrates around a fixed location
Does NOT compress or expand at all
too dense
Can be crystalline: a regular, repeating pattern
or noncrystalline (amorphous)
slightly higher D than liquids
exception: ice = 0.917 g/mL
Does NOT mix by diffusion
cannot mix uniformly this way
Liquid
VARIABLE shape, FIXED volume
does not compress or expand significantly
usually flow readily (viscosity)
Higher D than gases (due to IMF)
water = 1.0 g/mL
If soluble, they mix homogeneously
diffuse more slowly than gases
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Solid
FIXED shape and volume
vibrates around a fixed location
Does NOT compress or expand at all
too dense
Can be crystalline: a regular, repeating pattern
or noncrystalline (amorphous)
slightly higher D than liquids
exception: ice = 0.917 g/mL
Does NOT mix by diffusion
cannot mix uniformly this way
Liquid
VARIABLE shape, FIXED volume
does not compress or expand significantly
usually flow readily (viscosity)
Higher D than gases (due to IMF)
water = 1.0 g/mL
If soluble, they mix homogeneously
diffuse more slowly than gases
Gas
INDEFINITE shape and volume
Can expand a lot!
V increases as V of container increases
Can compress a lot!
if compressed enough, it will liquify and D increases
have low D
due to the space between the particles
air = 0.001 g/mL (at sea level)
mix completely with other gases in a container
Boiling Point
the temp at which a liquid will vaporize into a gas
atmospheric pressure equal to vapor pressure
freezing point
temperature at which a substance transitions from a liquid state to a solid state
melting
solid to liquid
T increases
freezing
liquid to solid
T decreases
sublimination
solid to gas
P decreases
deposition
gas to solid
P increases
evaporation
liquid to gas
P decrease
condensation
gas to liquid
P increases
kinetic energy
the energy an object has due to its motion
potential energy
the stored or pent-up energy of an object
temperature
a measure of the AVERAGE KINETIC ENERGY of a sample
pressure
a measure of the COLLISION OF PARTICLES
normal boiling point
the temperature at which the vapour pressure is equal to the standard sea-level atmospheric pressure (1 atm)
vaporization
conversion of a substance from the liquid or solid phase into the gaseous (vapour) phase
Evaporation and boiling
vapor pressure
the pressure exerted by vapor just above the surface of a liquid that is at its boiling point
atmospheric pressure
the force per unit area exerted by an atmospheric column above a specified area
critical point
the temp above which the gas cannot be liquified no matter how much pressure is applied
(the kinetic energy simply is too great for attractive forces to overcome)
triple point
the condition of temperature and pressure where ALL THREE phases exist in equilibrium
viscosity
the resistance of a liquid to flow
more viscous = stronger IMF
ex. honey
surface tension
energy required to increase the surface area of a liquid by a given amount
inward pull by particles in the interior of a liquid
stronger IMF = greater surface tension
drops on a penny
DIPOLE-DIPOLE
polar covalent molecule
result from the attraction of the + and - ends
‘DI’pole = 2 poles
opposite poles align to maximize attraction and minimize repulsion
unequal distribution of electron density within the molecule
london dispersion forces
exist between ALL atoms and molecules
if a molecule has electrons, it has LDFs
nonpolar molecule
ONLY has LDFs
an instantaneous/temporary dipole results from an unequal sharing of electrons.
one particle with an instantaneous (or temporary) dipole will affect other particles adjacent to it producing a short-range attractive interaction
what makes LDFs stronger
LARGER MOLAR MASS
larger particles
more electrons present
more polarizable electron clouds
stronger the force of attraction
what makes dipole-dipole stronger
larger dipole
stronger the force of attraction between the 2 molecules
hydrogen bonding (BINDING)
includes F, N, O
FORCE, not a bond!
when H atoms that are already covalently bonded to highly EN atoms (F,N,O) are also attracted to the - end of a dipole formed by the EN atom in a DIFFERENT molecule
or a different part of the same molecule
* INTERNAL OH TO ANOTHER OH
order of strength for intermolecular forces
LDF → dipole-dipole → H-bonding → ion-dipole
volatility
How readily a substance vaporizes.
intramolecular forces
exist within a molecule
is a BOND (ionic, PC, NPC)
stronger than intermolecular forces
intermolecular forces
exist between 2+ molecules
is a FORCE
the specific structure and size of the particles involved can play an important part in determining the overall strength of particular IMFs
weaker than intramolecular forces