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CHEMISTRY
UNIT 8: Solid, Liquid, & Gas
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Kinetic Molecular Theory
how matter is composed of small particles that are in constant random motion that has spaces between them.
KMT:
Gas molecules move very
fast
in straight-line paths.
Kelvin
temperature is proportional to the
average Kinetic Energy.
The space between molecules is very
far.
Gas collisions are
elastic.
Forces of attraction are
negligible.
Assumption of KMT in Gas:
indefinite
shape and volume
weak attraction
between molecules
free
random motion
Assumptions of KMT in Liquid:
definite
volume
but indefinite
shape.
molecules have enough
energy
to slide over one another.
attraction of particles are
stronger
than gas.
Assumptions of KMT in Solid:
definite
shape and volume.
tightly
packed
together and organized.
very strong attractive forces.
Surface Tension
force that causes the molecules on the surface of a liquid to be pushed together and form a layer.
Viscosity
resistance of a fluid to flow.
Vapor Pressure
measure of the tendency of a material to change into the gaseous or vapor state.
Boiling Point
temperature at which any liquid starts to boil.
Heat of Vaporization
amount of heat needed to vaporize.
Properties of Water:
High
Boiling Point
High
Specific Heat
Contracts
when cool
High
Heat of Vaporization
High
Surface Tension
Boiling point of water (in deg C)
100
Specific Heat of Water (in J/kg deg C)
4182
Capillary Action
ascension of liquid thru a tube.
Cohesion
attraction of molecules of the SAME kind.
Adhesion
attraction of molecules of the DIFFERENT kind.
Crystalline
Solids
atoms in the molecules are equally the same size, takes up less spaces, and has high ordered structure.
Amorphous
Solids
unequal sized molecules, takes up more spaces, less compact, irregular shape and order of atoms.
Volatile
liquids that evaporate easily
Allotrope
element exists into
two
or more forms w/o
changing state.
Latent heat of fusion
amt of heat that is absorbed by a solid as it
melts
to
liquid
Graham's Law of Diffusion
rate of diffusion is inversely proportional to the square root of their molecular weights.
Boyle's Law
pressure is inversely proportional to its volume.
Charles' Law
volume is directly proportional to its temperature.
Gay-Lussac's
Law
pressure is directly proportional to its temperature.
Avogadro's Law
volume is directly proportional to the number of molecules
Dalton's Law of Partial Pressures
the total pressure exerted by the mixture of gases is equal to the sum of the partial pressure of each gas.
This equation represents
Combined Gas Law.
This equation represents
Ideal Gas Law.