1. States of Matter Solid Liquid Gas definite volume definite shape
regular geometric
pattern
crystalline structure
vibrate in a fixed
location
strong forces of
attraction
Molecules far apart
no definite shape
no definite volume
no force of
attractions
Compressible
Completely fills its
container
Molecules farther
apart
definite volume
no definite shape
intermolecular forces
noncompressible

3. GAS LIQUID SOLID condense Entropy decrease Entropy Increase
Boiling
Evaporation
vaporization
LIQUID
freezing
Crystallization
solidification
Melting
Fusion
SOLID
Sublimation
Phase change from solid to gas
Examples-- CO2(s) I2 (s)
Entropy
amount of disorder
How messy the molecules are
Deposition
Change from a gas to a solid
Example --- snow

4. Phase Diagrams Heating Curve G boiling boiling BP L & G Temp L melting
S & L S
Time (heat added)

5. Melting Point Boiling Point
the temperature at which the solid and liquid phase of a substance are in equilibrium --- also freezing point
Water 0oC
the temperature at which the liquid
and gas phase of a substance are in
equilibrium --- also condensation point
Water 100oC

6. Cooling Curve
L & G
condensation
freezing
Time (heat removed)

7. Average kinetic energy or speed of the molecules Units: C or K
Heat
Temperature
Potential Energy
Average kinetic energy or
speed of the molecules
Units:
C or K
Stored energy
Energy that is contained
within a bond
Energy associated with
phase changes
A form of energy
Units:
Joule
calorie
Heat can be transferred
from one object to
another
Heat flows from hot to
cold ( high temp to
low temp)
Types of energy:
-chemical (bonds breaking/forming)
-mechanical- movement, machine
-electrical- transport of e-’s
-thermal- heat transfer
-nuclear- mass to energy
Exothermic
Endothermic
Release heat or energy
Energy is given off
Absorb heat or energy
Energy is taken in

8. Phase Diagrams Heating Curve  PE No change KE KE No change PE KE
temperature at which the vapor
pressure of the solid equals the vapor
pressure of the liquid
 PE
No change KE G KE
No change PE
boiling BP
L & G
Temp L KE
No change PE
 PE
No change KE
melting MP
S & L S
the temperature at which the vapor
pressure of the liquid equals the
atmospheric pressure above the
liquid KE
No change PE
Time (heat added)

9. Cooling Curve  KE No change PE L & G  KE  PE No change PE
condensation
 KE
No change PE
 PE
No change KE
freezing
 KE
No change PE
 PE
No change KE

10. GAS LIQUID SOLID condense freezing Evaporation vaporization
Boiling
Evaporation
vaporization
Entropy Increase
Entropy decrease
condense
Absorb energy
endo
Release energy
exo
LIQUID
Melting
Fusion
freezing
Crystallization
solidification
SOLID
Sublimation
Phase change from solid to liquid
Examples-- CO2(s) I2 (s)
Entropy
amount of disorder
How messy the molecules are
Deposition
Change from a gas to a solid
Example --- snow

11. Vapor Pressure
The pressure vapor exerts over it’s liquid on a closed system.
The more liquid that evaporates, the higher the vapor pressure!
Vapor pressure is temp. dependent. Up temp = up Vapor Pressure
If no cap- open system- VP= atm pressure

13. Boiling Boiling occurs when atmospheric pressure = vapor pressure.
Increase atmospheric pressure you increase boiling point.
Stronger intermolecular forces = higher BP
A normal boiling point- temperature when something boils at standard pressure kPa.

15. The point at which all 3
states of matter can exist
at the same time
Occurs at the end of the l/g line
Can not distinguish between a
liquid and a gas
Positive: the solid is more dense than the liquid (sink)
Negative: the solid is less dense than the liquid (float)