1. 3.1 Solids, Liquids, and Gases
1. Kinetic Theory = all particles of matter are in constant motion
2. States of Matter
A. Solids
strong attractions between particles in a solid
Usually have an orderly arrangement of particles
Particles vibrate around fixed locations
Have a definite shape and volume

2. B. Liquids
Particles in a liquid are not as affected by forces of attraction
Particles are close together, but their arrangement is more random
The average speed of a particle is faster than in a solid
Liquids have a definite volume but not shape

3. Particles have a lot of space between them, arrangement in random
C. Gases
At room temperature, particles in a gas move approximately 450 m/s on average
Particles have a lot of space between them, arrangement in random
Particles are unaffected by other particles unless they collide
Forces of attraction can be ignored
Have neither a definite volume nor shape

4. D. Plasmas
Exist at high temperatures
Form 99% of all matter in the universe
Occur when atoms are stripped of their electrons
Are gases consisting of nuclei and electrons

5. Force distributed over an area P = F/A More force, more pressure
Gas law lab
3.2 The Gas Laws
1. Pressure
Force distributed over an area P = F/A
More force, more pressure
More area, less pressure
Measured in pascals (Pa) or kilopascals (kPa)
2. Gas Pressure
Caused by collisions between gas and walls of the container

6. 3. Volume
If you decrease volume then you:
increase number of collisions
increase pressure

7. 4. Boyle’s Law
If temperature is kept constant then pressure is inversely proportional to volume
PV = constant
P1V1 = P2V2

8. 5. Temperature
If you increase temperature then you:
increase kinetic energy
increase speed of particles
increase number of collisions
increase pressure

9. 6. Charles’s Law
If pressure is kept constant, then volume is directly proportional to temperature (in Kelvin)
V/T = constant
V1/T1 = V2/T2

10. 7. Number of Particles
If you increase the number then you:
increase collisions
increase pressure

11. If the number of particles is kept constant then:
Vacuum, Handboiler, Soda can
Cartesian
8. Combined Gas Law
If the number of particles is kept constant then:
PV/T = constant
P1V1/T1 = P2V2/T2

12. May be exothermic or endothermic
Phase change lab
3.3 Phase Changes
When a substance changes from one state of matter to another, reversible
May be exothermic or endothermic
Exothermic = energy released
Endothermic = energy absorbed
Involves NO change in temperature
Energy is involved in breaking or forming bonds

13. A. Melting (solid to liquid)
Endothermic
Heat of fusion = energy absorbed as a substance melts (J/g)
Used to break bonds/attractions between molecules, NOT to raise temperature
Heat of fusion lab

14. B. Freezing (liquid to solid)
Exothermic
Freezing water makes rigid bonds and makes ice less dense

15. C. Vaporization (liquid to gas)
Endothermic
Heat of vaporization = energy absorbed as a substance vaporizes (J/g), used to break bonds
Vapor pressure = pressure caused by collisions of vapor with walls of a container

16. 1. Evaporation
Occurs at the surface of a liquid
Below the liquid’s boiling point
Some particles have enough energy to escape the liquid
2. Boiling
Occurs below the surface
Some particles have enough energy to escape the attraction of nearby particles and form a bubble of vapor that rises
Occurs when vapor pressure equals atmospheric pressure

17. D. Condensation (gas to liquid)
Exothermic (ex. Dew)
E. Sublimation (solid to gas)
Endothermic (ex. Dry ice)
F. Deposition (gas to solid)
Exothermic (ex. Frost on window)

18. Dippy Duck, vacuum boil