1. Chapter 3 – States of Matter

2. 3.1 Solids, Liquids, and Gases
Definite Shape
Definite Volume
Particles vibrate in fixed positions
Particles have low kinetic energy

3. Liquids Variable shape (takes the shape of the container)
Definite Volume
Particles can move around each other
Particles have medium Kinetic Energy

4. Gases Variable shape Variable volume (fills all space in a container)
Particles move about freely
Particles have high Kinetic Energy

5. Bose-Einstein Condensate
Plasma
Exists only at extremely high temperatures
99% of the matter in the UNIVERSE is plasma
Stars are plasma
Bose-Einstein Condensate
Exists only at extremely low temperatures
Groups of atoms behave as a single particle

6. Kinetic Theory Kinetic energy = energy an object has due to its motion
The faster an object is moving; the greater its kinetic energy.
Kinetic theory states that all particles of matter are in constant motion.
** View animation on visual concepts CD

7. 3.2 The Gas Laws
Pressure = the result of force distributed over an area
In a closed container, gases exert pressure when the particles of the gas collide with the walls of the container.

8. Factors That Affect Gas Pressure
Temperature – raising temp. will increase pressure if volume of gas and # of particles are kept constant
Inc. in temp.  part. move faster  part. collide with walls more frequently  increased pressure

9. Volume – Decreasing volume of a gas causes an increase in pressure if the temp. and # of part. are constant
Decrease in vol.  less space  particles collide with walls more often  inc. pressure

10. Number of particles – increasing the number of particles of a gas will increase pressure if temp. and volume are constant
Inc. # of particles  particles collide with container more often  inc. pressure

11. Gas Laws
Charles’ Law – volume of a gas is DIRECTLY PROPORTIONAL to temperature
Note: Temperature must be in Kelvins.
V1 = V2
T T2

13. Boyle’s Law – volume of a gas is INVERSELY PROPORTIONAL to pressure
For Example: Increase Volume x2 
Decreased pressure by ½
P1V1 = P2V2

15. The Combined Gas Law – relates temperature, volume and pressure of a gas.
P1V1 = P2V2
T T2

16. 3.3 Phase Changes
Phase change – reversible physical change that occurs when a substance changes from one state of matter to another
Temperature of a substance DOES NOT CHANGE during a phase change.
Energy is either absorbed or released during a phase change.
Endothermic – energy is absorbed
Exothermic – energy is released

17. Melting and Freezing Melting Solid changes to liquid
Particles absorb energy (endothermic)
Particles become less orderly

18. Freezing Liquid changes to solid Particles release energy (exothermic)
Particles become more orderly

19. Vaporization and Condensation
Liquid changes into a gas
Particles absorb energy (endothermic)
Particles become LESS orderly and more free to move
2 types of vaporization
Evaporation – takes place at the surface of a liquid
Boiling – occurs when a liquid is heated to its boiling point

20. Condensation Gas changes to a liquid
Particles release or lose energy (exothermic)
Particles become MORE orderly

21. Sublimation and Deposition
Changing from a solid
directly to a gas
Energy is absorbed
(endothermic)
Deposition
Changing from a gas directly to a solid
Energy is released (exothermic)

23. Phase Change Diagram