1. Chapter 3 – States of Matter

2. 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.

3. 3.1 Solids, Liquids, and Gases
Definite Shape
Definite Volume
Particles vibrate in fixed positions
Particles have low kinetic energy

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

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

7. Other states of matter 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

9. Day 2

10. 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.
More Collisions=More Pressure
Forces of attraction among gas particles so weak they can be ignored under ordinary conditions

11. Which shoes create the most pressure?

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

13. Volume – Decreasing volume of a gas causes an increase in pressure if the temp. and # of particles are constant
Decrease in vol.  less space  particles collide with walls more often  increase pressure
Factors That Affect Gas Pressure Cont…..

14. Factors That Affect Gas Pressure Cont…..
Number of particles – increasing the number of particles of a gas will increase pressure if temp. and volume are constant
Increase # of particles  particles collide with container more often  increase pressure

15. Charles’ Law
The volume and absolute temperature (K) of a gas are directly related
at constant mass & pressure
V1 = V2
T T2 V T

16. Boyle’s Law
The pressure and volume of a gas are inversely related
at constant mass & temp
P1V1 = P2V2

17. PV T V T P T PV = k P1V1 T1 = P2V2 T2 P1V1T2 = P2V2T1
Combined Gas Law PV T V T P T PV
= k
P1V1 T1 =
P2V2 T2
P1V1T2 = P2V2T1

19. Day 3

20. 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

21. Melting and Freezing Melting Solid changes to liquid
Particles absorb energy (endothermic)
Particles become less orderly
Heat of fusion- energy a substance must absorb in order to change from solid to liquid
Freezing
Liquid changes to solid
Particles release energy (exothermic)
Particles become more orderly

22. 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

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

24. 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)

26. Phase Change Diagram