1. Chemistry: Chapter 3
States of Matter

2. Phases of Matter
4 phases
Solid,
Liquid,
Gas,
Plasma,

3. Molecules packed closely together
Solid
Low kinetic energy because the molecules don’t have room to move.
Definite volume
Definite shape

4. Molecules move more freely, but close together
Liquids
Definite volume
No definite shape (Takes shape of container)
Medium kinetic energy

5. Viscosity  Resistance of a liquid to flow.
Liquids
Ex. Honey, Oil

6. Molecules are far apart and can move freely
Gas
No fixed volume
No definite shape (Takes shape of container)
High kinetic energy (more movement = more kinetic energy)

7. Particles have extremely large amounts of energy.
Plasma
Particles have extremely large amounts of energy.
Can be thought of as a gas consisting of electrons instead of atoms.
Most common phase of matter in the universe.
Short video on plasma

8. Interactive game on states of matter

9. Kinetic theory
Kinetic theory
1. All matter is composed of small particles. (atoms, molecules, etc.)
2. Particles are in constant, random motion.
3. These particles are colliding with each other and the walls of their container.

10. Particles are in random, constant motion.
The motion of the particles is unaffected unless they collide with one another.
Forces of attraction among particles in a gas can be ignored under ordinary conditions.
Kinetic Theory of Gases

11. Video on states of matter

12. The force distributed over an area.
SI unit: Pascal
Collisions between gas particles causes the pressure in a closed container.
Pressure

13. Temperature – Raising the temperature will increase the pressure.
Volume – Reducing the volume of a gas increases the pressure.
Number of Particles – Increasing the number of particles increases pressure.
Factors that affect Pressure

15. Ex: basketball in the summer as opposed to one in the winter
Charles’s Law
The volume of a gas varies directly (same way) with the temperature of the gas.
Temperature Volume
Temperature Volume
Ex: basketball in the summer as opposed to one in the winter

16. The volume of a gas varies inversely (opposite way) with the pressure of the gas.
Boyle’s Law
Pressure Volume
Pressure Volume

18. V1 = V2
T1 T2
P1V1 = P2V2
T T2
Charles’s Law
Boyle’s Law
Combined Gas Law

19. Practice Problems Gas Laws
1. At a temperature of 280K, the gas in a cylinder has a volume of 20.0L. If the volume of the gas is decreased to 10.0L, what must the temperature be for the gas pressure to remain constant?
What do we know? Which formula do we use? What are we solving for?

20. 2. If the volume of a cylinder is reduced from 8. 0L to 4
2. If the volume of a cylinder is reduced from 8.0L to 4.0L, the pressure of the gas in the cylinder will change from 70kpa to?
What do we know? What formula do we use? What are we solving for?

21. 3. If a gas has a volume of 1L at a pressure of 270kpa, what volume will it have when the pressure is increased to 540Kpa? Assume the temperature and number of particles are constant.
What do we know? What formula do we use? What are we solving for?

22. Gas law help GREAT website

23. Open the science of diving
Interactive powerpoint

24. Phase Changes
Changing from one phase to another by decreasing or increasing kinetic energy.
Kinetic Energy
*Reversible Physical Change

25. The temperature is one way to recognize a phase change.
The temperature will not change during the change, it will change once the transformation is complete!
Temperature and Phase Change

26. According the this chart, which phase of matter has the most heat energy?
gas

27. Solid – Liquid – Gas – Plasma
Energy is absorbed or released.
Endothermic – absorbed
Exothermic - released
Energy and Phase Change
Energy Increases
Solid – Liquid – Gas – Plasma
Energy Decreases

28. Melting
Solid  Liquid
Heat of fusion – amount of energy absorbed for water
Freezing
Liquid  Solid

29. Gas  Liquid Ex. clouds Liquid  Gas Condensation Vaporization
Energy must be absorbed – heat of vaporization
Evaporation  on the surface of a liquid at temperatures below the substances boiling point (100°C for water)

30. Solid  Gas (without changing to a liquid)
Sublimation
Solid  Gas (without changing to a liquid)
Ex. Dry ice

31. Gas  Solid (reverse of sublimation)
Deposition
Gas  Solid (reverse of sublimation)
Ex. Frost on windows