1. Warm Up: (5 minutes)
GET BINDERS OUT READY TO TAKE NOTES! (-5 FOR ANYONE NOT READY ONCE bell rings!)
We have learned about four states of matter, in which of the following 3 states do particles move the MOST  solids, liquids, or gases? (Do not have to write question, but answer in complete sentence).
What is the relationship between how fast these particles move and the shape and volume this state of matter has? (2 sentences) (Write question and answer)

2. Announcements New TOP 10 Doughnuts Friday Morning
Quiz on Friday – States of Matter & Gas Laws
Grades – next class
TEDx Interviews today

3. Answer to DO NOW
What is the relationship between how fast these particles move and the shape and volume this state of matter has? (2 sentences)
Particles in a gas are well separated with no regular arrangement/pattern. Gas particles move freely/collide at high speeds.

4. GASES! Get your notes set up: Title: Gas Laws
Date your notes in top right

5. Kinetic Molecular Theory
How particles in matter behave!
All matter is composed of particles
Particles are in constant motion
Particles also collide with other particles and may lose some energy

6. SOLID Molecular Motion: Atoms vibrate in place Packed closely together
DO NOT NEED TO COPY, you already know!
Molecular Motion: Atoms vibrate in place
Packed closely together
Arranged in a geometric pattern
Heat Index: At its freezing point
Attraction: Very close together

7. LIQUID Molecular Motion: atoms able to slide by one another
DO NOT NEED TO COPY
Molecular Motion: atoms able to slide by one another
Attraction: Still able to cling to each other
More kinetic energy
To slip out of the solid state, the particles had to gain in kinetic energy
Heat Index: Melting Point – when particles slip from a solid to a liquid

8. PLASMA Most common state in the universe Positively charged particles
DO NOT NEED TO COPY
Most common state in the universe
Positively charged particles
Molecular Motion: Moves extremely fast – electrons are stripped off Electrically charged

9. GAS Molecular Motion: Freely floats around Attraction: No Attraction
Will fill whatever container it is living in.
Heat Index: Vaporization – when liquid becomes a gas
Must escape its attractive forces

10. Standards by ClayCo
Just finished  SPS5a. Compare and contrast the atomic/molecular motion of solids, liquids, gases and plasmas.
Now  SPS5b. Relate temperature, pressure, and volume of gases to the behavior of gases.

11. Enduring understanding  For gaseous substances, pressure, volume, and temperature are interdependent.

12. OBJECTIVES
YOU will be able to identify Boyle’s Law, Charles Law, & Guy-Lussac’s Law
YOU will be able to relate temperature, pressure, and volume to the behavior of gases.

13. NEW VOCAB Today we are covering:
Intermolecular attraction – The amount of "stick togetherness"
Temperature – intensity of heat
Pressure - exertion of force upon a surface by an object (force per unit of area)
Specific Heat - amt of heat per unit mass required to raise the temp by one degree Celsius

14. Which balloon has HIGHER pressure? Vote: 1 2
Gases- Pressure
Which balloon has HIGHER pressure? Vote: 1 2

15. Gases- Pressure What is it?
Pressure is the amount of force exerted on a container from within, it is caused by gas particles colliding with each other.
Do MANY or FEW collisions cause a lot of pressure?
MANY, the more particles collide the more they Hit the walls of their container, putting force on the walls
Does having MORE or FEWER particles cause many collisions?
MORE, the more particles there are the more collisions there will be

16. Boyle’s Law Robert Boyle (1627 – 1691) British
Decrease the volume of the container of gas + a constant temperature = pressure of the gas will increase
Increase the volume of the container of gas + constant temperature = pressure of gas will decrease

17. (inversely proportional)
Boyle’s Law
As the pressure of a gas increases the volume of that gas decreases When Temperature is constant.
(inversely proportional)

18. Pressure and Volume (WHEN THE AMOUNT OF GAS IS CONSTANT)
Use arrow (up = increase, down = decrease) to fill in the blanks under the diagram V V P P

19. Pressure and Volume (WHEN THE AMOUNT OF GAS IS CONSTANT)
Use arrow (up = increase, down = decrease) to fill in the blanks under the diagram V V P P

20. Boyles Law
P1V1=P2V2

21. Charles Law Jacques Charles (1746 – 1823) – French
Volume of gases increases with increasing temperature as long as pressure doesn’t change.
Volume of gases decreases with decreased temperature as long as pressure doesn’t change.

22. (directly proportional)
Charles’s Law
As the temperature of a gas increases the volume of that gas increases The pressure is constant.
(directly proportional)

23. Temperature
Temperature

24. Charles Law
V1 = V2 T1 T2

25. (directly proportional)
Guy-Lussac’s Law
As the temperature of a gas increases the pressure of that gas increases When volume is constant.
(directly proportional)

26. Temperature
Temperature

27. Guy Lussac’s Law
P1 = P2 T1 T2

28. Practice BOYLE Prediction  solve
P1 = 20 atm V1 = 1 L P2 = 10 atm V2 = ? (greater than or less than 1 L?) Atm = atmospheric pressure (units of pressure)

29. Practice CHARLES Prediction  solve
T1 = 300 K V1 = 5 L T2 = 150 K V2 = ? (greater than or less than 5 L)

30. Practice GUY LUSSAC Prediction  solve
P1 = 20 atm T1 = 100 K P2 = 80 atm T2 = ? (greater than or less than 100 K)

31. Conclusion (2 min)
In your notes, write down your answer to this question: What does the set up of each equation tell us about how those two variables affect each other?

32. Boyle's gas law states: the volume of a gas is inversely proportional to the pressure of the gas when temperature is held constant.
Gay-Lussac's law constant volume, the pressure of a gas is directly proportional to its temperature.
Charles' Law states: If the pressure of a gas sample is kept constant, the volume of the sample will vary directly with the temperature