1. States of Matter Kinetic Theory
CH. 13 NOTES
States of Matter
Kinetic Theory

2. Types of Kinetic Energy
Kinetic Energy = motion
Translational: forward motion ( L G )
Rotational: spinning motion ( L G )
Vibrational: vibrating motion ( S L G )

3. All matter consists of tiny particles that are in constant motion.
Kinetic Theory
All matter consists of tiny particles that are in constant motion.

4. Kinetic Theory:
Particles in a gas are small, hard spheres (no volume)

5. Kinetic Theory
Gas particles are in rapid, constant, random motion.

6. Kinetic Theory
Collisions are perfectly elastic (travel in straight lines)

7. Kinetic Energy
-Kinetic Energy is directly proportional to Kelvin temperature.

8. Kinetic energy vs. Temperature
Average temperature doesn’t mean every molecule has the same kinetic energy
Absolute zero=all motion of particles ceases and has no kinetic energy K = oC + 273

9. Kinetic Theory
diffusion: tendency of molecules to move to areas of lower concentration until concentration is uniform throughout.

10. Gas Pressure -Gas pressure is caused by collisions of molecules
-Empty space with no particles is a vacuum.

11. Pressure -Barometer measures atmospheric pressure.
1atm = 760 mmHg = 760 torr = 101.3kPa
(Atm =atmospheres kPa = kilopascal)

12. Converting pressure 1. Convert 450 kPa to: a. mm Hg b. atm
2. Convert 2.5 atm to:
a. kPa b. mm Hg
1atm = 760 mmHg = 760 torr = 101.3kPa

13. Answers 1a. 450 kPa | 760 mmHg = 3376 mmHg | 101.3 kPa
1b 450 kPa | 1 atm = atm
2a kPa 2b mmHg

14. Ch. 13.2
The Nature of Liquids

15. Gases and Liquids are Fluid

16. Gases and Liquids are Fluid
Atoms and Molecules in a liquid move in a random pattern relative to one another bc the intermolecular forces are too weak to hold the atom and molecules in a solid form.

18. Vapor Pressure: pressure exerted by molecules that have evaporated from liquid.
Increase temperature=increase kinetic energy=increase vapor pressure

19. Dynamic equilibrium: occurs when vapor pressure no longer fluctuates (changes).
Rate of evaporation = rate of condensation

20. Boiling Point: When Vapor Pressure = Atmospheric Pressure
Make things boil by:
Increase temperature
Lower atmospheric pressure

21. Boiling point is lower in the mountains
Normal Boiling Point: temperature substance boils at

22. Vapor Pressure and Boiling Point
Which compound is:
Most volatile?
Strongest IMF (intermolecular forces)
Highest b.p.?

23. Phase Diagram

24. Phase Change Diagram