1. CH. 13.1 NOTES States of Matter

2. Types of Kinetic Energy Kinetic = motion Kinetic Energy: energy an object has – Translation: forward motion – Rotational: spinning motion – Vibrational: vibrating motion

3. Kinetic Theory All matter consists of tiny particles that are in constant motion. As a basis for this theory, there are 3 fundamental assumptions. They are:

4. Kinetic Theory: 1.Particles in a gas are small, hard spheres (no volume)

5. Kinetic Theory 2.Gas particles are in rapid, constant, random motion.

6. Kinetic Theory 3.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 = o C + 273

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

10. Properties of Gases Expansion: gases don’t have a definite shape so they completely fill any container they are in Fluidity: because there are no forces between the particles in a gas, they slide right by each other (fluid) What is another fluid?

11. Properties of Gases Low Density: gases are not dense because their particles are so far away from eachother Compressibility: The volume of a gas can be decreased significantly because particles are far away from each other. (think of air pressure in tires)

12. Properties of Gases Diffusion and Effusion: –Gases spread out and mix with one another without being stirred. –Diffusion: spontaneous mixing of two gases caused by random motion –Effusion: when gas particles pass through a tiny opening

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

14. PRESSURE Is defined as: Force/unit area of a surface Has the equation: P=F/A Uses the following units:

15. UnitSymbolConversion Factor Millimeters of mercury Mm HgPressure that supports 1 mm of Hg in a barometer AtmosphereAtm760 mm Hg 1.01 x 10 5 Pa PascalPa1N/m 2 Torr 1 mm Hg

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

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

18. Answers 1a. 450 kPa | 760 mmHg = 3376 mmHg | 101.3 kPa 1b 450 kPa | 1 atm = 4.44 atm | 101.3 kPa 2a. 253kPa2b. 1900mmHg

19. Ch. 13.2 The Nature of Liquids

20. Gases and Liquids are Fluid

21. Atoms and Mc’s in a liquid move in a random pattern relative to one another bc the intermolecular forces are too weak to hold the atom and mc’s in a solid form.

23. Vapor Pressure: pressure exerted by mc’s that have evaporated from liquid. – Increase temperature=increase kinetic energy=increase vapor pressure

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

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

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

27. Vapor Pressure and Boiling Point Which compound is: 1.Most volatile? 2.Strongest IMF (intermolecular forces) 3.Highest b.p.?

28. 13.4 Phase Changes

29. Phase diagram

30. Phase Diagram

32. Phase Change Diagram