1. What are Solids, Liquids, and Gases?
Chapter 13
States of Matter

2. Kinetic Molecular Theory (KMT)
“all matter is in constant, random motion”
Gases- particles move freely and independently of one another
Liquids- particles are attracted to one another, but are still able to slide past each other
Solids- particles are strongly attracted to each other and shake in place

3. Gases and KMT
Individual gas particles are super tiny and hold no actual volume
Particles move in straight lines until they collide
Collisions are elastic- no kinetic energy is lost

4. Gas Behavior
Compression- gases can be compressed because they have very LOW DENSITY
Expansion- gases will fill any size container because the particles are not held together

5. Graham’s Law Diffusion- movement of one material through another
Effusion- gas particles escaping through tiny holes in the container
Graham’s Law
Ratea = √molar massb
Rateb √molar massa

6. Gases and Pressure Pressure- force per unit area
Gases cause pressure by colliding with the walls of their container
Barometer-measures atmospheric pressure
Manometer-measures vapor pressure
Dalton’s Law:
Ptotal=P1+ P2+P3+...

7. Units of Pressure 1 atmosphere= normal atmospheric pressure
1atm = 760 mmHg = 14.7 psi = 101,325 Pascals = KPa
1.5 atm = ? mmHg
804 mmHg = ? psi

8. Assignment P. 388-392 # 1-12 Show all mathematical work
Answer in full sentences

9. Intermolecular Forces
Intermolecular Forces- the forces that exist between particles of a substance
3 Types (in order of INCREASING strength)
Dispersion- caused by electron movement
Dipole- caused by polar attractions
Hydrogen Bonds- caused by hydrogen and N,O,F

10. Particle Spacing
How do solids, liquids, and gases compare?

11. Liquid Behavior Density- much denser than gases, not compressible
Fluidity- diffuse slower than gases, still “flow”
Viscosity- measure of resistance to flow
Effect of temperature- higher temp, lower viscosity

12. Liquid Behavior Surface Tension Capillary Action
Causes drops and meniscus
Capillary Action
Water can climb narrow tubes

13. Solid Behavior
Density- more dense than gases and liquids and incompressible
Crystalline Solids
Unit Cells
Crystal Structure

14. Solid Behavior
Molecular Solids-dispersion, dipole, or H-bonds (ex: sugar)
Covalent Network Solids- covalent bonds with self (ex: diamond)
Ionic Solids- ionic attraction (ex: salt)
Metallic Solids- mobile electrons (ex: copper)
Amorphous Solids- irregular pattern (ex: glass)

16. Assignment
P. 395 # 13-16
P. 403 # 17-23
Full sentences

17. Phase Changes

18. Heating Curve

19. Endothermic Phase Changes
Melting- solid absorbs energy until particles have enough speed to break free of IM forces holding them in place
Vaporization-liquid absorbs energy until particles have enough speed to break free of IM forces holding them close together

20. Liquid to Gas Evaporation- occurs at surface
Boiling- occurs throughout when vapor pressure equals atmospheric pressure

21. Sublimation-solid to gas

22. Exothermic Phase Changes
Condensation
Deposition
Freezing

23. Phase Diagrams

24. Assignment
P. 409 # 24-28
Yes, sentences please
P. 4 in packet

25. Test
Review Assignment due the day before the test
Test: