States of Matter

1. States of Matter Self Study

2. Changesin State Four states of matter video clip: click here

4. Phase Diagram Book video clip: click here

5. Phase Diagram MELTING FREEZING CONDENSATION VAPORIZAITON SUBLIMATION TRIPLE POINT

6. What word describes Motion or Movement energy?

7. Kinetic Energy All matter’s particles are in constant motion

8. State of Matter is determined by • Particle arrangement • Energy of particles • Distance b/w particles

9. Kinetic Theory: Solids Atoms are vibrating on a fixed point in a solid

10. Types of Solids Book video clip: click here

11. Amorphous Solid Has no organized internal structure Rubber Plastic Glass Asphalt Cotton Candy

12. Compounds with the highest melting points are….

13. Melting Points Strongest ( highest): Ionic Bonding Hydrogen Bonding Dipole-Dipole Lowest ( weakest) Dispersion

14. 1. Ionic : strongest bond Bond kept together by…. Crystalline structure

15. Covalent Compounds have three interactions( intermolecular forces) that keep them together….

16. 2. Hydrogen Bonding strongest covalent Highest MP & BP of covalent Hydrogenattracted to: Nitrogen Oxygen Fluorine

17. 3. Dipole-Dipole [polar] - end attracted /// to + endof another

18. 4. Dispersion [nonpolar] weakest -a dipole is induced -lowest MP & BP interaction Induced + Induced -

19. Kinetic Theory: Liquids Particles are not bound together in fixed positions, but there is still some attractive forces keeping them close during movement.

20. Fluidity Particles flow, slide over each other

21. Viscosity

22. Kinetic theory of gases Book clip: clip here

23. Gas Particles Assumption #1: • Have a small volume • Far apart from each other • Independent : No attractive or repulsive forces

24. Gas Particles Assumption #2: • Move: • Rapid • Independent • Random • Straight paths • Only  direction when rebounding

25. Gas Particles Assumption #3 When particles collide, there collisions are elastic: • no loss of energy • it is transferred between the particles

26. Gas Pressure Force exerted when gas particles collide: click here

27. Pressure Units • SI unit : Pascal (Pa) • Sea level: 101.3 kPa • Millimeters of Mercury: mm Hg • blood pressure • Atmospheres: atm • Atmospheric pressure • Torr • Pounds per Square Inch: PSI • Tire pressure, scuba diving • Bar • Atmospheric pressure

28. Conversions of Pressure 1 atm = 760 mmHg = 101.3 kPa 1 torr = 1 mm Hg 1 atm = 14.7 PSI 1 bar = 1 atm

29. Vacuum no gas particles = no collisions = NO PRESSURE

30. Atmospheric Pressure Gas particles in Air colliding in earth’s atmosphere

31. Elevation and Atmospheric Pressure ↑ Elevation = ↓ Atmospheric Pressure b/c less gas particles =less collisions =  P Sea Level more gas particles = more P

32. More gas particles = More collisions= More pressure

33. Evaporation vs Condensation Eureka video clip: click here

34. Evaporation Video Clip: Click here

35. Equilibrium Book clip: click here

36. Evaporation/ Condensation Equilibrium

37. Evaporation/ Condensation Dynamic Equilibrium

38. Evaporation/ Condensation Dynamic Equilibrium

39. Boiling Liquid has enough HEAT/ENERGY to overcome the External Pressure Vapor Pressure = External Pressure

40. Boiling Video clip: click here

41. to make something boil Energy/Heat is added Or the EXTERNALpressure is changed

42. Affect of  Temp on Contained Liquid  KE of particles  particle collisions  VP This why a tea kettle whistles

44. Elevation and BP

45. Pressure Cooker Creates a HighExternal Pressure abubble of vapor can’t form unless KE= T  BP is = hotter liquid= shorter cooking time

46. Temperature Video clip: click here

47. Measuring Temperature Eureka video clip: click here

48. Temperature Movement of particles

49. Absolute Zero (0 K) No movement of particles

50. Absolute Zero (0 K) Video Clip: Click here