Phases & Behavior of Matter

1. 1 Phases & Behavior of Matter

2. 2 Phases and Behavior of Matter Goals 1. Compare and contrast the atomic/molecular motion of solids, liquids, gases & plasmas. 2. Explain the flow of energy in phase changes through the use of a phase diagram. 3. Relate temperature, pressure, and volume of gases to the behavior of gases. Solid Liquid Gas

3. 3 Review • Everything in the universe is either matter or energy. • Physical Science is the study of matter and energy. • Matter is anything that has mass and takes up space.

4. 4 Clip Kinetic Theory of Matter • All matter is composed of small particles (atoms). • These particles are in constant motion. • These particles are colliding with each other and the walls of their container.

5. 5 Kinetic Energy • Kinetic Energy is the energy of motion. • Temperature is the measurement of the KE in an object. • So, the more KE the higher the temp. • As the particles in an object gain KE, the temperature goes up.

6. 6 Clip Amorphous Solids Solids • Particles are closely packed together. • Most are geometric. • There are bonds between atoms/mol. • Rigid shapes. • Definite shape. • Definite volume.

7. 7 Clip Liquids • Particles in a liquid have more KE than particles in a solid. • Liquid particles have enough KE to overcome the forces that hold them together. • The particles can now move past one another. (flow) • Definite volume • No Definite shape. Viscosity

8. 8 Clip Gases • Gas particles have more KE than liquid particles. • They have enough energy to break all bonds and escape the liquid state. • No definite Shape • No definite Volume. Gases fill their container.

9. 9 Gases are compressible

10. 10.1 Clip Plasma • Most common state of matter in the universe • Extremely high temperatures. • Contains positively and negatively charged particles

11. Terrestrial plasmas • Lightning • The ionosphere • The polar aurorae • Artificially produced plasmas • Those found in plasma displays, including TVs • Inside fluorescent lamps (low energy lighting), neon signs • The electric arc in an arc lamp, an arc welder or plasma torch • Plasma ball (sometimes called a plasma sphere or plasma globe)

12. 10.2 • Force produced by high energy collisions strips electrons from atoms. • Sun, lighting bolts, neon and fluorescent tubes, auroras. ReviewClip

13. 10.3 • PHET Phases of matter simulation • STOP HERE>>>>>> • REVIEW

14. 11 Changing State

17. 12

18. 13 Boiling vs. Evaporation • Boiling is The vaporization of a liquid at its boiling point. • Evaporation is • The vaporization of a liquid below its boiling point. This occurs at the surface of the liquid.

19. 14 Sublimation • Some substances go from the solid state directly to the gaseous state.This happens when a substance was below it freezing point and is suddenly moved to a location where it is above its boiling point • EX: CO2

20. 15 • It takes energy to cause phase changes( soild-liq-gas) • Removal of energy (gas-liq-solid) Increase Energy Phase changes do not change the substance

21. 16 • The amount of energy required for a substance to go from a solid to a liquid is called the HEAT OF FUSION. • (EX) it takes 334,000 Joules of energy to melt 1 kg of ice. No temperature change. 0°C 0°C

22. 17 • The amount of energy required to change a liquid to a gas is called the …Heat of Vaporization • EX: It takes 2,260,000 Joules of energy to vaporize 1 kg of water. 100 °C 100 °C

23. 18.1 Clip Energy

24. The triple point of a substance is the temp. and pressure at which the three phases of that substance coexist • Phase depends not only on temp. but also pressure. 18.2

25. 19 When heat is added to most materials they expand. Thermal Expansion • When objects are heated, they expand. • When they are cooled, they contract. • Video Clip

26. Thermal Expansion Typical expansion joints on a steel span bridge.

27. 20 Thermometers • Work because of thermal expansion. • Because mercury expands and contracts uniformly, it was used in thermometers.

28. 19 21

29. 22 PRESSURE

30. 23 Force (N) Pressure (Pa)= Area (M2)

31. 24 Gases exert pressure on their container

32. Pressure:The amt of force exerted per unit of area. Gases exert pressure by colliding with “things.” Other particles of gas Sides of the container Objects within the area of the gas, like you.  24

33. Formula For Figuring Out Pressure: P = F/A   ThePascal (Pa) is the SI unit of pressure 26 Clip

34. 27 Boyle’s and Charles’ Law • Both deal with gases. • Boyle’s Law • As the volume decreases, the pressure increases. • Charles’ Law • As the temperature decrease, the volume of a gas decreases.

35. P1V1 = P2V2 Boyle’s Law • Relationship between volume and pressure. You tube Clip

36. 28 Boyle’s Law P1V1 = P2V2 If you decrease the volume, the pressure will increase ( no Δt)

37. 29

38. 30 P1 V1 = P2 V2 Boyle’s Law A volume of helium occupies 11.0 L at 98.0 kPa. What is the new volume if the pressure drops to 86.2 kPa? P1 V1 = P2 V2 (98.O kPa) (11.0 L) = (86.2 kPa) (V2) (98.O kPa) (11.0 L) = (V2) (86.2 kPa) (V2)=12.5 L

39. P1 V1 = P2 V2 • A sample of helium gas at 25°C is compressed from 200 cm3 to 0.240 cm3. Its pressure is now 3.00 cm Hg. What was the original pressure of the helium? • P1 = 3.60 x 10-3 cm Hg

40. Charles’ Law • Relationship between volume and temperature.

41. 31 Charles’ Law If you increase the temperature, the volume will increase

42. 32 Charles’ Law • V1/T1 = V2/T2

43. 33 Charles’ Law

44. Charles’ Law 34.1 What would be the resulting volume of a 2.0 L balloon at 25.0˚C that was placed in a container of ice water at 3.0˚C? V1 = V2 T1   T2                                                          . 2.0 L 25.0˚C V2 3.0˚C = V2 = 0.24 L

45. 0.40 L of a gas is collected at 50.0°C. What will be its volume upon cooling to 25.0°C? 0.2 L 34.2

46. PHET Phases of matter simulation

47. 34.3 EOCT Practice Question: A B C D

48. 34.4 EOCT Practice Question: A B C D

49. 35 Archimedes, Pascal, & Bernoulli

50. 36 Greek Mathematician Archimedes