Standard: SPS5a - Molecular Motion

1. Standard: SPS5a - Molecular Motion Activator EQ: How is molecular motion is based on temperature? Activator: : Kinetic theory and the states of matter Summarizer: The 5 states of matter graphic organizer HW: Density calculations Kinetic Theory Lecture/discussion/notes Introduction to Density Item 1 Item 2 Item 3 Homework

2. Standards: SPS5a States of matter, SPS2a - Density Activator EQEQ: Why do some objects sink while others float in water? EQ: How is molecular motion is based on temperature? Activator: Interpolation and Extrapolation Summarizer: Complete Dry Ice lab Questions HW: Complete Q 5 - 11of Graphing Relationships. Complete Density Lab Questions. Density Lab Dry Ice Lab Item 1 Item 2 Item 3 Homework

3. Measurement Lab Table

4. Standards: SPS2a Density Activator EQ: Why do some objects sink while others float in water? Activator: Density Enrichment Data Collection for Graphing Relationships HW: Density calculations Introduction to Density Density calculations Item 1 Item 2 Item 3 Homework

5. Kinetic Theory • Matter – anything that has mass and takes up space • The word “kinetic” means movement • Three main parts of the kinetic Theory theory: • All matter is made of tiny particles • These particles are in constant motion • The higher the temperature, the faster the particles move. At the same temperature, heavier particles move slower.

6. Kinetic Energy and Temperature • The state of matter is determined by how fast particles move and how often they bump into each other….. that is…..how much Kinetic energy they have. • The higher the temperature more kinetic energy the have and the faster the particles move.

7. Phase change names

9. Exothermic and Endothermic Exothermic Endothermic EXO – out like “exit” • Give off ( lose energy) • Particles slow down • Decrease in temperature of substance ENDO- in like “entrance” • Take in ( gain Energy) • Particles speed up • Increase in Temperature of substance

10. We all know about: SOLIDS LIQUIDS GASES Lower Temperature Higher Temperature

11. Two states of matter you did not know much about Plasma Bose-EinsteinCondensate

12. But what happens if you raise the temperature to super-high levels…between 1000°C and 1,000,000,000°C ?

13. Some places where plasmas are found… 1.Flames

14. 2. Lightning

15. 3. Aurora (Northern Lights)

16. 4. Neon lights

17. 5. Stars Stars make up 99% of the total matter in the Universe.Therefore, 99% of everything that exists in the entire Universe is in the plasma state.

18. 6. Clouds of gas and dust around stars 6

19. So now we know all about four states of matter: PLASMAS(only for low density ionized gases) LIQUIDS GASES SOLIDS Lower Temperature Higher Temperature

20. But now what happens if you lower the temperature way, way, down to100 nano degrees above “Absolute Zero” (-273°C) What is absolute zero?

21. In 1924, two scientists, Albert Einstein and Satyendra Bose got together to compare bad grey hairstyles... Who won??? Einstein Bose +

22. Neither man won but they predicted a 5th state of matter which would occur at very, very low temperatures Einstein Bose +

23. In 1995, an MIT scientist Wolfgang Ketterle and his team of graduate students discovered the 5th state of matter for the first time. Ketterle and his students And named it after the Great men who had theorized about it: Bose-Einstein Condensate

24. In a Bose-Einstein condensate, atoms can no longer bounce around as individuals. Instead they must all act in exactly the same way, and you can no longer tell them apart!

25. Some computer images of Bose-Einstein Condensates…

28. To really understand Bose-Einstein condensate you need to know Quantum Physics

29. Summary… PLASMAS(only for low density ionized gases) BOSE-EINSTEIN CONDENSATE LIQUIDS SOLIDS GASES Lower Temperature Higher Temperature

30. Phase Changes and Energy Transfer • Phase change is a physical change. • Molecules and atoms don’t change • The mass doesn’t change but the volume does change • The particle motion changes

31. Lower Temperature 5 States of Matter Bose-Einstein Condensate SOLID Particles are spread out Particles move all over the place Particles can flow Take the volume of whatever container they are in. Have lots of kinetic energy Particles are superheated to the point where they become equal amounts of positively and negatively charged particles. Particles are tightly packed Particles vibrate in place ( Definite Shape) Particles can not flow Constant volume Have very low kinetic energy Atoms can no longer bounce around as individuals. Instead they must all act in exactly the same way, and you can no longer tell them apart! Almost no kinetic energy LIQUID Particles are able to slide past each other Particles can flow Constant volume Have a medium kinetic energy level GAS PLASMA Higher Temperature

32. Mass, Volume, & Density

33. Mass Measurement of the amount of matter(or stuff) in an object Measured in grams (g) Volume Measurement of the amount of space an object takes up • Measured in milliliters (ml) or cm3

34. Which do you think would have the greater volume and he greater mass? 1 kg of rocks • 1 kg of feathers

35. Which one is more dense? Demonstration: People in a square How about this: Which square is more dense?

36. Which one is more dense? Now which one is more dense?

37. Density Density is defined as mass per unit volume. It is a measure of how tightly packed and how heavy the molecules are in an object. Density is the amount of matter (mass) within a certain volume. Density = Mass g Volume cm³

38. Units for density - g/cm3 or g/ml Formula: M = mass V= volume D = density M = D x V V = M / D D = M / V

39. Quick Practice 1 Frank has a paper clip. It has a mass of 9g and a volume of 3cm3. What is its density? 2. Frank also has an eraser. It has a mass of 3g, and a volume of 1cm3. What is its density? 3. Jack has a rock. The rock has a mass of 6g and a volume of 3cm3. What is the density of the rock? 4. Jill has a gel pen. The gel pen has a mass of 8g and a volume of 2cm3. What is the density of the rock?

40. Behavior of Gases

41. Particle Collisions and Pressure • We know from kinetic theory that Gas particles are constantly moving and colliding with anything in their path. • The collisions of these particles cause pressure. • Pressure is the amount of force per unit of area. • P = F/A. • The SI unit of pressure is Pascal (Pa).

42. Boyle's Law • According to Boyle's law, if you decrease the volume of a container of gas and hold the temperature constant, the pressure of the gas will increase. • An increase in the volume of the container causes the pressure to drop, while temperature remains constant. • Boyle’s law is written as P1V1 =P2V2

43. Graph of Boyle’s Law • Volume vs. Pressure for a Fixed Amount of Gas at Constant Temperature

44. Charles' Law • According to Charles's Law, the volume of a gas increases with increasing temperature long as pressure does not change. • The volume of a gas shrinks with decreasing temperature. • Charles’ Law can be written as V1/T1 = V2/T2 60ºC 30ºC

45. Graph of Charles’ Law • Temperature v. Volume for a Fixed Amount of Gas at Constant Pressure Volume m3 Temperature K