1. STATES OF MATTER

3. I. STATES OF MATTER A. Kinetic Theory of Matter 1.Matter exists as a solid, liquid, gas, or plasma. 2.Tiny particles (atoms) in constant motion make up all matter.

4. Gas Liquid Solid

5. I. STATES OF MATTER B. Solids 1. Mc tightly packed - can’t be compressed 2. Definite shape & volume 3.Least kinetic energy - mc only vibrating

6. I. STATES OF MATTER B. Solids 4. most are formed of crystals Crystal: atoms are arranged in a repeating geometric pattern.

7. I. STATES OF MATTER B. Solids amorphous 5. Some solids are amorphous: They lack an ordered internal structure. They appear to be solids, but are not made of crystals. Ex. rubber, plastic, glass, etc.Ex. rubber, plastic, glass, etc.

8. I. STATES OF MATTER C. Liquids 1.Mc less tightly packed than solids (slightly compressible) 2. Indefinite shape (mc flow past each other) 3. Definite volume 4. More kinetic energy than solids Liquid Solid

9. I. STATES OF MATTER D. Gases 1.Mc spread out. - very compressible 2. Indefinite shape and volume 3. More kinetic energy than solids and liquids Gas Liquid Solid

10. ALL TOGETHER NOW!

11. E. Plasma 1.Hot ionized gas particles 2.Particles are electrically charged

12. E. Plasma 3. Exists only at very high temp. 4. Most kinetic energy

13. I. STATES OF MATTER E. Plasma 5.The most common state of matter in the universe! –Not found naturally on earth. –Found on stars, the sun, inside fluorescent bulbs

14. II. Changes in State A. Thermal Expansion 1.Almost all matter expands as it gets hot and contracts as it cools Name an exception. 2.Different materials expand at different rates.

15. II. Changes in State B. Melting 1.the change from a solid to a liquid 2.Melting pt. – temp. at which a solid becomes a liquid

16. II. Changes in State C. Freezing the change from a liquid to a solid note: freezing pt. = melting pt.

17. II. Changes in State D. Vaporization 1. the change from a liquid to a gas

18. II. Changes in State D. Vaporization Boiling 2. Boiling – rapid; gas bubbles form throughout liquid –Boiling pt. temp. at which a liquid becomes a gas

19. II. Changes in State D. Vaporization 3. Evaporation liquid changes to a gas at temperatures below the boiling point Slow Occurs at the surface

20. II. Changes in State E. Condensation change from a gas to a liquid Note: Boiling pt. = Condensation pt.

21. II. Changes in State F. Sublimation A solid becomes a gas without first becoming a liquid Example: Dry Ice

22. II. Changes in State G. Deposition A gas becomes a solid without first becoming a liquid Example: Frost

23. THERMAL ENERGY

24. B. Motion & Energy 1. Atoms & Mc have KE solids a. solids: mc vibrate slowly in place and are closely packed mc vibrate a little faster and move slightly apart liquids b. liquids:

25. B. Motion & Energy 1. Atoms & Mc have KE solids a. solids: liquids b. liquids: gases c. gases: mc are in rapid motion and are widely separated

26. Phase Change Review Solid to LiquidMelting Liquid to Solid Liquid to Gas Gas to Liquid Solid to Gas Gas to Solid Freezing Vaporization Condensation Sublimation Deposition

27. A coupla videos to illustrate… boiling water to snow liquid nitrogen in pool

28. Phase diagram

29. http://www.chm.davidson.edu/vce/PhaseCh anges/HeatingCurve.htmlhttp://www.chm.davidson.edu/vce/PhaseCh anges/HeatingCurve.html

30. II. Temperature and Heat A. Temperature 1. is how hot or cold an object is higher 2. The higher the temp. faster the faster the mc move

31. Each beaker below contains one molecule of the same gas. Which beaker is at the higher temperature? Your Turn! AB

32. Each beaker below contains one molecule of the same gas. Which beaker is at the higher temperature? Your Turn! AB Answer: Beaker A

33. I. Temperature and Heat A. Temperature 3.Thermometer 3. Thermometer instrument for measuring temperature

34. 4. Temperature Scales Celsius (  C) metric, used in science Kelvin (K) 0 K is absolute zero (lowest temp. possible; where all motion stops) Fahrenheit (  F) English system A. Temperature

35. II. Temperature and Heat A. Temperature B. Heat - Thermal Energy 1.the amount of energy a substance has because of the movement of its particles internal energy 2. Thus heat is internal energy

36. II. Temperature and Heat B. Heat – Thermal Energy 3.is E transferred between objects at different temps Thermal Energy moves from an area of high heat to low heat

37. A. What is it? 3. Examples Sand vs Ocean Water Which feels hotter? 1 kg sand absorbs 6x more heat than 1 kg ocean water III. Specific Heat

38. A. What is it? 1. amount of heat needed to raise the temp. of 1 kg of a substance 1 o C 2. Units J/g. C o III. Specific Heat

39. A. Formula Q = m x c x  T Q Q = thermal energy m = mass (g) c =specific heat  T  T = change in temp. = final T – initial T TAKE NOTE: the “c” for water is 4.18 J/g. C o IV. Calculating Thermal E Changes

40. And now… The MATH

41. B. Sample Problem 1.The temperature of a 32.0 g silver spoon increases from 20.0 O C to 60.0 o C. If silver has a specific heat of 0.057 J/g.o C, what is the change in thermal energy of the spoon? IV. Calculating Thermal E Changes

42. B. Sample Problem m = 32.0 g m = 32.0 g  T = 60.0 o C – 20.0 O C = 40.0 o C  T = 60.0 o C – 20.0 O C = 40.0 o C C = 0.057 J/ o C Q = m x  T x C Q = 3240.0 o C 0.057 J/ o C Q = 32 g x 40.0 o C x 0.057 J/ o C Q = 72.96Jor73J IV. Calculating Thermal E Changes

43. Triple point diagram solid liquid gas