1. Matter & Energy

2. States of Matter  Solid- Definite volume and shape Particles are tightly packed Slight expansion when heated Incompressible

3. Solid Vibration around fixed points

4.  Liquid- Has definite volume, but no definite shape (assumes the shape of the container) Particles are loosely packed (can flow by sliding over each other) Easily expand when heated Considered incompressible States of Matter

5. Liquid Vibration around sliding points

6.  Gas- No definite shape or volume Expand to fill the container Particles are spaced far apart Compressible States of Matter

7. Gas Vibration around moving points

8.  Plasma- Consists of electrically charged particles It’s an ionized gas Common in space, but very rare on Earth Found in lightning, fluorescent lights and neon signs States of Matter

9. Plasma “Super-heated Gas” When atoms are so hot, they lose ALL of their electrons. When atoms are so hot, they lose ALL of their electrons.

10. Energy Amounts in States of Matter  Solid- little energy, particles vibrate and rotate  Liquid- more energy, they move freely by sliding over each other  Gas- even more energy, move quickly  Plasma- most energy, move extremely fast

11. All You Really Need To Know You Can Learn From Noah's Ark  5. Plan ahead. It wasn't raining when Noah built the ark.  6. Build your future on high ground.

12. Solid Liquid Gas Plasma Made of Atoms Holds its shape Atoms move past each other

13. States of Matter Changes of State Solid Liquid Gas Energy

14. Names of Phase Changes  Solid to Liquid= Melting  Liquid to Gas= Boiling/evaporation  Gas to Liquid= Condensation  Liquid to Solid= Freezing  Solid to Gas= Sublimation  Gas to Solid= Deposition

15. Boiling Melting Freezing Condensation DepositionDeposition

16. Sublimation When a solid turns directly into a gas. Sublimation When a solid turns directly into a gas. Dry ice is solid CO 2

17. MATTER, Definition, States, and Change of State Lets see if you can: 1. Define matter 2. Define the various states of matter and draw an example of each state 3. Recognize that particle motion determines the state of matter

18. States of Matter List the Location of Each Change of State Solid Liquid Gas Energy Melting DepositionFreezingSublimation CondensationBoiling Energy

19. List the Location of Each Enthapy Used to Change State Solid Liquid Gas Energy Heat of Fusion Heat of Vaporization Energy Endothermic   Exothermic

20. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Energy (calorie) T e m p. ( C)

21. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Ice and Water

22. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Both Water and Steam

23. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Heat of Fusion Heat of Vaporization

24. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Slope = Specific Heat Steam Water Ice

25. Moisture that collects on the outside of a cold glass results from the process of… 1. evaporation. 2. condensation. 3. sublimation. 4. vaporization. Moisture that collects on the outside of a cold glass results from the process of… 1. evaporation. 2. condensation. 3. sublimation. 4. vaporization.

26. Matter, Specific Heat of Matter At the conclusion of our time together, you should be able to: 1. Define specific heat 2. Use specific heat to determine energy changes

27. Thermochemistry  Some Definitions: Calorimeter – a device to measure the energy absorbed or released as heat in a chemical or physical change Temperature – measure of the average kinetic energy of the particles in a sample of matter Joule – the SI unit of heat

28. Thermochemistry  Some Definitions: Heat – energy transferred between samples of matter Specific Heat – the amount of energy required to raise the temperature of one gram of a substance by one Celsius degree or one Kelvin 1 Calorie/4.184 Joules – will do the above with water

29. Thermochemistry  Some Definitions: Enthalpy (Heat) of Fusion – amount of energy gained or lost by a system as heat during melting or freezing Enthalpy (Heat) of Vaporization – amount of energy gained or lost by a system as heat during boiling or condensation

30. Specific Heat Calculations:  q = c p x m x t: q = energy lost or gained c p = specific heat of the substance at a specific pressure m = mass of the sample t = change in temperature (final – initial)

31. Practice #1  q = c p x m x t: q = 59.912 J c p = x m = 36.359 g t = 152.0 o C 59.912 J = (x)(36.359 g)(152.0 o C) = 0.01084 J/g o C

32. Practice #2  q = c p x m x t: q = -800. J c p = 0.4210 J/g o C m = 73.174 g t = (x – 102.0 o C) -800. J = 0.4210 J / g o C (73.174 g)(x – 102.0 o C) -800. = 30.81x – 3142 2342 = 30.81x = 76.0 o C

33. Matter, Specific Heat of Matter Let’s see if you can : 1. Define specific heat 2. Use specific heat to determine energy changes

34. Define Specific Heat Specific Heat – the amount of energy required to raise the temperature of one gram of a substance by one Celsius degree or one Kelvin

35. Practice #3  q = c p x m x t: q = -185.4 J c p = 0.440 J/g o C m = x g t = -1475 o C -185.4 J = (0.440 J/g o C )(x)(-1475 o C) -185.4 J = -649 Jg = 0.29 g

36. Practice #4  q = c p x m x t: q = x J c p = 0.0335 cal/g o C (4.184 J/cal) m = 152.00 g t = -51.5 o C x = (0.140164 J/g o C )(152.00 g)(-51.5 o C) = -1.10 x 10 3 J