1. Unit 1: Matter

2. Essential Question
What are the characteristics of the various states of matter?

3. Definitions
Intermolecular force: the attractive forces between molecules
Kinetic energy: energy in motion

4. Picture or description Shape (fixed or variable)
State
Particles
Picture or description
Shape
(fixed or variable)
Volume (fixed or variable)
IMF (strong or weak)
Kinetic Energy (High or Low)
Solid
Liquid
Gas

5. Endothermic vs. Exothermic
Endothermic: When a system absorbs energy from its surroundings. Increases in KE, feels cold
Exothermic: a system releases energy to its surroundings, decreases in KE, feels warm

6. Solid
Gas
Liquid

7. Phase Diagram
List 3 things you notice about the phase diagram

8. Phase Diagram
What do A, B, and C represent?

9. Critical point
The point at which the boundary between two phases ceases to exist
No distinction between liquid and gas

10. Triple Point The point where either state of matter is possible.
Any slight change will determine which state of matter is present.

11. Phase Diagrams
What would the phase of carbon dioxide be at temperature 250 K and pressure 100 bars?

12. Phase Diagrams
What state(s) of matter can exist at 250K?

14. You Try!
Construct a temperature vs. energy plot based on the given information. Starting at 0 Joules, energy is added to a substance at a constant rate until 500 Joules have been added. The temperature of the substance increases from -10oC to 110oC. The melting point occurs at 5oC and the boiling point occurs at 85oC. Once your plot is finished label areas related to the heat of fusion and the heat of vaporization.

15. Energy vs. Temp Diagram

16. Plasmas
A gas that is made up of highly energized, positively and negatively charged ions.
Neon sign
Stars
Lightning
Grapes in a microwave.

17. Liquid crystals
Turn and Talk: what is a liquid crystal?

18. Liquid crystals
 a state of matter that has properties between those of a liquid, but particles are arranged like that of a solid crystal.
Computer screen
Soaps  

19. Do Now!
Dry ice is frozen carbon dioxide that goes from a solid state straight to a gas state.
1. Name the phase transition.
2. Is the phase transition endothermic or exothermic? How do you know?

20. Physical Properties
observed or measured without changing the composition of matter
Ex: Boiling point, brittleness, mass, etc

21. Chemical Properties
Properties of matter that deal with the chemical makeup or interactions with other matter.
Ex. Flammability
corrosive pH

22. Physical vs. Chemical properties

23. COPPER Physical Properties: Dense (8.96 g/mL) Heavy (63.55 g/mol)
High boiling point (2562 °C)

24. EXAMPLE: Chemical Properties
Which of these is a chemical property of hydrogen gas?
a. Has a molar mass of 2.02 g/mol
b. Reacts easily with oxygen
c. Melting point is °F
d. Found in planets and stars

25. Physical Vs. Chemical change
Physical Change:
Changes the physical form of the substance, but NOT the chemical makeup.
Chemical Change:
Changes the chemical make-up/properties of a substance.

26. 5 signs of a chemical change:
Color change
Formation of a solid
Odor Production
Production of energy (sound, light, heat)
Formation of a gas (bubbles)

27. Physical Change
Most commonly phase changes, or dissolving in water.

28. Physical Change or chemical change?
Dry ice sublimes when exposed to normal, atmospheric conditionsIron metal is melted
Iron combines with oxygen to form rust
Kool-Aid dissolves in water
Copper in Statue of Liberty changes from golden orange color to blue-green

29. Practice Determine if the following are Phys/Chem Properties.
The boiling point of ethyl alcohol is 78 °C
Diamond is very hard.
Sugar ferments to form ethyl alcohol
A block of aluminum has a mass of 56g.

30. Warm Up! 1. Physical changes are usually ___________ changes.
2. List 3 of the 5 ways you can tell that a chemical reaction has taken place

31. BELL RINGER!
Which is more dense? Ice or water? Why or how do you know?

32. Density (ρ) A physical property that defines a substance
Density is defined as mass (grams) per unit volume (mL or cm3)
D= m/v
1mL = 1 cm3
Density of water= 1g/mL

33. D=m/v

34. Density
In a solution, more dense component will be on bottom of less dense
← Least Dense
Vinegar
Oil
← Most Dense

35. Density

36. Let’s Practice!
Take out a calculator!
Worksheet due tomorrow!

37. BELL RINGER!
Think! What happens when you put red hot nickel into water? Describe what will happen.

38. What happened?
Why did the water not start boiling right away?
Think about energy transfer!

39. What will happen when you put a red hot ball of nickel into a bowl of Jell-O?’

40. Specific Heat Used to define a substance
Amount of energy needed to change the temperature of 1g, 1°C.
Stated another way: how easily something changes temperature.
Used frequently to determine the heat lost/gained
Water→4.184 J/g °C
Aluminum→ J/g °C
Q = m · C · ΔT

41. Specific heat triangle

42. Practice: if 1,000 joules of energy were added to each of the substances below, which would have the highest change in temperature?
    Metal
Specific Heat a.
Beryllium
1.82 J/g•°C b.
calcium
0.653 J/g•°C c.
copper
0.385 J/g•°C d.
gold
0.129 J/g•°C

43. If a substance changes temperature from 65 degrees Celsius to 35 degrees Celsius, calculate the change in temp.

44. Law of Conservation of Energy
Energy is neither created nor destroyed in a closed system
In an insulated system, heat lost by one substance is gained by the other
-Q = Q
-mm C mΔTm = mw C wΔTw

45. Let’s Practice!!!!

46. Do you remember this?

47. Do you remember this? State Particles Picture Shape
(fixed or variable)
Volume (fixed or variable)
IMF (strong or weak)
Solid
Liquid
Gas

48. Solid
Gas
Liquid

49. Do you remember this? Endothermic vs. exothermic?
Plasma and liquid crystals?

50. Do you remember this?
Lab instruments?

51. Phase Diagram
What do A, B, and C represent?

53. Do you remember this? Physical vs. chemical changes?
What changes are physical?
How can you tell that a chemical change has occurred? (there are 5)

54. Density?
Sink or float?
Equation?