1. Fluids and Dynamics Unit 3
Science 8
Tannant

2. Chapter 7
Kinetic Molecular Theory Explains The Characteristics of Solids, Liquids, and Gases

3. 7.1 States of Matter
Matter—anything that has mass and volume Mass = amount of ‘stuff’ or particles Volume = space or size

4. Example
The Basketball has greater volume, but the bowling ball has greater mass.

7. The Particle Model

8. 1. All matter is made of particles.
ATOMS

9. 2. There are spaces between the particles.

10. The amount of space is different for each state of matter.

11. 3. The particles are ALWAYS moving.

12. The more ENERGY particles have, the more they move.

13. 4. Particles are attracted to other particles.

14. The strength of attraction depends upon the type of particles.
Strong attraction = particles mix
Weak attraction = particles separate

15. Kinetic Molecular Theory
Kinetic = motion (energy)
Molecules (or atoms) are the particles in matter.
KMT = the THEORY that explains how matter behaves when the energy of particles changes and allows you to predict those behaviors.

16. The KMT and Particle Theory are almost identical.
Particle Theory of Matter
Kinetic Molecular Theory
1 All matter is made up of particles.
1. All matter is made up of atoms and molecules.
2. There are spaces between particles.
2. There is empty space between particles.
3. Particles are always moving.
3. Particles are always moving—they collide with each other and the sides of their container.
Solids = vibrate
Liquids = slide past each other
Gases = move quickly and are far apart from each other
4. Particles are attracted to each other.
4. Energy makes particles move. The more energy they have, the faster they move and the farther they move apart.

17. Thermal Expansion
As the heat (ENERGY) increases, The particles move faster  and farther apart The substance EXPANDS.

18. Thermal Contraction
As a substance LOSES energy, the particles move slower, and move closer together causing the substance to get smaller (decrease volume)

19. Contraction and Expansion

20. The Difference Between Heat and Temperature
Kinetic Energy = Energy of MOTION When particles heat up, they have more energy and MOVE more… So—Kinetic Energy is also THERMAL energy (or Heat energy)

21. Thermal Energy
The total amount of kinetic energy in a substance.

22. [High  Low] Energy Flow
If two substances with DIFFERENT thermal energies come into contact, the energy will ALWAYS flow from an area of HIGH energy to an area of LOW energy.
[High  Low]

23. Heat The energy transferred from one type of matter to another
(As a result of a difference in temperature or a change in state.)

24. Temperature
The AVERAGE kinetic energy of all a substances particles.

25. Energy Transfer and Heat Flow

26. Changes in State occur due to Changes in Energy

27. Melting Change in state from a solid to a liquid Energy is added
Particles spread out and slide/flow past each other.

28. Melting point
The temperature at which a solid changes state to a liquid.
Although energy is added—there is NO change in temperature
Example: The melting point (or freezing point) of water is 0˚C.

29. The melting point and freezing point are the same thing!

30. Evaporation Change of state from a liquid to a gas
More energy is added
Particles move rapidly and spread apart

31. Boiling Point
The temperature at which a liquid changes state to a gas.
Although energy is added, the temperature remains constant.
Example: The boiling point of water = 100˚C

32. Condensation Change in state from a gas to a liquid
LOSS of energy—particles move slower and get closer together.

33. Solidification/Freezing
Change of state from a liquid to a solid.
LOSS of energy—particles slow down (vibrate only) and get as close as possible together (contract)

34. Sublimation Direct change of state from solid to a gas
Example: Dry ice

35. Deposition
Direct change of state from a gas to a solid
Example: Frost

36. Change of State versus Temperature

37. 7.2 Fluids and Density

39. Fluid Liquids and Gases ONLY
Any form of matter that can flow (particles slide past each other)
Liquids and Gases ONLY

40. Density A property of matter
The amount of MASS contained in a given VOLUME.
How closely packed the particles are

42. Less dense particles ‘float’ on denser particles

43. Density and KMT As particles heat up they move faster….
As they move faster, they have more space between them…
The more space = LESS DENSE, so they ‘float’

44. Expansion
When substances heat up and particles expand (less dense)

45. Contraction When substances cool down and particles move closer
More dense

46. Water—the Exception Water is densest at 4˚C.
As water cools lower than 4˚C, the particles form rigid bonds that cause the water to expand!
That’s why ice floats!

47. Water Particles

48. Density
Generally, solids are denser than liquids, and liquids are denser than gases.
There are SOME exceptions…

49. Density Chart for Pure Substances

50. g/mL—liquids or gases g/cm3 –solids
Pay attention to units
g/mL—liquids or gases g/cm3 –solids

51. Comparing Density
Layering different substances works well to compare density

52. Measuring Density
To measure density, we must measure both the SIZE (volume) of the substance and its MASS (weight)

53. Volume = height x length x width Measured in mL or cubic cm (cm3)

54. Volume Displacement
Volume can also be recorded by the amount of water displaced by an object.

55. Meniscus Measurement
Using a Graduated Cylinder

56. Measuring Mass

57. Calculating Density

58. 1 mL of glycerol has a mass of 1.26 g. What is the density of glycerol?
Use the formula: D = m/v 1.26g 1 mL = 1.26 g/mL Density

59. What is the density of a 2 cm^3 sugar cube that has a mass of 3.18 g?

60. A 3 mL sample of oil has a mass of 2.64 g. What is the density?

61. Look on the density chart on p.262.
Which is more dense, lead or iron? How do you know?