1. Solids, Liquids, Gases
Ch 16
09-10

2. Objectives
16-1 Explain the 3 states of matter based on the arrangement of particles, movement of particles, shape and volume.
16-2 Explain and apply Gas Laws.
16-3 Determine the viscosity of a liquid.
16-4 Create a phase change graph.
16-5 Explain a phase change graph.
16-6 Define sublimation.
16-7 Complete density problems.

3. Phases of Matter AKA: states of matter
Section 1

4. Objectives
16-1 Explain the 3 states of matter based on the arrangement of particles, movement of particles, shape and volume.
16-4 Create a phase change graph.
16-5 Explain a phase change graph.
16-6 Define sublimation.
16-7 Complete density problems.

5. Kinetic Theory DEF: explanation of how particles in matter behave.
All matter composed of small particles
Particles in constant motion
Particles collide with each other and walls of container

6. Thermal Energy DEF: Total kinetic and potential energy of particles
Temperature
DEF: measure of the average kinetic energy of the particles in a substance.

7. Solids
DEF: State of matter that has a definite shape and definite volume.
Particle arrangement
Tightly packed together
Particle movement
Vibrate in place

8. Picture
Particle movement
Vibrate in place

9. Examples
Salt
Plastic
Ice
Diamond
Wax
Digital watch screens

10. Liquids Particle arrangement
DEF: State of matter that has a no definite shape, but definite volume.
Particle arrangement
Loosely packed

11. Picture
Particle movement
Slide past each other

12. Melting point - When a solid gains enough energy to break the structure holding it together
Heat of fusion - energy needed to change a solid to a liquid

13. Gases
DEF: State of matter that has no definite shape or no definite volume
Particle arrangement
Widely spread out

14. Picture
Particle movement
Move freely – don’t touch each other much

15. Other info Expand to fill whatever container they are in.
Heat of Vaporization  Energy needed to change a liquid to a gas at its boiling point

16. Solid
Liquid
Gas
Shape
Definite
Not definite
Volume

17. Plasma
DEF: State of matter made up of positively and negatively charged particles
The most common form of matter in the universe.

18. Plasma Examples
Neon signs, fluorescent bulbs, lightning bolts, Northern lights, fire, stars.

19. Phase Change Graphs
Shows the temperatures at which substances change from solids to liquids, liquids to gases
Can show time or energy needed to make the changes

20. Phase changes - Adding energy
Phases
Change
Example
Solid  liquid
Melting
Ice  water
Liquid  Gas
Boiling
Water  steam
Solid  Gas
Subliming
Dry ice  CO2 Gas

21. Phase changes – Giving Off energy
Phases
Change
Example
Liquid  solid
Freezing
water  ice
Gas  liquid
Condensing
steam  water
Gas  solid
Depositing
Water vapor  frost

22. Phase change Graph

23. Water Phase Change Graph

24. Density
DEF: amount of mass in a certain volume.

25. Circle Formula

26. Variable Units m = mass g D = density Liquids – g/ml Solids – g/cm3
V = volume
Liquids - ml
Solids - cm3

27. What is the density of a 140g block of plastic whose volume is 200mL?

28. What is the density of a piece of iron that has a mass of 59
What is the density of a piece of iron that has a mass of 59.8g and a volume of 2.08 cm3?

29. Steel has a density of 7. 8 g/cm3. What must the volume of 33
Steel has a density of 7.8 g/cm3. What must the volume of 33.3 g of steel be?

30. Granite has a density of 4. 7 g/cm3. What is the mass of 46
Granite has a density of 4.7 g/cm3. What is the mass of 46.8 cm3 of granite?

31. Floating VS Sinking Water’s density is 1g/mL.
Objects density < 1 will float in water
Objects density > 1 will sink. in water
Less dense objects float, more dense sink, this applies to all substances.

32. Gas Laws
Sections 2 - 3

33. Objectives 16-2 Explain and apply Gas Laws.
16-3 Determine the viscosity of a liquid.

34. Viscosity – DEF: Resistance to flow
High viscosity  slow moving
EX: cold syrup, molasses, cold magma
Low viscosity  fast moving
EX: water, hot magma, bubble soap

35. Pressure DEF: Amount of force exerted per unit area Units Pascals (Pa)
Atmospheres (atm)

36. Relationships Higher altitude = lower pressure
Lower altitude = higher pressure
Deeper under water = higher pressure

37. Thermal expansion in gases is involved with two different gas laws.
Boyle’s Law
Charles’ Law

38. Boyle’s Law
DEF: The pressure a gas exerts on the walls of its container is inversely related to the volume of the container.
Relationship  Indirect
Constants  Temperature

39. Variables Formula Pressure
Pascals (Pa) kiloPascals (kPa) OR atmospheres (atm)
Volume
L, mL, cm3
Formula
P1V1 = P2V2

40. Ways to remember
Teeter-totter
Boyle watches PV
Real life examples
Popping a balloon
Syringe and marshmallow
Scuba diving

41. Try One! – Boyles’ Law
The initial pressure on a balloon is 35kPa and the starting volume is 2L. If the final pressure is 10kPa, what is the final volume?

42. Charles’ Law
DEF: The volume of a gas is directly related to the temperature of the gas.
Relationship  direct
Constants  Pressure

43. Variables - units must be the same
Volume
L, mL, cm3
Temperature
K - kelvin
Formula
T1V2 = T2 V1

44. Ways to remember
Window washer
Charles watches TV
Real life examples
Helium balloon
Aerosol can
Scuba tank in a hot car

45. Try one! – Charles’ Law
If the original temperature was 5K and the final was 15K, how much did the volume increase from 20L?