1. Warm - Up
Are the following signs of physical change or chemical change?
Melting
Heating up
Rusting
Cookie rising
Bubbles
Gas being produced
7. Change in color
8. Solids forming
9. Dissolving
10. Precipitation
11. Cooling down
12. Release of light
13. Fire

2. Warm - up Round to correct sig fig answers addition / subtraction= = = =
Round to correct sig fig answers
multiplication / division
25.00 * =
3.0 * 1.25 =
80.0 / 4 =
0.025 * 3 =

4. States of Matter Ch.3 Wu 4

5. Energy and the four states of matter 5

6. Phet States of Matter 6

7. How Shape & Volume Classifies Materials
Materials can be classified as solids, liquids, or gases based on whether their shapes and volume are definite or variable
Definition: a solid is the state in which materials have a definite shape and definite volume
Definition: definite means that shape and volume won’t change unless the material is acted on by an outside force

10. Definition: a liquid is the state of matter in which material has a definite volume but not a definite shape
Liquids will take the shape of their container

11. Definition: a gas is the state of matter in which a material has no definite shape and no definite volume
Gases will expand to completely fill the volume & take the shape of their container

12. Almost all matter exists as a solid, liquid or gas on Earth
This is not true for the universe
In places with the temperature of stars, matter exists in a state called plasma
In 1995, scientists discovered a fifth state of matter called BCE (Bose-Einstein condensate)
At temperatures close to absolute zero (0 K or -273ºC), BCE groups of atoms behave as if they were a single particle

13. Plasma 99% of the matter in the universe
Common found on the hot temperatures present in stars
Ted-ed: Plasmas the spectacular and practical 13

14. Bose-Einstein Condensate
Predicted by Einstein in the 1920s
Near -273 oC or 0 K (absolute zero)
Groups of atoms behave as though they were a single particle 14

15. Kinetic Theory “Kinetic” = Greek for “to move”
Kinetic Energy is the energy an object has due to its motion
1. That all particles of matter are in constant motion
2. There are forces of attraction among all particles of matter 15

16. Kinetic theory of gasses says:
1. The constant motion of particles in a gas allows a gas to fill a container of any shape or size
2. Particles in a gas are in constant, rapid, random motion
3. The motion of 1 particle of gas is unaffected by other particles of gas unless they collide
4. Forces of attraction among particles of gas can be ignored under ordinary conditions

17. The Kelvin Temperature Scale
Directly proportional to average kinetic energy
At absolute zero
(0 K = -273 oC)
molecular movements cease
oC = K 17

18. 3.1 Short Response Q’s
How are shape and volume used to classify solids, liquids, and gases?
What does the kinetic theory say about the motion of atoms?
How is a gas able to fill a container of any size or shape
Use kinetic theory and attractive forces to explain why a liquid has a definite volume and a shape that can vary.
Explain why a solid has a definite shape and volume.
How does the arrangement of atoms in most solids differ from the arrangement of atoms in a liquid?
A hazardous chemical is leaking. Why are more people likely to be affected if the chemical is a gas, rather than a liquid?

20. Warm up

22. Ch 3.2 The Gas Laws
Pressure is the result of a force distributed over an area P=F/A
SI Unit is Pa (Pascals) = N/m2 (Newton / meter2)
Collision between the particles of gas and the walls of the container cause pressure.

23. How heavy is air?

24. Factors that affect gas pressure
Temperature
Volume
Number of particles

25. 1) Temperature P∝T

26. 2) Volume P∝1/V

27. 3) Number of Particles P∝n

28. As temperature inc. volume inc.
Charle’s Law
As temperature inc. volume inc.

29. As pressure inc. volume dec.
Boyle’s Law
As pressure inc. volume dec.

30. Combined Gas Law

31. Pressure as it applies to weather
Wind blows from high to low pressure
Uneven heating of the earth causes H/L pressure
High pressure (cold air) higher density
Low pressure (hot air) lower density

32. Ted-ed What Makes Wind?

33. 3.2 Short Response
How is the gas pressure produced in a closed container of gas?
What 3 factors affect gas pressure?
How does increasing the temperature affected the pressure of a contained gas?
What happens to the pressure of a gas if its volume is reduced?
How does increasing the number of particles of a contained gas affect its pressure?
What happens to the pressure in a tire if air is slowly leaking out of the tire? Explain
Some liquid products are sold in aerosol cans. Gas is stored in a can under pressure and is used to propel the liquid out of the can. Explain why an aerosol can should never be thrown in to a fireplace or incinerator.

35. 3.3 Phase Changes

37. Definition: a phase change is the reversible physical change that occurs when a substance changes from one state of matter to another
Six common phase changes: melting, freezing, vaporization, condensation, sublimation, and deposition

39. ex. Dry ice, snow “ghosts”

40. Ex. Frost

41. Ex. Dew, “sweat”

42. The temperature of a substance does not change during a phase change
For example, water temperature remains constant when boiling to go from liquid to gas or when condensing from a gas to liquid
Q: At what temperature does water boil and condense?

43. Energy is either absorbed or transferred during a phase change
The amount of energy absorbed depends on the substance & is a unique physical property for each substance
Definition: heat of fusion is the amount of energy absorbed when going from a solid to a liquid

44. Definition: exothermic changes occur when energy is released to the environment
An example of an exothermic change is water freezing since it releases its heat to the environment so that it can freeze
Definition: endothermic changes occur when energy is absorbed from the environment
An example is water melting since it gathers as much heat as possible from the environment to melt

46. Concept Question
When is it the coldest, before snow, when it is snowing, or after the snow when it is melting? Why?

47. The arrangement of molecules in water becomes less orderly as water melts and more orderly as water freezes
Solid water (ice) has molecules in a fixed position that vibrate about a fixed point
Freezing produces molecules in an orderly arrangement
Liquid water has molecules that are attracted to each other and slide past each other due to special chemical bonds
Melting allows a less orderly molecular arrangement

49. Definition: vaporization is a phase change from a liquid to a gas
Vaporization is endothermic since liquid water absorbs energy in the form of heat from the surroundings to go from liquid to gas
Definition: heat of vaporization is the amount of energy needed for a substance to change phases from liquid to gas
Heat of vaporization is a unique physical property for each substance

50. Definition: evaporation is the process that changes a substance from a liquid to a gas below the substance’s boiling point
Evaporation is a process that takes place at the surface of a liquid and occurs at temperatures below the boiling point
Definition: vapor pressure is the pressure caused by the collisions of vapor on the walls of the container
Vapor pressure increases as temperature increases

51. Boiling vs. evaporation

52. Q: How does surface area of a liquid affect the rate of evaporation?
Definition: the boiling point is where vapor pressure equals atmospheric pressure
Kinetic theory shows that as the temperature increases, water molecules move faster & faster until they have energy to overcome attractive forces of neighboring molecules

53. Concept Question
Where does the drops of liquid on the outside of a can of cola on a hot summer day come from and how do they form? 53

54. Why are there clouds?

55. 3.3 Short Response Name 6 common phase changes.
What happens to the temperature of a substance during a phase change?
How does the energy of a system change during a phase change?
What happens to the arrangement of water molecules as water melts and freezes?
What is the difference between evaporation and boiling?
Explain why sublimation and deposition are classified as physical change.
At room temperature, table salt is a solid and acetone is a liquid. Acetone is the main ingredient in nail polish remover. What conclusion can you draw about the melting points of these materials?
What are the steps must occur for a water molecular to start on the surface of hot bath water and end up on the surface of a bathroom mirror? Note whether each of the phase changes that takes place during the process are endothermic or exothermic.