1. UNIT 2: PHYSICAL BEHAVIOR OF MATTER
DO NOW: Answer the following questions:
1. What is matter?
2. What are the different states of matter and
list one example of each?

2. Aim # 1: What kinds of matter are there?
What is matter?
Has mass
Takes up space
Made up of atoms

3. AIM # 1: What kinds of matter are there? Classification of matter
SUBSTANCES
Elements and Compounds: are all HOMOGENEOUS
containing the same composition of material throughout the sample
Elements: substances that cannot be broken down by chemical change
Symbols are on Periodic Table
Ex. N (nitrogen) Ni (nickel)

4. Two or more element symbols combined Ex. NaCl, H2O
Compounds: substances that are made up of elements chemically bonded together, can be decomposed by chemical means.
Two or more element symbols combined
Ex. NaCl, H2O
constant composition
MIXTURES: combination of substances that are not chemically combined together, and can be broken down by physical means ratio will vary

5. AIM # 2: How can you turn one form of matter into another form?

6. Ex: salt water Ex: sand water
AIM # 2: How can you turn one form of matter into another form? Types of mixtures
MIXTURES
Homogeneous Mixture: solution of uniform composition (aq)
Ex: salt water
Heterogeneous Mixture: non uniform composition
Ex: sand water

7. AIM # 2: How can you turn one form of matter into another form?
Soluble- the ability to be dissolved, produces a solution (aq)
Water is the universal solvent
Insoluble- unable to dissolve in a liquid, can remain a solid, or separate from the solution (s)
Miscible- “mixable”, the ability to form a homogenous mixture, the ability to dissolve within one another
Seltzer and orange juice
Immiscible- incapable of being mixed with one another
Oil and water (Italian salad dressing)

8. AIM # 2: How can you turn one form of matter into another form
AIM # 2: How can you turn one form of matter into another form? Law of Conservation
MATTER CANNOT BE CREATED NOR DESTROYED, BUT CAN CHANGE FROM ONE FORM TO ANOTHER

9. Law of Conservation Examples:
If 40 grams of substance A are reacted with 20 grams of substance B to form substance C, what will the mass of substance C be?
35 grams of liquid water are evaporated off in a closed container. How many grams of water vapor will there be when the process is done?
Magnesium metal is reacted with oxygen to form magnesium oxide. How will the mass of the magnesium oxide be compared to the combined masses of the magnesium metal and the oxygen that formed it?

10. Particle Diagrams

11. Particle Diagrams

14. Aim # 3: What are the specific properties of matter?
Intensive property- a property of matter that is independent of the amount, does not need a specific quantity
Color, melting point, boiling point, density
Extensive property- a property of matter that is dependent on the amount
Mass, Volume, length, shape

15. AIM # 3: What are the specific properties of matter
AIM # 3: What are the specific properties of matter? Physical Properties and Changes
Physical Changes: changes that change only the appearance of the substance, not its chemical identity
Physical Properties: properties that can be observed though physical change

16. AIM #3 : What are the specific properties of matter?

17. Chemical Properties and Changes
Chemical Changes: changes that result in changing the chemical composition of a substance, can be reversed by another chemical change – results in a new substances being formed
Chemical Properties: properties that can only be observed through a chemical change

20. AIM # 4 : How does the proximity of atoms or molecules to each other affect properties they exhibit?
States of Matter

21. SOLIDS Particles tightly packed together
Particle Movement type: vibrate
Has definite shape
Has definite volume
If you put a sneaker in a box its volume doesn’t change

22. LIQUIDS Particles are moderately packed together
Particle movement: Vibrate and Rotate
No definite shape, Takes the shape of its container
Has Definite Volume

23. GAS (vapor) Particles are loosely packed
Particle movement: Vibrate, Rotate & bounce off container
Has No Definite Shape
Has No Definite Volume

24. Phases of Matter

25. Aim # 5: How can we explain phase changes in terms of energy?
Temperature: Measure of average kinetic energy of the particles of a substance
Heat : The flow of energy due to a temperature difference.
Heat always flows from high temp to low temp
Exothermic- heat is released
Endothermic- heat is absorbed
Kelvin Temperature: scale that is directly proportional to
average KE (See Table T )

26. Melting change from SOLID to LIQUID Heat is absorbed -ENDOTHERMIC
Molecules spread out
Fusion
-no temp change even though energy is added
Average KE of particles remains the same
Particles absorb heat as Potential Energy

27. FREEZING change from LIQUID to SOLID Heat is removed -EXOTHERMIC
Molecules get closer
Solidification
no temp change, P.E. decreases

28. EVAPORATION LIQUID to GAS Heat is absorbed Molecules spread out
Vaporization
No change in temp
gain P.E.

29. CONDENSATION
GAS to LIQUID
Heat is removed
Molecules get closer

30. SUBLIMATION/ DEPOSITION
Sublimation: SOLID to GAS
Molecules spread out
Deposition: GAS to SOLID
Molecules get closer

31. Heating and Cooling Curves
Graph of temperature vs. time
Showing the phase changes of a substance
Time increases but temperature stays constant represent phase changes with no slope
Places with a slope indicate temperature changes

33. What caused the water to change phases during this experiment?
What is happening at the two plateaus on the graph?
Why doesn’t the temperature change at these spots?
The melting point of water occurs at the same temperature as the point of water.
What other phase changes happen at the same temperature?
Heating the water, increasing the temperature
Phase change
Kinetic energy doesn’t change
Freezing
Condensation and evaporation