1. Are these things matter?
IPC02 Properties of Matter
Are these things matter?
Your book, your desk, your lunch, the air that you breathe and the water you drink?
How do you know?
RETURN TO TEACHER AFTER COPYING!!!

2. IPC02 Properties of Matter
Matter is anything that has mass and volume. 1. Mass is the amount of matter an object has. 2. Volume is the amount of space an object takes up.
Question: Will an inflated balloon weigh more, less, or the same as the same balloon deflated?
Make a hypothesis, then test it.
Obtain the mass of a balloon, then inflate it, and then obtain the new mass.
RETURN TO TEACHER AFTER COPYING!!!

4. What are some mixtures found in your kitchen?
Mixtures: contain more than one type of matter and are physically combined.
What are some mixtures found in your kitchen?
Homogeneous Mixture
(Solution)
uniform (same) throughout in composition
Examples:
coffee
air (mixture of gases) Alloys like:
brass (Cu & Zn)
steel (Fe & C)
Heterogeneous Mixture
not uniform (different) throughout in composition
Examples:
sand in water
tea with ice cubes
oil in water
chicken noodle soup

5. What is soda? Heterogenous or Homogeneous?
Heterogeneous
When you see the gas bubbles.
Homogeneous
When you don’t see the gas bubbles.
But if asked, say homogeneous!

6. Separation of Mixtures
Mixtures can be separated by physical means.
a) Filtration
b) Centrifuge
c) Chromatography
d) Distillation
e) Crystallization
Separate sand and salt?

7. Pure Substances: contain only one type of matter.
Compounds
made from more than one kind of atom
A molecule is the smallest particle of a compound that retains its properties.
Compounds cannot be separated by physical means! (only by chemical reactions)
Ex: salt, distilled water, sugar
Elements
made of only one kind of atom.
An atom is the smallest part of an element).
Ex:

8. Separation of Compounds
Compounds can be separated chemical means.
Examples:
a) Electrolysis of water
water  hydrogen gas and oxygen gas
b) Chemical Reactions
Magnesium + Acid  hydrogen gas
Mg + HCl (acid)  MgCl2 + H2
So the properties of compounds may be similar or different than the properties of their elements!

9. Classify Matter Element, Compound, Homogenous mixture, or Heterogeneous mixture
Boric Acid Solution
Oxygen gas (O2)
Carbon monoxide (CO)
Steel (Carbon, Iron)
Casserole
Homogeneous mixture
Element (molecule)
Compound
Homogeneous mixture
Heterogeneous mixture

10. Complete the classification chart now.
Classify each of the following as either:
(E) – Element (HomM) – Homogeneous Mixture
(C) – Compound (HetM) – Heterogeneous Mixture
Classify:
Type of Matter:
charcoal (carbon)
rock garden
chlorine (Cl)
air E
HetM E
HomM
Complete the classification chart now.
Skip the classification cards diagram below for now.
You will do it later. Its due at end of class

11. Starter Classify the following compounds
Finish the yellow homework (exit ticket)
Classify:
Type of Matter:
charcoal (carbon)
rock garden
chlorine (Cl)
air
Day 2

12. Properties of Matter Property – a characteristic
Physical properties:
characteristics that can be observed or measured without changing the identity of the substance.
Gasoline has a distinct odor, it is colorless, and a liquid at room temperature.
Chemical properties:
characteristics of a substance’s “ability” to change into a different substance.
Gasoline is combustible and flammable
Day 2

13. Hardness - resistance to scratching.
Physical Properties
More examples
Hardness - resistance to scratching.
luster – shine
Solubility – ability to dissolve in water
Elasticity – ability to be stretched or bounce
Which would you rather play “basketball” with?
A) bowling ball
B) volleyball

14. Brittleness –tendency to shatter
Physical Properties
More examples
Brittleness –tendency to shatter
Malleability –be pounded into thin sheets.
Ductility – be drawn into thin wire.
Tensile Strength – the tension it can withstand before breaking.

15. Phase Change –change to and from solids, liquids and gasses.
Physical Properties
More examples
Phase Change –change to and from solids, liquids and gasses.
Viscosity –the resistance to flow
Magnetism – attracted by a magnet.
Color – the current color.
Odor – the Smell.

16. Chemical Properties
More examples
CombustibilitY & Flammability – capable of catching fire and burning .
pH – measure of acidity.
reactivity – ability to react to form a new substance.

17. How many properties did you come up with?
Chemical
Physical
combustibility
flammability
reactivity
pH (acidity)
Ex: Silver will tarnish because of reactivity
density
hardness
luster
solubility
elasticity
brittleness
malleability
ductility
tensile strength
Electrical
conductivity
melting point
boiling point
freezing point
viscosity
magnetism
odor
color
solid
liquid
gas

18. Changes of Matter Physical Changes:
A change that does not produce a new substance.
Usually reversible.
Ex: Ice melts into water.
Chemical Changes:
A change that does produce a new substance.
Usually not reversible.
Ex: Iron rusts forming iron oxide.

19. How do you know a chemical change has occurred?
Evidence of a
Chemical Change:
Energy (Heat):
absorbed energy (endothermic)
released energy (exothermic)
Gas is produced (bubbles)
Solid (precipitate) forms
Odor or color change occurs
New
substances
are formed

20. Physical & Chemical Changes
Plant loses water through evaporation
Toothpick is broken
Sugar dissolves
Ice cube melts
Food coloring
Copper wire is cut
Chemical
Energy  ATP
Match burns
Bike rusts
Gasoline burns
Silver tarnishes
Leaves change color
Food is digested
Acid + Base  Salt

21. Why are these chemical changes?

22. IPC02 Properties of Matter
Tea Party Properties
In an envelope provided by the teacher are
Physical and Chemical Properties (Orange Cards)
Physical and Chemical Changes (Blue or White Cards)
Organize the orange cards into two piles: Physical and Chemical Properties.
RETURN TO TEACHER AFTER COPYING!!!

23. Physical & Chemical Changes in
The Rock Cycle
Where are physical changes occurring?
Where are chemical changes occurring?
Cooling & Melting
Weathering & Erosion
Deposition & Cementation
Forming Metamorphic Rock thru heat & pressure and forming Igneous Rock thru crystallization

24. Tarnishing in moist air Silver in color Conducts electricity
Identify the following as a physical property, a chemical property, a physical change, or a chemical change.
Ice melting
Tarnishing in moist air
Silver in color
Conducts electricity
Ability to explode
Recycled aluminum can
Ability to react with acid
Burned the popcorn
Physical change
Chemical change
Physical property
Physical property
Chemical property
Physical change
Chemical property
Chemical change
Do Worksheets

25. Starter
Quiz today Pick up white and green handout. Pick up returned HW.
What are each of these? HomM, HetM, Compound or Element?
What are each of these? ChemC, PhysC, ChemP or PhysP?  1
tap water (H2O, minerals)  2
salt water solution  3
quartz sand (SiO2)  4
vegetable soup  5
table salt (NaCl)  6
sugar (C6H12O6)  7
hydrochloric acid solution  8
neon gas (Ne)
aluminum is malleable __________
ability of sodium to react with chlorine__________
leaf turning red __________
a pond freezes over__________
iron rusting __________
paper being torn __________
TNT is explosive __________
acetone is volatile (vaporizes easily)__________
Day 3

26. Video: States of Matter
Oobleck
PLASMA
MythBusters

27. States of Matter Phase Shape Volume Fluidity Solid Definite
Fixed position
Liquid
Indefinite
Fluid
Gas
Plasma – “charged gas”.

28. Plasma
Plasma is a gas containing charged particles such as electrons and ions.
It is the most common state of matter in the universe.

29. Molecular Motion Increases
Changes of State
Solid Liquid Gas
Molecular Motion Increases

30. What is meant by “change of state”?

31. Change of State: a physical change between states of matter.
Temperature influences changes of state.
As temperature increases, the internal energy increases.
S L  G
(Boiling)
Temperature
Click Here and run applet

32. The Phase Change Graph Temp is
L & G
Temp is
constant
Phase changes require a gain or loss of Energy.
During a phase change, the temperature does NOT change.
When can two states coexist? During a phase change.
S & L
Temp is
constant

33. Solid: Substance with a definite shape and volume
Liquid: Substance with a definite volume but not a definite shape
Gas: Substance with no definite volume or shape
Plasma: Substance that is extremely high in energy and is rare on earth but common in stars

34. Phase changes in matter are:
Melting: change from a solid to a liquid
Freezing: change from a liquid to a solid
Vaporization: the change from liquid to gas
Evaporization: vaporization from the surface of a liquid.
Boiling: vaporization from within as well as from the surface of a liquid
Condensation: change from a gas to a liquid
Sublimation: change from a solid to a gas
Deposition: change from gas to solid

35. Real World Experiences!
How does it feel when you put rubbing alcohol on your skin? Why?
What happens to “dry ice” when left on the counter? Why?
What happens to “moth balls” left in storage trunks?
Your skin feels cold because when alcohol evaporates, it absorbs heat energy from your skin.
“Dry ice” (solid carbon dioxide) does not disappear, but it sublimes into a gas.
“Moth balls” (solid napthalene) do not disappear, but it sublimes into a gas. The fumes kill the moths.

36. Starter
Pick up green handout. Pick up homework and grades back tables.
Turn in white notes from last class and green demo lab pick up a calculator
1. In which of these materials do particles have the slowest motion and MOST ordered arrangement?
a gas such as nitrogen C. a solid compound such as baking soda
a liquid such as salt water D. a mixture such as coke a cola
2. How can scientists separate elements in compounds and in mixtures?
By heating them to their gaseous state.
By chemical reactions that recombine or rearrange atoms
They separate elements in compounds by chemical reactions, and elements in mixtures by physical processes.
They separate elements in compounds by physical reactions and elements in mixtures by physical processes.
3. At a Halloween party students observe dry ice at room temperature. The solid sublimes directly to the gas state. This sublimation is accompanied by which change in the carbon dioxide?
decrease in volume C. increase in mass
decrease in particle number D. increase in particle motion
Day 5

38. Matter is anything that has mass and volume. 1
Matter is anything that has mass and volume. 1. Mass is the amount of matter an object has. 2. Volume is the amount of space an object takes up.
Question: Will an inflated balloon weigh more, less, or the same as the same balloon deflated?
Make a hypothesis, then test it.
Obtain the mass of a balloon, then inflate it, and then obtain the new mass.

39. Mass vs. Weight Amount of matter Use a balance Kg
Doesn’t change with location
Pull of gravity
Use a scale
Newton
Does change with location

40. Which has more mass? A) 1 kilogram of feathers B) 1 kilogram of bricks
They are the same!
1 kg = 1 kg

41. Which takes up more space
Which takes up more space? A) 1 kilogram of feathers B) 1 kilogram of bricks
The Feathers

42. Measure matter by finding the density!
Which has the greater density? A) steel bar B) steel paper clip
The density of steel is the same! Size doesn’t matter!

43. Density of Steel
steel bar

44. Units for Density Metric Units: Solid: g/cm3 Liquid: g/mL
Density of water is 1g/mL (at 4º C)
Memorize
This!

45. Ice! Because it is less dense.
Which one floats? Why?
Density of Water: g/mL
Density of Ice: g/mL
Ice! Because it is less dense.

46. Which of the following will float on water
Which of the following will float on water? Why is it good to know the density?
Density
helps you
identify a substance
All those less
than 1.0 g/mL

47. Predict the correct “floating order” of the substances as they would appear in the “Density Column”.
Density g/cm3
Copper
8.8
Corn oil
0.925
Corn syrup
1.38
Glycerin
1.26
Mercury
13.6
Plastic
0.93
Rubber
1.34
Tar
1.02
Water
1.00
Wood
0.7

48. Make your own density column
Get out your density column handout.
Get some colored pencils, scissors and glue sticks
Color and arrange your density columns with the least dense on top and most dense on bottom
You have 15 minutes

49. Calculating Density d m v Obtain mass using a balance.
Obtain volume by any of these methods.
Ruler: Volume = L x W x H
Graduated cylinder
Water displacement
d = m/v m = d x v v = m/d d m v
“Magic Circles” 

50. Is the bar really gold or fool’s gold
Is the bar really gold or fool’s gold? Find the density of the bar if the mass is g and the dimensions are 3.5 cm by 3.5 cm by 8.0 cm.
Gold has a density of 19.3 g/cm3
V = L x W x H
D = M/V
g / 98 cm3
= 19.3 g/cm3 Yes it’s gold! m d v

51. Is this liquid water, alcohol, or kerosene
Is this liquid water, alcohol, or kerosene? Find the density of the liquid if the mass is g? Water g/mL Alcohol g/mL Kerosene 0.82 g/mL
Read the volume 
D = M/V
16.98 g / 21.5 mL
= 0.79 g/mL It is alcohol! m d v

52. Starter
Pick up HW, and yellow handout. Today we finish green. Yellow is HW
100 grams of a liquid completely fill a 200 mL bottle. What is the density of the liquid?
Mrs Butterworths pancake syrup has a density of 1.5 g/mL. What would be the approximate mass of the syrup in a 500 mL bottle?
These 4 liquids are poured into a graduated cylinder. What order would you pour them to keep them separate?
The air you breath everyday is what?
A compound, mixture, solution or
element?
Day 6
Honey
1.48 g/ml
Alcohol
0.79 g/ml
Water
1.00 g/ml
Shampoo
1.06 g/ml

53. Is the “Silver Surfer” really made of silver
Is the “Silver Surfer” really made of silver? We obtained a sample with a mass of g. Platinum 21.5 g/cm3 Silver 10.5 g/cm3 Tin 7.3 g/cm3
Find the volume by water displacement.
d = m/v
= g / 25 cm3
= 10.5 g/cm3 It is Silver! m d v

54. What is the volume in mL of this syrup if it has a density of 0
What is the volume in mL of this syrup if it has a density of 0.63 g/mL and a mass of 78 g?
v = m/d
= 78g ÷ 0.63 g/mL
= mL m d v

55. What is the mass in grams of this lead pipe if it has a density of 11
What is the mass in grams of this lead pipe if it has a density of 11.4 g/cm3 and a volume of 55 cc?
m = d x v
= 11.4 g/cm3 x 55 cc
= 627 g m d v

56. Lab: Determining
Density

57. Densities of Cylinders
0.64 Walnut Polyurethane
0.75 Oak Phenolic
0.77 Maple PVC
0.90 Polypropylene 1.42 Acetyl
0.92 LDPE Teflon
1.15 Nylon Aluminum
1.17 Acrylic Brass
8.91 Copper

58. Question: Can you create a stack of liquids?
Purpose: To measure the density of various liquids and decide how to stack the liquids. Then, use the density column to predict the density of other objects.
Materials:
molasses, water, vegetable oil
light corn, syrup, glycerin, cork
rubber stopper, graduated cylinder
plastic droppers,
 small steel object, paper towels

59. Procedure:
Obtain the precise mass of an empty plastic dropper. Record the mass: ________g Note: this mass should not change, but double check anyway.
Fill the plastic dropper completely with water (substance).
Obtain the mass of the dropper and the water (substance). Subtract the mass of the empty plastic dropper (from step 1). Record the mass of the water (substance) in Data Table 1.

60. Squirt the water from the dropper into a 10 mL graduated cylinder and measure the precise volume. Record the volume in Data Table 1. Note: this will be the volume for all the substances measured using this size plastic dropper.
Calculate the density and record in Data Table 1.
Repeat steps 2-3 for each substance in Data Table 1. Record your measurements. Set aside each dropper filled with substance for later. Do not throw away your droppers. Place them upside down in a beaker.
Once you have obtained your measurements and calculated density for each substance, determine the order of how you will stack your liquids to create a “density column”. List your order of your liquids in Data Table 2.

61. According to your list from Data Table 2, carefully squirt the contents of each dropper beginning with the bottom liquid into your graduated cylinder to create your density column.
In Data Table 3, predict where each solid object will “float” when placed in the density column.
Gently place the objects (one at a time) into the density column beginning with the object you believe will sink the furthest to the bottom.

62. Starter 10/7/13 Work questions 3 and 4 on the yellow HW problems.
The quiz will have the same sort of problems.
Day 7

63. is the tendency for a less dense substance to float in a
Buoyancy
is the tendency for a less dense
substance to float in a
more dense substance.
Boats are made so that they have a lower density than water.

64. Click on picture for demo.
Buoyant Force
The upward force exerted on an object immersed in a fluid is called the “buoyant force”.
Click on picture for demo.

65. Draw a vector to show the buoyant force (up) and the weight force (down).
Weight Force (Gravity)
Which liquid exerts a greater buoyant force on the block?
Blue or Clear?
Buoyant Force
Blue (greater)

66. Why does a block of steel sink, but a steel boat float?
The Titanic Sinks
What two forces are involved?

67. When will an object sink or float?
Weight Force > Buoyant Force
Density of object > density of fluid
Float
Weight Force < Buoyant Force
Density of object < density of fluid
(greater than)
(less than)

68. Archimedes Principle
The buoyant force exerted on an object in a fluid is equal to the weight of the fluid displaced by the object.
It explains:
the buoyancy of ships
the rise of a balloon in the air
the loss of weight of objects underwater.
Sink of Float
buoyancy.html
2 N
2 N

69. Archimedes’ Principle Practice:
Rock weighs 2.25 N
In water, the rock weighs 1.8 N
The water displaced by the rock:
2.25N – 1.8 N = 0.45 N.
So, the buoyant force exerted on the rock is 0.45 N.
0.45 N

70. Do all fluids exert the same buoyant force on an object?
Which liquid exerts a greater buoyant force?
Mercury

71. Buoyant force of stacked liquids?
If I stacked the liquids which liquid would have the greatest buoyant force on the tar ball?
Water
Glycerin
Corn syrup
Mercury

72. Buoyancy and Fluid How do Submarines work?

73. Lab: “Whatever floats your boat”
Can you make a clay boat float?
Virtual Lab:

74. Buoyancy and Gases Why do hot air balloons float?
A balloon will float when the weight of the balloon is less than the weight of the volume of air displaced.
Air in the balloon is heated to make it less dense than the surrounding air.

75. The beach ball and the basketball each contain the same amount of air.
Which has the greater amount of pressure and why?
The basketball has greater pressure than the beach ball because it has less volume causing the air particles to have less space.

76. flows slower? Starter etchor Molasses?
Ketchup
Why does ketchup flow so slow?Viscosity is the resistance to flow due to:
Large, bumpy molecules
Strong attraction between molecules

77. How does temperature affect viscosity?
As a gas gets warmer, its viscosity ___________.
Why?
As a liquid gets warmer, its viscosity __________.
Ex: cold honey vs. warm honey
decreases
increases
Because the number of collisions increase causing friction which slows the molecules down.

78. Why do companies want you to heat up your syrup before using it?
Increase temperature…
Decrease Viscosity…
Use more syrup!!
Buy more syrup!!

79. Viscosity Lab Virtual Viscosity Lab
Compare the viscosity of different fluids.
Observe the effects of temperature on viscosity.
Viscosity