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1. Matter Chapters 7 and 8
2. Matter anything that has mass and takes up space
3. Volume Amount of space taken up, or occupied, by an object
All matter takes up space
All objects have volume
Since all objects have volume, they cannot share the same space at the same time
4. Measuring Volume of Liquid The tool most commonly used in a Gradulated Cylinder
Another tool used is a Glass Beaker
5. Measuring Volume of Liquid The surface of a liquid is not flat
The curve of the liquid is called a Meniscus
A liquid in any container has a meniscus. If is harder to see in larger containers
Liters (L) or Milliliters (mL) are units most often used
6. Measuring Volume of Solid The volume of any solid object is expressed in Cubic units
Cubic means having 3-Dimensions
Cubic meter (mł) and cubic centimeters (cmł) are the units most often used
7. Volume of Irregularly Shaped Object
You can measure the volume of a solid object by measuring the volume of water that the object displaces.
8. Comparing Solid and Liquid Volumes
1 mL = 1 cmł
Volumes of solids are never expressed in Liters or Milliliters
9. Measuring the Volume of Gases
A Gas expands to fill its container
If you know the volume of the container a gas is in, you know the volume of the gas.
10. Propane Tank
11. Helium Tank
12. Mass Amount of matter in an object
Which has more mass: Elephant or Newborn Baby?
Is a Puppy like a Bowling Ball?
13. An objects mass can be changed only by changing the amount of Matter in the object
Bowling Ball – mass is constant (Mass never changes)
Puppy – mass is not constant (Mass changes)
14. Difference Mass and Weight Mass
Matter
Always Constant anywhere in Universe
Measured by Balance
Units: Kilograms (kg), Grams (g), and Milligrams (mg)
16. Difference Mass and Weight Weight
Mass plus Gravitational Force
? Gravity – force or attraction between two objects
? Attraction depends on masses of objects and distance between objects
17. Varies depending on where object is in Universe
Measured by Spring Scale
Unit: Newtons (N)
19. Inertia Tendency of an object to resist a change in motion
Object rest will remain at rest unless acted upon by outside force (Newton’s Laws)
Greater Mass = Greater Inertia
20. Physical Properties Can be measured or observed without changing the identity of the Matter
(Helps identify the Object)
-- Color
-- Odor
-- Mass
-- Volume
21. Thermal Conductivity -- the ability to transfer thermal energy from one area to another (Styrofoam Cup)
State – the physical form in which a substance exists, such as a solid, liquid, gas or plasma (Ice, Water, Water Vapor)
Malleability – the ability to be pounded into thin sheets (Aluminum)
22. Good Conductor of Heat
23. Poor Conductor of Heat
24. Aluminum Sheet
25. Ductile -- the ability to be drawn or pulled into a wire (barbed wire, copper wiring)
Solubility – the ability to dissolve in another substance (Sugar in Water)
Density -- mass per unit volume (lead sinker)
26. Barbed Wire
27. Copper Wiring
28. Density The amount of Matter in a given space or volume
Density of a substance is always the same at a given pressure and volume
Density of one substance is usually different from that of another
Does not depend on total amount of substance
29. Density = Mass Divided by Volume
(D = M / V)
Example:
Find the Density of a substance with a Mass of 5kg and a Volume of 43 mł
30. 5 kg / 43 mł
= 0.12 kg / mł
31. Example:
What is the Density of an object whose Mass is 25 g and whose Volume is
10 cmł?
32. 25g / 10 cmł
= 2.5 g / cmł
33. Example:
Find the Density of a substance that has a Mass of 45 kg and a volume of
43 mł.
34. 45 kg / 43 mł
1.05 kg / mł
35. Physical Change Change affects one or more physical properties of a substance
Identity of substance NEVER changes
Examples
-Freezing Water, Sanding Piece Wood, Cutting Hair, Crushing Aluminum Can, Mixing Oil and Vinegar, Mixing Sugar and Water, Butter on Popcorn, Clay (statue)
36. Chemical Properties Describes a substance based on its ability to change into a new substance with different properties
- Flammability (Wood)
Non Flammability (Gold)
Reactivity with Oxygen (Iron – Rust)
Reactivity with Water
Reactivity with Acid
37. Chemical properties can be observed with your senses but are more difficult to tell
Substances always have their chemical properties even if they are not showing at the time
Example : Iron of an old automobile rusting
38. Example of a Chemical Property: Iron on an old Automobile Rusting
39. Characteristic Property Always the same regardless of how large or small the sample is
Used to identify and classify substance
Physical Property – (density, solubility)
Chemical Property – (flammability, reactivity)
40. Chemical Change Occurs when one or more substances are changed into entirely new substances with different properties
Examples
-- Baking a Cake, Soured Milk, Statue of Liberty, Alka Seltzer Tablets
41. Chemical Changes and Chemical Properties are NOT the same thing
A Chemical Property describes a substances ability to go through a chemical change
A Chemical Change is the actual process in which that substance changes into another substance
42. Signs Chemical Change Change Color or Odor
Heat
Fizzing or Foaming
Sound or Light
43. Can Chemical Changes Be Undone? Due to new substances being formed, you cannot reverse chemical change using physical means
Try to un-bake cake . . . . . .
In some circumstances and the right conditions, you can reverse some chemical changes (Water)
44. 3 States of Matter Physical forms in which a substance can exist
All forms are Physical Changes ONLY (Water)
Solid
Liquid
Gas
45. Solid State of Matter that has a definite shape and volume
Particles are very close together
More attraction between particles than liquid or gas
Particles move but not fast enough to overcome the attraction
46. 2 Kinds of Solids Crystalline – very ordered, 3-D arrangement of particles (repeating pattern)
Example – Iron, Diamond, Ice, Crystal
Amorphous – no special arrangement
Example – Glass, Rubber, and Wax
49. Liquid State of Matter that has definite Volume but takes the shape of its container
Particles move fast enough to overcome some of the attraction
Particles slide past each other until takes shape of container
50. Unique Characteristics of Liquids Surface Tension – force acts on the particles at the surface of a liquid (shape)
Viscosity – liquids resistance to flow
High Viscosity – Honey
Low Viscosity -- Water
51. Gases State of Matter that has no definite shape or Volume
Particles move very quickly, so attraction broken completely
52. Gas Behavior Behave differently than Solids and Liquids
Differences
Gas particles have large amounts empty space
Gas particles can change (Temperature and Pressure)
53. Temperature Is measure of how fast the particles in an object are moving
High Temperature – gas particles are moving faster and hitting all portions container (gas expanding) (pushing on sides of container)
Low Temperature – gas particles have less energy
54. Thanksgiving Day Parade How much Helium is needed to fill a parade balloon?
Depends on the temperature outside
56. Pressure Amount of force exerted on a given area of surface
Number of times the gas particles hit the inside of container
Basketball v. Beach Ball
57. Gas Behavior Laws Temperature, Pressure, and Volume of a Gas are linked
The changing of one factor affects the other two
58. Boyle’s Law States that for a fixed amount of Gas at constant Temperature, the volume of Gas is INVERSELY related to the Pressure.
59. Charles Law States that for fixed amount of Gas at Constant Temperature, the Volume of the Gas changes in the same way that Temperature of the Gas changes.
61. 4th State -- Plasma Clouds of Protons, Neutrons, and Electrons where all Electrons have come loose from their Atoms or Molecules
Ionized Gas
62. Most common state of
Matter in Universe
99% of Universe
Rare on Earth
63. Universe – Sun, Core of Stars, Quasars, Pulsars Supernovas, Solar Wind
Earth – Flames, Lightning, Auroras (Northern Lights)
Artificial Lights – Neon Lights, Fluorescent Lights, Plasma TV, Plasma Lamp
81. Future 5th State : Bose-Einstein
-- low temperatures
-- colder than solid
82. Change of State Change of substance from one physical form to another
All Change of State’s are Physical Changes
5 Kinds
1. Melting, 2. Freezing,
3. Evaporation, 4. Condensation
5. Sublimation
83. 1. Melting Change of State from Solid to Liquid
Energy added (particles move faster) (Melt)
Adding Energy will increase Temperature
Endothermic (Energy Gained)
84. Melting
85. Melting Point Temperature at which the substance changes from Solid to Liquid
Substances have unique melting points that help identify them
Example:
Gallium – 30 degrees Celsius
Body Temperature – 37 degrees Celsius
Table Salt – 801 degrees Celsius
86. 2. Freezing Change of State from Liquid to Solid
Energy removed (particles move slower)
Exothermic (Energy Removed)
87. Freezing
88. Freezing Point Temperature at which substance changes from Liquid to Solid
Freezing and Melting occur at same Temperature
89. 3. Evaporation Change of State from Liquid to Gas
Boiling – conversion of a liquid to a vapor when vapor pressure of the liquid equals the atmospheric pressure
Boiling Point – temperature at which liquid boils
(Endothermic – Energy Gained)
90. 4. Condensation Change of State from Gas to Liquid
Condensation Point – temperature at which Gas becomes Liquid
(Exothermic – Energy Removed)
91. 5. Sublimation Change of State where Solid changes directly into a Gas
Endothermic – Energy Gained
92. Temperature Change vs. Change of State Temperature change affects the speed of the particles
As a substance loses or absorbs energy, one of two things will occur
The Temperature will Change
The State will Change