1. Chapter 2 Matter and Change
2.1 Properties of Matter
2.2 Mixtures
2.3 Elements and Compounds
2.4 Chemical Reactions

2. Objectives: 2.1 Properties of Matter
Identify properties of matter as extensive and intensive
Define physical properties
Differentiate between the 3 states of matter

3. KEY TERMS Mass Volume Extensive Property Intensive Property Substance
Physical Property
Solid
Liquid
Gas
Vapor
Physical Change

4. Definitions
Mass (m) – the amount of matter an object contains (a numerical value of its inertia)
Volume(V) – the amount of space an object occupies
Extensive property - a property that depends on the amount of matter an object contains
Intensive property – a property that depends on type of matter an object contains
Substance – matter with uniform properties
Physical property - a quality or condition of a substance that can be observed without changing the composition of the substance

5. Definitions cont.
Physical change - a change that do not affect the composition of a substance
Chemical property – a quality or condition of a substance that can be observed with changing the composition of the substance

6. Why are windows made of glass?
CHEMISTRY & YOU
Why are windows made of glass?
In this lesson, you will learn how properties can be used to classify and identify matter.
Glass is transparent and heat resistant. Plastics degrade with UV light

7. Describing Matter
What you observe when you look at a particular sample of matter is its properties.
Is a solid shiny or dull?
Does a liquid flow quickly or slowly?
Is a gas odorless, or does it have a smell?
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8. Some Criteria for the Classification of Matter
Properties
State (solid, liquid, gas)
Composition

9. Intensive and Extensive Properties
Sulfur

10. Recall that matter is anything that has mass and takes up space.
Extensive Properties
Recall that matter is anything that has mass and takes up space.
The mass of an object is a measure of the amount of matter the object contains.
The mass of a basketball is greater than the mass of a golf ball.
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11. Extensive Properties
The volume of an object is a measure of the space occupied by the object.
The volume of a basketball is greater than the volume of a golf ball.
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12. Who has a greater volume?

13. Mass and volume are both examples of extensive properties.
An extensive property is a property that depends on the amount of matter in a sample.
Examples: mass and volume
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14. Intensive Properties
An intensive property is a property that depends on the type of matter in a sample, not the amount of matter.
Examples include:
- Hardness of an object Color
Softness Boiling point
Absorbency Odor
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15. Identifying a Substance
Matter that has a uniform and definite composition is called a substance.
Aluminum and copper are examples of substances, which are also referred to as pure substances.
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16. Examples of Physical Properties
A physical property is a quality or condition of a substance that can be observed or measured without changing the substance’s composition.
Examples: Color, odor, hardness, density, melting point, boiling point, state, solubility.

17. Example: Physical Properties
Substance
State
Color
Melting
Point (C°)
Boiling Point (C°)
Density (g/cm3)
Oxygen O2
Gas
Colorless
-218
-183
0.0014
Mercury Hg
Liquid
Silvery-white
-39
357
13.5
Bromine
Br2
Red-brown -7 59
3.12
Water
H2O
100
1.00
Sodium Chloride
NaCl
Solid
White
801
1413
2.17

18. What are the 3 states of matter?
Solid
Liquid
Gas

19. States of Matter Property Solid Liquid Gas Yes No Definite mass
Definite volume No
Definite shape
Compressible
Molecule Drawing
Examples
rock, cookie, gold bar
Water, oil
Air, helium, nitrogen

20. States of Matter Solid fixed shape and volume, incompressible Liquid
fixed volume, takes the shape of its container
Gas
takes the volume and shape of its container

22. Bromine
Gas (Vapor)
Liquid

23. The melting point of gallium metal is 30˚C
The melting point of gallium metal is 30˚C. The figure at left shows how the heat from a person’s hand can melt a sample of gallium.
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24. Change of Phase Melting solid  liquid Condensation gas  liquid
Freezing liquid  solid
Deposition gas  solid
Evaporation liquid  gas
Sublimation solid  gas
*Boiling: Evaporation occurring beneath the liquid’s surface.

25. Is changing phase a physical or chemical change?

26. Physical Changes
During a physical change, some properties of a material change, but the composition of the material does not change.
Melting is a physical change.
Words such as boil, freeze, melt, and condense are used to describe physical changes.
So are words such as break, split, grind, cut, and crush.
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27. Do Now
Name the phase change you see in the images.

28. Name the phase change

29. Name the phase change

32. Video - https://www.youtube.com/watch?v=wln6WSv-cro

33. Chemical Properties
Chemical property – a quality or condition of a substance that can be observed with changing the composition of the substance
Examples:
Flammability
rusting
reactivity
corrosion

34. 2.2 MIXTURES
Objectives:
Categorize samples of matter into substance or mixture
Differentiate between homogeneous and heterogeneous
Describe two ways that components of mixtures can be separated

35. KEY TERMS Mixture - physical blend of 2 or more substances
Heterogeneous – mixture in which the composition is not uniform
throughout
Homogeneous – mixture with a uniform composition throughout
Phase – a part of a mixture with uniform composition
Solution – another name for homogeneous mixture
Filtration a process that separates a solid from a liquid
Distillation a process that separates a solid dissolved in a liquid/
separation of 2 miscible liquids with different boiling
temperatures
Miscible or more liquids that can form a homogeneous mixture

36. Matter that has a uniform and definite composition.
(Pure) Substance
Matter that has a uniform and definite composition.
Elements
Compounds

37. Classification of Matter (by composition)

38. A physical blend of two or more substances.
Mixture
A physical blend of two or more substances.

39. Most samples of matter are mixtures.
Describing Matter
Most samples of matter are mixtures.
Some mixtures are easier to recognize than others.
You can easily recognize chicken noodle soup as a mixture of chicken, noodles, and broth.
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40. Copper II Sulfate and its solution in water.

41. Mixtures can be classified as
Homogenous mixtures
Heterogeneous mixtures

42. A homogeneous mixture is a mixture in which the composition is the same throughout.
Examples: olive oil, lemonade, coffee, air, alloys

43. Describing Matter
Homogeneous Mixtures
The substances in the olive oil are evenly distributed throughout the mixture.
So, olive oil doesn’t look like a mixture.
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44. Example: Stainless Steel
A homogeneous mixture of:
-Iron (Fe)
-Chromium (Cr)
-Nickel (Ni)

45. Note: Mixtures can be physically separated
heterogeneous mixture: a mixture that is not uniform in composition; components are not evenly distributed throughout the mixture
Examples:
Oil and vinegar (mixed together)
Salad
Chicken soup
Note: Mixtures can be physically separated

46. Separation Methods
Use differences in the physical properties of the components of the mixture.

47. Example: Separate iron filings from sulfur using a magnet.

48. Filtration: separates a solid from a liquid in a heterogeneous mixture

49. Distillation: -separate dissolved solids from a liquid -uses boiling and condensation.

50. Distillation of Crude Oil (Refining)
Crude Oil is a mixture of Hydrocarbons

51. Distillation of Crude Oil

52. 2.3 Elements and Compounds

53. Elements The simplest substances.
Can not be separated into simpler substances.
Building blocks of all matter.
More than 100 known elements.
Represented by chemical symbols.

54. Chemical Symbols of Elements
System started by Jons Berzelius (Sweden, )
One or two first letters of name of the element.
Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

55. Examples: Americium, Am Einsteinium, Es Bromine, Br Helium, He
Lead(Plumbum), Pb
Niobium, Nb
Iron (Ferrum), Fe
Mendelevium, Md

56. Compound (Ex: H2O -> liquid O2 -> gas H2 -> gas)
A substance that contains two or more elements chemically combined.
Can be broken down into simpler substances
Compounds have different properties from the individual substances.
(Ex: H2O -> liquid O2 -> gas H2 -> gas)

57. Properties of Compounds
Distinguishing Elements and Compounds
Properties of Compounds
When the elements sodium and chlorine combine chemically to form sodium chloride, there is a change in composition and a change in properties.
Sodium chloride (commonly known as table salt) is a white solid.

58. Breaking down Compounds
Distinguishing Elements and Compounds
Breaking down Compounds
Breaking down NaCl
Sodium is a soft gray metal.

59. Breaking down Compounds
Distinguishing Elements and Compounds
Breaking down Compounds
Breaking down NaCl
Chlorine is a pale yellow poisonous gas.

60. If composition is fixed and may not change substance
Substance or mixture?
If composition is fixed and may not change
substance

62. 2.4 Chemical Properties and Chemical Changes

63. H2O composition is fixed- compound
Gaseous Phase
Liquid Phase

64. Chemical Properties
Chemical property - a quality or condition of a substance that can be observed with changing the composition of the substance
Example: Magnesium reacts with oxygen to form magnesium oxide.

65. Magnesium Mg

66. Burning of Magnesium 2Mg+ O2 2MgO

67. Physical Change vs Chemical Change
Physical change - Composition does not change.
May be reversible or irreversible.
Example of reversible:
Liquid water -> steam
Steam -> liquid water

68. Chemical Changes
When charcoal is broken into smaller pieces, the change is a physical change.
During a physical change, the composition of the matter never changes.
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69. Chemical Change
Chemical change - a change that produces matter with a different composition than the original matter.
Atoms rearrange themselves into new combinations.

70. Chemical Changes Words that describe chemical changes:
- Burn - decompose
- rot - ferment
- rust - corrode
- explode
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71. When the charcoal is heated and burned, a chemical change occurs.
Chemical Changes
When the charcoal is heated and burned, a chemical change occurs.
The substances in charcoal react with oxygen in the air to form other substances.
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72. Burning of Methane CH4 +2O2 CO2 + 2H2O

73. Burning of Methane CH4 + 2O2 CO2 + 2H2O

74. Recognizing a Chemical Change
energy exchange
production of a gas
color change
formation of a precipitate

75. Formation of a Precipitate
Cu(OH)2
Precipitate

76. The Law of Conservation of Mass (Antoine Lavoisier)
In any chemical or physical change, mass is neither created or destroyed
Mass is CONSTANT

77. END OF SHOW

78. Example: H2O