1. Matter Chapter 3 1

2. Why does soda fizz when you open the bottle?
Why is the sun hot? When iron rusts, what’s happening?

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Objectives
Observe and explain the difference between states of matter.
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4. Universe Classified
Matter is the part of the universe that has mass and volume
There are three states of matter
Solid, liquid, and gas
Chemistry is the study of matter
The properties of different types of matter
The way matter behaves when influenced by other matter and/or energy 3

5. Some Criteria for the Classification of Matter
Composition (elements and compounds)
State (solid, liquid, gas)
Properties

6. States of Matter YES YES YES YES YES NO YES NO NO NO NO YES Property
Solid
Liquid
Gas
Definite mass
Definite volume
Definite shape
Compressible
Molecule Drawing
Examples
YES
YES
YES
YES
YES NO
YES NO NO NO NO
YES

7. 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

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9. Figure 3.1: Liquid water takes the shape of its container.

10. Teacher Website Select Interactive 1
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11. Figure 3.11: In ice, the water molecules vibrate randomly about their positions in the solid. Their motions are represented by arrows.
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12. Figure 3.12: Equal masses of hot water and cold water separated by a thin metal wall in an insulated box.
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13. Figure 3.13: The H2O molecules in hot water have much greater random motions than the H2O molecules in cold water.
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14. Figure 3.14: The water samples now have the same temperature (50°C) and have the same random motions.
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15. Condensation gas  liquid Freezing liquid  solid
Phase Changes
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.

16. Gallium metal has such a low melting point (30°C) that it melts from the heat of a hand.

17. NAME THAT PHASE CHANGE

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

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Objectives
Explain the difference between elements and compounds.
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21. 3-3 Elements and Compounds
a pure substance
same composition throughout
Contains only one type of atom
Can not be broken down into simpler substances by ordinary chemical reactions (not a nuclear reaction) 11

22. Chemical Symbols of Elements
System started by Jons Berzelius (Sweden, )
90-91 naturally occurring elements
One or two first letters of name of the element.
Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

23. Examples: Americium, Am Einsteinium, Es Bromine, Br Helium, He
Lead(Plumbum), Pb
Niobium, Nb
Iron (Ferrum), Fe
Mendelevium, Md
Examples of other elements: O2, H2, I2

24. Compound – chemical combination of two or more elements
Have two properties in common with elements:
1. pure substance
2. Homogeneous – same chemical composition at all times

25. Compounds cont. Have two properties that differ from elements:
two or more elements that are chemically combined, in a definite ratio
2. Compounds can be broken down by chemical reactions using energy:
a) decomposition - uses heat
b) electrolysis - uses electricity

26. > 10 million compounds elements are represented by symbols
compounds are represented by chemical formulas
chemical formula
1. symbol --> tells which elements are present in compounds
2. subscript (little # lower right) --> tells the number of atoms of each element

27. Properties of Compounds
Distinguishing Elements and Compounds
Properties of Compounds
Compounds have different properties from their individual elements.
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.

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

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

30. Classification of Matter (by composition)

31. Classification of Matter12

32. 3-4 Mixtures Mixtures can be classified as: Homogeneous Mixtures
Heterogeneous Mixtures 12

33. Homogeneous mixture = uniform throughout, appears to be one layer
Also called solutions
Examples: olive oil, salt water, lemonade, coffee, air
The substances in the olive oil are evenly distributed throughout the mixture

34. Example: Stainless Steel
A homogeneous mixture of:
-Iron (Fe)
-Chromium (Cr)
-Nickel (Ni)

35. Heterogeneous mixture = non-uniform, contains regions with different properties than other regions
- Examples: oil and vinegar, salad, chicken soup

36. Pure Substances vs. Mixtures
All samples have the same physical and chemical properties
Constant Composition  all samples have the same composition
Homogeneous
Separate into components based on chemical properties
Mixtures
Different samples may show different properties
Variable composition
Homogeneous or Heterogeneous
Separate into components based on physical properties
All mixtures are made of pure substances 13

37. Figure 3.4: When table salt is stirred into water (left), a homogeneous mixture called a solution forms (right).
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Identity Each of the following as a Pure Substance, Homogeneous Mixture or Heterogeneous Mixture
Gasoline
A stream with gravel on the bottom
Copper metal
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Identity Each of the following as a Pure Substance, Homogeneous Mixture or Heterogeneous Mixture
Gasoline
a homogenous mixture
A stream with gravel on the bottom
a heterogeneous mixture
Copper metal
A pure substance (all elements are pure substances)
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40. 3-5 Separation of Mixtures
Separate mixtures based on different physical properties of the components
Evaporation
Volatility
Chromatography
Adherence to a Surface
Filtration
State of Matter (solid/liquid/gas)
Distillation
Boiling Point
Technique
Different Physical Property
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41. Example: Separate iron filings from sulfur using a magnet.

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

43. -separate dissolved solids from a liquid in a homogeneous mixture
Figure 3.6: Distillation of a solution consisting of salt dissolved in water.
-separate dissolved solids from a liquid in a homogeneous mixture
-uses boiling and condensation.
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44. Distillation of Crude Oil (Refining)
Crude Oil is a mixture of Hydrocarbons

45. Distillation of Crude Oil

46. Chromatography separates mixtures of substances into their components.
Paper Chromatography
Chromatography separates mixtures of substances into their components.
They all have:
a stationary phase (a solid, or a liquid supported on a solid)
and a mobile phase (a liquid or a gas).
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Properties of Matter
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48. Extensive Properties mass –
Volume –
The volume of a basketball is greater than the volume of a golf ball.
a measure of the amount of matter the object contains.
of an object is a measure of the space occupied by the object.

49. Who has a greater volume?

50. 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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Objectives
Observe and explain the difference between states of matter.
Explain the difference between physical and chemical changes.
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52. 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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53. Is changing phase a physical or chemical change?

54. 3-2 Physical and Chemical Properties and Changes
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55. Properties of Matter
Physical Properties are the characteristics of matter that can be changed without changing its composition
Characteristics that are directly observable
Examples: Color, odor, hardness, density, melting point, boiling point, state, solubility. 4

56. 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

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Properties of Matter
Chemical Properties are the characteristics that determine how the composition of matter changes as a result of contact with other matter
- Examples: burning, decompose, reactivity, corrode, tarnish, explode, ferment
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58. Classify Each of the following as Physical or Chemical Properties
The boiling point of ethyl alcohol is 78°C.
Diamond is very hard.
Sugar ferments to form ethyl alcohol.
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59. Classify Each of the following as Physical or Chemical Properties
The boiling point of ethyl alcohol is 78°C.
Physical property – describes inherent characteristic of alcohol – boiling point
Diamond is very hard.
Physical property – describes inherent characteristic of diamond – hardness
Sugar ferments to form ethyl alcohol.
Chemical property – describes behavior of sugar – forming a new substance (ethyl alcohol)
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60. Changes in Matter
Physical Changes are changes to matter that do not result in a change in the composition
State Changes – boiling, melting, condensing
Breaking, splitting, grinding, cutting
Chemical Changes involve a change in the composition of the substance
Produce a new substance
Chemical reaction
Reactants  Products 8

61. Indications of a Chemical Reaction
Color change
Solid forms (precipitate)
Gas bubbles
Odor
Temperature change
Fizzing
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62. Formation of a Precipitate
Cu(OH)2
Precipitate

63. Classify Each of the following as Physical or Chemical Changes
Iron metal is melted.
Iron combines with oxygen to form rust.
Sugar ferments to form ethyl alcohol.
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64. Classify Each of the following as Physical or Chemical Changes
Iron is melted.
Physical change – describes a state change, but the material is still iron
Iron combines with oxygen to form rust..
Chemical change – describes how iron and oxygen react to make a new substance, rust
Sugar ferments to form ethyl alcohol.
Chemical change – describes how sugar forms a new substance (ethyl alcohol)
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65. Oxygen combines with the chemicals in wood to produce flames
Oxygen combines with the chemicals in wood to produce flames. Is a physical or chemical change taking place?
Source:
Jim Pickerell/
Stone/Getty Images

66. Burning of Methane CH4 +2O2  CO2 + 2H2O
l_______________l l_________________l
l l
reactants products

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

68. In a chemical change, what happens to matter that appears to be lost?

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

70. END
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