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Title: Properties of Matter Andrew Jackson Duran Junior High Lesson


1
Properties of Matter
  • Andrew Jackson
  • Duran Junior High

2
Lesson 1 Our Ideas About Matter
  • You will perform a circuit of eight inquiries to
    observe how matter behaves. The inquiries
    involve the following different states of
    matter, changes of state, mass and volume,
    floating and sinking, thermal expansion,
    mixtures, solubility and insolubility, and
    chemical reactions.

3
Lesson 1
Question
  • What is matter?

4
Lesson 1
Conclusion
  • Matter - the physical material that has mass and
    occupies space.
  • Air is a gas.
  • Air and gases are forms of matter even though
    they are invisible.
  • The shape of an object does not affect its mass.
  • Some matter is soluble in water.
  • All liquids are not water or do not contain
    water.
  • Temperature change affects the volume of air.
  • Some liquids do not mix (immiscible).

5
Lesson 1 (1-3)
Vocabulary
  • 1. matter - the physical material that has mass
    and occupies space
  • 2. expansion - the increase in the volume of
    matter that occurs when matter is heated.
  • 3. contraction - decrease in volume of matter
    when matter is cooled.
  • 4. dissolving - the process that takes place
    when a solvent is mixed with a solute to make a
    solution.
  • 5. immiscible - liquids that are unable to
    dissolve in one another.
  • 6. miscible - liquids are able to dissolve in
    one another.

6
Lesson 1 - (2-3)
Vocabulary
  • 7. density - the mass of a known volume of a
    substance measured in g/cm3
  • 8. chemical reaction - any change that involves
    the formation of a new substance has reactants
    and products.
  • 9. mass - the amount of matter in an object
    measured in g or kg.
  • 10. volume - the amount of space occupied matter
    measured in L, mL, cm3, or m3.
  • 11. burning - a rapid chemical reaction between a
    substance and a gas that produces heat and light.
    Most burning or combustion takes place in the
    air and has oxygen as one of its reactants.

7
Lesson 1 (3-3)
Vocabulary
  • 12. solid - a phase or state of matter in which
    a substance has definite shape and volume.
  • 13. liquid - a state or phase of matter in which
    a substance has a definite volume but no definite
    shape. Liquids take the shape of the container
    they occupy.
  • 14. mixture - two or more elements or compounds
    that are mixed together but are not chemically
    combined.
  • 15. physical property - all the characteristic
    properties of a substance except those that
    determine how it behaves in a chemical
    reaction.

8
Lesson 2 Determining Density
  • You will use mass and volume measurements to
    calculate the densities of water, regular shaped
    objects, and irregular shaped objects.

9
Lesson 2
Question
  • How do you calculate mass, volume, and density?
  • What does density measure?

10
Lesson 2
  • If.then.because.

Hypothesis
11
Lesson 2

Procedure
12
Lesson 2

Results
13
  • 2.1 Calculating Mass

14
  • 2.2
  • Comparing the Densities of Different Substances

15
  • 2.3
  • Comparing the Densities of Different Substances

16
Lesson 2 -
Conclusion
  • Density is calculated by dividing the mass by the
    volume measured in grams per cubic centimeter
    (g/cm3).
  • Mass is the amount of matter in an object
    measured in grams. (quantity)
  • Volume is the amount of space taken up by an
    object measured in mL or cm3. (space)
  • Different objects made of the same material will
    have the same density. (characteristic property)
  • Changing the amount of a substance does not
    change the density of the substance.
  • Mass is not affected by shape.
  • Density is a characteristic property of matter.
  • Characteristic property - property that is
    independent of mass, volume, and shape..

17
Lesson 2 -
(1-2)
Vocabulary
  • 16. density - the mass of a known volume of a
    substance measured in g/cm3.
  • 17. weight - a measure of the force of gravity.
  • 18. mass - the amount of matter in an object
    measured in g or kg.
  • 19. gram - a metric unit used to measure mass
  • 20. volume - the amount of space occupied by
    matter measured in L, mL, cm3, or m3.

18
Lesson 2 - (2-2)
Vocabulary
  • 21. solid - a phase or state of matter in which
    a substance has definite shape and volume.
  • 22. characteristic property - an attribute that
    can be used to help identify a substance not
    affected by the mass, volume, or shape of a
    substance refers to substances, not
    objects.

19
Lesson 3 Density Predictions
  • You will predict whether the blocks you
    investigated in Inq. 2.2 will float or sink.
    After finding the density of three liquids, you
    will predict the order in which the liquids will
    layer when you build a density column. You will
    calculate and predict whether objects will float
    or sink in the density column.

20
Lesson 3 -
Question
  • How can you accurately predict if an object will
    float or sink when placed in a liquid?

21
Lesson 3
  • If.. then.. because..

Hypothesis
22
Lesson 3
Procedure
23
Lesson 3
Results
24
  • L3 Results of Floating Sinking Observations

25
  • L3 Calculating Density

26
Lesson 3 -
Conclusion
  • Liquids and solids have density.
  • Density can be used to predict whether an object
    will float or sink.
  • An object or substance floats when its density is
    less than that of the liquid in which it is
    placed.
  • An object or substance sinks when its density is
    more than that of the liquid in which it is
    placed.
  • Some liquids are immiscible (insoluble in one
    another.)

27
Lesson 3 -
Vocabulary
  • 23. immiscible - liquids that are unable to
    dissolve in one another.
  • 24. miscible - liquids that are able to dissolve
    in one another.
  • 25. liquid - a state or phase of matter in which
    a substance has a definite volume but no definite
    shape takes shape of the container it occupies.
  • 26. density - the mass of a known volume of a
  • substance measured in g/cm3 (m/v)
  • 27. floating - matter is less dense than
    substance it is in
  • 28. sinking - matter is more dense than
    substance it is in

28
Lesson 4 Do Gases Have Density
  • You will determine the mass, volume, and density
    of a bottle of air.

29
Lesson 4 -
Question
  • Does air have density?

30
Lesson 4
  • If then.. because ..

Hypothesis
31
Lesson 4
Procedure
32
Lesson 4
Results
33
  • L4 Finding the Density of Air

34
Lesson 4
Conclusion
  • Gases have mass, volume, and density.
  • Air is less dense than liquids and solids

35
Lesson 4 -
Vocabulary
  • 29. vacuum - space without matter.
  • 30. density - the mass of a known volume
  • of a substance usually measured in
  • g/cm3. (m/v)
  • 31. gas - a state or phase of matter in
  • which a substance has no definite
  • shape or volume

36
Lesson 5 Temperature Density
  • You will investigate the effect of temperature on
    the volume of matter by building and calibrating
    a thermometer filled with water. After
    constructing the liquid-filled thermometer, you
    will replace the water with air. You will also
    observe the effect of heat on a bimetal strip

37
Lesson 5
Question
  • What is the relationship between temperature,
    heat, and density?

38
Lesson 5
  • If then. because..

Hypothesis
39
Lesson 5

Procedure
40
Lesson 5

Results
41
  • L5
  • Draw your design for a thermometer.
  • Temperature of cold water bath ______
  • Temperature of hot water bath _______
  • Difference between the two temperatures____
  • Distance between the two marks on tubing___

42
Lesson 5 -
Conclusion
  • Heat is a form of energy that can move from a hot
    place to a cooler place (measured in joules).
  • Temperature is a measure of kinetic energy of
    particles of matter (measured by a thermometer in
    degrees Celsius).
  • Density changes with temperature
  • As temperature increases, density will decrease
    and volume will increase (mass stays the same).
  • expansion
  • As temperature decreases, density will increase
    and volume will decrease (mass stays the same).
  • contraction
  • Gas or liquid-filled thermometers work as the
    result of expansion or contraction.

43
Lesson 5 (1-3)
Vocabulary
  • 32. heat - a form of energy that can move from a
    hot place to a cooler place the transfer of
    energy from one body to another.
  • 33. temperature - a measure of the kinetic energy
    of the particles that make up matter the
    measurement of how hot something is.
  • 34. Celsius - a temperature scale with the
    melting point of ice at 0 degrees and the boiling
    point of water at 100 degrees.

44
Lesson 5
(2-3)
Vocabulary
  • 35. Fahrenheit - a temperature scale with the
    melting point of ice at 32 degrees and the
    boiling point of water at 212 degrees.
  • 36. Kelvin - a temperature scale with the lowest
    possible temperature at the zero point, which is
    called absolute zero ice melts at 273 K.
  • 37. calibrate - set measure to scale
  • 38. density - the mass of a known volume of a
    substance measured in g/cm3.

45
Lesson 5 (3-3)
Vocabulary
  • 39. expansion - the increase in the volume of
    matter that occurs when matter is heated.
  • 40. freeze - the change in state in which a
    liquid turns into a solid.
  • 41. volume - the amount of space occupied by
    matter measured in L, mL, cm3, and m3.

46
Lesson 6 Applying the Heat
  • You will heat pure substances and observe and
    classify changes that occur.

47
Lesson 6
Question
  • How does heat affect solid substances?

48
Lesson 6
  • Ifthen.. because..

Hypothesis
49
Lesson 6

Procedure
50
Lesson 6

Results
51
  • L6 Results - Heating substances

52
Lesson 6
Conclusion
  • Physical and chemical changes result from the
    application of heat.
  • The way a substance behaves when it is heated is
    a characteristic property of that substance.
  • Sublimation, evaporation, and condensation are
    caused when heat energy overcomes the forces that
    hold a solid together or keep a liquid in a fluid
    state.
  • Heating may cause a chemical change, phase
    change, or no change at all.
  • When cooling occurs after heating, changes in
    substances may be reversible or irreversible.
  • If a chemical reaction occurs, new substances
    with different observable properties are formed.
  • Chemical reactions have reactants and
    products..

53
Lesson 6
(1-2)
Vocabulary
  • 42. chemical reaction - a change in which new
    substances are formed has reactants and
    products.
  • 43. reactant - the starting substances in a
    chemical reaction.
  • 44. product - a substance formed by a chemical
    reaction.
  • 45. physical change - reversible through
    physical means and do not involve the formation
    of new substances no change in chemical
    properties.
  • 46. chemical change - not readily reversible and
    do involve the formation of new substances with
    different properties.

54
Lesson 6 (2-2)
Vocabulary
  • 47. sublimation - physical change in which a
    substance goes directly from a solid to a gas and
    then back to a solid.
  • 48. evaporation - the change of a substance from
    a liquid to a gas
  • 49. condensation - the change of state from a gas
    to a liquid..

55
Lesson 7 Just A Phase
  • As ice is heated, you will observe the phase
    changes that occur. You will also observe
    melting and boiling points.

56
Lesson 7
Question
  • How does heat affect phase changes?

57
Lesson 7
  • If then. because.

Hypothesis
Hypothesis
58
Lesson 7
Procedure
59
Lesson 7

Results
60
  • L 7.1

61
Lesson 7
Conclusion
  • Phase changes are dependent on temperature and
    pressure.
  • Three phases or states of matter solid, liquid,
    gas
  • Phase changes take place when molecules lose or
    gain kinetic energy (heat energy) and can be
    related to a change in temperature.
  • Lose kinetic energy molecules move
  • closer (gas gt liquid gt
    solid).
  • Gain kinetic energy molecules move
  • apart (solid gt liquid gt gas)
  • A change of state is not the result of a chemical
    reaction.

62
Lesson 7 -
Conclusion
  • The melting point and boiling point of a
    substance is a characteristic property of the
    substance.
  • Freezing and melting points are the same.
  • An increased input of heat has no effect on the
    boiling point of a substance, although it will
    make a fixed mass of matter change state faster.
  • Substances that boil are not always hot. Many
    substances melt and boil below 0 degrees C...

63
Lesson 7
(1-2)
Vocabulary
  • 50. solid - a phase or state of matter in
    which a substance has definite shape and volume
    particles are closely packed.
  • 51. liquid - a state of phase of matter in
    which a substance has a definite volume but no
    definite shape takes the shape of the container.
  • 52. gas - a state or phase of matter in which
    a substance has no definite shape or volume
    particles have more kinetic energy than particles
    in liquid and solid.
  • melting - the phase change in which a solid turns
    into a liquid.
  • 54 . melting point - the temperature at which a
    solid turns into a liquid the same temperature
    as freezing point altered by changes in
    pressure.

64
Lesson 7 (2-2)
Vocabulary
  • 55. freezing - the change in state in which a
    liquid turns into a solid.
  • 56. boiling - the process by which a liquid
    changes into a gas at its boiling point.
  • 57 boiling point - the temperature at which a
    liquid changes into a gas boiling point depends
    on air pressure.
  • 58. evaporate - to change from a liquid to a
    gas at the surface of a liquid at or below the
    boiling point.
  • 59. condense - changing from a gas to a liquid

65
Lesson 8 Changing Matter and Mass
  • You will determine what happens to the mass of
    ice when it melts and water when it freezes.

66
Lesson 8 -
Question
  • What happens to the mass of water when it changes
    from a solid to a liquid and a liquid to a solid?

67
Lesson 8
  • If..then.because..

Hypothesis
68
Lesson 8

Procedure
69
Lesson 8
Results
70
  • 8.1 Determining a Change in Mass

71
  • L8 Determing a Change in Mass

72
Lesson 8 -
Conclusion
  • Mass is conserved during phase changes

73
Lesson 8 -
Vocabulary
  • 60. law of conservation of mass - mass is neither
    created or destroyed the total mass of all
    substances remains the same regardless of any
    changes in phase or chemical reactions that
    occur.
  • 61. evaporate - to change from a liquid to a
    gas at or below the boiling point
  • 62. freeze - the change in state in which a
    liquid turns into a solid.
  • 63. mass - the amount of matter in an object
    measured in g or kg.
  • 64. phase - solids, liquids, and gases are three
    phases or states of matter.

74
Lesson 9 The Mystery Object
  • You will conduct an investigation to determine
    the substance that makes up a mystery object.

75
Lesson 9
Question
  • How can density be used to identify an unknown
    substance?

76
Lesson 9
Conclusion
  • Density can be used to determine the properties
    of pure substances

77
Lesson 9
Vocabulary
  • 65. characteristic property - an attribute that
    can be used to help identify a substance
    not affected by the amount or shape of a
    substance.
  • 66. composite - a material made from two or more
  • substances
  • 67. material - the substance from which something
  • is made
  • 68. density - the mass of a known volume of a
    substance measured in g/cm3.

78
Lesson 10 Starting the Anchor Activity
  • You will select an object and describe the
    following about the object
  • function
  • history
  • materials of which it is composed
  • origin of one of the materials

79
Lesson 10
Question
  • What substances were used to compose your object
    and why were these substances chosen?

80
Lesson 10
Conclusion
  • Raw materials must be processed before being used
    in the manufacturing process.
  • A variety of materials are used in the
    manufacturing of objects..

81
Lesson 10
Vocabulary
  • 69. composite - a material made from two
  • or more substances

82
Lesson 11 Pure Substance or Mixture
  • You will examine eight different substances to
    determine if they are pure substances or mixtures.

83
Lesson 11
Question
  • How can you determine the difference between pure
    substances and mixtures?

84
Lesson 11
  • If..thenbecause.

Hypothesis
85
Lesson 11
Procedure
86
Lesson 11
Results
87
  • L11 Identifying Pure Substances or Mixtures

88
Lesson 11
Conclusion
  • A pure substance has definite physical and
    chemical properties.
  • A mixture is made of two or more substances with
    each substance keeping its own properties.
  • Solutions are mixtures.
  • Compounds are not mixtures..

89
Lesson 11 (1-2)
Vocabulary
  • 70. pure substance - matter that has definite
    chemical and physical properties either an
    element or a compound
  • 71. mixture - two or more elements or compounds
    that are mixed together but are not chemically
    combined differ in physical and chemical
    properties.
  • 72. heterogeneous - different (poorly mixed)
  • 73. homogeneous - same (well-mixed)
  • 74. solution - a homogeneous mixture of a solvent
    and a solute

90
Lesson 11 (2-2)
Vocabulary
  • 75. characteristic property - an attribute that
    can be used to help identify a
  • substance not affected by the amount
  • or shape of a substance
  • 76. material - the substance from which
  • something is made
  • 77. composite - a material made from two
  • or more substances.

91
Lesson 12 What Happens When Substances are
Mixed with Water?
  • You will mix several pure substances with water
    and observe what happens.

92
Lesson 12 -
Question
  • What property of matter determines what type of
    mixture a pure substance will form when mixed
    with water?

93
Lesson 12
  • If.then.because.

Hypothesis
94
Lesson 12
Procedure
95
Lesson 12
Results
96
  • L 12 What Happens to a Solid?

97
Lesson 12
Conclusion
  • Solubility is a characteristic property of
    matter.
  • Solutions consist of a solvent and a solute.
  • A solvent is the substance present in the larger
    proportion in a solution.
  • A solute is the substance present in the smaller
    proportion.
  • The components of a solution can be solids,
    liquids, or gases.
  • When a solid is passed into solution, it is said
    to dissolve..

98
Lesson 12 - (1-3)
Vocabulary
  • 78. soluble - substances that will dissolve
  • 79. insoluble - substances that will not dissolve
  • 80. solubility - the amount of solute that will
    dissolve in a solvent at a given temperature and
    pressure the ability of one substance to
    dissolve in another.
  • 81. solvent - the substance that the solute is
    dissolved in the substance present in the
    larger proportion

99
Lesson 12 - (2-3)
Vocabulary
  • 82. solute - the substance that dissolves in a
    solvent the substance in the smaller proportion
    may be solids, liquids, or gases.
  • 83. solution - a mixture of a solvent and a
    solute.
  • 84. aqueous solution - solution in which water is
    the solvent
  • 85. electrolyte - conducts electricity

100
Lesson 12 - (2-3)
Vocabulary
  • 86. mixture - two or more elements or compounds
    that are mixed together but are not chemically
    combined
  • 87. pure substance - either an element or a
    compound has definite chemical and physical
    properties..

101
Lesson 13 How Much Solute Dissolves in a
Solvent?
  • You will make a saturated copper sulfate
    solution. You will also conduct an investigation
    to determine the solubility of two different
    chemicals.

102
Lesson 13
Question
  • Are different substances equally soluble in water?

103
Lesson 13
  • If.then.because.

Hypothesis
104
Lesson 13

Procedure
105
Lesson 13

Results
106
  • L 13 - Determining Solubility

107
Lesson 13
Conclusion
  • Solubility is the amount of a solute that will
    completely dissolve in a given amount of a
    solvent.
  • Solubility is a characteristic property of
    matter.
  • Different substance are not equally soluble in
    water.
  • A saturated solution has the maximum amount of
    solute dissolved in it.
  • When an unsaturated solution of a solid is
    cooled, it may become saturated.
  • Solubility is affected by temperature. Solids
    dissolved in water may increase or decrease in
    solubility with the rise in temperature. Gases
    always decrease in solubility with increased
    temperature.
  • Recrystallization occurs when a solution of a
    solid is cooled and some solid solute
    precipitates out.

108
Lesson 13 (1-2)
Vocabulary
  • 88. solubility - the amount of solute that
    will completely dissolve in a given amount of a
    specific solvent at a given temperature and
    pressure the ability of one substance to
    dissolve in another
  • 89. solute - the substance that dissolves in a
    solvent the substance in the smaller
    proportion.
  • 90. solvent - the substance that the solute is
    dissolved in the substance present in the larger
    proportion.

109
Lesson 13 (2-2)
Vocabulary
  • 91. saturated solution - a solution that has the
    maximum amount of solute dissolved in it at a
    specific temperature and pressure.
  • 92. exothermic - heat is given off (increase in
    solubility with a decrease in temp.)
  • 93. endothermic - heat is taken in (increase in
    solubility with increase in temp.)
  • 94. recrystallization - occurs when an
    unsaturated solution of a solid is cooled and
    becomes saturated and some solid solute
    precipitates out, usually as crystals..

110
Lesson 14 Mass, Volume, and Dissolving
  • You will use equal volumes of water and alcohol
    (you will mass each one separately) and will
    predict what will happen to the mass and volume
    after mixing the two substances.
  • You will also conduct an investigation to
    determine what happens to the mass of salt when
    it is dissolved in water.

111
Lesson 14
Question
  • What happens to the mass and volume of one type
    of matter when it is dissolved in another type of
    matter?
  • Is the volume and mass of a solution different
    from the combined volume and combined mass of the
    two separate substances that make up the
    solution?

112
Lesson 14
  • If..then.because.

Hypothesis
113
Lesson 14
Procedure
114
Lesson 14
Results
115
  • 14.1 Mixing Water and Alcohol

116
  • 14.2 Dissolving a Solid Measuring Mass

117
Lesson 14
Conclusion
  • Water has space between the molecules that allows
    soluble substances to occupy that space.
  • The combined volume of a separate solvent and a
    solute is greater than that of the solution they
    form.
  • Mass, not volume, is conserved during dissolving.

118
Lesson 14
Vocabulary
  • 95. solubility - the ability of one substance
    to dissolve in another at a given temperature and
    pressure.
  • 96. volume - the amount of space occupied by
    matter.
  • 97. mass - the amount of matter in an object.
  • 98. solid - state of matter in which a
    substance has definite shape and volume......

119
Lesson 15 -Separating a Soluble and an Insoluble
Substance
  • You will focus on two separation techniques that
    relate to solubility filtration evaporation.
  • You will use a filter to determine which
    substances will pass through.
  • You will also conduct an investigation to
    separate the soluble from the insoluble parts of
    rock salt.

120
Lesson 15 -
Question
  • How can you separate soluble and insoluble
    components of a mixture?

121
Lesson 15
  • If..then.because..

Hypothesis
122
Lesson 15
Procedure
123
Lesson 15
Results
124
  • 15.1 Filtering a Solution

125
Lesson 15 -
Conclusion
  • Filtration can be used to show that insoluble
    substances will not pass through a filter.
  • Solutions (the solvent and the solvent) will pass
    through a filter.
  • Evaporation can be used to recover a solid from a
    solution.
  • The rate of evaporation could be increased by
    heating, increasing the surface area, or
    increasing airflow over the surface of the
    solution. Dissolving the solute in the least
    amount of solvent greatly reduces evaporation
    time.

126
Lesson 15 - (1-2)
Vocabulary
  • 99. filtration - the process of separating a
    solid and a liquid by passing a mixture of the
    two through a mesh or filter paper.
  • 100. evaporation - change from liquid to a gas
    at or below the boiling point.
  • 101. characteristic property - an attribute
    that can be used to help identify a substance
    not affected by the amount of shape of a
    substance.

127
Lesson 15 - (2-2)
Vocabulary
  • 102. liquid - state of matter in which a
    substance has a definite volume but no definite
    shape takes shape of container.
  • 103. sedimentation - the process by which a
    solid settles out from a solid/liquid mixture.
  • 104. solution - a homogeneous mixture of a
    solvent and solute.

128
Lesson 16 -Researching Solvents
  • You will conduct an investigation to show how
    solvents can remove stains.

129
Lesson 16 -
Question
  • How effective are various solvents at removing
    stains from different sources?

130
Lesson 16
  • If.then.because.

Hypothesis
131
Lesson 16
Procedure
132
Lesson 16

Results
133
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134
Lesson 16 -
Conclusion
  • Water and other liquids can act as solvents.
  • Solubility depends on the nature of the solute
    and the solvent.

135
Lesson 16 -
Vocabulary
  • 105. solvent - the substance that the solute
    is dissolved in the substance present in the
    larger proportion.

136
Lesson 17 - Separating Solutes
  • You will use paper chromatography to separate
    solutes and to compare the dyes found in
    different colored inks.

137
  • Complete Inquiry 17.1. Draw your results.

138
Lesson 17 -
Question
  • What does the separation technique of paper
    chromatography indicate about an ink solution?

139
Lesson 17
  • Ifthenbecause.

Hypothesis
140
Lesson 17
Procedure
141
Lesson 17
Results
142
  • Use Student Sheet 17.1, 17.2, and 17.3.

143
Lesson 17 - (1-2)
Conclusion
  • Ink is made up of several dyes of different
    colors that are dissolved in water.
  • Chromatography is a technique used to analyze
    solutions.
  • Solutes in the ink must be soluble in the solvent
    and contained in the beaker for the chromatogram
    to be produced.
  • Different solutes move through paper at different
    speeds. As the solution moves up the paper, the
    various components of the solution separate out
    and occupy distinct areas on the paper.

144
Lesson 17 - (2-2)
Conclusion
  • Less soluble dyes move slower that more soluble
    dyes. The faster moving, more soluble dyes will
    eventually separate.
  • The characteristic properties of each solute
    determine the way in which that solute separated
    from a mixture of solutes in a solution.
  • Chromatography does not separate colors it
    separates solutes.
  • Chromatography is often used to separate
    colorless substances.

145
Lesson 17 - (1-2)
Vocabulary
  • 106. chromatography - a process used to separate
    different solutes from a solution by passing them
    through a medium.
  • 107. adsorption - a thin layer of molecules
    from a substance attaches to the surface of a
    solid.
  • 108. absorption - one substance penetrates into
    the inner structure of another.

146
Lesson 17 - (2-2)
Vocabulary
  • 109. sorption - the process of being taken up
    and held by either absorption or adsorption.
  • 110. desorption - the reverse of sorption
  • 111. solute - the substance that dissolves in
    a solvent.

147
Lesson 18 - Changing Mixtures
  • You will investigate how adding salt affects the
    melting and boiling points of water.
  • You will also investigate the melting points of
    three different tin alloys.

148
Lesson 18 -
Question
  • How do the properties of a mixture differ from
    the properties of the individual components of
    the mixture?
  • Does adding salt change the melting point and
    boiling point of water?
  • Do all metal alloys have the same melting point?

149
Lesson 18

Hypothesis
150
Lesson 18

Procedure
151
Lesson 18

Results
152
  • Use Student Sheet 18.1, 18.2, and 18.3.

153
Lesson 18 -
Conclusion
  • The properties of a mixture can be very different
    from the properties of the individual components
    that make up the mixture.
  • Adding salt to ice lowers the melting point. The
    change in the melting point of a solvent is
    directly proportional to the amount of solute in
    the mixture.
  • The boiling point of water rises when salt is
    added to water because solute particles interfere
    with the evaporation of a solvent.
  • An alloy is a mixture that contains at least one
    metal.

154
Lesson 18 -
(1-3)
Vocabulary
  • 112. alloy - solutions of solid metals
  • 113. solder - used to join together metal
    materials
  • 114. boiling point - temp. at which a liquid
    turns into a gas depends on air pressure
  • 115. freezing point - temp. at which liquid
    turns to a solid.
  • 116. melting point - temp. at which a solid
    turns into a liquid same temp. as freezing
    point.

155
Lesson 18 - (2-3)
Vocabulary
  • 117. material - substance from which something
    is made
  • 118. metal - group of elements usually hard
    solids have common characteristics - shiny, good
    conductivity, and malleability.
  • 119. mixture - two or more elements or
    compounds that are mixed together but are not
    chemically combined
  • 120. pure substance - either an element of a
    compound

156
Lesson 18 - (3-3)
Vocabulary
  • 121. solubility - the amount of solute that
    will dissolve in a solvent at a given temp. and
    pressure the ability of one substance to
    dissolve in another.
  • 122. solvent - the substance in a solution
    that dissolves the solute the substance present
    in the larger proportion.
  • 123. solute - the substance that dissolves in
    a solvent the substance in the smaller
    proportion
  • 124. temperature - the measurement of how hot
    something is

157
Lesson 19 - Assessing Our Progress
  • You will investigate a variety of mixtures.

158
Lesson 19 -
Question
  • What are the physical properties of substances
    that make up a mixture?

159
Lesson 19

Hypothesis
160
Lesson 19
Procedure
161
Lesson 19
Results
162
Lesson 19 -
Conclusion
  • Physical properties can be used to identify the
    substances that make up a mixture.

163
Lesson 19 -
Vocabulary
  • 125. mixture - two or more elements or
    compounds that are mixed together but are not
    chemically combined.

164
Lesson 20 - Breaking Down a Compound
  • You will use electrolysis to break down water.

165
Lesson 20 -
Question
  • What makes up water?

166
Lesson 20
  • If..then.because..

Hypothesis
167
Lesson 20
Procedure
168
Lesson 20
Results
169
  • Use Student Sheet 20.1.

170
Lesson 20 - (1-2)
Conclusion
  • Water is a compound made of the elements hydrogen
    and oxygen.
  • Elements are pure substances that cannot be
    broken down.
  • Compounds are pure substances made of more than
    one element.
  • Some pure substances are composed of two or more
    pure substances combined.

171
Lesson 20 - (2-2)
Conclusion
  • Compounds of pure substances can be decomposed by
    a chemical reaction.
  • The elements in compounds are combined in fixed
    proportions.

172
Lesson 20 - (1-2)
Vocabulary
  • 126. element - a substance that cannot be broked
    down into other substances by chemical or
    physical means
  • 127. compound - a pure substance consisting of
    two or more elements combined
  • 128. electrolyte - a solution or liquid that
    conducts electricity
  • 129. electrode - rods placed in an electrolyte.

173
Lesson 20 - (2-2)
Vocabulary
  • 130. electrolysis - the process of passing an
    electrical current through a liquid to decompose
    compounds into their constituent elements.
  • 131. liquid - a state of matter in which a
    substance has a definite volume but no definite
    shape take shape of container.
  • 132. pure substance - either an element of a
    compound has definite chemical and physical
    properties.

174
Lesson 21 - Examining and Grouping Elements
  • You will study the characteristics of 25 element
    samples and look at how they are grouped on the
    Periodic Table.

175
Lesson 21 -
Question
  • What properties of elements can be used in
    grouping elements?

176
Lesson 21
  • If..thenbecause..

Hypothesis
177
Lesson 21
Procedure
178
Lesson 21
Results
179
Lesson 21 - Examining and Grouping Elements
  • Use Student Sheet 21.1a.

180
Lesson 21 -
Conclusion
  • Elements are grouped according to similar
    chemical and physical properties.
  • The Periodic Table is used in predicting the
    chemical and physical properties of elements.
  • Each element can be identified by its
    characteristic properties.

181
Lesson 21 - (1-2)
Vocabulary
  • element - a substance that cannot be broken
    down into other substances by chemical or
    physical means.
  • isotope - an atom that has the same number of
    protons as other atoms of the same element do but
    has a different number of neutrons sum of
    neutrons and protons.
  • 135. reactivity - the readiness of a substance
    to react chemically.

182
Lesson 21 - (2-2)
Vocabulary
  • 136. conductivity - able to allow electricity or
    heat to pass through
  • 137. compound - a pure substance consisting of
    two or more elements combined
  • 138. conductor - carries electricity or heat
  • 139. magnetic - a substance that is attracted to
    a magnet.

183
Lesson 22 - Combining Elements
  • You will examine four substances and determine
    how they fit into two groups metals and
    nonmetals.

184
Lesson 22 -
Question
  • What are the two main groups of elements?
  • What happens when elements combine?

185
Lesson 22
  • If.then.because..

Hypothesis
186
Lesson 22
Procedure
187
Lesson 22
Results
188
Lesson 22 - Combining Elements
  • Draw Venn diagram from Student Sheet 22.1.
  • Use Student Sheet 22.2.

189
Lesson 22 -
Conclusion
  • The two major groups of elements are metals and
    nonmetals.
  • Elements combine to form new substances.
  • Compounds are substances formed by a chemical
    reaction between two or more elements.
  • Chemical reactions can be represented by
    equations.

190
Lesson 22 - (1-2)
Vocabulary
  • 140. chemical equation - a representation of a
    chemical reaction that uses symbols to show the
    relationship between the reactants and products.
  • 141. chemical reaction - any change that
    involves the formation of a new substance has
    reactants and products.

191
Lesson 22 - (2-2)
Vocabulary
  • 142. compound - a pure substance consisting of
    two or more elements combined by chemical bonds
  • 143. element - a substance that cannot be
    broken down into other substances by chemical or
    physical means
  • 144. reactant - the starting substances in a
    chemical reaction.
  • 145. product - a substance formed by a
    chemical reaction

192
Lesson 23 - Chemical Reactions
  • You will combine four different metals with
    hydrogen chloride and look for the reactivity of
    the metals. You will also compare the corrosion
    of different metals.

193
Lesson 23 -
Question
  • Why are some elements more reactive than others?

194
Lesson 23
  • If.then..because.

Hypothesis
195
Lesson 23
Procedure
196
Lesson 23
Results
197
  • Use Student Sheet 23.1 and 23.2.

198
Lesson 23 -
Conclusion
  • Some metals are more reactive than others.
  • The reactivity of metals determines how they can
    be used.
  • Metals on the right side of the periodic table
    are less reactive than the other elements.
  • Exothermic reactions give off heat.
  • Corrosion is a chemical reaction that causes the
    disintegration of a substance

199
Lesson 23 -
Vocabulary
  • 146. reactivity - the readiness of a substance
    to react chemically.
  • 147. corrosion - a chemical reaction, usually
    between a metal and the air.
  • 148. chemical reaction - any change that
    involves the formation of a new substance
  • 149. metals - a group of elements that are
    usually hard solids and that have common
    characteristics shiny, good conductivity, and
    malleability.
  • 150. smelting - the process by which a metal is
    extracted from ore usually involves heating the
    ore, usually with a source of carbon

200
Lesson 24 - Countering Corrosion
  • You will compare different substances that
    prevent rusting from occurring.

201
Lesson 24 -
Question
  • What causes rusting and how can it be prevented?

202
Lesson 24
  • If..then.because..

Hypothesis
203
Lesson 24
Procedure
204
Lesson 24
Results
205
  • 24.1

206
Lesson 24 -
Conclusion
  • Rusting occurs when iron is exposed to oxygen.
  • Rusting is a chemical reaction with reactants and
    products.

207
Lesson 24 -
Vocabulary
  • 151. metals - a group of elements that are
    usually hard solids and that have common
    characteristics shiny, good conductivity, and
    malleability.
  • 152. corrosion - a chemical reaction, usually
    between a metal and the air (ex. - rusting)
  • 153. density - the mass of a known volume of a
    subtance measured in g/cm3. (m/v)

208
Lesson 25 - Mass and Chemical Reactions
  • You will place an effervescent tablet in water in
    an open container and in a closed container. You
    will measure the mass before and after adding the
    tablet to see if the law of conservation of mass
    can be applied to chemical reactions.

209
Lesson 25 -
Question
  • What happens to the mass of matter in a chemical
    reaction when one of the products is a gas?

210
Lesson 25
  • If.then..because..

Hypothesis
211
Lesson 25
Procedure
212
Lesson 25
Results
213
  • Use Student Sheet 25.1.

214
Lesson 25 -
Conclusion
  • In a chemical reaction, the mass of the reactants
    and the mass of the products is the same.
  • The conservation of mass is demonstrated in a
    closed system.

215
Lesson 25 -
Vocabulary
  • 154. burning - a rapid chemical reaction between
    a substance and a gas that produces heat and
    light most burning takes place in the air and
    has oxygen as one of its reactants.
  • 155. chemical reaction - any change that
    involves the formation of a new substance has
    reactants and products.
  • 156. mass - the amount of matter in an object
  • 157. phase - solids, liquids, and gases are
    the three phases or states of matter
  • 158. product - a substance formed by a
    chemical reaction.
  • 159. reactant - the starting substances in a
    chemical reaction.
  • 160. solid - a phase or state of matter in
    which a substance has definite shape and volume.

216
Lesson 26
End of Module Assessment
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