properties of matter andrew jackson duran junior high

Properties of Matter

Andrew Jackson

Duran Junior High

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.

Lesson 1 –Our Ideas About Matter

What is matter?

Lesson 1 –

Lesson 1 – • 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)………….

Lesson 1 – (1-3)

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.

Lesson 1 - (2-3)

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.

Lesson 1 – (3-3)

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…………………….

Lesson 2 – Determining Density

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

• How do you calculate mass, volume, and density?

• What does density measure?

Lesson 2 –

Lesson 2

If….then….because….

Lesson 2

2.1 Calculating Mass

Volume of

Water (cm3)

Mass of

Graduated

Cylinder (g)

Mass of Graduated Cylinder

and Water (g)

Mass of

1 cm3 of water

(density in g/cm3)

25

50

2.2 Comparing the Densities of Different SubstancesSubstance Length (l)

(cm)

Width (w)

(cm)

Height (h)

(cm)

Volume (v)

(cm3)

(v=l x w x h)

Mass

(m)

(g)

Mass of

1 cm3

(density in

g/cm3)

(m/v)

2.3

Comparing the Densities of Different SubstancesObject/

substance

Mass

(g)

Volume of water

without object (mL)

Volume of water and

object (mL)

Volume of object (mL)

Density

(g/cm3)

Lesson 2 - • 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………………..

Lesson 2 - (1-2)

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.

Lesson 2 - (2-2)

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………………….

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.

How can you accurately predict if an object will float or sink when placed in a liquid?

Lesson 3 -

Lesson 3

If…….. then….. because……..

Lesson 3

L3 Results of Floating & Sinking Observations

Substance Density (g/cm3)

Floats or sinks?Prediction Results

wax block

white plastic block

transparent plastic block

aluminum block

steel screw

copper cylinder

nylon spacer

water

L3 Calculating Density

Liquid Volume

(cm3)

Mass

(g)

Calculation Density

(g/cm3)

Vegetable oil

Corn syrup

Water

Lesson 3 -

• 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.)……………………

Lesson 3 - 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 in28. sinking - matter is more dense than

substance it is in

Lesson 4 – Do Gases Have Density

You will determine the mass, volume, and density of a bottle of air.

Lesson 4 -

Does air have density?

Lesson 4

If …… then….. because …..

Lesson 4

L4 Finding the Density of Air

Volume of bottle

Mass of bottle,

washer, & rubber valve

(g)

Mass of bottle,

washer, & rubber

valve after removing

air (g)

Mass of air

(g)

Density of air

(m/v)

(g/cm3)

Lesson 4 –

Gases have mass, volume, and density.

Air is less dense than liquids and solids……………

Lesson 4 -

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……………

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

What is the relationship between temperature, heat, and density?

Lesson 5 –

Lesson 5

If…… then…. because…..

Lesson 5

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___

Lesson 5 - • 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………….

Lesson 5 – (1-3)

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.

Lesson 5 – (2-3)

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.

Lesson 5 – (3-3)

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…….

Lesson 6 – Applying the Heat

You will heat pure substances and observe and classify changes that occur.

Lesson 6 –

How does heat affect solid substances?

Lesson 6

If……then….. because…..

Lesson 6

L6 Results - Heating substances

Substance Appearance before heating

Changes observed

during heating

Appearance after cooling

Potassium permanganate

Ammonium chloride

Copper (II) sulfate

Sodium chloride

Zinc oxide

Sulfur

Copper carbonate

Lesson 6 – • 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………..

Lesson 6 – (1-2)

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.

Lesson 6 – (2-2)

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……………..

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.

Lesson 7 –

How does heat affect phase changes?

Lesson 7

If…… then…. because….

Lesson 7

L 7.1Time

(min. and s)

Temperature of water (C degrees)

Observations

0

30 s

1 min

1 min, 30 sec

2 min

2 min, 30 sec

3 min

3 min, 30 sec

4 min

4 min, 30 sec

Lesson 7 – • 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 > liquid > solid).

• Gain kinetic energy – molecules move apart – (solid > liquid > gas)• A change of state is not the result of a

chemical reaction.

Lesson 7 - 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…...

Lesson 7 – (1-2)

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.

53. 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.

Lesson 7 – (2-2)

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……

Lesson 8 –Changing Matter and Mass

You will determine what happens to the mass of ice when it melts and water when it freezes.

Lesson 8 -

What happens to the mass of water when it changes from a solid to a liquid and a liquid to a solid?

Lesson 8

If…..then….because…..

Lesson 8

8.1 Determining a Change in MassGroup # Mass of Ice and

BottleMass of Water and

BottleChange in Mass

( + or -)

L8 Determing a Change in Mass

Group Mass of Bottle and Water

Mass of Bottle and Ice

Change in Mass

(+ or -)

Lesson 8 -

• Mass is conserved during phase changes………

Lesson 8 - 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……….

Lesson 9 – The Mystery Object

You will conduct an investigation to determine the substance that makes up a “mystery” object.

Lesson 9 –

How can density be used to identify an unknown substance?

Lesson 9 –

Density can be used to determine the properties of pure substances……

Lesson 9 –

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 substances67. material - the substance from which

something is made 68. **density - the mass of a known volume of a

substance; measured in g/cm3…….

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

Lesson 10 –

What substances were used to compose your object and why were these substances chosen?

Lesson 10 –

• Raw materials must be processed before being used in the manufacturing process.

• A variety of materials are used in the manufacturing of objects……..

Lesson 10 –

69. **composite - a material made from two

or more substances……

Lesson 11 – Pure Substance or Mixture

You will examine eight different substances to determine if they are pure substances or mixtures.

Lesson 11 –

How can you determine the difference between pure substances and mixtures?

Lesson 11

If…..then…because….

Lesson 11

L11 Identifying Pure Substances or MixturesSample Pure

Substance or Mixture?

How did you reach your conclusion?

A

B

C

D

E

F

G

H

Lesson 11 –

• 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…..

Lesson 11 – (1-2)

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

Lesson 11 – (2-2)

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……….

Lesson 12 – What Happens When Substances

are Mixed with Water?

You will mix several pure substances with water and observe what happens.

Lesson 12 -

What property of matter determines what type of mixture a pure substance will form when mixed with water?

Lesson 12


L 12 What Happens to a Solid?

Name of Substance added to water

Appearance after being shaken 10 times

Does it dissolve?

(Yes or No)

Lesson 12 – • 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…………..

Lesson 12 - (1-3)

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

Lesson 12 - (2-3)

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

Lesson 12 - (2-3)

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……..

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.

Lesson 13 –

Are different substances equally soluble in water?

Lesson 13


L 13 - Determining SolubilityVolume of water (mL)

Substance Initial mass of jar & substance (g)

Final mass of jar & substance (g)

Amount of substance in

saturated solution (g)

10 Sodium chloride

10 Sodium nitrate

Lesson 13 – • 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.

Lesson 13 – (1-2)

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.

Lesson 13 – (2-2)

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………..

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.

Lesson 14 –

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?

Lesson 14

If…..then….because….

Lesson 14

14.1 Mixing Water and Alcohol

Liquid Volume of liquids (mL)

Initial mass of liquids and cylinders

Water 50.0

Alcohol 50.0

Predicted measurements

(water and alcohol)

Actual measurements

(water and alcohol)

Differences

14.2 Dissolving a Solid & Measuring Mass

Initial mass of test tubes,

beaker, salt and water (g)

Final mass of test tubes, beaker, and

dissolved salt solution (g)

Difference/ change in mass (g)

Lesson 14 –

• 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.

Lesson 14 –

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......

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.

Lesson 15 -

How can you separate soluble and insoluble components of a mixture?

Lesson 15


15.1 Filtering a Solution

Mixture Prediction Result

Copper (II) sulfate and

water

Zinc oxide and water

Lesson 15 - • 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.

Lesson 15 - (1-2)

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.

Lesson 15 - (2-2)

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.

Lesson 16 -Researching Solvents

You will conduct an investigation to show how solvents can remove stains.

Lesson 16 -

How effective are various solvents at removing stains from different sources?

Lesson 16


Stain Solvent results

Water Isopropyl alcohol

Kerosene

Ketchup

Chocolate syrup

Vegetable oil

Marker pen ink

Ballpoint pen ink

Lesson 16 -

• Water and other liquids can act as solvents.

• Solubility depends on the nature of the solute and the solvent.

Lesson 16 -

105. **solvent - the substance that the solute is dissolved in; the substance present in the larger proportion.

Lesson 17 - Separating Solutes

You will use paper chromatography to separate solutes and to compare the dyes found in different colored inks.

Complete Inquiry 17.1. Draw your results.

Lesson 17 -

What does the separation technique of paper chromatography indicate about an ink solution?

Lesson 17

If…then…because….

Lesson 17

Use Student Sheet 17.1, 17.2, and 17.3.

Lesson 17 - (1-2)

• 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.

Lesson 17 - (2-2)

• 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.

Lesson 17 - (1-2)

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.

Lesson 17 - (2-2)

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.

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.

Lesson 18 -

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?

Lesson 18

Use Student Sheet 18.1, 18.2, and 18.3.

Lesson 18 - • 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.

Lesson 18 - (1-3)

112. alloy - solutions of solid metals113. solder - used to join together metal

materials114. ** 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.

Lesson 18 - (2-3)

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

Lesson 18 - (3-3)

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

Lesson 19 - Assessing Our Progress

You will investigate a variety of mixtures.

Lesson 19 -

What are the physical properties of substances that make up a mixture?

Lesson 19

Lesson 19 -

• Physical properties can be used to identify the substances that make up a mixture.

Lesson 19 -

125. ** mixture - two or more elements or compounds that are mixed together but are not chemically combined.

Lesson 20 - Breaking Down a Compound

You will use electrolysis to break down water.

Lesson 20 -

What makes up water?

Lesson 20


Use Student Sheet 20.1.

• 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.

Lesson 20 - (1-2)

Lesson 20 - (2-2)

• Compounds of pure substances can be decomposed by a chemical reaction.

• The elements in compounds are combined in fixed proportions…….

Lesson 20 - (1-2)

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.

Lesson 20 - (2-2)

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.

Lesson 21 - Examining and Grouping ElementsYou will study the characteristics of 25

element samples and look at how they are grouped on the Periodic Table.

Lesson 21 -

What properties of elements can be used in grouping elements?

Lesson 21

If…..then……because…..

Lesson 21

Lesson 21 - Examining and Grouping ElementsUse Student Sheet 21.1a.

Lesson 21 -

• 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.

Lesson 21 - (1-2)

133.**element - a substance that cannot be broken down into other substances by chemical or physical means.

134. 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.

Lesson 21 - (2-2)

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.

Lesson 22 - Combining Elements

You will examine four substances and determine how they fit into two groups: metals and nonmetals.

Lesson 22 -

What are the two main groups of elements?

What happens when elements combine?

Lesson 22

If….then….because…..

Lesson 22

Lesson 22 - Combining Elements

Draw Venn diagram from Student Sheet 22.1.


Lesson 22 -

• 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.

Lesson 22 - (1-2)

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.

Lesson 22 - (2-2)

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

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.

Lesson 23 -

Why are some elements more reactive than others?

Lesson 23

If…….then…..because….

Lesson 23

Use Student Sheet 23.1 and 23.2.

Lesson 23 -

• 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……

Lesson 23 - 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 substance149. **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……

Lesson 24 - Countering Corrosion

You will compare different substances that prevent rusting from occurring.

Lesson 24 -

What causes rusting and how can it be prevented?

Lesson 24


24.1

Treatment Appearance of Nail

No treatment

Paint

Galvanizing

Petroleum jelly

Magnesium wrapped

Stainless steel nail

Lesson 24 -

• Rusting occurs when iron is exposed to oxygen.

• Rusting is a chemical reaction with reactants and products.

Lesson 24 -

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)

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.

Lesson 25 -

What happens to the mass of matter in a chemical reaction when one of the products is a gas?

Lesson 25

If….then…..because…..

Lesson 25

Lesson 25 -

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.

Lesson 25 - 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 object157. **phase - solids, liquids, and gases are the three

phases or states of matter158. **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.

Lesson 26

properties of matter andrew jackson duran junior high

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