Andrew Jackson Duran Junior High

Andrew Jackson Duran Junior High
Properties of Matter Andrew Jackson Duran Junior High

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.

Lesson 1 – Question What is matter?

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)………….

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.

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.

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.

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

Lesson 2 If….then….because…. Hypothesis

Lesson 2 Procedure

Lesson 2 Results

Mass of Graduated Cylinder and Water (g)
2.1 Calculating Mass Volume of Water (cm3) Mass of Graduated Cylinder (g) Mass of Graduated Cylinder and Water (g) 1 cm3 of water (density in g/cm3) 25 50

2.2 Comparing the Densities of Different Substances Substance
Length (l) (cm) Width (w) Height (h) Volume (v) (cm3) (v=l x w x h) Mass (m) (g) Mass of 1 cm3 (density in g/cm3) (m/v)

Volume of water without object (mL) Volume of water and object (mL)
2.3 Comparing the Densities of Different Substances Object/ substance Mass (g) Volume of water without object (mL) Volume of water and object (mL) Volume of object (mL) Density (g/cm3)

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………………..

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.

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.

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

Lesson 3 If…….. then….. because…….. Hypothesis

Lesson 3 Procedure

Lesson 3 Results

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
(g/cm3) Vegetable oil Corn syrup Water

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.)……………………

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

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

Lesson 4 - Question Does air have density?

Lesson 4 If …… then….. because ….. Hypothesis

Lesson 4 Procedure

Lesson 4 Results

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 Density of air (m/v) (g/cm3)

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

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……………

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

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

Lesson 5 If…… then…. because….. Hypothesis

Lesson 5 Procedure

Lesson 5 Results

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 - 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………….

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.

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.

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 – Question How does heat affect solid substances?

Lesson 6 If……then….. because….. Hypothesis

Lesson 6 Procedure

Lesson 6 Results

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 – 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………..

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.

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 – Question How does heat affect phase changes?

Lesson 7 If…… then…. because…. Hypothesis Hypothesis

Lesson 7 Procedure

Lesson 7 Results

Temperature of water (C degrees)
L 7.1 Time (min. and s) Temperature of water (C degrees) Observations 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 – 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 > 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 - 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…...

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.

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 - Question 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….. Hypothesis

Lesson 8 Procedure

Lesson 8 Results

Mass of Water and Bottle
8.1 Determining a Change in Mass Group # Mass of Ice and Bottle Mass of Water and Bottle Change in Mass ( + or -)

Mass of Bottle and Water
L8 Determing a Change in Mass Group Mass of Bottle and Water Mass of Bottle and Ice Change in Mass (+ or -)

Lesson 8 - Conclusion Mass is conserved during phase changes………

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……….

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

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

Lesson 9 – Conclusion Density can be used to determine the properties of pure substances……

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…….

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

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……..

Lesson 10 – Vocabulary 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 – Question How can you determine the difference between pure substances and mixtures?

Lesson 11 If…..then…because…. Hypothesis

Lesson 11 Procedure

Lesson 11 Results

Pure Substance or Mixture? How did you reach your conclusion?
L11 Identifying Pure Substances or Mixtures Sample Pure Substance or Mixture? How did you reach your conclusion? A B C D E F G H

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…..

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

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

Lesson 12 Procedure

Lesson 12 Results

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 – 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…………..

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

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

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 – Question Are different substances equally soluble in water?

Lesson 13 Procedure

Lesson 13 Results

L 13 - Determining Solubility
Volume 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 Sodium nitrate

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.

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.

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 – 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?

Lesson 14 If…..then….because…. Hypothesis

Lesson 14 Procedure

Lesson 14 Results

Initial mass of liquids and cylinders Predicted measurements
14.1 Mixing Water and Alcohol Liquid Volume of liquids (mL) Initial mass of liquids and cylinders Water 50.0 Alcohol Predicted measurements (water and alcohol) Actual measurements 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 – 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.

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......

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

Lesson 15 Procedure

Lesson 15 Results

Copper (II) sulfate and water
15.1 Filtering a Solution Mixture Prediction Result Copper (II) sulfate and water Zinc oxide and water

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.

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.

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

Lesson 16 Procedure

Lesson 16 Results

Stain Solvent results Water Isopropyl alcohol Kerosene Ketchup
Chocolate syrup Vegetable oil Marker pen ink Ballpoint pen ink

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

Lesson 16 - Vocabulary 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 - Question What does the separation technique of paper chromatography indicate about an ink solution?

Lesson 17 If…then…because…. Hypothesis

Lesson 17 Procedure

Lesson 17 Results

Use Student Sheet 17.1, 17.2, and 17.3.

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.

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.

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.

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 - 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?

Lesson 18 Hypothesis

Lesson 18 Procedure

Lesson 18 Results

Use Student Sheet 18.1, 18.2, and 18.3.

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.

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.

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

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

Lesson 19 Hypothesis

Lesson 19 Procedure

Lesson 19 Results

Lesson 19 - Conclusion Physical properties can be used to identify the substances that make up a mixture.

Lesson 19 - Vocabulary 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 - Question What makes up water?

Lesson 20 Procedure

Lesson 20 Results

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.

Compounds of pure substances can be decomposed by a chemical reaction. The elements in compounds are combined in fixed proportions…….

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.

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 Elements
You will study the characteristics of 25 element samples and look at how they are grouped on the Periodic Table.

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

Lesson 21 If…..then……because….. Hypothesis

Lesson 21 Procedure

Lesson 21 Results

Lesson 21 - Examining and Grouping Elements
Use Student Sheet 21.1a.

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.

**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.

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 - Question What are the two main groups of elements?
What happens when elements combine?

Lesson 22 If….then….because….. Hypothesis

Lesson 22 Procedure

Lesson 22 Results

Lesson 22 - Combining Elements
Draw Venn diagram from Student Sheet 22.1. Use Student Sheet 22.2.

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.

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.

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 - Question Why are some elements more reactive than others?

Lesson 23 If…….then…..because…. Hypothesis

Lesson 23 Procedure

Lesson 23 Results

Use Student Sheet 23.1 and 23.2.

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……

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……

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

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

Lesson 24 Procedure

Lesson 24 Results

24.1 Treatment Appearance of Nail No treatment Paint Galvanizing
Petroleum jelly Magnesium wrapped Stainless steel nail

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

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)

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

Lesson 25 If….then…..because….. Hypothesis

Lesson 25 Procedure

Lesson 25 Results

Use Student Sheet 25.1.

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.

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.

End of Module Assessment
Lesson 26 End of Module Assessment

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