The Properties of Matter Section 1 What Is Matter? Table of Contents Section 1 What Is Matter? Section 2 Physical Properties Section 3 Chemical Properties Objectives Describe the two properties of all matter. Identify the units used to measure volume and mass. Compare mass and weight. Explain the relationship between mass and inertia. Section 1 What Is Matter? Section 1 What Is Matter? Matter Matter Matter is anything that has mass and takes up space. Matter is made up of atoms and molecules which are always in motion Is air matter? Inertia What Is Inertia? Inertia is the tendency of an object to resist a change in motion. Mass: The Measure of Inertia An object that has a large mass is harder to move and harder to stop than an object that has less mass. The reason is that the object with the large mass has greater inertia. Is Light matter?
Section 2 Physical Properties Section 2 Physical Properties Bellringer If you were asked to describe an orange to someone who had never seen an orange, what would you tell the person? Write your response in your science journal. Objectives Identify six examples of physical properties of matter. Describe how density is used to identify substances. List six examples of physical changes. Explain what happens to matter during a physical change. Section 2 Physical Properties Physical Properties physical properties can be observed or measured without changing the matter s identity. Examples: Color shape mass density odor melting point boiling point Solubility
FYI Section 2 Physical Properties Physical Properties, continued Identifying Matter You use physical properties to identify matter. Density Density is the amount of matter in a given space, or volume. The two balls below have different densities. FYI Section 2 Physical Properties Physical Properties, continued Liquid Layers The graduated cylinder below contains six liquids. Each liquid is a different density so the liquids form layers. Density of Solids Knowing the density of a substance can also tell you what kind of substance it is. FYI Section 2 Physical Properties Physical Properties, continued Solving for Density To find an objects density (D), first measure its mass (m) and volume (V). Then use the following equation: FYI Section 2 Physical Properties Physical Properties, continued Using Density to Identify Substances Look at the table below to compare densities of several common substances. D = m/v
Section 2 Physical Properties Section 3 Chemical Properties Physical Changes Do Not Form New Substances Dissolving salt in water, cutting grass, melting ice are all physical changes Objectives Section 3 Chemical Properties Describe two examples of chemical properties. Section 3 Chemical Properties Chemical Properties Chemical property How a substance can react with another substance to make a new substance Explain what happens during a chemical change. Distinguish between physical and chemical changes.
Section 3 Chemical Properties Comparing Physical and Chemical Properties Click below to watch the Visual Concept. Visual Concept You may stop the video at any time by pressing the Esc key. Section 3 Chemical Properties Chemical Change a substance changes chemical properties--the identity of the matter changes Signs of Chemical Changes change in color, odor, production of heat, fizzing, and so on. Wood burning, a nail rusting, digesting your food are all chemical changes Section 3 Chemical Properties The substance can not be recovered by physical means
FYI Section 3 Chemical Properties Physical Versus Chemical Changes A Change in Composition Physical changes do not change the composition of a substance while chemical changes do. Reversing Changes Many physical changes are easily reversed, but most chemical changes cannot easily be reversed. Section 3 Chemical Properties Comparing Physical and Chemical Changes Click below to watch the Visual Concept. Visual Concept You may stop the video at any time by pressing the Esc key. The Properties of Matter The Properties of Matter Concept Map Use the terms below to complete the concept map on the next slide. matter mass motion volume milliliters cubic centimeters weight gravity
The Properties of Matter End of Show States of Matter Section 1 Three States of Matter Table of Contents Section 1 Three States of Matter Section 2 Behavior of Gases Objectives Describe the properties shared by particles of all matter. Describe three states of matter. Explain the differences between the states of matter.
Particles of Matter Section 1 Three States of Matter Thestates of matter are the physical forms in which a substance can exist. The three most familiar states of matter are solid, liquid, and gas. Matter is made up of tiny particles called atoms and molecules. These particles are always in motion and are always bumping into one another. States of Matter Solids atoms are rigid and can vibrate Definite shape and volume Liquids atoms can slide around each other but are attached Definite volume, but no definite shape Gas atoms are free from each other No definite shape or volume Plasma-- States of Matter Section 1 Three States of Matter
FYI Solids, continued Section 1 Three States of Matter There Are Two Kinds of Solids Crystalline solids have a very orderly, three-dimensional arrangement of particles. Iron, diamond, and ice are crystalline solids. Amorphous solids are made of particles that do not have a special arrangement. Glass, rubber, and wax are amorphous solids. FYI Liquids, continued Section 1 Three States of Matter Liquids Have Unique Characteristics Two special properties of liquids are surface tension and viscosity. Surface tension is a force that acts on the particles at the surface of a liquid. Viscosity is a liquid s resistance to flow. Section 1 Three States of Matter FYI Gases Bellringer Gas is the state of matter that has no definite shape or volume. The particles of a gas move quickly and can break away completely from one another. The amount of empty space between gas particles can change. Write a description of what must be done to liquid water to change it to ice or to change it to steam. Based on your explanation, predict what must happen to cause matter to change state. Write your answer in your science journal.
Objectives Changing states of matter involves energy, but does not change the makeup of the matter Describe how energy is involved in changes of state. Describe what happens during melting and freezing. Compare evaporation and condensation. Explain what happens during sublimation. Identify the two changes that can happen when a substance loses or gains energy. FYI Energy and Changes of State Achange of state is the change of a substance from one physical form to another. The particles of a substance move differently depending on the state of the substance. The particles also have different amounts of energy when the substance is in different states. FYI Melting: Solid to Liquid Melting is the change of state from a solid to a liquid. The temperature at which a solid changes to a liquid is its melting point. Adding Energy For a solid to melt, particles must overcome their attractions to each other. When a solid is at its melting point, any energy added is used to overcome attractions between particles.
FYI Freezing: Liquid to Solid Freezing is the change of state from a liquid to a solid. The temperature at which a liquid changes to a solid is its freezing point. Removing Energy When a liquid is at its freezing point, removing energy will cause the particles to begin locking into place. FYI Evaporation: Liquid to Gas Evaporation is the change of state from a liquid to a gas. Evaporation can occur at the surface of a liquid that is below its boiling point. Boiling is the change of a liquid to a gas throughout the liquid. The temperature at which a liquid boils is its boiling point. FYI Evaporation: Liquid to Gas, continued Effects of Pressure on Boiling Point The boiling point of a liquid decreases as atmospheric pressure decreases. Atmospheric pressure is caused by the weight of the gases in the atmosphere. Atmospheric pressure is lower at higher elevations. So, the boiling point is lower on top of mountains than it is at sea level.
FYI Condensation: Gas to Liquid Condensation is the change of state from a gas to a liquid. The condensation point of a substance is the temperature at which the gas becomes a liquid. Energy must be removed for condensation to occur. Removing energy slows the movement of gas particles which allows them to clump together. Vaporization and Condensation Click below to watch the Visual Concept. Visual Concept You may stop the video at any time by pressing the Esc key. FYI Sublimation: Solid to Gas Sublimation is the change of state in which a solid changes directly into a gas. For sublimation to occur, the attractions between the particles must be completely overcome. So, the substance must gain energy during sublimation. FYI Change of Temperature Vs. Change of State When most substances lose or gain energy, one of two things happens to the substance: its temperature changes or its state changes. But the temperature of a substance does not change until a change of state is complete. The graph on the next slide shows how temperature changes as energy is added to ice.
Section 2 Behavior of Gases Bellringer What gas is used in a balloon to make it float in the air? Have you ever seen a hot-air balloon floating in the sky? In your science journal, write an explanation of why you think the balloon can fly with only air in it and not helium. Objectives Section 2 Behavior of Gases Describe three factors that affect how gases behave. Predict how a change in pressure or temperature will affect the volume of a gas. FYI Section 2 Behavior of Gases Describing Gas Behavior Temperature Temperature is a measure of how fast the particles in an object are moving.the faster the particles are moving, the more energy they have. Volume Volume is the amount of space that an object takes up. Because gas particles spread out, the volume of any gas depends on the container that the gas is in. Pressure The amount of force exerted on a given area of surface is called pressure. You can think of pressure as the number of times the particles of a gas hit the inside of their container.
Gas Laws Boyle s Law When pressure is applied to a gas, the volume will decrease P 1 V 1 =P 2 V 2 Charles s Law As the temperature of a gas increases, so does its volume V 1 V 2 T 1 = T 2
Boyle s Questions Charles's Questions If a gas has a pressure of 10 kpa and a volume of 50cm3, what will the volume be if the pressure increases to 50 kpa? What if the pressure increases to 75 kpa? What if the pressure increases to 100 kpa? What if the pressure decreases to 25 kpa? Now graph the results Section 2 Behavior of Gases Laws of Conservation The following laws apply to all changes The law of conservation of Energy Energy cannot be created or destroyed The law of conservation of mass Mass cannot be created or destroyed
Section 2 Behavior of Gases States of Matter Gas Behavior Laws Boyle s Law Boyle s law states that for a fixed amount of gas at a constant temperature, the volume of the gas is inversely related to pressure. Charles s Law Charles s law states that for a fixed amount of gas at a constant pressure, the volume of the gas changes in the same way that the temperature of the gas changes. Concept Map Use the terms below to complete the concept map on the next slide. changes of state melting evaporating liquid condensing states of matter solid States of Matter Types of Matter The Atom is the smallest particle of an element that has the properties of the element.
Elements are pure substances that can t be broken down into simpler substances. Section 1 Elements Compounds compound = a pure substance made of 2 or more elements that are chemically combined. A particle of a compound is a called a molecule Water H 2 O Carbon Dioxide CO 2 Table Salt NaCl Mixtures Mixture is a combination of more than 1 pure substance not chemically bonded Orange Juice Sugar, water, pulp Soda Pop, Dirt, salt water A compound has properties that differ from those of the elements that form it.
Section 3 Mixtures Heterogeneous mixtures- look different throughout Homogeneous mixtures- look the same throughout Section 3 Mixtures Solutions Asolution is a mixture that appears to be a single substance. The process in which particles of substances separate and spread evenly throughout a mixture is known as dissolving. In a solution, the solute is the substance that is dissolved. The solvent is the substance in which the solute is dissolved.
Section 3 Mixtures Section 3 Mixtures Solutions, continued Examples of Solutions Liquid solutions include soft drinks, gasoline, and tap water. Solutions may also be gases, such as air. Solutions may also be solids, such as steel. Alloys are solid solutions of metals or nonmetals dissolved in metals. Solutes, Solvents, and Solutions Click below to watch the Visual Concept. Visual Concept You may stop the video at any time by pressing the Esc key. Section 3 Mixtures Section 3 Mixtures Solutions, continued Particles in Solutions The particles in solutions are so small that they never settle out. They also cannot be removed by filtering. The particles in solutions are so small that they don t even scatter light. Concentrations of Solutions A measure of the amount of solute dissolved in a solvent is concentration. Concentrated or Dilute? Solutions can be described as being concentrated or dilute. But these two terms do not tell you the amount of solute that is dissolved. The next slide shows how to calculate concentration. Copyright by Holt, Rinehart and Winston. All rights reserved.
Copyright by Holt, Rinehart and Winston. All rights reserved. Section 3 Mixtures Section 3 Mixtures Concentrations of Solutions, continued Solubility is the ability of a solute to dissolve in a solvent at a certain temperature. The solubility of most solids in water increases with temperature. The graph on the next slide shows this relationship. Copyright by Holt, Rinehart and Winston. All rights reserved. Section 3 Mixtures Section 3 Mixtures Concentrations of Solutions, continued Dissolving Gases in Liquids Gases become less soluble in liquids as the temperature is raised. Dissolving Solids Faster in Liquids Three ways to make a solute dissolve faster are mixing the solution, heating the solution, and crushing the solute into smaller particles. Copyright by Holt, Rinehart and Winston. All rights reserved. Copyright by Holt, Rinehart and Winston. All rights reserved.
Copyright by Holt, Rinehart and Winston. All rights reserved. Section 3 Mixtures Section 3 Mixtures Suspensions Asuspension is a mixture in which particles of a material are dispersed throughout a liquid or a gas but are large enough that they settle out. The particles in a suspension are large enough to scatter or block light. A suspension can be separated by passing it through a filter. Colloids Acolloid is a mixture in which the particles are dispersed throughout but are not heavy enough to settle out. Particles in a colloid are large enough to scatter light. A colloid cannot be separated by passing it through a filter. Copyright by Holt, Rinehart and Winston. All rights reserved. http://highered.mcgraw-hill.com/olc/dl/120073/bio14.swf States of Matter http://www.augustana.edu/users/chwanke/ch121/films/pv_reltn.mov http://video.yahoo.com/video/play?vid=1079192185 http://video.yahoo.com/video/play?vid=1095520662 http://video.yahoo.com/video/play?vid=1081423139 http://chemed.chem.purdue.edu/demos/movies/large_movies/4.12.mov
Interpreting Graphics End of Show The table below shows the properties of different substances. Use the table below to answer the questions that follow. 1. What could you use to tell pyrite (fool s gold) and gold apart? A volume B density C mass D state 1. What could you use to tell pyrite (fool s gold) and gold apart? A volume B density C mass D state
2. What do you think would happen if you placed a nugget of pyrite into a beaker of mercury? F The pyrite would sink. G The pyrite would dissolve. H The mercury and the pyrite would react. I The pyrite would float. 2. What do you think would happen if you placed a nugget of pyrite into a beaker of mercury? F The pyrite would sink. G The pyrite would dissolve. H The mercury and the pyrite would react. I The pyrite would float. 3. If a nugget of pyrite and a nugget of gold each have a mass of 50 g, what can you conclude about the volume of each nugget? A The volume of pyrite is greater than the volume of gold. B The volume of pyrite is less than the volume of gold. C The volumes of the substances are equal. D There is not enough information to determine the answer. 3. If a nugget of pyrite and a nugget of gold each have a mass of 50 g, what can you conclude about the volume of each nugget? A The volume of pyrite is greater than the volume of gold. B The volume of pyrite is less than the volume of gold. C The volumes of the substances are equal. D There is not enough information to determine the answer.
4. Which substance has the lowest density? F helium G pyrite H mercury I gold 4. Which substance has the lowest density? F helium G pyrite H mercury I gold Interpreting Graphics Use the chart below to answer the questions that follow. 1. Phillip wants to purchase antifreeze for his car. Antifreeze is added to the water in a car s radiator to lower the water s freezing point. The temperature in his area never falls below 10 C. Given the information in the chart above, which of the following brands of antifreeze would be the best for Phillip s car? A Ice-B-Gone B Freeze Free C Liqui-Freeze D Auntie Freeze
1. Phillip wants to purchase antifreeze for his car. Antifreeze is added to the water in a car s radiator to lower the water s freezing point. The temperature in his area never falls below 10 C. Given the information in the chart above, which of the following brands of antifreeze would be the best for Phillip s car? A Ice-B-Gone B Freeze Free C Liqui-Freeze D Auntie Freeze 2. Phillip wants to make a bar graph that compares the brands of antifreeze. If he puts the brand name of each antifreeze on the x-axis, what variable belongs on the y-axis? F Freezing point of water G Freezing point of water with antifreeze in it H Freezing point of the antifreeze only I Freezing point of the radiator 2. Phillip wants to make a bar graph that compares the brands of antifreeze. If he puts the brand name of each antifreeze on the x-axis, what variable belongs on the y-axis? F Freezing point of water G Freezing point of water with antifreeze in it H Freezing point of the antifreeze only I Freezing point of the radiator 3. Phillip s cousin lives in an area where it rarely freezes. The record low temperature for winter is 2 C. Which brand should Phillip s cousin purchase? A Ice-B-Gone B Freeze Free C Liqui-Freeze D Auntie Freeze
Section 1 Three States of Matter 3. Phillip s cousin lives in an area where it rarely freezes. The record low temperature for winter is 2 C. Which brand should Phillip s cousin purchase? A Ice-B-Gone B Freeze Free C Liqui-Freeze D Auntie Freeze Section 2 Behavior of Gases
Section 2 Physical Properties
Section 2 Physical Properties Section 2 Physical Properties Section 2 Physical Properties Interpreting Graphics The graph below was constructed from data collected during a laboratory investigation. Use the graph below to answer the questions that follow. Copyright by Holt, Rinehart and Winston. All rights reserved.
Copyright by Holt, Rinehart and Winston. All rights reserved. Section 3 Mixtures 1. Which of the following values is the amount of sodium nitrate that can dissolve in 100 ml of water at 40 C? A 0 g B 40 g C 80 g D 100 g Copyright by Holt, Rinehart and Winston. All rights reserved. 1. Which of the following values is the amount of sodium nitrate that can dissolve in 100 ml of water at 40 C? A 0 g B 40 g C 80 g D 100 g 2. How many grams of sodium chloride can dissolve in 100 ml of water at 60 C? F 40 g G 80 g H 125 g I 160 g Copyright by Holt, Rinehart and Winston. All rights reserved. Copyright by Holt, Rinehart and Winston. All rights reserved.
Copyright by Holt, Rinehart and Winston. All rights reserved. 2. How many grams of sodium chloride can dissolve in 100 ml of water at 60 C? F 40 g G 80 g H 125 g I 160 g 3. At what temperature will 80 g of potassium bromide completely dissolve in 100 ml of water? A approximately 20 C B approximately 42 C C approximately 88 C D approximately 100 C Copyright by Holt, Rinehart and Winston. All rights reserved. 3. At what temperature will 80 g of potassium bromide completely dissolve in 100 ml of water? A approximately 20 C B approximately 42 C C approximately 88 C D approximately 100 C 4. At 20 C, which solid is the most soluble? F sodium chloride G sodium chlorate H potassium bromide I sodium nitrate Copyright by Holt, Rinehart and Winston. All rights reserved. Copyright by Holt, Rinehart and Winston. All rights reserved.
Copyright by Holt, Rinehart and Winston. All rights reserved. 4. At 20 C, which solid is the most soluble? F sodium chloride G sodium chlorate H potassium bromide I sodium nitrate