table of contents objectives - vale middle...

The Properties of Matter

Section 1 What Is Matter?

Section 2 Physical Properties

Section 3 Chemical Properties

Chapter 2

Table of Contents

Section 1 What Is Matter?Chapter 2

• 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.

Objectives


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?

• Is Light 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.

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.

Chapter 2 Section 2 Physical PropertiesChapter 2

• 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.

Objectives

Section 2 Physical PropertiesChapter 2

Physical Propertiesphysical properties can be observed or

measured without changing the matter’s identity.Examples:

•Color•shape•mass•density•odor•melting point•boiling point•Solubility


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.

FYISection 2 Physical PropertiesChapter 2

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 thedensity of a substance can alsotell you what kind ofsubstance it is.

FYI


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:

D = m/V

FYISection 2 Physical PropertiesChapter 2

Physical Properties, continued• Using Density to Identify Substances Look at

the table below to compare densities of several common substances.

FYI


Physical Changes Do Not Form New Substances• Dissolving salt in water, cutting grass, melting

ice are all physical changes

Chapter 2 Section 3 Chemical Properties

Section 3 Chemical PropertiesChapter 2

• Describe two examples of chemical properties.

• Explain what happens during a chemical change.

• Distinguish between physical and chemical changes.

Objectives

Section 3 Chemical PropertiesChapter 2Chemical PropertiesChemical property—How a substance can react

with another substance to make a new substance


Comparing Physical and Chemical Properties

Click below to watch the Visual Concept.

You may stop the video at any time by pressing the Esc key.

Visual Concept

Section 3 Chemical PropertiesChapter 2• 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

• The substance can not be recovered by physical means



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.

FYI




Comparing Physical and Chemical Changes

Visual Concept

The Properties of Matter

Concept MapUse the terms below to complete the concept map on the next slide.

Chapter 2

milliliterscubic centimetersweightgravity

mattermassmotionvolume

The Properties of MatterChapter 2

The Properties of MatterChapter 2

End of Chapter 2 Show

Chapter 3 States of Matter

Section 1 Three States of Matter

Section 2 Behavior of Gases

Section 3 Changes of State

Table of Contents


Objectives

• Describe the properties shared by particles of all matter.

• Describe three states of matter.

• Explain the differences between the states of matter.

Chapter 3


Particles of Matter

• The states 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.

Chapter 3 States of MatterSolids—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 MatterSection 1 Three States of MatterChapter 3


Solids, continued

• 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.

Chapter 3

FYI


Liquids, continued

• 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.

Chapter 3

FYI


Gases

• 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.

Chapter 3

FYI


Bellringer

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.

Chapter 3


Objectives

• 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.

Chapter 3 Changing states of matter involves energy, but does not change the makeup of the matter


Energy and Changes of State

• A change 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.

Chapter 3

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.

Chapter 3

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.

Chapter 3

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.

Chapter 3

FYI

Section 3 Changes of StateChapter 3 Section 3 Changes of State

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.

Chapter 3

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.

Chapter 3

FYI


Vaporization and Condensation

Chapter 3



Visual Concept


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.

Chapter 3

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.

Chapter 3

FYI

Section 3 Changes of StateChapter 3 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.

Chapter 3


Objectives

• Describe three factors that affect how gases behave.

• Predict how a change in pressure or temperature will affect the volume of a gas.

Chapter 3 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.

Chapter 3

FYI

Gas LawsBoyle’s LawWhen pressure is applied to a gas, the volume will

decreaseP1V1=P2V2

Charles’s LawAs the temperature of a gas increases, so does its volume

V1T1

V2T2

=

Boyle’s QuestionsIf 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

Charles's Questions

Section 2 Behavior of GasesChapter 3Laws 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


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.

Chapter 3 States of Matter

Use the terms below to complete the concept map on the next slide.

Chapter 3

Concept Map

condensingstates of mattersolid

changes of statemeltingevaporatingliquid

States of MatterChapter 3 Types of MatterThe 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 ElementsChapter 4

Compoundscompound = a pure substance made of 2 or

more elements that are chemically combined.

A particle of a compound is a called a molecule

Water H2O Carbon Dioxide CO2

Table Salt NaCl

A compound has properties that differ from those of the elements that form it.

Mixtures

Mixture is a combination of more than 1 pure substance— not chemically bonded

Orange Juice—Sugar, water, pulpSoda Pop, Dirt, salt water

Section 3 MixturesChapter 4 Heterogeneous mixtures- look different throughout

Homogeneous mixtures- look the same throughout Section 3 Mixtures

Solutions

• A solution 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.

Chapter 4

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.

Chapter 4 Section 3 Mixtures

Solutes, Solvents, and Solutions

Chapter 4



Visual Concept

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.

Chapter 4

Copyright © by Holt, Rinehart and Winston. All rights reserved.

ResourcesChapter menu

Section 3 Mixtures

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.

Chapter 4



Section 3 MixturesChapter 4



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.

Chapter 4






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.

Chapter 4



Section 3 Mixtures

Suspensions

• A suspension 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.

Chapter 4



Section 3 Mixtures

Colloids

• A colloid 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.

Chapter 4

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http://www.augustana.edu/users/Chwanke/CH121/films/pv_reltn.mov

http://video.yahoo.com/video/play?vid=1079192185



http://chemed.chem.purdue.edu/demos/movies/large_movies/4.12.mov

States of MatterChapter 3

End of Chapter 3 Show

Interpreting Graphics

The table below shows the properties of different substances. Use the table below to answer the questions that follow.

Chapter 2 Standardized Test Preparation

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 isgreater than the volume of gold.

B The volume of pyrite isless than the volume of gold.

C The volumes of thesubstances are equal.

D There is not enoughinformation 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 isgreater than the volume of gold.

B The volume of pyrite isless than the volume of gold.

C The volumes of thesubstances are equal.

D There is not enoughinformation 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



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


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

Chapter 3 Standardized Test Preparation Section 1 Three States of MatterChapter 3

Section 2 Behavior of GasesChapter 3 Section 3 Changes of StateChapter 3

Section 3 Changes of StateChapter 3 Section 3 Changes of StateChapter 3

Chapter 3 Standardized Test Preparation Chapter 2 Section 2 Physical Properties

Chapter 2 Section 2 Physical Properties Chapter 2 Section 2 Physical Properties

Chapter 2 Section 2 Physical Properties




The graph below was constructed from data collected during a laboratory investigation. Use the graph below to answer the questions that follow.







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




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




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




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




4. At 20°C, which solid is the most soluble?

F sodium chloride

G sodium chlorate

H potassium bromide

I sodium nitrate


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