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To advance through the presentation, click the right-arrow key or the space bar.

From the resources slide, click on any resource to see a presentation for that resource.

From the Chapter menu screen click on any lesson to go directly to that lesson’s presentation.

You may exit the slide show at any time by pressing

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

Resources Chapter menu

Transparencies

Image and Math Focus Bank

Standardized Test Prep

Visual Concepts

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Table of Contents

Section 1 Elements

Section 2 Compounds

Section 3 Mixtures

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

Resources Chapter menu

Refer to Figure 4 in your book for help answering the following questions:

What do gold, iron, and aluminum have in common?

What do oxygen, neon, and sulfur have in common?

How is silicon different from aluminum or oxygen?

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• Describe pure substances.

• Describe the characteristics of elements, and give examples.

• Explain how elements can be identified.

• Classify elements according to their properties.

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

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• An element is a pure substance that cannot be separated into simpler substances by physical or chemical means.

• Only One Type of Particle A substance in which there is only one type of particle is a pure substance.

Elements are made of particles called atoms.

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• Each element can be identified by its unique set of properties. An element may share a property with

another element, but other properties can help you tell the elements apart.

• Identifying Elements by Their Properties

Elements can be identified by using their physical

properties and their chemical properties.

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

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• Categories of Elements Three major categories are:

• Metals are shiny, and they conduct heat energy and electric current.

• Nonmetals conduct heat and electricity poorly.

• Metalloids have properties of both metals and

nonmetals.

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continued

• Categories Are Similar By knowing the category to which an unfamiliar element belongs, you can predict some of its properties.

• The next slide show examples and properties of

metals, nonmetals, and metalloids.

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

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The word compound refers to something that consists of two or more parts. How might you make a compound using elements? What are some compounds that you know?

Write your answer in your science journal.

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

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• Explain how elements make up compounds.

• Describe the properties of compounds.

• Explain how a compound can be broken down into its elements.

• Give examples of common compounds.

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Compounds: Made of Elements

• A compound is a pure substance composed of two or more elements that are chemically combined.

Elements combine by reacting with one another.

A particle of a compound is a called a molecule.

Molecules of compounds are formed when atoms of

two or more elements join together.

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

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• The Ratio of Elements in a Compound Elements join in a specific ratio according to their masses to form a compound.

• For example, every sample of water has a 1:8 mass

ratio of hydrogen and oxygen.

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• Each compound can be identified by its physical and chemical properties.

• Properties: Compounds Versus Elements A

compound has properties that differ from those of the

elements that form it.

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

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• Compounds can be broken down into their elements or into simpler compounds by chemical changes.

• Methods of Breaking Down Compounds

Sometimes, energy is needed for a chemical change

to happen. Two ways to add energy are to apply heat

and to apply an electric current.

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• Compounds in Nature Some compounds found in nature are proteins, carbon dioxide, and

carbohydrates.

• Compounds in Industry Some compounds must be broken down for use in industry. Other compounds, are made in industry for use as medicines, food

preservatives, and synthetic fabrics.

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

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Bellringer

When you add sugar to coffee, tea, iced tea, or

lemonade, the sugar disappears. What do you think happens to the sugar?

Write your answer in your science journal.

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• Describe three properties of mixtures.

• Describe four methods of separating the parts of a mixture.

• Analyze a solution in terms of its solute

and solvent.

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

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Objectives, continued

• Explain how concentration affects a solution.

• Describe the particles in a suspension.

• Explain how a colloid differs from a solution and

a suspension.

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Properties of Mixtures

• A mixture is a combination of two or more substances that are not chemically combined.

• No Chemical Changes in a Mixture No chemical

changes happen when a mixture is made. So, each

substance has the same chemical makeup it had

before the mixture was formed.

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

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• Separating Mixtures Through Physical Methods Mixtures can be separated by using physical changes.

Physical changes do not change the identities of the substances.

• The next slide shows some common ways to

separate mixtures by using physical changes.

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

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• The Ratio of Components in a Mixture The

components of a mixture do not need to be mixed in a definite ratio.

• For example, granite is a mixture of three minerals.

Different ratios of the minerals give granite different

colors, but the mixture is always called granite.

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• 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.

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

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• 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.

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Click below to watch the Visual Concept.

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

Visual Concept

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

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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.

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• 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.

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(31)

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.

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

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• 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.

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

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• 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.

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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.

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

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

mixture colloid filter

element

suspension solution

compound

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

Resources Chapter menu

Reading

Read each of the passages. Then, answer the

questions that follow each passage.

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ever to set sail. This majestic ship was considered to be unsinkable. Yet, on April 15, 1912, the Titanic hit a large iceberg. The resulting damage caused the Titanic to sink, killing 1,500 of its passengers and crew.

How could an iceberg destroy the 2.5 cm thick steel plates that made up the Titanic’s hull?

Continued on the next slide

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

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Passage 1, continued Analysis of a recovered piece of steel showed that the steel contained large amounts of sulfur. Sulfur is a normal component of steel. However, the recovered piece has much more sulfur than today’s steel does. The excess sulfur may have made the steel brittle, much like glass. Scientists suspect that this

brittle steel may have cracked on impact with the

iceberg, allowing water to enter the hull.

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1. In this passage, what does the word brittle mean?

A likely to break or crack B very strong

C clear and easily seen through

D lightweight

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

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1. In this passage, what does the word brittle mean?

A likely to break or crack B very strong

C clear and easily seen through

D lightweight

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this passage?

F The Titanic’s hull was 2.5 cm thick.

G The steel in the Titanic’s hull may have been brittle.

H The large amount of sulfur in the Titanic’s hull may be responsible for the hull’s cracking.

I Scientists were able to recover a piece of steel from

the Titanic’s hull.

(46)

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

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this passage?

F The Titanic’s hull was 2.5 cm thick.

G The steel in the Titanic’s hull may have been brittle.

H The large amount of sulfur in the Titanic’s hull may be responsible for the hull’s cracking.

I Scientists were able to recover a piece of steel from

the Titanic’s hull.

(47)

3. What was the Titanic thought to be in 1912?

A the fastest ship afloat

B the smallest ship to set sail

C a ship not capable of being sunk

D the most luxurious ship to set sail

(48)

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

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3. What was the Titanic thought to be in 1912?

A the fastest ship afloat

B the smallest ship to set sail

C a ship not capable of being sunk

D the most luxurious ship to set sail

(49)

practiced by the ancient Egyptians, who rubbed their bodies with a substance made by soaking fragrant woods and resins in water and oil. Ancient Israelites also practiced the art of perfume making. This art was also known to the early Chinese, Arabs, Greeks, and Romans.

Continued on the next slide

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

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Over time, perfume making has developed into a fine art. A good perfume may contain more than 100

ingredients. The most familiar ingredients come from

fragrant plants, such as sandalwood or roses. These

plants get their pleasant odor from essential oils, which

are stored in tiny, baglike parts called sacs. The parts of

plants that are used for perfumes include the flowers,

roots, and leaves. Other perfume ingredients come

from animals and from human-made chemicals.

(51)

1. How did ancient Egyptians make perfume?

A by using 100 different ingredients

B by soaking woods and resins in water and oil C by using plants or flowers

D by making tiny, baglike parts called sacs

(52)

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

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1. How did ancient Egyptians make perfume?

A by using 100 different ingredients

B by soaking woods and resins in water and oil C by using plants or flowers

D by making tiny, baglike parts called sacs

(53)

F Perfume making hasn’t changed since ancient Egypt.

G The ancient art of perfume making has been replaced by simple science.

H Perfume making is a complex procedure involving many ingredients.

I Natural ingredients are no longer used in perfume.

(54)

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

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F Perfume making hasn’t changed since ancient Egypt.

G The ancient art of perfume making has been replaced by simple science.

H Perfume making is a complex procedure involving many ingredients.

I Natural ingredients are no longer used in perfume.

(55)

3. How are good perfumes made?

A from plant oils only

B by combining one or two ingredients C according to early Chinese formulas

D by blending as many as 100 ingredients

(56)

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

Resources Chapter menu

3. How are good perfumes made?

A from plant oils only

B by combining one or two ingredients C according to early Chinese formulas

D by blending as many as 100 ingredients

(57)

The graph below was constructed from data collected

during a laboratory investigation. Use the graph below

to answer the questions that follow.

(58)

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

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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

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sodium nitrate that can dissolve in 100 mL of water at 40°C?

A 0 g

B 40 g

C 80 g

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

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sodium chloride can dissolve in 100 mL of water at 60°C?

F 40 g

G 80 g

H 125 g

I 160 g

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sodium chloride can dissolve in 100 mL of water at 60°C?

F 40 g

G 80 g

H 125 g

I 160 g

(62)

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

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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

(63)

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

(64)

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

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

F sodium chloride

G sodium chlorate

H potassium bromide

I sodium nitrate

(66)

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

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Math

Read each question, and choose the best answer.

(67)

A 12 cm B 18 cm C 36 cm D 72 cm

12 cm

6 cm

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A 12 cm B 18 cm C 36 cm D 72 cm

12 cm

6 cm

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below were doubled, what would be the area of the larger rectangle?

F 36 cm

2

G 72 cm

2

H 144 cm

2

I 288 cm

2

12 cm

6 cm

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

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below were doubled, what would be the area of the larger rectangle?

F 36 cm

2

G 72 cm

2

H 144 cm

2

I 288 cm

2

12 cm

6 cm

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solvent. What is the concentration of a solution that is made by dissolving 65 g of sugar (the solute) in 500 mL of water (the solvent)?

A 0.13 g•mL

B 0.13 g/mL

C 7.7 g•mL

(72)

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solvent. What is the concentration of a solution that is made by dissolving 65 g of sugar (the solute) in 500 mL of water (the solvent)?

A 0.13 g•mL

B 0.13 g/mL

C 7.7 g•mL

D 7.7 g/mL

(73)

4. If 16/n  1/2, what is the value of n?

F 2

G 8

H 16

I 32

(74)

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4. If 16/n  1/2, what is the value of n?

F 2

G 8

H 16

I 32

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