Hstp ch04

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Chapter Presentation
Transparencies
Image and Math Focus Bank
Bellringers
Standardized Test Prep
Visual Concepts
Resources

Elements, Compounds, and Mixtures
Table of Contents
Section 1 Elements
Section 2 Compounds
Section 3 Mixtures
Chapter 4

Section 1 Elements
Bellringer
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?
Chapter 4

Section 1 Elements
Objectives
• Describe pure substances.
• Describe the characteristics of elements, and give
examples.
• Explain how elements can be identified.
• Classify elements according to their properties.
Chapter 4

Section 1 Elements
Elements, the Simplest Substances
• 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.
Chapter 4

Section 1 Elements
Properties of Elements
• 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.
Chapter 4

Section 1 Elements
Classifying Elements by Their Properties
• 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.
Chapter 4

Section 1 Elements
Classifying Elements by Their Properties,
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.
Chapter 4

Section 1 ElementsChapter 4

Section 2 Compounds
Bellringer
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.
Chapter 4

Section 2 Compounds
Objectives
• 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.
Chapter 4

Section 2 Compounds
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.
Chapter 4

Section 2 Compounds
Compounds: Made of Elements
• 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.
Chapter 4

Section 2 Compounds
Properties of Compounds
• 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.
Chapter 4

Section 2 Compounds
Breaking Down Compounds
• 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.
Chapter 4

Section 2 Compounds
Compounds in Your World
• 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.
Chapter 4

Section 3 Mixtures
Bellringer
Chapter 4

Section 3 Mixtures
Objectives
• 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.
Chapter 4

Section 3 Mixtures
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.
Chapter 4

Section 3 Mixtures
Properties of Mixtures
• A mixture is a combination of two or more
substances that are not chemically combined.
• No Chemical Changes in a Mixture
Chapter 4

Section 3 Mixtures
Properties of Mixtures, continued
• Separating Mixtures Through Physical Methods
• The next slide shows some common ways to
separate mixtures by using physical changes.
Chapter 4

Section 3 Mixtures
Properties of Mixtures, continued
• 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.
Chapter 4

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

Magnetic attraction

Filtration

Distillation

Evaporation

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
Click below to watch the Visual Concept.
You may stop the video at any time by pressing
the Esc key.
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

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

Elements, Compounds, and Mixtures
Use the terms below to complete the concept map
on the next slide.
Chapter 4
Concept Map
mixture
colloid
filter
element
suspension
solution
compound

Elements, Compounds, and MixturesChapter 4

End of Chapter 4 Show

Reading
Read each of the passages. Then, answer the
questions that follow each passage.
Chapter 4 Standardized Test Preparation

Passage 1 In 1912, the Titanic was the largest ship
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

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.

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

2. What is the main idea of the second paragraph of
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.

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

Passage 2 Perfume making is an ancient art. It was
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

Passage 2, continued
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.

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

2. What is the main idea of the second paragraph?
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.

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

Interpreting Graphics
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

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

4. At 20°C, which solid is
the most soluble?
F sodium chloride
G sodium chlorate
H potassium bromide
I sodium nitrate

Math
Read each question, and choose the best answer.

1. What is the perimeter of the rectangle shown below?
A 12 cm
B 18 cm
C 36 cm
D 72 cm
12 cm
6 cm

2. If the length of all the sides of the rectangle shown
below were doubled, what would be the area of the
larger rectangle?
F 36 cm2
G 72 cm2
H 144 cm2
I 288 cm2
12 cm
6 cm

ResourcesChapter menuChapter menu
2. If the length of all the sides of the rectangle shown
below were doubled, what would be the area of the
larger rectangle?
F 36 cm2
G 72 cm2
H 144 cm2
I 288 cm2
12 cm
6 cm

3. One way to calculate the concentration of a solution
is to divide the grams of solute by the milliliters of
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

4. If 16/n = 1/2, what is the value of n?
F 2
G 8
H 16
I 32

Hstp ch04

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