Table of Contents
Lousiana
Benchmarks
Louisiana Benchmarks Correlation Chart . . . . . . . . . . . . . . . . . . . . . . . .
Chapter 1
10
Scientific Inquiry
Lesson 1
Designing and Conducting Scientific
Investigations . . . . . . . . . . . . . . . . . . . . . . . . . 11
SI-H-A1, SI-H-A2
Lesson 2
Using Mathematics . . . . . . . . . . . . . . . . . . . . . 16
SI-H-A3
Lesson 3
Using Technology . . . . . . . . . . . . . . . . . . . . . . 20
SI-H-A3, SI-H-B3
Lesson 4
Models and Explanations . . . . . . . . . . . . . . . . 24
SI-H-A4, SI-H-A5,
SI-H-B1, SI-H-B2
Lesson 5
Communicating and Defending a Scientific
Argument. . . . . . . . . . . . . . . . . . . . . . . . . . . . . 30
SI-H-A6, SI-H-B4,
SI-H-B5
Lesson 6
Chapter 2
Safety Procedures. . . . . . . . . . . . . . . . . . . . . . 35
SI-H-A7
Lesson 7
Working with Quantitative Data. . . . . . . . . . . . 39
PS-H-A1
Lesson 8
The Language of Chemistry . . . . . . . . . . . . . . 44
PS-H-A2
Lesson 9
The Structure of Atoms and Isotopes. . . . . . . 48
PS-H-A2, PS-H-B1
Lesson 10
Radioactivity . . . . . . . . . . . . . . . . . . . . . . . . . . 52
PS-H-B2
Lesson 11
Elements, Compounds, and Mixtures. . . . . . . 58
PS-H-C1, PS-H-C4
Lesson 12
The Periodic Table of Elements . . . . . . . . . . . 62
PS-H-B3, PS-H-C2
Lesson 13
Physical Interactions and Phase Changes . . . 67
PS-H-C3, PS-H-C7
Lesson 14
Chemical Bonding. . . . . . . . . . . . . . . . . . . . . . 73
PS-H-C5, PS-H-C6
Lesson 15
Changes in Matter. . . . . . . . . . . . . . . . . . . . . . 79
PS-H-D1
Lesson 16
Acids, Bases, and pH . . . . . . . . . . . . . . . . . . . 84
PS-H-D2
Lesson 17
Chemical Reactions and Equations . . . . . . . . 88
PS-H-D3, PS-H-D4
Lesson 18
Conservation of Matter and Energy Changes
in Chemical Reactions . . . . . . . . . . . . . . . . . . 93
PS-H-D5, PS-H-D6
Important Chemical Reactions . . . . . . . . . . . . 97
PS-H-D7
Matter
Lesson 19
Chapter 3
Forces and Motion
Lesson 20
Forces of Nature . . . . . . . . . . . . . . . . . . . . . . 102
PS-H-E1
Lesson 21
Motion . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 107
PS-H-E2, PS-H-E4
Lesson 22
Newtonian Mechanics. . . . . . . . . . . . . . . . . . 113
PS-H-E3
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Chapter 4
Energy
Lesson 23
Energy, Work, Power, and Efficiency. . . . . . . 117
PS-H-F1
Lesson 24
Conservation of Matter, Energy,
and Momentum. . . . . . . . . . . . . . . . . . . . . . . 123
PS-H-F2
Transport of Energy by Waves . . . . . . . . . . . 128
PS-H-G1, PS-H-G3,
Lesson 25
PS-H-G4
Lesson 26
Chapter 5
Chapter 6
Electricity and Magnetism. . . . . . . . . . . . . . . 135
PS-H-G2
The Cell and Heredity
Lesson 27
Cells and Viruses. . . . . . . . . . . . . . . . . . . . . . 142
LS-H-A1, LS-H-C7
Lesson 28
Cellular Transport . . . . . . . . . . . . . . . . . . . . . 147
LS-H-A2
Lesson 29
Cell Differentiation and Comparative
Embryology . . . . . . . . . . . . . . . . . . . . . . . . . . 150
LS-H-A3
Lesson 30
Structures of Heredity . . . . . . . . . . . . . . . . . . 156
LS-H-B1
Lesson 31
Mitosis and Meiosis . . . . . . . . . . . . . . . . . . . 161
LS-H-B2
Lesson 32
Mendelian Genetics . . . . . . . . . . . . . . . . . . . 168
LS-H-B3
Lesson 33
Biotechnology: Pros and Cons . . . . . . . . . . . 175
LS-H-B4
Biological Processes
Lesson 34
Evidence of Evolution . . . . . . . . . . . . . . . . . . 179
LS-H-C1, LS-H-C2
Lesson 35
Patterns, Processes, and Rates of Evolution . 184
LS-H-C3
Lesson 36
Classifying Organisms. . . . . . . . . . . . . . . . . . 189
LS-H-C4, LS-H-C5
Lesson 37
Life Cycles. . . . . . . . . . . . . . . . . . . . . . . . . . . 196
LS-H-C6
Lesson 38
Biogeochemical Cycles. . . . . . . . . . . . . . . . . 202
LS-H-D1, SE-H-A6,
SE-H-A7
Lesson 39
Energy Flow in Ecosystems . . . . . . . . . . . . . 206
LS-H-D2, SE-H-A2
Lesson 40
Population Dynamics . . . . . . . . . . . . . . . . . . 210
LS-H-D3
Lesson 41
Impact of Human Activities on Ecosystems . 214
LS-H-D4, SE-H-A11
Lesson 42
Photosynthesis and Cellular Respiration . . . 218
LS-H-E1, LS-H-E2
Lesson 43
Levels of Biological Organization . . . . . . . . . 222
LS-H-E3, LS-H-F1
Lesson 44
Homeostasis . . . . . . . . . . . . . . . . . . . . . . . . . 226
LS-H-F2
Lesson 45
Responses to Stimuli . . . . . . . . . . . . . . . . . . 230
LS-H-F3, LS-H-F4
Lesson 46
Health . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 234
LS-H-G1, LS-H-G3
Lesson 47
Disease . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 238
LS-H-G2, LS-H-G3,
LS-H-G4, LS-H-G5
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Chapter 7
Chapter 8
Chapter 9
Earth Science
Lesson 48
Radiant Energy and Seasons . . . . . . . . . . . . 244
ESS-H-A1, ESS-H-A2
Lesson 49
Sources of Earth’s Heat . . . . . . . . . . . . . . . . 248
ESS-H-A3, ESS-H-A4
Lesson 50
Convection Currents . . . . . . . . . . . . . . . . . . . 252
ESS-H-A5, ESS-H-A7
Lesson 51
Geochemical Cycles . . . . . . . . . . . . . . . . . . . 257
ESS-H-B1, ESS-H-B2
Lesson 52
The Geology of Louisiana . . . . . . . . . . . . . . . 262
ESS-H-C3
Lesson 53
Fossils and Earth’s History . . . . . . . . . . . . . . 265
ESS-H-C4
Lesson 54
Rapid and Slow Change to Earth’s Surface . 269
ESS-H-A7, ESS-H-C5
Space Science
Lesson 55
The Origin and Age of the Universe . . . . . . . 274
ESS-H-D1
Lesson 56
Elements in the Stars . . . . . . . . . . . . . . . . . . 278
ESS-H-D4, ESS-H-D5
Lesson 57
Formation of the Solar System and Earth . . 282
ESS-H-C1, ESS-H-C2
Lesson 58
Orbits. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 287
ESS-H-D6
Lesson 59
The Technology of Earth and Space Science. 291
ESS-H-D7
Science and the Environment
Lesson 60
Earth’s Ecological Systems. . . . . . . . . . . . . . 296
SE-H-A1
Lesson 61
Biodiversity and Ecological Succession . . . . 300
SE-H-A4, SE-H-A9
Lesson 62
Adaptations of Plants and Animals. . . . . . . . 304
SE-H-A8
Lesson 63
Development and Earth’s Resources . . . . . . 309
SE-H-B3, SE-H-B6,
SE-H-C1, SE-H-C4
Glossary . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 314
Pretest . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 335
Posttest . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 359
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15
Changes in Matter
PS-H-D1
Getting the Idea
Key Words
physical property
physical change
chemical property
chemical change
density
solubility
viscosity
electrical
conductivity
oxidation
combustibility
corrosion
precipitate
Properties are characteristics that are used to identify and classify
matter. Different types of matter behave differently because of their
unique properties.
Characteristics of Matter
Physical and chemical properties describe the different ways that matter
behaves. A physical property is a characteristic of a substance that
can be observed directly or measured with a tool without changing the
composition of the substance. A physical change is any change in a
substance in which the composition of the substance does not change.
A chemical property describes a substance’s potential to change in a
way that alters its composition. A chemical change is any change that
forms new substances.
Physical Properties and Physical Changes
Physical properties include boiling point, freezing/melting point, density,
solubility, viscosity, and electrical conductivity. These properties can be
observed or measured without changing the substance. Examples of
physical changes include changes in state, size, and shape.
Evaporating, condensing, freezing, and melting are state changes, or
phase changes—the changing from one state of matter into another.
All state changes are physical changes because the composition of a
substance does not change during a state change.
A change in temperature can cause a substance to expand or contract.
These are physical changes. A substance can also change size by being
broken into smaller pieces or by being stretched or pulled. For example,
hammering a piece of metal into a thin sheet is a physical change. The
ability of metals to be hammered into thin sheets is called malleability, a
physical property unique to metals. Another unique property of metals is
that they can be drawn into thin wires. This physical property is known
as ductility.
A change in color sometimes indicates a physical change. When two
colors of paint or dye are mixed together, they form a mixture with a
completely different color. The substances are not chemically combined
because the atoms have not been rearranged.
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Density, the mass of a substance per unit volume, is another physical
property of matter. Recall that mass is the amount of matter in an object
and volume is the amount of space an object occupies. Density cannot
be measured directly. It is the ratio of two direct measurements: mass
and volume. The following equation is used to calculate density:
mass
density 5 _______
volume
__
D5m
V
Example: What is the density of a sample of gold that has a mass
of 386.4 g and a volume of 20.0 cm3?
Knowns:
m 5 386.4 g, V 5 20.0 cm3
Equation:
m
D 5 __
Solve:
386.4 g
D 5 _______3
V
20.0 cm
3
D 5 19.32 g / cm
3
The density of gold is 19.32 g / cm .
Because density is a ratio of mass to volume, as the mass of a
substance increases, its volume also increases. However, at a given
temperature and pressure the density of a substance remains constant.
Solubility is a measure of the amount of one substance that will dissolve
in another at a particular temperature and pressure. A solution is a kind
of mixture. The solute and solvent do not chemically combine when the
solute dissolves. Each substance retains its own properties. Therefore,
solubility is a physical property.
Water is a unique solvent because it readily dissolves many substances.
Water can dissolve solids such as salt and sugar, liquids such as acids
and bases, and gases such as oxygen and carbon dioxide.
Viscosity is a fluid’s resistance to flow. Fluids with high viscosity take
longer to pour than fluids with low viscosity. As temperature changes,
a fluid’s viscosity may also change. Because the composition of a fluid
does not change when it is poured, viscosity is a physical property.
Electrical conductivity is a material’s ability to conduct or move
electrical current. It is a physical property because conducting an
electrical current does not change the composition of matter. In general,
metals have high conductivity, and current flows through them easily.
Nonmetals have low conductivity and are good insulators because they
resist the flow of current.
Some solutions can conduct electrical currents. Solutes that form ions in
solution make solutions that conduct electricity. Such solutes are called
electrolytes.
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Lesson 15: Changes in Matter
The table below lists several physical properties and physical changes
of matter.
Physical Changes
Physical Properties
Physical Changes
temperature
volume
color
ductility
mass
density
solubility
shape
conductivity
viscosity
Chemical Properties and Chemical Changes
Chemical properties include the potential to oxidize, to combust, and to
corrode. Oxidation, combustion, and corrosion are chemical changes
because they form new substances. During a chemical change, there
is a change in the arrangement of atoms involved, forming a different
substance with different properties.
In oxidation, a substance combines with oxygen to form a new
substance with new properties. The new substance is a combination
of the atoms in the original substance with the oxygen atoms. It has
different physical and chemical properties from the original substances.
Burning hydrogen gas to produce water is an oxidation reaction. The
properties of water are very different from the properties of hydrogen
and oxygen.
Combustion, or burning, is a special case of oxidation. Combustibility
is a chemical property of substances that can combine rapidly with
oxygen and burn, forming products with new properties. Combustion
releases lots of energy in the form of heat and light. The burning of a
log in a fireplace is a common example of combustion. When it burns,
the wood in the log is changed into ash and carbon dioxide. The carbon
dioxide gas is released into the air.
Corrosion is a general term for chemical changes that weaken or
discolor useful metals. Many metals combine with oxygen, sulfur, and
other nonmetals to form products whose new properties include a
different color and brittleness. Corrosion produces compounds of metals
and nonmetals. A nail rusting is a typical example of corrosion, during
which the gray, shiny iron of the nail becomes the dull, red-brown rust.
In this chemical reaction, iron (Fe) in the nail combines with oxygen (O2)
in the air to form rust, or iron oxide (FeO2).
Reactions of substances with acids and bases are chemical changes.
An acid and a base react to form water and a salt. This is a chemical
change because the atoms in the original substances are rearranged
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to form new substances with different properties. For example,
hydrochloric acid (HCl) and the base sodium hydroxide (NaOH) react
to form water (H2O) and table salt, or sodium chloride (NaCl).
Evidence of Chemical Change
Chemical changes produce evidence. Formation of a gas or precipitate,
a change of color, energy changes, and presence of an odor are
evidence that some kind of change has taken place.
Bubbles can indicate that a chemical change has occurred. For
example, metals will replace the hydrogen in an acid solution to form
a salt and hydrogen gas. The hydrogen will produce bubbles in the
solution before it is released into the air.
The formation of a precipitate is also evidence of a chemical change.
A precipitate is a solid that forms when two liquids are mixed. For
example, a white precipitate of silver chloride forms when a solution
of silver nitrate is mixed with a solution of sodium chloride (salt water).
Silver chloride has a different composition than the original silver nitrate
and sodium chloride.
Chemical changes produce energy changes. For example, energy is
produced in the form of heat and light when a substance burns. The
heat and light are evidence that a chemical change may have occurred.
Color changes and odors may also indicate a chemical change. As iron
rusts, it changes from silvery to a red-brown color. When ammonium
carbonate is heated, an odor of ammonia gas can be identified.
The table below summarizes the evidence of chemical changes.
Chemical Changes
Evidence
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Observation
Formation of gas
Gas bubbles escape a solution.
Formation of precipitate
A solid forms in a solution.
Change in energy
The temperature increases or decreases, and the
substance may give off light.
Change in color
A new color appears when two or more substances react.
Presence of an odor
When a substance is heated or substances are mixed, an
odor is detected.
Duplicating any part of this book is prohibited by law.
Lesson 15: Changes in Matter
DISCUSSION QUESTION
A teacher mixes two substances for his students to observe. How can the
students determine whether a chemical change has taken place?
LESSON REVIEW
1.
2.
3.
4.
Which of these is a chemical change?
A.
formation of hydrogen gas when a metal is placed in a strong
acid
B.
evaporation of water from a puddle on a hot afternoon
C.
finding the density of a piece of silver by measuring its mass and
volume
D.
hammering aluminum metal into a thin sheet to be used for
aluminum foil
Which of the following is a physical change?
A.
Silver sulfide forms when silver reacts with sulfur in the air.
B.
The burning of methane gas produces water and carbon dioxide.
C.
Water vapor condenses on the outside of a cold can of soda.
D.
Vinegar and baking soda combine and form a salt and water.
When copper reacts with oxygen in the air, a color change takes place,
and the copper becomes green. This green color is called patina. What
type of chemical change produces patina?
A.
combustion
C.
conduction
B.
oxidation
D.
neutralization
When solutions of silver nitrate and sodium chloride are mixed, silver
chloride, a solid white substance, forms. What is the name for a solid
that forms when two solutions are mixed?
A.
acid
C.
precipitate
B.
liquid
D.
gas
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