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Chapter 10
Chemical Reactions
Table of Contents
Section 1 Forming New Substances
Section 2 Chemical Formulas and Equations
Section 3 Types of Chemical Reactions
Section 4 Energy and Rates of Chemical Reactions
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Chapter 10
Section 1 Forming New Substances
Bellringer
What do baking bread, launching the space shuttle,
and digesting food have in common?
Write your answer in your science journal.
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Chapter 10
Section 1 Forming New Substances
Objectives
• Describe how chemical reactions produce new
substances that have different chemical and physical
properties.
• Identify four signs that indicate that a chemical
reaction might be taking place.
• Explain what happens to chemical bonds during a
chemical reaction.
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Chapter 10
Section 1 Forming New Substances
Chemical Reactions
• A chemical reaction is a process in which one or
more substances change to make one or more new
substances.
• The chemical and physical properties of the new
substances differ from those of the original
substances.
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Chapter 10
Section 1 Forming New Substances
Chemical Reactions, continued
• Signs of Chemical Reactions include color
changes, gas formation, the formation of a precipitate
(a solid substance formed in a solution), and energy
given off as light, thermal energy, or electrical energy.
• A Change of Properties The most important sign of
a chemical reaction is the formation of new substances
that have different properties.
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Chapter 10
Section 1 Forming New Substances
Bonds: Holding Molecules Together
• A chemical bond is an attraction that holds atoms
together in a molecule.
• Breaking and Making Bonds If molecules bump
into each other with enough energy, the chemical
bonds in the molecules break. The atoms then
rearrange, and new bonds form to make new
substances.
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Chapter 10
Section 1 Forming New Substances
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Chapter 10
Section 1 Forming New Substances
Bonds: Holding Molecules Together,
continued
• New Bonds, New Substances When new
substances form, their properties differ from the
properties of the starting substances.
• For example, sodium is a violently reactive metal and
chlorine is a greenish poisonous gas. The two
elements combine to form a white solid called sodium
chloride, or table salt.
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Chapter 10
Section 2 Chemical
Formulas and Equations
Bellringer
Write the following chemical symbols in your science
journal. Then, try to write the names of the elements
matching the symbols.
H
O
C
Na
N
Cl
K
Mg
Ca
Al
Au
F
Cu
Fe
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Chapter 10
Section 2 Chemical
Formulas and Equations
Objectives
• Interpret and write simple chemical formulas.
• Write and balance simple chemical equations.
• Describe the basis for and the results of Lavoisier’s
work with reactions.
• Explain how a balanced equation shows the law of
conservation of mass.
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Chapter 10
Section 2 Chemical
Formulas and Equations
Chemical Formulas
• A chemical formula
is a combination of
chemical symbols and
numbers to represent
a substance. A
chemical formula
shows how many
atoms of each kind are
present in a molecule.
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Section 2 Chemical
Formulas and Equations
Chapter 10
Chemical Formulas, continued
• Writing Formulas for Covalent Compounds You
can use the name of a covalent compound to write its
chemical formula. The names of covalent compounds
use prefixes. Each prefix represents a number, as
shown below.
mono-
1
hexa-
6
di-
2
hepta-
7
tri-
3
octa-
8
tetra-
4
nona-
9
penta-
5
deca-
10
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Chapter 10
Section 2 Chemical
Formulas and Equations
Chemical Formulas, continued
• Writing Formulas for Ionic Compounds To write
the formula for an ionic compound, make sure the
compound’s charge is 0.
• The formula must have subscripts that cause the
charges of the ions to cancel out.
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Chapter 10
Section 2 Chemical
Formulas and Equations
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Chapter 10
Section 2 Chemical
Formulas and Equations
Chemical Equations
• Describing Reactions by Using Equations A
chemical equation uses chemical symbols and
formulas as a shortcut to describe a chemical reaction.
• From Reactants to Products The starting materials
in a reaction are reactants. The substances formed
from a reaction are products.
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Chapter 10
Section 2 Chemical
Formulas and Equations
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Chapter 10
Section 2 Chemical
Formulas and Equations
Chemical Equations, continued
• The Importance of Accuracy The symbol or
formula for each substance in a chemical equation
must be written correctly or it will not correctly describe
the reaction. The images below show how formulas
and symbols can be confused.
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Chapter 10
Section 2 Chemical
Formulas and Equations
Balancing Chemical Equations
• To correctly write a chemical equation, the equation
must be balanced. To understand why, you have to
know about closed systems.
• Nothing Goes In or Out No matter how substances
in a closed system interact with each other or how they
combine or break apart, the total mass of the system
remains the same.
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Chapter 10
Section 2 Chemical
Formulas and Equations
Balancing Chemical Equations, continued
• Carefully Measuring Material In the 1700s, French
chemist Antoine Lavoisier tested the concept of the
conservation of matter.
• This concept is described in the law of conservation
of mass, which states that mass is neither created nor
destroyed in ordinary chemical and physical changes.
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Chapter 10
Section 2 Chemical
Formulas and Equations
Balancing Chemical Equations, continued
• The Reason Equations Must Be Balanced Atoms
are never lost or gained in a chemical reaction. So, a
chemical equation must show the same numbers and
kinds of atoms on both sides of the arrow.
• When the number of atoms of each element in the
reactants equals the number of atoms of those same
elements in the products, the equation is balanced.
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Chapter 10
Section 2 Chemical
Formulas and Equations
Balancing Chemical Equations, continued
• How to Balance an Equation To balance an
equation, you must use coefficients.
• For an equation to be balanced, all atoms must be
counted. So, you multiply the subscript of each
element in a formula by the formula’s coefficient.
• The next slide shows how to use coefficients to
balance an equation.
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Chapter 10
Section 2 Chemical
Formulas and Equations
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Chapter 10
Section 3 Types of
Chemical Reactions
Bellringer
Are the products of a reaction always more complex
than the reactants? Could products be simpler than the
reactants? Explain your answers.
Write your responses in your science journal.
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Chapter 10
Section 3 Types of
Chemical Reactions
Objectives
• Describe four types of chemical reactions.
• Classify a chemical equation as one of four types of
chemical reactions.
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Chapter 10
Section 3 Types of
Chemical Reactions
Synthesis Reactions
• A synthesis reaction is a reaction in which two or
more substances combine to form one new compound.
Decomposition Reactions
• A decomposition reaction is a reaction in which a
single compound breaks down to form two or more
simpler substances.
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Chapter 10
Section 3 Types of
Chemical Reactions
Single-Displacement Reactions
• A single-displacement reaction is a reaction in
which an element replaces another element that is part
of a compound.
• Reactivity of Elements In a single-displacement
reaction, a more reactive element can displace a less
reactive element in a compound.
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Chapter 10
Section 3 Types of
Chemical Reactions
Double-Displacement Reactions
• A double-displacement reaction is a reaction in
which ions from two compounds exchange places.
• The next slide shows models of each of the four
types of chemical reactions.
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Chapter 10
Section 3 Types of
Chemical Reactions
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Bellringer
Now that you know a little about chemical reactions,
think about the many chemical reactions that take
place around you every day. Describe your favorite
chemical reaction. How do you think energy is involved
in the reaction?
Write your answer in your science journal.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Objectives
• Compare exothermic and endothermic reactions.
• Explain activation energy.
• Interpret an energy diagram.
• Describe five factors that affect the rate of a reaction.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Reactions and Energy
• By comparing the chemical energy of the reactants
with the chemical energy of the products, you can
decide if energy is released or absorbed in the
reaction.
• Exothermic Reactions are reactions in which
energy is released. Energy can be released as light,
electrical energy, or thermal energy.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Reactions and Energy, continued
• Endothermic Reactions are reactions in which
energy is taken in.
• The Law of Conservation of Energy states that
energy cannot be created or destroyed. The energy
released in exothermic reactions was first stored in the
chemical bonds of the reactants. And the energy taken
in during endothermic reactions is stored in the
products.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Rates of Reactions
• The speed at which new particles form is called the
rate of a reaction.
• Activation Energy is the smallest amount of energy
that molecules need to react. A chemical reaction
needs a boost of energy greater than or equal to the
activation energy before the reaction can start.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Rates of Reactions, continued
• Sources of Activation Energy Some sources
include friction, electric sparks, and light.
• The next slide shows how activation energy relates to
exothermic and endothermic reactions.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Factors Affecting Rates of Reactions
• Temperature A higher temperature causes a faster
rate of reaction.
• Concentration is a measure of the amount of one
substance when it is dissolved in another substance.
In general, a high concentration of reactants causes a
fast rate of reaction.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Factors Affecting Rates of Reactions,
continued
• Surface Area is the amount of exposed surface of a
substance. Increasing the surface area of solid
reactants increases the rate of a reaction.
• Inhibitors are substances that slow down or stop a
chemical reaction. The rate of a reaction decreases in
the presence of an inhibitor.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Factors Affecting Rates of Reactions,
continued
• Catalysts are substances that speed up a reaction
without being permanently changed. Because it is not
changed, a catalyst is not a reactant.
• A catalyst lowers the activation energy of a reaction,
which allows the reaction to happen more quickly.
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Chapter 10
Section 4 Energy and Rates
of Chemical Reactions
Factors Affecting Reaction Rate
Click below to watch the Visual Concept.
Visual Concept
You may stop the video at any time by pressing
the Esc key.
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Chapter 10
Chemical Reactions
Concept Map
Use the terms below to complete the concept map
on the next slide.
products
reactants
chemical equations
coefficients
chemical reactions
chemical formulas
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Chapter 10
Chemical Reactions
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Chapter 10
Chemical Reactions
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End of Chapter 10 Show
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Chapter 10
Standardized Test Preparation
Reading
Read each of the passages. Then, answer the
questions that follow each passage.
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Chapter 10
Standardized Test Preparation
Passage 1 The key to an air bag’s success during a
crash is the speed at which it inflates. Inside the bag is
a gas generator that contains the compounds sodium
azide, potassium nitrate, and silicon dioxide. At the
moment of a crash, an electronic sensor in the car
detects the sudden change in speed.
Continued on the next slide
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Chapter 10
Standardized Test Preparation
Passage 1, continued The sensor sends a small
electric current to the gas generator. This electric
current provides the activation energy for the chemicals
in the gas generator. The rate at which the reaction
happens is very fast. In 1/25 of a second, the gas
formed in the reaction inflates the bag. The air bag fills
upward and outward. By filling the space between a
person and the car’s dashboard, the air bag protects
him or her from getting hurt.
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Chapter 10
Standardized Test Preparation
1. Which of the following events happens first?
A The sensor sends an electric current to the gas
generator.
B The air bag inflates.
C The air bag fills the space between the person and
the dashboard.
D The sensor detects a change in speed.
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Chapter 10
Standardized Test Preparation
1. Which of the following events happens first?
A The sensor sends an electric current to the gas
generator.
B The air bag inflates.
C The air bag fills the space between the person and
the dashboard.
D The sensor detects a change in speed.
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Chapter 10
Standardized Test Preparation
2. What provides the activation energy for the reaction
to occur?
F the speed of the car
G the inflation of the air bag
H the hot engine
I the electric current from the sensor
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Chapter 10
Standardized Test Preparation
2. What provides the activation energy for the reaction
to occur?
F the speed of the car
G the inflation of the air bag
H the hot engine
I the electric current from the sensor
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Chapter 10
Standardized Test Preparation
3. What is the purpose of this passage?
A to convince the reader to wear a seat belt
B to describe the series of events that inflate an air bag
C to explain why air bags are an important safety
feature in cars
D to show how chemical reactions protect pedestrians
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Chapter 10
Standardized Test Preparation
3. What is the purpose of this passage?
A to convince the reader to wear a seat belt
B to describe the series of events that inflate an air bag
C to explain why air bags are an important safety
feature in cars
D to show how chemical reactions protect pedestrians
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Chapter 10
Standardized Test Preparation
Passage 2 An important tool in fighting forest fires is a
slimy, red goop. This mixture of powder and water is a
very powerful fire retardant. The burning of trees,
grass, and brush is an exothermic reaction. The fire
retardant slows or stops this self-feeding reaction by
increasing the activation energy for the materials to
which it sticks.
Continued on the next slide
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Chapter 10
Standardized Test Preparation
Passage 2, continued A plane can carry between
4,500 and 11,000 L of the goop. The plane then drops it
all in front of the raging flames of a forest fire when the
pilot presses the button. Firefighters on the ground can
gain valuable time when a fire is slowed with a fire
retardant. This extra time allows the ground team to
create a fire line that will finally stop the fire.
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Chapter 10
Standardized Test Preparation
1. Which of the following sentences best summarizes
the passage?
A The burning of forests and other brush is an
exothermic reaction.
B Dropping fire retardants ahead of a flame can help
firefighters on the ground stop a fire.
C Firefighters on the ground create a fire line that will
help stop the fire from spreading.
D The slimy, red goop used as a fire retardant is made
of a mixture of powder and water.
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Chapter 10
Standardized Test Preparation
1. Which of the following sentences best summarizes
the passage?
A The burning of forests and other brush is an
exothermic reaction.
B Dropping fire retardants ahead of a flame can help
firefighters on the ground stop a fire.
C Firefighters on the ground create a fire line that will
help stop the fire from spreading.
D The slimy, red goop used as a fire retardant is made
of a mixture of powder and water.
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Chapter 10
Standardized Test Preparation
2. Based on the passage, which of the following
statements is a fact?
F Fire retardants are always successful in putting
out fires.
G No more than 4,500 L of red goop are loaded
onto a plane.
H A fire retardant works by increasing the activation
energy for the materials that it sticks on.
I The burning of trees is an endothermic reaction.
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Chapter 10
Standardized Test Preparation
2. Based on the passage, which of the following
statements is a fact?
F Fire retardants are always successful in putting
out fires.
G No more than 4,500 L of red goop are loaded
onto a plane.
H A fire retardant works by increasing the activation
energy for the materials that it sticks on.
I The burning of trees is an endothermic reaction.
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Chapter 10
Standardized Test Preparation
Interpreting Graphics
Use the energy diagram below to answer the questions
that follow.
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Chapter 10
Standardized Test Preparation
1. Which letter represents
the energy of the products?
AA
BB
CC
DD
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Chapter 10
Standardized Test Preparation
1. Which letter represents
the energy of the products?
AA
BB
CC
DD
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Chapter 10
Standardized Test Preparation
2. Which letter represents
the activation energy of the
reaction?
FA
GB
HC
ID
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Chapter 10
Standardized Test Preparation
2. Which letter represents
the activation energy of the
reaction?
FA
GB
HC
ID
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Chapter 10
Standardized Test Preparation
3. Which of the following statements best describes the
reaction represented by the graph?
A The reaction is endothermic because the energy of
the products is greater than the energy of the reactants.
B The reaction is endothermic because the energy of
the reactants is greater than the energy of the products.
C The reaction is exothermic because the energy of the
products is greater than the energy of the reactants.
D The reaction is exothermic because the energy of the
reactants is greater than the energy of the products.
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Chapter 10
Standardized Test Preparation
3. Which of the following statements best describes the
reaction represented by the graph?
A The reaction is endothermic because the energy of
the products is greater than the energy of the reactants.
B The reaction is endothermic because the energy of
the reactants is greater than the energy of the products.
C The reaction is exothermic because the energy of the
products is greater than the energy of the reactants.
D The reaction is exothermic because the energy of the
reactants is greater than the energy of the products.
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Chapter 10
Standardized Test Preparation
Math
Read each question, and choose the best answer.
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Chapter 10
Standardized Test Preparation
1. Nina has 15 pens in her backpack. She has 3 red
pens, 10 black pens, and 2 blue pens. If Ben selects a
pen to borrow at random, what is the probability that
the pen selected is red?
A 2/15
B 1/5
C 1/3
D 2/3
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Chapter 10
Standardized Test Preparation
1. Nina has 15 pens in her backpack. She has 3 red
pens, 10 black pens, and 2 blue pens. If Ben selects a
pen to borrow at random, what is the probability that
the pen selected is red?
A 2/15
B 1/5
C 1/3
D 2/3
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Chapter 10
Standardized Test Preparation
2. How many atoms of nitrogen, N, are in the formula
for calcium nitrate, Ca(NO3)2?
F3
G2
H6
I1
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Chapter 10
Standardized Test Preparation
2. How many atoms of nitrogen, N, are in the formula
for calcium nitrate, Ca(NO3)2?
F3
G2
H6
I1
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Standardized Test Preparation
Chapter 10
3. Which letter best represents the number 2 3/5 on the
number line?
P
0
Q
1
R S
2
3
AP
BQ
CR
DS
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Chapter 10
3. Which letter best represents the number 2 3/5 on the
number line?
P
0
Q
1
R S
2
3
AP
BQ
CR
DS
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Chapter 10
Standardized Test Preparation
4. According to the following chemical equation, how
many reactants are needed to form water and carbon
dioxide?
H2CO3  H2O + CO2
F one
G two
H three
I four
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Chapter 10
Standardized Test Preparation
4. According to the following chemical equation, how
many reactants are needed to form water and carbon
dioxide?
H2CO3  H2O + CO2
F one
G two
H three
I four
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Chapter 10
Section 2 Chemical
Formulas and Equations
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Chapter 10
Section 2 Chemical
Formulas and Equations
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Chapter 10
Standardized Test Preparation
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