CP Chemistry– Curriculum Pacing Guide – 2012-2013
Content Areas
Pacing
SC Standards/
Indicators
C-1.2
C-1.4
C-1.6
C-1.7
C-1.8
Unit 1 - Introduction to Chemistry
Unit 2 - Measurement: Significant Digits, Scientific Notation
Daily - 10 days
A/B - 5 days
Daily - 15 days
A/B - 7 days
Use appropriate laboratory apparatuses, technology, and
techniques safely and accurately when conducting a
scientific investigation.
Design a scientific investigation with appropriate methods
of control to test a hypothesis (including independent and
dependent variables), and evaluate the designs of sample
investigations.
Evaluate the results of a scientific investigation in terms of
whether they verify or refute the hypothesis and what the
possible sources of error are.
Evaluate a technological design or product on the basis of
designated criteria.
Use appropriate safety procedures when conducting
investigations.
C-1.1
C-1.3
C-1.5
Apply established rules for significant digits, both in reading
a scientific instrument and in calculating a derived quantity
from measurement.
Use scientific instruments to record measurement data in
appropriate metric units that reflect the precision and
accuracy of each particular instrument.
Organize and interpret the data from a controlled scientific
investigation by using mathematics (including formulas,
scientific notation, and dimensional analysis), graphs,
models, and/or technology.
Content Focus
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Lab Techniques
Lab Safety
Scientific Method
Evaluate Scientific Investigations
Technological Design
Review of Properties and Classifications of Matter
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Significant Digits
Scientific Notation
Dimensional Analysis
Precision/Accuracy
Density Calculations
Suggested
Activities




Corn Starch Lab (text, p. 6)
Bubble Lab (salt) (text, p. 23)
Mystery Powder (text, p. 38)
Paper Chromatography (text, p. 45)
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
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Percent Composition M&M Lab (Graphing)
Measurement Lab
Sig Figures Lab (text, p. 72)
Candy Bar Density
Density Lab
Unit Conversions Lab (text, p. 87)
Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapters 1 and 2
Anderson School District Five
Prentice Hall Chemistry, 2008 Edition
Chapter 3
1
July 1, 2012
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Unit 3 - Atomic Structure and Electron Configuration
Unit 4 - Chemical Periodicity
Daily - 15 days
A/B - 7 days
Daily - 5 days
A/B - 3 days
Pacing
SC
Standards/
Indicators
C-2.1
Content
Focus
Tested 1st Nine Weeks



Illustrate electron configurations by using orbital
notation for representative elements.
C-2.2
First Nine Weeks Exam
Content
Areas
Structure of the Atom
Determining Valence Electrons
Using Mass Number and Atomic Weight
Tested 2nd Nine Weeks
Suggested
Activities
Textbook
Correlation
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
Quantum Numbers
Electron Configuration
Exceptions to Normal Filling Order
Explain Bright Line Spectrum
Wintergreen Mints Lab (not on disk)
Flame Tests (text, p. 142)
Electron Configurations of Selected Elements
Prentice Hall Chemistry, 2008 Edition
Chapter 4 and 6
Anderson School District Five
Summarize atomic properties (including electron
configuration, ionization energy, electron affinity, atomic
size, and ionic size).
C-2.3 Summarize the periodic table’s property trends (including
electron configuration, ionization energy, electron
affinity, atomic size, ionic size, and reactivity).

Electron Configurations

Ionization Energy

Electron Affinity

Atomic Radius

Ionic Radius

Reactivity

Electronegativity

Metals/Nonmetals/Metalloids

Structure of Periodic Table


Getting to Know the Periodic Table (Periodic Table Coloring)
Group 2: The Alkaline Earth Metals
Prentice Hall Chemistry, 2008 Edition
Chapter 6
2
July 1, 2012
Content Areas
Pacing
SC Standards/
Indicators
C-3.1
C-3.2
C-3.3
C-5.1
Unit 5 - Names and Formulas
Ionic/Covalent
Unit 6 - Carbon Chemistry
Daily - 30 days
A/B - 15 days
Daily - 5 days
A/B - 3 days
Predict the type of bonding (ionic or covalent) and the
shape of simple compounds by using Lewis dot
structures and oxidation numbers.
Interpret the names and formulas for ionic and covalent
compounds.
Explain how the types of intermolecular forces present
in a compound affect the physical properties of
compounds (including polarity and molecular shape).
Explain the effects of the intermolecular forces on the
different phases of matter.
C-3.2
C-3.4
C-3.5
Interpret the names and formulas for ionic and covalent
compounds.
Explain the unique bonding characteristics of carbon that
have resulted in the formation of a large variety of
organic structures.
Illustrate the structural formulas and names of simple
hydrocarbons (including alkanes and their isomers and
benzene rings).
Content Focus
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Ionic and Covalent Bonding
Hydrogen Bonding
Covalent Bonds
Shapes of Molecules
Lewis Dot Structures
Ionic Bonds
Oxidation Numbers
Polyatomic Ions
Naming and Writing Formulas
Polar, Nonpolar
Degree of Ionic Character
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Bonding in Carbon
Sp3 Hybridization
Single, Double, Triple Bonds
Ring Structures
Covalent Network
IUPAC Naming
Naming Alkanes
Isomers
Benzene
Structural/Molecular Formulas
Suggested
Activities

Making Ionic Compounds (text, p. 279)


Molecular Models PowerPoint
Building Hydrocarbons with Models
Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapters 7, 8, and 9
Anderson School District Five
Second Nine Weeks Exam
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Prentice Hall Chemistry, 2008 Edition
Chapters 22 and 23’
3
July 1, 2012
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Pacing
Unit 7 - Moles/Chemical Quantities
Unit 8 - Chemical Reactions
Daily - 15 days
A/B - 10 days
Daily - 15 days
A/B - 10 days
(Begin teaching in 2nd nine weeks; not tested until 3rd nine
weeks)
SC Standards/
Indicators
C-4.4
Apply the concept of moles to determine the number of
particles of a substance in a chemical reaction, the
percent composition of a representative compound, the
mass proportions, and the mole-mass relationships.
Content Focus
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Mole Relationships
Percent Composition
Molar Mass
Molar Volume for Gases
Suggested
Activities

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
Mole Bean Lab
Composition of Hydrates Lab
Everyday Moles
Mole Tray Demo (not on disk)
Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapter 10
Anderson School District Five
C-4.1
Analyze and balance equations for simple synthesis,
decomposition, single replacement, double replacement,
and combustion reactions.
C-4.2 Predict the products of acid-base neutralization and
combustion reactions. (No Neutralization)

Types of Reactions

Symbols for equations

Predicting Products

Write and Balance Equations

Activity Series

Solubility Rules


Observing Chemical Reactions
Types of Chemical Reactions Lab
Third Nine Weeks Exam
Content Areas
Prentice Hall Chemistry, 2008 Edition
Chapter 11
4
July 1, 2012
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Content Areas
Unit 9 - Stoichiometry
Unit 10 - Matter
Daily - 20 days
A/B - 10 days
Pacing
Daily - 3 days
A/B - 2 days
(Begin teaching in 3rd nine weeks; not tested until end of year)
SC Standards/
Indicators
C-4.5
Predict the percent yield, the mass of excess, and the
limiting reagent in chemical reactions.
Content Focus
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
Stoichiometric Calculations
Mass-Mass
Limiting Reactants
Percent Yield
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Phase Changes
Phase Diagrams
Temperature/Time Graph
Evaporation vs. Boiling
Suggested
Activities


Reaction Lab 2 (not on disk)
How Much Carbon Dioxide is Given Off in Alka-Seltzer Lab

Heat of Fusion of Ice (text, p. 522)
Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapter 12
Anderson School District Five
C-5.4
Illustrate and interpret heating and cooling curves (including
how boiling and melting points can be identified and how
boiling points vary with changes in pressure).
Prentice Hall Chemistry, 2008 Edition
Chapter 13
5
July 1, 2012
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Content Areas
Pacing
SC Standards/
Indicators
C-5.2
C-5.3
Unit 11 - Gases and Gas Laws
Unit 12 - Nuclear
Daily - 7 days
A/B - 4 days
Daily - 3 days
A/B - 2 days
Explain the behaviors of gas; the relationship among
pressure, volume, and temperature; and the significance of
the Kelvin (absolute temperature) scale, using the kineticmolecular theory as a model.
Apply the gas laws to problems concerning changes in
pressure, volume, or temperature (including Charles’s law,
Boyle’s law, and the combined gas law).
Content Focus
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Kinetic and Molecular Theory
Temperature and Average Kinetic Energy
Charles’ and Boyle’s Laws
Suggested
Activities


Balloon in a Bell Jar (not on disk)
Grahams Law Lab (not on disk)
Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapter 14
Anderson School District Five
C-2.4
C-2.5
C-2.6
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
Compare the nuclear reactions of fission and fusion to
chemical reactions (including the parts of the atom involved
and the relative amounts of energy released).
Compare alpha, beta, and gamma radiation in terms of
mass, charge, penetrating power, and the release of these
particles from the nucleus.
Explain the concept of half-life, its use in determining the
age of materials, and its significance to nuclear waste
disposal.
Half-Life
Alpha, Beta, and Gamma Waves
Writing Nuclear Reactions
Fission/Fusion Chemical Reactions
Half-Life, (text, p. 809)
Prentice Hall Chemistry, 2008 Edition
Chapter 25
6
July 1, 2012
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Content Areas
Pacing
SC Standards/
Indicators
C-6.1
C-6.2
C-6.3
C-6.4
Unit 13 - Solutions
Unit 14 - Reaction Rates
Daily - 7 days
A/B - 4 days
Daily - 5 days
A/B - 3 days
Summarize the process by which solutes dissolve in
solvents, the dynamic equilibrium that occurs in saturated
solutions, and the effects of varying pressure and
temperature on solubility.
Compare solubility of various substances in different
solvents (including polar and nonpolar solvents and organic
and inorganic substances).
Illustrate the colligative properties of solutions (including
freezing point depression and boiling point elevation and
their practical uses).
Carry out calculations to find the concentration of solutions
in terms of molarity and percent weight (mass).
C-4.3
C-4.6
Analyze the energy changes (endothermic or exothermic)
associated with chemical reactions.
Explain the role of activation energy and the effects of
temperature, particle size, stirring, concentration, and
catalysts in reaction rates.
Content Focus
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Solubility of Various Substances
Colligative Properties
Molarity and Percent Weight
Solutions, Suspensions, and Colloids
LeChatelier’s Principle
Saturated, Unsaturated, and Supersaturated Solutions
Like Dissolves Like

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Endothermic/Exothermic Reactions
Enthalpy
Entropy
Activation Energy Diagram
Suggested
Activities

Solubility Lab – Polar and Non-polar


Alka-Seltzer Demo (not on disk)
Mentos and Diet Coke Demo (not on disk)
Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapter 16
Anderson School District Five
Prentice Hall Chemistry, 2008 Edition
Chapter 18 (section 18.4)
Chapter 1
7
July 1, 2012
CP Chemistry– Curriculum Pacing Guide – 2012-2013
Content Areas
Unit 15 - Acids and Bases
SC Standards/
Indicators
C-4.2
C-6.5
C-6.6
C-6.7
Predict the products of acid-base neutralization and
combustion reactions. (Only neutralization)
Summarize the properties of salts, acids, and bases.
Distinguish between strong and weak common acids and
bases.
Represent common acids and bases by their names and
formulas.
Suggested
Activities
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Textbook
Correlation
Prentice Hall Chemistry, 2008 Edition
Chapter 19
Content Focus
Properties of Acids, Bases, and Salts
Differentiate Strong/Weak vs. Concentrated/Dilute
Recognize Ionization Reactions
Define/Contrast Acids and Bases
Conjugate Acid/Base Pairs
Recognize Common Acid and Base Formulas
Acids and Bases Activity
Red Cabbage Indicators Scale
Anderson School District Five
8
End of Course Exam
Daily - 6 days
A/B - 3 days
Pacing
July 1, 2012