AP CHEMISTRY
Textbook:
Brown, LeMay and Bursten, Chemistry, the Central
Science, 10th Edition, Prentice Hall, 2006.
Supplemental Texts:
Chang, Chemistry, 9th Ed, McGraw-Hill, 2007.
Zumdahl, Chemistry, 7th Ed, Houghton Mifflin, 2007.
Ebbing, Gammon, General Chemistry, 7th Ed, Houghton
Mifflin, 2002.
ABOUT THE AP CHEMISTRY COURSE
AP Chemistry is designed to offer a rigorous and challenging course that covers
the chemistry and chemical principles typical of college and university general
chemistry courses. Students learn the usefulness and relevance of chemistry in
both their intended areas of study and in the everyday world. This course is
designed to enable the students to attain a depth of understanding of
fundamentals and a reasonable competence in dealing with chemical problems. The
course contributes to the development of the students’ abilities to think clearly
and to express their ideas, orally and in writing, with clarity and logic. This course
provides a rigorous treatment of college-level chemistry with such topics as
chemical behavior, bonding theory, thermodynamics, quantum theory, kinetics,
equilibrium, electrochemistry, and organic chemistry. Emphasis on problem solving
and extensive laboratory work prepare students for the AP examination in
chemistry. A college credit option is also available through the University of
Pittsburgh’s College in High School Chemistry course.
Since this is a college level course taught in high school, it is very demanding, both
in time and effort required. Much of the work involves solving math-type problems.
It is highly recommended that AP Chemistry students be concurrently enrolled in
one of the highest-level mathematics courses available (successful completion of
Algebra II). With the exception of laboratory experiment days, homework will
likely be assigned each day until the final review for the AP Chemistry exam. The
amount of work outside of class depends upon the student; however, students
should be prepared to spend anywhere from 45 minutes to an hour each night after
school on just their AP Chemistry homework. Because class time is limited,
students will be given opportunities to work on certain topics in chemistry over
breaks.
The first semester will cover material from your introductory chemistry course,
but with greater depth and complexity. Most of the material in the second and
third trimester will be new; it is fairly sophisticated and requires a sound
understanding of the earlier material. Learning in science is approached in terms of
unifying concepts and logical reasoning, rather than by memorization.
GOALS AND OBJECTIVES
1. Learning and understanding the factual and conceptual aspects of chemistry,
and developing the ability to handle the complex interactions of chemical systems.
2. Developing analytical and critical skills, problem solving ability and independent
thinking.
3. Learning to communicate with logic and clarity in science.
4. Attaining a degree of competence in the conceptual and practical aspects of
laboratory work.
5. Developing an interest in science and an awareness of its relation to everyday
life.
6. Appreciating the personal challenge and satisfaction of dealing with the unknown
7. Providing an appropriate environment whereby there is a desire to learn and
think, a respect for others and their opinions, a participatory atmosphere and a
commitment to the course.
Overall themes running throughout the course:
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Relationship between cause and effect
Relationship between lab chemistry and chemistry at the atomic or molecular
levels
Problem solving: (integrating information and thinking in chemical terms)
Analysis of known facts and experimental data
Communicating in chemistry
Relevance and application of chemical knowledge
COURSE CONTENT
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Matter & Measurement; Atoms,Molecules, and Ions; Stoichiometry:
Calculations w/Chemical Formulas and Equations
Aqueous Reactions & Solution Stoichiometry
Thermochemistry
Electronic Structure of Atoms
Periodic Properties of Elements; Chemistry of Nonmetals
Basic Concepts of Chemical Bonding
Molecular Geometry: Bonding Theories
Gases
Intermolecular Forces, Liquids, & Solids
Properties of Solutions
Chemical Kinetics
Chemical Equilibrium
Acid-Base Equilibria
Additional Aspects of Aqueous Equilibria
Chemical Thermodynamics
Electrochemistry
Nuclear Chemistry
Coordination Compounds
Chemistry of Life: Organic & Biological Chemistry
GENERAL POLICIES
1. You are expected to be on time for class and to have the required materials
with you. These include a writing implement, a calculator, paper, 3-Ring Notebook,
and the textbook. Repeated lateness is disrespectful and will not be tolerated.
2. You must keep up with the appropriate reading and other homework as an
ongoing responsibility. Class will not be held up for individuals who are not
prepared.
3. Problem questions are assigned for homework as a learning process, not as "plug
and chug" work (if you know what to do when you read a question, it is an exercise,
not a problem). You are expected to be persistent in doing these problems as they
are all within your capabilities (hint: take a short break or do some other homework
and then try again).
4. You are expected to keep useful class notes. This includes recording the steps
of problems worked during class since just working them on your calculator does
not give you any record for subsequent studying and review. All handouts and tests
should be kept in a binder from which they can be retrieved. A separate notebook
is required for labs. Your review for the AP in the spring will be meaningless
without a record of what you’ve done during the year.
5. You should be prepared for labs by reading the handouts ahead of time, and
understanding what you are to do. Interpretation and discussion of data are an
important part of the lab report.
6. Homework must be completed and assignments (notably lab reports) must be
handed in on time at the beginning of class in order to receive full credit. Your
homework is due, by unit, the day after each test. I will allow one day’s lateness
(and its subsequent grade-level deduction); the homework will then receive a zero.
I will periodically check daily homework to see who is keeping up, and thus
contributing to the class. All work handed in for grading (including tests) should be
organized and legible. If I can’t read it, it’s wrong.
7. It is each person's responsibility to make up work promptly after an absence.
You may not have a test postponed for any reason except an excused absence.
8. You are encouraged to discuss the concepts of assigned material (e.g., lab
reports) with each other. However, work which is to be handed in for grading must
be done independently. Each person must be responsible for the integrity and the
understanding of such assignments.
9. You are expected to participate in class, to contribute to discussions, to
respect the right of others to express their opinions, and to promote an
atmosphere conducive to thinking and learning.
10. Try to think independently, but ask when you do not understand or are
confused (if you have done your homework, you are probably not the only person in
the class who is feeling this way). This is particularly important because much of
the material has a pyramid structure which will collapse if the foundation is not
secure.
Required each day in class
 Textbook
 3-Ring Lecture Notebook (2-3”) - Keep Chapter Syllabuses, Handouts,
Classroom Notes, Chapter Outlines, and Completed Tests.
 Notebook paper, Pencil and pen
 Lab Notebook: bound notebook (on laboratory days)
 Calculator: Logarithmic and Scientific Notation functions.
Lab reports: See separate handout on writing formal lab reports. (Students are
required to submit a complete report for each lab experiment, including a
hypothesis, procedure, data and observations, calculations, and a conclusion.) You
will be given specific handouts for individual labs before they are performed. Lab
reports are important and are graded on two criteria. The first is for accuracy and
for fulfilling the stated requirements. The second is for depth in the analysis and
interpretation of data which you collect. There will also be short reports on
demonstrations or mini-labs.
Grading scale:
AP Chemistry will consist of the approximate grade break down:
40% Tests
20% Quizzes
15% Class activities and Homework
25% Laboratory preparation/performance and Write-ups
Participation is taking an active learning role in the classroom. Participation is (but
is not limited to):
 Safe, active participation in laboratory activities (e.g., written data
collection)
 Active participation in classroom discussions, group work, etc.
 Active, on-task, note-taking during lectures
 Active, on-task, reading, writing and production of reports and syntheses
 Active, on-task, completion of homework assignments.
All students are expected to physically and mentally participate in the active roles
of classroom learning citizenship. Attendance is physical and mental participation
during the course of a class period. The instructor reserves the right to arbitrate
participation and attendance for each student. Exceptions may be made for
extenuating circumstances depending upon the situation and the student.
Grades will be based on a point-based system. Letter grades will be issued on the
percentage of total possible points accumulated throughout the semester.
Late/Missing work:
All assignments and projects are to be turned in at the beginning of the class period on
the due date.
It is your responsibility to get your missed assignments. If you miss…
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The day an assignment is due, you’ll be expected to turn that homework in the
day you get back (especially if absence was for a field trip or school activity)
The day the assignment was given out, you will receive one extra day on the due
date
A day or two before the due date, but were present when the assignment was
given, you are expected to turn in the assignment on the original due date
The scheduled due date with an unexcused absence (i.e., you skipped), you lose
25% of the assignment value right off the top. Credit may not be earned for the
work or projects completed during the absence.
It is your responsibility to get your missed quizzes and tests. If you miss…
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The scheduled quiz/test day, you’ll be expected to take the quiz/test the day you
get back (especially if absence was for a field trip or school activity)
A day or two before a quiz/test, but were present for the review you are
expected to take the quiz/test on the scheduled day
The review day, and are back on the scheduled quiz/test day, you must take the
quiz/test the NEXT DAY (day after the scheduled test day)
The scheduled quiz/test day with an unexcused absence, (i.e., you skipped) you
lose 25% of the quiz/test points off the top. Credit may not be earned for the
work or projects completed during the absence.
AP CHEMISTRY COURSE SYLLABUS 2006-2007
AP Chemistry meets every day for 75 minutes for an entire school year; averaging at least two periods
per week for laboratories. Labs are also conducted after school and during the students’ free periods
throughout the week.
All of the experiments below, except where noted with *, will require hands-on work in the laboratory.
The laboratory experience is enhanced by the occasional use of technology via Vernier LabPro, computerinterfaced sensors, Odyssey (Wavefunction) molecular modeling software, and the Virtual Chem Lab. All
students work in pairs and often collaborate with other groups or the entire class when
presenting/discussing data interpretation. However, each student is responsible to complete his or her
own lab write-up, which consists, but is not limited to, a hypothesis, procedure, observations/data,
calculations, and a conclusion.
Chapter tests consist of approximately 15-20 multiple choice questions and approximately 4 to 5 freeresponse questions. The multiple choice and free-response questions come from retired AP released
exams whenever possible. All students have the option to take a “re-test” once they have taken the
initial test. The re-test is another test similar to the first test, but it does not replace the first test.
The re-test gives the student the opportunity to improve, while sharpening their test-taking ability. The
re-test is taken during a student’s free period.
Topics Covered
Description
Chapter
#
Name
Correlation with
School weeks/
Number of
weeks on topic
Assigned
Problems
Laboratory
* Virtual Chem Lab (VCL)
(Woodfield, Asplund, BYU)
companion CD to accompany Brown,
LeMay, and Bursten. All of these
labs are conducted outside of class
by the student
Classifications and
properties of matter, Units
of measurement and
uncertainty in
measurement, Dimensional
Analysis, Molecules and
molecular compounds, Ions
and ionic compounds,
Naming inorganic
compounds and simple
organic compounds,
Empirical formulas,
Quantitative information
from balanced equations,
Limiting reagents and
theoretical yields
General properties of
aqueous solutions,
Precipitation reactions,
Acid-Base reactions,
Oxidation-reduction
reactions, Concentration of
solutions, Solution
stoichiometry
Most of these topics
were learned in the
first-year course, so a
minimal amount of time
will be spent reviewing
and relearning the
fundamental and
important ideas of
chemical formulas and
nomenclature. Students
need to be able to think
holistically about
problem solving using
the fundamental ideas
of the mole and
stoichiometry
1,2,3
Matter &
Measurement;
Atoms,Molecules,
and Ions;
Stoichiometry:
Calculations
w/Chem. Form. &
Eqs.
Week 1-2
1.5 weeks
(Review Summer
Assignment,
given during the
summer)
1.2, 1.4, 1.6,
1.12 through
1.28 evens,
1.30 through
1.40 evens,
1.46, 1.50,
1.56; 2.2,
2.4, 2.6,
2.10, 2.14,
2.16, 2.18,
2.22, 2.30,
2.36, 2.38,
2.42 through
2.64 evens;
3.2 through
3.20 evens,
3.24, 3.28
through 3.36
evens, 3.40,
3.46, 3.48,
3.50, 3.58,
3.60, 3.66,
3.70, 3.72,
3.74, 3.76
Weekly Quizzes on topics covered, Test on Material in Ch. 1,2,3
4.1, 4.4, 4.8,
Lays the foundation for
Aqueous Reactions
4
Week 2-3
4.10, 4.14,
students to successfully
write chemical equations
as well as be able to
understand and apply
later complex
quantitative ideas about
how matter changes in
& Solution
Stoichiometry
1.5 weeks
4.16, 4.18,
4.20, 4.24,
4.26, 4.32,
4.34, 4.40,
4.46, 4.50,
4.52, 4.56,
4.60, 4.64,
4.70, 4.74,
*VCL: 2-5 Names and Formulas of
Ionic Compounds
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Silver One-Pot Demo
(Instructor-led demoShakhashiri),
Solubility Lab:
Determination of the
Formula of Anhydrous
Copper Sulfate
(AP Lab:1,2) (4 lab
4.78, 4.80
terms of unseen atoms
and molecules
Enthalpy, Enthalpies of
Reaction, Calorimetry,
Hess’s Law, Enthalpies of
Formation
Wave nature of light,
Qunatized energy and
photons, line spectra and
the Bohr model, The wave
behavior of matter,
Quantum mechanics and
atomic orbitals,
representations of orbitals,
electron configurations
Thermochemistry lays
the groundwork for
understanding energy as
it relates not only to
chemical reactions and
thermodynamics, but
also to electron
configurations,
periodicity, and chemical
bonding
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Weekly Quizzes on Topics Covered
Thermochemistry
5
Week 4-5
2 weeks
5.2, 5.5,
5.18, 5.22,
5.24, 5.26,
5.28, 5.34,
5.38, 5.46,
5.52, 5.54,
5.58, 5.62,
5.64, 5.68,
5.70, 5.72
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Weekly Quizzes on Topics Covered, Test on Ch. 4,5
6.3, 6.6, 6.7,
Understanding the wave
Electronic
6
Week 6-7
6.10, 6.14,
nature of light and
quantum ideas leads to
an understanding of
atomic structure and
electron configurations
of atoms which, in turn,
leads to a fundamental
understanding of
periodic relationships,
ionic and covalent
bonding, and chemical

Structure of
Atoms
1.5 weeks
6.18, 6.20,
6.24, 6.34,
6.38, 6.46,
6.50, 6.56,
6.60, 6.68,
6.70, 6.74
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periods)
Qualitative Analysis of
Cations and Anions: The 14
Bottle Problem (AP Lab: 14)
(approx.8 lab periods mostly
conducted during student
free periods)
Determining the Mole Ratios
in a Chemical Reaction (1 lab
period)
Determining the Enthalpy of
a Chemical Reaction
(AP Labs 9,13) (1 lab
period)
*VCL: 5-3 Specific Heat of
Aluminum
*VCL: 5-5 Heat of
Combustion: Chicken Fat
*VCL: 6-4 Atomic Emission
Spectra
Odyssey molecular modeling
software
reactivity
Effective nuclear charge,
Sizes of atoms and Ions,
Ionization Energy, Electron
Affinities, Metals,
Nonmetals, and Metalloids,
Group trends for the active
metals and select
nonmetals
Students should be able
to explain the trends in
atomic radius, ionic
radius, ionization
energy, and electron
affinity in terms of the
shielding effect and
effective nuclear
charge as well as explain
the anomalies in the
trends of first
ionization energy and
electron affinity
Chemical bonds, Lewis
symbols, and the Octet
rule, Ionic and Covalent
bonding, Bond polarity and
Electronegativity, Drawing
Lewis structures,
Resonance structures,
Exceptions to the Octet
rule, Strengths of Covalent
bonds
Students should be able
to write both octet and
non-octet Lewis
structures for atoms,
ions, and molecules,
determine bond polarity
from electronegativity
values, draw resonance
structures, correlate
bond multiplicity to
bond length and
strength, and calculate
enthalpies or reactions
from bond dissociation
energies
Weekly Quizzes on Topics Covered
Periodic
7,22
Week 7-8
Properties of
Elements;
Chemistry of
Nonmetals
1.5 weeks
7.10 (b),
7.14, 7.22,
7.24, 7.26,
7.28, 7.34,
7.38, 7.40,
7.46, 7.50,
7.62, 7.64,
7.68, 7.70,
7.73
Weekly Quizzes on Topics Covered, Test on Ch. 6,7
8.4, 8.5, 8.6,
Basic Concepts
8
Week 9-10
8.10, 8.12,
of Chemical
Bonding
1.5 weeks
Weekly Quizzes on Topics Covered
8.14, 8.16,
8.20, 8.22,
8.30. 8.32,
8.36, 8.38,
8.40, 8.50,
8.54, 8.62,
8.66
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Chromatography Lab:
Skittles (AP Lab 18) (2 lab
periods)
*VCL: 7-1 Flame Test for
Metals
Conductimetric Titration
and Gravimetric
Determination of a
Precipitate (AP Lab 16) (3
lab periods)
The VSEPR model,
Molecular shape and bond
polarity, covalent bonds
and orbital overlap, hybrid
orbitals, multiple bonds
The Gas laws, Ideal gas
equation, further
applications of the ideal
gas equation, gas mixtures
and partial pressures,
Kinetic Molecular Theory,
Molecular Effusion and
Diffusion, Real gases:
deviation from Ideal
behavior
Students should be able
to apply the VSEPR
theory to both octet
and non-octet Lewis
structures od ions and
molecules, explain
molecular shape and
bond angles in terms of
both bonding and nonbonding pairs of
electrons, determine
polarity of molecules
and orbital
hybridization from their
geometries, and
distinguish between
sigma and pi bonds
9
Molecular
Geometry:
Bonding
Theories
Week 10-11
1.5 weeks
9.4, 9.5, 9.7,
9.8, 9.12,
9.16, 9.22,
9.24, 9.26,
9.36,9.40,
9.42,9.44,
9.48, 9.50,
9.54,9.60,
9.62, 9.68,
9.70
Weekly Quizzes on Topics Covered, Test on Ch. 8,9
10.18,
The ideal-gas equation is
Gases
10
Week 13-14 10.5,
10.24, 10.32,
yet another way to
calculate moles, which in
turn can be useful in
solving stoichiometry
problems involving gas
densities and molar
mass. Mastering partial
pressures is essential in
understanding kinetics
and equilibrium later in
the course. The kinetic
molecular theory is a
valuable tool in
explaining both the
2 weeks
10.40, 10.48,
10.56, 10.60,
10.66, 10.76
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Model Kits
Odyssey molecular modeling
software
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The Molar mass of a Volatile
Liquid (AP Lab 3) (1 lab
period)
Molar Mass of a Gas (AP
Lab 5) (1 lab period)
*VCL:10-5 Dalton’s Law of
Partial Pressures
*VCL:10-6 Ideal vs Real
Gases
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quantitative and
qualitative macroscopic
behaviors of solids,
liquids, and gases in
terms including
Graham’s law of
effusion.
Intermolecular Forces,
Vapor Pressure, Phase
Diagrams
Weekly Quizzes on Topics Covered, Test on Ch. 10
11.2, 11.3,
Intermolecular forces,
Intermolecular
Week 15
11.5, 11.6,
especially hydrogen
Forces, Liquids, &
11.16, 11.18,
11
1.5 weeks
bonding, explain many
Solids
11.20, 11.26,
11.32, 11.34,
11.38, 11.46,
11.62, 11.72
macroscopic behaviors
of matter in terms of
unseen atoms, ions, and
molecules including
vapor pressure of
liquids, the structure of
ice, and the melting and
boiling points of
substances
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*VCL: 11-1 Heat of Fusion of
Water
*VCL:11-3 The Boiling Point
of Water at High Altitude
Weekly Quizzes on Topics Covered
WEEK 16-17: WINTER BREAK
TAKE HOME WORK: CH. 13 & PRACTICE EXAM
13.7,
Ways of Expressing
In preparation for the
Properties of
 Ice cream Lab (AP Lab 4) (1
13
Week 13.1,
13.8,
13.12,
Concentration, Colligative
critical quantitative
Solutions
lab period)
13.14, 13.20,
16-17
Properties
concepts in the future,
 *VCL: 13-3 Converting
it is imperative to have
a fundamental
understanding of how
solution concentrations
are expressed and
interconverted
mathematically. Vapor
2
weeks
13.24, 13.30,
13.34, 13.40,
13.46, 13.56,
13.64, 13.66,
13.80
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Concentrations to Different
Units
*VCL:13-7 Molar Mass
Determination by Freezing
Point Depression
pressure lowering,
freezing point
depression, and boiling
point elevation are often
used to calculate the
molar mass of
compounds.
Factors that Affect
Reaction Rate, Reaction
Rates, Concentration and
Rate, The Change of
Concentration with Time,
Temperature and Rate,
Reaction Mechanics
The Concept of Equilibrium,
The Equilibrium Constant,
Heterogeneous Equilibria,
Calculating Equilibrium
Constants, Applications of
Equilibrium Constants, Le
Chatelier’s Principle
Weekly Quizzes on Topics Covered, Test on Ch.11, 13
14.12,
A thorough knowledge
Chemical Kinetics
14
Week 14.2,
14.14,
14.20,
of kinetics and its
14.22,
14.26,
18-20
interrelationships is
essential. Students
must be able to
determine a rate law
and its units from
tabular data, use it to
calculate rates and
concentrations under
specified conditions, and
match a suitable
mechanism to a rate law.
3
weeks
14.28, 14.30,
14.32, 14.36,
14.40, 14.44,
14.50, 14.54,
14.56, 14.62,
14.66, 14.68
Weekly Quizzes on Topics Covered, Test on Ch. 14
15.10,
Calculations involving
Chemical
15
Week 15.3,
15.12,
15.14,
gaseous equilibria using
Equilibrium
15.18, 15.20,
21-22
Kc and Kp expressions
and the explanation of
the effects of shifting
equilibria in terms of Le
Chatelier’s principle are
very important ideas to
master in this chapter.
2
weeks
15.22, 15.32,
15.38, 15.42,
15.44, 15.52,
15.54
Weekly Quizzes on Topics Covered, Test on Ch.15
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The Decomposition of
Hydrogen Peroxide (to 1812
overture) (AP Lab 12) (3 lab
periods)
Determining the
Concentration of a Solution:
Beer’s Law (AP Lab 17) (2
lab periods)
The Determination of an
Equilibrium Constant (AP
Lab 10) (2 lab periods)
Bronsted-Lowry Acids and
Bases, The Autoionization
of Water, The pH scale,
Strong Acids and Bases,
Weak Acids, Weak Bases,
Relationship Between Ka
and Kb, Acid-Base
Properties of Salt
Solutions, Acid-Base
Behavior and Chemical
Structure, Lewis Acids and
Bases
The Common Ion Effect,
Buffered Solutions, AcidBase Titrations, Solubility
Equilibria, Factors that
Affect Solubility
It is important to be
able to calculate
quantitative
parameters, especially
pH, of solutions of
strong and weak acids
and bases. Writing and
understanding chemical
equations illustrating
the Bronsted-Lowry
definition of acids and
bases and their
relationships to the Ka
and Kb expressions,
understanding acid-base
hydrolysis of salt
solutions and how the
chemical structure
affects acid-base
behavior are all
important.
16
Acid-Base
Equilibria
Week
23-24
2
weeks
Weekly Quizzes on Topics Covered
WEEK 26:TAKE HOME WORK: CH. 17
Add’l. Aspects of
17
Week
Aqueous
27
Equilibria
Calculations involving
buffer solutions and
solubility equilibria are
very important topics to
master. Students must
also master the
quantitative
relationships that
govern various points
1 week
16.16, 16.20,
16.26, 16.28,
16.38, 16.46,
16.54, 16.56,
16.64, 16.78,
16.84, 16.92,
16.102
17.12, 17.14,
17.20, 17.26,
17.28, 17.32,
17.40, 17.42,
17.48 a & b,
17.50, 17.52,
17.62, 17.64,
17.66
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
Investigating Indicators and
Standardization Lab (AP Lab
11) (2 lab periods)
*VCL: 16-1 Ionization
Constants of Weak Acids
*VCL:16-2 Acid-Base
Classification of Salts
Titration of Orange Juice
(AP LAB 6,7,9) (2 lab
periods)
*VCL: 17-1 Study of AcidBase Titrations-Monoprotic
Acids
during the titrations of
weak acids and bases
and be able to match
suitable indicators to
particular titrations.
Spontaneous Reactions,
Entropy and the Second
Law of Thermodynamics,
The Molecular
Interpretation of Entropy,
Entropy Changes in
Chemical Reactions, Gibbs
Free Energy, Free Energy
and Temperature, Free
Energy and the Equilibrium
Constant
Oxidation-Reduction
Reactions, Balancing
Oxidation-Reduction
Equations, Voltaic Cells,
Cell EMF, Spontaneity of
Redox Reactions, The
Effect of Concentration on
EMF, Electrolysis
Weekly Quizzes on Topics Covered, Test on Ch. 16,17
19.22,
Students must
Chemical
19
Week 19.12,
19.28,
19.38,
recognize, in both a
Thermodynamics
19.48,
19.52,
28-30
qualitative and a
quantitative sense, the
complex relationship
between the spontaneity
of a chemical reaction
and its free energy,
enthalpy, and entropy.
Calculations involving
changes in entropy,
enthalpy, and free
energy and their
relationship to the
equilibrium constant of
a chemical reaction must
be mastered.
2
weeks
2
weeks
*VCL: 19-1 The Balance
Between Enthalpy and
Entropy

Electrochemistry: Voltaic
Cells(AP Lab 20) (1 lab
period)
Electroplating (AP Lab 21) (1
lab period)
An Oxidation-Reduction
Titration: The Reaction of
Fe2+ and Ce4+ (AP Lab 8) (2
19.54,19.60,
19.72, 19.76,
19.80
WEEK 29-30: TAKE HOME WORK: CH. 19 & PRACTICE EXAM
20.14,
Electrochemistry
Students need to
20
Week 20.12,
20.18,
20.20,
understand the concept
20.24,
31-32
of electrochemical cells
and the difference
between voltaic and
electrolytic cells. They
must calculate cell EMF
and quantitatively

20.26,
20.34,
20.40,
20.42,
20.48,
20.52,
20.58,


20.60,
20.64,
20.70,
20.80, 20.86
determine spontaneity.
Calculations using the
Nernst equation relating
cell EMF to
concentrations are
performed as well as
quantitative electrolysis
determinations using
Faraday’s constant,
time, amperage, and
moles of substances.
Radioactivity, Rates of
Radioactive Decay
Weekly Quizzes on Topics Covered, Test on Ch. 19,20
21.14,
Students need to
Nuclear
21
Week 21.12,
21.18,
21.20,
understand the types of
Chemistry
21.28,
21.34,
33
radioactive decay and
how to write and
balance nuclear
equations. A good
application of
quantitative kinetics is
to apply the rates of
radioactive decay to the
calculations based on
half-lives of first order
reactions.
Metal Complexes, Ligands,
Ligands with More than
One Donor Atom; General
Characteristics of Organic
Molecules, Hydrocarbons,
Alkanes, Unsaturated

Students need to know
the general rules for
forming metal
complexes and the
common geometries
exhibited by
1 week
Weekly Quizzes on Topics Covered
Coordination
24,25
Week
Compounds;
34-35
Chemistry of
Life: Organic &
Biological
Chemistry
1.5
lab periods)
*VCL: 20-3 Analysis of a
Ferrous chloride sample
No Labs
21.36, 21.46,
21.58
24.12, 24.14,
25.1, 25.8,
25.14, 25.20,
25.22


The Synthesis and Analysis
of Aspirin (AP Lab 22) (4
lab periods)
The Synthesis and Analysis
of Alum (AP Lab 15) (4 lab
periods)
Hydrocarbons, Functional
Groups: Alcohols and
Ethers
coordination complexes
for different
geometries; Students
need to know how to
name simple
hydrocarbons, alcohols,
and ethers and to
understand structural,
geometrical, and optical
isomers.
week
Weekly Quizzes on Topics Covered, Test on Ch. 21,24,15
AP Chemistry Practice Exam Saturday, May 5th 2007
REVIEW FOR AP CHEMISTRY EXAM
Week
(work problems/practice exams)
35-36
1.5
weeks
AP CHEMISTRY EXAM