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AP Chemistry Syllabus
Office Hours:
2:30 pm until 3:10 pm.
I can occasionally be reached from 7:35 am – 8:00 am
AP Chemistry
AP Chemistry is a course designed to provide you with a good background in a first year
college chemistry course. There will be many times where outside work will be required. You
will need to make arrangements around any extracurricular activities, work, employment, etc.
as needed. Homework and laboratory assignments will be provided in the first week of class.
It is your responsibility to come prepared each day for class. Lectures will be given three days
per week for approximately 1 ½ hours. Two days per week will be spent conducting
laboratories. Classes are on block scheduling for a total of 90 minute classes. Tutoring is
available with scheduling.
Class will be comprised of lecture, lab procedures, occasional practice problems (to reinforce
presented material), group discussion and minimal review. Tests may be given after each unit
has been covered. Quizzes will be given and will be both announced and unannounced. Lab
notebooks and homework will be graded on effort and accuracy.
Students who enter this class should have a good understanding of the following topics:
 Proficient use of the Metric System
 IUPAC Nomenclature
 Names, Charges, and Formulas for Polyatomic Ions
 Gas laws ( KMT, Boyle’s, Charles’, Avogadro’s Laws)
 Stoichiometry and Molar Relationships
 Electronic Structure (i.e. configurations, Lewis structures, electronegativity, VSEPR)
 Nuclear Chemistry
 Solution Chemistry (i.e. pH, pOH, molarity, dilutions and titrations, colligative
properties, Intermolecular and Intramolecular bonding)
 Good laboratory techniques and proper lab notebook format
If you feel you do not have a good understanding of any of these topics please make
arrangements to meet with me privately.
Prerequisites
Chemistry I and II are required with no less than a “C” average in both classes. Your lab
performances from these classes will also be evaluated for consideration of this course.
Interactive Math I and II are prerequisites with no less than a “C” average in either class.
Interactive III is preferred, but arrangements may be made accordingly.
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Required Texts
Chemistry the Central Science, Brown, Lemay, Bursten, Murphy, 11th edition,
Prentice Hall, 2009. ISBN 0-13-601879-3
Chemistry Matter and Change, Buthelezi, Dingrando, Hainen, Wistrom, Zike, McGrawHill,
2008. ISBN 978-0-07-874637-6
Additional texts may be utilized in the school library.
Course Goals

Provide students with the knowledge required to function in a scientific setting in order
to complete laboratories, participate in group settings and work efficiently with others.

Each student will be able to write a college-level laboratory report that includes but is
not limited to the procedure outline, basis for results, chart, graphs, calculations as
necessary, and conclusions.

Students will produce and maintain a professional laboratory notebook and record
pertinent data in an organized manner.

Students will be able to function in a college setting where an instructor’s input is
minimal.

Students will learn to utilize resources such as the Handbook of Chemistry, other
chemistry texts and procedure manuals.

Each student will complete the AP Chemistry Exam in May and be able to make an
acceptable score.
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Laboratory Procedures
Proper laboratory safety and procedures will be discussed at the beginning of
the class. If a student is unable to follow these guidelines, the following will
result:
1st offense – Depending on severity – a warning,
2nd offense – Student will be dismissed from the lab and receive a grade of zero.
Labs will be conducted approximately two days a week. You are allotted one absence from
laboratory experiments without penalty. The next absence will need to be made up before
school on a date predetermined by the instructor.
Laboratory notebooks will be graded once per term. Lab notebooks will be reduced by 50% if
they are late.
Laboratory exercises will require you to work in a group setting. You will not only employ
your lab partner, but the group as a whole. It will require you to collect any pertinent data,
utilize that data as necessary, research any additional material needed, and formally report your
conclusions. All laboratory experiments are hands on. This process will not be one that is
completed in only one day or hour. It may take multiple attempts, days and collaborations with
other lab groups. Laboratory procedures may also require additional information from
references other than your book. You will need to be familiar with the Handbook of
Chemistry. If you have forgotten the skills needed to use this book please see me for
assistance before the day of lab.
There will be a laboratory examination at the end of the course. Students will need to be able
to apply concepts, mathematical data and relationships, and general chemical and laboratory
knowledge in order to succeed on this exam.
IT IS YOUR RESPONSIBILITY TO COME TO LAB DRESSED APPROPRIATELY!
DO NOT ASK TO BORROW, CHANGE, OR CALL HOME FOR CLOTHES!
INAPPROPRIATE DRESS WILL RESULT IN A ZERO!
Grading Scale and Policy
Students will be graded based on the school’s present system. This scale can be found in the
School Policy/Procedures Handbook.
The following content will be evaluated. These percentages are subject to change depending
upon the material covered. Other content may be added and evaluated by the instructor.
30%
20%
20%
15%
15%
Tests
Homework (effort and accuracy)
Lab Notebook (neatness, effort, and calculations/results)
Laboratory Procedures
Quizzes
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Grading Scale and Policy cont’d
Students that score below 70% on tests will need to complete test corrections.
Simply changing the answer will not be sufficient. The student must explain
in a professional manner how they reached the corrected answer. You will need to analyze
what you did wrong and how you resolved the problem. These corrections will be due three
days after receiving the test back from the instructor. Test corrections are MANDATORY, no
exceptions.
Homework is due at the end of each section. We will discuss any problems you had with the
homework before the Unit Test. The problems will be provided the first week of class with the
laboratory experiment outline. If you are aware you will be absent the day homework is due
make sure to turn it in early. Late homework will be reduced by 50%.
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Curriculum Map Coordinated with Understanding By Design
Course: AP Chemistry
# of Weeks
2
1
Unit/Major Topic
Introduction and Review
Gases
Subtopic(s)
Laboratory Safety
Metric Conversions
Atomic Structure and
Models
Nomenclature
Stoichiometry ( Percent
Composition, Limiting
Reactants,
Empirical/Molecular
Formulas)
Net Ionic Equations
General Solution
Chemistry
Boyle's, Charles' and
Avogadro's Law
Ideal Gas Law
Partial Pressures,
Combined Gas Law
Kinetic Molecular Theory
Van der Waals Equation
AP Standards
I. A. Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by chemical and
physical means
3. Atomic number and mass number; isotopes
Laboratory Experiments
II. States of Matter
C. Solutions
2. Methods of expressing concentration (use of
normalities is not tested)
B. Stoichiometry
1. Ionic and molecular species present in chemical
systems: net ionic equations
3. Mass and volume relations with emphasis on the
mole concept, including empirical formulas and
limiting reactants
II. States of Matter
A. Gases
1. Laws of ideal gases
a. Equation of state for an ideal gas
b. Partial pressures
2. Kinetic molecular theory
a. Interpretation of ideal gas laws on the basis of this
theory
b. Avogadro’s hypothesis and the mole concept
c. Dependence of kinetic energy of molecules on
temperature
d. Deviations from ideal gas laws
Using Metric Equipment for
Measurements
Synthesis of Alum
Grahams Law
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# of Weeks
Unit/Major Topic
1
Reactions in Aqueous
Solutions -- Oxidation
and Reduction
2
Thermochemistry
Subtopic(s)
AP Standards
I. Structure of Matter
A. Atomic theory and atomic structure
5. Periodic relationships including, for example,
atomic radii, ionization energies, electron affinities,
oxidation states
Laboratory Experiments
III. Reactions
A. Reaction types
2. Precipitation reactions
3. Oxidation-reduction reactions
a. Oxidation number
b. The role of the electron in oxidation-reduction
Oxidation States
Balancing OxidationReduction Equations
State Functions
Enthalpy
Hess's Law
Heat of Formation and
Reaction
Constant Pressure
Calorimetry
Alternative Fuel Sources
Coal and Our Region
Entropy and Free Energy
Calculating Free Energy
through Enthalpy and
Entropy
B. Stoichiometry
2. Balancing of equations including those for redox
reactions
III. Reactions
E. Thermodynamics
1. State functions
2. First law: change in enthalpy; heat of formation;
heat of reaction; Hess’s law; heats of vaporization
and fusion; calorimetry
3. Second law: entropy; free energy of formation; free
energy of reaction; dependence of change in free
energy on enthalpy and entropy changes
Determining Iron by Redox
Titration
Calorimetry Constants and
Determining Specific Heat
through Calorimetry
Heats of Metal/Acid Reactions
Enthalpy of Sodium Hydroxide
and Hydrochloric Acid
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# of Weeks
2
Unit/Major Topic
Subtopic(s)
Bonding
Quantum Mechanical
Model (VSEPR)
Trends in the Periodic
Table (electronegativity,
ionization, atomic radii)
Lewis Structures &
Electron Configuration
Review
Hybridization of Orbitals
(Atomic & Molecular)
1
Liquids and Solids
Dipole Moments
Van der Waals Forces
Phase Change Diagrams
Solubility Conditions
Ideal Solutions
(Raoult's Law)
Colligative Properties
Osmosis
AP Standards
I. Structure of Matter
A. Atomic theory and atomic structure
4. Electron energy levels: atomic spectra, quantum
numbers, atomic orbitals
Laboratory Experiments
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding,
van der Waals (including London dispersion forces)
c. Polarity of bonds, electronegativities
2. Molecular models
a. Lewis structures
b. Valence bond: hybridization of orbitals, resonance,
sigma and pi bonds
c. VSEPR
3. Geometry of molecules and ions, dipole moments
of molecules
II. States of Matter
B. Liquids and solids
4. Structure of solids; lattice energies
Molecular Structure and Models
I. Structure of Matter
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding,
van der Waals (including London dispersion forces)
b. Relationships to states, structure, and properties of
matter
II. States of Matter
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular
viewpoint
2. Phase diagrams of one-component systems
3. Changes of state, including critical points and triple
points
C. Solutions
3. Raoult’s law and colligative properties (nonvolatile
solutes); osmosis
Molecular Mass by Freezing
4. Nonideal behavior (qualitative aspects)
Point Determination
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# of Weeks
1
Unit/Major Topic
Subtopic(s)
Kinetics
Reaction Rates and Laws
Mechanisms
Homogeneous and
Heterogeneous Catalysts
1
1
1
Equilibrium
Electrochemistry
Equilibrium Constants
Calculating Equilibrium
Positions and Solving
Problems
Brief Review of Oxidation
Reduction
Galvanic Cells
Reduction Potentials
Nernst Equation and
Faraday's Laws
Batteries
AP Standards
III. Reactions
D. Kinetics
1. Concept of rate of reaction
2. Use of experimental data and graphical analysis to
determine reactant order, rate constants, and reaction
rate laws
3. Effect of temperature change on rates
4. Energy of activation; the role of catalysts
5. The relationship between the rate-determining step
and a mechanism
II. States of Matter
C. Solutions
1. Types of solutions and factors affecting solubility
III. Reactions
C. Equilibrium
1. Concept of dynamic equilibrium, physical and
chemical; Le Chatelier’s principle; equilibrium
constants
III. Reactions
3. Oxidation-reduction reactions
c. Electrochemistry: electrolytic and galvanic cells;
Faraday’s laws; standard half-cell potentials; Nernst
equation; prediction of the direction of redox
reactions
E. Thermodynamics
4. Relationship of change in free energy to
equilibrium constants and electrode potentials
Laboratory Experiments
Clock Reaction
Determination of Equilibrium
Constant for the Formation of
FeSCN
Electrode Potential Lab
I. Structure of Matter
B. Chemical bonding
1. Binding forces
b. Relationships to states, structure, and properties of
matter
Representative and
Transition Metals
Group Presentation Project
Coordination Compounds
Naming and Bonding in
Coordination Compounds
3. Geometry of molecules and ions, structural
isomerism of simple organic molecules and
coordination complexes;; relation
of properties to structure
Qualitative Analysis of Cations
and Anions
Qualitative Determinations
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# of Weeks
1
1
Unit/Major Topic
Organic Chemistry
Test Review
Subtopic(s)
Review Nomenclature of
Hydrocarbons and
Functional Groups
Isomers
Enantiomers
Addition Reactions
Review Test Format
Practice Test Questions for
Essay Questions
AP Standards
I. Structure of Matter
B. Chemical bonding
3. Geometry of molecules and ions, structural
isomerism of simple organic molecules and
coordination complexes; relation of properties to
structure
Laboratory Experiments
Synthesis of Esters
Optional Weekend Review
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This is to certify that I have read the syllabus and am aware of the laboratory policy, grading
policy and course fees. This is also to certify that my parent/guardian has read the course
syllabus and is aware of the instructor's phone number, office hours, e-mail address, laboratory
policy, grading policy and course fees.
Parents/Guardians please feel free to contact me at any time about concerns.
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Student
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