Download Goals of the Course:

AP Chemistry Syllabus 2007-2008
Text
Chemistry by Zumdahl and Zumdahl, 6th ed., Houghton Mifflin Company, 2003
ISBN: 0-618-22156-5. In addition, the student will have individual access to the study
guide, software, and solution manual provided y the author.
Other Resources and References
Laboratory Experiments for Advanced Placement Chemistry by Sally Ann
Vonderbrink, 2nd ed., Flinn Scientific Inc., 2006
ISBN 978-1-933709-02-4
Advanced Placement Chemistry with Vernier, 1st ed., by Jack Randall, Vernier Software
and Technology, 2004.
ISBN 1-929075-36-7
The Ultimate Chemical Equations Handbook 1st ed., by George R Hague, Jr. and Jane D
Smith, Flinn Scientific Inc., 2001
ISBN 1-877991-63-5
Student Requirements
Each student is expected to complete required assignments and to seek clarification on
assigned work when necessary. Moreover, each student is responsible for keeping an
individual lab notebook. This notebook serves as documentation of laboratory work.
The lab will be available at least one afternoon per week.
Goals of the Course
Goal 1: The learner will develop abilities necessary to do and understand scientific
inquiry.
1.01 Design, conduct and analyze investigations to answer questions related to
chemistry.
 Identify questions and suggest hypotheses.
 Identify variables including controls
 Select and use appropriate measurement tools.
 Collect and analyze data in tables, charts, and graphs.
 Explain observations and make inferences and predictions.
 Explain the relationship between evidence and explanation.
 Identify how scientists share findings.
1.02 Analyze reports of scientific investigations.
 Select appropriate sample and evaluate adequacy of experimental controls
 Examine the replication of findings.
 Consider alternative interpretations of the data.
1.03 Analyze experimental designs with regard to safety.


Identify potential safety hazards and procedures
Use MSDS to assess chemical hazards.
Goal 2: The learner will develop an understanding of the composition and
properties of matter.
2.01 Analyze the structure of matter at the atomic level.
 Review evidence for the atomic theory.
 Determine atomic masses by chemical and physical means.
 Understand atomic number, mass number and isotopes.
 Understand electron energy levels, atomic spectra, quantum numbers, and atomic
orbitals.
 Review periodic relationships including atomic radii, ionization energy, electron
affinities, electronegativity, oxidation states, and melting points.
2.02 Examine the types and nature of chemical bonds.
 Types: ionic, covalent, metallic, hydrogen bonding, dipole-dipole and London
dispersion forces.
 Relationships to states, structure, and properties of matter.
 Polarity of bonds and electronegativity.
2.03 Analyze the conceptual models of bonding and molecular shapes and their
relationships chemical and physical properties.
 Lewis structures.
 VSEPR.
 Valence bond: hybridization of orbitals, resonance, sigma, and pi bonds.
 Geometry of molecules and ions, structural isomerism of simple organic
molecules and coordination complexes; dipole moments of molecules; relation of
properties to structure.
2.04 Assess the impact of nuclear chemistry
 Nuclear decay equations.
 Half-life and radioactivity.
 Chemical applications.
Goal 3: The learner will build an understanding of the states of matter and the
connection to chemical and physical properties.
3.01 Examine the relationships between pressure, volume, and the temperature of ideal
gases
 Laws of ideal gases: Boyle’s, Charles’
 The ideal gas law and equation
 Partial pressures and Dalton’s Law.
3.02 Analyze kinetic-molecular theory
 Interpretation of ideal gas laws on the basis of this theory.
 Avogadro’s hypothesis and the mole concept.
 Dependence of kinetic energy of molecules on temperature.
 Deviations from ideal gas laws.
3.03 Assess the nature of liquids and solids
 Liquids and solids from the kinetic-molecular viewpoint.
 Phase diagrams of one-component systems.
 Changes of state, including critical points and triple points.
 Structures of solids; lattice energies
3.04 Examine the nature of solutions
 Types of solutions and factors affecting solubility.
 Methods of expressing concentration (The use of normalities is not tested.)
 Raoult’s Law and the colligative properties (nonvolatile solutes); osmosis.
 Non-ideal behavior (qualitative aspects).
Goal 4: The leaner will develop an understanding of chemical reactions.
4.01 Analyze the various types of common chemical reactions
 Acid-base reactions; concepts of Arrhenius, Bronstead-Lowry, and Lewis.
 Coordination complexes; amphoterism
 Precipitation reactions.
 Oxidation- reduction reactions including understanding of oxidation numbers, the
role of the electron in oxidation-reduction, electrolytic and galvanic cells,
Faraday’s laws, standard half-cell potentials, the Nernst equation and prediction
of the direction redox reactions.
4.02 Apply the principle of stoichiometry
 Ionic and molecular species present in chemical systems: net ionic equations.
 Balancing of equations including those for redox reactions.
 Mass and volume relations with emphasis on the mole concept, including
empirical formulas and limiting reactants.
4.03 Analyze systems in dynamic equilibrium
 Concept dynamic equilibrium, both physical and chemical; Le Chatlier’s
principle; equilibrium constants.
 Quantitative treatment for gaseous reactions using Kp and Kc
 Quantitative treatment for reactions in solution Kc
 Quantitative treatment of acids and bases; using Ka and Kb, pKa and pKb
 Quantitative for precipitation reactions and the dissolution of slightly soluble
compounds using the solubility product constant, Ksp.
 Common ion effect: buffers; hydrolysis.
4.04 Analyze chemical kinetics
 Concept of rate of reaction.
 Use of differential rate laws to determine order of reaction and rate constant from
experimental data.
 Effect of temperature change on rates.
 Energy of activation; the role of catalysts.
 The relationship between the rate-determining step and a mechanism.
4.05 Analyze chemical thermodynamics
 State functions.
 First law: change in enthalpy; heat of formation; heat of reaction; Hess’s Law;
heats of vaporization and fusion; calorimetry.
 Second law: entroy; free energy of formation; free energy of reaction; dependence
of change in free energy on enthalpy and entropy changes.

Relationship of change in free energy to equilibrium constants and electrode
potentials.
Goal 5: The learner will build knowledge of descriptive chemistry
5.01 Examine chemical reactivity and predict the products of chemical reactions.
5.02 Analyze the relationships in the periodic table: horizontal, vertical, and diagonal
with examples from alkali metal, alkaline earth metals, halogens, and the first series
of transition elements.
5.03 Explore organic chemistry on an introductory level
 Hydrocarbons and functional groups (structure, nomenclature, chemical
properties).
 Physical and chemical properties of simple organic compounds should also be
included as exemplary material for the study of other areas such as bonding,
equilibrium involving weak acids, kinetics, colligative properties, and
stoichemetric determinations of empirical and molecular formulas.
Table 1: Course Syllabus
Date
8/27/07
9/4/07
9/10/07
9/17/07
9/24/03
10/8/07
10/15/07
10/22/07
10/29/07
11/12/07
11/19/07
12/3/07
12/17/07
1/2/08
1/14/08
1/22/08
2/4/08
2/11/17
2/25/08
3/3/08
3/10/08
3/17/08
3/31/08
4/7/08
4/14/08
4/21/08
Chapter & Subject
Measurements
Atoms, molecules, and ions
Mass Stoichiometry
Solution Stoichiometry
Gases
Thermochemistry
Fun in Lab Week
Atomic Structure and Periodicity
Chemical Bonding
Liquids and Solids
Properties of Solutions
Chemical Kinetics
Catch Up and Review Week
Chemical Equilibrium
Acids and Bases & Aqueous Equilibria
Midterm Exam
Spontaneity, Entropy, and Free Energy
Electrochemistry
Nuclear Chemistry
Cation Analysis Lab
Anion Analysis Lab
Descriptive Chemistry
Writing Equations and Products
Basic Organic Nomenclature
Transition Metals and Coordination
Chemistry
Review Until Exam
Research Projects After Exam
Evaluation
Test 9/7/07
Test 9/21/07
Test 10/5/07
Test 10/15/07
None
Test 10/26/07
Test 11/7/07
Test 11/30/07
Test 12/14/07
Test 1/11/08
Test 2/1/08
Test 2/8/08
Test 2/22/08
Test 2/29/08
Results
Results
Test 3/28/08
Test 4/4/08
Test 4/11/08
Test 4/18/08
Days
5
5
5
6
7
6
5
5
8
6
5
10
3
9
14
1
5
9
5
5
5
5
5
5
5
Chapters
1,2
3,4
5
6
7
8, 9
10,11
12
13
14,15
16
17
18
NA
NA
19,20
NA
22
21
Table II: Lab Syllabus (1.5 hours per period)
Hands-On
Virtual
Hands-On
Virtual
Source (See Lab Manuals)
Hands-On
Virtual
Hands-On
Hands-On
Davidson College WebWare Using spectrophotometers to
determine maximum absorbance and concentration.
Laboratory Experiments for Advanced Placement
Chemistry
Laboratory Experiments for Advanced Placement
Chemistry
Laboratory Experiments for Advanced Placement
Chemistry
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
1
Hands-On
Advanced Placement Chemistry with Vernier
1
Hands-On
Advanced Placement Chemistry with Vernier
1
1
2
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
1
1
!
1
1
Hands-On
Journal of Chemical Education Feb.2007, Vol ,.84, No. 2,
p.318
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
1
1
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
1
45
5
1
1
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
1
1
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
Hands-On
Advanced Placement Chemistry with Vernier
H or V
Student Selected
Week of
Laboratory
Days
8/27/07
1
9/4/07
Review of Basic Laboratory Techniques &
Measurements
Introduction to spectrophotometry
9/10/07
Empirical Formula of a Silver Oxide
1
9/17/07
Analysis of Silver in an Alloy
2
Hands-On
9/24/03
Molar Volume of a Gas
1
Hands-On
10/8/07
10/15/07
Enthalpy of a Reaction
Spectrophotometry: Analysis of Iron in
Spinach
Spectrometry: Difference in Compositions
of Olive Oils
Flame Tests
Emission Spectrum (Ocean Optics)
Determining Mole Ratios
Beer’s Law Concentration
Liquid and Thin Layer Chromatography
1
1
Rate and Order Of a Reaction
Standardizing a Solution of NaOH
Determining an Equilibrium Constant
Acid-Base Titration
Determining KA by the Half Titrations of a
Weak A
Hydration and the % of Water
Electrochemistry: Voltaic Cells &
Electroplating
Buffers
Cation Analysis Lab
Anion Analysis Lab
Oxidation-Reduction Titration
Conductive Titration and Gravimetric
Determination of a Precipitate
Synthesis and Analysis of Aspirin
Determining Ksp of Calcium Hydroxide
Construct Nomenclature Flowcharts for
Organic Compounds, Functional Groups,
and Complex Ions
Research Project
10/22/07
10/22/07
10/29/07
11/12/07
11/19/07
12/3/07
12/17/07
1/2/08
1/14/08
1/22/08
2/4/08
2/11/08
2/25/08
3/3/08
3/10/08
3/17/08
3/31/08
4/7/08
4/14/08
4/21/08
After
Exam
2
15
JCE Chempages Laboratory