Fairfax Senior High School
C. Arkenberg
2015-16
AP CHEMISTRY COURSE SYLLABUS
COURSE DESCRIPTION
This AP Chemistry course is designed to be the equivalent of the general chemistry
course usually taken during the first year of college. For some students, the course will
enable one to undertake, as a freshman, second year work in the chemistry sequence
at your chosen institution or to register in courses in other fields where general
chemistry is a prerequisite. This course is structured around the six big ideas articulated
in the AP Chemistry curriculum framework provided by the College Board [CR2]. A
special emphasis is placed on seven science practices, which capture important
aspects of the work that scientists engage in, with learning objectives that combine
content with inquiry and reasoning skills.
This AP Chemistry course is geared toward preparation for the Advanced Placement
Exam in Chemistry. Passing the AP exam shows mastery of the equivalent of one year
of college-level general chemistry and as such can count for college credit. AP
Chemistry is open to all students that have completed a year of chemistry who wish to
take part in a rigorous and academically challenging course.
(Exceptions can be made in extenuating cases)
COURSE STRUCTURE
BIG IDEAS
Big Idea 1: Structure of Matter
Big Idea 2: Properties of matter-characteristics, states and forces of attraction
Big Idea 3: Chemical reactions
Big Idea 4: Rates of chemical reactions
Big Idea 5: Thermodynamics
Big Idea 6: Equilibrium
SCIENCE PRACTICES
Science Practice 1: The student can use representations and models to communicate
scientific phenomena and solve scientific problems. Science Practice 2: The student can use mathematics properly.
Science Practice 3: The student can engage in scientific questioning to extend thinking
or to guide investigations within the context of the AP course.
Science Practice 4: The student can plan and implement data collection strategies in
relation to a particular scientific question.
Science Practice 5: The student can perform data analysis and evaluation of evidence.
Science Practice 6: The student can work with scientific practices and theories.
Science Practice 7: The student is able to connect and relate knowledge across
various scales.
TEXTBOOK, LABORATORY MANUAL, AND STUDY GUIDES
Primary Textbook:
Zumdahl, Steven S., et. al., Chemistry, 7th Edition. Boston, New York, Houghton Mifflin
Company, 2007. [CR1]
Other Course Materials:
The College Board. AP Chemistry Guided Inquiry Experiments: Applying the Science
Practices. 2013.
Moog, Richard S., and Farrell, John J., Chemistry A Guided Inquiry, 5th Edition, John
Wiley and Sons, Inc., 2011.
Shakashiri, Bassam and Rodney Schreiner, Workbook for General Chemistry, 3rd
Edition, Madison, Wisconsin, Stipes Publishing, 2004.
Zumdahl, Stephen and Susan Zumdahl, Fast Track to a Five, Evanston, IL, Houghton
Mifflin Company, 2006.
READING AND ASSIGNMENTS
Daily reading and homework assignments will be given. Students are expected to read
all new material prior to coverage in the classroom. Students are responsible for all
material covered in reading (even if not discussed in class). Make sure to keep up with
all readings, we move very quickly and it is easy to fall behind. To be successful in this
AP Chemistry class, students will have to spend at least five hours a week studying
outside of class. ASSIGNMENTS-QUIZZES-EXAMS
Problem-sets from each chapter of the textbook will be assigned. Students have
approximately one week to complete these problem sets. In addition, daily problem
sets will be given. These assignments are due at the beginning of class on the
following day. We will have at least one to two quizzes per week. An exam will be
given at the end of each unit. Quiz and exam questions are frequently taken from
released AP Chemistry exams. A comprehensive exam is given at the end of each
semester and reflects questions like students will see on the AP Exam. If absent, it is
your responsibility to make-up all missed assignments.
LABORATORIES
We will carry out approximately two hands-on labs per month. Each experiment will take
about 1-3 hours to complete. You will work with a lab partner and will be in groups of
four. In each lab you will collect data, and complete a lab report. The lab report
including calculations, results, graphs (using EXCEL or graph paper), and conclusions
will be due two days after completing of the experiment. Specific requirements for each
lab report will be indicated. Fifty percent of the labs will be teacher guided while the
other fifty percent will be self- guided. Because of the length of time required to conduct
each experiment, some labs may be held on Saturday sessions from 9am-12noon.
You must maintain a composition book to record your observations and data. Please
note all lab reports will be typed. (See laboratory format and procedures)
CLASS NOTEBOOK
You are required to maintain a three subject notebook containing all class notes, warmups, class assignments, tables, released AP exams etc…(See notebook guidelines)
TUTORING
Tutoring can be provided after school on Monday, Wednesday and every other Friday.
Make sure to let me know a day ahead of time so that arrangements can be made.
GRADES
Grades will be based on the following percentages:
Exams
50%
Quizzes
5%
Labs and Notebook
25%
Final Exam
20%
GRADING SCALE
A = 90-100 %
B = 80-89%
C = 70-79%
D = 60-69%
F = 59 - 0%
WEBSITE
http://www.fairfaxhs.org/apps/pages/index.jsp?uREC_ID=60609&type=u
Class calendar, assignments, handouts, and announcements will
periodically be posted.
Engrade
All grades will be accessible on the Engrade website (www.engrade.com)
Please see me for your login code.
First Semester: AP Chemistry A
Week
1,2
2,3
Chapter
1
1,2
4
2
5
3
TOPICS
Chemical Foundations
Mathematics review
Units of Measurement
Uncertainty in Measurement
Scientific Notation
Significant Figures
Solving Equations
Dimensional Analysis
Density
Laboratory Safety
Scientific Method
Classification of Matter
Reading: p. 1-30
Problem Set: 16, 18, 20, 24, 26, 28, 30, 34,
36, 38, 40, 42, 46, 50, 52, 56, 59, 60, 64, 66,
70, 75
Experiments
Lab#1
Metric Measurement
Atoms, Molecules, and Ions
Elements & Compounds
Chemical and Physical Properties
Atomic Theory & Dalton
Rutherford’s Gold Foil Experiment
Subatomic particles
Modern Atom
Isotopes
The Periodic Table
Nomenclature
Reading: p. 39-69
Problem Set: 16, 18, 20, 24, 26, 30, 32, 34,
38, 40, 42, 44, 46, 48, 50, 52, 54, 56, 60, 62,
64, 70, 72, 74, 77, 82
Lab#3
Paper Chromatography
Compounds and Molecules
Ionic compounds
Molecular Compounds
Naming Acids
Nomenclature
Stoichiometry
Chemical Equations
Balancing Equations
Reaction Types
Product Prediction
Lab#4
Synthesis of an Ionic
Compound-MgO
Lab#2
Density Determination
Optional Labs:
Ion Chromatography
Fractional Distillation
Lab#3a
Turning a penny to "Gold"
Optional Labs:
Determination of
Avogadro’s Number
Lab#5
Chemical Reactions"Reaction Action" 6 Types
of Reactions
Reading: p. 77-115
Problem Set: 24, 26, 28, 30, 36, 38, 40, 50,
52, 54, 58, 62, 65, 70, 72, 74, 76, 80, 82, 84,
90, 94, 98, 104, 106
Optional Labs:
Determination for the
Formula of a Compound
Finding the Ratio of the
Moles of a Reactant of a
Compound
Chemical Reactions of
Copper and Percent Yield
51
3
6
3
7
4
Molecular Weight
The MOLE
Mole Conversions
Empirical/Molecular formulas, Percent
Composition
Mole-Mole Stoichiometry
Mass-Mass, Mixed Stoichiometry
Limiting Reactants
Percent Yield
Types of Chemical Reactions and
Solution Stoichiometry
Electrolytes and non-electrolytes
Precipitation reactions and Solubility rules
Acid-Base reactions and salt formation
Combustion reactions
Decomposition reactions
Addition Reactions
Single & Double replacement reactions
Reading: p. 127-170
Problem Set: 10, 12, 16, 18, 20, 22, 24, 26,
30, 32, 36, 38, 40, 44, 48, 52, 56, 58, 62, 64,
66, 68, 74, 76, 80, 81
Lab#6
Percent of H2O in popcorn
Percent of CO2 in NaHCO3
Lab#7
Empirical Formula of a
hydrate-MgSO4XH2O
Lab#8
Limiting Reactants"Balloons"
Lab#9
%Yield of NaCl
Lab#10
Activity Series Lab (Metals
and Halogens)
Optional Labs:
Use of a Primary Standard
KHC8H4O4
Reduction of
Permanganate
8
4
9
5
Oxidation-Reduction Reactions (REDOX)
Activity Series
Molarity and Normality
Solution Stoichiometry
Titrations
Redox titrations
Gravimetric calculations
Gases
Pressure, Temperature, STP
Molar Volume of Gases
Progressive Precipitation
Lab#11
Acid-Base Titration:
Determination of Acid
Concentration
Lab#12
Boyle's Law
Using Pasco Xplorer
Boyle’s Law, Charles’ Law,
Combined Gas Law
Ideal Gas Law & real gases
Gas Density & Molecular Weight
Dalton’s Law
Kinetic Molecular Theory
Gas Stoichiometry
Graham’s Law of Effusion
10
Lab#13
Determination of the Molar
Mass of a Gas
Optional Labs:
Investigating Graham’s
Law
Ideal Gas Lab
The Determination of Molar
Mass of a Volatile Liquid
Reading: p. 179-216
Problem Set: 20, 24, 28, 31, 32, 34, 42, 44,
46, 52, 58, 60, 62, 67, 70, 72, 74, 76, 80, 82,
86, 88, 97, 99
11
6
Thermochemistry
Energy
Work & Heat
Internal Energy
Potential & Kinetic Energies
1st Law of Thermodynamics
Exothermic & Endothermic Reactions
Calorimetry, Heat Capacity & Specific Heat
Enthalpy
Optional Labs:
Hess’s Law
Heat of Combustion of
Magnesium
Reading: p. 229-265
Problem Set: 10, 12, 19, 22, 26, 28, 32, 34, 36,
38, 42, 46, 50, 52, 56, 58, 62, 64, 68, 79, 82
12
6
13
7
Heat of Reaction
Hess’s Law
Heat of Formation/Combustion
Bond Energies
Atomic Structure and Periodicity
Electromagnetic Radiation c =  , E = h
Photons
Bohr’s Model
Atomic Spectra of Hydrogen
Reading: p. 275-320
Problem Set: 18, 20, 22, 24, 26, 30, 32, 34,
38, 40, 42, 46, 55, 58, 62, 66, 68, 70, 74, 78,
81, 84, 86, 92, 104,112
Lab#14
Calorimetry-Heat of
Reaction
Lab#15
Flame Test
Optional Labs:
Relationship Between the
Spectrum and Absorbance
of Light
Periodic Table Dry Lab
14
7
Orbitals
Electron Configuration-Aufbau Principle
Orbital Diagrams
Lab#16
Qualitative Analysis Lab
Quantum Mechanics-Quantum Numbers
15
7
16
8
17
9
Periodic Properties
Periodic Trends
Atomic Radii
Ionization Energy
Electron Affinity
Metals and Nonmetals
Group Trends
PES (Photoelectron Spectroscopy)
Bonding: General Concept
Ionic, Covalent, Metallic
Ion Size
Lewis Structure
Multiple Bonds-Sigma and Pi
Electronegativity, Resonance, Octet Rule
Reading: p. 329-381
Problem Set: 14, 16, 18, 20, 22, 28, 32, 36,
38, 42, 46, 48, 52, 54, 56, 64, 66, 68, 70, 74,
75, 77, 80, 86, 90, 92, 96,103
Lab#16 Part 2
Qualitative Analysis Lab
Covalent Bonding: Orbitals
VSEPR
Hybrid Orbitals
Reading: p. 391-417
Problem Set: 8, 10, 14, 16, 24, 26, 30, 34,
36, 38, 42, 44, 50, 52, 56
Lab#17
Molecular Model Building
PhET Simulation
Optional Labs:
Determination of the
Formula of a Hydrate
Optional Labs:
Conductivity of Solids &
Metals
Atomic Theory Dry Lab
18
10
Liquids and Solids
Ion-dipole forces, dipole-dipole, London
dispersion, Hydrogen bonding
Phase Changes
Viscosity, surface tension
Vapor Pressure
Phase Diagrams
Reading: p. 425-574
Problem Set: 16, 20, 28, 32, 34, 36, 38, 39,
42, 44, 48, 50, 52, 54, 60, 62, 64, 72, 80, 82,
84, 86, 88, 89, 90, 92
Optional Labs:
The Structure of Crystals
Enthalpy of Vaporization of
Water
Liquid Dry Ice Activity
WINTER BREAK
Second Semester: AP Chemistry B
19
10
20
11
21
12
22
12
23
13
Heating-cooling curves
Solids-crystalline, amorphous
Molecular, covalent network and
Ionic solids
Properties of Solutions
Composition of Solutions
Colloids and Suspensions
Separation techniques
Effects on biological systems
Reading: p. 485-518
Problem Set: 12, 14, 16, 22, 24, 26, 28, 30,
32, 36, 40, 44, 46, 48, 52, 54, 58, 60, 64, 70,
74, 76, 78, 80, 84, 85, 89
Lab#18
Beer’s Law Lab
Chemical Kinetics
Reaction rate
Reaction pathways
Factors affecting reaction rates
Concentration and Rate Laws/Equation
1st and 2nd order rate laws
Integrated rate laws
Reading: p. 527-566
Problem Set: 10, 12, 16, 20, 24, 26, 28, 29,
31, 33, 35, 37, 41, 43, 47, 49, 51, 53, 55, 59,
63, 65, 67
Lab#19
Reaction Rate-"Iodine
Clock Reaction" rate and
concentration
Temperature and rate -Arrhenius Equation
Collision model-Activation energy
Boltzmann distribution
Reaction mechanisms
Catalysis
Chemical Equilibrium
Characteristics and conditions of
equilibrium
Equilibrium constant/expression
Factors affecting equilibrium
Equilibrium constant
Calculating Keq, Kp
Reading: p. 578-612
Problem Set: 13, 17, 18, 20, 22, 26, 28, 30,
32, 36, 38, 40, 44, 46, 48, 54, 58, 64, 67,74
Lab#20
Reaction Rate and
Temperature
Optional Labs:
Freezing Point Depression
Optional Labs:
Rate Law Determination:
Crystal Violet Reaction
Lab#21
Straw Lab
Optional Labs:
Equilibrium of Ethyl
Acetate
24
13
25
14
“ICE” calculations
LeChâtelier's Principle
Effect of catalysis
Acids and Bases
Acid and Bases structure
Arrhenius, Brönsted-Lowry, Lewis
Conjugate acid-base pairs
pH scale
pH of strong and weak acids and bases
pH of salts
Polyprotic acids
Kw
Reading: p. 623-672
Problem Set: 17, 25, 28, 30, 32, 34, 38, 40,
42, 44, 52, 60, 64, 66, 70, 72, 76, 78, 84, 88,
98, 102, 104, 114, 116, 118, 122,124
Lab#22
LeChatelier's Principle
Java Activity
Lab#23
pH-Acid Base Titration
Curve
Optional Labs:
Determination of
Dissociation Constant of
Weak Acids
Hydrolysis of Salts
Determination of Vitamin C
and Aspirin Content
25
15
Application of Aqueous Equilibria
Ka, Kb
Common Ion effect
Buffers
Acid-Base titrations, titration curves
Acid Base indicators
Solubility Product, Ksp
Reading: p. 681-739
Problem Set: 22, 24, 26, 32, 40, 44, 46, 48,
52, 56, 57, 62, 66, 70, 76, 80, 86, 92, 94, 98,
100, 104, 108,112
Lab#24
Determination of Ka
Lab#25
Preparation of a buffer
Optional Labs:
Acid-Base Titration
Titration of a Diprotic Acid
Titration Curves of Strong
and Weak Acids and
Bases
Determination of a
Solubility Product Constant
26-27
16
Spontaneity, Entropy, and Free Energy
Entropy and Enthalpy
Spontaneous processes
Second law of thermodynamics
Gibb's free energy G = H - TS
Free energy and temperature
Free energy and equilibrium G = -RTlnK
Rate and Spontaneity
Reading: p. 749-782
Problem Set: 18, 20, 21, 24, 26, 28, 30, 32,
34, 36, 38, 44, 46, 48, 49, 54, 58, 60, 62,70
28-29
17
Electrochemistry
Redox reactions, balancing redox reactions
Voltaic cells
Calculating EMF
Nernst Equation
Electrolysis
Reading: p. 791-829
Problem Set: 17, 21, 26, 28, 30, 32, 36, 39,
50, 56, 58, 59, 64, 72, 76, 80, 84, 86, 88, 92,
95
Optional Labs:
Determination of Soluble
Chloride
Percentage Calcium in
Calcium Supplements
Lab#26
Redox reactionDetermination of oxalate
Lab#27
Electrochemistry-Making a
battery
Lab#28
Electrolysis of water
Optional Labs:
Chemical Activity Series
Corrosion
Electroplating
Electrochemical Cells
30
31
18
19
The Nucleus: A Chemist’s View
Nuclear equations
Types of Radioactive decay
Kinetics of Radioactive decay
Radioactivity uses
Nuclear transformation
Half-life
Thermodynamic Stability of the nucleus
Fission and Fusion
Reactors
Effects of Radiation
Lab#30
Cadmium ½ Life Lab
Reading: p. 841-868
Problem Set: 12, 14, 15,17, 20, 21, 23, 24,
25, 27, 28, 31, 33, 36, 38, 41, 42, 44, 45, 47,
50, 51, 52, 53, 57, 58, 61, 62, 66, 70
The Representative Elements: Groups 1A Optional Labs:
Through 4A
Using Conductivity to Find
Representative Elements
an Equivalence Point
Properties
Reading: p. 875-895
Problem Set: 2, 8, 10, 16, 18, 19, 22, 24, 26,
28, 30, 32, 34, 36, 39, 42, 44, 46, 48, 51, 53,
56, 57, 62
31
20
The Representative Elements: Groups 5A
Through 8A
Properties
Optional Labs:
Percent Sulfate in a
Mixture
Reading: p. 901-935
Problem Set: 2, 6, 8, 10, 12, 14, 16, 18, 20,
22, 23, 25, 28, 29, 32, 33, 38, 46
32
21
33
22
Transitional Metals and Coordination
Chemistry
Coordination Complexes
Transitional Metal properties
Nomenclature
Crystals and Metallurgy
Reading: p. 943-989
Problem Set: 1, 3, 4, 5, 7, 9, 11, 13, 15, 17,
19, 21, 22, 23, 24, 25, 27, 29, 31, 34, 37, 38,
41, 43, 45, 49, 51, 55, 57,61, 66, 71
Organic and Biological Molecules
Hydrocarbons
Alkanes, Alkenes, Alkynes
Polymers
Nomenclature
Reading: p. 997-1044
Problem Set: 13, 17, 19, 21, 22, 26, 27, 32,
33, 34, 35, 40, 41, 47,49, 51, 54, 57, 59, 63,
67, 69, 72, 75, 79, 81, 83, 87, 91, 95, 97, 99,
32-34
AP Test Preparation
Lab#30 Practical
To Be Announced
Optional Labs:
The Green Crystal Lab
Reading: AP Chemistry Preparation and
Method
Problem Set: 3 AP Style Review Exams + 1
Mock AP Chemistry Exam
!!!!! AP Chemistry Exam Tuesday 8:00 am May 2nd 2016 !!!!!
35-36
22
Organic and Biological Molecules
Hydrocarbons: Alkanes, Alkenes, Alkynes,
Hydrocarbon Derivatives:
Alcohols, Aldehydes, Ketones, Carboxylic
Acids, Esters, and Amines
Polymers:
Proteins
Carbohydrates
Nucleic acids
Lab#31
Synthesis of esters
Lab#32
Synthesis of Aspirin
Lab#33
Purification of Caffeine