AP Chemistry 2007-2008
Instructor:
Room:
Phone /E-mail:
Mr. Paul Birkenfeld
324
662-2509 / paulb@cksd.wednet.edu
Course Overview: A.P. Chemistry a college level course, which requires students to put forth their best effort on a daily basis, both
in and out of class. In this course, the student will cover a complete exploration of chemistry with emphasis on: matter and
measurement; atoms and elements; molecules-ions-compounds and their nomenclature; stoichiometry; electron configurations and
periodic trends; atomic models and molecular structures; bonding and intermolecular forces; properties of gases, liquids, solids and
solutions; chemical kinetics; chemical equilibrium; chemical thermodynamics (free-energy, enthalpy and entropy); electrochemistry;
nuclear chemistry and descriptive chemistry of the elements, including some organic chemistry. Chapters 1-21 and 23 of Kotz &
Treichel’s Chemistry and Chemical Reactivity (Fifth Edition) encompasses the entire course of study. The use of mathematics as a
tool in problem solving and in derivations is expected to play a dominate role in the course. Time spent outside of class on textbook
problems, reading, formal laboratory write-ups, advanced placement problem sets, and studying is typical for a student enrolled in the
course. The hands-on laboratory component of this course is essential in the student’s understanding of the concepts and
applications of chemistry; at least one question on the A.P. Exam focuses on the laboratory experience.
Students are encouraged from the first day of class to form a study group to work with in and out of class – student success is
improved through cooperative study groups!
Course Goals (abbreviated from 2006-2007 College Board AP Physics Course Description):
Students should…
 Read, understand, and interpret chemical and physical information and problems
 Use the scientific method to analyze particular chemical and physical phenomenon or problem.
 Use basic mathematical reasoning in a chemical or physical situation or problem
 Design and perform hands-on experiments, interpret the results of observations and communicate including uncertainty
assessment
Text books and Materials:
Chemistry and Chemical Reactivity -Fifth Edition, by John C Kotz and Paul M. Treichel Jr. (© 2003.
Thompson Learning, Inc.)
A scientific calculator and three ring binder with dividers is mandatory. It is required that students keep (in a neat and organized
fashion) all materials collected throughout the semester: Syllabus, Notes, Homework, AP Problem Sets, Laboratories (Portfolio of
Completed Formal Lab Write-ups), Quizzes, Exams, Final Exam. These will be kept in a three ring binder. These may or may not be
graded for organization and completeness at any time (announced or unannounced) throughout the school year.
Grading Policy:
 Quizzes
 Tests
 Labs and Problem Sets
Overall percentages:
93% - 100% = A
90% - 92% = A85% - 89% = B+
80% - 84% = B
40 %
40 %
20 %
75% - 79% = B70% - 74% = C+
63% - 69% = C
60% - 62% = C-
55% - 59% = D+
50% - 54% = D
0% - 49% = F
Class Website: All the materials for the course can be downloaded from the website. It is your responsibility to visit the site to get
materials as they are needed. You are required to visit regularly.
http://www-ckhs.cksd.wednet.edu/Mr%20b%20Web%20Page/HOME.htm
Course Notes: Notes be available on-line from the class website. Course notes amplify the content of the whole course. The notes are
vitally important to students as they form a permanent, hard copy record that summarizes of all the knowledge and understanding that
students will need to acquire in order to perform well on the AP Chemistry Examination. These objectives and notes should be
downloaded, printed, and ready for use at the start of each unit. Each set of notes should be completed in class and annotated however
the student sees fit. They should be used as the basis for continual study. Failure to do this may make it hard for a student to keep
pace with the lecture/notes being reviewed in class.
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Assignments/AP Problem Sets: Reading from the textbook, reviewing notes, and taking advantage of outside resources is highly
recommended. Although most problems are found within the notes, textbook problems/questions may be assigned up to two or three
times a week consisting of about five problems that may or may not graded. It is imperative that you take your daily class
assignments seriously so that you can get the most out of the lecture in the next arranged class meeting. A.P. Problem Sets, which will
be graded, are generally assigned over a weekend and/or at the end of a unit. All problems (whether multiple choice or free-response)
involving calculations must have work shown completely. For essay or short answer questions, answer questions in complete
sentences. It is the student’s responsibility to ask questions about homework, problem sets, or other information they don’t
understand.
Laboratories: Hands-on Labs will be performed in class, requiring advanced reading, and followed up by a formal lab write-up. Our
lab write-up will be similar to what is required by Washington State University Physics students (See Appendix A). All labs must be
typed and strictly adhere to the model provided to receive full credit. A portfolio of the completed labs must be retained by each
student. Missed laboratories must be made-up the Friday of the week that the laboratory was missed. It is the students
responsibility to arrange this with the instructor.
Quizzes: Quizzes can consist of both multiple choice and free-response like questions. Most quizzes last a full class period, usually
given on a Friday, and being returned on Monday. I might try short daily quizzes, rather than weekly quizzes, in an attempt to
improve student learning. Quizzes may contain extra points (extra credit), and are directed at the concepts and basic knowledge over
newly learned material, where as, tests involve multiple concepts, and will include previously tested material in their questions.
Missed quizzes must be made up before the next class meeting, best if done in the library before school. If a prolonged absence
of more than two days takes place, arrangements will be made on a student to student determination by the instructor, on how
the missed quiz will be handled.
Classroom Expectations:
Attendance, punctuality, courtesy and good behavior of the highest levels are expected at all times whether in lecture or laboratory.
Laboratory safety is always of paramount importance. Your exemplary behavior and observance of safety procedures is required at all
times (or you may lose lab privileges).
Students are asked to…
- give the instructor their undivided attention
- respect the right of other students to study and work in
peace.
- come to class on time, prepared to do class work, and/or
participate in class discussions.
- handle all chemicals and lab materials in a safe manner.
- handle all equipment with care and returned to where it came
from.
- follow all instructions provided at the start of a laboratory
- respect others and their property.
- not bring any food or drink (including water) into the classroom.
- sign-out of class and pick-up the hall pass prior to leaving the
classroom”
- follow the “nice or neutral” policy when interacting with others.
Furthermore…
Absolutely no form of cheating will be tolerated (copying work, allowing work to be copied, copying exams or quizzes, allowing
exams or quizzes to be copied, plagiarism, etc…).
The Consequences…
1st occurrence : A warning
2nd occurrence : Conference with instructor after class
3rd occurrence : 30 minute after school detention (with
instructor), referral to a counselor, and parental
contact
4th occurrence : Removal from classroom, Referral to Assistant
Principal’s office, and parent conference.
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Late Work Policy: An assignment or any activity (lab, worksheet, etc…) is considered late if it is not ready to be turned in by the
start of class on its due date. Ready to be turned in means stapled and easily accessible. Late work is accepted for up to ½ credit if
one day late and is not accepted after that except under extreme circumstances with teacher permission. Due to the pace of this
course, material will be covered daily that builds upon material from the day before and leads into material that will be covered the
following day. If you are to keep up with the material it is imperative that you attend class daily. If you miss a class(es) it is your
responsibility to determine what you missed and complete and submit the missed work. Students found to be truant on the day of a
quiz, the day an assignment is due, the day a lab was due or performed, or the day any other work was due or performed will receive a
0 for that work. Any student that accrues more than 10 absences (excused or unexcused) per semester may lose the opportunity to
complete any make-up work. A decision of whether or not to provide make-up work lies solely with the instructor.
Book Check-out/Check-in Procedure:
If you have a text book issued to you, that book becomes your responsibility while you remain enrolled in the course. You are not to
mark, write in or damage the text in any fashion. At the time it is issued you will be asked to record the books number and its
condition. It is imperative that you record the specific condition of the book at the time of issuance to avoid a fine when you return
the book. Books must be turned in to me at the end of the school year OR when you terminate your enrollment in the course
or you will be fined according to the fines below.
Replacement of Text Book...
Book Re-binding...
$120.00
$ 20.00
**Getting Extra-Help / Tutoring:
Each weekday 7:00—7:45 AM (by appointment) OR Monday – Thursday from 3:30 – 5:00 PM in the CKHS Library.
Examinations: Below is a tentative listing of exams taken in the first and second semester.
First Semester (18 weeks)
Unit One Exam
Lab Equipment, Procedures and Safety
Unit Two Exam
Chapters 1-3
Matter, Measurement, Atoms, Elements,
and Compounds
Unit Three Exam
Chapters 4-6
Stoichiometry, Reaction Prediction,
and Thermochemistry (Enthalpy)
Unit Four Exam
Chapters 7-8
Atomic Structure, Electron Configurations,
and Periodicity
Unit Five Exam
Chapters 9-10 & 13
Bonding and Intermolecular Forces
Unit Six Exam
Chapters 12-14
Solids, Liquids, Gases, Solutions and
Phase Diagrams
FINAL EXAM
CHAPTERS 1-14 (EXCLUDING CHAPTER 11)
Second Semester (14 weeks)
Unit Seven Exam
Chapters 15-16
Chemical Kinetics and Equilibrium I
Unit Eight Exam
Chapters 19-20
Thermodynamics (Enthalpy, Entropy, and Free
Energy) and Electrochemistry
Unit Nine Exam
Chapter 17-18
Equilibrium II: Acids, Bases, Salts, Buffers, and
Solubility Products (Ksp)
Unit Ten Exam
Chapters 21 and 11
Nuclear Chemistry and Organic Chemistry
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Exams are scheduled a week in advance giving the student plenty of time to prepare for the examination. Missed exams involving
only a one or two day absence prior to the exam, students will be expected to take the exam immediately upon their return. Longer
absences will be handled on an individual basis for each student. If you know your going to be absent the day of the test, try to make
prior arrangement with the teacher. Failure to comply with the above may result in a “zero” grade being entered for your score.
Remember it is your responsibility to make arrangements with the instructor on when exams can be rescheduled and completed.
Lab Experiments: Approximately twenty percent of the course is devoted to the laboratory component of the course with each
lab being a hands-on experience for the student. A.P. Chemistry meets five days a week for 57 minutes; averaging about two
periods per week for hands-on laboratory experiences. The experience gained by manipulating equipment, recording and organizing
data, and drawing conclusions is a critical part of any science course. It is important for the student, using a spreadsheet (MS Excel),
to be able to establish relationships between the data collected. This can be done by properly defining the independent and dependent
variables, and establishing the best curve or line of best fit by establishing a linear relationship between variables. All labs will be
typed following a university format as will be explained in class (see Appendix A). Each student must keep a copy of all labs in their
three ring binder, so that they may be presented (in portfolio format) at any university in order to show that they have completed the
lab component of their A.P. Chemistry course. If the situation should arise where you need to miss a laboratory for athletics, cocurricular or illness, students must make-up the laboratory after school on the first Friday following the missed laboratory. Other
arrangements to make up a missed lab will only be at the discretion of your instructor. Students are expected to follow all lab safety
guidelines at all times. Students found not following safety rules may lose credit for that lab and may lose lab privileges for the
remainder of the course (resulting in a score of zero for the remaining laboratories).
We do not use a lab manual but rather a compilation of laboratories from various sources. These include:
1. Hope College Lab Program. Hope College, Michigan
2. Experimental Chemistry -Third Edition, by James F. Hall (© 1993. DC Heath and Company)
3. Laboratory Experiments for Advanced Placement Chemistry, by Sally Vonderbrink, Ph.D. (© 1995.
Flinn Scientific Inc.
Experiment List
Lab # Chapter(s)
1
2
1-3
3
1-3
4
1-3
5
1-3
6
4-6
7
4-6
8
4-6
9
4-6
10
4-6
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
4-6
12-14
12-14
12-14
12-14
15-16
15-16
15-16
19-20
19-20
17-18
17-18
17-18
17-18
Experiment
Safety Lab
Use of Equipment and Significant Figures: Density of Solids and Liquids
Chromatography Lab
Empirical Formula of MgO
Formula of a Hydrate
Stoichiometry Lab I: Gravimetric Analysis of Sulfate
Stoichiometry Lab II: Single Replacement
Stoichiometry Lab III: Acid/Base Titration
Stoichiometry Lab IV: Redox Titration
Heat of Solution Lab- Calorimetry and Hess’s Law
i. Acid/Base Neutralization
ii. Single Replacement
Heat of Combustion of Candle Wax
Molar Mass of Volatile Liquid
Molar Mass of Butane
Molar Volume of Hydrogen
Molar Mass from Freezing Point Depression (BHT Solvent)
Kinetics of Iodine Clock Reaction (Microscale)
Beer’s Law: Quantitative Colorimetric Analysis of FeSCN
Determination of Keq of FeSCN
Construction of a Series of Galvanic Cells (and Activity Series)
Construction of a Series of Electrolytic Cells
Titration Curves: Weak Acid (Mono and Diprotic), Weak Base, and Salts
Buffers
Hydrolysis of salts
Ksp of Ca(OH)2 by pH
Qualitative Analysis of Cations and Anions
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Course Schedule:
Semester One (18 weeks)
Unit One:
Lab Equipment, Procedures and Safety
Unit Two:
Matter, Measurement, Atoms, Elements, and Compounds (Chapters 1-3)
I. Matter, Measurement
A. Matter and Measurement
a. Elements and Atoms
b. Identifying Elements, Compounds or Mixtures
B. The Measures of Science
a. Qualitative Measurements
i. SI Units (Base and Derived)
ii. Prefixes
iii. Significant Figures in Measurements and Arithematic
iv. Scientific Notation
v. Unit Conversions
C. Accuracy and Precision of Laboratory Measurements (% error and standard deviation)
D. Properties of Matter
a. Chemical Properties
b. Physical Properties
i. Intensive (Focus on: Density)
ii. Extensive
c. Quantitative Measurements
E. Temperature vs. Heat
a. Temperature and Its Units
b. Heat and Its Units
F. Matter: Physical and Chemical Changes
a. Physical Changes
b. Chemical Changes
c. Law of Conservation of Matter
d. Energy and Physical and Chemical Changes of Matter
G. Classifying Matter
a. States of Matter
b. Heating and Cooling Curves
c. Homogeneous vs Heterogeneous Matter
H. The Scientific Method (Graphing Data with Microsoft Excel)
II. Atoms and Elements
A. Atomic Theory: Protons, Electrons, and Neutrons
B. Atomic Numbers, Mass Numbers, and Isotopes
C. Atomic Mass of Elements and the Mole– Counting-By-Weighing
D. Introduction to the Periodic Table and Overview of the Elements
III. Compounds
A. Defining and Classifying Compounds
a. Molecular Compounds
i. Structural and Molecular Formulas
ii. Naming and Writing Formulas for Molecular Compounds
1. Acid Covalent
2. Non-Acid Covalent
iii. Inter- and Intramolecular Forces: An Introduction
b. Ionic Compounds
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i. Ions
1. Monatomic (Including multivalent ions)
2. Polyatomic
ii. Naming and Writing Formulas for Ionic Compounds
iii. Crystal Lattices and Properties of Ionic Compounds
iv. Ionic Compounds and Coulomb’s Law
B. Atoms, Ions, Molecules, and Formula Units and the Mole – Counting-By-Weighing
C. Describing Compound Formulas
a. Percent Composition
b. Empirical and Molecular Formulas
c. Calculating Empirical and Molecular Formulas
d. Calculating Empirical and Molecular Formulas of Hydrocarbons from Combustion Data
e. Hydrated Ionic Compounds: Nomenclature, Percent Water, and Empirical Formula
Determination.
Unit Three: Stoichiometry and Thermochemistry (Chapters 4-6)
A. Stoichiometry
a. Chemical Equations (word and formula)
b. Balancing Chemical Equations
c. Stoichiometry – A,B,C,D Table Stoichiometry
i. General
ii. Identifying Limiting Reactant
iii. Actual, Theoretical, and Percent Yields
iv. Identifying Unknown Metals and Non-Metals Using Stoichiometry
d. Chemical Equations and Chemical Analysis
i. Analysis of Substance Purity (Gravimetric, Redox, Acid –Base)
ii. Determination of Empirical Formula of Hydrocarbon from Combustion Data
B. Aqueous Solutions and Solution Stoichiometry (Triangle Stoichiometry)
a. Properties of Solutions (Solute and Solvent)
i. Dilute vs. Concentrated
ii. Separating the Components of a Solution
iii. The Solution Process
iv. Classifying Solutes: Conductivity of Solutions (Strong, Weak, Non-Electrolytes)
v. Solubility of Compounds – Using the Solubility Table
b. Precipitation Reactions
i. Predicting if a Reaction will Occur
ii. Formula, Complete Ionic and Net Ionic Equations
c. Acid/Base Neutralization Reactions
i. Predicting if a Reaction will Occur
ii. Formula, Complete Ionic and Net Ionic Equations
iii. Metal Oxides and Non-Metal Oxides Reacting with Water
d. Gas Forming Reactions
i. Predicting if a Reaction will Occur
ii. Formula, Complete Ionic and Net Ionic Equations
e. Redox Reactions
i. Predicting if a Reaction will Occur
ii. Formula, Complete Ionic and Net Ionic Equations
iii. Balancing Redox Reactions Using Half-Reaction Method (Acid and Base Environments)
iv. Identification element being oxidized, element being reduced, oxidizing agent, reducing
agent, and moles of electrons involved
C. Measuring Concentration of Compounds in Solution
a. Molarity
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D.
E.
F.
G.
b. Preparing a Solution of Known Molarity…
i. By Diluting a Stock Solution
ii. By Using a Solid Solute
pH Scale: An Introduction
Stoichiometry of Reactions Involving Aqueous Solutions
a. General Triangle Stoichiometry
b. Titration Stoichiometry (Acid/Base and Redox)
Reaction Prediction
a. Combination (Sythesis) Reactions
b. Decomposition Reactions
c. Single Replacement Reactions
d. Double Replacement Reactions
e. Combustion Reactions
Energy: Chemical and Physical Changes
a. Energy Some Basic Principles
b. Specific Heat Capacity and Heat Transfer
c. Energy and Changes of State (including Heating and Cooling Curves)
d. Determining Heat Involved in Physical and Chemical Changes
i. Calorimetry (Coffee-Cup and Bomb)
ii. Hess’s Law
iii. Heats of Formation
iv. Bond Energies
e. Laws of Thermodynamics (State Functions)
f. Enthalpy Diagrams, Enthalpy Equations, and Thermochemical Equations
g. Thermochemical Stoichiometry
Unit Four: Atomic Structure, Electron Configurations, and Periodicity (Chapters 7-8)
A. Atomic Structure
a. Historical Development of MODERN ATOMIC THEORY
b. Bohr Model (including Heisenberg’s Uncertainty Principle)
c. Quantum Mechanical Model
d. Quantum Numbers
B. Electron Configurations
a. Electron Configurations (including Pauli Exclusion Principle, Aufbau, and Hund’s Rule)
i. Spdf Notation
ii. Noble Gas Notation
iii. Orbital / Box Notation
iv. Lewis Electron Dot Notation
b. Diamagnetism and Paramagnetism
c. Exceptions to Aufbau Filling Diagram
d. Excited vs Ground State Electron Configurations - Flame Tests for Cations
e. Isoelectronic Species
C. Atomic Properties and Periodic Trends
a. Z-Effective; Shielding and Nuclear Charge
b. Atomic Size, Ionic Size, Ionization Energy, Electron Affinity, and Electronegativity
i. Trends Across a Period
ii. Trends Down a Group
Unit Five: Bonding and Intermolecular Forces (Chapters 9-10 & 13)
Bonding and Molecular Structure
a. Valence electrons
b. Chemical Bond Formation (Ionic, Polar Covalent, and Covalent)
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c. Ionic Bonding
i. Bond (Lattice) energy
ii. Properties
d. Metallic Bonding
i. Bond energy
ii. Properties
iii. Alloys (Substitutional and Interstitial)
e. Covalent bonding and Intermolecular Forces
i. Valence Electrons
ii. Lewis Structures (Including Exceptions to Octet Rule)
iii. Resonance Structures
iv. Molecular Shapes, Geometries, Bond Angles and Symmetry
v. Formal Charges: Determining the Correct Lewis Structure for a Molecule
vi. Bond vs Molecular Polarity
vii. Intermolecular Force ( London, Dipole-Dipole, and Hydrogen Bonding)
viii. Bond Properties (Bond Order, Bond Length, Bond Energy, Bond Vibrational Frequency)
ix. Sigma vs Pi Bonds
x. Hybridization of Atomic Orbitals of the Central Atom in a Molecule
xi. Special Case: Giant Molecules of Carbon
Unit Six:
Solids, Liquids, Gases, Phase Diagrams, and Solutions (Chapters 12-14)
A. Solid State Chemistry (Covalent Networks, Ionic, Metallic, and Molecular Solids)
B. Liquids
a. Vaporization
b. Vapor Pressure
c. Boiling
d. Surface Tension
e. Capillary Action
C. Gases
a. Kinetic Molecular Theory
b. Properties of Gases (P, V, n T)
c. Pressure
i. Atmospheric
ii. Samples of Gas in Lab (Open and Closed Manometers)
d. Gas Laws
i. Boyle’s Law
ii. Charle’s Law
iii. Avogadro’s Law
iv. Gay-Lussac’s Law
v. Ideal Gas Law:
PV = nRT
vi. Combined Gas Law: P1V1/n1T1 = R = P2V2/n2T2
e. Gas Laws and Stoichiometry
i. STP Conditions
ii. Non-STP conditions
f. Gas Mixtures and Partial Pressures (Dalton’s Law)
g. Kelvin Temperature: Kinetic Energy and Molecular Velocity
i. Kinetic Energy
ii. Molecular Velocity
h. Graham’s Law of Effusion and Diffusion
i. Non-Ideal Gas Behavior (van der Waals Equation)
D. Phase Diagrams (Triple point, Normal MP, Normal BP, Critical point, and Density differences by
looking at a phase diagram)
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E. Mixtures
a. Suspensions
b. Colloidal Dispersions
c. Solutions
i. Units of Concentration (molarity, molality, percent by mass, mole fraction, PPM)
ii. Solution Process
1. Factors Affecting Dissolution Rate
2. The Nature of Solutions
a. Conductivity
b. Solubility and Solubility Curves
c. Factors Impacting Solubility
i. “Like Dissolves Like”
ii. Temperature
iii. Pressure (Henry’s Law)
3. Heats of Solution
iii. Colligative Properties
1. Vapor Pressure (Raoult’s Law)
2. Boiling Point Elevation
3. Freezing Point Depression
4. Osmotic Pressure
iv. Spectrophotometry: Determining the Concentration of a Colored Solution
SEMESTER ONE FINAL EXAM
Chapters 1-14 (excluding chapter 11)
Semester Two (14 weeks)
Unit Seven:
Chemical Kinetics and Equilibrium I (Chapters 15 and 16)
A. Rates of Chemical Reactions
a. Macroscopic Level
i. Rates of Chemical Reaction – Inititial, Average, and Instantaneous Rates
ii. Reaction Conditions and Rate
1. Reactant Concentration
2. Temperature
3. Catalyst
4. Surface Area of Reactants
iii. Differential Rate Laws (zero-, first-, and second-order)
iv. Integrated Rate Laws (zero-, first-, and second-order)
v. Reaction Half-Life
b. Microscopic View of reaction Rates
i. Collision Theory of Reaction rates
ii. Arrhenius Equation
iii. Reaction Mechanisms
B. Chemical Equilibrium I
a. Nature of the Equilibrium State
b. The Reaction Quotient and Equilibrium Constant (Keq)
c. Relationship Between Kc and Kp
d. Manipulating the Equilibrium Expression
e. The Meaning of the Equilibrium Constant
i. Reactant or Product Favored
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ii. Comparing Qeq with Keq
f. Calculating an Equilibrium Constant (Using ICE Diagrams)
g. Given a Kc and Initial Molarities– Solve for Equilibrium Concentrations
h. Special Equilibrium Values:
i. Solubility Product (Ksp)
ii. Acid Dissociation Constant (Ka)
iii. Base Dissociation Constant (Kb)
i. Disturbing an Equilibrium – Le Chatelier’s Principle
i. Temperature Effects
ii. Addition or Removal of Product,
iii. Volume Changes
Unit Eight:
Thermodynamics (Enthalpy, Entropy, and Free Energy) and Electrochemistry
(Chapters 19 and 20)
A. Thermodynamics
a. Enthalpy
i. Definition
ii. Methods for Calculating: Calorimetry, Hess’s Law, Heats of Formation, Bond Energies,
ΔGoRxn = ΔHoRxn - T ΔSoRxn
b. Entropy
i. Definition
ii. Entropy Changes
iii. ΔSouniverse, ΔSoSystem, ΔSoSurroundings
iv. Methods for Calculating:
1. ΣSProducts - ΣSReactants = ΔSRxn
2. ΔGoRxn = ΔHoRxn - T ΔSoRxn
c. Free Energy
i. Definition
ii. Free-Energy Changes
iii. Methods for Calculating:
1. ΣGProducts - ΣGReactants = ΔGRxn
2. ΔGoRxn = ΔHoRxn - T ΔSoRxn
d. Free Energy, Enthalpy, and Temperature – Predicting Spontaneity
e. Free Energy and the Equilibrium Constant (K eq)
B. Electrochemistry
a. Balancing Redox Reactions
b. Electrochemical Cells
i. Galvanic
ii. Electrolytic
c. Calculating Eo, Go, and Keq for an Electrochemical Cell
d. Calculating E at Non-Standard Conditions – Nernst Equation
e. Electrochemical Stoichiometry
Unit Nine: Equilibrium II: Acids, Bases, Salts, Buffers, and Solubility Products (Ksp)
(Chapters 17 and 18)
A. Water and the pH Scale
a. Water
b. The pH Scale
c. Measuring pH in the laboratory
B. Acids
a. Definitions
b. Properties
c. Strong vs Weak Acids
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d. What structural properties make an acid strong or weak?
e. Non-Metal Oxides and water – Acid Rain
f. Calculations involving strong acids.
i. Given [Acid Initial], calculate pH
ii. Given the solutions pH, calculate the [Acid]
iii. Given a mixture of strong acids, calculate equilibrium [ ]’s, % ionization, and pH
g. Calculations involving weak acids
i. Given a Ka for an acid and [Acid Initial] calculate equilibrium [ ]’s, % ionization,
and pH
ii. Given the Ka of a Weak Acid Calculate the [ ] of the weak acid at equilibrium.
iii. Given a % ionization or pH an [Acid Initial] for an acid, calculate its Ka.
iv. Given a mixture of weak acids, calculate equilibrium [ ]’s, % ionization, and pH
h. Calculations involving polyprotic acids
Given a Ka1, Ka2, etc… for an acid and [Acid Initial]-- calculate equilibrium [ ]’s, % ionization, and
pH
C. Bases
a. Properties
b. Strong vs Weak Bases
c. Calculations involving strong bases (metal hydroxides)
i. Given [Base Initial], calculate the solutions pH
ii. Given the solutions pH, calculate the [Base Initial]
d. Calculations involving weak acids (ammonia and ammonia-like bases)
i. Given a Kb for an acid and [Base Initial] calculate its equilibrium [ ], % ionization, and pH
ii. Given a % ionization or pH an [Base Initial] for an acid, calculate its Kb.
iii.Given a mixture of weak bases, calculate its equilibrium [ ], % ionization, and pH
D. Acidic, Basic, and Neutral Salts
a. Identifying Acidic, Basic, and Neutral Salts
b. Calculations involving basic salts (Conjugate Bases to Weak Acids)
i. Writing out the hydrolysis reaction
ii. Calculating the Ka for the conjugate acid of a weak base (Ka . Kb = Kw)
iii. Use Kb to determine the pH and equilibrium concentrations
c. Calculations involving acidic salts (Conjugate Acids to Weak Bases)
i. Writing out the hydrolysis reaction
ii. Calculating the Ka for the conjugate acid of a weak base (Ka . Kb = Kw)
iii.. Use Ka to determine the pH and equilibrium concentrations
E. Buffered Solutions
a. Common Ion Effect
b. How does buffering work?
c. Calculating the pH of a Buffered Solution
i. Weak Acid Buffer
ii.Weak Base Buffer
d. Picking the Best Buffer Solution and Buffer Capacity
i. Picking the Best Buffer System
ii.Buffer Capacity
e. Preparing a Buffer System / Identifying a Buffer System
f. Acid-Base Titration Curves
F. Solubility Equilibria (Precipitation Reactions)
a. Write out Ksp equations
b. Given a Solubility Solve for the Salts Ksp
c. Given a Ksp for a Salt Calculate the Salts Molar Solubility
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d. Comparing Ksp to Identify the least soluble saltsGiven a Ksp for a Salt Calculate the Salts
Molar Solubility
e. Calculating the Solubility of a Salt in a Solution with a Common Ion Present?
f. Calculating the Solubility of a Salt in a Solution with a Common Ion Present?
Unit Ten:
Nuclear Chemistry and Organic Chemistry (Chapters 23 and 11)
A. Nuclear Chemistry
a. Natural Radioactivity
b. Nuclear Reactions and Radioactive Decay
c. Decay Series
d. Stability of Atomic Nuclei (Neutron/Proton Ratio)
i. Zone of Stability
ii. Prediciting Decay Types
iii. Binding Energy
e. Rates of Nuclear Decay and Half-Lives
f. Radiocarbon Dating
g. Nuclear Fission and Fusion
h. Nuclear Reactors – The Basics
i. Radiation Health and Safety
B. Organic Chemistry
a. Structural Diversity
i. Isomers (Structural isomers, sterioisomers, optical isomers)
ii. Stability of Carbon Compounds
c. Hydrocarbons
i. Alkanes – Recognition, Properties, and Nomenclature
ii. Alkenes – Recognition, Properties, and Nomenclature
iii. Alkynes – Recognition, Properties, and Nomenclature
iv. Aromatics – Recognition, Properties, and Nomenclature
d. Common Functional Groups and Derivatives of Alkanes:
i. Alcohols, Ethers, and Amines
ii. The Carbonyl Group- Aldehydes, Ketones, Carboxylic Acids, Esters, and Amides
e. Polymers
i. Addition Polymers
ii. Condensation Polymers
SEMESTER TWO FINAL EXAM
SAT II Exam and/or Chemistry Regents Exam
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APPENDIX A:
A.P Chemistry
Lab Report Format
(Revised from the WSU-Physics Report Format at: http://www.physics.wsu.edu/academics/labs/LabReportFormat (7-7-03).htm)
This guide gives the overall format that lab reports are to follow, with the approximate weight of each section contained in
the lab report. Note that the percentages given below are rough guidelines. More or less weight may be given in certain
circumstances. The lab report should be self-contained so that anyone (not necessarily with a chemistry or physics
background!) can read it and understand what you did.
General Format
Lab reports are expected to BE TYPED and LOOK LIKE COLLEGE LEVEL WORK. Your reports are expected to
be free of grammatical, syntax, and spelling errors, and look like a respectable presentation of your work. You are
therefore advised to proofread your work before submitting it. Your lab report should generally include the following
sections:
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Title Page (5%)
Purpose of Lab (5%)
Pre-Lab Questions (5%)
Procedure (10%)
Experiment Description, and Observations (15%)
Analysis (Calculations, Graphs, etc.) (40%)
Discussion, Conclusions, and Post-Lab Questions (20%)
Each of these components is discussed in detail below. It is your job to present information in a clear, understandable way.
The goal is to have a self-contained report that can tell someone without a chemistry or physics background and without a
lab manual what you did. As the semester progresses, the presentation aspect of the lab report should improve, so more
points may be taken off for excessively sloppy, unorganized reports. Take this opportunity to practice your
presentation/organization skills, as these skills will help you in whatever career you choose. Different laboratory
exercises may lend themselves to different overall formats. Nevertheless each report must contain some form of the
various components listed above. Don’t hesitate to ask your instructor(s) about the appropriateness of a particular format
that you wish to use.
Title Page (5%)
The first page of the lab report is the title page consisting of:
 The title of the experiment
 Lab group members names
 Lab station number
 The date that the lab was performed
 The date that the lab was submitted
Nothing else should appear on the title page, and the entire report should be stapled in the upper left-hand corner. Prior to handing in
a laboratory, all members of a lab group should have reviewed the report and then initialed by their name. This indicates to
me that they have read through the report and will accept the grade that it earns.
Purpose (5%)
Clearly explain the purpose or purposes of the experiment. Why did we do this lab?
Pre-Lab Questions (5%)
Complete all pre-lab questions clearly showing all work/calculations and using completing complete sentences when answering short
answer questions.
Procedure (10%)
Briefly describe the procedure you followed and draw a picture of the experimental set-up to meet the purpose of the lab.
This should include the equipment being used. The procedure section should be adequate so that anyone without a chemistry or
physics background could read it and follow along. In other words, someone else could repeat your experiment following the steps
outline in your procedure.
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Experiment and Observation (15%)
Record all data in an organized (table format) fashion. Include relevant symbols and appropriate units when recording data. When
making measurements please record the appropriate number of significant figures.
Analysis (40%)
Calculations
Complete the calculations outlined in the laboratory in this section. Show ALL WORK for each calculation. If your lab involves
multiple trials show ONE complete example of substituting in numerical values (indicate where the numerical values come from, say
Table I, run#2, for clarity). If your calculation (s) involves unit conversions be sure to show all conversion factors with units.
Display ALL the results of your calculations (tables can be very useful here) including the appropriate units.
Graphs
If a graph is required for a given lab, each graph is to be done on a separate page OR clearly and neatly inserted into your word
document from MS EXCEL (See Appendix B). Each graph must have a title and the axes clearly labeled. Be sure independent data is
plotted on the x-axis and dependent data is plotted on the y-axis. If you're asked to draw a curve through your data points, this should
always be a best-fit curve (for example, a straight line that best represents your data, not a dot-to-dot connection of data points). If
you're asked to calculate the formula that relates your data use MS EXCEL and record the equation on your graph, indicating clearly
which points on the graph you used in your analysis.
Discussion, Conclusions, and Post-Lab Questions (20%)
The discussion section should be three paragraphs in length (with a maximum of one page). It should be carefully organized (you may
even wish to make a rough draft outline first!) and must include consideration of ALL of the following aspects of your experiment:
results, interpretation of results, and uncertainty in results (see below). Each of these aspects is discussed in detail in the following
paragraphs. Your discussion should be written in paragraph form (don’t submit the outline), and you may find it convenient to
organize the various aspects differently for different labs. “Consideration” does not simply mean answering each question below, but
placing your experiment in the context formed by these questions and reporting your results. Cite specific experimental results
liberally to support your conclusions. Not all of the following questions will apply to every lab!
Results
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
What is the connection between your measurements and your final results?
What were the results of your calculations?
If your lab involved graphing variables…
 What trends were noticeable (linear, inverse, polynomial, exponential) ?
 Clearly identify the dependent and independent variables used in the lab. How did the independent variables
affect the dependent variables? (For example, did an increase in a given measured (independent) variable result in
an increase or decrease in the associated calculated (dependent) variable?
Interpretation of results
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What is the theory or model behind the experiment you performed?
Do your experimental results substantiate/agree with the theory? (Be sure to refer specifically to YOUR
experimental results!) Why or why not?
Were these results consistent with your original beliefs, or were you forced to re-evaluate your prior conceptions?
Uncertainty in results
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How much did your results deviate from expected values (percent error)?
Are the deviations due to error/uncertainty in the experimental method, or are they due to idealizations inherent in
the theory (or both)? If the deviations are due to error/uncertainty in the method what are the possible
sources – Be Specific!!! For example, if your value was higher than the true value what could have caused
this? DO NOT SAY “HUMAN ERROR” WAS THE CAUSE.
If the correct value is unknown or difficult to find, what range of values would seem reasonable for this quantity?
Draw on your own experiences or site values for similar material.
In which of the measurements or observations that you made do you have the least confidence? How would
variations in this value (if it were too high or too low) affect your results?
Post-Lab Questions
 Complete all post-lab questions clearly showing all work/calculations and using completing complete sentences
when answering short answer questions
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APPENDIX B:
GRAPHING WITH MS EXCEL
1. Start MS Excel and add data to cells then
2. Select XY Scatter plot, then click next
click on the chart wizard (looks like a little graph)
3. Click on “Series” tab
then click on “Remove”
4. Click on the “Add”
button.
5. Click on the grid button next to the
“X Value”
6. Highlight the independent data (X) in your
spreadsheet, then close the chart source window
8. Highlight the dependent data (Y) in your
spreadsheet, then close the chart source window
7. Click on the grid button next to the
“Y Value”
9. Click Next
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10. Add Chart Title, and Label Axes with variable
and units.
11. Unless you have more than one data series
remove the legend from the graph
12. Save the graph as a new sheet.
13. To print the equation for the graph on the chart
right mouse click on any data point on your graph
and select “Add Trendline”
14. Choose the type of regression you wish to use in producing your trendline, then click on the “Options” tab
and check that the option to “Display equation on chart” and “Display R squared Value on chart” are checked
15. Edit your equation so that instead of “X” or “Y” the independent and dependent variables (respectively) that
you plotted show-up in the equation.
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APPENDIX C:
Central Kitsap High School
CLASSROOM GUIDELINES
CKHS staff values student behavior that reflects caring, trustworthiness, respect,
truthfulness, honesty, and good school citizenship.
1. ATTENDANCE
Class attendance is important every day. Any student who misses more than ten (10) days may lose the
opportunity to complete make-up work.
2. TARDIES
Each student is expected to be in class on time. Tardies will now be tracked on a cumulative basis across each
students schedule. See consequences for tardiness listed below.
When a student reaches 3 tardies in any one week, he or she will move up one step along the following list for
consequences:
Step 1:
Step 2:
Step 3:
Step 4:
Step 5:
Step 6:
Warning from ISS Monitor
Work Detail assigned by ISS Monitor
Double Work Detail assigned by ISS Monitor
In School Suspension day assigned by Administrator with phone call home
Thursday School(s) assigned by Administrator with phone call home
Suspension consequence (out-or in-school) with parent/administrator conference
Student tardies will be reset to zero at the end of the semester.
3. PASSES
Students need a pass to be in the hallways during class time. Students without a pass will be escorted
back to class by security.
4. FOOD/DRINKS
NO food or drink is allowed anywhere except the cafeteria and in front of the building. Bottled water is
allowed with the teacher’s permission.
5. BEHAVIOR
Students are expected to display appropriate behavior and use appropriate language in the classrooms
and the halls. Harassment, profanity, and fighting, as well as possession of weapons, will not be tolerated and
will be dealt with swiftly and in accordance with district/building policy Walkman or CD players, laser pointers,
and/or communication devices such as pagers and cell phones may not be used during school hours.
6. DEFACING SCHOOL PROPERTY
Students are expected to respect school property. They are expected to place waste in proper recycling and
trash receptacles. Students shall not deface or mark on lockers, desks, tabletops, walls, textbooks, carpeting etc.
7. CHEATING
Cheating in any form will not be tolerated. Cheating includes plagiarism and copying another student’s
homework or test. Students copying the work and students willingly allowing others to copy their work or test
shall be held accountable for cheating; teachers who witness the copying of homework in hallways or other
classes will follow-up with the student’s teacher. Suggested district consequences for the first offense of
cheating include a seven (7) day suspension from school.
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