Chemistry Course Syllabus
Mr. Shakeri
Room D204
Canyon Crest Academy
kaveh.shakeri@sduhsd.net
858-350-0253 x4134
Course Description
Advanced placement chemistry is designed to be the equivalent of the general college chemistry course.
Chemistry is the study of atoms and molecules and how they interact according to physical laws. Chemistry is
applicable to everyday life and such connections will be demonstrated throughout the course. This course will
focus understanding chemistry through solving problems. The California State Standards below will be covered
through demonstrations, discussions, class assignments and laboratory investigations.
 Atomic and Molecular Structure
 Chemical Thermodynamics
 Chemical Bonds
 Reaction Rates
 Conservation of Matter and Stoichiometry
 Chemical Equilibrium
 Gases and Their Properties
 Organic Chemistry and Biochemistry
 Acids and Bases
 Nuclear Processes
 Solutions
Textbook
General Chemistry Ebbing, Gammon Houghton Mifflin, 2005 8th Edition
Your success in the course will directly reflect on the amount of time and energy you put into it. Here are
some helpful hints for success.

Come to class prepared daily and on time.

Participate actively and ask questions, routinely check class website.

Keep detailed notes about demonstrations and examples presented in class.

Keep up with all assigned work and sample problems and read chapters as they are assigned

Be open to a variety of learning styles and activities

Be able to work productively in groups and independently.
Materials: Please bring the following materials to class daily:

Scientific calculator or graphing calculator – it should be able to perform logarithmic and exponential
functions, as well as scientific notation.

Blue/black pen, #2 pencil, and ruler.

Chemistry spiral notebook (that has 3 hole punch) or loose leaf paper for notes

Highlighter and colored pencils (optional)
Grading
The grades that students receive in the AP Chemistry course are independent of the grades received on the
AP Chemistry exam. Each assignment will have a point value all points are equal.
100 – 90% A
89 – 80% B
70 – 79% C
60 – 69% D
59% and below F
The grades are based on a point system. Every point is equal. Different activities will have different
point values. The following breakdown gives an estimate to how those points will be distributed during the
course.
Tests
Quizzes
Labs
Homework
Extra credit
~45% (some exams may have curves)
~20%
~30%
~5%
minimal if any
Grades will be posted on ParentPortal and will be up to date. You may always contact me with email or
come in at lunch, before or after school to discuss your grade. I will not discuss grades during class time.
Homework
There is always homework to do for AP Chemistry. The bookwork is assigned on a chapter basis. Each
chapter will be covered in 3-5 class periods, you are expected to pace yourself so all the work does not fall
onto one night.
Laboratories
Laboratories are used to reinforce topics covered in class or to introduce a new topic. The labs will need to
follow the laboratory guidelines. There will be at least one lab per unit as time permits. Good lab practice is
essential to report data with great confidence and accuracy. Each student will submit their own labs with
their own individual thought, data maybe shared within a group. Making up labs will be made up at
discretion of the instructor, due to availability of materials. Alternative assignments may be used in place of
missed labs.
Class Rules:
1) Respect and Common Courtesy
2) Safety Rules will be enforced to the highest degree. Any infractions will be dealt with in a severe
manor. Some first time offenses may result in removal from lab activities and possible further
administrative repercussions. You will sign and return a safety contract, you are expected to follow these
rules.
3) I will enforce all rules as followed by the Canyon Crest Discipline policy. (Academic Honesty, Tardy
and cell phones)
Consequences:
Managing a safe and effective classroom is my number one priority. Students who consistently break rules
are a distraction to everyone's education and safety. Infractions will be dealt with by:
1. Warning and/or call home
3. Removal from class and call home
2. Detention and/or additional projects and/or call home
4. Referral to the Vice Principal and
call home
These steps need not occur in this order, dependent on the severity of inappropriate behavior. Alternative
actions may be taken and are reserved for the discretion of the teacher.
Absence
 If you are absent on the day of a test you need to be prepared to take the test on the day you return.
 If you are absent the assignments due the day you were absent are due the day you return.
 Any labs, assignments or homework covered when absent are given three days to make up work.
 If you are absent YOU ARE RESPONSIBLE to find out what you missed while you were out. You may
use email to reach me our other classmates; You may also use your lab partner or other “class
buddy”; You may also use the class website to find out what you missed while you were away.
*****If your absence is unexcused then you will not be allowed to make up any missed test, labs or turn in
any work.*******
Website:
Access is available through the CCA homepage or http://teachers.sduhsd.net/kshakeri/. I add my notes,
handouts, practice AP test questions and any other forms I give out in class as I create them.
We will also use blackboard. Blackboard will be used for take home quizzes for the chapters. We have a
facebook group for students. Students are encourage to chat with classmates and post questions. The
facebook page is an extension of the classroom. Only students enrolled in class are permitted in the group.
All school and classroom behavior expectations are expected in the facebook group.
Late Work
Late work will be accepted up to one day after the assignment due date and will automatically loose 50%
credit. Late assignments should be handed directly to the instructor either before or after class.
Tardy Policy If you are not in your seat before the final bell, you will be considered tardy. A tardy will
follow with the school wide consequences.
Academic Dishonesty
A student who commits or facilitates cheating will be referred to the Administrative team at Canyon Crest
Academy. The student will receive a zero for the assignment and will not be allowed to make it up. A second
occurrence of cheating will result in a failing grade for the quarter.
Open Door Policy
I will be available for help everyday usually in the mornings (by 7:30am). My room is open at lunch, but this
is usually when I need to take a break and eat some food. Do not expect tutoring during lunch time. You
may be able to catch me at the beginning of lunch.
I have a free 4th period. My room will be open this time to study and get school work done.
I will have tutoring time after school Monday-Thursday for up to 30 minutes or so after school.
There will be weekly study session in AP chemistry. The time and date is still undecided, most likely
Thursday or Wednesday after school.. I encourage students to meet with classmates to work on homework,
study for tests and any other chemistry related material. The times will change according to my travel
schedule for my Master’s program schedule.
ALL STUDENTS ENROLLED IN ADVANCES PLACMENT CHEMSITRY ARE EXPECTED TO
TAKE THE AP EXAM IN MAY!
Topic Outline 2013
Below is a descriptive list that will be used as topic guideline for the AP Chemistry Course (provided
by College Board).
1. Structure of Matter
2. States of Matter
3. Reaction Types
4. Descriptive Chemistry
5. Laboratory Work
1. Structure of Matter (20% of multiple-choice questions)
A. Atomic theory and atomic structure
1)
2)
3)
4)
5)
Evidence for the atomic theory
Atomic masses; determination by chemical and physical means
Atomic number and mass number; isotopes
Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
Periodic relationships including, for example, atomic radii, ionization energies,
electron affinities, oxidation states
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
c) Polarity of bonds, electronegativity
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, structural isomerism of simple organic molecules and coordination
complexes; dipole moments of molecules; relation of properties to structure
C. Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical
applications
2. States of Matter (20% of multiple-choice questions)
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
B. Liquids and solids
1)
2)
3)
4)
Liquids and solids from the kinetic-molecular viewpoint
Phase diagrams of one-component systems
Changes of state, including critical points and triple points
Structure of solids; lattice energies
C. Solutions
1)
2)
3)
4)
Types of solutions and factors affecting solubility
Methods of expressing concentration (use of normalities is not tested)
Raoult’s law and colligative properties (nonvolatile solutes); osmosis
Nonideal behavior (qualitative aspects)
3. Reactions (35 – 40% of multiple-choice questions)
A. Reaction types
1)
Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis;
coordination complexes; amphoterism
2) Precipitation reactions
3) Oxidation-reduction reactions
a) Oxidation number
b) The role of the electron in oxidation-reduction
c) electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst
equation; prediction of the direction of redox reactions.
B. Stoichiometry
1)
2)
3)
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
C. Equilibrium
1)
2)
Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle; equilibrium constants
Quantitative treatment
a)
Equilibrium constants for gaseous reactions: Kp, Kc
b)
Equilibrium constants for reactions in solution
(1) Constants for acids and bases; pK; pH
(2) Solubility product constants and their application to precipitation and the dissolution of
slightly soluble compounds
(3) Common ion effect; buffers; hydrolysis
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
E. Thermodynamics
1)
2)
3)
4)
State functions
First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law;
heats of vaporization and fusion; calorimetry
Second law: entropy; 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
4. Descriptive Chemistry (10 –15% of multiple-choice questions)
Knowledge of specific facts of chemistry is essential for an understanding of principles and concepts. These
descriptive facts, including the chemistry involved in environmental and societal issues, should not be
isolated from the principles being studied but should be taught throughout the course to illustrate and
illuminate the principles. The following areas should be covered:
1) Chemical reactivity and products of chemical reactions
2) Relationships in the periodic table: horizontal, vertical, and diagonal with examples
from alkali metals, alkaline earth metals, halogens, and the first series of transition
elements
3) Introduction to organic chemistry: hydrocarbons and functional groups (structure,
nomenclature, chemical properties)
5. Laboratory (5 –10% of multiple-choice questions)
The differences between college chemistry and the usual secondary school chemistry course are especially
evident in the laboratory work. The AP Chemistry Exam includes some questions based on experiences and
skills students acquire in the laboratory:

making observations of chemical reactions and substances

recording data

calculating and interpreting results based on the quantitative data obtained

communicating effectively the results of experimental work

Chemical Calculations in Sections 1-5 above
The following list summarizes types of problems either explicitly or implicitly included
in the preceding material. Attention should be given to significant figures, precision of
measured values, and the use of logarithmic and exponential relationships. Critical
analysis of the reasonableness of results is to be encouraged.
1)
2)
3)
4)
5)
6)
Percentage composition
Empirical and molecular formulas from experimental data
Molar masses from gas density, freezing-point, and boiling-point measurements
Gas laws, including the ideal gas law, Dalton’s law, and Graham’s law
Stoichiometric relations using the concept of the mole; titration calculations
Mole fractions; molar and molal solutions
Faraday’s laws of electrolysis
Equilibrium constants and their applications, including their use for simultaneous
equilibria
9) Standard electrode potentials and their use; Nernst equation
10) Thermodynamic and thermochemical calculations
11) Kinetics calculations
7)
8)
Lab Report Format:
Title: Usually identifies the type of lab you will be doing.
Purpose: A summary of the concepts involved in the chemical process of the lab.
Background Information: This area contains the pertinent information needed to answer the most of the
conclusion questions. Often, a historical perspective is provided or chemical equations/reactions are shown.
This should give a preview of the laboratory experiment.
Procedure: The steps you should follow in order with careful attention to detail. How well you carry out each step
will determine the accuracy of your data.
Safety: Identify the safety concerns that will be addressed in the laboratory. Include 5 safety rules and
specific safety concerns.
Materials: Not required if you have a detailed procedure.
Data Table: The data table has a title that describes the information recorded in the table. It should contain
neat (use a ruler) column and row headings. If a table is not provided, you will have to draw one.
 Units (ºC, mol, g, mL, etc.) must be recorded with each piece of data recorded in the data table or in the
parentheses provided at the top of the column.
 Use correct significant figures and scientific notation
 No fractions, only decimals!
Data Analysis: This section is where math calculations and graphical analysis are made using data collected
from the lab. All work must be shown with equations for credit. You will get an automatic revisit for this
section if your work is not shown.
1) Write all calculations in this section. One sample calculation is needed where the same calculation is
repeated. Make sure the equation is written, numbers are plugged into the equation with units and final
answer represented with units and proper significant figures.
 All graphs must have a title (X vs Y for (name of the lab))
 Each axis must be labeled with the quantity and units.
 Draw a best-fit line or best-fit curve.
 Use the whole graph!
 Staple the graphs to the back of your lab write-up.
Conclusion: This section contains questions that test your understanding of the lab and the concepts involved.
In a few paragraphs
a. Was the lab successful, was your data acceptable (precision, accuracy, reliability) discuss percent error in
mentioning the lab’s success. State your purpose and apply background information on the lab to discuss the
lab’s success.
b. Relate the information to the concepts you are studying. Discuss the patterns of the graphs how they relate
to the concept. If there is no graph, use the data to help explain the concept.
Error Analysis (Sources of Error): This is the last section where you explain what errors were committed
during the lab. No experiment is perfect. There is always some fault, whether it is human error or scientific
error. Include as many possible sources of error although only 3 are required.
 You should explain how your errors impacted the data
 What could be done to improve the experiment next time.
Any follow up questions: Include all discussion questions associated with the lab in the end. Write the
question (or summarize) and answer in complete sentences.
Miscellaneous Information:
1. Put your name (first and last) and period legibly in the upper right hand corner of your lab. Your partners name
goes underneath
2. Do not use white-out! If you make an error, simply put a single line through the error and write the correct
information either above the error or to the side of an error.
3. Skip a line between each section of the lab report.
4. Excessive sloppy reports will lose points (i.e. illegible writing or no name). You will not turn in printed data
tables, etc. You will use a ruler to neatly write all reports.
5. No more than 2-3 persons in a group.
Course Outline: Spring 2013 Canyon Crest Academy
Topic
Matter and Measurement

General
Chemistry
Chapters
1
TimeLine
Labs
1day
- chromatography lab
(18, 1b)
2
3 days
Review of factor-label method, conversion factors between
units.
Atoms, Ions, & Nomenclature



-empirical formula of an
oxide (1.3a)
- Qualitative analysis of
Ions (14.22a)
Review nuclear nomenclature, average atomic mass.
Review Avogadro’s Number, mole concept, molarity in
solutions.
Chemical nomenclature review, including complex ions.
Stoichiometry
3
1 days
4
4 days
7, 8
2 days
Balancing equations, the moles, atomic/molar mass, percent
composition, writing chemical equations, empirical formuals,
limiting reactants, percent yield
Chemical Reactions
Net Ionic equations, Solubility, Acid Base,
Neutralization, Redox Reactions
Electronic Configuration
- absorption spectrum of
Cobalt (II) Chloride
(17. 7)

Quantum Theory principles - energy, frequency and
wavelength relationships, Absorption/emission spectra, Bohr atom
calculations.

De Broglie wavelengths, Wave function, electron cloud
probability, electron configurations and orbital diagrams,
Quantum Numbers.
States of Matter: Solids and Liquids
-Hydrated Salts (2,9.3B)
-Preparing a standard
solution
-Acid v. Carbonate
Titration
- Gravimetric analysis of
titration of Ba(OH)2
and H2SO4 (16. Vernier)
-Redox Titration,
Determination of oxalate
(6, 8. Lab WS)
11
2 days
Shakashiri Demos
5
3 days
-Molar Volume of a Gas
- Molar Mass of Butane
(5.AP WS)
8
1 day
9, 10
3 days
-Molecular Models
6, 19
6 days
-Thermochemsitry and
Hess’ Law (12.6)
23
1 day
- Nickle Compound
Complexes
Intermolecular forces, liquid and solid states, metallic
bonding, phase diagrams
States of Matter: Gases
Ideal gas law, partial pressure, combined gas law, kinetic model,
effusion and diffusion (Graham’s law), real gases
Periodicity
Electronegativity, atomic radius, ionic radius,
1st 2nd 3rd ionization energies in groups and periods.
Bonding



Theory of chemical bonding, periodic properties, Lewis dot
structures,
bond polarity, bond energies.
Molecular bonding theories (VSEPR, bond hybridization,
molecular orbitals), geometries, bond angles, molecular
polarities, molecular orbital configurations.
Thermochemistry
Enthalpy and calorimetry, Hess’s Law, equations of state,
standard enthalpy of formation.
Thermodynamics
Enthalpy and the first law of thermodynamics
Entropy and the second law.
Free energy and the third law.
Transition Metal Basics
First row transition metals, coordination compounds,
isomerixation, crytal field model
Organics
(15. page 969 Summerlin
demo)
24
2 day
15
5 days
16, 17
6 days
14
5 days
20
5 days
12, 18
3 day
21
Spring
break
Alkanes, alkenes, alkynes, aromatic hydrocarbons, functional
groups, polymers, amino acids
Equilibrium
Conditions, constants, Kc v. Kp, Le Chatelier’s Principle
Acids & Bases



pH, pOH, [OH-], and [H+] relationships, strong and weak
acids/bases.

Reactions of salts in water.
Reactions of acids/bases in water (proper ionic notation),
acid/base titrations.
Acid/Base titration curves, pH at endpoint, acid/base
theories.
Kinetics
st
nd
Reaction Rates, 1 order, 2 order, reaction mechanisms,
catalysis
Electrochemistry
Galvanic cells, standard reduction potential,
cell potential, work, free energy, concentration effects,
batteries, corrosion, electrolysis
Solutions
Colligative Properties, composition and concentration,
energetics, Raoutl’s law, BP elevation, FP depression,
osmotic pressure
Ksp, common ion effect, complex ion,
Nuclear Chemistry
Alpha and beta decay, radioactivity,
mass – energy calculations, fusion and fission,
rate of decay, ½ life
-Synthesis, Isolation, and
Purification of an Ester
(22.Flinn Science Kit #22)
-Determining an
equilibrium constant
(10.15B)
Le Chatelier’s Principle
simulation
-Acid versus Hydroxide
Titration, including
weak acid and base.
(6,7,11.17B)
- Buffer virtual lab (19.
summerlin chem.. demo.
Vol 2 page 713)
-Iodine or sulfur clock
reaction
(12.14)
-Predicting REDOX
Reactions
Determination of
electrochemical series.
(20)
Measurements using
electrochemical cells and
electroplating (21)
- Freezing Point
Depression (4.12a)