AP CHEMISTRY SYLLABUS
ANDRE 2011-2012
PREREQUISITES:
Successful completion of either Pre-AP Chemistry or both Integrated Science I and II, and Algebra I.
TEXT:
CHEMISTRY by Zumdahl and Zumdahl, 8th Edition, Advanced Placement Edition, Houghton Mifflin Co.,
2010. ISBN-13: 9780547168173 ISBN-10: 0547168179.
Chemistry, Principles and Reactions, 5th ed., Thomson/Brooks/Cole, 2006. ISBN: 0495011401. (Reference)
CLASS WEBSITE: www.nhscrazy4chem.pbworks.com
INSTRUCTOR EMAIL: basma.andre@browardschools.com
GOALS:
▫ Students will improve their analytical reading and problem solving skills.
▫ Students will be able to safely and efficiently conduct laboratory experiments using appropriate lab apparatus/materials in order to make meaningful observations, collect and isolate meaningful data, analyze that data over a broad topic range to verify or reject hypotheses, as well as to be able to report findings formally and informally.
▫ Students will be aware of the interconnection of chemistry to all the other sciences.
▫ Students will earn an acceptable score on the AP Chemistry test in May.
COURSE NOTEBOOK:
Students will be required to outline (handwritten) each chapter before it is discussed in class. Key vocabulary words MUST be highlighted throughout the notes. Chapter outline notes will be due on the 1 st
day of lecture for that chapter. Chapter notes will be graded as homework. A 2”-3” 3-ring binder will also be required. All course materials, including notes, homework, practice problems, etc will be kept in this binder. All material is to be sorted by topic using dividers in the binder. The course notebook will be checked for a grade at least once per semester (more frequently at the instructor’s discretion).
VOCAB QUIZZES:
Every week (the last class day of that week) students will be given a vocabulary quiz on concept vocabulary.
The quizzes will assess 3 vocabulary words (5 points each). There will be an emphasis on definition and understanding of the concept. Vocabulary words assessed will be cumulative throughout the year.
CHEM CARDS:
During a chapter lecture students will write down important AP concepts on a large index card (5” x 8”).
Students may use front and back. Chem cards will be collected for all chapters covered during a unit on the day of the unit test. Chem cards will be graded and place an emphasis on active listening and participation during lecture. Chem cards are to be kept in the course notebook.
FRQ GROUPS:
At the conclusion of a chapter students will be assigned into groups of 4 by the instructor. In groups, students will complete AP free response questions (FRQ) assigned by the instructor. The following class each group will present answers to the free response question selected by the instructor. Grading will be based on participation of all group members and accuracy to answers of the question.
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HOMEWORK:
Homework will be due on the class after it is assigned. Homework will be assigned as practice for the quizzes and tests. Late homework will not be accepted under any circumstances. Homework is to be completed on loose-leaf paper (unless otherwise instructed by the instructor) in your course notebook.
LABORATORY NOTEBOOK:
The laboratory notebook is mandatory and should be brought to class the day before and the day of the laboratory experiment. Labs are to be completed on lined paper (graph paper is acceptable) in the same color ink and kept in a 3-prong folder. Missed labs must be made up after school.
TESTS/QUIZZES:
Tests and quizzes will be prepared using multiple AP Chemistry resources. Most tests will be prepared using a format similar to that of the AP Chemistry Exam (part multiple choice and part problem-solving). Quizzes will given at the instructor’s discretion (they will be announced ahead of time). Tests given will be unit tests that will cover more than one chapter. The chapters covered by a test will be held to the discretion of the instructor.
*If a student is absent on the day of a test, it MUST be made up in class on the day they return to class.
*If a student is absent for a test review day, the student must still take the test as scheduled.
GRADE DISTRIBUTION:
Tests/Labs 60%
Vocab Quizzes
Homework/Notebook
10%
10%
FRQ Presentations
Chem Cards
10%
10%
MATERIALS:
2”-3” Binder
Dividers (at least 20)
Loose-leaf Paper
3-Prong Folder (lab folder)
Large Index Cards (5” x 8”)
Scientific calculators
Writing utensils (both pens and pencils)
Highlighters and colored pencils are highly encouraged for note-taking.
*If financial assistance is needed for course materials please speak to the instructor privately for the proper accommodations. Otherwise materials are expected to be in class everyday.
ATTENDANCE:
Attendance in a timely fashion to class is mandatory. If a student is caught skipping class an administrative referral will be issued and no make-up work will be accepted. It is the student’s responsibility to find out what was missed in class from a peer in class. The student will have 2 school days to turn in make-up work. Also, after the first tardy the student will be given a verbal warning. In the event of a second tardy the student will receive a Saturday detention.
STUDENT CONDUCT:
Students will abide by all rules in the Student Code of Conduct at all times. Any disruptive or disrespectful behavior in class will result in consequences such as contact home, after school detention, or an administrative referral.
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SEMESTER I COURSE CONTENT:
STRUCTURE OF MATTER
Atoms, Molecules, and Ions – 1 day (review) Chapter 02
Development of atomic theory, atomic structure, effective use of the periodic chart, predicting oxidation numbers, writing formulas (molecular and ionic)
Matter and Measurement – 1 day (review)
Significant figures, metric conversion, dimensional analysis setup, uncertainty in measurement
Chapter 01
Electron Configuration and the Periodic Table – 4 days Chapter 07 light, photons, and atomic spectra, dual nature of light, E=hv=hc/wavelength, Bohr’s model using hydrogen, spectrum analyses, use of both Rydberg and Bohr constants in calculations of E, excited vs. ground state, electron configuration, Heisenberg Uncertainty Principle, Hund’s Rule, Pauli Exclusion Principle (spin),
Aufbau Principle, use of the periodic chart to predict expected electron configuration as opposed to diagonal rule, electron configurations of monatomic ions, quantum numbers, and periodic trends for the comparison of atomic radii, ionic radii, electronegativity, and ionization energy
Covalent Bonding and Molecular Geometry – 4 days
Increased stability with electron pairing, valence electrons, Lewis
Chapter 08 structures, types of covalent bonds, octet rule, S=NA, resonance, octet rule and exceptions, expanded octets,
VSEPR modeling, prediction of geometry of molecules and the reasons this is important, effect of unshared electron pairs and numbers of bonded atoms on a central atom on molecular geometry, bond polarity, atomic orbitals and hybridization, sigma and pi bonds, molecular orbital theory and calculation of bond order.
Nuclear Chemistry – TBA Chapter 19
Half-life, alpha and beta decay, gamma radiation, positron emission, electron capture, fission and fusion.
Unit Test #1
INTRO TO REACTIONS
Stoichiometry – 5 days_______________ Chapter 03
Atomic mass determination from relative abundances of isotopes and molar masses from formulas, mole relationships, mass relations in chemical formulas mass %, balancing equations, using balanced equations to predict yield, limiting reactants, % yield
Reactions in Aqueous Solutions – 5 days________ Chapter 04
Precipitation reactions based on rules of solubility, introduction of acid/base reactions, REDOX reactions, writing of balanced molecular and NET ionic equations, as well as equations for more sophisticated REDOX reactions, molarity, molality, normality, solution stoichiometry (heavy emphasis on limiting reactant problems)
Unit Test #2
STATES OF MATTER
Gases – 4 days________________________ Chapter 05
Kelvin temperature, STP, units of pressure, gas laws (Charles’, Boyles”, Gay Lussac’s, mixed, ideal, Grahams
Law of Effusion, average speed, calculations involving all laws, stoichiometry of gaseous reactions, molar mass and density calculations as versions of ideal gas law, mole fractions, Dalton’s law of partial pressures, calculations involving collection of gases by water displacement (water vapor pressure effect), kinetic theory of
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gases, calculations to determine average speed as function of molar mass, derivation of time and distance effusion laws from rate law, conditions for deviation from ideal gas law.
Liquids and Solids – 4 days_______________ Chapter 10
Molecular compounds and general characteristics, intermolecular forces (dispersion forces, dipole forces, hydrogen bonding (N, O, F), network covalent, ionic, and metallic solids examples and characteristics of, calculations involving simple unit cells, liquid vapor equilibrium, vapor pressure defined and the influence of temperature on vapor pressure (Clausius Clapeyron), boiling, melting, and freezing points, critical temperature and pressure defined, interpretation of and construction of phase diagrams
Solutions – 4 days________________________ Chapter 11
Molarity, mole fraction, mass %, molality, mole fraction, ppm, molarity molality conversions, solubility, temperature effects on solubility of gases, colligative properties defined, non-electrolytes vs electrolytes, effect of solutes on f. pt. and b. pt., Van’t Hoff factor, effect of solutes on vapor pressure, osmotic pressure, calculation of molar mass from colligative properties
Unit Test #3
REACTIONS
Thermochemistry – 4 days_______________________ Chapter 06
Principles of heat flow (system vs. surroundings), enthalpy defined, significance of the sign on answers to heat flow calculations, magnitude of heat flow, joule/kilojoules/calories as units of heat energy, q=ms(deltaT), coffee cup and bomb calorimetry principles and calculations, writing appropriate thermo-chemical equations, stoichiometric calculations, application of First Law of Thermodynamics, applications of theories to gases
Chapter 17 Spontaneity of Reaction – 2 days___________________
Definition of spontaneous reactions, entropy, entropy changes and computations, free energy, Gibb’s free energy, effects of temperature, pressure and concentration on reaction spontaneity, coupled reactions
Reaction Rate/Chemical Kinetics – 2 days____________ Chapter 12
Definition, measuring rate, effect of concentrations of reactants on rate, rate expressions and rate constant, order of reaction defined, calculation of reaction order when two rates are known with only a single reactant, order of reaction with more than one reactant, reactant concentration and time, half life calculations, zero and second order reactions, models for reaction rate, reaction rate and temperature, Arrhenius equation, catalysis, reaction mechanisms and rate determining steps, deduction of rate expression from a proposed mechanism.
Unit Test #4
SEMESTER II COURSE CONTENT:
Gaseous/Chemical Equilibrium – 5 days________________ Chapter 13
Defining equilibrium, N
2
O
4
NO
2
equilibrium system, equilibrium constant expression, reciprocal rule, rule of multiple equilibria, k as a function of partial pressures or molarity, applications of the equilibrium constant to determine trends in the equilibrium system, comparison of “Q” and Kc, effect of changes on the equilibrium system, Le Chatelier Principle, relationship of Kp and Kc
Precipitation Equilibria – 3 days____________ Chapter 16
Equilibria in precipitation reactions, Ksp and solubility in water, common ion effect on solution equilibria, dissolving of precipitates using acids or bases (strong acid anion to react with basic anions or complexing agent such as NH3 or OH to react with metal cations)
Unit Test #5
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Acid/Base Chemistry – 4 days______________________ Chapter 14
Various definitions of acids/bases, conjugate acids/bases, amphoteric/amphiprotic defined, dissociation of water molecules into ions, Kw, pH and pOH, relationship of pH and pOH to Kw, strong/weak acids and bases, Ka and
Kb used to determine molar concentrations in aquatic solutions, polyprotic acids and their subsequent Ka’s, acid/base properties of salt solution, neutralization reactions of acids and bases (again).
Buffer Systems – 2 days Chapter 15
Calculations from titration data, indicators, choosing appropriate indicators, buffers and buffer systems, calculations of [H+] and [OH] in buffer systems, “worrying’ a buffer system (calculations of pH and pOH after addition of certain compounds, breaking a buffer system.
Electrochemistry – 3 days__________________________ Chapter 18
Voltaic cells, zinc/copper connection, anode/cathode reactions, function of salt bridge, identification of parts of the voltaic cell, identification of oxidation/reduction reactions, cell notation, cell voltage related to spontaneity, standard voltage, standard voltage for overall reactions, determination of spontaneity in a reaction, stand free energy changes
Unit Test #6
DESCRITPIVE CHEMISTRY
Organic Chemistry – TBA _____________ Chapter 22
General characteristics, alkanes, alkenes, alkynes, basic functional groups (halogens, alcohols, ketones, aldehydes, ethers, esters, carboxyl groups, amines, amides), benzene, and basic naming of organic compounds.
The Representative Elements – TBA Chapter 20
A very descriptive chapter with emphasis on writing equations for reactions with nonmetals. Also covers reactivity of common nonmetals and molecules.
Transition Metals & Coordination Chemistry – TBA Chapter 21
A very descriptive chapter which concentrates upon the chemistry of transition metals on one hand and transition metals on the other.
Covalent Bonding: Orbitals – TBA Chapter 15
A closer look at hybridization and the localized electron model. Also a look at the Molecular Orbital Model.
Unit Test #7 (If time allows)
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LABORATORY TECHNIQUES
*Lab topics are subject to change based on equipment and lab availability (2hr 50 minute/lab) .
#1 Introduction/Safety & Lab Technique
#2 Physical Properties
#3 % Barium chloride dihydrate
#4
Boyle’s Law and Gases
#5 Determination of Empirical Formula
#6 Chemical Reactions
#7 Molar Volume of Oxygen and Weight of Mg
#8 Electrolytes
#9 Evaporation
#10 Formula Weight of a Volatile Liquid
#11 Acid/Base Titration
#12 Redox Titration
#13 Calorimetric Determination of Iron
#14 Qualitative Analysis Chloride Group
#15 Qualitative Analysis Basic Sulfide Group
#16 Qualitative Analysis Soluble Group
#17 Qualitative Analysis Unknown
#18 Qualitative Analysis Unknown
#19 Calorimetry
#20 Kinetics of a Chromium EDTA Complex
#21 Iodine Clock
#22 Acid/Base Titration
#23 Electrolytic Cells
#24 Organic Functional Groups
*This syllabus is tentative and subject to change based on the instructors discretion in order
to better serve students.
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AP CHEMISTRY SYLLABUS
ANDRE 2011-2012
Acknowledgement Form
Student Name (print) ________________________________________ Period ____
Parent/Guardian Contact Information
Parent/Guardian Name 1 (Print) ________________________________________________
Parent/Guardian Name 2 (Print) ________________________________________________
Parent/Guardian Contact #1 ________________________________________________
Parent/Guardian Contact #2 ________________________________________________
Parent/Guardian Email(optional)________________________________________________
I acknowledge that I have received, read, and understand all components of the AP Chemistry
Syllabus attached for the 2011-2012 school year.
Parent/Guardian Signature Date
______________________________________ ________________
Student Signature Date
______________________________________ _________________
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