Vasquez High School -- AP Chemistry -- Syllabus -- 2013 - 2014
Instructor: Jeff Berkeley, M.S.
MAIN TEXT: Chemistry, 8th Edition, Raymond Chang, McGraw-Hill, 2005, ISBN 0-07-293027-6
Supporting Materials:
1) Student Study Guide and Student Solutions Manual for Chang, ISBNs 0-07-254993-9 and 0-07-254992-0
2) Chemistry: The Central Science, 11th Edition, Brown, LeMay, Bursten, Murphy;
Pearson/Prentice Hall, 2009, ISBN 978-0-13-601250-4
3) Laboratory Experiments for Chemistry: The Central Science, 11/E
Brown, LeMay, Bursten, Murphy, Woodward, Nelson & Kemp
©2009 | Prentice Hall | Spiral Bound; 616 pp
ISBN-10: 0136002854 | ISBN-13: 9780136002857
4) Instructor Resource DVD/CD-ROM for Chemistry: The Central Science, 11/E
Brunauer, Cook, Kreuz, Chatellier & Bookstaver
©2009 | Prentice Hall | Multiple Media Package
ISBN-10: 0136002811 | ISBN-13: 9780136002819
5) Instructor Resource Manual for Chemistry: The Central Science, 11/E
Brown, Brunauer & Cook ©2009 | Prentice Hall | Paper; 384 pp
ISBN-10: 0136002374 | ISBN-13: 9780136002376
6) AP Exam Workbook for Chemistry: The Central Science, 11/E
Brown & Waterman ©2009 | Prentice Hall | Paper; 464 pp
ISBN-10: 0136002846 | ISBN-13: 9780136002840
7) Solutions to Exercises for Chemistry: The Central Science, 11/E
Wilson & Brown ©2009 | Prentice Hall | Paper; 752 pp
ISBN-10: 0136003257 | ISBN-13: 9780136003250
8) Online Resources for Both Students and Instructor to be found at:
http://wps.prenhall.com/wps/media/access/Pearson_Default/5524/5656731/login.html
9) Online Homework and Grading via http://www.webassign.net/
10) Instructor’s Website at http://www.jeffberkeley.com
11) Instructor’s Personal Library of chemistry texts, demonstration modules, pedagogical tools and software
This advanced placement course in chemistry is to be taught at the freshman university level, and as such
requires the dedication and focus worthy of such an endeavor. In general, emphasis will be placed in the areas
of the structure of matter (atomic theory and atomic structure, chemical bonding), states of matter (gases, liquids
and solids, solutions), reactions (reaction types, stoichiometry, equilibrium, kinetics, thermodynamics),
descriptive chemistry (relationships and trends in the periodic table), laboratory (physical manipulations,
processes and procedures, observations and data collection and manipulation, intra- and inter-group
communication, group collaboration, and the laboratory report), and an increased focus on calculational skills.
These six areas and more are covered in the outlined syllabus that follows. Throughout the outline, they are
annotated belonging to the six areas (plus demos) using the following legend:
C1 = the structure of matter
C2 = the states of matter
C3 = reactions
C4 = descriptive chemistry
C5 = laboratory skills and exercises
C6 = calculational skills
C7 = applicable demonstrations
STUDENT REQUIREMENTS AND POLICIES:
1) Students should be in class on time and prepared with all of the necessary materials: books, calculators, AP study guides, etc.
2) Students will bring in a bound class notebook, to be turned in at the end of each semester, that will include all class notes, organized in such a way as to facilitate a comprehensive and progressive understanding of the material.
3) Students will also keep a detailed lab notebook to be turned in periodically. Lab notebooks are to include all collected data, labelled and dated, and demonstration notes, including materials, observations, equations and conclusions.
4) Students are required to participate in all labs; make-ups will be provided.
5) Students are required to do their assigned homework when assigned and with due care. Collaboration amongst students is not preferred but will be allowed if the collaborative instruction is done without plagiarism. Late or incomplete homework is granted at best half-credit.
6) If a student is absent, they will have that many extra days to make up homework or lab reports. Students will be allowed to make up exams provided they have an excused absence.
7) It is higly recommended that students download and review chapter study questions and answers from instructor’s website before each chapter exam. These questions are a culled combination of publisher’s and instructor’s resources.
8) Students will prepare for the AP chemistry exam given in May and will dedicate themselves to passing the exam with a score of 4 or 5. Students who score a 4 or 5, and who have completed all required
assignments throughout the year, will automatically receive a grade of A for the spring semester.
Students who score a 3 and have also completed said assignments will gain a bonus of one-half grade
to their spring semester grade.
I. Introduction and Review
A.
Safety rules and procedures [C5]
B.
The Scientific Method [C6]
C. Branches and careers in chemistry [C4]
D.
Scientific Notation [C6]
E.
Accuracy, precision, significant figures [C6]
F. Control vs. test and other types of experimentation [C5]
II. Measurement [C5,6]
A. System Internationale units (SI) vs. English units
B.
Metricsystemand prefixes
C. Dimensional analysis conversions and technique
D. Percentage error calculation
E. Density, area, and volume calculations
F. Temperature scales and conversions
III. Matter [C2,3]
A. Mass vs. weight
B. Hetero- vs. Homogeneous matter [C1]
C. Extensive, intensive, physical and chemical properties [C1]
D. Phases of matter and changes in phase [C2,7]
E. Physical vs. chemical changes in matter [C2,3,7]
F. Elemental occurrences in nature, ores, minerals [C1,4]
G. Laws of conservation of matter/energy [C2,5,7]
H. Compounds vs. mixtures [C1]
IV. Energy [C2,3,6]
A.
Definitions and units of energy, work, joules
B. Kinetic vs. potential, types of potential [C3]
C. Endothermic vs. exothermic [C3,5,7]
D. Forms of energy, changes in form
E. Heat vs. Temperature, cal, kcal, Cal, kinetic theory of matter [C2,3,4,6,7]
F.
Activation energy, calorimetry, specific heat capacity [C5]
G.
Specific heat calculations [C6]
H.
Electrostatic forces, current, voltage, resistance, insulators, conductors
V. Gases
A.
B. C. D. Pressure defined, various units of pressure
Atmospheric pressure, barometer, manometer [C5]
Standard temperature and pressure (STP) [C3,5,6,7]
Boiling, melting, viscosity, changes in water [C2,5,6,7]
VI. The Gas Laws [C2,3,5,6,7]
A. Boyle’s Law (PV = k), Charles’ Law (V = kT), combined laws (PV = kT) with calculations
B. Dalton’s Law of partial pressures
C. Graham’s Law of Diffusion (relative particle velocities)
D. Avogadro’s hypothesis and number
E. Mole concept, molar volume and calculations [C3,6,7]
F. Kinetic theory, “ideal” gases, PV = nRT
VII. Liquids and Solids [C2,3,4,5,6,7]
A. Mechanism of Evaporation [C2]
B. Vapor vs. Gas, volatility, vapor pressure [C2]
C. Liquid-vapor equilibrium and pressure at equilibrium [C2]
D. What is Boiling? [C2]
E. Liquefaction, critical temperature and pressure [C2,4]
F. Heats of vaporization, condensation, fusion, and crystallization
G. Fractional distillation, hydration, cracking and related terms [C4,5,7]
VIII.
Atomic Structure and Theory (Part 1) [C1,4]
A. Democritus, Lavoisier, Proust, Dalton, etc.
B.
Atomos, conservationof matter experiments, laws of definite and multipleproportions
C.
Dalton’s Modern Atomic Theory (1803) and its limitations
D. Crookes, Thomson, Millikan, Rutherford, Chadwick
E. Crookes tube, anode, cathode, cathode ray tubes
F. Charge-to-mass ratio of an electron - Oil Drop experiment
G. Discovery of the nucleus - Gold Foil experiment
H. Relative charges and masses of subatomic particles
I. Isotopes, avg. atomic masses, notation, important carbon and hydrogen isotopes
J. Atomic number vs. atomic mass
K. Waves and their characteristics (amplitude, wavelength, crest, trough, frequency, velocity, etc.)
L. Electromagnetic spectrum [C4,6]
M. c = ln, E = hn (or c = lf and E = hf) [C6]
IX. Atomic Structure and Theory (Part 2) [C1,4]
A. Four branches of mechanics
B. Planck, Einstein, de Broglie, Heisenberg, Schroedinger, Bohr, Roentgen, Becquerel, Curie, Pauli
C. Wave particle duality of nature, exclusion principle, uncertainty principle, quantum theory, Hund’s Rule
D. Ground state, excited states, standing waves, nodes, modes of vibration, spectroscopy
E. Four quantum numbers for each electron (principal, sublevel, orbital, spin)
F.
Electron configurations, valence shell electrons
G. Kernel concept, electron clouds, quantum mechanical probabilities [C1,4]
H.
X-rays, transmutation, radioactivity (alpha, beta, gamma radiations), fission, fusion
I. Half-life calculations, nuclear equations, rates of nuclear decay [C6]
X. Chemical Bonding (Part 1) [C1,4]
A. Chemical bonding, reactions and valence electrons [C1,4]
B. Noble gases and stable octets, octet rule and exceptions [C1,4]
C. Ionization energies, cations, anions [C1,4,6]
D.
Electron dot diagrams, Lewisnotation, configurations
E. Ionic bonding, crystal lattices, 42 crystal varieties [C1,4]
F. Covalent bonding, coordinate covalency, resonance [C1,4]
G. Metallic bonding, hydrogen bonding, Van der Waals forces, London forces [C1,4]
XI. Chemical Bonding (Part 2) [C1,4]
A. Electronegativity and the magic 1.7
B. Polar vs. non-polar compounds [C1,4,5,7]
C. Molecules and network solids, ionic crystals, Bragg equation, diamagnetism and
paramagnetism [C1,4]
D. The VSEPR model, hybrid orbitals, pi and sigma bonds, bond order
E. Polyatomic ions, old vs. new names for cations [C1,4]
F. Bond energies, bond angles, bond geometries
XII. The Periodic Table [C1,4]
A. Dobreiner, Newlands, Meyer, Mendeleev et al
B. Periodicity and the Periodic Law [C1,4,5,7]
C. Periods, groups, families - trends and characteristics, compare and contrast [C1,4]
D.
Ionic radii, cations vs.anions,electron affinity, atomic sizes[C1,4]
E. Metals, non-metals, metalloids [C1,4,7]
XIII. Chemical Formulas [C1,3,4,6]
A. Empirical formulas, molecular formulas, valences of ions, multivalent ions (old vs. new names) [C1,4,5,6]
B.
Naming of compounds, prefixes, suffixes, per-, hypo-, -ous, -ic, binary, ternary compounds
C. Coordination compounds, ligands, metallic bonds, isomerism
XIV. Chemical Equations [C1,2,3,4,5,6,7]
A. Reactants vs. products
B. Balancing a chemical equation
C. Phases in chemical equations
D. Four types of chemical reactions (synthesis, decomposition, single- and double-replacement) [C1,2,3,5,7]
XV. Stoichiometry [C1,2,3,4,5,6,7]
A. The mole - Avogadro’s number
B. Molecular formula mass, formula weights [C5,6,7]
C. Percentage composition [C5,6,7]
D. Determining formula from percentages [C5,6,7]
E. Limiting reagents, theoretical yields, spectator ions [C3,5,6,7]
F. Mass-mass & mass-volume problems [C3,5,6,7]
G. Net ionic equations, redox reactions, activity series [C5,6,7]
XVI. Solutions [C1,2,3,5,6,7]
A. Characteristics of solutions, solute, solvent, solution [C1,4,7]
B. Types of solutions [C1,4,7]
C. What affects solubility, Henry’s Law, etc. [C2,5,6,7]
D. Factors affecting rate of solution [C2,4,5,6,7]
E. Solubility curves [C5,6]
F. Unsaturated, saturated, supersaturated [C4,5,7]
G. Dilute vs. concentrated [C4,5,7]
XVII.
Expressing Solution Concentrations [C4,5,6]
A. Percentage by mass
B. Mass of solute per unit volume of solution
C. Parts per million, billion, trillion
D. Molarity and molality [C5,6]
XVIII. Colligative Properties of Solutions [C4,5,6]
A. Electrolytes, non-electrolytes, vapor pressure, conductivity[C4,5,7]
B. Freezing point depression, boiling point elevation with calculations of same [C4,5,6,7]
XIX. Chemical Kinetics [C3,4,5,6,7]
A. Reaction rates and effective collisions [C1,3,4,5,6,7]
B. Hetero- vs. homogeneous reactions [C3,4,7]
C. Catalysis [C3,4,5,7]
D. Reaction mechanisms, rate-controlling steps [C3,4,5,6,7]
E. Potential energy diagrams w/activation energies w/ and w/o catalysts, activation complex
XX. Enthalpy and Entropy [C3,5,6,7]
A. Enthalpy and heat content [C3,5,6,7]
B. Heats of formation vs. stability of a compound, Hess’ Law [C3,5,6]
C. Entropy changes (DS), thermodynamic basics [C3,4,5,6]
D. Gibbs Free Energy equation, spontaneity [C3,5,6]
XXI.
Chemical Equilibrium [C2,3,4,5,6,7]
A. Reversible reactions [C2,3,4,7]
B. What is equilibrium? [C2,3,4]
C. Equilibrium constant (K eq) and the mass-action expression [C2,3,5,6,7]
D. Le Chatelier’s principle and its changes, the Haber Process [C2,3,5,6,7]
XXII.
Solubility Products [C2,3,5,6,7]
A. Solubility product K sp [C2,3,5,6,7]
B. Two uses for K sp
C. Prediction of precipitation [C2,3,5,7]
XXIII. Acids, Bases and Salts [C1,2,3,4,5,6,7]
A. Ionization vs dissociation, weak vs. strong acids and bases [C1,2,3,4,5,7]
B.
Definition of acids and bases (Arrhenius, Bronsted-Lowry, Lewis) [C4]
C.
Ionization constants of acids and bases, Ka and Kb [C3,5,6]
D. Properties, consumer uses, and preparations of common acids and bases [C4,7]
E. Four types of salts, acid-base reactions w/gas formation [C4,7]
F. Ionization of water, Kw, and calculations [C3,5,6,7]
G.
Definition andcalculation of pH, pH + pOH= 14 [C3,5,6,7]
H. Buffers, amphoterism, conjugates, titrations, indicators, neutralizations, hydrolysis, normality [C3,4,5,6,7]
XXIV. Electrochemistry [C1,3,5,6,7]
A. Redox revisited, voltaic cells, activity series potentials, half-reactions [C1,3,5,6,7]
B. Batteries, Nernst equation, EMF, corrosion, electrical work, fuel cells [C3,4,6,7]
XXV. Organic Chemistry [C1,2,3,4,5,7]
A. Structural formulas, isomers, saturated vs. unsaturated
B. Hydrocarbon chains and names [C4]
C. Benzene rings and related ideas
D. Alkanes, alkenes, alkynes, alcohols, aldehydes, ketones, ethers, esters, and organic esters [C5,7]
XXVI. Laboratory Section
Below you will find a listing of the labs we will perform during theschool year. Most we will perform “wet,”
and students are required to attend and conduct these in a timely and professional manner. A few they will be
allowed to conduct “dry” or “virtually” as facilities and time permit.
Each lab report shall be taken directly from the prescribed lab manual, unless substituted for or specified
otherwise, andpre-labquestions are to be completed before the labs begin. Students are to come prepared and
informed regarding each lab and should have questions of procedure and handling apparatus, both for safety and
operational reasons, covered before beginning the actual lab period. All collected data is to be written in
students’ lab notebook.
Lab reports shall include a title, an objective, a list of materials, a procedure, relevant pre- and post-lab
questions with answers, data collection, interpretation, and presentation, error considerations, applicable safety
considerations, and disposal techniques employed. Furthermore an overall conclusion must be included, one
intimately tied to the particular lab issue at hand.
A. B.
C. D. E. F. G. H. I. J. Finding the Ratio of Moles of Reactants in a Chemical Reaction
Identification of Alum, KAl(SO4)2 • 12H2O
An Activity Series
Thermochemistry and Hess’ Law
Molecular Mass of a Volatile Liquid
Molecular Mass by Freezing Point Depression
Vapor Pressure and Enthalpy of Vaporization of Water
Analysis of a Commercial Bleach
Determination of the Hardness of Water
Study of the Kinetics of a Reaction
K. L. M. N. O. P. Q. R. S. T. U.
V. Determination of the Solubility Product of an Ionic Compound
Determination of the Equilibrium Constant for the Formation of FeSCN2+
Determination of the Dissociation Constants of Weak Acids
Determination of the Equivalent Mass and pKa of an Unknown Acid
Equilibrium and Le Chatelier’s Principle
Determination and Comparison of Solubility Curves
Qualitative Analysis Using Paper Chromatography
Determination of Percentage Copper in an Alloy
Determination of the Formula of Various Hydrates
An Exploration Into Electrochemical Half-Cells
Laboratory Techniques for the Identification of Unknown Cations
The Preparation of Esters
XXVIII. Demonstrations
I will perform roughly four dozen demonstrations throughout the course of the school year culled from my
collection of over 500 that will supplement the student’s comprehension of chemical principles. Most of these
are either too dangerous for the students to perform in groups or are subject to limitations in the stockroom.
SCHEDULE
As a rule, students will be assigned homework three to four nights a week, plus labs, based of course on the
material being covered. Schedule is malleable, worked around the prevailing school schedule.
Week 1: Introduction and Review Week 2: Measurement
Week 3: Matter and Energy (chapter 1) Week 4: Aoms, Molecules and Ions - nomenclature (chapter 2)
Week 5: Stoichiometry (chapter 3) Week 6: Stoichiometry (chapter 3)
Week 7: Aqueous Reactions and Solutions (chapter 4)
Week 8: Aqueous Reactions and Solutions (chapter 4)
Week 9: Gases and Gas Laws (chapter 5)
Week 10: Gases and Gas Laws (chapter 5)
Week 11: Thermochemistry - part 1 (chapter 6)
Week 12: Thermochemistry - part 2 (chapter 18)
Week 13: Electronic Structure of Atoms, Modern physics/chemistry (chapter 7)
Week 14: Electronic Structure of Atoms, Modern physics/chemistry (chapter 7)
Week 15: Periodic Properties of the Elements (chapter 8)
Week 16: Basic Concepts of Chemical Bonding (chapter 9)
Week 17: Molecular Geometry and Bonding Theory (chapter 10)
Week 18: Intermolecular Forces (chapter 11)
Week 19: Properties of Solutions, Colligative Properties (chapter 12)
Week 20: Chemical Kinetics (chapter 13)
Week 21: Chemical, Acid-Base Equilibria (chapters 14/15/16)
Week 22: Chemical, Acid-Base Equilibria (chapters 14/15/16)
Week 23: Chemical, Acid-Base Equilibria (chapters 14/15/16)
Week 24: Electrochemistry (chapter 19)
Week 25: Nuclear Chemistry (chapter 23)
Week 26: Coordination Compounds (chapter 22)
Week 27: Organic Chemistry (chapter 24)
Week 28: AP Test Prep and remaining topics
Week 29: AP Test Prep and remaining topics
Week 30: AP Test Prep and remaining topics
Week 31: AP Test Prep and remaining topics