Download AP Syllabus 95-96 - Bremen High School District 228

5/2/17
AP© Chemistry
Course Syllabus 2012-13
Instructor:
Mr. Matthew Spreadbury
Course Number:
440
Course Description
Advanced Placement Chemistry is designed to be the equivalent of the general chemistry course usually
taken during the first year of college. Students should attain an understanding of the fundamental
principles of chemistry appropriate for this level. They should also achieve competence in using
calculations to solve chemical problems and in formulating chemical principles mathematically.
Topics of instruction include Structure of Matter (atomic theory and structure, bonding, nuclear chemistry),
States of Matter (gases, liquids, solids, solutions), Reactions (reaction types, stoichiometry, equilibrium,
kinetics, thermodynamics), Descriptive Chemistry (periodic and group properties and relationships,
organic chemistry).
The laboratory component of the course includes both qualitative and quantitive laboratory work
comparable to that typically done at the college general chemistry level. Students will usually work with a
partner to perform procedures using common laboratory apparatus and instruments, make observations
and collect data, perform additional analysis and manipulation of the data, and submit a laboratory report.
Students will also be required to maintain a lab notebook and/or portfolio of lab reports.
A student lab fee is assessed and students may be required to purchase supplementary books or
materials. A scientific calculator is strongly recommended. The Advanced Placement Exam is given in the
spring, and students who perform well may be granted credit and/or placement by their college or
university.
Due to the time required for adequate laboratory experience, this course is scheduled as a double period
class daily.
Credit: 2 credits, AP level
Grade level: 11, 12
Prerequisites:
1. Successful completion of Biology and Chemistry, at least one of which is at the honors level, or
approval of instructor.
2. Grade average of B or getter in all previous science classes, or approval of instructor.
3. Recommendation of the science teacher in the course immediately preceding the AP course.
4. Approval of the current AP teacher, based on the above prerequisites and other criteria such as
overall academic record and any other pertinent information.
Textbooks
Zumdahl, Steven and Zumdahl, Susan. Chemistry, Seventh Ed., Houghton Mifflin 2007
(This is a widely-accepted AP Chemistry textbook that uses a clear writing style and a conceptual approach to problem-solving.)
Shakhashiri, Bassam. Workbook for General Chemistry. Stipes 2004
(This workbook provides support for problem solving in all major topics.)
Laboratory Manuals
A collection of labs from various sources is used. The sources include:
Experimental Chemistry, Hall; Houghton Mifflin, 2007
Chemical Principles in the Laboratory, Masterton, Slowinski, Wolsey; Saunders, 2003
Chemistry with Computers, Holmquist and Volz; Vernier, 2003
Laboratory Experiments for Advanced Chemistry, Vonderbrink; Flinn, 2005
Laboratory Experiments for Chemistry The Central Science, Nelson, Kemp; Prentice Hall, 2006
AP Chem Syllabus
AP Curricular Requirements for Chemistry
The course outline includes abbreviated references to these five major content areas:
C1: The course provides instruction in each of the five content areas outlined in the Course Description,
the first of which is Structure of Matter (Atomic theory and atomic structure, Chemical bonding).
C2: The course provides instruction in each of the five content areas outlined in the Course Description,
the second of which is States of Matter (Gases, Liquid and solids, Solutions).
C3: The course provides instruction in each of the five content areas outlined in the Course Description,
the third of which is Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and
Thermodynamics).
C4: The course provides instruction in each of the five content areas outlined in the Course Description,
the fourth of which is Descriptive Chemistry (including relationships in the periodic table).
C5: The course provides instruction in each of the five content areas outlined in the Course Description,
the fifth of which is Laboratory (Physical manipulations; Processes and Procedures; Observations and
data manipulations; Communication, Group collaboration, and the laboratory report).
Course Outline
Review of Fundamentals (Summer)
A. Measurement and Significant Figures
B. Nomenclature Review
C. Moles, Molar mass, Percent composition
D. Identification of Famous Chemists
Related chemical calculations:
Use of metric units in measurement, conversion, significant figures.
Calculation and conversion of mass, moles, and percent composition of compounds.
Related AP Curricular Requirements
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
Unit 1—Introduction and Chemical Reactions
(4 weeks—to approx. Sept. 21)
Ch. 2 Atoms, Molecules, and Ions
A. History of Atomic Theory
B. Modern Atomic Theory (evidence, atomic numbers and masses, isotopes)
C. Introduction to the Periodic Table
Ch. 18 Nuclear Chemistry
A. Radioactive decay, half-lives
B. Nuclear equations
C. Fission, fusion, transmutation
D. Applications of nuclear chemistry (medical, energy, industrial)
Ch. 3 Stoichiometry
A. Percent composition
B. Empirical and Molecular Formulas
C. Writing and balancing equations (including redox)
D. Stoichiometric calculations (mass and mole relationships, limiting reactants)
Ch. 4 Types of Chemical Reactions and Solution Stoichiometry
A. Properties and composition of solutions
B. Types of reactions (acid-base, precipitation, redox)
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AP Chem Syllabus
C. Net ionic equations
D. Solution stoichiometry
Related chemical calculations:
Rates of radioactive decay and half-lives.
Empirical and molecular formulas from analytical data.
Balancing chemical equations (including redox), stoichiometric calculations (mass, moles,
volumes, limiting reactants, percent yield)
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Chemical Formulas (empirical and molecular)
2) Resolution of Mixtures (fractional crystallization)
3) Resolution of Mixtures (chromatography)
4) Stoichiometry (mass and mole relationship in a reaction)
Related AP Curricular Requirements:
C1: Structure of Matter (Atomic theory and atomic structure, Chemical bonding).
C2: States of Matter (Gases, Liquid and solids, Solutions).
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
C4: Descriptive Chemistry (including relationships in the periodic table).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
Unit 2—Gases and Thermochemistry
(4 weeks—to approx. Oct 21)
Ch. 5 Gases
A. Gas Laws (Ideal Gas Law and related laws, Dalton’s law of partial pressures)
B. Gas stoichiometry
C. Kinetic Molecular Theory (including temperature and kinetic energy, relate to
Avogadro and Ideal gas laws, deviations from ideal behavior)
Ch. 6 Thermochemistry
A. Enthalpy
B. Calorimetry
C. Hess’ Law
D. Heat of formation, Heat of reaction
Related chemical calculations:
Gas law calculations involving pressure, temperature, volume, moles, mass, density, kinetic
energy, ideal and non-ideal behavior. Thermochemistry calculations involving heats of formation
and heats of reaction, Hess’ Law, calorimetry, heat stoichiometry.
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Molar Mass of a Volatile Liquid (vapor density method)
2) Molar Volume of a Gas
3) Calorimetry (specific heats and calorimeter constant)
4) Calorimetry (enthalpy change for a reaction)
Related AP Curricular Requirements
C2: States of Matter (Gases, Liquid and solids, Solutions).
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
Unit 3—Atomic and Electronic Structure, Bonding
(3 weeks—to approx. Nov 14)
Ch. 7 Atomic Structure and Periodicity
A. Development of atomic structure, Bohr model, spectra
B. Quantum mechanical model (quantum numbers, energy levels, atomic orbitals)
C. Development of the Periodic Table
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AP Chem Syllabus
D. Periodic properties and groups properties (atomic radii, ionization energies, electron
affinities, oxidation states)
Ch. 8 Bonding: General Concepts
A. Electronegativity and bond polarity and type
B. Ionic and covalent bonding
C. Valence bond model—Lewis structures, resonance, VSEPR
D. Molecular geometry, dipole moments, relate structure to properties, structural
isomerism
Ch. 9 Covalent Bonding: Orbitals
A. Hybrid orbital model
B. Sigma and Pi bonds
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Hydrates: Properties and Composition
2) Molecular Geometry (models)
3) Preparation and Analysis of a Coordination Compound (4 hours)
Related AP Curricular Requirements:
C1: Structure of Matter (Atomic theory and atomic structure, Chemical bonding).
C4: Descriptive Chemistry (including relationships in the periodic table).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
Unit 4--Liquids, Solids, Solutions
(4 weeks—to approx. Dec. 15)
Ch. 10 Liquids and Solids
A. Intermolecular forces (dipole forces, van der Waals forces, London dispersion forces,
hydrogen bonds)
B. Structure of solids (as related to crystal type)
C. Properties and bonding in solids (including metallic bonds)
D. Phase diagrams, changes of state, critical and triple points
E. Energy and changes of state (heat of vaporization, heat of fusion, specific heat,
heating and cooling curves
Ch. 11 Solutions
A. Concentratipn
B. Types of solutions and factors affecting solubility
C. Raoult’s law
D. Colligative properties (boiling point elevation, freezing point depression, osmotic
pressure, vapor pressure lowering)
E. Nonideal solutions
Related chemical calculations:
Energy and changes of state.
Solution concentration and solubility, vapor pressure, boiling point elevation, freezing point
depression, osmotic pressure.
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Molar Mass by Freezing Point Depression
2) Beer’s Law (spectrophotometric determination of concentration)
3) Gravimetric Determination of Sulfate
Related AP Curricular Requirements:
C1: Structure of Matter (Atomic theory and atomic structure, Chemical bonding).
C2: States of Matter (Gases, Liquid and solids, Solutions).
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
Unit 5--Kinetics and Equilibrium
(7 weeks—to approx. Feb 28)
Ch. 12 Chemical Kinetics
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AP Chem Syllabus
A.
B.
C.
D.
Reaction Rates
Rate Laws (differential and integrated forms)
Use of experimental data and graphical analysis to determine rate law
Factors affecting reaction rates (temperature, concentration, activation energy,
catalysis)
E. Mechanism of reaction, rate-determining step
Ch. 13 Chemical Equilibrium
A. Dynamic equilibrium, LeChatelier’s principle
B. Equilibrium constants (Kp and Kc)
Ch. 14 Acids and Bases
A. Acid-base theories (Arrhenius, Bronsted, Lewis)
B. Equilibrium constants (Ka, Kb, Kw, Ksp)
C. pK, pH, pOH
Ch. 15 Applications of Aqueous Equilibria
A. Common ion effect, buffers, hydrolysis
B. precipitation and solubility (Ksp)
C. Titration and pH curves
Related chemical calculations:
Differential and integrated rate laws, rate constants, activation energy, times for reactions,
amounts of reactants/products used/formed.
Equilibrium constants and amounts of reactants/products in terms of pressures and
concentrations, weak acid and base equilibria, pH and pOH, buffer concentrations and pH,
solubility and Ksp, titration calculations.
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Reaction Kinetics (reaction rate and order, Ea, catalysis) (4 hours)
2) Determination of an Equilibrium Constant
3) Standardization of a Base and Titration of a Weak Acid (4 hours)
4) Preparation and Properties of Buffers
5) Acid-Base Indicators and pH
Related AP Curricular Requirements
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
C4: Descriptive Chemistry (including relationships in the periodic table).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
Unit 6--Thermodynamics and Electrochemistry
(3 weeks—to approx. Mar 21)
Ch. 16 Spontaneity, Entropy, and Free Energy
A. Second Law of Thermodynamics, entropy
B. Free energy and spontaneity
C. Free energy as related to entropy, enthalpy, and temperature.
D. Free energy and equilibrium constants
Ch. 17 Electrochemistry
A. Galvanic cells and cell potentials
B. Electrolytic cells
C. Electron transfer in redox reactions
D. Nernst equation, cell potentials and concentration
Related chemical calculations:
Entropy, enthalpy, free energy, spontaneity of reactions, equilibrium constants.
Cell potentials, Nernst equation and concentrations.
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Redox Titration of Iron
2) Electrochemical series
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AP Chem Syllabus
3) Electrochemical cells
Related AP Curricular Requirements
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
Unit 7--Descriptive Chemistry (3 weeks—to approx. Apr. 14)
Ch. 19 The Representative Elements: Groups 1A through 4A (1, 2, 13, 14)
A. Hydrogen
B. Alkali metals
C. Alkaline Earth metals
D. Boron group (13)
E. Carbon group (14)
Ch. 20 The Representative Elements: Groups 5A through 8A (15,16,17,18)
A. Nitrogen group (15)
B. Oxygen group (16)
C. Halogens (group 17)
D. Noble gases (group 18)
Ch. 21 Transition Metals and Coordination Chemistry
A. Properties of first-row transition metals
B. Coordination chemistry (bonding, structure and isomers)
Ch. 22 Organic and Biological Molecules
A. Hydrocarbons
B. Functional groups (properties, and typical reactions)
C. Polymers
Laboratory Experiments (each 2 hours unless otherwise noted):
1) Inorganic Qualitative Analysis (4 hours)
2) Preparation and Analysis of Aspirin
Related AP Curricular Requirements:
C1: Structure of Matter (Atomic theory and atomic structure, Chemical bonding).
C3: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, and Thermodynamics).
C4: Descriptive Chemistry (including relationships in the periodic table).
C5: Laboratory (Physical manipulations; Processes and Procedures; Observations and data
manipulations; Communication, Group collaboration, and the laboratory report).
POLICIES ON GRADES, ATTENDANCE, ASSIGNMENTS, AND RELATED ITEMS:
AP courses are college level courses offered in a high school setting. This requires some compromise in
the handling of routine matters, such as attendance and makeup work. Stated below are certain policies
for this course. Some flexibility may apply in special circumstances and students are encouraged to
discuss any such problems with the instructor.
Students who miss class should plan to make up exams, quizzes, and labs promptly upon return to
school. Make up work must be done outside of class time, usually after school, so that a student who has
already missed class does not miss even more class time. Since this is a 2-period class, make up exams
and/or labs may require up to two hours after school. Students who miss class for field trips, vacations, or
other planned activities not related to illness or emergency should get assignments and make plans with
the instructor in advance of the absence.
Exams: Tests may be given by chapter or by topic (multiple chapters), and will be the major component
of the grade.
Quizzes: Quizzes may be for short topics or entire chapters.
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AP Chem Syllabus
Written Assignments: Problem/question sets, either from the text or from other sources, will be
assigned regularly. Some will be checked for completeness of effort (a reasonable attempt to answer
every question) and discussed in class. Others will be collected and graded. Students are expected to
routinely do work on time, and to do make up work promptly. Missing, incomplete, and/or late
assignments will be penalized.
Projects: Several special projects will be required. More information about these is provided
separately.
Laboratory Assignments: Labs will often relate to the lecture topic, and will be graded on the results
(precision and accuracy), the report, and the notebook. Students are expected to follow guidelines for lab
notebooks and safety (provided separately from this syllabus), and failure to do so will be reflected in the
lab component of the grade.
EVALUATION:
Points for each assignment will be recorded. The grade for each grading period will be determined by the
student’s percentage of the possible points, according to the following scale:
80% = A
70% = B
60% = C
50% = D
The first semester grade will be weighted 1/5 on the semester exam and 4/5 on the percentage of
possible points for the full term, determined according to the same scale. There is no final exam for the
second semester, and the grade will be determined solely by the percentage of possible points (same
scale).
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