Honors Pre-A.P. Chemistry II / A.P. Chemistry -- Course Syllabus—2008-2009
Teacher: Crystal Duggar
Text: Zumdahl, S. S. and Zumdahl, S. A. (2003). Chemistry, Sixth Edition.
Boston: Houghton Mifflin Company.
Lab Manual: Hall, J. F. (2003). Experimental Chemistry, Sixth Edition.
Boston: Houghton Mifflin Company.
Course Information
Welcome to Honors Chemistry II / A. P. Chemistry! The goal of this class is
to provide the content and experiences that students would encounter in a
college-level general chemistry course. Additionally, this class will
prepare students for the A. P. Chemistry Exam, which will be given in May.
In addition to the content covered in class, students must spend significant
time each day studying and doing homework. Please seriously consider whether
or not you can make this necessary time commitment.
Both semesters of the class focus on problem-solving and application of
concepts. During the Honors Chemistry II semester, students will review
Chemistry I content and achieve a deeper understanding of those fundamental
chemical concepts. We will also introduce some new ideas that build on
Chemistry I material. In A.P. Chemistry, the second semester of the course,
students will explore the major areas emphasized on the A. P. exam that were
not introduced in Chemistry I: electrochemistry, thermodynamics, chemical
equilibria, and acid/base chemistry. Throughout the two semesters, inquiry,
problem solving, lectures, demonstrations, hands-on laboratory
investigations, individual studies and group activities will all be part of
the learning experience.
Success on the A.P. Chemistry Exam requires not only in-depth knowledge of
chemistry, but also knowledge of how to approach and answer the test.
Practice tests, test-taking skills specific to the A.P. Chemistry Exam, and
review of material prior to the exam will also be an important component of
the course.
Required Materials
In addition to the basic necessities such as pencil or pen and paper, you
will also need the following items for class and lab: scientific
calculator, large 3-ring binder and section dividers, pack of 300 note
cards, rubber gloves, dish soap, pot holder or oven mitt, roll of paper
towels and a small 3-ring binder for use as a lab notebook
Recommended Materials
A graphing calculator may be helpful as we move into the later course topics
such as kinetics and equilibrium. Students who are serious about scoring
well on the A.P. Exam should purchase an A.P. Chemistry review book. Since
publishers often release updated editions of review manuals for the new
year, we will discuss ordering a review book as a group during the second
semester.
Policies and Expectations
1. Be on time and bring all materials needed for class.
A. Be in your seat when the tardy bell rings.
B. Bring your textbook, notebook, pen or pencil, calculator and completed
homework assignments with you.
2. Be respectful.
A. Use appropriate language and make only positive or helpful comments.
B. Please hold questions or comments until your raised hand has been
acknowledged.
C. Ask before borrowing.
3. Be safe.
A. Move into, out of, and around the classroom in a safe manner.
B. Follow all safety procedures during lab activities.
C. Know the locations of emergency equipment in the lab.
4. Be honest. Cheating will result in a zero for the assignment.
Class Work
Realizing that AP Chemistry is essentially a two-semester college-level
laboratory science course, even the best students must expect to spend a
significant amount of time studying outside of class. Students should expect
to study and/or complete homework assignments every night in order to
prepare for new material and/or to reinforce concepts taught during class.
All class notes and homework should be kept in a notebook to facilitate
review for midterm and final exams and the A.P. Chemistry exam.
Grading
The honors grading scale is as follows: The A.P. grading scale is as
follows:
90-100 A 90-100 A
82-89 B 80-89 B
72-81 C 70-79 C
67-71 D 65-69 D
below 67 F below 65 F
Grade percentages are as follows: tests 65%, labs 25%, of the , homework
and quizzes will make up the remainder of the grade. Students may do test
corrections for credit, but the corrections must be done in the classroom
before or after school or at lunch.
Homework
Please refer to the homework policy for the science department which is
attached.
Make-up Work
Missed work due to an excused absence may be made up during lunch or after
school. Obtaining the assignment and scheduling make-up exams within five
days of his or her return to school is the student’s responsibility. The
five-day period may be extended if the student has missed three or more
consecutive school days. If an absence is planned for a trip or school
event, please obtain assignments ahead of time so that you do not fall
behind.
Course Content & Tentative Schedule
Please note that times are approximate. School activities, changes in school
schedules and the needs of the students in the class will affect the time
spent on each topic. Lab activities are subject to change.
ChemicalFoundations(Review): Orientation to A.P. Chemistry, Laboratory
Safety, Chapter 1—“Chemical Foundations” --Scientific method --Units of
measurement --Significant figures --Dimensional analysis --Classification of
matter Chapter 2—“Atoms, Molecules & Ions” --History of chemistry --
Fundamental laws--Dalton’s Atomic theory --Modern atomic model --
Nomenclature Chapter 7—“Atomic Structure & Periodicity” --Electromagnetic
spectrum --Atomic spectra & Bohr model --Quantum mechanics --Quantum
numbers --Electron arrangements --Electron configurations --Aufbau
principle, Hund’s rule, Pauli exclusion principle, Heisneberg uncertainty
principle Lab: Paper Chromatography: Identification of Dyes in Skittles
Candies Exp. 8 Separation of a Mixture by Filtration and Simple Distillation
Exp. 18 A & B Spectroscopy Lab: Emission Spectra of Hydrogen
Approximate Time: 3 1/2 weeks
Periodicity,Families of Elements: Chapter 7—“Atomic Structure &
Periodicity” --Writing electron configurations using the periodic table --
Predictions of oxidation numbers of representative elements --Periodic
trends in atomic radii --Periodic trends in ionization energies --Periodic
trends in electron affinity --Periodic trends in electronegativity Chapter
19—“Representative Elements: Groups 1,2, 13 & 14” Chapter 20—“Representative
Elements: Groups 15-18” Chapter 21—“Transition Metals & Coordination
Chemistry” --Student research & presentations on the families and specific
elements Exp. 20 Properties of Some Representative Elements Exp. 44
Qualitative Analysis of the Group II Cations
Approximate Time: 2 weeks
Bonding Chapter 8—“Bonding: General Concepts”--Types of bonds &
electronegativity--Bond polarity & dipole moments --Ion size --Formation of
binary ionic compounds & calculation of lattice energy --Covalent bonding &
calculation of bond energy --Localized electron model --Lewis structures --
Resonance --VSEPR model—Molecular geometry --Relationships between geometry,
polarity, structure and properties --Intermolecular forces (Hydrogen
bonding, dipole-dipole forces, van der Waal’s Forces) Chapter 9—“Covalent
Bonding: Orbitals” --Hybridization & Localized electron model --Sigma & pi
bonds --Molecular orbital model --Bonding in homonuclear & heteronuclear
diatomic molecules Exp. 6: The Solubility of a Salt Exp. 19: Molecular
Models and Properties
Approximate Time: 3 1/2 weeks
MIDTERM EXAM
Stoichiometry: Chapter 3—“Stoichiometry” --Atomic masses --The mole & molar
mass --Percent composition calculation --Empirical and molecular formula
calculations --Writing and balancing chemical equations --Calculations of
limiting and excess reactants Lab: Percent Water in a Hydrate Exp. 11-I:
Stoichiometry and Limiting Reactant
Approximate Time: 2 weeks
States of Matter: Chapter 10—“Liquids & Solids” --Intermolecular forces and
relationship to state and structure of matter --Kinetic molecular theory
pertaining to liquids & solids --Liquid state characteristics --Structure of
solids --Calculation of lattice energy --Calculations of crystal size,
atomic radius, density, etc. of closest packed structures --Bonding in
metals --Network atomic solids --Molecular and ionic solids --Vapor pressure
and changes of state --Phase diagrams, critical point and triple point --
Heats of vaporization and fusion Chapter 5—“Gases” --Ideal vs. real gases --
Pressure --Calculations using Boyle’s, Charles’, ---Gay Lussac’s &
Avogadro’s Laws --Ideal gas law calculations --Dalton’s law calculations --
Gas stoichiometry (Mole concept) --Kinetic molecular theory and relationship
to ideal gas laws --Dependence of kinetic energy on gas temperature --
Effusion & diffusion and Graham’s Law calculations Exp. 5 Determination of
Melting Point Exp. 13 Preparation and Properties of Some Common Gases Exp.
14-III: Graham’s Law
Approximate Time: 3 weeks
Solutions, Reactions & Solution Stoichiometry: Chapter 11—“Properties of
Solutions” --Mixtures: solutions, colloids and suspensions --Solution
concentration calculations—molarity, normality, molality, mole fraction and
mass percent --Solution composition --Energies of solution formation --
Factors affecting solubility --Henry’s Law calculations --Vapor pressures of
solutions and --Raoult’s Law calculations --Colligative properties of
solutions --Calculations of molar mass from freezing point depression and
boiling point elevation --Osmotic pressure --Ideal vs. non-ideal solutions
Chapter 4—“Types of Chemical Reactions & Stoichiometry” --Water and the
nature of aqueous solutions --Types of chemical reactions --Precipitation
reactions and net ionic equations --Acid-base reactions --Redox reactions --
Determination of oxidation numbers --Coordination complexes Exp. 23
Determination of Molar Mass by Freezing Point Depression Lab: Reactions of
Copper Exp. 31: Determination of Iron by Redox Titration
Approximate Time: 3 1/2 weeks
FINAL EXAM FOR HONORS PRE-A. P. CHEMISTRY II
Organic Chemistry: Chapter 22—“Organic and Biological Molecules” --Alkanes,
alkenes & alkynes --Aromatic hydrocarbons --Functional groups --Polymers --
Structures and isomerism Exp. 39: Preparation and Properties of Esters
Approximate Time: 1 1/2 weeks
Kinetics: Chapter 12—“Chemical Kinetics” --Reaction rates --Differential
rate laws --Determining the form of rate laws from initial rates --
Calculation of the rate constant --Inetgrated rate law --Graphical
determination of rate laws --Reaction mechanisms and rate determining steps -
-Molecularity of elementary steps--Factors affecting reaction rates --
Activation energy --Collision theory --Catalysis Exp. 25-I: Experimental
Determination of a Rate Law Lab: Qualitative Effects of a catalyst (Loosely
based on Exp. 41)
Approximate Time: 2 Weeks
Equilibrium: Chapter 14—“Chemical Equilibrium” --Dynamic equilibrium --The
equilibrium constant --Law of mass action and equilibrium expressions --
Relationship between Kc and Kp --Calculation of equilibrium constant from
equilibrium concentrations --Calculations of equilibrium and initial
concentrations of reactants and/or products --Heterogeneous equilibria --
Reaction quotient calculations --Common ion effect --LeChatelier’s Principle
Exp. 26-II: Spectrophoto- metric determination of an equilibrium constant
Exp. 26-III: LeChatelier’s Principle
Approximate Time: 2 ½ weeks
Acids and Bases Chapter 14—“Acids and Bases” --The nature of acids and
bases --Three definitions of acids and bases --Amphoterism --Acid & base
strength --Acid and base dissociation equations and dissociation constants --
Autoionization of water, Kw & pKw --The pH scale --Calculations of hydronium
& hydroxide concentrations, pH & pOH --Calculations of pH of strong acids &
bases --Calculations of pH of weak acids & bases --Polyprotic acids and
bases --Acid-base properties of salts --Effect of structure on acids and
bases Chapter 15—“Applications of Aqueous Equilibria” --Common ions in
acid/base solutions --Buffers --Calculations using Henderson-Hasselbalch
equation --Titration and pH curves --Acid-Base indicators --Calculations of
pH throughout a weak/strong titration --Solubility equilibria and solubility
product constants --Calculation of molar solubilities and Ksp values --
Prediction of precipitation reactions Lab: Measuring and Calculating pH &
pOH Exp. 29-I: Analysis of an Unknown Acid Sample Exp. 27: The Solubility
Product of Silver Acetate
Approximate Time: 3 weeks
A.P. Chemistry Midterm Exam
Thermochemistry & Thermodynamics: Chapter 6-“Thermochemistry” --The nature
of energy --Enthalpy and calorimetry calculations --Standard enthalpies of
formation --Heat of reaction --Hess’s Law Chapter 16—“Spontaneity, Entropy &
Free Energy” --Spontaneous processes & entropy --First Law of Thermodynamics
(review) --Second Law of Thermodynamics --Entropy changes --State functions -
-Free energy --Free energy changes and chemical reactions --Dependence of
free energy on enthalpy and entropy changes --Temperature and spontaneity --
Dependence of free energy on pressure --Free energy and equilibrium --Free
energy and work Exp. 17-I: Determination of a Calorimeter Constant Exp. 17-
II: Specific Heats of Metals and GlassExp. 17-V: Heat of Solution of a Salt
Approximate Time: 2 weeks
Electrochemistry: Chapter 17—“Electrochemistry” --Galvanic cells --
Faraday’s laws calculations --Writing half reactions --Standard reduction
potentials --Calculations of cell potential --Cell potentials, electrical
work & free energy --Prediction of direction of redox reactions --Dependence
of cell potential on concentrations --Nernst equation --Relationship of free
energy change and electrode potentials --Corrosion --Electrolytic cells /
electrolysis Exp. 32: Electrochemistry I: Chemical Cells
Approximate Time: 1 ½ weeks
Nuclear Chemistry: Chapter 18—“The Nucleus: A Chemist’s View” --Nuclear
stability and radioactive decay --Half-lives --Kinetics and radioactive
decay --Transmutation & nuclear equations --Detection and applications of
radioactivity --Effects of radiation --Thermodynamic stability of the
nucleus --Nuclear fission and fusion Lab: Modeling Nuclear Decay
Approximate Time: 1 week
Review for A.P. Chemistry Exam: Topic overviews, Problem sets, A.P.
Chemistry Free Response Questions, Practice Multiple Choice Tests, Exp. 48:
Identification of an Unknown Salt, Lab: Inquiry: Design a Method to Properly
Inflate an Air Bag
