Chaminade
College
Preparatory School
2006-2007
Science Department
AP Chemistry
Course Syllabus
Course Number: chem. 470
Credit Hours: Two Semesters, 1.0 Credit
Grade Level: 10th grade
Faculty Name: Dr. Howard Wright
Classroom Location: Room 301
Block Period:
Teaching Blocks:
Available Blocks:
Office: Frishe Hall, Room
Faculty Telephone: 314-993-4400 x
Faculty E-mail: @chaminade-stl.com
Faculty Website: www.ccpscience.com
I. Course Description
This is an advanced placement course designed to prepare the student for the AP Chemistry exam. The course covers the equivalent of one full year of college level General Chemistry, comparable to a first year course at a college or university. The course is a rigorous math-based course, with a strong laboratory component. It is intended for students who have demonstrated a willingness to commit considerable time to studying and completing assignments outside of class, and who have successfully completed a prior course in chemistry in high school.
Since passing the AP exam may qualify the student to by-pass a first-year college chemistry course, AP Chemistry should not be considered "college prep". Rather, this is a college class, with college level expectations for behavior, participation and effort.
The course will cover molecular and ionic substances; colligative properties, expressing concentration of solutions, stoichiometry, thermochemistry, electron structure of atoms and its effects on properties of the elements, electron structure hybridization and resulting geometry of compounds and its effect on their properties. It will also cover properties of gases, liquids and solids; chemical kinetics and equilibrium, including acid/base equilibrium; electrochemistry and nuclear chemistry. Emphasis will be placed on writing chemical equations and predicting products, and applying concepts to experimental data.
II. Desired Learning Outcomes and Evidence for Assessment
Students completing the AP Chemistry course should be proficient in first year college chemistry and be able to pass the AP exam
1. Construct a properly drawn graph with x and y axis labels
2. Calculate the value of a variable from a simple single variable equation
3. Search a subject on line and generate a summary document
4. Take notes in a concise and detailed manner
5. Make and record detailed observations
6. Follow detailed written instructions
III. Class Texts and Materials
Text: Zumdahl fifth edition copy write 2004
Barons Passing the AP Exam
IV. Website
Internet: http://www.ccpscience.com/1wright/ The lecture notes will, for most of the lectures, be available on the Internet at ccpscience.com. These notes are critical to those individuals that are absent from class or need assistance during the lecture to follow the lesson.
V. Laptop Usage
In AP chemistry we used the computers to give each student a Organizational grid to help them take notes complete their homework complete online quizzes and complete labs In addition progress reports are emailed to the students and online web quests are performed on the laptops.
VI. Performance Expectations
Students should be able to pass the standardized state test in Chemistry and pass the AP exam in Chemistry
VII. Student Evaluation/Grading
Grading will be divided
15% homework
15% quizzes
20% lab work
30% midterm exams
20% final exam
Homework and Problem Sets: Homework and problem sets will be given as per the syllabus and is graded on a pass, ½, or fail basis. The homework and problem sets will account for 15% or the overall grade. Homework is to clarify what you heard in lecture. No homework will be acceptable more than 2 days late. Chemistry involves the use of very simple mathematics and the understanding of often abstract concepts. Completion of homework is critical to the successful completion of high school chemistry. Answers to homework along with detailed explanations of these answers should be obtained from Dr. Wright or via the Internet under the heading homework at ___ ccpscience.com
Quizzes: Quizzes will be given as per the syllabus and graded in class. Quizzes will account for 15 % of the overall grade. Quizzes will cover the homework material and will consist of 5 to 7 questions.
Midterm Exams: Midterm exams are given as per the syllabus. The exams will be cumulative in nature with questions spanning all material covered from the beginning of the course. Midterm exams will typically include 50 questions derived principally from the quizzes. Midterm exams will account for 30% of the overall grade. It would be highly recommended for all students to keep past quizzes as a guide for studying for the exams.
Final Exams: Final Exam will be given as per the syllabus. The final exam will be cumulative in nature with questions spanning all material covered from the beginning of the course. The final exam will include 100 questions derived from both the quizzes and the midterm exams. The final exam will account for 20% of the overall grade
Laboratory Reports: Observations are critical when performing a lab therefore a note and data sheet will be provided when you do labs. The lab write up will be done on computer and handed in the day after the lab. Both the formally written up lab and the dirty, crumpled, accurate and detailed data sheet must be attached to the clean through lab write up. The neatness, form and accuracy of each lab will be graded using a rubric format that will be posted on a scale from 0 to 15. The laboratory notebook will account for 20% of the overall course grade. Anyone not turning in a lab after being present for the lab must be present before school to write up the lab. Detailed instructions as to what is expected in the lab and how it is to be graded can be found on the bulletin board in the classroom and in subsections chemlab write-up and grading rubric in CCP Science.com
VIII. Classroom Decorum
Classroom decorum will be referred to classroom ethics: The definition of ethics is “A principle of right or good conduct or a body of such principles.” As students at Chaminade College Preparatory we have agreed to such principles of honesty. In the light of these principles it must be understood that the debasing of another individual will not be tolerated. We all enjoy humor and the interaction of our friends and classmates but we must not allow such bantering to become destructive and harmful. Demeaning another individual will not be tolerated.
IX. Attendance Expectations
Students should attend all classes
X. Cheating, Plagiarism
Cheating is not allowed. Science is a pursuit of truth and understanding. The antithesis of truth is lies. There is no place in the study of chemistry for lies. If a below average grade is earned on an exam I will give the student ample opportunity to bring that grade up. There is no reason to cheat. Cheating on an exam will be met with failure on the exam and a referral to the school administration. All labs will be subjected to “Turnitin.com” to minimize the copying of last year, other students or plagiarism of online sources. To clarify what plagiarism is check out http://www.csubak.edu/ssric/Modules/Other/plagiarism.htm
XI. Topical Outline
Structure of Matter
A. Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by chemical and physical means
3. Atomic number and mass numbers; isotopes
4. Electron energy levels; atomic spectra, quantum numbers, atomic orbitals
5. Periodic relationships, including atomic radii, ionization energies, electron affinity, oxidation states
B. Chemical Bonding
1. Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
b. Relationship to states, structure, and properties of matter
c. Polarity of bonds, electronegativities
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
II. States of Matter
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. Liquids and solids from the kinetic-molecular viewpoint
2. Phase diagrams of one-component systems
3. Changes of state, including critical points and triple points
4. Structure of solids; lattice energies
C. Solutions
1. Types of solutions and factors affecting solubility
2. Methods of expressing concentration (excluding normalities)
3. Raoult’s law and colligative properties (nonvolatile solutes); osmosis
4. Non-ideal behavior (qualitative aspects)
III. Reactions
A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Bronsted-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; Faraday’s laws; standard half-cell potentials; Nernst equation;
prediction of the direction of redox reactions
B. Stoichiometry
1. Ionic and molecular species present in chemical systems: net ionic equations
2. Balancing of equations including those for redox reactions
3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle, equilibrium constants
2. Quantitative treatment
a. Equilibrium constants for gaseous reactions: Kp, Kc
b. Equilibrium constants for reactions in solution
-Constants for acids and bases; pK, pH
-Solubility product constants and their application to precipitation
and the dissolution of slightly soluble compounds
-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. State functions
2. First law: change in enthalpy; heat of formation; heat of reaction; Hess’s Law; heats of vaporization and fusion; calorimetry
3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on
enthalpy and entropy changes
4. Relationship of change in free energy to equilibrium constants and electrode potentials
IV. Descriptive Chemistry
A. Chemical reactivity and products of chemical reactions
B. 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
C. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)
V. Laboratory
A. Making observations of chemical reactions and substances
B. Recording data
C. Calculating and interpreting results based on the quantitative data obtained
D. Communicating effectively the results of experimental work