Honors College Chemistry (AP)
SC77W– General Chemistry I & II
Dobson High School
Course Syllabus 2010-11
Class Meeting
Academic Year: 2010-11
Days: M-F 9:49 a.m. – 10:36 a.m. (2nd hour)
Instructor: Mr. Hayes
Best time to call M - F 6:15 – 7:50 a.m.
Office Hours: M - F, 1:10 – 2:01 (5th hr.)
Dobson High School Room, B-510
1501 W. Guadalupe Rd, Mesa, AZ 85202
Text:
Suggested
Additional Text
Zumdahl, Steven S. and Susan A,. Chemistry, 5th edition.
Houghton Mifflin Company, Boston, 2000
Fast Track To a 5 (supplemental handbook)
Preparing for the AP* chemistry Examination: To accompany Chemistry
6th & 7th editions by Zumdahl and Zumdahl
Course Description
SC77W
A detailed study of the principles of chemistry designed for science majors and
students in pre-professional curricula. Prerequisites: a grade of B- or better in SC72W
and at least a B+ grade or better for regular high school chemistry and completion of
intermediate algebra or the equivalent.
Course Description
SC77W
A study of the chemical properties of the major groups of elements, equilibrium
theory, thermodynamics, electrochemistry and other selected topics. Prepares students
for all sophomore chemistry courses. Prerequisites: Successful completion of a full
year of chemistry at suggested grade.
Attendance Policy
Attendance is important in this course. If you are absent on exam day, you must take
the test within two days. Dobson’s attendance policy will be followed.
Disability
Statement
The school will make reasonable accommodations for persons with documented
disabilities. Students should notify Student Services and the instructor of any special
needs.
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Evaluation
Exams:
There will be an exam at the end of each unit. At the end of each semester a final exam will
be given during the regularly scheduled final exam period.
Quizzes and Homework:
Homework assignments are included in each unit. There will be regular quizzes over the
homework assignments. Any late assignment will be marked down. No late assignments will
be accepted after completion of the unit.
Grades for Course:
Unit Exams & quizzes
Labs & Homework
Final Exam
60%
25%
15%
100%
Grades will be determined by the following scale:
A: 90-100% B:80-89% C:70-79% D:60-69% F :0-59%
Reminder:
This is a weighted course and student must earn at least a C- to obtain credit. No credit
allowed for grades below a C-.
Course Goals
and Objectives
1. Define chemistry and describe its main branches.
2. Use the Factor-Label (Dimensional Analysis) Method in solving chemistry-related
problems.
3. Use metric and SI systems of units
4. Classify matter as elements, compounds or mixtures.
5. Write formulas for and give names of simple inorganic compounds.
6. Classify a property or change as physical or chemical.
7. Complete and balance chemical equations.
8. Write a net ionic equation from a given reaction.
9. Determine the empirical and molecular formula from percentage composition or mass
data.
10. Perform calculations using the mole concept of mass and number.
11. Identify substances as electrolytes or non-electrolytes.
12. Define the relationships between matter and energy.
13. Calculate heats of reaction from calorimeter data and/or bond energies.
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14. Solve problems involving energy changes that result from physical state changes and
from chemical reactions.
15. Apply Hess's Law to a given set of equations.
16. Solve stoichiometry problems, including problems involving solutions and heats of
reaction.
17. Deduce the electronic structure of atoms and show the relationship between electronic
structure and the chemical properties of atoms.
18. Describe the properties of metallic and non-metallic elements.
19. Use the Periodic Table to estimate the properties of elements and compounds.
20. Describe the properties of ionic and covalent compounds.
21. Write the electron dot structure for an atom, ion, ionic formula, or a covalently bonded
species.
22. Use the concepts of electronegativity and bond polarity in conjunction with VSEPR
Theory to predict the shapes and polarities of simple ions and molecules.
23. Describe chemical bonding in terms of Valence Bond Theory and Molecular Orbital
Theory.
24. Solve problems involving the Ideal Gas Laws.
25. Describe the physical states of matter with the aid of the Kinetic Molecular Theory.
26. Classify a crystal as molecular, ionic, covalent or metallic.
27. Classify intermolecular forces in a given substance as ionic, covalent, London, dipoledipole, hydrogen bonding, or metallic.
28. Describe the properties of solutions
29. Describe the progress of a chemical reaction in terms of Collision Theory or Transition
State Theory.
30. Determine the rate law expression and the order of a reaction with respect to a reactant
and order.
31. Determine whether a proposed mechanism agrees with the rate law for a reaction.
32. Estimate the influence of temperature, catalyst, pressure and concentrations of
reactants on reaction rate and on position of equilibrium.
33. Write correct equilibrium expressions and calculate the value of K, or calculate
concentrations of reactants and products at equilibrium.
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34. Solve problems involving the formation and dissolving of precipitates.
35. Solve equilibrium problems involving weak acids, weak bases, and buffer systems.
36. Calculate pH and pOH of a given solution or mixture of solutions.
37. State the three laws of thermodynamics.
38. Calculate changes in enthalpy, free energy, and entropy from appropriate thermodynamic
data.
39. Predict the spontaneity of chemical reactions from thermodynamic data.
40. Complete and balance redox equations.
41. Solve problems involving Faraday's Law of Electrolysis.
42. Use the Nernst Equation to calculate cell potentials.
43. Complete and write nuclear reactions
44. Compare and contrast chemical and nuclear reactions.
45. Describe applications of radiochemistry.
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AP Lab Syllabus
Course Description
Laboratory experience in support of SC77W. Prerequisites: SC72W or equivalent Lab
experience from SC71 consists of application of lecture content to related chemistry
experiments.
Attendance Policy
Attendance is important in this course. If you miss a lab it must be made up promptly
while the lab set-up is still available. After the class has finished and the lab set-up has
been taken down no make-ups will be permitted
Safety Regulations
Arizona Statute ARS 15-151 specifies that every student, teacher, and visitor must
wear appropriate protective eyewear while participating in or when observing
vocational, technical, industrial arts activities involving exposure to: molten metals,
molten materials; cutting, shaping and grinding of materials; heat treatment; tempering
or kiln firing of any metal or other materials; welding fabrication processes; explosive
materials; caustic solutions, and radioactive materials
If you are not wearing goggles while in the lab area when any lab work is in progress
you will be asked to leave the lab area, and you will lose credit for the lab.
If you behave in an unsafe manner, do not follow directions, or disrupt another
student’s work, you will not continue the lab and will lose credit for the lab.
Evaluation
You will be assigned to a lab group. You will perform the lab cooperatively with your
group and you may work together on analyzing the results. However, you will write
and be responsible for submitting your own individual lab report for each lab.
No late assignments will be accepted after completion of the unit.
Lab Goals &
Objectives
1.
2.
3.
4.
Record observations accurately, using appropriate chemical terminology.
Use scientific measuring devices to obtain chemical data.
Apply principles, concepts, and procedures of chemistry to lab experiments.
Use scientific method in interpreting chemical data to arrive at rational
conclusions.
5. Use lab equipment properly to perform a variety of chemical procedures and
techniques.
This syllabus is subject to modification as determined by the instructor
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