Community College of Allegheny County
General Chemistry 1 – CHM151-01
Summer 2008
Instructor: John Harrell
E-mail: jharrell@ccac.edu
Secretary Phone: (412)369-4106
(Michele Romanias)
(If email is used, please include your name and course number on the subject line of the
email, otherwise the message will be deleted.)
Textbook: General Chemistry, Ebbing, required.
Catalog Course Description:
This is a chemistry course appropriate for science and engineering majors. The topics
include: measurements, classification and properties of matter, atomic and molecular
structure, chemical bonding, periodicity, stoichiometry, thermochemistry, chemical
reactions, and the structure. Laboratory experiments deal with the quantitative and
qualitative determination of physical and chemical properties of chemical substances
Prerequisites: CHM109 or CHM 110/111 or “B” or better in high school chemistry
within the past five years and MAT 108 or MAT 111 or equivalent
Evaluation: The course grade will be based on 4 unit exams, one cumulative final, the
laboratory grade, quizzes and collected homework assignments.
Exams
Lab Grade/Quizzes
80%
20%
(4 unit exams; 1 final – 16% each)
(Quizzes will be announced/unannounced.)
Note: There is no rounding or curving of grades. There is no “extra-credit”. Your
grade in the class is the result of the above calculation, PERIOD.
Missed Classes: MAKE - UP EXAMS AND LABS ARE NOT GIVEN. A zero is
recorded in the event of a missed assignment, exam or lab. If a student misses class, it is
the student’s responsibility to contact a classmate for missed work, handouts, and notes.
Therefore, it is highly recommended that each student inquire from at least 3 classmates,
their phone number, in the event that an absence occurs. Note: All flowcharts are due at
the beginning of each lecture period regardless of a class absence prior.
Attendance Policy: Students are expected to attend all classes. Regular attendance is
taken. No late work is accepted. Missed exams, labs, quizzes and collected assignments
cannot be made up and a grade of a zero is recorded. Missing more than two labs
causes the students lab grade to become a 0% and will fail the lab section of the
course.
Office Hours and Appointment Policy: I have no office hours. If you have questions
ask them prior to the lecture/lab time that we have together.
Special Notes:
1. The syllabus may be changed at the discretion of the instructor.
2. The lab/exam schedule is extremely tentative and often changes. DO NOT RELY
ONLY ON the syllabus for the labs that we will perform or possible exam dates. In this
manner, class attendance is mandatory.
3. Students are required to have a flowchart completed at the beginning of each lecture
period. If the flowchart is not completed, students will not be permitted to attend lab and
will forfeit points accumulated that day. This will be recorded as a lab absence.
4. Students must not arrive late for lecture or lab meetings. This is disruptive as well as a
safety hazard for everyone. Students that are late will be asked to leave and will
forfeit points accumulated that day. This will be recorded as a lab absence.
LISTED TOPICS:
1. Measurements
2. Classification of matter
3. Chemical nomenclature
4. Type of chemical reactions
5. Calculations involving the mole concept
6. Classification and balancing of equations
7. Reaction stoichiometry and its applications
8. Atomic Structure
9. Periodicity and electron configurations
10. Ionic, covalent, and metallic bonding
11. Molecular geometry
12. Valance bond and molecular orbital bonding theories
13. Properties of gases and the gas laws
LEARNING OUTCOMES:
Upon successful completion of this course a student will:
1. List the common SI units of measurement, the values of selected prefixes, and the use
of dimensional analysis to interconvert units of measurement.
2. Classify matter on the basis of physical and chemical properties and physical and
chemical changes.
3. Describe the structure of the atom in terms of subatomic particles; write the isotopic
symbol for any isotope of a given element and an atoms electronic configuration.
4. Use the periodic table to categorize elements, infer the physical and chemical
properties of elements, and to determine electron configurations.
5. Write proper formulas and name common ions, ionic, covalent and organic compounds
including acid base nomenclature where appropriate.
6. Apply the mole concept to the determination of mass, % composition, empirical and
molecular formulas.
7. Apply the mole concept to stoichiometry calculations such as yield and per cent yield.
8. Discuss the role of heat in chemical reactions, perform calorimetric calculations or use
enthalpy tables to determine the heat of reaction.
9. Discuss the properties of electromagnetic radiation with respect to wavelength,
frequency, energy and spectral region and be able to calculate the energy, frequency or
wavelength from appropriate data.
10. Compare and contrast the Bohr and quantum theories of atomic structure and how
they account for location of electrons in atoms and spectral lines.
11. Write Lewis structures for ions, ionic and covalent compounds and use these
structures and VSPER theory to predict molecular and ionic geometries.
12. Compare and contrast valance bond, molecular orbital and metallic bonding theories
and how each accounts for molecular structures and properties.
13. Use kinetic molecular theory to account for the properties of gases and the gas laws.
14. Use gas laws to calculate the pressure, volume, temperature, number of moles or
molecular weight from appropriate data.
Date:
Class Content:
5/19
Chapter 1: Introduction and Basic Concepts
Lab: Safety, Check in.
5/20
Chapter 2: Atoms, Molecules and Ions.
Lab: Safety Quiz & Lab Techniques
5/22
Chapter 4: Chemical Reactions
Lab: Identification of an Unknown Compound.
5/26
No Lecture/Lab---Memorial Day
Day:
5/27
Class Content:
Chapter 4: Chemical Reactions
Chapter 3: Stoichiometry
Lab: Ionic Reactions
5/29
Exam #1 – Chapters 1,2,4
Chapter 3: Stoichiometry
Chapter 6: Thermochemistry
Lab: Separation of a mixture.
6/2
Chapter 6: Thermochemistry
Lab: Chemicals in every day life
6/3
Chapter 6: Thermochemistry
Chapter 7: Quantum Theory
Lab: Formula of a hydrate
6/5
Exam #2 - Chapters 3 and 6
Chapter 7: Quantum Theory
Chapter 8: Electron Arrangement and Periodicity
Lab: Hess’s Law
6/9
Chapter 8: Electron Arrangement and Periodicity
Lab: Hess’s Law
6/10
Chapter 9: Ionic and Covalent Bonding
Lab: Titration, acetic acid in vinegar
6/12
Exam #3 – Chapters 7 & 8
Chapter 9: Ionic and Covalent Bonding
Lab: Spectroscopy, CoCl2.
6/16
Chapter 10: Molecular Geometry and Bonding Theories
Lab: Spectroscopy, CoCl2..
6/17
Chapter 10: Molecular Geometry and Bonding Theories
Chapter 5: Gasses
Lab: Qualitative analysis Pb2+, Ag, Hg..
6/19
Exam #4 (Chapters 9,10)
Chapter 5: Gasses
Lab: Molecular Geometry
6/23
Chapter 5: Gasses
Lab: Gas Laws
6/24
Chapter 5: Gasses
Lab Exam/Check out
6/26
Final Exam
No Lab
All dates above are tentative and subject to change.
Dates to Remember:
No class on Memorial Day, Monday, May 26
Last day to withdraw with a “W” is Monday, June 16.
INFORMED CONSENT
I have read the course outline and have been given the opportunity to ask questions
and/or clarify any policy which is unclear. I understand and agree to the academic criteria
and requirements for this course. I agree to abide by the behavior policies and standards
of this course. I understand that, while unlikely, changes in the course outline may be
necessary at the professor’s discretion.
Course: General Chemistry 1, CHM151-NC01
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Student Signature, if student is a minor, parental signature is also required.
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Student Name, Print
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Date