Oakton Community College
Generic Course Syllabus
I.
Course
Prefix
Course
Number
Course Name
CHM
122
General College Chemistry II
II.
Credit Lecture
4
3
Lab
3
Prerequisites:
CHM 121 with minimum grade of C, and MAT 140 or MAT 149 with minimum
grade of C, or consent of instructor.
III.
Course (Catalog) Description
Course continues CHM 121. Content includes kinetics, chemical equilibrium,
acid-base theory and equilibria, solubility equilibria, electrochemistry,
thermodynamics, nuclear chemistry, coordination compounds, and an introduction
to organic and biochemistry. Weekly laboratory activities.
IV.
Learning Objectives
Students who successfully complete this course will be able to do the following at
an acceptable level.
A. State the meaning of reaction rate and discuss the factors which affect it
B. Write the rate law for a reaction given an appropriate set of initial
concentrations of reactants and associated initial rates
C. Calculate the amount of reactant remaining after a given period of time when
furnished with the half life, for either first or second order reactions
D. Write possible multi-step mechanisms consistent with a given chemical
reaction, and determine the rate law for a reaction predicted by a particular
simple mechanism.
E. Determine the equilibrium constant for a reaction equation given 1) the
equilibrium concentrations of reactants and products, or 2) the initial
concentrations of reactants and products and the equilibrium concentration of
one of them
F. Calculate the equilibrium concentration of reactants and products given the
equilibrium constant for the reaction and the initial concentrations
G. Understand the concept of (and ways of) shifting the equilibrium position of a
chemical system
H. Understand the common ion effect
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I. Describe the various acid-base theories
J. Calculate the pH, [H3O+], pOH, or [OH-] of a solution at 25oC given the value
of any one of these variables and at any temperature given Kw for that
temperature
K. Calculate concentrations of all species present in a solution of a weak
polyprotic acid when the initial concentration and all Ka values are given
L. Calculate the pH of an aqueous solution (a) of a salt of known concentration,
(b) of a strong or weak acid or base of known initial concentration, (c) of a
buffer system with known initial concentrations, and (d) at various stages of
an acid/base titration, given the relevant Ka or Kb values.
M. Describe the function of an indicator and select an appropriate indicator for a
specified acid/base reaction
N. Calculate the solubility of a slightly soluble salt (in water or in a solution with
a common ion) and the equilibrium concentration of all ions present, given
the Ksp
O. Calculate the Ksp value of a slightly soluble salt from solubility data
P. Understand the meaning and significance of Ssys, Ssurr, Suniverse, and the
qualitative relationship between Suniverse and Gsys
Q. Predict which physical or chemical processes increase a system's entropy
R. Understand the meaning of “exothermic”, “endothermic”, “spontaneous”, and
“non-spontaneous”, and be able to determine through calculation which of
these correspond to a proposed reaction if conditions and appropriate
thermodynamic data are given.
S. Describe the meaning of, and qualitative and quantitative relationships
between Q, G, and Ecell.
T. Describe the meaning of, and relationships between K, Go, and Ecello and
distinguish these from Q, G, and Ecell
U. Balance equations of oxidation-reduction reactions occurring in acidic or
basic solution
V. Sketch electrolytic or voltaic cells indicating cathode, anode, positive and
negative electrode, direction of current flow, Ecell, and half reactions
W. Determine EMF (Ecell) for standard cells from values of standard reduction
(or oxidation) potentials, and for non-standard cells using the Nernst equation
X. Discuss the basic chemistry of common metals
Y. Name, describe the geometry, and identify isomer possibilities for
coordination compounds formed from common metal ions and ligands
Z. Describe the physical phenomena which lead to a compound being colored
AA. Describe common nuclear reaction types and energy changes associated
with them
BB. Use the n/p ratio and band of stability to predict the most likely nuclear decay
reaction for a nuclide
CC. Name and draw structural formulas for simple alkanes, alkenes, alkynes,
aromatics, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, and
amino acids
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DD.
Identify the building blocks making up proteins and nucleic acids;
describe different levels of structure for proteins and nucleic acids and relate
structure and function
EE. Describe and give examples of carbohydrates and lipids (particularly
triglycerides)
FF. Determine the presence or absence of various cations in aqueous solution by
using qualitative analysis logic and reactions
GG. Determine the concentration of various species through titration and
spectrophotometric techniques
V.
Academic Integrity
Students and employees at Oakton Community College are required to
demonstrate academic integrity and follow Oakton’s Code of Academic Conduct.
This code prohibits:
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cheating,
plagiarism (turning in work not written by you, or lacking proper citation),
falsification and fabrication (lying or distorting the truth),
helping others to cheat,
unauthorized changes on official documents,
pretending to be someone else or having someone else pretend to be you,
making or accepting bribes, special favors, or threats, and
any other behavior that violates academic integrity.
There are serious consequences to violations of the academic integrity policy.
Oakton’s policies and procedures provide students a fair hearing if a complaint is
made against you. If you are found to have violated the policy, the minimum
penalty is failure on the assignment, and a disciplinary record will be established
and kept on file in the office of the Vice President for Student Affairs for a period
of 3 years.
Details of the Code of Academic Conduct can be found in the Student Handbook.
VI.
Outline of Lecture Topics
A. Kinetics
 Factors affecting rates of chemical reactions
 Determining rate and rate laws from experimental data
 Half life and first order reactions; half life and second order reactions
 Rate laws and reaction mechanisms
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B. Equilibrium
 Concept, and determination of equilibrium constants
 Predicting the direction of a reaction for a system not at equilibrium
 Equilibrium concentration of reactants and products
 Effect of pressure and temperature on equilibrium
C. Acids and Bases
 Acid – base theory
 Definition and determination of pH and pOH
 Relative strength of various acids and bases
 Determination of the pH of strong acids and bases
D. Acid – Base Equilibria
 Determination of the pH of weak acids and bases
 Hydrolysis of salts; determination of the pH of salt solutions
 Polyprotic acids
 Buffers and common ion effect
 Titration curves
E. Solubility of Slightly Soluble Compounds
 Determination of solubility product and dissociation constants
 Common ion effect on solubility
 Effect of pH on solubility
 Qualitative analysis of metal ions
F. Thermodynamics
 Enthalpy and the first law of thermodynamics
 Entropy and the second law of thermodynamics
 Exothermic and endothermic reactions; spontaneous and nonspontaneous reactions
 Gibbs free energy and spontaneity; standard Gibbs free energy and
equilibrium constants
G. Electrochemistry
 Voltaic cells
 Electrolytic cells
 Half reactions of water; electrolysis of aqueous solutions
 Standard EMF and equilibrium constants
H. Nuclear Chemistry
 Nuclear equations
 Nomenclature of subatomic particles
 Nuclear decay and half life
 Applications
I. Descriptive Chemistry
 Main group elements
 Transition metals including structure and nomenclature of complexes
J. Structure of Carbon and Carbon Compounds
 Overview of organic functional groups, including nomenclature and
properties
 Introduction to isomerism in organic compounds
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 Polymers
J. Biochemistry
 Amino acids and proteins
 Nucleotides and nucleic acids
 Sugars and starches
 Lipids (especially triglycerides)
Laboratory Activities
The laboratory activities will include a safety overview including the location and
demonstration of the use of laboratory safety equipment. There are weekly
hands-on activities which include 12-14 of the specific activities listed below.
A.
B.
C.
D.
E.
F.
G.
H.
I.
J.
K.
L.
M.
N.
O.
Analysis of an Unknown Chloride
Rates of Chemical Reactions. I – The Iodination of Acetone
Rates of Chemical Reactions. II – A Clock Reaction
Determination of Equilibrium Constant for a Chemical Reaction
Qualitative Analysis of Group I Cations
pH Measurements—Buffers and Their Properties
Acid-Base Titration Curve
Determination of Solubility Product Constant of PbI2
Qualitative Analysis of Group III Cations
Voltaic Cell Measurements
Preparation of Copper(I) Chloride
Determination of an Equivalent Mass by Electrolysis
Determination of the Hardness of Water
Preparation of Aspirin
Absorption Spectra of Some Ni2+ Complexes
VII. Methods of Instruction
 Lectures which may be supplemented with classroom discussion, use of
molecular models, use of multimedia, and/or use of computer based materials
at the discretion of the instructor.
 Hands-On Laboratory Activities
 Individual and/or Group Problem Solving
VIII. Course Practices Required
 College-level writing skills on tests and laboratory write-ups
 Communication skills for discussion and articulation of questions
 Adherence to standard safety practices while in the laboratory
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IX.
Instructional Materials
The course textbook is Chemistry: A Molecular Approach, 2nd edition Tro, c
2011 or comparable text.
The laboratory text is Chemical Principles in the Laboratory, customized 9th
edition by Emil Slowinski, Wayne Wolsey, and William Masterton, c 2009 or
comparable text.
Beginning with the Spring 2007 semester, students will be required to purchase
their own Chemical Safety/Splash Goggles. These goggles must meet the
following criteria:
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Fit snuggly against the forehead and face, protecting against splashes
Be impact resistant; ANSI rating of Z87 or higher
Include only indirect venting
Two varieties of such goggles compliant with the above criteria are available for
purchase in the bookstore (cost range ~ $6-$12). Students may also elect to find
an alternative source for purchase, so long as the goggles meet the above criteria
and are approved by the instructor.
X.
Methods of Evaluating Student Progress
Depending upon the instructor, any combination of the following assessments
may be used to evaluate student progress and determine the course grade.
 Quizzes, tests, and/or examinations which may include essay, short answer,
multiple choice, true/false, and/or problem solving questions
 Laboratory assignments, reports, results and/or practicals
 Individual and/or group written reports
 Individual and/or group oral reports
 Individual and/or group problem solutions
XI.
Other Course Information
A. Reading the text and laboratory material ahead of the class or laboratory
session is expected.
B. Regular attendance at all sessions is expected. Missed laboratory sessions
will not be able to be made-up.
C. Class policies on make-up of exams and accepting of late work will be
determined by the individual instructor.
D. Students will be required to review and sign off on their review,
understanding, and adherence to basic laboratory safety regulations.
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E. Support services include the availability of open computer laboratories, the
college library, and the availability of free tutoring through the Learning
Center and/or office hours with the course instructor.
F. Students who have a documented learning, psychological, or physical
disability may be entitled to reasonable academic accommodations or
services. To request accommodations or services, the student needs to
contact the ASSIST office in the Learning Center. All students are expected
to fulfill essential course requirements. The college will not waive any
essential skill or requirement of a course or degree program.
G. Oakton Community College recognizes the broad diversity of religious
beliefs of its constituencies. The college has embraced a practice of shared
responsibility in the event a religious observance interferes with class work or
assignments. Students who inform instructors in advance of an intended
absence for a major religious observance will not be penalized. The
instructor will make reasonable accommodation for students, which may
include providing a make-up test, altering assignment dates, permitting a
student to attend another section of the same course for a class period or
similar remedies. Instructors are not responsible for teaching material again.
Instructors should inform students of this practice at the beginning of the
semester so that arrangements can be made accordingly. Similar
consideration is accorded to faculty, staff and administrators and is provided
for in their respective contracts.
Effective beginning term:
Fall 2011
Ending term:
Syllabus prepared by:
Gary Mines
Date:
Reviewed by Dept./Prog. Chair:
Approval by Dean:
John Carzoli
Nancy Prendergast
5/2011
Date:
5/2011
Date:
5/2011
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