General College Chemistry II

I.     Course Prefix/Number: CHM 122

       Course Name: General College Chemistry II

       Credits: 4 (3 lecture; 3 lab)

II.    Prerequisite

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

  1. General Education.
    1. Identify, define, analyze, interpret, and evaluate: ideas, concepts, information, problems, solutions, and consequences. This includes the ability to compute and comprehend quantitative information and to engage in the scientific process.
  2. Lecture.
    1. Apply differential rate laws and integrated rate laws.
    2. Relate reaction mechanisms to differential rate laws.
    3. Apply the collision model (transition state theory) and Arrhenius equation.
    4. Apply the concept of dynamic equilibrium and quantify the equilibrium constant (K) and reaction quotient (Q) for homogeneous and heterogeneous reactions.
    5. Apply Arrhenius, Brønsted-Lowry and Lewis theories of acids and bases.
    6. Characterize acid strength by evaluating molecular structure.
    7. Quantify the acid and base ionization constants (Ka and Kb) of monoprotic and polyprotic acids and bases.
    8. Relate the autoionization of water to solution acidity or basicity and to the pH and pOH scales.
    9. Classify salt solutions as acidic, basic or neutral.
    10. Quantify the dissociation of polyprotic acids.
    11. Summarize the nature of a buffer and represent the associated equilibrium using the Ka expression or the Henderson-Hasselbalch equation.
    12. Quantify titrations of acids with bases.
    13. Apply the concepts of entropy, spontaneity and Gibb’s free energy change (∆G).
    14. Balance oxidation-reduction equations.
    15. Describe an electrochemical cell (galvanic and electrolytic) and quantify the cathode-anode voltage difference under standard conditions (Eºcell) and nonstandard conditions (Ecell).
    16. Differentiate between types of radioactivity.
    17. Apply the kinetics of radioactive decay and half-life.
    18. Apply the concepts of mass defect and nuclear binding energy.
    19. Describe the basic structure of organic molecules, biomolecules and simple organic functional groups.
    20. Describe the structure of coordination compounds.
    21. Apply crystal field theory to explain optical and magnetic properties of transition metal complexes.
  3. Laboratory.
    1. Minimize risk to self and others by adhering to documented and verbalized laboratory safety policies.
    2. Safely demonstrate basic laboratory skills including filtration, titration, observation and testing of properties of various unknowns, as well as use of a Bunsen burner, high-precision balances, and other basic equipment and glassware.
    3. Perform routine laboratory measurements including mass, volume, and temperature, and record them with proper precision and units; distinguish between measured quantities (raw data) and calculated quantities.

V.    Academic Integrity and Student Conduct

Students and employees at Oakton Community College are required to demonstrate academic integrity and follow Oakton's Code of Academic Conduct. This code prohibits:

• 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.

Please review the Code of Academic Conduct and the Code of Student Conduct, both located online at
www.oakton.edu/studentlife/student-handbook.pdf

VI.   Sequence of Topics

  1. 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
  2. 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
  3. Acids and Bases
    • Acid – base theory
    • Acid-base conjugates
    • Definition and determination of pH and pOH
    • Relative strength of various acids and bases
    • Determination of the pH of strong acid and base solutions
  4. Acid – Base Equilibria
    • Definition of acid and base ionization and Ka, and Kb
    • Definition of water autoionization and Kw
    • Determination of the pH of weak acid and base solutions
    • Determination of the pH of salt solutions
    • Polyprotic acids
    • Buffers and the common ion effect
    • Titration curves
  5. Solubility of Slightly Soluble Compounds
    • Determination of solubility product constants (Ksp)
    • Common ion effect on solubility
    • Effect of pH on solubility
    • Qualitative analysis of metal ions
  6. Thermodynamics
    • Enthalpy and the first law of thermodynamics
    • Entropy and the second law of thermodynamics
    • Exothermic and endothermic reactions; spontaneous and non-spontaneous reactions
    • Gibbs free energy and spontaneity; standard Gibbs free energy and equilibrium constants
  7. Electrochemistry
    • Voltaic cells
    • Electrolytic cells
    • Half reactions of water; electrolysis of aqueous solutions
    • Standard EMF and equilibrium constants
  8. Nuclear Chemistry
    • Nuclear decays, radioactivity, and associated equations
    • Nuclear decay and half life
    • Applications
  9. Transition Metals (TM) and Coordination Compounds
    • Electron Configurations of TM cations
    • Structure and isomerism of coordination complexes
    • Origin of Color in coordination complexes
  10. Introduction to Organic Molecules
    • Alkanes: isomers and nomenclature
    • Structures of organic functional groups
    • Introduction to isomerism in organic compounds

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.

  1. Analysis of an Unknown Chloride
  2. Rates of Chemical Reactions. I – The Iodination of Acetone
  3. Rates of Chemical Reactions. II – A Clock Reaction
  4. Determination of Equilibrium Constant for a Chemical Reaction
  5. Qualitative Analysis of Group I Cations
  6. pH Measurements—Buffers and Their Properties
  7. Acid-Base Titration Curve
  8. Determination of Solubility Product Constant of PbI2
  9. Qualitative Analysis of Group III Cations
  10. Voltaic Cell Measurements
  11. Preparation of Copper(I) Chloride
  12. Determination of an Equivalent Mass by Electrolysis
  13. Determination of the Hardness of Water
  14. Preparation of Aspirin
  15. 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

Course may be taught as face-to-face, hybrid or online course.

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
  • Course may be taught as face-to-face, hybrid or online course.

 

IX.   Instructional Materials

Note: Current textbook information for each course and section is available on Oakton's Schedule of Classes.

Lecture text: Chemistry: A Molecular Approach, 2nd ed. (2011) by Nivaldo Tro (ISBN: 978-0-3216-5178-5) OR Oakton’s custom version of this text for CHM 122 (“Volume 2”) (ISBN: 978-0-5588-1392-5), or comparable text.

Laboratory manual: Chemistry 122 Lab Manual (ISBN: 978-0-4958-3139-6), which is a custom version of Chemical Principles in the Laboratory, 8th edition by Emil Slowinski, Wayne Wolsey, and William Masterton, (2005), 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:

  • 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. Students may also elect to find an alternative source for purchase, as 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

  1. Reading of the text and laboratory material ahead of the class or laboratory session is expected.
  2. Regular attendance at all sessions is expected.  Missed laboratory sessions are not able to be made up.
  3. Class policies on make-up of exams and accepting of late work will be determined by the individual instructor.
  4. Students will be required to review and sign off on their review, understanding, and adherence to basic laboratory safety regulations.
  5. 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.


If you have a documented learning, psychological, or physical disability you may be entitled to reasonable academic accommodations or services. To request accommodations or services, contact the Access and Disability Resource Center at the Des Plaines or Skokie campus. 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.

Oakton Community College is committed to maintaining a campus environment emphasizing the dignity and worth of all members of the community, and complies with all federal and state Title IX requirements.

Resources and support for
  • pregnancy-related and parenting accommodations; and
  • victims of sexual misconduct
can be found at www.oakton.edu/title9/.

Resources and support for LGBTQ+ students can be found at www.oakton.edu/lgbtq.