SAN ANTONIO COLLEGE

1300 San Pedro Avenue, San Antonio, Texas 78212-4289

 

CHEMISTRY 1312 Syllabus

 

Department:    Chemistry, Earth Science and Astronomy   Effective date:    Spring 2005

Course number and title:     Chemistry 1312- General Chemistry II Lecture

Credit Hours:   3   Hrs/wk    Lec. 3     Hrs/wk       lab    0     Lec/Lab comb.   3

 

 

DISCLAIMER: This syllabus is provided only for general information to indicate typical course organization. Actual course organization may deviate from that shown below.

 

I. Catalog description

 

This course is a continuation of Chemistry 1311 including molecular and ionic equilibria, elementary thermodynamics, redox, electrochemistry, kinetics, nuclear chemistry, and other topics. This course is equivalent to the lecture portion of CHEM 1412.  This course is math intensive (MI).

 

II. Required background (List any experience, prerequisites, co requisites necessary to enroll in the course.)

 

Completion of Chemistry 1311 or its equivalent with the grade of "C" or better.

 

III. Texts, other reference materials (List textbooks, readings, and materials all students are required to provide)

 

General Chemistry (7th Ed.), K. W. Whit ten, R E. Davis, M. L. Peck and G. C Stanley, Thomson/ Brooks/ Cole Publishing, Belmont, CA.(2004).

 

IV. Method of instruction (List the methods to be used to present course content)

 

                                                            1. Textbook reading assignments

                                                            2. Lecture

                                                            3. Films

                                                            4. Homework and/or quizzes

                                                            5. Exams

 

V. Course Content

 

Unit I - Chemical Thermodynamics

 

  1. The Three Laws of Thermodynamics
  2. Enthalpy Change.
  3. Hess's Law of Heat Summation
  4. Standard Thermodynamic States
  5. Entropy
  6. Gibbs Free Energy
  7. Predicting Spontaneity using the Gibbs Free Energy
  8. Standard Entropies and Free Energies
  9. Free Energy and Chemical Equilibrium

 

Unit II - Redox reactions and Electrochemistry

 

1.      Oxidation-Reduction Reactions

2.      Balancing Redox Equations by the lon-Electron Method

3.      Electroylsis

4.      Faraday' s Law

5.      Voltaic Cells

6.      Standard Reduction Potentials and Cell Potentials

7.      Thermodynamic Equilibrium Constants and Standard Cell Potentials

8.      The Nernst Equation

 

Unit III - Chemical Kinetics

 

  1. Determination of Reaction Rates and Rate Laws
  2. Half Life of a Reaction.
  3. Collision Theory
  4. Transition State Theory
  5. Reaction Mechanisms
  6. Factors affecting Reaction Rate

 

Unit IV - Chemical Equilibrium

 

  1. The Equilibrium Constant
  2. The Reaction Quotient
  3. Equilibrium Calculations
  4. LeChatelier's Principle and Chemical Equilibrium
  5. The relationship between Kc and Kp
  6. Heterogeneous Equilibria
  7. Equilibrium Calculations

 

Unit V - Equilibria in Aqueous Solutions

 

  1. The Arrhenius Theory of Acids and Bases
  2. Bronsted-Lowry Definition of Acids and Bases
  3. Lewis theory of Acids and Bases
  4. Auto-ionization of Water and pH
  5. Ionization Constants of Weak Electrolytes
  6. Ionization Constants of Polyprotic Acids
  7. Common Ion Effect and Buffers
  8. Hydrolysis Constants
  9. Acid-Base Titration Curves.
  10. Acid-Base Indicators

 

Unit VI - Solubility and Equilibria

 

  1. Solubility and Ksp
  2. Relationship of Ion Product to Solubility
  3. Fractional Precipitation.

 

Unit VII - Nuclear Chemistry

 

  1. Radioactive Decay
  2. Nuclear Transformations
  3. Nuclear Stability and Binding Energy 4. Nuclear Fission and Fusion

 

VI.       Learning Outcomes (Competencies) and methods of Evaluation used to determine the students have achieved the outcome (competencies):

 

Competencies

 

Unit I -THERMODYNAMICS

 

The student should be able to:

  1. Interpret the three laws of thermodynamics.
  2. Calculate DE from work and heat.
  3. Calculate DH, DS, and DG using Hess' Law and also from standard tabulated thermodynamic values.
  4. Calculate DG using the Gibbs-Helmholtz equation.
  5. Predict the spontaneity of a chemical reaction at various temperatures based upon the signs of DH and DS

 

Unit II -REDOX AND ELECTROCHEMISTRY

 

The student should be able to:

  1. Balance equations for redox reactions by the change in oxidation number method or the ion-electron method.
  2. Describe electrolytic and galvanic cells.
  3. Describe the electrode reactions in electrochemical cells.
  4. Perform calculations using Faraday's Law.
  5. Perform calculations involving the Nersnt equation.
  6. Use cell potential to predict spontaneity.
  7. Use cell potential to predict the sign of DG and the relative size of the equilibrium constant.

 

Unit III - KINETICS

 

The student should be able to:

  1. Determine the rate law of a reaction from initial rate.
  2. Use collision theory and transition state theory to explain qualitatively the effect of temperature, molecular orientation, catalysts and concentration on the rate of a chemical reaction.
  3. Given a mechanism, correlate the order of a reaction with respect to a reactant.
  4. Write the rate law for a one-step reaction.

 

 

Unit IV- CHEMICAL EQUILIBRIUM

 

The student should be able to:

1.      Describe chemical equilibrium in terms of rates of forward and reverse reactions.

2.      Write the equilibrium constant expression for a reaction using a balanced chemical equation.

3.      Use equilibrium concentration expression to calculate the equilibrium constant K or equilibrium concentrations at constant temperature.

4.      Compare the reaction quotient and equilibrium constant to predict the direction of a chemical reaction.

5.      Apply LeChatelier's Principle to equilibrium systems and make calculations for K involving new equilibrium concentrations.

6.      Identify reactions in which equilibrium constant in molarity is equal to the equilibrium constant in partial pressures.

7.      Use the qualitative relationship of free energy change and equilibrium constant to determine the spontaneity of a reaction.

 

Unit V- EQUILIBRIUM IN AQUEOUS SOLUTIONS

 

The student should be able to:

1.      Explain, identify, and define acids and bases according to the Arrhenius, Bronsted-Lowry and Lewis concepts.

2.      Explain autoionization of water and the meaning of pH and the equilibrium constant for water.

3.      Compare the relative strengths of acids and bases using ionization constants.

4.      Perform calculations relating to equilibria of weak acids and bases.

5.      Calculate pH, pOH, hydronium and hydroxide ion concentrations for acids and bases.

6.      Calculate the pH of acidic and basic buffers.

7.      Qualitatively rank the concentration of all species present in a solution of a weak polyprotic acid.

 

Unit VI -SOLUBILITY AND EQUILIBRIA

 

The student should be able to:

1.      Determine the solubility product constant given the solubilities.

2.      Calculate the solubility of a salt give the solubility product constant.

3.      Use the ion product to predict precipitation.

4.      Describe fractional precipitation.

 

Unit VII -NUCLEAR CHEMISTRY

 

The student should be able to:

1.      Explain the concepts of radioactive decay, nuclear stability, nuclear fission, nuclear fusion, and nuclear binding energy.

2.      Complete and balance nuclear reaction equations.

3.   Perform calculations dealing with half-life and rates of decay.

4.   Discuss the application of radioactive isotopes.

 

 

Evaluation: The above competencies will be measured using written exams and a mandatory comprehensive written final exam. Homework and quizzes may be used to supplement evaluation of performance, at the instructor's discretion.

 

SCANS Competencies:  N/A

VII.     Course requirements and grade computation

A.        College Requirements:

A written, comprehensive final examination, not to exceed three hours in length, shall be given at the end of each semester for each course at the regularly scheduled time. Any exceptions to these requirements must be approved by the appropriate dean. Other examinations are given at the discretion of the instructor.

A student who must be absent from a final examination should petition that instructor for permission to postpone the examination. A student absent without permission from a final examination is graded "F." Postponed examinations result in a grade of "I." The final exam must be taken within 120 calendar days from the end of the semester or the grade automatically becomes an "F." (San Antonio College Bulletin, Faculty Handbook - January 1995)

B.         Departmental Requirements:  N/A        

C.        Instructor Requirements:  

            l. Homework and/or quizzes

            2. Tests

            3. Final exam

            4. Laboratory work

 

                        A = 90 - 100

                        B = 80 - 89

                        C = 70 - 79

                        D = 60 - 69

                        F = Below 60

 

VIII.      College Policies:

A.        "Students are urged not to bring children to either a class or a lab. Minors   under the age of twelve (12) must not be left unattended on campus."

 

        College Academic Council - April, 1998 Adopted by the College Academic      Council on May 10, 2000

B.    ADA Statement: "As per Section 504 of the Vocational Rehabilitation Act             of 1973 and the Americans with Disabilities Act of 1990, if accommodation        is needed contact the Office of DisABILITY Support Services, CAC 124C,    Phone: 733-2347".

C.    Academic Dishonesty: Students may be subject to disciplinary proceedings            resulting in an academic penalty or disciplinary penalty for academic    dishonesty. Academic dishonesty includes, but is not limited to, cheating on          a test, plagiarism and collusion. For additional information refer to the "Student Code of Conduct" in the San Antonio College Bulletin.

D.     Students are required to silence all electronic devices (e.g., pagers, cellular             phones, etc.) when in classrooms, laboratories and the library.

        College Academic Council, January 2000.

E.      Students must also abide by the policies, procedures, and rules set forth in             the "Student Code of Conduct" and all other policies set forth in the San        Antonio College Bulletin.          

Format of Syllabus Adopted by the College Academic Council on May 10, 2000