CHE 112 - General Chemistry II



Authorizing Signature:

Date:

LEHIGH CARBON COMMUNITY COLLEGE

COURSE OUTLINE

for

CHE 112 - GENERAL CHEMISTRY II

Cluster/Division/Department:

Credit Hours: 4

Lecture Hours: 3

Laboratory Hours: 3

Other: 0

Course Origination Date:

Reviewed/Revised Date: September 1997

Submitted by:

Prerequisite(s): General Chemistry I

Corequisite(s): None

Course Description

Continuation of General Chemistry I emphasizing solutions, kinetics, gaseous and solution equilibrium, acid/base and solubility equilibria, thermodynamics, electrochemistry, balancing redox equations, descriptive chemistry of main group elements, coordination chemistry, and introduction to organic chemistry.

Computers are used in lecture and the laboratory. The laboratory uses microscale techniques.

Course Objectives

Having completed the course, the student will be able to:

1. Solve problems involving

a. The Clausius-Clapeyron equation.

b. Molarity, molality, mole fraction, and weight percent.

c. Raoult’s Law.

d. Colligative properties.

e. Chemical kinetics.

f. Chemical equilibrium.

g. Electrochemistry.

2. Recognize zero, first, and second order reactions.

3. Discuss the molecular basis of chemical kinetics.

4. Write expressions for both homogeneous and also heterogeneous equilibria.

5. State the significance of a K equilibrium value as to extent of a chemical reaction.

6. Predict shifts in the position of equilibrium using Le Chatelier’s Principle.

7. Classify acids and bases in Bronsted and Lewis Theories.

8. Discuss acid/base strength using Ka values and use the pH scale to relate hydronium and hydroxide concentrations.

9. Discuss and solve problems involving titration, buffers, and the hydrolysis of ions.

10. Predict whether a precipitate will form when two solutions are mixed and solve K problems.

11. Understand and relate enthalpy, entropy, and free energy as they relate to chemical reactions and equilibrium.

12. Discuss the working of both the voltaic and electrochemical cells and solve problems involving them.

Course Content

I. Properties of Solutions

A. The Solution Process

B. Ways of Expressing Concentration

C. Saturated Solutions and Solubility

D. Factors Affecting Solubility

E. Colligative Properties

F. Colloids

II. Chemical Kinetics

A. Reaction Rates

B. The Dependence of Rate on Concentration

C. Change of Concentration With Time

D. Temperature and Rate

E. Reaction Mechanism

F. Catalysis

III. Chemical Equilibrium

A. The Concept of Equilibrium

B. The Equilibrium Constant

C. Heterogeneous Equilibria

D. Calculating Equilibrium Constants

E. Applications of Equilibrium Constants

F. Factors Affecting Equilibrium: Le Chatelier’s Principle

IV. Acid-Base Equilibria

A. The Dissociation of Water

B. Bronsted-Lowry Acids and Bases

C. The pH Scale

D. Strong Acids and Bases

E. Weak Acids

F. Weak Bases

G. Relation Between Ka and Kb

H. Acid-Base Properties of Salt Solutions

I. Acid-Base Behavior and Chemical Structure

J. Lewis Acids and Bases

V. Additional Aspects of Aqueous Equilibria

A. The Common Ion Effect

B. Acid-Base Titrations

C. Buffered Solutions

D. Solubility Equilibria

E. Criteria for Precipitation or Dissolution

F. Qualitative Analysis for Metallic Elements

VI. Chemical Thermodynamics

A. Spontaneous Processes

B. Spontaneity, Enthalpy, and Entropy

C. A Molecular Interpretation of Entropy

D. Calculation of Entropy Changes

E. Gibbs Free Energy

F. Free Energy and Temperature

G. Free Energy and the Equilibrium Constant

VII. Electrochemistry

A. Oxidation-Reduction Reactions

B. Balancing Oxidation-Reduction Equations

C. Voltaic Cells

D. Cell EMF

E. Spontaneity of Redox Reactions

F. Effect of Concentration on Cell EMF

G. Commercial Voltaic Cells

H. Electrolysis

I. Quantitative Aspects of Electrolysis

VIII. Chemistry of Coordination Compounds

A. Structure of Complexes

B. Chelates

C. Nomenclature

D. Isomerism

E. Ligand-Exchange Rates

F. Color and Magnetism

G. Crystal-Field Theory

IX. Introduction to Organic Chemistry

A. Alkanes

B. Unsaturated Hydrocarbons

C. Hydrocarbon Derivatives

X. Chemistry of Main Group Elements

A. Periodic Trends

B. Chemical Reactions

C. Hydrogen, Oxygen, Nitrogen, and Carbon

D. The Noble-Gas Elements

E. The Halogens

F. Group 6A Elements

G. Group 5A Elements

H. Group 4A Elements

Suggested Laboratory Experiments

1. A Cycle of Reactions of Copper

2. Molar Mass From Freezing Point Depression in T-butyl Alcohol

3. Kinetic Study of a Chemical Reaction

4. Chemical Equilibrium Using Spectroscopy

5. Studying Equilibria and Applying Le Chatelier’s Principle

6. Using Microscale Techniques

7. Determination of Ka of a Weak Acid

8. The Chemistry and Qualitative Analysis of Group I Cations

9. Group I Unknown

10. A Study of pH, Dissociation, Hydrolysis, and Buffers

11. Chemistry and Qualitative Analysis of Group II Cations

12. Group II Unknown

13. The Chemistry and Qualitative Analysis of Groups III and IV Cations

14. Unknown Group III and IV

15. The Chemistry and Qualitative Analysis of Anions

16. Anion Unknown

Teaching and Grading Procedures

Chemistry is taught using a combination of teaching techniques:

1. Lecture

2. Overhead Transparencies

3. Coordinated Lecture-Laboratory

4. Computer Simulations

5. VCR/Film/Videodisc - demonstrations

Student progress is evaluated with quizzes, lecture exams, and laboratory reports. Exams and quizzes - 80% and Laboratory Reports - 20%

Textbook(s)

Birk, James P., Chemistry, Houghton Mifflin Company, 1994.

Brown, Lemay, Bursten, Chemistry the Central Science, 7th Edition, Prentice Hall Inc., 1997.

Ebbing, Darrell D., General Chemistry, 5th Edition, Houghton Mifflin Company, 1996.

Kotz and Percell, Chemistry and Chemical Reactivity, 3rd Edition, Saunders College Publishing, 1996.

Petrucci and Harwood, General Chemistry, 7th Edition, Macmillan Publishing Co., 1997.

Zumdahl, Steven S., Chemistry, 4th Edition, D.C. Heath and Company, 1997.

Suggested Laboratory Manuals

Neidig, H. A., Program Editor, Modular Program in Chemistry, Chemical Education Resources.

Nelson, J., and Kemp, K., Laboratory Experiments 7/E, 1997, Macmillan/Prentice Hall.

Milio, Debye, and Metz, Experiments in General Chemistry, 1991, Saunders College Publishing.

Pike, R., Szafran, Z., Foster, J., Microscale General Chemistry Laboratory Manual, 1993, John Wiley & Sons Publishing.

Weiss, G., Experiments in General Chemistry, 6/E, 1993, Macmillan/Prentice Hall.

PERM CHE112

10/21/97

OFFICIAL

Lehigh Carbon Community College

|Course Number and Title: |CHE 112, General Chemistry II |Date: |Jan. 12, 2005 |

Course-Specific Student Learning Competencies

|Objective |Means for Addressing Objective |Means for Measuring Objective |

|Solve problems involving |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|The Clausius-Clapeyron equation, Molarity, |Experiments, Class discussion |Reports |

|molality, mole fraction, and weight percent, | | |

|Raoult’s Law, Colligative properties, Chemical | | |

|kinetics, Chemical equilibrium, | | |

|Electrochemistry. | | |

|Recognize zero, first, and second order |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|reactions. |Experiments, Class discussion |Reports |

|Discuss the molecular basis of chemical |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|kinetics. |Experiments, Class discussion |Reports |

|Write expressions for both homogeneous and also|Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|heterogeneous equilibria. |Experiments, Class discussion |Reports |

|State the significance of a K equilibrium value|Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|as to extent of a chemical reaction. |Experiments, Class discussion |Reports |

|Predict shifts in the position of equilibrium |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|using Le Chatelier’s Principle. |Experiments, Class discussion |Reports |

|Classify acids and bases in Bronsted and Lewis |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|Theories |Experiments, Class discussion |Reports |

|Discuss acid/base strength using Ka values and |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|use the pH scale to relate hydronium and |Experiments, Class discussion |Reports |

|hydroxide concentrations. | | |

|Discuss and solve problems involving titration,|Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|buffers, and the hydrolysis of ions. |Experiments, Class discussion |Reports |

|Predict whether a precipitate will form when |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|two solutions are mixed and solve K problems. |Experiments, Class discussion |Reports |

|Understand and relate enthalpy, entropy, and |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|free energy as they relate to chemical |Experiments, Class discussion |Reports |

|reactions and equilibrium. | | |

|Discuss the working of both the voltaic and |Textbook, Homework, Lecture, Laboratory |Quizzes, Homework grades, Exams, Laboratory |

|electrochemical cells and solve problems |Experiments, Class discussion |Reports |

|involving them | | |

PERM CHE112 (2/25/05)

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