BERGEN COMMUNITY COLLEGE

Division of Science and Health

STUDENT COURSE OUTLINE

NOTE: This Syllabus is a general overview of CHM100: The actual homework assignments, test dates,
             grading policy, lab schedule, etc are given in the Master Course Schedule, Laboratory Schedule,
             Grading  Policy and Grading Algorithm as well as Addendum to Syllabus found on this web page.

COURSE TITLE:                                 CHM 100 Introduction to Chemistry

PREREQUISITE:                                 MAT 011 OR A PASSING SCORE ON THE Basic Skills Exam

COURSE DESCRIPTION:   CHM-100 Introduction to Chemistry is designed to give non-science majors an awareness and an understanding of the fundamental concepts of modern chemistry.  Topics include measurement, atomic theory, chemical bonding, the periodic table, chemical reactions, and stoichiometry.  The course includes a writing and communications requirement that relates the topics covered to a broad historical, social, and cultural context.  This is a General Education course.

TEXTBOOK:                 Introductory Chemistry, 2^nd Edition, Russo, S. and Silver, M, Addison Wesley Longman,

                                        2002.

STUDENT LEARNING OBJECTIVES

The student will be able to:

1.        Demonstrate a knowledge of scientific terms.

2.        Write and to understand chemical equations.

3.        Use Metric units.

4.        Solve chemical word problems.

5.        Explain how historically important experiments led to current knowledge of atomic structure and other aspects of modern chemical theory.

6.        Explain how modern chemical theory relates to the properties of substances encountered in everyday life.

COURSE CONTENT:

Chapter 1               Introduction    Scientific Method. Study Skills.  Elements and Compounds.  Physical and Chemical changes.

                                Symbols for Elements.

Chapter 2               Math Skills:  Problem Solving.  Density Problems.  Using Scientific Notation.

                                Measurements:  Metric System.  The Use of the Factor-Label Method and

                                its Application to Problem Solving.  Precision and Accuracy.

Chapter 3               Atomic Theory   Historical Perspectives.  Daltons Atomic Theory.  Exact Atomic Weights.  The

                                Rutherford Model.  Isotopes.

                                The Periodic Table.  Mendeleev's Law of Periodicity of Properties.  The Modern Periodic Table.

                                Other Variations in Properties.  Atomic Sizes.  Ionization Energy.  Electron Affirmity.

Chapter 4               Light:  Wave Properties of Light.  Introduction to Modern Theories of the Nature of Light

                                as Wave and Particle.  Sprectra and Identification of Elements.

                                Electron Arrangement and Chemical Properties:  Bohr Model and the Explanation of the

                                Uniqueness of Spectral Lines of Elements.  Electron Configurations According to the Bohr

                                Model (Atomic Numbers 1-20).  Qualitative Description of the Quantum Mechanical Model

                                for the Atom.

Chapter 5               Chemical Bonds:  Energy and Chemical Bonds.  The Octet Rule.  Ionic Bonds.  Properties of

                                Ionically Bonded Substances.  Covalent Bonds.  Properties of Covalently Bonded Substances. 

                                Lewis Dot Diagrams.  Electronegativity.  Polar and Nonpolar Covalent Bonds.

                                Chemical Nomenclature:  Naming Salts, Binary Covalently Bonded Compounds, Ternary

                                Compounds, Binary Acids, Oxy-Acids.

Chapter 6               Shapes and Polarities of Molecules    Prediction of Shape.  Prediction of Polarity.  Effect of

                                Polarity on Boiling Point and on Solubilty of substances.

Chapter 7               Introduction to Chemical Reactions:  Writing and Balancing Chemical Equations.

                                Types of Reactions:  Combination, Decomposition, Single Displacement and Double Displacement.

                                (Supplementary material will be distributed to students.)

                                Types of Reactions:  Acid-Base, Precipitation, and Redox.  Refer also to Sections 15.2-15.4

Chapter 8               Chemical Arithmetic:  Formula Mass.  Molar Mass.  Chemical Formulas From Percent Composition.

                                Reaction Stoichiometry.  (Limiting Reactant Problems are Optional).  Moles of Gases at STP.  Energy

                                Changes and Chemical Reactions.  Refer Also to Sections 13.1-13.3.

Chapter 9               Electron Transfer Reactions:  Oxidation States and Changes in Oxidation States.  Recognizing Electron Transfer Reactions.  Electricity from Chemical Reactions.  Prevention of Corrosion.              

Chapter 10             Forces of Attraction Between Molecules:  Forces of Attraction and Changes in State.

Chapter 12             Sections 1,4,5,6,7.  Solutions:  Forces of Attraction and the Formation of Solutions.  Introduction to Quantitative Measures of Solute Concentration, (Mass Percent and Molarity).  Omit: Dilution, Titration.

Chapter 15             Further Study of Acids and Bases:  Bronsted Acids and Bronsted Bases.

                                The pH scale.  Buffers.

Notes:               1.        Students will be required to complete at least one written assignment in order to demonstrate the ability to explain some of the concepts studied in this course.  Exams should include definitions and an essay question.

                           2.        All students must complete the laboratory portion of the course in order to receive a passing grade in the course.

                           3.        Any student caught cheating (including using unauthorized formula sheets of any kind) will receive a grade of zero on that particular examination.

EVALUATION:                                 A.  Examinations (and quizzes) . . . . . . . .  75%

                                                             B.  Laboratory Work  . . . . . . . . . . . . . . .    25%

                                                                                                                                         100%

Examinations will include essay questions.  Instructors may require additional writing assignments.  The

scheduled examinations must be completed in order to receive a grade. A student will be allowed either to take

one make-up exam or to use his/her final examination grade in place of one missed examination (policy to be

established by the instructor).

INSTRUCTIONAL RESOURCES:

Special Edition of The Chemistry Place for Introductory Chemistry.  (web site and CD-ROM)

Problem Solving Guide and Workbook for Introductory Chemistry 2^nd edition, Saundra Yancy McGuire.

Basic Concepts of Chemistry, Leo J. Malone, John Wiley & Sons, Inc., (any edition)

SPECIAL NOTES:     Students experiencing difficulty with the arithmetic or problem solving aspects of this course should acquaint themselves with the tutorial services at the Tutorial Center.

OFFICE HOURS:              DAY                                                             TIME

                                     1.

                                     2.

                                     3.

FACULTY ABSENCE PROCEDURE:

A daily listing of canceled classes will appear in the glass case located outside the Evening Office (L-113) as well as in the glass case adjacent to the Hotel/Restaurant bulleting board in East Hall.  If students find a class canceled which has not been listed, they should report this to the Divisional Dean's office, S-338, or the Evening Office.

CHM100 - INTRODUCTION TO CHEMISTRY

LABORATORY SCHEDULE

Text:                 Corwin, Charles.  Laboratory Experiments for Basic Chemistry by Seese and Daub,  Seventh edition.

Week                                                  Topic                                                                                      Page

 1                        Check in; Safety, Basic Laboratory Techniques                                               1-6

                           Instructor should distribute and discuss Divisional

                           Safety rules for the Chemistry Laboratory

 2                        Experiment 2:  Metric System Measurements                                                    15

 3                        Experiment 3:  Density of a Liquid and Solid                                                       29

                           Note:  Part A, on p.32 is to be done as a demonstration. 

 4                        Experiment 5  Physical and Chemical Properties                                               49

                           Note: Part B, Step 1b should be done by the instructor

                           as a demonstration.

 5                        Experiment 7:  Periodic Classification of the elements                                      67

                           Another liquid has been substituted for CC1₄. Includes a

                           discusssion of  Light in Emission Spectra and work with

                           student Spectroscopes observing spectra of flame tests.

6                         *Experiment 8:  Structure of Compounds                                                           75

7                         Experiment 9:  Cation Analysis                                                                             91

                           Collaborative Learning Exercise 1a (Chemical

                           Formulas II)

8                         Experiment 10: Anion Analysis.                                                                           101

                           Collaborative Learning Exercise 1b (Chemical Formulas I)

 9                        Experiment 13: Empirical Formula.                                                                        129

                           Notes:  Part A only to be done by students

                           Part B can only be done by instructor as a demonstration in hood.

10-11                 Experiment 14: Chemical Reactions - Note: Part A,                              137

                           Example 2, p. 140, should be done by the instructor as a demonstration.

                           Students should not do this part.

                           Collaborative Learning Exercise 2 (Balancing Equations and

                           Types of Reactions)

12-13                 Experiment 16: Analysis by Precipitation                                                           157

                           Collaborative Learning Exercise 3 (Stoichiometry)

14                       Experiment 19: Solutions                                                                                       189

15                       Experiment 6:  Change in State                                                                            57

                           Notes:  Use mortar and pestle for grinding materials used   in Part B.

                           Do not grind materials with any other equipment.  Use melting point tubes

                           provided in lab when doing the work for Part B.

*Experiment 8:  Structure of  Compounds may be done at any point in the schedule at the instructor's discretion.

You'll find directions how to do this at <http://go.bergen.edu/email>.

CHM100SCO.Fa00