COURSE OUTLINE

Chemistry 103

General Chemistry I

 

 

Fall Semester 2007

 

Instructor: Fred King

Room: P-459

 

 

 

 

Lecture E0E

  1:00 – 1:50 p.m.

MWF

P387

Lab E01

  8:00 - 11:50 a.m.

M

P475

Lab E02

  1:00 - 4:50 p.m.

T

P475

Lab E03

  8:00 - 11:50 a.m.

F

P475

 

Lecture Text:                John C. Kotz, Paul M. Treichel, and Gabriela C. Weaver, Chemistry and Chemical Reactivity, sixth edition, Thomson Brooks/Cole, Belmont Ca, 2006.

 

Laboratory Text:           Chemistry 103 Laboratory Manual, University of Wisconsin - Eau Claire

 

COURSE OBJECTIVES:

 

Chemistry 103 is the first course in the freshman chemistry sequence.  It establishes the foundations for following courses in chemistry, and therefore a solid grasp of the important concepts in 103 is essential for future studies in chemistry.  For those not continuing in chemistry, this course offers an exposure to scientific thinking, a necessity for all educated people.

 

I expect that each student master the following principal course objectives.

 

1.      Understand what constitutes a valid scientific argument.

 

2.      Understand the systematic approach to solve chemistry problems.

 

3.      Obtain a solid working vocabulary of chemical terms.  The Glossary at the back of the textbook (terms highlighted in blue) will be most helpful to you for reviewing.

 

4.      Be familiar with the names of the elements and their chemical compounds and their symbolic representation and the common oxidation numbers.  Be familiar with the periodic table.

 

5.      The writing and interpretation of chemical equations.  Be able to carry out quantitative calculations for chemical reactions.

 

6.      Have some ideas on the nature of the chemical bond and the resulting consequences.

 

7.      Have the basic ideas about electronic configurations and shapes of molecules.

 

8.      Have an understanding of the basic molecular shapes and structures of simple molecules, and their relationship to observable properties.

 

103 TOPICS

 

 

Topic

 

Introduction

a.      Units and Conversion Factors.

b.      Significant Figures.

c.      Graphs and data.

d.      Physical and Chemical Properties.

e.      Classification of Matter: Substance, Elements, Compounds, Mixtures. Analytical Methods.

f.              Scientific Method.

 

Gas Laws

a.      Boyle's and Charles' Laws. Avogadro's Hypothesis.

b.      Ideal Gas Law and Evaluation of the Gas Constant R.

c.      Dalton's Law of Partial Pressures.

d.      Real Gases.

e.      Kinetic Theory of Gases.

 

Atoms, Molecules, and Ions

a.      Laws of Definite and Multiple Proportions.

b.      Atoms: Protons, Neutrons, Electrons. Atomic Number.

         Historical, data-driven development of atomic/particle theories.

c.      Molecules and Ions. Molecular and Ionic Compounds.

d.      Atomic Mass, Molecular Mass. Isotopes.

e.      Avogadro's Number.

f.       Inorganic Nomenclature.

g.      Empirical and Molecular formulas.

 

Chemical Formulas and Equations

a.      Stoichiometry.

b.      The mole concept and molar relationships.

c.      Interpretation of Chemical Equations. Precipitation reactions. Oxidation-reduction.

d.      Limiting reagent.

e.      Molecular and Ionic Equations. Net ionic equations.

f.       Reactions Involving Gases.

 

Periodic Table

a.      Structure of the Periodic Table.

b.      Periodic chemical and physical properties in relation to the periodic table. Predictions.

 

Electronic structure of atoms

a.      Energy levels of Atoms.

b.      Atomic Spectra.

c.      Quantum numbers, n, l, ml, ms .

d.      Atomic orbitals.

e.      Atomic electron configurations.

 

Chemical Bonding

a.      Ionic and covalent bonds. Historical, data-driven development of bonding theories.

b.      Electronegativity. Polarity. Bond Energies.

c.      Lewis Structures. Resonance, formal charge.

d.      Molecular Geometry and its relation to polarity. Dipole moments, bond dipoles.

 

Liquids and Solids

a.      Types of Intermolecular Forces. Impact of IMFs on boiling point, miscibility, the solution process.

b.      Degrees of Molecular Order and Disorder.

c.      Vapor Pressure and Boiling Point. Critical Point.

d.      Sublimation. Fusion. Phase Diagrams.

e.      Solid Structure Types (Ionic, Molecular, etc.).

f.       Crystal Structures.

 

Solutions

a.      Saturation, Unsaturation and Supersaturation.

b.      Concentration Units.

c.      Colligative Properties: freezing point depression, boiling point elevation, osmotic pressure.

d.      Determination of Molar Mass in Solution. Effect of Ionization and Aggregation.

e.             Change of Solubility with Temperature.

 

 

Acids and Bases

a.      Arrhenius' Definitions of Acids, Bases and Salts.

b.      Ionization of Water and Kw.

c.      Calculation of pH in Strong Acids and Bases and their Mixtures.

d.      Nature of Weak Acids. Indicators.

e.      Brønsted-Lowry and Lewis Definitions of Acids and Bases.

 

We may cover other topics in addition to these as time permits, but a great deal of chemical thinking is based on the above topics.

 

OFFICE HOURS

These are posted on my door. I am also happy to meet with you at other times as is necessary.

 

STUDY SUGGESTIONS

In any course, it is particularly advantageous to keep up with the material as it's presented. If you need help with your questions - come see me as soon as possible. The sooner your questions are answered, the easier it will be for you to move on and master the next section of material.

 

You will find it particularly valuable to read assigned material before it is covered in lecture.

 

It is necessary to read each lab experiment in advance of the scheduled lab.

 

 

REQUIRED ITEMS

 (i)     Safety goggles. These must be worn at ALL times when in the lab when experimental work is in progress. You need these for the second lab period.

(ii)     A calculator will be required for lecture exams and some lecture quizzes.

 

ATTENDANCE POLICY

I will record attendance in class as required by university regulations. I will not count attendance as part of the grade. It is particularly important that every effort be made to attend each scheduled lab. ALL laboratory experiments must be completed to receive a passing grade in the course.

 

WORK DUE

A penalty of -20% may be assessed for late work. No work will be accepted once solutions are posted or papers returned. I grade problem sets with amazing speed so you should plan on getting your work completed by the assigned deadline.

 

EXAMS

There will be three exams plus a final exam. The tentative dates for the exams will be October 1, October 29, and November 19. Note: Exam III is just before Thanksgiving recess, keep this in mind when you plan your break. You cannot take Exam III early.

 

There will be 5 lecture quizzes during the semester. If no quizzes are missed, the lowest score will be dropped. Quizzes will be announced.

 

GRADES

The grade obtained in this course will be a composite of your efforts in exams, quizzes, assignments and laboratory work.

 

+ and - grades will be given.

 

Grading breakdown of points

 

Exams (lecture)                                                   

300

Quizzes (lecture)

120

Assignments (Lecture)

130

Laboratory work

250

Final Exam (comprehensive)

200

Course Total

1000

 

 

 

 

 

 

 

 

 

 

 

TENTATIVE LECTURE SCHEDULE

 

Approximate

number

of lectures                                   TOPIC                                                  CHAPTER(s) in TEXT

3

Introduction, Units and Conversion Factors, Significant Figures, Physical and Chemical Properties, Classification of Matter: Substance, Elements, Compounds, Mixtures, Analytical Methods, Scientific Method.

1

2-3

Atoms, Molecules, and Ions. Laws of Definite and Multiple Proportions. Atoms: Protons, Neutrons, Electrons. Atomic Number. Historical, data-driven development of atomic/particle theories. Molecules and Ions. Molecular and Ionic Compounds. Atomic Mass, Molecular Mass. Isotopes. Avogadro's Number. Inorganic Nomenclature. Empirical and Molecular formulas.

2

4-5

Gas Laws. Boyle's and Charles' Laws. Avogadro's Hypothesis. Ideal Gas Law and Evaluation of the Gas Constant R. Dalton's Law of Partial Pressures. Real Gases. Kinetic Theory of Gases.

12

5-6

Chemical Formulas and Equations. Stoichiometry. The mole concept and molar relationships. Interpretation of Chemical Equations. Precipitation reactions. Oxidation-reduction. Limiting reagent. Molecular and Ionic Equations. Net ionic equations. Reactions Involving Gases.

3, 4, 5

3

Electronic structure of atoms. Energy levels of Atoms. Atomic Spectra. Quantum numbers, n, l, ml, ms . Atomic orbitals. Atomic electron configurations.

7, 8

2

Periodic Table. Structure of the Periodic Table. Periodic chemical and physical properties in relation to the periodic table. Predictions.

8

7-8

Chemical Bonding. Ionic and covalent bonds. Historical, data-driven development of bonding theories. Electronegativity. Polarity. Bond Energies. Lewis Structures. Resonance, formal charge. Molecular Geometry and its relation to polarity. Dipole moments, bond dipoles.

9,10

3

Liquids and Solids. Types of Intermolecular Forces. Impact of IMFs on boiling point, miscibility, the solution process. Degrees of Molecular Order and Disorder. Vapor Pressure and Boiling Point. Critical Point. Sublimation. Fusion. Phase Diagrams. Solid Structure Types (Ionic, Molecular, etc.). Crystal Structures.

13

3

Solutions. Saturation, Unsaturation and Supersaturation. Concentration Units. Colligative Properties: freezing point depression, boiling point elevation, osmotic pressure. Determination of Molar Mass in Solution. Effect of Ionization and Aggregation. Change of Solubility with Temperature.

14

3

Acids and Bases*. Arrhenius' Definitions of Acids, Bases and Salts. Ionization of Water and Kw. Calculation of pH in Strong Acids and Bases and their Mixtures. Nature of Weak Acids. Indicators. Brønsted-Lowry and Lewis Definitions of Acids and Bases.

17*

* We will work on acids and bases at several points in the course, including the lab. A handout will be given on pH calculations.