Section 11 Syllabi

Central Michigan University College of Arts and Sciences Course Syllabus CHM 131 Desig No.

Introduction to Chemistry I Title

4(3-3) Credit(mode)

I.

Bulletin Description Fundamental Concepts of Chemistry. CHM 131 and 132 are recommended to constitute the standard one-year course for science majors. Satisfies University Program Group II laboratory requirement. Group (II-B)

II.

Prerequisites High School Algebra (one unit)

III.

Rationale for Course Level Introductory Course

IV.

Textbooks and Other Materials To Be Furnished by the Student 1. T. L. Brown; LeMay Jr., H.E.; Bursten, B.E. “Chemistry: The Central Science”, 8th Edition, 2000 2. "Chemistry 131 Laboratory Experiments", Current ed, CMU Press 3. Approved Safety Goggles 4. Laboratory Notebook 5. Calculator - Scientific - should do the standard arithmetic, exponential, and logarithmic calculations.

V.

Special Requirements of the Course To earn a passing grade in the course requires that passing grades be earned in both laboratory and lecture.

VI.

General Methodology Used in Conducting the Course Lecture and Laboratory

VII.

Course Objectives Upon completion of the course students will be able to: 1. Produce a general description (both microscopic and macroscopic) of matter. 2. Write and balance chemical equations.

3. 4. 5. 6. 7. 8. 9. VIII.

Carry out calculations necessary to quantitatively interpret chemical equations in terms of moles, mass, volume of solutions and energy. Describe the electronic structure of atoms in terms of elementary Bohr and quantum mechanical models. Use the periodic law to describe the behavior & properties of substances. Carry out calculations necessary to quantitatively describe the bonding in simple substances in terms of elementary covalent and ionic bonding models. Describe the molecular structure of simple covalent species using the VSEPR model. Carry out calculations necessary to quantitatively describe the properties and behavior of substances in the gaseous state. Follow a laboratory procedure, make and record observations, obtain expected results, and carry out calculations necessary for interpretation.

Course Outline Lecture Component 1. Introduction & Basic concepts (1 week) A. Matter B. Units & Measurement C. Problem solving 2. Microscopic Structure of Matter (1 week) A. Atoms B. Periodic Table C. Molecules & Ions D. Nomenclature 3. Mass relationships – Stoichiometry (2 weeks) A. Formulas B. Equations C. Reaction types D. Calculations from Equations 4. Solutions & Reactions in Solution (2 weeks) A. Solution composition B. Reactions in solution C. Solution Stoichiometry 5. Thermochemistry (1 week) A. Energy B. Energy Changes in Chemical Systems C. Energy Change- Enthalpy D. Calorimetry E. Energy in Foods & Fuels 6. Electronic Structure of Atoms (1 week) A. Quantum Theory B. The Bohr Model C. The Quantum Mechanical Model 7. Periodic Properties & the Periodic Table (1 week)

A. Development & History B. Electronic Structure C. Periodic Properties D. Element Types E. Groups/Families 8. Chemical Bonds (2 weeks) A. Lewis/Electron Dot Structures B. Covalent Bonds C. Polar Bonds & Polar Molecules D. Ionic Bonds E. Oxidation Numbers 9. Molecular Geometry & Bonding Theories (2 weeks) A. Prediction of geometries B. Polar Molecules C. Valence Bond Theory 10. Gases (1 week) A. Characteristics & Pressure B. The Gas Laws C. Molar Mass & Densities D. Mixtures & Reactions E. Kinetic Molecular Theory F. Effusion and Diffusion G. Real Gases & the van der Waals Equation

Laboratory Component 1. Density Measurements 2. Experimental Analysis of Hydrates 3. Elemental Analysis of a Metal Oxide 4. Stoichiometry of a Reaction 5. Metathesis Reactions 6. Activity Series of Metals 7. Thermochemistry 8. Preparation and Standardization of a Sodium Hydroxide Solution 9. Volumetric Analysis of an Acid of Unknown Concentration 10. Qualitative Analysis of Anions 11. 9:00 am class: Infrared Spectroscopy 10:00 am class: Molecular Models Lab 12. 9:00 am class: Molecular Models Lab 10:00 am class: Infrared Spectroscopy IX.

Evaluation Four one-hour exams and a final exam (75%) and instructor evaluation of laboratory reports (25%). Writing in the University Program

CHM 131 satisfies the requirement for “A significant amount of meaningful writing” in the following ways. The laboratory portion of the course requires weekly written laboratory reports which include significant writing and calculations. The laboratory portion of the course constitutes 25% of the course grade. The lecture portion of the course requires 5 multiple choice examinations. At least half of the questions on each examination require calculations. The lecture portion of the course counts 75% of the course grade. Therefore, more than half of the course grade in CHM 131 is based on a combination of meaningful writing and calculations. X.

Bibliography Bodner, G.M. & Pardue, H.L., “Chemistry an Experimental Science”, 2 Edition, John Wiley & Sons Inc., NY, NY, 1995 Chang, R., “Chemistry”, 7th Edition, McGraw-Hill Inc., NY, NY, 2002 Masterton, W.L. & Hurley, C.N., 4th Edition, “Chemistry - Principles & Reactions”, Harcourt Brace Jovanovich, NY, NY, 2001 McMurry, J. & Fay, R.C., 3rd Edition, “Chemistry”, Prentice-Hall, Englewood Cliffs, NJ, 2001 Olmsted, J III & Williams, G.M., “Chemistry - The Molecular Science”, Mosby, St. Louis, MO, 1994. Silberburg, M., 2nd Edition, “Chemistry - The Molecular Nature of Matter and Change”, Mosby, St. Louis, MO, 2000 Syllabus Prepared By:

____Calvin D. Tormanen_________________ Name _____________________________________ Signature _____May 14, 2002_____________________ Date

Central Michigan University College of Arts and Sciences Course Syllabus CHM 132 Desig No. (mode)

Introduction to Chemistry II Title

4(3-3) Credit

I.

Bulletin Description Continuation of Chemistry 131

II.

Prerequisites CHM 131, or permission of instructor

III.

Rationale for Course Level Continuation of Introductory Course

IV.

Textbooks and Other Materials To Be Furnished by the Student 1. T. L. Brown; LeMay Jr., H.E.; Bursten, B.E. "Chemistry: The Central Science", 6e, 1994 2. "Chemistry 132 Laboratory Experiments", Current ed, CMU Press 3. Approved Safety Goggles 4. Laboratory Notebook: National Brand 43-644 (Avery Dennison) 5. Calculator - Scientific - should do the standard arithmetic, exponential, and logarithmic calculations.

V.

Special Requirements of the Course To earn a passing grade in the course requires that passing grades be earned in both laboratory and lecture.

VI.

General Methodology Used in Conducting the Course Lecture and Laboratory

VII. Course Objectives Upon completion of the course students will be able to: 1. Describe the properties and behavior of substances in the solid and liquid states. 2. Carry out calculations necessary to describe the properties and behavior of substances in solution. 3. Carry out calculations necessary to interpret kinetic data in terms of energy and reaction mechanism. 4. Carry out calculations necessary to describe simple chemical systems at equilibrium. 5. Carry out calculations necessary to describe the electrochemical behavior of selected chemical species.

6. Use the calculation methods of elementary thermodynamics to describe/interpret the behavior of selected chemical systems. 7. Follow a laboratory procedure, make and record observations, obtain expected results, and carry out calculations necessary for interpretation VIII. Course Outline Lecture Component 1. Liquids and Solids (2 weeks) A. Kinetic Molecular Theory of Liquids and Solids B. Intermolecular Forces C. Properties of Liquids D. Changes of State E. Vapor Pressure F. Phase Diagrams G. Structures of Solids H. Bonding in Solids 2. Solutions (2 weeks) A. Concentration Units B. The Solution Process C. Solubility D. Factors Affecting Solubility E. Colligative Properties F. Colloids 3. Chemical Kinetics (2 weeks) A. Reaction Rate B. Reaction Rate and Concentration: Rate Laws C. Reaction Rate and Temperature: Activation Energy D. Mechanisms of Reactions E. Catalysis 4. Chemical Equilibrium (2 weeks) A. Concepts & Models B. The Equilibrium Constant: Concentrations & Equilibrium C. Evaluating Equilibrium Constants D. Le Châtelier's Principle 5. Acid-Base Equilibrium (2 weeks) A. Acids and Bases: BrØnsted-Lowry Model B. Water: The pH Scale C. Strong Acids & Bases D. Weak Acids & Bases E. Conjugate Pairs: Ka and Kb F. Salts with Acid-Base Properties G. Molecular Structure and Acid-Base Behavior H. Acids and Bases: Lewis Model

6. More Equilibrium (1 week) A. Common-Ion Effect B. Buffer Solutions C. Titration Curves: pH vs. Volume of Titrant D. Solubility Equilibria: Slightly Soluble Substances E. Dissolution and Precipitation: Ksp 7. Electrochemistry (1 week) A. Redox Reactions and Equations B. Balancing Redox Equations C. Voltaic Cells D. Cell EMF E. Electrolysis F. Electro-stoichiometry 8. Thermodynamics (1 week) A. Spontaneous Processes B. Enthalpy (H), Entropy (S) and Spontaneity C. Gibbs Free Energy: G D. AG and Keq Laboratory Component 1. Chromatographic Separation of a Mixture (1 week) 2. Spectrophotometric Quantitation: Beer-Lambert Law (1 week) 3. Colligative Properties (1 week) 4. Inorganic Synthesis (1 week) 5. Chemical Kinetics (1 week) 6. Effect of Temperature on the Rate of Reaction (1 week) 7. Chemical Equilibrium and Le Châtelier's Principle (1 week) 8. Spectrophotometric Analysis of NO2, an Air Pollutant (1 week) 9. Spectrophotometric Determination of the pKa of an acid-Base Indicator (1 week) 10. Weak Acids and Buffer Solutions (1 week) 11. The Solubility Product (1 week) 12. Oxidation-Reduction Reactions (1 week) 13. Electrochemistry (1 week) IX. Evaluation Four one-hour exams, quizzes, and a final exam (75%) and instructor evaluation of laboratory reports (25%). X. Bibliography Bodner, G.M. & Pardue, H.L., "Chemistry an Experimental Science", 2e, John Wiley & Sons Inc., NY, NY, 1995 Chang, R., "Chemistry", 5e, McGraw-Hill Inc., NY, NY, 1994 Masterton, W.L. & Hurley, C.N., "Chemistry - Principles & Reactions", Harcourt Brace Jovanovich, NY, NY, 1993 McMurry, J. & Fay, R.C., "Chemistry", Prentice-Hall, Englewood Cliffs, NJ, 1995

Olmsted, J III & Williams, G.M., "Chemistry - The Molecular Science", Mosby, St. Louis, MO, 1994. Silberburg, M., "Chemistry - The Molecular Nature of Matter and Change", Mosby, St. Louis, MO, 1996 Syllabus Prepared By:

Kenneth R. Magnell Name Signature October 31, 1995 Date

Central Michigan University College of Science and Technology Master Course Syllabus CHM 161H I.

Principles of Chemistry

5(4-4)

Bulletin Description

Intensive introduction to chemical principles for the well-prepared, motivated student. Satisfies University Program Group II laboratory requirements. Prerequisites: Algebra (1 unit), Chemistry (1 unit), or CHM 120; satisfactory Chemistry Placement Test score. (Group II-B) II.

Prerequisites

Algebra (1 unit), Chemistry (1 unit), or CHM 120; satisfactory Chemistry Placement Test score. III.

Rationale for Course Level

This is an introductory honors-level course in chemistry intended primarily for freshmen or other beginning chemistry students. The prerequisites are high school algebra and chemistry, or a lower-level college chemistry course. It is appropriate that this course be at the 100level. IV.

Textbooks and Other Materials to be Furnished by the Student

1. Oxtoby, Gillis, and Nachtrieb “Principles of Modern Chemistry", 4th Ed., Saunders College Publishing (1999) 2. Chemistry 161H Laboratory Manual, CMU Press, Current Edition 3. Pfeiffer, "Pocket Guide to Technical Writing", 2nd Ed., Prentice Hall (2001) 4. Approved safety goggles 5. Laboratory notebook (must have alternating carbonless sheets with detachable original) 6. Calculator (should do standard arithmetic and logarithmic calculations including exponentials, ln, etc.) Non-programmable, non-graphing calculators only will be permitted at quizzes and exams. V.

Special Requirements of the Course

None VI.

General Methodology Used in Conducting the Course

Classroom instruction (four periods per week) involves traditional lectures, problem solving, and inclass quizzes. Laboratory (one four-hour period per week) involves experimentation and data analysis. VII. Course Objectives Upon completion of this course, the student will be able to: 1. Employ basic mathematics (algebra, logarithms, etc.) to solve chemical problems in each of the areas covered. 2. Perform statistical analyses of experimental data, and distinguish between random and systematic errors in experimental results. 3. Employ the Scientific Method to trace the development of ideas from hypothesis through theory to scientific law. 4. Balance chemical equations and demonstrate a practical understanding of their descriptive and quantitative usage. 5. Write proper Lewis dot diagrams for simple covalent molecules and predict their geometries as well as polarities. 6. Use the gas laws to calculate and/or predict the behavior of ideal gases. 7. Explain the essential features of the kinetic-molecular theory and describe the different properties of gases, liquids and solids at the molecular level. 8. Analyze the colligative properties of solutions (vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure) both qualitatively and quantitatively, especially as they are concerned with molecular weight determination. 9. Calculate the thermodynamic properties ΔH, ΔS, and ΔG given adequate experimental data; determine from knowledge of ΔG whether a given reaction is possible; relate ΔGo to the equilibrium constant of a given reaction. 10. Derive mathematical expressions for the equilibrium constant for any chemical reaction; use experimental data to calculate yields; and predict the effects of temperature, pressure, and concentration on the position of equilibrium and the value of the equilibrium constant. 11. Write expressions for the rate of a chemical reaction in terms of its concentrations of reactants and products; determine the kinetic order of a chemical reaction from experimental data; predict the effects of temperature, pressure, concentrations, catalysts, and the energy of activation on reaction rates. 12. Predict the conditions of temperature, pressure and concentrations necessary to produce the maximum yield of a chemical reaction in the minimum amount of time. 13. Describe the structure of the atom and specify the ground state electron configuration for a given atom; use the laws of periodicity to predict the chemical reactivity of the elements based on their position in the Periodic Table. VIII.

Course Outline (Fifteen weeks of lecture and one week for final exam) 1. Introduction: matter: substances and mixtures; elements; laws of chemical combination; atoms; periodic table; molecules; energy (One week) 2. Stoichiometry: empirical and molecular formulas; balanced equations; mass relationships in chemical reactions; limiting reactant and percentage yield (One week)

3. Chemical bonding: electronegativity; ionic bonding; covalent bonds; Lewis diagrams; polar covalent bonding; Shapes of molecules: VSEPR (One week) 4. Gases: chemistry of gases; pressure: Boyle's law; Charles' law; ideal gas law; chemical calculations for gases; mixtures of gases; kinetic theory of gases; Graham's law of effusion; real gases (One week) 5. Liquids and solids: bulk properties of liquid & solids; intermolecular forces; phase equilibria, transitions, diagrams (One week) 6. Solutions: composition of solutions; nature of dissolved species; colligative properties; colloids (One week) 7. Thermochemistry: systems, states and processes; energy, work and heat; heat capacity, enthalpy and calorimetry (One week) 8. Thermodynamics: nature of spontaneous processes; entropy; Gibbs free energy changes and chemical reactions (One week) 9. Equilibrium: nature of chemical equilibrium; thermodynamic description; equilibrium calculations for gas phase reactions; magnitude of K and direction of change; Le Chatelier's principle (One week) 10. Acids and bases: classification of acids and bases; Bronsted-Lowry scheme; acid and base strength; equilibria; buffer solutions; acid-base titration curves (One week) 11. Solubility equilibria (One week) 12. Chemical kinetics: rates of chemical reactions; rate laws; integrated rate laws; reaction mechanisms; reaction mechanisms and rate; effect of temperature on reaction rates; catalysis (Two weeks) 13. Electronic structure: wave motion and light; energy quantization; Bohr model; waves, particles, Schrodinger equation; hydrogen atom; many electron atoms and the periodic table; experimental measures of orbital energies (Two weeks) IX.

Evaluation

Exams count 60% and labs 40% toward overall grade. A passing grade (D-) requires that passing scores be earned in both parts of the course. Exam average is based on three in-semester exams, the average of all in-semester quizzes, and the final exam, all equally weighted. Lab average is based on the percentage of the total available points earned on lab reports. Overall (Exams & Laboratory)* >87 = A; 77-87 = B; 67-77 = C; 57-67 = D; 86 = A; 76-86 = B; 66-76 = C; 56-66 = D; 90 = A; 80-90 = B; 70-80 = C; 60-70 = D;