CH 104 Section 002: Introductory Chemistry
Fall, 2009
4 Credit Hours
Primary Instructor: Stephen Woski
Core Designation: Natural Science
Office Hours: MWF 10:00-11:00 am or by appt.
Four credit hours; three 50-minute lectures, one recitation/exam period, and one 3-hour laboratory per week. University core designation: NS.
Learning Outcomes: Students will learn to:
Chapter 1: Matter
1. Distinguish between a physical and a chemical change.
2. Describe the three states of matter.
3. Classify matter as an element, compound, or a mixture.
4. Identify the name and symbol of an element.
Chapter 2: Measurements in Chemistry
1. Name the units and abbreviations for the metric system.
2. Use prefixes to change units to larger and smaller units.
3. Distinguish between measured numbers and exact numbers.
4. Determine the number of significant figures in a measurement.
5. Round off a calculator answer to report an answer with the correct number of significant figures.
6. In problem solving, convert the initial unit of a measurement to another unit.
7. Calculate temperature values in degrees Celsius and kelvins.
8. Understand the concepts of density and specific gravity.
Chapter 3: Atoms and the Periodic Table
1. Describe the three primary particles in the atom and their locations, charges, and relative masses.
2. Use atomic and mass numbers to determine the numbers of protons, neutrons, and electrons in an atom.
3. Explain what isotopes are and how they affect the atomic mass of an element.
4. Explain how the periodic table is organized and how the position of an element can be used to predict some of its properties such as atomic size and ionization energy.
5. Write the electron configurations for elements in the periodic table.
6. Write the electron dot symbol for a representative element.
Chapter 4: Ionic Bonds Compounds and Their Bonds
1. Be able to describe ions (cations and anions) and ionic bonds
2. Use the octet rule to predict the ionic charge of ions for elements.
3. Be able to name ionic compounds from its formula.
4. Write ionic formulas and names of compounds with polyatomic ions.
5. Recognize common acids and bases.
Chapter 5: Molecular Compounds
1. Be able to describe the nature of covalent bonds.
2. Use the octet rule to predict the number of covalent bonds formed by elements
3. Draw the Lewis structures for covalent compounds.
4. Use VSEPR theory to determine the shape and bond angles of a molecule.
5. Use electronegativity values to identify polar and nonpolar covalent bonds.
6. Identify a covalent compound as polar or nonpolar.
Chapter 6: Chemical Reactions: Classification and Mass Relationships
1. Show that a balanced equation has an equal number of atoms of each element on both sides.
2. Write a balanced equation for a chemical reaction when given the formulas of the reactants and products.
3. Understand the concept of a “mole”.
4. Determine the molar mass of a compound from its formula.
5. Use the molar mass to convert between the grams of a substance and the number of moles.
6. Using a given number of moles/grams of a starting material, determine the corresponding number of moles and/or grams of a product, and visa versa.
7. Determine the limiting reactant, and calculate the amount of product formed.
8. Given the actual yield of a product, calculate the percent yield.
9. Define solubility.
10. Identify a salt as soluble or insoluble.
11. Recognize oxidation-reduction and neutralization reactions.
Chapter 7: Chemical Reactions: Energy, Rates, and Equilibrium
1. Describe potential and kinetic energy.
2. Be able to define enthalpy, entropy, and free energy changes.
3. Describe how temperature, concentration, and catalysts affect the rate of a reaction.
4. Use the concept of reversible reactions to explain chemical equilibrium.
5. Calculate the equilibrium constant for a reversible reaction using concentrations of the reactants and products at equilibrium.
6. Use an equilibrium constant to calculate equilibrium concentrations.
7. Use LeChatelier's principle to describe the shifts in equilibrium concentrations when conditions change.
Chapter 8: Gases, Liquids, and Solids
1. Describe the kinetic theory of gases.
2. Use the gas laws to determine the new pressure, volume, or temperature of an amount of gas.
3. Use the ideal gas law to solve for pressure, volume, temperature, or moles of gas when given three of the variables.
4. Use partial pressure to calculate the total pressure of a gas mixture.
5. Identify the types of forces that hold particles together in liquids and solids and use these to predict physical properties.
6. Calculate the calories lost or gained by an amount of a substance for a specific temperature change.
Chapter 9: Solutions
1. Identify the solute and solvent in a solution.
2. Distinguish between a solution, a colloid, and a suspension.
3. Calculate the percent concentration and molarity of a solution.
4. Use the molarity of a solution in a chemical reaction to calculate the volume or quantity of a reactant or product.
5. Calculate the concentration of a solution prepared by dilution.
6. Describe electrolytes in a solution.
7. Describe osmosis and dialysis.
Chapter 10: Acids and Bases
1. Describe the characteristics of acids and bases.
2. Predict the effect of acid and base strengths on the outcome of reactions.
3. Write balanced equations for reactions of an acid with metals, carbonates, and bases.
4. Use the ion product of water to calculate [H3O+], [OH¯], and pH.
5. Calculate the concentration of an acid solution from titration data.
6. Describe the function of a buffer and the qualities that make a good buffer.
Chapter 11: Nuclear Chemistry
1. Write equations for atoms that undergo radioactive decay.
2. Identify the types of radiation as alpha particles, beta particles, or gamma radiation.
3. Be able to explain the concept of “half-life”.
4. Calculate the amount of radioisotope that remains after a given number of half-lives.
5. Describe nuclear fission and fusion.
Tentative lecture schedule: CH 104 Fall 2009
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Oct 12 CH 7 |
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Aug 19 Review Syllabus |
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Oct 14 CH 8 Gases, Liquids & Solids |
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Aug 20 no recitation |
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Oct 15 recitation |
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Aug 21 CH 1 Matter |
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Oct 16 CH 8 |
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Aug 24 CH 2 Measurements in Chemistry |
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Oct 19 CH 8 |
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Aug 26 CH 2 |
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Oct 21 review |
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Aug 27 recitation |
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Oct 22 Exam 3 (CH 7, 8) |
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Aug 28 CH 3 Atoms and the Periodic Table |
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Oct 23 CH 9 Solutions |
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Aug 31 CH 3 |
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Oct 26 CH 9 |
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Sep 02 CH 3 |
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Oct 28 CH 9(Last Day to Drop) |
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Sep 03 recitation |
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Oct 29 recitation |
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Sep 04 CH 3 |
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Oct 30 CH 9 |
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Sep 07 Labor Day |
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Nov 02 CH 10 Acids & Bases |
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Sep 09 review |
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Nov 04 CH 10 |
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Sep 10 Exam 1 (CH 1, 2, 3) |
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Nov 05 recitation |
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Sep 11 CH 4 Ionic Compounds |
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Nov 06 CH 10 |
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Sep 14 CH 4 |
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Nov 09 CH 10 |
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Sep 15 CH 5 Molecular Compounds |
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Nov 11 CH 11 Nuclear Chemistry |
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Sep 17 recitation |
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Nov 12 recitation |
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Sep 18 CH 5 |
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Nov 13 CH 11 |
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Sep 21 CH 5 |
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Nov 16 CH 11 |
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Sep 23 CH 6 Chemical Reactions |
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Nov 18 review |
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Sep 24 recitation |
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Nov 19 Exam 4 (CH 9, 10, 11) |
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Sep 25 CH 6 |
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Nov 20 review |
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Sep 28 CH 6 |
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Nov 23 no class |
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Sep 30 review |
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Nov 25 No class-Thanksgiving |
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Oct 01 Exam 2 (CH 4, 5, 6) |
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Nov 26 No class-Thanksgiving |
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Oct 02 CH 7 Energy, Rates & Equilibria |
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Nov 27 No class-Thanksgiving |
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Oct 05 CH 7 |
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Nov 30 review |
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Oct 07 CH 7 |
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Dec 02 review |
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Oct 08 mid-semester break |
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Dec 03 recitation |
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Oct 09 mid-semester break |
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Dec 04 review |
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Wed |
Dec 09 Final Exam 11:30 am — 2:00 pm |
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Sections 002 and 003 |
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Thu |
Dec 10 Final Exam 11:30 am — 2:00 pm |
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Section 001 |
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Examinations:
There will be four one-hour exams (100 pts each). Each exam will focus on the material of two or three chapters. A cumulative final exam (100 pts) is scheduled during the prescribed time. The lowest grade of the four one-hour exams will be dropped. The final exam can be skipped with an average exam grade >92%.
Graded homework:
Homework will be assigned using MasteringGOBChemistry. Homework will NOT be accepted late unless excused by the instructor (for illness, etc). The homework grade will be determined as the percentage of successfully completed will count 100 pts toward the course grade.
Laboratory:
Students are required to register for a laboratory section for this course. The grading and policies of the laboratory are set by the Laboratory Coordinator (Ms. Erica Livingston). The laboratory will count for 100 pts toward the course grade. Note that absences from three (3) or more labs will result in failure of the course.
Week of : Lab Experiment:
Aug. 24 Check-in
Aug. 30 Measurement and Significant Figures
Sep. 7 No Labs – Labor Day
Sep. 14 Atomic Structure
Sep. 21 Physical and Chemical Properties and Changes
Sep. 28 Chemical Reactions and Equations
Oct. 5 No Labs – Fall Break
Oct.12 Energy and Matter
Oct. 19 Gas Laws
Oct. 26 Solutions
Nov. 2 Reaction Rates and Equilibrium
Nov. 9 Acids and Bases
Nov. 16 Nuclear Radiation
Nov. 23 No labs – Thanksgiving
Dec. 30 Check-out
The course grade will be determined from the sum of:
3 highest exam grades 300 pts total
final exam grade 100 pts
homework grade 100 pts
laboratory grade 100 pts
total 600 pts
The total points earned will be divided by 6, and grades will be assigned using the scale below:
Score Grade
100-90 A+ / A / A-
89-80 B+ / B / B-
79-70 C+ / C / C-
69-60 D+ / D / D-
59-0 F
Any scaling of grades will be done at the end of the semester and at the discretion of the instructors. Because this is out of your control, DO NOT RELY ON A SCALE BEING APPLIED TO YOUR SCORES!
Attendance at examinations is mandatory unless previous arrangements are made with the instructor. If an exam is missed without prior arrangements being made, a grade of zero will be assigned unless the absence is determined by the instructor to be excused. Excused absences will be granted only with a legitimate, documented excuse (such as illness or death) and should be obtained as early as possible. In these cases, make-up exams will typically not be given, but other arrangements can be made (using drop exam, double-counting of final, etc).
Calculator:
A non-programmable scientific calculator is required for this course. One recommended type is the Casio FX-260 which is available in the SUPE store for ~$10.
All students in attendance at the University of Alabama are expected to be honorable and to observe standards of conduct appropriate to a community of scholars. The University expects from its students a higher standard of conduct than the minimum required to avoid discipline. Academic misconduct includes all acts of dishonesty in any academically related matter and any knowing or intentional help or attempt to help, or conspiracy to help, another student.
The Academic Misconduct Disciplinary Policy will be followed in the event of academic misconduct.
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