Instructor: Michael Davis Office: 3226 Phone: 773 907 4718 Office Hours: Tues 9:00 12:00 Wed 1:00 3:00 Thurs 9:00 12:00 Email: mdavis@ccc.edu Website: http://faradaysclub.com http://ccc.blackboard.com Class Schedule: Monday 8:30 12:10 PM Lecture/Lab Room 3831 Wednesday 8:30 12:10 PM Lecture Room 3831 Class will begin promptly at the starting time on each day we meet. Textbook Title: Chemistry a Molecular Approach 3 rd Edition Author: Tro ISBN 9781323039571 NOTE: This is a custom version of a traditional textbook. You can purchase or rent the entire textbook from Amazon. The book itself is recommended, not required. Any general chemistry text will suffice. Textbooks can be ordered through ccc.textbookx.com. Required Equipment Eye protection, scientific calculator, Mastering General Chemistry access codes, and Laboratory Notebook. All students will be required to wear proper eye protection at all times while in the laboratory. Students with glasses will be required to obtain either safety shields or goggles in addition to their glasses. Goggles tend to be more comfortable than safety glasses if you already wear glasses. A scientific calculator is most useful for this class, but it need not be expensive. The ability to input scientific notation will be most helpful.
Examination Three exams will be given at five-week intervals throughout the semester and a final exam at the end of the semester. These exams will include material from 3-4 chapters of the text covered previous to the exam. Conflicts with exam times that are associated with college-approved activities may be rescheduled for an earlier date per consultation with the instructor. In Class Work Grades are not attendance based per se, but a certain amount of graded work will be assigned and collected in class. This work will be done individually or in groups, and can only be completed on the day it is assigned. Laboratory Laboratory experiences are an integral portion of this course. We will complete at least one lab per week throughout the semester. Labs must be completed in order to successfully complete the course. Labs will be handed out at the start of each week. Grading Task Value Three Exams 300 points Final Exam (Cumulative) 100 points In Class Work 80 points Quizzes 80 points Homework 110 points Labs (14) 280 points Final Assessment ACS 50 points Exit exam Total 1000 Point values are approximate and are subject to change. Letter grades Percentage Letter Grade 100 90 A 89 80 B 79 70 C 69 60 D 59 0 F
There will be NO make-up exams, quizzes, homework, or laboratory sessions. Everything will be collected at the START of class on the day it is due. Late work will not be accepted. Catalog Course Description Topics include the periodic table of the elements, atomic structure, basic concepts of quantum theory, bonding, stoichiometry of compounds and reactions, thermo chemistry, the gaseous state, basic concepts of liquid and solid states, solutions, acids and bases. Writing assignments as appropriate to the discipline are part of the course. Quizzes Brief quizzes will be given on a weekly basis covering content from laboratory and lecture. These quizzes will generally have 3 to 4 questions and will be taken individually. The same quiz will be given in small groups of four or five, and the recorded score will be the average of the two. Online Homework All homework will be completed online using the Mastering General Chemistry submission system. This is provided by the book publisher and may be purchased separately or through the publisher directly. This is a required portion of the class. Information about this system can be found on the class website. Exceptions Course Name: Chemistry 201 Course Code: davis34362 Taking into consideration that from time to time people have a need to focus their attention on the nonacademic portion of their lives, the following exceptions will be made to the grading scheme. The lowest of the 20-point labs will be dropped. The lowest of the 10-point homework assignments will be dropped. The lowest of the 10-point quizzes will be dropped. Academic Honesty All students are expected to adhere to the academic honesty policies as laid out in the CCC Student Policy Manual. Any student found in violation of this policy will meet with the appropriate punishment.
Student Learning Outcomes Upon successful completion of this course a student will be able to: Solve quantitative chemistry problems and demonstrate reasoning clearly and completely. Integrate multiple ideas in the problem solving process. Describe, explain and model chemical and physical processes at the molecular level in order to explain macroscopic properties. Classify matter by its state and bonding behavior using the Periodic Table as a reference. Apply important theories such as the Kinetic Molecular Theory of Gases or the Quantum Mechanical Theory of the Atom to the solution of general chemistry problems. Perform general chemistry laboratory experiments using standard chemistry glassware and equipment and demonstrate appropriate safety procedures. Record, graph, chart and interpret data obtained from experimentation and use that information to correctly identify/analyze assigned unknown substances. Objectives Each course objective is cross referenced with a specific General Education Goal (GEG). Upon successful completion of this course, the successful student will be able to: Scientific Method (R) Describe the scientific method. (R) Define and explain the terms: law, hypothesis, and theory. Chemical Calculations (R) Use exponential notation. (R) Do mathematical calculations involving significant figures. (R) Differentiate between mass and weight. (R) Convert from the English system to the metric system (& vise versa) common units of length, mass, volume, and temperature. (R) Use the metric system in calculations. Heat and Temperature (R) Differentiate between heat and temperature. (R) Do simple calculations of heat changes using specific heat. Define and use the terms standard state, standard enthalpy change, molar enthalpy of formation. Density (R) Solve problems using density as the relationship between mass and volume. Properties of Matter
(R) Use and define (describe or explain) basic chemical concepts with respect to properties of matter: physical states of matter, physical and chemical properties of matter, physical and chemical changes, the law of conservation of mass, the law of conservation of energy, the law of definite composition, classification of elements. (R) Distinguish between pure substances (elements and compounds) and mixtures (homogeneous and heterogeneous). List the names and chemical symbols of at least 48 elements. Atomic Theory and Structure, Molecular Theory and Structure (R) Distinguish between ionic and molecular compounds. (R) Determine the number and types of atoms represented in a chemical formula. Use basic chemical nomenclature for inorganic compounds. Write the formulas of binary ionic compounds, common binary molecular compounds, and at least 12 common acids, 4 common bases, inorganic ternary compounds using 15 common polyatomic ions. Use oxidation numbers to distinguish oxidation states of metals in compounds. (R) Balance chemical equations given the formulas of the reactants and products. Calculate the oxidation number of each element, given the formulas of the reactants and products. Balance redox equations using oxidation numbers. (R) List the basic principles of Dalton's atomic theory and indicate how the theory has been further developed in this century. (R) State the basic properties of the subatomic particles: protons, neutrons, and electrons. (R) Describe the Rutherford atom. (R) Define atomic number, mass number, and isotopes. (R) Define the atomic mass unit and Avogadro's number. (R) Use the conversion factor from grams to amu in simple calculations. Calculate the average atomic mass from isotopic masses and percent abundances. (R) Apply the terms: metals, nonmetals, alkali metals, alkaline earth metals, metalloids, transition metals, noble gases, halogens, and inner transition metals to the arrangement of elements in the periodic table. (R) Describe the arrangement of the elements in the periodic table. (R) Use the periodic table to predict formulas of compounds. (R) Define the terms anion, cation, and polyatomic ion. Describe how ionic and covalent bonds are formed. Calculate the oxidation number of each element in a chemical formula. Mole-Mass Calculations (R) Calculate the percent composition of compounds, given the formulas.
(R) Calculate the empirical formula, given the percent composition. (R)Calculate the empirical formula of compound given the mass of the sample, the mass of CO2 and mass of H2O produced in a combustion reaction. (R) Distinguish between empirical and molecular formulas. (R) Explain the concepts of the chemical quantity, the mole, and relate it to counting of atoms and molecules. (R) Convert mass in grams to moles, formula units, molecules (and/or atoms) using atomic weights, formula weights, and molecular weights. List the basic rules which predict whether a salt is soluble in water. Stoichiometry Write the balanced equations describing several examples of combustion, acid-base, precipitation, and exchange reactions. Write the equations in the molecular, total ionic and net ionic format. (R) Explain the information given by the balanced chemical equations. Perform stoichiometric calculations from a given chemical equation. Use calculations determine the limiting reagent, how much excess reagent is left, and the theoretical and percentage yield of each product. Solutions List the properties of solutions and distinguish true solutions from heterogeneous and colloidal mixtures. Define solubility, percent concentration, molarity, mole fraction, and molality. Explain factors affecting solubility and the rate of dissolving. Write molecular, total ionic and net ionic equations which show that the solution is the reaction medium. Use percent concentration, molarity, and molality in stoichiometric calculations.
Tentative Semester Schedule Week starting Topic Chapter Jan. 12 Scientific Method / Inquiry / Measurement 1 Jan. 19 Measurement / Atoms & Elements 1, 2 NOTE: No Class Monday Jan. 26 Chemical Reactions 2, 3 Feb. 2 Chemical Quantities 4 Feb. 9 Exam 1 Feb. 16 Phases of Matter Gases 5 Feb. 23 Phases of Matter Solutions 12 Mar. 2 Solutions / Thermochemistry 12, 6 Mar. 9 Quantum Mechanics 7 Mar. 16 Exam 2 Mar. 23 Periodic Properties 8 Mar. 30 Spring Break No Class N/A April 6th Chemical Bonding 9 April 13 th Chemical Bonding 10 April 20 th Intermolecular Forces 11 April 27 th Exam 3 May 4 th Final Exam ACS Assessment