SAN ANTONIO COLLEGE
Chemistry 1311 Syllabus
Department Chemistry & Earth Sciences Effective date Spring, 2005
Course number and title Chemistry 1311 - General Chemistry I Lecture
Credit Hours 3 Hrs/wk lecture 3 Hrs/wk lab 0 Lec/Lab comb. 3_
DISCLAIMER: This syllabus is provided only for general information to indicate typical course organization. Actual course organization may deviate from that shown below.
I. Catalog description: This is a lecture course that covers the fundamental principles of inorganic chemistry: modern atomic theory, chemical bonding, states of matter, solutions, stoichiometry, and other topics. This course is suitable for science majors. If a laboratory is also needed, the student should also enroll in CHEM 1111. CHEM 1311 is equivalent to the lecture portion of CHEM 1411. This course is math-intensive (MI).
II. Required background (List any experience, prerequisites, co-requisites necessary to enroll in the course.): To enroll, the student must show credit for College Algebra (MATH 1314) with a grade of C or better.
III. Textbook, readings and materials (List textbooks, readings, and materials all students are required to provide)
General Chemistry, by Whitten, Davis, Peck and Stanley, 7th ed., Thomson (Brooks/Cole)(2004)
IV. Method of instruction (List the methods to be used to present course content)
1. Textbook reading assignments
2. Lecture
3. Films
4. Homework and/or quizzes
5. Exams
Unit I ‑ Introduction, Measurements and Terminology
1. Elements, Compounds and Mixtures
2. Elemental Symbols
Unit II ‑ Atomic Structure and the Periodic Table
1. The Atomic Theory of Dalton
2. Atomic Weights
3. Subatomic Particles and Their Locations in the Atom: Protons, Neutrons, and Electrons
4. Atomic Number, Mass Number and Isotopes
5. The Periodic Law
6. Wave Properties of Electromagnetic Radiation, Atomic Spectra
7. The Bohr Theory of the Hydrogen Atom
8. The Electron Configuration of the Elements
9. Hund's Rule
10. The Periodic Table Based on Electron Configuration
11. Shapes of s and p Orbitals
12. Classification of the Elements: Metals, Metalloids and Nonmetals and Their Periodic Properties
Unit III ‑ The Mole and Chemical Formulas
1. The Mole, Molar Mass and Avogadro's number
2. Percentage Composition
3. Chemical Formulas
4. Empirical Formulas
5. Molecular Formulas
Unit IV - Stoichiometry
1. The Law of Conservation of Mass
2. Balancing Chemical Equations by Inspection
3. Calculations Involving Chemical Equations based on Mass, Moles and Number of Particles
4. Limiting‑Reagent Calculations
5. Theoretical Yield and Percentage Yield
6. Molar Concentration and Solution Stoichiometry
Unit V ‑ Chemical Bonding
1. Lewis Symbols and Formulas, Including Exceptions to the Octet Rule
2. Formation of Ionic and Covalent Bonds
3. Electronegativity and Polar Covalent Bonds
4. Multiple Bonds
5. Oxidation Numbers
6. The Naming of Inorganic Chemical Compounds
Unit VI ‑ Molecular Structure
1. Valence Shell Electron‑Pair Repulsion Theory
2. Valence Bond Theory
3. Shapes of Polyatomic Species
4. Molecular Polarity
5. Hybrid Orbitals
6. Multiple Bonds
7. Resonance
8. Sigma and Pi Bonds
Unit VII ‑ Chemical Reactions in Aqueous Solution
1. Electrolytes
2. Oxidation and Reduction
3. Classification of Chemical Reactions
Unit VIII ‑ States of Matter: Gases, Liquids and Solids
1. Boyle's Law
2. Charles' Law
3. Gay‑Lussac's law
4. The Combined Gas Law
5. Dalton's Law of Partial Pressures
6. Avogadro's Law and Standard Molar Volume
7. The Ideal Gas Law
8. Graham's Law
9. Kinetic Molecular Theory
10. Deviation of Real Gases from the Ideal Gas Law
11. Intermolecular Attractive Forces
12. Heat of Vaporization
13. Vapor Pressures of Liquids
14. Boiling Points and Freezing Points
15. Types of Solids
16. Sublimation
Unit IX ‑ Properties of Solutions
1. Solute, Solvents and Types of Solutions
2. Molality and Percent Concentration by Mass
3. Factors Affecting the Dissolving of Solutes in Liquid Solvents
4. Colligative Properties of Solutions (Qualitative)
VI. Learning Outcomes (Competencies) and methods of Evaluation used to determine the students have achieved the outcome (competencies):
Competencies
UNIT I - INTRODUCTION, MEASUREMENTS AND TERMINOLOGY
The student should be able to:
1. Classify examples of matter as being either elements, compounds or mixtures.
2. Identify different types and forms of energy.
3. Perform conversions between the Celsius and Kelvin temperature scales.
4. Perform simple calculations relating to specific heat.
UNIT II - ATOMIC STRUCTURE AND THE PERIODIC TABLE
The student should be able to:
5. Describe the development of atomic theory from Dalton's theory to modern atomic theory.
6. Calculate atomic weights from abundances of naturally occurring isotopes.
7. Determine the number of protons, neutrons and electrons in an atom, given a nuclide symbol.
8. Correlate the wavelength, frequency and energy of electromagnetic radiation with electronic transitions.
9. Write the complete electron configuration of any of the first 36 elements.
10. Classify elements according to Periods and Groups, common family names and s, p, d and f blocks on the Periodic Table.
11. Write the valence shell electron configuration and orbital diagram for any representative element, using the Periodic Table.
12. Determine if an element is a metal, a metalloid, a nonmetal, a representative element, a transition element, an inner-transition element or a noble gas, using the Periodic Table.
13. Interpret trends in electronegativity, ionization energy, electron affinity and atomic size, using the Periodic Table.
14. Interpret trends in ionic size, using the Periodic Table.
UNIT III - THE MOLE AND CHEMICAL FORMULAS
The student should be able to:
15. Convert between moles, mass and number of particles for a given substance.
16. Give the number of atoms or ions specified in the chemical formulas of ionic or molecular substances.
17. Determine the percentage composition of a compound.
18. Determine the empirical formula of a compound from its percent composition or mass analysis.
19. Determine the molecular formula of a substance from an empirical formula and molecular weight.
UNIT IV - STOICHIOMETRY
The student should be able to:
20. Balance chemical equations by inspection.
21. Perform calculations involving chemical equations based on mass, moles and number of particles.
22. Perform calculations involving reactions in solution.
23. Perform limiting reagent calculations.
24. Perform percent yield calculations
UNIT V - CHEMICAL BONDING
The student should be able to:
25. Write Lewis formulas for molecules and polyatomic ions.
26. Differentiate between ionic, covalent and multiple bonds.
27. Rank the polarity of covalent bonds, based upon the electronegativities of the bonded atoms.
28. Write the names and formulas of ionic and covalent inorganic compounds.
29. Determine oxidation numbers for atoms in compounds and polyatomic ions.
UNIT VI - MOLECULAR STRUCTURE
The student should be able to:
30. Write structural formulas illustrating the shapes of linear, angular, trigonal planar, pyramidal and tetrahedral molecules and polyatomic ions.
31. Predict the bond angles of simple molecules and polyatomic ions, based upon VSEPR theory.
32. Use the valence bond theory to explain the bonding in various molecules and polyatomic ions, including hybridization of atomic orbitals.
33. Identify polar and nonpolar molecules based upon their molecular shapes and bond dipoles.
UNIT VII - CHEMICAL REACTIONS IN AQUEOUS SOLUTIONS
The student should be able to:
34. Identify strong and weak electrolytes, including the common strong acids and bases.
35. Write balanced molecular, total ionic and net ionic equations.
36. Identify combination, decomposition, single displacement and metathesis reactions.
37. Identify neutralization and precipitation reactions.
38. Identify redox reactions and indicate the oxidizing and reducing agents.
UNIT VIII - STATES OF MATTER: GASES, LIQUIDS AND SOLIDS
The student should be able to:
39. Qualitatively compare the behavior of real and ideal gases.
40. Apply the combined gas law, Dalton's law, Graham's law and Guy-Lussac's law in calculations involving gases.
41. Apply the ideal gas law in calculations involving gases.
42. Apply the kinetic molecular theory qualitatively to explain the behavior of gases on a molecular level, including the distribution of molecular velocity.
43. Describe changes of state through molecular motion.
44. Relate trends in boiling and melting points to the strength of intermolecular forces.
45. Differentiate between amorphous and crystalline solids.
UNIT IX - SOLUTIONS
The student should be able to:
46. Differentiate between solutions and heterogeneous mixtures.
47. Describe the dissolving process of molecular and ionic substances in polar and non-polar liquids.
48. Perform calculations using the concentration unit of molarity, including dilution.
49. Perform calculations using the concentration unit of molality.
50. Qualitatively explain the effect of solute concentration on the four colligative properties of a solution.
UNIT X - LABORATORY COMPETENCIES
The student should be able to:
51. Use chemicals safely.
52. Use chemical equipment and instruments skillfully.
53. Collect data from observations and measurements by performing qualitative and quantitative methods using the metric system.
54. Interpret results and draw conclusions.
55. Evaluate data by applying the concepts of significant figures and scientific notation in carrying out calculations using the factor-label method, including computations involving density and specific gravity.
56. Apply the concepts of: precision and accuracy, physical and chemical properties and changes, exothermic and endothermic changes.
Evaluation: The above competencies will be measured using written exams and a mandatory comprehensive written final exam. Homework and quizzes may be used to supplement evaluation of performance, at the instructor's discretion
SCANS Competencies: N/A
VII. Course requirements and grade computation
A. College Requirements:
A written, comprehensive final examination, not to exceed three hours in length, shall be given at the end of each semester for each course at the regularly scheduled time. Any exceptions to these requirements must be approved by the appropriate dean. Other examinations are given at the discretion of the instructor.
A student who must be absent from a final examination should petition that instructor for permission to postpone the examination. A student absent without permission from a final examination is graded "F." Postponed examinations result in a grade of "I." The final exam must be taken within 120 calendar days from the end of the semester or the grade automatically becomes an "F." (San Antonio College Bulletin, Faculty Handbook - January 1995)
B. Departmental Requirements: N/A
C. Instructor Requirements:
l. Homework and/or quizzes
2. Tests
3. Final exam
A = 90 - 100
B = 80 - 89
C = 70 - 79
F = Below 60
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VIII. College Policies: A. "Students are urged not to bring children to either a class or a lab. Minors under the age of twelve (12) must not be left unattended on campus."
College Academic Council - April, 1998 Adopted by the College Academic Council on May 10, 2000 B. ADA Statement: "As per Section 504 of the Vocational Rehabilitation Act of 1973 and the Americans with Disabilities Act of 1990, if accommodation is needed contact the Office of DisABILITY Support Services, CAC 124C, Phone: 733-2347". C. Academic Dishonesty: Students may be subject to disciplinary proceedings resulting in an academic penalty or disciplinary penalty for academic dishonesty. Academic dishonesty includes, but is not limited to, cheating on a test, plagiarism and collusion. For additional information refer to the "Student Code of Conduct" in the San Antonio College Bulletin. D. Students are required to silence all electronic devices (e.g., pagers, cellular phones, etc.) when in classrooms, laboratories and the library. College Academic Council, January 2000. E. Students must also abide by the policies, procedures, and rules set forth in the "Student Code of Conduct" and all other policies set forth in the San Antonio College Bulletin. |
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Format of Syllabus Adopted by the College Academic Council on May 10, 2000 |