DESCRIPTION: This is a one semester introductory course designed to provide a broad overview of chemical principles including measurements, atomic theory and bonding, chemical symbols, formulas and equations, inorganic and organic compounds, acid-base theory, and the biochemical highlights of carbohydrates, lipids, proteins, nucleic acids and metabolism. One recitation and two laboratory hours per week.
PREREQUISITES: One year of high school algebra and an acceptable placement score, or DSPM 0800.
NOTE: This course is specifically for students who have had little or no previous chemistry, and who want to prepare to take further college courses in chemistry and/or anatomy and physiology.
INSTRUCTOR:
OFFICE HOURS WILL BE POSTED OUTSIDE THE DOOR BY THE SECOND WEEK OF THE SEMESTER.
REQUIRED MATERIALS
Textbook: Chemistry: An Introduction to General, Organic, and Biological Chemistry, Timberlake, 8th Ed., Harper-Collins.
Laboratory Notebook: A lab notebook with duplicate pages is needed for the laboratory portion of this course that can be purchased in the VSCC bookstore.
Calculator: A scientific calculator is essential for this course.
Additional Requirements: As this is an internet course, all course work should be done via the internet and E-mail.
GENERAL EDUCATION GOAL: This course will provide the student with the essential knowledge necessary for continued study in general chemistry and serve as a foundation for human anatomy and physiology. Chemistry 111 is a laboratory science course that counts toward the natural science general education requirement for non-science majors. Upon successful completion of this course, the student will have demonstrated mastery of sufficient chemical concepts for continued study in chemistry or biology.
OTHER GOALS: This course also seeks to develop the ability to perform mathematical operations on measurements and seeks to provide a means of teaching students to express themselves in a logical and lucid manner as determined by the use of discussion questions on regularly scheduled exams.
OUTCOME STATEMENTS: Upon successful completion of this course, students will have demonstrated the ability to:
2. Use the numerical values of prefixes to write a metric equality.
3. Write a conversion factor for two units that describe the same quantity.
4. Report answers to calculations using the correct number of significant figures.
5. Use a conversion factor to change from one unit to another.
6. Calculate the density or specific gravity of a substance.
7. Use the density or specific gravity to calculate the mass or volume of a substance.
8. Describe forms of energy.
9. Given the temperature, calculate a corresponding temperature on another scale (K, ° F, ° C).
10. Given the mass of a sample and the temperature change, calculate the heat lost or gained.
11. Calculate the energy of a sample using calorimetry data.
12. Identify the physical state of a substance as a solid, liquid, or gas.
13. Given the name of an element, write its correct symbol.
14. Given the symbol of an element, write its correct name.
15. Describe the electrical charge, mass (amu), and location in an atom for a proton, neutron, and electron.
16. Given the atomic number and mass number of an atom, state the number of protons, neutrons, and electrons.
17. Use the periodic table to identify the group and the period of an element, and whether it is a metal or nonmetal.
18. Given the name or symbol of one of the first 20 elements in a periodic table, write the electron configuration.
19. Use the electron configuration of an element to state its group number and to explain periodic law.
20. Using the periodic table, write the electron-dot structures for the first 20 elements.
21. Illustrate the octet rule using the electron-dot structures of the noble gases.
22. Write the formulas of the simple ions for metals and nonmetals.
23. Using charge balance, write the correct formula for an ionic compound.
24. Write a formula of a compound containing a polyatomic ion.
25. Given the formula of an ionic compound, write the correct name.
26. Diagram the electron-dot structure for a covalent molecule.
27. Given the formula of a covalent compound, write its correct name.
28. Given the name of a covalent compound, write its correct formula.
29. Using electronegativity values, classify a bond a covalent, polar covalent, or ionic.
30. Given the chemical formula, determine the formula weight.
31. Given the chemical formula of a substance, calculate the molar mass.
32. Given the number of moles of a substance, calculate the mass in grams.
33. Given the mass of a substance, calculate the number of moles.
34. Classify a change in matter as chemical or physical.
35. Write a balanced equation for a chemical reaction from the formulas of the reactants and products.
36. Describe the energy in exothermic and endothermic reactions.
37. From a balanced equation, write conversion factors for any of the mole relationships.
38. Given the quantity of a reactant or product in a balanced equation, calculate the quantity of another substance in the reaction.
40. Describe the hydrogen bonding in water.
41. Identify the solute and solvent in a solution.
42. Describe the process of dissolving an ionic solute in water,
43. Describe the effects of temperature and nature of the solute on its solubility in a liquid.
44. Calculate the molarity of a solution.
45. Use molarity as a conversion factor to calculate the moles of solute or the volume needed to prepare a solution.
46. From its properties, identify a mixture as a solution, a colloid, or a suspension.
47. Describe the changes in concentration of solute and solvent in the processes of osmosis and dialysis.
48. Identify the components in solutions of electrolytes and nonelectrolytes.
49. Calculate the number of equivalents for an electrolyte.
50. Describe acids and bases using the Arrhenius and the Bronsted-Lowry concepts.
51. Write an equation for the ionization of strong and weak acids.
52. Write a balanced equation for the neutralization reaction of an acid and a base.
53. Use the ion product of water to calculate the hydronium and hydroxide ion concentrations in solution.
54. Calculate the pH from hydronium ion concentration.
55. Given the pH, calculate, the hydronium and hydroxide ion concentrations.
56. Describe the role of buffers in maintaining the pH of a solution.
57. Calculate the molarity or volume of an acid or base from titration information.
58. From its properties, classify a compound as organic or inorganic.
59. Draw the full structural formula and the condensed structural formula for an alkane.
60. Draw the full or condensed structural formulas for the structural isomers of an alkane.
61. Use the IUPAC system to name alkanes.
62. Classify carbohydrates as monosaccharides, disaccharides, and polysaccharides.
63. Classify a monosaccharide as an aldose, or ketose and indicate the number of carbon atoms.
64. Draw and identify Fischer projections for carbohydrate molecules.
65. Draw the open-chain structures for d-glucose, d-galactose, and d-fructose.
66. Draw and identify the cyclic structures of monosaccharides.
67. Describe the monosaccharide units and linkages in disaccharides.
68. Describe the structural features of amylose, amylopectin, glycogen, and cellulose.
69. Describe the classes of lipids.
70. Identify a fatty acid as saturated or unsaturated.
71. Write the structural formula of a wax, fat, or oil produced by the reaction of a fatty acid and an alcohol or glycerol.
72. Draw the structure of the product from the reaction of a triglyceride with hydrogen, an acid or base, or an oxidizing agent.
73. Describe the components of phosphoglycerides, sphingolipids, and glycolipids.
74. Describe the structure of a steroid and cholesterol.
75. Describe the steroid hormones.
76. Classify proteins by their functions in the cells.
77. Draw the structure for an amino acid in neutral or zwitterion form.
78. Describe a peptide bond.
79. Draw the structure for a peptide.
80. Distinguish between the 1° , 2° , 3° , 4° structures of a protein.
81. Describe the enzymes and their functions.
82. Describe the role of an enzyme in an enzyme-catalyzed reaction.
83. Discuss the effect of cofactors, temperature, and pH on enzyme-catalyzed reactions.
84. Describe the effects of an inhibitor upon enzyme activity.
85. Describe the nucleotides contained in DNA and RNA.
86. Describe the structures of RNA and DNA.
87. Explain the process of DNA replication.
88. Describe the structures and characteristics of three types of RNA.
89. Describe the synthesis of mRNA (transcription).
90. Describe the function of the codons in the genetic code.
91. Describe the process of protein synthesis (translation).
92. Describe some ways in which DNA is altered to cause mutations.
93. Explain cellular regulation of protein synthesis.
POLICIES AND PROCEDURES:
Grading: The grades in all chemistry courses will be as follows:
A: 90 - 100 Superior
B: 80 - 89 Above Average
C: 70 - 79 Average
D: 60 - 69 Below Average
F: 0 - 59 Failing
I = Incomplete (see notes below)
W = Withdrawn from course (see notes below)
The grades in chemistry courses will be determined according to the following approximate weighting scheme:
Tests. . . . . . . . . . . . . . . . . . . . . 50%
Final Examination. . . . . . . . . . . .20%
Laboratory Work. . . . . . . . . . . .30 %
Every student must take the comprehensive final exam. Failure to take the final examination will result in a grade of F for the course. In the case where a final examination is missed and the instructor has been notified in advance, it may be possible (at the discretion of the instructor) for the student to receive a grade of I. If the course work is not completed by one week before the first day of final examinations for the next semester, this grade will be automatically converted to a grade of F by the Office of Admissions and Records. (See College Catalog for policies.)
Make-up Tests: There will be no opportunity for a make-up test in this course. At the discretion of the instructor, the grade earned on the comprehensive final exam will be substituted for one missed test. Any other test missed will incur a grade of zero (0).
Make-up Labs: It is rare that a student will be able to make-up missed laboratory work. However, if the instructor is notified in advance and if all instructors involved approve, the student may be allowed to perform the laboratory work at another scheduled laboratory period during the same week. A grade of zero (0) will be assigned for each lab missed but not made up.
Deficiencies: A student who has an average of D or F on work completed and evaluated up to mid semester will receive a mid-term deficiency notice by mail indicating the need for improvement if a course grade of C or better is to be achieved. If a student receives a deficiency notice, he/she should explore with the instructor the wisdom of dropping or continuing in the course.
Cheating: Cheating on a test or exam will incur a grade of zero on that test or exam. Repeated incident will result in an F in the course.
Recommended Problems: These problems and exercises may be handed in for grading upon the direction of your instructor. It is not unusual for questions or problems similar to those assigned to appear on tests or examinations.
Other Regulations: A student is bound by all rules and regulations appearing in the Student Handbook.
Basic Concepts: Definitions, Measurement, Metric System, Dimensional Analysis
Energy & Matter: States, Temperature, Heats, Calorimetry
Atoms & Elements: Elements, the Periodic Table, Periodic Law, Electron Arrangement
Compounds & Their Bonds: Valence Electrons, Bonding, Polarity, Nomenclature
Chemical Quantities & Reactions: Formula Weight, The Mole Concept, Chemical Changes and Equations
Solutions: Molarity, Solubility
Acids & Bases: Electrolytes, the pH Scale, Titrations
Organic Chemistry: Organic Compounds, Alkanes, Isomers, IUPAC Nomenclature
Carbohydrates: Classification of Carbohydrates, Mono-, Di-, and Polysaccharides
Lipids: Fatty Acids, Chemical Properties of Triglycerides, Steroids, Cholesterol
Amino Acids, Proteins, & Enzymes: Types of Proteins, Peptides, Enzyme Action and Inhibition
Nucleic Acids: Structures of Nucleic Acids, RNA, and DNA, Protein Synthesis, Genetic Mutations and Regulation.
ADA Statement:
In compliance with the Americans with Disabilities Act, students are encouraged to register with the Office of Student Disability Services for assistance with accommodations. It is the student's responsibility to voluntarily and confidentially disclose information regarding the nature and extent of a disability. The College does not assume responsibility for providing accommodations or services to students who have not identified themselves as having a qualifying disability.
Equal Opportunity Statement:
Volunteer State Community College is an equal opportunity Affirmative Action Educational Institution. No person shall be excluded from participation in, be denied the benefit of, or be subjected to discrimination under any program or activity of the College because of race, color, national origin, age, or handicap. The College also complies with the Age Discrimination in Employment Act of 1967, as amended and with the Vietnam Era Veterans' Readjustment Act of 1974. The commitment to equal opportunity applies to all aspects of recruitment, employment and education of individuals at all levels throughout the College.