Prerequisites: MA091 or equivalent; completion within the past five years with a grade of C or better of one year of high school chemistry or CH100.
Three hours of lecture, four hours of laboratory each week
4 semester hours
The current text book for this course is "Chemistry, The Central science" tenth edition by Brown, Lemay and Bursten.
The following is a typical syllabus for material covered in the course. Note: the exact coverage of the material and order of coverage may vary depending on the instructor.
Chapter 1: Scientific method, law of conservation of mass, properties of matter (elements, compounds, mixtures), measurements and the metric system, significant figures, dimensional analysis, density
Chapter 2: Dalton's atomic theory, structure and composition of the atom, isotopes, atomic masses , periodic table, chemical formulas and nomenclature, writing and balancing chemical equations
Chapter 3: Concept of electrolytes and nonelectrolytes, molecular versus ionic equations, classes of chemical reactions, balancing oxidation-reduction reactions
Chapter 4: Molecular and formula masses, concept of the mole, percent composition, determination of empirical formulas, stoichiometry (limiting reactants, percent yield), concept of solution concentration (molarity) and dilution, titrations
Note: with the exception of balancing oxidation-reduction reactions, the material in the first four chapters is considered to be review material. Consequently, it is covered at a fairly rapid rate. If you have never taken chemistry before, or a few years have passed since your last chemistry course, it is highly recommended that you take CH100A (Introductory Chemistry) first before attempting this course. If you feel that you do not need to take CH100A, but could use a review of some of the concepts in the first four chapters then consider registering for Chem. 101-R along with Chem. 101 for a quick review.
Chapter 5: Concepts of thermochemistry, forms of energy, specific heat and heats of reaction, concept of enthalpy and changes in reactions, measuring heats of reaction, Hess's Law, standard enthalpies of formation
Chapter 6: Electromagnetic spectrum and concept of waves (wavelength, frequency), photons, Bohr model of the atom, quantum numbers, atomic orbitals
Chapter 7: Electron configurations of elements, and general trends in the periodic table for atomic radius, ionization energy, and electron affinity
Chapter 8: Lewis dot structures, ionic versus covalent bonding, electronegativity, resonance, formal charges, bond order and bond length, bond energy
Chapter 9: VSEPR concept and molecular geometry, concept of polar bonds and polar versus nonpolar molecules, valence bond theory of covalent bonds and hybrid orbitals, concept of multiple bonding
Chapter 10: Properties of gases, various gas laws, ideal gas law, gases in stoichiometry calculations, partial pressures, kinetic-molecular theory, diffusion and effusion, concept of real gases
Chapter 11: Concepts of phase transitions, vapor pressure, phase diagrams, surface tension, viscosity, intermolecular forces, types of solids
Chapter 13: Solutions and concepts of solubility and factors affecting solubility of different solids, liquids, and gases in liquids, concentration concepts of molarity, mass percentage, molality, and mole fraction, vapor pressure of solutions and colligative properties (boiling point elevation, freezing point depression, osmotic pressure, colloids)
RCH101 LABORATORY SCHEDULE Spring 2006
| Week (dates) | Activity | Exercise (page) |
| 1. (1/23 - 28) |
Safety Orientation (Required for all subsequent activities) Introduction to the Chemistry Laboratory Grid Experiment |
I (10 - 12) I (3,6, 7 - 9) I (15) |
| 2. (1/30 - 2/4)
|
Measurement Check-In & sign "Statement of Understanding" Signficant figures (appendix*; bring answers to class.) |
I (19) I (4,5,13) III (117) |
| 3. (2/6 - 11) |
The Formula of a Hydrate Pick up reference worksheet. (Due next week) |
3 (27) |
| 4. (2/13 - 18) | Properties of Oxygen and Oxides | 15 (75) |
| 5. (2/20 - 25) | Relative Oxidizing Power of Metal Cations | 5 (33) |
| 6. (2/27 - 3/4) |
Solution Preparation Standardization |
16 (79) 17 (81) |
| 7. (3/6 - 11) |
Molar Weight of an Unknown Acid Percent Acetic Acid in Vinegar Solving Concentration Problems (pgs. 181-182) |
18 (83) 19 (85) XI (177) |
| 8. (3/13 - 18) |
Heat of Reaction and Hess's Law (Mid term cleaning of Lab) |
6 (35) |
| 9. (3/20 - 26) |
Spring Recess, no classes |
|
| 10. (3/27 - 4/1) | Synthesis of Alum Crystals from Aluminum | 12 (63) |
| 11. (4/3 - 8) |
Alum (weigh product and take melting point) Paper chromatography |
2 (23) |
| 12. (4/10 - 15) | Models of Structure and Bonding | 14 (69) |
| 13. (4/17 - 22) |
Boyle's Law - Volume and Pressure Gay-Lussac's Law - Pressure and Temperature Gas Law Data |
9 (49) 10 (53) 11 (59) |
| 14. (4/24 - 29)
|
Molar Gas Volume & Universal Gas Constant Solving Gas Law Problems (first set - pgs. 165 - 166; bring answers to class.) NOTE: No experiments peformed after Saturday, April 29, 2006 |
7 (341 IX (159) |
| 15. (5/1 - 6) | Lab practical and checkout | |
| 16. | All day classes take the final exam on Thursday, May 11, from 2:45 - 4:45 pm in assigned rooms. | |
*Note: Worksheets for all assigned Appendices are to be done before class.
Also, always check the bulletin board outside the Study Room (Rm 13) for the latest information.