CHM 113 - Introduction to Chemistry
Lecture Hours/Week: 3
Lab Hours/Week: 3
Credit Hours: 4
Prerequisites: MAT 132, or one year of high school mathematics and science
Final Exam Required: Yes
Course Description:
Course Objectives: To provide the student with sufficient skills in chemistry to enable the student to continue his/her studies in fields that require the equivalent of high school chemistry as a prerequisite. These fields include fire science, nursing, biology, and any area that requires general chemistry.
Content Outline:
| Week | Topics |
|---|
| 1-2 | Measurements and calculations: significant figures, dimensional analysis and density |
| 3 | Matter: states of matter, elements, compounds, mixtures and pure substances.
Chemical foundations: symbols for elements, structure of atoms, isotopes, the Periodic Table, formulas for compounds, ions. |
| 4 | Chemical foundations (continued)
Nomenclature: naming binary compounds between metals and nonmetals, compounds that contain polyatomic ions, and acids |
| 5 | Nomenclature (continued):
Chemical reactions: evidence of a chemical reaction, chemical equations, balancing chemical equations |
| 6 | Reactions in aqueous solution: precipitation reactions, acid-base reactions, oxidation-reduction reactions, molecular equations, complete ionic and net ionic equations |
| 7 | Chemical composition: atomic masses, the mole, molar mass, and percent composition of compounds
Chemical quantities: mole ratios, mass calculations, limiting reactants and percent yield |
| 8 | Chemical quantities (continued) |
| 9 | Liquids and solutions: intermolecular forces only (electronegativity, bond polarity and dipole moments first)
Solutions: solution composition (mass percent and molarity), dilution, stoichiometry of solution reactions, and neutralization reactions |
| 10 | Solutions (continued) |
| 11 | Solutions (continued)
Atomic theory: orbitals, electron arrangement of the first 18 atoms in the Periodic Table, electron configuration and the Periodic Table, and atomic properties and the Periodic Table |
| 12 | Atomic theory (continued):
Chemical bonding: types of chemical bonds (ionic, covalent, and polar covalent), electronegativity, bond polarity, dipole moment, stable electron configurations, charges on ions, introduction to Lewis structures and molecular structure |
| 13 | Chemical bonding (continued)
Gases: pressure, Boyle's Law, Charles' Law, Avogadro's Law and the Ideal Gas Law |
| 14 | Gases (continued)
Acids and bases: equilibrium, strong and weak definition of pH, calculation of pH and buffered solutions acids |
| 15 | Acids and bases (continued) |
| 16 | Final Exam |
Laboratory:
| Week | Topics |
|---|
| 1 | Check-in and Safety |
| 2 | Scientific Calculators, Significant Figures and Scientific Notation |
| 3 | Density Determination |
| 4 | The Use of Volumetric Glassware |
| 5 | Take a Breath |
| 6 | Hydrometry |
| 7 | Precipitation Reactions |
| 8 | Graphing Relationships |
| 9 | Stoichiometry of Magnesium Oxide |
| 10 | Stoichiometry of Gas Evolution |
| 11 | Synthesis of Fragrances and Soap |
| 12 | Acid-base Titration, Molarity Calculation |
| 13 | Stoichiometry Review |
| 14 | Molecular Models |
| 15 | Molar Mass of Volatile Liquid |
| 16 | Check-out |
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