General Chemistry w/Lab II
A continuation of general chemistry including bonding and molecular structure, states of matter, solutions, kinetics, equilibria, and acids and bases. Laboratory work includes elementary quantitative analysis. 4 lecture hours; 4 lab hours. Satisfies specified elective requirement for the AA degree.
Prerequisites: A grade of "C" or better in both CHEM& 161 and MATH& 141 (or placement in MATH& 142). Corequisite: Concurrent enro llment in CHEM& 162 Lab.
- Explain the formation of ionic, covalent, and metallic bonds.
- Draw Lewis symbols for atoms and monatomic ions.
- Draw Lewis structures and use VSEPR Theory to predict the shapes of molecules and polyatomic ions; assign formal charges and apply the resonance concept.
- Use Valence Bond Theory and hybridization to explain the structures of molecules and polyatomic ions.
- Apply Molecular Orbital Theory to diatomic molecules and ions.
- Describe and explain the properties of gases, liquids, and solids.
- Know and explain gas laws, including the ideal gas law, using Kinetic Molecular Theory; solve problems using these laws.
- Define and identify the different types of intermolecular forces of attraction and use them to explain the physical properties of liquids and molecular solids.
- Interpret phase diagrams.
- Classify crystalline solids; solve problems involving metallic and ionic crystals.
- Understand the role of intermolecular forces of attraction in the solution process.
- Convert between solution concentration units.
- Know the colligative properties of solutions; solve problems involving these properties, including determining the molar mass of a solute.
- Know the factors that affect the rates of chemical reactions; use the Arrhenius equation to relate rate constants and temperature.
- Write rate laws based on experimental data; propose reaction mechanisms based on experimental rate laws.
- Explain how catalysts function.
- Understand the concept of chemical equilibrium; solve problems involving equilibrium constants, including the effect of temperature on equilibrium.
- Use LeChatlier’s Principle to predict the effects of changes on a system in equilibrium.
- Know and apply the Arrhenius, Bronsted-Lowry, and Lewis definitions of acids and bases.
- Apply the basic concepts of equilibrium to acids and bases, including the use of acid/base dissociation constants.
- Understand the pH concept; calculate the pH of a solution of an acid, base, or salt.