CHEM 112 General Chemistry 2*
The study of elementary theoretical chemistry and its application to analytical practice. The lecture includes redox, kinetics, coordination, and nuclear chemistry plus the aqueous equilibria of acids, bases, complexes, and slightly soluble compounds. The laboratory work consists of the qualitative separation and identification of cations and selected inorganic experiments.
CHEM 112General Chemistry 2*
Please note: This is not a course syllabus. A course syllabus is unique to a particular section of a course by instructor. This curriculum guide provides general information about a course.
I. General Information
II. Course Specification
Course Type
{D7A8FC71-978F-4003-9933-512C476323B2}
Credit Hours Narrative
5 Credits
Semester Contact Hours Lecture
45
Semester Contact Hours Lab
90
Prerequisite Narrative
CHEM 111 and MATH 147 or MATH 143.
Corequisite Narrative
CHEM 112L
III. Catalog Course Description
The study of elementary theoretical chemistry and its application to analytical practice. The lecture includes redox, kinetics, coordination, and nuclear chemistry plus the aqueous equilibria of acids, bases, complexes, and slightly soluble compounds. The laboratory work consists of the qualitative separation and identification of cations and selected inorganic experiments.
IV. Student Learning Outcomes
Upon completion of this course, a student will be able to:
- Describe the factors that affect the rates of chemical reactions. Students will be able to calculate rate laws, determine rate constants, use reaction mechanisms and determine the change in the concentration of reactants as a function of time.
- Define the concepts of dynamic equilibrium in chemical reactions. Students will be able to predict the direction of equilibrium as a function of changes in temperature, concentration and pressure.
- Calculate equilibrium concentrations of products and reactants in different types of chemical reactions including acid-base equilibria, slightly soluble compounds, and complex formation.
- Classify acids and bases according to the Arrhenius, Bronsted –Lowry, and Lewis definitions.
- Calculate the concentration of electrolyte and nonelectrolyte solutions using different units. Students will be able to determine the effect of concentration on the physical properties of solutions (vapor pressure, melting point, freezing point, and osmotic pressure).
- Apply the basic laws of thermodynamics to determine if a chemical reaction is spontaneous. Students will use thermodynamic values such as Gibbs free energy, enthalpy of formation, and standard entropy to quantitatively determine if a reaction is spontaneous.
- Identify intermolecular forces present in samples of different substances based on their structure. Students will be able to determine the roles these forces play in determining properties such as solubility, viscosity, surface tension, and vapor pressure
- Interpret phase diagrams for simple compounds and calculate the energy involved in phase changes.
- Identify different types of solids and perform basic cubic crystal structure calculations.
- Use acid-base titration data to calculate the pH of a solution at different stages of a titration. Students will identify buffers based on the composition of a solution and will be able to calculate their corresponding pH.
- Define the principles of electrochemistry. Students will be able to distinguish between voltaic and electrolytic cells, calculate cell potentials for spontaneous and non-spontaneous electrochemical reactions determine the relationship between the amount of charge and amount of products formed in electrolytic cells.
- Describe the connection between Gibbs free energy (∆G°), standard cell potential (E°cell), and the equilibrium constant of a reaction (Keq).
- Balance redox equations in acidic and basic media.
- Define the basic concepts of nuclear reactions. Students will be able to identify the different modes of nuclear decay, write and balance nuclear reactions, and perform half-life and mass-energy calculations.
- Describe the basic properties of transition metal complexes and use crystal field theory to predict color in these complexes.
V. Topical Outline (Course Content)
VI. Delivery Methodologies