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SYLLABUS

Catalog Description

Part II of the general study of atomic systems including: kinetics, catalysis, acid-base systems, thermodynamics, electrochemistry, nuclear chemistry, reaction optimization, industrial processes, and coordination chemistry. For engineering and pre-professional majors. Prerequisite: MATH 185 or equivalent, CHEM 111 or equivalent. Semester Offered-Fall and Spring.

General Objectives: Upon completion of the course, the student should have a working knowledge of the following:
 

1. Solutions
2. Kinetics
3. Equilibrium principles
4. Acid-base systems
5. Thermodynamics
6. Electrochemistry
7. Nuclear Chemistry
8. Chemical process industries
9. Coordination compounds
10. Ultraviolet/visible spectroscopy
11. Qualitative analysis

Specific Objectives: Upon completion of the course the student should be able to:
 

• 1.1 Identify important factors in the solution process.
• 1.2 Express concentrations in mass percent, parts per million, mole fraction, molarity, and molality.
• 1.3 Predict the effect of pressure and temperature on solubility.
• 1.4 Use Rault's law in vapor pressure lowering and distillation problems.
• 1.5 Use boiling point elevation and freezing point depression to determine molar mass.
• 1.6 Calculate osmotic pressure.
• 2.1 Determine rate laws using the method of initial rates.
• 2.2 Determine first order rate laws from data.
• 2.3 Relate rate laws to reaction mechanisms.
• 2.4 Draw reaction pathway diagrams illustrating catalysis pathways and activation energy.
• 2.5 Use the Arrhenius equation to calculate rate constants at different temperatures.
• 3.1 Calculate equilibrium constants and equilibrium concentrations.
• 3.2 Predict effects on equilibrium using LeChatelier's Principle.
• 4.1 Calculate the pH, pOH, [H+], [OH-], and dissociation constants for acid-base, salt, and buffer solutions.
• 4.2 Calculate concentrations, solubilities, and solubility product constants for slightly soluble compounds.
• 4.3 Calculate concentrations, solubilities, and formation constants for complex ions.
• 5.1 Relate the first, second, and third laws of thermodynamics to spontaneous processes.
• 5.2 Calculate and interpret enthalpy, entropy, and free energy changes for chemical systems.
• 5.3 Calculate equilibrium constants from thermodynamic data.
• 6.1 Balance oxidation-reduction reactions.
• 6.2 Draw and explain processes in galvanic, voltaic, and electrolytic cells.
• 6.3 Calculate cell emf, concentrations, equilibrium constants, enthalpy, and entropy using electrochemical methods.
• 6.4 Calculate stoichiometric quantities in electrolytic processes.
• 7.1 Describe and predict radioactive processes using nuclear equations.
• 7.2 Use first order kinetics in radiocarbon dating and other decay processes.
• 7.3 Calculate the mass defect, and binding energy, of nuclei.
• 7.4 Describe nuclear fission and fusion processes and calculate the associated energy changes.
• 8.1 Describe the production of important nonmetals and nonmetal compounds.
• 8.2 Describe the production of important metals.
• 8.3 Describe the production of sulfuric and nitric acids.
• 8.3 Use the Haber process along with thermodynamic and kinetic considerations to optimize typical chemical production.
• 8.4 Describe band theory in terms of orbital overlap and how this effects electrical conduction.
• 8.5 Describe atomic positions of interstitial and substitutional alloys.
• 9.1 Identify the components and structure of complexes.
• 9.2 Use crystal field theory to determine electronic, optical, and magnetic properties of octahedral complexes.
• 10.1 Describe the componenets and purpose of a uv-vis spectrophotometer.
• 10.2 Perform quantitative analysis using colorimetry and Beer's law.
• 11.1 Develop and use a qualitative analysis scheme to separate and Identify a mixture of cations and anions.