CHM 175 - General Chemistry II

1. Evaluate the molecular basis of colligative properties in chemical solutions.
   1. Use Raoult’s Law to solve for vapor pressure in solutions with volatile and non-volatile solutes.
   2. Determine the freezing and boiling point of various solutions based on concentration.
   3. Model osmotic pressure in solutions mathematically.
   4. Apply the van’t Hoff factor to problems involving colligative properties in chemical solutions.
2. Examine reaction rates and their relationships to reaction mechanisms. 
   1. Express reaction rates quantitatively.
   2. Identify factors that influence reaction rates. 
   3. Quantitatively relate experimental data, reaction rates, rate laws and rate parameters. 
   4. Model reactions with collision theory and transition state theory. 
   5. Relate kinetic outcomes to plausible reaction mechanisms. 
3. Analyze basic principles of chemical equilibrium. 
   1. Describe a system at equilibrium. 
   2. Solve problems involving equilibrium constants. 
   3. Use the reaction quotient to predict if a system is at equilibrium. 
   4. Describe how stresses on a system affect the equilibrium position. 
   5. Using thermodynamic data, calculate the equilibrium constant. 
4. Assess principles related to acid-base chemistry. 
   1. Compare acid-base behavior according to three major theories (Arrhenius, Bronsted-Lowry, and Lewis). 
   2. Identify conjugate acid-base pairs. 
   3. Rank relative strengths of acids and bases. 
   4. Construct quantitative calculations related to acid-base equilibria, titrations, buffer systems, and salt solutions.  
   5. Solve quantitative calculations related to acid-base equilibria, titrations, buffer systems, and salt solutions.  
5. Examine equilibrium principles for slightly soluble strong electrolytes. 
   1. Solve problems involving solubility product constants. 
   2. Describe solubility using solubility product constants. 
   3. Calculate fractional and simultaneous equilibrium problems using solubility product constants. 
   4. Describe methods of dissolving precipitates. 
6. Relate thermodynamics to chemical and physical processes 
   1. Use bond energy values to estimate enthalpy changes for chemical processes. 
   2. Relate chemical or physical changes to entropy changes. 
   3. Calculate entropy and free energy changes from thermodynamic data. 
   4. Use the relationship between enthalpy, entropy, and temperature to determine whether a reaction is spontaneous, non-spontaneous, or at equilibrium. 
   5. Relate the concept of spontaneity to the relative value of an equilibrium constant to determine whether or not a reaction will proceed as written in a chemical equation.  
7. Relate oxidation-reduction processes to electrochemistry. 
   1. Write balanced redox reactions and use half-reactions to represent processes occurring in electrochemical cells. 
   2. Calculate quantities for electrochemical cells under standard and nonstandard conditions. 
   3. Relate cell potentials to concepts of free energy change and equilibrium. 
   4. Calculate quantities for electrolysis reactions.  
8. Examine various aspects of nuclear chemistry.
   1. Review the composition of the nucleus.
   2. Relate neutron-proton ratio to nuclear stability.
   3. Describe various modes of radioactive decay.
   4. Use half-life to solve problems involving radioactive decay.
   5. Write equations for various radioactive decays.
   6. Distinguish between fission and fusion.
   7. Calculate binding energies for atomic nuclei.
9. Perform various laboratory exercises.  
   1. Collect experimental data from a variety of procedures.
   2. Use laboratory equipment as instructed.  
   3. Compare experimental results to those predicted in theory.  
   4. Handle chemicals safely.
   5. Derive conclusions from experimental measurements.