Jan 26, 2022  
2021-2022 Course Catalog 
2021-2022 Course Catalog
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CHM 175 - General/ Inorg Chemistry II

Credits: 4
Lecture Hours: 3
Lab Hours: 3
Practicum Hours: 0
Work Experience: 0
Course Type: Core
A continuation of General and Inorganic Chemistry I.
Prerequisite: CHM 165  or equivalent
  1. Explain reaction rates and their relationships to reaction mechanisms.
    1. Define and express reaction rates quantitatively, and identify factors that influence them.
    2. Quantitatively relate experimental data, reaction rates, rate laws and rate parameters.
    3. Model reactions with collision theory and transition state theory.
    4. Relate kinetic outcomes to plausible reaction mechanisms.
  2. Apply basic principles of chemical equilibrium.
    1. Describe a system at equilibrium.
    2. Solve and evaluate 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 equilibruim position.
    5. Using thermodynamic data, calcuate the equilibrium constant.
    6. Use Lewis theory to explain acid-base behavior
    7. Use molarity to solve acid-base stoichiometry problems
    8. Use equivalents to describe acid-base reactions
    9. Solve acid-base stoichiometric problems using normality
  3. Investigate principles related to acid-base chemistry.
    1. Compare acid-base behavior according to three major theories (Arrhenius, bronsted-Lowry, and Lewis).
    2. Identify conuugated acid-base pairs.
    3. Determine relative strengths of acids and bases.
    4. Perform quantitative calculations related to acid-bas equilibria, titrations, buffer systems, and salt solutions.
    5. Determine bond energies from thermodynamic data
    6. Describe the relationship between energy and entropy in predicting the spontaneity of a process
    7. Calculate entropy changes from thermodynamic data
    8. Calculate free energy changes from thermodynamic data
    9. Estimate the temperature range over which a particular process would be spontaneous
    10. Recognize the limitations of thermodynamics in predicting path-dependent information
  4. Apply equilibruim principles to slightly soluble strong electrolytes.
    1. Solve problems involving solubility product constants.
    2. Describe how the nature of reactants can affect reaction rates
    3. Derive rate law expressions for reactions using experimental data
    4. Determine the order of a reaction
    5. Solve problems involving the half-life of a first order reaction
    6. Use collision theory to model chemical reactions
    7. Use transition state theory to model chemical reactions
    8. Explain the relationship of activation energy to reaction rates
    9. Relate rate data to simple reaction mechanisms
    10. Explain how temperature affects reaction rates
    11. Describe the effect of a catalyst on the rate of a reaction
  5. Apply the basic principles of chemical equilibrium
    1. Describe the characteristics of a process at equilibrium
    2. Determine the value of an equilibrium constant in terms of molari­ty
    3. Use the reaction quotient to predict where a reaction is with respect to equilibrium
    4. Solve problems involving equilibrium constants
    5. Evaluate the equilibrium constant for a reaction involving gases in terms of partial pressures
    6. Describe equilibrium shifts caused by various changes in experi­mental conditions
    7. Determine the new position of equilibrium after a shift has oc­curred
    8. Distinguish between homogeneous and heterogeneous equilibria
    9. Solve problems involving heterogeneous equilibria
    10. Calculate equilibrium constants at standard temperature from thermodynamic data
    11. Estimate equilibrium constants at non-standard temperatures using thermodynamic data
  6. Relate equilibrium principles to acid-base chemistry
    1. Review differences between strong and weak electrolytes
    2. Determine the pH of a solution
    3. Calculate ionization constants for weak electrolytes
    4. Determine the percent ionization of a weak electrolyte
    5. Use ionization constants to solve problems
    6. Explain how acid-base indicators work
    7. Illustrate the effect of a common ion on the ionization of a weak electrolyte
    8. Describe the action of a buffer solution
    9. Relate the composition of a buffer solution to the pH of the solu­tion
    10. Select appropriate materials to make a buffer solution with a specif­ic pH.
    11. Predict the change in pH caused by adding an acid or base to the buffer solution
    12. Describe the ionization of polyprotic weak electrolytes using two or more ionization constants
    13. Solve problems involving the ionization of polyprotic weak electro­lytes
  7. Apply equilibrium principles to hydrolysis and acid-base titrations
    1. Recognize ions that will undergo hydrolysis.
    2. Determine ionization constants for ions that hydrolyze
    3. Calculate the pH of solutions of various classes of salts
    4. Determine the percent hydrolysis of various ions
    5. Extend the concept of hydrolysis to ions derived from polyprotic weak electrolytes
    6. Determine the pH at various points in the titration of a strong acid with a strong base
    7. Determine the pH at various points in the titration of a weak acid with a strong base
    8. Determine the pH at various points in the titration of a strong acid with a weak base
    9. Select appropriate indicators for use in a particular titration
  8. Apply equilibrium principles to slightly soluble strong electrolytes
    1. Calculate solubility product constants
    2. Solve problems involving solubility product constants
    3. Determine which of two species will precipitate first in a fractional precipitation
    4. Use ionization constants in conjunction with solubility products to solve problems on simultaneous equilibria
    5. Describe various methods for dissolving slightly soluble strong electrolytes
    6. Use dissociation constants for complex ions to solve problems
    7. Calculate the quantities of materials needed to dissolve slightly soluble strong electrolytes
  9. Relate oxidation-reduction processes to electrochemistry
    1. Review the principles of oxidation-reduction chemistry
    2. Balance redox reactions via the half-reaction method
    3. Apply the equivalent concept to oxidizing or reducing agents
    4. Use normality to solve problems involving redox stoichiometry
    5. Distinguish between electrolytic and galvanic cells
    6. Determine which electrode serves as anode or cathode
    7. Apply Faraday’s Law to electrolytic cells
    8. Explain the operation of a simple galvanic cell
    9. Use standard electrode potentials to determine the potential of a galvanic cell
    10. Diagram electrochemical cells
    11. Use the Nernst equation to calculate the potential of cells under non-standard conditions
    12. Relate the cell potential to the free energy change
    13. Use standard potentials to determine equilibrium constants
  10. Examine various aspects of nuclear chemistry
    1. Review the composition of the nucleus
    2. Relate neutron-proton ratio to nuclear stability
    3. Calculate binding energies for atomic nuclei
    4. Describe various modes of radioactive decay
    5. Predict the type or types of decay that are most likely for certain kinds of nuclei
    6. Use half-life to solve problems involving radioactive decay process­es
    7. Write equations for various radioactive decays
    8. Compare natural radioactivity to artificial transmutation
    9. Distinguish between fission and fusion
  11. Perform various laboratory exercises
    1. Collect experimental data from a variety of procedures
    2. Use laboratory equipment as instructed
    3. Analyze unknowns using semi-micro qualitative analysis
    4. Compare experimental results to those predicted in theory
    5. Handle chemicals safely
    6. Derive conclusions from experimental measurements

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