CHEM-142: Principles of General and Inorganic Chemistry II

School
Science, Technology, Engineering & Math
Department
Chemistry
Academic Level
Undergraduate
Course Subject
Chemistry
Course Number
142
Course Title
Principles of General and Inorganic Chemistry II
Credit Hours
5.00
Instructor Contact Hours Per Semester
107.00 (for 15-week classes)
Student Contact Hours Per Semester
107.00 (for 15-week classes)
Grading Method
A-E
Pre-requisites
CHEM-141 with a grade of C or better. MATH-175 recommended.
Catalog Course Description

Emphasizes properties of liquids and solutions, reaction rates, chemical equilibria, thermodynamics, electrochemistry, acid/base chemistry, nuclear chemistry and descriptive chemistry of the more common elements (as time allows). Three hours of lecture and four hours of laboratory per week.

Goals, Topics, and Objectives

Goal Statement

This course is designed to prepare students for further courses in chemistry or to satisfy the requirement in other fields of science for a two semester sequence in general chemistry. In addition to extending the student’s knowledge of the basic principles of chemistry, the course objective for CHEM 142 is to assist the student in developing critical thinking and problem solving skills.

Core Course Topics
  1. The condensed phases
    • Liquids, solids, intermolecular forces, vapor pressure and other physical properties, phase diagrams
  2. Properties of solutions
    • Solubility, concentration units, colligative properties
  3. Chemical kinetics
    • Rate laws, integrated forms of the rate laws, mechanisms
  4. Chemical equilibria: definitions, LeChatelier’s Principle, equilibrium constants
  5. Acid/Base equilibria: acids, bases, buffers, pH, titrations, hydrolysis of salts
  6. Equilibria involving solids and complexes
    • Precipitate formation, selective precipitation, precipitation from complex ions, dissolving precipitates in favor of complex ions, naming complex ions
  7. Chemical thermodynamics
    • Laws of thermodynamics, heat, work, enthalpy, entropy, free energy, spontaneity, and equilibrium constants
  8. Electrochemistry
    • Voltaic and electrolytic cells, standard reduction potentials, Nernst Equation, Faraday’s laws, relationship to free energy and equilibrium constants
  9. Nuclear chemistry
    • Types of nuclear decay, stability of nuclei, writing nuclear equations, occurrences of natural and man-made radiation in the environment, disposal of nuclear waste and other contemporary issues related to use of radionuclides, kinetics and thermodynamic calculations associated with nuclear systems
  10. Safety and related environmental concerns in the chemistry laboratory
Core Course Learning Objectives (Separated)
  1. Identify the intermolecular forces in the condensed phases of  pure substances
  2. Predict the physical properties of pure substances using intermolecular forces
  3. Solve vapor pressure problems for pure materials
  4. Use cooling/warming curves to calculate heat changes for pure materials
  5. Calculate various concentration units for solutions
  6. Solve problems involving colligative properties of solutions
  7. Describe and explain the factors affecting reaction rates
  8. Determine the rate law for a reaction from experimental data
  9. Solve problems utilizing the integrated form of the rate law
  10. Evaluate a proposed mechanism for a reaction in light of experimental data
  11. Solve chemical equilibria problems in the gas phase and in solution with special emphasis on acid-base chemistry
  12. Describe how to construct buffers by the two common laboratory methods
  13. Solve buffer problems utilizing the Henderson-Hasselbalch equation
  14. Identify, interpret, and construct titration curves from experimental data for the four most encountered systems
  15. Calculate the pH at any point on a titration curve
  16. Solve chemical equilibria problems for systems involving solids and complex ions
  17. Write names and formulas for complex ions
  18. Describe mathematically and verbally the laws of thermodynamics
  19. Solve problems involving thermodynamic quantities
  20. Use Standard Reduction Potentials to differentiate voltaic and electrolytic cells
  21. Apply the Nernst Equation to voltaic cell systems
  22. Apply Faraday’s laws to electrochemical systems
  23. Apply standard thermodynamic and electrochemical data to equilibrium systems
  24. Differentiate the various types of nuclear decays, their interactions with matter and their impact upon the environment
  25. Write nuclear reactions
  26. Solve problems based on nuclear equations
  27. Display professional behavior, courtesy, and attitude in both lecture and laboratory environments
  28. Observe, analyze, and interpret laboratory data, collected from experiments/exercises built on the core course topics,  both qualitatively and quantitatively
  29. Demonstrate proficiency in laboratory techniques used in various experiments
  30. Demonstrate critical thinking skills in identification of unknowns
  31. Practice appropriate safety procedures in the laboratory
  32. Use environmentally sound chemistry laboratory practices
  33. Prepare neatly and accurately written lab reports using calculations, graphs, explanations, and chemical equations

Assessment and Requirements

Assessment of Academic Achievement

Students will be assessed in lecture using exams, assignments/quizzes/homework, and a comprehensive final. Students will be assessed in lab using reports, quizzes, and lab-tests. The overall course grade is determined using the categories and values listed below.

Category Percentage
Lecture Exams 40-50%
Laboratory (reports, quizzes, lab-tests) 25%
Paper or presentation or homework up to 10%
Final Exam (cumulative) 25%

No student will receive a passing grade in CHEM 142 unless that student has earned at least a 55% in the laboratory.

Outcomes

General Education Categories
  • Natural Sciences
Institutional Outcomes
  • Scientific Reasoning
MTA Categories
  • Category 6.1: Natural Sciences
  • Category 6.2: Natural Sciences with Laboratory Experience

Approval Dates

Effective Term
Fall 2019
ILT Approval Date
12/10/2018
AALC Approval Date
12/19/2018
Curriculum Committee Approval Date
01/16/2019