Course Snapshot for CHE 112 - General College Chemistry II with Lab: GT-SC1
The information listed below is subject to change. Please review the course syllabus within your online course at the start of class.
Course Competencies
The competencies you will demonstrate in this course are as follows:
- Solutions
- Calculations involving measures of concentration: molarity, molality, mass percent and mole fraction b
- Calculation using colligative properties: freezing point depression, boiling point elevation, vapor pressure depression and osmotic pressure
- Use of colligative properties to find the molar mass of an unknown
- Chemical kinetics
- Reaction rates
- Factors affecting reaction rate
- Rate law: rate equation
- Zero order
- First order
- Second order
- Half-lives
- Reaction rate and temperature
- Arrhenius equation
- Reaction rates and reaction mechanisms
- Deducing reaction mechanisms from rate Laws
- Catalysis
- Chemical equilibrium
- Reverse reactions
- Equilibrium constant, Kc
- Equilibrium constant, Kp
- Calculations involving chemical equilibrium in gaseous, aqueous, and heterogeneous phases
- Applications of equilibrium constants
- Le Chatelier's Principle
- Chemical equilibrium and chemical kinetics
- Aqueous equilibria: acids and bases
- Acid-base concepts: Bronsted-Lowry theory and Lewis acid/base theory
- Acid and base strength
- Ionization of water
- pH scale and measurement of pH
- Equilibria in solutions of weak acids and bases
- Calculating equilibrium concentrations in solutions of weak acids and bases
- Relationship between Ka and Kb
- Acid/base properties of salts
- Common ion effect and buffer solutions
- pH titration curves
- Strong acid-strong base
- Weak acid-strong base
- Weak base-strong acid
- Solubility equilibria
- Solubility
- Solubility product constant, Ksp
- Calculations involving Ksp
- Factors affecting solubility
- Precipitation and separation of ions
- Thermodynamics
- Terminology
- Laws of thermodynamics
- Calculation of entropy changes
- Calculation of free energy changes
- Free energy under standard and non-standard conditions
- Free energy and chemical equilibrium
- Electrochemistry
- Terminology
- Balancing redox reactions using half-reaction method under acidic and basic conditions
- Electrolysis
- Electrolytic and voltaic cells
- Cell potentials and electrode potentials
- Effect of concentration on cell potentials: The Nernst equation
- Standard cell potentials and equilibrium constants
- Applications of electrochemistry
- Nuclear chemistry (Recommended Topic)
- Nuclear reactions and radioactivity
- Types of radioactive decay
- Rate of radioactive decay and half-life
- Nuclear stability
- Energy change in nuclear reactions
- Fission and Fusion
- Detecting and measuring radioactivity
- Biological effects of radiation
- Applications of nuclear radiation
Module Outcomes Mapped to Competencies
Module 1
|
Outcomes |
Competencies |
1 |
Describe the process of solution formation and the factors influencing solubility. |
Ia, Ib |
2 |
Compare the different terms that describe solubility. |
Ia, Ib |
3 |
Practice solving molarity problems as they apply to chemical experiments. |
Ia, Ib, Ic |
4 |
Calculate and convert molality. |
Ib, Ic |
5 |
Describe what the colligative properties are and calculate results. |
Ib, Ic |
6 |
Define chemical reaction rate. |
IIa |
7 |
Describe the effects of chemical nature, physical state, temperature, concentration, and catalysis on reaction rates. |
IIb |
8 |
Use rate and concentration data to identify reaction orders and derive rate laws. |
IIci - iii |
9 |
Explain the form and function of an integrated rate law. |
IIciv |
10 |
Use the Arrhenius equation in calculations relating rate constants to temperature. |
IId |
11 |
Derive the rate law consistent with a given reaction mechanism. |
IIe - f |
12 |
Explain the function of a catalyst in terms of reaction mechanisms and potential energy diagrams. |
IIf |
13 |
Perform hands-on chemistry experiments that demonstrate theoretical concepts. |
Ia - c, IIa - c, g |
Module 2
|
Outcomes |
Competencies |
1 |
Explain chemical equilibria and reversible reactions. |
IIIa |
2 |
Define the equilibrium constant in terms of solutions, gases and solids. |
IIIa - c |
3 |
Calculate the equilibrium constant from empirical data. |
Ia, IIId |
4 |
Relate equilibrium to real world situations. |
IIIa, b, e |
5 |
Define LeChatelier's Principle. |
IIIf |
6 |
Predict outcomes using LeChatelier's Principle. |
IIId, f |
7 |
Write chemical equations and equilibrium expressions representing solubility equilibria. |
Va - b |
8 |
Carry out equilibrium computations involving solubility, equilibrium expressions, and solute concentrations. |
Ia, Va - c |
9 |
Describe examples of systems involving two (or more) simultaneous chemical equilibria. |
Vd - e |
10 |
Perform hands-on chemistry activities and labs with observations of demonstrations and simulations playing a secondary role. |
I, II, III, IV, V, VII |
Module 3
|
Outcomes |
Competencies |
1 |
Recognize and name acids and bases, including common weak and strong acids and bases. |
IVa |
2 |
Identify the chemical species that are involved in acid base chemistry. |
IVa, IVc |
3 |
Determine the relative strength of acids and bases. |
IVb - Ivd |
4 |
Calculate pH of weak acids and bases in solution. |
IVc - IVg |
5 |
Evaluate pH titration curves. |
IVc |
6 |
Investigate the effects of pH on environmental and industrial applications. |
Ivd, IVe, IVf, IVj |
7 |
Define buffers and calculate their pH. |
IVh - IVi |
8 |
Investigate experimental techniques for measuring pH and evaluating buffers. |
IVb, Ivd, IVi, IVj |
9 |
Perform hands-on chemistry experiments that demonstrate theoretical concepts. |
Ia - c, IIa - c, g |
Module 4
|
Outcomes |
Competencies |
1 |
Distinguish between spontaneous and nonspontaneous processes. |
VIa |
2 |
Define entropy. |
VIa |
3 |
State and explain the second and third laws of thermodynamics. |
VIa, VIb |
4 |
Define Gibbs free energy, and describe its relation to spontaneity. |
VIa, VIb |
5 |
Calculate free energy change for a process using free energies of formation for its reactants and products. |
VIc, VId |
6 |
Calculate entropy changes for phase transitions and chemical reactions under standard conditions and non-standard conditions. |
Ia, VIc - VIe |
7 |
Define electrochemistry and a number of important associated terms. |
VIIa |
8 |
Produce balanced oxidation-reduction equations for reactions in acidic or basic solution. |
VIIb |
9 |
Describe the basic components of galvanic cells. |
VIIbii, VIIbvi |
10 |
Determine standard cell potentials for oxidation-reduction reactions. |
VIIbiii |
11 |
Use the Nernst equation to determine cell potentials at nonstandard conditions. |
Ia, VIIbiv |
12 |
Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants. |
VIIbv |
13 |
List some of the characteristics and limitations of batteries and provide a general description of a fuel cell. |
VIIa, VIIbii, VIIbvi |
14 |
Describe electrolytic cells and their relationship to galvanic cells and perform various calculations related to electrolysis. |
VIIa, VIIbii, VIIbvi |
15 |
Perform hands-on chemistry experiments that demonstrate theoretical concepts. |
Ia - c, IIa - c, g |
Module 5
|
Outcomes |
Competencies |
1 |
Recognize and balance nuclear reactions. |
VIIIa - b |
2 |
Explain the interaction of radiation with matter, and the potential health effects of exposure to it. |
VIIIe - f |
3 |
Apply the principles of kinetics to nuclear reactions. |
VIIIc |
4 |
Calculate the energy change associated with nuclear reactions |
VIIIa |
5 |
Understand why certain elements are unstable and radioactive. |
VIIIa, e |
6 |
Perform hands-on chemistry experiments that demonstrate theoretical concepts. |
Ia - c, IIa - c, g |
Course Time Commitment and Expectations
The semester schedule for this course may be 15 weeks or 10 weeks in duration. Based on the course format, this table shows the approximate amount of time you should plan to spend per week on this course. This includes time to read/listen to the online content, participate in discussion forums, complete all assignments, and study the course material.
For accelerated courses, the amount of time required per week is greater. Note that regardless of course format, the course material is the same and all course competencies, module outcomes, and assignments will be covered.
Course Activity Hours and Student Learning Hours
Course Credit Hours |
Course Format (Duration) |
Pace Relative to a 15 Week Course |
Course Activity Hours |
Student Learning Hours Per Week |
5 |
15 Weeks |
- |
225 |
14.5 to 15.5 |
5 |
10 Weeks |
1.5x faster |
225 |
21.5 to 23.5 |
Aside from typical reading assignments, this course has the following (Please Note: This list is subject to change based on the discretion of the instructor facilitating this course.):
Summary of Grading
Assignment |
Points |
% |
Discussions (10 @ 20 points each) |
200 |
20% |
Module Exams (3 @ 35 points each) |
105 |
10.5% |
Labs (14 @ 20 points each) |
280 |
28% |
Projects (5 @ 30 points each) |
150 |
15% |
Midterm Exam |
100 |
10% |
Final Exam |
150 |
15% |
Safety Quiz |
15 |
1.5% |
TOTAL |
1000 |
100% |
Grading Scale
A = 90 to 100% |
B = 80 to 89% |
C = 70 to 79% |
D = 60 to 69% |
F = 59% and below |
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