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Each student should be able to:
1. All requirements from Redox (Oxidation-reduction section) of 1st year chemistry class, [Objectives of Chemical Reactions and Redox Reaction]
2. Understand the concept of electrical (really chemical energy) potential, ξ , (and its unit of Volts) and how it related to a Half cell reaction (either Reduction or Oxidation).
3. Understand and use the Standard Reduction Potential Table(s) including how it is derived (formation of hydrogen gas as standard or ξ = 0V).
4. Application of Redox Reactions: Chemical Energy to Electrical Energy: (called Electrochemical Cell or Daniel Cell or Voltaic Cell)
- a) Student will be able to determine the correct Half cell to provide the most positive ξ cell include actual voltage (V) and net ionic reaction (including number of electrons moving) and what it means energy wise if it is positive.
- b) Student will be able to draw a picture of the Electrochemical cell include anode location (what Half cell is occurring there), anode electrode material, anode solution cation/anion, the same for the cathode, an arrow indicating direction of electron flow, cell voltage, and salt bridge/semipermeable membrane information.
- c) Student will be able to explain what happens as the cell is used.
- d) Student will be able to give example of different types of Electrochemical cells including batteries, corrosion of metals and fuel cells.
5. Application of Redox Reactions: Electrical Energy to Chemical Energy: (called either Electrolysis or Electroplating)
- a) Student will be able to determine the correct Half cells to produce the most negative ξcell including what it means to have a negative value.
- b) Student will understand that Electrolysis is often use to break compounds up into their elemental parts (i.e. H2O1 (l) to O2 (g) and H2 (g)).
- c) Student will understand that Electroplating causes metal ions to change to their elemental form (via electron addition) and are deposited onto a desired surface.
- d) Student will be use Faraday's constant and equations to either calculate chemical information (i.e. how much mass of a metal will be deposited during a given time and Voltage or visa versa) or electrical information (how time will it take to deposit a give amount of metal mass if given the voltage or visa versa). These calculations also apply to any material that is generated at the cathode and anion of the negative voltage generating Redox reaction.
6. Application of Electrochemistry and Thermodynamics: Nernst Equation (2017-2018 Not on Electrochemistry Test)
- a) Using the concept of ΔG, student will be able to not only explain the significance of the positive and negative sign of the ξcell but also explain what is happening in the cell while it is running (what is happening to the energy) and when it "dies".
- b) Using non standard state ξcell to determine the affect of running a cell for a period of time and/or how long it can run until one achieve a specific solution condition (i.e. using Nernst Equation).