Chapter 20 - Learning Goals

1. Identify the oxidant and the reductant in an oxidation reduction reaction.

2. Balance oxidation-reduction reactions by the method of half-reactions.

3. Diagram voltaic and electrolytic cells; label the anode, the cathode, and the direction of ion and electron movement.

4. Given appropriate electrode potentials calculate the voltage generated by a voltaic cell.

5. Use electrode potentials to predict whether a reaction will be spontaneous.

6. Interconvert E, G, and K for reactions.

7. Use the Nernst equation to calculate a cell potential under nonstandard conditions.

8. Use the Nernst equation to calculate the concentration of an ion, given E, E, and the concentrations of the remaining ions.

9. Describe the lead storage battery, the dry cell, and the nickel-cadmium cell.

10. Given appropriate electrode potentials calculate the minimum potential required to cause electrolysis.

11. Interrelate time, current, and the amount of substance produced or consumed in an electrolysis reaction; given two of the quantities you should be able to calculate the third.

12. Describe corrosion in terms of the electrochemistry involved, and explain the principles that underlie cathodic protection.