Objectives

You have completed this lesson when you can:

1. Determine the oxidation state of any atom in any given substance.

2. Use oxidation states to identify whether a given atom has lost or gained electrons in a reaction.

3. Define and describe oxidation-reduction reactions, recognize examples, and explain why oxidation and reduction must occur at the same time.

4. Correctly use the terms "oxidant," "reductant," "oxidized," and "reduced" to describe the transfer of electrons.

5. Describe what happens when an electric current is passed through a metal, an aqueous solution, or a molten salt.

6. Describe the process of electrolysis. Identify the cathode and anode in an electrolytic process. Write simple equations for the half-reactions occur in an electrolytic process.

7. Describe the processes of electroplating and molten salt electrolysis.

8. Determine which of two chemicals will be more easily oxidized (or reduced), either from trends on the periodic table or from information on an experiment involving the two elements or from a standard oxidation potential (SOP) list.

9. Use a standard oxidation potential (SOP) list to:

• determine which of several substances has the greatest tendency to be oxidized or reduced.

• identify the oxidized and reduced forms of chemicals.

• determine which oxidation-reduction reactions will occur.

• calculate the voltage of a voltaic cell.

10. Describe voltaic cells:

• explain how oxidation-reduction reactions can be used to produce electricity.

• identify anode, cathode, and salt bridge; describe their functions.

• describe the flow of electricity.

• explain what happens to the chemicals involved for a given oxidation-reduction reaction.

11. Describe the principles of cathodic protection of metal substances from corrosion.