Chapter 19 & 20

1. A species that undergoes a decrease in oxidation state.
4. A substance that has the potential to cause another substance to be reduced.
5. Processes in which the oxidation state of an element decreases are reduction processes.
6. A process in which a substance acts as both an oxidizing agent and a reducing agent.
10. A single electrode immersed in a solution of its ions
11. Use spontaneous oxidation-reduction reactions to convert chemical energy into electrical energy. Voltaic cells are also called galvanic cells.
12. A conductor used to establish electrical contact with a nonmetallic part of a circuit, such as an electrolyte.
13. The electrode where reduction occurs.
16. Processes in which the atoms or ions of an element experience an increase in oxidation state.
19. The process of passing a current through a cell for which the cell potential is negative and causing an oxidation-reduction reaction to occur.
20. The part of the reaction involving oxidation or reduction alone.
21. This tendency for the half-reaction of either copper or zinc to occur
22. The electrode where oxidation occurs.

2. The branch of chemistry that deals with electricity-related applications of oxidation-reduction reactions.
3. The potential of a half-cell under standard conditions measured relative to the standard hydrogen electrode.
7. If electrical energy is required to produce a redox reaction and bring about a chemical change in an electrochemical cell.
8. The difference in potential between an electrode and its solution.
9. Any chemical process in which elements undergo changes in oxidation number.
14. a reduction half-reaction in an electrochemical cell.
15. A substance that has the potential to cause another substance to be oxidized.
17. A species whose oxidation number increases.
18. An electrolytic process in which a metal ion is reduced and solid metal is deposited on a surface.