| A | B |
|---|
| Anode | in both electrolytic and voltaic cells it is the electrode where oxidation takes place (that is where a species loses an electron) (607); it is negative in voltaic cells, and positive in electrolytic cells |
| Autooxidation | a process in which a substance acts as both an oxidizing agent and a reducing agent (605) |
| Cathode | in both electrolytic cells and voltaic cells it is the electrode where reduction takes place; that is where species gain electrons (their oxidation number is reduced by adding negative electrons) (607) It is positive in voltaic cells, and negative in electrolytic cells |
| Electrochemical Cell | a system of electrodes and electrolytes in which either chemical reactions produce electrical energy or an electric current produces chemical change (607) |
| Electrochemistry | the branch of chemistry that deals with electricity-related applications of oxidation-reduction reactions (606) |
| Electrode | a conductor used to establish electrical contact with a nonmetallic part of a circuit, such as an electrolyte (607) |
| Electrode Potential | the difference in potential between an electrode and its solution (613) |
| Electrolysis | the process in which an electric current is used to produce an oxidation-reduction reaction (610) |
| Electrolytic Cell | an electrochemical cell in which electrical energy is required to produce a redox reaction and FORCE a NON-SPONTANEOUS chemical change (610) |
| Electroplating | an electrolytic process in which a metal ion is reduced and solid metal is deposited on a surface (611) |
| Half-Cell | a single electrode immersed in a solution of its ions (607) |
| Half-Reaction | the part of a reaction involving oxidation or reduction alone (593) |
| Oxidation | a reaction in which the atoms or ions of an element experience an increase in oxidation state (i.e. the oxidation number goes up b/c of the loss of a negatively charged electron) (592); LEO, Lose Electron(s) = Oxidized [LEO] LEO the lion says GER |
| Oxidation-Reduction Reaction | any chemical process in which elements undergo changes in oxidation number (593) |
| Oxidized | having experienced an increase in oxidation number (i.e. a species that lost negative electrons, will now have a higher oxidation number) (592) ); LEO, Lose Electron(s) = Oxidized [LEO] |
| Oxidizing Agent | a substance that has the potential to cause another substance to be oxidized (causing the other substance to lose electron(s) (602) The oxidizing agent is itself reduced when it reacts. |
| Redox Reaction | any chemical process in which elements undergo changes in oxidation number (593) |
| Reduced | having experienced a decrease in oxidation state (593) (a species that has gained negative electron(s) will have a lower oxidation number, or a REDUCED oxidation number. [GER: Gain Electron(s) Reduced: GER] LEO the lion says GER |
| Reducing Agent | a substance that has the potential to cause another substance to be reduced (to gain electrons) (602); Reducing agents themselves are oxidized, but cause the reduction of anothe species, basically they give electrons to someone else) |
| Reduction | a reaction in which the oxidation state of an element decreases (593) [GER: Gain Electron(s) Reduced: GER] LEO the lion says GER |
| Reduction Potential | the measurement of the tendency for a half-reaction to occur as a reduction half-reaction in an electrochemical cell (613) (given in volts) |
| Standard Electrode Potential | a half-cell potential measured relative to a potential of zero for the standard hydrogen electrode (614) |
| Voltaic Cell | an electrochemical cell in which the redox reaction occurs naturally and produces electrical energy (608) |
