| A | B |
|---|
| combustion | a chemical change in which oxygen reacts with another substance often producing energy in the form of heat and light |
| oxidation | complete or partial loss of electrons or gain of oxygen |
| oxidizing agent | a substance that accepts electrons in a redox reaction |
| corrosion | oxidation of metals to metallic ions by oxygen and water in the environment |
| zinc | a metal that loses electrons easily |
| gold | a metal that resists corrosion |
| half-reaction method | balancing a redox equation by first balancing the oxidation and reduction half-reactions |
| spectator ions | ions that are present but do not participate in or change during the reaction |
| anions | ions that can serve as reducing agents |
| oxidation half-reaction | Fe2+ Fe3+ + e- |
| half-reaction | equation showing either the reduction or the oxidation of a species in an oxidation-reduction reaction |
| oxidation-number change method | balancing a redox equation by comparing the increase and decrease in oxidation numbers |
| reduction half-reaction | 2e- + Br2 2Br- |
| half-reaction | a reaction that involves the transfer of electrons between reactants during a chemical change |
| half-reaction method | a method for balancing a redox equation by balancing the oxidation and reduction half-reactions |
| oxidation | a process that involves complete or partial loss of electrons or a gain of oxygen; it results in an increase in the oxidation number of an atom |
| oxidation number | a positive or negative number assigned to a combined atom according to a set of arbitrary rules |
| oxidation-number-change method | a method of balancing a redox equation by comparing the increases and decreases in oxidation numbers |
| oxidation-reduction reaction | an equation showing either the reduction or the oxidation of a species in an oxidation-reduction reaction |
| oxidizing agent | substance in a redox reaction that accepts electrons |
| redox reaction | another name for an oxidation-reduction reaction |
| reducing agent | a substance in a redox reaction that donates electrons |
| reduction | a process that involves a complete or partial gain of electrons or the loss of oxygen; it results in a decrease in the oxidation number of an atom |
| dry cell | a commercial voltaic cell in which the electrolyte is a moist paste |
| voltaic cells | electrochemical cells used to convert chemical energy into electrical energy |
| cathode | the electrode at which reduction occurs |
| battery | a group of voltaic cells that are connected together |
| fuel cell | a voltaic cell in which a fuel substance undergoes oxidation to continuously produce electrical energy |
| electrochemical cell | any device that converts chemical energy into electrical energy or electrical energy into chemical energy |
| anode | the electrode at which oxidation occurs |
| electrical potential | the measure of a cell's ability to produce an electric current |
| reduction potential | the tendency of a given half-reaction to occur as a reduction |
| spontaneous reaction | a reaction having a positive cell potential |
| 0.00 V | the standard reduction potential of the hydrogen electrode |
| cell potential | the difference between the reduction potentials of the two half-cells |
| E oxid | standard reduction potential for the oxidation half-cell |
| electrolysis | the process in which electrical energy is used to make a nonspontaneous reaction go forward |
| electrolytic cell | an electrochemical cell used to cause a chemical change through the application of electrical energy |
| brine | a concentrated solution of sodium chloride |
| electroplating | the deposition of a thin layer of metal on an object in an electrolytic cell |
| electro refining | an electrolytic method for obtaining ultrapure metals |
