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Oxidation and Reduction Set 2: Electrochemistry
Terms in this set (9)
Describes controlled ReDox reactions that will either create an electrical current or utilize electricity to liberate ions for specific uses.
Voltaic Cell (Spontaneous Reaction)
Redox reaction set up as 2 half-cells in 2 separate containers connected by a wire and a salt-bridge. The electrons that transfer travel through a wire to produce an electrical current.
Electrolytic Cells (Nonspontaneous Reaction)
use electricity from an external source to produce a desired redox reaction
A process in which electrical energy is used to bring about a chemical change (ie: the electrolysis of water produces hydrogen and oxygen)
When electricity forces the ionization of a metal
A conductor placed in a solution in order to pass electricity through it.
Electrode at which oxidation occurs during a cell's redox reaction. Electrons always flow away from the anode in an electrochemical cell. For a Voltaic/Galvanic Cell, it is Negative, but for the Electrolytic Cell, it is Positive. For more details go to http://chemistry.stackexchange.com/questions/16785/positive-or-negative-anode-cathode-in-electrolytic-galvanic-cell
Electrode at which reduction occurs during a cell's redox reaction. Electrons always flow toward the cathode in an electrochemical cell. For a Voltaic/Galvanic Cell, it is Positive, but for the Electrolytic Cell, it is Negative. For more details go to http://chemistry.stackexchange.com/questions/16785/positive-or-negative-anode-cathode-in-electrolytic-galvanic-cell
A U-tube containing a salt solution; used to bridge the gap between two halves of a voltaic cell.
A pathway to maintain solution neutrality by allowing passage of ions from one side to another
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