Editing Electrochemistry (section)

== <span style="color: #FFFFFF;">Remembering</span> ==
* '''Electrochemistry''' — The study of chemical reactions which take place at the interface of an electrode and an electrolyte.
* '''Oxidation''' — The loss of electrons by an atom or molecule.
* '''Reduction''' — The gain of electrons by an atom or molecule ("Reduction is Gain").
* '''Redox Reaction''' — A chemical reaction involving the transfer of electrons between two species.
* '''Electrode''' — A conductor through which electricity enters or leaves an electrolyte.
* '''Anode''' — The electrode where oxidation occurs (Negative in a battery).
* '''Cathode''' — The electrode where reduction occurs (Positive in a battery).
* '''Electrolyte''' — A substance that produces an electrically conducting solution when dissolved in a polar solvent.
* '''Galvanic (Voltaic) Cell''' — An electrochemical cell that derives electrical energy from spontaneous redox reactions.
* '''Electrolytic Cell''' — An electrochemical cell that uses electrical energy to drive a non-spontaneous redox reaction.
* '''Salt Bridge''' — A tube containing an electrolyte that connects the two half-cells of a galvanic cell, maintaining electrical neutrality.
* '''Electromotive Force (EMF)''' — The maximum potential difference between the electrodes of a cell.
* '''Standard Reduction Potential''' — A measure of the tendency of a chemical species to be reduced.
* '''Corrosion''' — The gradual destruction of materials (usually metals) by chemical reaction with their environment (e.g., Rusting).
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