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Also known as: electrochemical cell
Written and fact-checked by
The Editors of Encyclopaedia Britannica
Article History
- Key People:
- Johann Wilhelm Ritter
- Auguste-Arthur de La Rive
- Related Topics:
- battery
- fuel cell
- lithium cell
- storage battery
- dry cell
See all related content →
electrolytic cell, any device in which electrical energy is converted to chemical energy, or vice versa. Such a cell typically consists of two metallic or electronic conductors (electrodes) held apart from each other and in contact with an electrolyte (q.v.), usually a dissolved or fused ionic compound. Connection of the electrodes to a source of direct electric current renders one of them negatively charged and the other positively charged. Positive ions in the electrolyte migrate to the negative electrode (cathode) and there combine with one or more electrons, losing part or all of their charge and becoming new ions having lower charge or neutral atoms or molecules; at the same time, negative ions migrate to the positive electrode (anode) and transfer one or more electrons to it, also becoming new ions or neutral particles. The overall effect of the two processes is the transfer of electrons from the negative ions to the positive ions, a chemical reaction (see oxidation-reduction reaction). An example is the electrolysis of sodium chloride (common salt), forming sodium metal and chlorine gas; the energy required to make the reaction proceed is supplied by the electric current. Other common applications of electrolysis include electrodeposition for refining or plating of metals and the production of caustic soda.
In the case of substances that generate energy, rather than consume it, when they react with each other, some or all of this energy can be converted to electricity if the reaction can be divided into an oxidation and a reduction that can be made to occur at separate electrodes. In the lead-acid storage battery, for example, lead dioxide, lead metal, and sulfuric acid react to form lead sulfate and water; the separate processes are the oxidation of lead to lead sulfate at one electrode and the reduction of lead dioxide to lead sulfate at the other while electric charge is transported through the electrolyte by the migration of hydrogen ions. These processes create a driving force (a voltage or electrical potential) that causes electricity to flow through an external circuit joining the two electrodes. Many other chemical combinations have been utilized in cells and batteries.
Other cells for generating electricity by means other than motion of a conductor in a magnetic field include solar cells, in which electron flow between semiconductors results from absorption of light, and fuel cells, in which a continuous supply of liquid or gaseous oxidizing agent, such as oxygen, removes electrons from the cathode as a reducing agent, such as hydrogen, supplies electrons to the anode.
