electrolytesis

Electrolysis is a process that uses an electric current to drive an otherwise non-spontaneous chemical reaction. It is a crucial technique in chemistry and industry for separating compounds. The process involves passing an electric current through a substance called an electrolyte, which is typically a molten ionic compound or an aqueous solution containing dissolved ions.

The electrolyte is placed in an electrolytic cell, which contains two electrodes, an anode and a cathode. The electrodes are connected to a direct current power source. At the anode, oxidation occurs, meaning a substance loses electrons. At the cathode, reduction occurs, meaning a substance gains electrons. These electrode reactions are driven by the applied voltage.

The ions in the electrolyte are attracted to the electrodes with opposite charges. Cations, which are positively charged ions, migrate to the negatively charged cathode and gain electrons (reduction). Anions, which are negatively charged ions, migrate to the positively charged anode and lose electrons (oxidation).

Common applications of electrolysis include the production of metals like aluminum, copper, and sodium from their ores. It is also used for electroplating, a process where a thin layer of metal is deposited onto another object to improve its appearance or corrosion resistance. Electrolysis is fundamental to many industrial chemical processes and in the purification of substances.