Redox

A chemical process in which electrons are transferred between substances, oxidizing one as another is reduced. Oxidation and reduction always occur together.

Oxidation state: A bookkeeping value assigned to an atom to track electron ownership in compounds and ions. Changes in oxidation state identify which atoms lose or gain electrons.
Electron: A negatively charged subatomic particle found in atoms and responsible for chemical bonding and electrical current. Electron transfer is the defining event in redox chemistry.
Galvanic cell: An electrochemical cell that produces electrical energy from a spontaneous redox reaction. It channels spontaneous electron transfer into usable electric current.
Acid–base reaction: A chemical reaction involving proton transfer between an acid and a base. Unlike redox, a proton transfer need not change oxidation states.
Oxidation: A process in which a substance loses electrons or increases its oxidation state. This is the electron-loss half of every redox process.
Ion: An atom or molecule with a net electric charge because it has gained or lost electrons. Electron exchange often changes the charge of participating species.
Electrolysis: The use of electrical energy to drive a nonspontaneous chemical reaction. External current forces redox changes that would not proceed spontaneously.
Precipitation reaction: A reaction in which dissolved species form an insoluble solid product. Precipitation can occur through ion exchange without electron transfer.
Reduction: A process in which a substance gains electrons or decreases its oxidation state. This is the electron-gain half paired with oxidation.
Chemical bond: An attraction that holds atoms or ions together through interactions involving their electrons. Redox can reorganize bonding as electrons shift between substances.

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