- A list of various chemical species arranged in order of reactivity. It is usually used to describe the ability of various metals to displace hydrogen from water or from acids.
- In an electrochemical cell, the electrode at which the oxidation half-reaction occurs.
- The description of a modified metal surface through reaction with another chemical component, forcing the metal surface to undergo oxidation (i.e., act as an anode).
- In an electrochemical cell, the electrode at which the reduction half-reaction occurs.
Coordinate covalent bond
- A covalent bond between two atoms, where one of the atoms provides both electrons that form the bond. This usually takes place between a ligand and a metal cation.
- An electrochemical cell in which the redox process is forced to run in the nonspontaneous direction.
- The other term for the voltage associated with an electrochemical reaction.
- An electrochemical cell in which the redox process involved occurs spontaneously.
- A chemical reaction balanced with electrons to show only the reduction half or the oxidation half of an electrochemical reaction.
- An ion or molecule that binds through a coordinate covalent bond to a central metal atom to form a coordination complex.
- Loss of electrons by one species over the course of a chemical reaction.
- The natural oxidation of a metal surface by exposure to other chemical species, so that it is prevented from further oxidation.
- Also referred to as "voltage," the work done by (or required by) a redox process to transfer electrons.
- The shorthand term for a "reduction-oxidation" reaction.
- A reaction in which an atom, molecule, or ion gains electrons. Reduction is always accompanied by a separate oxidation process, a reaction in which another reactant loses the electrons.
Standard reduction potential
- For a reduction half-reaction, a value for the electromotive force or voltage generated when that half-reaction is paired with a standard electrode.
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