The electrochemical series ranks substances according to their oxidizing and reducing power, i.e., their standard electrode potential. Not all oxidizers and reducers are created equal.
Reaction mechanisms in organometallic chemistry ( oxidative addition, reductive elimination) involve changes in the oxidation states of metals.Electrochemistry provides a way to measure equilibrium constants for dissolution/precipitation, complexation, and other reactions.Energy conversion and storage technologies (solar water splitting, batteries, electrolyzers, fuel cells) rely on inorganic redox reactions and catalysis.
Many inorganic compounds catalyze redox reactions (which are especially useful in industrial and biological applications).Main group elements (N, halogens, O, S.) also have multiple oxidation states and important redox chemistry.Transition metals can have multiple oxidation states.Oxidation-reduction reactions are important to understanding inorganic chemistry for several reasons: the formation of rust on iron) is a redox reaction involving oxidation of a metal. In a car engine, hydrocarbons in the fuel are oxidized to carbon dioxide and water, while oxygen is reduced to water. Another example of redox is fire or combustion, such as in a car engine. For example, the metabolism of sugars to CO 2, which stores energy in the form of ATP, is a redox reaction. In terms of everyday life, redox reactions occur all of the time around us. In redox reactions, one element or compound is reduced (gains electrons) and another is oxidized (loses electrons). These four oxidation states form the basis of the vanadium flow battery, a storage device for electricity generated from sunlight and wind. From left to right the oxidation state goes from +5 to +2. Oxidation states of vanadium in acidic solution.
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