Iron(III)

Iron(III) is iron in the +3 oxidation state, commonly represented as Fe³⁺ in ionic compounds. Its compounds include oxides, salts, and coordination complexes.

Iron(III) ion: The Fe³⁺ cation is an iron atom that has lost three electrons. This is the ionic form most directly meant by iron in the +3 oxidation state.
Oxidation state: A formal charge assigned to an atom by treating its bonds as ionic. The +3 designation records iron's electron accounting in a compound.
Iron(III) oxide: The iron oxide Fe₂O₃, found in minerals and used as a red-brown pigment. It is a familiar solid compound in which iron has the +3 oxidation state.
Iron(II) oxide: The compound FeO, a black solid containing iron predominantly in the +2 oxidation state. It contrasts with Fe₂O₃ in iron valence, stoichiometry, and typical color.
Iron(II): Iron(II) is iron in the +2 oxidation state, commonly represented as Fe²⁺. The one-electron reduction from Fe³⁺ produces this neighboring oxidation state.
Coordination complex: A structure in which a central metal atom or ion binds surrounding molecules or ions. Iron(III) commonly occurs inside complexes rather than as an isolated ion.
Iron(III) chloride: The compound FeCl₃, a Lewis acid used in chemical synthesis and metal etching. Its reactions illustrate the strong Lewis acidity of many iron(III) compounds.
Iron(II) sulfate: A family of sulfate salts containing Fe²⁺, commonly encountered as hydrated crystals. Its ferrous ion is more readily oxidized than iron(III) in many aqueous settings.
Redox reaction: A chemical reaction involving transfer of electrons and changes in oxidation states. Iron(III) compounds gain or lose electrons through redox reactions.
Hydrolysis: A reaction in which a substance reacts with water, often changing its bonds or ionization. Water molecules bound to Fe³⁺ can release protons, making solutions acidic.

Linked from 9 pages