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The Pourbaix diagram for vanadium in water, which shows the redox potentials between various vanadium species in different oxidation states [39] Vanadium(V) forms various peroxo complexes, most notably in the active site of the vanadium-containing bromoperoxidase enzymes. The species VO(O 2)(H 2 O) 4 + is stable in acidic solutions.
The Pourbaix diagram for vanadium in water, which shows the redox potentials between various vanadium species in different oxidation states. [10] Vanadium(V) forms various peroxo complexes, most notably in the active site of the vanadium-containing bromoperoxidase enzymes. The species VO(O) 2 (H 2 O) 4 + is stable in acidic
Vanadium forms oxides in the +2, +3, +4 and +5 oxidation states, forming vanadium(II) oxide (VO), vanadium(III) oxide (V 2 O 3), vanadium(IV) oxide (VO 2) and vanadium(V) oxide (V 2 O 5). Vanadium(V) oxide or vanadium pentoxide is the most common, being precursor to most alloys and compounds of vanadium, and is also a widely used industrial ...
The oxidation numbers of the most stable chemical compounds follow trends in the periodic table. [5]: ... such as vanadium with oxidation states +2, +3, +4, and +5.
The oxidation states are also maintained in articles of the elements (of course), and systematically in the table {{Infobox element/symbol-to-oxidation-state}} See also [ edit ]
Vanadium(V) oxide (vanadia) is the inorganic compound with the formula V 2 O 5. Commonly known as vanadium pentoxide, it is a dark yellow solid, although when freshly precipitated from aqueous solution, its colour is deep orange. Because of its high oxidation state, it is both an amphoteric oxide and an oxidizing agent.
In chemistry, a vanadate is an anionic coordination complex of vanadium. Often vanadate refers to oxoanions of vanadium, most of which exist in its highest oxidation state of +5. The complexes [V(CN) 6] 3− and [V 2 Cl 9] 3− are referred to as hexacyanovanadate(III) and nonachlorodivanadate(III), respectively.
Oxidation states are unitless and are also scaled in positive and negative integers. Most often, the Frost diagram displays oxidation state in increasing order, but in some cases it is displayed in decreasing order. The neutral species of the pure element with a free energy of zero (nE° = 0) also has an oxidation state equal to zero. [2]