Odtnhj

Vanadium(V) oxide
	;
	;
Names;
	; IUPAC name; Divanadium pentaoxide;
	Other names; Vanadium pentoxide; Vanadic anhydride; Divanadium pentoxide;
Identifiers;
; CAS Number;	; ; 1314-62-1 Y; ;
; 3D model (JSmol);	; Interactive image; ;
; ChEBI;	; ; CHEBI:30045 Y; ;
; ChemSpider;	; ; 14130 Y; ;
; ECHA InfoCard;	; 100.013.855;
; EC Number;	215-239-8;
; KEGG;	; ; C19308 N; ;
; ; PubChem CID; ;	; 14814; ;
; RTECS number;	YW2450000;
; UN number;	2862;
	; ; InChI; ; InChI=1S/5O.2V Y; Key: GNTDGMZSJNCJKK-UHFFFAOYSA-N Y; ; ; ; InChI=1/5O.2V/rO5V2/c1-6(2)5-7(3)4; Key: GNTDGMZSJNCJKK-HHIHJEONAP; ; ; ;
	; ; SMILES; O=[V](=O)O[V](=O)=O; ;
Properties
; Chemical formula;	V2O5
; Molar mass;	181.8800 g/mol ;
Appearance;	Yellow solid;
; Density;	3.357 g/cm3
; Melting point;	690 °C (1,274 °F; 963 K) ;
; Boiling point;	1,750 °C (3,180 °F; 2,020 K) (decomposes);
; Solubility in water;	8.0 g/L (20 °C);
; ; Magnetic susceptibility (χ);	+128.0·10−6 cm3/mol;
Structure
; Crystal structure;	; Orthorhombic;
; Space group;	Pmmn, No. 59;
; Lattice constant;	; ; a = 1151 pm, b = 355.9 pm, c = 437.1 pm;
; Coordination geometry;	Distorted trigonal bipyramidal (V);
Thermochemistry;
; ; Std molar; entropy (So298);	130.54 J/mol·K
; ; Std enthalpy of; formation (ΔfHo298);	-1550.590 kJ/mol
; ; Gibbs free energy (ΔfG˚);	-1419.435 kJ/mol
Hazards;
; Safety data sheet;	; ICSC 0596;
; GHS pictograms;	;
; GHS signal word;	DANGER;
; GHS hazard statements;	; H341, H361, H372, H332, H302, H335, H411;
; NFPA 704;	; ; ; ; ; 0; ; ; 4; ; ; 0; ; ; ;
; Flash point;	Non-flammable ;
	Lethal dose or concentration (LD, LC):;
; ; LD50 (median dose);	10 mg/kg (rat, oral); 23 mg/kg (mouse, oral)
; ; LCLo (lowest published);	500 mg/m3 (cat, 23 min); 70 mg/m3 (rat, 2 hr)
	US health exposure limits (NIOSH):;
; ; PEL (Permissible);	C 0.5 mg V2O5/m3 (resp) (solid) ; ; C 0.1 mg V2O5/m3 (fume);
Related compounds;
; Other anions; ;	; Vanadium oxytrichloride;
; Other cations; ;	; Niobium(V) oxide; Tantalum(V) oxide;
; Related vanadium oxides; ;	; Vanadium(II) oxide; Vanadium(III) oxide; Vanadium(IV) oxide;
	; Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).;
	; N verify (what is YN ?);
	; Infobox references;
;	;

Vanadium(V) oxide (vanadia) is the inorganic compound with the formula V₂O₅. Commonly known as vanadium pentoxide, it is a brown/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. From the industrial perspective, it is the most important compound of vanadium, being the principal precursor to alloys of vanadium and is a widely used industrial catalyst.^[6]

The mineral form of this compound, shcherbinaite, is extremely rare, almost always found among fumaroles. A mineral trihydrate, V₂O₅·3H₂O, is also known under the name of navajoite.

Chemical properties

Reduction to lower oxides

Upon heating a mixture of the pentoxide and V₂O₃, comproportionation occurs to give vanadium(IV) oxide, as a deep-blue solid:^[7]

V₂O₅ + V₂O₃ → 4 VO₂

The reduction can also be effected by oxalic acid, carbon monoxide, and sulfur dioxide. Further reduction using hydrogen or excess CO can lead to complex mixtures of oxides such as V₄O₇ and V₅O₉ before black V₂O₃ is reached.

Acid-base reactions

V₂O₅ it is an amphoteric oxide. Unlike most metal oxides, it dissolves slightly in water to give a pale yellow, acidic solution. Thus V₂O₅ reacts with strong non-reducing acids to form solutions containing the pale yellow salts containing dioxovanadium(V) centers:

V₂O₅ + 2 HNO₃ → 2 VO₂(NO₃) + H₂O

It also reacts with strong alkali to form polyoxovanadates, which have a complex structure that depends on pH.^[8] If excess aqueous sodium hydroxide is used, the product is a colourless salt, sodium orthovanadate, Na₃VO₄. If acid is slowly added to a solution of Na₃VO₄, the colour gradually deepens through orange to red before brown hydrated V₂O₅ precipitates around pH 2. These solutions contain mainly the ions HVO₄²⁻ and V₂O₇⁴⁻ between pH 9 and pH 13, but below pH 9 more exotic species such as V₄O₁₂⁴⁻ and HV₁₀O₂₈⁵⁻ (decavanadate) predominate.

Upon treatment with thionyl chloride, it converts to the volatile liquid vanadium oxychloride, VOCl₃:^[9]

V₂O₅ + 3 SOCl₂ → 2 VOCl₃ + 3 SO₂

Other redox reactions

Hydrochloric acid and hydrobromic acid are oxidised to the corresponding halogen, e.g.,

V₂O₅ + 6HCl + 7H₂O → 2[VO(H₂O)₅]²⁺ + 4Cl⁻ + Cl₂

Vanadates or vanadyl(V) compounds in acid solution are reduced by zinc amalgam through the colourful pathway:

VO₂⁺yellow → VO²⁺blue → V³⁺green → V²⁺purple^[10]

The ions are all hydrated to varying degrees.

Preparation

The orange, partly hydrated form of V₂O₅

Precipitate of "red cake", which is hydrous V₂O₅

Technical grade V₂O₅ is produced as a black powder used for the production of vanadium metal and ferrovanadium.^[8] A vanadium ore or vanadium-rich residue is treated with sodium carbonate and an ammonium salt to produce sodium metavanadate, NaVO₃. This material is then acidified to pH 2–3 using H₂SO₄ to yield a precipitate of "red cake" (see above). The red cake is then melted at 690 °C to produce the crude V₂O₅.

Vanadium(V) oxide is produced when vanadium metal is heated with excess oxygen, but this product is contaminated with other, lower oxides. A more satisfactory laboratory preparation involves the decomposition of ammonium metavanadate at 500-550 °C:^[11]

2 NH₄VO₃ → V₂O₅ + 2 NH₃ + H₂O

Uses

Ferrovanadium production

In terms of quantity, the dominant use for vanadium(V) oxide is in the production of ferrovanadium (see above). The oxide is heated with scrap iron and ferrosilicon, with lime added to form a calcium silicate slag. Aluminium may also be used, producing the iron-vanadium alloy along with alumina as a by-product.^[8]

Sulfuric acid production

Another important use of vanadium(V) oxide is in the manufacture of sulfuric acid, an important industrial chemical with an annual worldwide production of 165 million metric tons in 2001, with an approximate value of US$8 billion. Vanadium(V) oxide serves the crucial purpose of catalysing the mildly exothermic oxidation of sulfur dioxide to sulfur trioxide by air in the contact process:

2 SO₂ + O₂ ⇌ 2 SO₃

The discovery of this simple reaction, for which V₂O₅ is the most effective catalyst, allowed sulfuric acid to become the cheap commodity chemical it is today. The reaction is performed between 400 and 620 °C; below 400 °C the V₂O₅ is inactive as a catalyst, and above 620 °C it begins to break down. Since it is known that V₂O₅ can be reduced to VO₂ by SO₂, one likely catalytic cycle is as follows:

SO₂ + V₂O₅ → SO₃ + 2VO₂

followed by

2VO₂ +½O₂ → V₂O₅

It is also used as catalyst in the selective catalytic reduction (SCR) of NO_x emissions in some power plants. Due to its effectiveness in converting sulfur dioxide into sulfur trioxide, and thereby sulfuric acid, special care must be taken with the operating temperatures and placement of a power plant's SCR unit when firing sulfur-containing fuels.

Other oxidations

Maleic anhydride is produced by the V₂O₅-catalysed oxidation of butane with air:

C₄H₁₀ + 4 O₂ → C₂H₂(CO)₂O + 8 H₂O

Maleic anhydride is used for the production of polyester resins and alkyd resins.^[12]

Phthalic anhydride is produced similarly by V₂O₅-catalysed oxidation of ortho-xylene or naphthalene at 350–400 °C. The equation is for the xylene oxidation:

C₆H₄(CH₃)₂ + 3 O₂ → C₆H₄(CO)₂O + 3 H₂O

Phthalic anhydride is a precursor to plasticisers, used for conferring pliability to polymers.

A variety of other industrial compounds are produced similarly, including adipic acid, acrylic acid, oxalic acid, and anthraquinone.^[6]

Other applications

Due to its high coefficient of thermal resistance, vanadium(V) oxide finds use as a detector material in bolometers and microbolometer arrays for thermal imaging. It also finds application as an ethanol sensor in ppm levels (up to 0.1 ppm).

Vanadium redox batteries are a type of flow battery used for energy storage, including large power facilities such as wind farms.^[13]

Biological activity

Vanadium(V) oxide exhibits very modest acute toxicity to humans, with an LD50 of about 470 mg/kg. The greater hazard is with inhalation of the dust, where the LD50 ranges from 4–11 mg/kg for a 14-day exposure.^[6] Vanadate (VO³⁻
₄), formed by hydrolysis of V₂O₅ at high pH, appears to inhibit enzymes that process phosphate (PO₄³⁻). However the mode of action remains elusive.^[8]

References

^ Weast, Robert C., ed. (1981). CRC Handbook of Chemistry and Physics (62nd ed.). Boca Raton, FL: CRC Press. p. B-162. ISBN 0-8493-0462-8..mw-parser-output cite.citationfont-style:inherit.mw-parser-output qquotes:"""""""'""'".mw-parser-output code.cs1-codecolor:inherit;background:inherit;border:inherit;padding:inherit.mw-parser-output .cs1-lock-free abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-limited a,.mw-parser-output .cs1-lock-registration abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-subscription abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolor:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:help.mw-parser-output .cs1-hidden-errordisplay:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em.

^ Shklover, V.; Haibach, T.; Ried, F.; Nesper, R.; Novak, P. (1996), "Crystal structure of the product of Mg²⁺ insertion into V₂O₅ single crystals", J. Solid State Chem., 123 (2): 317–23, doi:10.1006/jssc.1996.0186.

^ ^a^b^c R. Robie, B. Hemingway, and J. Fisher, “Thermodynamic Properties of Minerals and Related Substances at 298.15K and 1bar Pressure and at Higher Temperatures,” US Geol. Surv., vol. 1452, 1978. [1]

^ ^a^b "NIOSH Pocket Guide to Chemical Hazards #0653". National Institute for Occupational Safety and Health (NIOSH).

^ ^a^b "Vanadium dust". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).

^ ^a^b^c Günter Bauer, Volker Güther, Hans Hess, Andreas Otto, Oskar Roidl, Heinz Roller, Siegfried Sattelberger "Vanadium and Vanadium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a27_367

^ G. Brauer (1963). "Vanadium, Niobium, Tantalum". In G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed. NY: Academic Press. p. 1267.

^ ^a^b^c^d Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 1140, 1144. ISBN 0-08-022057-6..

^ G. Brauer (1963). "Vanadium, Niobium, Tantalum". In G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed. NY: Academic Press. p. 1264.

^ [rsc.org/learn-chemistry/resource/download/res00002003/cmp00006650/pdf RSC instructions for performing the reduction of vanadium(V) to vanadium(II)]

^ G. Brauer (1963). "Vanadium, Niobium, Tantalum". In G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed. NY: Academic Press. p. 1269.

^ Tedder, J. M.; Nechvatal, A.; Tubb, A. H., eds. (1975), Basic Organic Chemistry: Part 5, Industrial Products, Chichester, UK: John Wiley & Sons.

^ REDT Energy Storage. "Using VRFB for Renewable applications".

External links

How Vanadium Oxide Is Used In Energy Storage

International Chemical Safety Card 0596

"NIOSH Pocket Guide to Chemical Hazards #0653". National Institute for Occupational Safety and Health (NIOSH).

"NIOSH Pocket Guide to Chemical Hazards #0654". National Institute for Occupational Safety and Health (NIOSH).

Vanadium Pentoxide and other Inorganic Vanadium Compounds (Concise International Chemical Assessment Document 29)

IPCS Environmental Health Criteria 81: Vanadium

IPCS Health and Safety Guide 042: Vanadium and some vanadium salts

This page is only for reference, If you need detailed information, please check here

[1] Weast, Robert C., ed. (1981). CRC Handbook of Chemistry and Physics (62nd ed.). Boca Raton, FL: CRC Press. p. B-162. ISBN 0-8493-0462-8..mw-parser-output cite.citationfont-style:inherit.mw-parser-output qquotes:"""""""'""'".mw-parser-output code.cs1-codecolor:inherit;background:inherit;border:inherit;padding:inherit.mw-parser-output .cs1-lock-free abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-limited a,.mw-parser-output .cs1-lock-registration abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-subscription abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolor:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:help.mw-parser-output .cs1-hidden-errordisplay:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em.

[2] Shklover, V.; Haibach, T.; Ried, F.; Nesper, R.; Novak, P. (1996), "Crystal structure of the product of Mg²⁺ insertion into V₂O₅ single crystals", J. Solid State Chem., 123 (2): 317–23, doi:10.1006/jssc.1996.0186.

[usgs-3] R. Robie, B. Hemingway, and J. Fisher, “Thermodynamic Properties of Minerals and Related Substances at 298.15K and 1bar Pressure and at Higher Temperatures,” US Geol. Surv., vol. 1452, 1978. [1]

[PGCH|0653-4] "NIOSH Pocket Guide to Chemical Hazards #0653". National Institute for Occupational Safety and Health (NIOSH).

[IDLH-5] "Vanadium dust". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).

[Ullmann-6] Günter Bauer, Volker Güther, Hans Hess, Andreas Otto, Oskar Roidl, Heinz Roller, Siegfried Sattelberger "Vanadium and Vanadium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a27_367

[7] G. Brauer (1963). "Vanadium, Niobium, Tantalum". In G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed. NY: Academic Press. p. 1267.

[G&E-8] Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 1140, 1144. ISBN 0-08-022057-6..

[9] G. Brauer (1963). "Vanadium, Niobium, Tantalum". In G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed. NY: Academic Press. p. 1264.

[10] [rsc.org/learn-chemistry/resource/download/res00002003/cmp00006650/pdf RSC instructions for performing the reduction of vanadium(V) to vanadium(II)]

[11] G. Brauer (1963). "Vanadium, Niobium, Tantalum". In G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed. NY: Academic Press. p. 1269.

[12] Tedder, J. M.; Nechvatal, A.; Tubb, A. H., eds. (1975), Basic Organic Chemistry: Part 5, Industrial Products, Chichester, UK: John Wiley & Sons.

[13] REDT Energy Storage. "Using VRFB for Renewable applications".

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb₂O₄) Cobalt(II,III) oxide (Co₃O₄) Europium(II,III) oxide (Eu₃O₄) Iron(II,III) oxide (Fe₃O₄) Lead(II,IV) oxide (Pb₃O₄) Manganese(II,III) oxide (Mn₃O₄) Silver(I,III) oxide (Ag₂O₂) Triuranium octoxide (U₃O₈) Carbon suboxide (C₃O₂) Mellitic anhydride (C₁₂O₉) Praseodymium(III,IV) oxide (Pr₆O₁₁) Terbium(III,IV) oxide (Tb₄O₇)
+1 oxidation state	Copper(I) oxide (Cu₂O) Dicarbon monoxide (C₂O) Dichlorine monoxide (Cl₂O) Gallium(I) oxide (Ga₂O) Lithium oxide (Li₂O) Potassium oxide (K₂O) Rubidium oxide (Rb₂O) Silver oxide (Ag₂O) Thallium(I) oxide (Tl₂O) Sodium oxide (Na₂O) Water (hydrogen oxide) (H₂O)
+2 oxidation state	Aluminium(II) oxide (AlO) Barium oxide (BaO) Beryllium oxide (BeO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Europium(II) oxide (EuO) Germanium monoxide (GeO)) Iron(II) oxide (FeO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S₂O₂) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Zinc oxide (ZnO)
+3 oxidation state	Aluminium oxide (Al₂O₃) Antimony trioxide (Sb₂O₃) Arsenic trioxide (As₂O₃) Bismuth(III) oxide (Bi₂O₃) Boron trioxide (B₂O₃) Cerium(III) oxide (Ce₂O₃) Dibromine trioxide (Br₂O₃) Chromium(III) oxide (Cr₂O₃) Dinitrogen trioxide (N₂O₃) Dysprosium(III) oxide (Dy₂O₃) Erbium(III) oxide (Er₂O₃) Europium(III) oxide (Eu₂O₃) Gadolinium(III) oxide (Gd₂O₃) Gallium(III) oxide (Ga₂O₃) Holmium(III) oxide (Ho₂O₃) Indium(III) oxide (In₂O₃) Iron(III) oxide (Fe₂O₃) Lanthanum oxide (La₂O₃) Lutetium(III) oxide (Lu₂O₃) Manganese(III) oxide (Mn₂O₃) Neodymium(III) oxide (Nd₂O₃) Nickel(III) oxide (Ni₂O₃) Phosphorus trioxide (P₄O₆) Praseodymium(III) oxide (Pr₂O₃) Promethium(III) oxide (Pm₂O₃) Rhodium(III) oxide (Rh₂O₃) Samarium(III) oxide (Sm₂O₃) Scandium oxide (Sc₂O₃) Terbium(III) oxide (Tb₂O₃) Thallium(III) oxide (Tl₂O₃) Thulium(III) oxide (Tm₂O₃) Titanium(III) oxide (Ti₂O₃) Tungsten(III) oxide (W₂O₃) Vanadium(III) oxide (V₂O₃) Ytterbium(III) oxide (Yb₂O₃) Yttrium(III) oxide (Y₂O₃)
+4 oxidation state	Americium dioxide (AmO₂) Carbon dioxide (CO₂) Carbon trioxide (CO₃) Cerium(IV) oxide (CeO₂) Chlorine dioxide (ClO₂) Chromium(IV) oxide (CrO₂) Dinitrogen tetroxide (N₂O₄) Germanium dioxide (GeO₂) Hafnium(IV) oxide (HfO₂) Lead dioxide (PbO₂) Manganese dioxide (MnO₂) Neptunium(IV) oxide (NpO₂) Nitrogen dioxide (NO₂) Osmium dioxide (OsO₂) Plutonium(IV) oxide (PuO₂) Praseodymium(IV) oxide (PrO₂) Protactinium(IV) oxide (PaO₂) Rhodium(IV) oxide (RhO₂) Ruthenium(IV) oxide (RuO₂) Selenium dioxide (SeO₂) Silicon dioxide (SiO₂) Sulfur dioxide (SO₂) Tellurium dioxide (TeO₂) Terbium(IV) oxide (TbO₂) Thorium dioxide (ThO₂) Tin dioxide (SnO₂) Titanium dioxide (TiO₂) Tungsten(IV) oxide (WO₂) Uranium dioxide (UO₂) Vanadium(IV) oxide (VO₂) Zirconium dioxide (ZrO₂)
+5 oxidation state	Antimony pentoxide (Sb₂O₅) Arsenic pentoxide (As₂O₅) Dinitrogen pentoxide (N₂O₅) Niobium pentoxide (Nb₂O₅) Phosphorus pentoxide (P₂O₅) Protactinium(V) oxide (Pa₂O₅) Tantalum pentoxide (Ta₂O₅) Vanadium(V) oxide (V₂O₅)
+6 oxidation state	Chromium trioxide (CrO₃) Molybdenum trioxide (MoO₃) Rhenium trioxide (ReO₃) Selenium trioxide (SeO₃) Sulfur trioxide (SO₃) Tellurium trioxide (TeO₃) Tungsten trioxide (WO₃) Uranium trioxide (UO₃) Xenon trioxide (XeO₃) Iridium trioxide (IrO₃)
+7 oxidation state	Dichlorine heptoxide (Cl₂O₇) Manganese heptoxide (Mn₂O₇) Rhenium(VII) oxide (Re₂O₇) Technetium(VII) oxide (Tc₂O₇)
+8 oxidation state	Osmium tetroxide (OsO₄) Ruthenium tetroxide (RuO₄) Xenon tetroxide (XeO₄) Iridium tetroxide (IrO₄) Hassium tetroxide (HsO₄)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide
Oxides are sorted by oxidation state. Category:Oxides

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Odtnhj

Vanadium(V) oxide

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