Manganese heptoxide: Difference between revisions

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			{{Short description\|Chemical compound}}
	{{Chembox		{{Chembox
			\| Verifiedfields = changed
	\| verifiedrevid = 431916363
			\| Watchedfields = changed
	\| Name = Manganese(VII) oxide
			\| verifiedrevid = 450876772
	\| ImageFile1 = Mn2O7.png
			\| Name = Manganese(VII) oxide
	\| ImageSize1 =
			\| ImageFile = Mn2O7.svg
	\| ImageName1 = Manganese(VII) oxide
			\| ImageSize =
	\| ImageFile2 = Manganese-heptoxide-3D-balls.png
			\| ImageName = Manganese(VII) oxide
	\| ImageSize2 =
	\| ~~ImageName2~~ = ~~Ball-and-stick~~ ~~model~~ of ~~manganese~~ heptoxide		\| ImageFile1 = Manganese-heptoxide-3D-balls.png
			\| ImageSize1 =
	\| ImageFile3 = Manganese heptoxide.jpg
			\| ImageName1 = Ball-and-stick model of manganese heptoxide
	\| ImageName3 = Manganese(VII) oxide
	\| ~~IUPACName~~ = Manganese~~(VII) oxide~~		\| ImageFile2 = Manganese-heptoxide-3D-vdW.png
			\| ImageName2 = Manganese(VII) oxide
	\| OtherNames = Permanganic acid<br />Manganic oxide<br /> dimanganese heptoxide
			\| ImageFile3 = Manganese_heptoxide.jpg
	\| Section1 = {{Chembox Identifiers
			\| ImageName3 =
	\| SMILES = O=(O=)(O=)MnOMn(=O)(=O)=O
			\| IUPACName = Manganese(VII) oxide
	\| CASNo = 12057-92-0
			\| OtherNames = Manganic oxide<br /> dimanganese heptoxide<br/>Permanganic anhydride<br /> Permanganic oxide
	\| RTECS =
			\| SystematicName =
	}}
	\| ~~Section2~~ = {{Chembox ~~Properties~~		\| Section1 = {{Chembox Identifiers
			\| CASNo_Ref = {{cascite\|correct\|??}}
	\| Formula = Mn<sub>2</sub>O<sub>7</sub>
			\| CASNo = 12057-92-0
	\| MolarMass = 221.87 g/mol
			\| ChemSpiderID = 9944714
	\| Appearance = dark red oil (room temp.), green if in contact with sulfuric acid
			\| EINECS = 235-025-8
	\| Density = 2.79 g/cm<sup>3</sup>
			\| PubChem = 13879826
	\| Solubility = decomposes to permanganic acid, HMnO4
			\| StdInChI=1S/2Mn.7O/q;;7*-2
	\| MeltingPt = 5.9 °C, 279.1 K
			\| StdInChIKey = ZEFXULJEOUCCOQ-UHFFFAOYSA-N
	\| BoilingPt = explodes on heating<br /> sublimes at −10 °C
			\| SMILES = O=(=O)(=O)O(=O)(=O)=O
	}}

	\| Section3 = {{Chembox Structure
			}}
	\| Coordination = bitetrahedral
			\| Section2 = {{Chembox Properties
	\| CrystalStruct = monoclinic
			\| Formula = Mn<sub>2</sub>O<sub>7</sub>
	}}
			\| MolarMass = 221.87 g/mol
	\| Section7 = {{Chembox Hazards
			\| Appearance = dark red oil (room temp.), green if in contact with sulfuric acid
	\| ExternalMSDS =
			\| Density = 2.79 g/cm<sup>3</sup>
	\| MainHazards = explosive, strong oxidizer, very corrosive
			\| Solubility = decomposes to ], HMnO4
	\| RPhrases =
	\| ~~SPhrases~~ =		\| MeltingPtC = 5.9
			\| MeltingPt_notes =
	}}
			\| BoilingPt = explodes on heating
	\| Section8 = {{Chembox Related
			}}
	\| OtherCpds = ] ]<br /> ]
			\| Section3 = {{Chembox Structure
	}}
			\| Coordination = bitetrahedral
			\| CrystalStruct = monoclinic
			}}
			\| Section4 =
			\| Section5 =
			\| Section6 =
			\| Section7 = {{Chembox Hazards
			\| ExternalSDS =
			\| MainHazards = explosive, strong oxidizer, very corrosive
			\| GHSPictograms = {{GHS01}}{{GHS03}}{{GHS05}}{{GHS06}}
			\| GHSSignalWord = Danger
			\| HPhrases = {{H-phrases\|201}}, {{H-phrases\|271}}, {{H-phrases\|314}}, {{H-phrases\|300+310+330}}
			\| PPhrases = {{P-phrases\|260}}, {{P-phrases\|284}}, {{P-phrases\|283}}, {{P-phrases\|221}}
			\| NFPA-H = 4
			\| NFPA-F = 4
			\| NFPA-R = 4
			\| NFPA-S = OX
			}}
			\| Section8 = {{Chembox Related
			\| OtherCompounds = ]<br /> ]<br /> ]<br /> ]
			}}
	}}		}}

	'''Manganese(VII) oxide''' is an ] with the ] Mn~~<sub>~~2~~</sub>~~O~~<sub>~~7~~</sub>.~~ ~~This~~ volatile liquid is highly reactive and ~~more~~ ~~often~~ ~~discussed~~ ~~than~~ ~~intentionally~~ ~~prepared.~~ It is a ~~dangerous~~ ~~oxidizer and~~ was first described in 1860.<ref>Aschoff, H. Ann. Phys. Chem. Ser. 2 volume 111 (1860) page 217 and page 224.</ref>		'''Manganese(VII) oxide''' (manganese heptoxide) is an ] with the ] {{chem2\|]2]7}} Manganese heptoxide is a volatile liquid with an oily consistency. It is a highly reactive and powerful ] that reacts explosively with nearly any ]. It was first described in 1860.<ref>Aschoff, H. Ann. Phys. Chem. Ser. 2 volume 111 (1860) page 217 and page 224.</ref> It is the ] of ].

	== Properties ==		== Properties ==
			The ] form of this chemical compound is dark green. The liquid is green by reflected light and red by transmitted light.<ref name=brauer>{{cite book\|author=H. Lux\|chapter=Manganese(VII) Oxide\|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. \|editor=G. Brauer\|publisher=Academic Press\|year=1963\|place=NY, NY\|volume=1\|pages=1459–1460}}</ref> It is soluble in ], and decomposes when in contact with water.
	The ] form of this chemical compound is dark green. It is soluble in ], and decomposes when in contact with water. It melts at only 5.9 °C, and sublimes at −10 °C{{Clarify\|date=June 2010}}. These properties indicate a ] molecular species, which is confirmed by its structure. The molecules consist of a pair of tetrahedra that share a common vertex. The vertices are occupied by oxygen atoms and at the centers of the tetrahedra are the Mn(VII) centers. The connectivity is indicated by the formula O<sub>3</sub>Mn-O-MnO<sub>3</sub>. The terminal Mn-O distances are 1.585 Å and the bridging oxygen is 1.77 Å distant from the two Mn atoms. The Mn-O-Mn angle is 120.7°.<ref>{{cite journal \| author = Simon, A.; Dronskowski, R.; Krebs, B.; Hettich, B. \| title = The Crystal Structure of Mn<sub>2</sub>O<sub>7</sub> \| journal = ] \| year = 1987 \| volume = 26 \| pages = 139–140 \| doi = 10.1002/anie.198701391}}</ref>

			==Structure==
	It contains manganese in its highest oxidation state. This oxidation state, +7, is shared by ]s, which are more stable compounds.
			Its solubility properties indicate a ] molecular species, which is confirmed by its structure. The molecules consist of a pair of ] that share a common vertex. The vertices are occupied by oxygen atoms and at the centers of the tetrahedra are the Mn(VII) centers. The connectivity is indicated by the formula O<sub>3</sub>Mn−O−MnO<sub>3</sub>. The terminal Mn−O distances are 1.585 Å and the bridging oxygen is 1.77 Å distant from the two Mn atoms. The Mn−O−Mn angle is 120.7°.<ref>{{cite journal \|author1=Simon, A. \|author2=Dronskowski, R. \|author3=Krebs, B. \|author4=Hettich, B. \| title = The Crystal Structure of Mn<sub>2</sub>O<sub>7</sub> \| journal = ] \| year = 1987 \| volume = 26 \|issue=2 \| pages = 139–140 \| doi = 10.1002/anie.198701391}}</ref>

	Pyrosulfate, pyrophosphate, and dichromate adopt structures similar to that of ~~Mn<sub>2</sub>O<sub>7</sub>~~. Probably the most similar main group species is ]. Focusing on comparisons within the transition metal series, ] and ~~Mn<sub>2</sub>O<sub>7</sub>~~ are structurally similar but the ~~Tc-O-Tc~~ angle is 180°. Solid ] is not molecular but consists of crosslinked Re centers with both tetrahedral and octahedral sites,<ref>{{cite journal \| ~~author~~ = Krebs, B.; Mueller, A.; Beyer, H. H. \| title = The Crystal Structure of Rhenium(VII) Oxide \| journal = ] \| year = 1969 \| volume = 8 \| pages = 436–443 \| doi = 10.1021/ic50073a006}}</ref> in the vapour phase it is molecular with a similar structure to Tc<sub>2</sub>O<sub>7</sub>.<ref>Wells A.F. (1962) ''Structural Inorganic Chemistry'' 3d edition Oxford University Press</ref>		], ], and ] adopt structures similar to that of {{chem2\|Mn2O7}}. Probably the most similar main group species is {{chem2\|]}}. Focusing on comparisons within the transition metal series, {{chem2\|]}} and {{chem2\|Mn2O7}} are structurally similar but the Tc−O−Tc angle is 180°. Solid {{chem2\|]}} is not molecular but consists of crosslinked Re centers with both tetrahedral and octahedral sites;<ref>{{cite journal \|author1=Krebs, B. \|author2=Mueller, A. \|author3=Beyer, H. H. \| title = The Crystal Structure of Rhenium(VII) Oxide \| journal = ] \| year = 1969 \| volume = 8 \|issue=3 \| pages = 436–443 \| doi = 10.1021/ic50073a006}}</ref> in the vapour phase it is molecular with a similar structure to Tc<sub>2</sub>O<sub>7</sub>.<ref>Wells A.F. (1962) ''Structural Inorganic Chemistry'' 3d edition Oxford University Press</ref>

	== Synthesis and reactions ==		== Synthesis and reactions ==
	~~Mn<sub>2</sub>O<sub>7</sub>~~ arises as a dark green oil by the addition of concentrated ] to ]. The reaction initially produces permanganic acid, ~~HMnO<sub>4</sub>~~ (structurally, ~~HOMnO<sub>3</sub>~~), which is dehydrated by sulfuric acid to form its ], ~~Mn<sub>2</sub>O<sub>7</sub>.~~		{{chem2\|Mn2O7}} arises as a dark green oil by the addition of cold concentrated {{chem2\|]}} to solid {{chem2\|]}}.<ref name=brauer/> The reaction initially produces ], {{chem2\|HMnO4}} (structurally, {{chem2\|HOMnO3}}), which is dehydrated by cold sulfuric acid to form its ], {{chem2\|Mn2O7}}:
			:{{chem2\|2 KMnO4 + 2 H2SO4 -> Mn2O7 + H2O + 2 KHSO4}}
	:2 KMnO<sub>4</sub> +(cold) 2 H<sub>2</sub>SO<sub>4</sub> → Mn<sub>2</sub>O<sub>7</sub> + H<sub>2</sub>O + 2 KHSO<sub>4</sub>

	~~Mn<sub>2</sub>O<sub>7</sub>~~ can react further with sulfuric acid to give the remarkable cation ~~MnO<sub>3</sub><sup>~~+~~</sup>~~, which is ] with ]~~:{{Citation needed\|date=June 2010~~}}		{{chem2\|Mn2O7}} can react further with sulfuric acid to give the remarkable manganyl(VII) cation {{chem2\|MnO3+}}, which is ] with {{chem2\|]}}:
			:{{chem2\|Mn2O7 + 2 H2SO4 -> 2 +- + H2O}}

			{{chem2\|Mn2O7}} decomposes near room temperature, explosively so above {{convert\|55\|C}}. The explosion can be initiated by striking the sample or by its exposure to oxidizable organic compounds. The products are {{chem2\|]}} and {{chem2\|]}}.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN\|0-12-352651-5}}.</ref> ] is also produced, giving a strong smell to the substance. The ozone can spontaneously ignite a piece of paper impregnated with an alcohol solution.{{Citation needed\|date=June 2024}}
	:Mn<sub>2</sub>O<sub>7</sub> + 2 H<sub>2</sub>SO<sub>4</sub> → 2 {{chem\|\|+\|\|-}} + H<sub>2</sub>O

			Manganese heptoxide reacts with ] in presence of ], liberating ] and ]:
	Mn<sub>2</sub>O<sub>7</sub> decomposes near room temperature, explosively so at > 55 °C. The explosion can be initiated by striking the sample or by its exposure to oxidizable organic compounds. The products are ] and ].<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> ] is also produced, giving a strong smell to the substance. The ozone can spontaneously ignite a piece of paper impregnated with an alcohol solution. The production of manganese heptoxide is an undesirable byproduct in many situations.{{Citation needed\|date=September 2011}}
			:{{chem2\|2 Mn2O7 + 2 ] + 4 ] -> 4 ] + 6 ] + 2 ] + 3 ]}}

	== References ==		== References ==
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	{{Manganese compounds}}		{{Manganese compounds}}
			{{Oxides}}

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Latest revision as of 00:58, 16 December 2024

Chemical compound

Manganese(VII) oxide
Names




IUPAC name Manganese(VII) oxide
Other names Manganic oxide dimanganese heptoxide Permanganic anhydride Permanganic oxide
Identifiers
CAS Number	12057-92-0
3D model (JSmol)	Interactive image
ChemSpider	9944714
ECHA InfoCard	100.031.829
EC Number	235-025-8
PubChem CID	13879826
CompTox Dashboard (EPA)	DTXSID10894891
InChI InChI=1S/2Mn.7O/q;;7*-2Key: ZEFXULJEOUCCOQ-UHFFFAOYSA-N
SMILES O=(=O)(=O)O(=O)(=O)=O
Properties
Chemical formula	Mn₂O₇
Molar mass	221.87 g/mol
Appearance	dark red oil (room temp.), green if in contact with sulfuric acid
Density	2.79 g/cm
Melting point	5.9 °C (42.6 °F; 279.0 K)
Boiling point	explodes on heating
Solubility in water	decomposes to permanganic acid, HMnO4
Structure
Crystal structure	monoclinic
Coordination geometry	bitetrahedral
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	explosive, strong oxidizer, very corrosive
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H201, H271, H314, H300+H310+H330
Precautionary statements	P260, P284, P283, P221
NFPA 704 (fire diamond)	4 4 4 OX
Related compounds
Related compounds	Re₂O₇ KMnO₄ Tc₂O₇ Cl₂O₇
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). N verify (what is ?) Infobox references

Chemical compound

Manganese(VII) oxide (manganese heptoxide) is an inorganic compound with the formula Mn₂O₇ Manganese heptoxide is a volatile liquid with an oily consistency. It is a highly reactive and powerful oxidizer that reacts explosively with nearly any organic compound. It was first described in 1860. It is the acid anhydride of permanganic acid.

Properties

The crystalline form of this chemical compound is dark green. The liquid is green by reflected light and red by transmitted light. It is soluble in carbon tetrachloride, and decomposes when in contact with water.

Structure

Its solubility properties indicate a nonpolar molecular species, which is confirmed by its structure. The molecules consist of a pair of tetrahedra that share a common vertex. The vertices are occupied by oxygen atoms and at the centers of the tetrahedra are the Mn(VII) centers. The connectivity is indicated by the formula O₃Mn−O−MnO₃. The terminal Mn−O distances are 1.585 Å and the bridging oxygen is 1.77 Å distant from the two Mn atoms. The Mn−O−Mn angle is 120.7°.

Pyrosulfate, pyrophosphate, and dichromate adopt structures similar to that of Mn₂O₇. Probably the most similar main group species is Cl₂O₇. Focusing on comparisons within the transition metal series, Tc₂O₇ and Mn₂O₇ are structurally similar but the Tc−O−Tc angle is 180°. Solid Re₂O₇ is not molecular but consists of crosslinked Re centers with both tetrahedral and octahedral sites; in the vapour phase it is molecular with a similar structure to Tc₂O₇.

Synthesis and reactions

Mn₂O₇ arises as a dark green oil by the addition of cold concentrated H₂SO₄ to solid KMnO₄. The reaction initially produces permanganic acid, HMnO₄ (structurally, HOMnO₃), which is dehydrated by cold sulfuric acid to form its anhydride, Mn₂O₇:

2 KMnO₄ + 2 H₂SO₄ → Mn₂O₇ + H₂O + 2 KHSO₄

Mn₂O₇ can react further with sulfuric acid to give the remarkable manganyl(VII) cation MnO+3, which is isoelectronic with CrO₃:

Mn₂O₇ + 2 H₂SO₄ → 2 [MnO₃][HSO₄] + H₂O

Mn₂O₇ decomposes near room temperature, explosively so above 55 °C (131 °F). The explosion can be initiated by striking the sample or by its exposure to oxidizable organic compounds. The products are MnO₂ and O₂. Ozone is also produced, giving a strong smell to the substance. The ozone can spontaneously ignite a piece of paper impregnated with an alcohol solution.

Manganese heptoxide reacts with hydrogen peroxide in presence of sulfuric acid, liberating oxygen and ozone:

2 Mn₂O₇ + 2 H₂O₂ + 4 H₂SO₄ → 4 MnSO₄ + 6 H₂O + 2 O₃ + 3 O₂

References

Aschoff, H. Ann. Phys. Chem. Ser. 2 volume 111 (1860) page 217 and page 224.
^ H. Lux (1963). "Manganese(VII) Oxide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1. NY, NY: Academic Press. pp. 1459–1460.
Simon, A.; Dronskowski, R.; Krebs, B.; Hettich, B. (1987). "The Crystal Structure of Mn₂O₇". Angew. Chem. Int. Ed. Engl. 26 (2): 139–140. doi:10.1002/anie.198701391.
Krebs, B.; Mueller, A.; Beyer, H. H. (1969). "The Crystal Structure of Rhenium(VII) Oxide". Inorganic Chemistry. 8 (3): 436–443. doi:10.1021/ic50073a006.
Wells A.F. (1962) Structural Inorganic Chemistry 3d edition Oxford University Press
Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.

v t e Manganese compounds
Manganese(−I)	MnH(CO)₅
Manganese(0)	Mn₂(CO)₁₀
Manganese(I)	(C₅H₄CH₃)Mn(CO)₃ Mn(CO)₅Br Na₅Mn(CN)₆
Manganese(II)	MnC₂O₄ MnO Mn₃(PO₄)₂ MnS MnSe MnTe Mn(NO₃)₂ MnCO₃ MnCl₂ MnSO₄ MnF₂ MnBr₂ MnI₂ MnTiO₃ MnMoO₄ Mn(CH₃COO)₂ Mn(OH)₂ MnSe₂ Mn(ClO₃)₂ Mn(ClO₄)₂ Mn(C₅H₅)₂ Mn(C₃H₅O₃)₂ C ₂₄H ₄₈MnO ₄ C ₃₆H ₇₀MnO ₄
Manganese(II,III)	Mn₃O₄
Manganese(II,IV)	Mn₅O₈
Manganese(III)	MnCl₃ Mn₂O₃ MnF₃ K₆Mn₂O₆ MnAs MnPO₄ Mn(CH₃COO)₃
Manganese(IV)	MnS₂ MnCl₄ MnO₂ MnF₄ MnSi MnGe
Manganese(V)	K₃MnO₄ MnF₅ (predicted)
Manganese(VI)	H₂MnO₄ MnO₃ Na₂MnO₄ K₂MnO₄ BaMnO₄ MnO₂F₂ (predicted)
Manganese(VII)	Mn₂O₇ KMnO₄ MnO₃F

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb₂O₄) Boron suboxide (B₁₂O₂) Carbon suboxide (C₃O₂) Chlorine perchlorate (Cl₂O₄) Chloryl perchlorate (Cl₂O₆) Cobalt(II,III) oxide (Co₃O₄) Dichlorine pentoxide (Cl₂O₅) Iron(II,III) oxide (Fe₃O₄) Lead(II,IV) oxide (Pb₃O₄) Manganese(II,III) oxide (Mn₃O₄) Mellitic anhydride (C₁₂O₉) Praseodymium(III,IV) oxide (Pr₆O₁₁) Silver(I,III) oxide (Ag₂O₂) Terbium(III,IV) oxide (Tb₄O₇) Tribromine octoxide (Br₃O₈) Triuranium octoxide (U₃O₈)
+1 oxidation state	Aluminium(I) oxide (Al₂O) Copper(I) oxide (Cu₂O) Caesium monoxide (Cs₂O) Dibromine monoxide (Br₂O) Dicarbon monoxide (C₂O) Dichlorine monoxide (Cl₂O) Gallium(I) oxide (Ga₂O) Iodine(I) oxide (I₂O) Lithium oxide (Li₂O) Mercury(I) oxide (Hg₂O) Nitrous oxide (N₂O) 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) Berkelium monoxide (BkO) Beryllium oxide (BeO) Boron monoxide (BO) Bromine monoxide (BrO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chlorine monoxide (ClO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N₂O₂) Europium(II) oxide (EuO) Germanium monoxide (GeO) Iron(II) oxide (FeO) Iodine monoxide (IO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Niobium monoxide (NbO) Palladium(II) oxide (PdO) Phosphorus monoxide (PO) Polonium monoxide (PoO) Protactinium monoxide (PaO) Radium oxide (RaO) 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) Yttrium(II) oxide (YO) Zirconium monoxide (ZrO) Zinc oxide (ZnO)
+3 oxidation state	Actinium(III) oxide (Ac₂O₃) Aluminium oxide (Al₂O₃) Americium(III) oxide (Am₂O₃) Antimony trioxide (Sb₂O₃) Arsenic trioxide (As₂O₃) Berkelium(III) oxide (Bk₂O₃) Bismuth(III) oxide (Bi₂O₃) Boron trioxide (B₂O₃) Caesium sesquioxide (Cs₂O₃) Californium(III) oxide (Cf₂O₃) Cerium(III) oxide (Ce₂O₃) Chromium(III) oxide (Cr₂O₃) Cobalt(III) oxide (Co₂O₃) Dinitrogen trioxide (N₂O₃) Dysprosium(III) oxide (Dy₂O₃) Einsteinium(III) oxide (Es₂O₃) Erbium(III) oxide (Er₂O₃) Europium(III) oxide (Eu₂O₃) Gadolinium(III) oxide (Gd₂O₃) Gallium(III) oxide (Ga₂O₃) Gold(III) oxide (Au₂O₃) 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) Berkelium(IV) oxide (BkO₂) Bromine dioxide (BrO₂) Californium dioxide (CfO₂) Carbon dioxide (CO₂) Carbon trioxide (CO₃) Cerium(IV) oxide (CeO₂) Chlorine dioxide (ClO₂) Chromium(IV) oxide (CrO₂) Curium(IV) oxide (CmO₂) Dinitrogen tetroxide (N₂O₄) Germanium dioxide (GeO₂) Iodine dioxide (IO₂) Iridium dioxide (IrO₂) Hafnium(IV) oxide (HfO₂) Lead dioxide (PbO₂) Manganese dioxide (MnO₂) Molybdenum dioxide (MoO₂) Neptunium(IV) oxide (NpO₂) Nitrogen dioxide (NO₂) Niobium dioxide (NbO₂) Osmium dioxide (OsO₂) Platinum dioxide (PtO₂) Plutonium(IV) oxide (PuO₂) Polonium dioxide (PoO₂) Praseodymium(IV) oxide (PrO₂) Protactinium(IV) oxide (PaO₂) Rhenium(IV) oxide (ReO₂) Rhodium(IV) oxide (RhO₂) Ruthenium(IV) oxide (RuO₂) Selenium dioxide (SeO₂) Silicon dioxide (SiO₂) Sulfur dioxide (SO₂) Technetium(IV) oxide (TcO₂) 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) Bismuth pentoxide (Bi₂O₅) Dinitrogen pentoxide (N₂O₅) Niobium pentoxide (Nb₂O₅) Phosphorus pentoxide (P₂O₅) Protactinium(V) oxide (Pa₂O₅) Tantalum pentoxide (Ta₂O₅) Tungsten pentoxide (W₂O₅) Vanadium(V) oxide (V₂O₅)
+6 oxidation state	Chromium trioxide (CrO₃) Molybdenum trioxide (MoO₃) Polonium trioxide (PoO₃) Rhenium trioxide (ReO₃) Selenium trioxide (SeO₃) Sulfur trioxide (SO₃) Tellurium trioxide (TeO₃) Tungsten trioxide (WO₃) Uranium trioxide (UO₃) Xenon trioxide (XeO₃)
+7 oxidation state	Dichlorine heptoxide (Cl₂O₇) Manganese heptoxide (Mn₂O₇) Rhenium(VII) oxide (Re₂O₇) Technetium(VII) oxide (Tc₂O₇)
+8 oxidation state	Iridium tetroxide (IrO₄) Osmium tetroxide (OsO₄) Ruthenium tetroxide (RuO₄) Xenon tetroxide (XeO₄) Hassium tetroxide (HsO₄)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxypnictide
Oxides are sorted by oxidation state. Category:Oxides

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