Cobalt(II) oxide: Difference between revisions

Browse history interactively ← Previous editContent deleted Content addedVisual WikitextInline

Revision as of 16:37, 23 July 2011 editMartinBotIII (talk \| contribs)136,346 editsm fix MSDS link (ilo.org) using AWB ← Previous edit		Latest revision as of 11:17, 5 March 2024 edit undo192.167.164.69 (talk) The antiferromagnetic temperature is now expressed in Kelvin degrees that is the measurement unit used from the article cited. In general, Kelvin degrees are used more often for magnetic order temperatures.
(65 intermediate revisions by 51 users not shown)
Line 1:		Line 1:
			{{redirect\|CoO\|\|COO (disambiguation)}}
	{{chembox		{{chembox
			\| Watchedfields = changed
	\| verifiedrevid = ~~401965605~~		\| verifiedrevid = 441022830
	\| ~~Name~~ = Cobalt(II) oxide		\| Name = Cobalt(II) oxide
	\| ImageFile =NaCl polyhedra.png
	\| ~~ImageName~~ = Cobalt(II) oxide		\| ImageFile = Cobalt(II)-oxide-3D-vdW.png
	\| ~~IUPACName~~ = Cobalt(II) oxide		\| ImageName = Cobalt(II) oxide
	\| ~~OtherNames~~ = ~~Cobaltous~~ ~~oxide<br/>~~Cobalt ~~monoxide~~		\| IUPACName = Cobalt(II) oxide
			\| OtherNames = Cobaltous oxide<br/>Cobalt monoxide
⚫	\| Section1 = {{Chembox Identifiers
			\| SystematicName =
⚫	\| ChemSpiderID_Ref = {{chemspidercite\|correct\|chemspider}}
		⚫	\| Section1 = {{Chembox Identifiers
		⚫	\| ChemSpiderID_Ref = {{chemspidercite\|correct\|chemspider}}
	\| ChemSpiderID = 8117730		\| ChemSpiderID = 8117730
	\| InChI = 1/Co.O/rCoO/c1-2		\| InChI = 1/Co.O/rCoO/c1-2
Line 20:		Line 23:
	\| StdInChIKey = IUYLTEAJCNAMJK-UHFFFAOYSA-N		\| StdInChIKey = IUYLTEAJCNAMJK-UHFFFAOYSA-N
	\| CASNo = 1307-96-6		\| CASNo = 1307-96-6
	\| CASNo_Ref = {{cascite\|correct\|CAS}}		\| CASNo_Ref = {{cascite\|correct\|CAS}}
			\| UNII_Ref = {{fdacite\|correct\|FDA}}
	\| PubChem = 9942118
	\| ~~RTECS~~ = ~~GG2800000~~		\| UNII = V9X9644V7Q
	\| ~~UNNumber~~ = ~~3288~~		\| PubChem = 9942118
	\| ~~EINECS~~ = ~~215-154-6~~		\| RTECS = GG2800000
			\| UNNumber = 3288
			\| EINECS = 215-154-6
	}}		}}
	\| Section2 = {{Chembox Properties		\| Section2 = {{Chembox Properties
	\| Formula = CoO		\| Formula = CoO
	\| MolarMass = 74.9326 g/mol		\| MolarMass = 74.9326 g/mol
	\| Appearance = ~~black~~ powder		\| Appearance = olive or gray powder
	\| Odor = odorless		\| Odor = odorless
			\| Density = 6.45 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref>
	\| Density = 6.44 g/cm<sup>3</sup> <ref>{{cite book \| last =Patnaik \| first =Pradyot \| year = 2003 \| title =Handbook of Inorganic Chemical Compounds \| publisher = McGraw-Hill \| page =\| isbn =0070494398 \| url= http://books.google.com/?id=Xqj-TTzkvTEC&pg=PA119 \| accessdate = 2009-06-06}}</ref>
	\| Solubility = insoluble in water<ref>http://www.alfa.com/content/msds/german/44354.pdf</ref>		\| Solubility = insoluble in water<ref> {{Webarchive\|url=https://web.archive.org/web/20110719172732/http://www.alfa.com/content/msds/german/44354.pdf \|date=2011-07-19 }}. Alfa.com. Retrieved on 2011-11-19.</ref>
	\| MeltingPtC = 1933		\| MeltingPtC = 1933
	\| BoilingPt =		\| BoilingPt =
			\| MagSus = +4900.0·10<sup>−6</sup> cm<sup>3</sup>/mol
	}}		}}
	\| Section3 = {{Chembox Structure		\| Section3 = {{Chembox Structure
	\| CrystalStruct = ], ]		\| CrystalStruct = ], ]
	\| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225		\| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225
	}}		}}
			\| Section4 =
⚫	\| Section7 = {{Chembox Hazards
			\| Section5 =
⚫	\| ~~ExternalMSDS~~ =
			\| Section6 =
	\| EUIndex = 027-002-00-4
		⚫	\| Section7 = {{Chembox Hazards
	\| EUClass = Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''')
		⚫	\| ExternalSDS =
	\| RPhrases = {{R22}}, {{R43}}, {{R50/53}}
			\| MainHazards =
	\| SPhrases = {{S2}}, {{S24}}, {{S37}}, {{S60}}, {{S61}}
			\| GHSPictograms = {{GHS07}}{{GHS09}}
⚫	\| NFPA-H =
			\| GHSSignalWord = Warning
⚫	\| NFPA-F =
			\| HPhrases = {{H-phrases\|302\|317\|410}}
	\| NFPA-R =
			\| PPhrases = {{P-phrases\|260\|280\|284\|301+310+330\|304+340+310\|342+311\|403+233}}
⚫	\| FlashPt = Non-flammable
	\| ~~LD50~~ = ~~202 mg/kg~~		\| NFPA-H = 3
		⚫	\| NFPA-F = 0
		⚫	\| NFPA-R = 0
		⚫	\| FlashPt = Non-flammable
			\| LD50 = 202 mg/kg
	}}		}}
	\| Section8 = {{Chembox Related		\| Section8 = {{Chembox Related
	\| OtherAnions = ]<br/>]		\| OtherAnions = ]<br/>]
	\| OtherCations = ]<br/>]		\| OtherCations = ]<br/>]
	\| ~~OtherCpds~~ = ]<br/>]		\| OtherCompounds = ]<br/>]
	}}		}}
	}}		}}

	'''Cobalt(II) oxide~~''' or '''cobalt monoxide~~''' is an inorganic compound that ~~appears~~ as ~~olive-green to red crystals, or~~ as a ~~greyish~~ ~~or black powder.~~<ref~~>{{cite~~ ~~web \|url~~=~~http:~~/~~/msds.chem.ox.ac.uk/CO/cobalt_oxide.html~~ ~~\|title=Safety~~ ~~(MSDS)~~ ~~data for cobalt oxide \|publisher~~=~~The Physical and Theoretical Chemistry Laboratory, Oxford University \|accessdate=2008-11-11}}<~~/~~ref~~> It is used extensively in the ]s industry as an additive to create blue colored glazes and enamels as well as in the chemical industry for producing cobalt(II) salts.		'''Cobalt(II) oxide''' is an ] that has been described as an ]<ref name=G&E/> or ]<ref name=Ullmann/> ]. It is used extensively in the ]s industry as an additive to create blue-colored ] and ], as well as in the chemical industry for producing cobalt(II) salts. A related material is ], a black solid with the ] Co<sub>3</sub>O<sub>4</sub>.

	== Structure and properties ==		== Structure and properties ==
	CoO crystals adopt the ] (]) structure with a lattice constant of 4.~~2615Å~~<ref>{{cite journal\|doi=10.1103/PhysRevB.35.6847\|title=Percolation effects and magnetic properties of the randomly diluted fcc system CopMg1-pO\|year=1987\|~~author~~=Kannan, R.; Seehra, Mohindar S.\|journal=Physical Review B\|volume=35\|pages=~~6847~~}}</ref>.		CoO crystals adopt the ] (]) structure with a lattice constant of 4.2615 Å.<ref>{{cite journal\|doi=10.1103/PhysRevB.35.6847\|title=Percolation effects and magnetic properties of the randomly diluted fcc system CopMg1-pO\|year=1987\|author1=Kannan, R. \|author2=Seehra, Mohindar S. \|journal=Physical Review B\|volume=35\|pages=6847–6853\|issue=13\|pmid=9940938 \|bibcode=1987PhRvB..35.6847K }}</ref>

	It is ] below ~~16°C~~ <ref>{{cite journal\|doi=10.1103/PhysRevB.24.419\|title=Principal magnetic susceptibilities and uniaxial stress experiments in CoO\|year=1981\|~~author~~=Silinsky, P. S.; Seehra, Mohindar S.\|journal=Physical Review B\|volume=24\|pages=~~419~~}}</ref>.		It is ] below 289 K.<ref>{{cite journal\|doi=10.1103/PhysRevB.24.419\|title=Principal magnetic susceptibilities and uniaxial stress experiments in CoO\|year=1981\|author1=Silinsky, P. S. \|author2=Seehra, Mohindar S. \|journal=Physical Review B\|volume=24\|issue=1 \|pages=419–423\|bibcode=1981PhRvB..24..419S }}</ref>

	==Preparation==		==Preparation==
			Cobalt(II) oxide is prepared by oxidation of cobalt powder with air or by thermal decomposition of ] or the carbonate.<ref name=G&E>{{Greenwood&Earnshaw2nd}}</ref><ref name=Ullmann>{{Ullmann \|doi=10.1002/14356007.a07_281.pub2\|title=Cobalt and Cobalt Compounds\|year=2005\|last1=Donaldson\|first1=John Dallas\|last2=Beyersmann\|first2=Detmar}}</ref>
⚫	] decomposes to cobalt(II) oxide at 950 °C:<ref>Process for making a cobalt oxide catalyst, James, Leonard E. ~~(Richmond,~~ ~~VA)~~ Crescentini, Lamberto ~~(Chester~~, ~~VA)~~
	Fisher, William B. (Chester, VA) 1983. http://www.freepatentsonline.com/4389339.html</ref>

		⚫	] decomposes to cobalt(II) oxide at 950 °C:<ref>{{cite patent \| title = Process for making a cobalt oxide catalyst \| invent1 = James, Leonard E. \| invent2 = Crescentini, Lamberto \| invent3 = Fisher, William B. \| pubdate = 1983-06-21 \| number = 4389339 \| country = US }}</ref>
	:2 Co<sub>3</sub>O<sub>4</sub> → 6 CoO + O<sub>2</sub>		:2 Co<sub>3</sub>O<sub>4</sub> → 6 CoO + O<sub>2</sub>

		⚫	It may also be prepared by precipitating the hydroxide, followed by thermal dehydration:{{cn\|date=March 2021}}
	Though commercially available, cobalt(II) oxide may be prepared in the laboratory by electrolyzing a solution of cobalt(II) chloride<ref>Kern, S.; J. Chem. Soc.; 1876. Part 1. p880.</ref>:
		⚫	: CoX<sub>2</sub> + 2 KOH → Co(OH)<sub>2</sub> + 2 KX

	~~CoCl<sub>2</sub>~~ ~~+ H~~<sub>2</sub>O → CoO + H<sub>2</sub> ~~+ Cl<sub>2</sub>~~		: Co(OH)<sub>2</sub> → CoO + H<sub>2</sub>O

⚫	It may also be prepared by precipitating the hydroxide, followed by thermal ~~decomposition~~:

⚫	: CoX + 2 ~~NaOH~~ → Co(OH)<sub>2</sub> + ~~Na<sub>~~2~~</sub>X~~
	: Co(OH)<sub>2</sub> → CoO + H<sub>2</sub>O

	==Reactions==		==Reactions==
	As can be expected, cobalt(II) oxide reacts with mineral acids to form the corresponding cobalt salts:		As can be expected, cobalt(II) oxide reacts with mineral acids to form the corresponding cobalt salts:{{cn\|date=March 2021}}
	: CoO + 2 HX → CoX<sub>2</sub> + H<sub>2</sub>O		: CoO + 2 HX → CoX<sub>2</sub> + H<sub>2</sub>O

	==Applications==		==Applications==
	Cobalt(II) oxide has for centuries used as a coloring agent on ] fired pottery~~; the earliest examples go back to 12th century German pottery.<ref>Zamek, Jeff: "A Problem With Cobalt?" ''Ceramics Today'' http://www.ceramicstoday.com/articles/zamek_cobalt~~.~~htm</ref>~~ The additive provides a deep shade of blue named ]. The band gap (CoO) is around 2.4 eV.		Cobalt(II) oxide has for centuries been used as a coloring agent on ] fired pottery. The additive provides a deep shade of blue named ]. The band gap (CoO) is around 2.4 eV.{{Citation Needed\|date=October 2017}}
	It also is used in ].		It also is used in ].

			==See also==
			*]
		⚫	*]
		⚫	*]

	== References ==		== References ==
Line 93:		Line 103:

	{{Cobalt compounds}}		{{Cobalt compounds}}
			{{Oxygen compounds}}
			{{Oxides}}

	]		]
	]		]
			]

	]
	]
⚫	]
	]
	]
	]
	]
⚫	]
	]
	]
	]

Latest revision as of 11:17, 5 March 2024

"CoO" redirects here. For other uses, see COO (disambiguation).

Cobalt(II) oxide
Names

IUPAC name Cobalt(II) oxide
Other names Cobaltous oxide Cobalt monoxide
Identifiers
CAS Number	1307-96-6
3D model (JSmol)	Interactive image Interactive image
ChemSpider	8117730
ECHA InfoCard	100.013.777
EC Number	215-154-6
PubChem CID	9942118
RTECS number	GG2800000
UNII	V9X9644V7Q
UN number	3288
CompTox Dashboard (EPA)	DTXSID6051649
InChI InChI=1S/Co.O/q+2;-2Key: IUYLTEAJCNAMJK-UHFFFAOYSA-N InChI=1/Co.O/rCoO/c1-2Key: IVMYJDGYRUAWML-NNYFCMOLAO InChI=1/Co.O/q+2;-2Key: IUYLTEAJCNAMJK-UHFFFAOYAY
SMILES =O .
Properties
Chemical formula	CoO
Molar mass	74.9326 g/mol
Appearance	olive or gray powder
Odor	odorless
Density	6.45 g/cm
Melting point	1,933 °C (3,511 °F; 2,206 K)
Solubility in water	insoluble in water
Magnetic susceptibility (χ)	+4900.0·10 cm/mol
Structure
Crystal structure	cubic, cF8
Space group	Fm3m, No. 225
Hazards
GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H302, H317, H410
Precautionary statements	P260, P280, P284, P301+P310+P330, P304+P340+P310, P342+P311, P403+P233
NFPA 704 (fire diamond)	3 0 0
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	202 mg/kg
Safety data sheet (SDS)	ICSC 1551
Related compounds
Other anions	Cobalt(II) sulfide Cobalt(II) hydroxide
Other cations	Iron(II) oxide Nickel(II) oxide
Related compounds	Cobalt(II,III) oxide Cobalt(III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Y verify (what is ?) Infobox references

Chemical compound

Cobalt(II) oxide is an inorganic compound that has been described as an olive-green or gray solid. It is used extensively in the ceramics industry as an additive to create blue-colored glazes and enamels, as well as in the chemical industry for producing cobalt(II) salts. A related material is cobalt(II,III) oxide, a black solid with the formula Co₃O₄.

Structure and properties

CoO crystals adopt the periclase (rock salt) structure with a lattice constant of 4.2615 Å.

It is antiferromagnetic below 289 K.

Preparation

Cobalt(II) oxide is prepared by oxidation of cobalt powder with air or by thermal decomposition of cobalt(II) nitrate or the carbonate.

Cobalt(II,III) oxide decomposes to cobalt(II) oxide at 950 °C:

2 Co₃O₄ → 6 CoO + O₂

It may also be prepared by precipitating the hydroxide, followed by thermal dehydration:

CoX₂ + 2 KOH → Co(OH)₂ + 2 KX

Co(OH)₂ → CoO + H₂O

Reactions

As can be expected, cobalt(II) oxide reacts with mineral acids to form the corresponding cobalt salts:

CoO + 2 HX → CoX₂ + H₂O

Applications

Cobalt(II) oxide has for centuries been used as a coloring agent on kiln fired pottery. The additive provides a deep shade of blue named cobalt blue. The band gap (CoO) is around 2.4 eV. It also is used in cobalt blue glass.

References

Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, Florida: CRC Press. ISBN 0-8493-0487-3.
Advanced Search – Alfa Aesar – A Johnson Matthey Company Archived 2011-07-19 at the Wayback Machine. Alfa.com. Retrieved on 2011-11-19.
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Donaldson, John Dallas; Beyersmann, Detmar (2005). "Cobalt and Cobalt Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a07_281.pub2. ISBN 978-3527306732.
Kannan, R.; Seehra, Mohindar S. (1987). "Percolation effects and magnetic properties of the randomly diluted fcc system CopMg1-pO". Physical Review B. 35 (13): 6847–6853. Bibcode:1987PhRvB..35.6847K. doi:10.1103/PhysRevB.35.6847. PMID 9940938.
Silinsky, P. S.; Seehra, Mohindar S. (1981). "Principal magnetic susceptibilities and uniaxial stress experiments in CoO". Physical Review B. 24 (1): 419–423. Bibcode:1981PhRvB..24..419S. doi:10.1103/PhysRevB.24.419.
US 4389339, James, Leonard E.; Crescentini, Lamberto & Fisher, William B., "Process for making a cobalt oxide catalyst", published 1983-06-21

v t e Cobalt compounds
Cobalt(I)	HCo(CO)₄
Cobalt(II)	CoBr₂ Co(CN)₂ CoCO₃ CoC₂O₄ CoCl₂ Co(ClO₃)₂ Co(ClO₄)₂ CoF₂ Co(HCO₂)₂ CoI₂ Co(NO₃)₂ Co₃(PO₄)₂ Co(OAc)₂ CoGeO₃ CoO Co(OH)₂ CoS Co(OCN)₂ Co(SCN)₂ CoSO₄ CoSe Co₃P₂ CoH₂ Co(C₃H₆O₃)₂ C ₂₄H ₄₈CoO ₄ C ₃₆H ₇₀CoO ₄
Cobalt(0,III)	CoSi CoGe
Cobalt(II,III)	Co₃O₄
Cobalt(III)	CoAs CoCl₃ Co(NO₃)₃ Co₂O₃ CoF₃ Co(OH)₃ LiCoO₂
Cobalt(III,IV)	Na_xCoO₂
Cobalt(IV)	CoF₄ Cs₂CoF₆ CoC₂₈H₄₄
Cobalt(V)	Na₃CoO₄

v t e Oxygen compounds
Ag₄O₄ Al₂O₃ AmO₂ Am₂O₃ As₂O₃ As₂O₅ Au₂O₃ B₂O₃ BaO BeO Bi₂O₃ BiO₂ Bi₂O₅ BrO₂ Br₂O₃ Br₂O₅ Br ₃O ₈ CO CO₂ C₃O₂ CaO CaO₂ CdO CeO₂ Ce₃O₄ Ce₂O₃ ClO₂ Cl₂O Cl₂O₂ Cl₂O₃ Cl₂O₄ Cl₂O₆ Cl₂O₇ CoO Co₂O₃ Co₃O₄ CrO₃ Cr₂O₃ Cr₂O₅ Cr₅O₁₂ CsO₂ Cs₂O₃ CuO Dy₂O₃ Er₂O₃ Eu₂O₃ FeO Fe₂O₃ Fe₃O₄ Ga₂O Ga₂O₃ GeO GeO₂ H₂O H₂O H₂O H₂O H₂O₂ HfO₂ HgO Hg₂O Ho₂O₃ IO I₂O₄ I₂O₅ I₂O₆ I₄O₉ In₂O₃ IrO₂ KO₂ K₂O₂ La₂O₃ Li₂O Li₂O₂ Lu₂O₃ MgO Mg₂O₃ MnO MnO₂ Mn₂O₃ Mn₂O₇ MoO₂ MoO₃ Mo₂O₃ NO NO₂ N₂O N₂O₃ N₂O₄ N₂O₅ NaO₂ Na₂O Na₂O₂ NbO NbO₂ Nd₂O₃ O₂F OF OF₂ O₂F₂ O₃F₂ O₄F₂ O₅F₂ O₆F₂ O₂PtF₆ more...

Oxygen compounds

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

Categories: