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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.
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			{{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
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	| 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&nbsp;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&nbsp;°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> &rarr; 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 ==
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	{{Cobalt compounds}}		{{Cobalt compounds}}
			{{Oxygen compounds}}
			{{Oxides}}
	]		]
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