| 词条 | Cobalt(II) oxide |
| 释义 |
| Watchedfields = changed | verifiedrevid = 441022830 | Name = Cobalt(II) oxide | ImageFile =NaCl polyhedra.png | ImageName = Cobalt(II) oxide | IUPACName = Cobalt(II) oxide | OtherNames = Cobaltous oxide Cobalt monoxide |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 8117730 | InChI = 1/Co.O/rCoO/c1-2 | SMILES = [Co]=O | InChIKey = IVMYJDGYRUAWML-NNYFCMOLAO | InChI1 = 1/Co.O/q+2;-2 | InChIKey1 = IUYLTEAJCNAMJK-UHFFFAOYAY | SMILES1 = [Co+2].[O-2] | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/Co.O/q+2;-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = IUYLTEAJCNAMJK-UHFFFAOYSA-N | CASNo = 1307-96-6 | CASNo_Ref = {{cascite|correct|CAS}} | PubChem = 9942118 | RTECS = GG2800000 | UNNumber = 3288 | EINECS = 215-154-6 |Section2={{Chembox Properties | Formula = CoO | MolarMass = 74.9326 g/mol | Appearance = black powder | Odor = odorless | Density = 6.44 g/cm3 [1] | Solubility = insoluble in water[2] | MeltingPtC = 1933 | BoilingPt = | MagSus = +4900.0·10−6 cm3/mol |Section3={{Chembox Structure | CrystalStruct = cubic, cF8 | SpaceGroup = Fm3m, No. 225 }} |Section7={{Chembox Hazards | ExternalSDS = ICSC 1551 | MainHazards = Toxic (T) Harmful (Xn) Dangerous for the environment (N) | EUClass = {{Hazchem T}}{{Hazchem Xn}}{{Hazchem N}} | RPhrases = {{R22}}, {{R43}}, {{R50/53}} | SPhrases = {{S2}}, {{S24}}, {{S37}}, {{S60}}, {{S61}} | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 0 | FlashPt = Non-flammable | LD50 = 202 mg/kg |Section8={{Chembox Related | OtherAnions = Cobalt(II) sulfide Cobalt(II) hydroxide | OtherCations = Iron(II) oxide Nickel(II) oxide | OtherCompounds = Cobalt(II,III) oxide Cobalt(III) oxide }} 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.[3] 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. Structure and propertiesCoO crystals adopt the periclase (rock salt) structure with a lattice constant of 4.2615 Å.[4] It is antiferromagnetic below 16 °C.[5] PreparationCobalt(II,III) oxide decomposes to cobalt(II) oxide at 950 °C:[6]2 Co3O4 → 6 CoO + O2 Though commercially available, cobalt(II) oxide may be prepared in the laboratory by electrolyzing a solution of cobalt(II) chloride.[7] CoCl2 + H2O → CoO + H2 + Cl2 It may also be prepared by precipitating the hydroxide, followed by thermal dehydration: CoX + 2 KOH → Co(OH)2 + K2X Co(OH)2 → CoO + H2O ReactionsAs can be expected, cobalt(II) oxide reacts with mineral acids to form the corresponding cobalt salts: CoO + 2 HX → CoX2 + H2O ApplicationsCobalt(II) oxide has for centuries 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.{{Citation Needed|date=October 2017}} It also is used in cobalt blue glass. See also
References1. ^{{cite book | last =Patnaik | first =Pradyot | year = 2003 | title =Handbook of Inorganic Chemical Compounds | publisher = McGraw-Hill | page =| isbn =0-07-049439-8 | url= https://books.google.com/books?id=Xqj-TTzkvTEC&pg=PA119 | accessdate = 2009-06-06}} {{Cobalt compounds}}{{Oxygen compounds}}{{Oxides}}2. ^Advanced Search – Alfa Aesar – A Johnson Matthey Company. Alfa.com. Retrieved on 2011-11-19. 3. ^{{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}} 4. ^{{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}} 5. ^{{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|pages=419–423}} 6. ^{{cite patent | title = Process for making a cobalt oxide catalyst | invent1 = James, Leonard E. | invent2 = Crescentini, Lamberto | invent3 = Fisher, William B. | year = 1983 | number = 4389339 | country = US }} 7. ^{{cite journal|author=Kern, S.|journal= J. Chem. Soc.|year= 1876|page=880|doi=10.1039/JS8762900876|volume=29|title=Inorganic chemistry}} 2 : Cobalt compounds|Oxides |
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