| 词条 | Cobalt(II) nitrate | ||||
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 476999100 | Name = Cobalt(II) nitrate | ImageFile1 = Cobalt(II)-nitrate-hexahydrate-sample.jpg | ImageName1 = Cobalt (II) Nitrate Hexahydrate Sample | OtherNames = Cobaltous nitrate Nitric acid, cobalt(2+) salt |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 23369 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = 65W79BFD5V | InChI = 1/Co.2NO3/c;2*2-1(3)4/q+2;2*-1 | SMILES = [Co+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O | InChIKey = UFMZWBIQTDUYBN-UHFFFAOYAS | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/Co.2NO3/c;2*2-1(3)4/q+2;2*-1 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = UFMZWBIQTDUYBN-UHFFFAOYSA-N | CASNo_Ref = {{cascite|correct|CAS}} | CASNo = 10141-05-6 | PubChem = 25000 | ChEBI_Ref = {{ebicite|changed|EBI}} | ChEBI = 86209 | EINECS = 233-402-1 | RTECS = GG1109000 |Section2={{Chembox Properties | Formula = Co(NO3)2 | MolarMass = 182.943 g/mol (anhydrous) 291.03 g/mol (hexahydrate) | Appearance = pale red powder (anhydrous) red crystalline (hexahydrate) | Odor = odorless (hexahydrate) | Density = 2.49 g/cm3 (anhydrous) 1.87 g/cm3 (hexahydrate) | Solubility = anhydrous:[1] 84.03 g/100 mL (0 °C) 334.9 g/100 mL (90 °C) soluble (anhydrous) | SolubleOther = soluble in alcohol, acetone, ethanol, ammonia (hexahydrate), methanol 2.1 g/100 mL | MeltingPtC = 100 | MeltingPt_notes = decomposes (anhydrous) 55 °C (hexahydrate) | BoilingPtC = 100 to 105 | BoilingPt_notes = decomposes (anhydrous){{citation needed|date=February 2017}} 74 °C, decomposes (hexahydrate) |Section3={{Chembox Structure | MolShape = | Coordination = monoclinic (hexahydrate) | CrystalStruct = | Dipole = |Section7={{Chembox Hazards | ExternalSDS = Cobalt (II) Nitrate MSDS | EUClass = Carc. Cat. 2 Muta. Cat. 3 Repr. Cat. 2 Toxic (T) Dangerous for the environment (N) | RPhrases = {{R49}}, {{R60}}, {{R42/43}}, {{R68}}, {{R50/53}} | SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}} | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = OX | LD50 = 434 mg/kg; rat, oral (anhydrous) 691 mg/kg; rat, oral (hexahydrate) |Section8={{Chembox Related | OtherAnions = Cobalt(II) sulfate Cobalt(II) chloride Cobalt oxalate | OtherCations = Iron(III) nitrate Nickel(II) nitrate | OtherCompounds = }}Cobalt Nitrate is the Inorganic compound with the formula Co(NO3)2.xH2O. It is cobalt(II) salt. The most common form is the hexahydrate Co(NO3)2·6H2O, which is a red-brown deliquescent salt that is soluble in water and other polar solvents.[2] Composition and structuresAs well as the anhydrous compound Co(NO3)2, several hydrates of cobalt(II) nitrate exist. These hydrates have the chemical formula Co(NO3)2·nH2O, where n = 0, 2, 4, 6. Anhydrous cobalt(II) nitrate adopts a three-dimensional polymeric network structure, with each cobalt(II) atom approximately octahedrally coordinated by six oxygen atoms, each from a different nitrate ion. Each nitrate ion coordinates to three cobalts.[3] The dihydrate is a two-dimensional polymer, with nitrate bridges between Co(II) centres and hydrogen bonding holding the layers together. The tetrahydrate consists of discrete, octahedral [(H2O)4Co(NO3)2] molecules. The hexahydrate is better described as hexaaquacobalt(II) nitrate, [Co(OH2)6][NO3]2, as it consists of discrete [Co(OH2)6]2+ and [NO3]− ions.[4] Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate.[2] UsesIt is commonly reduced to metallic high purity cobalt.[2] It can be absorbed on to various catalyst supports for use in Fischer-Tropsch catalysis.[5] It is used in the preparation of dyes and inks.[6] ProductionThe hexahydrate is prepared treating metallic cobalt or one of its oxides, hydroxides, or carbonate with nitric acid: Co + 4 HNO3 + 4 H2O → Co(H2O)6(NO3)2 + 2 NO2 CoO + 2 HNO3 + 5 H2O → Co(H2O)6(NO3)2 CoCO3 + 2 HNO3 + 5 H2O → Co(H2O)6(NO3)2 + CO2
References1. ^Perrys' Chem Eng Handbook, 7th Ed {{Cobalt compounds}}{{nitrates}}2. ^1 2 John Dallas Donaldson, Detmar Beyersmann, "Cobalt and Cobalt Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. {{DOI|10.1002/14356007.a07_281.pub2}} 3. ^{{ cite journal | first1 = G. A. | last1 = Tikhomirov | first2 = K. O. | last2 = Znamenkov | first3 = I. V. | last3 = Morozov | first4 = E. | last4 = Kemnitz | first5 = S. I. | last5 = Troyanov | journal = Z. anorg. allg. Chem. | year = 2002 | volume = 628 | issue = 1 | pages = 269–273 | title = Anhydrous Nitrates and Nitrosonium Nitratometallates of Manganese and Cobalt, M(NO3)2, NO[Mn(NO3)3], and (NO)2[Co(NO3)4]: Synthesis and Crystal Structure | doi = 10.1002/1521-3749(200201)628:1<269::AID-ZAAC269>3.0.CO;2-P }} 4. ^{{ cite journal | journal = Cryst. Struct. Commun. | first1 = P. V. | last1 = Prelesnik | first2 = F. | last2 = Gabela | first3 = B. | last3 = Ribar | first4 = I. | last4 = Krstanovic | volume = 2 | issue = 4 | year = 1973| pages = 581–583 | title = Hexaaquacobalt(II) nitrate}} 5. ^Ernst B, Libs S, Chaumette P, Kiennemann A. Appl. Catal. A 186 (1-2): 145-168 1999 6. ^Lewis, Richard J., Sr. (2002). Hawley's Condensed Chemical Dictionary (14th Edition). John Wiley & Sons. http://www.knovel.com/knovel2/Toc.jsp?BookID=704&VerticalID=0 3 : Cobalt compounds|Nitrates|Oxidizing agents |
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