| 词条 | Cobalt(II) cyanide |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 430345231 | Name = Cobalt(II) cyanide | ImageFile = | ImageName = | IUPACName = Cobalt(II) cyanide | OtherNames = cobaltous cyanide |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 61631 | InChI = 1/2CN.Co/c2*1-2;/q2*-1;+2 | SMILES = [Co+2].[C-]#N.[C-]#N | InChIKey = CWZOMTYLSNXUEL-UHFFFAOYAR | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/2CN.Co/c2*1-2;/q2*-1;+2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = CWZOMTYLSNXUEL-UHFFFAOYSA-N | CASNo = 542-84-7 | CASNo_Ref = {{cascite|correct|??}} | CASNo2_Ref = {{cascite|changed|??}} | CASNo2 = 20427-11-6 | CASNo2_Comment = (dihydrate) | CASNo3_Ref = {{cascite|changed|??}} | CASNo3 = 26292-31-9 | CASNo3_Comment = (trihydrate) | PubChem = 68336 | RTECS = |Section2={{Chembox Properties | Formula = Co(CN)2 | MolarMass = 110.968 g/mol (anhydrous) 147.00 g/mol (dihydrate) 165.02 g/mol (trihydrate) | Appearance = deep-blue powder hygroscopic (anhydrous) reddish-brown powder (dihydrate) | Density = 1.872 g/cm3 (anhydrous) | Solubility = insoluble[1] | SolubleOther = dihydrate degraded with dissolution by NaCN, KCN, NH4OH, HCl | MeltingPtC = 280 | MeltingPt_notes = (anhydrous) | BoilingPt = | MagSus = +3825·10−6 cm3/mol |Section3={{Chembox Structure | Coordination = | CrystalStruct = |Section7={{Chembox Hazards | ExternalSDS = | EUClass = | RPhrases = | SPhrases = |Section8={{Chembox Related | OtherAnions = Cadmium chloride, Cadmium iodide | OtherCations = Zinc cyanide, Calcium cyanide, Magnesium cyanide }} Cobalt(II) cyanide is the inorganic compound with the formula Co(CN)2. It is coordination polymer that has attracted intermittent attention over many years in the area of inorganic synthesis and homogeneous catalysis. UsesCobalt(II) cyanide has been used as a precursor to cobalt carbonyl.[2] PreparationThe trihydrate salt is obtained as a reddish-brown precipitate by adding potassium cyanide to a cobalt salt solution.:[3] CoCl2(H2O)6 + 2 KCN → Co(CN)2 + 2 KCl + 6 H2O Hydrated Co(CN)2 dissolves in the presence of excess potassium cyanide, forming a red solution of K4Co(CN)6. This material further oxidizes to yellow K3Co(CN)6. References1. ^{{RubberBible87th}} {{Cobalt compounds}}{{Cyanides}}{{inorganic-compound-stub}}2. ^Heinz W. Sternberg, Irving Wender, Milton Orchin Cobalt Tetracarbonyl Hydride: (Cobalt Hydrocarbonyl) Inorganic Syntheses, 1957, vol. V, p. 192. {{DOI|10.1002/9780470132364.ch55}} 3. ^John H. Bigelow, "Potassium Hexacyanocobaltate(III)" Inorganic Syntheses, 1946, Volume I1, p. 225. 2 : Cobalt compounds|Cyanides |
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