| 词条 | Manganese(II) acetate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 486589107 | Name = Manganese(II) acetate | ImageFile = Manganese acetate.png | ImageSize = | ImageName = | IUPACName = Manganese(II) acetate | OtherNames = Manganese diacetate | Reference = [1] |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|CAS}} | CASNo = 638-38-0 | CASNo_Comment = (anhydrous) | CASNo2_Ref = {{cascite|changed|??}} | CASNo2 = 19513-05-4 | CASNo2_Comment = (dihydrate) | CASNo3_Ref = {{cascite|changed|??}} | CASNo3 = 6156-78-1 | CASNo3_Comment = (tetrahydrate) | SMILES = CC([O-])=O.CC([O-])=O.[Mn+2] | RTECS = | EINECS = | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 12008 | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/2C2H4O2.Mn/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = UOGMEBQRZBEZQT-UHFFFAOYSA-L | PubChem = 12525 |Section2={{Chembox Properties | Formula = Mn(CH3CO2)2 (anhydrous) Mn(CH3CO2)2·4H2O (tetrahydrate) | MolarMass = 173.027 g/mol (anhydrous) 245.087 g/mol (tetrahydrate) | Appearance = white crystals (anhydrous) light pink monoclinic crystals (tetrahydrate) | Density = 1.74 g/cm3 (anhydrous) 1.59 g/cm3 (tetrahydrate) | MeltingPtC = 210 | MeltingPt_notes = (anhydrous) 80 °C (tetrahydrate) | BoilingPt = | SolubleOther = soluble in water, methanol, acetic acid (anhydrous) soluble in water, ethanol (tetrahydrate) | MagSus = +13,650·10−6 cm3/mol |Section3={{Chembox Structure | Coordination = | CrystalStruct = |Section7={{Chembox Hazards | ExternalSDS = | NFPA-H = 1 | NFPA-F = 0 | NFPA-R = 0 | RPhrases = | SPhrases = | FlashPt = > | FlashPtC = 130 | FlashPt_notes = (tetrahydrate) | LD50 = 2940 mg/kg (rat, oral)[2] |Section8={{Chembox Related | OtherAnions = Manganese(II) fluoride Manganese(II) chloride Manganese(II) bromide | OtherCations = Zinc acetate Mercury(II) acetate Silver acetate }}Manganese(II) acetate are chemical compounds with the formula Mn(CH3CO2)2.(H2O)n where n = 0, 2, 4.. It is used as a catalyst and as fertilizer.[3] ReactionsManganese(II) acetate can be formed by treating either manganese(II,III) oxide or manganese(II) carbonate with acetic acid:[4] MnCO3 + 2 CH3CO2H → Mn(CH3CO2)2 + CO2 + H2O StructureThe anhydrous material and dihydrate Mn(CH3CO2)2.2H2O are coordination polymers. The dihydrate has been characterized by X-ray crystallography. Each Mn(II) center is surrounded by six oxygen centers provided by aquo ligands and acetates. References1. ^{{Citation| last = Lide| first = David R.| author-link = | last2 = | first2 = | author2-link =| publication-date =| date =| year = 1998| title = Handbook of Chemistry and Physics| edition = 87| volume = | series =| publication-place = Boca Raton, FL| place = | publisher = CRC Press| id =| isbn = 0-8493-0594-2| doi =| oclc =| pages = 3–354, 4–68| url = | accessdate =}} {{clear}}{{Acetates}}{{manganese compounds}}{{DEFAULTSORT:Manganese(Ii) Acetate}}2. ^{{IDLH|7439965|Manganese compounds (as Mn)}} 3. ^{{Citation| title = Concise encyclopedia chemistry| author = Thomas Scott| author2 = Mary Eagleson| publisher = Walter de Gruyter| year = 1994| isbn = 3-11-011451-8| page = 620| url = https://books.google.com/books?id=Owuv-c9L_IMC&pg=PA620&dq=%22Manganese%28II%29+acetate%22| accessdate = 2009-07-20}} 4. ^{{cite encyclopedia|authors=Arno H. Reidies|title=Manganese Compounds|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|year=2002|publisher=Wiley-VCH|place= Weinheim|doi=10.1002/14356007.a16_123}} 5. ^{{cite journal|authors=Chih-Yi Cheng, Sue-Lein Wang|title=Structure of manganese acetate dihydrate|journal=Acta Crystallographica Section C|page=1734|doi=10.1107/S0108270191002202|year=1991|volume=47}} 2 : Manganese compounds|Acetates |
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