| 词条 | Iron(II) oxalate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 409714131 | ImageFile1 = Iron(II)-oxalate-sample.jpg | ImageFile2 = Fe(C2O4)-2D-ionic.png | IUPACName = Iron(II) oxalate | OtherNames = Iron oxalate Ferrous oxalate |Section1={{Chembox Identifiers | CASNo1_Ref = {{cascite|changed|??}} | CASNo1 = 516-03-0 | CASNo2_Ref = {{cascite|changed|??}} | CASNo2 = 6047-25-2 | CASNo2_Comment = (dihydrate) | PubChem =10589 | EINECS = 208-217-4 | SMILES = [Fe+2].O=C([O-])-C([O-])=O | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/3C2H2O4.2Fe/c3*3-1(4)2(5)6;;/h3*(H,3,4)(H,5,6);;/q;;;2*+3/p-6 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = VEPSWGHMGZQCIN-UHFFFAOYSA-H }} |Section2={{Chembox Properties | Formula = FeC2O4 (anhydrous) FeC2O4{{hydrate|2}} (dihydrate) | MolarMass = 143.86 g/mol (anhydrous) 179.89 g/mol (dihydrate) | Appearance = yellow powder | Odor = odorless | Density = 2.28 g/cm3 | MeltingPtC = 190 | MeltingPt_notes = (anhydrous)[1] {{convert|150-160|C|F K}} (dihydrate) decomposes | BoilingPtC = 365.1 | BoilingPt_notes = (anhydrous)[1] | Solubility = dihydrate: 0.097 g/100ml (25 °C)[2] }} |Section3={{Chembox Hazards | GHSPictograms = {{GHSp|GHS07}}[3] | GHSSignalWord = Warning | HPhrases = {{H-phrases|302|312}}[3] | PPhrases = {{P-phrases|280}}[3] | MainHazards = | FlashPtC = 188.8 | AutoignitionPt = }} Ferrous oxalate, or iron(II) oxalate, is a inorganic compound with the formula FeC2O4{{hydrate|{{mvar|x}}}} where {{mvar|x}} is typically 2. These are orange compounds, poorly soluble in water. StructureThe dihydrate FeC2O4{{hydrate|2}} is a coordination polymer, consisting of chains of oxalate-bridged ferrous centers, each with two aquo ligands.[4] When heated, it dehydrates and decomposes into a mixture of iron oxides and fun iron metal, with release of carbon dioxide, carbon monoxide, and water.[5] See alsoA number of other iron oxalates are known
References1. ^1 http://www.guidechem.com/cas-516/516-03-0.html {{Iron compounds}}{{Oxalates}}2. ^http://chemister.ru/Database/properties-en.php?dbid=1&id=2084 3. ^1 2 {{Sigma-Aldrich|id=255971|name=Iron(II) oxalate dihydrate|accessdate=2014-05-03}} 4. ^{{ cite journal |first1= Takuya |last1= Echigo |first2= Mitsuyoshi |last2= Kimata |title= Single-crystal X-ray diffraction and spectroscopic studies on humboldtine and lindbergite: weak Jahn–Teller effect of Fe2+ ion |journal= Phys. Chem. Minerals |year= 2008 |volume= 35 |pages= 467–475 |doi= 10.1007/s00269-008-0241-7 }} 5. ^{{cite journal |title= Thermal behaviour of iron(II) oxalate dihydrate in the atmosphere of its conversion gases |first1= Martin |last1=Hermanek |first2=Radek |last2=Zboril |first3=Miroslav |last3=Mashlan |first4=Libor |last4=Machala |first5=Oldrich |last5=Schneeweiss |display-authors= 3 |journal= J. Mater. Chem. |date= 2006 |volume= 16 |pages= 1273–1280}} 2 : Iron(Ⅱ) compounds|Oxalates |
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