| 词条 | Ferric oxalate |
| 释义 |
| Name = | ImageFile = Ferric oxalate.svg | IUPACName = | SystematicName = iron(3+) ethanedioate (2:3) | OtherNames = Iron(III) oxalate |Section1={{Chembox Identifiers | Abbreviations = | CASNo = 2944-66-3 | CASNo_Comment = (Anhydrous) | CASNo1 = 166897-40-1 | CASNo1_Comment = (hexahydrate) | EINECS = 220-951-7 | PubChem = 168963 | ChemSpiderID = 147789 | SMILES = [Fe+3].[Fe+3].O=C([O-])C([O-])=O.[O-]C(=O)C([O-])=O.[O-]C(=O)C([O-])=O | InChI = InChI=1S/3C2H2O4.2Fe/c3*3-1(4)2(5)6;;/h3*(H,3,4)(H,5,6);;/q;;;2*+3/p-6 | RTECS = | MeSHName = | ChEBI = | KEGG = }} |Section2={{Chembox Properties | Formula = C6Fe2O12 | MolarMass = 375.747 g/mol | Appearance = Pale yellow solid (anhydrous) Lime green solid (hexahydrate) | Odor = odorless | Density = | MeltingPt = | MeltingPt_notes = | BoilingPt = | BoilingPt_notes = | Solubility = slightly soluble | SolubleOther = | Solvent = | LogP = | VaporPressure = | HenryConstant = | AtmosphericOHRateConstant = | pKa = | pKb = |Section3={{Chembox Structure | CrystalStruct = | Coordination = | MolShape = |Section4={{Chembox Thermochemistry | DeltaHf = | DeltaHc = | Entropy = | HeatCapacity = |Section5={{Chembox Pharmacology | AdminRoutes = | Bioavail = | Metabolism = | HalfLife = | ProteinBound = | Excretion = | Legal_status = | Legal_US = | Legal_UK = | Legal_AU = | Legal_CA = | Pregnancy_category = | Pregnancy_AU = | Pregnancy_US = |Section6={{Chembox Explosive | ShockSens = | FrictionSens = | DetonationV = | REFactor = |Section7={{Chembox Hazards | ExternalSDS = | EUClass = | MainHazards = | NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S = | RPhrases = | SPhrases = | RSPhrases = | FlashPt = | AutoignitionPt = | ExploLimits = | LD50 = | PEL = |Section8={{Chembox Related | OtherAnions = | OtherCations = | OtherFunction = | OtherFunction_label = | OtherCompounds = }} Ferric oxalate, also known as iron(III) oxalate, is a chemical compound composed of ferric ions and oxalate ligands; it may also be regarded as the ferric salt of oxalic acid. The anhydrous material is pale yellow; however, it may be hydrated to form several hydrates, such as {{chem|Fe|2|(|C|2|O|4|)|3}}{{hydrate|6}} which is bright green in colour StructureTetrahydrateThe crystal structure of the tetrahydrate {{chem|Fe|2|(|C|2|O|4|)|3}}{{hydrate|4|nolink=yes}} was determined in 2015. It has a triclinic unit cell containing two iron atoms. Each iron atom has octahedral coordination bonds to the oxygen atoms of three oxalate molecules and one water molecule. Two of those three oxalates, lying in approximately perpendicular planes, are tetradentate, and connect the iron atoms into zigzag chains. The third oxalate molecule is bidentate, and connects iron atoms of adjacent chains, creating an open-layered structure. Half of the water molecules lie, unbound, between those chains. Mössbauer spectrum of {{chem|Fe|2|(|C|2|O|4|)|3}}{{hydrate|4|nolink=yes}} indicates that iron is present in a unique environment with an isomer shift of 0.38 mm/s and a quadrupole splitting of 0.40 mm/s, suggesting a high spin {{chem2|Fe(3+)}} in octahedral coordination.[1] UsesDentistryLike many oxalates, ferric oxalate has been investigated as a short term treatment for dentin hypersensitivity.[2] It is used in certain toothpaste formulations; however, its effectiveness has been questioned.[3] PhotographyFerric oxalate is used as the light-sensitive element in the Kallitype photographic printing process; and the platinotype process Platinum/Palladium Printing. BatteriesFerric oxalate tetrahydrate has been investigated as a possible cheap material for the positive electrode of lithium-iron batteries. It can intercalate lithium ions at an average potential of 3.35 V, and has shown a sustainable capacity of 98 mAh/g.[1] See alsoA number of other iron oxalates are known:-
References1. ^1 Hania Ahouari, Gwenaëlle Rousse, Juan Rodríguez-Carvajal, Moulay-Tahar Sougrati, Matthieu Saubanère, Matthieu Courty, Nadir Recham, and Jean-Marie Tarascon (2015): "Unraveling the Structure of Iron(III) Oxalate Tetrahydrate and Its Reversible Li Insertion Capability". Chemistry of Materials, volume 27, issue 5, pages 1631–1639. {{doi|10.1021/cm5043149}} {{iron compounds}}{{Oxalates}}2. ^{{cite journal|last1=Gillam|first1=D. G.|last2=Newman|first2=H. N.|last3=Davies|first3=E. H.|last4=Bulman|first4=J. S.|last5=Troullos|first5=E. S.|last6=Curro|first6=F. A.|title=Clinical evaluation of ferric oxalate in relieving dentine hypersensitivity|journal=Journal of Oral Rehabilitation|volume=31|issue=3|pages=245–250|doi=10.1046/j.0305-182X.2003.01230.x}} 3. ^{{cite journal|last1=Cunha-Cruz|first1=J.|last2=Stout|first2=J. R.|last3=Heaton|first3=L. J.|last4=Wataha|first4=J. C.|title=Dentin Hypersensitivity and Oxalates: a Systematic Review|journal=Journal of Dental Research|date=29 December 2010|volume=90|issue=3|pages=304–310|doi=10.1177/0022034510389179|pmc=3144108}} 2 : Iron(Ⅲ) compounds|Oxalates |
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