Iron(III) acetate
| Iron(III) acetate[1] | |
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iron(III) acetate |
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Other names
basic iron(III) acetate , iron(III) oxyacetate, iron(III) Acetate |
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| Identifiers | |
| CAS number | 1834-30-6 |
| PubChem | 164887 |
| ChemSpider | 144555 |
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| Properties | |
| Molecular formula | C14H27Fe3O18 |
| Molar mass | 233 g/mol |
| Appearance | brownish-red amorphous powder |
| Solubility in water | insoluble[citation needed] |
| Solubility | soluble in ethanol |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
| Infobox references | |
Ferric acetate is the coordination compound more commonly known as "basic iron acetate". With the formula [Fe3O(OAc)6(H2O)3]OAc (OAc is CH3CO2-), it is a salt, composed of the cation [Fe3(μ3-O)(OAc)6(H2O)3]+ and an acetate anion.[2] The formation of the red-brown complex has long been used as a test for ferric ions.[3]
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[edit] Structure and synthesis
Basic iron acetate forms on treating aqueous solutions of iron(III) sources with acetate salts.[4]
Early work showed that it is trinuclear.[5] The Fe centres are equivalent, each being octahedral, being bound to six oxygen ligands, including a triply bridging oxide at the center of the equilateral triangle.[6] The compound was an early example of a molecular compound of iron that features an oxide ligand. Ignoring its 24 hydrogen centres, the cation has D3h symmetry.
[edit] Reactions
The terminal aqua ligands on the trimetallic framework can be substituted with other ligands, such as pyridine and dimethylformamide. Many different salts are known by exchanging the anion, e.g. [Fe3(μ3-O)(OAc)6(H2O)3]Cl. Reduction of the cation affords the neutral mixed-valence derivative that contains one ferrous and two ferric centers.[2] Mixed metal species are known such as [Fe2CoO(OAc)6(H2O)3].[7]
[edit] Related compounds
Chromium(III), ruthenium(III), vanadium(III), and rhodium(III) form analogous compounds.[8] Iron(III) acetate (lacking the oxo ligand) has been claimed as a red coloured compound from the reaction of silver acetate and iron(III) chloride.[9]
[edit] Uses
Materials prepared by heating iron, acetic acid, and air, loosely described as basic iron acetates, are used as dyes and mordants.[2]
[edit] References
- ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–63. ISBN 0849305942.
- ^ a b c J. Burgess, M. V. Twigg "Iron: Inorganic & Coordination Chemistry" Encyclopedia of Inorganic Chemistry, R. Bruce King, Editor, J. Wiley, ISBN 978-0-470-86078-6
- ^ H. Brearley, F. Ibbotson "The Analysis of Steel-Works Materials," 1902, Longmans, Green, &Co.: London.
- ^ Manual of Chemistry , W. Simon , p.474 google books link
- ^ R. Weinland and E. Gussmann, "Über Salze einer Hexaacetato(formiato)-trichrombase. II" Berichte der Deutschen Chemischen Gesellschaft 1909, volume 42, 2997-3018). doi:10.1002/cber.19090420318.
- ^ Figgis, B. N.; Robertson, G. B. “Crystal-Molecular Structure and Magnetic Properties of Cr3(CH3.COO)6OCl.5H2O” Nature 1965, volume 205, pages 694-5. doi:10.1038/205694a0. This paper describes the isostructure chromium and iron compounds.
- ^ Blake, A. B. Yavari, A.; Hatfield, W. E.; Sethulekshmi, C. N. “Magnetic and Spectroscopic Properties of Some Heterotrinuclear Basic Acetates of Chromium(III), Iron(III), and Divalent Metal Ions” Journal of the Chemical Society, Dalton Transactions, 1985, pp. 2509-2520. doi:10.1039/DT9850002509.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Ram C. Paul, Ramesh C. Narula and Sham K. Vasisht "Iron(III) acetates" Transition Metal Chemistry, 1978, Volume 3, pp.35-38. doi:10.1007/BF01393501.
