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{{Short description|Anion in which a Fe<sup>3+</sup> ion is complexed by 6 CN<sup>−</sup> ions}} |
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{{distinguish|ferrocyanide}} |
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{{Chembox |
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{{Chembox |
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|Watchedfields = changed |
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| verifiedrevid = 407813661 |
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|verifiedrevid = 444964110 |
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| ImageFile = HexacyanidoferratIII_2.svg |
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|ImageFile = HexacyanidoferratIII_2.svg |
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| ImageSize = 175 |
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| ImageFile1 = Ferricyanide-3D.png |
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|ImageSize = 175 |
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|ImageFile1 = Ferricyanide-3D.png |
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| ImageSize1 = 240 |
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|ImageSize1 = 240 |
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|IUPACName = iron(3+) hexacyanide |
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| ImageAlt1 = |
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|SystematicName = hexacyanidoferrate(III) |
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| ImageName1 = |
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|OtherNames =ferric hexacyanide; hexacyanidoferrate(3−); hexacyanoferrate(III) |
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| IUPACName = iron(3+) hexacyanide |
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|Section1 = {{Chembox Identifiers |
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| SystematicName = hexacyanidoferrate(III) |
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|CASNo_Ref = {{cascite|correct|CAS}} |
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| OtherNames =ferric hexacyanide; hexacyanidoferrate(3-); hexacyanoferrate(III) |
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|CASNo = 13408-62-3 |
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| Section1 = {{Chembox Identifiers |
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| CASNo = |
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|ChEBI = 5020 |
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| PubChem = 439210 |
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|KEGG = C00324 |
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|PubChem = 439210 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = |
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|ChemSpiderID = 388349 |
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| SMILES =#N.#N.#N.#N.#N.#N. |
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|SMILES = N#C(C#N)(C#N)(C#N)(C#N)C#N |
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| InChI = |
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|StdInChI=1S/6CN.Fe/c6*1-2;/q6*-1;+3 |
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}} |
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|StdInChIKey = YAGKRVSRTSUGEY-UHFFFAOYSA-N |
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}} |
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|Section2 = {{Chembox Properties |
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|Formula = <sup>3−</sup> |
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}} |
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|Section8 = {{Chembox Related |
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|OtherCompounds=] |
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|OtherCations=] |
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}} |
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}} |
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}} |
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'''Ferricyanide''' is the ] <sup>3−</sup>. Its ] is '''hexacyanidoferrate(III)''', in older nomenclature '''hexacyanoferrate(III)'''. The most common salt of this anion is ], a red crystalline material that is used as an oxidant in ]. |
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'''Ferricyanide''' is the ] <sup>3−</sup>. It is also called '''hexacyanoferrate(III)''' and in rare, but ], hexacyanidoferrate(III). The most common salt of this anion is ], a red crystalline material that is used as an ] in ].<ref name=Ullmann>{{Ullmann |author1=Gail, E. |author2=Gos, S. |author3=Kulzer, R. |author4=Lorösch, J. |author5=Rubo, A. |author6=Sauer, M. |author7=Kellens, R. |author8=Reddy, J. |author9=Steier, N. |author10=Hasenpusch, W. | title = Cyano Compounds, Inorganic |date=October 2011 | doi = 10.1002/14356007.a08_159.pub3 }}</ref> |
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== Properties == |
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== Properties == |
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<sup>3−</sup> consists of a Fe<sup>3+</sup> center bound in ] to six ] ]s. The complex has O<sub>h</sub> ]. The iron is ] and easily reduced to the related ] ion <sup>4−</sup>, which is a ferrous (Fe<sup>2+</sup>) derivative. This redox couple is reversible and entails no making or breaking of Fe–C bonds: |
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:<sup>3−</sup> + e<sup>−</sup> ⇌ <sup>4−</sup> |
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This ] is a standard in ]. |
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Compared to main group ]s like ], ferricyanides are much less toxic because of the strong bond between the cyanide ion (CN<sup>−</sup>) and the Fe<sup>3+</sup>. They do react with mineral acids, however, to release highly toxic ] gas. |
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<sup>3−</sup> consists of an Fe<sup>3+</sup> center bound in ] to six ] ]s. The complex has O<sub>h</sub> ]. |
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The iron is ] and easily reduced to the related ] ion <sup>4−</sup>, which is a ferrous (Fe<sup>2+</sup>) derivative. This redox couple is reversible and entails no making or breaking of Fe-C bonds: |
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:<sup>3−</sup> + e<sup>−</sup> → <sup>4−</sup> |
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This couple is a standard in ]. |
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Compared to normal ]s like ], ferricyanides are much less toxic because of the tight hold of the CN<sup>-</sup> to the Fe<sup>3+</sup>. They do react with mineral acids, however, to release highly toxic ] gas. |
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== Uses == |
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== Uses == |
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Treatment of ferricyanide with iron(II) salts affords the brilliant, long-lasting pigment ], the traditional color of ]. |
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Treatment of ferricyanide with ferrous salts affords the brilliant, long-lasting pigment ], the traditional color of ]. |
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==See also== |
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==See also== |
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==References== |
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{{Reflist}} |
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{{Cyanides}} |
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