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{{Chembox |
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| verifiedrevid = 404375994 |
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| ImageFile = Tetrakis(methylammonium)hexachloroferratechloride.svg |
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| ImageFile = Tetrakis(methylammonium)hexachloroferratechloride.svg |
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| IUPACName = Tetrakis (methylammonium) hexachloroferrate (III) chloride |
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| IUPACName = Tetrakis(methylammonium) hexachloroferrate(III) chloride |
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| OtherNames = |
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| OtherNames = |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo = 21995-64-2 |
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| CASNo = 21995-64-2 |
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| ChemSpiderID = 35763475 |
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| PubChem = |
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| PubChem = 71308279 |
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| SMILES = C.C.C.C..Cl(Cl)(Cl)(Cl)(Cl)Cl}} |
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| SMILES = C.C.C.C..Cl(Cl)(Cl)(Cl)(Cl)Cl |
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| Section2 = {{Chembox Properties |
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| StdInChI=1S/4CH5N.7ClH.Fe/c4*1-2;;;;;;;;/h4*2H2,1H3;7*1H;/q;;;;;;;;;;;+3/p-3 |
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| Formula = (CH<sub>6</sub>N)<sub>4</sub>Cl |
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| StdInChIKey = WWEONMZLNZBJCO-UHFFFAOYSA-K |
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| MolarMass = 432.3 g/mol |
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| Appearance = orange crystals |
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|Section2={{Chembox Properties |
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| Density = |
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| C = 4 | H = 24 | Cl = 7 | Fe = 1 | N = 4 |
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| Appearance = orange crystals |
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| Density = 1.58 g cm<sup>−3</sup><ref name=James/> |
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| MeltingPtC = 155 |
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| MeltingPtC = 155 |
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Tetrakis (methylammonium) hexachloroferrate (III) chlorideis a chemical compound with the formula (CH<sub>6</sub>N)<sub>4</sub>Cl |
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'''Tetrakis(methylammonium) hexachloroferrate(III) chloride''' is a chemical compound with the formula (CH<sub>3</sub>NH<sub>3</sub>)<sub>4</sub>Cl. |
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==Properties== |
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==Properties== |
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The compound has the form of orange crystals <ref> “Stabilzation of the Hexachlorferrate (III) Anion by the Methylammonium Cation”. Inorganic Chemistry vol 7, 2662</ref>. Six chlorines are coordinated to the central iron atom leading to octahedral geometry. Interstatial chlorine ions are surrounded by the electrostatically attracted positively charged methylammonium groups <ref>B. D. James, M. Bakalova, A. H. Whte “The hexachloroferrate(III) anion stabilized in hydrogen bonded packing arrangements. A comparison of the X-ray crystal structures and low temperature magnetism of tetrakis (methylammonium) hexachloroferrate (III) chloride (I) and tetrakis (hexamethylenediammonium)hexachloroferrate (III) tetrachloroferrate (III) tetrachloride (II)” Inorganica Chimnica Acta 247 169-174</ref>. The NH3 groups are bonded to the 3- . The iron within the molecule is in the three coordinate state. |
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The compound has the form of ] orange crystals.<ref name=Clausen>{{cite journal |last1=Clausen |first1=C. A. |last2=Good |first2=M. L. |year=1968 |title=Stabilization of the hexachloroferrate(III) anion by the methylammonium cation |journal=] |volume=7 |issue=12 |pages=2662–2663 |doi=10.1021/ic50070a047}}</ref> The hexachloroferrate(III) anion is a ] centred on an iron atom in the +3 ] that is ] to six chloride atoms arranged ] around it. ] chloride anions are each surrounded by four methylammonium cations, with ]-like links between the ammonium cations and the ]s of the hexachloroferrate(III) ].<ref name=James>{{cite journal |last1=James |first1=B. D. |first2=M. |last2=Bakalova |first3=J. |last3=Lieseganga |first4=W. M. |last4=Reiff |first5=D. C. R. |last5=Hockless |first6=B. W. |last6=Skelton |first7=A. H. |last7=White |year=1996 |title=The hexachloroferrate(III) anion stabilized in hydrogen bonded packing arrangements. A comparison of the X-ray crystal structures and low temperature magnetism of tetrakis(methylammonium) hexachloroferrate(III) chloride ('''I''') and tetrakis(hexamethylenediammonium) hexachloroferrate(III) tetrachloroferrate(III) tetrachloride ('''II''') |journal=] |volume=247 |issue=2 |pages=169–174 |doi=10.1016/0020-1693(95)04955-X}}</ref> Each <sup>3+</sup> unit balances a <sup>3–</sup>, analogous to how hexachloroferrate(III) forms stable compounds with various large triply-cationic atoms<ref name=James/> and other triply-cationic complexes.<ref name=Clausen/> |
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The molecular weight is 432.3 g/mol. The density of this compound is 1.58 g/cm3 . Crystal dimensions are.25 x .35 x .16 mm. The melting point is 155 oC. The 3- acts as a lewis acid, while the ammonium group acts as a Lewis base. It is a hydroscopic compound . |
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==Synthesis== |
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==Synthesis== |
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The compound is synthesised by reacting ], CH<sub>3</sub>NH<sub>3</sub>Cl, with anhydrous ] and adding ] with heating. Crystals of the product, which precipitate as the solvent evaporates, are collected and dried using vacuum ].<ref name=Clausen/> |
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To synthesize 13.3 g of compound |
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==Infrared analysis== |
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Add 9.94g methyl ammonium chloride, 5.04g anhydrous iron chloride into a 400 mL beaker. Add 68 mL of HCl. Heat on a low setting 2/10 on a hot plate for 3 hours. The crystals will precipitate after enough solvent has vaporized. To dry product use vacuum filtration using a Buchner funnel, a water aspirator, and fine porosity filter paper. Dry the product overnight in a vacuum dessicator . |
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There is a series of bands from 3129 to 2830 cm<sup>−1</sup> that represent stretching modes of the nitrogen–hydrogen bonds. In addition, a distinct peak is found at 2517 cm<sup>−1</sup>, whereas the corresponding signal for methylammonium chloride is at 2476 cm<sup>−1</sup>.<ref name=James/><ref>"methyl ammonium chloride" http://riodb01.ibase.aist.go.jp/sdbs/cgi-bin/direct_frame_top.cgi</ref> The 31 cm<sup>−1</sup> shift is due to the coordination of an ammonium hydrogen with the hexachloroferrate(III). |
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==CAS Registry Number == |
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21995-64-2 |
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==Infrared Analysis== |
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There is a series of nitrogen hydrogen amine stretching from 3129-2830 cm-1. In addition a distinct peak is found at 2517 cm-1 which corresponds well with the peak at 2476 cm-1 for methylammonium chloride and the literature estimate of a peak present near 2500 cm-1 <ref>"methyl ammonium chloride" http://riodb01.ibase.aist.go.jp/sdbs/cgi-bin/direct_frame_top.cgi</ref>,. The 31 cm-1 shift indicates changes in the methylammonium chloride due to coordination with chlorine in the product crystals. |
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==Notes== |
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==Notes== |
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{{Reflist}} |
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{{Reflist}} |
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==References== |
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1. “Stabilzation of the Hexachlorferrate (III) Anion by the Methylammonium Cation”. Inorganic Chemistry vol 7, 2662 |
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2. B. D. James, M. Bakalova, A. H. Whte “The hexachloroferrate(III) anion stabilized in hydrogen bonded packing arrangements. A comparison of the X-ray crystal structures and low temperature magnetism of tetrakis (methylammonium) hexachloroferrate (III) chloride (I) and tetrakis (hexamethylenediammonium)hexachloroferrate (III) tetrachloroferrate (III) tetrachloride (II)” Inorganica Chimnica Acta 247 169-174 |
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3. "methyl ammonium chloride" http://riodb01.ibase.aist.go.jp/sdbs/cgi-bin/direct_frame_top.cgi |
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] |
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