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Revision as of 18:32, 13 December 2010 editCheMoBot (talk | contribs)Bots141,565 edits Updating {{chembox}} (no changed fields - added verified revid - updated 'ChemSpiderID_Ref', 'StdInChI_Ref', 'StdInChIKey_Ref') per Chem/Drugbox validation (report [[Wikipedia_talk:WikiProject_Ch← Previous edit		Latest revision as of 03:58, 18 December 2024 edit undo99.177.90.225 (talk) Updated SMILES code to the correct one
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	{{chembox		{{chembox
			| Verifiedfields = changed
⚫	| verifiedrevid = 402180875
			| Watchedfields = changed
⚫	| Name = Iron(III) nitrate
		⚫	| verifiedrevid = 402182963
⚫	| ImageFile = Ferric nitrate nonahydrate.jpg
		⚫	| Name = Iron(III) nitrate
	<!-- | ImageSize = 200px -->
			| ImageFile1 = (Fe(aq)6)(NO3)3.svg
⚫	| ImageName = Iron(III) nitrate nonahydrate
			| ImageName1 =
⚫	| IUPACName = Iron(III) nitrate
			| ImageCaption1 = Chemical structure of ferric nitrate aquo complex
⚫	| OtherNames = Ferric nitrate<br/>Nitric acid, iron(3+) salt
		⚫	| ImageFile2 = Ferric nitrate nonahydrate.jpg
⚫	| Section1 = {{Chembox Identifiers
		⚫	| ImageName2 = Iron(III) nitrate nonahydrate
⚫	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
			| ImageCaption2 = Sample of ferric nitrate nonahydrate
		⚫	| IUPACName = Iron(III) nitrate
		⚫	| OtherNames = Ferric nitrate<br/>Nitric acid, iron(3+) salt
		⚫	|Section1={{Chembox Identifiers
		⚫	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 10670706		| ChemSpiderID = 10670706
	| UNII_Ref = {{fdacite|correct|FDA}}		| UNII_Ref = {{fdacite|correct|FDA}}
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	| InChI = 1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;		| InChI = 1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;
	| InChIKey = SZQUEWJRBJDHSM-UHFFFAOYAC		| InChIKey = SZQUEWJRBJDHSM-UHFFFAOYAC
	| SMILES = .O.O.O.O.O.O.O.O.O.O=().()=O.()=O		| SMILES = (=O)().(=O)().(=O)().
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;		| StdInChI = 1S/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = SZQUEWJRBJDHSM-UHFFFAOYSA-N		| StdInChIKey = SZQUEWJRBJDHSM-UHFFFAOYSA-N
	| CASNo = 10421-48-4		| CASNo = 10421-48-4
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
			| CASNo1_Ref = {{cascite|correct|CAS}}
	| CASOther = <br>13476-08-9 (hexahydrate)<br/>7782-61-8 (nonahydrate)
	| PubChem = 16211566		| CASNo1 = 7782-61-8
			| CASNo1_Comment = (nonahydrate)
⚫	| RTECS = NO7175000
			| PubChem = 25251
		⚫	| RTECS = NO7175000
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
	| Formula = Fe(NO<sub>3</sub>)<sub>3</sub>		| Formula = Fe(NO<sub>3</sub>)<sub>3</sub>
	| MolarMass = 241.86 g/mol (anhydrous) <br> 403.999 g/mol (nonahydrate)		| MolarMass = 403.999 g/mol (nonahydrate) <br/> 241.86 g/mol (anhydrous)
	| Appearance = Pale violet crystals <br> ]		| Appearance = Pale violet crystals <br/> ]
	| Density = 1.68 g/cm<sup>3</sup> (nonahydrate)		| Density = 1.68 g/cm<sup>3</sup> (hexahydrate) <br/> 1.6429 g/cm<sup>3</sup>(nonahydrate)
	| Solubility = very soluble		| Solubility = 150 g/100 mL (hexahydrate)
	| SolubleOther = soluble		| SolubleOther = soluble in ], ]
			| MeltingPtC = 47.2
	| Solvent = alcohol, acetone
	| MeltingPt = 47.2 °C (nonahydrate)<br/>125 °C (decomp.)		| MeltingPt_notes = (nonahydrate)
			| BoilingPtC = 125
			| BoilingPt_notes = (nonahydrate)
			| MagSus = +15,200.0·10<sup>−6</sup> cm<sup>3</sup>/mol
	}}		}}
	| Section3 = {{Chembox Structure		|Section3={{Chembox Structure
	| Coordination = octahedral		| Coordination = octahedral
	}}		}}
	| Section7 = {{Chembox Hazards		|Section7={{Chembox Hazards
	| Reference = <ref>{{GHS class NZ|id=1777|accessdate=2010-09-19}}.</ref>		| Hazards_ref = <ref>{{GHS class NZ|id=1777|access-date=2010-09-19}}.</ref>
			| ExternalSDS =
	| ExternalMSDS =
			| GHSPictograms = {{GHS03|Ox. sol. 3}}{{GHS07|Acute tox. 4 (oral); Eye irrit. 1}}<ref name=sds>{{cite web |title=Iron(III) Nitrate Nonahydrate |url=https://www.americanelements.com/iron-iii-nitrate-nonahydrate-7782-61-8 |publisher = ] |access-date = June 20, 2019}}</ref>
	| EUIndex = not listed
		⚫	| GHSSignalWord = WARNING
	| GHSPictograms = {{GHS03|Ox. sol. 3}}{{GHS07|Acute tox. 4 (oral); Eye irrit. 1}}
			| HPhrases = {{H-phrases|272|302|319}}
⚫	| GHSSignalWord = WARNING
	| HPhrases = {{H-phrases|272|302|319}}		| PPhrases = {{P-phrases|210|220|221|264|270|280|301+312|305+351+338|330|337+313|370+378|501}}
		⚫	| NFPA-H = 1
	| PPhrases = {{P-phrases|210|220|221|264|270|280|301+312|305+351+338|330|337+313|370+378|501}}
	| NFPA-H = 1		| NFPA-R = 0
	| NFPA-R = 0		| NFPA-F = 0
	| NFPA-F = 0		| NFPA-S = OX
		⚫	| FlashPt = non-flammable
⚫	| NFPA-O = OX
			| REL = TWA 1 mg/m<sup>3</sup><ref>{{PGCH|0346}}</ref>
⚫	| FlashPt = non-flammable
	}}		}}
	| Section8 = {{Chembox Related		|Section8={{Chembox Related
	| OtherCpds = ]<br/>]		| OtherAnions = ]<br/>]
			| OtherCompounds = ]
	}}		}}
	}}		}}
	'''Iron(III) nitrate''', or '''ferric nitrate''', is the ] with the formula Fe(NO<sub>3</sub>)<sub>3</sub>. Since it is ], it is commonly found in its nonahydrate form Fe(NO<sub>3</sub>)<sub>3</sub>·] in which it forms colourless to pale violet crystals.		'''Iron(III) nitrate''', or '''ferric nitrate''', is the name used for a series of ]s with the formula Fe(NO<sub>3</sub>)<sub>3</sub><sup>.</sup>(H<sub>2</sub>O)<sub>n</sub>. Most common is the nonahydrate Fe(NO<sub>3</sub>)<sub>3</sub><sup>.</sup>(H<sub>2</sub>O)<sub>9</sub>. The hydrates are all pale colored, water-soluble paramagnetic salts.
	==Preparation==		==Hydrates==
			Iron(III) nitrate is ], and it is commonly found as the nonahydrate Fe(NO<sub>3</sub>)<sub>3</sub>·], which forms colourless to pale violet crystals. This compound is the trinitrate salt of the ] <sup>3+</sup>.<ref>{{cite journal |doi=10.1021/ic50168a006|title=Structure of Hexaaquairon(III) Nitrate Trihydrate. Comparison of Iron(II) and Iron(III) Bond Lengths in High-Spin Octahedral Environments|year=1977|last1=Hair|first1=Neil J.|last2=Beattie|first2=James K.|journal=Inorganic Chemistry|volume=16|issue=2|pages=245–250}}</ref>
			Other ] {{chem|Fe|(NO|3|)|3}}·''x''{{chem|H|2|O}}, include:
			* tetrahydrate (''x''=4), more precisely triaqua dinitratoiron(III) nitrate monohydrate, {{chem2|1=NO3·H2O}}, has complex cations wherein Fe<sup>3+</sup> is coordinated with two nitrate anions as ] ligands and three of the four water molecules, in a ] configuration with two water molecules at the poles.<ref name=schm2012>H. Schmidt, A. Asztalos, F. Bok and W. Voigt (2012): "New Iron(III) Nitrate Hydrates: {{chem2|1=Fe(NO3{{!}}3·''x''H2O}} with ''x'' = 4, 5 and 6". ''Acta Crystallographica Section C - Inorganic Compounds'', volume C68, pages i29-i33. {{doi|10.1107/S0108270112015855}}</ref>
	The compound is prepared by treating iron metal or iron oxides with ].
			* pentahydrate (''x''=5), more precisely penta-aqua nitratoiron(III) dinitrate, {{chem2|1=(NO3)2}}, in which the Fe<sup>3+</sup> ion is coordinated to five water molecules and a unidentate nitrate anion ligand in ].<ref name=schm2012/>
			* hexahydrate (''x''=6), more precisely hexaaquairon(III) trinitrate, {{chem2|1=(NO3)3}}, where the Fe<sup>3+</sup> ion is coordinated to six water molecules in octahedral configuration.<ref name=schm2012/>
			==Reactions==
	:Fe<sub>2</sub>O<sub>3</sub> + 6 HNO<sub>3</sub> → 2 Fe(NO<sub>3</sub>)<sub>3</sub> + 3 H<sub>2</sub>O
			Iron(III) nitrate is a useful precursor to other iron compounds because the nitrate is easily removed or decomposed. It is for example, a standard precursor to ] {{chem2|K2FeO4}}.<ref>{{cite book|author1=H. Lux|chapter=Potassium Ferrate (VI) K<sub>2</sub>FeO<sub>4</sub>|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=2|pages=1504}}</ref>
			When dissolved, iron(III) nitrate forms yellow solutions. When this solution is heated to near boiling, nitric acid evaporates and a solid precipitate of ] {{chem|Fe|2|O|3}} appears.<ref name=matij>Egon Matijević and Paul Scheiner (1978): "Ferric Hydrous Oxide Sols: III. Preparation of Uniform Particles by Hydrolysis of Fe(III)-Chloride, -Nitrate, and -Perchlorate solutions". ''Journal of Colloid and Interface Science'', volume 63, issue 3, pages 509-524. {{doi|10.1016/S0021-9797(78)80011-3}}</ref> Another method for producing iron oxides from this nitrate salt involves neutralizing its aqueous solutions.<ref>{{cite book|author1=H. Lux|chapter=Iron (III) Hydroxide FeO(OH)|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=2|pages=1499}}</ref>
			==Preparation==
			The compound can be prepared by treating ] metal powder with ], as summarized by the following idealized equation:<ref name=Ull>{{ullmann|first1=Egon|last1=Wildermuth|first2=Hans|last2=Stark|first3=Gabriele|last3=Friedrich|first4=Franz Ludwig|last4=Ebenhöch|first5=Brigitte|last5=Kühborth|first6=Jack|last6=Silver|first7=Rafael|last7=Rituper|title=Iron Compounds}}</ref>
			:{{chem2 | Fe + 4 HNO3 + 7 H2O -> Fe(NO3)3(H2O)9 + NO }}
	==Applications==		==Applications==
		⚫	Ferric nitrate has no large scale applications. It is a catalyst for the synthesis of ] from a solution of ] in ]:<ref>{{OrgSynth | author = Hampton, K. G. | author2 = Harris, T. M. | author3 = Hauser, C. R. | title = 2,4-Nonanedione | collvol = 5 | collvolpages = 848 | year = 1973 | prep = cv5p0848}} As of 2007, 22 other entries describe similar preparations in Organic Syntheses</ref>
	===In the chemical laboratory===
			:{{chem2 | 2 NH3 + 2Na -> 2 NaNH2 + H2 }}
⚫	Ferric nitrate is the catalyst of choice for the synthesis of ] from a solution of ] in ]:<ref>{{OrgSynth | author = Hampton, K. G. Harris, T. M.; Hauser, C. R. | title = 2,4-Nonandione | collvol = 5 | collvolpages = 848 | year = 1973 | prep = cv5p0848}} As of 2007, 22 other entries describe similar preparations in Organic Syntheses</ref>
	: 2 NH<sub>3</sub> + 2 Na &rarr; 2 NaNH<sub>2</sub> + H<sub>2</sub>
	Certain ]s impregnated with ferric nitrate have been shown to be useful oxidants in ]. For example, ferric nitrate on ]—a ] called "Clayfen"—has been employed for the oxidation of ]s to ]s and ]s to ]s.<ref>Cornélis, A. Laszlo, P.; Zettler, M. W. "Iron(III) Nitrate–K10 Montmorillonite Clay" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.</ref>		Certain ]s impregnated with ferric nitrate have been shown to be useful oxidants in ]. For example, ferric nitrate on ]—a ] called Clayfen—has been employed for the oxidation of ]s to ]s and ]s to ]s.<ref>Cornélis, A. Laszlo, P.; Zettler, M. W. "Iron(III) Nitrate–K10 Montmorillonite Clay" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. {{doi|10.1002/047084289X}}.</ref>
	===Other applications===
	Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.		Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.
	==References==		==References==
			{{Reflist}}
	<references/>
	{{Iron compounds}}		{{Iron compounds}}
			{{nitrates}}
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