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{{em tradução|en:Iron(III) chloride}}
{{mais-notas}}
{{Info/Química
{{Info/Química
| Watchedfields = changed
| verifiedrevid = 476995973
| ImageFile = Iron(III)_chloride_hexahydrate.jpg
| ImageFile = Iron(III)_chloride_hexahydrate.jpg
| ImageSize = 200px
| ImageSize = 200px
Linha 7: Linha 9:
| ImageFileR1 = Iron-trichloride-sheets-stacking-3D-polyhedra.png
| ImageFileR1 = Iron-trichloride-sheets-stacking-3D-polyhedra.png
| ImageSizeR1 = 150px
| ImageSizeR1 = 150px
| IUPACName = Cloreto de ferro (III)
| IUPACName = Cloreto de ferro (III)<br/>Tricloreto de ferro
| OtherNames = Cloreto férrico<br />Tricloreto de ferro<br />[[molisite]] (mineral)<br />Flores martis<br />percloreto de ferro
| OtherNames = Cloreto férrico<br/>Molysite<br/>Flores martis
| Section1 = {{Chembox Identifiers
| Section1 = {{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| Abbreviations =
| ChemSpiderID = 22792
| InChI = 1S/3ClH.Fe/h3*1H;/q;;;+3/p-3
| InChIKey = RBTARNINKXHZNM-DFZHHIFOAF
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 30808
| SMILES = Cl[Fe](Cl)Cl
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/3ClH.Fe/h3*1H;/q;;;+3/p-3
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = RBTARNINKXHZNM-UHFFFAOYSA-K
| InChIKey1 = RBTARNINKXHZNM-UHFFFAOYSA-K
| CASNo = 7705-08-0
| CASNo = 7705-08-0
| CASNo_Ref = {{cascite}}
| CASNo_Ref = {{cascite|correct|CAS}}
| CASOther = <br/>10025-77-1 (hexa-hidrato) <!-- This number is also verified against the Chemical Abstracts Service list -->
| CASOther = <br/>10025-77-1 (hexaidrato) <!-- This number is also verified against the Chemical Abstracts Service list -->
| EINECS =
| EINECS =
| PubChem = 24380
| PubChem = 24380
| SMILES =
| InChI =
| InChI =
| RTECS = LJ9100000
| RTECS = LJ9100000
| UNNumber = 1773 (anidro)<br/>2582 (sol. aq.)
| UNNumber = 1773 (anidro)<br/>2582 (sol. aq.)
}}
| MeSHName =
| ChEBI =
| KEGG =
| ATCCode_prefix =
| ATCCode_suffix =
| ATC_Supplemental =}}
| Section2 = {{Chembox Properties
| Section2 = {{Chembox Properties
| Formula = FeCl<sub>3</sub>
| Formula = FeCl<sub>3</sub>
| MolarMass = 162.2&nbsp;g·mol<sup>-1</sup>
| MolarMass = 162.2 g/mol (anidro) <br/>270.3 g/mol (hexaidrato)
| Appearance = verde-escuro por luz refletida; vermelho púrpura por luz transmitida<br/>hexaidrato: sólido amarelo<br/>solução aquosa: marrom
| MolarMass_notes =<br />hexaidrato:&nbsp;270.3&nbsp;g·mol<sup>−1</sup>
| Odor = leve de [[ácido clorídrico|HCl]]
| Appearance = verde-preto com luz refletida; púrpura-vermelho com luz transmitida;<br />hexaidrato: sólido amarelo<br /> soluções aq.: marrom
| Density = 2.80&nbsp;g·cm<sup>−3</sup><br />solução a 40%: 1.4&nbsp;g·ml<sup>−1</sup>
| Density = 2.898 g/cm<sup>3</sup> (anidro) <br> 1.82 g/cm<sup>3</sup> (hexaidrato)
| MeltingPt = 306 °C (anidro) <br> 37 °C (hexa-hidrato)
| MeltingPt= 306 °C (anidro) <br> 37 °C (hexaidrato)
| Melting_notes =
| Melting_notes =
| BoilingPt = 315 °C (anidro, decomp) <br> 280 °C (hexa-hidrato, decomp)
| BoilingPt = 315 °C (anidro, decomp) <br> 280 °C (hexaidrato, decomp)
| Boiling_notes = decomposição parcial em FeCl<sub>2</sub>+Cl<sub>2</sub>
| Boiling_notes = decomposição parcial a FeCl<sub>2</sub> + Cl<sub>2</sub>
| Solubility = 74.4 g/100 mL (0 °C) <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> <br> 92 g/100 mL (20 °C) <br> 92 g/100 mL (hexahydrate, 20 °C)
| Solubility = 74.4 g/100 mL (0 °C)<!--<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref>--> <br> 92 g/100 mL (hexaidrato, 20 °C)
| SolubleOther = 63&nbsp;g/100&nbsp;ml (18&nbsp;°C)<br />altamente solúvel<br />83&nbsp;g/100&nbsp;ml<br /> altamente solúvel
| SolubleOther = 63&nbsp;g/100&nbsp;ml (18&nbsp;°C)<br/>highly soluble<br/>83&nbsp;g/100&nbsp;ml<br/> highly soluble
| Solvent = [[acetona]]<br />[[metanol]]<br />[[etanol]]<br />[[etóxietano]]
| Solvent = [[acetona]]<br/>[[Metanol]]<br/>[[Etanol]]<br/>[[Éter dietílico]]
| pKa =
| pKa =
| pKb =
| pKb =
| Viscosity = solução a 40%&nbsp;12&nbsp;c[[Poise|P]]}}
| Viscosity = 40%&nbsp;solution: 12&nbsp;c[[Poise|P]]
}}
| Section5 = {{Chembox Structure
| Section5 = {{Chembox Structure
| CrystalStruct = [[hexagonal]]
| CrystalStruct = [[hexagonal|hexagonal]]
| SpaceGroup =
| SpaceGroup =
| Coordination = [[octaédrica]]
| Coordination = [[octaédrica]]
Linha 54: Linha 62:
| MolShape =
| MolShape =
| OrbitalHybridisation =
| OrbitalHybridisation =
| Dipólo = }}
| Dipole =
}}
| Section7 = {{Chembox Hazards
| Section7 = {{Chembox Hazards
| Reference =<ref>{{GHS class NZ|id=10764|accessdate=2010-09-19}}</ref><ref>[http://webcomm.bcd.tamhsc.edu/bcdfacilities/msds9.html Various suppliers], collated by the Baylor College of Dentistry, [[Texas A&M University]]. (accessed 2010-09-19)</ref>{{#tag:ref|Uma classificação GHS alternativa do Japanese GHS Inter-ministerial Committee (2006)<ref>{{GHS class JP|id=831|accessdate=2010-09-19}}</ref> nota a possibilidade de irritação do trato respiratório pelo FeCl<sub>3</sub> e difere pouco em outros aspectos da classificação usada aqui.|group=Note}}
| ExternalMSDS = [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc14/icsc1499.htm ICSC 1499]
| ExternalMSDS = {{ICSC-small|1499}}
| EUClass =
| EUIndex =
| EUIndex = não listado
| GHSPictograms = {{GHS05|Corr. Met. 1; Skin Corr. 1C; Eye Dam. 1}}{{GHS07|Acute Tox. 4 (oral)}}
| MainHazards = Muito corrosivo
| GHSSignalWord = DANGER
| NFPA-H = 3
| HPhrases = {{H-phrases|290|302|314|318}}
| NFPA-F =
| PPhrases = {{P-phrases|234|260|264|270|273|280| 301+312|301+330+331|303+361+353|363|304+340|310|321|305+351+338|390| 405|406|501}}
| NFPA-R = 1
| FlashPt = não inflamável
| NFPA-O =
| NFPA-F = 0 | NFPA-H = 2 | NFPA-R = 0 | NFPA-O =
| RPhrases = {{R22}}, {{R34}}
| SPhrases = {{S26}}, {{S28}}
| RSPhrases =
| FlashPt =
| Autoignition =
| ExploLimits =
| PEL = }}
| Section8 = {{Chembox Related
| OtherAnions = [[Fluoreto de ferro (III)]]<br />[[Brometo de ferro (III)]]<br />[[Sulfeto de ferro (III)]]
| OtherCations = [[Cloreto de ferro (II)]]<br />[[Cloreto de manganês (II)]]<br />[[Cloreto de cobalto (II)]]<br />[[Cloreto de rutênio (III)]]
| Function = [[coagulante]]s
| OtherFunctn = [[Sulfato de ferro (II)]]<br />[[Cloreto de alumínio]]
| OtherCpds =
}}
}}
| Section15 = {{Chembox Related
| OtherAnions = [[Fluoreto de ferro (III)]]<br/>[[Brometo de ferro (III)]]
| OtherCations = [[Cloreto de ferro (II)]]<br/>[[Cloreto de manganês (II)]]<br/>[[Cloreto de cobalto (II)]]<br/>[[Cloreto de rutênio (III)]]
| OtherFunctn = [[Sulfato de ferro (II)]]<br/>[[Cloreto de alumínio|Cloreto de polialumínio]]
| Function = [[Floculação|coagulantes]]
| OtherCpds = }}
}}
}}
'''Cloreto de ferro (III)''', também chamado '''cloreto férrico''', é um [[composto químico]] de escala industrial, de fórmula [[Ferro|Fe]][[Cloro|Cl]]<sub>3</sub>. A cor dos cristais de cloreto de ferro (III) depende do ângulo de visão: por luz refletida os cristais parecem verde-escuro, mas por [[luz transmitida]] parecem vermelho-púrpura. Cloreto férrico anidro é [[deliquescente]], formando névoas de [[ácido clorídrico]] no ar úmido. É raramente observado em sua forma natural, o mineral '''molysite''', muito conhecido de algumas [[fumarola]]s.
O '''cloreto de ferro (III)''' ou '''cloreto férrico''', cuja forma hexahidratada é conhecida como '''percloreto de ferro''', é um [[sal]] de [[fórmula química]] FeCl<sub>3</sub>.


Quando dissolvido em água, o cloreto férrico sofre [[hidrólise]] e libera calor ([[reação exotérmica]]). A solução castanha, ácida e [[corrosão|corrosiva]] resultante é usada como [[floculante]] no [[tratamento de esgoto]] e na [[tratamento de água|purificação de água]], bem como [[fresagem química|fresador]] para metais cuprosos em [[circuito impresso|circuitos impressos]]. Cloreto de ferro (III) anidro é um [[ácido de Lewis]] razoavelmente forte, e é usado como catalisador em muitas sínteses orgânicas.
Em [[solução]] com água, é utilizado na [[corrosão]] de placas para a preparação de [[circuito impresso|circuitos impressos]] usados em [[eletrônica]]. Para esta aplicação o [[persulfato de amônia]] pode ser usado com os mesmos resultados. Também é usado como [[floculação|floculante]] para tratamento de água e [[esgoto]].
<!--
==Nomenclature==
The descriptor hydrated or anidro is used when referring to iron(III) chloride, to distinguish between the two common forms. The hexaidrato is usually given as the simplified empirical formula FeCl<sub>3</sub>⋅6H<sub>2</sub>O. It may also be given as ''trans''-[Fe(H<sub>2</sub>O)<sub>4</sub>Cl<sub>2</sub>]Cl⋅2H<sub>2</sub>O and the systematic name tetraaquadichloroiron(III) chloride dihydrate, which more clearly represents its structure.


==Structure and properties==
== Manuseio do cloreto de ferro (III) ==
anidro iron(III) chloride adopts the [[bismuth(III) iodide|BiI<sub>3</sub>]] structure, which features [[octahedral]] Fe(III) centres interconnected by two-coordinate chloride [[Ligand|ligands]]. Iron(III) chloride hexaidrato consists of ''trans''-[Fe(H<sub>2</sub>O)<sub>4</sub>Cl<sub>2</sub>]<sup>+</sup> cationic [[Coordination complex|complexes]] and chloride anions, with the remaining two H<sub>2</sub>O molecules embedded within the [[monoclinic]] crystal structure.<ref>{{cite journal | first = M. D. | last = Lind | title = Crystal Structure of Ferric Chloride hexaidrato | journal = J. Chem. Phys. | volume = 47 | pages = 990 | year = 1967 | doi = 10.1063/1.1712067}}</ref>
=== Riscos quanto à saúde ===
Caso aconteça: Utilizar o EPI - Equipamento de proteção individual
* Contato com o produto: Lavar a área por pelo menos 5 minutos em água corrente.
* Contato com os olhos: Pode haver irritação – lavar em água corrente.
* Ingestão: provocar vômito e tomar leite de magnésia ou bastante água.
* Caso note algo estranho na pele ou nos olhos depois de lavar vá de imediato consultar um medico.
* Complicações por ingestão: procurar um médico e indicar a natureza do produto e quantidade ingerida.


Iron(III) chloride has a relatively low melting point and boils at around 315&nbsp;°C. The vapour consists of the dimer Fe<sub>2</sub>Cl<sub>6</sub> (''c.f.'' [[aluminium chloride]]) which increasingly dissociates into the monomeric FeCl<sub>3</sub> (D<sub>3h</sub> [[symmetry group|point group]] [[molecular symmetry]]) at higher temperature, in competition with its reversible decomposition to give [[iron(II) chloride]] and [[chlorine]] gas.<ref>{{cite book | last = Holleman | first = A. F. | coauthors = Wiberg, E. | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | year = 2001 | isbn = 0-12-352651-5}}</ref>
=== Cuidados ===
* Haverá um auto-aquecimento natural da solução (pode chegar a 70&nbsp;°C).
* Uma fumaça não tóxica poderá ser observada.
* Inicialmente a solução ficará marrom, chegando à cor de café no final.
* O percloreto de ferro possui grande poder oxidante. Mancha tecidos de forma irremediável. Muito cuidado com as roupas.


==Preparation==
{{referências}}
anidro iron(III) chloride may be prepared by union of the elements:<ref>{{cite journal | first = B. R. | last = Tarr | title = anidro Iron(III) Chloride | journal = Inorganic Syntheses | volume = 3 | pages = 191–194 | year = 1950 | doi = 10.1002/9780470132340.ch51 | last2 = Booth | first2 = Harold S. | last3 = Dolance | first3 = Albert | series = Inorganic Syntheses | isbn = 978-0-470-13234-0}}</ref>
{{DEFAULTSORT:Cloreto Ferro (Iii)}}


:2&nbsp;Fe([[solid|s]]) + 3&nbsp;Cl<sub>2</sub>([[Gas|g]]) → 2&nbsp;FeCl<sub>3</sub>(s)
[[Categoria:Sais]]
[[Categoria:Cloretos|Ferro]]
[[Categoria:Compostos de ferro]]


Solutions of iron(III) chloride are produced industrially both from iron and from ore, in a closed-loop process.
{{Bom interwiki|en}}

#Dissolving pure [[iron]] in a solution of iron(III) chloride
#:Fe(s) + 2&nbsp;FeCl<sub>3</sub>(aq) → 3&nbsp;FeCl<sub>2</sub>(aq)
#Dissolving [[iron ore]] in [[hydrochloric acid]]
#:Fe<sub>3</sub>O<sub>4</sub>(s) + 8&nbsp;HCl(aq) → FeCl<sub>2</sub>(aq) + 2&nbsp;FeCl<sub>3</sub>(aq) + 4&nbsp;H<sub>2</sub>O
#Oxidation of [[iron (II) chloride]] with [[chlorine]]
#:2&nbsp;FeCl<sub>2</sub>(aq) + Cl<sub>2</sub>(g) → 2&nbsp;FeCl<sub>3</sub>(aq)
-->
<!--Like many other hydrated metal chlorides, hydrated iron(III) chloride can be converted to the anidro salt by refluxing with [[thionyl chloride]].<ref>{{cite journal | title = anidro Metal Chlorides | first = Alfred R. | last = Pray | coauthors = Richard F. Heitmiller, Stanley Strycker | journal = [[Inorganic Syntheses]] | volume = 28 | pages = 321–323 | doi = 10.1002/9780470132593.ch80 | year = 1990 | ISBN = 978-0-470-13259-3}}</ref> Conversion of the hydrate to anidro iron(III) chloride is not accomplished by heating, as HCl and [[iron oxychloride]]s are produced.

==Reactions==
[[File:Iron(III) chloride.JPG|thumb|left|A brown, acidic solution of iron(III) chloride]]
Iron(III) chloride undergoes hydrolysis to give an acidic solution. When heated with [[iron(III) oxide]] at 350&nbsp;°C, iron(III) chloride gives iron oxychloride, a layered solid and [[Intercalation (chemistry)|intercalation]] host.{{Citation needed|date=June 2009}}
:FeCl<sub>3</sub> + Fe<sub>2</sub>O<sub>3</sub> → 3&nbsp;FeOCl

It is a moderately strong [[Lewis acid]], forming [[adduct]]s with [[Lewis base]]s such as [[triphenylphosphine oxide]], e.g. FeCl<sub>3</sub>(OPPh<sub>3</sub>)<sub>2</sub> where Ph = [[phenyl]]. It also reacts with other [[chloride]] salts to give the yellow [[tetrahedral]] FeCl<sub>4</sub><sup>−</sup> ion. Salts of FeCl<sub>4</sub><sup>−</sup> in [[hydrochloric acid]] can be extracted into [[diethyl ether]].

Alkali metal [[alkoxide]]s react to give the metal alkoxide complexes of varying complexity.<ref>The chemistry of metal alkoxides, Nataliya Ya Turova, 12.22.1 'Synthesis', p. 481 [http://books.google.co.uk/books?id=_-KugzJApGsC&pg=RA2-PA481&lpg=RA2-PA481&dq=iron+III+chloride+alkoxide&source=bl&ots=x514HvH2GM&sig=KsnQWOP4eerBnqlOu80wJ8tMH7o&hl=en&ei=aX0OTJqjFJiT4gbDsPyZDA&sa=X&oi=book_result&ct=result&resnum=6&ved=0CCwQ6AEwBTgK#v=onepage&q&f=false google books link]</ref> The compounds can be dimeric or trimeric.<ref>Alkoxo and aryloxo derivatives of metals By D. C. Bradley, 3.2.10, Alkoxides of later 3d metals, p. 69 [http://books.google.co.uk/books?id=ixNEpx8aDHUC&pg=PA69&dq=iron+trialkoxides+dimer+trimer&cd=1#v=onepage&q&f=false google books links]</ref> In the solid phase a variety of multinuclear complexes have been described for the nominal stoichiometric reaction between FeCl<sub>3</sub> and [[sodium ethoxide]]:<ref>Fe<sub>9</sub>O<sub>3</sub>(OC<sub>2</sub>H<sub>5</sub>)<sub>21</sub>·C<sub>2</sub>H<sub>5</sub>OH—A New Structure Type of an Uncharged Iron(III) Oxide-Alkoxide Cluster, Michael Veith, Frank Grätz, Volker Huch, European Journal of Inorganic Chemistry, Vol 2001, Issue 2, pp. 367–368 [http://www3.interscience.wiley.com/journal/76503520/abstract?CRETRY=1&SRETRY=0 online link]</ref><ref>The synthesis of iron (III) ethoxide revisited: Characterization of the metathesis products of iron (III) halides and sodium ethoxide, Gulaim A. Seisenbaevaa, Suresh Gohila, Evgeniya V. Suslovab, Tatiana V. Rogovab, Nataliya Ya. Turovab, Vadim G. Kesslera, Inorganica Chimica Acta, Volume 358, Issue 12, 1/8/2005, pp. 3506–3512, [http://www.sciencedirect.com/science?_ob=ArticleURL&_udi=B6TG5-4GGWGK1-1&_user=10&_coverDate=08/01/2005&_rdoc=1&_fmt=high&_orig=search&_sort=d&_docanchor=&view=c&_acct=C000050221&_version=1&_urlVersion=0&_userid=10&md5=eedf65ccda9e4c440ab9f5170a4739b2 online link]</ref>

:FeCl<sub>3</sub> + 3 [C<sub>2</sub>H<sub>5</sub>O]<sup>-</sup>Na<sup>+</sup> → Fe(OC<sub>2</sub>H<sub>5</sub>)<sub>3</sub> + 3 NaCl

[[Oxalic acid|Oxalate]]s react rapidly with aqueous iron(III) chloride to give [Fe(C<sub>2</sub>O<sub>4</sub>)<sub>3</sub>]<sup>3−</sup>. Other [[carboxylate]] salts form complexes, e.g. [[Citric acid|citrate]] and [[tartaric acid|tartrate]].

===Oxidation===
Iron(III) chloride is a mild [[Redox|oxidising agent]], for example, it is capable of oxidising [[copper(I) chloride]] to [[copper(II) chloride]].

: FeCl<sub>3</sub> + CuCl → FeCl<sub>2</sub> + CuCl<sub>2</sub>

It also reacts with iron to form iron(II) chloride:

: 2 FeCl<sub>3</sub> + Fe → 3 FeCl<sub>2</sub>

Reducing agents such as [[hydrazine]] convert iron(III) chloride to complexes of iron(II).

==Uses==
===Industrial===
In industrial application, iron(III) chloride is used in [[sewage treatment]] and [[water treatment|drinking water production]].<ref name="wtcbrochure">{{cite book | title = Water Treatment Chemicals | url = http://www.akzonobel.com/ic/system/images/AkzoNobel_WTCBrochureENG_tcm18-9982.pdf |format=PDF| publisher = [[Akzo Nobel|Akzo Nobel Base Chemicals]] | year = 2007 | accessdate = 2007-10-26}}</ref> In this application, FeCl<sub>3</sub> in slightly basic water reacts with the [[hydroxide]] ion to form a [[Flocculation|floc]] of iron(III) hydroxide, or more precisely formulated as FeO(OH)<sup>-</sup>, that can remove suspended materials.
:[Fe(H<sub>2</sub>O)<sub>6</sub>]<sup>3+</sup> + 4 HO<sup>−</sup> → [Fe(H<sub>2</sub>O)<sub>2</sub>(HO)<sub>4</sub>]<sup>−</sup> + 4 H<sub>2</sub>O → [Fe(H<sub>2</sub>O)O(HO)<sub>2</sub>]<sup>−</sup> + 6 H<sub>2</sub>O

It is also used as a leaching agent in chloride hydrometallurgy,<ref>Separation and Purification Technology 51 (2006) pp. 332–337</ref> for example in the production of Si from FeSi. (Silgrain process)<ref>Chem. Eng. Sci. 61 (2006) pp. 229–245</ref>

Another important application of iron(III) chloride is etching [[copper]] in two-step [[redox]] reaction to [[copper(I) chloride]] and then to [[copper(II) chloride]] in the production of [[printed circuit boards]].<ref>{{cite book | first = N. N. | last = Greenwood | coauthors = A. Earnshaw | title = Chemistry of the Elements | edition = 2nd | publisher = [[Butterworth-Heinemann]] | location = Oxford | year = 1997}}</ref>
:FeCl<sub>3</sub> + Cu → FeCl<sub>2</sub> + CuCl
:FeCl<sub>3</sub> + CuCl → FeCl<sub>2</sub> + CuCl<sub>2</sub>

Iron(III) chloride is used as catalyst for the reaction of [[ethylene]] with [[chlorine]], forming ethylene dichloride ([[1,2-dichloroethane]]), an important commodity chemical, which is mainly used for the industrial production of [[vinyl chloride]], the [[monomer]] for making [[polyvinyl chloride|PVC]].
:H<sub>2</sub>C=CH<sub>2</sub> + Cl<sub>2</sub> → ClCH<sub>2</sub>CH<sub>2</sub>Cl

===Laboratory use===
In the laboratory iron(III) chloride is commonly employed as a [[Lewis acid]] for [[catalyst|catalysing]] reactions such as [[chlorination]] of [[aromatic compound]]s and [[Friedel-Crafts reaction]] of aromatics. It is less powerful than [[aluminium chloride]], but in some cases this mildness leads to higher yields, for example in the alkylation of benzene:

:[[Image:FeCl3 Friedel-Crafts.gif|400px|Iron(III) chloride as a catalyst]]

The [[ferric chloride test]] is a traditional colorimetric test for [[phenols]], which uses a 1% iron(III) chloride solution that has been neutralised with [[sodium hydroxide]] until a slight precipitate of FeO(OH) is formed.<ref>{{cite book | first = B. S. | last = Furnell | coauthors = et al. | title = Vogel's Textbook of Practical Organic Chemistry | edition = 5th | publisher = [[Longman]]/[[John Wiley & Sons|Wiley]] | location = New York | year = 1989}}</ref> The mixture is filtered before use. The organic substance is dissolved in water, [[methanol]] or [[ethanol]], then the neutralised iron(III) chloride solution is added—a transient or permanent coloration (usually purple, green or blue) indicates the presence of a phenol or enol.

This reaction is exploited in the [[Trinder spot test]], which is used to indicate the presence of salicylates, particularly [[salicylic acid]], which contains a phenolic OH group.

===Other uses===
* Used in anidro form as a drying reagent in certain reactions.
* Used in water and wastewater treatment to precipitate phosphate as iron (III) phosphate.
* Used by American coin collectors to identify the dates of [[Buffalo nickel]]s that are so badly worn that the date is no longer visible.
* Used by knife craftsmen and sword smiths to stain blades, as to give a contrasting effect to the metal, and to view metal layering or imperfections.
* Used to etch the [[widmanstatten pattern]] in iron [[meteorites]].
* Necessary for the etching of [[photogravure]] plates for printing photographic and fine art images in [[Intaglio (printmaking)|intaglio]] and for etching [[rotogravure]] cylinders used in the printing industry.
* Used to make printed circuit boards(PCBs).
* Used in veterinary practice to treat overcropping of an animal's claws, particularly when the overcropping results in bleeding.
* Reacts with cyclopentadienylmagnesium bromide in one preparation of [[ferrocene]], a metal-sandwich complex.<ref>{{cite journal | first = T. J. | last = Kealy | title = A New Type of Organo-Iron Compound | journal = Nature | volume = 168 | page = 1040 | year = 1951 | doi = 10.1038/1681039b0 | last2 = Pauson | first2 = P. L. | issue=4285}}</ref>
* Sometimes used in a technique of [[Raku ware]] firing, the iron coloring a pottery piece shades of pink, brown, and orange.
* Used to test the pitting and crevice corrosion resistance of stainless steels and other alloys.
* Used in conjunction with NaI in acetonitrile to mildly reduce organic azides to primary amines.<ref>{{cite journal | first = Ahmed | last = Kamal | title = Mild and efficient reduction of azides to amines: synthesis of fused [2,1-''b'']quinazolines | journal = Tetrahedron Letters | volume = 43 | page = 6961 | year = 2002 | doi =10.1016/S0040-4039(02)01454-5 | last2 = Ramana | first2 = K. | last3 = Ankati | first3 = H. | last4 = Ramana | first4 = A | issue = 38 }}</ref>
* Used in an animal thrombosis model.<ref>{{cite journal | first = Michael | last = Tseng | title = Transendothelial migration of ferric ion in FeCl<sub>3</sub> injured murine common carotid artery | journal = Thrombosis Research | volume = 118 | pages = 275–280 | year = 2006 | doi =10.1016/j.thromres.2005.09.004 | pmid = 16243382 | last2 = Dozier | first2 = A. | last3 = Haribabu | first3 = B. | last4 = Graham | first4 = U. M. | issue = 2}}</ref>

==Safety==
Iron(III) chloride is toxic, highly corrosive and acidic. The anidro material is a powerful dehydrating agent.
-->
==Ver também==
* [[Sulfato de ferro (II)]]
* [[Cloreto de alumínio]]

==Notas e referências==
===Notas===
{{reflist|group=Note}}

===Referências===
{{reflist}}

==Leitura posterior (em inglês)==
# ''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
# ''The Merck Index'', 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
# D. Nicholls, ''Complexes and First-Row Transition Elements'', Macmillan Press, London, 1973.
# A.F. Wells, '''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984.
# J. March, ''Advanced Organic Chemistry'', 4th ed., p.&nbsp;723, Wiley, New York, 1992.
# ''Handbook of Reagents for Organic Synthesis: Acidic and Basic Reagents'', (H. J. Reich, J. H. Rigby, eds.), Wiley, New York, 1999.

{{Compostos do ferro}}

{{DEFAULTSORT:Cloreto de ferro()}}
[[Category:Cloretos]]
[[Category:Compostos do ferro]]
[[Category:Haletos metálicos]]
[[Category:Compostos de coordenação]]
[[Category:Substâncias deliquescentes]]
[[Category:Agentes desidratantes]]


[[ar:كلوريد الحديد الثلاثي]]
[[ar:كلوريد الحديد الثلاثي]]
Linha 114: Linha 211:
[[es:Cloruro de hierro (III)]]
[[es:Cloruro de hierro (III)]]
[[fa:کلرید آهن(III)]]
[[fa:کلرید آهن(III)]]
[[fi:Ferrikloridi]]
[[fr:Chlorure de fer(III)]]
[[fr:Chlorure de fer(III)]]
[[hr:Željezov(III) klorid]]
[[hr:Željezov(III) klorid]]
[[hu:Vas(III)-klorid]]
[[id:Besi(III) klorida]]
[[id:Besi(III) klorida]]
[[it:Cloruro ferrico]]
[[it:Cloruro ferrico]]
[[ja:塩化鉄(III)]]
[[hu:Vas(III)-klorid]]
[[nl:IJzer(III)chloride]]
[[nl:IJzer(III)chloride]]
[[ja:塩化鉄(III)]]
[[pl:Chlorek żelaza(III)]]
[[pl:Chlorek żelaza(III)]]
[[ro:Clorură de fier (III)]]
[[ro:Clorură de fier (III)]]
Linha 128: Linha 224:
[[sk:Chlorid železitý]]
[[sk:Chlorid železitý]]
[[sl:Železov(III) klorid]]
[[sl:Železov(III) klorid]]
[[fi:Ferrikloridi]]
[[sv:Järn(III)klorid]]
[[sv:Järn(III)klorid]]
[[uk:Хлорид заліза(ІІІ)]]
[[uk:Хлорид заліза(ІІІ)]]

Revisão das 16h35min de 22 de outubro de 2012

Cloreto de ferro(III)
Alerta sobre risco à saúde
Nome IUPAC Cloreto de ferro (III)
Tricloreto de ferro
Outros nomes Cloreto férrico
Molysite
Flores martis
Identificadores
Número CAS 7705-08-0,
10025-77-1 (hexaidrato)
PubChem 24380
ChemSpider 22792
ChEBI 30808
Número RTECS LJ9100000
SMILES
Propriedades
Fórmula molecular FeCl3
Massa molar 162.2 g/mol (anidro)
270.3 g/mol (hexaidrato)
Aparência verde-escuro por luz refletida; vermelho púrpura por luz transmitida
hexaidrato: sólido amarelo
solução aquosa: marrom
Odor leve de HCl
Densidade 2.898 g/cm3 (anidro)
1.82 g/cm3 (hexaidrato)
Ponto de fusão

306 °C (anidro)
37 °C (hexaidrato)

Ponto de ebulição

315 °C (anidro, decomp)
280 °C (hexaidrato, decomp) (decomposição parcial a FeCl2 + Cl2)

Solubilidade em água 74.4 g/100 mL (0 °C)
92 g/100 mL (hexaidrato, 20 °C)
Solubilidade em acetona
Metanol
Etanol
Éter dietílico 		63 g/100 ml (18 °C)
highly soluble
83 g/100 ml
highly soluble
Viscosidade 40% solution: 12 cP
Estrutura
Estrutura cristalina hexagonal
Geometria de
coordenação 		octaédrica
Riscos associados
MSDS Predefinição:ICSC-small
Índice UE não listado
NFPA 704
0
2
0
 
Ponto de fulgor não inflamável
Compostos relacionados
Outros aniões/ânions Fluoreto de ferro (III)
Brometo de ferro (III)
Outros catiões/cátions Cloreto de ferro (II)
Cloreto de manganês (II)
Cloreto de cobalto (II)
Cloreto de rutênio (III)
coagulantes relacionados Sulfato de ferro (II)
Cloreto de polialumínio
Página de dados suplementares
Estrutura e propriedades n, εr, etc.
Dados termodinâmicos Phase behaviour
Solid, liquid, gas
Dados espectrais UV, IV, RMN, EM
Exceto onde denotado, os dados referem-se a
materiais sob condições normais de temperatura e pressão
Referências e avisos gerais sobre esta caixa.
Alerta sobre risco à saúde.

Cloreto de ferro (III), também chamado cloreto férrico, é um composto químico de escala industrial, de fórmula FeCl3. A cor dos cristais de cloreto de ferro (III) depende do ângulo de visão: por luz refletida os cristais parecem verde-escuro, mas por luz transmitida parecem vermelho-púrpura. Cloreto férrico anidro é deliquescente, formando névoas de ácido clorídrico no ar úmido. É raramente observado em sua forma natural, o mineral molysite, muito conhecido de algumas fumarolas.

Quando dissolvido em água, o cloreto férrico sofre hidrólise e libera calor (reação exotérmica). A solução castanha, ácida e corrosiva resultante é usada como floculante no tratamento de esgoto e na purificação de água, bem como fresador para metais cuprosos em circuitos impressos. Cloreto de ferro (III) anidro é um ácido de Lewis razoavelmente forte, e é usado como catalisador em muitas sínteses orgânicas.

Ver também

Notas e referências

Notas

Referências

Leitura posterior (em inglês)

  1. Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
  2. The Merck Index, 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
  3. D. Nicholls, Complexes and First-Row Transition Elements, Macmillan Press, London, 1973.
  4. A.F. Wells, 'Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK, 1984.
  5. J. March, Advanced Organic Chemistry, 4th ed., p. 723, Wiley, New York, 1992.
  6. Handbook of Reagents for Organic Synthesis: Acidic and Basic Reagents, (H. J. Reich, J. H. Rigby, eds.), Wiley, New York, 1999.

Predefinição:Compostos do ferro

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