| Revision as of 14:38, 9 August 2011 editCheMoBot (talk | contribs)Bots141,565 edits Updating {{chembox}} (no changed fields - added verified revid - updated 'DrugBank_Ref', 'ChEMBL_Ref', 'ChEBI_Ref', 'KEGG_Ref') per Chem/Drugbox validation (report [[Wikipedia_talk:WikiProject_Ch← Previous edit |
Latest revision as of 15:08, 30 June 2024 edit undoAnDeargMor (talk | contribs)Extended confirmed users803 edits Added comments and tethyd modelTag: Visual edit |
| (134 intermediate revisions by 76 users not shown) |
| Line 1: |
Line 1: |
|
{{chembox |
|
{{chembox |
|
|
| Verifiedfields = changed |
|
| verifiedrevid = 443878729 |
|
|
|
| Watchedfields = changed |
|
| Name = Iron(II) chloride |
|
|
|
| verifiedrevid = 443880274 |
|
| ImageFile = Iron(II)-chloride-xtal-sheet-3D-balls-A.png |
|
|
|
| Name = Iron(II) chloride |
|
| ImageFile2 = FeCl2.png |
|
|
|
| ImageFileL1 = Iron(II) chloride anhydrate.jpg |
|
| ImageSize2 = 20px |
|
|
|
| ImageCaptionL1 = Anhydrous |
|
| IUPACName = Iron(II) chloride<br/>Iron dichloride |
|
|
| OtherNames = Ferrous chloride,<br/>] |
|
| ImageFileR1 = Ferrous chloride tetrahydrate.jpg |
|
|
| ImageCaptionR1 = Tetrahydrate |
|
| Section1 = {{Chembox Identifiers |
|
|
|
| ImageFileL2 = Iron(II)-chloride-xtal-sheet-3D-balls-A.png |
|
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|
|
|
| ImageCaptionL2 = Structure of anhydrous ferrous chloride ({{colorbox|purple}} Fe, {{colorbox|green}} Cl) |
|
|
| ImageFileR2 = Trans-FeCl2(H2O)4.png |
|
|
| ImageCaptionR2 = structure of tetrahydrate |
|
|
| IUPACName = Iron(II) chloride<br/>Iron dichloride |
|
|
| OtherNames = Ferrous chloride<br/>] |
|
|
| Section1 = {{Chembox Identifiers |
|
|
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|
| ChemSpiderID = 22866 |
|
| ChemSpiderID = 22866 |
|
| UNII_Ref = {{fdacite|correct|FDA}} |
|
| UNII_Ref = {{fdacite|correct|FDA}} |
| Line 17: |
Line 24: |
|
| ChEBI = 30812 |
|
| ChEBI = 30812 |
|
| SMILES = ClCl |
|
| SMILES = ClCl |
|
|
| SMILES_Comment = anhydrous |
|
|
| SMILES1 = Cl(Cl)()()() |
|
|
| SMILES1_Comment = tetrahydrate |
|
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
|
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
|
| StdInChI = 1S/2ClH.Fe/h2*1H;/q;;+2/p-2 |
|
| StdInChI = 1S/2ClH.Fe/h2*1H;/q;;+2/p-2 |
| Line 22: |
Line 32: |
|
| StdInChIKey = NMCUIPGRVMDVDB-UHFFFAOYSA-L |
|
| StdInChIKey = NMCUIPGRVMDVDB-UHFFFAOYSA-L |
|
| CASNo = 7758-94-3 |
|
| CASNo = 7758-94-3 |
|
| CASNo_Ref = {{cascite|correct|CAS}} |
|
| CASNo_Ref = {{cascite|correct|CAS}} |
|
|
| CASNo2_Ref = {{cascite|changed|??}} |
|
| CASOther = <br> 16399-77-2 (dihydrate) <br/>13478-10-9 (tetrahydrate) |
|
|
| PubChem = 24458 |
|
| CASNo2 = 16399-77-2 |
|
|
| CASNo2_Comment = (dihydrate) |
|
| RTECS = NO5400000 |
|
|
|
| CASNo3_Ref = {{cascite|changed|??}} |
|
| EINECS = |
|
|
|
| CASNo3 = 13478-10-9 |
|
}} |
|
|
|
| CASNo3_Comment = (tetrahydrate) |
|
| Section2 = {{Chembox Properties |
|
|
|
| PubChem = 24458 |
|
| Formula = FeCl<sub>2</sub> |
|
|
|
| RTECS = NO5400000 |
|
| MolarMass = 126.751 g/mol (anhydrous)<br/>198.8102 g/mol (tetrahydrate) |
|
|
|
| EINECS = 231-843-4}} |
|
| Appearance = tan solid (anhydrous)<br/>pale green solid (di-tetrahydrate) |
|
|
|
| Section2 = {{Chembox Properties |
|
| Density = 3.16 g/cm<sup>3</sup> (anhydrous) <br> 2.30 g/cm<sup>3</sup> (dihydrate) <br> 1.39 g/cm<sup>3</sup> (tetrahydrate) |
|
|
|
| Formula = FeCl<sub>2</sub> |
|
| Solvent = ] |
|
|
|
| MolarMass = 126.751{{nbsp}}g/mol (anhydrous)<br/>198.8102{{nbsp}}g/mol (tetrahydrate) |
|
| SolubleOther = soluble |
|
|
|
| Appearance = Tan solid (anhydrous)<br/>Pale green solid (di-tetrahydrate) |
|
| Solubility = 64.4 g/100 mL (10°C),<br/>68.5 g/100mL (20°C),<br/>105.7 g/100 mL (100°C) |
|
|
|
| Density = 3.16{{nbsp}}g/cm<sup>3</sup> (anhydrous) <br /> 2.39{{nbsp}}g/cm<sup>3</sup> (dihydrate) <br /> 1.93{{nbsp}}g/cm<sup>3</sup> (tetrahydrate) |
|
| Solvent2 = ] |
|
|
|
| Solvent1 = THF |
|
| SolubleOther2 = 100 g/100 mL |
|
|
|
| Solubility1 = Soluble |
|
| MeltingPt = 677 °C (anhydrous) <br> 120 °C (dihydrate) <br> 105 °C (tetrahydrate) <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> |
|
|
|
| Solubility = 64.4{{nbsp}}g/100{{nbsp}}mL (10 °C),<br/>68.5{{nbsp}}g/100{{nbsp}}mL (20 °C),<br/>105.7{{nbsp}}g/100{{nbsp}}mL (100 °C) |
|
| BoilingPt = 1023 °C (anhydrous) |
|
|
|
| MeltingPtC = 677 |
|
}} |
|
|
|
| MeltingPt_notes = (anhydrous) <br /> 120 °C (dihydrate) <br /> 105 °C (tetrahydrate) |
|
| Section3 = {{Chembox Structure |
|
|
|
| BoilingPtC = 1023 |
|
| Coordination = octahedral at Fe |
|
|
|
| BoilingPt_notes = (anhydrous) |
|
| CrystalStruct = ] |
|
|
|
| LogP = −0.15 |
|
}} |
|
|
|
| MagSus = +{{val|14750}}·10<sup>−6</sup>{{nbsp}}cm<sup>3</sup>/mol}} |
|
| Section7 = {{Chembox Hazards |
|
|
|
| Section3 = {{Chembox Structure |
|
| ExternalMSDS = |
|
|
|
| Coordination = Octahedral at Fe |
|
| EUClass = |
|
|
|
| CrystalStruct = ]}} |
|
| EUIndex = |
|
|
|
| Section6 = {{Chembox Pharmacology |
|
|
| ATCCode_prefix = B03 |
|
|
| ATCCode_suffix = AA05}} |
|
|
| Section7 = {{Chembox Hazards |
|
|
| ExternalSDS = |
|
| MainHazards = |
|
| MainHazards = |
|
| NFPA-H = 3 |
|
| NFPA-H = 3 |
|
| NFPA-F = 0 |
|
| NFPA-F = 0 |
|
| NFPA-R = 0 |
|
| NFPA-R = 0 |
|
| NFPA-O = |
|
| NFPA-S = |
|
| RPhrases = |
|
|
| SPhrases = |
|
|
| FlashPt = |
|
| FlashPt = |
|
|
| REL = TWA 1{{nbsp}}mg/m<sup>3</sup><ref>{{PGCH|0346}}</ref>}} |
|
| PEL = |
|
|
|
| Section8 = {{Chembox Related |
|
}} |
|
|
|
| OtherAnions = ]<br/>]<br/>] |
|
| Section8 = {{Chembox Related |
|
|
| OtherAnions = ]<br/>]<br/>] |
|
| OtherCations = ]<br/>]<br/>]}} |
|
| OtherCations = ]<br/>]<br/>] |
|
|
}} |
|
|
}} |
|
}} |
|
|
|
|
|
'''Iron(II) chloride''', also known as '''ferrous chloride''', is the ] of formula FeCl<sub>2</sub>. It has a high melting point, ] solid, usually obtained as an off-white solid. FeCl<sub>2</sub> ] from water as the greenish ], which is the form that is most commonly encountered in commerce and the laboratory. There is also a dihydrate. The compound is also soluble in water; aqueous solutions of FeCl<sub>2</sub> are yellow. |
|
'''Iron(II) chloride''', also known as '''ferrous chloride''', is the ] of formula FeCl<sub>2</sub>. It is a ] solid with a high melting point. The compound is white, but typical samples are often off-white. FeCl<sub>2</sub> ] from water as the greenish ], which is the form that is most commonly encountered in commerce and the laboratory. There is also a dihydrate. The compound is highly soluble in water, giving pale green solutions. |
|
|
|
|
|
==Production== |
|
==Production== |
|
|
] |
|
Hydrated forms of ferrous chloride are generated by treatment of wastes from steel production with ]. Such solutions are designated "spent acid," especially when the ] is not completely consumed: |
|
|
|
Hydrated forms of ferrous chloride are generated by treatment of wastes from ] with ]. Such solutions are designated "spent acid," or "pickle liquor" especially when the hydrochloric acid is not completely consumed: |
|
:] + 2 HCl → FeCl<sub>2</sub> + ] |
|
|
|
:Fe + 2 HCl → FeCl<sub>2</sub> + H<sub>2</sub> |
|
The spent acid requires treatment before its disposal. It is also byproduct from titanium production, since some ] ]s contain iron.<ref name=Ullmann>Egon Wildermuth, Hans Stark, Gabriele Friedrich, Franz Ludwig Ebenhöch, Brigitte Kühborth, Jack Silver, Rafael Rituper “Iron Compounds” in Ullmann’s Encyclopedia of Industrial Chemistry Wiley-VCH, Wienheim, 2005.</ref> |
|
|
|
The production of ferric chloride involves the use of ferrous chloride. Ferrous chloride is also a byproduct from the production of titanium, since some ]s contain iron.<ref name=Ullmann>Egon Wildermuth, Hans Stark, Gabriele Friedrich, Franz Ludwig Ebenhöch, Brigitte Kühborth, Jack Silver, Rafael Rituper "Iron Compounds" in ''Ullmann's Encyclopedia of Industrial Chemistry''. Wiley-VCH, Wienheim, 2005.</ref> |
|
|
|
|
|
|
==Anhydrous FeCl<sub>2</sub>== |
|
==Laboratory preparation== |
|
|
Ferrous chloride is conveniently prepared by addition of iron powder to a solution of ] and concentrated ] under an inert atmosphere. This reaction gives the methanol solvate, which upon heating in a vacuum at about 160 °C gives ] FeCl<sub>2</sub>.<ref>{{cite journal | author = G. Winter | title = Iron(II) Halides | journal = ] | year = 1973 | volume = 14 | pages = 99–104 | doi = 10.1002/9780470132456.ch20 | last2 = Thompson | first2 = D. W. | last3 = Loehe | first3 = J. R.}}</ref> FeBr<sub>2</sub> and FeI<sub>2</sub> can be prepared analogously. |
|
Ferrous chloride is prepared by addition of iron powder to a solution of ] in methanol. This reaction gives the methanol solvate of the dichloride, which upon heating in a vacuum at about 160 °C converts to ] FeCl<sub>2</sub>.<ref>{{cite book | author = G. Winter | journal = ] | year = 1973 | volume = 14 | pages = 99–104 | doi = 10.1002/9780470132456.ch20 | last2 = Thompson | first2 = D. W. | last3 = Loehe | first3 = J. R.| title = Inorganic Syntheses | chapter = Iron(II) Halides | isbn = 978-0-470-13245-6 }}</ref> The net reaction is shown: |
|
|
: Fe + 2 HCl → FeCl<sub>2</sub> + H<sub>2</sub> |
|
|
FeBr<sub>2</sub> and FeI<sub>2</sub> can be prepared analogously. |
|
|
|
|
|
An alternative laboratory synthesis of FeCl<sub>2</sub> entails the reaction of ] with ]:<ref>{{cite journal | author = P. Kovacic and N. O. Brace | journal = ] | year = 1960 | volume = 6 | pages = 172 | doi = 10.1002/9780470132371.ch54 | title = Iron(II) Chloride}}</ref> |
|
An alternative synthesis of anhydrous ferrous chloride is the reduction of ] with ]:<ref>{{cite book | author = P. Kovacic and N. O. Brace | title = Inorganic Syntheses | journal = ] | year = 1960 | volume = 6 | pages = 172–173 | doi = 10.1002/9780470132371.ch54 | chapter = Iron(II) Chloride| isbn = 978-0-470-13237-1 }}</ref> |
|
:2 FeCl<sub>3</sub> + C<sub>6</sub>H<sub>5</sub>Cl → 2 FeCl<sub>2</sub> + C<sub>6</sub>H<sub>4</sub>Cl<sub>2</sub> + ] |
|
:2 FeCl<sub>3</sub> + C<sub>6</sub>H<sub>5</sub>Cl → 2 FeCl<sub>2</sub> + C<sub>6</sub>H<sub>4</sub>Cl<sub>2</sub> + HCl |
|
|
|
|
FeCl<sub>2</sub> prepared in this way exhibits convenient solubility in ], a common solvent for chemical reactions. In one of two classic syntheses of ], ] generated FeCl<sub>2</sub> by heating FeCl<sub>3</sub> with iron powder.<ref>{{OrgSynth | author = G. Wilkinson | title = Ferrocene | collvol = 4 | collvolpages = 473 | year = 1963 | prep = cv4p0473}}</ref> Ferric chloride decomposes to ferrous chloride at high temperatures. |
|
|
|
For the preparation of ] ferrous chloride is generated ''in situ'' by comproportionation of FeCl<sub>3</sub> with iron powder in ] (THF).<ref name=orgsyn>{{OrgSynth|title = Ferrocene|authorlink = Geoffrey Wilkinson|last = Wilkinson|first = G.|volume = 36|page = 31|year = 1956|doi = 10.15227/orgsyn.036.0031}}</ref> Ferric chloride decomposes to ferrous chloride at high temperatures. |
|
|
|
|
|
==Hydrates== |
|
|
The dihydrate, FeCl<sub>2</sub>(H<sub>2</sub>O)<sub>2</sub>, crystallizes from concentrated hydrochloric acid.<ref>{{cite book | author1 = K. H.. Gayer| author2 = L. Woontner | title = Inorganic Syntheses | chapter = Iron(II) Chloride 2-Hydrate | journal = ] | year = 1957 | volume = 5 | pages = 179–181 | doi = 10.1002/9780470132364.ch48 | isbn = 978-0-470-13236-4 }}</ref> The dihydrate is a ]. Each Fe center is coordinated to four doubly ]s. The octahedron is completed by a pair of mutually trans ]s.<ref>{{cite journal|title=Crystal structures of manganese(II) and iron(II) chloride dihydrate|author1=Morosin, B.|author2=Graeber, E. J.|journal=Journal of Chemical Physics|year=1965|volume=42|issue=3|pages=898–901|doi=10.1063/1.1696078|bibcode=1965JChPh..42..898M}}</ref> |
|
|
] |
|
|
|
|
|
==Reactions== |
|
==Reactions== |
|
|
] is prepared by treating ferrous chloride with ].<ref>{{cite book |doi=10.1002/9780470132326.ch64|chapter=Tetrapyridino-Ferrous Chloride (Yellow Salt)|year=1939|last1=Baudisch|first1=Oskar|last2=Hartung|first2=Walter H.|title=Inorganic Syntheses|pages=184–185|volume=1|isbn=978-0-470-13232-6}}</ref>]] |
|
FeCl<sub>2</sub> forms complexes with many ligands. It reacts with two molar equivalents of Cl to give the salt <sub>2</sub>. Related compounds that can be prepared similarly include the <sup>2<nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, and <sup>2<nowiki>−</nowiki></sup> salts.<ref>{{cite journal | author = N. S. Gill, F. B. Taylor | journal = ] | year = 1967 | volume = 9 | pages = 136–142 | doi = 10.1002/9780470132401.ch37 | title = Tetrahalo Complexes of Dipositive Metals in the First Transition Series}}</ref> |
|
|
|
|
|
|
FeCl<sub>2</sub> and its hydrates form complexes with many ligands. For example, solutions of the hydrates react with two molar equivalents of Cl]] to give the salt <sub>2</sub>.<ref>{{cite book | author = N. S. Gill, F. B. Taylor | title = Inorganic Syntheses | journal = ] | year = 1967 | volume = 9 | pages = 136–142 | doi = 10.1002/9780470132401.ch37 | chapter = Tetrahalo Complexes of Dipositive Metals in the First Transition Series| isbn = 978-0-470-13240-1 }}</ref> |
|
|
|
|
|
The anhydrous FeCl<sub>2</sub>, which is soluble in THF,<ref name=FACica/> is a standard precursor in organometallic synthesis. FeCl<sub>2</sub> is used to generate ]es in situ for ]s.<ref>{{cite journal|journal=Org. Synth.|year=2014|volume=91|pages=83–92|doi=10.15227/orgsyn.091.0083|title=Cross-Coupling of Alkenyl/Aryl Carboxylates with Grignard Reagents via Fe-Catalyzed C-O Bond Activation|author=Bi-Jie Li |author2=Xi-Sha Zhang |author3=Zhang-Jie Shi |doi-access=free}}</ref> |
|
|
|
|
|
==Applications== |
|
==Applications== |
|
Ferrous chloride has a variety of niche applications, but the related compounds ] and ] enjoy more applications. Aside from use in the laboratory synthesis of iron complexes, ferrous chloride serves as a reducing ] in wastewater treatment, especially for wastes containing ]. It is the precursor to hydrated iron(III) oxides that are magnetic pigments.<ref name=Ullmann/> Ferrous chloride is employed as a reducing agent in many ] reactions. |
|
Unlike the related ] and ], ferrous chloride has few commercial applications. Aside from use in the laboratory synthesis of iron complexes, ferrous chloride serves as a coagulation and ] agent in ], especially for wastes containing ] or ]s.<ref>{{cite journal|jstor = 25046917|title = The Use of Ferrous Chloride to Control Dissolved Sulfides in Interceptor Sewers|journal = Journal (Water Pollution Control Federation)|volume = 61|issue = 2|pages = 230–236|last1 = Jameel|first1 = Pervez|year = 1989}}</ref> It is used for odor control in wastewater treatment. It is used as a precursor to make various grades of hematite that can be used in a variety of pigments. It is the precursor to hydrated iron(III) oxides that are magnetic pigments.<ref name=Ullmann/> FeCl<sub>2</sub> finds some use as a ] in ].<ref>{{cite encyclopedia|author=Andrew D. White |author2=David G. Hilmey |encyclopedia=Encyclopedia of Reagents for Organic Synthesis|doi=10.1002/047084289X.ri055.pub2|year=2009|chapter=Iron(II) Chloride|isbn = 978-0-471-93623-7}}</ref> |
|
|
|
|
|
==Natural occurrence== |
|
|
], (Fe,Ni)Cl<sub>2</sub>, is the natural counterpart, and a typically (though rarely occurring) meteoritic mineral.<ref>{{Cite web|url=https://www.mindat.org/min-2351.html|title=Lawrencite}}</ref> The natural form of the dihydrate is rokühnite - a very rare mineral.<ref>{{Cite web|url=https://www.mindat.org/min-3440.html|title=Rokühnite}}</ref> Related, but more complex (in particular, basic or hydrated) minerals are ], ] and ]. |
|
|
|
|
|
==References== |
|
==References== |
|
|
{{reflist}} |
|
<references/> |
|
|
|
|
|
|
==See also== |
|
==See also== |
| Line 92: |
Line 118: |
|
* ] |
|
* ] |
|
|
|
|
|
|
{{Antianemic preparations}} |
|
{{Iron compounds}} |
|
{{Iron compounds}} |
|
|
{{Chlorides}} |
|
|
|
|
|
] |
|
] |
|
] |
|
] |
|
] |
|
|
] |
|
] |
|
|
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|