Iron(II) oxalate: Difference between revisions
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|ImageFile1 = Iron(II)-oxalate-sample.jpg |
|ImageFile1 = Iron(II)-oxalate-sample.jpg |
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|ImageFile2 = Fe(C2O4)-2D-ionic.png |
|ImageFile2 = Fe(C2O4)-2D-ionic.png |
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|IUPACName = Iron(II) oxalate |
|IUPACName = Iron(II) oxalate |
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|OtherNames = Iron oxalate<br> Ferrous oxalate |
|OtherNames = Iron oxalate<br> Ferrous oxalate |
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|Section1 |
|Section1={{Chembox Identifiers |
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|CASNo1_Ref = {{cascite|correct|CAS}} |
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|CASNo1 = 516-03-0 |
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|CASNo2_Ref = {{cascite|correct|CAS}} |
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|CASNo2 = 6047-25-2 |
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|CASNo2_Comment = (dihydrate) |
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|UNII1_Ref = {{fdacite|correct|FDA}} |
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|UNII1 = DZP4YV3ICV |
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|UNII2_Ref = {{fdacite|correct|FDA}} |
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|UNII2 = Z6X3YBU50D |
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|UNII2_Comment = (dihydrate) |
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|EINECS = 208-217-4 |
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|Section2 |
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|Formula = FeC<sub>2</sub>O<sub>4</sub> (anhydrous)<br> FeC<sub>2</sub>O<sub>4</sub>{{hydrate|2}} (dihydrate) |
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|MolarMass = 143.86 g/mol (anhydrous)<br> 179.89 g/mol (dihydrate) |
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|Appearance = yellow powder |
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|Odor = odorless |
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|Density = 2.28 g/cm<sup>3</sup> |
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|MeltingPt = |
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| MeltingPtC = 190 |
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|MeltingPt_notes = dihydrate: {{convert|150-160|C|F K}}<br> (decomposes) |
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|BoilingPtC = |
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| Boiling_notes = <br> (anhydrous)<ref name=guidechem /> |
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|Solubility = dihydrate:<br> 0.097 g/100ml (25 °C)<ref>{{Cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=2084|title = Iron(II) oxalate dihydrate}}</ref> |
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| EUClass = {{Hazchem Xn}} |
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| RPhrases = {{R21/22}} |
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| SPhrases = {{S24/25}} |
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| FlashPtC = 188.8 |
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'''Ferrous oxalate''' |
'''Ferrous oxalate''' ('''iron(II) oxalate''') are [[inorganic compound]] with the formula FeC<sub>2</sub>O<sub>4</sub>(H<sub>2</sub>O)<sub>x</sub> where x is 0 or 2. These are orange compounds, poorly soluble in water. |
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==Structure and reactions== |
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Like other iron oxalates, ferrous oxalates feature octahedral Fe centers. The dihydrate FeC<sub>2</sub>O<sub>4</sub>(H<sub>2</sub>O)<sub>x</sub> is a [[coordination polymer]], consisting of chains of oxalate-bridged ferrous centers, each with two aquo ligands.<ref>{{ cite journal |first1= Takuya |last1= Echigo |first2= Mitsuyoshi |last2= Kimata |title= Single-crystal X-ray diffraction and spectroscopic studies on humboldtine and lindbergite: weak Jahn–Teller effect of Fe<sup>2+</sup> ion |journal= [[Physics and Chemistry of Minerals]] |year= 2008 |volume= 35 |issue= 8 |pages= 467–475 |doi= 10.1007/s00269-008-0241-7 |bibcode= 2008PCM....35..467E |s2cid= 98739882}}</ref><br /> |
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[[File:Fe(C2O4)(H2O)2-chain-from-xtal-2008-CM-3D-balls.png|400px|Ball-and-stick model of a chain in the crystal structure of iron(II) oxalate dihydrate]] |
[[File:Fe(C2O4)(H2O)2-chain-from-xtal-2008-CM-3D-balls.png|400px|Ball-and-stick model of a chain in the crystal structure of iron(II) oxalate dihydrate]] |
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When heated to 120 °C, the dihydrate dehydrates, and the anhydrous ferrous oxalate decomposes near 190 °C.<ref>{{cite journal |doi=10.1016/0040-6031(81)80175-x |title=Thermal decomposition of carbonates, carboxylates, oxalates, acetates, formates, and hydroxides |date=1981 |last1=Mu |first1=Jacob |last2=Perlmutter |first2=D.D. |journal=Thermochimica Acta |volume=49 |issue=2–3 |pages=207–218 }}</ref> The products of thermal decomposition is a mixture of iron oxides and [[pyrophoric]] iron metal, as well as released [[carbon dioxide]], [[carbon monoxide]], and water.<ref>{{cite journal |title= Thermal Behaviour of Iron(II) Oxalate Dihydrate in the Atmosphere of Its Conversion Gases |first1= Martin |last1=Hermanek |first2=Radek |last2=Zboril |first3=Miroslav |last3=Mashlan |first4=Libor |last4=Machala |first5=Oldrich |last5=Schneeweiss |journal= J. Mater. Chem. |date= 2006 |volume= 16 |issue= 13 |pages= 1273–1280|doi= 10.1039/b514565a}}</ref> |
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When heated, it dehydrates and decomposes into [[carbon dioxide]], [[carbon monoxide]], iron oxides and [[pyrophoric]] black iron. |
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<ref>{{cite journal |title= Thermal behaviour of iron(II) oxalate dihydrate in the atmosphere of its conversion gases |first1= Martin |last1=Hermanek |first2=Radek |last2=Zboril |first3=Miroslav |last3=Mashlan |first4=Libor |last4=Machala |first5=Oldrich |last5=Schneeweiss |display-authors= 3 |journal= J. Mater. Chem. |date= 2006 |volume= 16 |pages= 1273-1280}}</ref> |
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Ferrous oxalates are precursors to [[iron phosphate]]s, which are of value in batteries.<ref>{{cite journal |doi=10.1038/nmat2007 |title=A multifunctional 3.5 V iron-based phosphate cathode for rechargeable batteries |date=2007 |last1=Ellis |first1=B. L. |last2=Makahnouk |first2=W. R. M. |last3=Makimura |first3=Y. |last4=Toghill |first4=K. |last5=Nazar |first5=L. F. |journal=Nature Materials |volume=6 |issue=10 |pages=749–753 |pmid=17828278 |bibcode=2007NatMa...6..749E }}</ref> |
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==Natural occurrence== |
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==Safety== |
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Anhydrous iron(II) oxalate is unknown among minerals as of 2020. However, the dihydrate is known as [[humboldtine]].<ref>{{Cite web|url=https://www.mindat.org/min-1946.html|title=Humboldtine}}</ref><ref name=IMA>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> A related, though much more complex mineral is [[stepanovite]],<br> |
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{{Unreferenced section|date=February 2015}} |
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Na[Mg(H<sub>2</sub>O)<sub>6</sub>] [Fe<sup>3+</sup>(C<sub>2</sub>O<sub>4</sub>)<sub>3</sub>]·3H<sub>2</sub>O - an example of trioxalatoferrate(III).<ref>{{Cite web|url=https://www.mindat.org/min-3763.html|title=Stepanovite}}</ref><ref name=IMA>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> |
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Iron(II) oxalate is harmful when swallowed. It may cause irritation to eyes and skin. |
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==See also== |
==See also== |
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A number of other iron oxalates are known |
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* [[Iron(III) oxalate]] |
* [[Iron(III) oxalate]] |
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* [[Potassium ferrioxalate]] |
* [[Potassium ferrioxalate]] |
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{{Iron compounds}} |
{{Iron compounds}} |
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{{Oxalates}} |
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[[Category:Iron compounds]] |
[[Category:Iron(II) compounds]] |
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[[Category:Oxalates]] |
[[Category:Oxalates]] |
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[[Category:Inorganic compounds]] |
Latest revision as of 03:54, 5 February 2024
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Names | |
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IUPAC name
Iron(II) oxalate
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Other names
Iron oxalate
Ferrous oxalate | |
Identifiers | |
3D model (JSmol)
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ECHA InfoCard | 100.007.472 |
EC Number |
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PubChem CID
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UNII |
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CompTox Dashboard (EPA)
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Properties | |
FeC2O4 (anhydrous) FeC2O4 · 2 H2O (dihydrate) | |
Molar mass | 143.86 g/mol (anhydrous) 179.89 g/mol (dihydrate) |
Appearance | yellow powder |
Odor | odorless |
Density | 2.28 g/cm3 |
Melting point | dihydrate: 150–160 °C (302–320 °F; 423–433 K) (decomposes) |
dihydrate: 0.097 g/100ml (25 °C)[1] | |
Hazards | |
GHS labelling: | |
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Warning | |
H302, H312[2] | |
P280[2] | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ferrous oxalate (iron(II) oxalate) are inorganic compound with the formula FeC2O4(H2O)x where x is 0 or 2. These are orange compounds, poorly soluble in water.
Structure and reactions
[edit]Like other iron oxalates, ferrous oxalates feature octahedral Fe centers. The dihydrate FeC2O4(H2O)x is a coordination polymer, consisting of chains of oxalate-bridged ferrous centers, each with two aquo ligands.[3]
When heated to 120 °C, the dihydrate dehydrates, and the anhydrous ferrous oxalate decomposes near 190 °C.[4] The products of thermal decomposition is a mixture of iron oxides and pyrophoric iron metal, as well as released carbon dioxide, carbon monoxide, and water.[5]
Ferrous oxalates are precursors to iron phosphates, which are of value in batteries.[6]
Natural occurrence
[edit]Anhydrous iron(II) oxalate is unknown among minerals as of 2020. However, the dihydrate is known as humboldtine.[7][8] A related, though much more complex mineral is stepanovite,
Na[Mg(H2O)6] [Fe3+(C2O4)3]·3H2O - an example of trioxalatoferrate(III).[9][8]
See also
[edit]References
[edit]- ^ "Iron(II) oxalate dihydrate".
- ^ a b c Sigma-Aldrich Co., Iron(II) oxalate dihydrate. Retrieved on 2014-05-03.
- ^ Echigo, Takuya; Kimata, Mitsuyoshi (2008). "Single-crystal X-ray diffraction and spectroscopic studies on humboldtine and lindbergite: weak Jahn–Teller effect of Fe2+ ion". Physics and Chemistry of Minerals. 35 (8): 467–475. Bibcode:2008PCM....35..467E. doi:10.1007/s00269-008-0241-7. S2CID 98739882.
- ^ Mu, Jacob; Perlmutter, D.D. (1981). "Thermal decomposition of carbonates, carboxylates, oxalates, acetates, formates, and hydroxides". Thermochimica Acta. 49 (2–3): 207–218. doi:10.1016/0040-6031(81)80175-x.
- ^ Hermanek, Martin; Zboril, Radek; Mashlan, Miroslav; Machala, Libor; Schneeweiss, Oldrich (2006). "Thermal Behaviour of Iron(II) Oxalate Dihydrate in the Atmosphere of Its Conversion Gases". J. Mater. Chem. 16 (13): 1273–1280. doi:10.1039/b514565a.
- ^ Ellis, B. L.; Makahnouk, W. R. M.; Makimura, Y.; Toghill, K.; Nazar, L. F. (2007). "A multifunctional 3.5 V iron-based phosphate cathode for rechargeable batteries". Nature Materials. 6 (10): 749–753. Bibcode:2007NatMa...6..749E. doi:10.1038/nmat2007. PMID 17828278.
- ^ "Humboldtine".
- ^ a b "List of Minerals". 21 March 2011.
- ^ "Stepanovite".