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{{chembox
{{chembox
| Verifiedfields = changed
|Verifiedfields = changed
| Watchedfields = changed
|Watchedfields = changed
| verifiedrevid = 409714131
|verifiedrevid = 409714131
|ImageFile1 = Iron(II)-oxalate-sample.jpg
|ImageFile1 = Iron(II)-oxalate-sample.jpg
|ImageFile2 = Fe(C2O4)-2D-ionic.png
|ImageFile2 = Fe(C2O4)-2D-ionic.png
|IUPACName = Iron(II) oxalate
|IUPACName = Iron(II) oxalate
|OtherNames = Iron oxalate<br> Ferrous oxalate
|OtherNames = Iron oxalate<br> Ferrous oxalate
|Section1 = {{Chembox Identifiers
|Section1={{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
|CASNo1_Ref = {{cascite|correct|CAS}}
| CASNo = 516-03-0
|CASNo1 = 516-03-0
|CASNo2_Ref = {{cascite|correct|CAS}}
⚫
| PubChem =10589
| EINECS = 208-217-4
|CASNo2 = 6047-25-2
|CASNo2_Comment = (dihydrate)
⚫
| SMILES = [Fe+3].[Fe+3].O=C([O-])C([O-])=O.[O-]C(=O)C([O-])=O.[O-]C(=O)C([O-])=O
|UNII1_Ref = {{fdacite|correct|FDA}}
⚫
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
|UNII1 = DZP4YV3ICV
⚫
| StdInChI = 1S/3C2H2O4.2Fe/c3*3-1(4)2(5)6;;/h3*(H,3,4)(H,5,6);;/q;;;2*+3/p-6
|UNII2_Ref = {{fdacite|correct|FDA}}
⚫
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
|UNII2 = Z6X3YBU50D
⚫
| StdInChIKey = VEPSWGHMGZQCIN-UHFFFAOYSA-H
|UNII2_Comment = (dihydrate)
⚫
|PubChem =10589
|EINECS = 208-217-4
⚫
|SMILES = [Fe+2].O=C([O-])-C([O-])=O
⚫
|StdInChI_Ref = {{stdinchicite|changed|chemspider}}
⚫
|StdInChI = 1S/3C2H2O4.2Fe/c3*3-1(4)2(5)6;;/h3*(H,3,4)(H,5,6);;/q;;;2*+3/p-6
⚫
|StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
⚫
|StdInChIKey = VEPSWGHMGZQCIN-UHFFFAOYSA-H
}}
}}
|Section2 = {{Chembox Properties
|Section2={{Chembox Properties
| Formula = FeC<sub>2</sub>O<sub>4</sub> (anhydrous)<br> FeC<sub>2</sub>O<sub>4</sub>·2 H<sub>2</sub>O (dihydrate)
|Formula = FeC<sub>2</sub>O<sub>4</sub> (anhydrous)<br> FeC<sub>2</sub>O<sub>4</sub>{{hydrate|2}} (dihydrate)
| MolarMass = 143.86 g/mol (anhydrous)<br> 179.89 g/mol (dihydrate)
|MolarMass = 143.86 g/mol (anhydrous)<br> 179.89 g/mol (dihydrate)
| Appearance = yellow powder
|Appearance = yellow powder
| Odor = odorless
|Odor = odorless
| Density = 2.28 g/cm<sup>3</sup>
|Density = 2.28 g/cm<sup>3</sup>
|MeltingPt =
| MeltingPtC = 190
| Melting_notes = <br> (anhydrous)<ref name=guidechem>http://www.guidechem.com/cas-516/516-03-0.html</ref><br> {{convert|150-160|C|F K}}<br> (dihydrate) decomposes
|MeltingPt_notes = dihydrate: {{convert|150-160|C|F K}}<br> (decomposes)
| BoilingPtC = 365.1
|BoilingPtC =
|BoilingPt_notes =
| Boiling_notes = <br> (anhydrous)<ref name=guidechem />
| Solubility = dihydrate:<br> 0.097 g/100ml (25 °C)<ref>http://chemister.ru/Database/properties-en.php?dbid=1&id=2084</ref>
|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>
⚫
}}
⚫
|Section3={{Chembox Hazards
⚫
|GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=255971|name=Iron(II) oxalate dihydrate|accessdate=2014-05-03}}</ref>
⚫
|GHSSignalWord = Warning
⚫
|HPhrases = {{H-phrases|302|312}}<ref name="sigma" />
⚫
|PPhrases = {{P-phrases|280}}<ref name="sigma" />
}}
}}
⚫
|Section3 = {{Chembox Hazards
⚫
| GHSPictograms = {{GHSp|GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=255971|name=Iron(II) oxalate dihydrate|accessdate=2014-05-03}}</ref>
⚫
| GHSSignalWord = Warning
⚫
| HPhrases = {{H-phrases|302|312}}<ref name="sigma" />
⚫
| PPhrases = {{P-phrases|280}}<ref name="sigma" />
| EUClass = {{Hazchem Xn}}
| RPhrases = {{R21/22}}
| SPhrases = {{S24/25}}
| MainHazards =
| FlashPtC = 188.8
| Autoignition =
⚫
}}
}}
}}


'''Ferrous oxalate''', or '''iron(II) oxalate''', is a [[chemical compound]] consisting of one [[Ferrous|iron(II) ion]] (Fe<sup>2+</sup>) and one [[oxalate]] ion (C<sub>2</sub>O<sub>4</sub><sup>2−</sup>). It has the [[chemical formula]] FeC<sub>2</sub>O<sub>4</sub>.
'''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.


==Structure and reactions==
Iron(II) oxalate is more commonly encountered as the [[hydrate|dihydrate]], FeC<sub>2</sub>O<sub>4</sub>·2H<sub>2</sub>O, CAS # 6047-25-2. Its crystal structure consists of chains of oxalate-bridged iron atoms, capped by water molecules.<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|Phys. Chem. Minerals]] |year= 2008 |volume= 35 |pages= 467–475 |doi= 10.1007/s00269-008-0241-7 }}</ref><br />
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 />
[[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]]


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>
When heated, it dehydrates and decomposes into [[carbon dioxide]], [[carbon monoxide]], iron oxides and [[pyrophoric]] black iron.

<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>
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>


==Natural occurrence==
==Safety==
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>
{{Unreferenced section|date=February 2015}}
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>
Iron(II) oxalate is harmful when swallowed. It may cause irritation to eyes and skin.


==See also==
==See also==
A number of other iron oxalates are known
* [[Iron(III) oxalate]]
* [[Iron(III) oxalate]]
* [[Potassium ferrioxalate]]
* [[Potassium ferrioxalate]]
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{{Iron compounds}}
{{Iron compounds}}
{{Oxalates}}


[[Category:Iron compounds]]
[[Category:Iron(II) compounds]]
[[Category:Oxalates]]
[[Category:Oxalates]]
[[Category:Inorganic compounds]]

Latest revision as of 03:54, 5 February 2024

Iron(II) oxalate
Names
IUPAC name
Iron(II) oxalate
Other names
Iron oxalate
Ferrous oxalate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.007.472 Edit this at Wikidata
EC Number
  • 208-217-4
UNII
  • InChI=1S/3C2H2O4.2Fe/c3*3-1(4)2(5)6;;/h3*(H,3,4)(H,5,6);;/q;;;2*+3/p-6 ☒N
    Key: VEPSWGHMGZQCIN-UHFFFAOYSA-H ☒N
  • [Fe+2].O=C([O-])-C([O-])=O
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:
GHS07: Exclamation mark[2]
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).
☒N verify (what is checkY☒N ?)

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]
Ball-and-stick model of a chain in the crystal structure of iron(II) oxalate dihydrate

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]
  1. ^ "Iron(II) oxalate dihydrate".
  2. ^ a b c Sigma-Aldrich Co., Iron(II) oxalate dihydrate. Retrieved on 2014-05-03.
  3. ^ 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.
  4. ^ 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.
  5. ^ 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.
  6. ^ 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.
  7. ^ "Humboldtine".
  8. ^ a b "List of Minerals". 21 March 2011.
  9. ^ "Stepanovite".
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