Iron(II) oxalate

Iron(II) oxalate
Names
	IUPAC name Iron(II) oxalate
	Other names Iron oxalate; Ferrous oxalate
Identifiers
CAS Number	516-03-0 ; 6047-25-2 (dihydrate) ;
3D model (JSmol)	Interactive image;
ECHA InfoCard	100.007.472
EC Number	208-217-4;
PubChem CID	10589;
UNII	DZP4YV3ICV ; Z6X3YBU50D (dihydrate) ;
CompTox Dashboard (EPA)	DTXSID4060159 ;
	InChI InChI=1S/3C2H2O4.2Fe/c33-1(4)2(5)6;;/h3(H,3,4)(H,5,6);;/q;;;2*+3/p-6 Key: VEPSWGHMGZQCIN-UHFFFAOYSA-H ;
	SMILES [Fe+2].O=C([O-])-C([O-])=O;
Properties
Chemical formula	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	190 °C (374 °F; 463 K) ; (anhydrous); 150–160 °C (302–320 °F; 423–433 K); (dihydrate) decomposes
Boiling point	365.1 °C (689.2 °F; 638.2 K) ; (anhydrous)
Solubility in water	dihydrate:; 0.097 g/100ml (25 °C)
Hazards
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H302, H312
Precautionary statements	P280
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Ferrous oxalate, or iron(II) oxalate, is an inorganic compound with the formula FeC₂O₄ · $x$ H₂O where $x$ is typically 2. These are orange compounds, poorly soluble in water.

Structure

The dihydrate FeC₂O₄ · 2 H₂O is a coordination polymer, consisting of chains of oxalate-bridged ferrous centers, each with two aquo ligands.^[4]

When heated, it dehydrates and decomposes into a mixture of iron oxides and pyrophoric iron metal, with release of carbon dioxide, carbon monoxide, and water.^[5]

References

^ ^a ^b http://www.guidechem.com/cas-516/516-03-0.html
^ http://chemister.ru/Database/properties-en.php?dbid=1&id=2084
^ ^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". Phys. Chem. Minerals. 35: 467–475. doi:10.1007/s00269-008-0241-7.
^ Hermanek, Martin; Zboril, Radek; Mashlan, Miroslav; et al. (2006). "Thermal behaviour of iron(II) oxalate dihydrate in the atmosphere of its conversion gases". J. Mater. Chem. 16: 1273–1280.

[guidechem-1] ttp://www.guidechem.com/cas-516/516-03-0.html

[2] ttp://chemister.ru/Database/properties-en.php?dbid=1&id=2084

[sigma-3] Sigma-Aldrich Co., Iron(II) oxalate dihydrate. Retrieved on 2014-05-03.

[4] Echigo, Takuya; Kimata, Mitsuyoshi (2008). "Single-crystal X-ray diffraction and spectroscopic studies on humboldtine and lindbergite: weak Jahn–Teller effect of Fe²⁺ ion". Phys. Chem. Minerals. 35: 467–475. doi:10.1007/s00269-008-0241-7.

[5] Hermanek, Martin; Zboril, Radek; Mashlan, Miroslav; et al. (2006). "Thermal behaviour of iron(II) oxalate dihydrate in the atmosphere of its conversion gases". J. Mater. Chem. 16: 1273–1280.

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Structure

See also

References