Iron(II) oxalate
Chemical compound From Wikipedia, the free encyclopedia
Ferrous oxalate (iron(II) oxalate) refers to inorganic compounds with the formula FeC2O4(H2O)x where x is 0 or 2. These are yellow compounds. Characteristic of metal oxalate complexes, these compounds tend to be polymeric, hence their low solubility in water.
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Names | |
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IUPAC name
Iron(II) oxalate | |
Other names
Iron oxalate Ferrous oxalate | |
Identifiers | |
3D model (JSmol) |
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ChemSpider | |
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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Structure and reactions
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
Anhydrous iron(II) oxalate is unknown among minerals as of 2020. However, the dihydrate is known as humboldtine.[7][8] A related, although much more complex mineral is stepanovite.
Na[Mg(H2O)6][Fe(III)(C2O4)3]·3H2O is an unusual example of a naturally-occurring ferrioxalate.[9][8]
See also
References
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