Iron(II) oxalate
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| Iron(II) oxalate | ||
|---|---|---|
-oxalate-sample.jpg) | ||
-2D-ionic.png) | ||
| Other names Iron oxalate | ||
| Identifiers | ||
| CAS number | 516-03-0  | |
| PubChem | 10589 | |
| EC number | 208-217-4 | |
| Properties | ||
| Molecular formula | FeC2O4 | |
| Molar mass | 143.91 g/mol | |
| Appearance | yellow powder | |
| Odor | odorless | |
| Density | 2.28 g/cm3 (dihydrate) | |
| Melting point | 150-160 °C, decomp (dihydrate) | |
| Solubility in water | slightly soluble | |
(verify) (what is: / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | ||
| Infobox references | ||
Ferrous oxalate, or iron(II) oxalate, is a chemical compound consisting of one iron(II) ion (Fe2+) and one oxalate ion (C2O42−). It has the chemical formula FeC2O4.
Iron(II) oxalate is more commonly encountered as the dihydrate, FeC2O4·2H2O, CAS # 6047-25-2. Its crystal structure consists of chains of oxalate-bridged iron atoms, capped by water molecules.[1]
(H2O)2-chain-from-xtal-2008-CM-3D-balls.png)
When heated, it dehydrates and decomposes into carbon dioxide, carbon monoxide, iron oxides and pyrophoric black iron. [2]
References
- ↑ 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.
- ↑ Thermal behaviour of iron(II) oxalate dihydrate in the atmosphere of its conversion gases, Martin Hermanek, Radek Zboril, Miroslav Mashlan, Libor Machala and Oldrich Schneeweiss 1. Centre for Nanomaterial Research,Palacky University, Svobody 26, , Czech Republic 2. Institute of Physics of Materials AS CR, Žižkova 22, , Czech Republic J. Mater. Chem., 2006,16, 1273-1280
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