Iron(II) oxalate

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Iron(II) oxalate
Iron(II)-oxalate-sample.jpg
Fe(C2O4)-2D-ionic.png
Identifiers
CAS number 516-03-0 YesY
PubChem 10589
EC number 208-217-4
Jmol-3D images Image 1
Properties
Molecular 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)[2]
150–160 °C (302–320 °F; 423–433 K)
(dihydrate) decomposes
Boiling point 365.1 °C (689.2 °F; 638.2 K)
(anhydrous)[2]
Solubility in water dihydrate:
0.097 g/100ml (25 °C)[1]
Hazards
GHS pictograms GHS-pictogram-exclam.svg[3]
GHS signal word Warning
GHS hazard statements H302, H312[3]
GHS precautionary statements P280[3]
EU classification Harmful Xn
R-phrases R21/22
S-phrases S24/25
Flash point 188.8 °C (371.8 °F; 461.9 K)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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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.[4] Ball-and-stick model of a chain in the crystal structure of iron(II) oxalate dihydrate

When heated, it dehydrates and decomposes into carbon dioxide, carbon monoxide, iron oxides and pyrophoric black iron. [5]

Safety[edit]

Harmful when swallowed. It may cause irritation to eyes and skin. Avoid inhalation of dusts.

References[edit]

  1. ^ http://chemister.ru/Database/properties-en.php?dbid=1&id=2084
  2. ^ a b http://www.guidechem.com/cas-516/516-03-0.html
  3. ^ a b c 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. ^ 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