Iron(II) carbonate
Template:Short description Template:Chembox Iron(II) carbonate, or ferrous carbonate, is a chemical compound with formula Template:Chem, that occurs naturally as the mineral siderite. At ordinary ambient temperatures, it is a green-brown ionic solid consisting of iron(II) cations Template:Chem and carbonate anions Template:Chem.[1] The compound crystallizes in the same motif as calcium carbonate. In this motif, the carbonate dianion is nearly planar. Its three oxygen atoms each bind to two Fe(II) centers, such that the Fe has an octahedral coordination geometry.[2]
Preparation
Ferrous carbonate can be prepared by reacting solution of the two ions, such as iron(II) chloride and sodium carbonate:[1]
Ferrous carbonate can be prepared also from solutions of an iron(II) salt, such as iron(II) perchlorate, with sodium bicarbonate, releasing carbon dioxide:[3]
- Template:Chem(Template:Chem)2 + 2Template:Chem → Template:Chem + 2Template:Chem + Template:Chem + Template:Chem
Sel and others used this reaction (but with Template:Chem instead of Template:Chem(Template:Chem)2) at 0.2 M to prepare amorphous Template:Chem.[4]
Care must be taken to exclude oxygen Template:Chem from the solutions, because the Template:Chem ion is easily oxidized to Template:Chem, especially at pH above 6.0.[3]
Ferrous carbonate also forms directly on steel or iron surfaces exposed to solutions of carbon dioxide, forming an "iron carbonate" scale:[5]
Properties
The dependency of the solubility in water with temperature was determined by Wei Sun and others to be
where T is the absolute temperature in kelvins, and I is the ionic strength of the liquid.[5]
Iron carbonate decomposes at about Template:Convert.[6]
Uses
Ferrous carbonate has been used as an iron dietary supplement to treat anemia.[7] It is noted to have very poor bioavailability in cats and dogs.[8]
Toxicity
Ferrous carbonate is slightly toxic; the probable oral lethal dose is between 0.5 and 5 g/kg (between 35 and 350 g for a 70 kg person).[9]
Iron(III) carbonate
Unlike iron(II) carbonate, iron(III) carbonate has not been isolated. Attempts to produce iron(III) carbonate by the reaction of aqueous ferric ions and carbonate ions result in the production of iron(III) oxide with the release of carbon dioxide or bicarbonate.[10]
References
- ↑ 1.0 1.1 (1995): "Kirk-Othmer Encyclopedia of Chemical Technology". 4th ed. Volume 1.
- ↑ Template:Cite journal
- ↑ 3.0 3.1 Template:Cite journal
- ↑ Ozlem Sel, A.V. Radha, Knud Dideriksen, and Alexandra Navrotsky (2012): "Amorphous iron (II) carbonate: Crystallization energetics and comparison to other carbonate minerals related to CO2 sequestration". Geochimica et Cosmochimica Acta, volume 87, issue 15, pages 61–68. Template:Doi
- ↑ 5.0 5.1 Wei Sun (2009): "Kinetics of iron carbonate and iron sulfide scale formation in CO2/H2S corrosion". PhD Thesis, Ohio University.
- ↑ Template:Cite journal
- ↑ A .Osol and J. E. Hoover and others, eds. (1975): "Remington's Pharmaceutical Sciences". 15th ed. Mack Publishing. Page 775
- ↑ Template:Cite web
- ↑ Gosselin, R.E., H.C. Hodge, R.P. Smith, and M.N. Gleason. Clinical Toxicology of Commercial Products. 4th ed. Baltimore: Williams and Wilkins, 1976., p. II-97
- ↑ Template:Cite book
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Template:Carbonates Template:Iron compounds Template:Antianemic preparations