Iron(III) phosphate

Iron(III) phosphate, also ferric phosphate,[3][4] is the inorganic compound with the formula FePO₄. Several related materials are known, including four polymorphs of FePO₄ and two polymorphs of the dihydrate FePO₄·(H₂O)₂. These materials find few technical applications as well as occurring in the mineral kingdom.[5][6]

Iron(III) phosphate

Names
IUPAC name Iron(III) phosphate
Other names Ferric orthophosphate, Ferric phosphate
Identifiers
CAS Number	10045-86-0 (anhydrous) 13463-10-0 (dihydrate)
3D model (JSmol)	Interactive image
ChEBI	CHEBI:131371
ChemSpider	23244
ECHA InfoCard	100.030.123
PubChem CID	24861
UNII	N6BAA189V1
CompTox Dashboard (EPA)	DTXSID9035672
InChI InChI=1S/Fe.H3O4P/c;1-5(2,3)4/h;(H3,1,2,3,4)/q+3;/p-3 Key: WBJZTOZJJYAKHQ-UHFFFAOYSA-K
SMILES [O-]P(=O)([O-])[O-].[Fe+3]
Properties
Chemical formula	FePO4
Molar mass	150.815 g/mol (anhydrous)
Appearance	yellow-brown solid
Density	3.056 g/cm^3 (anhydrous) 2.87 g/cm^3 (20 °C, dihydrate)
Melting point	250 °C (482 °F; 523 K) (dihydrate) decomposes[1]
Solubility in water	anhydrous: insoluble dihydrate: 0.642 g/100 mL (100 °C)[1]
Magnetic susceptibility (χ)	+11,500.0·10^−6 cm^3/mol
Thermochemistry
Heat capacity (C)	180.5 J/mol·K (dihydrate)[1]
Std molar entropy (S^o298)	171.3 J/mol·K (dihydrate)[1]
Std enthalpy of formation (ΔfH^⦵298)	-1888 kJ/mol (dihydrate)[1]
Hazards
GHS pictograms	[2]
GHS Signal word	Warning
GHS hazard statements	H315, H319, H335[2]
GHS precautionary statements	P261, P305+351+338[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Structure

The most common form of FePO₄ adopts the structure of α-quartz. As such the material consists of tetrahedral Fe(III) and phosphate sites.[7] As such the P and Fe have tetrahedral molecular geometry. At high pressures, a phase change occurs to a more dense structure with octahedral Fe centres. Two orthorhombic structures and a monoclinic phase are also known. In the two polymorphs of the dihydrate, the Fe centre is octahedral with two mutually cis water ligands.[8]

Uses

Iron(III) phosphate can be used in steel and metal manufacturing processes. When bonded to a metal surface, iron phosphate prevents further oxidation of the metal. Its presence is partially responsible for the corrosion resistance of the Iron pillar of Delhi.

Iron phosphate coatings are commonly used in preparation for painting or powder coating, in order to increase adhesion to the iron or steel substrate, and prevent corrosion, which can cause premature failure of subsequent coating processes. It can also be used for bonding fabrics, wood, and other materials to iron or steel surfaces.

Anhydrous iron phosphate has been investigated as an intercalation electrode in a lithium-ion battery despite having low electronic conductivity.

Pesticide

Iron phosphate is one of the few molluscicides approved for use in the practice of organic farming.[9]

Pesticide pellets containing iron phosphate plus a chelating agent, such as EDTA, leach heavy metals from soil into groundwater.[10] The Research Institute of Organic Agriculture (FiBL) reported the EDTA content and stated products were likely to be no safer than metaldehyde baits.[11] Ferric phosphate slug and snail baits marketed in the U.S. contain EDTA.[12]

Legislation

Iron(III) phosphate is not allowed as food additive in the European Union. It was withdrawn from the list of allowed substances in the directive 2002/46/EC in 2007.

See also

• Iron(II) phosphate, commonly known as ferrous phosphate, the lower phosphate of iron
• Lithium iron phosphate battery, a battery that uses iron phosphate
• Phosphate conversion coating, an industrial process used to protect newly manufactured iron and steel from corrosion

References

1. "iron(III) phosphate dihydrate". chemister.ru. Retrieved 3 July 2014.
2. Sigma-Aldrich Co., Iron(III) phosphate dihydrate. Retrieved on 2014-05-03.
3. "Iron(III) Phosphate". NIH, U.S. National Library of Medicine. Retrieved 22 January 2016.
4. "FERRIC PHOSPHATE". EndMemo.com. Retrieved 22 January 2016.
5. Roncal-Herrero, T., Rodriguez-Blanco, J.D., Benning, L.G., Oelkers, E.H. (2009) Precipitation of Iron and Aluminium Phosphates Directly from Aqueous Solution as a Function of Temperature from 50 to 200°C. Crystal Growth & Design, 9, 5197-5205. doi: 10.1021/cg900654m.
6. Song, Y.; Zavalij, P. Y.; Suzuki, M.; Whittingham, M. S. (2002). "New Iron(III) Phosphate Phases: Crystal Structure and Electrochemical and Magnetic Properties" (PDF). Inorganic Chemistry. 41 (22): 5778–5786. doi:10.1021/ic025688q. PMID 12401083. Archived from the original (PDF) on 14 July 2014. Retrieved 3 July 2014.
7. Haines, J.; Cambon, O.; Hull, S. (2003). "A neutron diffraction study of quartz-type FePO4: High-temperature behavior and α–β phase transition". Zeitschrift für Kristallographie - Crystalline Materials. 218 (3): 193. Bibcode:2003ZK....218..193H. doi:10.1524/zkri.218.3.193.20755. S2CID 98195900.
8. Zaghib, K.; Julien, C. M. (January 2005). "Structure and electrochemistry of FePO₄·2H₂O hydrate". Journal of Power Sources. 142 (1–2): 279–284. Bibcode:2005JPS...142..279Z. doi:10.1016/j.jpowsour.2004.09.042. Retrieved 3 July 2014.
9. "COMMISSION REGULATION (EC) No 889/2008". European Union law. Retrieved 3 July 2014.
10. "The Regional Institute - Slugs, Snails and Iron based Baits: An Increasing Problem and a Low Toxic Specific Action Solution 1". www.regional.org.au. 11 September 2018.
11. "Archived copy" (PDF). Archived from the original (PDF) on 2007-07-10. Retrieved 2016-03-05.CS1 maint: archived copy as title (link)
12. "National Organic Standards Board Crops Subcommittee Petitioned Material Proposal Ferric Phosphate (to Remove)" (PDF). August 15, 2012.

External links