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[4][5] is an inorganic compound with the formula FePO4. Four polymorphs of anhydrous FePO4 are known. Additionally, two polymorphs of the dihydrate FePO4·(H2O)2 are known. These polymorphs have attracted interest as potential cathode materials in batteries.

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.[6] 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.[7]

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.[citation needed]

Iron phosphate is used[8] to make lithium iron phosphate, the cathode in lithium iron phosphate batteries.[9][10]

Pesticide

Iron phosphate is one of the few molluscicides approved for use in the practice of organic farming.[11] Pesticide pellets can contain iron phosphate alone, or with a chelating agent, such as EDTA.[12]

Mineral

Strengite is the mineral form of hydrated ferric phosphate.

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 It was withdrawn from the list of allowed substances in the directive 2002/46/EC in 2007.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

References

  1. 1 2 3 “iron(III) phosphate dihydrate”. chemister.ru. Retrieved 3 July 2014.
  2. ↑ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  3. ↑ Sigma-Aldrich Co., Iron(III) phosphate dihydrate. Retrieved on 2014-05-03.
  4. ↑ “Iron(III) Phosphate”. NIH, U.S. National Library of Medicine. Retrieved 22 January 2016.
  5. ↑ “FERRIC PHOSPHATE”. EndMemo.com. Archived from the original on 28 February 2020. Retrieved 22 January 2016.
  6. ↑ 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.
  7. ↑ “Lithium iron phosphate comes to America”. Chemical & Engineering News. Retrieved 2023-09-12.
  8. ↑ 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.
  9. ↑ 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.
  10. ↑ “COMMISSION REGULATION (EC) No 889/2008”. European Union law. Retrieved 3 July 2014.
  11. ↑ “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.