Iron(III) phosphate
Names
IUPAC name
Iron(III) phosphate
Other names
Ferric orthophosphate, Ferric phosphate
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.123
UNII
  • InChI=1S/Fe.H3O4P/c;1-5(2,3)4/h;(H3,1,2,3,4)/q+3;/p-3 checkY
    Key: WBJZTOZJJYAKHQ-UHFFFAOYSA-K checkY
  • [O-]P(=O)([O-])[O-].[Fe+3]
Properties
FePO4
Molar mass 150.815 g/mol (anhydrous)
Appearance yellow-brown solid
Density 3.056 g/cm3 (anhydrous)
2.87 g/cm3 (20 °C, dihydrate)
Melting point 250 °C (482 °F; 523 K)
(dihydrate) decomposes[1]
anhydrous:
insoluble
dihydrate:
0.642 g/100 mL (100 °C)[1]
9.91×10−16[2]
+11,500.0·10−6 cm3/mol
Thermochemistry
180.5 J/mol·K (dihydrate)[1]
171.3 J/mol·K (dihydrate)[1]
-1888 kJ/mol (dihydrate)[1]
Hazards
GHS labelling:
GHS07: Exclamation mark[3]
Warning
H315, H319, H335[3]
P261, P305+P351+P338[3]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Iron(III) phosphate, also ferric phosphate,[4][5] is the 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 materials have attracted much 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.

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 contain iron phosphate plus 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 4 5 "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. 1 2 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. 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. ↑ 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.
  8. ↑ "Lithium iron phosphate comes to America". Chemical & Engineering News. Retrieved 2023-09-12.
  9. ↑ 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.
  10. ↑ 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.
  11. ↑ "COMMISSION REGULATION (EC) No 889/2008". European Union law. Retrieved 3 July 2014.
  12. ↑ "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.
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