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Tricalcium phosphate

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Tricalcium phosphate
Names
IUPAC name
Calcium phosphate
Other names
Tribasic calcium phosphate, tricalcium bis(phosphate)
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.028.946 Edit this at Wikidata
EC Number
  • 231-840-8
UNII
  • InChI=1S/3Ca.2H3O4P/c;;;2*1-5(2,3)4/h;;;2*(H3,1,2,3,4)/q3*+2;;/p-6 checkY
    Key: QORWJWZARLRLPR-UHFFFAOYSA-H checkY
  • InChI=1S/3Ca.2H3O4P/c;;;2*1-5(2,3)4/h;;;2*(H3,1,2,3,4)/q3*+2;;/p-6
    Key: QORWJWZARLRLPR-CYFPFDDLAC
  • Key: QORWJWZARLRLPR-UHFFFAOYSA-H
  • [O-]P(=O)([O-])[O-].[O-]P(=O)([O-])[O-].[Ca+2].[Ca+2].[Ca+2]
Properties
Ca3(PO4)2
Molar mass 310.18 g/mol
Appearance White amorphous powder
Density 3.14 g/cm3[1]
Melting point 1,670 °C (3,040 °F; 1,940 K)[1]
1.2 mg/kg[1]
2.07×10−33[2]
Thermochemistry
−4126 kJ/mol (α-form)[3]
Pharmacology
A12AA01 (WHO)
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Flash point Non-flammable
Related compounds
Other anions
 Calcium pyrophosphate
Other cations
 Trimagnesium phosphate
Trisodium phosphate
Tripotassium phosphate
Related compounds
 Monocalcium phosphate
Dicalcium phosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Tricalcium phosphate (sometimes abbreviated TCP), more commonly known as Calcium phosphate, is a calcium salt of phosphoric acid with the chemical formula Ca3(PO4)2. It is also known as tribasic calcium phosphate and bone phosphate of lime (BPL). It is a white solid of low solubility. Most commercial samples of "tricalcium phosphate" are in fact hydroxyapatite.[4][5]

It exists as three crystalline polymorphs α, α′, and β. The α and α′ states are stable at high temperatures.

Nomenclature

[edit]
Main article: Calcium phosphate

Calcium phosphate refers to numerous materials consisting of calcium ions (Ca2+) together with orthophosphates (PO3−
4), metaphosphates or pyrophosphates (P
2O4−
7) and occasionally oxide and hydroxide ions. Especially, the common mineral apatite has formula Ca5(PO4)3X, where X is F, Cl, OH, or a mixture; it is hydroxyapatite if the extra ion is mainly hydroxide. Much of the "tricalcium phosphate" on the market is actually powdered hydroxyapatite.[5]

Preparation

[edit]

Tricalcium phosphate is produced commercially by treating hydroxyapatite with phosphoric acid and slaked lime.[4]

It cannot be precipitated directly from aqueous solution. Typically double decomposition reactions are employed, involving a soluble phosphate and calcium salts, e.g. (NH4)2HPO4 + Ca(NO3)2.[6] is performed under carefully controlled pH conditions. The precipitate will either be "amorphous tricalcium phosphate", ATCP, or calcium deficient hydroxyapatite, CDHA, Ca9(HPO4)(PO4)5(OH), (note CDHA is sometimes termed apatitic calcium triphosphate).[6][7][8] Crystalline tricalcium phosphate can be obtained by calcining the precipitate. β-Ca3(PO4)2 is generally formed, higher temperatures are required to produce α-Ca3(PO4)2.

An alternative to the wet procedure entails heating a mixture of a calcium pyrophosphate and calcium carbonate:[7]

CaCO3 + Ca2P2O7 → Ca3(PO4)2 + CO2

Structure of β-, α- and α′- Ca3(PO4)2 polymorphs

[edit]

Tricalcium phosphate has three recognised polymorphs, the rhombohedral β form (shown above), and two high temperature forms, monoclinic α and hexagonal α′. β-Tricalcium phosphate has a crystallographic density of 3.066 g cm−3 while the high temperature forms are less dense, α-tricalcium phosphate has a density of 2.866 g cm−3 and α′-tricalcium phosphate has a density of 2.702 g cm−3 All forms have complex structures consisting of tetrahedral phosphate centers linked through oxygen to the calcium ions.[9] The high temperature forms each have two types of columns, one containing only calcium ions and the other both calcium and phosphate.[10]

There are differences in chemical and biological properties between the β and α forms, the α form is more soluble and biodegradable. Both forms are available commercially and are present in formulations used in medical and dental applications.[10]

Occurrence

[edit]

Calcium phosphate is one of the main combustion products of bone (see bone ash). Calcium phosphate is also commonly derived from inorganic sources such as mineral rock.[11] Tricalcium phosphate occurs naturally in several forms, including:

  • as a rock in Morocco, Israel, Philippines, Egypt, and Kola (Russia) and in smaller quantities in some other countries. The natural form is not completely pure, and there are some other components like sand and lime which can change the composition. The content of P2O5 in most calcium phosphate rocks is 30% to 40% P2O5 by weight.
  • in the skeletons and teeth of vertebrate animals
  • in milk.

Biphasic calcium phosphate, BCP

[edit]

Biphasic calcium phosphate, BCP, was originally reported as tricalcium phosphate, but X-Ray diffraction techniques showed that the material was an intimate mixture of two phases, hydroxyapatite (HA) and β-tricalcium phosphate.[12] It is a ceramic.[13] Preparation involves sintering, causing irreversible decomposition of calcium deficient apatites[7] alternatively termed non-stoichiometric apatites or basic calcium phosphate.[14] An example is:[15]

Ca10−δ(PO4)6−δ(HPO4)δ(OH)2−δ → (1−δ) Ca10(PO4)6(OH)2 + 3δ Ca3(PO4)2

β-TCP can contain impurities, for example calcium pyrophosphate, Ca2P2O7 and apatite. β-TCP is bioresorbable. The biodegradation of BCP involves faster dissolution of the β-TCP phase followed by elimination of HA crystals. β-TCP does not dissolve in body fluids at physiological pH levels, dissolution requires cell activity producing acidic pH.[7]

Uses

[edit]

Food additive

[edit]

Tricalcium phosphate is used in powdered spices as an anticaking agent, e.g. to prevent table salt from caking. The calcium phosphates have been assigned European food additive number E341.

Health and beauty products

[edit]

It is also found in baby powder, antacids and toothpaste.[4] Toothpastes with functionalized β-tricalcium phosphate (fTCP) may help remineralize tooth enamel.[16][17][18]

Biomedical

[edit]

It is also used as a nutritional supplement[19] and occurs naturally in cow milk,[citation needed] although the most common and economical forms for supplementation are calcium carbonate (which should be taken with food) and calcium citrate (which can be taken without food).[20] There is some debate about the different bioavailabilities of the different calcium salts.

It can be used as a tissue replacement for repairing bony defects when autogenous bone graft is not feasible or possible.[21][22][23] It may be used alone or in combination with a biodegradable, resorbable polymer such as polyglycolic acid.[24] It may also be combined with autologous materials for a bone graft.[25][26]

Porous β-tricalcium phosphate scaffolds are employed as drug carrier systems for local drug delivery in bone.[27]

Natural occurrence

[edit]

Tuite, a natural analogue of tricalcium orthophosphate(V), is a rare component of some meteorites. Its formation is related to shock metamorphism.[28]

References

[edit]
  1. ^ a b c Haynes, William M., ed. (2016). CRC Handbook of Chemistry and Physics (97th ed.). Boca Raton, FL: CRC Press. p. 4.54. ISBN 9781498754293.
  2. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1-138-56163-2.
  3. ^ Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
  4. ^ a b c Klaus Schrödter; Gerhard Bettermann; Thomas Staffel; Friedrich Wahl; Thomas Klein; Thomas Hofmann (2012). "Phosphoric Acid and Phosphates". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_465.pub3. ISBN 978-3527306732.
  5. ^ a b El Moussaoui, Youssef; Terrisse, Hélène; Quillard, Sophie; Ropers, Marie-Hélène; Humbert, Bernard (January 2023). "The True Nature of Tricalcium Phosphate Used as Food Additive (E341(iii))". Nanomaterials. 13 (12): 1823. doi:10.3390/nano13121823. ISSN 2079-4991. PMC 10303396. PMID 37368253.
  6. ^ a b Destainville, A.; Champion, E.; Bernache-Assollant, D.; Laborde, E. (2003). "Synthesis, characterization and thermal behavior of apatitic tricalcium phosphate". Materials Chemistry and Physics. 80 (1): 269–277. doi:10.1016/S0254-0584(02)00466-2.
  7. ^ a b c d Rey, C.; Combes, C.; Drouet, C.; Grossin, D. (2011). "1.111 – Bioactive Ceramics: Physical Chemistry". In Ducheyne, Paul (ed.). Comprehensive Biomaterials. Vol. 1. Elsevier. pp. 187–281. doi:10.1016/B978-0-08-055294-1.00178-1. ISBN 978-0-08-055294-1.
  8. ^ Dorozhkin, Sergey V. (December 2012). "Amorphous calcium (ortho)phosphates". Acta Biomaterialia. 6 (12): 4457–4475. doi:10.1016/j.actbio.2010.06.031. PMID 20609395.
  9. ^ Yashima, M.; Sakai, A.; Kamiyama, T.; Hoshikawa, A. (2003). "Crystal structure analysis of β-tricalcium phosphate Ca3(PO4)2 by neutron powder diffraction". RNAl of Solid State Chemistry. 175 (2): 272–277. Bibcode:2003JSSCh.175..272Y. doi:10.1016/S0022-4596(03)00279-2.
  10. ^ a b Carrodeguas, R.G.; De Aza, S. (2011). "α-Tricalcium phosphate: Synthesis, properties and biomedical applications". Acta Biomaterialia. 7 (10): 3536–3546. doi:10.1016/j.actbio.2011.06.019. PMID 21712105.
  11. ^ Yacoubou, Jeanne, MS. Vegetarian Journal's Guide To Food Ingredients "Guide to Food Ingredients". The Vegetarian Resource Group, n.d. Web. 14 Sept. 2012.
  12. ^ Daculsi, G.; Legeros, R. (2008). "17 – Tricalcium phosphate / hydroxyapatite biphasic ceramics". In Kokubo, Tadashi (ed.). Bioceramics and their Clinical Applications. Woodhead Publishing. pp. 395–423. doi:10.1533/9781845694227.2.395. ISBN 978-1-84569-204-9.
  13. ^ Salinas, Antonio J.; Vallet-Regi, Maria (2013). "Bioactive ceramics: from bone grafts to tissue engineering". RSC Advances. 3 (28): 11116–11131. Bibcode:2013RSCAd...311116S. doi:10.1039/C3RA00166K.
  14. ^ Elliott, J.C. (1994). "3 – Hydroxyapatite and Nonstoichiometric Apatites". Studies in Inorganic Chemistry. Vol. 18. Elsevier. pp. 111–189. doi:10.1016/B978-0-444-81582-8.50008-0. ISBN 978-0-444-81582-8.
  15. ^ Vallet-Regí, M.; Rodríguez-Lorenzo, L.M. (November 1997). "Synthesis and characterisation of calcium deficient apatite". Solid State Ionics. 101–103, Part 2: 1279–1285. doi:10.1016/S0167-2738(97)00213-0.
  16. ^ Hamba H, Nakamura K, Nikaido T, Tagami J, Muramatsu T (October 2020). "Remineralization of enamel subsurface lesions using toothpaste containing tricalcium phosphate and fluoride: an in vitro µCT analysis". BMC Oral Health. 20 (1): 292. doi:10.1186/s12903-020-01286-1. PMC 7590595. PMID 33109184.
  17. ^ Meyer F, Amaechi BT, Fabritius HO, Enax J (2018). "Overview of Calcium Phosphates used in Biomimetic Oral Care". The Open Dentistry Journal. 12: 406–423. doi:10.2174/1874210601812010406. PMC 5997847. PMID 29988215.
  18. ^ Limeback H, Enax J, Meyer F (July 2023). "Improving Oral Health with Fluoride-Free Calcium-Phosphate-Based Biomimetic Toothpastes: An Update of the Clinical Evidence". Biomimetics. 8 (4): 331. doi:10.3390/biomimetics8040331. PMC 10452078. PMID 37622936.
  19. ^ Bonjour JP, Carrie AL, Ferrari S, Clavien H, Slosman D, Theintz G, Rizzoli R (March 1997). "Calcium-enriched foods and bone mass growth in prepubertal girls: a randomized, double-blind, placebo-controlled trial". J. Clin. Invest. 99 (6): 1287–1294. doi:10.1172/JCI119287. PMC 507944. PMID 9077538.
  20. ^ Straub DA (June 2007). "Calcium supplementation in clinical practice: a review of forms, doses, and indications". Nutr Clin Pract. 22 (3): 286–296. doi:10.1177/0115426507022003286. PMID 17507729.
  21. ^ Paderni S, Terzi S, Amendola L (September 2009). "Major bone defect treatment with an osteoconductive bone substitute". Musculoskelet Surg. 93 (2): 89–96. doi:10.1007/s12306-009-0028-0. PMID 19711008. S2CID 33413039.
  22. ^ Moore DC, Chapman MW, Manske D (1987). "The evaluation of a biphasic calcium phosphate ceramic for use in grafting long-bone diaphyseal defects". Journal of Orthopaedic Research. 5 (3): 356–365. doi:10.1002/jor.1100050307. PMID 3040949. S2CID 41579389.
  23. ^ Lange TA, Zerwekh JE, Peek RD, Mooney V, Harrison BH (1986). "Granular tricalcium phosphate in large cancellous defects". Annals of Clinical and Laboratory Science. 16 (6): 467–472. PMID 3541772.
  24. ^ Cao H, Kuboyama N (September 2009). "A biodegradable porous composite scaffold of PGA/β-TCP for bone tissue engineering". Bone. 46 (2): 386–395. doi:10.1016/j.bone.2009.09.031. PMID 19800045.
  25. ^ Erbe EM, Marx JG, Clineff TD, Bellincampi LD (October 2001). "Potential of an ultraporous β-tricalcium phosphate synthetic cancellous bone void filler and bone marrow aspirate composite graft". European Spine Journal. 10 (Suppl 2): S141–S146. doi:10.1007/s005860100287. PMC 3611552. PMID 11716011.
  26. ^ Bansal S, Chauhan V, Sharma S, Maheshwari R, Juyal A, Raghuvanshi S (July 2009). "Evaluation of hydroxyapatite and beta-tricalcium phosphate mixed with bone marrow aspirate as a bone graft substitute for posterolateral spinal fusion". Indian Journal of Orthopaedics. 43 (3): 234–239. doi:10.4103/0019-5413.49387 (inactive 1 November 2024). PMC 2762171. PMID 19838344.{{cite journal}}: CS1 maint: DOI inactive as of November 2024 (link)
  27. ^ Kundu, B; Lemos A; Soundrapandian C; Sen PS; Datta S; Ferreira JMF; Basu D (2010). "Development of porous HAp and β-TCP scaffolds by starch consolidation with foaming method and drug-chitosan bilayered scaffold based drug delivery system". J. Mater. Sci. Mater. Med. 21 (11): 2955–2969. doi:10.1007/s10856-010-4127-0. PMID 20644982. S2CID 6483779.
  28. ^ Tuite. Mindat.org
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