Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Tricalcium phosphate: Difference between pages

| Watchedfields = changed

| verifiedrevid = 476998399

| ImageFile1 = Ca3(PO4)2 from crystallography.jpg

| ImageFile2 = Tricalcium phosphate.svg

| ImageSize =

| IUPACName = Calcium phosphate

| OtherNames = Tribasic calcium phosphate, tricalcium bis(phosphate)

|Section1={{Chembox Identifiers

| EINECS = 231-840-8

| CASNo_Ref = {{cascite|correct|CAS}}

|Section2={{Chembox Properties

| Formula = Ca₃(PO₄)₂

| MolarMass = 310.18 g/mol

| Density = 3.14 g/cm³<ref name=crc>{{RubberBible97th|page=4.54}}</ref>

| MeltingPtC = 1670

| MeltingPt_ref =<ref name=crc/>

| BoilingPt_notes =

| Solubility = 1.2 mg/kg<ref name=crc/>

| SolubilityProduct = {{val|2.07|e=-33}}<ref name="crc2">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1-138-56163-2 |pages=5–188|edition=99 |language=English}}</ref>

|Section5={{Chembox Thermochemistry

| DeltaHf = −4126 kJ/mol (α-form)<ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A21}}</ref>

|Section6={{Chembox Pharmacology

| ATCCode_prefix = A12

| ATCCode_suffix = AA01

}}

|Section7={{Chembox Hazards

| NFPA-S =

| HPhrases =

| PPhrases =

| GHS_ref =

|Section8={{Chembox Related

| OtherAnions = [[Calcium pyrophosphate]]

| OtherCations = [[Trimagnesium phosphate]]<br/>[[Trisodium phosphate]]<br/>[[Tripotassium phosphate]]

| OtherCompounds = [[Monocalcium phosphate]]<br/>[[Dicalcium phosphate]]

'''Tricalcium phosphate''' (sometimes abbreviated '''TCP'''), more commonly known as '''Calcium phosphate''', is a [[calcium]] [[Salt (chemistry)|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]].<ref name=Ullmann>{{Ullmann|author1=Klaus Schrödter|author2=Gerhard Bettermann|author3=Thomas Staffel|author4=Friedrich Wahl|author5=Thomas Klein|author6=Thomas Hofmann|title=Phosphoric Acid and Phosphates|doi=10.1002/14356007.a19_465.pub3|year=2012}}</ref><ref name=":0">{{Cite journal |last1=El Moussaoui |first1=Youssef |last2=Terrisse |first2=Hélène |last3=Quillard |first3=Sophie |last4=Ropers |first4=Marie-Hélène |last5=Humbert |first5=Bernard |date=January 2023 |title=The True Nature of Tricalcium Phosphate Used as Food Additive (E341(iii)) |journal=Nanomaterials |language=en |volume=13 |issue=12 |page=1823 |doi=10.3390/nano13121823 |pmid=37368253 |pmc=10303396 |issn=2079-4991 |doi-access=free }}</ref>

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

==Nomenclature==

{{Main|Calcium phosphate}}

''Calcium phosphate'' refers to numerous materials consisting of calcium ions (Ca²⁺) together with [[orthophosphate]]s ({{chem|PO|4|3−}}), [[metaphosphate]]s or [[pyrophosphate]]s ({{chem|P|2|O|7|4−}}) and occasionally oxide and [[hydroxide]] ions. Especially, the common mineral [[apatite]] has formula Ca₅(PO₄)₃''X'', where ''X'' is [[Fluoride|F]], [[Chloride|Cl]], [[Hydroxide|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]].<ref name=":0" />

== Preparation ==

Tricalcium phosphate is produced commercially by treating [[hydroxyapatite]] with [[phosphoric acid]] and [[Calcium hydroxide|slaked lime]].<ref name=Ullmann/>

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.<ref name="Destainville">{{cite journal |title=Synthesis, characterization and thermal behavior of apatitic tricalcium phosphate |author=Destainville, A. |author2=Champion, E. |author3=Bernache-Assollant, D. |author4=Laborde, E. |doi=10.1016/S0254-0584(02)00466-2 |date=2003 |volume=80 |issue=1 |pages=269–277 |journal=Materials Chemistry and Physics }}</ref> 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).<ref name="Destainville" /><ref name="Bioactive">{{cite book |last1=Rey, C. |last2=Combes, C. |last3=Drouet, C.|last4=Grossin, D.|year= 2011 |chapter= 1.111 – Bioactive Ceramics: Physical Chemistry |editor1-last=Ducheyne |editor1-first=Paul |title=Comprehensive Biomaterials |volume=1 |publisher=Elsevier |publication-date=2011 |pages=187–281 |doi=10.1016/B978-0-08-055294-1.00178-1 |isbn=978-0-08-055294-1 }}</ref><ref name ="Dorozhkin2012">{{cite journal |title= Amorphous calcium (ortho)phosphates |author=Dorozhkin, Sergey V. |doi=10.1016/j.actbio.2010.06.031 |pmid= 20609395 |date=December 2012|volume=6|issue=12|pages= 4457–4475 |journal=Acta Biomaterialia }}</ref> 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:<ref name="Bioactive"/>

:CaCO₃ + Ca₂P₂O₇ → Ca₃(PO₄)₂ + CO₂

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

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&nbsp;g&nbsp;cm⁻³ while the high temperature forms are less dense, α-tricalcium phosphate has a density of 2.866&nbsp;g&nbsp;cm⁻³ and α′-tricalcium phosphate has a density of 2.702&nbsp;g&nbsp;cm⁻³ All forms have complex structures consisting of tetrahedral phosphate centers linked through oxygen to the calcium ions.<ref>{{cite journal|title=Crystal structure analysis of β-tricalcium phosphate Ca₃(PO₄)₂ by neutron powder diffraction|author1=Yashima, M.|author2=Sakai, A.|author3=Kamiyama, T.|author4=Hoshikawa, A.|journal=RNAl of Solid State Chemistry|year=2003|volume=175|issue=2|pages=272–277|doi=10.1016/S0022-4596(03)00279-2|bibcode=2003JSSCh.175..272Y}}</ref> The high temperature forms each have two types of columns, one containing only calcium ions and the other both calcium and phosphate.<ref name="Carrodeguas2011">{{cite journal |title=α-Tricalcium phosphate: Synthesis, properties and biomedical applications |author1=Carrodeguas, R.G. |author2=De Aza, S. |doi=10.1016/j.actbio.2011.06.019 |pmid=21712105 |volume=7 |issue=10 |year=2011 |pages=3536–3546 |journal=Acta Biomaterialia }}</ref>

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.<ref name="Carrodeguas2011" />

==Occurrence==

[[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.<ref>Yacoubou, Jeanne, MS. [http://www.vrg.org/ingredients/index.php Vegetarian Journal's Guide To Food Ingredients] "Guide to Food Ingredients". The Vegetarian Resource Group, n.d. Web. 14 Sept. 2012.</ref>

Tricalcium phosphate occurs naturally in several forms, including:

* as a rock in [[Morocco]], [[Israel]], [[Philippines]], [[Egypt]], and [[Kola peninsula|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#Cow's milk|milk]].

==Biphasic calcium phosphate, BCP==

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.<ref name="Bioceramicschap17">{{cite book |last1=Daculsi |first1=G. |last2=Legeros |first2=R. |year=2008 |chapter=17 – Tricalcium phosphate{{hsp}}/{{hsp}}hydroxyapatite biphasic ceramics |editor1-last=Kokubo |editor1-first=Tadashi |title=Bioceramics and their Clinical Applications |publisher=Woodhead Publishing |pages=395–423 |doi=10.1533/9781845694227.2.395 |isbn=978-1-84569-204-9 }}</ref> It is a ceramic.<ref name="Salinas2013">{{Cite journal |last1=Salinas |first1=Antonio J. |last2=Vallet-Regi |first2=Maria |year=2013 |title=Bioactive ceramics: from bone grafts to tissue engineering |journal= RSC Advances |volume=3 |issue=28 |pages=11116–11131 |doi=10.1039/C3RA00166K |bibcode= 2013RSCAd...311116S}}</ref>

Preparation involves [[sintering]], causing irreversible decomposition of calcium deficient apatites<ref name="Bioactive" /> alternatively termed non-stoichiometric apatites or basic calcium phosphate.<ref name="Elliot">{{cite book |last1=Elliott |first1=J.C. |year=1994 |chapter=3 – Hydroxyapatite and Nonstoichiometric Apatites |title=Studies in Inorganic Chemistry |volume=18 |publisher=Elsevier |pages=111–189 |doi=10.1016/B978-0-444-81582-8.50008-0 |isbn=978-0-444-81582-8 }}</ref> An example is:<ref name="ValletRegi2011">{{cite journal |title=Synthesis and characterisation of calcium deficient apatite |last1=Vallet-Regí |first1=M. |last2=Rodríguez-Lorenzo |first2=L.M. |doi=10.1016/S0167-2738(97)00213-0 |date=November 1997 |volume=101–103, Part 2 |pages=1279–1285 |journal=Solid State Ionics }}</ref>

:Ca_10−''δ''(PO₄)_6−''δ''(HPO₄)_''δ''(OH)_2−''δ'' → (1−''δ'') Ca₁₀(PO₄)₆(OH)₂ + 3''δ'' Ca₃(PO₄)₂

β-TCP can contain impurities, for example calcium pyrophosphate, {{chem2|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.<ref name="Bioactive" />

==Uses==

===Food additive===

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===

It is also found in [[baby powder]], [[antacids]] and [[toothpaste]].<ref name=Ullmann/> Toothpastes with functionalized β-tricalcium phosphate (fTCP) may help [[Remineralisation of teeth|remineralize]] [[tooth enamel]].<ref name="pmid33109184">{{cite journal |vauthors=Hamba H, Nakamura K, Nikaido T, Tagami J, Muramatsu T |title=Remineralization of enamel subsurface lesions using toothpaste containing tricalcium phosphate and fluoride: an in vitro µCT analysis |journal=BMC Oral Health |volume=20 |issue=1 |pages=292 |date=October 2020 |pmid=33109184 |pmc=7590595 |doi=10.1186/s12903-020-01286-1 |doi-access=free }}</ref><ref name="pmid29988215">{{cite journal |vauthors=Meyer F, Amaechi BT, Fabritius HO, Enax J |title=Overview of Calcium Phosphates used in Biomimetic Oral Care |journal=The Open Dentistry Journal |volume=12 |pages=406–423 |date=2018 |pmid=29988215 |pmc=5997847 |doi= 10.2174/1874210601812010406 |doi-access=free}}</ref><ref name="pmid37622936">{{cite journal |vauthors=Limeback H, Enax J, Meyer F |title=Improving Oral Health with Fluoride-Free Calcium-Phosphate-Based Biomimetic Toothpastes: An Update of the Clinical Evidence |journal=Biomimetics |volume=8 |issue=4 |date=July 2023 |page=331 |pmid=37622936 |pmc=10452078 |doi=10.3390/biomimetics8040331 |doi-access=free}}</ref>

===Biomedical===

It is also used as a [[nutritional supplement]]<ref name="pmid9077538">{{cite journal |vauthors=Bonjour JP, Carrie AL, Ferrari S, Clavien H, Slosman D, Theintz G, Rizzoli R |title=Calcium-enriched foods and bone mass growth in prepubertal girls: a randomized, double-blind, placebo-controlled trial |journal=[[J. Clin. Invest.]] |volume=99 |issue=6 |pages=1287–1294 |date=March 1997 |pmid=9077538 |pmc=507944 |doi=10.1172/JCI119287}}</ref> and occurs naturally in [[cow]] [[milk]],{{Citation needed|date=March 2013}} 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).<ref name="pmid17507729">{{cite journal | doi = 10.1177/0115426507022003286 | author = Straub DA | title = Calcium supplementation in clinical practice: a review of forms, doses, and indications | journal = Nutr Clin Pract |volume = 22 | issue = 3 | pages = 286–296 |date=June 2007 | pmid = 17507729 }}</ref> There is some debate about the different [[bioavailability|bioavailabilities]] of the different calcium salts.

It can be used as a tissue replacement for repairing bony defects when [[autotransplantation|autogenous]] [[bone graft]] is not feasible or possible.<ref name="pmid19711008">{{cite journal |vauthors=Paderni S, Terzi S, Amendola L | title = Major bone defect treatment with an osteoconductive bone substitute| journal = Musculoskelet Surg | volume = 93 | issue = 2 | pages = 89–96 |date=September 2009 | pmid = 19711008 | doi = 10.1007/s12306-009-0028-0 | s2cid = 33413039}}</ref><ref name="pmid3040949">{{cite journal |vauthors=Moore DC, Chapman MW, Manske D | title = The evaluation of a biphasic calcium phosphate ceramic for use in grafting long-bone diaphyseal defects | journal = [[Journal of Orthopaedic Research]] | volume = 5 | issue = 3 | pages = 356–365 | year = 1987 | pmid = 3040949 | doi = 10.1002/jor.1100050307 | s2cid = 41579389 }}</ref><ref name="pmid3541772">{{cite journal |vauthors=Lange TA, Zerwekh JE, Peek RD, Mooney V, Harrison BH | title = Granular tricalcium phosphate in large cancellous defects | journal = [[Annals of Clinical and Laboratory Science]] | volume = 16 | issue = 6 | pages = 467–472 | year = 1986 | pmid = 3541772 }}</ref> It may be used alone or in combination with a [[biodegradable]], [[resorbable]] [[polymer]] such as [[polyglycolic acid]].<ref name="pmid19800045">{{cite journal |vauthors=Cao H, Kuboyama N | title = A biodegradable porous composite scaffold of PGA/β-TCP for bone tissue engineering | journal = [[Bone (journal)|Bone]] | volume = 46 | issue = 2 | pages = 386–395 |date=September 2009 | pmid = 19800045 | doi = 10.1016/j.bone.2009.09.031 }}</ref> It may also be combined with autologous materials for a bone graft.<ref name="pmid11716011">{{cite journal |vauthors=Erbe EM, Marx JG, Clineff TD, Bellincampi LD | title = Potential of an ultraporous β-tricalcium phosphate synthetic cancellous bone void filler and bone marrow aspirate composite graft | journal = [[European Spine Journal]] | volume = 10 | pages = S141–S146 |date=October 2001 | issue = Suppl 2 | pmid = 11716011 | doi = 10.1007/s005860100287| pmc = 3611552 }}</ref><ref name="pmid19838344">{{cite journal |vauthors=Bansal S, Chauhan V, Sharma S, Maheshwari R, Juyal A, Raghuvanshi S |title=Evaluation of hydroxyapatite and beta-tricalcium phosphate mixed with bone marrow aspirate as a bone graft substitute for posterolateral spinal fusion |journal=Indian Journal of Orthopaedics |volume=43 |issue=3 |pages=234–239 |date=July 2009 |pmid=19838344 |pmc=2762171 |doi=10.4103/0019-5413.49387 |doi-broken-date=2024-04-24 |doi-access=free}}</ref>

Porous β-tricalcium phosphate scaffolds are employed as drug carrier systems for local drug delivery in bone.<ref>{{cite journal | last = Kundu | first = B |author2=Lemos A |author3=Soundrapandian C |author4=Sen PS |author5=Datta S |author6=Ferreira JMF |author7= Basu D | title= Development of porous HAp and β-TCP scaffolds by starch consolidation with foaming method and drug-chitosan bilayered scaffold based drug delivery system | journal = J. Mater. Sci. Mater. Med. | volume = 21 | pages = 2955–2969 | year = 2010 | doi = 10.1007/s10856-010-4127-0 | pmid=20644982 | issue=11| s2cid = 6483779 }}</ref>

==Natural occurrence==

[[Tuite (mineral)|Tuite]], a natural analogue of tricalcium orthophosphate(V), is a rare component of some meteorites. Its formation is related to shock metamorphism.<ref>[https://www.mindat.org/min-25637.html Tuite]. Mindat.org</ref>

==References==

{{Reflist|30em}}

{{Calcium compounds}}

{{Phosphates}}

{{Authority control}}

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[[Category:Biomaterials]]

[[Category:Calcium compounds]]

[[Category:Phosphates]]

[[Category:E-number additives]]