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Phosphide
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<h2 id="binary-phosphides">Binary phosphides</h2> <p>Binary phosphides include phosphorus and one other element. An example of a group 1 phosphide is <a href="/facts/Sodium_phosphide/Pdwv6N1V">sodium phosphide</a> (Na3P). Other notable examples include <a href="/facts/Aluminium_phosphide/9MvAsh3S">aluminium phosphide</a> (AlP) and <a href="/facts/Calcium_phosphide/rCnNpWds">calcium phosphide</a> (Ca3P2), which are used as pesticides, exploiting their tendency to release toxic <a href="/facts/Phosphine/aYysn5TS">phosphine</a> upon hydrolysis. Magnesium phosphide (Mg3P2) also is moisture sensitive. <a href="/facts/Indium_phosphide/IEW8ApM2">Indium phosphide</a> (InP) and <a href="/facts/Gallium_phosphide/DAFg8pfj">gallium phosphide</a> (GaP) are used as a semi-conductors, often in combination of related <a href="/facts/Arsenide/UpkRk4uf">arsenides</a>.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a> <a href="/facts/Copper_phosphide/6EtxNqQQ">Copper phosphide</a> (Cu3P) illustrates a rare stoichiometry for a phosphide. These species are insoluble in all solvents - they are 3-dimensional solid state polymers. For those with electropositive metals, the materials hydrolyze: </p> Ca3P2 + 6 H2O → 3 Ca(OH)2 + 2 PH3 <h2 id="polyphosphides">Polyphosphides</h2> <p>Polyphosphides contain P−P bonds. The simplest polyphosphides would be derivatives of P4−2. The free anions are rarely encountered because they are so basic. Most members follow the octet rule. </p><p>Well studied polyphosphides are derivatives of P3−7.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a> </p><p>The nomenclature for polyphosphides can be deceptive. As confirmed by <a href="/facts/X-ray_crystallography/WtI0F5DN">X-ray crystallography</a> <a href="/facts/Tin_triphosphide/mM6lDRLM">tin triphosphide</a> and germanium triphosphide are not triphosphides, but hexaphosphides. They consist of ruffled <i>cyclo</i>-P6−6 subunits.<a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a> Another example of deceptive nomenclature is "thorium pentaphosphide", which consists of a polymeric polyphosphide related to <a href="/facts/Hittorf%27s_phosphorus/GarX3byj">Hittorf's phosphorus</a>.<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a> </p><p> Several polyphosphides contain the cluster P3−11 ions and polymeric chain anions (e.g. the helical (P−)<i>n</i> ion) and complex sheet or 3-D anions.<a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a> The range of structures is extensive. <a href="/facts/Potassium/FWPwS7Rj">Potassium</a> has nine phosphides: K3P, K4P3, K5P4, KP, K4P6, K3P7, K3P11, KP10.3, KP15. Eight mono- and polyphosphides of <a href="/facts/Nickel/KwMCHYRP">nickel</a> also exist: (Ni3P, Ni5P2, Ni12P5, Ni2P, Ni5P4, NiP, NiP2, NiP3).<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a> </p><p>Two polyphosphide ions, P4−3 found in K4P3 and P5−4 found in K5P4, are <a href="/facts/Radical_anion/N4vFqKrV">radical anions</a> with an odd number of <a href="/facts/Valence_electron/mXPA15VP">valence electrons</a>.<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a> </p> <h2 id="preparation-of-phosphide-and-polyphosphide-materials">Preparation of phosphide and polyphosphide materials</h2> <p>There are many ways to prepare phosphide compounds. One common way involves heating a metal and <a href="/facts/Red_phosphorus/GarX3byj">red phosphorus</a> (P) under inert atmospheric conditions or vacuum. In principle, all metal phosphides and polyphosphides can be synthesized from elemental phosphorus and the respective metal element in stoichiometric forms. However, the synthesis is complicated due to several problems. The <a href="/facts/Exothermic_reaction/w5IjYYfL">exothermic reactions</a> are often explosive due to local overheating. Oxidized metals, or even just an oxidized layer on the exterior of the metal, causes extreme and unacceptably high temperatures for beginning phosphorination.<a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a> Hydrothermal reactions to generate nickel phosphides have produced pure and well crystallized nickel phosphide compounds, Ni2P and Ni12P5. These compounds were synthesized through a solid-liquid reaction between NiCl2·12H2O and red phosphorus at 200 °C for 24 and 48 hours, respectively.<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a> </p><p>Metal phosphides are also produced by reaction of <a href="/facts/Tris(trimethylsilyl)phosphine/rY8UI4JM">tris(trimethylsilyl)phosphine</a> with metal halides. In this method, the halide is liberated as the volatile <a href="/facts/Trimethylsilyl_chloride/CKlvuSgR">trimethylsilyl chloride</a>. </p> <p> A method for the preparation of K2P16 from red phosphorus and <a href="/facts/Potassium_ethoxide/W98L04pz">potassium ethoxide</a> has been reported.<a class="footnote-ref" id="fnref:12" href="#fn:12"><sup>12</sup></a> </p><h2 id="molecular-phosphides">Molecular phosphides</h2> <p>Compounds with triple bonds between a metal and phosphorus are rare. The main examples have the formula P≡Mo(NR2)3, where R is a bulky organic substituent.<a class="footnote-ref" id="fnref:13" href="#fn:13"><sup>13</sup></a> </p> <h2 id="organic-phosphides">Organic phosphides</h2> <p class="note">See also: <a href="/facts/Phosphaalkyne/j5a6bI11">Phosphaalkyne</a></p> <p>Many organophosphides are known. Common examples have the formula R2PM where R is an organic substituent and M is a metal. One example is <a href="/facts/Lithium_diphenylphosphide/4grep8IN">lithium diphenylphosphide</a>. The <a href="/facts/Zintl_cluster/RdV0yDXf">Zintl cluster</a> P3−7 is obtained with diverse alkali metal derivatives. </p> <h2 id="natural-examples">Natural examples</h2> <p>The mineral <a href="/facts/Schreibersite/EsYNkM5E">schreibersite</a> (Fe,Ni)3P is common in some meteorites. </p> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Von Schnering, H.G. and Hönle , W. (1994) "Phosphides - Solid-state Chemistry" in Encyclopedia of Inorganic Chemistry. R. Bruce King (ed.). John Wiley & Sons ISBN 0-471-93620-0 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Blackman, C. S.; Carmalt, C. J.; O'Neill, S. A.; Parkin, I. P.; Molloy, K. C.; Apostolico, L. (2003). "Chemical vapour deposition of group Vb metal phosphide thin films" (PDF). Journal of Materials Chemistry. 13 (8): 1930. doi:10.1039/b304084b. <a href="/wiki/Claire_J._Carmalt" target="_blank">/wiki/Claire_J._Carmalt</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Meyer, Teodoro; Hönle, Wolfgang; von Schnering, Hans Georg (1987). "Zur Chemie und Strukturchemie von Phosphiden und Polyphosphiden. 44. Tricäsiumheptaphosphid Cs3P7: Darstellung, Struktur und Eigenschaften". Zeitschrift für Anorganische und Allgemeine Chemie. 552 (9): 69–80. doi:10.1002/zaac.19875520907. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li> <li id="fn:5"><p>Gullman, Jan; Olofsson, Olle (1 November 1972). "The crystal structure of SnP3 and a note on the crystal structure of GeP3". Journal of Solid State Chemistry. 5 (3): 441–445. doi:10.1016/0022-4596(72)90091-6. ISSN 0022-4596. Retrieved 28 March 2024. <a href="https://www.sciencedirect.com/science/article/abs/pii/0022459672900916" target="_blank">https://www.sciencedirect.com/science/article/abs/pii/0022459672900916</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></p></li> <li id="fn:6"><p>Olofsson, Olle; Gullman, Jan; Søtofte, Inger; Beronius, P.; Engebretsen, Jan E.; Ehrenberg, L. (1971). "The Crystal Structure of TlP5". Acta Chemica Scandinavica. 25: 1327–1337. doi:10.3891/acta.chem.scand.25-1327. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> <li id="fn:7"><p>Jeitschko, W.; Möller, M. H. (1987). "Phosphides and Polyphosphides of the Transition Metals". Phosphorus and Sulfur and the Related Elements. 30 (1–2): 413–416. doi:10.1080/03086648708080608. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></p></li> <li id="fn:8"><p>Von Schnering, H.G. and Hönle , W. (1994) "Phosphides - Solid-state Chemistry" in Encyclopedia of Inorganic Chemistry. R. Bruce King (ed.). John Wiley & Sons ISBN 0-471-93620-0 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></p></li> <li id="fn:9"><p>Von Schnering, H.G. and Hönle , W. (1994) "Phosphides - Solid-state Chemistry" in Encyclopedia of Inorganic Chemistry. R. Bruce King (ed.). John Wiley & Sons ISBN 0-471-93620-0 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:9" class="footnote-back-ref">↩</a></p></li> <li id="fn:10"><p>von Schnering, Hans-Georg; Hönle, Wolfgang (1988). "Bridging Chasms with Phosphides". Chemical Reviews. 88: 243–273. doi:10.1021/cr00083a012. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:10" class="footnote-back-ref">↩</a></p></li> <li id="fn:11"><p>Liu, Zongyi; Huang, Xiang; Zhu, Zhibin; Dai, Jinhui (2010). "A simple mild hydrothermal route for the synthesis of nickel phosphide powders". Ceramics International. 36 (3): 1155–1158. doi:10.1016/j.ceramint.2009.12.015. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:11" class="footnote-back-ref">↩</a></p></li> <li id="fn:12"><p>Dragulescu-Andrasi, Alina; Miller, L. Zane; Chen, Banghao; McQuade, D. Tyler; Shatruk, Michael (March 14, 2016). "Facile Conversion of Red Phosphorus into Soluble Polyphosphide Anions by Reaction with Potassium Ethoxide". Angewandte Chemie International Edition. 55 (12): 3904–3908. doi:10.1002/anie.201511186. PMID 26928980. <a href="https://doi.org/10.1002%2Fanie.201511186" target="_blank">https://doi.org/10.1002%2Fanie.201511186</a> <a href="#fnref:12" class="footnote-back-ref">↩</a></p></li> <li id="fn:13"><p>Cossairt, B. M.; Piro, N. A.; Cummins, C. C. (2010). "Early-Transition-Metal-Mediated Activation and Transformation of White Phosphorus". Chemical Reviews. 110 (7): 4164–77. CiteSeerX 10.1.1.666.8019. doi:10.1021/cr9003709. PMID 20175534. <a href="/wiki/CiteSeerX_(identifier)" target="_blank">/wiki/CiteSeerX_(identifier)</a> <a href="#fnref:13" class="footnote-back-ref">↩</a></p></li> </ol>