Allotropes of phosphorus

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The four common allotropes of phosphorus

Elemental phosphorus can exist in several allotropes; the most common of which are white and red solids. Solid violet and black allotropes are also known. Gaseous phosphorus exists as diphosphorus and atomic phosphorus.

White phosphorus and resulting allotropes

White phosphorus[edit]

This section is about the chemistry of white phosphorus. For military applications, see white phosphorus munitions.
White phosphorus sample

White phosphorus, yellow phosphorus or simply tetraphosphorus (P4) exists as molecules made up of four atoms in a tetrahedral structure. The tetrahedral arrangement results in ring strain and instability. The molecule is described as consisting of six single P–P bonds. Two different crystalline forms are known. The α form, which is stable under standard conditions, has a body-centered cubic crystal structure. It transforms reversibly into the β form at 195.2 K. The β form is believed to have a hexagonal crystal structure.[1]

White phosphorus is a translucent waxy solid that quickly becomes yellow when exposed to light. For this reason it is also called yellow phosphorus. It glows greenish in the dark (when exposed to oxygen), is highly flammable and pyrophoric (self-igniting) upon contact with air as well as toxic (causing severe liver damage on ingestion and phossy jaw from chronic ingestion or inhalation). The odour of combustion of this form has a characteristic garlic smell, and samples are commonly coated with white "diphosphorus pentoxide", which consists of P4O10 tetrahedral with oxygen inserted between the phosphorus atoms and at their vertices. White phosphorus is only slightly soluble in water and it can be stored under water. Indeed, white phosphorus is only safe from self-igniting when it is submerged in water. It is soluble in benzene, oils, carbon disulfide, and disulfur dichloride.

Production and applications[edit]

The white allotrope can be produced using several different methods. In the industrial process, phosphate rock is heated in an electric or fuel-fired furnace in the presence of carbon and silica.[2] Elemental phosphorus is then liberated as a vapour and can be collected under phosphoric acid. An idealized equation for this carbothermal reaction is shown for calcium phosphate (although phosphate rock contains substantial amounts of fluoroapatite):

2 Ca3(PO4)2 + 8 C → P4 + 8 CO2 + 6 Ca
Tetraphosphorus molecule

White phosphorus has an appreciable vapour pressure at ordinary temperatures. The vapour density indicates that the vapour is composed of P4 molecules up to about 800 °C. Above that temperature, dissociation into P2 molecules occurs.

It ignites spontaneously in air at about 50 °C, and at much lower temperatures if finely divided. This combustion gives phosphorus (V) oxide:

+ 5 O

Because of this property, white phosphorus is used as a weapon. The use of white phosphorus in combination with enriched uranium by the U.S.A. army in Fallujah in 2005 caused a big increase of the number of cancers and deformed babies (14,7% of all children born) in that city.[3]

Non-existence of cubic-P8[edit]

Although white phosphorus converts to the thermodynamically more stable red allotrope, the formation of the cubic P8 molecule is not observed in the condensed phase. Derivatives of this hypothetical molecule have been prepared from phosphaalkynes.[4]

Red phosphorus[edit]

Red phosphorus
Red phosphorus structure

Red phosphorus may be formed by heating white phosphorus to 300°C (482 °F) in the absence of air or by exposing white phosphorus to sunlight. Red phosphorus exists as an amorphous network. Upon further heating, the amorphous red phosphorus crystallizes. Red phosphorus does not ignite in air at temperatures below 240 °C, whereas pieces of white phosphorus ignite at about 30 °C. Ignition is spontaneous at room temperature with finely divided material. Heating red phosphorus in the presence of moisture creates phosphine gas, which is both highly flammable and toxic.

Hittorf's violet phosphorus[edit]

Violet phosphorus (right) by a sample of red phosphorus (left)
Violet phosphorus structure
Hitorff phosphorus structure

Monoclinic phosphorus, or violet phosphorus, is also known as Hittorf's metallic phosphorus.[5][6] In 1865, Johann Wilhelm Hittorf heated red phosphorus in a sealed tube at 530 °C. The upper part of the tube was kept at 444 °C. Brilliant opaque monoclinic, or rhombohedral, crystals sublime. Violet phosphorus can also be prepared by dissolving white phosphorus in molten lead in a sealed tube at 500 °C for 18 hours. Upon slow cooling, Hittorf's allotrope crystallises out. The crystals can be revealed by dissolving the lead in dilute nitric acid followed by boiling in concentrated hydrochloric acid.[7] In addition, a fibrous form exists with similar phosphorus cages.

Reactions of violet phosphorus[edit]

It does not ignite in air until heated to 300 °C and is insoluble in all solvents. It is not attacked by alkali and only slowly reacts with halogens. It can be oxidised by nitric acid to phosphoric acid.

If it is heated in an atmosphere of inert gas, for example nitrogen or carbon dioxide, it sublimes and the vapour condenses as white phosphorus. If it is heated in a vacuum and the vapour condensed rapidly, violet phosphorus is obtained. It would appear that violet phosphorus is a polymer of high relative molecular mass, which on heating breaks down into P2 molecules. On cooling, these would normally dimerize to give P4 molecules (i.e. white phosphorus) but, in vacuo, they link up again to form the polymeric violet allotrope.

Black phosphorus[edit]

Black phosphorus ampoule
Black phosphorus
Black phosphorus structure

Black phosphorus is the thermodynamically stable form of phosphorus at room temperature and pressure. It is obtained by heating white phosphorus under high pressures (12,000 atmospheres). In appearance, properties, and structure, black phosphorus is very much like graphite with both being black and flaky, a conductor of electricity, and having puckered sheets of linked atoms. Phonons, photons, and electrons in layered black phosphorus structures behave in a highly anisotropic manner within the plane of layers, exhibiting strong potential for applications to thin film electronics and infrared optoelectronics.[8] Light absorption in black phosphorus is sensitive to the polarization of incident light, film thickness, and doping.[9][10] Black phosphorus photo-transistors exhibit hyper-spectral detection attributes in the infrared and visible spectrum.[11][12]

Black phosphorus has an orthorhombic structure and is the least reactive allotrope, a result of its lattice of interlinked six-membered rings where each atom is bonded to three other atoms.[13][14] Black and red phosphorus can also take a cubic crystal lattice structure.[15] A recent synthesis of black phosphorus using metal salts as catalysts has been reported.[16]

The similarities to graphite also include the possibility of scotch-tape delamination (exfoliation), resulting in phosphorene, an anisotropic, graphene-like material with excellent charge transport properties[17] and high (~100 Wm-1K-1) thermal conductivity.[18] Exfoliated black phosphorus oxidizes when exposed to water and oxygen,[19] and sublimes at 400 °C in vacuum.[20] It has recently been shown that high-quality, few-layer black phosphorus nanosheets can be produced in large quantities by liquid phase exfoliation.[21][22]


Main article: Diphosphorus
Structure of diphosphorus
Diphosphorus molecule

The diphosphorus allotrope (P2) can normally be obtained only under extreme conditions (for example, from P4 at 1100 kelvin). In 2006, the diatomic molecule was generated in homogenous solution under normal conditions with the use of transition metal complexes (for example, tungsten and niobium).[23]

Diphosphorus is the gaseous form of phosphorus, and the thermodynamically stable form between 1200 °C and 2000 °C. The dissociation of tetraphosphorus (P
) begins at lower temperature: the percentage of P
at 800 °C is ≈ 1%. At temperatures above about 2000 °C, the diphosphorus molecule begins to dissociate into atomic phosphorus.

Phosphorus nanorods[edit]

P12 nanorod polymers were isolated from CuI-P complexes using low temperature treatment.[24]

Red/brown phosphorus was shown to be stable in air for several weeks and have significantly different properties from red phosphorus. Electron microscopy showed that red/brown phosphorus forms long, parallel nanorods with a diameter between 3.4 Å and 4.7 Å.[24]


Properties of some allotropes of phosphorus[25][26]
Form white(α) white(β) violet black
Symmetry Body-centred cubic Triclinic Monoclinic Orthorhombic
Pearson symbol aP24 mP84 oS8
Space group I43m P1 No.2 P2/c No.13 Cmca No.64
Density (g/cm3) 1.828 1.88 2.36 2.69
Bandgap (eV) 2.1 1.5 0.34
Refractive index 1.8244 2.6 2.4


  1. ^ Durif, M.-T. Averbuch-Pouchot ; A. (1996). Topics in phosphate chemistry. Singapore [u.a.]: World Scientific. p. 3. ISBN 981-02-2634-9. 
  2. ^ Threlfall, R.E., (1951). 100 years of Phosphorus Making: 1851–1951. Oldbury: Albright and Wilson Ltd
  3. ^
  4. ^ Streubel, Rainer (1995). "Phosphaalkyne Cyclooligomers: From Dimers to Hexamers—First Steps on the Way to Phosphorus–Carbon Cage Compounds". Angewandte Chemie International Edition in English 34 (4): 436. doi:10.1002/anie.199504361. 
  5. ^ Curry, Roger. "Hittorf`s Metallic Phosphorus of 1865". LATERAL SCIENCE. Retrieved 16 November 2014. 
  6. ^ Monoclinic phosphorus formed from vapor in the presence of an alkali metal U.S. Patent 4,620,968
  7. ^ Hittorf, W. (1865). "Zur Kenntniss des Phosphors". Annalen der Physik 202 (10): 193–228. Bibcode:1865AnP...202..193H. doi:10.1002/andp.18652021002. 
  8. ^ Xia, Fengnian; Wang, Han; Jia, Yichen (21 July 2014). "Rediscovering black phosphorus as an anisotropic layered material for optoelectronics and electronics". Nature Communications 5. arXiv:1402.0270. Bibcode:2014NatCo...5E4458X. doi:10.1038/ncomms5458. 
  9. ^ Low, Tony; Rodin, A. S.; Carvalho, A.; Jiang, Yongjin; Wang, Han; Xia, Fengnian; Castro Neto, A. H. (27 August 2014). "Tunable optical properties of multilayer black phosphorus thin films". Physical Review B 90 (7). arXiv:1404.4030. Bibcode:2014PhRvB..90g5434L. doi:10.1103/PhysRevB.90.075434. 
  10. ^ Tran, Vy; Soklaski, Ryan; Liang, Yufeng; Yang, Li (26 June 2014). "Layer-controlled band gap and anisotropic excitons in few-layer black phosphorus". Physical Review B 89 (23). Bibcode:2014PhRvB..89w5319T. doi:10.1103/PhysRevB.89.235319. 
  11. ^ Low, Tony; Engel, Michael; Steiner, Mathias; Avouris, Phaedon (29 August 2014). "Origin of photoresponse in black phosphorus phototransistors". Physical Review B 90 (8). arXiv:1407.7286. Bibcode:2014PhRvB..90h1408L. doi:10.1103/PhysRevB.90.081408. 
  12. ^ Buscema, Michele; Groenendijk, Dirk J.; Steele, Gary A.; van der Zant, Herre S.J.; Castellanos-Gomez, Andres (28 August 2014). "Photovoltaic effect in few-layer black phosphorus PN junctions defined by local electrostatic gating". Nature Communications 5: 4651. arXiv:1407.2863. Bibcode:2014NatCo...5E4651B. doi:10.1038/ncomms5651. 
  13. ^ Brown, A.; Rundqvist, S. (1965). "Refinement of the crystal structure of black phosphorus". Acta Crystallographica 19 (4): 684. doi:10.1107/S0365110X65004140. 
  14. ^ Cartz, L.; Srinivasa, S. R.; Riedner, R. J.; Jorgensen, J. D.; Worlton, T. G. (1979). "Effect of pressure on bonding in black phosphorus". The Journal of Chemical Physics 71 (4): 1718. Bibcode:1979JChPh..71.1718C. doi:10.1063/1.438523. 
  15. ^ Ahuja, Rajeev (2003). "Calculated high pressure crystal structure transformations for phosphorus". Physica status solidi (b) 235 (2): 282. Bibcode:2003PSSBR.235..282A. doi:10.1002/pssb.200301569. 
  16. ^ Lange, Stefan; Schmidt, Peer; Nilges, Tom (2007). "Au3SnP7@Black Phosphorus: An Easy Access to Black Phosphorus". Inorganic Chemistry 46 (10): 4028–35. doi:10.1021/ic062192q. PMID 17439206. 
  17. ^ Liu, Han; Neal, Adam T.; Zhu, Zhen; Luo, Zhe; Xu, Xianfan; Tománek, David; Ye, Peide D. (21 March 2014). "Phosphorene: An Unexplored 2D Semiconductor with a High Hole Mobility". ACS Nano 8 (4): 140324154339003. doi:10.1021/nn501226z. 
  18. ^ Jang, Hyejin; Wood, Joshua D.; Ryder, Christopher R.; Hersam, Mark C.; Cahill, David G. (30 October 2015). "Anisotropic Thermal Conductivity of Exfoliated Black Phosphorus". Advanced Materials. arXiv:1510.00051. doi:10.1002/adma.201503466. 
  19. ^ Wood, Joshua D.; Wells, Spencer A.; Jariwala, Deep; Chen, Kan-Sheng; Cho, EunKyung; Sangwan, Vinod K.; Liu, Xiaolong; Lauhon, Lincoln J.; Marks, Tobin J.; Hersam, Mark C. (7 November 2014). "Effective Passivation of Exfoliated Black Phosphorus Transistors against Ambient Degradation". Nano Letters 14 (12): 6964–6970. arXiv:1411.2055. Bibcode:2014NanoL..14.6964W. doi:10.1021/nl5032293. 
  20. ^ Liu, Xiaolong D.; Wood, Joshua D.; Chen, Kan-Sheng; Cho, EunKyung; Hersam, Mark C. (9 February 2015). "In Situ Thermal Decomposition of Exfoliated Two-Dimensional Black Phosphorus". Journal of Physical Chemistry Letters 6: 773–778. doi:10.1021/acs.jpclett.5b00043. 
  21. ^ Kang, Joohoon; Wood, Joshua D.; Wells, Spencer A.; Lee, Jae-Hyeok; Liu, Xiaolong; Chen, Kan-Sheng; Hersam, Mark C. (18 March 2015). "Solvent Exfoliation of Electronic-Grade, Two-Dimensional Black Phosphorus". ACS Nano. doi:10.1021/acsnano.5b01143. 
  22. ^ Damien Hanlon, Claudia Backes, (8 Jan 2015). "Liquid exfoliation of solvent-stabilised black phosphorus: applications beyond electronics". Cornell University. arXiv:1501.01881. Retrieved 14 January 2015. 
  23. ^ Piro, Na; Figueroa, Js; Mckellar, Jt; Cummins, Cc (2006). "Triple-bond reactivity of diphosphorus molecules". Science 313 (5791): 1276–9. Bibcode:2006Sci...313.1276P. doi:10.1126/science.1129630. PMID 16946068. 
  24. ^ a b Pfitzner, A; Bräu, Mf; Zweck, J; Brunklaus, G; Eckert, H (Aug 2004). "Phosphorus nanorods – two allotropic modifications of a long-known element". Angewandte Chemie (International ed. in English) 43 (32): 4228–31. doi:10.1002/anie.200460244. PMID 15307095. 
  25. ^ A. Holleman, N. Wiberg (1985). "XV 2.1.3". Lehrbuch der Anorganischen Chemie (33 ed.). de Gruyter. ISBN 3-11-012641-9. 
  26. ^ Berger, L. I. (1996). Semiconductor materials. CRC Press. p. 84. ISBN 0-8493-8912-7. 

External links[edit]

White phosphorus