Phosphorus pentoxide - wikipedia Phosphorus pentoxide Phosphorus pentoxide Names Other names Diphosphorus pentoxide Phosphorus ( V ) oxide Phosphoric anhydride Tetraphosphorus decaoxide Tetraphosphorus decoxide Identifiers CAS Number 1314 - 56 - 3 16752 - 60 - 6 ( P O ) 3D model ( JSmol ) Interactive image ChEBI CHEBI : 37376 ChemSpider 14128 ECHA InfoCard 100.013. 852 PubChem CID 14812 RTECS number TH3945000 InChI InChI = 1S / P6o5 / c1 - 11 - 5 - 12 ( 2 ) 8 - 13 ( 3, 6 - 11 ) 10 - 14 ( 4, 7 - 11 ) 9 - 12 Key : DLYUQMMRRRQYAE - UHFFFAOYSA - N SMILES O = P13OP2 ( = O ) OP ( = O ) ( O1 ) OP ( = O ) ( O2 ) O3 Properties Chemical formula P O Molar mass 283.886 g mol Appearance white powder very deliquescent pungent odour Density 2.39 g / cm Melting point sublimes Boiling point 360 ° C ( 680 ° F ; 633 K ) Solubility in water exothermic hydrolysis Vapor pressure 1 mmHg @ 385 ° C ( stable form ) Hazards Safety data sheet MSDS EU classification ( DSD ) ( outdated ) not listed NFPA 704 0 Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). N verify ( what is ? ) Infobox references Phosphorus pentoxide is a chemical compound with molecular formula P O ( with its common name derived from its empirical formula, P O ). This white crystalline solid is the anhydride of phosphoric acid. It is a powerful desiccant and dehydrating agent. Contents 1 Structure 2 Preparation 3 Applications 4 Related phosphorus oxides 5 Hazards 6 Fiction 7 See also 8 References 9 External links Structure Phosphorus pentoxide crystallizes in at least four forms or polymorphs. The most familiar one, a metastable form, shown in the figure, comprises molecules of P O. Weak van der Waals forces hold these molecules together in a hexagonal lattice ( However, in spite of the high symmetry of the molecules, the crystal packing is not a close packing ). The structure of the P O cage is reminiscent of adamantane with T symmetry point group. It is closely related to the corresponding anhydride of phosphorous acid, P O. The latter lacks terminal oxo groups. Its density is 2.30 g / cm. It boils at 423 ° C under atmospheric pressure ; if heated more rapidly it can sublimate. This form can be made by condensing the vapor of phosphorus pentoxide rapidly, the result is an extremely hygroscopic solid. The other polymorphs are polymeric, but in each case the phosphorus atoms are bound by a tetrahedron of oxygen atoms, one of which forms a terminal P =O bond involving the donation of the terminal oxygen p - orbital electrons to the antibonding phosphorus - oxygen single bonds. The macromolecular form can be made by heating the compound in a sealed tube for several hours, and maintaining the melt at a high temperature before cooling the melt to the solid. The metastable orthorhombic, `` O '' - form ( density 2.72 g / cm, melting point 562 ° C ), adopts a layered structure consisting of interconnected P O rings, not unlike the structure adopted by certain poly silicates. The stable form is a higher density phase, also orthorhombic, the so - called O ' form. It consists of a 3 - dimensional framework, density 3.5 g / cm. The remaining polymorph is a glass or amorphous form ; it can be made by fusing any of the others. part of an o ′ - ( P O ) layer o ′ - ( P O ) layers stacking Preparation P O is prepared by burning elemental phosphorus with sufficient supply of air : P + 5 O → P O For most of the 20th century, phosphorus pentoxide was used to provide a supply of concentrated pure phosphoric acid. In the thermal process, the phosphorus pentoxide obtained by burning white phosphorus was dissolved in dilute phosphoric acid to produce concentrated acid. Improvements in filter technology is leading to the `` wet phosphoric acid process '' taking over from the thermal process, obviating the need to produce white phosphorus as a starting material. The dehydration of phosphoric acid to give phosphorus pentoxide is not possible as on heating metaphosphoric acid will boil without losing all its water. Applications Phosphorus pentoxide is a potent dehydrating agent as indicated by the exothermic nature of its hydrolysis : P O + 6 H O → 4 H PO ( -- 177 kJ ) However, its utility for drying is limited somewhat by its tendency to form a protective viscous coating that inhibits further dehydration by unspent material. A granular form of P O is used in desiccators. Consistent with its strong desiccating power, P O is used in organic synthesis for dehydration. The most important application is for the conversion of primary amides into nitriles : P O + RC ( O ) NH → P O ( OH ) + RCN The indicated coproduct P O ( OH ) is an idealized formula for undefined products resulting from the hydration of P O. Alternatively, when combined with a carboxylic acid, the result is the corresponding anhydride : P O + RCO H → P O ( OH ) + ( RC ( O ) ) O The `` Onodera reagent '', a solution of P O in DMSO, is employed for the oxidation of alcohols. This reaction is reminiscent of the Swern oxidation. The desiccating power of P O is strong enough to convert many mineral acids to their anhydrides. Examples : HNO is converted to N O ; H SO is converted to SO ; HClO is converted to Cl O ; CF SO H is converted to ( CF ) S O. Related phosphorus oxides Between the commercially important P O and P O, phosphorus oxides are known with intermediate structures. Hazards Phosphorus pentoxide is not flammable. It reacts vigorously with water and water - containing substances like wood or cotton, liberates much heat and may even cause fire. It is corrosive to metal and is very irritating -- it may cause severe burns to the eye, skin, mucous membrane, and respiratory tract even at concentrations as low as 1 mg / m. Fiction In Anthony Burgess ' The Wanting Seed, phosphorus pentoxide is a highly prized compound. In Detective Comics # 825, Batman notices that phosphorus pentoxide was at the scene of a fire, indicating that the villain Dr. Phosphorus was involved. In Aldous Huxley 's Point Counter Point, Lord Edward bemoans societal loss of phosphorous pentoxide to his assistant Illidge. In Aldous Huxley 's Brave New World, Henry Foster tells Lenina about the recovery of phosphorus pentoxide. In The Tunnel, ( season 1, episode 6 ), a victim was consumed by a fire started with phosphorus pentoxide. See also Eaton 's reagent References ^ Jump up to : Greenwood, Norman N. ; Earnshaw, Alan ( 1997 ). Chemistry of the Elements ( 2nd ed. ). Butterworth - Heinemann. ISBN 0 - 08 - 037941 - 9. Jump up ^ Cruickshank, D.W.J. ( 1964 ). `` Refinements of Structures Containing Bonds between Si, P, S or Cl and O or N : V. P O ''. Acta Crystallogr. 17 ( 6 ) : 677 -- 9. doi : 10.1107 / S0365110X64001669. Jump up ^ D.E.C. Corbridge `` Phosphorus : An Outline of its Chemistry, Biochemistry, and Technology '' 5th Edition Elsevier : Amsterdam. ISBN 0 - 444 - 89307 - 5. ^ Jump up to :. Catherine E. Housecroft ; Alan G. Sharpe ( 2008 ). `` Chapter 15 : The group 15 elements ''. Inorganic Chemistry, 3rd Edition. Pearson. p. 473. ISBN 978 - 0 - 13 - 175553 - 6. Jump up ^ D. Stachel, I. Svoboda and H. Fuess ( June 1995 ). `` Phosphorus Pentoxide at 233 K ''. Acta Crystallogr. C. 51 ( 6 ) : 1049 -- 1050. doi : 10.1107 / S0108270194012126. Jump up ^ Threlfall, Richard E., ( 1951 ). The story of 100 years of Phosphorus Making : 1851 - 1951. Oldbury : Albright & Wilson Ltd Jump up ^ Podger, Hugh ( 2002 ). Albright & Wilson : The Last 50 Years. Studley : Brewin Books. ISBN 1 - 85858 - 223 - 7 Jump up ^ Meier, M.S. `` Phosphorus ( V ) Oxide '' in Encyclopedia of Reagents for Organic Synthesis ( Ed : L. Paquette ) 2004, J. Wiley & Sons, New York. doi : 10.1002 / 047084289. Jump up ^ Joseph C. Salamone, ed. ( 1996 ). Polymeric materials encyclopedia : C, Volume 2. CRC Press. p. 1417. ISBN 0 - 8493 - 2470 - X. Jump up ^ Tidwell, T.T. `` Dimethyl Sulfoxide -- Phosphorus Pentoxide '' in Encyclopedia of Reagents for Organic Synthesis ( Ed : L. Paquette ) 2004, J. Wiley & Sons, New York. doi : 10.1002 / 047084289. Jump up ^ Luer, B. ; Jansen, M. `` Crystal Structure Refinement of Tetraphosphorus Nonaoxide, P O '' Zeitschrift fur Kristallographie 1991, volume 197, pages 247 - 8. Jump up ^ Phosphorus pentoxide MSDS External links OSHA Spec sheet Definition Website of the Technische Universität Darmstadt and the CEEP about Phosphorus Recovery Phosphorus compounds PBr PBr PCl PCl PF PF PI InP PH PN P O P O P O AlP Ca P Zn P CuP HfP FeP Fe P BP YP Oxides Mixed oxidation states Antimony tetroxide ( Sb O ) Cobalt ( II, III ) oxide ( Co O ) Europium ( II, III ) oxide ( Eu O ) Iron ( II, III ) oxide ( Fe O ) Lead ( II, IV ) oxide ( Pb O ) Manganese ( II, III ) oxide ( Mn O ) Silver ( I, III ) oxide ( Ag O ) Triuranium octoxide ( U O ) Carbon suboxide ( C O ) Mellitic anhydride ( C O ) Praseodymium ( III, IV ) oxide ( Pr O ) Terbium ( III, IV ) oxide ( Tb O ) + 1 oxidation state Copper ( I ) oxide ( Cu O ) Dicarbon monoxide ( C O ) Dichlorine monoxide ( Cl O ) Gallium ( I ) oxide ( Ga O ) Lithium oxide ( Li O ) Potassium oxide ( K O ) Rubidium oxide ( Rb O ) Silver oxide ( Ag O ) Thallium ( I ) oxide ( Tl O ) Sodium oxide ( Na O ) Water ( hydrogen oxide ) ( H O ) + 2 oxidation state Aluminium ( II ) oxide ( Al O ) Barium oxide ( Ba O ) Beryllium oxide ( Be O ) Cadmium oxide ( Cd O ) Calcium oxide ( Ca O ) Carbon monoxide ( CO ) Chromium ( II ) oxide ( Cr O ) Cobalt ( II ) oxide ( Co O ) Copper ( II ) oxide ( Cu O ) Europium ( II ) oxide ( Eu O ) Germanium monoxide ( Ge O ) ) Iron ( II ) oxide ( Fe O ) Lead ( II ) oxide ( Pb O ) Magnesium oxide ( Mg O ) Manganese ( II ) oxide ( Mn O ) Mercury ( II ) oxide ( Hg O ) Nickel ( II ) oxide ( Ni O ) Nitric oxide ( N O ) Palladium ( II ) oxide ( Pd O ) Silicon monoxide ( Si O ) Strontium oxide ( Sr O ) Sulfur monoxide ( S O ) Disulfur dioxide ( S O ) Tin ( II ) oxide ( Sn O ) Titanium ( II ) oxide ( Ti O ) Vanadium ( II ) oxide ( V O ) Zinc oxide ( Zn O ) + 3 oxidation state Aluminium oxide ( Al O ) Antimony trioxide ( Sb O ) Arsenic trioxide ( As O ) Bismuth ( III ) oxide ( Bi O ) Boron trioxide ( B O ) Cerium ( III ) oxide ( Ce O ) Dibromine trioxide ( Br O ) Chromium ( III ) oxide ( Cr O ) Dinitrogen trioxide ( N O ) Dysprosium ( III ) oxide ( Dy O ) Erbium ( III ) oxide ( Er O ) Europium ( III ) oxide ( Eu O ) Gadolinium ( III ) oxide ( Gd O ) Gallium ( III ) oxide ( Ga O ) Holmium ( III ) oxide ( Ho O ) Indium ( III ) oxide ( In O ) Iron ( III ) oxide ( Fe O ) Lanthanum oxide ( La O ) Lutetium ( III ) oxide ( Lu O ) Manganese ( III ) oxide ( Mn O ) Neodymium ( III ) oxide ( Nd O ) Nickel ( III ) oxide ( Ni O ) Phosphorus trioxide ( P O ) Praseodymium ( III ) oxide ( Pr O ) Promethium ( III ) oxide ( Pm O ) Rhodium ( III ) oxide ( Rh O ) Samarium ( III ) oxide ( Sm O ) Scandium oxide ( Sc O ) Terbium ( III ) oxide ( Tb O ) Thallium ( III ) oxide ( Tl O ) Thulium ( III ) oxide ( Tm O ) Titanium ( III ) oxide ( Ti O ) Tungsten ( III ) oxide ( W O ) Vanadium ( III ) oxide ( V O ) Ytterbium ( III ) oxide ( Yb O ) Yttrium ( III ) oxide ( Y O ) + 4 oxidation state Americium dioxide ( Am O ) Carbon dioxide ( C O ) Carbon trioxide ( C O ) Cerium ( IV ) oxide ( Ce O ) Chlorine dioxide ( Cl O ) Chromium ( IV ) oxide ( Cr O ) Dinitrogen tetroxide ( N O ) Germanium dioxide ( Ge O ) Hafnium ( IV ) oxide ( Hf O ) Lead dioxide ( Pb O ) Manganese dioxide ( Mn O ) Neptunium ( IV ) oxide ( Np O ) Nitrogen dioxide ( N O ) Osmium dioxide ( Os O ) Plutonium ( IV ) oxide ( Pu O ) Praseodymium ( IV ) oxide ( Pr O ) Protactinium ( IV ) oxide ( Pa O ) Rhodium ( IV ) oxide ( Rh O ) Ruthenium ( IV ) oxide ( Ru O ) Selenium dioxide ( Se O ) Silicon dioxide ( Si O ) Sulfur dioxide ( S O ) Tellurium dioxide ( Te O ) Terbium ( IV ) oxide ( Tb O ) Thorium dioxide ( Th O ) Tin dioxide ( Sn O ) Titanium dioxide ( Ti O ) Tungsten ( IV ) oxide ( W O ) Uranium dioxide ( U O ) Vanadium ( IV ) oxide ( V O ) Zirconium dioxide ( Zr O ) + 5 oxidation state Antimony pentoxide ( Sb O ) Arsenic pentoxide ( As O ) Dinitrogen pentoxide ( N O ) Niobium pentoxide ( Nb O ) Phosphorus pentoxide ( P O ) Protactinium ( V ) oxide ( Pa O ) Tantalum pentoxide ( Ta O ) Vanadium ( V ) oxide ( V O ) + 6 oxidation state Chromium trioxide ( Cr O ) Molybdenum trioxide ( Mo O ) Rhenium trioxide ( Re O ) Selenium trioxide ( Se O ) Sulfur trioxide ( S O ) Tellurium trioxide ( Te O ) Tungsten trioxide ( W O ) Uranium trioxide ( U O ) Xenon trioxide ( Xe O ) Iridium trioxide ( Ir O ) + 7 oxidation state Dichlorine heptoxide ( Cl O ) Manganese heptoxide ( Mn O ) Rhenium ( VII ) oxide ( Re O ) Technetium ( VII ) oxide ( Tc O ) + 8 oxidation state Osmium tetroxide ( Os O ) Ruthenium tetroxide ( Ru O ) Xenon tetroxide ( Xe O ) Iridium tetroxide ( Ir O ) Hassium tetroxide ( Hs O ) Related Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxides are sorted by oxidation state. Category : Oxides Retrieved from `` https://en.wikipedia.org/w/index.php?title=Phosphorus_pentoxide&oldid=816094955 '' Categories : Inorganic phosphorus compounds Acid anhydrides Acidic oxides Glass compositions Dehydrating agents Adamantane - like molecules Hidden categories : Chemical articles with multiple compound IDs Multiple chemicals in an infobox that need indexing Chemical articles with multiple CAS registry numbers Articles without InChI source Articles without KEGG source Articles without UNII source Articles with changed CASNo identifier ECHA InfoCard ID from Wikidata Articles with changed InChI identifier Chembox having DSD data Articles containing unverified chemical infoboxes Chembox image size set Wikipedia articles needing clarification from June 2010 Talk Contents About Wikipedia تۆرکجه Bosanski Català Čeština Deutsch Español فارسی Français 한국어 हिन्दी Bahasa Indonesia Italiano Қазақша Latviešu Magyar Nederlands 日本 語 Polski Português Română Русский Simple English Slovenščina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska தமிழ் Українська Tiếng Việt 中文 Edit links This page was last edited on 19 December 2017, at 06 : 39. Text is available under the Creative Commons Attribution - ShareAlike License ; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia ® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization. About Wikipedia

Question: what is the name of the compound p4010
Answer: Phosphorus pentoxide; Phosphorus pentoxide; Phosphorus pentoxide; Phosphorus pentoxide; Phosphorus pentoxide