Phosphorus pentoxide

{{chembox

| ImageFileL1 = Phosphorus-pentoxide-2D-dimensions.svg

| ImageSizeL1 = 150px

| ImageClassL1 = skin-invert

| ImageNameL1 = Phosphorus pentoxide

| ImageFileR1 = Phosphorus-pentoxide-3D-balls.png

| ImageSizeR1 = 150px

| ImageClassR1 = bg-transparent

| ImageNameR1 = Phosphorus pentoxide

| ImageFile2 = Sample of Phosphorus pentoxide.jpg

| ImageSize2 = 150

|IUPACName=Tetraphosphorus decaoxide
Tricyclo[3.3.1.1^3,7]tetraphosphoxane 1,3,5,7-tetraoxide

|SystematicName=2,4,6,8,9,10-Hexaoxa-1λ⁵,3λ⁵,5λ⁵,7λ⁵-tetraphosphatricyclo[3.3.1.1^3,7]decane 1,3,5,7-tetraoxide

| OtherNames = Diphosphorus pentoxide
Phosphorus(V) oxide
Phosphoric anhydride
Tetraphosphorus decaoxide
Tetraphosphorus decoxide

| Section1 = {{Chembox Identifiers

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChI = 1S/O10P4/c1-11-5-12(2)8-13(3,6-11)10-14(4,7-11)9-12

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey = DLYUQMMRRRQYAE-UHFFFAOYSA-N

| ChEBI_Ref = {{ebicite|correct|EBI}}

| ChEBI = 37376

| SMILES = O=P13OP2(=O)OP(=O)(O1)OP(=O)(O2)O3

| SMILES_Comment = molecular form

| SMILES1 = P12(=O)OP3(=O)OP4(=O)OP5(=O)OP6(=O)OP(=O)(O1)OP7(=O)OP(=O)OP(=O)OP(=O)(O2)OP(=O)OP(=O)OP(=O)(O3)OP(=O)OP(=O)OP(=O)(O4)OP(=O)OP(=O)OP(=O)(O5)OP(=O)OP(=O)OP(=O)(O6)OP(=O)OP(=O)(O7)O

| SMILES1_Comment = crystal o′ form

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

| CASNo = 1314-56-3

| CASNo2_Ref = {{cascite|correct|CAS}}

| CASNo2 = 16752-60-6

| CASNo2_Comment = (P₄O₁₀)

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 51SWB7223J

| PubChem = 14812

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChemSpiderID = 14128

| RTECS = TH3945000

}}

| Section2 = {{Chembox Properties

| Formula = P₄O₁₀

| MolarMass = 283.9 g mol⁻¹

| Appearance = White powder
Very deliquescent

| Odor = Odorless

| Density = 2.39 g/cm³

| Solubility = exothermic hydrolysis

| MeltingPtC = 340

| BoilingPt = 360 °C (sublimes)

| VaporPressure = 1 mmHg @ 385 °C (stable form)

}}

| Section7 = {{Chembox Hazards

| GHSPictograms = {{GHS05}}

| GHSSignalWord = DANGER

| HPhrases = {{H-phrases|314}}

| PPhrases = {{P-phrases|280|301+330+331|303+361+353|305+351+338|310}}

| MainHazards = reacts with water, strong dehydrating agent, corrosive

| ExternalSDS = [http://hazard.com/msds/mf/baker/baker/files/p4116.htm MSDS]

| NFPA-H = 3

| NFPA-R = 3

| NFPA-F = 0

| NFPA-S = W

}}

Phosphorus pentoxide is a chemical compound with molecular formula P₄O₁₀ (with its common name derived from its empirical formula, P₂O₅). This white crystalline solid is the anhydride of phosphoric acid. It is a powerful desiccant and dehydrating agent.

Structure

Phosphorus pentoxide crystallizes in at least four forms or polymorphs. The most familiar one, a metastable form{{Greenwood&Earnshaw2nd}} (shown in the figure), comprises molecules of P₄O₁₀. 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{{cite journal|author=Cruickshank, D. W. J. |title=Refinements of Structures Containing Bonds between Si, P, S or Cl and O or N: V. P₄O₁₀|journal=Acta Crystallogr. |year=1964|volume=17|issue=6|pages=677–9|doi=10.1107/S0365110X64001669|doi-access=free}}). The structure of the P₄O₁₀ cage is reminiscent of adamantane with T_d symmetry point group.D. E. C. Corbridge "Phosphorus: An Outline of its Chemistry, Biochemistry, and Technology" 5th Edition Elsevier: Amsterdam. {{ISBN|0-444-89307-5}}. It is closely related to the corresponding anhydride of phosphorous acid, P₄O₆. The latter lacks terminal oxo groups. Its density is 2.30 g/cm³. 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, and the result is an extremely hygroscopic solid..{{cite book

| title = Inorganic Chemistry, 3rd Edition

| chapter = Chapter 15: The group 15 elements

| author1 = Catherine E. Housecroft

| author2 = Alan G. Sharpe

| publisher = Pearson

| year = 2008

| isbn = 978-0-13-175553-6

| page = 473

}}

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/cm³, melting point 562 °C) adopts a layered structure consisting of interconnected P₆O₆ rings, not unlike the structure adopted by certain polysilicates. 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/cm³.{{cite journal|journal = Acta Crystallogr. C |volume = 51|issue = 6|date=June 1995|pages = 1049–1050|doi = 10.1107/S0108270194012126|title = Phosphorus Pentoxide at 233 K|author = D. Stachel, I. Svoboda and H. Fuess| bibcode=1995AcCrC..51.1049S }} The remaining polymorph is a glass or amorphous form; it can be made by fusing any of the others.

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| File:Phosphorus-pentoxide-sheet-from-xtal-3D-balls.png

File:Phosphorus-pentoxide-xtal-3D-balls.png

Part of an o′-(P₂O₅)_∞ layer

o′-(P₂O₅)_∞ layers stacking

Preparation

P₄O₁₀ is prepared by burning white phosphorus with a sufficient supply of oxygen:Threlfall, Richard E., (1951). The story of 100 years of Phosphorus Making: 1851 - 1951. Oldbury: Albright & Wilson Ltd

: P₄ + 5 O₂ → P₄O₁₀

The dehydration of phosphoric acid to give phosphorus pentoxide is not possible, as on heating it forms various polyphosphates but will not dehydrate sufficiently to form P₄O₁₀.

Applications

Phosphorus pentoxide is a potent dehydrating agent as indicated by the exothermic nature of its hydrolysis producing phosphoric acid:

:P₄O₁₀ + 6 H₂O → 4 H₃PO₄ (−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 P₄O₁₀ is used in desiccators.

Consistent with its strong desiccating power, P₄O₁₀ is used in organic synthesis for dehydration. The most important application is for the conversion of primary amides into nitriles:Meier, M. S. "Phosphorus(V) Oxide" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. {{doi|10.1002/047084289X}}.

:P₄O₁₀ + RC(O)NH₂ → P₄O₉(OH)₂ + RCN

The indicated coproduct P₄O₉(OH)₂ is an idealized formula for undefined products resulting from the hydration of P₄O₁₀.

Alternatively, when combined with a carboxylic acid, the result is the corresponding anhydride:{{cite book|url=https://books.google.com/books?id=pzRpQC7CO6sC&pg=PA1417|page=1417|title=Polymeric materials encyclopedia: C, Volume 2|editor=Joseph C. Salamone|publisher=CRC Press|year=1996|isbn=0-8493-2470-X}}

:P₄O₁₀ + RCO₂H → P₄O₉(OH)₂ + [RC(O)]₂O

The "Onodera reagent", a solution of P₄O₁₀ in DMSO, is employed for the oxidation of alcohols.Tidwell,

T. T. "Dimethyl Sulfoxide–Phosphorus Pentoxide" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. {{doi|10.1002/047084289X}}. This reaction is reminiscent of the Swern oxidation.

The desiccating power of P₄O₁₀ is strong enough to convert many mineral acids to their anhydrides. Examples: HNO₃ is converted to N₂O₅; H₂SO₄ is converted to SO₃; HClO₄ is converted to Cl₂O₇; CF₃SO₃H is converted to (CF₃)₂S₂O₅.

= As a proxy measurement =

{{Chem2|P2O5}} content is often used by industry as proxy value for all the phosphorus oxides in a material. For example, fertilizer grade phosphoric acid can also contain various related phosphorous compounds which are also of use. All these compounds are described collectively in terms of '{{Chem2|P2O5}} content' to allow convenient comparison of the phosphorous content of different products. Despite this, phosphorus pentoxide is not actually present in most samples as it is not stable in aqueous solutions.

Hazards

Phosphorus pentoxide itself is not flammable. Just like sulfur trioxide, it reacts vigorously with water and water-containing substances like wood or cotton, liberates much heat and may even cause fire due to the highly exothermic nature of such reactions. 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/m³.[http://hazard.com/msds/mf/baker/baker/files/p4116.htm Phosphorus pentoxide MSDS]