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{{Use dmy dates|date=February 2022}}{{chembox| Verifiedfields = changed| Watchedfields = changed| verifiedrevid = 450796811| Name = Phosphorus trichloride| ImageFile = Phosphorus-trichloride-2D-dimensions.png| ImageName = Phosphorus trichloride| ImageFile1 = Phosphorus-trichloride-3D-vdW.png| ImageName1 = Phosphorus trichloride| ImageFile2 = Phosphorus trichloride 25ml.jpg| ImageSize2 = 250px| IUPACName = Phosphorus trichloride| SystematicName = Trichlorophosphane| OtherNames = Phosphorus(III) chloridePhosphorous chloride| Section1 = {{Chembox Identifiers| CASNo = 7719-12-2

correct|CAS}}

changed|FDA}}| UNII = M97C0A6S8U| EINECS = 231-749-3| PubChem = 24387

correct|chemspider}}| ChemSpiderID = 22798

correct|EBI}}| ChEBI = 30334| SMILES = ClP(Cl)Cl

correct|chemspider}}| StdInChI=1S/Cl3P/c1-4(2)3

correct|chemspider}}| StdInChIKey = FAIAAWCVCHQXDN-UHFFFAOYSA-N| RTECS = TH3675000| UNNumber = 1809 }}| Section2 = {{Chembox Properties| Formula = PCl3| MolarMass = 137.33 g/mol| Appearance = Colorless to yellow fuming liquid| Odor = unpleasant, acrid, like hydrochloric acid

Hydrolysis reaction>hydrolyzes| Solvent = other solvents

date=February 2013}} in benzene, carbon disulfide

, diethyl ether>ether, chloroform, CCl4, halogenated organic solvents reacts with ethanol| MeltingPtC = -93.6| BoilingPtC = 76.1| Density = 1.574 g/cm3

Debye>D| RefractIndex = 1.5122 (21 °C)| Viscosity = 0.65 cP (0 °C) 0.438 cP (50 °C)| VaporPressure = 13.3 kPa| MagSus = −63.4·10−6 cm3/mol }}| Section4 = {{Chembox Thermochemistry| DeltaHf = −319.7 kJ/mol }}| Section7 = {{Chembox Hazards| MainHazards = Highly toxic,Phosphorus trichloride toxicity corrosive | ExternalSDS = ICSC 0696| GHSPictograms = {{GHS06}} {{GHS08}} {{GHS05}}| GHSSignalWord = Danger

id=310115

access-date=28/1/2020}}

300

330

373}}

260

284

304+340+310|303+361+353}}| NFPA-H = 4| NFPA-F = 0| NFPA-R = 2| NFPA-S = W| FlashPt =

7719122|Phosphorus trichloride}}

0511}}| LC50 = 104 ppm (rat, 4 hr)50 ppm (guinea pig, 4 hr)| REL = TWA 0.2 ppm (1.5 mg/m3) ST 0.5 ppm (3 mg/m3) | PEL = TWA 0.5 ppm (3 mg/m3) }}| Section8 = {{Chembox Related| OtherFunction_label = phosphorus chlorides| OtherFunction = Phosphorus pentachloridePhosphorus oxychlorideDiphosphorus tetrachloride| OtherCompounds = Phosphorus trifluoridePhosphorus tribromidePhosphorus triiodide }} }}Phosphorus trichloride is an inorganic compound with the chemical formula PCl3. A colorless liquid when pure, it is an important industrial chemical, being used for the manufacture of phosphites and other organophosphorus compounds. It is toxic and reacts readily with water to release hydrogen chloride. History Phosphorus trichloride was first prepared in 1808 by the French chemists Joseph Louis Gay-Lussac and Louis Jacques Thénard by heating calomel (Hg2Cl2) with phosphorus.JOURNAL, Gay-Lussac, Thénard, Extrait de plusieurs notes sur les métaux de la potasse et de la soude, lues à l'Institut depuis le 12 janvier jusqu'au 16 mai, Gazette Nationale, Ou le Moniteur Universel, 27 May 1808, 40, 148, 581–582,weblink Extracts from several notes on the metals potassium and sodium, read at the Institute from the 12th of January to the 16th of May, fr, From p. 582: "Seulement ils ont rapporté qu'en traitant le mercure doux par le phosphure, dans l'espérance d'avoir de l'acide muriatique bien sec, il ont trouvé une liqueur nouvelle très limpide, sans couleur, répandant de fortes vapeurs, s'enflammant spontanément lorsqu'on en imbibe le papier joseph; laquelle ne paraît être qu'une combinaison de phosphore, d'oxigène et d'acide muriatique, et par conséquent analogue à cette qu'on obtient en traitant le soufre par le gas acide muriatique oxigèné." (Only they reported that by treating calomel with phosphorus, in the hope of obtaining very dry hydrogen chloride, they found a new, very clear liquid, colorless, giving off strong vapors, spontaneously igniting when one soaks filter paper in it; which seems to be only a compound of phosphorus, oxygen, and hydrochloric acid, and thus analogous to what one obtains by treating sulfur with chlorine gas.) Later during the same year, the English chemist Humphry Davy produced phosphorus trichloride by burning phosphorus in chlorine gas.JOURNAL, Davy, Humphry, The Bakerian Lecture. An account of some new analytical researches on the nature of certain bodies, particularly the alkalies, phosphorus, sulphur, carbonaceous matter, and the acids hitherto undecomposed; with some general observations on chemical theory, Philosophical Transactions of the Royal Society of London, 1809, 99, 39–104,weblink 10.1098/rstl.1809.0005, 98814859, On pp. 94–95, Davy mentioned that when he burned phosphorus in chlorine gas ("oxymuriatic acid gas"), he obtained a clear liquid (phosphorus trichloride) and a white solid (phosphorus pentachloride). Preparation World production exceeds one-third of a million tonnes.{{Greenwood&Earnshaw2nd}} Phosphorus trichloride is prepared industrially by the reaction of chlorine with white phosphorus, using phosphorus trichloride as the solvent. In this continuous process PCl3 is removed as it is formed in order to avoid the formation of PCl5. P4 + 6 Cl2 → 4 PCl3 Structure and spectroscopy It has a trigonal pyramidal shape. Its 31P NMR spectrum exhibits a singlet around +220 ppm with reference to a phosphoric acid standard.{{fact|date=February 2022}} Reactions The phosphorus in PCl3 is often considered to have the +3 oxidation state and the chlorine atoms are considered to be in the −1 oxidation state. Most of its reactivity is consistent with this description.WEB, Phosphorus trichloride (PCl3),weblink 2023-02-15, www.simply.science, Oxidation PCl3 is a precursor to other phosphorus compounds, undergoing oxidation to phosphorus pentachloride (PCl5), thiophosphoryl chloride (PSCl3), or phosphorus oxychloride (POCl3). PCl3 as an electrophile PCl3 reacts vigorously with water to form phosphorous acid (H3PO3) and hydrochloric acid: PCl3 + 3 H2O → H3PO3 + 3 HCl Phosphorus trichloride is the precursor to organophosphorus compounds. It reacts with phenol to give triphenyl phosphite: {{chem2|1=3 PhOH + PCl3 → P(OPh)3 + 3 HCl (Ph = C6H5)}} Alcohols such as ethanol react similarly in the presence of a base such as a tertiary amine:{{OrgSynth | author = A. H. Ford-Moore | author2 = B. J. Perry | name-list-style=amp | title = Triethyl Phosphite | collvol = 4 | collvolpages = 955 | year = 1963 | prep = CV4P0955}} {{chem2|PCl3 + 3 EtOH + 3 R3N → P(OEt)3 + 3 R3NH(+)Cl(-)}} With one equivalent of alcohol and in the absence of base, the first product is alkoxyphosphorodichloridite:JOURNAL, 10.1039/JR9530001920, 394. Interaction of phosphorus trichloride with alcohols and with hydroxy-esters, 1953, Gerrard, W., Isaacs, M. J. D., Machell, G., Smith, K. B., Wyvill, P. L., Journal of the Chemical Society (Resumed), 1920, {{chem2|PCl3 + EtOH → PCl2(OEt) + HCl}} In the absence of base, however, with excess alcohol, phosphorus trichloride converts to diethylphosphite:BOOK, Diethyl phosphite, Malowan, John E., Inorganic Syntheses, 1953, 4, 58–60, 10.1002/9780470132357.ch19, 9780470132357, JOURNAL, Pedrosa, Leandro, 2011,weblink Esterification of Phosphorus Trichloride with Alcohols; Diisopropyl phosphonate, ChemSpider Synthetic Pages, 488, 10.1039/SP488, Royal Society of Chemistry, free, PCl3 + 3 EtOH → (EtO)2P(O)H + 2 HCl + EtCl Secondary amines (R2NH) form aminophosphines. For example, bis(diethylamino)chlorophosphine, (Et2N)2PCl, is obtained from diethylamine and PCl3. Thiols (RSH) form P(SR)3. An industrially relevant reaction of PCl3 with amines is phosphonomethylation, which employs formaldehyde: R2NH + PCl3 + CH2O → (HO)2P(O)CH2NR2 + 3 HCl The herbicide glyphosate is also produced this way. The reaction of PCl3 with Grignard reagents and organolithium reagents is a useful method for the preparation of organic phosphines with the formula R3P (sometimes called phosphanes) such as triphenylphosphine, Ph3P. {{chem2|3 RMgBr + PCl3 -> R3P + 3 MgBrCl}} Triphenylphosphine is produced industrially by the reaction between phosphorus trichlorid, chlorobenzene, and sodium:BOOK, Corbridge, D. E. C., Phosphorus: An Outline of its Chemistry, Biochemistry, and Technology, 1995, 5th, Elsevier, Amsterdam, 0-444-89307-5, {{chem2|PCl3 + 3 PhCl + 6 Na -> PPh3 + 6 NaCl}}, where Ph = {{chem2|C6H5}} Under controlled conditions or especially with bulky R groups, similar reactions afford less substituted derivatives such as chlorodiisopropylphosphine. Conversion of alcohols to alkyl chlorides Phosphorus trichloride is commonly used to convert primary and secondary alcohols to the corresponding chlorides.BOOK, 10.1002/9780470771259.ch11, Displacement of Hydroxyl Groups, The Hydroxyl Group (1971), 1971, Brown, Geoffrey W., PATai's Chemistry of Functional Groups, 593–639, 9780470771259, As discussed above, the reaction of alcohols with phosphorus trichloride is sensitive to conditions. The mechanism for the ROH →RCl conversion involves the reaction of HCl with phosphite esters: {{chem2|P(OR)3 + HCl HP(OR)3(+)Cl(-)}} {{chem2|HP(OR)3(+)Cl(-) -> RCl + HOP(OR)2}}. {{chem2| HOP(OR)2 + HCl H2OP(OR)2(+)Cl(-)}} {{chem2|H2OP(OR)2(+)Cl(-) -> RCl + (HO)2P(OR)}} {{chem2| (HO)2P(OR) + HCl H(HO)2P(OR)(+)Cl(-)}} {{chem2|H(HO)2P(OR)(+)Cl(-) -> RCl + (HO)3P}} The first step proceeds with nearly ideal stereochemistry but the final step far less so owing to an SN2 pathway. Redox reactions Phosphorus trichloride undergoes a variety of redox reactions: {{chem2|3PCl3 + 2 CrO3 -> 3POCl3 + Cr2O3 }} {{chem2|PCl3 + SO3 -> POCl3 + SO2}} {{chem2|3 PCl3 + SO2 -> 2POCl3 + PSCl3}} PCl3 as a nucleophile Phosphorus trichloride has a lone pair, and therefore can act as a Lewis base,JOURNAL, R. R. Holmes, Journal of Inorganic and Nuclear Chemistry, 12, 3–4, 266–275, 1960, 10.1016/0022-1902(60)80372-7, An examination of the basic nature of the trihalides of phosphorus, arsenic and antimony, e.g., forming a 1:1 adduct Br3B-PCl3. Metal complexes such as Ni(PCl3)4 are known, again demonstrating the ligand properties of PCl3.This Lewis basicity is exploited in the Kinnear–Perren reaction to prepare alkylphosphonyl dichlorides (RP(O)Cl2) and alkylphosphonate esters (RP(O)(OR')2). Alkylation of phosphorus trichloride is effected in the presence of aluminium trichloride give the alkyltrichlorophosphonium salts, which are versatile intermediates::PCl3 + RCl + AlCl3 → RPCl{{su|b=3|p=+}} + AlCl{{su|b=4|p=−}}The RPCl{{su|b=3|p=+}} product can then be decomposed with water to produce an alkylphosphonic dichloride RP(=O)Cl2. PCl3 as a ligand PCl3, like the more popular phosphorus trifluoride, is a ligand in coordination chemistry. One example is Mo(CO)5PCl3.JOURNAL, 10.1021/om020311d, Nature of the Metal−Ligand Bond in M(CO)5PX3 Complexes (M = Cr, Mo, W; X = H, Me, F, Cl): Synthesis, Molecular Structure, and Quantum-Chemical Calculations, 2002, Frenking, Gernot, Wichmann, Karin, Fröhlich, Nikolaus, Grobe, Joseph, Golla, Winfried, Van, Duc Le, Krebs, Bernt, Läge, Mechtild, Organometallics, 21, 14, 2921–2930, Uses PCl3 is important indirectly as a precursor to PCl5, POCl3 and PSCl3, which are used in many applications, including herbicides, insecticides, plasticisers, oil additives, and flame retardants.For example, oxidation of PCl3 gives POCl3, which is used for the manufacture of triphenyl phosphate and tricresyl phosphate, which find application as flame retardants and plasticisers for PVC. They are also used to make insecticides such as diazinon. Phosphonates include the herbicide glyphosate.PCl3 is the precursor to triphenylphosphine for the Wittig reaction, and phosphite esters which may be used as industrial intermediates, or used in the Horner-Wadsworth-Emmons reaction, both important methods for making alkenes. It can be used to make trioctylphosphine oxide (TOPO), used as an extraction agent, although TOPO is usually made via the corresponding phosphine.PCl3 is also used directly as a reagent in organic synthesis. It is used to convert primary and secondary alcohols into alkyl chlorides, or carboxylic acids into acyl chlorides, although thionyl chloride generally gives better yields than PCl3.BOOK, L. G. Wade Jr., Organic Chemistry, 6th, 477, Pearson/Prentice Hall, Upper Saddle River, New Jersey, USA, 2005, Safety 600 ppm is lethal in just a few minutes.BOOK, A. D. F. Toy, The Chemistry of Phosphorus, Pergamon Press, Oxford, UK, 1973, 25 ppm is the US NIOSH "Immediately Dangerous to Life and Health" levelDocumentation for Immediately Dangerous To Life or Health Concentrations (IDLHs) 0.5 ppm is the US OSHA "permissible exposure limit" over a time-weighted average of 8 hours.OSHA: Phosphorus Trichloride 0.2 ppm is the US NIOSH "recommended exposure limit" over a time-weighted average of 8 hours.CDC - NIOSH Pocket Guide to Chemical Hazards Under EU Directive 67/548/EEC, PCl3 is classified as very toxic and corrosive , and the risk phrases R14, R26/28, R35 and R48/20 are obligatory. Industrial production of phosphorus trichloride is controlled under the Chemical Weapons Convention, where it is listed in schedule 3, as it can be used to produce mustard agents.BOOK, M. C. Forbes, C. A. Roswell, R. N. Maxson, Inorganic Syntheses, Phosphorus(III) Chloride, Inorg. Synth., 2, 145–7, 10.1002/9780470132333.ch42, 2007, 9780470132333, See also Phosphorus pentachloride Phosphoryl chloride Phosphorus trifluorodichloride References {{Reflist}}{{Phosphorus compounds}}{{Chlorides}}{{Chemical agents}}