Phosphoryl chloride

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Phosphoryl chloride
Phosphoryl chloride
Names
Preferred IUPAC name
Phosphoryl trichloride[1]
Other names
  • Phosphorus(V) oxychloride
  • Phosphoric trichloride
  • Trichlorophosphate
  • Phosphorus(V) oxide trichloride
Identifiers
3D model (
JSmol
)
ChEBI
ChemSpider
ECHA InfoCard
 100.030.030 Edit this at Wikidata
EC Number
  • 233-046-7
2272
RTECS number
  • TH4897000
UNII
UN number 1810
  • InChI=1S/Cl3OP/c1-5(2,3)4 checkY
    Key: XHXFXVLFKHQFAL-UHFFFAOYSA-N checkY
  • InChI=1/Cl3OP/c1-5(2,3)4
    Key: XHXFXVLFKHQFAL-UHFFFAOYAS
  • O=P(Cl)(Cl)Cl
  • [O-][P+](Cl)(Cl)Cl
Properties
POCl3
Molar mass 153.32 g·mol−1
Appearance colourless liquid, fumes in moist air
Odor pungent and musty
Density 1.645 g/cm3, liquid
Melting point 1.25 °C (34.25 °F; 274.40 K)
Boiling point 105.8 °C (222.4 °F; 378.9 K)
Reacts
Solubility highly soluble in benzene, chloroform, carbon disulfide, carbon tetrachloride
Vapor pressure 40 mmHg (27 °C)[2]
1.460
Structure
Tetrahedral at the P atom
2.54 D
Thermochemistry[3]
138.8 J·mol−1·K−1 (liquid), 84.9 J·mol−1·K−1 (gas)
222.5 J·mol−1·K−1 (liquid), 325.5 J·mol−1·K−1 (gas)
Std enthalpy of
formation
(ΔfH⦵298)
 −597.1 kJ·mol−1 (liquid), −558.5 kJ·mol−1 (gas)
−520.8 kJ·mol−1 (liquid), −512.9 kJ·mol−1(gas)
Enthalpy of fusion (ΔfH⦵fus)
 13.1 kJ·mol−1
38.6 kJ·mol−1
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
corrosive; releases HCl on contact with water[2]
GHS labelling:
GHS05: CorrosiveGHS06: ToxicGHS07: Exclamation markGHS08: Health hazard
Danger
H302, H314, H330, H372
P260, P264, P270, P271, P280, P284, P301+P312, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P314, P320, P321, P330, P363, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
3
0
2
W
Lethal dose or concentration (LD, LC):
380 mg/kg (rat, oral)
NIOSH (US health exposure limits):
PEL (Permissible)
 none[2]
REL (Recommended)
 TWA 0.1 ppm (0.6 mg/m3) ST 0.5 ppm (3 mg/m3)[2]
IDLH
(Immediate danger)
 N.D.[2]
Safety data sheet (SDS) ICSC 0190
Related compounds
Related compounds
Supplementary data page
Phosphoryl chloride (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Phosphoryl chloride (commonly called phosphorus oxychloride) is a colourless liquid with the formula

phosphate esters
.

Structure

Unit cell of phosphoryl chloride.[5]

Like phosphate, POCl3 is tetrahedral in shape.

dative π back-bond that produces an effective [P+]-[O−] configuration.[7]

Phosphoryl chloride exists as neutral POCl3 molecules in the

ionic form [PCl4]+[PCl6]− (tetrachlorophosphonium hexachlorophosphate(V)) in the solid state. The average bond lengths in the crystal structure of POCl3 are 1.98 Å for P–Cl and 1.46 Å for P=O.[5]

Physical properties

It has a

anions
.

Chemical properties

POCl3 reacts with water to give hydrogen chloride and phosphoric acid:

O=PCl3 + 3 H2O → O=P(OH)3 + 3 HCl

Intermediates in the conversion have been isolated, including pyrophosphoryl chloride, O(−P(=O)Cl2)2.[9]

Upon treatment with excess

phosphate esters
:

O=PCl3 + 3 ROH → O=P(OR)3 + 3 HCl

Such reactions are often performed in the presence of an HCl acceptor such as pyridine or an amine.

POCl3 can also act as a

Lewis acids such as titanium tetrachloride
:

POCl3 + TiCl4 → POCl3·TiCl4

The

Friedel-Crafts reaction
.

POCl3 reacts with hydrogen bromide in the presence of Lewis-acidic catalysts to produce POBr3.

Preparation

Phosphoryl chloride can be prepared by many methods. Phosphoryl chloride was first reported in 1847 by the French chemist

Adolphe Wurtz by reacting phosphorus pentachloride with water.[10]

By oxidation

The commercial method involves oxidation of phosphorus trichloride with oxygen:[11]

2 PCl3 + O2 → 2 POCl3

An alternative method involves the oxidation of phosphorus trichloride with potassium chlorate:[12]

3 PCl3 + KClO3 → 3 POCl3 + KCl

Oxygenations

The reaction of phosphorus pentachloride (PCl5) with phosphorus pentoxide (P4O10).

6 PCl5 + P4O10 → 10 POCl3

The reaction can be simplified by chlorinating a mixture of PCl3 and P4O10, generating the PCl5 in situ. The reaction of phosphorus pentachloride with boric acid or oxalic acid:[12]

3 PCl5 + 2 B(OH)3 → 3 POCl3 + B2O3 + 6 HCl
PCl5 + (COOH)2 → POCl3 + CO + CO2 + 2 HCl

Other methods

Reduction of tricalcium phosphate with carbon in the presence of chlorine gas:[13]

Ca3(PO4)2 + 6 C + 6 Cl2 → 3 CaCl2 + 6 CO + 2 POCl3

The reaction of phosphorus pentoxide with sodium chloride is also reported:[13]

2 P2O5 + 3 NaCl → 3 NaPO3 + POCl3

Uses

Phosphoryl chloride is used on an industrial scale for the manufacture of

2-ethylhexyl diphenyl phosphate) and hydraulic fluids.[11]
POCl3 is also used in the production of organophosphate insecticides.

In the semiconductor industry, POCl3 is used as a safe liquid phosphorus source in diffusion processes. The phosphorus acts as a dopant used to create

n-type
layers on a silicon wafer.

As a reagent

In the laboratory, POCl3 is a reagent in dehydrations. One example involves conversion of formamides to isonitriles (isocyanides);[14] primary amides to nitriles:[15]

RC(O)NH2 + POCl3 → RCN + P(O)OHCl + 2 HCl

In a related reaction, certain aryl-substituted amides can be cyclized using the

Bischler-Napieralski reaction
.

Such reactions are believed to proceed via an imidoyl chloride. In certain cases, the imidoyl chloride is the final product. For example, pyridones and pyrimidones can be converted to chloro- derivatives such as 2-chloropyridines and 2-chloropyrimidines, which are intermediates in the pharmaceutical industry.[16]

In the

Vilsmeier-Haack reaction, POCl3 reacts with amides to produce a "Vilsmeier reagent", a chloro-iminium salt, which subsequently reacts with electron-rich aromatic compounds to produce aromatic aldehydes upon aqueous work-up.[17]

References

  1. ISBN 978-0-85404-182-4
    .
  2. ^ a b c d e NIOSH Pocket Guide to Chemical Hazards. "#0508". National Institute for Occupational Safety and Health (NIOSH).
  3. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link
    )
  4. OCLC 152398514
    .
  5. ^
    doi:10.1107/S0567740871004138
    .
  6. ^ Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann.
  7. ISSN 0002-7863
    .
  8. ^ "Phosphoryl chloride".
  9. doi:10.1002/zaac.19633240102
    .
  10. ^ Wurtz, Adolphe (1847). "Sur l'acide sulfophosphorique et le chloroxyde de phosphore" [On monothiophosphoric acid and phosphoryl chloride]. Annales de Chimie et de Physique. 3rd series (in French). 20: 472–481.; see Chloroxyde de phosphore, pp. 477–481. (Note: Wurtz's empirical formulas are wrong because, like many chemists of his day, he used the wrong atomic mass for oxygen.)Roscoe, Henry Enfield; Schorlemmer, Carl; Cannell, John, eds. (1920). A Treatise on Chemistry. Vol. 1 (5th ed.). London, England: Macmillan and Co. p. 676.
  11. ^
    ISBN 978-3527306732
    ..
  12. ^
    ISBN 0-07-049439-8
    .
  13. ^
    ISBN 978-1-4398-1312-6
    .
  14. doi:10.1039/D0GC02722G
    .
  15. ISBN 978-0-471-60180-7
    .
  16. ^ Elderfield, R. C. (ed.). Heterocyclic Compound. Vol. 6. New York, NY: John Wiley & Sons. p. 265.
  17. doi:10.15227/orgsyn.007.0024
    .

Further reading

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