10025-87-3 Usage
Chemical Description
Different sources of media describe the Chemical Description of 10025-87-3 differently. You can refer to the following data:
1. Phosphorus oxychloride is used in the synthesis of N,N,N′,N′-tetramethyl-2-(N-phthaloyl)vinamidinium perchlorate.
2. Phosphorus oxychloride is a highly toxic and corrosive liquid that is used as a reagent in organic synthesis, but is restricted in many countries due to its environmental impact and health hazards.
3. Phosphorus oxychloride is a colorless liquid used as a chlorinating and dehydrating agent.
Chemical Characteristics
Phosphorus oxychloride (chemical formula: POCl3), is a type of industrial raw material. It is a colorless and transparent liquid, and it has an unpleasant irritating odor. It will smoke intensely in humid air. Its relative density is 1.68, melting point is 1.25℃, boiling point is 105.1℃. It breaks down into phosphoric acid and hydrogen chloride in water and ethanol. When suddenly combined with a large amount of water, an intense reaction may occur. POCl3 reacts with water and alcohol to create phosphoric acid or phosphate. If alcohol replaces the water in the reaction, the end product will be trialkyl phosphate. This type of reaction often occurs in pyridine or ammonia, as it absorbs the produced HCl to stimulate the reaction. When catalyzed by a Lewis acid such as manganese chloride, POCl3 and a large amount of phenol (ArOH) heats to produce triaryl phosphate, such as in the reaction below: 3 C6H5OH + O=PCl3 → O=P(OC6H5)3 + 3 HCl. Phosphorus oxychloride is a Lewis base, and it produces compounds with many Lewis acids, such as in its reaction with titanium tetrachloride: Cl3P5+O? + TiCl4 → Cl3P5+O-?TiCl4. Its adduct with aluminum chloride (POCl3?AlCl3) is very stable, and thus POCl3 is used to remove the AlCl3 in the end products of Friedel-Crafts reactions. In the presence of AlCl3, POCl3 reacts with hydrogen bromide to create POBr3.
Usage
Phosphorus oxychloride can be used as a semiconductor dopant, and it is a raw material for light-conducting fibers. It is widely used in pesticides, pharmaceuticals, dyes, phosphates and flame retardant production. It is a raw material for producing organic phosphorus herbicide and chlordimeform, and it is a plasticizer in plastic production. Phosphorus oxychloride is also used in the chlorination of long-acting sulfa drugs, is an intermediate in dye production and a catalyst in organic synthesis of chlorinating agents, and it is an extracting agent in uranium mining. It is also used in producing pharmaceuticals.
Toxicology
Toxicity is similar to phosphorus trichloride, phosphorus pentachloride and phosgene. Large mice, oral, LD50: 380 mg/kg; inhaled, LC50: 32 ppm/4H. Acute poisoning in small mice results in restlessness, upper respiratory tract and conjunctival irritation, depression, convulsions, unsteady walking, lying on the side, and eventually, death. For large mice, in addition to the symptoms above, also exhibited tearing, cornea clouding, and pulmonary edema. Subacute and chronic toxicity: large mice, inhaled for 60 days at a concentration of 33.5mg/m3, exhibited slowed weight gain, skin ulcers, decreases survival rates in lung macrophages, no liver and kidney functions, and organ characteristic changes.
This product has a strong oxidizing and liposoluble effects; besides burning the digestive tract, it can also cause acute necrosis and autolysis in the liver when absorbed through the digestive tracts. Additionally, besides burning the skin, when completely absorbed through the skin, 3% can cause death in animals. When phosphorus oxychloride is inhaled and comes in contact with the moist respiratory tract mucosa, it will break down into phosphoric acid and hydrogen chloride, and it will irritate and corrode the mucosa. When humans contact at a concentration of 70mg/m3, they will usually exhibit symptoms after a 2-6h latency period, including respiratory tract mucosa irritation and eye pain. Serious cases include a choking sensation, cyanosis, pulmonary edema, heart failure, anemia, liver damage, and proteinuria. When the temperature in the car is high and the humidity is relatively low, there is a high risk of inhalation and poisoning.
The highest permitted concentration is 0.05 mg/m3. Handlers should wear protective equipment, and production equipment must be tightly sealed. Processors can also wear filtering gas masks. Take care to protect skin and eyes.
After inhalation, emergency response and treatment is similar to chlorine, hydrogen chloride and other irritating gases. If contacted with skin, first use paper or cotton to absorb the liquid, then rinse with water for at least 15 minutes; if directly rinsed with water, it may produce phosphoric acid and continue to burn the skin. Treat injury as an acid burn.
Danger regulations GB8.1 type 81040. Iron regulation: Level one inorganic acidic corrosive product, 91022. UN No. 1810. IMDG CODE page 8197, type 8.
Warnings and Precautions
Phosphorus oxychloride is often used in industrial production; there are many details to take note of when using phosphorus oxychloride to prevent safety concerns and accidents:
1. Phosphorus oxychloride preparation: As many factories use water jet vacuums to store phosphorus oxychloride, great attention must be paid to the switch order to prevent accidents. The buffer vacuum tank must be frequently inspected to prevent the water from being sucked into storage containers and causing accidents.
2. Phosphorus oxychloride with hydrogen chloride: take care to not add an excess of phosphorus chloride. If there is an excess, slowly drop in water to hydrolyze the phosphorus chloride, and then remove the produced phosphoric acid.
3. Slowly place any materials containing phosphorus oxychloride into a hydrolysis kettle containing cold water and mix continuously. Avoid adding water to the material.
4. Whenever using systems containing phosphorus oxychloride, take care to measure the water content in all the components to prevent an excess of water from causing an explosion.
5. Frequently inspect reactors for cracks and imperfections to prevent water from leaking in and coming in contact with the phosphorus oxychloride.
6. When adding phosphorus oxychloride to a reactor, remain observant and stop adding material immediately if there are any abnormal occurrences. Only continue adding material after investigating the cause of these occurrences.
7. Phosphorus oxychloride reacts slowly with water when at a lower temperature. Thus, drop in slowly to prevent sudden intense reactions.
8. Phosphorus oxychloride can be used in combination with dichloroethane and toluene solutions, but not with alcohol and ammonia solutions.
Hazards & Safety Information
Category Corrosive items
Toxicity grading highly toxic
Acute Toxicity Oral-Rat LD50: 380 mg/kg
Flammability and Hazardous characteristics being explosive upon coming across water with release of toxic chloride, phosphorus oxide gas
Storage and transportation characteristics Ventilated, low temperature and dry; and store it separately from alkali
Fire Extinguishing agent dry sand, dry stone powder; prohibit the usage of water
Occupational Standard TLV-TWA 0.1 PPM (0.6 mg/m3); STEL 0.5 PPM (3 mg/m3)
Chemical Properties
Phosphorus oxychloride is a clear, colorless to yellow, fuming, oily liquid with a pungent and musty odor.
Physical properties
Colorless fuming liquid with a pungent odor; density 1.645 g/mL; freezes at 1°C; boils at 105.5°C; reacts with water and ethanol.
Uses
Different sources of media describe the Uses of 10025-87-3 differently. You can refer to the following data:
1. In the manufacture of pesticides, pharmaceuticals, plasticizers, gasoline
additives, and hydraulic fluid.
2. Phosphorus oxychloride is used to produce hydraulic fluids, plasticizers, and fireretarding agents; as a chlorinating agent; and as a solvent in cryoscopy.
3. Phosphorus oxychloride is an important intermediate in the production of triarylphosphate esters (e.g., triphenyl phosphate and tricresyl phosphate), which have been used as flame retardants and plasticizers for PVC. It is acutely toxic to the eyes, throat, and respiratory tract. Phosphorus oxychloride is also used in nuclear reprocessing, as chlorinating agent, especially to replace oxygen in organic compounds, as solvent in cryoscopy and the semiconductor industry.
Definition
A white crystalline
solid. It is a monobasic acid forming the
anion H2PO2
– in water. The sodium salt,
and hence the acid, can be prepared by
heating yellow phosphorus with sodium
hydroxide solution. The free acid and its
salts are powerful reducing agents.
Preparation
Phosphorus oxychloride can be prepared from phosphorus trichloride or phosphorus pentachloride. It can be obtained from phosphorus trichloride by cautious addition of potassium chlorate:3PCl3 + KClO3 → 3POCl3 + KCl The oxychloride also is obtained by the action of boric acid or oxalic acid with phosphorus pentachloride: 3PCl5 + 2B(OH）3 → 3POCl3 + B2O3 + 6HCl PCl5 + (COOH）2 → POCl3 + CO + CO2 + 2HCl Phosphorus oxychloride also is made by heating calcium phosphate in a current of chlorine and carbon monoxide at 350°C: 2Ca3(PO4）2 + 9Cl2 + 6CO → 4POCl3 + 6CaCO3 Alternatively, heating a mixture of calcium phosphate and carbon in a current of chlorine at 750°C yields the oxychloride.
General Description
A colorless fuming liquid with a pungent odor. Density 14.0 lb / gal. Very toxic by inhalation and corrosive to metals and tissue. Used in gasoline additives and hydraulic fluids.
Reactivity Profile
Phosphorus oxychloride is water reactive. Incompatible with strong oxidizing agents, alcohols, bases (including amines). May react vigorously or explosively if mixed with diisopropyl ether or other ethers in the presence of trace amounts of metal salts [J. Haz. Mat., 1981, 4, 291]. Combining the chloride with zinc dust caused immediate ignition, due to the formation of phosphine gas which ignites, [Mellor, 1940, Vol. 8, 1025]. An exotherm starting with the mixing of Phosphorus oxychloride with acetone (a ketone) lead to an explosion, may behave similarly with other ketones, [Organic Process Research and Development, Vol.4, No. 6,200, "Phosphorus oxychloride and Acetone: An Incompatibility Investigation Using ARC."]
Hazard
The compound is highly irritating to skin, eyes and mucous membranes. Inhaling its vapors can cause pulmonary edema.
Health Hazard
Inhalation of vapors of phosphorus oxychloride produced acute and chronic toxicity in test subjects. In humans, exposure to its vapors may cause headache, dizziness, weakness, nausea, vomiting, coughing, chest pain, bronchitis, and pulmonary edema. Most of these symptoms are manifested from chronic exposure to its vapors.LC50 value, inhalation (rats): 48 ppm (301 mg/m3)/4 hVapors of this compound are an irritant to the eyes and mucous membranes. The liquidis corrosive and can cause skin burns. An oral LD50 value for rats is documented to be 380 mg/kg (NIOSH 1986)..
Fire Hazard
Poisonous, corrosive, and irritating gases are generated when Phosphorus oxychloride is heated or is in contact with water. Phosphorus oxychloride may ignite other combustible materials (wood, paper, oil, etc.). Phosphorus oxychloride reacts violently with water. When heated to decomposition, Phosphorus oxychloride emits toxic fumes of chlorides and oxides of phosphorus; Phosphorus oxychloride will react with water or steam to produce heat and toxic and corrosive fumes. Incompatible with carbon disulfide; N,N-dimethylformamide; 2,5-dimethylpyrrole; 2,6-dimethyl- pyridine N-oxide; dimethylsulfoxide; Ferrocene-1,1-dicarboxylic acid; water; and zinc. Do not store with combustible materials, particularly fibrous organic materials, or with electrical or other equipment that can be corroded. Reacts violently with moisture.
Safety Profile
Poison by inhalation and ingestion. A corrosive eye, skin, and mucous membrane irritant. Potentially explosive reaction with water evolves hydrogen chloride and phosphine, which then ignites. Explosive reaction with 2,6dimethylpyridine N-oxide, dimethyl sulfoxide, ferrocene1 ,l'-dicarboxylic acid, pyridne N-oxide (above bO'C), sodmm + heat. Violent reaction or ignition with BI3, carbon disulfide, 2,5-dimethyl pyrrole + dimethyl formamide, organic matter, zinc powder. Reacts with water or steam to produce heat and toxic and corrosive fumes. Incompatible with carbon disulfide, N,Ndimethyl-formamide, 2,5-dunethylpyrrole, 2,6-dimethylpyridine N-oxide, dimethylsulfoxide, ferrocene1 ,I-dicarboxylic acid, water, zinc. When heated to decomposition it emits highly toxic fumes of Cland POx
Potential Exposure
Phosphorus oxychloride is used in the manufacture of pesticides, pharmaceuticals, plasticizers, gasoline additives; and hydraulic fluids.
Shipping
UN1810 Phosphorus oxychloride, Hazard class: 6.1; Labels: 6.1-Poisonous materials, 8-Corrosive material, Hazard Zone B.
Purification Methods
Distil the liquid under reduced pressure to separate it from the bulk of the HCl and the phosphoric acid (from hydrolysis); the middle fraction is re-distilled into ampoules containing a little purified mercury. These ampoules are sealed and stored in the dark for 4-6weeks with occasional shaking to facilitate reaction of any free chloride with the mercury. The POCl3 is then again fractionally distilled and stored in sealed ampoules in the dark until required [Herber J Am Chem Soc 82 792 1960]. Lewis and Sowerby [J Chem Soc 336 1957] refluxed their distilled POCl3 with Na wire for 4hours, then removed the Na and again distilled. Use Na only with almost pure POCl3 to avoid explosions. HARMFUL VAPOURS; work in an efficient fume cupboard.
Incompatibilities
A powerful oxidizer. Violently decomposes in water, forming heat and hydrochloric and phosphoric acids. Violent reaction with alcohols, phenols, amines, reducing agents; combustible materials; carbon disulfide; dimethylformamide, and many other many materials. Rapid corrosion of metals, except nickel and lead.
Waste Disposal
Pour onto sodium bicarbonate. Spray with aqueous ammonia and add crushed ice. Neutralize and pour into drain with running water. In accordance with 40CFR165, follow recommendations for the disposal of pesticides and pesticide containers. Must be disposed properly by following package label directions or by contacting your local or federal environmental control agency, or by contacting your regional EPA office.
Check Digit Verification of cas no
The CAS Registry Mumber 10025-87-3 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,0,0,2 and 5 respectively; the second part has 2 digits, 8 and 7 respectively.
Calculate Digit Verification of CAS Registry Number 10025-87:
(7*1)+(6*0)+(5*0)+(4*2)+(3*5)+(2*8)+(1*7)=53
53 % 10 = 3
So 10025-87-3 is a valid CAS Registry Number.
InChI:InChI:1S/Cl3OP/c1-5(2,3)4
10025-87-3Relevant articles and documents
On the Reaction of Chlorine Nitrate ClONO2 with PCl3, AsCl3, SbCl3 and AsCl4+AsF6-
Minkwitz, Rolf,Hertel, Thomas,Meier, Ralf
, p. 1064 - 1066 (1996)
The reaction of ClONO2 with PCl3 yields POCl3 and NO2+NO3-. With AsCl3 chlorine nitrate forms a compound of the analytical composition AsCl2(NO3)3 , in contrast to SbCl3, which does not react with ClONO2. The reaction of ClONO2 with AsCl4+AsF6- was reported to yield As(ONO2)4+AsF6-. We found no reaction below 273 K. Reaction at 293 K yields NO2+AsF6- as solid product. SbCl5 does react, but the reaction yields no reproduceable products.
Sheldon, J. C.,Tyree, S. Y.
, p. 4775 - 4778 (1958)
OXIDATION OF PHOSPHORUS(III) HALIDES BY RED PHOTOLYSIS OF OZONE COMPLEXES IN SOLID ARGON
Moores, Brian W.,Andrews, Lester
, p. 1902 - 1907 (1989)
PCl3-O3 and PBr3-O3 complexes in solid argon photolyze to give phosphoryl halides with red visible radiation that has no effect on isolated ozone.These observations and similar results for PH3-O3 and P4-O3 complexes show that the complex markedly increases the cross section for red photodissociation of ozone and suggest that this increase is due to the complex effectively lowering the barrier to dissociation by providing a strongly exothermic dissociation-recombination process.
Tarbutton, G.,Egan, E. P.,Frary, S. G.
, p. 1782 - 1789 (1941)
Smith, E. F.,Harris, H. B.
, p. 654 - 656 (1895)
Pennington, M. E.
, p. 38 - 67 (1896)
CRYSTAL STRUCTURES OF A CESIUM IRON(III) PHOSPHATE, Cs3Fe4(PO4)5, AND A CESIUM IRON(III) OXYPHOSPHATE, Cs7Fe7(PO4)8O2.
Andrews-Allen,Robinson
, p. 88 - 97 (1988)
The reaction of FePO//4 with molten CsCl produces Cs//3Fe//4(PO//4)//5, Cs//7Fe//7(PO//4)//8O//2, or Fe//2O//3, depending on the length of the reaction. The crystal structure of Cs//3Fe//4(PO//4)//5 consists of an interlocking network of corner-sharing phosphate tetrahedra and iron trigonal bipyramids with cesium atoms situated in tunnels. The Cs//7Fe//7(PO//4)//8O//2 structure can be described as a three-dimensional array containing linked phosphate tetrahedra and iron octahedra, trigonal bipyramids, and square pyramids. In addition to the phosphate oxygen atoms, three of the iron polyhedra share a common oxide ion. The cesium atoms are located in tunnels.
Reaction kinetics of PO2Cl-, PO2Cl 2-, POCl2- and POCl3 - with O2 and O3 from 163 to 400 K
Fernandez, Abel I.,Midey, Anthony J.,Miller, Thomas M.,Viggiano
, p. 9120 - 9125 (2004)
Rate constants and product ion branching fractions for the gas-phase reactions of O2 and O3 with the anions (a) PO 2Cl-, (b) POCl3-, (c) POCl 2-, and (d) PO2Cl2- were measured in a selected-ion flow tube (SIFT). The kinetics were measured at temperatures of 163-400 K and a He pressure of 0.4 Torr. Only PO 2Cl- reacts with O2 to a measurable extent, having k(163-400 K) = 1.1 × 10-8(T/K)-1.0 cm 3 molecule-1 s-1, while O3 reacts with all of the anions except PO2Cl2-. The fitted rate constant expressions for the O3 reaction with anions a-c are as follows: ka(163-400 K) = 3.5 × 10-6(T/K) -1.6, kb(163-400 K) = 4.0 × 10 -7(T/K)-1.2, and kc(163-400 K) = 3.7 × 10-7(T/K)-1.4 cm3 molecule-1 s -1. Calculations were performed at the G3 level of theory to obtain optimized geometries, energies, and electron affinities (EAs) of the reactant and product species, as well as to determine the reaction thermochemistry to help understand the experimental results. The POxCly - anions that have lower electron binding energies (eBE) and higher spin multiplicities are more reactive. The doublets are more labile than the singlets. How the extra electron density is distributed in the anion does not predict the observed reactivity of the ion. The reactions of PO 2Cl- with O2 and O3 yield predominantly PO3- and PO4-. The reaction of POCl2- with O3 yields mostly Cl- and PO2Cl2-, while the POCl 3- reaction with O3 yields mostly O 3- and PO2Cl2-.
Reaction of P(III) chlorides with aldehydes: III. Reaction of primary intermediates with oxidants and chlorinating agents
Gazizov,Khairullin,Karimova
, (2014)
Primary intermediates of P(III) chlorides reaction with aldehydes have been converted into the corresponding phosphates by treating with oxidants: dimethylsulfoxide and tert-butyl hypochlorite. In reactions of the intermediates with chlorinating agents (P
Schlundt, H.
, p. 503 - 526 (1900)
Cross-linked poly(4-vinylpyridine-N-oxide) as a polymer-supported oxygen atom transfer reagent
Bauer, Anna M.,Ramey, Erin E.,Oberle, Kjersti G.,Fata, Gretchen A.,Hutchison, Chloe D.,Turlington, Christopher R.
, (2019)
Oxygen atom transfer (OAT) reagents are common in biological and industrial oxidation reactions. While many heterogeneous catalysts have been utilized in OAT reactions, heterogeneous OAT reagents have not been explored. Here, cross-linked poly(4-vinylpyridine-N-oxide), called x-PVP-N-oxide, was tested as a heterogeneous OAT reagent and its oxidation chemistry compared to its molecular counterpart, pyridine-N-oxide. The insoluble oxidant x-PVP-N-oxide demonstrated comparable reactivity to pyridine-N-oxide in direct oxidation reactions of phosphines and phosphites in acetonitrile, but x-PVP-N-oxide did not react in other solvents. The polymer backbone of x-PVP-N-oxide, however, allowed for easy filtering and recycling in sequential oxidation reactions. In addition, x-PVP-N-oxide was tested as the stoichiometric oxidant in a copper-catalyzed OAT reaction to α-diazo-benzeneacetic acid methyl ester. The heterogeneous oxidant was much less reactive than pyridine-N-oxide, indicating that interaction with the metal catalyst was challenging. These results demonstrated a proof-of-concept that recyclable, polymer-supported OAT reagents could be a viable OAT reagents in direct oxidation reactions without metal catalysts.
-
Bannard et al.
, p. 976,981 (1953)
-
Batey, H. H.,Sisler, H. H.
, p. 3408 - 3410 (1952)
Haszeldine, R. N.,Iserson, H.
, p. 1361 - 1362 (1957)
ORGANIC ELECTROLUMINESCENT ELEMENT AND MANUFACTURING METHOD THEREOF, ORGANIC COMPOUND CONTAINING PHOSPHORUS AND MANUFACTURING METHOD THEREOF
-
, (2008/06/13)
An organic electroluminescent element comprising an anode, a cathode and a plurality of organic compound layers sandwiched between the anode and cathode, the organic compound layers including: a hole-transporting layer made of an organic compound insoluble in alcohols; and an electron-transporting layer formed on the hole-transporting layer by a wet method, the electron-transporting layer being made of a phosphorus-containing organic compound soluble in the alcohols.
