10294-34-5 Usage
Chemical Description
Boron trichloride is a boron compound used as a reactant.
Description
Boron trichloride, also known as boron trichloride or BCl3, is a colorless, acidic gas with a pungent odor. It is a fuming liquid made by passing dry chlorine over heated boron and is rapidly hydrolyzed by water. Boron trichloride is a Lewis acid, forming stable addition compounds with electron-pair donors such as ammonia and amines. It is corrosive to metals and tissue and is toxic.
Uses
1. Used in the Electronics Industry:
Boron trichloride is used as a source of pure boron (reduction with hydrogen) for the electronics industry.
It is used in the production of optical fibers, as a p-type dopant for thermal diffusion in silicon, and for ion implantation.
2. Used in the Chemical Industry:
Boron trichloride is used as a catalyst in chemical manufacture, promoting reactions that liberate electron-pair donors such as ammonia and amines.
3. Used in the Metal Refining Industry:
It is used in the refining of aluminum, copper, magnesium, and zinc to remove oxides, nitrides, and carbides from the molten metal.
Boron trichloride can remove carbon monoxide, hydrogen, and nitrogen from an aluminum melt, improving its tensile strength and allowing remelting without a major change in the grain structure.
4. Used in the Semiconductor Industry:
Boron trichloride is used in semiconductors for various applications.
5. Used in the Bonding of Iron and Steels:
It is used in the bonding of iron and steels.
6. Used in the Purification of Metal Alloys:
Boron trichloride is used for the purification of metal alloys to remove oxides, nitrides, and carbides.
7. Used in the Preparation of Boranes:
It is used for the preparation of boranes by reaction with metal hydrides.
8. Used in Soldering Fluxes:
Boron trichloride is used in soldering fluxes for many other uses.
Chemical Properties:
Boron trichloride reacts violently with water, and on decomposition and hydrolysis, it yields hydrochloric and boric acid. It has a pungent, highly irritating odor. Occupational exposure to boron and boron compounds can occur in industries that produce special glass, washing powder, soap and cosmetics, leather, cement, etc.
Preparation
Boron trichloride can be prepared by high temperature chlorination of boron trioxide, boric acid, metal borates or other boron compounds. Chlorine, hydrogen chloride, phosgene, silicon tetrachloride, metal chlorides, carbontetrachloride, sulfuryl chloride and phosphorus tri- and pentachlorides are some of the common chlorinating agents. The reaction is carried out at temperatures varying between 400° to 1,400°C, depending on the reactants used. In commercial processes, carbon is generally used to reduce boron oxide during its chlorination. Some of the preparative reactions are outlined below:
B2O3 + 2PCl3 → 2BCl3 + P2O3
2B2O3 + 3CCl4 → 4BCl3 + 3CO2
B2O3 + 3C+ 3Cl2 → 2BCl3 + 3CO
2B(OH)3 +3C + 3Cl2 → 2BCl3 + 3CO + 3H2O
B2O3 + 3C + 6HCl → 2BCl3 + 3CO + 3H2
Na2B4O7 + 7C + 14HCl → 4BCl3 + 2NaCl + 7CO + 7H2
2KBF4 + 3MgCl2 → 2BCl3 + 2KF + 3MgF2
Boron trichloride may also be obtained by high temperature chlorination of boron:
2B + 3Cl2 → 2BCl3
B + 3AgCl → BCl3 + 3Ag
In the laboratory, boron trichloride may be made at ordinary temperatures by the reaction of boron trifluoride with aluminum chloride:
BF3 + AlCl3 → BCl3 + AlF3
Air & Water Reactions
Fumes in air, including moisture in air and soil, to form hydrochloric acid [Merck 11th ed. 1989]. Reacts vigorously with water and forms hydrochloric acid fumes and boric acid.
Reactivity Profile
Boron trichloride vigorously attacks elastomers and packing materials. Contact with Viton, Tygon, Saran and natural and synthetic rubbers is not recommended. Highly corrosive to most metals in the presence of moisture. Reacts energetically with nitrogen dioxide/dinitrogen tetraoxide, aniline, phosphine, triethylsilane, or fat and grease [Mellor 5:132 1946-47]. Reacts exothermically with chemical bases (examples: amines, amides, inorganic hydroxides).
Health Hazard
Boron trichloride is highly irritating and corrosive to the eyes, skin, and mucous membranes of the respiratory and gastrointestinal tracts.may cause severe burns to skin. May result in marked fluid and electrolyte loss and shock. On acute inhalation, boron trichloride result in sneezing, hoarseness, choking, laryngitis, and respiratory tract irritation along with bleeding of the nose and gums, ulceration of the nasal and oral mucosa, bronchitis, pneumonia, dyspnea, chest pain, and pulmonary edema.
Fire Hazard
When heated to decomposition, Boron trichloride emits toxic fumes of chlorides. Boron trichloride will react with water or steam to produce heat, and toxic and corrosive fumes. In hot water, decomposes to hydrochloric acid and boric acid. Fumes and hydrolyzes in moist air to form hydrochloric acid and oily, irritating corrosives. Avoid aniline, hexafluorisopropylidene amino lithium, nitrogen dioxide, phosphine, grease, organic matter, and oxygen. Nitrogen peroxide, phosphine, fat or grease react energetically with Boron trichloride . Oxygen and Boron trichloride react vigorously on sparking. Boron trichloride and aniline react violently in the absence of a coolant or diluent. Stable.
Potential Exposure
Used in refining of aluminum, magnesium,
copper alloys, and in polymerization of styrene.
Manufacture and purification of boron; catalyst in organic
reactions; semiconductors; bonding of iron or steel; purification
of metal alloys to remove oxides, nitrides, and
carbides; chemical intermediate for boron filaments; soldering
flux; electrical resistors; and extinguishing magnesium
fires in heat treating furnaces.
Physiological effects
Boron trichloride is irritating and corrosive to
all living tissue. Exposure of skin tissue to
higher concentrations of boron trichloride or the
liquid can cause hydrochloric acid bums and
skin lesions resulting in tissue destruction and
scarring. Chemical pneumonitis (deep lung inflammation)
and pulmonary edema (abnormal
fluid buildup in the lungs) result trom excessive
exposure to the lower respiratory tract and deep
lung. Bums to the eyes result in lesions and
possible loss of vision. Symptoms of exposure
include tearing of eyes, coughing, labored
breathing, and excessive salivary and sputum
formation.
ACGIH has not established a Threshold Limit
Value (TLV?) for boron trichloride. It is recommended
that compliance with the 5 ppm
ceiling limit (TLV-C) for hydrogen chloride be
used.
storage
Boron trichloride cylinders should be protected from physical damage. The cylinders
should be stored upright and fi rmly secured to prevent falling or being knocked over,
in a cool, dry, well-ventilated area of non-combustible construction away from heavily
traffi cked areas and emergency exits
Purification Methods
Purify it (from chlorine) by passage through two mercury-filled bubblers, then fractionally distil it under a slight vacuum. In a more extensive purification the nitrobenzene addition compound is formed by passage of the gas over nitrobenzene in a vacuum system at 10o. Volatile impurities are removed from the crystalline yellow solid by pumping at -20o, and the BCl3 is recovered by warming the addition compound at 50o. Passage through a trap at -78o removes entrained nitrobenzene, the BCl3 finally condensing in a trap at -112o [Brown & Holmes J Am Chem Soc 78 2173 1956]. Also purify it by condensing it into a trap cooled in acetone/Dry-ice, where it is pumped for 15minutes to remove volatile impurities. It is then warmed, recondensed and again pumped. [Gamble Inorg Synth III 27 1950.] TOXIC.
Incompatibilities
Incompatible with lead, graphiteimpregnated
asbestos, potassium, sodium. Vigorously
attacks elastomers, packing materials, natural and synthetic
rubber; viton, tygon, saran, silastic elastomers.
Avoid aniline, hexafluorisopropylidene amino lithium,
nitrogen dioxide, phosphine, grease, organic matter; and
oxygen. Nitrogen peroxide, phosphine. Fat or grease
react vigorously with boron trichloride. It reacts with
water or steam to produce heat, boric acid, and corrosive
hydrochloric acid fumes. Oxygen and boron trichloride
react vigorously on sparking. Attacks most metals in the
presence of moisture.
Waste Disposal
Return refillable compressed
gas cylinders to supplier. Nonrefillable cylinders should be
disposed of in accordance with local, state, and federal regulations.
Allow remaining gas to vent slowly into atmosphere
in an unconfined area or exhaust hood. Refillabletype
cylinders should be returned to original supplier with
any valve caps and outlet plugs secured and valve protection
caps in place.
Precautions
Boron trichloride vigorously attacks elastomers and packing materials, natural and synthetic rubbers. It also reacts energetically with nitrogen dioxide/dinitrogen tetraoxide, aniline, phosphine, triethylsilane, or fat and grease. It reacts exothermically with chemical
bases such as amines, amides, and inorganic hydroxides. Occupational workers should
use gloves of neoprene or butyl rubber, PVC or polyethylene, safety goggles, or glasses and
face shield, and safety shoes.
GRADES AVAILABLE
Boron trichloride is available for commercial
and industrial purposes with a minimum purity
of99.9 percent by weight.Boron trichloride is also available in ultra
high purity grades for use in the electronics industry.
Gas purity guidelines have been developed
and published by the Semiconductor
Equipment and Materials International and can
be found in the Book ofSEMI Standards.
Check Digit Verification of cas no
The CAS Registry Mumber 10294-34-5 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,0,2,9 and 4 respectively; the second part has 2 digits, 3 and 4 respectively.
Calculate Digit Verification of CAS Registry Number 10294-34:
(7*1)+(6*0)+(5*2)+(4*9)+(3*4)+(2*3)+(1*4)=75
75 % 10 = 5
So 10294-34-5 is a valid CAS Registry Number.
InChI:InChI=1/B.3ClH/h;3*1H/q+3;;;/p-3
10294-34-5Relevant articles and documents
Kotz,Post
, p. 1661,1664 (1970)
Freeman, A. G.,Larkindale, J. P.
, (1969)
Wartik, T.,Moore, R.,Schlesinger, H. I.
, p. 3265 - 3266 (1949)
A study of boron halide-phosphorus halide complexes
Armington,Weiner,Moates
, p. 483 - 484 (1966)
-
Waddington,Klanberg
, (1960)
Urrey, G.,Wartik, T.,Moore, R. E.,Schlesinger, H. I.
, p. 5293 - 5298 (1954)
A Novel Graphite-Like Material of Composition BC3, and Nitrogen-Carbon Graphites
Kouvetakis, John,Kaner, Richard B.,Sattler, Margaret L.,Bartlett, Neil
, p. 1758 - 1759 (1986)
Interaction of benzene with boron trichloride at 800 deg C yields a graphite-like metallic solid of composition BC3, and chlorine-pyridine mixtures at 800 deg C give a nitrogen-carbon also having a graphite-like structure.
Airey, W.,Sheldrick, G. M.
, p. 1827 - 1829 (1970)
[(acridine)BCl2]+: A borenium cation that is a strong boron- and carbon-based lewis acid
Clark, Ewan R.,Ingleson, Michael J.
, p. 6712 - 6717 (2013)
[(acridine)BCl2][AlCl4] was synthesized by halide abstraction from (acridine)BCl3 with AlCl3. The hydride ion affinity of the C9 position in [(acridine)BCl2]+ was calculated to be 14 kcal mol-1 greater than that at boron. [(acridine)BCl2][AlCl4] reacts with 1 equiv of acridine to form the strained boronium cation [(acridine)2BCl 2][AlCl4] and with P(mesityl)3 by photoinduced one-electron transfer to form the 9,9′-biacridane moiety by radical coupling. A stable frustrated Lewis pair (FLP) was formed on combining [(acridine)BCl2][AlCl4] and 2,4,6-tri-tert-butylpyridine (TBP), which heterolytically activated H2 at 100 C. The ultimate location of the hydride from H2 activation was the C9 position of acridine and not boron. Carbon Lewis acid based reactivity also occurred when thieno[3,2-b]thiophene was added to the [(acridine)BCl2][AlCl 4]/TBP FLP or to [(acridine)2BCl2][AlCl 4], with arylation of acridine at C9 observed for both.
-
Lynds,Stern
, p. 5006 (1959)
-
Dobson et al.
, p. 452 (1968)
Murib, J. H.,Horvitz, D.,Bonecutter, C. A.
, p. 273 - 280 (1965)
Lynds, L.,Bass, C. D.
, p. 1590 - 1593 (1964)
Wartik, T.,Apple, E. F.
, p. 6155 - 6158 (1958)
Dichloroboronation of aromatic hydrocarbons. Mechanistic aspects
Muetterties,Tebbe
, p. 2663 - 2664 (1968)
-
Thermodynamic properties of dichloroborane
Lynds, Lahmer,Bass, C. David
, p. 1147 - 1149 (1964)
The disproportionation reaction for HBCl2, 6HBCl2 ? 4BCl3 + B2H6, was followed spectrophotometrically in the infrared region and an equilibrium constant (Kp (298° K.) = 532 ± 15 atm.-1
A self-contained regeneration scheme for spent ammonia borane based on the catalytic hydrodechlorination of BCl3
Reller, Christian,Mertens, Florian O.R.L.
, p. 11731 - 11735 (2013/01/15)
Recycling: A self-contained procedure for the recycling of BNH-waste, based on the three major steps: polymer break-up, amine supported catalytic hydrodehalogenation of boron halogens, and the base exchange in borane amine adducts, is developed (see picture). Beyond the original task of recycling spent ammonia borane, the process provides a new means to produce borohydride species efficiently, by the direct use of molecular hydrogen. Copyright
Silicon-boron-carbon-nitrogen ceramics and precursor compounds, methods for the production and use thereof
-
Page 6, (2010/02/05)
The present invention relates to novel processes for preparing borylsilylamines, novel amines, novel borosilazane compounds, novel oligoborosilazane or polyborosilazane compounds which have the structural feature Si—N—B, ceramic material and methods of producing and using them.