7637-07-2 Usage
Description
Boron trifluoride is the inorganic compound with the formula BF3. It is a highly toxic, colorless and nonflammable gas with a penetrating and pungent odor. It dissolves quickly in water and any organic compounds containing nitrogen or oxygen. It can be slowly hydrolyzed by cold water to give off hydrofluoric acid, and can also hydrolyzes to form white dense fumes in moist air. Its vapors are heavier than air. Inhaling the gas will irritate the respiratory system and burns can result if the gas touches the skin in high concentrations.
boron trifluoride lewis structure
Boron trifluoride is most importantly used as a reagent, typically as a Lewis acid, to catalyze such diverse operations as isomerization, alkylation, polymerization, esterfication, condensation, cyclization, hydration dehydration, sulfonation, desulfurization nitration, halogenation oxidation and acylation. Besides, it can also be used as a versatile building block for other boron compounds.
Chemical Properties
Different sources of media describe the Chemical Properties of 7637-07-2 differently. You can refer to the following data:
1. Boron trifluoride, BF3, is a colorless gas with a vapor density of 2.34, which is heavier than air. It is water-soluble and does not support combustion. It is also water-reactive, toxic by inhalation, and corrosive to skin and tissue. The TLV is 1 ppm, and the IDLH is 100 ppm in air. The boiling point is ?148°F (64°C). The four-digit UN identification number is 1008. The NFPA 704 designation is health 4, flammability 0, and reactivity 1. The primary uses are as a catalyst in organic synthesis, in instruments for measuring neutron intensity, in soldering fluxes, and in gas brazing.
2. Boron trifluoride is a nonflammable, colorless gas with an acrid suffocating odor. It forms thick acidic fumes in moist air. Dry boron trifluoride is used with mild steel, copper, copper-zinc and copper-silicon alloys, and nickel. Moist gas is corrosive to most metallic materials and some plastics. Therefore, Kel-F and Teflon are the preferred gasketing materials. Mercury containing manometers should not be used because boron trifluoride is soluble in mercury. It decomposes in hot water yielding hydrogen fluoride, Shipped as a nonliquefied compressed gas.
References
1. https://en.wikipedia.org/wiki/Boron_trifluoride
2. https://cameochemicals.noaa.gov/chemical/255
3. http://www.c-f-c.com/specgas_products/boron-trifluoride.htm
4.https://www.praxairdirect.com/Specialty-Gas-Information-Center/Pure-Gas-Specifications/Boron-Trifluoride.html
Physical properties
Colorless gas; pungent suffocating odor; density 2.975 g/L; fumes in moist air; liquefies at -101°C; solidifies at -126.8°; vapor pressure at -128°C is 57.8 torr; critical temperature -12.2°C; critical pressure 49.15 atm; critical volume 115 cm3/mol; soluble in water with partial hydrolysis; solubility in water at 0°C 332 g/100g; also soluble in benzene, toluene, hexane, chloroform and methylene chloride; soluble in anhydrous concentrated sulfuric acid.
Uses
Boron trifluoride is used as a catalyst for polymerizations, alkylations, and condensation reactions; To protect molten magnesium and its alloys from oxidation; as a gas flux for internal soldering or brazing; in ionization chambers for the detection of weak neutrons; and as a source of B10 isotope. ?By far the largest application of boron trifluoride is in catalysis with and without promoting agents.
Preparation
Boron trifluoride is prepared by treating borax with hydrofluoric acid; or boric acid with ammonium bifluoride. The complex intermediate product is then treated with cold fuming sulfuric acid.
General Description
Boron trifluoride is a colorless gas with a pungent odor. Boron trifluoride is toxic by inhalation. Boron trifluoride is soluble in water and slowly hydrolyzed by cold water to give off hydrofluoric acid, a corrosive material. Its vapors are heavier than air. Prolonged exposure of the containers to fire or heat may result in their violent rupturing and rocketing.
Air & Water Reactions
Fumes in air. Soluble in water and slowly hydrolyzed by cold water to give hydrofluoric acid. Reacts more rapidly with hot water.
Reactivity Profile
Boron trifluoride is a colorless, strongly irritating, toxic gas. Upon contact with water, steam or when heated to decomposition, Boron trifluoride will produce toxic fluoride fumes. Incompatible with alkyl nitrates, calcium oxide. Reaction with alkali metals or alkaline earth metals (except magnesium) will cause incandescence [Bretherick, 5th ed., 1995, p. 65].
Hazard
Toxic by inhalation, corrosive to skin and
tissue. Lower respiratory tract irritant, and pneu-
monitis.
Health Hazard
Boron trifluoride (and organic complexes such as BF3-etherate) are extremel corrosive substances that are destructive to all tissues of the body. Upon contact with moisture in the skin and other tissues, these compounds react to form hydrofluoric acid and fluoroboric acid, which cause severe burns. Boron trifluoride gas is extremely irritating to the skin, eyes, and mucous membranes. Inhalation of boron trifluoride can cause severe irritation and burning of the respiratory tract, difficult breathing, and possibly respiratory failure and death. Exposure of the eyes to BF can cause severe burns and blindness. This compound is not considered to have adequate warning properties. Boron trifluoride has not been found to be carcinogenic or to show reproductive or developmental toxicity in humans. Chronic exposure to boron trifluoride gas can cause respiratory irritation and damage.
Fire Hazard
When heated to decomposition or upon contact with water or steam, Boron trifluoride will produce toxic and corrosive fumes of fluorine containing compounds. Decomposes upon heating or on contact with moist air, forming toxic and corrosive fumes of boric acid and hydrofluoric acid. Reacts with alkalis and fumes in moist air, producing particulates which reduce visibility. Reacts with alkali metals, alkaline earth metals (except magnesium), alkyl nitrates, and calcium oxide. Boron trifluoride hydrolyzes in moist air to form boric acid, hydrofluoric acid, and fluoboric acid.
Flammability and Explosibility
Boron trifluoride gas is noncombustible. Water should not be used to extinguish any
fire in which boron trifluoride is present. Dry chemical powder should be used for
fires involving organic complexes of boron trifluoride.
Materials Uses
Dry boron trifluoride does not react with the
common metals of construction, but If moisture
is present the acidic hydrates formed (BF3·H2O
and BF3·2H2O) can corrode many common metals
rapidly. Consequently, lines, pressure regulators,
and valves in boron trifluoride service
must be well protected from the entrance of
moist air between periods of use. Cast iron must
not be used because active fluorides attack its
structure. If steel piping is used for boron
trifluoride, forged-steel fittings must be used
instead of cast-iron fittings. Stainless steel, Monel,
nickel, and Hastelloy C are good materials
of construction.
Among materials suitable for gaskets are
Teflon, Kel F, and other appropriate fluorocarbon
or chlorofluorocarbon plastics. Most plastics
become embrittled in boron trifluoride
service. The use of polyvinyl chloride should be
avoided.
Physiological effects
Boron trifluoride irritates the nose, mucous
membranes, and other parts of the respiratory
system. Concentrations as low as I ppm in air
can be detected by the sense of smell and are
readily visible.
ACGIH recommends a Threshold Limit
Value-Ceiling (TLV-C) of 1 ppm (2.8 mg/m3)
for boron trifluoride. The TLV-C is the concentration
that should not be exceeded during
any part of the working exposure.
storage
All work with boron trifluoride should be conducted in a
fume hood to prevent exposure by inhalation, and splash goggles and impermeable gloves
should be worn to prevent eye and skin contact. Cylinders of boron trifluoride should be
stored in locations appropriate for compressed gas storage and separated from alkali metals,
alkaline earth metals, and other incompatible substances. Solutions of boron trifluoride should
be stored in tightly sealed containers under an inert atmosphere in secondary containers.
Purification Methods
The usual impurities-bromine, BF5, HF and non-volatile fluorides-are readily separated by distillation. Brown and Johannesen [J Am Chem Soc 72 2934 1950] passed BF3 into benzonitrile at 0o until the latter was saturated. Evacuation to 10-5mm then removed all traces of SiF4 and other gaseous impurities. [A small amount of the BF3-benzonitrile addition compound sublimes and is collected in a U-tube cooled to -80o]. The pressure is raised to 20mm by admitting dry air, and the flask containing the BF3 addition compound is warmed with hot water. The BF3 that evolves is passed through a -80o trap (to condense any benzonitrile) into a tube cooled in liquid air. The addition compound with anisole can also be used. BF3 can be dried by passing it through H2SO4 saturated with boric oxide. It fumes in moist air. [It is commercially available as a 1.3M solution in MeOH or PrOH.] [Booth & Wilson Inorg Synth I 21 1939, Kwasnik in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 219-222 1963.] TOXIC.
Precautions
Exposures to boron trifl uoride in occupational work areas cause irritating effects,
painful burns, lesions, and loss of vision. Workers with potential exposure to boron
trifl uoride should not wear contact lenses. Prompt medical attention is mandatory
in all cases of overexposure to boron trifl uoride and the rescue personnel should be
equipped with proper protectives. Occupational workers should handle/use boron trifl uoride only in well-ventilated areas. The valve protection caps must remain in place.
Workers should not drag, slide, or roll the cylinders, and use a suitable hand truck for
cylinder movement. Compressed gas cylinders shall not be refi lled without the express
written permission of the owner. Boron trifl uoride is listed as an extremely hazardous
substance (EHS).
The cylinder should not be heated by any means to increase the discharge rate of the
product from the cylinder. The cylinder of boron trifl uoride should be kept stored in a cool,
dry, well-ventilated area of non-combustible construction away from heavily traffi cked
areas and emergency exits
GRADES AVAILABLE
Boron trifluoride is available for commercial
and industrial use in technical grades having
much the same component proportions from one
producer to another.Boron trifluoride is also available in
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, Gases
Volume.
Check Digit Verification of cas no
The CAS Registry Mumber 7637-07-2 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,6,3 and 7 respectively; the second part has 2 digits, 0 and 7 respectively.
Calculate Digit Verification of CAS Registry Number 7637-07:
(6*7)+(5*6)+(4*3)+(3*7)+(2*0)+(1*7)=112
112 % 10 = 2
So 7637-07-2 is a valid CAS Registry Number.
InChI:InChI=1S/BF3/c2-1(3)4
7637-07-2Relevant articles and documents
Synthesis, thermal investigations and kinetic data of Zn(BF 4)2?6H2O
Nikolova, Deyanka,Georgiev
, p. 319 - 321 (2009)
The thermal dehydration and decomposition of Zn(BF4) 2?6H2O have been studied by TG, DTA and DSC analyses. It is found that the dehydration occurs in two steps. Following the experimental results a thermal decomposition sc
The chloryl cation, ClO2+
Christe, Karl O.,Schack, Carl J.,Pilipovich, Donald,Sawodny, Wolfgang
, p. 2489 - 2494 (1969)
The 1:1 adducts ClO2F·AsF5 and ClO2F·BF3 have been investigated. Whereas ClO2F·AsF5 is stable at ambient temperature, the ClO2F·BF3 adduct shows a dissociation pressure of 225 mm at 25°. A pressure-temperature curve gives a heat of reaction of 24.0 kcal mol-1, for the dissociation process: ClO2F·BF3(s) = ClO2F(g) + BF3(g). The X-ray powder patterns of ClO2F·AsF5 and ClF3·AsF5 were recorded and indexed. Infrared and Raman measurements show that ClO2F·AsF5 and ClO2F·BF3 have the ionic structures ClO2+AsF6- and ClO2+BF4-, respectively, in the solid state. All fundamental vibrations were observed and a valence force field was calculated for ClO2+.
Booth, H. S.,Wilson, K. S.
, p. 2273 - 2280 (1935)
Preparation and properties of perfluoroammonium tetrafluoroborate, NF4+BF4-, and possible synthesis of nitrogen pentafluoride
Goetschel,Campanile,Curtis,Loos,Wagner,Wilson
, p. 1696 - 1701 (1972)
A new crystalline compound, NF4+BF4-, has been prepared by exposing the heterogeneous ternary system NF3-BF3-F2 to 3-MeV bremsstrahlung at 77°K. The G value for the reaction (molecules isolated per 100 eV absorbed) is about unity. The compound is stable at room temperature in dry air; it decomposes above 250° to the reactants. It reacts rapidly with moisture and with organic substances. The indicated ionic structure is confirmed by infrared and Raman spectroscopy. The X-ray powder pattern can be indexed on the basis of a tetragonal unit cell with a = 7.01 and c = 5.22 A?. Irradiation of mixtures of nitrogen trifluoride and excess fluorine at 77°K has led to isolation in low yields of a white solid. It decomposes below 143°K to liberate nitrogen trifluoride and reacts with boron trifluoride at low temperature to form NF4BF4. Its most likely identity is perfluoroammonium fluoride.
Mechanism of the benzenediazonium tetrafluoroborate thermolysis in the solid state
Koval'chuk, Eugen P.,Reshetnyak, Oleksandr V.,Kozlovs'ka, Zoryana Ye.,B?azejowski, Jerzy,Gladyshevs'kyj, Roman Ye.,Obushak, Mykola D.
, p. 1 - 5 (2006)
The thermolysis of benzenediazonium tetrafluoroborate was studied by thermogravimetry in dynamic mode. The decomposition of [ArN{triple bond, long}N]+BF4- in the solid state with the formation of C6H5F, BF3, C6H6, and N2 starts at T > 348 K. The speed of the thermolysis was estimated gravimetrically and by infrared spectroscopy, considering the change of the intensity of the absorption band at 1498 cm-1, which corresponds to fluorobenzene. The maximal rate of thermolysis observes at the 366.5 K. A kinetic scheme, which includes the formation of a neutral complex [C6H5δ+?BF4 δ-], is proposed for the thermolysis of arenediazonium tetrafluoroborate. The decomposition of the complex with the formation of free-radical intermediates explains the chain character of the thermolysis.
Cotton, F. A.,George, J. W.
, p. 397 - 403 (1958)
Nucleophilicity of Alkyl Zirconocene and Titanocene Precatalysts, and Kinetics of Activation by Carbenium Ions and by B(C6F5)3
Berionni, Guillaume,Kurouchi, Hiroaki,Eisenburger, Lucien,Mayr, Herbert
supporting information, p. 11196 - 11200 (2016/08/03)
Kinetics of activation of methyl and benzyl metallocene precatalysts by benzhydrylium ions, tritylium ions, and triarylborane B(C6F5)3were measured spectrophotometrically. The rate constants correlate linearly with the electrophilicity parameter E of the benzhydrylium and tritylium ions employed, allowing us to determine the σ-nucleophilicities of the metal–carbon bond of several zirconocenes and titanocenes. Bridging, substitution, metal, and ligand effects on the rates of metal–alkyl bond cleavage (M=Zr, Ti) were studied and structure–reactivity correlations were used to predict the kinetics of generation of metallocenium ions pairs, which are active catalysts in polymerization reactions and are highly electrophilic Lewis acids in frustrated Lewis pair catalysis.
Quantum-chemical calculations and IR spectra of the (F2)MF 2 molecules (M = B, Al, Ga, In, Tl) in solid matrices: A new class of very high electron affinity neutral molecules
Wang, Xuefeng,Andrews, Lester
, p. 3768 - 3771 (2011/04/26)
Electron-deficient group 13 metals react with F2 to give the compounds MF2 (M = B, Al, Ga, In, Tl), which combine with F 2 to form a new class of very high electron affinity neutral molecules, (F2)MF2, in solid argon and neon. These (F 2)MF2 fluorine metal difluoride molecules were identified through matrix IR spectra containing new antisymmetric and symmetric M-F stretching modes. The assignments were confirmed through close comparisons with frequency calculations using DFT methods, which were calibrated against the MF3 molecules observed in all of the spectra. Electron affinities calculated at the CCSD(T) level fall between 7.0 and 7.8 eV, which are in the range of the highest known electron affinities.
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