7787-71-5 Usage
Chemical Properties
Different sources of media describe the Chemical Properties of 7787-71-5 differently. You can refer to the following data:
1. fuming colourless or light yellow liquid,
2. Bromine trifluoride is a noncombustible, colorless
to gray-yellow fuming liquid. Extremely irritating odor.
Physical properties
Colorless liquid; hygroscopic; density 2.803 g/mL; boils at 125.8°C; solidifies at 8.8°C; vapor pressure 8 torr at 21°C; decomposes violently in water.
Uses
Different sources of media describe the Uses of 7787-71-5 differently. You can refer to the following data:
1. The commercial uses of this compound arevery limited. It is used as a solvent forfluorides.
2. Solvent for fluorides.
Preparation
Bromine trifluoride may be prepared by fluorination of bromine at 80°C. The halogen mixtures may be diluted in nitrogen or an inert gas.
General Description
A colorless to yellow, fuming liquid with a pungent odor. Solidifies at 48°F. Very toxic by inhalation and corrosive to metals and tissue. Containers exposed to prolonged heat may violently rupture and rocket.
Air & Water Reactions
Fumes in air. Reacts with water with explosive force, oxygen being evolved [Handbook of Chemistry and Physics].
Reactivity Profile
BROMINE TRIFLUORIDE is a very reactive oxidizing agent. Reacts violently on contact with water to evolve oxygen. Accelerates the burning of combustible material. Mixing with the following hydrogen-containing substances is likely to cause a fire or explosion: acetic acid, ammonia, benzene, ethanol, 2-pentanone, hydrogen, hydrogen sulfide, methane, cork, grease paper , wax. Mixing with acids, halogens, ammonium halides, metal halides, metals, nonmetals, or metal oxides at ambient or slightly above ambient temperatures has resulted in violent reactions. Specifically, reacts dangerously with nitric acid, sulfuric acid, chlorine, iodine, ammonium chloride, potassium iodide, boron powder, selenium, tellurium, aluminum powder, bismuth, cobalt powder, iron powder, arsenic, nickel powder, chromium trioxide, charcoal, red phosphorus, sulfur dioxide, magnesium oxide.
Hazard
Corrosive to skin. Very reactive and dan-
gerous.
Health Hazard
Different sources of media describe the Health Hazard of 7787-71-5 differently. You can refer to the following data:
1. The vapors of bromine trifluoride are highlyirritating to the eyes, skin, and mucousmembranes. Upon contact with the skin, theliquid can cause severe burns. The toxicitydata for this compound are not available.
2. Inhalation causes severe irritation of upper respiratory system. Contact with liquid or vapor causes severe burns of eyes and can cause ulcers and blindness. Contact with skin causes severe burns. Ingestion causes severe burns of mucous membranes.
Fire Hazard
Behavior in Fire: Forms very toxic and irritating fumes.
Safety Profile
Poisonous and
corrosive. Very reactive, a powerful oxidizer.
Explosive or violent reaction with organic
materials, water, acetone, ammonium
halides, antimony, antimony trichloride
oxide, arsenic, benzene, boron, bromine,
carbon, carbon monoxide, carbon
tetrachloride, carbon tetraiodlde,
chloromethane, cobalt, ether, halogens,
iodine, powdered molybdenum, niobium, 2
pentanone, phosphorus, potassium
hexachloroplatinate, pyridine, sihcon,
silicone grease, sulfur, tantalum, tin
dichloride, titanium, toluene, vanadurn,
uranium, uranium hexafluoride.
Incompatible with Sb203, BaCl2, Bi205,
CdCl2, CaCl2, CsCl, LiCl, MnI03, metals,
Nb205, PtBr4, PtCl4, (Pt + KFO), Iar, KCl,
KI, RhBr4, RbCl, AgCl, NaBr, NaCl, NaI,
Ta205, Sn, W, UO,, rubber, plastics. The
product of reaction with pyridine ignites
when dry. When heated to decomposition it
emits toxic fumes of Fand Br-. Very
dangerous. See also BROMINE
Potential Exposure
Bromine Trifluoride is used as a fluorinating
agent and an electrolytic solvent.
Shipping
UN1746 Bromine trifluoride, Hazard class 5.1;
Labels: 5.1—Oxidizer, 6.1—Poison Inhalation Hazard, 8—
Corrosive material, Inhalation Hazard Zone B.
Incompatibilities
A powerful oxidizer; highly reactive and
a dangerous explosion hazard. Contact with water or other
hydrogen containing materials forms hydrogen fluoride gas.
Reacts with almost all elements except for inert gases.
Violent reaction with reducing agents; organic materials;
strong acids; strong bases; halogens, salts (antimony salts),
metal oxides; and many other materials. Attacks some plastics,
rubber, or coatings.
Check Digit Verification of cas no
The CAS Registry Mumber 7787-71-5 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,7,8 and 7 respectively; the second part has 2 digits, 7 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 7787-71:
(6*7)+(5*7)+(4*8)+(3*7)+(2*7)+(1*1)=145
145 % 10 = 5
So 7787-71-5 is a valid CAS Registry Number.
InChI:InChI=1/BrF3/c2-1(3)4
7787-71-5Relevant articles and documents
PbF[Br2F7], a Fluoridobromate(III) of a p-Block Metal
Bandemehr, Jascha,Sachs, Malte,Ivlev, Sergei I.,Karttunen, Antti J.,Kraus, Florian
, p. 64 - 70 (2020)
The compound PbF[Br2F7] represents the first fluoridobromate(III) of a p-block element. It was synthesized in form of needle-shaped crystals among its colorless powder from the direct reaction of PbF2 with BrF3. Powder X-ray diffraction, IR and Raman spectroscopy show that it was obtained in almost pure form with Pb3F8 and Pb2F6 as by-products. The single crystal structure was determined by X-ray diffraction. PbF[Br2F7] crystallizes in space group P21/c (No. 14) with a = 4.3698(3), b = 13.3767(7), c = 12.0836(8) ?, β = 97.509(5)°, V = 700.27(8) ?3, Z = 4 at T = 100 K. PbF[Br2F7] decomposes above 50 °C due to loss of BrF3 and pure PbF2 remains. Quantum chemical calculations were performed on the crystal structure of the compound to assign the bands of the vibrational spectra and to obtain electron density difference maps that visualize the electron density around the Pb atoms. CHARDI calculations support the assignment of the oxidation states +II, +III, and –I to the Pb, Br, and F atoms, respectively.
Preparation of Two Quantum-Chemically Predicted, Isomeric [Br4F13]– Anions in the Solid State
Bandemehr, Jascha,Ivlev, Sergei I.,Karttunen, Antti J.,Kraus, Florian
, p. 4568 - 4576 (2020)
Two isomeric tridecafluoridotetrabromate(III) anions, [Br4F13]–, both previously predicted by quantum-chemical calculations, have serendipitously been obtained from the reaction of BrF3 with BaF2. Single crystals of Ba2[Br3F10]2[Br4F13]2 were selected from the reaction mixture at approximately 10 °C. The crystal structure contains two novel, isomeric [Br4F13]– anions besides the known, star-shaped [Br3F10]– anions. It crystallized in the monoclinic space group P1n1 (No. 7) with a = 8.8519(18), b = 15.217(3), c = 14.628(3) ?, β = 90.34(3)°, V = 1970.4(7) ?3 and Z = 2, mP124 at 100 K. The compound was additionally investigated using quantum-chemical solid-state calculations. If however crystals from the above reaction mixture were selected at room temperature, the compound Ba[Br3F10]2·BrF3 was obtained containing disordered BrF3 molecules of crystallization besides [Br3F10]– anions. The [Br4F13]– molecules were no longer present. Ba[Br3F10]2·BrF3 crystallized in the cubic space group Pa3 (No. 205) with a = 12.4903(14) ?, V = 1948.6(7) ?3, Z = 4, cP124, T = 100 K. The much easier to handle latter compound was additionally investigated using powder X-ray diffraction, as well as IR and Raman spectroscopy.
Enthalpy of sublimation of platinum tetrafluoride
Bondarenko, A. A.,Korobov, M. V.,Mitkin, V. N.,Sidorov, L. N.
, p. 299 - 304 (1988)
The saturated vapour of platinum tetrafluoride was studied by Knudsen-cell mass spectrometry.The only gaseous species found was PtF4(g).The molar sublimation enthalpy: ΔsubHm0(PtF4, 298.15 K) = (207 +/- 16)kJ.mol-1/s
Synthesis of difluoroaryldioxoles using BrF3
Hagooly, Youlia,Welch, Michael J.,Rozen, Shlomo
, p. 902 - 905 (2011/03/22)
A novel synthesis of different aromatic and heteroaromatic difluorodioxole derivatives has been developed. The starting materials were catechols, which, after treatment with thiophosgene, formed at 0 °C the respective thiodioxoles. The latter were reacted for a short time with commercially available bromine trifluoride, producing potentially biologically important difluoroaryldioxoles in moderate to high yields.
