7790-91-2 Usage
Uses
Used in Chemical Industry:
Chlorine trifluoride is used as a fluorinating agent for various chemical reactions, enabling the incorporation of fluorine into different compounds.
Used in Aerospace Industry:
Chlorine trifluoride is used as a rocket propellant and igniter due to its ability to produce high-energy combustion when mixed with an oxidizer.
Used in Nuclear Industry:
Chlorine trifluoride is utilized in the processing of nuclear reactor fuel, where it serves as a fluorinating agent to help extract or purify uranium or other fissile materials.
Used in Military Applications:
Chlorine trifluoride is employed in incendiaries and as an igniter for its ability to burn or ignite materials that are otherwise difficult to set on fire.
Used in Polymer Industry:
Chlorine trifluoride is used as a pyrolysis inhibitor for fluorocarbon polymers, preventing their decomposition at high temperatures and improving their stability and performance.
Preparation
Chlorine trifluoride is obtained by heating chlorine or chlorine monofluoride with fluorine:
Cl2 + 3F2 2ClF3
ClF + F2 ClF3
The gas is purified by distillation in a special steel apparatus.
Reference
[1]Handbook-of-inorganic-chemicals
Air & Water Reactions
A violent reaction occurs with water or ice generating acidic HF and chlorine, [Sidgwick, 1156(1950)]. The release of CHLORINE TRIFLUORIDE to the atmosphere rapidly generates two toxic reaction products: HF and Chlorine Dioxide, [Lombardi, D.A. and M.D. Cheng 1996. "Modeling Accidental Releases of CHLORINE TRIFLUORIDE to the Atmosphere," Paper No. 96-WP66B.02, presented at the 89th Annual Meeting of the Air and Waste Management Association, Nashville, Tennessee, June 23-26].
Reactivity Profile
CHLORINE TRIFLUORIDE is a low-boiling liquid (b.p. 12° C), in gaseous state irritating and toxic. A highly reactive oxidant reagent, spontaneously flammable, used as a rocket propellant. Incompatible with fuels, nitro compounds. Interaction with water is violent and may be explosive, even with ice [Sidgwick, 1950, p. 1156]. Immediate explosive reaction with hydrocarbons or halocarbons even at -70° C [Brower, K. R., J. Fluorine Chem., 1986, 31, p. 333]. Solution with carbon tetrachloride capable of detonation, solutions with nitroaryl compounds (TNT, hexanitrobiphenyl) or highly chlorinated compounds are extremely shock-sensitive. Violent, sometimes explosive reaction with hydrogen containing materials, e.g., acetic acid, ammonia, benzene, ether, coal gas, hydrogen, hydrogen sulfide, methane, or fluoroamino compounds. Ignition with fibrous materials (cotton, paper, wood). [Mellor, 1956, vol. 2, suppl. 1, p. 155]. Explosive gaseous products (chlorodifluoroamine) formed with ammonium fluoride or ammonium hydrogen fluoride [Gardner, D. M. et al., Inorg., Chem., 1963, 2, p. 413]. Ignition on contact with iodine, boron-containing materials (boron powder, tetraboron carbide, boron-aluminum), fibrous or finely divided refractory materials (asbestos, glass, wool, sand, tungsten carbide). Violent reaction with mineral acids (nitric acid, sulfuric acid), chromium trioxide, ruthenium metal, selenium tetrafluoride. [Bretherick, 5th ed., 1995, p. 1235]. CHLORINE TRIFLUORIDE is a hypergolic oxidizer and contact with a number of metals and their oxides (aluminum, antimony, arsenic, calcium, copper, iridium, iron, lithium, lead, magnesium, molybdenum, osmium, potassium, rhodium, sodium, selenium, silver, tellurium, tin, tungsten, zinc), nonmetals (phosphorus, silicon, sulfur), salts (mercury iodide, potassium iodide, silver, nitrate, potassium carbonate) will result in a violent reaction often followed by ignition [Mellor, 1956, vol. 2, suppl. 1, p. 155; Sidgwick, 1950, p. 1156].
Hazard
Explodes in contact with organic materials or with water. Dangerous fire risk. A poison,
very toxic, corrosive to skin. Lung damage, eye,
and upper respiratory tract irritant. Questionable
carcinogen.
Health Hazard
Chlorine trifluoride is a severe irritant tothe skin, eyes, and mucous membranes.Exposure to this gas can cause lung dam age. A 30-minute exposure to 400 ppm waslethal to rats. It decomposes in the presenceof moisture to chlorine, chlorine dioxide,and hydrogen fluoride, all of which arehighly toxic. Chronic inhalation study on ani mals for a period of 6 months (6 hours/day,5 days/week) indicated that at an exposurelevel of nearly 1 ppm the early symptomswere sneezing, salivation, and expulsionof frothy fluid from the mouth and nose(ACGIH 1986). This progressed to mus cle weakness, pneumonia, and lung damage.Some animals died.In humans, exposure to this gas can pro duce severe injury to the eyes, skin, andrespiratory tract, and pulmonary edema. Theliquid is severely corrosive to the skin andeyes. Skin contact can cause painful burns.
Health Hazard
Inhalation causes extreme irritation of respiratory tract; pulmonary edema may result. Vapors are very irritating to eyes and skin; liquid causes severe burns.
Fire Hazard
Nonflammable gas; dangerously reactive.
Chlorine trifluoride reacts explosively with
water, forming hydrogen fluoride and chlo rine. It reacts violently with most elements
and common substances. Paper, cloth, wood,
glass, wool, charcoal, and graphite burst
into flame in contact with the liquid. The
vapors, even when diluted, can set fire to
organic compounds. Reactions with most metals are vigorous to violent, often caus ing a fire. It catches fire when mixed with
phosphorus, arsenic, antimony, silicon, sul fur, selenium, tellurium, tungsten, osmium,
and rhodium (Mellor 1946, Suppl. 1956).
Among the alkali- and alkaline–earth metals,
reaction is violent with potassium at ordinary
temperatures, and with sodium, calcium, or
magnesium it reacts violently at elevated
temperatures. Violent reaction occurs with
oxides, sulfides, halides, and carbides of
metals, causing flames. Chlorine trifluoride
attacks sand, glass, and asbestos. Prolonged
contact can ignite glass. Explosive reactions
occur with many common gases, includ ing hydrogen, lower hydrocarbons, carbon
monoxide, ammonia, hydrogen sulfide, and
sulfur dioxide. Reactions with mineral acids
and alkalies are violent.In case of a small fire involving chlorine
trifluoride, use a dry chemical or water
spray in large amounts (NFPA 1997). Allow
large fires to burn. Avoid contact of chlorine
trifluoride with the body or with protective
clothing.
Safety Profile
Human poison by
inhalation. An eye irritant. See also
FLUORIDES, CHLORINE, and
FLUORINE. Spontaneously flammable. A
powerful oxidant whch may react violently
with oxidzable materials. A rocket
propellant.
Explosive reaction with water,
bis (trifluoromethyl) sulfide or -disulfide,
polychlorotrifluoroethylene,
trifluoromethanesulfenyl chloride, and other
hydrogencontaining materials (e.g.,
ammonia, coal gas, hydrogen, hydrogen
sulfide, methane, acetic acid, benzene, ether,
cotton, paper, wood). Forms shock-sensitive
explosive mixtures with highly chlorinated
compounds (e.g., carbon tetrachloride),
nitroaryl compounds (e.g., trinitrotoluene,
hexanitrobiphenyl, hexanitrodiphenyl amine,
hexanitrodiphenyl sulfide, hexanitrobphenyl
ether). Reaction with ammonium fluoride or
ammonium hydrogen fluoride forms
explosive gaseous products.
materials, iodine, finely dvided refractory
materials (e.g., asbestos, glass wool, sand,
tungsten carbide), fluorinated polymers
(with flowing trifluoride).
sulfuric), chromium trioxide, ruthenium,
selenium tetrafluoride (above 106℃),
metals, metal oxides, metal salts, nonmetals,
nonmetal salts, organic matter, glass wool,
acetic acid, Al, Sb, As, Cu, Ir, Fe, Pb, Mg,
Mo, Os, P, Ir, Rh, Se, Si, Ag, Na, S, Te, Sn,
W, Zn, oxides, CO, graphite, HgI2, HNO3,
Ignition on contact with boron-containing
Violent reaction with acids (e.g., nitric or K2CO3, KI, rubber, AgN3, AgNO3, NaOH,
V2P5, wo3. Incompatible with fuels, nitro
compounds. When heated to decomposition
or in reaction with water or steam it emits
toxic fumes of Fand Cl-.
Potential Exposure
Chlorine trifluoride is used as a fluorinating agent. It may be used as an igniter and propellant in
rockets. It is used in nuclear fuel processing.
storage
Chlorine trifluoride is stored and shippedin special steel cylinders. It is stored inmoisture-free, cool, and isolated areas sepa rated from other chemicals. The cylinders arekept upright, covered, and protected againstphysical damage.
Shipping
UN1749 Chlorine trifluoride, Hazard class: 2.3;
Labels: 2.3-Poisonous gas, 5.1-Oxidizer, 8-Corrosive material, Inhalation Hazard Zone B. Cylinders must be transported in a secure upright position, in a well-ventilated
truck. Protect cylinder and labels from physical damage.
The owner of the compressed gas cylinder is the only entity
allowed by federal law (49CFR) to transport and refill
them. It is a violation of transportation regulations to refill
compressed gas cylinders without the express written permission of the owner.
Purification Methods
Impurities include chloryl fluoride, chlorine dioxide and hydrogen fluoride. Passed it first through two U-tubes containing NaF to remove HF, then through a series of traps in which the liquid is fractionally distilled. It can be purified via the KF complex; KClF4, formed by adding excess ClF3 to solid KF in a stainless steel cylinder in a dry-box and shaking overnight. After pumping out the volatile materials, pure ClF3 is obtained by heating the bomb to 100-150o and condensing the evolved gas in a -196o trap [Schack et al. Chem Ind (London) 545 1967]. It attacks glass very vigorously. HIGHLY TOXIC.
Incompatibilities
A powerful oxidizer. Keep away from
acids. Most combustible materials ignite spontaneously
on contact with chlorine trifluoride. Explodes on contact
with organic materials. The liquid can explode if mixed
with halocarbons or hydrocarbons. It reacts violently
with oxidizable materials, finely divided metals and
metal oxides; sand, glass, asbestos, silicon-containing
compounds. Emits highly toxic fumes on contact with
acids. Chlorine trifluoride decomposes above 220C,
forming Thermal decomposition products may include
hydrogen chloride and HF. Reacts violently with water,
forming chlorine gas and hydrofluoric acid. Reacts with
most forms of plastics, rubber, coatings, and resins;
except the highly fluorinated polymers, such as Teflon
and “K el-F.”
Check Digit Verification of cas no
The CAS Registry Mumber 7790-91-2 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,7,9 and 0 respectively; the second part has 2 digits, 9 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 7790-91:
(6*7)+(5*7)+(4*9)+(3*0)+(2*9)+(1*1)=132
132 % 10 = 2
So 7790-91-2 is a valid CAS Registry Number.
InChI:InChI=1/ClF3/c2-1(3)4
7790-91-2Relevant academic research and scientific papers
Disproportionation of chlorine in hydrogen fluoride and related media
Gambardella, Mario,Kongpricha, Santad,Pitts, James J.,Jache, Albert W.
, p. 1828 - 1831 (2007/10/02)
Chlorine can be made to disproportionate to chlorine monofluoride and chloride, taking advantage of Le Chatelier's principle in several different ways.It will disproportionate to form insoluble silver chloride and chlorine monofluoride when silver fluoride is present.It will disproportionate in a melt of alkali metal fluorides to form alkali metal chlorides and chlorine monofluoride.The alkali metal chlorides will react with hydrogen fluoride to regenerate the metal fluorides and hydrogen chloride.Chlorine will also disproportionate in hydrogen fluoride containing antimony pentafluoride to yield antimony pentafluoride adducts of chlorine monofluoride and of hydrogen chloride.These adducts are readily decomposed to yield the disproportionation products and the original antimony pentafluoride.Key words: hydrogen fluoride, disproportionation, chlorine, waterlike, solvent system
Synthesis and characterization of NF4CrF6 and reaction chemistry of CrF5
Bougon, Roland,Wilson, William W.,Christe, Karl O.
, p. 2286 - 2292 (2008/10/08)
NF4CrF6, a new stable NF4+ salt containing an energetic counterion, was prepared by treatment of CrF5 with an excess of NF4HF2 in HF solution. The composition and ionic nature of NF4CrF6 was established by elemental analysis, vibrational and 19F NMR spectroscopy, and its X-ray powder pattern. Reactions of CrF5 with H2O in HF, ClF3, FNO, Cl2, CFCl3, and KrF2 were studied to determine its acidity and oxidizing power. With FNO, a stable 1:1 adduct is formed, which on the basis of its vibrational spectra has the ionic structure NO+CrF6-. The reaction of NOCrF6 with NO produced (NO+)2CrF62-, which by controlled pyrolysis was converted to NO+CrF5-. With stoichiometric amounts of H2O in HF, CrF5 did not form a stable OH3+CrF6- salt but the reaction resulted in hydrolysis to CrF3O. The influence of the strong Lewis acids AsF5 and SbF5 on the oxidizing power of CrF5 was also investigated. On the basis of the fact that CrF5-SbF5 mixtures can oxidize O2 (IP = 12.06 eV) but not NF3 (IP = 13.00 eV), the following qualitative oxidizer strength scale is proposed: KrF+ > PtF6 > SbF5 + F2 + activation energy > CrF5-SbF5. The results of a normal-coordinate analysis of CrF6- and CrF62- show the expected decrease in force constants with increasing negative charge.
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