Bromine chloride fluoride

In 1844, H. B. Leesen2 claimed to have made a brom ine fluoride by leading fluorine into bromine, but fluorine was not unequivocally isolated until 1886, and therefore this claim does not hold good some other products must have been formed. The same remark applies to M. Aubr6e, M. Millet, and M. Leborgne s claim to the use of bromine chloride in photographic work. 

At ambient temperature xenon difluoride is very soluble in hydrogen fluoride, bromine trifluoride, iodine pentafluoride, sulfur dioxide, sulfuryl chloride fluoride, acetonitrile it is... 

The mechanism of displacement of chlorine and bromine by fluoride from the side chain of these systems is of interest. It has been suggested that an Sn2 type of displacement of fluorine from 3-trifluoromethylquinoline occurs in reactions with sodium eth-oxide [141] (Figure 9.55), and a similar process could account for the displacements of chloride or bromide by fluoride from 9.54A that were indicated in Figure 9.54. 

Olefin additions Bromine azide. Bromine chloride. Bromine (chlorine) dipyridine nitrate. N-Bromoacetamine. N-Bromoacetamide-DMSO-Water. N-Bromoacetamide-Hydrogen fluoride. n-Butyllithium. Dichloroketene. Dichloromethyl 2-chloromethyl ether. N,N-Dichlorourethane. Dichlorovinylene carbonate. Difluoramine. Ethyl azidoformate. Ethyl bromoacetate. Iodine azide. Iodine isocyanate. Iodine nitrate, lodobenzene dichloride. 1-lodoheptafluoropropane. Mercuric acetate. Nitrosyl chloride. Nitrosyl fluoride. Nitryl iodide. Rhodium trichloride. Silver fluoride. 

ACIDE SULFHYDRIQUE (French) (7783-06-4) A highly flammable and reactive gas. Violent reaction with strong oxidizers, metal oxides, metal dusts and powders, bromine penta-fluoride, chlorine trifluoride, chromium trioxide, chromyl chloride, dichlorine oxide, nitrogen trichloride, nitryl hypofluorite, oxygen difluoride, perchloryl fluoride, phospham, phosphorus persulfide, silver fulminate, soda-lime, sodium peroxide. Incompatible with acetaldehyde, chlorine monoxide, chromic acid, chromic anhydride, copper, nitric acid, phenyldiazonium-chloride, sodium. Forms explosive material with benzenediazonium salts. Flow or agitation of substance may generate electrostatic charges due to low conductivity. Attacks many metals. 

MAGNESIUM CHLORIDE (7786-30-3) Violent reaction or ignition with bromine penta-fluoride. oxygen difluoride, potassium, potassium-sodium alloy, tetrahydrofuran. Incompatible with zinc. Reacts with water, evolving significant heat. Attacks steel in the presence of moisture. 

Tervalent phosphorus acid esters, and triphenylphosphine, attack 2-bromothiazole (34) at bromine in alcoholic solvents to give thiazole and the oxidised phosphorus compounds. A similar attack of tris(diethylamino)phosphine on the bromine atom of bromopentafluorobenzene was used to prepare a series of main-group-four pentafluorophenyl derivatives, e.g. (35). A full paper has appeared on the fluoridation of trimethylsilyl phosphites, or phosphoramidites, with sulphury chloride fluoride. The mild conditions allowed the preparation of sensitive nucleoside derivatives, e.g. (36) and (37). 

Boron tribromide Boron trichloride Boron trifluoride Bromine chloride Bromine trifluoride Dinitrophenol Dinitroresorcinol Carbonyl fluoride Chlorine pentafluoride Chlorine trifluoride Cyanogen Cyanogen chloride Diborane Dichlorosilane Dinitrogen tetroxide Fluorine Germane... 

Thus alkali sulphides are soluble in liquid sulphur dioxide, alkali fluorides in bromine (III) fluoride and alkali chlorides in molten iodine monochloride. For many other ionic compounds the energy released in the reaction with an acceptor solvent is often too small to allow reasonable solubilities. 

Complex fluorides are easily prepared by making use of both the fluorinating and ionizing properties of bromine (III) fluoride. Compounds which will yield the acidic and basic fluorides by fluorination are mixed and allowed to react with excess bromine (III) fluoride. A mixture of equivalent amounts of potassium chloride and antimony (III) fluoride, for example, may be used to obtain potassium... 

On the other hand phosphorus(V) fluoride gives the hexafluorophosphate ion in solutions of bromine(III) fluoride. Thus phosphorus(V) chloride is a solvo-... 

The halogens form a series of compounds with each other, which are called interhalogens. Examples are bromine chloride (BrCl), iodine bromide (IBr), bromine fluoride (BrF), and chlorine fluoride (CIF). Which compound is expected to have the lowest boiling point at any given pressure Explain. 

Beryllium, pciwder Beryllium Chloride Beryllium Compounds, n.o.s. Beryllium Fluoride Beryllium Nitrate Bifluorides, n.o.s. Biomedical Waste, n.o.s. 1567 1566 1566 1566 2464 1740 3291 32 53 53 53 42 60 24 Bromine Bromine Chloride Bromine Pentafluoride Bromine Solutions Bromine Trifluoride Bromoacetic Acid, solid Bromoacetic Acid, solution 1744 2901 1745 1744 1746 1938 1938 59 20 44 59 44 60 60... 

Iron hahdes react with haHde salts to afford anionic haHde complexes. Because kon(III) is a hard acid, the complexes that it forms are most stable with F and decrease ki both coordination number and stabiHty with heavier haHdes. No stable F complexes are known. [FeF (H20)] is the predominant kon fluoride species ki aqueous solution. The [FeF ] ion can be prepared ki fused salts. Whereas six-coordinate [FeCy is known, four-coordinate complexes are favored for chloride. Salts of tetrahedral [FeCfy] can be isolated if large cations such as tetraphenfyarsonium or tetra alkylammonium are used. [FeBrJ is known but is thermally unstable and disproportionates to kon(II) and bromine. Complex anions of kon(II) hahdes are less common. [FeCfy] has been obtained from FeCfy by reaction with alkaH metal chlorides ki the melt or with tetraethyl ammonium chloride ki deoxygenated ethanol. 

Ha.logen Compounds. Fluorine is unreactive toward ozone at ordinary temperatures. Chlorine is oxidized to Cl20 and Cl20y, bromine to Br Og, and iodine to I2O2 and I4O2. Oxidation of haUde ions by ozone increases with the atomic number of haUde. Fluoride is unreactive chloride reacts slowly, ultimately forming chlorate and bromide is readily oxidized to hypobromite (38). Oxidation of iodide is extremely rapid, initially yielding hypoiodite the estimated rate constant is 2 x 10 (39). HypohaUte ions are oxidized to haUtes hypobromite reacts faster than hypochlorite (40). 

Thallium (ITT) fluoride has been prepared by the action of fluorine or bromine trifluoride on thaUium(III) oxide at 300°C. It is stable to ca 500°C but is extremely sensitive to moisture. Thallium (ITT) chloride can be obtained readily as the tetrahydrate [13453-33-3] by passing chlorine through a boiling suspension of HCl in water. It can be dehydrated with thionyl chloride. Thallium (ITT) bromide tetrahydrate [13453-29-7] is prepared similarly, whereas the iodide prepared in this manner is thaUium(I) triiodide [13453-37-7] H" F2-... 

At 225—275°C, bromination of the vapor yields bromochloromethanes CCl Br, CCl2Br2, and CClBr. Chloroform reacts with aluminum bromide to form bromoform, CHBr. Chloroform cannot be direcdy fluorinated with elementary flourine fluoroform, CHF, is produced from chloroform by reaction with hydrogen fluoride in the presence of a metallic fluoride catalyst (8). It is also a coproduct of monochlorodifluoromethane from the HF—CHCl reaction over antimony chlorofluoride. Iodine gives a characteristic purple solution in chloroform but does not react even at the boiling point. Iodoform, CHI, may be produced from chloroform by reaction with ethyl iodide in the presence of aluminum chloride however, this is not the route normally used for its preparation. 

Antimony trichloride, pentachloride and pentafluoride Beryllium chloride Boron trichloride Bromine Chlorine Calcium fluoride Chromic fluoride Chromous fluoride Fluorine Iodine... 

The last example represents a fairly rare elimination of hydrogen fluoride in preference to hydrogen chloride, a reaction that deserves a more detailed discussion A comparison of bond dissociation energies of carbon-halogen bonds shows that the carbon-fluorine bond is much stronger than the carbon-chlorine, carbon-bromine, and carbon-iodme bonds 108-116, 83 5, 70, and 56 kcal/mol, respec-... 

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