Decomposition Of Bis Research Articles

Formation and Decomposition of Bis(chloromethyl) Ether in Aqueous Media

Abstract Reports that bis(chloromethyl) ether (BCME) is carcinogenic have prompted numerous investigations into the formation and decomposition of the compound. In this study, it is shown that the compound forms rapidly in a chloromethylating medium (HC1-HCHO-ZnC12) at low levels (100 ppm) and attains a fairly steady concentration of 300-500 ppm. Methods for destroying BCME are discussed including the rates of destruction in homogeneous and heterogeneous media. Although BCME is considered reactive, it is not readily decomposed by water or aqueous base because of its low solubility. In homogeneous media such as MeOH-H2O. the rate of hydrolysis is much faster. The reaction of BCME with aqueous ammonia is very fast and a reaction path to hexamethylenetetramine is suggested. Gaseous BCME reacts rapidly with aqueous systems, particularly alkaline solutions, due to greater contact efficiency.

Reactivity of bis (tribenzylsilyl) mercury

1. The thermal decomposition of bis(tribenzylsilyl)mercury and its reaction with 1,5-dibromopentane, 1,2-dibromoethane, mercuric bromide, sulfur, triethylchlorostannane, triethylethoxystannane, and acetic acid proceed with a cleavage of the Si-Hg-Si fragment. 2. The reactivity of bis(tribenzylsilyl)mercury is substantially lower than that of other silylmercury compounds.

Kinetics of the thermal decomposition of bis-(2,2-dinitropropyl)-N-nitroamine

The kinetics of the thermal decomposition of bis(2,2-dinitropropyl)-N-fluoroamine are studied in the liquid phase. The reaction is autocatalytic in a melt. In dilute solution, the reaction rate is described by the first-order law. It is tens of times faster in polar sulfolan than in weakly polar dimethyl phthalate. A mechanism of the decomposition involving the formation of a cyclic transition state at the first, limiting stage of the process is suggested.

Kinetics of the thermal decomposition of bis(nitroalkyl)-N-nitrosoamines

1. The kinetics of the thermal decomposition of bis-(2,2-dinitropropyl)-N-nitrosoamine, bis-(2,2-dinitro-2-fluoroethyl)-N-nitrosoamine, and bis-(2,2,2-trinitroethyl)-N-nitrosoamine was studied. 2. The reactions are described by a first-order equation. The activation energies and preexponential factors were determined. 3. The reaction center in the bis-(2,2,2-trinitroethyl)-N-nitrosoamine molecule is the trinitromethyl group, while in the other two compounds it is the nitrosoamine group. The mechanism of the decomposition is discussed. 4. The enthalpy of formation of the (NO2)2CCH2N(NO)CH2C(NO2)3 radical was calculated.

Organosilicon compounds. Part L. Kinetics of the thermal decomposition of bis(trimethylsilyl)mercury in solution

The thermal decomposition of solutions of bis(trimethylsilyl)mercury in benzene or cyclohexane shows second-order kinetics, except that a small first-order contribution appears at very low concentrations in cyclohexane. In toluene mixed second- and (pseudo)-first-order kinetics are observed, and in anisole, (pseudo)-first-order kinetics only. Bis(trimethylsilyl)mercury appears to decompose mainly by bimolecular reactions, either with itself or with the solvent, with unimolecular homolysis seemingly unimportant. From the small first-order contribution to the reaction in cyclohexane, a rough lower limit of 200 kJ mol–1 for D(Me3Si–HgSiMe3) can be derived.

The decomposition of bis(pentafluorobenzoyl) peroxide in dilute solution

The decomposition of bis(pentafluorobenzoyl) peroxide in benzene at 60° has been studied by radiotracer methods. By using low concentrations of the peroxide, the induced decomposition previously observed has been eliminated. The mechanism of the decomposition is found to be fundamentally similar to that for benzoyl peroxide under the same conditions. The rate constant for the decomposition (7 · 4 × 10 −6 sec −1) is considerably larger than that for benzoyl peroxide, although the energy of activation for the dissociation (about 120 kJ mole −1) is of similar magnitude.

Organosilicon compounds. Part XLIX. Some reactions of bis(triphenylsilyl)mercury

Bis(triphenylsilyl)mercury, prepared by the reaction of dibenzylmercury with triphenylsilane, decomposes on heating to give mercury and hexaphenyldisilane, along with traces of triphenylsilane, tetraphenylsilane, pentaphenyldisilane, and octaphenyltrisilane. Photolysis or pyrolysis in benzene gives the above products, with larger quantities of tetraphenylsilane; the reaction in toluene at 81 and at 220° gives additionally the tolyltriphenylsilanes (at the low temperature only), benzyltriphenylsilane (more at the higher temperature), and bibenzyl. Though the solid mercury compound is fairly stable to air and water, solutions in inert solvents react rapidly with air (to give mercury and hexaphenyldisiloxane) and with water (to give mercury, triphenylsilanol, and hydrogen as the major products). Radical and molecular reactions are proposed. The thermal decomposition of bis(triphenylsilyl)mercury appears to involve homolytic fission, in contrast to that of bis(trimethylsilyl)mercury, for which molecular reactions appear to be important.

Decomposition of bis(.alpha.-naphthoyl) and .alpha.-naphthoyl benzoyl peroxides

Decomposition of bis(.alpha.-naphthoyl) and .alpha.-naphthoyl benzoyl peroxides

Bis(triphenylgermyl) cadmium

1. The previously undescribed bis(triphenylgermyl)cadmium and its tetrahydrofurane complex were prepared by the reaction of triphenylgermane with diethylcadmium. 2. The thermal decomposition of bis(triphenylgermyl)cadmium and its reactions with benzoyl peroxide and 1,2-bromoethane were investigated. All these reactions involved rupture of the Ge-Cd bond.

Syntheses of analgesics. XVII. Antipyrine derivatives. 4.

The decomposition of bis [(N-4-antipyrinyl-N-methyl) amino] methane (II) with paraformaldehyde and potassium cyanide was effected by heating in glacial acetic acid, and afforded (N-4-antipyrinyl-N-methyl) aminoacetonitrile (VI) and 4-methylaminoantipyrine (I). The condensation of 4-methylaminoantipyrine (I) with paraformaldehyde and potassium cyanide on being warmed in glacial acetic acid also furnished (VI). The respective action of an excess of paraformaldehyde on (I) and (III) in dil. hydrochloric acid gave (II). However, in conc. hydrochloric acid, the respective action of an excess of paraformaldehyde on (I), (II), (III), and (VII) afforded (IV).