ChemInform Abstract: Selective Si-Si Bond Cleavage of Decaisopropylbicyclo[2.2.0]hexasilane with Hydrobromic Acid and Hydrochloric Acid.

ChemInform ◽  
2010 ◽  
Vol 33 (19) ◽  
pp. no-no
Author(s):  
Akira Meguro ◽  
Haruaki Sakurai ◽  
Kei Kato ◽  
Soichiro Kyushin ◽  
Hideyuki Matsumoto
Keyword(s):  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Bond Cleavage

Selective Si–Si Bond Cleavage of Decaisopropylbicyclo[2.2.0]hexasilane with Hydrobromic Acid and Hydrochloric Acid

2001 ◽  
Vol 30 (12) ◽  
pp. 1212-1213 ◽  
Author(s):  
Akira Meguro ◽  
Haruaki Sakurai ◽  
Kei Kato ◽  
Soichiro Kyushin ◽  
Hideyuki Matsumoto
Keyword(s):  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Bond Cleavage

scholarly journals A new radio-active element, which evolves thorium emanation. Preliminary communication

1905 ◽  
Vol 76 (508) ◽  
pp. 115-117 ◽  
Keyword(s):  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Dilute Hydrochloric Acid ◽  
Active Element ◽  
Preliminary Estimation ◽  
New Radio ◽  
Preliminary Communication ◽  
Final Residue

[The material for this investigation was provided by Sir William Ramsay; it was the final residue remaining after fusion with bisulphate of 5 cwt. of the cubical ore from Ceylon, for which the name “thorianite” has been suggested by Professor Dunstan. This residue was fused with carbonates,, the silica was removed, and the carbonates dissolved in dilute hydrochloric acid. Lead was precipitated as sulphide, and the carbonates again precipitated. These preliminary operations were carried out by Mr. Charles Tyrer and by Dr. Denison.] This residue weighed about 18 grammes, and a preliminary estimation of radio-activity led to the belief that it would yield about 15 milligrammes of pure radium bromide. The carbonates were dissolved in pure aqueous hydrobromic acid, and the bromides fractionated according to Giesel’s method. But difficulties were soon encountered; the more soluble portion did not fall off in radio-activity, but gradually grew more strongly radio­ active; the radium concentrated at the least soluble end, and the middle fractions became relatively weak in radio-activity.

XVII. On the properties of electro-deposited antimony (concluded)

1862 ◽  
Vol 152 ◽  
pp. 323-331 ◽  
Keyword(s):  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Usual Manner

92. In addition to the variety of electro-deposited antimony obtained from a solution of teroxide of antimony and hydrochloric acid, a second variety may be obtained from a solution of terbromide of antimony in the following manner. 93. Dissolve one part of teroxide of antimony in 10 parts of hydrobromic acid of sp. gr. about 1⋅3, filter the solution through a funnel loosely plugged with asbestus, and electrolyse it by means of three Smee’s elements and an anode of antimony in the usual manner, at a speed of deposition of about 3 to 5 grains per square inch per hour. The exact proportion of the ingredients of the solution is not a matter of great importance.

Formation of isomeric monohalo-n-alkanoic acids in the reactions of γ- and δ-n-alkanolactones with hydrogen halides

1993 ◽  
Vol 71 (6) ◽  
pp. 864-871 ◽  
Author(s):  
Alessandro Granata ◽  
Arthur S. Perlin
Keyword(s):  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Ring Opening ◽  
Hydriodic Acid ◽  
Hydrogen Halides ◽  
Chlorine Atoms ◽  
Halogen Atoms ◽  
Alkanoic Acids ◽  
Main Factors

In 57% hydriodic acid or 48% hydrobromic acid, under reflux, n-alkanoic γ- or δ-lactones of from 5 to 18 carbon atoms undergo facile ring opening to monohalo-n-alkanoic acids. With both reagents the ratio of acid to lactone at equilibrium varies widely, ranging from about 1:3 for γ-valerolactone (C5) to 3:1 or more for γ-octanolactone and the larger members of the series. Extensive scrambling of the halogen atoms accompanies the formation of the haloacids, whereby mixtures of monohalo isomers substituted at all positions from C-4 to the penultimate carbon are found. In an 18 h reaction with HBr, for example, γ-caprolactone was converted into a 1:3 mixture of 4- and 5-bromohexanoic acids, and γ-decanolactone into a 1:1.4:1.4:1.4:2.3:2.3 mixture of 4-, 5-, 6-, 7-, 8-, and 9-bromodecanoic acids. By contrast, the γ-lactones containing 14 or 16 carbon atoms gave only 10:1 mixtures of the 4- and 5-bromoacids, and at the level of 18 carbon atoms rearrangement was no longer evident; i.e., γ-octadecanolactone afforded only 4-bromooctadecanoic acid. Similar isomer distributions were obtained for the iodoacid homologs. Hydrochloric acid (37%) was far less effective in opening the lactone rings, and also in inducing rearrangement of the chlorine atoms introduced. Differences in entropy and in solvation appear to be the main factors contributing to the variations observed among isomeric lactones.

scholarly journals III. On the absorption and radiation of heat by gaseous matter.—Second memoir

1862 ◽  
Vol 11 ◽  
pp. 558-561
Keyword(s):  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Chemical Combination ◽  
New Apparatus

Resuming with a new apparatus his experiments on the influence of chemical combination on the absorption and radiation of heat by gases, the author in the present investigation first examines the deportment of chlorine as compared with hydrochloric acid, and of bromine as compared with hydrobromic acid, and finds that the act of combination, which in each of these two cases notably diminishes the density of the gas, and renders the coloured gas perfectly transparent to light, renders it more opake for obscure heat. He also draws attention to the fact that sulphur, which is partially opake to light, is transparent to 54 per cent, of the rays issuing from a source of 100°C., while its compound, heavy spar, which is sensibly transparent to light, is quite opake to the rays from a source of 100°C.

scholarly journals II. Contributions to the history of the opium alkaloids. —Part III

1872 ◽  
Vol 20 (130-138) ◽  
pp. 8-21
Keyword(s):  
Hydrochloric Acid ◽  
Methyl Iodide ◽  
Hydrobromic Acid ◽  
Hydriodic Acid ◽  
Large Excess ◽  
Appreciable Quantity ◽  
Opium Alkaloids ◽  
Free Iodine ◽  
History Of

In Parts I. and II. of these researches the action of hydrobromic acid on codeia and its derivatives has been partially investigated; and as the action of this acid appears to be in some respects similar to, but in others different from, that of hydrochloric acid, it appeared to be of interest to examine the action of hydriodic acid also. Some preliminary experiments on this subject made two or three years ago in conjunction with the late Dr. A. Matthiessen, showed that when codeia is boiled with a large excess of strong hydriodic acid, no appreciable quantity of methyl iodide is evolved even after some hours treatment; a brown tarry mass containing much free iodine was produced, but at the time nothing fit for analysis was obtained from this; since then, Dr. Matthiessen and Mr. Burnside have corroborated the non-formation of methyl iodide under these circumstances.

scholarly journals The effect of solvent on reaction velocity. V.-The interaction of N-chloroacetanilide and hydrobromic acid in dilute aqueous solution

1934 ◽  
Vol 144 (853) ◽  
pp. 643-655
Keyword(s):  
Aqueous Solution ◽  
Hydrochloric Acid ◽  
Hydrobromic Acid ◽  
Ion Concentration ◽  
True Rate ◽  
Simultaneous Formation ◽  
Ion Concentrations ◽  
Hückel Theory ◽  
Dilute Aqueous Solution ◽  
Acid Reaction

The interaction of N-chloroacetanilide and hydrobromic acid to form p - bromoacetanilide and hydrochloric acid has, unlike the corresponding reaction with hydrochloric acid. received comparatively little attention from a kinetic standpoint. It possesses, however, the advantage over the hydrochloric acid reaction, that its speed is much greater. It thus allows of the examination of mixtures containing only 0·001 M hydrobromic acid and of salt effects in the region of dilute concentration where the Debye-Hückel theory applies. The mechanism of the interaction is analogous to that of the chloroamine- hydrochloric acid reaction, where the first stage C 6 H 5 NClAC + HCL I → Cl 2 + C 6 H 5 NHAc II → ClC 6 H 4 NHAc +HCl determines the rate of transformation of the chloroamine in aqueous solution. Two corrections are necessary in this reaction if the true rate of interaction of chloroamine and acid is to be determined. The first correction is for the hydrolysis of the chloroamine under the influence of the acid, a rate mainly dependent on the H • ion concentration. Since the rate of the transformation depends on the product of the H • and Cl' ion concentrations, the correction for hydrolysis cannot l>e regarded as forming a constant fraction of the observed speed, particularly when the ratio of these ion concentrations is widely varied. The second correction is for the simultaneous formation of the chloroamim of the chloroanilides present. These chloroamines, which are formed pro-gressively, appear in the chloroamine titre and cause the measured reaction rate to be slower by 4-10% than the actual rat* of production of chlorine. This complication can be avoided by the presence of easily chlorinated sub-stances. such as anisole, p -cresol, or acetanilide, which remove the chlorine as formed.

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