Bromide iodine

Brom-jod, n. iodine bromide, -kalium, n. potassium bromide, -kalzium, n., kalk, tn. calcium bromide, -kampher, tn. bromo-camphor, Pharm.) monobromated camphor, -kohlenstoff, tn. carbon (tetra)bromide. -korper, tn. Colloids) "bromide body (bromide ion), -kupfer, n. copper bromide, lauge, /. bromine lye (solution of sodium hypobromite and bromide made by passing bromine into sodium hydroxide solution), -lithium, n. lithium bromide. -Idsung, /. bro-nune solution, -magnesium, n. magnesium bromide. -metall, n. metallic bromide. 

To determine molecular motions in real time necessitates the application of a time-ordered sequence of (at least) two ultrafast laser pulses to a molecular sample the first pulse provides the starting trigger to initiate a particular process, the break-up of a molecule, for example whilst the second pulse, time-delayed with respect to the first, probes the molecular evolution as a function of time. For isolated molecules in the gas phase, this approach was pioneered by the 1999 Nobel Laureate, A. H. Zewail of the California Institute of Technology. The nature of what is involved is most readily appreciated through an application, illustrated here for the photofragmentation of iodine bromide (IBr). 

Figure 1.3. Real-time femtosecond spectroscopy of molecules can be described in terms of optical transitions excited by ultrafast laser pulses between potential energy curves which indicate how different energy states of a molecule vary with interatomic distances. The example shown here is for the dissociation of iodine bromide (IBr). An initial pump laser excites a vertical transition from the potential curve of the lowest (ground) electronic state Vg to an excited state Vj. The fragmentation of IBr to form I + Br is described by quantum theory in terms of a wavepacket which either oscillates between the extremes of or crosses over onto the steeply repulsive potential V[ leading to dissociation, as indicated by the two arrows. These motions are monitored in the time domain by simultaneous absorption of two probe-pulse photons which, in this case, ionise the dissociating molecule.

Potassium ignites in fluorine and in dry chlorine (unlike sodium). In bromine vapour it incandesces, and explodes violently in liquid bromine. Mixtures with iodine incandesce on heating, and explode weakly on impact. Potassium reacts explosively with molten iodine bromide and iodine, and a mixture with the former is shock-sensitive and explodes strongly. Molten potassium reacts explosively with iodine pentafluoride [1], Contact with iodine trichloride causes ignition [2],... 

Sodium ignites in fluorine gas but is inert in the liquefied gas [1]. Cold sodium ignites in moist chlorine [2] but may be distilled unchanged in the dry gas [1]. Sodium and liquid bromine appear to be unreactive on prolonged contact [3], but mixtures may be detonated violently by mechanical shock [4]. Finely divided sodium luminesces in bromine vapour [1], Iodine bromide or iodine chloride react slowly with sodium, but mixtures will explode under a hammer-blow [1]. Interaction of iodine pentafluoride with solid sodium is initially vigorous, but soon slows with film-formation, while that with molten sodium is explosively violent... 

See Ammonium nitrate Metals Chlorine Metals Chlorine trifluoride Metals Copper(II) nitrate Tin Fluorine Metals Iodine bromide Metals Iodine heptafluoride Metals Potassium dioxide Metals Sodium peroxide Metals Sulfur Metals Tellurium Tin... 

From l,l,-/)i.v-(3-methyl-4-imidazoline-2-selone)methane with iodine bromide, a solid compound containing disordered molecules with T-shaped CSeI2 and Br-Se(C)-I functions in the same crystal was isolated from 1,2-fe-(3-methyl-4-imidazoline-2-selone)ethane with iodine bromide, a solid... 

The reaction of phenyl-1,2-propadiene with iodine bromide in MeOH afforded a 100% yield of 2-iodo-3-phenyl-3-methoxy-l-propene whereas the reaction in CS2 at 0°C provided a l 4mixture of 2-iodo-3-phenyl-3-bromo-l-propene and l-phenyl-2-iodo-3-bromo-l-propene [16]. The corresponding chlorination shows a lower regios-... 

The methyl of the CHsO group is converted into methyl iodide (Zeisel s method) by boiling with hydriodic acid and the methyl iodide is converted into the corresponding bromide with formation of iodine bromide ... 

The iodine bromide is oxidised to iodic acid by excess of bromine BrI + 2Br2 + 3HaO = HI03 + 5HBr. 

Iodine bromide, 0254 Iodine chloride, 4013 Iodine heptafluoride, 4378 Iodine pentafluoride, 4355 Iodine trichloride, 4139... 

The halogen fluorides are usually regarded as normal covalent hquids, in spite of the fact that the iodine chlorides and iodine bromide conduct electricity both in the molten state and in solution (2). 

J. J. van Laar has shown how the form of the vap. press, curves of a liquid mixture can furnish an indication, not a precise computation, of the degree of dissociation of any compound which maybe formed, on the assumption that the different kind of molecules in the liquid—12, Br2, and IBr—possess partial press, each of which is equal to the product of the vap. press, of a given component in the unmixed state and its fractional molecular concentration in the liquid. It is assumed that in the liquid, there is a balanced reaction 2IBr I2-)-Br2, to which the law of mass action applies, where K is the equilibrium constant, and Clt C2, and C respectively denote the concentration of the free iodine, free bromine, and iodine bromide. From this, P. C. E. M. Terwogt infers that at 50 2°, K for the liquid is 7j and that for iodine monobromide about 20 per cent, of the liquid and about 80 per cent, of the vapour is dissociated. That the vapour of iodine monobromide is not quite dissociated into its elements is evident from its absorption spectrum, which shows some fine red orange and yellow lines in addition to those which characterize iodine and bromine. In thin layers, the colour of the vapour is copper red. 0. Ruff29 could uot prove the formation of a compound by the measurements of the light absorption of soln. of iodine and bromine in carbon tetrachloride. 

A. J. Balard showed that bromic acid is decomposed by hydrobtomic add into bromine and water by hydrochloric acid into water an d bromine chloride and by hydriodic acid into water and iodine bromide. There are nine reactions belonging to this set, namely, chloric, bromic, and iodic acids each with each of the three haloid acids—HC1, HBr, and HI. The kinetics of these reactions have been studied extensively.29 W. Bray has shown that the velocity of the reaction between... 

RATE COEFFICIENTS FOR REACTION OF TETRAALKYLTINS WITH IODINE BROMIDE AND... 

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