No, you can not have nitrosyl bromide just like that (except if you meant it as a minor equilibrium species). That is because nitrosyl bromide reacts
with bromide anions and so do many other species involved. It is all a matter of an equilibrium resting on redox potentials. Such systems are called
dynamic equilibriums (see J. Phys. Chem., 93 (1989) 2801–2807). Essentially if you could distil out bromine without it being accompanied by nitrogen oxides, this
method could be of preparative use, but since this is not simple...
Yet understanding dynamic equilibriums (that is equilibriums with low equilibrium constants) is one of the basic knowledges you need to understand
which path a chemical reaction take. Many reaction pathways, particularly in organic chemistry, are actually composed of a series of dynamic
equilibriums leading toward a thermodinamicaly somewhat more stable product.
…there is a human touch of the cultist “believer” in every theorist that he must struggle against as being
unworthy of the scientist. Some of the greatest men of science have publicly repudiated a theory which earlier they hotly defended. In this lies their
scientific temper, not in the scientific defense of the theory. - Weston La Barre (Ghost Dance, 1972)
Read the The ScienceMadness Guidelines!
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