A hydrogen halide has formula , with hydrogen bonded to a halogen. Hydrogen fluoride, hydrogen chloride, hydrogen bromide, and hydrogen iodide are familiar examples.
Their gas-phase molecules must be distinguished from their aqueous acid solutions. Bond strengths, solvation, and association change across the series, so increasing bond polarity alone does not predict every acid-strength trend.
The diatomic molecule containing one hydrogen atom and one iodine atom. Its measured spectroscopic wavenumbers include anharmonic corrections beyond the two-term Morse oscillator model.[ref]
Hydrogen iodide: Constants of diatomic molecules by Klaus P. Huber and others. Ground-state diatomic constants and higher anharmonic coefficients
The gaseous hydrogen halide consisting of one hydrogen atom and one bromine atom. Its molecular vibration can be studied through its vibrational fundamental and weak vibrational overtones. The aqueous acid and the isolated diatomic molecule should be distinguished when specifying a dissociation process.[ref]
Aqueous hydrogen iodide is strongly acidic, and iodide can also participate in reductive transformations. These roles must be separated when explaining a reaction.
Articles by others on the same topic
There are currently no matching articles.