In addition to mechanical methods, radon levels can also be decreased by using chemical reactions which trap and ultimately remove it before it becomes dangerous.
Reacting with Halogen Fluorides Forcing an inert noble gas to react is quite difficult due to their full valence electron orbitals and unwillingness to lose or gain electrons; this causes a challenge for possible chemical methods of radon removal. However, studies have shown that noble gases are not absolutely inert, contrary to chemists’ assumptions for many years.
Research involving the use of radon poses danger to those involved, due to all radon isotopes being unstable and radioactive. Comparable to radon, xenon is the next largest noble gas, and exists as a stable isotope; this makes it a good alternative to use for preliminary research.
XeF 4 was found to form easily and remain stable at room temperature; however when exposed to water, XeF 4 undergoes a complex hydrolysis reaction, forming elemental xenon( shown in Reaction 1).
XeF 4
+ 2H 2 O → Xe + O 2
+ 4HF( 1)
If radon tetrafluoride were to have similar properties, as predicted through studying xenon, this reaction would not be beneficial to the problem at hand as it would allow radon isotopes to be reformed. However, studies have shown radon fluorides to be more stable than xenon fluorides. In one study of the stability of radon fluoride, trace amounts of radon fluoride were left at room temperature for several days. Afterward, no elemental radon was found, implying the reverse reaction does not occur as favorably. The reaction between radon and fluorine gas( Reaction 2) proceeds in low concentrations at 400 ℃, and spontaneously at room