# Are Group 2 metal fluoride salts less soluble in organic solvents than Group 1 fluorides?

It is clear that Group 1 metal fluoride salts DO NOT readily form solutions in organic medium. The amount of solvation that can occur leading to the eventual release of a fluoride ion depends on many factors, one is the polarity of solvent (described by dielectric constant). Most examples seen in the literature seem to evolve around using $$\ce{CsF}$$ or $$\ce{KF}$$ in the vicinity of 18-crown-6 ether as common examples for the release of fluoride ions (not considering TBAF). However, I cant seem to find any description for $$\ce{MgF2}$$ or $$\ce{CaF2}$$ salts and how their solubility in organic medium affects the release of fluoride ions.

Getting fluoride ions into solution with organic solvents is typically done with bulky 1+ cations, such as N,N,N-trimethyl-(2,2-dimethyl-prop-1-yl)ammonium ion, $$\ce{C_{8}H_{20}N^+}$$. See Reference [1] as an example. The use of cryptand-complex alkali-metal complexes fits this paradigm because such ions are also bulky.