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.
Don't get your hopes up.  Wikipedia identifies magnesium fluoride as insoluble in ethanol.  Calcium fluoride fares no differently in acetone.  While these data are hardly exhaustive, they suggest strongly that Group 2 fluorides are not a good way to get fluoride ions into solution.  Of course, we would not expect Group 2 ionic compounds with their doubly charged ions to get vary far in organic solvents generally.
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.
Reference
1.
Victoria K. Davis, Stephen Munoz, Jeongmin Kim, Christopher M. Bates, Nebojslš a Momčilović, Keith J. Billings, Thomas F. Miller III, Robert H. Grubbs and Simon C. Jones, &quot;Fluoride-ion solvation in non-aqueous electrolyte solutions&quot;, Mater. Chem. Front.,
2019, 3, 2721