Much research has been done on the solubility of alkali metals in liquid ammonia, but what has been learned that I can generalize to other metals?
How should I model the gibbs free energy of solvation for metals besides alkali metals that can still give up electrons rather easily, like zirconium, magnesium or aluminum? For the metal's half of the reaction, is the gibbs free energy related to the first ionization energy, the valence ionization energy, or something else?
The metal-nonmetal transition observed in solutions of alkali metals should have an effect on the gibbs free energy, but are there any predictive models for finding the concentration of metal ions at which this transition occurs? And how should this phase transition change the way I model the gibbs free energy? The solubility limit of other metals may be low enough that this is unimportant, but it would be useful to know. Also is there a predictive model I can use to determine whether the ammonia will react chemically with the metal instead of dissolving it?
Sincerely, a math student trying to do chemistry.
Dear Michael,
I would suggest you might first wish to consult the following paper:
Germán Sciaini, Ernesto Marceca, Roberto Fernández-Prini, 'Solubility of crystalline alkali metal iodides in supercritical ammonia', The Journal of Supercritical Fluids -
Volume 35, Issue 2, September 2005, Pages 106–110.
Respectfully yours,
Jewgeni
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