Although the phenomenon of electron solvation has been known for at least one and a half centuries, [1,2] explanations of the detailed behavior of solvated electrons in molecular liquids, in particular in metal/ammonia solutions, [1][2][3] have remained controversial. At low concentrations, metal/ammonia solutions behave like electrolytes whereas they undergo a transition to a metallic liquid-heralded by changing their color from blue to bronze-on increasing the metal content. [2,3] Also, adding metal lowers the density of the solution drastically compared to the neat liquid. This is thought to lead to the formation of voids hosting the unbound electrons, [4,5] which percolate at sufficiently high metal content. [6,7] Distinct from this viewpoint is a more chemical perspective [8,9] whereby the solvated electron in ammonia is believed to be some sort of open-shell molecular species and, in the limiting case, even an anionic radical as such. However, with increasing concentration close to saturation the influence of the metal ion cores, particularly their solvation and ion-pair formation, can no longer be neglected. Indeed, recent diffraction data of Li/NH 3 solutions up to 21 mol % metal (21 MPM) clearly demonstrate that they are highly structured over both the short and intermediate length scales.[10] In particular, the studies suggest that these solutions can be constructed from two major structural units: tightly bound [Li(NH 3 ) 4 ] + tetrahedra and empty voids. [10] In addition, inelastic X-ray scattering close to the saturation limit uncovered not only plasmon resonances and strong deviations from the Jellium model of simple metals, but also excitations that are associated with vibrations of these quasimolecular complexes.[11] Finally, the protonic self-diffusion coefficient is nonmonotonic in the liquid state; it first increases with metal concentration before decreasing again on reaching saturation, an observation that is explained in terms of competing influences of electron and ion solvation.[12] Together these novel findings raise the question of how the intricate realspace structure and the delocalized electronic structure are interrelated in the metallic liquid.Unfortunately, known density functionals do not provide the correct structure and energetics of the ammonia-ammonia interactions in that they predict an essentially linear hydrogen bond for the dimer, similar to classical force field models.[13] To cure this deficiency in the description of the solvent the HCTH/407 + functional [13] has been designed for the simulation of ammonia systems. By using HCTH/407 + , a 21-MPM lithium/ammonia solution at 230 K was simulated in terms of 6 Li and 23 NH 3 in a periodic box of 11.314 by diagonalizing the finite-temperature free-energy functional [14,15] iteratively as implemented in CPMD [15,16] to account for metallicity in terms of partially occupied KohnSham orbitals. The orbitals were expanded in plane waves at the G point up to 50 Ry, H and N were represented as usual by one and five valence-electron...