S-4(AsF6)(2). AsF3 was prepared by the reaction of sulfur with arsenic pentafluoride in liquid AsF3 (quantitatively) and in anhydrous HF in the presence of trace amounts of bromine. A single-crystal X-ray structure of the compound has been determined: monoclinic, space group P2(1)/c, Z = 4, a = 7.886(1) Angstrom, b = 9.261(2) Angstrom, c = 19.191(3) Angstrom, beta = 92.82(1)degrees, V = 1399.9(4) Angstrom(3), T = 293 K, R-1 = 0.052 for 1563 reflections (I > 2 sigma(I) 1580 total and 235 parameters). We report a term-by-term calculation of the lattice potential energy of this salt and also use our generalized equation, which estimates lattice energies to assist in probing the homopolyatomic cation thermochemistry in the solid and the gaseous states. We find S-4(ASF(6))(2). ASF(3) to be more stable (Delta(f)H degrees[S-4(AsF6)(2). AsF3,c] approximate to -4050 +/- 105 kJ/mol) than either the unsolvated S-4(AsF6)(2) (Delta(f)H degrees[S-4(ASF(6))(2),c] approximate to -3104 +/- 117 kJ/ mel) by 144 kJ/mol or two moles of S2AsF6 (c) and AsF3 (1) by 362 kJ/mol. The greater stability of the S-4(2+) Salt arises because of the greater lattice potential energy of the 1:2 solvated salt (1734 kJ/mol) relative to twice that of the 1:1 salt (2 x 541 = 1082 kJ/mol). The relative lattice stabilization enthalpies of M-4(2+) ions relative to two M-2(+) ions (i.e., in M-4(AsF6)(2) (c) With respect to two M2AsF6 (c) (M = S, Se, and Te)) are found to be 218, 289, and 365 kJ/mol, respectively. Evaluation of the thermodynamic data implies that appropriate presently available anions are unlikely to stabilize M-2(+) in the solid phase. A revised value for Delta(f)H degrees[Se-4(AsF6)(2),c] = -3182 +/- 106 kJ/mol is proposed based on estimates of the lattice energy of Se-4(AsF6)(2) (c) and a previously calculated gasphase dimerization energy of 2Se(2)(+) to Se-4(2+).