Sulfur is the element with the largest number of modifications and usually exists as S n ring molecules; those with n = 6-14, 18, and 20 [1,2] have been structurally characterized. Thermodynamically, the two most stable rings are D 4d S 8 and D 3d S 12 . [1a, 2] In contrast to the rich structural chemistry of elemental sulfur, the coordination chemistry of neutral sulfur molecules is underdeveloped and, to our knowledge, limited to [Ag (S 8 and [Re 2 (m-X) 2 (CO) 6 (S 8 )] (X = Br, I). [4b] The coordination chemistry of the other chalcogens, Se and Te, is also restricted [5a] to few examples including [(OSO)AgSe 6 Ag-(OSO)] 2+ and [(Se 6 Ag + ) n ]. [5b] In agreement with this, the sulfur ring molecules usually undergo redox degradation when treated with transition metal cations, leading to simpler metal (poly-)sulfide complexes, rather than forming coordination compounds. [6] However, Fourier transform ion cyclotron resonance mass spectrometry (FTICR-MS) gas phase investigations of transition metal monocations M + with sulfur vapor (mainly S 8 ) detected strong signals for [MS n ] + complexes (n = 2-4, 6-8, 10, 12, and 14), suggesting that such coordination complexes can exist. [7] However, it remains unclear, if the observed compounds are true coordination compounds of the S n molecule or if M + oxidatively added to the S À S bond, forming a (n + 1)-heterocycle. Recent quantum chemical studies on [MS n ] + complexes (M = Li, Ca, V, Cu) suggested complexation of the metal cation to the ring structures. [8] Another open question from the pioneering mass spectrometric study [7] is whether the [MS n ] + complexes contain a single S n molecule or two (or more) smaller molecules S x and S y (x + y = n). For Ag + and S 8 , the mass spectrum showed two main signals, for [AgS 8 ] + and [AgS 16 ] + , both of which were also fully characterized as [Ag(h 4 -S 8 )] + and [Ag(h 4 -S 8 ) 2 ] + incorporated in the corresponding salts in the solid state, [3] using large and weakly coordinating anions