Bulk boron, which is characterized by 3D cage-like structural features, is a refractory material. [1,2] However, 3D cage structures were suggested to be unstable for small boron clusters, and planar or quasi-planar structures have been proposed instead. [3][4][5] Experimental studies combined with high-level calculations have shown that small boron cluster ions are planar up to at least B 20 À , [6][7][8][9][10] whereas B n + ions have been found to be planar up to n = 16.[11] The chemical bonding in the planar boron clusters has been found to be quite remarkable; [6][7][8][9] in addition to the strong and localized bonding in the circumferences, there are two types of delocalized bonding-the in-plane s and the out-of-plane p bonding, each of which follows the (4 N + 2) Hückel rule for aromaticity. In particular, systems with six s and six p electrons (N = 1) are doubly aromatic, and give rise to highly symmetric planar clusters, such as B 8 2À and B 9 À , which each contain a central B atom and a B 7 and B 8 monocyclic ring, respectively.[6] In the D 7h B 8 2À and D 8h B 9 À molecular wheels, each B atom in the circumference contributes two electrons to the B-B peripheral covalent bonds and one electron to the delocalized bonds, whereas the central B atom contributes all its valence electrons to the delocalized bonds. These novel bonding situations suggest that other atoms with appropriate numbers of valence electrons and sizes may be able to replace the central boron atom to produce MB n -type clusters. [12] Hexagonal, heptagonal, and octagonal CB n -type clusters have been proposed from theoretical calculations as examples of hexa-, hepta-, and octacoordinate planar carbons. [13][14][15] However, photoelectron spectroscopy (PES) studies showed that carbon occupies the peripheral position in such clusters rather than the center, [16,17] because C is more electronegative than B and thus prefers to participate in localized two-center-two-electron (2 c-2 e) s bonding, which is possible only at the circumference of the wheel structure. Transition-metal atoms are better suited for the central position in the MB n clusters, as these metals favor participation in delocalized bonding at the center over localized bonding at the periphery. For an MB n cluster, the electronic requirement for the central atom is x = 12 À n or x = 12 À n À k for an MB n kÀ anion, where x is the valence of the transitionmetal atom M, in order to satisfy the peripheral BÀB s bonding and the s and p Hückel aromaticity for N = 1. Indeed, all 3d transition-metal atoms have been tested computationally for the MB n -type hypercoordinate complexes. [18][19][20][21] Two complexes, namely CoB 8 À and FeB 9 À , in which the Co and Fe atoms are trivalent and divalent, respectively, were found to be closed-shell global minima, in agreement with our electronic design principle.We have focused our experimental efforts on transitionmetal-doped boron clusters that involve Group 8 (Fe, Ru, Os) and 9 (Co, Rh, Ir) elements. The experiments were carried out usi...