Ad onor-stabilized 1,3-disila-2,4-diazacyclobutadiene presents an exceptionally short nonbonded Si···Si distance (2.23 ), which is as short as that of Si=Si bonds (2.15-2.23 ). Theoretical investigations indicate that there is no bond between the two silicon atoms,a nd that the unusual geometry can be related to as ignificant coulomb repulsion between the two ring nitrogen atoms.T his chemical pressure phenomenon could provide an alternative and superior way of squeezing out van der Waals space in highly strained structures, as compared to the classical physical methods.Two atoms approaching within ad istance shorter than the sum of van der Waals radii, without bonding interactions, results in significant repulsion. High pressure can force molecules to approach each other, thus violating the van der Waals space. [1] Such high compression of molecules,which leads to intermolecular overlaps of molecular orbitals, induces,i ns ome cases,u nique physical phenomena such as metallization of neutral molecules (i.e., O 2 at 95 GPa, SiH 4 at 91 GPa, N 2 Op redicted above 177 GPa). [2][3][4][5] Endohedral confinement of atoms within small cage compounds also leads to unusual nonbonded structures with short internuclear distances. [6] Indeed, two atoms of He in C 60 were predicted to exist as weakly bonded van der Waals complexes,H e 2 @C 60 (see Figure 3a), [7] and asmaller hydrocarbon cage,C 20 H 20 ,can force two He atoms to ah igh-energy structure in which the He···He distance is two times smaller than the van der Waals radius of helium. [8] However under these conditions,i na ny case,n onbonded interatomic distances never approached alength as short as that of acovalent single bond.An exception is the nonbonded Si···Si dihedral distance (2.31 )found in the 1,3-diosiloxane I,and it is even shorter than Si À Si covalent bonds (2.36 ). [9][10][11] Computational calculations have predicted an even shorter Si···Si distance (2.06 )for the related bicyclic molecule II. [12] Theelectronic origin of the exceptionally short nonbonded distances,called a"phantom bond", has been the subject of many experimental and theoretical investigations [13] and several models with particular orbital interactions [unsupported p-bond model, [14,15] s-bridged p-bonding model, [16] and cyclic (n,d,d) delocalization model [17] ]h ave been proposed to explain the unusual geometry of 1,3-disiloxanes.A lternatively,t he ring deformation resulting from the elongation of the O···O diagonal distance arising from the electrostatic repulsion was also considered. [1a] Several related four-membered cyclic compounds (III)a re also known to deform to diamondshaped patterns for the same reason, [18][19][20] although they do not exhibit adiagonal distance shorter than acovalent single bond. [15a, 21] In spite of these theoretical studies,none of them are supported by experimental evidence.The lack of available molecules,o ther than 1,3-disiloxanes,h as limited further discussion. Here we report the synthesis of the phosphinestabilized 1,3-disila-2,4-diazacycl...