In contrast, weak Lewis bases, such as N2, due to extremely weak stabilizing intermolecular interactions, resulting in longbonded and, therefore, weakly bonded adducts. These complexes preserve the near-planar geometry of the Lewis acid because the weakly stabilizing ΔEint cannot compensate for the ΔEstrain required to significantly deform the acid. As a result, the energy minimum van der Waals complex occurs at a longer bond distance where strain energy is minimally destabilizing. Importantly, N2 does not form short-bonded minima because its ΔEint lacks the strength to overcome the destabilizing strain energy at shorter B-N distances. Furthermore, this general trend can be observed in I3B•••N2, which features a shallow, short-bonded minimum in its interaction energy. This adduct highlights the nuanced balance between interaction strength and structural deformation in determining bond characteristics.