Strong Lewis bases, such as NH3, enter into a stronger overall interaction, resulting in highly stable adducts because the stabilizing ΔEint dominates over the destabilizing ΔEstrain, even at shorter B-N bond distances. However, this comes at the cost of Please do not adjust margins Please do not adjust margins significant deformation in the Lewis acid, as NH3 induces an unfavorable deformation from the trigonal planar equilibrium geometry earlier along the B-N bond distance. This deformation towards a trigonal pyramidal geometry increases strain energy but is offset by the increasingly stabilizing ΔEint (Figure ), driving the system to adopt a short-bonded minimum. Notably, NH3 does not form a long-bonded minimum because it enters into strongly stabilizing covalent interactions at long interatomic distances with the Lewis acids (Figure ). In general, once the Lewis acid deforms and the interaction becomes sufficiently strong, forming the short-bonded adduct is accessible energetically.