Chemical bonding is fundamental to all areas of chemistry as it dictates molecular structure, stability, and reactivity, influencing diverse fields from organic synthesis and catalysis to materials science and biochemistry. 1 A deep understanding of bonding enables the rational design of new molecules and materials with tailored properties, impacting advancements in drug discovery, energy storage, and nanotechnology. Covalent or donor-acceptor bonding, as defined by IUPAC, involves a region of accumulated electron density between nuclei, arising from electron sharing. Covalent bond energies typically span 40 to 150 kcal mol -1 for single bonds involving main block elements, with bond distances generally ranging from 0.9 to 2.0 Å, depending on the size and electronegativity of the bonded atoms. Advanced quantum chemical investigations have illuminated the nature of bonding between atoms or fragments A and B through analysis of the electronic wavefunction, providing invaluable insights into molecular structure and reactivity. A more nuanced and accurate perspective of the chemical bond beyond simple electron sharing acknowledges the synergy of multiple interactions within covalent bonds, including electrostatic attraction, Pauli repulsion, orbital interactions, and dispersion interactions. At the opposite end of the chemical bonding range, we have the intermolecular (commonly referred to as "noncovalent") interactions that often correspond to any interaction that is weaker than covalent bonds but typically present bond strengths below 15 kcal mol -1 . These interactions exhibit a rich diversity and encompass a broad spectrum in their own right, including ionic, 9 hydrogen, 10 halogen, 11 chalcogen, 12 pnictogen, 13 π-interactions, 14 and van der Waals forces (dipole-dipole interactions, dipole-induced dipole interactions, and induced dipole-induced dipole interactions), significantly expanding the chemical bonding landscape. These intermolecular interactions play a crucial role in molecular recognition and are essential for maintaining the structural integrity of biomolecules, supramolecular assemblies, and materials. 17 Recent research has illuminated the nuanced nature of intermolecular interactions and covalent bonds, revealing that their boundaries are not always distinct. For example, it has been shown that traditional intermolecular interactions, such as hydrogen,10 c, 10 e, 10 f chalcogen,12 c and pnictogen bonding,13 can contain a substantial covalent character due to stabilizing donor-acceptor interactions. These strengthened interactions can exhibit bond lengths and energies comparable to traditional covalent bonds, challenging the conventional dichotomy between covalent and noncovalent bonding. Recent studies have also shown that intermolecular interactions can be strengthened to the point where they resemble covalent bonds, blurring the traditional boundaries between these two types of bonding motifs. In this work, we quantum-chemically explore the chemical bonding realm in Lewis acid-base pairs using boron trihalides