Thermodynamically Stable Cationic Dimers in Carboxyl-Functionalized Ionic Liquids: The Paradoxical Case of "Anti-Electrostatic" Hydrogen Bonding.

We show that carboxyl-functionalized ionic liquids (ILs) form doubly hydrogen-bonded cationic dimers (c=c) despite the repulsive forces between ions of like charge and competing hydrogen bonds between cation and anion (c-a). This structural motif as known for formic acid, the archetype of double hydrogen bridges, is present in the solid state of the IL 1-(carboxymethyl)pyridinium bis(trifluoromethylsulfonyl)imide [HOOC-CH-py][NTf]. By means of quantum chemical calculations, we explored different hydrogen-bonded isomers of neutral (HOOC-(CH)-py)(NTf), single-charged (HOOC-(CH)-py)(NTf), and double-charged (HOOC- (CH)-py) complexes for demonstrating the paradoxical case of "anti-electrostatic" hydrogen bonding (AEHB) between ions of like charge. For the pure doubly hydrogen-bonded cationic dimers (HOOC- (CH)-py), we report robust kinetic stability for = 1-4. At = 5, hydrogen bonding and dispersion fully compensate for the repulsive Coulomb forces between the cations, allowing for the quantification of the two equivalent hydrogen bonds and dispersion interaction in the order of 58.5 and 11 kJmol, respectively. For = 6-8, we calculated negative free energies for temperatures below 47, 80, and 114 K, respectively. Quantum cluster equilibrium (QCE) theory predicts the equilibria between cationic monomers and dimers by considering the intermolecular interaction between the species, leading to thermodynamic stability at even higher temperatures. We rationalize the H-bond characteristics of the cationic dimers by the natural bond orbital (NBO) approach, emphasizing the strong correlation between NBO-based and spectroscopic descriptors, such as NMR chemical shifts and vibrational frequencies.