Solvent and salt effect on Lithium ion solvation and contact ion pair formation in organic carbonates: a quantum chemical perspective

TL;DR

This study uses quantum chemical calculations to explore how solvents and salts influence lithium ion solvation and contact ion pair formation in organic carbonate electrolytes, shedding light on ionic conductivity mechanisms.

Contribution

It provides detailed insights into the molecular-scale effects of solvent composition and salt presence on lithium ion solvation structures and contact ion pair formation.

Findings

Dimethyl carbonate increases dipole moments of solvation clusters.

Contact ion pair formation reduces the number of carbonate molecules coordinating Li+.

Solvent and salt effects influence ionic conductivity in electrolytes.

Abstract

Quantum chemical calculations have been employed to investigate the solvation of lithium cations in ethylene carbonate/propylene carbonate and propylene carbonate/dimethyl carbonate mixed electrolytes. The impact of the presence of the counteranion on the solvation of Li+ in pure propylene carbonate and dimethyl carbonate was also studied. The calculations revealed small free-energy changes for the transitions between different preferred structures in mixed solvents. This implies that transitions between distinct local arrangements can take place in the mixtures. The addition of dimethyl carbonate causes a significant increase of the dipole moment of solvation clusters, indicating important molecular-scale modifications when dimethyl carbonate is used as a co-solvent. The presence of an anion in the solvation shell of Li+ modifies the intermolecular structure comprising four carbonate molecules in dilute solutions, allowing only two carbonate molecules to coordinate to Li+. The bidentate complexation of Li+ with the anion electron donor atoms, however, maintains the local tetrahedral structure on interatomic length scales. The neutralization of the solvation shell of Li+ due to contact ion pair formation and the consequent implications on the underlying mechanisms provide a rational explanation for the ionic conductivity drop of electrolyte solutions at high salt concentrations.