Although the exact electrolytic composion for present day lithium ion batteries (LIBs) may differ among different scenarios, the electrolytes usually employ a mixture of alkyl carbonates such as ethylene carbonate (EC)), dimethyl carbonate (DMC)) and lithium conducting salts (e.g., LiPF 6 ) . Neverthless, alkyl carbonates are flammable, and this has been the main cause of safety concerns to the LIB technology . For these reasons, therefore, there have been considerable research efforts to mitigate those safety concerns, and to design alternative electrolyte compositions with improved thermal stability that would be able to work in a broader operative temperature range . The primary design concept in electrolyte engineering involves balancing conflicting physicochemical properties such as low viscosity with high conductivity, and low charge transfer resistance with electrode passivation . The LIB electrolyes constitute mixtures of solvents with high (e.g. EC ε ∼ 90 at 40°C) and low (DMC ε ∼ 3.1 at 25°C) dielectric constants which have distinct roles in the electrolyte . The linear carbonates (e.g. DMC) serve to mitigate the viscosity and lower the melting point. The cyclic carbonates (e.g. EC), on the other hand, have high dielecric constants which can easily dislove the lithium salts, which eventually solvates the cations and anions enabling fast mobility of the Li + ions between the electrodes . Despite large variation in the magnitude of their dielectric constants, both cyclic and linear carbonates actively participate in forming the lithium solvation sheath . For these reasons, therefore, EC is mixed with other linear carbonates such as di-ethyl, di-methyl, or ethyl-methyl carbonate, thus forming a liquid mixture with good polar characteristics.