CHELATOR-IN-IONIC LIQUID ELECTROLYTES

Abstract

The invention provides electrolyte compositions including a metal cation, an ionic liquid, and a chelator that coordinates the metal cation. The electrolyte compositions are advantageous as they exhibit increased ion transference, and thus increased total conductivity, relative to a pure ionic liquid electrolyte that coordinates the metal cation. The invention provides a general strategy to control the cation-anion dynamics that govern ionic liquid performance. Electrolytes of the invention may be useful for any suitable purpose, e.g., in primary and secondary batteries, supercapacitors, and solar cells.

Claims

1. An electrolyte comprising a metal cation, an ionic liquid, and a chelator that coordinates the metal cation.

2. The electrolyte of claim 1, wherein the metal cation is selected from the group consisting of Na, Li, K, Ca, Mg, Zn, Ag, Cu, and V.

3. The electrolyte of claim 1, wherein the metal cation is Li.

4. The electrolyte of claim 1, wherein the metal cation is Na.

5. The electrolyte of claim 1, wherein the ionic liquid comprises N-alkylimidazolium, N-alkylipyridinium, N-alkylpyrrolidinium, or N-alkylammonium, N-alkylpiperidinium, alkylphosphonium, N-alkylpyrazinium, or a quaternary amine.

6. The electrolyte of claim 1, wherein the ionic liquid comprises 1-ethyl-3-methylimidazolium (EMIM), 1-butyl-3-methylimidazolium (BMIM), 1-hexyl-3-methylimidazolium (HMIM), or 1-methyl-3-propylimidazolium (MPIM).

7. The electrolyte of claim 1, wherein the ionic liquid comprises EMIM.

8. The electrolyte of claim 1, wherein the ionic liquid comprises a halide, C.sub.1-6 carboxylate, triflate, chlorate, bistriflimide (TFSI.sup.−), bis(fluorosulfonyl)imide (FSI.sup.−), PF.sub.6.sup.−, BF.sub.4.sup.−, or N-alkylsulfate.

9. The electrolyte of claim 8, wherein the ionic liquid comprises triflate.

10. The electrolyte of claim 8, wherein the ionic liquid comprises formate.

11. The electrolyte of claim 1, wherein the chelator is selected from the group consisting of optionally substituted C.sub.8-20 crown ethers, optionally substituted C.sub.8-20 azacrown ethers, optionally substituted C.sub.8-20 thiacrown ethers, optionally substituted C.sub.6-20 podands, optionally substituted calix[n]arenes, and optionally substituted calix[n]crowns, wherein n is from 4-8.

12. The electrolyte of claim 1, wherein the chelator is one of lithium ionophores I-IV and VI-VIII or a species of formula (a) through (m): ##STR00008## ##STR00009## ##STR00010##

13. The electrolyte of claim 1, wherein the chelator is optionally substituted 12-crown-4, optionally substituted 18-crown-6, or optionally substituted 14-crown-4 or an azacrown or thiacrown derivative thereof.

14. The electrolyte of claim 11, wherein the optionally substituted C.sub.6-20 podand is a glyme or an aza- or thia-derivative thereof.

15. The electrolyte of claim 14, wherein the glyme is triglyme.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

[0033] FIGS. 1A-1F: Molecular structure of the ionic liquid cation [EMIM].sup.+ (FIG. 1A), the [TFO].sup.−, [HCOO].sup.−, and [TFSI].sup.− anions (FIGS. 1B, 1C, and 1D, respectively), and the 12-crown-4 (FIG. 1E) and 18-crown-6 (FIG. 1F) molecules.

[0034] FIGS. 2A-2B: Density plots for the Li.sup.+[EMIM].sup.+[TFO].sup.−-12-crown-4 and the Li.sup.+[EMIM].sup.+[HCOO].sup.−-12-crown-4 systems. FIG. 2A shows the absolute density values as a function of temperature and system composition for Li.sup.+[EMIM].sup.+[TFO].sup.−-12-crown-4. FIG. 2B shows the percentage difference at 358K for both chemistries and different compositions. Ensemble uncertainty is always present but not always appreciable on the scale of the plot.

[0035] FIGS. 3A-3D: Radial distribution function (RDF) between Li.sup.+ and oxygen atoms of [TFO].sup.− (FIG. 3A), and Li.sup.+ and oxygen atoms of 12-crown-4 (FIG. 3B). For both FIGS. 3A and 3B, three different compositions are shown. FIGS. 3C and 3D present the differences in RDF between the different compositions in FIGS. 3A and 3B, respectively. In all curves, the shaded area highlights the standard deviation among the ensemble of four structures for each composition.

[0036] FIGS. 4A-4D: Clustering between Li.sup.+ atoms and [TFO].sup.− molecules at different system compositions, i.e., different number n of added 12-crown-4 molecules. FIG. 4A is n=0, and FIG. 4B is n=150. Inset FIGS. 4C and 4D show an anion-only (C.sub.1;A.sub.4).sup.−3 cluster and an ionophore-disrupted (C.sub.1;A.sub.1).sup.0 cluster from an MD snapshot, respectively.

[0037] FIGS. 5A-5B: Persistence of the Li.sup.+ coordination (exclusively oxygen atoms from [TFO].sup.−) as a function of time. FIG. 5A shows the breakdown in oxygen coordination for three different compositions. FIG. 5B shows the dependence on the persistence of Li.sup.+ coordination on the number of 12-crown-4 molecules.

[0038] FIGS. 6A-6D: Summary of the transport for all the compositions studied. FIG. 6A shows the total conductivity κ. FIG. 6B shows the Li.sup.+ transference number t.sup.+.sub.Li. FIG. 6C shows Li.sup.+ conductivity computed as κ.sub.Li=κ.Math.t.sup.+.sub.Li. FIG. 6D shows the Li.sup.+ effective charge.

[0039] FIG. 7: Comparison of transport properties with 12-crown-4 and triglyme. FIG. 7 shows total conductivity κ (left y-axis) and transference number (right y-axis) against O.sup.Ionophore to Li ratio (x-axis).

DETAILED DESCRIPTION OF THE INVENTION

[0040] The invention provides electrolyte compositions containing a metal cation, an ionic liquid (IL), and a chelator, e.g., a cyclic chelator, that coordinates the metal cation. The electrolyte compositions of the invention are advantageous as they exhibit increased ion transference, and thus increased total conductivity, relative to a pure ionic liquid electrolyte that coordinates the metal cation. In the case of lithium, the addition of chelator effectively helps in “breaking” the Li.sup.+-anion clusters by competing for the lithium coordination and causing positively-charged clusters as well as free Li.sup.+ atoms to appear in the systems. This is in stark contrast with the results from the pure IL-based electrolytes, where all clusters contained a greater number of anion than cation, and no anion-free lithium was found. We further found that not only the overall cluster population is, on average, less asymmetrical, but also clusters are less persistent in time. In other words, the persistence of a given lithium coordination cage due to IL anions is progressively reduced the more chelator molecules are added to the systems, signaling a faster decoupling of the anion-cation motions. We also observed that all transport properties are improved by adding the chelator, as compared to the reference system with no added chelator. Of particular importance is the result showing increasing transference number when more chelators are added, to the point that even the sign of the transference number can be inverted from negative to positive, therefore significantly increasing the lithium contribution to the total conductivity. This invention provides a general strategy to control the cation-anion correlated dynamics that can be leveraged to improve the transport properties of IL-based electrolytes, providing improved designs of metal-salt/ionic liquid electrolytes.

[0041] Electrolytes of the invention may be employed for any suitable purpose, e.g., in primary and secondary batteries, supercapacitors, and solar cells.

[0042] Metal cations suitable for the electrolyte compositions of the present invention include, but are not limited to, Na, Li, K, Ca, Mg, Zn, Ag, Cu, and V. Exemplary metal cations are Li and Na.

[0043] Ionic liquids, which are salts in a liquid state, include a weakly associated cation and anion pair. Ionic liquid cations useful for the electrolyte compositions of the present invention include, but are not limited to, N-alkylimidazolium, N-alkylipyridinium, N-alkylpyrrolidinium, or N-alkylammonium, N-alkylpiperidinium, alkylphosphonium, N-alkylpyrazinium, and quaternary amines. An exemplary class of ionic liquids include the N-alkylimidazolium series, e.g., 1-ethyl-3-methylimidazolium (EMIM), 1-butyl-3-methylimidazolium (BMIM), 1-hexyl-3-methylimidazolium (HMIM), or 1-methyl-3-propylimidazolium (MPIM). An exemplary N-alkylimidazolium ionic liquid for electrolyte compositions of the present invention is EMIM. FIG. 1A shows the molecular structure of [EMIM].sup.+.

[0044] Ionic liquid anions useful for the electrolyte compositions of the present invention include, but are not limited to, halides (e.g., Cl.sup.−, Br.sup.−, F.sup.−, or I.sup.−), C.sub.1-6 carboxylates (e.g., formate or acetate), triflate (CF.sub.3SO.sub.3.sup.−, TFO.sup.−), chlorate (ClO.sub.3.sup.−), bistriflimide ([(CF.sub.3SO.sub.2).sub.2N].sup.−, TFSI.sup.−), bis(fluorosulfonyl)imide ([(SO.sub.2F).sub.2N].sup.−, FSI.sup.−), PF.sub.6.sup.−, BF.sub.4.sup.−, or N-alkylsulfate (e.g., lauryl sulfate or laureth sulfate). Exemplary ionic liquid anions are triflate and formate. FIGS. 1B-1D show molecular structures of the [TFO].sup.− (FIG. 1B), [HCOO].sup.− (FIG. 1C), and [TFSI].sup.− (FIG. 1D) anions.

[0045] Chelators useful for electrolyte composition of the present invention include, but are not limited to, optionally substituted C.sub.8-20 crown ethers, optionally substituted C.sub.8-20 thiacrown ethers, optionally substituted C.sub.8-20 azacrown ethers, optionally substituted C.sub.6-20 podands (e.g., ethylene glycol diethyl ethers or ethylene glycol dimethyl ethers, e.g., diglyme, triglyme, tetraglyme, etc., or an aza- or thia-derivative thereof), optionally substituted calix[n]arenes, and optionally substituted calix[n]crowns, where n is from 4-8.

[0046] Examples of chelators include optionally substituted 12-crown-4, optionally substituted 14-crown-4, optionally substituted 18-crown-6, and azacrown and thiacrown derivatives thereof (i.e., where one or more of the ring oxygens is replaced by N or S), e.g., 12-crown-4, 14-crown-4, or 18-crown-6.

[0047] In some embodiments, the chelator is one of the series of lithium ionophores I-IV or VI-VIII:

##STR00004##

[0048] In some embodiments, the chelator is one of formulas (a) through (m):

##STR00005## ##STR00006## ##STR00007##

[0049] Exemplary electrolyte compositions of the present invention include Li.sup.+-[EMIM].sup.+[TFO].sup.−-12-crown-4; Li.sup.+-[EMIM].sup.+[HCOO].sup.−-12-crown-4; Li.sup.+-[EMIM].sup.+[TFSI].sup.−-12-crown-4; and Li.sup.+-[EMIM].sup.+[TFO].sup.−-18-crown-6.

[0050] The metal cation, e.g., lithium or sodium, may be present at any suitable molar ratio with the chelator. In particular, the molar ratio of the metal cation to the chelator may range from 0.01:1 to 1:0.01, e.g., 0.1:1 to 1:0.1, 0.5:1 to 1:0.5, or 0.9:1 to 1:0.9, such as 1:1. With respect to other components in the electrolyte, the metal cation, e.g., lithium or sodium, may be present in any suitable concentration, e.g., 0.01 to 10 M or 0.1 to 4 M. In embodiments, the metal cation mole fraction in the electrolyte may be at most 0.8, e.g., at most 0.7, 0.6, 0.5, 0.4, 0.3, 0.2, 0.1 or 0.05.

EXAMPLES

Example 1—Structure Generation

[0051] We investigated four distinct polymer-in-ionic-liquid systems: Li.sup.+-[EMIM].sup.+ with 1. [TFO].sup.−-12-crown-4, 2. [HCOO].sup.−-12-crown-4, 3. [TFSI].sup.−-12-crown-4, and 4. [TFO].sup.−-18-crown-6. To create a low-density non-overlapping initial structure, we placed Li.sup.+, [EMIM].sup.+, [TFO].sup.− (or [HCO].sup.−/[TFSI].sup.−), and 12-crown-4 (or 18-crown-6), as shown in FIGS. 1A-1F, randomly on the vertices of a three-dimensional cubic grid..sup.19,20,22

[0052] We focus on the molar fraction of Li.sup.+[ANION].sup.− equal to 0.5, which corresponds to the composition with the most negative t.sup.+.sub.Li for these chemistries..sup.19 To such systems we add n ionophore molecules, n ranging from 0 to 150. For every composition, we generated four independent IL-lithium-salt-ionophore structures which we then used to compute averages and uncertainties as standard deviations among such ensembles.

Molecular Dynamics

[0053] All molecular dynamics (MD) simulations have periodic boundary conditions and were performed using the Large-scale Atomic/Molecular Massively Parallel Simulator (LAMMPS)..sup.23 We adopt the AII-Atom Optimized Potentials for Liquid Simulation (OPLS-AA) force-field to model the atomic interactions..sup.24,25 Following the established practice in the ionic liquid literature, in this work we rescale the point charges assigned to every atomic species, to 80% of the original value, with the aim to mimic the average charge screening due to polarization, and charge transfer effects..sup.26-28 The cost-effective charge-rescaling is adopted in the literature in favor of polarizable models, as for instance self-consistent inducible dipoles.sup.29 or Drude oscillators,.sup.30 since their positive gains are counterbalanced by a significant increase in computational cost and difficulty in parameterization. We chose OPLS-AA parameters and charge rescaling for the ionic liquid species..sup.26,31,32 For consistency, we used the same choice of force-field for the ionophores, and the parameters were obtained from the official Jorgensen OPLS-AA distribution..sup.33-35 We used a timestep of t=1:0 fs in the velocity-Verlet algorithm to evolve the equation of motions. Nose-Hoover barostat (1000 t coupling) and thermostat (100 t coupling) enforced pressure and temperature, respectively..sup.36-38 Following the structure generation, to overcome local energy barriers in search of lower energy minima, we adopted an equilibration procedure comprising a set of energy minimizations, compression/decompression, and annealing stages..sup.19,20

[0054] We present a summary of the number of molecules and total number of atoms for every composition in Tables 1-4, with the ionic liquid OPLS-AA parameters taken from ref. 32 and the ionophore OPLS-AA parameters takes from refs. 33-35. The stages used to equilibrate the generated structures are described in Table 5.

TABLE-US-00001 TABLE 1 Total number of atoms and molecules for the Li.sup.+[EMIM].sup.+[TFO].sup.−-12-crown-4 system. X.sub.LiTFO Li.sup.+ [EMIM].sup.+ [TFO].sup.− 12-crown-4 Total # atoms 0.5 97 97 194 0 3492 25 4192 50 4892 75 5592 100 6292 125 6992 150 7692

TABLE-US-00002 TABLE 2 Total number of atoms and molecules for the Li.sup.+[EMIM].sup.+[HCOO].sup.−-12-crown-4 system. X.sub.LiHCOO Li.sup.+ [EMIM].sup.+ [HCOO].sup.− 12-crown-4 Total # atoms 0.5 125 125 250 0 3500 25 4200 50 4900 75 5600 100 6300 125 7000

TABLE-US-00003 TABLE 3 Total number of atoms and molecules for the Li.sup.+[EMIM].sup.+[TFSI].sup.−-12-crown-4 system. X.sub.LiTFSI Li.sup.+ [EMIM].sup.+ [TFSI].sup.− 12-crown-4 Total # atoms 0.5 70 70 140 0 3500 25 4200 75 5600 125 7000

TABLE-US-00004 TABLE 4 Total number of atoms and molecules for the Li.sup.+[EMIM].sup.+[TFO].sup.−-18-crown-6 system. X.sub.LiTFO Li.sup.+ [EMIM].sup.+ [TFO].sup.− 18-crown-6 Total # atoms 0.5 70 70 140 0 3492 25 4542 75 6642

TABLE-US-00005 TABLE 5 Stages used to equilibrate all the initial structures. The 13 stages are sequentially run. During heating/cooling and compression/decompression stages, the initial/final temperature/pressure is indicated in the table as “Initial .fwdarw. Final.” The change in temperature/pressure is performed at a constant rate over the entire duration of the stage. Stage Stage duration (ns) Total time (ns) Temp. (K) Pressure (MPa) Energy Minimization — — — — NVT 0.50 0.50 — — Energy Minimization — — — — NPH (compression) 0.50 1.00 — 0 .fwdarw. 40 NPT 0.40 1.40 278 40 NPT (decompression) 0.60 2.00 278 40 .fwdarw. 0  NPT (heating) 0.40 2.40 278 .fwdarw. 368 0 .fwdarw. 10 NPT (cooling) 0.40 2.80 368 .fwdarw. 278 10 .fwdarw. 0.1  NPT (compression) 0.30 3.10 278 0.1 .fwdarw. 40   NPT (decompression) 0.30 3.40 278 40 .fwdarw. 0.1  NVT 0.80 4.20 278 — NPT (heating) 1.00 5.20 278 .fwdarw. 358 0.1 NPT 2.00 7.20 358 0.1

Example 2—Transport Properties

[0055] To compute transport properties, we evolved every system for 60 ns in the canonical ensemble. The volume was kept equal to that of the last stage of the equilibration routine, and the temperature was maintained constant at 358K. Throughout the simulations the position of the center of mass of the three charged species in a given structure was recorded every 10 kδt=10 ps for post-processing. We analyzed the trajectories using the position correlation function modification.sup.20 of the Wheeler-Newman approach,.sup.39 which yields transport properties that account for the intra- and inter-species correlation. While it required longer trajectories to converge (as compared to standard mean squared displacement method), the adoption of fully correlated transport theory was a vital step to uncover transport anomalies such as a negative t.sup.+.sub.Li, which are otherwise impossible to find with a dilute solution theory approach..sup.19,20 The center of mass of the entire system is our choice of reference position, as there was no single species that could be treated as a “solvent.” The effective lithium charge, q.sup.ε.sub.Li hereafter, was computed as shown in Eq. 1..sup.19

[00001]$\begin{array}{cc}{q}_{\mathrm{Li}}^{ϵ}=\mathrm{Sign}\left(t_{\mathrm{Li}}^{+}\right)\sqrt{\frac{K_B{T}_K^{\mathrm{UC}}.Math.t_{\mathrm{Li}}^{+}.Math.}{e^2{n}_{\mathrm{Li}}{D}_{\mathrm{Li}}}}& \left(1\right)\end{array}$

Example 3—Density and Radial Distribution Functions

[0056] We methodically characterized the Li.sup.+[EMIM].sup.+[TFO].sup.− and Li.sup.+[EMIM].sup.+[HCOO].sup.− systems by computing the density at different temperature values ranging from 278K to 358K at steps of 10K. FIGS. 2A-2B summarize the density vs. temperature results for Li.sup.+[EMIM].sup.+[TFO].sup.−-12-crown-4 (FIG. 2A), and the density percent difference vs. system composition at 358K (FIG. 2B). We observed a decrease in the density for the [TFO].sup.− system with the addition of 12-crown-4 molecules as compared to the pure Li.sup.+-salt-ionic liquid system. From n=25 to n=150 the density decreases further, at a progressively slower rate. The same qualitative trend of decreasing density with the addition of 12-crown-4 molecules was observed for [HCOO].sup.−, albeit to a different extent.

[0057] FIGS. 3A-3D show the Li.sup.+-oxygen (from either [TFO].sup.− (FIGS. 3A, 3C) or 12-crown-4, (FIGS. 3B, 3D)) radial distribution function (RDF) to explore the structural equilibrium properties of the [TFO].sup.− system. FIGS. 3A and 3B show the RDF curves for three different electrolyte compositions, while the FIGS. 3C and 3D shows the differences in the RDFs. For all curves, the shaded area indicates the uncertainty, computed as the standard deviation on the ensemble of structures sharing the same composition (and propagated in the case of the bottom row). We observed that even for large numbers of inserted 12-crown-4 molecules, the location of the RDF extrema (both peaks and minima) remained substantially unaltered, indicating minimal structural changes. In particular, the first RDF minima, necessary for the Li.sup.+[TFO].sup.− cluster analysis, was found at approximately 2.85 Å. Looking at the RDF differences in FIGS. 3C and 3D, we observed that the intensity of the peak corresponding to [TFO].sup.−-oxygen coordination is reduced for increasing number of added 12-crown-4 molecules. This observation indicated that the 12-crown-4 molecules compete with the [TFO].sup.− anion molecules to coordinate the lithium atoms. Consequently, we expect the 12-crown-4 molecules to profoundly alter the Li.sup.+[TFO].sup.− clustering and, ultimately, have an impact on the transport properties of such systems.

Example 4—Li.SUP.+.-[TFO].SUP.− Clustering

[0058] The molecular resolution of our simulations allowed us to analyze the Li.sup.+[TFO].sup.− cluster population, and thereby help understand the role of the 12-crown-4 molecules in breaking the Li.sup.+-anion coordination. After the equilibration routine, the structures were evolved for a total of 6.0 ns in the canonical ensemble, where the volume was set to the value obtained from the last stage of the equilibration routine, and temperature was 358K. Snapshots of the structures containing the positions of all atoms were saved every 100 δt=0.1 ps for post-processing. We analyzed clusters of Li.sup.+ cations and [TFO].sup.− anions by looking at their spatial correlation during the simulation, i.e., agglomerates where anions and cations are located nearby..sup.19,20 Li.sup.+ and [TFO].sup.− were iteratively grouped based on a threshold distance of 2.85 Å between Li.sup.+ and oxygen atoms from [TFO].sup.−, corresponding to the first minima of their RDF. With (C.sub.i;A.sub.j).sup.i−j we denote a cluster comprising i Cations (Li.sup.+), j Anions ([TFO].sup.−), and charge i−j. Therefore, with “positive cluster” and “negative cluster” we refer to configurations with i>j and i<j, respectively, with i and j integers greater or equal to zero. At every snapshot and for the four structures sharing the same composition, the type and number of appearances of every cluster was saved. The final reported cluster frequency is the ratio between the number of cluster appearances and the total number of appearances of all clusters.

[0059] In FIGS. 4A-4D, we present a graphical summary of our findings for Li.sup.+[EMIM].sup.+[TFO].sup.− with: 0 (FIG. 4A), and 150 (FIG. 4B) added 12-crown-4 molecules. The oblique, solid lines mark i=j, i.e., where neutral clusters with equal number of anions and cations would lie, and the vertical, dashed lines indicate the total number of Li.sup.+ atoms in the systems, effectively acting as an upper bound to the number of cations in the clusters. As previously observed,.sup.19 as shown in FIG. 4A, the system organizes in either small clusters or a single, large cluster comprising nearly all Li.sup.+ atoms. Importantly, we notice that all clusters lie above the i=j line, indicating that all clusters are asymmetrical in nature, i.e., contain a greater number of anions than cations. The most common cluster composition is (C.sub.1;A.sub.4).sup.−3 with a total frequency of appearance of 15%.

[0060] The addition of 12-crown-4 molecules profoundly alters the coordination landscape, as shown in FIG. 4B. First, we observed that the 12-crown-4 molecules prevented the formation of a single cluster including all Li.sup.+ atoms in the system, as the right panel of FIG. 4B is not populated. Second, on average the cluster population is closer to the i=j line, indicating neutral clusters, and, in particular, the most frequent cluster is now (C.sub.1;A.sub.1).sup.0 with 59% of recorded appearances. Third, positively-charged clusters are now possible and account for a non-trivial fraction of the total cluster population; for example, (C.sub.2;A.sub.1).sup.1 appears at 4%. Lastly, the system now contains 12% of (C.sub.1;A.sub.0).sub.1, i.e., Li.sup.+ atoms that are completely not coordinated by any oxygen atoms from [TFO].sup.−. The cluster analysis provides an instantaneous picture of the Li.sup.+ coordination, i.e., without considering time evolution and dynamics of the clusters, thus we now investigate the persistence of the [TFO].sup.− coordination.

Example 5—Persistence of Li.SUP.+ Coordination

[0061] We want to study: 1. the persistence of the Li.sup.+ coordination by the oxygen atoms from [TFO].sup.−, and 2. the relative contribution to the overall Li.sup.+ coordination by the [TFO].sup.− and the 12-crown-4 molecules. Here, we use the same MD trajectories as in the clustering analysis as in Example 4. The persistence for a lithium i, (t), is defined as the fraction of oxygen atoms (from [TFO].sup.−) coordinating (i.e., within 2:85 Å) a Li.sup.+ atom at time t that remains the same as at time 0, written as:.sup.20,40,41

[00002]$\begin{array}{cc}{𝒫}^i\left(t\right)=\frac{G_0^i.Math.G_t^i}{.Math.G_0^i.Math.}& \left(2\right)\end{array}$

where G.sup.i.sub.0 and G.sup.i.sub.t are the sets containing the indices of the oxygen atoms coordinating Li.sup.+ i at time 0 and t, respectively.

[0062] FIGS. 5A-5B show the persistence value over time, averaged over all the Li.sup.+ atoms and structures with same concentration, for three different compositions. For all systems, the persistence starts at one, and it decays over time, meaning that the specific oxygen atoms contributing to the coordination change over time. We highlight that this behavior is different than in polymer electrolyte systems, where the cation coordination cage can remain unaltered over hundreds of nanoseconds..sup.42 Additionally, the persistence shows an interesting dependence on the number of added 12-crown-4 molecules. As is shown in FIG. 5B, going from n=0 to n=150, the persistence has a sharper initial drop, indicating that Li.sup.+ coordination is renewed at a faster rate. Thus, the addition of 12-crown-4 molecules not only reduces the asymmetry in the Li.sup.+[TFO].sup.− cluster population, but also decreases the fraction of time lithium atoms spend coordinated by the same anion molecules. In other words, the competition between 12-crown-4 molecules and [TFO].sup.− anion for coordinating Li.sup.+ atoms reduced the cation-anion correlation. This result is promising for improving the transport properties, as a reduced Li.sup.+-[TFO].sup.− correlation should result in an increase in the lithium transference number..sup.19-21 Lastly, the coordination histograms shown in FIG. 5A reinforce the observation that the 12-crown-4 molecules compete with the [TFO].sup.− anions to coordinate lithium.

Example 6—Transport Properties

[0063] FIGS. 6A-6D summarize the transport properties for all four ionic liquid-based electrolyte systems investigated here as a function of the number n of added ionophore molecules. The panels show:

[0064] (A) The total conductivity κ. For the Li.sup.+[EMIM].sup.+[TFO].sup.− systems we observe that the total conductivity increases by ˜80% over the range of added 12-crown-4 molecules. On the other hand, we observe that for the Li.sup.+[EMIM].sup.+[HCOO].sup.− systems the total conductivity remains, within uncertainty, largely unaltered by the 12-crown-4 addition. Similar considerations apply to the other two systems. Whether the more significant decrease in density for Li.sup.+[EMIM].sup.+[TFO].sup.− than for Li.sup.+[EMIM].sup.+[HCOO].sup.− explains the observed difference in total conductivity is unclear. Since the focus of this work is on the decoupling of the Li+-anion motions, the origin of the observed differences in conductivity will be uncovered in a future study.

[0065] (B) The lithium transference number t.sup.+.sub.Li. t.sup.+.sub.Li measures the relative contribution of the cation of interest to the total conductivity. We observed that the addition of ionophore molecules has a surprising, profound, and positive consequence on t.sup.+.sub.Li. The lithium transference number linearly increases the more ionophore molecules are added to the systems, even becoming positive in the case of Li.sup.+[EMIM].sup.+[TFO].sup.− (with both ionophores, circles and pointing-down triangles from FIGS. 6A-6D) and Li.sup.+[EMIM].sup.+[TFSI]+ (diamonds from FIGS. 6A-6D). This result corroborates the importance of decoupling the cation and anion motion in order to increase t.sup.+.sub.Li, and suggests a general recipe to increase the fraction of conductivity carried by Li.sup.+.

[0066] (C) The conductivity carried by lithium computed as κ.Math.t.sup.+.sub.Li. It is important to highlight that the charge/discharge rates of the electrolyte are controlled by the trade-off between t.sup.+.sub.Li and total ionic conductivity: a high t.sup.+.sub.Li with a low conductivity is as technologically impractical as the opposite. As a consequence, κ.sub.Li is often regarded as a good practical indicator for electrolyte optimization. Since, as a function of added ionophore molecules, the total conductivity is either not affected or increased, and the lithium transference number increased, also κ.sub.Li shows an overall increasing trend.

[0067] (D) The lithium effective charge q.sup.ε.sub.Li calculated as in Eq. 1. The lithium atom at the center of a given cluster can diffuse together with any number ranging from all to none of the surrounding coordinating anions. Thus, q.sup.ε.sub.Li provides an average picture, both over time and Li.sup.+ atoms, of the charge carried by the lithium-containing clusters. We observe an increase in q.sup.ε.sub.Li for all systems, albeit more modest in Li.sup.+[EMIM].sup.+[HCOO].sup.− than in Li.sup.+[EMIM].sup.+[TFO].sup.−, for instance. We attribute this to lower increase in transference number, and to the approximately constant density, implying that the lithium number density, n.sub.Li in Eq. 1, also is maintained approximately constant. Finally, we note that q.sup.ε.sub.Li for the Li.sup.+[EMIM].sup.+[TFO].sup.− (12-crown-4, n=150) system is still far from unity, indicating Li.sup.+ movement is not yet completely decoupled from that of the anion, as also shown by t.sup.+.sub.Li being far equal to unity as shown in FIG. 6B.

[0068] FIG. 7 shows the transport properties of Li.sup.+[TFSI].sup.− with a podand (triglyme) compared to Li.sup.+[TFSI].sup.− with a crown ether with equal number of O atoms (12-crown-4) across an increasing series of O.sup.Ionophore to Li ratios. The triglyme system shows both greater total conductivity κ and lithium transference number t.sup.+.sub.Li than the equivalent crown ether. The gap widens with increasing O.sup.Ionophore to Li ratio.

REFERENCES

[0069] (1) Rogers, R. D.; Seddon, K. R. Ionic liquids-solvents of the future? Science 2003, 302, 792-793.

[0070] (2) Welton, T. Room-temperature ionic liquids. Solvents for synthesis and catalysis. Chemical reviews 1999, 99, 2071-2084.

[0071] (3) Olivier-Bourbigou, H.; Magna, L.; Morvan, D. Ionic liquids and catalysis: Recent progress from knowledge to applications. Applied Catalysis A: General 2010, 373, 1-56.

[0072] (4) van Rantwijk, F.; Sheldon, R. A. Biocatalysis in ionic liquids. Chemical reviews 2007, 107, 2757-2785.

[0073] (5) Wasserscheid, P.; Keim, W. Ionic liquids: new solutions for transition metal catalysis. Angewandte Chemie International Edition 2000, 39, 3772-3789.

[0074] (6) Armand, M.; Endres, F.; MacFarlane, D. R.; Ohno, H.; Scrosati, B. Materials for Sustainable Energy: A Collection of Peer-Reviewed Research and Review Articles from Nature Publishing Group; World Scientific, 2011; pp 129-137.

[0075] (7) Dokko, et al. Solvate ionic liquid electrolyte for Li—S batteries. Journal of The Electrochemical Society 2013, 160, A1304-A1310.

[0076] (8) Xu, K. Nonaqueous liquid electrolytes for lithium-based rechargeable batteries. Chemical reviews 2004, 104, 4303-4418.

[0077] (9) Zakeeruddin, S. M.; Grätzel, M. Solvent-free ionic liquid electrolytes for mesoscopic dye-sensitized solar cells. Advanced Functional Materials 2009, 19, 2187-2202.

[0078] (10) MacFarlane, D. R.; Tachikawa, N.; Forsyth, M.; Pringle, J. M.; Howlett, P. C.; Elliott, G. D.; Davis, J. H.; Watanabe, M.; Simon, P.; Angell, C. A. Energy applications of ionic liquids. Energy & Environmental Science 2014, 7, 232-250.

[0079] (11) Kim, T. Y.; Lee, H. W.; Stoller, M.; Dreyer, D. R.; Bielawski, C. W.; Ruoff, R. S.; Suh, K. S. High-performance supercapacitors based on poly (ionic liquid)-modified graphene electrodes. ACS nano 2010, 5, 436-442.

[0080] (12) Chen, Y.; Zhang, X.; Zhang, D.; Yu, P.; Ma, Y. High performance supercapacitors based on reduced graphene oxide in aqueous and ionic liquid electrolytes. Carbon 2011, 49, 573-580.

[0081] (13) Balducci, A.; Dugas, R.; Taberna, P.-L.; Simon, P.; Plee, D.; Mastragostino, M.; Passerini, S. High temperature carbon-carbon supercapacitor using ionic liquid as electrolyte. Journal of Power Sources 2007, 165, 922-927.

[0082] (14) Balducci, A.; Bardi, U.; Caporali, S.; Mastragostino, M.; Soavi, F. Ionic liquids for hybrid supercapacitors. Electrochemistry communications 2004, 6, 566-570.

[0083] (15) Olivier-Bourbigou, H.; Magna, L. Ionic liquids: perspectives for organic and catalytic reactions. Journal of Molecular Catalysis A: Chemical 2002, 182, 419-437.

[0084] (16) Balducci, A. Ionic liquids in Lithium-ion batteries. Topics in Current Chemistry 2017, 375, 20.

[0085] (17) Lewandowski, A.; Swiderska-Mocek, A. Ionic liquids as electrolytes for Li-ion batteries: An overview of electrochemical studies. Journal of Power sources 2009, 194, 601-609.

[0086] (18) Watanabe, M.; Thomas, M. L.; Zhang, S.; Ueno, K.; Yasuda, T.; Dokko, K. Application of ionic liquids to energy storage and conversion materials and devices. Chemical reviews 2017, 117, 7190-7239.

[0087] (19) Molinari, N.; Mailoa, J. P.; Kozinsky, B. General Trend of Negative Transference Number in Li Salt/Ionic Liquid Mixtures. 2019.

[0088] (20) Molinari, N.; Mailoa, J. P.; Craig, N.; Christensen, J.; Kozinsky, B. Transport Anomalies Emerging from Strong Correlation in Ionic Liquid Electrolytes. 2019.

[0089] (21) Gouverneur, M.; Schmidt, F.; Schonhoff, M. Negative effective Li transference numbers in Li salt/ionic liquid mixtures: does Li drift in the “Wrong” direction? Physical Chemistry Chemical Physics 2018, 20, 7470-7478.

[0090] (22) Fadel, E.; Faglioni, F.; Samsonidze, G.; Molinari, N.; Merinov, B. V.; Goddard III, W. A.; Grossman, J. C.; Mailoa, J. P.; Kozinsky, B. Effects of solvent-salt charge-transfer complexes on oxidative stability of Li-ion battery electrolytes. 2018.

[0091] (23) Plimpton, S. Fast parallel algorithms for short-range molecular dynamics. Journal of computational physics 1995, 117, 1-19.

[0092] (24) Jorgensen, W. L.; Tirado-Rives, J. The OPLS [optimized potentials for liquid simulations] potential functions for proteins, energy minimizations for crystals of cyclic peptides and crambin. Journal of the American Chemical Society 1988, 110, 1657-1666.

[0093] (25) Jorgensen, W. L.; Maxwell, D. S.; Tirado-Rives, J. Development and testing of the OPLS all-atom force field on conformational energetics and properties of organic liquids. Journal of the American Chemical Society 1996, 118, 11225-11236.

[0094] (26) Doherty, B.; Zhong, X.; Gathiaka, S.; Li, B.; Acevedo, O. Revisiting OPLS force field parameters for ionic liquid simulations. Journal of chemical theory and computation 2017, 13, 6131-6145.

[0095] (27) Mogurampelly, S.; Ganesan, V. Structure and Mechanisms Underlying Ion Transport in Ternary Polymer Electrolytes Containing Ionic Liquids. J. Chem. Phys. 2017, 146, 074902.

[0096] (28) Pal, T.; Beck, C.; Lessnich, D.; Vogel, M. Effects of Silica Surfaces on the Structure and Dynamics of Room-Temperature Ionic Liquids: A Molecular Dynamics Simulation Study. The Journal of Physical Chemistry C 2017, 122, 624-634.

[0097] (29) Borodin, O. Polarizable force field development and molecular dynamics simulations of ionic liquids. The Journal of Physical Chemistry B 2009, 113, 11463-11478.

[0098] (30) Schröder, C.; Steinhauser, O. Simulating polarizable molecular ionic liquids with Drude oscillators. The Journal of chemical physics 2010, 133, 154511.

[0099] (31) Sambasivarao, S. V.; Acevedo, O. Development of OPLS-AA force field parameters for 68 unique ionic liquids. Journal of chemical theory and computation 2009, 5, 1038-1050.

[0100] (32) Acevedo, O. Ionic liquid force field parameters (OPLS-20091L and OPLS-VSIL), GitHub.

[0101] (33) Jorgensen, W. L.; Tirado-Rives, J. Potential energy functions for atomic-level simulations of water and organic and biomolecular systems. Proceedings of the National Academy of Sciences 2005, 102, 6665-6670.

[0102] (34) Dodda, L. S.; Vilseck, J. Z.; Tirado-Rives, J.; Jorgensen, W. L. 1.14* CM1A-LBCC: localized bond-charge corrected CM1A charges for condensed-phase simulations. The Journal of Physical Chemistry B 2017, 121, 3864-3870.

[0103] (35) Dodda, L. S.; Cabeza de Vaca, I.; Tirado-Rives, J.; Jorgensen, W. L. LigParGen web server: an automatic OPLS-AA parameter generator for organic ligands. Nucleic acids research 2017, 45, W331-W336.

[0104] (36) Hoover, W. G. Canonical dynamics: equilibrium phase-space distributions. Physical review A 1985, 31, 1695.

[0105] (37) Nosé, S. A unified formulation of the constant temperature molecular dynamics methods. The Journal of chemical physics 1984, 81, 511-519.

[0106] (38) Hoover, W. G. Constant-pressure equations of motion. Physical Review A 1986, 34, 2499.

[0107] (39) Wheeler, D. R.; Newman, J. Molecular dynamics simulations of multicomponent diffusion. 1. Equilibrium method. J. Phys. Chem. B 2004, 108, 18353-18361.

[0108] (40) Molinari, N.; Angioletti-Uberti, S. Nanoparticle Organization Controls Their Potency as Universal Glues for Gels. Nano letters 2018, 18, 3530-3537.

[0109] (41) Molinari, N.; Sutton, A.; Mostofi, A. Mechanisms of reinforcement in polymer nanocomposites. Physical Chemistry Chemical Physics 2018, 20, 23085-23094.

[0110] (42) Webb, M. A.; Jung, Y.; Pesko, D. M.; Savoie, B. M.; Yamamoto, U.; Coates, G. W.; Balsara, N. P.; Wang, Z.-G.; Miller III, T. F. Systematic computational and experimental investigation of lithium-ion transport mechanisms in polyester-based polymer electrolytes. ACS central science 2015, 1, 198-205.

[0111] Other embodiments are in the claims.