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Article

Theoretical Investigation of Carbon Dioxide Adsorption on Li+-Decorated Nanoflakes

by
Igor K. Petrushenko
1,*,
Nikolay A. Ivanov
1 and
Konstantin B. Petrushenko
2
1
Irkutsk National Research Technical University, 83 Lermontov St., 664074 Irkutsk, Russia
2
AE Favorsky Irkutsk Institute of Chemistry, Siberian Branch of the Russian Academy of Sciences, 1 Favorsky St., 664033 Irkutsk, Russia
*
Author to whom correspondence should be addressed.
Molecules 2021, 26(24), 7688; https://doi.org/10.3390/molecules26247688
Submission received: 22 November 2021 / Revised: 13 December 2021 / Accepted: 14 December 2021 / Published: 20 December 2021
(This article belongs to the Section Computational and Theoretical Chemistry)
Browse Figures
Versions Notes

Abstract

:
Recently, the capture of carbon dioxide, the primary greenhouse gas, has attracted particular interest from researchers worldwide. In the present work, several theoretical methods have been used to study adsorption of CO2 molecules on Li+-decorated coronene (Li+@coronene). It has been established that Li+ can be strongly anchored on coronene, and then a physical adsorption of CO2 will occur in the vicinity of this cation. Moreover, such a decoration has substantially improved interaction energy (Eint) between CO2 molecules and the adsorbent. One to twelve CO2 molecules per one Li+ have been considered, and their Eint values are in the range from −5.55 to −16.87 kcal/mol. Symmetry-adapted perturbation theory (SAPT0) calculations have shown that, depending on the quantity of adsorbed CO2 molecules, different energy components act as the main reason for attraction. AIMD simulations allow estimating gravimetric densities (GD, wt.%) at various temperatures, and the maximal GDs have been calculated to be 9.3, 6.0, and 4.9% at T = 77, 300, and 400 K, respectively. Besides this, AIMD calculations validate stability of Li+@coronene complexes during simulation time at the maximum CO2 loading. Bader’s atoms-in-molecules (QTAIM) and independent gradient model (IGM) techniques have been implemented to unveil the features of interactions between CO2 and Li+@coronene. These methods have proved that there exists a non-covalent bonding between the cation center and CO2. We suppose that findings, derived in this theoretical work, may also benefit the design of novel nanosystems for gas storage and delivery.

Graphical Abstract

1. Introduction

Carbon dioxide (CO2) is a greenhouse gas that has severe environmental and health effects. An important source of atmospheric CO2, which is responsible for climate change, is fossil fuel consumption. The permanent increase of the concentration of carbon dioxide in the atmosphere is a menace to the safety of living species, and it renders a major problem to the environment. Numerous steps have been proposed to overcome this problem, such as the use of renewable energy, a decrease of deforestation, and the decarbonization of buildings and infrastructure. These pathways need sophisticated equipment and large assets; therefore, the idea of direct capture and further conversion of CO2 becomes very appealing.
In recent times, research efforts have been focused on the enhancement of current CO2 capture methods to alleviate anthropogenic greenhouse gas emissions. There exist a number of carbon dioxide uptake techniques, which depend on such parameters of the gas to be adsorbed including the flow, concentration, temperature, and pressure. In that regard, the well-established technology is the chemical absorption in liquid amines. This methodology, though, holds numerous drawbacks, such as low CO2 capacity, equipment corrosion, amine degradation by SO2, NO2, and O2 existed in the flue gases, low energy efficiency owing to the high temperatures utilized during absorbent regeneration, and, finally, large size of the equipment [1].
For the more efficient cyclic usage, the capture techniques based on physical adsorbents are seemingly preferred. A large variety of solid-state media have been systematically investigated for CO2 adsorption, e.g., zeolites, aluminophosphates, pristine and doped activated carbons, carbon nanotubes, graphene-based materials, metal organic frameworks (MOFs), and different nanomaterials [2,3,4,5,6,7,8,9,10,11,12,13,14].
Carbon-based adsorbents (e.g., activated carbon, graphene, carbon nanotubes, etc.) have been widely used for CO2 uptake owing to their low cost, widespread availability, and high thermal stability. Physical adsorption in this case is driven by London dispersion forces, and, generally speaking, these forces are weak. Consequently, the applications are limited to a high gas pressure or low temperatures. Nowadays, researchers focus on two ways of CO2 storage capacity, namely, fabricating a pore structure or modification of surface to increase alkalinity. These methods are principally applicable to graphene. A decade ago, graphene attracted considerable attention owing to its unique structure and impressive mechanical, thermal, and electrical properties [15,16,17]. It was also used as an adsorbent for gas storage [18,19]. However, pristine graphene does not seem to be used as a powerful adsorbent because its electronic structure is responsible for establishing London dispersion forces with molecules accommodated at its surface [19]. More specifically, graphene exhibits a comparatively good adsorption strength for CO2, that is stronger than those for the main constituent of natural gas (CH4) and the main atmosphere gas (N2) [20,21]. At the same time, pristine graphene is a one-atom-thick two-dimensional material, and this structural feature renders it to be a feasible, but low-capacity, gas adsorbent.
The weight percent (wt.%) ratio for the gas uptake can be sufficiently increased by constructing three-dimensional (3D) graphene-based architectures [22,23]. Another technique for the increase in the gas capture is the graphene decoration with atoms or cations of alkali, alkali-earth, and transition metals [24,25,26,27,28]. It is essential to note the successful implementation of the last two methods leads to construction of Li-decorated pillared graphene frameworks with H2 uptake of 20.68 wt.% [29]. These techniques are also feasible for the increase in CO2 adsorption. Thus, for example, porous graphene frameworks have been shown to provide a substantial enhancement of both H2 and CO2 adsorption capacity. The recent studies on CO2 interactions with Al-decorated, Ca-decorated, Se-decorated, Pt-doped, Ni-, and Co-doped graphene have been reported [25,30,31,32,33,34]. Thus, there are reasons to believe that such a method can enhance CO2 adsorption, and decorated graphenes may be considered as candidates for CO2 storage.
In this work, we focus on studying CO2 adsorption on the Li+-decorated coronene (Li+@coronene) model, which can be considered as a small graphene nanocluster. The data obtained from the density functional theory (DFT) method are complemented with energy calculations by using the symmetry-adopted perturbation theory (SAPT0) method [35], which allows obtaining the constituents of interaction energy. The independent gradient model (IGM) method [36,37], Bader’s theory of atoms and molecules (QTAIM) [38] as well as ab initio molecular dynamics (AIMD) computations help us to predict the behavior of CO2 molecules in the vicinity of Li+@coronene and its adsorption properties at different temperatures. In this regard, this theoretical investigation goes beyond the pristine graphene studies, and broadens our understanding of the mechanisms of a CO2 uptake using decorated graphene.

2. Results and Discussions

2.1. CO2 Adsorption on Li+@coronene Complexes

To explicitly study carbon dioxide adsorption on Li+@coronene complexes, we add CO2 molecules above the surface (in the vicinity of Li+) in the step-by-step mode. Optimized geometries (BLYP-D3/def2-SVP) of several complexes are presented in Figure 1. We divide adsorbed CO2 into three layers, and each of them contains four CO2 molecules (twelve molecules in total). The behavior of the CO2 molecules in these layers is different. First, we check the distances between the Li cation and the substrate after optimization when four, eight, and twelve molecules are considered. The distance is constantly increasing, and its values are calculated to be 2.877, 2.919, and 3.350 Å in the case of four, eight, and twelve adsorbed CO2 molecules, respectively (Figure 1). The obtained values are significantly larger than that for the single Li+ adsorbed at coronene (1.874 Å [39]). Hence, we should further examine the behavior of such complexes in detail.
For the first layer, we can easily determine that all the CO2 molecules lie in one plane, which is parallel to the plane of the adsorbent. The distances between the O atom of the CO2 molecule and Li+ are in the range of 2.012–2.068 Å (Figure 1). It has been established elsewhere that the optimized distances (d) between CO2 and a pentagraphene nanosheet are in the range of 3.064–3.212 Å [40]. Very recently, the d value between the CO2 molecule and the graphene quantum dot (GQD) has been assessed to be 3.615 Å, and Eint for CO2 adsorption on GQD has been calculated to be −0.39 kcal/mol [24]. This distance is typical for physisorption, but such a low Eint value is not generally sufficient for CO2 storage. The transition metal (TM) adatoms doping increases the Eint values for CO2@TM@GQD adsorption [24]. Thus, for example, Co decoration helps one to reach Eint of ~−17.30 kcal/mol (d = 2.300 Å), Cr decoration increases Eint up to ~−27.67 kcal/mol (d = 1.562 Å), whereas Ti-decorated GQD demonstrates very high Eint values of ~−46 kcal/mol (d = 1.633 Å) [24]. However, in the last case, the CO2 molecule undergoes dissociation, and it seems that a chemical bond between the adsorbate and the adsorbent occurs. It should be noted that the values discussed above concern only a single CO2 molecule adsorbed. Another work, studying CO2 adsorption on pristine and defected graphene, yields the following values: Eint of −5.37 kcal/mol and d of 2.983 Å [41]. The results of that paper also support our outcomes on very marginal, although favorable, interactions between CO2 and pristine graphene [41]. Cabrera-Sanfelix [42] and Liu and Wilcox [43] reported the Eint magnitudes of ~−3.14 kcal/mol (d = 3.47 Å) and −4.84 kcal/mol (d = 3.45 Å) for CO2 adsorption on defected graphene, respectively. At the same time, experimental studies demonstrated Eint of −0.55 (for adsorption on SWCNTs) [44], −4.1 [45], and from −4 to −9 kcal/mol [46], respectively. The results presented above witness that the typical distances between the graphene both pristine and defected are slightly larger than 3 Å, whereas atomic/cation decoration increases the Eint magnitudes, but decreases the d values. In terms of both distances and energy (Table 1) the values obtained herein are intermediate ones compared with literature data.
In the present case, the molecules of the second layer acquire the tilted configuration; however, we link this behavior with adsorption at the edge of our model. In general, the d values of 4.126–4.168 Å are significantly larger than those for typical physisorption. On the contrary, the CO2 molecules representing the third layer show the distances of intermediate magnitudes compared with the previous cases (2.032–4.040 Å) (Figure 1). It witnesses in favor of considering these molecules as adsorbed ones.
We next turn to comparison of Eint and different energy constituents for CO2 adsorption (Table 1). The ideal adsorption energy window for CO2 storage is from −9.22 to −18.45 kcal/mol (from −0.4 to −0.8 eV) [25].
The first four CO2 molecules attached are of especial interest as they show the highest Eint values. Their magnitudes are in the range from −16.87 to −11.26 kcal/mol. These values correspond well the optimal energy range for a CO2 uptake. They are characterized by high Eel and Eind magnitudes, whereas Edisp is slightly lower. The non-zero quadrupole moment of the CO2 molecule promotes large Eel magnitudes, whereas Li+ shifts the electronic density of the CO2 molecules, and, thereby, enhances the Eind term. At the same time, the small quantity of the neighbor molecules accounts for the small dispersion interactions; the similar situation was observed earlier for hydrogen adsorption in hollow pores [47] or Li+-decorated nanostructures [48,49,50]. A close analysis was carried out for the next four molecules adsorbed. One may easily note the significant decrease in Eint values compared with the previous case. Besides this, the contribution of Eind to the total attractive interactions is rather small here, and it gives only one tenth of all attractive interactions. The significance of London dispersion is much higher, and the contributions of Edisp and Eel terms are nearly equal (Table 1).
Finally, for the last four CO2 molecules, the trend slightly varies, and one can observe the intermediate Eint values, which are significantly lower compared with the first four molecules. However, they are high enough to be superior compared with the second four molecules. Indeed, the Edisp term diminishes as the small quantity of CO2 is located above the Li cation. At the same time, Eind is much higher as the positions of the adsorbed molecules are closer to Li+ (Figure 1, Table 1). To sum up, the first four molecules are described by the highest Eint, the second four molecules exhibit the smallest Eint, and the Eint values for the last four CO2 molecules fall between them. We suppose that 1–4 CO2 molecules should play a major role in determining the CO2 uptake value for Li+@coronene, but we should keep in mind 9–12 CO2 molecules and thoroughly study the behavior of the systems in detail further.
Now we compare the obtained Eint energies with those obtained elsewhere. Lu et al. studied CO2 adsorption on pentagraphene, and the Eint energies were in the range from −3.44 to −4.82 kcal/mol. Darvishnejad and Reisi-Vanani investigated CO2 adsorption on pristine and Sr-decorated graphynes (Gy). It was established that Eint values for the first adsorbed CO2 molecule are −5.81 and −9.80 kcal/mol for Gy and Sr-decorated Gy, respectively [51]. According to Ref. [25], the obtained Eint values for 1–4 CO2 molecules fall inside the optimal range for CO2 capture. Besides, Eint of some of the 9–12 CO2 molecules also fall into this energy window. Moreover, Eint values obtained herein are generally higher than those obtained elsewhere.
To visualize the interactions between CO2 molecules and Li+@coronene, we implement here the independent gradient model (IGM) method [36,37]. Lefevbre et al. implemented this method as a straightforward tool to study inter- and intramolecular interactions. The new descriptors which are defined in the framework of this method allow obtaining a measure of electron sharing (δg), and separately describe interactions inside each molecular fragment (δgintra) or between fragments (δginter). According to the definition, the blue color regions indicate strong binding (e.g., hydrogen bonds), and the green color ones represent weak interactions (e.g., van der Waals interactions).
As shown in Figure 2, for the first CO2 molecule adsorbed on Li+@coronene, there exist a green-blue lobe in the vicinity of Li+, which denotes a strong attraction and a purely green lobe (between the CO2 molecule and the coronene surface), which denotes weak van der Waals interactions. We then inspect the case of the fifth adsorbed CO2 molecule. The scene changes significantly, and we can observe only three green lobes and no blue-green ones. It accounts for the increased significance of London dispersion and the decrease contribution of induction interactions into attraction. The interaction of the 9th molecule with the system is characterized by the small quantity of green lobes, which denotes generally lower dispersion contribution, and the very small blue-green isosurface. These observations are in line with the results of energy decomposition analysis by the SAPT0 method (Table 1). These cases treat the adsorbed system as two fragments, one of which is the CO2 molecule (first, fifth, or ninth) and another one is the rest molecules and the Li+@coronene substrate. The fourth studied system is the one including twelve adsorbed CO2 molecules. Here, we treat the system as thirteen isolated parts (one of them is Li+@coronene and another twelve are studied CO2 molecules). The results are presented in Figure 2 (bottom, right). It approves our previous outcomes that for one to four adsorbed CO2 molecules, Eind plays an important role (a blue-green isosurface in the vicinity of Li+). On the contrary, a large number of green lobes validate our conclusions on the important role of Edisp in the case of five to eight adsorbed CO2 molecules. Finally, the smaller density of green lobes for nine to twelve CO2 molecules indicates the decrease of the Edisp contribution into total attraction interactions and the simultaneous increase of Eel and Eind ones (cf. Table 1).

2.2. Analysis of Non-Covalent Interactions between CO2 Molecules and the Li+@coronene Complex by Quantum Theory of Atoms in Molecules (QTAIM)

To obtain profound information on the nature of interactions between CO2 molecules and the studied adsorbent, we involve here the Bader’s quantum theory of atoms in molecules (QTAIM). We obtain such quantities as: electron density (ρ(r)) at the (3, −1) bond critical point (BCP), its Laplacian (∇2ρ(r)), the electronic energy density (H(r)), the kinetic energy density, G(r), and the potential energy density, V(r). These values are summarized in Table 2.
First, it is worth noticing that no BCPs between five to eight CO2 molecules and the Li cation are observed. It witnesses that smaller Eint values (Table 1) for these molecules are mainly due to Edisp interaction between CO2 molecules, and the interactions between the cation center and these molecules are feeble ones. The values of electron density (ρ(r)) at the BCPs provide valuable information on the strength of bonding. The magnitudes of ρ(r) are in line with Eint values obtained at the SAPT0 level of theory. As is expected, the first adsorbed molecules are described by the significant magnitudes of Eint. The positive (negative) values of ∇2ρ(r) at the BCPs indicate a non-covalent (covalent) bond existence [52]. Table 2 shows that physisorption is the sole type of adsorption here. Besides this, we inspect the H(r) values, and the positive sign of all the values exhibits the non-covalent interactions [53]. The last criterion we inspect is the magnitude of the following ratio: −G(r)/V(r). As it is larger than unity, the interactions can be classified as the non-covalent ones.

2.3. AIMD Simulations of CO2 Adsorption on Li+@coronene

For the sake of completeness, we carry out the ab initio molecular dynamics (AIMD) simulations to inspect the thermal stability of adsorbed Li cations as well as CO2 molecules. Additionally, the data obtained is utilized for CO2 gravimetric density calculations (GD, wt.%) at different temperatures. In this work, we use three temperatures (T): 77 K (liquid nitrogen T), 300 K (room T), and 400 K (elevated T for a flue gas).
First, we study the system consists of four CO2 molecules adsorbed on Li+@coronene (Figure S1, Supplementary Materials). For the lowest studied T = 77 K, and at this moment of time (t) = 500 fs, we can observe only small reorientations of carbon dioxide molecules adsorbed at Li+. All the CO2 molecules can be considered as adsorbed at t = 500 and 1000 fs. Only minute structural changes of Li+@coronene can be observed in this case. However, the significant displacement of Li+ from the origin is worth mentioning. Earlier it was established that the edge six-membered cycles of PAHs can accommodate Li cations more favorably than the central ones [54]. Besides, it appears that potential barriers for Li+ migration on the surface of PAHs are rather small. At room T = 300 K, no significant changes can be noted. Even at the elevated T = 400 K and t = 1000 fs, the CO2 molecules all acquire tilted configuration, but the distancing from Li+ is feeble.
Second, we take into consideration eight CO2 molecules adsorbed (Figure S2, Supplementary Materials). For T = 77 K, the small shift of Li+ and adsorbed CO2 molecules from the initial position (at t = 500 and 1000 fs) can be noted. However, even at t = 1000 fs, all the molecules are at nearly the same distances from Li+ compared with the initial moment of time. For T = 300 K, it can be easily observed that the four molecules, which comprise the second layer, are well spaced (at t = 500 and 1000 fs). For T = 400 K, a sufficient displacement of Li+ occurs, and only first four CO2 molecules can be considered as adsorbed; the rest ones are at very large distances from Li+.
Finally, we study adsorption behavior of twelve CO2 molecules (Figure S3, Supplementary Materials). For T = 77 K, we also note only small deviations of both Li+ and CO2 molecules from the initial positions. For T = 300 K and t = 1000 fs, the adsorbed system can be characterized by the moderate distancing of some CO2 molecules, which constitute the second layer, from Li+. Moreover, for T = 400 K and t = 1000 fs, not only the above-mentioned molecules, but also molecules from the third layer become well spaced from the Li cation. In the last case, only four CO2 molecules can be considered as adsorbed.
We also identify the thermostability of the Li+@coronene complex itself with 12 adsorbed CO2 molecules for the liquid nitrogen temperature (77 K) and for the general operating mode (300 and 400 K). We inspect the distances between all pairs of the consecutive steps (e.g., the initial position of the Li cation is fixed as the origin and its position after 1.0 fs of equilibration is the position at the second step) during the simulation time, and then calculate the shifts between each pair of steps. As it can be easily seen in Figure 3, the Li+-coronene distance is still stable during the whole simulation time. The Li+ shifts fluctuate around the mean values of ~0.005, 0.010, and 0.010 Å for 77, 300 and 400 K, respectively. Additionally, the results obtained show the very similar patterns for T = 300 and 400 K. The displacements of Li+ (at the end of simulation (i.e., t = 1.0 ps)) are measured to be ~1.45, 3.25, and 4.00 Å for 77, 300, and 400 K, respectively. The large traveling distance of Li+ for the elevated temperatures require careful monitoring of the complexes (Figure S2 and S3, Supplementary Materials). As it was established above, we observe the large distancing of several CO2 molecules, but the Li+@coronene complex as a whole can be considered stable for CO2 adsorption.
Using the present AIMD data and the results of DFT calculations derived above, we now assess the CO2 uptake by the Li+@coronene system. The CO2 gravimetric density (GD, wt.%) may be estimated as:
G D = M n C O 2 M n C O 2 + M c o m p l e x × 100 %
where, M n C O 2 is the mass of n adsorbed CO2 molecules, and M c o m p l e x is the mass of the complex.
We calculate several GDs for the Li+@coronene complex. The first GD value is calculated using our DFT and SAPT0 results, and it includes all twelve molecules adsorbed. As some of the molecules are weakly linked with the cation center, we adopt this value as the highest limit of CO2 uptake, and it is calculated to be 7.3 (13.35) wt.% for one-side (double-side) adsorption. Furthermore, the QTAIM computations derived above approve our outcomes on the weakly bound five to eight CO2 molecules. We, hence, exclude them from the further considerations. AIMD simulations can help one to reveal the molecules both adsorbed and released as well as quantify their number. Table 3 shows that the increase in T leads to the substantial decrease in GDs.
Now, it is worth comparing the GD values tabulated above with those on carbonaceous adsorbents obtained elsewhere. It was established that the typical CO2 adsorption capacity of activated carbons is 5 wt.% [55,56]. Zhao et al. demonstrated adsorption capacity of 4.65 wt.% at 303 K and 1 bar for CO2/N2 mixture for ethylenediamine (EDA)-intercalated graphene oxide [57]. Surface-microporous 3D graphene has been shown to provide high CO2 capacity of ~10%. The KOH activation further increases its capacity up to ~13.8% [22]. Different mesoporous molecular sieves exhibited 3.3–13.3% carbon dioxide uptake [1]. At the same time, a theoretical assessment of CO2 capacity of pristine and Sr-decorated graphyne shows very high values, namely, 18.63 and 31.68 wt.%, respectively [51]. Thiruvenkatachari et al. synthesized honeycomb-shaped carbon fiber adsorbents for CO2 capture. The average CO2 adsorption uptake was shown to be 11.9 wt.% for a gas mixture [58]. The comparison clearly shows that the proposed complex exhibits considerable CO2 physisorption, and, hence, we believe that the studied system owing to its simplicity can help the researchers to design efficient new systems for CO2 capture. This work, presumably, will be useful for waste gases treatment to decrease the negative impact from industrial plants and vehicles.

3. Computational Methods

3.1. Computational Details

Geometries of all structures studied herein have been optimized using the BLYP [59,60] density functional in conjunction with the def2-SVP [61] basis set. Grimme’s dispersion correction (D3) [62] has been employed for the accurate treatment of van der Waals interactions. The BLYP-D3 method has been shown to provide reliable results on different graphene nanoflake complexes [63,64,65,66,67]. Frequency calculations have been performed to validate equilibrium geometries.
The interaction energy (Eint) between the adsorbent and the adsorbate molecules has been calculated for all the studied complexes using zeroth-order symmetry-adapted perturbation theory (SAPT0) [35] with the jun-cc-pVDZ basis set [68,69]. This method helps one to decompose Eint into the meaningful components: exchange (Eex), electrostatic (Eel), dispersion (Edisp), and induction (Eind) ones. We involve the PSI4 code (v.1.2) [70] to perform SAPT0 calculations, whereas the Orca 4.2.1 [71] program has been used for geometry optimizations. It is worth noticing that a more negative Eint value denotes a stronger interaction. Additionally, the SAPT0 interaction energies are free from the so-called basis set superposition errors (BSSE). The SAPT0 description is given in Supplementary Materials in more detail. The procedure of obtaining energy constituents was the following: first, the geometries of Li+@coronene along with the adsorbed CO2 molecules were optimized at the BLYP/def2-SVP level of theory. Then, the SAPT0 method was used to obtain the magnitudes of aforementioned energy terms.
The initial structures for ab initio molecular dynamics (AIMD) simulations have been optimized using the BLYP/def2-SVP method. AIMD computations have been also done by the Orca 4.2.1 program suite. All AIMD simulations used a time step of one femtosecond, a canonical constant volume and constant temperature NVT ensemble using a Berendsen thermostat [72] and a velocity Verlet algorithm for integrating the equation of motion. The time period of 1000 femtoseconds (fs) has been used for the full AIMD computation cycle. The time step has been chosen to be 1 fs.

3.2. Validation of Methodology

First, it should be noted here that the combination of methods (BLYP/def2-SVP) suits well for the study of adsorption phenomena. Besides, the SAPT0/jun-cc-pVDZ method is shown to provide very reliable results for non-covalent interactions [73].
Second, to further validate the methodology used, we compare the obtained Eint value for Li+ adsorption on coronene (−40.52 kcal/mol) with those for the relevant systems. The result of Gal et al. (at the B3LYP/6-311G(3df,2p) level of theory) is of ~−44.46 kcal/mol for Li+@coronene interactions. Eint calculated for Li+ adsorption on triphenylene central ring is of −44.4 kcal/mol [74]. As studies on Li+ interactions with PAHs are rather scarce, we compare the obtained values with those on Li+@benzene interactions (a benzene molecule can be adopted as a central ring of coronene). The experimentally observed Eint for Li+@benzene adsorption are as follows: −38.3 [75] and −38.5 ± 3.2 kcal/mol [76].
Our previous Eint result on Li+ adsorption on benzene (MP2/SAPT2) has shown to be −36.92 kcal/mol [77]. The Eint values for Li+ adsorbed on curved PAHs were also given as an instance. Thus, Li+ adsorption on concave and convex sites of corannulene (C20H10) and sumanene (C21H12) yields −44.57, −44.87 kcal/mol [78] and −40.48, −37.97 kcal/mol [79], respectively (these values are for adsorption on the central rings of the sorbents). At the same time, adsorption on the central hexagonal ring of circumtrindene (C36H12) exhibits slightly higher values of −46.83 and −46.18 kcal/mol for the concave and convex site, respectively [80]. Hence, it seems evident that the obtained result is in a reasonably good accordance with the available literature data. The difference can be explained by the various computational methods involved.

4. Conclusions

To summarize, the Li+@coronene complex was theoretically studied as a new platform for a carbon dioxide capture. DFT and SAPT0 calculations of the 1–12 CO2 molecules adsorbed at Li+@coronene exhibit larger Eint values compared with those for pristine graphene, however, some of them do not satisfy the optimal energy range for CO2 storage. At the same time, the AIMD results show that the cation center of the Li+@coronene complex can favorably accommodate numerous CO2 molecules that leads to the maximal gravimetric density (GD) of 5.0 (9.3) wt.% for one-side (double-side) adsorption.
The SAPT0 analysis also reveals that the different ratio of the interaction energy terms affects CO2 molecules attached. The first four CO2 molecules are mainly attracted by electrostatic forces, whereas dispersion and induction energy terms are of less importance. For the next four CO2 molecules adsorbed, electrostatic and dispersion terms are equally important, and only one tenth of the whole attraction is due to dispersion. These molecules are characterized by the lowest Eint values. For nine to twelve CO2 molecules, large influence of electrostatic interactions can be observed, they are followed by the dispersion and induction ones. The IGM analysis visually complements the outcomes of SAPT0 calculations, whereas QTAIM calculations approve the existence of weak non-covalent interactions between the CO2 molecules and Li+@coronene. AIMD simulations reveal stability of the Li+@coronene complexes. At T of 77 K, we note that all the molecules are at the anchoring cation during the whole process of simulation. However, for CO2 adsorption at T = 300 K and especially at T = 400 K, the considerable distancing of the molecules is observed; it leads to the decrease of GDs. Thus, involving a set of theoretical methods that reveal the nature of CO2/adsorbent interactions, our paper establishes that the Li+@coronene cluster may be useful as a novel medium for the carbon dioxide storage.

Supplementary Materials

Figure S1: AIMD simulations snap shots of four adsorbed CO2 molecules on Li+@coronene complexes at T = 77 K (A), 300 K (B), 400 K (C). Atomic color code: carbon—yellow, oxygen—red, hydrogen—light-blue, lithium cation—magenta. Figure S2. AIMD simulations snap shots of eight adsorbed CO2 molecules on Li+@coronene complexes at T = 77 K (A), 300 K (B), 400 K (C). Atomic color code: carbon—yellow, oxygen—red, hydrogen—light-blue, lithium cation—magenta. Figure S3. AIMD simulations snap shots of twelve adsorbed CO2 molecules on Li+@coronene complexes at T = 77 K (A), 300 K (B), 400 K (C). Atomic color code: carbon—yellow, oxygen—red, hydrogen—light-blue, lithium cation—magenta.

Author Contributions

I.K.P.: Conceptualization, Methodology, Investigation, Writing—original draft, Writing—review & editing. N.A.I.: Investigation, Writing—original draft. K.B.P.: Methodology, Investigation, Writing—original draft. All authors have read and agreed to the published version of the manuscript.

Funding

This work was supported by Ministry of Science and Higher Education of the Russian Federation in the framework of the scientific and educational center “Baikal” (grant no. FZZS-2021-0007).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Acknowledgments

Generous allotment of computational time from Computational Center of Novosibirsk State University (www.nusc.ru, accessed on 21 November 2021) is gratefully acknowledged.

Conflicts of Interest

The authors declare no conflict of interest.

Sample Availability

Samples of the compounds are not available from the authors.

References

  1. Yu, C.-H.; Huang, C.-H.; Tan, C.-S. A Review of CO2 Capture by Absorption and Adsorption. Aerosol Air Qual. Res. 2012, 12, 745–769. [Google Scholar] [CrossRef] [Green Version]
  2. Lu, C.; Shi, X.; Liu, Y.; Xiao, H.; Li, J.; Chen, X. Nanomaterials for adsorption and conversion of CO2 under gentle conditions. Mater. Today 2021. [Google Scholar] [CrossRef]
  3. Song, X.; Liu, Y.; Yang, Y.; Li, W.; Zhao, M. Strain-tunable CO2 storage by black phosphorene and alpha-PC from combined first principles and molecular dynamics studies. Phys. Chem. Chem. Phys. 2019, 21, 20107–20117. [Google Scholar] [CrossRef] [PubMed]
  4. Akilan, R.; Ravichandran, D.; Vinnarasi, S.; Shankar, R. Adsorption of H2 and CO2 gas molecules on Li/Na decorated Si2BN nano-sheet for energy harvesting applications—A density functional study. Mater. Lett. 2020, 279, 128487. [Google Scholar] [CrossRef]
  5. Regufe, M.J.; Ribeiro, A.M.; Ferreira, A.F.P.; Rodrigues, A. CO2 Storage on Zeolites and Other Adsorbents. In Nanoporous Materials for Gas Storage. Green Energy and Technology; Kaneko, K., Rodríguez-Reinoso, F., Eds.; Springer: Singapore, 2019; pp. 359–381. [Google Scholar]
  6. Yu, Y.; Li, X.; Krishna, R.; Liu, Y.; Cui, Y.; Du, J.; Liang, Z.; Song, X.; Yu, J. Enhancing CO2 Adsorption and Separation Properties of Aluminophosphate Zeolites by Isomorphous Heteroatom Substitutions. ACS Appl. Mater. Interfaces 2018, 10, 43570–43577. [Google Scholar] [CrossRef]
  7. Al Mesfer, M.K.; Danish, M. Breakthrough adsorption study of activated carbons for CO2 separation from flue gas. J. Environ. Chem. Eng. 2018, 6, 4514–4524. [Google Scholar] [CrossRef]
  8. Shi, S.; Liu, Y. Nitrogen-doped activated carbons derived from microalgae pyrolysis by-products by microwave/KOH activation for CO2 adsorption. Fuel 2021, 306, 121762. [Google Scholar] [CrossRef]
  9. Chen, S.-Y.; Hui, Y.; Yang, Y.-B. Monte Carlo simulations of adsorption and separation of binary mixtures of CO2, SO2, and H2S by charged single-walled carbon nanotubes. Soft Mater. 2020, 18, 262–273. [Google Scholar] [CrossRef]
  10. Lee, K.-J.; Kim, S.-J. Theoretical Investigation of CO2 Adsorption on Graphene. Bull. Korean Chem. Soc. 2013, 34, 3022–3026. [Google Scholar] [CrossRef] [Green Version]
  11. Mao, X.; Tang, C.; He, T.; Wijethunge, D.; Yan, C.; Zhu, Z.; Du, A. Computational screening of MN4 (M = Ti-Cu) based metal organic frameworks for CO2 reduction using the d-band centre as a descriptor. Nanoscale 2020, 12, 6188–6194. [Google Scholar] [CrossRef]
  12. Meconi, G.M.; Zangi, R. Adsorption-induced clustering of CO2 on graphene. Phys. Chem. Chem. Phys. 2020, 22, 21031–21041. [Google Scholar] [CrossRef] [PubMed]
  13. Mishra, A.K.; Ramaprabhu, S. Carbon dioxide adsorption in graphene sheets. AIP Adv. 2011, 1, 032152. [Google Scholar] [CrossRef]
  14. Xia, K.; Xiong, R.; Chen, Y.; Liu, D.; Tian, Q.; Gao, Q.; Han, B.; Zhou, C. Tuning the pore structure and surface chemistry of porous graphene for CO2 capture and H2 storage. Colloids Surf. A Physicochem. Eng. Asp. 2021, 622, 126640. [Google Scholar] [CrossRef]
  15. Papageorgiou, D.G.; Kinloch, I.A.; Young, R.J. Mechanical properties of graphene and graphene-based nanocomposites. Prog. Mater. Sci. 2017, 90, 75–127. [Google Scholar] [CrossRef]
  16. Kumar, A.; Sharma, K.; Dixit, A.R. A review of the mechanical and thermal properties of graphene and its hybrid polymer nanocomposites for structural applications. J. Mater. Sci. 2018, 54, 5992–6026. [Google Scholar] [CrossRef]
  17. Geim, A.K.; Novoselov, K.S. The rise of graphene. Nat. Mater. 2007, 6, 183–191. [Google Scholar] [CrossRef]
  18. Gadipelli, S.; Guo, Z.X. Graphene-based materials: Synthesis and gas sorption, storage and separation. Prog. Mater. Sci. 2015, 69, 1–60. [Google Scholar] [CrossRef] [Green Version]
  19. Singla, M.; Jaggi, N. Theoretical investigations of hydrogen gas sensing and storage capacity of graphene-based materials: A review. Sens. Actuators A Phys. 2021, 332, 113118. [Google Scholar] [CrossRef]
  20. D’Alessandro, D.M.; Smit, B.; Long, J.R. Carbon dioxide capture: Prospects for new materials. Angew. Chem. 2010, 49, 6058–6082. [Google Scholar] [CrossRef] [Green Version]
  21. Politakos, N.; Barbarin, I.; Cordero-Lanzac, T.; Gonzalez, A.; Zangi, R.; Tomovska, R. Reduced Graphene Oxide/Polymer Monolithic Materials for Selective CO2 Capture. Polymers 2020, 12, 936. [Google Scholar] [CrossRef] [Green Version]
  22. Tian, Y.; Lin, Y.; Hagio, T.; Hu, Y.H. Surface-microporous graphene for CO2 adsorption. Catal. Today 2020, 356, 514–518. [Google Scholar] [CrossRef]
  23. dos Santos, T.C.; Mancera, R.C.; Rocha, M.V.J.; da Silva, A.F.M.; Furtado, I.O.; Barreto, J.; Stavale, F.; Archanjo, B.S.; de M. Carneiro, J.W.; Costa, L.T.; et al. CO2 and H2 adsorption on 3D nitrogen-doped porous graphene: Experimental and theoretical studies. J. CO2 Util. 2021, 48, 101517. [Google Scholar] [CrossRef]
  24. Ghosh, K.; Mridha, N.K.; Khan, A.A.; Baildya, N.; Dutta, T.; Biswas, K.; Ghosh, N.N. CO2 activation on transition metal decorated graphene quantum dots: An insight from first principles. Phys. E Low-Dimens. Syst. Nanostructures 2022, 135, 114993. [Google Scholar] [CrossRef]
  25. Liu, A.; Long, J.; Yuan, S.; Cen, W.; Li, J. Synergetic promotion by oxygen doping and Ca decoration on graphene for CO2 selective adsorption. Phys. Chem. Chem. Phys. 2019, 21, 5133–5141. [Google Scholar] [CrossRef]
  26. Tawfik, S.A.; Cui, X.Y.; Ringer, S.P.; Stampfl, C. Multiple CO2 capture in stable metal-doped graphene: A theoretical trend study. RSC Adv. 2015, 5, 50975–50982. [Google Scholar] [CrossRef] [Green Version]
  27. To, J.W.; He, J.; Mei, J.; Haghpanah, R.; Chen, Z.; Kurosawa, T.; Chen, S.; Bae, W.G.; Pan, L.; Tok, J.B.; et al. Hierarchical N-Doped Carbon as CO2 Adsorbent with High CO2 Selectivity from Rationally Designed Polypyrrole Precursor. J. Am. Chem. Soc. 2016, 138, 1001–1009. [Google Scholar] [CrossRef]
  28. Re Fiorentin, M.; Gaspari, R.; Quaglio, M.; Massaglia, G.; Saracco, G. Nitrogen doping and CO2 adsorption on graphene: A thermodynamical study. Phys. Rev. B 2018, 97. [Google Scholar] [CrossRef]
  29. Öztürk, Z. Lithium decoration characteristics for hydrogen storage enhancement in novel periodic porous graphene frameworks. Int. J. Hydrog. Energy 2021, 46, 11804–11814. [Google Scholar] [CrossRef]
  30. Ni, J.; Quintana, M.; Song, S. Adsorption of small gas molecules on transition metal (Fe, Ni and Co, Cu) doped graphene: A systematic DFT study. Phys. E Low-Dimens. Syst. Nanostructures 2020, 116, 113768. [Google Scholar] [CrossRef]
  31. Esrafili, M.D.; Sharifi, F.; Nematollahi, P. A comparative theoretical study of CO oxidation reaction by O2 molecule over Al- or Si-decorated graphene oxide. J. Mol. Graph. Model. 2016, 69, 8–16. [Google Scholar] [CrossRef]
  32. Kheirabadi, R.; Vakili, M. Computational modeling in enhanced CO2 and C2H2 capture on chalcogen atom (Se, Te)-decorated graphene: Structural and mechanistic aspects. J. Iran. Chem. Soc. 2021. [Google Scholar] [CrossRef]
  33. Kumar, R.; Suresh, V.M.; Maji, T.K.; Rao, C.N. Porous graphene frameworks pillared by organic linkers with tunable surface area and gas storage properties. Chem. Commun. 2014, 50, 2015–2017. [Google Scholar] [CrossRef]
  34. Salih, E.; Ayesh, A.I. Pt-doped armchair graphene nanoribbon as a promising gas sensor for CO and CO2: DFT study. Phys. E Low-Dimens. Syst. Nanostructures 2021, 125, 114418. [Google Scholar] [CrossRef]
  35. Jeziorski, B.; Moszynski, R.; Szalewicz, K. Perturbation Theory Approach to Intermolecular Potential Energy Surfaces of van der Waals Complexes. Chem. Rev. 1994, 94, 1887–1930. [Google Scholar] [CrossRef]
  36. Lefebvre, C.; Rubez, G.; Khartabil, H.; Boisson, J.-C.; Contreras-García, J.; Hénon, E. Accurately extracting the signature of intermolecular interactions present in the NCI plot of the reduced density gradient versus electron density. Phys. Chem. Chem. Phys. 2017, 19, 17928–17936. [Google Scholar] [CrossRef] [PubMed]
  37. Lefebvre, C.; Khartabil, H.; Boisson, J.-C.; Contreras-García, J.; Piquemal, J.-P.; Hénon, E. The Independent Gradient Model: A New Approach for Probing Strong and Weak Interactions in Molecules from Wave Function Calculations. ChemPhysChem 2018, 19, 724–735. [Google Scholar] [CrossRef] [PubMed]
  38. Bader, R.F.W. A quantum theory of molecular structure and its applications. Chem. Rev. 1991, 91, 893–928. [Google Scholar] [CrossRef]
  39. Umadevi, D.; Sastry, G.N. Molecular and Ionic Interaction with Graphene Nanoflakes: A Computational Investigation of CO2, H2O, Li, Mg, Li+, and Mg2+ Interaction with Polycyclic Aromatic Hydrocarbons. J. Phys. Chem. C 2011, 115, 9656–9667. [Google Scholar] [CrossRef]
  40. Wang, M.; Zhang, Z.; Gong, Y.; Zhou, S.; Wang, J.; Wang, Z.; Wei, S.; Guo, W.; Lu, X. Penta-graphene as a promising controllable CO2 capture and separation material in an electric field. Appl. Surf. Sci. 2020, 502, 144067. [Google Scholar] [CrossRef]
  41. Wang, C.; Fang, Y.; Duan, H.; Liang, G.; Li, W.; Chen, D.; Long, M. DFT study of CO2 adsorption properties on pristine, vacancy and doped graphenes. Solid State Commun. 2021, 337, 114436. [Google Scholar] [CrossRef]
  42. Cabrera-Sanfelix, P. Adsorption and reactivity of CO(2) on defective graphene sheets. J. Phys. Chemistry. A 2009, 113, 493–498. [Google Scholar] [CrossRef]
  43. Liu, Y.; Wilcox, J. CO2 adsorption on carbon models of organic constituents of gas shale and coal. Environ. Sci. Technol. 2011, 45, 809–814. [Google Scholar] [CrossRef] [PubMed]
  44. Cinke, M.; Li, J.; Bauschlicher, C.W.; Ricca, A.; Meyyappan, M. CO2 adsorption in single-walled carbon nanotubes. Chem. Phys. Lett. 2003, 376, 761–766. [Google Scholar] [CrossRef]
  45. Vidali, G.; Ihm, G.; Kim, H.-Y.; Cole, M.W. Potentials of physical adsorption. Surf. Sci. Rep. 1991, 12, 135–181. [Google Scholar] [CrossRef]
  46. Montoya, A.; Mondragón, F.; Truong, T.N. CO2 adsorption on carbonaceous surfaces: A combined experimental and theoretical study. Carbon 2003, 41, 29–39. [Google Scholar] [CrossRef]
  47. Okamoto, Y.; Miyamoto, Y. Ab Initio Investigation of Physisorption of Molecular Hydrogen on Planar and Curved Graphenes. J. Phys. Chem. B 2001, 105, 3470–3474. [Google Scholar] [CrossRef]
  48. Petrushenko, I.K.; Tikhonov, N.I.; Petrushenko, K.B. Hydrogen adsorption on pillar[6]arene: A computational study. Phys. E Low-Dimens. Syst. Nanostructures 2021, 130, 114719. [Google Scholar] [CrossRef]
  49. Petrushenko, I.K.; Bettinger, H.F. Hydrogen adsorption on inorganic benzenes decorated with alkali metal cations: Theoretical study. Phys. Chem. Chem. Phys. 2021, 23, 5315–5324. [Google Scholar] [CrossRef] [PubMed]
  50. Petrushenko, I.K.; Tsar’kova, A.I.; Petrushenko, K.B. Hydrogen adsorption on BN-embedded tetrabenzopentacene as a promising nanoflake for energy storage: Theoretical insights. Diam. Relat. Mater. 2020, 108, 107968. [Google Scholar] [CrossRef]
  51. Darvishnejad, M.H.; Reisi-Vanani, A. Multiple CO2 capture in pristine and Sr-decorated graphyne: A DFT-D3 and AIMD study. Comput. Mater. Sci. 2020, 176, 109539. [Google Scholar] [CrossRef]
  52. Venkataramanan, N.S.; Suvitha, A.; Kawazoe, Y. Intermolecular interaction in nucleobases and dimethyl sulfoxide/water molecules: A DFT, NBO, AIM and NCI analysis. J. Mol. Graph. Model. 2017, 78, 48–60. [Google Scholar] [CrossRef] [PubMed]
  53. Du, J.; Sun, X.; Zhang, L.; Zhang, C.; Jiang, G. Hydrogen storage of Li4&B36 cluster. Sci. Rep. 2018, 8, 1940. [Google Scholar] [CrossRef] [PubMed]
  54. Gal, J.F.; Maria, P.C.; Decouzon, M.; Mo, O.; Yanez, M.; Abboud, J.L. Lithium-cation/pi complexes of aromatic systems. The effect of increasing the number of fused rings. J. Am. Chem. Soc. 2003, 125, 10394–10401. [Google Scholar] [CrossRef]
  55. Sevilla, M.; Fuertes, A.B. CO2 adsorption by activated templated carbons. J. Colloid Interface Sci. 2012, 366, 147–154. [Google Scholar] [CrossRef] [Green Version]
  56. Himeno, S.; Komatsu, T.; Fujita, S. High-Pressure Adsorption Equilibria of Methane and Carbon Dioxide on Several Activated Carbons. J. Chem. Eng. Data 2005, 50, 369–376. [Google Scholar] [CrossRef]
  57. Zhao, Y.; Ding, H.; Zhong, Q. Preparation and characterization of aminated graphite oxide for CO2 capture. Appl. Surf. Sci. 2012, 258, 4301–4307. [Google Scholar] [CrossRef]
  58. Thiruvenkatachari, R.; Su, S.; Yu, X.X.; Bae, J.-S. Application of carbon fibre composites to CO2 capture from flue gas. Int. J. Greenh. Gas. Control. 2013, 13, 191–200. [Google Scholar] [CrossRef]
  59. Lee, C.; Yang, W.; Parr, R.G. Development of the Colle-Salvetti correlation-energy formula into a functional of the electron density. Phys. Rev. B 1988, 37, 785–789. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  60. Becke, A.D. Density-functional exchange-energy approximation with correct asymptotic behavior. Phys. Rev. A 1988, 38, 3098–3100. [Google Scholar] [CrossRef]
  61. Weigend, F.; Ahlrichs, R. Balanced basis sets of split valence, triple zeta valence and quadruple zeta valence quality for H to Rn: Design and assessment of accuracy. Phys. Chem. Chem. Phys. 2005, 7, 3297. [Google Scholar] [CrossRef]
  62. Grimme, S. Semiempirical GGA-type density functional constructed with a long-range dispersion correction. J. Comput. Chem. 2006, 27, 1787–1799. [Google Scholar] [CrossRef] [PubMed]
  63. Qu, Z.; Sun, F.; Liu, X.; Gao, J.; Qie, Z.; Zhao, G. The effect of nitrogen-containing functional groups on SO2 adsorption on carbon surface: Enhanced physical adsorption interactions. Surf. Sci. 2018, 677, 78–82. [Google Scholar] [CrossRef]
  64. Rafique, M.; Uqaili, M.A.; Mirjat, N.H.; Tunio, M.A.; Shuai, Y. Ab-initio investigations on titanium (Ti) atom-doped divacancy monolayer h-BN system for hydrogen storage systems. Phys. E Low-Dimens. Syst. Nanostructures 2019, 109, 169–178. [Google Scholar] [CrossRef]
  65. Muhammad, R.; Shuai, Y.; Irfan, A.; He-Ping, T. First-principles investigations of manganese oxide (MnOx) complex-sandwiched bilayer graphene systems. RSC Adv. 2018, 8, 23688–23697. [Google Scholar] [CrossRef] [Green Version]
  66. Muhammad, R.; Shuai, Y.; Tan, H.-P. First-principles study on hydrogen adsorption on nitrogen doped graphene. Phys. E Low-Dimens. Syst. Nanostructures 2017, 88, 115–124. [Google Scholar] [CrossRef]
  67. Rafique, M.; Shuai, Y.; Tan, H.-P.; Hassan, M. Manipulating intrinsic behaviors of graphene by substituting alkaline earth metal atoms in its structure. RSC Adv. 2017, 7, 16360–16370. [Google Scholar] [CrossRef] [Green Version]
  68. Hohenstein, E.G.; Sherrill, C.D. Density fitting and Cholesky decomposition approximations in symmetry-adapted perturbation theory: Implementation and application to probe the nature of π-π interactions in linear acenes. J. Chem. Phys. 2010, 132, 184111. [Google Scholar] [CrossRef] [Green Version]
  69. Hohenstein, E.G.; Sherrill, C.D. Wavefunction methods for noncovalent interactions. Wiley Interdiscip. Rev. Comput. Mol. Sci. 2012, 2, 304–326. [Google Scholar] [CrossRef]
  70. Turney, J.M.; Simmonett, A.C.; Parrish, R.M.; Hohenstein, E.G.; Evangelista, F.A.; Fermann, J.T.; Mintz, B.J.; Burns, L.A.; Wilke, J.J.; Abrams, M.L.; et al. Psi4: An open-source ab initio electronic structure program. Wiley Interdiscip. Rev. Comput. Mol. Sci. 2012, 2, 556–565. [Google Scholar] [CrossRef]
  71. Neese, F. Software update: The ORCA program system, version 4.0. Wiley Interdiscip. Rev. Comput. Mol. Sci. 2018, 8, e1327. [Google Scholar] [CrossRef]
  72. Berendsen, H.J.C.; Postma, J.P.M.; van Gunsteren, W.F.; DiNola, A.; Haak, J.R. Molecular dynamics with coupling to an external bath. J. Chem. Phys. 1984, 81, 3684–3690. [Google Scholar] [CrossRef] [Green Version]
  73. Gryn’ova, G.; Corminboeuf, C. Steric “attraction”: Not by dispersion alone. Beilstein J. Org. Chem. 2018, 14, 1482–1490. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  74. Hassan, A.; Dinadayalane, T.C.; Leszczynski, J. Effect of ring annelation on Li+–benzene interaction: A computational study. Chem. Phys. Lett. 2007, 443, 205–210. [Google Scholar] [CrossRef]
  75. Ma, J.C.; Dougherty, D.A. The Cation-pi Interaction. Chem. Rev. 1997, 97, 1303–1324. [Google Scholar] [CrossRef]
  76. Amicangelo, J.C.; Armentrout, P.B. Absolute Binding Energies of Alkali-Metal Cation Complexes with Benzene Determined by Threshold Collision-Induced Dissociation Experiments and ab Initio Theory. J. Phys. Chem. A 2000, 104, 11420–11432. [Google Scholar] [CrossRef]
  77. Petrushenko, I.K.; Shipitsin, N.V.; Petrushenko, K.B. Cation-π interactions of inorganic benzenes with Li, Na, and Mg cations: Theoretical insights. Inorg. Chem. Commun. 2020, 118, 108043. [Google Scholar] [CrossRef]
  78. Vijay, D.; Sakurai, H.; Subramanian, V.; Sastry, G.N. Where to bind in buckybowls? The dilemma of a metal ion. Phys. Chem. Chem. Phys. 2012, 14, 3057–3065. [Google Scholar] [CrossRef]
  79. Petrushenko, I.K.; Shipitsin, N.V.; Petrushenko, K.B. N-substituted sumanene and cation-π interactions towards Li cations: A theoretical study. Phys. E Low-Dimens. Syst. Nanostructures 2022, 135, 114949. [Google Scholar] [CrossRef]
  80. Reisi-Vanani, A.; Shabani, Z. Evaluation of the hydrogen adsorption onto Li and Li+ decorated circumtrindene (C36H12): A theoretical study. Int. J. Hydrogen Energy 2017, 42, 22973–22986. [Google Scholar] [CrossRef]
Molecules 26 07688 g001 550
Figure 1. Four (a), eight (b) and twelve (c) CO2 molecules adsorbed on Li+@coronene. The distances are in Å.
Figure 1. Four (a), eight (b) and twelve (c) CO2 molecules adsorbed on Li+@coronene. The distances are in Å.
Molecules 26 07688 g001
Molecules 26 07688 g002 550
Figure 2. Independent gradient model (IGM) analysis of CO2 adsorption (isovalue = 0.01). Atomic color code: carbon—blue-green, hydrogen—white, oxygen—red, lithium cation—pale red. Color code: green-colored lobes denote weak non-covalent interactions, blue lobes denote strong attractive interactions.
Figure 2. Independent gradient model (IGM) analysis of CO2 adsorption (isovalue = 0.01). Atomic color code: carbon—blue-green, hydrogen—white, oxygen—red, lithium cation—pale red. Color code: green-colored lobes denote weak non-covalent interactions, blue lobes denote strong attractive interactions.
Molecules 26 07688 g002
Molecules 26 07688 g003 550
Figure 3. Time evolution of Li+ shifts between each pair of consecutive steps at three studied temperatures.
Figure 3. Time evolution of Li+ shifts between each pair of consecutive steps at three studied temperatures.
Molecules 26 07688 g003
Table
Table 1. SAPT0/jun-cc-pVDZ energies (electrostatic (Eel), exchange (Eex), induction (Eind), dispersion (Edisp), and interaction (Eint)) for CO2 adsorption. The percentage contributions into attractive interactions are given in parentheses. All energies are in kcal/mol.
Table 1. SAPT0/jun-cc-pVDZ energies (electrostatic (Eel), exchange (Eex), induction (Eind), dispersion (Edisp), and interaction (Eint)) for CO2 adsorption. The percentage contributions into attractive interactions are given in parentheses. All energies are in kcal/mol.
No. CO2EelEexEindEdispEint
1−14.34
(50)		11.98−8.99
(31)		−5.52
(19)		−16.87
2−13.83
(47)		13.06−8.48
(29)		−7.32
(25)		−16.57
3−13.4
(49)		12.79−7.11
(26)		−6.57
(24)		−14.29
4−11.08
(45)		13.15−5.44
(23)		−7.89
(32)		−11.26
5−6.44
(44)		9.03−1.58
(10)		−6.75
(46)		−5.73
6−7.52
(46)		9.36−1.74
(11)		−6.95
(43)		−6.85
7−7.02
(46)		9.04−1.62
(11)		−6.65
(43)		−6.24
8−5.96
(44)		7.9−1.37
(10)		−6.13
(46)		−5.55
9−6.88
(48)		7.29−3.29
(22)		−4.28
(30)		−7.16
10−8.65
(47)		9.92−3.71
(20)		−5.96
(33)		−8.94
11−10.11
(48)		11.47−4.24
(20)		−6.85
(32)		−9.73
12−5.94
(48)		6.31−1.48
(12)		−5.03
(40)		−6.14
Table
Table 2. Selected QTAIM topological parameters (a.u.) for the systems studied.
Table 2. Selected QTAIM topological parameters (a.u.) for the systems studied.
Complexρ(r)∇2ρ(r)H(r)V(r)G(r)
1st CO20.02790.21170.0121−0.02870.0408
2nd CO20.02710.20840.0121−0.02790.0400
3rd CO20.02460.19130.0113−0.02520.0365
4th CO20.01600.11450.0065−0.01560.0221
9th CO20.01440.09690.0050−0.01430.0193
10th CO20.00680.02380.0005−0.00490.0054
11th CO20.00940.04150.0019−0.00670.0085
12th CO20.00770.03320.0016−0.00520.0067
Table
Table 3. Carbon dioxide GDs (wt.%) obtained from DFT and AIMD calculations.
Table 3. Carbon dioxide GDs (wt.%) obtained from DFT and AIMD calculations.
Li+@coronene
GD, DFTGD, AIMD
-77 K300 K400 K
5.0 (9.3) 15.0 (9.3)3.2 (6.0)2.6 (4.9)
1 Values in parentheses denote GDs upon double-side adsorption.
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Petrushenko, I.K.; Ivanov, N.A.; Petrushenko, K.B. Theoretical Investigation of Carbon Dioxide Adsorption on Li+-Decorated Nanoflakes. Molecules 2021, 26, 7688. https://doi.org/10.3390/molecules26247688

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Petrushenko IK, Ivanov NA, Petrushenko KB. Theoretical Investigation of Carbon Dioxide Adsorption on Li+-Decorated Nanoflakes. Molecules. 2021; 26(24):7688. https://doi.org/10.3390/molecules26247688

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Petrushenko, Igor K., Nikolay A. Ivanov, and Konstantin B. Petrushenko. 2021. "Theoretical Investigation of Carbon Dioxide Adsorption on Li+-Decorated Nanoflakes" Molecules 26, no. 24: 7688. https://doi.org/10.3390/molecules26247688

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