Reversible Hydrogen Storage Media by g-CN Monolayer Decorated with NLi₄: A First-Principles Study

Abstract

A two-dimensional graphene-like carbon nitride (g-CN) monolayer decorated with the superatomic cluster NLi₄ was studied for reversible hydrogen storage by first-principles calculations. Molecular dynamics simulations show that the g-CN monolayer has good thermal stability at room temperature. The NLi₄ is firmly anchored on the g-CN monolayer with a binding energy of −6.35 eV. Electronic charges are transferred from the Li atoms of NLi₄ to the g-CN monolayer, mainly due to the hybridization of Li(2s), C(2p), and N(2p) orbitals. Consequently, a spatial local electrostatic field is formed around NLi₄, leading to polarization of the adsorbed hydrogen molecules and further enhancing the electrostatic interactions between the Li atoms and hydrogen. Each NLi₄ can adsorb nine hydrogen molecules with average adsorption energies between −0.152 eV/H₂ and −0.237 eV/H₂. This range is within the reversible hydrogen storage energy window. Moreover, the highest achieved gravimetric capacity is up to 9.2 wt%, which is superior to the 5.5 wt% target set by the U.S. Department of Energy. This study shows that g-CN monolayers decorated with NLi₄ are a good candidate for reversible hydrogen storage.

1. Introduction

Hydrogen energy is a promising alternative to traditional fossil fuels due to its highest energy density and the environmental friendliness of its combustion products. Therefore, interest in hydrogen storage is growing due to increasing environmental protection requirements and the trend of low-carbon development. It is expected that the demand in the global hydrogen storage market will expand at a rate of 5.8% from 2019 to 2025 [1]. However, there is a gap between this demand and existing storage technology, where materials play a critical role.

Conventional strategies such as high-pressure compression and liquefaction suffer from low safety and high cost [2]. Therefore, solid-state hydrogen storage is becoming an attractive alternative. A suitable storage medium should have good reversibility between adsorption and desorption and an adequate binding energy of about −0.1 to −0.2 eV per H₂ [3]. The energy requirement for reversible adsorption just falls into the range of physical adsorption, which guarantees reversible and fast dynamics. Motivated by this consideration, researchers have focused on various nanostructured materials, including two-dimensional (2D) sheets (boron-based nanomaterials, graphene-like nanomaterials, MXenes, MoS₂, CxNy, etc.) [4,5,6,7,8,9,10,11,12,13], metal atom-modified covalent organic frameworks (COFs) [14,15,16], and metal organic frameworks (MOFs) [17,18,19,20,21]. These materials can exhibit significantly improved kinetics during the adsorption process by decreasing the enthalpy of formation and hydrogenation temperature, and they exhibit many other catalytic effects [22,23,24].

Two-dimensional materials are believed to provide a pathway for the design of next-generation hydrogen storage media due to their superior physical and chemical properties, including their large surface-to-volume ratios, abundant active sites, light weight, and adjustability [25]. However, it is challenging for 2D materials to directly adsorb H₂ molecules because pure 2D materials fail to provide strong electrostatic interaction. The adsorption energies of H₂ on graphene and BN are only 0.07 eV [26] and 0.03 eV [27], respectively. Therefore, modification and decoration are necessary to improve their storage capacity. Some research has demonstrated that dopants such as alkali metals, alkaline earth metals, transition metals, and functional groups can improve the storage ability of pristine 2D sheets [26,27,28,29,30,31,32,33,34]. Decorating Mg [28], Ti [35], Ca [36], and Li [26] on graphene-like or carbon-based sheets can provide gravimetric capacities in the range of 7.96 wt% to 10.81 wt%, which meet the 5.5 wt% target value proposed by the U.S. Department of Energy (DOE) in 2020. In addition to single particles, superatomic clusters such as NLi₄ are also an eye-catching option. The suitability of these clusters has been confirmed by time-of-flight powder neutron diffraction experiments [37,38]. Like alkali metal ions, NLi₄ has low ionization potentials, which means that decorated NLi₄ can easily transfer electrons to the substrate and become positively charged. Consequently, an enhanced local electrostatic field can be obtained, which is beneficial for improving hydrogen storage capacity compared to the use of single particles. However, unlike their alkali metal counterparts, the robust binding of Li-N provides superior stability for these clusters. This guarantees a stable connection between the clusters and substrate in addition to less aggregation between the clusters. Some research has provided theoretical support for the significant potential of NLi₄ for hydrogen storage [33,38,39]. ** and hydrogen storage. The PDOS for the 2s/2p orbitals of the nitrogen and carbon atoms in the g-CN monolayer were calculated, as presented in Figure 2. Hybridizations exist between the C-2p and N-2p orbitals in the energy range of −6 eV to 4 eV, and the valence bands are mainly occupied by C-2p and N-2p. The band gap of g-CN is about 1.3 eV, i.e., the g-CN is a semiconductor. The thermodynamic stability of the g-CN monolayer at room temperature (300 K) was estimated by first-principles molecular dynamics (MD) simulation with the Nose–Hoover thermostat algorithm. As shown in Figure 3, the system energy slightly oscillates around −406.5 eV. Even after exerting thermal perturbation, the original planar structure with the CN 6-membered rings and 18-membered rings is well-retained, reflecting the good thermodynamic stability of the g-CN.

The porous structure of the g-CN monolayer makes it an ideal host for various dopants, including metal atoms and nanoclusters. According to the DFT calculation, the four possible binding sites of NLi₄ on the g-CN monolayer were tested, including the inner cavity of the large CN 18-membered ring in the center, and the inner cavity of the surrounding small NC rings, C-C bonds, and C-N bonds. It was determined that NLi₄ can be easily doped on the cavity formed by the large CN 18-membered rings via the formation of ionic bonds between the Li atoms of the NLi₄ cluster and the N atoms of the g-CN, as shown in Figure 4. The binding energy E_b was also calculated according to Formula (1) [55].

$${\mathrm{E}}_{\mathrm{b}}={\mathrm{E}}_{{\mathrm{NLi}}_4\text{@}\mathrm{g}-\mathrm{CN}}-{\mathrm{E}}_{{\mathrm{NLi}}_4}-{\mathrm{E}}_{\mathrm{g}-\mathrm{CN}}$$

(1)

where ${\mathrm{E}}_{{\mathrm{NLi}}_4\text{@}\mathrm{g}-\mathrm{CN}}$, ${\mathrm{E}}_{{\mathrm{NLi}}_4}$, and ${\mathrm{E}}_{\mathrm{g}-\mathrm{CN}}$ are the energies of the single NLi₄-decorated g-CN monolayer, an isolated NLi₄ cluster, and the pure g-CN monolayer, respectively. The binding energy of NLi₄ and g-CN is −6.35 eV, meaning that a stable interaction exists between NLi₄ and the g-CN monolayer. The top and side views of the optimized NLi4@g-CN structure (Figure 4) show that g-CN is not twisted by the decoration of NLi₄. Therefore, the complex still has a high surface-to-volume ratio. The side view shows that the superatomic cluster has a “pyramid building” appearance on the g-CN surface. This is a stable connection and provides enough space for subsequent H₂ adsorption.

The nature of the interaction between the NLi₄ dopant and g-CN was investigated by PDOS and charge density difference analysis. NLi₄ decoration can improve the conductivity of g-CN, supporting our assumption that binding formation and charge transfer occur between NLi₄ and g-CN. Figure 5 shows that the bandgap disappears at the Fermi level, indicating the transformation of the complex from semiconductor to conductor due to the do** of NLi₄. Clear hybridization between the Li(2s) orbital and the C(2p)/N(2p) orbitals is present at −0.2 and −0.5 eV below the Fermi level, indicating that charge transfer and the formation of ion bonds occur during the combination process. The charge density difference of NLi₄@g-CN (Figure 6) also provides evidence for this mechanism. There is a clear charge transfer from NLi₄ to the substrate g-CN. NLi₄ loses part of its charge, displaying electronegativity. Meanwhile, the g-CN gains charge and displays electropositivity. Thus, a polarization field is formed around NLi₄, paving the way for subsequent H₂ adsorption. In addition, the highly charged NLi₄ superatomic clusters strongly repel each other, which inhibits the aggregation of NLi₄ molecules. To quantitatively investigate the charge transfer between the dopants and substrate, Bader charge analysis was performed, showing that this transformation is about 0.87 e⁻/atom. This indicates that bonding is formed by strong ionic interaction between the NLi₄ clusters and g-CN. In other words, a novel material was developed by decorating NLi₄ on a g-CN monolayer with a large surface-to-volume ratio and favorable electron structure. This is highly promising for achieving excellent H₂ adsorption performance.

4. Hydrogen Adsorption Performance of NLi₄@g-CN

To thoroughly investigate the H₂ adsorption performance of the NLi₄@g-CN monolayer, hydrogen molecules were systematically added to the top and side of the Li ions of NLi₄, followed by structural optimization to obtain the most stable configurations. The corresponding results are shown in the Figure 7. Each NLi₄ anchored on the g-CN can accommodate a maximum of nine H₂ molecules. As displayed in Figure 6, the Li ions of the NLi₄ cluster partially transfer their charge to the substrate, forming a local electrostatic field around the NLi₄ decoration sites. This is favorable for hydrogen adsorption. This assumption also was confirmed by charge density difference analysis of the NLi₄@g-CN with adsorbed H₂, as shown in Figure 8. The notable positive electronic potential around the Li of the NLi₄ superatomic cluster induces the adsorbed H₂ to have an unbalanced charge distribution. The center of the H-H bond is a charge-abundant area while the ends are charge-deficient, indicating the polarization of the H₂ molecules. Therefore, H₂ is smoothly adsorbed by NLi₄@g-CN due to the polarization mechanism, and the length of the H-H bond is elongated to 0.76 Å (the bond length of free H₂ is 0.75 Å [11]). To perform a more quantitative analysis, the average adsorption energy per H₂ and storage capacity were calculated using Formulas (2) and (3). The average adsorption energy per H₂ can be written as:

$${\mathrm{E}}_{\mathrm{ad}}=({\mathrm{E}}_{{\mathrm{NLi}}_4{\text{@}\mathrm{g}-\mathrm{CN}-\mathrm{nH}}_2}-{\mathrm{E}}_{{\mathrm{NLi}}_4\text{@}\mathrm{g}-\mathrm{CN}}-n{\mathrm{E}}_{{\mathrm{H}}_2})/n$$

(2)

where ${\mathrm{E}}_{\mathrm{ad}}$, ${\mathrm{E}}_{{\mathrm{NLi}}_4{\text{@}\mathrm{g}-\mathrm{CN}-\mathrm{nH}}_2}$, ${\mathrm{E}}_{{\mathrm{NLi}}_4\text{@}\mathrm{g}-\mathrm{CN}}$, ${\mathrm{E}}_{{\mathrm{H}}_2}$, and $n$ are the average adsorption energy per H₂, the energy of the NLi₄-decorated g-CN monolayer with adsorbed H₂, the energy of the NLi₄@g-CN complex, the energy of a single H₂, and the number of H₂ molecules, respectively. The storage capacity can be defined as:

$${\mathrm{W}}_{\mathrm{t}}=\frac{n(\mathrm{H})*\mathrm{M}(\mathrm{H})}{[n(\mathrm{C})*\mathrm{M}(\mathrm{C})+n(\mathrm{N})*\mathrm{M}(\mathrm{N})+n\left(\mathrm{Li}\right)*\mathrm{M}\left(\mathrm{Li}\right)]}$$

(3)

where ${\mathrm{W}}_{\mathrm{t}}$, $n(\mathrm{H})$, $n(\mathrm{C})$,$n(\mathrm{N})$, and $n\left(\mathrm{Li}\right)$ denote the storage capacity of the complex and the number of H, C, N, and Li atoms, respectively. $\mathrm{M}(\mathrm{H})$, $\mathrm{M}(\mathrm{C})$, $\mathrm{M}(\mathrm{N})$, and $\mathrm{M}\left(\mathrm{Li}\right)$ denote the molar masses of H, C, N, and Li atoms, respectively. The calculated results are listed in

Table 1. Caption. The average adsorption energy per H₂, average bond length of H-H, hydrogen storage density and desorption temperature of H₂ in g-CN system decorated with NLi₄.

Systems	Ead (eV)	RH-H Length (A)	HSC (wt%)	Td (k)
1NLi4@g-CN 1H2	−0.237	0.76	0.30	303
1NLi4@g-CN 8H2	−0.177	0.76	2.42	227
1NLi4@g-CN 9H2	−0.170	0.76	2.70	217
2NLi4@g-CN 18H2	−0.155	0.76	5.10	198
3NLi4@g-CN 27H2	−0.152	0.76	7.30	194
4NLi4@g-CN 36H2	−0.155	0.76	9.20	198

.

To systematically estimate the conditions for hydrogen desorption from NLi₄@g-CN, the desorption temperature was calculated by the van’t Hoff equation, which can be written as:

$${\mathrm{T}}_{\mathrm{d}}=\frac{{\mathrm{E}}_{\mathrm{ad}}}{{\mathrm{K}}_{\mathrm{B}}}{(\frac{\mathsf{\Delta }\mathrm{S}}{\mathrm{R}}-\mathrm{lnp})}^{-1}$$

(4)

where ${\mathrm{T}}_{\mathrm{d}}$, ${\mathrm{E}}_{\mathrm{ad}}$, ${\mathrm{K}}_{\mathrm{B}}$, $\mathsf{\Delta }\mathrm{S}$, $\mathrm{R}$ and $\mathrm{p}$ are the desorption temperature, the average adsorption energy per H₂, Boltzmann’s constant, the entropy change of H₂ from gas to solid, the universal gas constant, and the equilibrium pressure, respectively [56]. This work focused on the desorption temperature T_d at standard atmospheric pressure, so $\mathrm{p}$ = 1 atm and $\mathsf{\Delta }\mathrm{S}$ = 75.44 J K⁻¹ mol⁻¹ were used for calculation. The estimated desorption temperatures are also listed in Table 1. Table 1 shows that the R_H-H value is about 0.76 Å and the T_d is between 198–303 K, which is much higher than the critical temperature of H₂. The average adsorption energy per H₂ is in the range of −0.152 eV to −0.237 eV, which falls into the range of appropriate reversible adsorption energy. Table 1 also shows that for a single NLi₄ superatomic cluster, the average adsorption energies per H₂ are negatively correlated with the number of adsorbed H₂ molecules, which means that the average adsorption energy per H₂ decreases with increasing H₂ loading. This is caused by the repulsion among the adsorbed H₂, which is in agreement with the behavior reported in Ref. [11]. With an increasing number of NLi₄ clusters, the adsorption energies per H₂ maintain proximity as a constant, which means that the storage capacity of g-CN is largely determined by the number of NLi₄ superatomic clusters. Finally, the highest gravimetric capacity is 9.2 wt%, which surpasses the DOE target of 5.5 wt%.

5. Conclusions

In summary, we proposed a promising NLi₄-decorated g-CN material and estimated its performance for H₂ storage by first-principles calculations. The NLi₄ superatomic cluster can be firmly anchored on a g-CN monolayer with a bonding energy of −6.35 eV. The adsorption energies for H₂ are between −0.152 eV and −0.237 eV, lying within the range of reversible hydrogen storage. Moreover, the storage capacity is as high as 9.2 wt%, which is much higher than the benchmark set by the U.S. DOE. This superior hydrogen storage capacity is attributed to the formation of a spatial local electrostatic field around the NLi₄ caused by charge transfer from the NLi₄ superatomic cluster to the g-CN. Hydrogen molecules tend to be polarized due to the formation of this electrostatic field. Thus, electrostatic interaction is enhanced between the hydrogen molecules and the substrate and the adsorption capacity is favorably improved. In addition, the spatial and electronic properties of the NLi₄ cluster inhibit NLi₄ aggregation and the repulsion between multiple H₂ molecules. In the future, we hope that more advanced hydrogen storage materials will be developed along this direction.