Maitreyi Robledo*a,
Sergio Díaz-Tenderoac,
Fernando Martínabc and
Manuel Alcamíab
aDepartamento de Química, Módulo 13, Universidad Autónoma de Madrid, 28049 Madrid, Spain. E-mail: Maitreyi.robledo@uam.es
bInstituto Madrileño de Estudios Avanzados en Nanociencias (IMDEA_Nanociencia), Cantoblanco, 28049, Spain
cCondensed Matter Physics Center (IFIMAC), Universidad Autónoma de Madrid, 28049 Madrid, Spain
First published on 10th March 2016
In this work we present a density functional theory study of the interaction between a positively charged exohedral metallofullerene and several hydrogen molecules. For this purpose we have chosen Li+, Ti+, V+ and Cu+ as the metal cations, since they represent a good sample of ionic or covalent interactions with the carbon cage. We have found that the interaction between the hydrogen molecules and the metal cation strongly depends on the type of interaction between the metal cation and the fullerene. Furthermore, the hydrogen saturation around the metal is also determined by the nature of the metal.
On the other hand, following this line of carbon structures, fullerenes have also been studied as promising hydrogen storage devices. A first approach mainly considered their capacity to store H2 inside the cage. For instance, C110 fullerene was found to encapsulate up to 19 H2 molecules;13 these hydrogen atoms cannot be attached to the inner wall of the structure and therefore they exist in their molecular form. Other studies14 have investigated, by molecular dynamics simulations, the possibility of H2 storage in carbon clusters (as well as in boron nitride clusters) finding out that H2 molecules are able to abide stable in a C60 fullerene at 298 K and 0.1 MPa, however it has been confirmed that pressures up to 5 MPa are needed to store H2 molecules in the C60 cage.
Recent studies5,15 propose to decorate carbon structures with metals, for instance titanium-decorated fullerenes5 or carbon nanotubes,16 as efficient materials to store H2. It was shown how a titanium atom coated on a single-walled nanotube or to a fullerene binds up to four hydrogen molecules, thus offering an efficient storage material for practical applications. Y. Zhao et al.16 showed by means of Density Functional Theory calculations that C60Sc12 could bind up to 5 hydrogen molecules per transition metal; with binding energy between 0.26 and 0.45 eV/H2 and storage density of 7 wt%. The main inconvenience using transition metals is that the former tend to cluster on the fullerene outer shell. Thus, an alkaline-earth metal as calcium,15,17 which binds directly to the hexagonal and pentagonal faces, without forming droplets, would be more suitable for the final goal of hydrogen storage. C60Ca32 can adsorb up to 62 H2 in two different layers. The first of them with an average binding energy of 0.45 eV/H and the second one, 0.11 eV/H2, which makes Ca coated C60 a practical hydrogen storage material at near ambient temperatures. Other promising elements to store hydrogen are alkaline metals such as lithium,18 since they enhance the H2 adsorption capacity of fullerenes; this effect is more pronounced for Na, with a hydrogen adsorption capacity of 9.5 wt%,19 than for Li. Other experimental studies20 have shown how a Li doped fullerene can reversibly desorb up to 5 wt% (at 270 °C), which is significantly less than the desorption temperature of an hydrogenated fullerene (C60Hx) (500–600 °C).
In this work we present a thorough study of the binding energies and geometries of a series of complexes of the form [C60M(H2)n]+, where M is Li, Ti, V or Cu and n = 1–5 hydrogen molecules. The choice of charged clusters is relevant since recent mass spectrometry experiments have allowed characterization of the sequential absorption of H2 molecules on C60 fullerenes21 as well as other molecules.22 Furthermore, Rao and Jena have shown23–25 that positively charged atoms would be able to bind a large amount of H2 molecules due to the charge polarization effect, which is in fact the main interaction mechanism we found between a metal cation and the fullerene cage in a previous work.26 All [M–C60]+ interactions are mainly governed by an ion-induced dipole interaction due to the positively charged metal and the large polarizability of the C60 cage. Concerning Li+ and Cu+ ions, our conclusion was that they present a larger ionic and covalent character, respectively; while for Ti+ and V+, the interaction between the metal and the carbon cage presented a shared character between ionic and covalent. Thus, in contrast with previous works we present four different metals (i.e. Li+, Cu+, Ti+ and V+), which interact distinctly with the C60 carbon cage (i.e. covalently, ionically or with a mixed character) and that present different abilities to storage H2 molecules, according to their type of interaction. We thus, provide a simple guide to predict the behavior of other metals coating the fullerene for their ability to storage H2.
Calculations were carried out with the Gaussian 09 program package.35 In order to determine the most stable isomer, we considered in our previous work26 5 types of initial geometries with the metal atom interacting with the fullerene external surface: the hexagonal (h) and pentagonal (p) rings, the double (hh) and single (hp) bonds and on top of a carbon atom (C). Furthermore, several spin multiplicities were also computed for the ground state. According to these results, we present here only the interaction between the most stable isomer for each [MC60]+ complex and the H2 molecules. This is for [C60Li]+ the h isomer with singlet spin multiplicity, for [C60Ti]+ the h isomer with quadruplet spin multiplicity, for [C60V]+ the h isomer with quintuplet spin multiplicity and the hh isomer with singlet spin multiplicity for [C60Cu]+.
The hydrogenation energy has been determined as follows:
EHyd = E[C60M(H2)n+] − (E[C60M(H2)n−1+] + E[H2]) |
We have as well calculated the adsorption energy per H2, defined as
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Fig. 1 Optimized structures for [C60Li(H2)n]+ and [C60Cu(H2)n]+, n = 1–5, with M06-2X/6-311++G(d,p). |
The result shows that the four systems present a certain limit number of hydrogen molecules that can be attached to the metal, i.e. there is a saturation limit. This limit is four hydrogen molecules for [C60Cu(H2)n]+, three H2 molecules for the [C60Li(H2)n]+ and [C60Ti(H2)n]+ systems and two H2 molecules for the [C60V(H2)n]+ (see Fig. 2). This behavior is observed at the three different levels of theory considered in this work. In fact the differences between the H2-cage distances, when H2 molecules are adsorbed to the metallofullerene system (i.e. when the saturation limit is not reached yet) is in the order of 0.5–2%. Although the three theory levels show similar trends, differences increase significantly (up to ∼30%) for those distances corresponding to H2 molecules weakly bound by the system. On the other hand, the H–H bond distances of H2 molecules in [C60Li]+ are 0.74 Å until saturation is reached (i.e. up to three hydrogen molecules), then it decreases (0.73 Å for [C60Li(H2)4]+ and [C60Li(H2)5]+). For [C60Ti]+, it changes from 0.76 Å to 0.73 Å in [C60Ti(H2)4]+ and [C60Ti(H2)5]+. For [C60V]+ it decreases from 0.76 Å when the complex is not saturated to 0.73 Å from the third H2 molecule onwards. And finally, for [C60Cu]+ it changes from 0.76 Å up to saturation of the complex to 0.75 Å in [C60Cu(H2)3]+ and 0.73 Å in [C60Cu(H2)4]+ and [C60Cu(H2)5. Hence, the H–H distance increases when the H2 molecule is interacting with the metal cation.
This is a consequence of the H–H bond disruption by the metal; similar results were obtained by previous works5 on C60Ti12 where it was described that each Ti atom was able to bind 4 H2 molecules, but the first one was attached as a single H atom to Ti. Thus, the metal cation prefers to attach one single H atom, and form the hydride.
Fig. 3 shows the hydrogenation energy and the total adsorption energy per H2, as defined before. Among the four studied metals, Li shows the lowest adsorption energies and its saturation limit is reached almost at 3 H2 molecules. The interaction is caused by a polarization of the hydrogen molecule by the Li+ cation, which results in an electrostatic interaction between the metallofullerene and the H2 molecule.
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Fig. 3 Hydrogenation energy, EHyd., and adsorption energy, EAds., in kcal mol−1, for [C60Li(H2)n]+, where M = Li, Ti, V, Cu and n = 1–5. |
Ti hydrated complexes also show a saturation limit of 3 H2 molecules, though adsorption energies are larger (∼5 kcal mol−1) compared to [C60Li(H2)n]+. [C60V(H2)n]+ shows a saturation limit of two hydrogen molecules, and the third H2 molecule releases ∼7 kcal mol−1 to be adsorbed. Among all the studied metals, Cu has the lowest H2 adsorption capability; [C60Cu(H2)]+ releases almost 10 kcal mol−1 to attached a second H2 molecule. All the studied complexes show an electrostatic interaction due to polarization. However, the adsorption energies are significantly larger for Ti, V and Cu, than for Li, especially for the adsorption of the first H2 molecule (5.56 kcal for TiC60+, 8.77 kcal for VC60+ and 10.10 kcal for CuC60+). Furthermore, if we take into account our previous conclusions on the type of interaction between these cations and the fullerene cage,26 we can establish a relation between the pure interaction M+–C60 and the adsorption energies H2–MC60+: Cu interacts with the carbon cage with larger covalent character and therefore presents a stronger M–C binding. This feature involves stable adsorption of the hydrogen molecules as well as high adsorption energy. On the other hand, Ti+ and V+ present a shared character, in between ionic and covalent, in their interaction with the fullerene. The double character of the M+–C60 binding will enhance this polarization and consequently the adsorption energies will be higher when more than one H2 molecule is adsorbed by the metallofullerene. The enhancement of the adsorption energy is due to the polarization that the positive metal exerts on the H2 molecule.
In order to give a deeper insight on the interaction, we have also evaluated the charge, in the framework of the Mulliken population analysis, on the metal cation after the interaction, as well as the charge on each H2 molecule after adsorption to the hydrated complex (see Fig. 4). The metal cation is initially charged with one single positive charge. The interaction between the metal cation and the fullerene cage involves the polarization of the latter by the former and, thus a gain of electron density (reducing the charge on the metal). This leads to a very localized reactivity, which results in the involvement of the closest carbon atoms in the interaction with the metal cation.
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Fig. 4 Charge localized on the metal cation and the surrounding hydrogen molecules, with the Mulliken approach. |
When hydrogen molecules are added to the MC60+ complex, positive charge decreases on the metal and increases in some of the hydrogen molecules. This loss of neutrality by the H2 molecules, once attached to the complex, is the signature of the induced polarizability and thus, of induced dipole type of interaction between the metal and the H2 molecule. The charge in the metal is reduced and also shows a limit similar to the saturation limit.
This study provides important new insight into the adsorption of hydrogen molecules in exohedral metalofullerenes cationic complexes, showing the importance of the charge and the correct choice of a metal for hydrogen storage at the nanoscale.
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