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Neutral and charged boron-doped fullerenes for CO2 adsorption

  1. ,
  2. ,
  3. and
School of Chemistry, Physics and Mechanical Engineering, Queensland University of Technology, Brisbane 4001, Australia
  1. Corresponding author email
This article is part of the Thematic Series "Nanostructures for sensors, electronics, energy and environment II".
Guest Editor: N. Motta
Beilstein J. Nanotechnol. 2014, 5, 413–418. https://doi.org/10.3762/bjnano.5.49
Received 20 Dec 2013, Accepted 12 Mar 2014, Published 07 Apr 2014
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Abstract

Recently, the capture and storage of CO2 have attracted research interest as a strategy to reduce the global emissions of greenhouse gases. It is crucial to find suitable materials to achieve an efficient CO2 capture. Here we report our study of CO2 adsorption on boron-doped C60 fullerene in the neutral state and in the 1e−-charged state. We use first principle density functional calculations to simulate the CO2 adsorption. The results show that CO2 can form weak interactions with the BC59 cage in its neutral state and the interactions can be enhanced significantly by introducing an extra electron to the system.

Keywords: adsorption; boron doping; CO2 capture; density functional theory (DFT); heterofullerene

Introduction

The continuous dependence on fossil fuel combustion for the generation of energy has dramatically increased the atmospheric CO2 concentrations over the last century. Despite concerns for global climatic changes and many attempts to sustainably generate energy, fossil fuel combustion continues to be the main source of electricity while releasing 13 Gt of CO2 [1] to the atmosphere each year. Therefore CO2 capture and storage (CCS) technology is a promising solution to reduce atmospheric CO2 emissions [2]. Solvent absorption that is based on amines is the most common technology for the capture of CO2. However this method is criticized for its very high energy consumption and operational limitations such as corrosion, slow uptake rates, foaming and large equipment. Hence there is a huge interest in solid adsorbent materials for CCS [3-6]. In past few years metal organic frameworks (MOFs) have emerged as solid CO2 adsorbent materials due to their tuneable chemical and physical properties.

Particularly, there is growing interest for metal free carbon-based nanomaterials for gas adsorption. Carbon-based nanomaterials such as fullerene, carbon nanotubes and graphene offer excellent thermal and chemical stability as CO2 adsorbents [7,8]. Heterofullerenes are fullerene structures in which one or more cage carbon atoms are substituted by heteroatoms [9]. In addition to the properties mentioned above, which are inherent to carbon-based nanomaterials, heterofullerenes also offer excellent tuneable chemical and physical properties [10]. Gas adsorption on heterofullerenes is an appealing subject. B. Gao et al. [11] studied CO2 adsorption on calcium decorated C60 fullerene and F. Gao et al. [12] studied O2 adsorption on nitrogen-doped fullerene.

Boron-doped C60 fullerenes are one of the most structurally stable heterofullerenes [9]. Guo et al. synthesized B-doped C60 fullerenes for the first time, in microscopic amounts by laser vaporisation [13]. Zou et al. [14] demonstrated the synthesis of B-doped C60 fullerene by using radio frequency plasma-assisted vapour deposition. Recently Dunk et al. [15] introduced a method to produce BC59 directly from exposing C60 fullerene to boron vapour. Wang et al. [16] stated that substituting a single C atom of the C60 fullerene with a B atom does not cause a significant distortion in the cage structure. The net change in the dihedral angle due to the doping is only 1.6% and Kurita et al. [17] predicted that due to the similarity between the C–B bond and the C–C bond, the changes in the bond lengths are less than 5%. Therefore the BC59 fullerene has a similar structural and thermal stability as C60 fullerene. Despite the numerous study results, which confirm the structural stability of B-doped C60 fullerene, very little studies have been done on applications of B-doped fullerene. Here, for the first time we report a study about the CO2 adsorption on B-doped C60 fullerene, in which a single C atom is replaced with a B atom.

Sun et al. [8] predicted an enhanced CO2 adsorption on 1e−- and 2e−-charged boron nitride sheets and nanotubes, which show very little chemical affinity towards CO2 in their neutral state. Also Sun et al. [18] showed that chemical interactions between boron–carbon nanotubes (B2CNT) and CO2 can be enhanced by introducing extra electrons to the system. The enhanced interaction of CO2 with adsorbent materials by electron injection has been further proved by Jiao et al. [19]. Therefore, we will investigate the CO2 adsorption on BC59 fullerene in both the neutral and the 1e−-charged states.

Computational Details

First-principles density functional theory (DFT) calculations were carried out to study CO2 adsorption on the BC59 cage. The BC59 structure was fully optimized in the given symmetry. The calculations were carried out at B3LYP [20-22] level of theory while using the split valance polarized basis set 6-31G(d). B97d [23,24] with the same basis set was used for calculations when non-covalent interactions are predominant. The CO2 adsorption on BC59 was studied in the neutral state and in the 1e−-charged state. The electron distribution and transfer were analysed with Mulliken population analysis method [25]. The adsorption energies were calculated using the following equation.

[2190-4286-5-49-i1]
(1)

where Eads is the adsorption energy, [Graphic 1] is the total energy of the BC59 cage with a CO2 molecule adsorbed and [Graphic 2] and [Graphic 3] are the energies of the isolated BC59 cage and CO2 molecule, respectively. For a favourable adsorption the calculated adsorption energy should have a negative value. To provide more accurate results for the chemisorption energy the counterpoise corrected energy [26,27] was also calculated.

The transition state was located by using the synchronous transit-guided quasi-Newton (STQN) method [28,29], which was then fully optimized by using the Berny algorithm at the B3LYP/6-31G(d) level. The optimized transition structure was used for IRC calculations at the same level of theory [30,31]. All calculations were carried out by using the Gaussian 09 package [32]. The GaussView 5 package [33] was used to visualize the optimized molecular structures, molecular orbitals and charge distributions.

Results and Discussion

The substitution of a C atom in the C60 fullerene by a B atom causes a charge transfer between C and B atoms, which results in an unbalanced charge distribution in the fullerene cage. The unbalanced charge distribution forms B–C complex sites for the adsorption of CO2 (Figure 1). Here we considered two possible sites for the CO2 adsorption: the B–C atomic site between two hexagonal rings (HH B–C site) and two identical B–C sites between a hexagonal ring and pentagonal ring (HP B–C site).

[2190-4286-5-49-1]

Figure 1: Sites for CO2 adsorption on BC59. The B and C atoms of HH B–C and HP B–C sites are represented as ‘ball and bond’-type and the rest of the atoms are represented as ‘wireframes’. Atom colour code: grey, carbon; pink, boron.

Adsorption of CO2 on uncharged BC59 fullerenes

According to our simulation results, the CO2 molecules can only form weak interactions with BC59 cage in its neutral state. The physisorption energy is a weak −2.04 kcal/mol (−4.1 kcal/mol for B97D/6-31G(d) calculations) and the weak interactions are mainly van der Waals interactions between the CO2 molecule and the adsorbent. The CO2 physisorbed configuration is shown in Figure 2. The CO2 molecule sits parallel to the boron–carbon plane of the BC59 fullerene cage. The B…O and C…O bond distances are 3.25 Å and 3.71 Å, respectively. The CO2 molecule undergoes very slight structural changes upon physisorption on the uncharged BC59 fullerene cage. The O–C–O angle is slightly bent to 179.7° and the changes to the C=O bond lengths are negligibly small. The doped fullerene cage hardly undergoes any structural change. The charge transfer between CO2 and BC59 is only 0.008e.

[2190-4286-5-49-2]

Figure 2: Configuration of physisorbed CO2 on neutral BC59. Atom colour code: grey, carbon; pink, boron; red, oxygen.

Effects of charges on the structure

Kim et al. [34] predicted that C59B− should be a stable entity because of the isoelectronic configuration with C60. This claim is further validated by experimental observations by Dunk et al. [15]. The Mulliken charge analysis and the electron density distributions of the lowest unoccupied molecular orbitals (LUMO) are adopted to assess the influence of changing the charge state of BC59. Figure 3 shows that the LUMO of the neutral BC59 is noticeably concentrated on the B atom and the neighbouring C atoms. Furthermore experimental results of Guo et al. [13] showed that boron doping creates an electron defficient site at the B atom. This suggests that an additional electron added to the system will be accepted by the B atom. This hypothesis is consistent with theoretical predictions of Kurita et al. [17] and Xie et al. [35], who stated that the doped B atom in C60 fullerene acts as an electron acceptor. The comparison of the Mulliken population analysis of the neutral and the 1e−-state of BC59 proves that the negative charge introduced to the system is essentially accepted by the B atom. The Mulliken atomic charge of the B atom in the BC59 structure in the neutral state has changed from 0.138 to 0.012 upon the introduction of the negative charge, while as shown in Figure 4 the charges on the C atoms are not changed significantly.

[2190-4286-5-49-3]

Figure 3: LUMO of neutral BC59. The orbitals are drawn at an isosurface value of 0.02. The colours of the orbitals: red, positive wave function; green, negative wave function. Atom colour code: pink, boron; grey, carbon.

[2190-4286-5-49-4]

Figure 4: Mulliken charge distribution of (a) neutral BC59 and (b) 1e−-BC59. The atoms are shaded based on the charge distribution on each atom. The comparison suggests that the most notable charge transfer is on the B atom.

CO2 adsorption on BC59 fullerene in the 1e−-state

Next we studied the CO2 adsorption on a 1e−-charged BC59 cage. The results confirm that the negatively charged BC59 fullerene exhibits a stronger interaction with CO2. Unlike the neutral BC59, for which the interaction with CO2 molecule was only physical, here the charged BC59 forms a substantial chemical interaction with CO2 causing the molecule to undergo significant structural deformations. A stable CO2 adsorption is observed at the HH B–C site. The chemisorption energy of −15.41 kcal/mol (−64.48 kJ/mol) (−13.48 kcal/mol with BSSE correction) agrees well with the ideal range of chemisorption energy (40–80 kJ/mol) for a good CO2 adsorbent [36].

The CO2 molecule undergoes considerable distortion upon chemically adsorbing on the 1e−-charged BC59 fullerene. A C=O bond of the CO2 molecule is broken when one oxygen atom forms a bond with the boron atom (which will be referred as Oa in the following discussion and the other oxygen atom as Ob) and the C atom of the CO2 molecule forms a bond with the C atom on the HH B–C site of the cage structure. The linear O–C–O bond of CO2 is bent to 128.0° in the adsorbed form. The C=Ob bond which is originally 1.169 Å (experimentally 1.162 Å [37]) is elongated to 1.208 Å, while the length of the C–Oa bond is expanded to 1.336 Å.The adsorption site of the BC59 fullerene also undergoes considerable stretching. The HH B–C site is protruded outwards by about 0.05 Å. The B–C bond of the HH B–C site has stretched from 1.496 to 1.672 Å. The Mulliken population analysis shows that a charge transfer of 0.42 has occurred from the BC59 fullerene to the CO2 molecule. Comparison of the charge distribution on BC59− before (Figure 4b) and after (Figure 5c) CO2 adsorption, confirms that the injected electron is occupied by the CO2 molecule.

[2190-4286-5-49-5]

Figure 5: (a) CO2 chemisorption and (b) transition structure for CO2 chemisorption on 1e−-charged BC59. Atom colour code: grey, carbon; pink, boron; red, oxygen. (c) Charge distribution after CO2 chemisorption.

The higher adsorption energy and the significant distortions in the structure confirm a stronger interaction between CO2 molecule and negatively charged BC59 than its neutral state. These interactions can be explained due to the Lewis acidity of CO2, which prefers to accept electrons [18]. On the other hand the B atom of the BC59 becomes less positively charged upon the addition of an extra electron. Therefore it becomes more likely to donate electrons to the CO2 molecule leading to stronger interactions between the two molecules.

Figure 6 shows the minimum energy pathway for the adsorption from the physisorbed state to the chemisorbed configuration. We performed frequency calculations on the optimized transition structure, which confirms that it is a first order saddle point and hence an actual transition structure. From this figure, the activation barrier for the chemisorption is estimated to be 13.25 kcal/mol (55.43 kJ/mol). The low barrier of the reaction indicates that the reaction is energetically favourable.

[2190-4286-5-49-6]

Figure 6: Intrinsic reaction pathway for CO2 chemisorption on 1e−-charged BC59 from the physisorbed configuration. The total energy = 0 point corresponds to the total energy of ECO2 + EBC59−1.

For the desorption step, the removal of the added charge will decrease the stability of the bond between CO2 and the doped fullerene. The thermodynamic analysis of the reaction shows that the CO2 chemisorption is spontaneous only for temperatures less than 350 K. Therefore we suggest a method of manipulating the charge state and the temperature of the system for adsorbent recycling. Charging the system can be achieved by electrochemical methods, electrospray, and electron beam or gate voltage control methods [8].

Conclusion

By using DFT calculations we have studied the adsorption mechanisms of CO2 on a C60 fullerene cage, in which a single C atom is substituted by a B atom. Our calculation results show that the BC59 cage, in its neutral state, shows a low chemical interaction with CO2 molecule, which only physisorbs with Eads = −2.04 kcal/mol. However CO2 adsorption on the BC59 can be significantly enhanced by injecting negative charges into the structure. The CO2 molecule chemisorbs on the 1e−-charged BC59 with Eads = −15.41 kcal/mol. This study suggests that we can conclude 1e−-charged BC59 cage structure is a promising CO2 adsorbent.

Acknowledgements

Support provided by the ARC Discovery grant (DP130102120) and the High Performance Computer (HPC) resources in Queensland University of Technology (QUT) are gratefully acknowledged.

References

  1. International Energy Agency, Ed. World Energy Outlook 2011; IEA Publications: Paris, 2011.
    Return to citation in text: [1]
  2. Kheshgi, H.; de Coninck, H.; Kessels, J. Mitigation and Adaptation Strategies for Global Change 2012, 17, 563–567. doi:10.1007/s11027-012-9391-5
    Return to citation in text: [1]
  3. Lee, K. B.; Sircar, S. AIChE J. 2008, 9, 2293–2302. doi:10.1002/aic.11531
    Return to citation in text: [1]
  4. Jiao, Y.; Du, A.; Zhu, Z.; Rudolph, V.; Smith, S. C. J. Mater. Chem. 2010, 20, 10426–10430. doi:10.1039/c0jm01416h
    Return to citation in text: [1]
  5. Jiao, Y.; Du, A.; Zhu, Z.; Rudolph, V.; Smith, S. C. J. Phys. Chem. C 2010, 114, 7846–7849. doi:10.1021/jp911419k
    Return to citation in text: [1]
  6. Sun, Q.; Wang, M.; Li, Z.; Du, A.; Searles, D. J. J. Phys. Chem. C 2014, 118, 2170–2177. doi:10.1021/jp407940z
    Return to citation in text: [1]
  7. Lee, H.; Li, J.; Zhou, G.; Duan, W.; Kim, G.; Ihm, J. Phys. Rev. B 2008, 77, 235101. doi:10.1103/PhysRevB.77.235101
    Return to citation in text: [1]
  8. Sun, Q.; Li, Z.; Searles, D. J.; Chen, Y.; Lu, G. (M.); Du, A. J. Am. Chem. Soc. 2013, 135, 8246–8253. doi:10.1021/ja400243r
    Return to citation in text: [1] [2] [3]
  9. Chen, Z.; King, R. B. Chem. Rev. 2005, 105, 3613–3642. doi:10.1021/cr0300892
    Return to citation in text: [1] [2]
  10. Tenne, R. Adv. Mater. 1995, 7, 965–995. doi:10.1002/adma.19950071203
    Return to citation in text: [1]
  11. Gao, B.; Zhao, J.-x.; Cai, Q.-h.; Wang, X.-g.; Wang, X.-z. J. Phys. Chem. A 2011, 115, 9969–9976. doi:10.1021/jp2016853
    Return to citation in text: [1]
  12. Gao, F.; Zhao, G.-L.; Yang, S.; Spivey, J. J. J. Am. Chem. Soc. 2013, 135, 3315–3318. doi:10.1021/ja309042m
    Return to citation in text: [1]
  13. Guo, T.; Jin, C.; Smalley, R. E. J. Phys. Chem. 1991, 95, 4948–4950. doi:10.1021/j100166a010
    Return to citation in text: [1] [2]
  14. Zou, Y. J.; Zhang, X. W.; Li, Y. L.; Wang, B.; Yan, H.; Cui, J. Z.; Liu, L. M.; Da, D. A. J. Mater. Sci. 2002, 37, 1043–1047. doi:10.1023/A:1014368418784
    Return to citation in text: [1]
  15. Dunk, P. W.; Rodríguez-Fortea, A.; Kaiser, N. K.; Shinohara, H.; Poblet, J. M.; Kroto, H. W. Angew. Chem. 2013, 125, 333–337. doi:10.1002/ange.201208244
    Return to citation in text: [1] [2]
  16. Wang, S.-H.; Chen, F.; Fann, Y.-C.; Kashani, M.; Malaty, M.; Jansen, S. A. J. Phys. Chem. 1995, 99, 6801–6807. doi:10.1021/j100018a008
    Return to citation in text: [1]
  17. Kurita, N.; Kobayashi, K.; Kumahora, H.; Tago, K.; Ozawa, K. Chem. Phys. Lett. 1992, 198, 95–99. doi:10.1016/0009-2614(92)90054-Q
    Return to citation in text: [1] [2]
  18. Sun, Q.; Wang, M.; Li, Z.; Ma, Y.; Du, A. Chem. Phys. Lett. 2013, 575, 59–66. doi:10.1016/j.cplett.2013.04.063
    Return to citation in text: [1] [2]
  19. Jiao, Y.; Zheng, Y.; Smith, S. C.; Du, A.; Zhu, Z. ChemSusChem 2014, 7, 435–441. doi:10.1002/cssc.201300624
    Return to citation in text: [1]
  20. Becke, A. D. J. Chem. Phys. 1993, 98, 5648–5652. doi:10.1063/1.464913
    Return to citation in text: [1]
  21. Lee, C.; Yang, W.; Parr, R. G. Phys. Rev. B 1988, 37, 785–789. doi:10.1103/PhysRevB.37.785
    Return to citation in text: [1]
  22. Stephens, P. J.; Devlin, F. J.; Chabalowski, C. F.; Frisch, M. J. J. Phys. Chem. 1994, 98, 11623–11627. doi:10.1021/j100096a001
    Return to citation in text: [1]
  23. Grimme, S. J. Comput. Chem. 2006, 27, 1787–1799. doi:10.1002/jcc.20495
    Return to citation in text: [1]
  24. Grimme, S.; Ehrlich, S.; Goerigk, L. J. Comput. Chem. 2011, 32, 1456–1465. doi:10.1002/jcc.21759
    Return to citation in text: [1]
  25. Mulliken, R. S. J. Chem. Phys. 1955, 23, 1833–1840. doi:10.1063/1.1740588
    Return to citation in text: [1]
  26. Simon, S.; Duran, M.; Dannenberg, J. J. J. Chem. Phys. 1996, 105, 11024–11031. doi:10.1063/1.472902
    Return to citation in text: [1]
  27. Boys, S. F.; Bernardi, F. Mol. Phys. 1970, 19, 553–566. doi:10.1080/00268977000101561
    Return to citation in text: [1]
  28. Peng, C.; Schlegel, H. B. Isr. J. Chem. 1993, 33, 449–454. doi:10.1002/ijch.199300051
    Return to citation in text: [1]
  29. Hratchian, H. P.; Schlegel, H. B. Finding minima, transition states, and following reaction pathways on ab initio potential energy surfaces; Elsevier: Amsterdam, The Netherlands, 2005.
    Return to citation in text: [1]
  30. Peng, C.; Ayala, P. Y.; Schlegel, H. B.; Frisch, M. J. J. Comput. Chem. 1996, 17, 49–56. doi:10.1002/(SICI)1096-987X(19960115)17:1<49::AID-JCC5>3.3.CO;2-#
    Return to citation in text: [1]
  31. Gonzalez, C.; Schlegel, H. B. J. Chem. Phys. 1989, 90, 2154–2161. doi:10.1063/1.456010
    Return to citation in text: [1]
  32. Gaussian 09, Revision B.01; Gaussian, Inc.: Wallingford, CT, USA, 2009.
    Return to citation in text: [1]
  33. GaussView, Version 5; Semichem Inc.: Shawnee Mission, KS, USA, 2009.
    Return to citation in text: [1]
  34. Kim, K.-C.; Hauke, F.; Hirsch, A.; Boyd, P. D. W.; Carter, E.; Armstrong, R. S.; Lay, P. A.; Reed, C. A. J. Am. Chem. Soc. 2003, 125, 4024–4025. doi:10.1021/ja034014r
    Return to citation in text: [1]
  35. Xie, R.-H.; Bryant, G. W.; Zhao, J.; Smith, V. H., Jr..; Di Carlo, A.; Pecchia, A. Phys. Rev. Lett. 2003, 90, 206602. doi:10.1103/PhysRevLett.90.206602
    Return to citation in text: [1]
  36. Chu, S.; Majumdar, A. Nature 2012, 488, 294–303. doi:10.1038/nature11475
    Return to citation in text: [1]
  37. Foresman, J. B.; Frisch, Æ. Exploring chemistry with electronic structure methods: A Guide to Using Gaussian; Gaussian, Inc.: Pittsburgh, PA, USA, 1996.
    Return to citation in text: [1]

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