Table of Contents Author Guidelines Submit a Manuscript
Journal of Nanomaterials
Volume 2015 (2015), Article ID 296486, 5 pages
Research Article

Synthesis of Renewable Energy Materials, Sodium Aluminum Hydride by Grignard Reagent of Al

School of Science, North University of China, Taiyuan 030051, China

Received 19 May 2015; Accepted 12 July 2015

Academic Editor: Xiaogang Han

Copyright © 2015 Jun-qin Wang et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.


The research on hydrogen generation and application has attracted widespread attention around the world. This paper is to demonstrate that sodium aluminum hydride can be synthesized under simple and mild reaction condition. Being activated through organics, aluminum powder reacts with hydrogen and sodium hydride to produce sodium aluminum hydride under atmospheric pressure. The properties and composition of the sample were characterized by FTIR, XRD, SEM, and so forth. The results showed that the product through this synthesis method is sodium aluminum hydride, and it has higher purity, perfect crystal character, better stability, and good hydrogen storage property. The reaction mechanism is also discussed in detail.

1. Introduction

Hydrogen is considered as one of the most important energy carriers for future energy vectors because of the higher energy storage density, environmental friendliness, and broadened sources [1]. Complex metal hydride composites in the form of ABH4, where A is an alkali metal and B is a group III element, have been widely studied in solution as proton acceptors to enhance H2 adsorption abilities. NaAlH4 is different from any other metal hydrides and borohydrides with similar structures since it is capable of reversibly storing H2 after doping with transition metals (e.g., Ti, Fe, or Zr) [2, 3]. NaAlH4 is one of the most useful solid hydrogen storage materials [4]. It could be produced by many methods such as liquid-phase synthesis method [5, 6], solid-phase synthesis method [7], and milling synthesis [8]. However, all these synthesis methods have some disadvantages [4, 9], like lower yield rate, higher consumption of raw material, higher temperature and higher pressure, and so forth [10], which make them difficult for industrial production.

This paper will describe a simple and efficient method to synthesize sodium aluminum hydride under moderate condition. The synthesis could be split into two steps. First, aluminum powder is activated by organics to produce activated aluminum. Secondly, the activated aluminum reacts with hydrogen and sodium hydride to produce final product [11]. The raw material for this synthesis method is easy to get, and the utilization of the raw material and yield rate are really high. All these features of the synthesis demonstrate that this method is promising for the industrialization of sodium aluminum hydride [12, 13]. It is established that hydrogen storage material sodium alanate can be obtained from low cost starting materials [4].

2. Experimental

2.1. Reagents and Materials

Aluminum powder (granularity, 200, purchased from Beijing Chemical Reagent Factory) was dried in a vacuum oven. Anhydrous aluminum chloride (purchased from Tianjin Chemical Reagent Factory) and iodine (purchased from Zhengzhou Chemical Reagent Factory) were sealed and stored in a dark environment as the initiator. In addition, commercial NaH (purity 60%, purchased from Aladdin) was stored under N2 atmosphere to prevent oxygen/moisture exposure. Toluene and tetrahydrofuran (THF) (AR, purchased from Tianli Chemical Reagent Co. Ltd.) were distilled over sodium metal under N2 atmosphere to remove water. H2 (purity 99.999%, purchased from Taiyuan Industrial Gases Factory) was removed moisture through a scrubber, as the purpose of a protective and reaction gas. Several freeze-pump-thaw cycles were performed for halogenated hydrocarbons (AR, purchased from Tianjin Chemical Reagent Factory) to remove trace amounts of O2 and water.

2.2. Synthesis Method

All reactions were carried out under anhydrous and oxygen-free environment (hydrogen circumstance). Since there are some impurities in aluminum powder and NaH surface wrapping in mineral oil, their dosage should be slightly more than the theoretical value. Aluminum powder 2 g, exact amounts of anhydrous aluminum chloride and iodinine, and freshly sealed halogenated hydrocarbons 8 mL were added to a 250 mL of three-neck flask after replacement repeatedly with H2. The mixture was heated to 40°C and refluxed in hydrogen stream with stirring. About 25 minutes later, the reaction has been initiated; as a result, aluminum powder is activated to form an organic aluminum reagent intermediates and active aluminum.

One hour later, 3.5 g NaH and 30 mL of toluene (as the dispersant) were put into the flask. The mixture was heated to 85°C and refluxed with stirring for 6 h before it was cooled down to room temperature. After separation and crystallization, the gray powder was dried in vacuo at 60°C for 12 h.

The gray solid was dissolved in a mixed solvent of toluene and tetrahydrofuran, and then insoluble matter was filtered off. The solvent was removed from the filtrate under reducing atmosphere, and the resulting white slid was dried in vacuo at 80°C for 12 h.

2.3. Characterization

All powder X-ray diffraction experiments were performed on a Rigaku Ultima IV diffractometer equipped with a Cu-Kα source operated at 40 kV, 44 mA, and 1.76 kW with the step size of 5° in the scanning range of the diffraction angle and a scintillation counter detector. The samples were confirmed by comparison with the appropriate pattern from the International Center for Diffraction Database (ICDD) crystallographic database. All Fourier transform infrared (FTIR) spectroscopic measurements were made on a Shimadzu model FTIR-8400S spectrometer equipped with an attenuated total reflectance (ATR) attachment. The sample morphologies were characterized with SEM on an Hltachi model Su-1500. Online Mass Spectrometry analysis was performed using PFEIFFER Omni Star.

3. Results and Discussion

3.1. Infrared Spectroscopy Analysis

The absorption peak of [AlH4] corresponding to Al-H bond stretching was usually used to determine sodium aluminum hydride. As shown in Figures 1(a) and 1(b), there are Al-H bond characteristic peaks that appear in the vicinity of 1660 cm−1 and 710 cm−1. Figure 1(c) is the intermediate from reaction started about an hour; there is a clear characteristic peak of aluminum alkyl in the vicinity of 1250 cm−1, 1040 cm−1, and 650 cm−1. It indicates the formation of alkyl-aluminum. It can also be seen from the figure that the purity of the sample is improved after recrystallization, with a significant reduction of impurity peak. By comparing this is consistent with previous results reported in the literature [14, 15]. This indicates that the product has the presence of NaAlH4.

Figure 1: FTIR spectra of the sample: (a) sample after recrystallization, (b) sample after completion of the reaction, and (c) intermediate from reaction started about an hour.
3.2. Elemental Analysis of Samples

H elemental analysis was performed using Germany ELTRA ONH-2000 elemental analyzer. Al elemental analysis was performed using anti-titration according to GB/T 5121.13-2008. Metallic sodium content was measured by Prodigy Full Spectrum Direct Reading ICP emission spectrometer (Leeman Labs, US), and the sample analysis results are listed in Table 1. It can be seen that the actual measured value of these three elements is close to the theoretical value, and the contents of different element are approximately consistent with the theoretical values. The melting point of the sample is between 182°C–185°C. It has a melting process, it is a range, not a specific temperature point. In other words, it started to melt from 182°C, and melted completely at 185°C. Combining the results of the elemental analysis indicates that the molecular of our product is NaAlH4.

Table 1: Analysis data of the sample elemental composition.
3.3. X-Ray Diffraction Analysis

Figure 2 shows the diffractograms of the synthesized samples and the sample after recrystallization. The characteristic peaks of those samples are clearly discernible and consistent with the JCPDF index-card 22-1337 [16]. Based on this result as well as those of FTIR and elemental analysis, it can be conclude that the final product prepared by this method is NaAlH4. It has a monoclinic crystal structure (cell parameters:  Å,  Å) and I41/a (88) space group. These results are consistent with other studies on the same NaAlH4 and similar ones (despite being synthesized by different methods and at higher temperatures). It can also be seen from the figure that there are impurities present in the sample before recrystallization. In other words, the purity of the product is improved after recrystallization.

Figure 2: XRD patterns of (a) products after recrystallization and (b) products after completion of the reaction.
3.4. Reaction Mechanism

The reaction mechanism can be described as follows:

At first, aluminum powder is activated in the presence of initiator and the intermediate with a high activity can directly react with hydrogen to form aluminum hydride. The produced AlH3 then further react with NaH and hydrogen to form final product, NaAlH4.

This is confirmed by FTIR and XRD as seen in Figures 1(c), 3, and 4. In Figure 1(c), there is a strong absorption peak at 1640 cm−1, which can be attributed to the Al-H bond vibration absorption [17]. Because in the absence of sodium hydride, therefore it can not be [AlH4] vibration peak, it should AlH3 vibration absorption.

Figure 3: XRD patterns of mixture obtained after 1 h of reaction.
Figure 4: XRD patterns of mixture obtained after 5 h of reaction after adding NaH.

To further confirm this reaction mechanism, we also ran some other experiments. Figures 3 and 1(c) show XRD and FTIR of the product without addition of sodium hydride. The results illustrate the generation of different crystal forms of aluminum hydride in the first reaction step. The intermediate obtained at a reaction time of 5 h was detected by XRD and the result is shown in Figure 4. It can be seen that the resulting intermediate contains multiple components including Na3AlH6, AlH3, NaH, and NaAlH4. This result adds to and provides for our reaction mechanism [18].

3.5. Scanning Electron Microscopy Analysis

Two scanning electron microscopy (SEM) photomicrographs of the sample surface are depicted in Figure 5. Figure 5(a) shows the microstructure of synthesized NaAlH4, where plurality of smaller sized irregular particles and loose structure can be observed on the whole porous surface. This microstructure has large specific surface area; and it is beneficial to improve the capacity of hydrogen storage and release of materials [19]. The sample after recrystallization is shown in Figure 5(b); its surface is smooth but has a lot of voids there, which suggests that there is certain functional materials storage of gas. Based on this phenomenon, compounds with different morphologies can be obtained using this method.

Figure 5: SEM micrographs of obtained NaAlH4 before its recrystallization (a) and that after recrystallization (b) for magnified 1000 times.
3.6. Performance Analysis of Dehydrogenation

According to the literature [20], the de/hydrogenation reactions of NaAlH4 take place in three steps as follows:

Online Mass Spectrometry is a gas collection device, in which acquisition gaseous substances are released during heating under the protection of N2, so as to get its content. The heating rate of hydrogen online MS is 5°C per minute; the peak of the figure represents hydrogen release.

Figure 6 is the Online Mass Spectrometry of hydrogen from synthesized samples. It can be seen that hydrogen was released during the decomposition of the sample. This result showed that the synthesized sodium aluminum hydride has hydrogen storage capability. There are approximately 3.62 wt% H2 released at 340°C and 0.35 wt% H2 releasing at about 100°C, which can be attributed to the decomposition of remnant aluminum hydride [17] and influence of impurities. This shows that the stability to get NaAlH4 is not good.

Figure 6: Online MS of hydrogen from synthesized NaAlH4.

Figure 7 shows the Online Mass Spectrometry of hydrogen from samples after recrystallization. By comparing Figures 6 and 7, there is only a hydrogen release peak at 370°C in Figure 7, and its content is about 3.87 wt%. This shows that the sample is more stable after recrystallization and has better purity.

Figure 7: Online MS of hydrogen after recrystallization from synthesized NaAlH4.

It is concluded that sodium aluminum hydride obtained by this method has a hydrogen storage capacity from Online Mass Spectrometry and SEM. The hydrogen storage capacity is less than those reported in the literature by calculation. As the temperature increases, there will be a release of hydrogen; this also provides evidence for the stability. In summary, the sample has more stable and more complete polymorph after recrystallization.

4. Conclusions

From the above discussion, it can be concluded that NaAlH4 was successfully synthesized by a very effective method in this paper. Our preparation way has some advantages including low cost, mild reaction conditions, and high output rate. The synthesized NaAlH4 has hydrogen storage capacity and more moderate desorption conditions and better stability after recrystallization. All these advantages indicate that our process has potential application for the industrial production of NaAlH4. This provides a strong guarantee of the research and development for other hydrogen storage materials.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.


The authors gratefully acknowledge the financial support of this work by the International Science & Technology Cooperation Program of China (no. 2011DFA51980) and Shanxi Science & Technology Cooperation Program of China (no. 2011DFA51980). Acknowledgement is made to the National Key Laboratory for Electronic Measurement Technology and Shanxi Polymer Composite Materials Engineering Research Center for the support of equipment and offering a variety of test equipment.


  1. X. Xiao, S. Wang, X. Fan et al., “Improved de/hydrogenation properties and favorable reaction mechanism of CeH2 + KH co-doped sodium aluminum hydride,” International Journal of Hydrogen Energy, vol. 39, no. 12, pp. 6577–6587, 2014. View at Publisher · View at Google Scholar · View at Scopus
  2. K.-S. Lin, Y.-J. Mai, S.-R. Li, C.-W. Shu, and C.-H. Wang, “Characterization and hydrogen storage of surface-modified multiwalled carbon nanotubes for fuel cell application,” Journal of Nanomaterials, vol. 2012, Article ID 939683, 13 pages, 2012. View at Publisher · View at Google Scholar · View at Scopus
  3. K.-S. Lin, Y.-J. Mai, S.-W. Chiu, J.-H. Yang, and S. L. I. Chan, “Synthesis and characterization of metal hydride/carbon aerogel composites for hydrogen storage,” Journal of Nanomaterials, vol. 2012, Article ID 201584, 9 pages, 2012. View at Publisher · View at Google Scholar · View at Scopus
  4. L. E. Klebanoff and J. O. Keller, “Corrigendum to ‘5 years of hydrogen storage research in the U.S. DOE Metal Hydride Center of Excellence (MHCoE)’ [Int J Hydrog Energy 38 (2013) 4533–4576],” International Journal of Hydrogen Energy, vol. 38, no. 19, 8022 pages, 2013. View at Publisher · View at Google Scholar
  5. H. M. Lee, S.-Y. Choi, and J.-Y. Yun, “Preparation of aluminum-organic nanocomposite materials via wet chemical process,” Advanced Powder Technology, vol. 22, no. 5, pp. 608–612, 2011. View at Publisher · View at Google Scholar · View at Scopus
  6. T. A. Semelsberger and K. P. Brooks, “Chemical hydrogen storage material property guidelines for automotive applications,” Journal of Power Sources, vol. 279, pp. 593–609, 2015. View at Publisher · View at Google Scholar · View at Scopus
  7. R. Bhattacharyya and S. Mohan, “Solid state storage of hydrogen and its isotopes: an engineering overview,” Renewable & Sustainable Energy Reviews, vol. 41, pp. 872–883, 2015. View at Publisher · View at Google Scholar · View at Scopus
  8. J. Huot, D. B. Ravnsbæk, J. Zhang, F. Cuevas, M. Latroche, and T. R. Jensen, “Mechanochemical synthesis of hydrogen storage materials,” Progress in Materials Science, vol. 58, no. 1, pp. 30–75, 2013. View at Publisher · View at Google Scholar · View at Scopus
  9. G. Lefèvre, “In situ Fourier-transform infrared spectroscopy studies of inorganic ions adsorption on metal oxides and hydroxides,” Advances in Colloid and Interface Science, vol. 107, no. 2-3, pp. 109–123, 2004. View at Publisher · View at Google Scholar · View at Scopus
  10. B. Hu, M. He, B. Chen, and L. Xia, “Liquid phase microextraction for the analysis of trace elements and their speciation,” Spectrochimica Acta Part B: Atomic Spectroscopy, vol. 86, pp. 14–30, 2013. View at Publisher · View at Google Scholar · View at Scopus
  11. E. David and J. Kopac, “Hydrolysis of aluminum dross material to achieve zero hazardous waste,” Journal of Hazardous Materials, vol. 209-210, pp. 501–509, 2012. View at Publisher · View at Google Scholar · View at Scopus
  12. R. Pedicini, B. Schiavo, P. Rispoli et al., “Progress in polymeric material for hydrogen storage application in middle conditions,” Energy, vol. 64, pp. 607–614, 2014. View at Publisher · View at Google Scholar · View at Scopus
  13. S. Veeraswamy, K. I. Reddy, R. V. Ragavan, K. T. Reddy, S. Yennam, and A. Jayashree, “An efficient one-step chemoselective reduction of alkyl ketones over aryl ketones in β-diketones using LiHMDS and lithium aluminium hydride,” Tetrahedron Letters, vol. 53, no. 35, pp. 4651–4653, 2012. View at Publisher · View at Google Scholar · View at Scopus
  14. E. M. A. Khalil, F. H. ElBatal, Y. M. Hamdy, H. M. Zidan, M. S. Aziz, and A. M. Abdelghany, “Infrared absorption spectra of transition metals-doped soda lime silica glasses,” Physica B: Condensed Matter, vol. 405, no. 5, pp. 1294–1300, 2010. View at Publisher · View at Google Scholar · View at Scopus
  15. V. D'Anna, A. Spyratou, M. Sharma, and H. Hagemann, “FT-IR spectra of inorganic borohydrides,” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 128, pp. 902–906, 2014. View at Publisher · View at Google Scholar · View at Scopus
  16. T.-T. Chen, C.-H. Yang, and W.-T. Tsai, “In-situ synchrotron X-ray diffraction study on the dehydrogenation behavior of NaAlH4 modified by multi-walled carbon nanotubes,” International Journal of Hydrogen Energy, vol. 37, no. 19, pp. 14285–14291, 2012. View at Publisher · View at Google Scholar · View at Scopus
  17. B. Xu, J. Liu, and X. Wang, “Preparation and thermal properties of aluminum hydride polymorphs,” Vacuum, vol. 99, pp. 127–134, 2014. View at Publisher · View at Google Scholar · View at Scopus
  18. L.-Y. Han, X.-Z. Xiao, X.-L. Fan et al., “Enhanced dehydrogenation performances and mechanism of LiBH4/Mg17Al12-hydride composite,” Transactions of Nonferrous Metals Society of China, vol. 24, no. 1, pp. 152–157, 2014. View at Publisher · View at Google Scholar · View at Scopus
  19. L. J. Murray, M. Dinc, and J. R. Long, “Hydrogen storage in metal-organic frameworks,” Chemical Society Reviews, vol. 38, no. 5, pp. 1294–1314, 2009. View at Publisher · View at Google Scholar · View at Scopus
  20. F. Sterpone, S. Bonella, and S. Meloni, “Early stage of the dehydrogenation of NaAlH4 by ab initio rare event simulations,” The Journal of Physical Chemistry C, vol. 116, no. 37, pp. 19636–19643, 2012. View at Publisher · View at Google Scholar · View at Scopus