Reversibility and Improved Hydrogen Release of Magnesium Borohydride Rebecca J. Newhouse, †,‡ Vitalie Stavila,* ,‡ Son-Jong Hwang, § Leonard E. Klebanoff, ‡ and Jin Z. Zhang † Department of Chemistry and Biochemistry, UniVersity of California, Santa Cruz, California 95064, Sandia National Laboratories, LiVermore, California 94551, and DiVision of Chemistry and Chemical Engineering, California Institute of Technology, Pasadena, California 91125 ReceiVed: December 9, 2009; ReVised Manuscript ReceiVed: February 4, 2010 Desorption and subsequent rehydrogenation of Mg(BH 4 ) 2 with and without 5 mol % TiF 3 and ScCl 3 have been investigated. Temperature programmed desorption (TPD) experiments revealed a significant increase in the rate of desorption as well as the weight percentage of hydrogen released with additives upon heating to 300 °C. Stable Mg(B x H y ) n intermediates were formed at 300 °C, whereas MgB 2 was the major product when heated to 600 °C. These samples were then rehydrogenated and subsequently characterized with powder X-ray diffraction (pXRD), Raman, and NMR spectroscopy. We confirmed significant conversion of MgB 2 to fully hydrogenated Mg(BH 4 ) 2 for the sample with and without additives. TPD and NMR studies revealed that the additives have a significant effect on the reaction pathway during both dehydrogenation and rehydrogenation reactions. This work suggests that the use of additives may provide a valid pathway for improving intrinsic hydrogen storage properties of magnesium borohydride. Introduction Complex metal hydrides have long been discussed as possible hydrogen storage materials because of their exceptional volu- metric and gravimetric densities, yet their high thermal stabilities ostensibly excluded them from consideration as practical, on- board hydrogen storage materials. 1–4 However, after the initial demonstration 5 of low temperature hydrogen release at ∼100 °C as well as reversibility with catalyzed NaAlH 4 , hydrogen release and decomposition pathways of complex metal hydrides have become an active area of research. 6–16 In particular, magnesium borohydride, Mg(BH 4 ) 2 , is a light- weight borohydride that stores 14.9% hydrogen by weight. Early studies of the synthesis and thermal decomposition of Mg(BH 4 ) 2 proved inconsistent, perhaps as a result of premature decom- position from high desolvation temperatures and/or incomplete desolvation. 17–21 It was not until recently that the crystal structures of both the low and high temperature phases (R and , respectively) were solved. 22–24 Previous studies estimated ΔH ≈ 40 kJ/mol H 2 , which implies desorption temperatures within the desired range as well as potential reversibility. 25–27 Li et al., however, experimentally determined a higher enthalpy, ΔH ) 57 kJ/mol H 2 , for the first desorption step. 28 Recent studies revealed a more complicated multistep decomposition pathway than previously thought, with the proposed formation of an amorphous intermediate similar in structure to MgB 12 H 12 . 29–31 In addition, studies have shown an inverse correlation between electronegativity of the cation and borohydride stability. The Pauling electronegativity of Mg ( ) 1.31) is less than that for Na, Li, and Ca ( ) 0.93, 0.98, and 1.00, respectively), and pure Mg(BH 4 ) 2 has been observed to initiate decomposition around 270 °C, much lower than Li, Na, and Ca borohydride. 32,33 In contrast, titanium borohydride ( of Ti ) 1.54) is unstable at room temperatures. 33,34 Another advantage of Mg(BH 4 ) 2 is that the fully dehydrogenated product is a single phase material, MgB 2 22,29,30 In contrast, several other borohydrides of interest, such as LiBH 4 , NaBH 4 , and Ca(BH 4 ) 2 , decompose to their corresponding binary hydrides. The stabilities of lithium, sodium, and calcium hydrides are formidable and in fact they melt before decomposi- tion at temperatures significantly greater than 600 °C, essentially sequestering the hydrogen. Even above these high temperatures needed for hydride decomposition, there still exists a two phase system of elemental metal and boron species that does not necessarily favor formation of a single phase. This is important since phase separation necessarily hinders reversibility. Despite the significant advantages of Mg(BH 4 ) 2 over other lightweight borohydrides, further destabilization is desired. Various methods have been successfully applied to complex metal hydrides to promote hydrogen desorption at lower temperatures and reversibility including confinement in nano- porous scaffolds, 35 destabilization with metal hydrides, 11,16 metal oxides 6 and transition metals additives. 5,36,37 Ti-doped NaAlH 4 reported by Bogdanovic ´ 5,38,39 and the MgH 2 -LiBH 4 system presented by Vajo et al. 16 demonstrate the dramatic role additives can have in destabilizing materials to enable much lower temperatures of hydrogen release as well as imparting previously unattainable reversibility. In particular, stoichiometric amounts of ScCl 3 and TiF 3 have previously been shown to promote hydrogen release at lower temperatures in borohydrides. ScCl 3 milled with LiBH 4 results in LiSc(BH 4 ) 4 which starts releasing hydrogen at ∼177 °C as opposed to >400 °C for pure LiBH 4 32,40 and TiF 3 addition results in hydrogen desorption at <100 °C in Li(BH 4 ) 2 . 41 Destabilization of Mg(BH 4 ) 2 has not yet been extensively explored, although recently it has been incorporated into activated carbon, and hydrogen release was observed * To whom correspondence should be addressed. E-mail: vnstavi@ sandia.gov. Phone: 925-294-3059. † University of California, Santa Cruz. ‡ Sandia National Laboratories. § California Institute of Technology. Mg(BH 4 ) 2 f MgB 2 + 4H 2 (I) J. Phys. Chem. C 2010, 114, 5224–5232 5224 10.1021/jp9116744  2010 American Chemical Society Published on Web 02/25/2010