Christoph J.
Sahle
*a,
Christian
Sternemann
b,
Carlotta
Giacobbe
a,
Yigang
Yan
c,
Christopher
Weis
b,
Manuel
Harder
bd,
Yury
Forov
b,
Georg
Spiekermann
de,
Metin
Tolan
b,
Michael
Krisch
a and
Arndt
Remhof
cf
aEuropean Synchrotron Radiation Facility, 71 Avenue des Martyrs, 38000 Grenoble, France. E-mail: christoph.sahle@esrf.fr
bFakultät Physik/DELTA, Technische Universität Dortmund, Dortmund, Germany. E-mail: christian.sternemann@tu-dortmund.de
cMaterials for Energy Conversion, Empa, Ch-8600 Dübendorf, Switzerland
dDeutsches Elektronen-Synchrotron DESY, Notkestrasse 85, 22607 Hamburg, Germany
eDeutsches GeoForschungsZentrum, Section 3.3, Potsdam, Germany
fCrystallography, Institute for Geo- and Environmental Science, Albert-Ludwigs-University Freiburg, D-79098 Freiburg im Breisgau, Germany
First published on 22nd June 2016
Using a combination of high resolution X-ray powder diffraction and X-ray Raman scattering spectroscopy at the B K- and Ca L2,3-edges, we analyzed the reaction products of Ca(BH4)2 after annealing at 350 °C and 400 °C under vacuum conditions. We observed the formation of nanocrystalline/amorphous CaB6 mainly and found only small contributions from amorphous B for annealing times larger than 2 h. For short annealing times of 0.5 h at 400 °C we observed neither CaB12H12 nor CaB6. The results indicate a reaction pathway in which Ca(BH4)2 decomposes to B and CaH2 and finally reacts to form CaB6. These findings confirm the potential of using Ca(BH4)2 as a hydrogen storage medium and imply the desired cycling capabilities for achieving high-density hydrogen storage materials.
Ca(BH4)2 has a gravimetric hydrogen density of 11.6 mass% (or 124.1 kg m−3)2,7,8 and thus is a promising candidate for use as a reversible hydrogen storage medium. For this material, different desorption pathways under various experimental conditions are vividly discussed and researchers suggest different (amorphous) intermediates and final decomposition products such as CaB2Hx-species,5,8–10 amorphous CaB12H12,9,11–13 and amorphous boron (a-B).8–10,13 Marketable technical applications demand storage media free of these stable phases e.g. by yielding only CaB6 after hydrogen release, which would make complete cycling feasible. Two competing reaction pathways are mainly discussed for Ca(BH4)2, one leading to CaB6 as a favorable end product (1), and the other one resulting in CaB12H12(2):
Ca(BH4)2 → (amorphous) intermediate |
→ CaB2Hx + (4 − x/2)H2 |
→ 1/3CaB6 + 2/3CaH2 + (x/2 − 2/3)H2 | (1) |
Ca(BH4)2 → (amorphous) intermediate |
→ 1/6CaB12H12 + 5/6CaH2 + 13/6H2. | (2) |
The formation of CaB2Hx was critically discussed, see e.g.ref. 14, 15 and 16. Riktor et al. assigned this intermediate to be crystalline CaB2H2 with an orthorhombic unit cell and either a Pnna or a Pbna space group using X-ray diffraction (XRD).5 A structure with an orthorhombic unit cell was also found by Aoki et al.17 for this intermediate without reporting the stoichiometry. Recently, based on NMR studies, Yan et al. did not observe CaB12H12 among the decomposition products and identified the intermediate to be CaB2H6 for decomposition between 320 °C and 350 °C.10
In a temperature range close to the melting point of Ca(BH4)2 at 370 °C,18 reaction paths (1) and (2) might compete. Partial and almost complete reversibility of the process was achieved under moderate reaction conditions (ca. 345 °C and 90–185 bar H2).9,10 At decomposition temperatures of 400 °C and 450 °C, amorphous boron has been identified as the major boron containing species, suggesting a third decomposition pathway along19
Ca(BH4)2 → 2B + CaH2 + 3H2. | (3) |
Here, we report how we used a combination of high resolution powder XRD and X-ray Raman scattering (XRS) spectroscopy at both the K-edge of B and the L2,3-edges of Ca to analyze the thermal decomposition products of Ca(BH4)2. XRD provides accurate information about the crystalline reaction products and yields boundary conditions for a detailed quantitative analysis of the XRS spectra in order to identify the nano-crystalline and/or amorphous decomposition products of the material after hydrogen desorption and thus validate the reaction paths (1), (2), and (3), the suggested decomposition pathways around 400 °C.
XRD is a well established and accurate structural analysis probe and is routinely used for the study of hydrogen storage materials; for XRD studies on Ca(BH4)2, see e.g.ref. 5, 8, 9, 13, 17 and 20. XRS, on the other hand, is less known, but is an emerging technique to probe soft X-ray absorption edges using hard X-rays.21 XRS enables us to study lightweight elements with bulk sensitivity even when contained in a matrix of heavier elements. Consequently, XRS allows for in situ studies of chemical reactions under realistic reaction conditions, i.e. of samples inside chemical reaction cells under realistic reaction atmospheres. Thus, this inelastic X-ray scattering technique combines the sensitivity of absorption spectroscopy to reveal information about the local atomic and electronic structures with the unique properties of hard X-rays. XRS can be employed for the analysis of low Z-element containing samples, both crystalline and amorphous, under in situ conditions.
XRS was used to study e.g. chemical reactions22–24 or to investigate low-Z materials under extreme pressure and temperature conditions.25,26 This method was applied to analyze the B K-edge e.g. in MgB2, BN, C2B10H12, B2O3, and Li2B4O7.25,27–30 The Ca L2,3-edges were studied so far using only electron energy loss spectroscopy or soft X-ray absorption spectroscopy e.g. to characterize materials of geological and biological relevance31,32 with the exception of a high pressure XRS study of the Ca L-edge in CaSiO3 glass.33 Recently, in situ XRS spectroscopy was used to investigate hydrogen desorption in LiBH4, LiBH4 nano-composites, and Mg(BH4)2.23,34,35
The high resolution powder XRD data were collected at ID22 of the ESRF (Grenoble, France) using a multi-channel detector. We measured the different patterns in two different runs (using incident wavelengths of λ = 0.40 Å and λ = 0.32 Å, respectively). The capillaries were mounted on a rotating support and were spun at approximately 2 Hz to improve the powder average. We collected data to cover a momentum transfer range of 0.0 < |q| < 9.0 Å−1 and binned the data onto a constant step size of 0.002 Å−1.
We performed the measurements of the B K-edge at beamline ID20 of the ESRF using the multi-analyzer-crystal XRS spectrometer. The analyzer energy was fixed at 9.7 keV using the Si(660) Bragg reflection and the incident energy was scanned to obtain energy losses in the vicinity of the B K-edge from 180 eV to 225 eV. The spectrometer is equipped with 6 Maxipix Timepix area detectors, one for each set of 12 spherically bent Si analyzer crystals. We utilized three of these analyzer arrays and set the mean scattering angles of these arrays to 50° for an average momentum transfer of 4.2 ± 0.2 Å−1. With this setup, we achieved an overall energy resolution of 0.6 eV. We measured the Ca L2,3- and B K-edges at beamline P01 of PetraIII (Hamburg, Germany) using 11 Si(660) analyzers focused on 4 avalanche photodiodes. The scattering angle was 32° resulting in an average momentum transfer of 2.9 ± 0.4 Å−1 and an overall energy resolution of 0.9 eV. The incident energy was scanned to measure the Ca L2,3-edges (B K-edge) for the energy loss between 340 eV (173 eV) and 375 eV (223 eV). For the final spectra shown in this report, we averaged over the scattering signals from the different analyzer crystals. Before further processing, we corrected for the valence electrons' response as discussed in ref. 36 and 37. Details of the experimental data processing can be found in ref. 37. After background subtraction, we normalized the B K-edge XRS spectra to their integrated intensity between 183 and 223 eV energy loss and the Ca L2,3-edge spectra to their integrated intensity between 345 and 373 eV energy loss. Both these intergrated intensities relate to the scattering of one B and one Ca atom in each compound, respectively.
For all annealing conditions with the exception of 400 °C and 0.5 h, we find nanocrystalline contributions from CaB6. The averaged size of the CaB6 nanocrystals is the smallest at 350 °C and increases at higher annealing temperatures (compare the table in the ESI†). This supports the improved cycling capabilities when Ca(BH4)2 is decomposed at 350 °C compared to 400 °C due to the increased crystallinity at 400 °C.10 We could not identify crystalline CaB12H12 or crystalline B in any of the samples. CaH2 is found to be a constituent in all samples and its amount increases with annealing time. For the sample annealed at 400 °C for 0.5 h, we can identify a crystalline intermediate with a diffraction pattern that resembles the one observed earlier.5,17
It has to be noted that according to pathway (1), the ratio between CaH2 and CaB6 should be 2:
1. Instead, based on XRD, we observe a higher ratio in favor of CaH2. This can be ascribed to amorphous contributions from CaB6 or to the formation of amorphous B. Thus, we cannot exclude the competing pathways (2) and (3) because XRD is not sensitive to extract and distinguish possible amorphous contributions from CaB12H12, CaB6, and B in such complex systems. These amorphous contributions can be accessed by XRS spectroscopy.
At 400 °C after annealing for only 0.5 h, we find a strong contribution of native Ca(BH4)2 to the Ca L2,3- and B K-edge spectra. For all other annealing conditions this native compound is not observed. As we verified a crystalline intermediate by XRD, it is likely that this compound exhibits a similar spectral shape to the native reference samples. Consequently, the Ca(BH4)2 content at 400 °C after 0.5 h might indicate the amount of intermediate present in the sample. However, we have no access to a pure reference sample of the intermediate so that we cannot draw a final conclusion here. It is also possible that Ca(BH4)2 melts at 370 °C18 and occurs in the amorphous state after partial solidification as no signal of Ca(BH4)2 was observed by XRD. As both, the intermediate and the native sample, have the same Ca:
B ratio, we are still able to use the results for a stoichiometric analysis. We would like to note that we cannot identify CaB6 in the first annealing phase at 400 °C (0.5 h) as proposed in reaction path (1). All fit results are summarized in Fig. 4b (see the ESI† for error bars of the fit results).
At this point, we can conclude that the fit results obtained at 400 °C for 2 h and 15 h point toward reaction path (1) but the ratio of CaH2:
CaB6 indicates that a minor part of the reaction follows pathway (3). Consequently, we expect some contribution from amorphous boron. We can exclude reaction pathway (2) as we find no formation of CaB12H12. The situation changes remarkably when the composition of the sample annealed at 400 °C for only 0.5 h is considered. Here, we clearly observe an intermediate state. Surprisingly, no CaB6 is observed and we have identified CaH2 together with CaB2Hx/Ca(BH4)2. The sample annealed for 50 h at 350 °C resembles closely the composition of the sample annealed for 2 h at 400 °C due to the lower activation temperature.
We have no direct evidence for B from the fits of the Ca L2,3-edges, but based on the amount of CaH2 from the Ca L2,3-edges and the reactions (1) and (3), we can estimate the amount of B contained in the samples in the form of CaB6 and elemental B, respectively, by assigning all excess CaH2 from pathway (1) to the partial decomposition occurring via pathway (3). These values are reported in Fig. 4d and we can confront them with the values derived from a multi-component fit of the B K-edge as follows.
![]() | ||
Fig. 4 (a) Results of a quantitative phase analysis using the Rietveld method of the high resolution powder XRD patterns showing the relative abundence of (nano-)crystalline constituents. (b) Results of a fingerprinting analysis of the Ca L2,3-edge showing the relative content of the used Ca containing reference compounds (both amorphous and crystalline). (c) Results of a fingerprinting analysis of the B K-edge showing the relative abundance of B containing phases in different samples (both amorphous and crystalline). The hatched area shows the relative content of B containing phases from a two-component fit. (d) Extraction of the B content from the fit results of the Ca L2,3-edge via the reaction pathways (1) and (3) (both amorphous and crystalline). |
The results of this fit procedure are shown in Fig. 4c and are compiled in a tabular form in the ESI.† In general, all experimental spectra are well reproduced by the results of the component fits. Larger differences can be observed around 200 eV where the structure related to CaB6 is less pronounced and for the energy loss above 205 eV where the spectra are less structured than the respective best fits. This can be related to the fact that all boron containing decomposition products occur in amorphous or nanocrystalline form, whereas the reference spectra are recorded from crystalline or partly amorphous samples.
Except for the sample annealed at 400 °C for 0.5 h we find very good agreement between the fit results with respect to the content B and CaB6 and the compositions derived from the Ca L2,3-edges via reaction pathways (1) and (3) (compare Fig. 4c and d). The composition estimated for the sample in the intermediate state (400 °C, 0.5 h) disagrees with the fit results of the B K-edge as the estimate based on the Ca L2,3-edges suggests no contribution from CaB6. We used these B K-edge fit results (marked with an asterisk in the ESI†) to model the shape of the corresponding Ca L-edge shown as a solid line in Fig. 3a. It deviates significantly from the shape found experimentally. As the fit of the boron K-edge might be less sensitive to distinguish between elemental B and CaB6 due to the similar spectral shape, as can be inferred from the error bars of the fit (see the table in the ESI†), we repeated the fit of this spectrum by neglecting the CaB6 contribution, i.e. considering only B and Ca(BH4)2. The results of this fit (see the hatched bar in Fig. 4c and ESI† tables) are in line with the estimated boron content using stoichiometric considerations (Fig. 4d and ESI† tables) and the shape of the fitted spectrum deviates from the measured spectrum around the edge onset but agrees well with the experiment at a slightly higher energy loss.
Longer annealing times of up to 15 h initiate the formation of CaB6 from CaH2 and B. This is supported by the increase of the CaB6 proportion at the expense of CaH2 and the B content as observed after longer thermal treatment. Comparing the standard enthalpy of formation of CaH2 (ΔH0 = 186 kJ mol−1) and CaB6 (ΔH0 = 121 kJ mol−1), CaH2 is found to be more stable. However, with increasing temperature the entropy gain from the release of gaseous H2 (TΔS ≈ 90 kJ mol−1, at T = 400 °C and ΔS(H2) = 135 J mol−1 K−1) supports the formation of CaB6 in line with our observations. The degree of crystallinity of CaB6, as observed by XRD, could be the key for the reversibility of the hydrogen release reaction, i.e. the rehydrogenation of the decomposition products. Yan et al. observed that the rehydrogenation conditions degrade with respect to the initial decomposition temperature.10 Here, we see that the crystallite size together with the amorphous contribution of CaB6 may be an indicator to tune the material for improved reversibility at lower temperatures.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c6cp02495e |
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