Electronic properties of Ir3Li and ultra-nanocrystalline lithium superoxide formation
Graphical Abstract
Introduction
Developing batteries with comparable energy densities to internal combustion technology is essential in order to fully transition to an electrified transportation-based society. Li-O2 batteries, are seen as the ‘holy grail’ of battery technologies since they have the highest theoretical energy density of all current battery technologies [1]. Current state-of-the-art Li-O2 batteries suffer from limited practical capacity and large charge overpotentials resulting from the build-up of Li2O2 on the cathode surface [2]. The insulating nature of bulk Li2O2 with a large band gap of 2.02 eV can prevent efficient charge transport from the cathode to the reaction interface, leading to parasitic reactions and reduced cycling efficiency [3]. Among the solutions to high overpotentials on charge are the use of soluble catalysts or use of cathodes that result in discharge products with good electronic conductivity. Soluble catalysts, known as redox mediators, oxidize the surface of the Li2O2 so electronic conductivity is not an issue and they can avoid side reactions as well [4], [5]. One disadvantage of redox mediators is that they may degrade with cycling due to reactions with the cathode or the discharge product. Discharge products with good electronic conductivity can include Li2O2 with amorphous grain boundaries, Li2O2 that is amorphous, and LiO2. The LiO2 based Li-O2 batteries can also potentially provide longer cycle life compared with Li2O2 based Li-O2 batteries since oxidation of LiO2 during charging will likely not produce singlet oxygen since LiO2 is a doublet and decomposition will lead to a triplet O2 not singlet O2. Singlet O2 is produced during oxidation of Li2O2, and causes significant parasitic reactions that limit cell longevity [6].
The stabilization of the LiO2 discharge product, which limits Li2O2 formation, has been the subject of recent research. Experimental and theoretical studies have indicated that LiO2 has a much higher electronic conductivity compared with Li2O2, and this difference has been correlated to lower charge overpotentials [7], [8], [9], [10]. Lu et al. employed an Ir nanoparticle-based rGO cathode in a Li-O2 battery and demonstrated the formation of LiO2 rods as the sole discharge product, which could be cycled for up to 40 cycles with low charge cell potentials (3.3–3.5 V). The LiO2 was identified by TEM, scanning electron microscopy (SEM), X-ray diffraction (XRD), Fourier-transform infrared spectroscopy (FTIR), differential electrochemical mass spectrometry (DEMS), and Raman spectroscopy [7]. LiO2 was identified by titration in a similar, subsequent study [11]. Surprisingly, TEM analysis identified the formation of Ir3Li on Ir surfaces during electrochemical discharge of the Li-O2 cell [7]. Density functional (DFT) studies demonstrated a strong lattice match between LiO2 (111) and epitaxial Ir3Li (121), which provided explanation for the stabilization mechanism of LiO2 on Ir3Li [7].
In subsequent work Halder et al. employed TEM to investigate the formation of Ir3Li layers on Ir nanoparticles, which were supported on an rGO cathode [12]. The researchers observed a core-shell structure comprised of an Ir core and Ir3Li shell of a few nanometers thickness, which was subsequently covered by LiO2 during discharge in a Li-O2 cell. Furthermore, it was shown through TEM analysis of cycled cathodes that Ir3Li was electrochemically stable once formed in an Li-O2 environment. TEM results demonstrated that after the initial formation of Ir3Li surfaces during the initial discharge, the Ir3Li surfaces remained inert over 10 discharge/charge cycles. Discharge tests were also performed in an argon atmosphere to demonstrate that Ir3Li did not form from the direct intercalation of lithium (Li) into Ir. DFT calculations indicated that the Ir3Li formation mechanism during discharge in a Li-O2 cell (reaction (1)) was thermodynamically favorable (−5.9 eV at 0 K) [12].LiO2(s) + 3Ir(s) → Ir3Li(s) + O2(g),
The synthesis of intermetallic Ir3Li particles was first reported by Donkersloot et al., in 1976 [13]. The authors heated a mixture of Ir powders and Li metal at 800 °C for seven days in order to produce a phase pure Ir3Li product that was characterized using single crystal XRD. The material was found to have a body-centered orthorhombic unit cell structure, with lattice constants of a = 2.6726 Å, b = 8.6949 Å and c = 4.6703 Å. Sangster and Pelton used thermodynamic calculations and experimental data to describe the phase diagram of the Ir-Li binary system. The authors described two Ir-Li phases: a Li rich IrLi phase with a layered structure and the Ir3Li phase with stacked Li columns [14].
Aside from identification of the crystal structure and calculated Ir3Li phase diagram [13], [14], little is known about the physical properties of the material especially regarding its efficiency in serving as a template for LiO2 in Li-O2 batteries [12]. Experimental characterization and a comprehensive understanding of the Ir3Li electronic properties is necessary in order to optimize the material for effective implementation in LiO2-based Li-O2 batteries. More importantly, understanding Ir3Li key material properties may provide guidance for the design of non-precious-metal-based cathodes for economically viable LiO2 based batteries. Further investigation of the formation of LiO2 on iridium-based particles is also essential in order to develop an understanding of properties of LiO2, which is difficult to study due to its prominent disproportionation to Li2O2 and O2.
In the current study, we demonstrate the first implementation of ex-situ synthesized Ir3Li particles in a Li-O2 battery. Comprehensive spectroscopic and microscopic analysis including, XRD, SEM, conductive atomic force microscopy (CAFM), X-ray photoelectron spectroscopy (XPS), Raman, superconducting quantum interference device (SQUID) measurements, and electron paramagnetic resonance (EPR) were performed on the Ir3Li particles in order to better understand key properties of this novel material. The cathode based on bulk Ir3Li successfully led to formation of a LiO2 discharge product with much larger particle size and stability than previously found. TEM studies were carried out on the LiO2 discharge product to better understand the morphology of the LiO2. DFT studies provided evidence for the LiO2 stabilization mechanism.
Section snippets
Synthesis
Ir3Li synthesis was performed similar to that reported previously [13]. Ir powder (Aldrich powders, 99.9%) and Li foil (MTI, 99.9%) were sealed in a tantalum tube inside an argon filled glovebox using a 3:1.2 Ir:Li molar ratio. The lithium foil was carefully placed over the Ir powders to keep the two reagents in close contact. The tantalum tube with a crimped lid was taken out of the glovebox and immediately sealed with an arc torch under argon. The tantalum tube was further sealed in a quartz
Synthesis and characterization of Ir3Li
In order to prepare phase pure Ir3Li, the previously reported high temperature route was implemented as described in the previous section [13]. The synthesized Ir3Li powders were analyzed with use of the XRD technique at Argonne’s high resolution synchrotron beamline. Metallic Ir was not observed and the XRD spectrum was nearly identical to that of the ICSD Ir3Li standard, thereby confirming phase pure Ir3Li formation. Fig. 1a shows the Ir3Li powder XRD spectrum with comparison to the ICSD
Conclusions
Ir3Li particles ranging from 200 nm to 5 µm were synthesized using a thermal reaction between Ir and Li metals at 800 °C. The powder was characterized using XRD and was demonstrated to be phase pure. The Ir3Li catalyst was deposited onto an rGO cathode and discharged in a Li-O2 battery. Raman and titration analysis confirmed the presence of LiO2 as the dominant discharge product. TEM was used to characterize the LiO2 discharge product. It was found that LiO2 secondary particles > 200 nm,
CRediT authorship contribution statement
All Authors contributed equally to this manuscript.
Declaration of Competing Interest
The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.
Acknowledgements
This work was supported by the U.S. Department of Energy under Contract No. DE-AC02-06CH11357 from the Vehicle Technologies Office, Office of Energy Efficiency and Renewable Energy. Work (D.Y.C. and D.P.) in the Materials Science Division of Argonne National Laboratory (magnetometry and thermal synthesis) was supported by the U.S. Department of Energy, Office of Science, Basic Energy Sciences, Materials Science and Engineering Division under Contract No. DE-AC02-06CH11357. Use of the Center for
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