Application of Operando X-ray Diffraction and Raman Spectroscopies in Elucidating the Behavior of Cathode in Lithium-Ion Batteries
- 1IREQ-Hydro Québec, Varennes, QC, Canada
- 2Centre d'Excellence en Électrification des Transports et Stockage d'Énergie, Varennes, QC, Canada
With the advances in characterization techniques, various operando/in-situ methods were applied in studying rechargeable batteries in order to improve the electrochemical properties of electrode materials, prolonging the battery life and developing new battery materials. In the present review, we focus on the characterization of electrode materials with operando/in-situ X-ray diffraction and Raman spectroscopies. By correlating the results obtained via these two techniques in different electrode chemistry: (a) intercalation materials, such as layered metal oxides and (b) conversion materials, such as elemental sulfur. We demonstrate the importance of using operando/in-situ techniques in examining the microstructural changes of the electrodes under various operating conditions, in both macro and micro-scales. These techniques also reveal the working and the degradation mechanisms of the electrodes and the possible side reactions involved. The comprehension of these mechanisms is fundamental for ameliorating the electrode materials, enhancing the battery performance and lengthening its cycling life.
Rechargeable batteries are the main energy source for electric vehicles (EV), consumer electronics, and promising candidates for renewable energy storage, owing to their relative high energy and power densities, light weight, long cycle life and environmental acceptability (Tarascon and Armand, 2001; Palacín, 2009; Dunn et al., 2011; Budde-Meiwes et al., 2013). For the large-scale commercialization of EVs and the utilization of renewable energy, the energy storage capacity, cycle life, rate capacity and safety of most commercial batteries still need to be improved (Armand and Tarascon, 2008; Etacheri et al., 2011; Wen et al., 2012). To achieve these goals, the scientific community is devoting a major effort to improve the existing materials and identify new ones to meet these requirements.
Among the many rechargeable battery materials, the layered oxide family of LiMeO2 (Me = Ni, Co, Mn, and their mixtures) has been widely studied. These oxides yield high specific energy and/or power, and structural and thermal stability, as well as long cycling life (Hwang et al., 2003; Hu et al., 2009; Huang et al., 2011; Park et al., 2012; Liao et al., 2016; Berckmans et al., 2017), but they still suffer from poor rate capability, especially at high C-rates (Chen et al., 2016b). Spinel Li(Mn,Ni)2O4 (LMN) is of great interest due to its high working voltage and high energy density, relatively low cost and environmentally benign. However, its fast capacity fade at elevated temperatures makes it unsuitable for practical applications (Amine et al., 1996; Ohzuku et al., 1999; Goodenough and Kim, 2010; Yang et al., 2013; Julien et al., 2014). Olivine structured LiFePO4 (LFP) is another promising cathode with reasonable high capacity, superior cycle life, structural and thermal stability, low cost, high safety and non-toxicity. However, its low operating voltage and low conductivity limit its wide applications (MacNeil et al., 2002; Sarkar and Mitra, 2014; Zhao et al., 2016). In addition to the Li-ion families mentioned above, Li-sulfur and Li-air batteries are also being intensively investigated owing to their high theoretical capacities, low cost and environmentally benign. Unfortunately, the present performance of both Li-S and Li-air batteries, such as energy density, rate capability, cyclability, Li-metal fading and safety, are unable to satisfy the requirements of commercial applications (Girishkumar et al., 2010; Ji and Nazar, 2010; Mikhaylik et al., 2010; Kraytsberg and Ein-Eli, 2011; Manthiram et al., 2013; Yang et al., 2018).
To further improve the performance of the batteries already present in the market, such as those based on LiCoO2 (LCO), Li(Ni,Co,Mn)O2, and LFP cathodes, it is essential to have a clear picture of the working and failure mechanisms of these batteries. Various ex-situ materials characterization techniques, such as X-Ray Diffraction (XRD), X-ray Absorption Spectroscopy (XAS), X-ray computed tomography (micro CT) (Carter et al., 2018), neutron diffraction, neutron magnetic resonance (NMR) (Ogata et al., 2014), Raman spectroscopy, Fourier-Transform Infrared (FTIR), Ultraviolet and Visible (UV-Vis) spectroscopy, Scanning and Transmission Electron Microscopies (SEM, TEM) etc. are employed to investigate the pristine and cycled electrodes at both macro and atomic scales. However, these ex-situ analyses cannot provide real-time information of the electrodes during cycling, which is crucial for understanding the working and degradation mechanisms of the batteries. In recent years, operando and in-situ (operando and in-situ will be used interchangeably hereafter) characterization techniques have been advanced and widely applied in following the real-time situation of electrodes in batteries under various operating conditions. Operando XRD is used to investigate the phase transformation and crystal structure changes of electrodes during cycling (Yang et al., 2002; Yang and Nam, 2010; Sun et al., 2013; Zhang et al., 2014; Zhu et al., 2014; Wang and Wang, 2016). Neutron diffraction is also applied to study the structure and phase developments in cycling cells (Wang et al., 2012; Bobrikov et al., 2014, 2017; Dolotko et al., 2014; Li et al., 2015) because it is more sensitive to the light elements (such as lithium) as compared to XRD, an important issue in understanding the behavior of lithium in Li-ion batteries. Operando XAS is employed to probe the changes in the local environment of a cation and its electronic structure in relation to the electrochemical processes happening on electrode surfaces (Chan et al., 2006; Dominko et al., 2009; Giorgetti, 2013; Menzel et al., 2013; Fehse et al., 2014; Giuliana et al., 2017). The absorption spectrum is divided into the X-ray Absorption Near-Edge Structure (XANES) region and the Extended X-ray Absorption Fine Structure (EXAFS) region; the former examines the oxidation state, coordination number, electronic configuration and site symmetry, whereas the latter provides information on average interatomic distances. Raman spectroscopy is also used to explore the variation in the local structure and oxidation state, as well as the thermal stability of electrode surfaces or electrode-electrolyte interfaces during charge-discharge and heat treatment (Dokko et al., 2002; Hardwick et al., 2008; Membreno et al., 2013; Stancovski and Badilescu, 2013; Wu et al., 2013); FTIR is another effective tool for studying the surface and evolution of electrode-electrolyte interfaces under cell operating conditions (Aurbach and Chusid, 1997; Chusid et al., 2001; Cheng et al., 2007; Ye et al., 2016). In addition to these spectroscopic techniques, operando SEM (Miller et al., 2013; Hovington et al., 2014; Marceau et al., 2016) and TEM (Liu, S. et al., 2014; Janish and Carter, 2015; Wang, 2015; Chen et al., 2016a; Xu et al., 2016) show the evolution of direct images of cycling electrode at the micro- and nano-scales. By combining the images with energy dispersive X-ray spectroscopy, electron energy loss spectroscopy and electron diffraction, the information on particle morphology, crystal structure, phase transformation, multi-phase interface behavior, element distribution and element positions are obtained as a function of the electrochemical process. In short, operando measurements or multi-operando measurements reveal indispensable information on how the electrodes behave and how their structures change under working conditions. These insights enable researchers to correlate the electrochemical process with the crystal structure, composition, oxidation state of ions and stresses etc. at both macro- and micro-scales, which are essential to understand the operation and failure mechanisms of batteries. The outcome of this effort is to identify new solutions being able to improve the performance of electrodes to meet the requirements for electric vehicles and storage of renewable electrical energy. Ideally the best operando techniques must be non-invasive and performed under real battery cycling. Among all the possibilities, operando X-ray diffraction is the most widely used due to the instrument availability, simple cell design, examining “bulk” material and most importantly, revealing the information on crystal structure, phase transformation as well as stresses, etc.; whereas operando TEM involves complicated cell design; testing conditions are far from real operating conditions; damage of the analyzed materials and decomposition of the liquid electrolyte are often induced due to intense electron beam used, but the technique provides information on the structural morphological changes in nano-scale. On the other hand, operando XAS and Raman techniques are also used to study the local structure of the electrode materials, but unfortunately the former need to be performed with synchrotron radiation source which is not accessible to many researchers whereas Raman spectrometer is widely available in many research facilities. In the present work, we focus on the applications of XRD and Raman to four types of electrodes, i.e., LCO, LMN, LFP and elemental sulfur. We demonstrate the contribution of these techniques to the fundamental comprehension of electrode behavior under operating conditions that are critical for raising the capacity and life span of the batteries from the current state.
The Operando X-ray Diffraction
The operando XRD, both reflection and transmission modes are used to monitor crystal structure and phase changes of electrodes during battery cycling. Different in-situ cell configurations were designed (Li et al., 1993; Leriche et al., 2010; Zhu W. et al., 2013; Roberts et al., 2014; Bleith et al., 2015) with an x-ray transparent window, such as a beryllium disk (Reimers and Dahn, 1992; Ma et al., 2013; Cañas et al., 2017), polymer films (Kapton, Mylar) (Mohanty et al., 2013; Sun et al., 2013) and aluminum foil (Zhu W. et al., 2013; Roberts et al., 2014). A beryllium window has the advantages of maintaining contact between cell components and is nearly 100% x-ray transparent due to disk rigidity and low x-ray absorption. However, beryllium corrosion was observed, especially at high voltage >4.2 V (Reimers and Dahn, 1992; Morcrette et al., 2002). In addition, beryllium is toxic and expensive compared to many other materials. Kapton, Mylar and aluminum are stable, low cost and non-toxic. They also allow X-rays to pass through with certain absorption, but it is difficult to keep cell pressurized with a large area window due to their flexibility. Aluminum foil is used as a current collector in many cases; the same aluminum foil is also used as an x-ray window to reduce undesired diffraction peaks in the spectra. While synchrotron based high-energy X-rays are used, the transmission mode can be applied (Leriche et al., 2010; He et al., 2013; Harks et al., 2015) to follow the evolution of both cathode and anode simultaneously. Figure 1A is a schematic diagram of the principle of X-ray diffraction analysis; (Figure 1a1) in situ XRD cell design; (Figure 1a2) the X-rays diffracted by the atoms on a (hkl) crystal plane satisfying the Bragg's law; (Figure 1a3) The information collected by the detector can be expressed as a plot of Intensity vs. d-spacing or 2θ; (Figure 1a4) Determination of the crystal structure from the spectrum; the unit cell size and symmetry can be obtained from peak positions whereas the number of atoms and their positions in the cell depend on the peak intensities.
Figure 1. (A) A schematic diagram of the principle of X-ray diffraction analysis; (a1) in situ XRD cell design; (a2) The incident X-ray satisfying Bragg's law is diffracted; (a3) The diffracted X-ray is plotted as a function of Intensity vs. d-spacing or 2θ; (a4) Determination of the crystal structure from the spectrum. Schematic diagrams of the in-situ Raman cells for analyzing the electrode surface and electrolyte on the lithium metal side or separator surface are plotted in (b1,b2) respectively; (b3) shows the Raman signal is collected after filtering the other radiation out and expressed as a function of Intensity and Raman shift (b4) from which the local structure information can be obtained (b5).
The Operando Raman Spectroscopy
Raman spectroscopy is a technique used to obtain unique structural information at the atomic scale, and it can analyze both solids and liquids. Raman spectroscopy is sensitive to the ion oxidation state and local structure of the material, thus it is useful in monitoring valence and bond change, as well as the corresponding phase transformation of the electrode under operating conditions. The operando Raman cell has a laser-transparent glass window. The cell components can be arranged in different configurations, depending on the components to be examined. Various cell components are amenable to analysis, for example, the changes in the electrodes, the species in the electrolyte on both sides of the separator or changes to the separator surface (Zhu et al., 2017). Figures 1b1,b2 show the schematic diagrams of the in-situ Raman cells for analyzing the electrode surface (Figure 1b1) and electrolyte on the lithium metal side or separator surface (Figure 1b2); (Figure 1b3) after filtering the elastic scattered radiation out, the inelastic Raman scattering signal is collected (Figure 1b3) and expressed in (Figure 1b4) from where the local structure, such as chemical bonds and symmetry, oxidation state of the ions can be obtained (Figure 1b5).
The Operando Studies on Cathodes
Layered oxide compounds are the most widely used cathodes for lithium-ion batteries. To achieve high capacity and long life, major effort is focused on understanding the crystal structure change at different stages of charge-discharge, with operando XRD studies making significant contributions in revealing various phase transformations in different cathode materials (Lu and Dahn, 2002; Godbole et al., 2011; Mohanty et al., 2013), especially in the LiCoO2 family. The operando XRD investigations showed the complicated phase transitions involved in the delithiation of LixCoO2 (0 ≤ x ≤ 1). Figure 2A plots the XRD spectra collected during the first charge at rate of C/4.5 in which phases H1, H2, O1a and O1 are observed as a function of cell voltage, where H1 is the fully lithiated phase at x = 1 and O1 is the completely delithiated phase at x = 0, the others are partially delithiated with 0 < x < 1. The phase-transformation steps are: H1 → H2 → O1a → O1 (Sun et al., 2001; Chung et al., 2006, 2007). The H1 and H2 have hexagonal lattice in space group (S.G.) Rm, with similar lattice parameter a, but different in c, cH1 = 14.089 A, cH2 = 14.370A respectively (Yang et al., 2000), therefore, the (003) peak shifted to the lower 2θ direction as lattice parameter c increased during the H1 to H2 phase transition; on the other hand, the positions of (101) and (102) are almost unchanged. As the charge voltage reached ~ 4.6 V, (100) and (101) peaks of O1a phase (hexagonal lattice, S.G. Rm, a = 2.823 A, c = 27.07 A, Chen et al., 2002) appeared and their intensities increased thereafter at the expense of H2 phase. H2 phase completely disappeared as O1 phase started to form, finally, all the O1a phase transformed to O1 phase (hexagonal lattice, a = 2.83 A, c = 4.24 A, S.G.: Pm1; Amatucci et al., 1996; Yang et al., 2000). A monoclinic phase formed near x = 0.5 and other transitional phase, such as H2a, were also detected via operando XRD in different studies under various experimental conditions (Reimers and Dahn, 1992; Ohzuku and Ueda, 1994; Morcrette et al., 2002; Chen and Dahn, 2004). Figure 2E is the spectra recorded during the 5th charge to 4.8 V at C/4.5 (Chung et al., 2006). The spectra show no O1 phase formation at the end of charge, instead, the existing phases are O1a and H2 suggesting a delayed phase transformation, which indicates the loss of capacity in the previous cycles. The electrode was further cycled to 8.35 V at C/4.5 during the 12th cycle (not shown here) (Chung et al., 2007). At 4.8 V, the major phases are H1 and H2, O1a was first observed at 5.04 V, and O1a to O1 phase transition completed ~ 6.05 V, which demonstrates the further delayed phase transformation compare to the 5th cycle. After the transformation to O1 is completed at 6.05 V, no new phase was found even up to 8.35 V, indicating all Li ions or almost all Li ions are removed from the structure. The charging curves show that the first voltage plateaus are ~4.0, 4.1, and >4.7 V for the 1st, 5th, and 12th cycles respectively, indicating the cell polarization increase caused by the impedance augmentation due to the electrolyte decomposition at high voltage.
Figure 2. Operando XRD and Raman measurements on LiCoO2 electrodes; (A) XRD spectra during the first charge to 4.8 V at C/4.5, demonstrating a complete phase transformation from H1 to O1. (Chung et al., 2006); (B) Raman spectra from first charge, 3.5–4.4 V at C/2.5 rate (Nishi et al., 2013); (C) In situ Raman images at various potentials during first charge to 4.4 V at C/2.5 rate with corresponding optical graph at the left (Nishi et al., 2013); (D) In situ Raman images at various potential during first discharge, 4.4–2.5 V at 1C rate (Nishi et al., 2013); (E) XRD spectra from 5th charge to 4.8 V at C/4.5, showing an incomplete phase transition between H1 and O1. (Chung et al., 2006); (F) In situ Raman images collected from 1st and 2nd cycles; after galvanostatic discharge to 2.5 V at 1C, the cell voltage was relaxed from 2.5 to 3.7 V, the cell was then discharged to 3 V at C/5 followed by holding at 3 V for 3 h which reduced the delithiated particles (Nishi et al., 2013); Legends: Red arrows, particles charged and discharged at a slower rate during both cycles; yellow arrows, particles charged at a slower rate in the 1st charge and could not be discharged in the following cycle; blue arrows, particles charged and discharged at a slower rate during the 2nd cycle. Green, black and blue colors in the image represent the discharged LiCoO2, charged LiCoO2 and carbon; Panels (A, E) with permission from Elsevier. Panels (B–D, F) with permission from ECS.
The phase transformation mechanism is well-described with the operando XRD results, but the origin of the electrode degradation is still unclear. Therefore, Raman spectroscopy is used to probe the local structure (~ μm scale) changes of LiCoO2 (Inaba et al., 1997; Itoh et al., 1997; Nishi et al., 2013; Gross and Hess, 2014) in order to understand the causes of capacity loss. Factorial group analysis indicates that LiCoO2 has two Raman active modes, A1g and Eg; the former originates from two adjacent oxygen layers moving against each other and parallel to the c-axis, whereas the latter is from the atomic displacements perpendicular to the c-axis (Baddour-Hadjean and Pereira-Ramos, 2010). The Eg and A1g vibration modes were observed experimentally at 486 and 596 cm−1 (Inaba et al., 1997). Figure 2B plots the development of Raman spectra of a LiCoO2 cathode as the voltage increased from 3.5 to 4.4 V during the first charge. The spectra show: (1) the broadening of Eg and A1g bands due to the formation of shoulder peaks; (2) the shifts of Eg and A1g to the low wave number direction; and (3) the decrease of the band intensities. The appearance of the shoulder peaks on the low wave number side is due to the formation of H2 phase with larger c-axis that causes the downward shifts of both bands. At 4.4 V, the Eg and A1g bands contain mainly H2 phase component with a very small H1 phase shoulder, which agrees with the in-situ XRD results. The voltage difference for the first detection of the H2 phase in XRD and Raman measurements reflects the difference between the average particles and individual particle. The band intensity decrease is attributed to the reduced optical skin depth of the incident laser beam due to increasing conductivity from the semiconducting H1 phase transforming to metallic H2 (Inaba et al., 1997). Figures 2C,D are the evolutions of Raman images, measured over 180 × 70 μm2 with 400 × 150 Raman spectra, during the first charge and discharge respectively, which were constructed using the intensity distributions of the A1g mode of LiCoO2 and the carbon G band at ~1,600 cm−1. Starting with fully lithiated LCO (green) at 3.5 V, delithiated LCO (black) formed and grew during charge, eventually reached 94% of the total measured area at 4.4 V, and holding the cell at 4.4 V for an additional 16 h did not delithiate LCO completely (~2.5% of total measured area remained green), Figure 1C. The images show a reversed change, the lithiated areas (green) increase to 90% at 2.5 V when the electrode is discharged at 1C rate (Figure 1D). These images illustrate that both charge and discharge rates are significantly different from particle to particle. Figure 2F is a comparison of the Raman images of the 1st and 2nd cycles. Most of the particles were charged and discharged normally, but the behavior of two types of particles directly contributes to the capacity loss: (1) particles were charged at a slower rate in the 1st charge process and could not be discharged in the following cycle (yellow arrows); (2) particles were charged and discharged at a slower rate during the 2nd cycle (blue arrows) resulted in an accumulated delithiated particles of 16% at the end of the 2nd discharge which is more than that of the 1st cycle (10%). The degradation of the electrode with cycling is consistent with the delayed and incomplete phase transformation in comparison of the operando XRD spectra of 1st and 5th cycles (Figures 2A,E). After stopping the discharge at 2.5 V, the cell voltage relaxed back to 3.7 V, then was discharged again to 3 V at C/5 and held for 3 h, the delithiated particles were reduced from 10 to 2% for the first cycle (no data was reported for the 2nd cycle). The existence of these “slow” particles is mainly due to the poor local conductivities (Nishi et al., 2013). The operando Raman measurements expose the cause of degradation, i.e., the inhomogeneity of carbon distribution on micrometer scale which makes some particles “slow.” This situation will be aggravated at high cycling rate and after more cycles (Kostecki and McLarnon, 2004). Operando XRD measurements show that phase transformation proceeds progressively, whereas Raman analysis adds details to this progressive transition which is mainly attributed to the reaction speed difference of individual particles caused by local conductivity difference.
LiMn1.5Ni0.5O4 is a high-voltage cathode material with high energy density and low cost, but its cycling stability at high rates needs to be improved for use in practical applications. LiMn1.5Ni0.5O4 has two different structures, disordered and order, based on the Ni and Mn cation distributions in the LMN. The disordered LMN has a cubic spinel structure with space group Fdm, where the Ni and Mn ions are randomly distributed at the octahedral 16d sites. In contrast, the ordered LMN has the P4332 space group, in which the Ni and Mn ions are located in an orderly fashion at the split 4a and 12d sites (Kim et al., 2004; Takahashi et al., 2004; Amdouni et al., 2006). The disordered LMN has better rate capacity because of its higher electric conductivity (Kunduraci et al., 2006) and lithium ions diffusivity (Minami et al., 2005).
The phase evolution during lithium de-intercalation/ intercalation of these two structures was studied using in-situ XRD (Kunduraci and Amatucci, 2006; Rhodes et al., 2011; Wang et al., 2011; Hugues et al., 2014; Zhu et al., 2014; Komatsu et al., 2015; Saravanan et al., 2015; Samarasingha et al., 2016) and in situ Raman (Dokko et al., 2002, 2004; Zhu et al., 2015). Figure 3A displays the development of the XRD spectra of a LixMn1.45Ni0.45Cr0.1O4 (Cr-LMN) cathode cycled at C/24 with expanded views of peaks (311) and (511) in Figure 3B. The initial phase is cubic spinel (S.G. Fdm) with a = 8.177 A (Phase-1). All the diffraction peaks shift to higher 2θ angles as the lithium ions are continuously removed from the host structure and two more phases (Phase-2 and Phase-3) form during charge. Upon discharge, the evolution of the spectra changes reversibly. The analysis of the XRD patterns shows that all the phases in the spectra are cubic spinel (S.G. Fdm), and the lattice parameters for each phase as a function of lithium content (x) are obtained from Rietveld refinement of the spectra and plotted in Figure 3D. Figure 3E shows the variation of the cell voltage with x and the corresponding phases. As charge proceeds from x = 1, a solid solution is in the range of 1 ≤ x ≤ 0.72; the decrease in Li results only in the decrease of the lattice parameter of the cubic Phase-1. A new cubic spinel phase (Phase-2) starts to emerge and the system entered in a two-phase domain, 0.72 ≤ x ≤ 0.54, in which the Phase-2 grows at the expense of the Phase-1 and Phase-1 eventually disappears at x = 0.54. Below this concentration, 0.54 ≤ x ≤ 0.37, the Cr-LMN is again a solid solution of the Phase-2 only. The system re-enters a two-phase region in the range 0.37 < x < 0.13 with the coexistence of Phase-2 and a new phase (Phase-3) that grows at the expense of Phase-2. Finally, a solid solution with Phase-3 only is observed in the range x ≤ 0.13. There is a difference between charge and discharge curves in Figure 3E that suggest the thermodynamic equilibrium is not reached even at a slow rate of C/24. The off-equilibrium effects evidenced by hysteresis in the structure and electrochemical properties between charge and discharge as a function of x are also linked to its cation disorder (Zhu W. et al., 2013).
Figure 3. Operando XRD (Zhu W. et al., 2013) and Raman (Zhu et al., 2015) measurements on LixMn1.45Ni0.45Cr0.1O4 cathodes during galvanostatic cycle at C/24; (A) Evolution of XRD patterns as a function of lithium concentration; (B) XRD patterns focused on (311) and (511) peaks which clearly show the three different phases present during charge; (C) Development of Raman spectra during cycle, the appearance of new bands at 170 and 539 cm−1 toward the end of charge attributed to the vibration modes of Ni4+-O bond; the two bands are initially observed at ~4.76 V corresponding to Phase-3 formation detected by operando XRD. Blue: charge; black: discharge; voltage and x values of orange spectra are labeled; (D) Variation of the lattice parameters of different cubic phases in Cr-LMN as a function of Li concentration; (E) Relation of cell voltage, lithium concentration and phases determined via operando XRD.
While the phase-lithium content relation is determined by operando XRD, the oxidation state of Ni ions is investigated via operando Raman. The vibration modes of Cr-LMN are experimentally detected at 162(T2g(T)), 408(Eg(Ni2+/Mn4+)), 498(T2g(Ni2+)), 528 (T2g(Ni2+)), 593(A1g(Mn4+)), 613(A1g(Ni2+)), 639 (A1g(Mn3+/ Ni2+)), 672 cm−1(T2g(Cr3+)) (Zhu et al., 2015). The evolution of the Raman spectra of a Cr-LMN electrode cycled at C/24 is shown in Figure 3C and has the following characteristics:
(1) Near the end of charge, the intensity of the 162 cm−1 band decreases and finally disappears, accompanied by the formation and growth of a new band at 170 cm−1 which is first observed at ~4.76 V (x~0.39), and assigned to the translation mode of the lattice vibration, T2g(T). This 4.76 V is close to the potential of the 2nd anodic peak in the plot of dQ/dV vs. V (Zhu et al., 2015) which is related to the oxidation of Ni3+ to Ni4+. Compared to the phase diagram in Figure 3E, it is reasonable to assume that the appearance of the 170 cm−1 band corresponds to the presence of Phase-3 with less lithium. The lattice parameter of Phase-3 is ~2% smaller than that of Phase-1 leading to the up shift of this vibration mode from 162 to 170 cm−1.
(2) A new band at ~539 cm−1 is observed at the same time as the 170 cm−1 band and reaches its maximum as the voltage approaches 4.9 V, it is identified as the symmetric vibration of the Ni4+-O bond, T2g(Ni4+); simultaneously, the band at 528 cm−1 (T2g(Ni2+)) fades away. The initial broadening of the 528 cm−1 band is attributed to the formation of the Ni3+-O bond, and its disappearance indicates the Ni2+/Ni3+ are oxidized to Ni4+.
(3) A small band is detected at ~586 cm−1 as the voltage approaches 4.9 V and is attributed to the asymmetric vibration of the Ni4+-O bond, which evolved from A1g(Ni2+-O) at 613 cm−1.
(4) The broadening of the 498 cm−1 band is seen near 4.9 V, leading to the presence of a small new band at ~486 cm−1 at ~ 4.9 V (x ~ 0.12), which is ascribed to a stretching mode of Ni4+-O.
(5) During discharge, the evolution of the Raman bands proceeds reversely, all the new bands formed during charge fade away and the bands in the pristine cathode reappear.
In summary, the operando Raman spectroscopy study of Cr-LMN establishes the relation of oxidation state of Ni ion and the corresponding phases, i.e., Phase-2 is associated to the phase where all Ni2+ are converted to Ni3+, i.e., Li0.55Mn1.45Ni0.45 Cr0.1O4. Similarly, Li0.1Mn1.45Ni0.45Cr0.1O4 is Phase-3 at equilibrium, corresponds to the state where all of the nickel ions are converted to Ni4+.
Lithium iron phosphate is one of the most investigated cathode material for lithium-ion batteries due to its high theoretical capacity (170 mAh/g), long cycle life, good thermal stability, high reversibility, low cost, non-toxicity and high safety characteristics (Joachin et al., 2009; Ramana et al., 2009; Dong et al., 2017). LiFePO4 and FePO4 (FP) have similar crystal structure described by space group Pnma, but different lattice parameters. When the LiFePO4 cathode is charged and discharged, the Li+ ions are de-intercalated and intercalated, respectively, along a channel in the  direction (Islam et al., 2005; Li et al., 2018). Several models, such as Shrinking core model (Padhi et al., 1997), Domino cascade model (Delmas et al., 2008) describe the phase transformation between LiFePO4 and FePO4, but the mechanism is still in debate. As a result, several operando techniques were applied to understand the process (Perea et al., 2012; Orikasa et al., 2013; Ouvrard et al., 2013; Dong et al., 2017), especially using operando XRD (Shin et al., 2008; Roberts et al., 2014) and operando Raman (Wu et al., 2013; Siddique et al., 2015). The LFP↔FP transition is generally considered as a two-phase reaction (Chen et al., 2006; Laffont et al., 2006; Zhu Y. et al., 2013), also confirmed by XRD measurements conducted on slow cycled cells (Andersson et al., 2000; Shin et al., 2011; Siddique et al., 2015). Figure 4A shows the diffraction patterns (top) and corresponding cycling curve (bottom) at rate of 1C. The transformation of LFP to FP was first observed at Li = 0.62 at 1C, the same authors also reported the beginning of FP formation at Li = 0.80 at slower rate of C/5. The content of FP increases at the expense of LFP as charge proceeds, LFP disappeared completely after voltage reached 4.3 V; and the development of the phase reverses during discharge. The diffraction patterns show that the peak positions of the two phases are unchanged, suggesting a two phase reaction mechanism at the cycling rate of 1C or slower. The same technique is also used to explore the behavior of LFP nano-particles cycled at high rate. Figure 4B shows diffraction patterns (bottom) and the image plot of diffraction patterns (top) for (200), (211), (020), and (311) lines obtained on a LFP cathode cycled at 10C rate by using synchrotron X-ray (λ = 0.7272A). Authors indexed all the peaks observed to either the Li-rich Li1−αFePO4 or the Li-poor LiβFePO4 in the space group Pnma. As expected in the cycling at slow rate, Li1−αFePO4 peaks disappear on charge and are restored on discharge; LiβFePO4 peaks start to form and grow on charge and disappear on discharge. Unlike in the case of slow cycling, there are appreciable positive intensities within the 8.15° (LPF(200)) to 8.4° (FP(200)), 13.95° (LFP (211)/(020)) to 14.1° (FP(211)), and 15.15° (LFP(301)) to 15.4° (FP(301)) 2θ ranges, which indicate the existence of phases with lattice parameters that deviate from those of LiFePO4 and FePO4 under equilibrium (the corresponding (hkl) of LFP/FP are labeled in the parentheses). The phenomenon is more pronounced at 20C (not shown here). Figure 4B2 shows that all the peaks are symmetrical at the onset of the first charge, the LFP(200) and (301) started to broaden asymmetrically toward higher angles as charge proceeded. The most severe asymmetrical broadening is around beginning of discharge in both 1st and 2nd cycles. Neither the peak position nor the peak shape of LFP is restored to that of the original state at the end of the discharge, indicating a solid solution of Li1−αFePO4 was formed, which has smaller unit cell and more disordered structure compare to the pristine LFP. These results reveal a different mechanism at high cycling rate, i.e., LFP transforms to FP through a non-equilibrium solid solution instead of two-phase reaction. Capacity fading mechanism in a 18,650 commercial battery was also explored by in situ XRD; the authors observed a different mechanism in LFP/FP conversion after long cycling by formation of a single Li1−xFePO4 phase (Liu et al., 2018). These operando XRD investigations indicate that the working mechanism of the electrode materials may vary with the operating conditions, which may also shed the light on the failure mechanisms under different conditions.
Figure 4. (A) C-coated LiFePO4 charged at 1C rate (A1) Evolution of XRD spectra shows that the FP is first detected at Li = 0.62, and the LFP disappears completely at 4.3 V; (A2) corresponding charge-discharge curve (Shin et al., 2011 with permission from Elsevier); (B) LFP cycled at a rate of 10C (Liu, H. et al., 2014); (B1) image plot of diffraction patterns for (200), (211), (020), and (301) reflections during first five cycles; the scale bars of diffraction intensity are shown on top. The corresponding voltage curve is plotted to the right. (B2) diffraction patterns from first two cycles stacked against the voltage profile; black vertical lines mark the positions of LFP peaks at the start of reaction; red vertical lines mark the position of FP peaks formed during the first cycle; with permission from AAAS. (C) Raman spectra collected on LFP electrode surface at a cycling rate of 0.3C (Siddique et al., 2015); (C1) carbon-rich spot A during charge; (C2) spot A during discharge; (C3) carbon-poor spot B during charge; (C4) spot B during discharge; (C5) corresponding electrochemical cell performance curve with vertical lines indicating the moment when the Raman spectra were taken; with permission from Wiley-VCH Verlag GmbH&Co. KGaA, Weinheim.
The operando XRD examines the collective behavior of LFP particles on a centimeter scale, whereas Raman spectroscopy explores the local-phase transformation in the micrometer region. The conductivity of LFP is enhanced by adding carbon to the electrode. Figure 4C presents the Raman spectra collected from carbon-rich (Figures 4C1,2) and carbon-poor (Figures 4C3,4) regions of the electrodes during cycling at 0.3C. The bands at ~950 and 960 cm−1 are attributed to the symmetric stretching mode of in LFP and FP. During charge (Figure 4C1), the spectra show little change to the end of the 3.5 V plateau, then the 950 cm−1 band vanishes and 960 cm−1 band appears suddenly (red dot in Figure 4C5); the reverse change during discharge (Figure 4C2) is observed after the beginning of the discharge plateau (green dot in Figure 4C5). The evolution of the spectra demonstrates that the phase transformation between the LFP and FP particles is fast in the carbon-rich environment. A different phenomenon is seen in the carbon-poor area, where no abrupt phase change is detected during charge and discharge, (Figures 4C3,4); the main part of LFP does not participate in the reaction, which indicates that less carbon in the area reduces the local conductivity between the LFP particles, thus decreasing electrochemical charge transfer in the active material and leading to capacity loss. These results point out that the problem of capacity loss can be mitigated by converting the non-active regions of the electrode to active regions via homogenizing carbon distribution on a nano-scale. It is clear from both XRD and Raman that the progressive phase transformation observed via XRD is mainly attributed to the increase in the number of completely transformed particles.
Lithium–sulfur batteries have a high theoretical capacity of 1,675 mAhg−1 and utilize low-cost materials. The discharge mechanism of the sulfur electrode is a complex and controversial issue, which was investigated by various in situ techniques (Nelson et al., 2012; Cañas et al., 2013; Cui et al., 2013; Cuisinier et al., 2013; Hagen et al., 2013; Patel et al., 2013; Gorlin et al., 2015; Marceau et al., 2016; Paolella et al., 2016). These studies indicate that elemental sulfur discharge is a multi-step process involving different intermediate species that are sensitive to the electrolyte and the operating conditions.
Operando XRD is used to study the battery working mechanism, but it cannot recognize the intermediate poly-sulfides (PSs) due to their non-crystalline nature. The phases which can be identified are the initial phase of α-S8 (orthorhombic, a = 10.465, b = 12.866, c = 24.486, S.G.: Fddd), the end product of discharge Li2S(a = 5.72 A, S.G.: Fmm), and end product of charge, β-S8 (monoclinic, a = 10.926, b = 10.855, c = 10.790 A, β = 95.92, S.G.: P21/c) (Walus et al., 2013; Lowe et al., 2014), as shown in Figure 5b (Walus et al., 2013). To study this problem, fused silica is added to the electrolyte because it reacts with the intermediate species and leads to specific absorption of long chain poly-sulfides to form an organized layer (Lay et al., 2003; Hwang et al., 2016) from which the finger prints of the absorbed poly-sulfides are detected via XRD. Figure 5a (Conder et al., 2017) shows the evolution of the XRD spectra from the cell with fused silica during the first cycle (left), the corresponding contour plot (right), and the galvanostatic curve (center). The starting red pattern is from α-S8. It disappears quickly as discharge begins, and two broad peaks are observed at 25.56° and 28.32° immediately (labeled PS1 and PS2 respectively). At this early stage of lithiation, the peaks may be related only to the long-chain PSs, the authors attributed them to Li2S8, or toLi2S6. These two peaks reach a maximum at the end of the first discharge plateau on which the lithiation corresponds to a liquid-liquid equilibrium and Li2S8 is reduced to Li2S6, then to Li2S4. Near the end of discharge, a new peak at ~27° is detected (orange pattern) that is ascribed to cubic Li2S. Meanwhile PS1 and PS2 decrease toward the end of the discharge, but do not disappear completely, indicating the incomplete reduction of PS1/PS2. During charge, the phase evolution process is reversed, except the final product is monoclinic β-S8 (green) instead of α-S8.
Figure 5. (a) Development of XRD patterns of a Li-S cell with fused silica additive during first cycle (left), corresponding galvanostatic curve at C/50 (center) and XRD image plot (right). The colored patterns (left) correspond to colored dots on the cycling curve (center). α-S8 and β-S8 are represented by white lines with diamond and oval symbols, respectively (right). PS1 and PS2 are attributed to the PSs–SiO2 interactions (vertical black dashed lines). Li2S is symbolized by a dashed-dotted black vertical line; * is from cell package (Conder et al., 2017); with permission from Springer Nature; (b) XRD patterns of a cell during 1st cycle with corresponding electrochemical plot; arrow, Li2S; *, cell package; bold lines indicate initial appearance of solid phase and subsequent disappearance (Walus et al., 2013); with permission from RSC; (c) Raman spectra from 1 M LiTFSI–DOL–DME electrolyte on the lithium side during first cycle; * separator (Zhu et al., 2017). (dA-C) Raman spectra of sulfur cathode during discharge; (dD) Cyclic voltammetry of as-prepared sulfur-carbon cathode and potential dependence of the peak intensities (Wu et al., 2015); with permission from ACS.
The nature of the non-crystalline intermediate PSs formed during cycling makes the XRD analysis difficult, even with the above-mentioned method. On the other hand, Raman spectroscopy can clearly detect different species formed in the cathode and dissolved in the electrolyte (Yeon et al., 2012; Hannauer et al., 2015; Paolella et al., 2018). Figure 5c (Zhu et al., 2017) displays the development of Raman spectra of the electrolyte (1M LiTFSI-DME-DOL) near the lithium anode during the 2nd cycle. It is interesting to note that elemental sulfur is observed at the end of charge near lithium anode; this sulfur is β-S8 according to operando XRD, which cannot be distinguished from α-S8 by Raman spectra in the measured region. The loss of active material near the lithium anode reduces the local conductivity and corrodes the lithium, which has a negative effect on battery capacity and cycle life. The effect of the electrolyte on the discharge mechanism was also studied in the same work. The species detected in the 1M LiTFSI-DME-DOL electrolyte near the Li electrode of an as made cell are and , indicating a rapid self-discharge in this widely used liquid electrolyte. In contrast, self-discharge is much slower in an ionic liquid, where elemental S8 began to appear on the lithium side at the middle of the high-voltage plateau, and remains until the end of the plateau where and are observed. The mechanism and kinetics of sulfur reduction in LiTFSI-TEGDME-DIOX electrolyte was investigated by operando Raman, and the results are shown in Figure 5d (Wu et al., 2015). S8/, , S4− and S3·− are detected at different stages of discharge, and the process is summarized as (1) the formation of long chain PSs as S8 ring opens at ~2.4 V; (2) the short chain PSs start to form at ~2.3 V and they decompose again at 1.6 V. The rate constants of different species are obtained from the evolution of the spectra by fitting the appearance and disappearance of bands to a pseudo first order reaction. Compared to the PSs observed in LiTFSI-DME-DOL, an additional specie S3·− is detected in LiTFSI-TEGDME-DIOX, indicating that the intermediate PSs are sensitive to the electrolyte used, thus the different discharge mechanisms may vary with the electrolyte chosen. The insights gained from operando Raman analysis provide an explanation for one of the causes of capacity fade, and may be a helpful guide in the selection of a more appropriate electrolyte.
We reviewed the application of operando X-ray diffraction and operando Raman techniques to characterize operating batteries along with the importance of these techniques to help researchers to understand how the rechargeable batteries work, why they behave in their specific ways, how and why they fail. Operando XRD provides information on the average crystal structural changes of electrodes during cycling. Operando Raman probes the structure of individual particle on the electrode surface, the electrode-electrolyte interface and the electrolyte as well as the species in it to reveal information related to the oxidation state of ions and the interatomic bond length, etc. Raman maps constructed from the information collected describe the behavior of individual electrode particles under operating condition and their influence on the kinetics of phase transformation that is directly related to the battery rate capacity and cycle life. The information obtained by both in situ XRD and Raman methods leads to an atomic level understanding of the variations of structure and its stability, the development of surface and interface structures, which are critical to the battery performance. But for the improvement of the existing electrode materials, the design of new high performance materials, we need more advanced in-situ techniques to reveal the working and degradation mechanisms of different materials. For this purpose, the present operando techniques have to be ameliorated and developed in the directions of (1) multi-functioning, to allow collecting different types of information simultaneously; (2) capability of obtaining 3D morphology information of electrode which is important for improving electrode quality; (3) rapid measurement/fast data collection, to monitor the non-equilibrium state and the rate effect on the materials; (4) ability of measuring the desired materials in the same environment and conditions as the battery in practical applications.
WZ wrote the draft. All authors contributed to the writing, discussion and revision of the final version.
Centre d'excellence en électrification des transports et stockage d'énergie, Québec, Canada.
Conflict of Interest Statement
The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.
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Keywords: operando/in-situ XRD, operando/in-situ Raman, lithium-sulfur, layered metal oxide, LiFePO4, spinel oxide
Citation: Zhu W, Liu D, Paolella A, Gagnon C, Gariépy V, Vijh A and Zaghib K (2018) Application of Operando X-ray Diffraction and Raman Spectroscopies in Elucidating the Behavior of Cathode in Lithium-Ion Batteries. Front. Energy Res. 6:66. doi: 10.3389/fenrg.2018.00066
Received: 28 February 2018; Accepted: 19 June 2018;
Published: 31 July 2018.
Edited by:Verónica Palomares, University of the Basque Country (UPV/EHU), Spain
Reviewed by:Zhixiang Shi, Southeast University, China
Xifei Li, Xi'an University of Technology, China
Copyright © 2018 Zhu, Liu, Paolella, Gagnon, Gariépy, Vijh and Zaghib. This is an open-access article distributed under the terms of the Creative Commons Attribution License (CC BY). The use, distribution or reproduction in other forums is permitted, provided the original author(s) and the copyright owner(s) are credited and that the original publication in this journal is cited, in accordance with accepted academic practice. No use, distribution or reproduction is permitted which does not comply with these terms.
*Correspondence: Karim Zaghib, firstname.lastname@example.org