Chunrong
Ma
ab,
Zhengguang
Fu
cd,
Yanchen
Fan
e,
Hui
Li
ab,
Zifeng
Ma
f,
Wei
Jiang
ab,
Guangshuai
Han
*g,
Haoxi
Ben
*ab and
Hui (Claire)
Xiong
*h
aCollege of Textiles & Clothing, Qingdao University, Qingdao 266071, China
bKey Laboratory of Bio-Fibers and Eco-Textiles, Qingdao University, Qingdao 266071, China
cSchool of Polymer Science and Engineering, Qingdao University of Science and Technology, Qingdao 266110, China
dInstitute of Bioenergy and Bioprocess Technology, Chinese Academy of Sciences, Qingdao 266101, China
ePetroChina Shenzhen New Energy Research Institute, Shenzhen, 518000, China
fSchool of Chemistry and Chemical Engineering, Shanghai Jiao Tong University, Shanghai 200240, China
gInstitute for Advanced Study, Tongji University, Shanghai 200092, China
hMicron School of Materials Science and Engineering, Boise State University, Boise, ID 83725, USA. E-mail: clairexiong@boisestate.edu
First published on 7th May 2024
Transition metal sulfides (TMS) have gained significant attention as potential anode materials for sodium ion batteries (SIBs) due to their high theoretical capacity and abundance in nature. Nevertheless, their practical use has been impeded by challenges such as large volume changes, unstable solid electrolyte interphase (SEI), and low initial coulombic efficiency (ICE). To address these issues and achieve both long-term cycling stability and high ICE simultaneously, we present a novel approach involving surface engineering, termed as the “dual-polar confinement” strategy, combined with interface engineering to enhance the electrochemical performance of TMS. In this approach, CoS crystals are meticulously coated with polar TiO2 and embedded within a polar S-doped carbon matrix, forming a composite electrode denoted as CoS/TiO2-SC. Significantly, an ether-based electrolyte with chemical stability and optimized solvation properties synergistically interacts with the Co–S–C bonds to create a stable, ultra-thin SEI. This concerted effect results in a notably high ICE, reaching approximately 96%. Advanced characterization and theoretical simulations confirm that the uniform surface modification effectively facilitates sodium ion transport kinetics, restrains electrode pulverization, and concurrently enhances interaction with the ether-based electrolyte to establish a robust SEI. Consequently, the CoS/TiO2-SC electrode exhibits high reversible capacity, superior rate capability, and outstanding cycling stability.
Beyond electrode structure engineering, the electrochemical behavior of materials also hinges on the electrolyte. Recent research has shed light on the pivotal role of electrolytes in shaping the structural evolution and electrochemical behavior of SIB anodes.19–22 For instance, Huo et al. demonstrated noticeable differences in SEI films formation on CoS2 electrode when employing electrolytes like NaClO4/propylene carbonate (PC) and NaPF6/diethylene glycol dimethyl ether (DEGDME).23 They achieved superior cycling performance using the NaPF6/DEGDME electrolyte, suggesting that electrolytes containing NaPF6 in glymes are beneficial for forming a stable SEI layer that has good passivating properties for reversible operation. However, this strategy faces challenges from recent research indicating that the presence of NaPF6 during SEI formation may inevitably generate harmful hydrofluoric acid with trace water, which could attack electrolytes and degrade their performance if it is not controlled.24,25 Furthermore, most research efforts have concentrated on comparing the performance of electrode materials in different electrolyte systems, often overlooking the profound influence of the choice of electrolyte on the electrode itself. It is crucial to recognize that understanding the intricate interplay between the electrode and electrolyte is of paramount importance as it directly affects electrode kinetics and SEI chemistry. Therefore, in the pursuit of exceptional electrochemical properties for CoS-based anode materials, it is imperative not only to design composite assembly structures but also to comprehend the effects of various electrolytes.
Here, a new “dual-polar confinement” strategy is proposed, wherein the inner polar TiO2 coated CoS crystals, encapsulated within an outer polar S-doped carbon matrix, are fabricated through a sequence of co-precipitation and self-assembly process, followed by high-temperature sulfuration (denoted as CoS/TiO2-SC). The TiO2 layer plays a crucial role in anchoring dissolved polysulfide intermediates, thereby preserving the structural stability of the CoS particles during charge and discharge cycles. Importantly, we have identified that a DEGDME-based electrolyte, with exceptional electrochemical stability and optimized solvation properties, synergistically interacts with the Co–S–C bonds to form a stable, ultra-thin SEI. This results in an exceptionally high ICE in SIBs. The SEI composition and the composite structural stability have been comprehensively validated through a range of ex situ characterizations and theoretical simulations. As a result of this synergistic approach involving surface engineering with a dual-polar layer and interphase engineering via electrolyte modulation, CoS-based anode materials exhibit impressive high capacity and rate performance, even after 3000 cycles. This study provides a theoretical and technological foundation for understanding the interfacial and structural stability of various metal sulfide anode materials for long-term operation, offering a significant contribution to the field of sodium-ion battery research.
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Fig. 1 (a) Scheme illustration of the synthesis process of CoS/TiO2-SC composite, (b–d) SEM images, (e–g) TEM images of CoS/TiO2-SC composite. |
The crystal structure of the as-prepared CoS/TiO2-SC composite is presented in Fig. 2a. The X-ray diffraction (XRD) pattern of the sample reveals distinct diffraction peaks at various angles, including 30.5°, 35.2°, 46.8°, 54.3°, 62.5°, 66.3°, and 74.5°. These peaks correspond to the (100), (101), (102), (110), (103), (201), and (202) planes of hexagonal CoS (PDF. 75-0605). Additionally, a broad peak at 24.5° corresponds to the diffraction peak of carbon. No distinct TiO2 diffraction peaks are detected, likely due to the amorphous nature of TiO2. Raman spectroscopy was employed to examine the surface properties of the CoS/TiO2-SC composite (Fig. 2b). Two characteristic peaks are observed at 1357 and 1580 cm−1, corresponding to the D and G bands, respectively. The ratio of ID/IG provides insight into the degree of disorder in the carbon structure.26,27 A calculated ID/IG value of 1.35 for CoS/TiO2-SC indicates a high level of disorder and defect, and this disorder may be attributed to S-doping. Moreover, five peaks within the black box in Fig. 2b are consistent with TiO2,28 and the peak at 687 cm−1 is characteristic of CoS.29 These results confirm the successful synthesis of CoS/TiO2 embedded within the carbon structure. The chemical state and composition of CoS/TiO2-SC were further analyzed through X-ray photoelectron spectroscopy (XPS). The XPS survey (Fig. S3a†) reveals the presence of Co, S, Ti, O, and C elements in the CoS/TiO2-SC composite. In the high-resolution Co 2p spectrum (Fig. 2c), peaks at binding energies of 778.3 and 797.2 eV correspond to Co3+, while peaks at 780.6 and 802.2 eV are attributed to Co2+.30,31 A pair of broad satellite peaks accompanies these Co peaks. The peak-fitting analysis of the Ti 2p spectra (Fig. 2d) reveals two peaks at binding energies of 458.5 and 464.2 eV, corresponding to Ti 2p3/2 and Ti 2p1/2, respectively.32 The S 2p spectrum (Fig. 2e) exhibits two peaks at 161.8 and 163.6 eV, corresponding to S 2p3/2 and S 2p1/2, respectively. Additionally, peaks at 165.7 and 169.0 eV can be ascribed to C–S and SOx bonds, with a small peak at 160.3 eV indicating chemical interaction between CoS and carbon through the C–S–Co combination.33 The high-resolution O 1s spectrum (Fig. S3b†) features three peaks at 529.6, 531.5, and 532.2 eV, corresponding to Ti–O, C–O, and H–O bonds, respectively.34 The C 1s spectrum (Fig. 1f) displays two prominent peaks at 284.4 and 288.1 eV, attributed to C–C and C–S bonds, suggesting the presence of S groups within the carbon structure.35 Doped sulfur is known to modify the electronic properties of carbon, facilitating ion transport.36 These findings provide detailed information about the chemical composition and state of the elements within the CoS/TiO2-SC composite. The carbon mass in the CoS/TiO2-C composite was determined via Thermogravimetric Analysis (TGA). As depicted in Fig. S4,† a marginal weight increase was observed between ∼200 and 420 °C, attributed to the oxidation of CoS. Subsequent weight loss occurring within the range of 400–900 °C was attributed to the combustion of carbon and further oxidation of CoS to metal oxides.37 The calculated carbon content in the CoS/TiO2-C composite samples was approximately 38%.
The electrochemical performance of the synthesized CoS/TiO2-SC composite in DEGDME-based electrolyte is thoroughly examined by assembling CR2032 half-cells. Fig. 3a depicts the charge–discharge profiles of the CoS/TiO2-SC electrode at a current density of 0.2 A g−1 within the voltage range of 0.01–3 V. In the initial cycle, the CoS/TiO2-SC electrode exhibits a discharge and charge specific capacity of 813 and 769 mA h g−1, respectively, resulting in a high ICE of 94.5%. This ICE is notably higher than the 79% ICE observed for the CoS-SC electrode (Fig. S5†). In the initial cycle, the CoS/TiO2-SC electrode exhibits a discharge and charge specific capacity of 813 and 769 mA h g−1, respectively, resulting in a high ICE of 94.5%. The improved ICE could be attributed to the incorporation of TiO2, which has the ability to adsorb polysulfides, thereby mitigating the escape of polysulfide intermediates. Importantly, the CoS/TiO2-SC electrode shows a CE that rapidly approaches ∼100% within the first 3 cycles, indicating the formation of a stable SEI. In contrast, the CoS-SC electrode maintains an average CE of ∼95% over the initial 3 cycles. Furthermore, the CoS/TiO2-SC electrode displays a superior specific capacity and better capacity reversibility in subsequent cycles. To gain deeper insights into the Na+ storage behavior of the CoS/TiO2-SC electrode, cyclic voltammetry (CV) are conducted within the voltage window of 0.01–3 V (Fig. 3b). For the CoS/TiO2-SC electrode, a broad peak appears at ∼0.88 V during the initial cathodic scan and disappears in subsequent scans, indicating the formation of the SEI.6,38–40 The peak at ∼0.75 V corresponds to the conversion reaction of CoS to Co and Na2S.7 After the initial cathodic scan, the reduction peak divides into four peaks at 0.63, 0.96, 1.21, and 1.65 eV. In the anodic process, the 1.45 and 1.77 V peaks can be attributed to the reverse reaction, forming metal sulfides. A pair of small peaks near 0 V reflects reversible Na storage in the carbon.41,42 The cycling performances of the CoS/TiO2-SC and CoS-SC electrodes are compared (Fig. 3c). The CoS/TiO2-SC electrode delivers a high reversible capacity of 780 mA h g−1 at a current density of 0.2 A g−1, whereas the CoS-SC electrode achieves only 387 mA h g−1 under the identical conditions. After 100 cycles, the CoS/TiO2-SC electrode maintains a stable capacity, while capacity fading is observed in the CoS-SC electrode. Furthermore, the CE of the CoS/TiO2-SC electrode rapidly stabilizes at 100% after the initial cycles. In contrast, the CE of the CoS-SC electrode continuously fluctuates around an average value of 95%, likely due to the continuous formation of the SEI (Fig. S6†). The rate capability of both electrodes is evaluated (Fig. 3d). The CoS/TiO2-SC electrode consistently outperforms the CoS-SC electrode at all tested current densities, with the capacity gap increasing as the current density rises. Specific capacities of 592, 578, 554, and 512 mA h g−1 are achieved for the CoS/TiO2-SC electrode at current densities of 1, 2, 5, and 8 A g−1, respectively. Even at a high current density of 10 A g−1, the CoS/TiO2-SC electrode still delivers 478 mA h g−1. Upon returning to a current density of 0.2 A g−1, the specific capacity promptly returns to 764 mA h g−1. In contrast, the CoS-SC electrode exhibits a low capacity of 236 mA h g−1 at a high current density of 10 A g−1, with significant capacity fading, primarily due to slow reaction kinetics and poor reversibility. The long-term cycling stability is crucial for evaluating sodium storage performance. The CoS/TiO2-SC electrode is subjected to cycling at a high current density of 5 A g−1. As shown in Fig. 3e, the CoS/TiO2-SC electrode maintains a reversible capacity of 510 mA h g−1 after 3000 cycles, demonstrating excellent electrochemical reversibility. The effect of surface engineering involving the introduction of TiO2 coating on the sodium storage is investigated by density functional theory (DFT) calculations. As shown in Fig. S7,† the introduction of TiO2, providing it as polysulfide adsorbent, exhibits a considerably higher adsorption capacity for polysulfides in comparison to carbon-based materials. Consequently, the designed CoS/TiO2-SC composite, featuring the polar TiO2 and S–C bond, could effectively inhibits the escape of the polysulfide intermediates through a polar–polar interaction mechanism,43 thus ensuring the cycling stability. To better understand the Na+ storage mechanism, CV experiments were conducted at varying scan rates, ranging from 0.1 to 2 mV s−1. Notably, the CV curves maintain their characteristic shape at the scan rate increases (Fig. 3f). Typically, the charge total charge storage can be described by the following formula:44
i = avb | (1) |
i = k1v + k2v1/2 | (2) |
![]() | (3) |
Notably, the sodium ion diffusion kinetics in CoS/TiO2-SC electrode demonstrate a faster rate compared to those in CoS-SC electrode (Fig. 3h). This distinction stands as a primary contributing factor to the superior rate capability observed in the CoS/TiO2-SC electrode. The average value of corresponding DNa+ in CoS/TiO2-SC electrode was 6 × 10−10 during discharge process. For a deeper insight into the impact of surface engineering through TiO2 coating on sodium storage, DFT calculations are performed to assess the polysulfide adsorption capability of the introduced TiO2 in comparison to conventional carbon materials. As depicted in Fig. S7,† it is observed that the carbon, TiO2, and TiO2@C structures exhibit negative adsorption energies, indicating their suitability for interacting with polysulfides. Remarkably, the TiO2@C structure displays a more robust polysulfide capture capability compared to both carbon and TiO2. This dual-polar effect effectively hinders the escape of polysulfide intermediates, thereby ensuring enhanced cycling stability.
The structural transformation occurring in the CoS/TiO2-SC electrode during charge and discharge processes were further investigated through in situ XRD analysis. As shown in Fig. 4a, the characteristic peaks corresponding to CoS gradually decrease as the discharge process proceeds, indicating the involvement of CoS in the sodiation reaction. Subsequently, new peaks (24.3°) emerge and persist as the discharge progresses to lower potentials, indicating the formation of Na2S during the sodiation reaction. As the discharge process proceeds, the CoS peaks continue to weaken, while the Na2S peaks concurrently intensify until the CoS peaks completely vanish, indicating the full conversion of CoS into Co and Na2S. Throughout the charging process, the Na2S diffraction peaks gradually weaken and eventually disappear, accompanied by the reemergence of CoS peaks, indicating the desodiation process. Simultaneously, the CoS peaks gradually reappear during the desodiation until the end of charging, suggesting the regrowth of the CoS phase. Importantly, no Na2S peaks are detected at the fully charged state, indicating the reversibility of the process. Co peaks are not observed during the charge/discharge process, which could be attributed to the low crystallinity of the generated Co.48 The conversion reaction mechanism of the CoS/TiO2-SC electrode is presented in Fig. 4b. To gain more insight into the kinetic process, the sodium adsorption energy of CoS, TiO2, and CoS/TiO2 was computed. As shown in Fig. 4c–e, CoS/TiO2 exhibits the smallest Na adsorption energy of −2.88 eV, indicating an exceptional sodium affinity of the surface-engineered composite. These interactions effectively inhibit the dissolution of soluble active cobalt species and enhance long-term cycling stability during the charge/discharge process. Furthermore, the charge difference maps (DOS) of the structures involved in this work are detailed in Fig. 4f–h. The adsorbed Na atom loses electrons, facilitating charge transfer. Meanwhile, electrons accumulate on the surfaces of CoS and TiO2, indicating that both materials can capture sodium ions, thus providing a synergistic effect on sodium ion storage performance. When compared to single CoS or TiO2, the CoS/TiO2 composite structure demonstrate a greater propensity for enhancing both Na adsorption and diffusion.
To further elucidate the factors contributing to the exceptional electrochemical performance, the morphological evolution of the CoS/TiO2-SC electrode was analyzed using TEM. After 50 cycles, the surface of CoS displayed a porous-like structure (Fig. 5a). With extended cycling, this porous structure became even more pronounced after 100 cycles (Fig. 5b), ultimately resulting in the establishment of a stable porous structure. Notably, this porous nanostructure maintained its interconnected integrity without significant cracks, and the outer TiO2 shell remained intact. The morphological evolution of CoS is schematically illustrated in Fig. 5e. The porous structure observed in the active materials is primarily the outcome of the strong chemical adsorption of DME molecule on the surface of CoS. This interaction induces the movement of CoS surfaces atoms and aids in the formation of a porous structure during cycling, effectively reducing interfacial strain energy.49 This porous structure is advantageous for facilitating electrolyte penetration into the active materials and relieving stress during the charge/discharge process. Consequently, this structure feature significantly contributes to the exceptional rate capability and long-term cycling stability of the electrode. In the high-resolution TEM image of the CoS electrode after 100 cycles, presented in Fig. 5(c1), the observed lattice fringes corresponded to the (101) planes of CoS. Furthermore, selected area electron diffraction (SAED) patterns (Fig. 5d) confirmed the presence of CoS. These results indicate that the crystal structure of CoS remains unchanged during the solid–liquid conversion behavior between solid-state CoS and soluble sodium polysulfide. The surface of the CoS/TiO2-SC electrode was also analyzed for the formation of the SEI film. As a comparison, an electrolyte based on EC/DEC was used. As shown in Fig. 4f, in the DEGDME-based electrolyte, the SEI film appeared uniform and thinner than that in the EC/DEC-based electrolyte (Fig. S10†). Such a uniform and thin SEI film can promote cycling stability. The composition of the SEI film was further analyzed using ex situ XPS. In the DEGDME electrolyte, the main components of the SEI film were sodium alkoxides (RCH2ONa) and polyethers, as indicated by the C 1s and O 1s spectra (Fig. 5g–h). In contrast, the SEI in the EC/DEC-based electrolyte mainly consisted of sodium alkylcarbonates (ROCO2Na) and polyester. ROCO2Na is known to be unstable and further decomposes into RCH2ONa and Na2CO3, leading to an unstable SEI in EC/DEC electrolyte.50 The F 1s high-resolution spectra (Fig. 5i) revealed two distinct peaks corresponding to organic C–F and inorganic NaF components. Notably, the proportion of these two components in the SEI layer was significantly higher (48%) in the DEGDME-based electrolyte. These fluorinated species contribute to the formation of a dense and robust SEI layer on the surface of the active electrode, protecting it from electrolyte corrosion and contributing to the superior electrochemical performance of the CoS/TiO2-SC electrode in DEGDME electrolyte.50 Furthermore, DFT calculations were employed to gain fundamental insights into the effect of the two different electrolytes on the electrode. Specifically, solvation energy (Es) and desolvation energy (Edes,x) calculations were conducted for various [Na–solventx]+ complexes. The corresponding Es values for [Na–DEGDME]+, [Na–DEGDME2]+, [Na–EC]+, [Na–EC2]+, [Na–DEC]+, [Na–DEC2]+, and [Na–EC/DEC]+ complexes were calculated and compared, as shown in Fig. 5j. Relative to the DEGDME-based electrolyte, the EC/DEC-based electrolytes exhibited weaker solvation energy, making the carbonate solvation sheath more prone to accepting electrons and decomposing. In contrast, DEGDME exhibited a higher Es value of −1.38 eV, indicating strong solvation with Na+ ions. This solvation isolates PF6− anions and enables them to preferentially decompose, forming a fluorine-rich inorganic SEI inner layer. Additionally, the desolvation behavior at the interface between the electrodes and electrolyte can significantly impact the electrochemical reaction. The calculated desolvation energy, as shown in Fig. 5k, revealed that the [Na–DEGDME]+ complexes exhibit the highest desolvation energy among the [Na–solventx]+ complexes. This suggests that [Na–DEGDME]+ complexes are more likely to combine with the electrode, thereby promoting rate capability and cycling stability.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: https://doi.org/10.1039/d4sc02587c |
This journal is © The Royal Society of Chemistry 2024 |