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Article

Spinel-Structured, Multi-Component Transition Metal Oxide (Ni,Co,Mn)Fe2O4−x as Long-Life Lithium-Ion Battery Anode Material

by
Lishan Dong
1,2,†,
Zigang Wang
1,†,
Yongyan Li
1,*,
Chao Jin
1,
Fangbing Dong
1,
Weimin Zhao
1,*,
Chunling Qin
1 and
Zhifeng Wang
1,2,*
1
School of Materials Science and Engineering, Hebei University of Technology, Tianjin 300401, China
2
Key Laboratory for New Type of Functional Materials in Hebei Province, Hebei University of Technology, Tianjin 300401, China
*
Authors to whom correspondence should be addressed.
†
These authors contributed equally to this work.
Batteries 2023, 9(1), 54; https://doi.org/10.3390/batteries9010054
Submission received: 15 December 2022 / Revised: 7 January 2023 / Accepted: 10 January 2023 / Published: 12 January 2023
(This article belongs to the Special Issue Li-Ion Battery Materials: Latest Advances and Prospects)
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Versions Notes

Abstract

:
Metal oxide anode materials are affected by severe volume expansion and cracking in the charging/discharging process, resulting in low capacity and poor cycle stability, which limits their application in lithium-ion batteries (LIBs). Herein, a new strategy is uncovered for a preparing spinel-structured, multi-component transition metal oxide, (Ni,Co,Mn)Fe2O4−x, with oxygen vacancies as an LIB anode material. The as-fabricated material presented excellent reversible capacity and cycling stability, delivering a discharge capacity of 1240.2 mAh g−1 at 100 mA g−1 for 200 cycles and then at 300 mA g−1 for 300 additional cycles. It presented extremely long cycle stability even at 2 A g−1, revealing 650.5 mAh g−1 after 1200 cycles. The good lithium storage capacity can be ascribed to the entropy stabilization effect, the multi-cation synergistic effect, abundant oxygen vacancies and the spinel structure. This study provides a new opportunity to fabricate and optimize conversion-type anodes for LIBs with satisfactory electrochemical performance.

1. Introduction

A great challenge for advanced batteries is the successive exploration of electrode materials with excellent energy density and stable performance to meet the ever-increasing demands in the field of smart grids and electric vehicles [1,2,3]. The ideal electrode should meet the demands of high Li storage capacity, low lithiation/delithiation potential and high ionic conductivity [4]. Transition metal oxides (TMOs) have been regarded as potential anode materials because of their high energy density, suitable potential and abundant resources since they were proposed in 2000 [5]. The mechanism for Li storage is associated with a conversion reaction that follows the equation of MOx + 2xLi ↔ M+ xLi2O, where M refers to transition metals such as Co, Fe, Ni and Cu [6]. Accompanied by the conversion reactions that occur, the structure and morphology of active electrode particles completely change during the regeneration of the initial particles when charging a perfect conversion-type electrode [4,7,8]. Unfortunately, the voltage hysteresis caused by reaction limitations usually leads to lower energy efficiency and poor capacity. Moreover, TMOs can catalyze the decomposition of electrolytes to some extent and thus deteriorate the cycle life of batteries. The severe volume changes during the charging/discharging process usually induce the cracking and pulverization of active particles and further damage the performance [9,10,11,12,13].
To solve the problem of pulverization and improve cycling stability, it was reported that the introduction of additional atoms on the basis of a single transition metal oxide can be an effective approach [14,15,16]. The lithium storage performance of bimetallic oxides such as AFe2O4 (A = Zn, Ni, Co, Cu, Cd) [15] and MCo2O4 (M = Mn, Zn, Fe, Ni, Co) [14,17,18] and high-entry oxides (HEOs) such as (FeCoNiCrMn)3O4 [19,20,21,22] and (CrMnFeNiCu)3O4 [23,24] were reported, which confirmed that multi-component oxides can effectively inhibit the phenomenon of pulverization through stepwise lithium storage. Furthermore, the introduction of rationally designed nanostructures could also provide an efficient diffusion pathway for Li+, thereby enhancing the reaction kinetics [25,26,27,28]. Therefore, it is necessary to make further efforts and adopt reasonable design strategies to develop TMO anode materials with good cycle stability and high specific capacity that are suitable for practical applications.
Inspired by the aforementioned progress, we open up a new opportunity for the fabrication of a multi-component TMO as anode for LIBs. A spinel-structured, AB2O4-type, multi-component transition metal oxide, (Ni,Co,Mn)Fe2O4, with oxygen vacancies was obtained by dealloying (Ni0.2Co0.2Mn0.2Fe0.4)5Al95, where Ni, Co and Mn occupy the A sites and Fe occupies the B sites. The synergism of multiple metal cations resulted in a stable cycle life, which could be cycled for more than 1200 times at 2 A g−1 with no dramatic performance fading. Meanwhile, a large number of oxygen vacancies were found to promote the adsorption toward the Li atom and boost the electrochemical reactivity according to density functional theory (DFT) calculations. Moreover, combined with SEM observations, the active material showed a stable structural retention capacity during the (de)lithiation process because of the entropy stabilization effect. The current study discloses a route for the fabrication of spinel-structured, multi-component transition metal oxides, which can have positive effects on the composition design and development of novel anode materials for LIB applications.

2. Materials and Methods

The materials were prepared using the previously reported melt-spinning and dealloying method [29,30,31,32]. Firstly, an electric-arc-melted NiCoMnFe2 high-entropy alloy ingot and an Al ingot were remelted to form a Ni2Co2Mn2Fe4Al90 master alloy ingot. After that, Ni2Co2Mn2Fe4Al90 ribbons (3 mm wide, 20 μm thick and several centimeters long) were produced using the melt-spinning technique. Then, 2 g of as-obtained ribbons was etched in 1 M NaOH solutions (500 mL) at 25 °C for 12 h and cleaned thrice with ultrapure water. Finally, the product was placed in an oven and dried for 12 h at 70 °C for follow-up tests. In the etching process, Al atoms were corroded away from the precursor, while the residual Ni, Co, Mn and Fe atoms were self-assembled and oxidized to multi-element transition metal oxide (Ni,Co,Mn)Fe2O4−x nanoplates. A schematic of the material fabrication process is displayed in Figure 1. Two contrast materials of pure Fe3O4 and Fe3O4/Mn3O4 composite were also synthesized by etching Fe10Al90 and Fe5Mn5Al90 ribbons, respectively, through the same process. Material characterization, electrochemical measurements and DFT calculation processes are introduced in detail in Supporting S1.

3. Results and Discussion

The SEM images of the three dealloyed products are presented in Figure S1a–c. All the samples displayed nanoplate morphology. With the increase in the element types of the precursors, the size of the nanoplates decreased gradually. Figure S1d–g compare the length and thickness of the nanoplates in the three samples. The length of the nanoplates was reduced from several microns (dealloyed Fe10Al90) to less than 1 micron (dealloyed Ni2Co2Mn2Fe4Al90), while the thickness of the nanoplates was reduced from hundreds of nanometers (dealloyed Fe10Al90) to tens of nanometers (dealloyed Ni2Co2Mn2Fe4Al90). Figure 2 characterizes dealloyed Ni2Co2Mn2Fe4Al90 in more detail. Figure 2a,b reveal the special morphology of these nanoplates, showing that some small nanoplates (tens of nanometers in diameter) grew on the tip of the main nanoplates (~1 μm in diameter). The corresponding SAED patterns (Figure 2c) consisted of diffraction spots, corresponding to the (311), (13−1) and (440) planes of spinel structure oxides such as NiFe2O4 with a zone axis of [−112] [33]. The HRTEM image in Figure 2d shows that the interplanar distance was around 0.254 nm, relating to the (311) planes of the spinel structure oxide. In addition, there were a large number of defects formed by the vacancy of oxygen on material surfaces [34]. EPR tests (Figure S2) further uncovered the existence of oxygen vacancies [35], which can provide abundant active sites for electrochemical reactions in batteries. Figure 2e–j and Figure S3a show EDS elemental mappings of the as-prepared material, demonstrating a uniform distribution of O, Ni, Co, Mn and Fe elements. The atomic ratio of O:Fe:Co:Ni:Mn was approximately 56.18:29.51:4.84:5.01:4.46, as detected using EDS (Figure S3b). All the above results confirm that the dealloyed product was (Ni,Co,Mn)Fe2O4 with abundant oxygen vacancies, namely, (Ni,Co,Mn)Fe2O4−x, in this work.
To study the crystal structure of NiCoMnFe2, the precursors and the corresponding dealloyed products, XRD tests were performed (Figure 3a and Figure S4). In Figure 3a, the NiCoMnFe2 alloy exhibits an fcc structure with typical diffraction lattice planes of (111), (200), (220) and (311) [36]. After alloying with Al, it mainly presented Al phase, Fe phase and Al-M phases (M = Mn, Ni and Co), which was similar to the solidification phase of the Fe10Al90 and Fe5Mn5Al90 precursors (Figure S4a–c). After dealloying, however, the corresponding oxides could be obtained. Fe3O4 and Fe3O4/Mn3O4 could be identified from the dealloyed Fe10Al90 and Fe5Mn5Al90 products, respectively (Figure S4d,e), while spinel oxides with (311), (400) and (440) diffraction lattice planes [37] could be found for dealloyed Ni2Co2Mn2Fe4Al90 (Figure 3a). The diffraction peaks of this spinel oxide were near those of NiFe2O4, CoFe2O4 and MnFe2O4 and could be attributed to (Ni,Co,Mn)Fe2O4−x according to the series of the above results. With the enhancement of the components, the peak intensity declined, and the peak width widened. These diffraction peaks of as-obtained polyoxides are similar to those of some high-entropy oxides [37,38,39].
An XPS test was performed to analyze the element and valence state of dealloyed Ni2Co2Mn2Fe4Al90. The XPS survey spectrum demonstrated the co-existence of Mn, Fe, Ni, Co and O elements (Figure 3b), which was in good agreement with the EDS result (Figure 2e–j). Figure 3c displays that the Fe 2p spectra of the dealloyed product were composed of two main peaks at 724.5 eV (Fe 2p1/2) and 711.2 eV (Fe 2p3/2) [40]. The Fe 2p1/2 peak was superimposed by two doublets (724.4 eV and 727.1 eV), while Fe 2p3/2 was composed by two doublets at 710.6 eV and 713.4 eV. The green peaks at 710.6 eV and 724.4 eV corresponded to Fe2+; meanwhile, the blue peaks at 713.4 eV and 727.1 eV were related to Fe3+ [41,42,43]. The orange peaks represented satellite peaks of the corresponding main peaks. Similar doublets could also be found in the core-level spectra of Co 2p, Ni 2p and Mn 2p. Both the bivalent and trivalent (Ni, Co), as well as trivalent and tetravalent (Mn), states of these elements could be discovered [44,45,46]. The O 1s core-level spectrum (Figure 3g) was divided into three peaks [47]. The peak at 531.1 eV could be attributed to OH−, which probably originated from the residual etchant (NaOH). The peak located at 529.7 eV was due to the OM oxygen (M refers to metals), relating to the O2- in the metal oxide. The other peak at 533.2 eV related to O in H2O.
Figure 4 presents the N2 adsorption–desorption isotherm and the matching pore-size distribution of the (Ni,Co,Mn)Fe2O4−x sample. A type III curve with an H3-type hysteresis loop is revealed in Figure 4a [29], demonstrating the existence of plentiful mesopores on the nanoplates (Figure 2e). The specific surface area of the material was about 112.69 m2 g−1, which was higher than those of spinel CoFe2O4 and NiFe2O4 oxide nanosheets (40~90 m2 g−1) obtained with traditional dealloying [47,48]. The pore size mainly ranged from 1.5 to 10 nm (Figure 4b). These micropores and mesopores increased the contact areas between the electrolyte and the active materials [49].
To reveal the electrochemical performance of the three dealloying products ((Ni,Co,Mn)Fe2O4−x, Fe3O4/Mn3O4 and Fe3O4), a series of tests were carried out (Figure 5). Cyclic voltammetry (CV) curves of the battery assembled with a (Ni,Co,Mn)Fe2O4−x anode were measured, as shown in Figure 5a, at 0.1 mV/s within 0.01–3.0 V. The CV curves of the three products (Figure 5a and Figure S5) are similar in shape (with a certain extent of position offset) but differ in peak intensities. It can be seen that the CV curves of Fe3O4 and Fe3O4/Mn3O4 show relatively sharp redox peaks, while that of (Ni,Co,Mn)Fe2O4−x presents broad redox peaks, indicating that its reaction was not completed in a short time and in a rapid way but was carried out slowly in successive substeps. This electrochemical reaction characteristic displays a vital function in alleviating the huge volume variation during the cycle and inhibiting the cracking and pulverization of the active materials. In the initial cycle, two cathodic peaks at 1.2 V and 0.6 V can be found (Figure 5a), which corresponded to the reduction of metallic oxides to corresponding metal states and the creation of Li2O [50]. In the following cycles, the reduction peaks shift to 1.5 V and 0.8 V. This position offset was the result of the formation of an SEI layer and the surface structural rearrangement of active materials in the lithiation process. The redox peaks nearly remain changeless after three cycles, reflecting the excellent cycling stability and reversibility of the (Ni,Co,Mn)Fe2O4−x anode. The Mn3O4/Fe3O4 electrode and the Fe3O4 electrode show a CV tendency similar to that of the (Ni,Co,Mn)Fe2O4−x anode in the first two cycles but much sharper recession in the closed area after three cycles (Figure S5), revealing their bad cycling stability. In the charging process, the Fe3O4 electrode shows clear and sharp peaks at 1.1 V, 1.5 V and 1.8 V, relating to two-step oxidation from Fe0 to LixFe3O4 and from LixFe3O4 to Fe3+, respectively (Figure S5a). For the (Ni,Co,Mn)Fe2O4−x electrode, however, two broad anodic peaks around 1.5 V and 2.1 V can be seen, corresponding to the intertwined multistep oxidation of multiple metals, Fe, Co, Mn and Ni, to their oxides. The CV curves of the (Ni,Co,Mn)Fe2O4−x electrode present better repeatability than those of the Mn3O4/Fe3O4 electrode and the Fe3O4 electrode, implying its good cycling stability and reversibility.
Figure S6a shows the representative galvanostatic profiles of the (Ni,Co,Mn)Fe2O4−x anode at 100 mA g−1 for different cycles. There are two discharge platforms at 1.4–1.7 V and 0.6–0.9 V, respectively, in the discharging process, while two charging platforms, 1.4–1.7 V and 2.0–2.5 V, can be found in the charging process. The above platform potential ranges correspond well with the peak voltage in the CV curve. The first charging/discharge capacity was about 978.5/1223.1 mAh g−1 with a first Coulombic efficiency of 80%. This serious capacity loss was probably induced by the generation of irreversible SEI films [51,52]. As the number of cycles increases (1–50 cycles), the charge/discharge curve gradually moves to the left, indicating that the battery capacity gradually decreased. On the other hand, as the number of cycles further increases, the battery capacity increased slowly. It can be seen that the reversible capacity at the 200th cycle was even higher than that at the first cycle. In the following cycles, the battery was tested at 300 mA g−1 (Figure S6b). The curves at the 201st, 300th, 400th and 500th cycles are close to each other, revealing that the (Ni,Co,Mn)Fe2O4−x electrode possessed good electrochemical stability in later cycling.
Figure 5b shows the cycling performance of the three materials at 100 mA g−1 for 200 cycles and then at 300 mA g−1 for 300 cycles. During the first 66 cycles, the reversible capacity of (Ni,Co,Mn)Fe2O4−x slowly reduced to about 630 mAh g−1 and then gradually increased to 1369.9 mAh g−1 (at the 200th cycle). This phenomenon is known as the U-shape increase [53,54], which is usually found in transition metal oxide materials. The decrease in the initial tens of cycles was due to the consumption of SEI film, the rearrangement of the atomic structure on the material surface and electrode activation, while the increase in the later period may have been related to the consumption of electrolyte. At the same time, the Fe3O4/Mn3O4 and Fe3O4 electrodes presented higher first discharge capacity than (Ni,Co,Mn)Fe2O4−x, while their capacities dropped dramatically. The reversible capacities reached their lowest points after cycling for about 35 cycles. Although the capacities of both cells (Fe3O4/Mn3O4 and Fe3O4) gradually increased during subsequent cycles, the increase rate was relatively slower than that of (Ni,Co,Mn)Fe2O4−x. At the 200th cycle, the reversible capacities reached 1275.8 (Fe3O4/Mn3O4) and 1051.3 (Fe3O4), which were lower than the 1389.9 of (Ni,Co,Mn)Fe2O4−x. During the following 300 cycles at 300 mA g−1, the (Ni,Co,Mn)Fe2O4−x electrode showed good cycling stability. It maintained a discharge capacity of 1240.2 mAh g−1 after the latest 300 cycles, while those of the other anodes dropped dramatically, delivering the reversible capacities of 500.7 (Fe3O4/Mn3O4) and 321.6 (Fe3O4) mAh g−1, respectively. The above results demonstrate that the (Ni,Co,Mn)Fe2O4−x electrode presented the best electrochemical property among the three anodes in long cycling.
Figure 5c shows the cyclic performance of the three electrodes cycling at a high current density of 2 A g−1 for 1200 cycles. During cycling, the capacities of Fe3O4/Mn3O4 and Fe3O4 electrodes decreased sharply and resulted to be around 230 mAh g−1 after 1200 cycles, while the U-shape increase could also be found for the (Ni,Co,Mn)Fe2O4−x electrode. It delivered 650.5 mAh g−1 after 1200 cycles. Figure 5d shows the rate performance of the three electrodes at increased current densities from 50 to 1500 mA g−1. Although the (Ni,Co,Mn)Fe2O4−x electrode displayed relatively low reversible capacity when cycling at 50 mA g−1 (low current density), among the three electrodes, it presented the best reversible capacity when cycling at higher current densities (500~1500 mA g−1). It delivered discharge capacities of 1003, 891, 747, 661 and 508 mAh g−1 at 50, 100, 500, 1000 and 1500 mA g−1, respectively. The reversible capacity of the (Ni,Co,Mn)Fe2O4−x electrode could be recovered as 809 mAh g−1 when cycling at 100 mA g−1 again, indicating acceptable reversibility. The voltage profiles of the three electrodes at the current density of 1500 mA g−1 are presented in Figure S6c, uncovering an obvious advantage in the charge/discharge capacity of (Ni,Co,Mn)Fe2O4−x compared with those of Fe3O4/Mn3O4 and Fe3O4. Figure 5e shows the EIS diagram of the three electrodes before and after cycling. The EIS curves show semicircles in the high-frequency area and oblique lines in the low-frequency region, relating to charge transfer resistance and ion diffusion resistance, respectively. Though the EIS diagram of the three fresh electrodes shows similar curve shapes and overlap among them to a certain extent, the (Ni,Co,Mn)Fe2O4−x electrode showed the lowest resistance after cycling for 500 cycles, which can explain the good cycle stability of the battery in the long cycling process. Table S2 presents the Li-ion diffusion coefficients calculated using EIS; it can be seen that (NiCoMn)Fe2O4−x showed a higher diffusion coefficient after cycling than the fresh one, revealing good reaction kinetics of (NiCoMn)Fe2O4−x. On the other hand, the diffusion coefficients of the contrast materials were decreased, demonstrating their poor reaction kinetics.
In order to reveal the structural stability of the electrode materials during the cycling process, the SEM images of the (Ni,Co,Mn)Fe2O4−x, Fe3O4/Mn3O4 and pure Fe3O4 electrodes before and after cycling were characterized (Figure 6a–f). Figure 6a and b show that (Ni,Co,Mn)Fe2O4−x retained its initial nanoplate shape without any crack or pulverization phenomenon, though it expanded its size slightly (from 0.5~1 μm to 2~3 μm) after cycling. Different from the phenomenon of (Ni,Co,Mn)Fe2O4−x, the contrast Fe3O4/Mn3O4 (Figure 6c,d) and pure Fe3O4 (Figure 6e,f) electrodes expanded and cracked significantly after cycling from 1~2 μm to 20~30 μm and from 3~4 μm to 50~80 μm, respectively. Figure 6g uncovers a schematic diagram of the structural changes in the three electrodes before and after cycling. It can be found that mono-metal oxide Fe3O4 develops drastic expansion and severe cracking after cycling. The expansion and cracking degree of Fe3O4/Mn3O4 are alleviated with the increase in oxide components. However, the expansion and cracking of (Ni,Co,Mn)Fe2O4−x are significantly inhibited when more elements are added. This phenomenon is related to the composition of the material, but also to the initial size of the material. Moreover, slight expansion and no crack correspond to relatively good cyclic stability, while severe expansion and cracking of the active material lead to the drastic deterioration of the electrochemical properties. The changes in these electrode materials are consistent with the current electrochemical properties.
The effects of oxygen vacancies on the Li-ion adsorption ability and electronic structure of (Ni,Co,Mn)Fe2O4−x were analyzed using DFT calculations. The atomic structural models of (Ni,Co,Mn)Fe2O4 and (Ni,Co,Mn)Fe2O4−x were constructed and are displayed in Figure 7a,b, respectively. The adsorption energy of oxygen vacancy-rich (Ni,Co,Mn)Fe2O4−x was −2.09 eV, which was lower than that of pristine (Ni,Co,Mn)Fe2O4 (−1.89 eV; Figure 7c), supporting that the introduction of oxygen vacancies can promote the adsorption and diffusion toward lithium as well as provide more active sites at the same time. Figure 7d and e show the projected density of state (PDOS) of pristine (Ni,Co,Mn)Fe2O4 and oxygen vacancy-rich (Ni,Co,Mn)Fe2O4−x. Neither of them have a bandgap, suggesting their band-conducting feature. Meanwhile, in the PDOSs of (Ni,Co,Mn)Fe2O4 and (Ni,Co,Mn)Fe2O4−x, the energy 0 point was chosen as the Fermi energy level. Around the Fermi levels, the PDOS of (Ni,Co,Mn)Fe2O4−x appears more dense than that of (Ni,Co,Mn)Fe2O4, which confirms that oxygen vacancies can modulate the electronic structure and may further promote Li+ storage [34]. According to the above analysis, it was revealed that the oxygen defects on the (NiCoMn)Fe2O4 surface can provide outstanding Li capture capacity, leading to excellent electrochemical properties and lifetime.
Table S1 shows a comparison of the electrochemical properties of as-obtained (Ni,Co,Mn)Fe2O4−x and previously reported materials. It can be found from the table that the lithium storage performance of the (Ni,Co,Mn)Fe2O4−x material is higher than that of many reported spinel-structured oxides and multi-component metal oxides. It seems that high-entropy oxides with five cations present lower electrochemical properties than (Ni,Co,Mn)Fe2O4−x. In fact, regardless of high-entropy oxides with five cations or the material designed in this paper, electrochemical properties are determined by the composition and crystal structure of materials, as well as the size, specific surface area, three-dimensional structure and other factors. To develop high-performance anode materials, the above aspects need to be carefully designed and balanced. Good Li storage properties could be ascribed to three aspects. Firstly, the lithiation/delithiation process of multi-component transition metal oxides is carried out stepwise (wide CV peak), which is related to the entropy stabilization effect and the multi-cation synergistic effect [19,20,21,22,38]. This greatly inhibits the expansion and cracking of active materials (Figure 6) caused by short time and drastic volume changes in monometallic oxides and improves the electrochemical stability of materials in long cycling. Secondly, a large number of oxygen vacancies provide abundant active sites, improve the adsorption capacity of oxides towards lithium, improve the electronic structure of the material and thus enhance the cyclic stability and rate performance of the material. Thirdly, spinel oxides possess the advantages of narrow band gap and higher electroconductibility than traditional oxides, which are beneficial to improving the rate performance of materials. This paper provides a strategy for the preparation of spinel-structured, multi-component transition metal oxides with abundant oxygen vacancies, which can have positive effects on the composition design and development of related materials and the improvement of the properties of novel anode materials for LIB applications.

4. Conclusions

In summary, a spinel-type, multi-component transition metal oxide, (Ni,Co,Mn)Fe2O4−x, with oxygen vacancies was designed and prepared using a melt-spinning and dealloying strategy. When utilized as anode material for LIBs, the (Ni,Co,Mn)Fe2O4−x material presented good electrochemical properties, delivering a reversible capacity of 1240.2 mAh g−1 at 100 mA g−1 for 200 cycles and then at 300 mA g−1 for 300 cycles. It also presented extremely long cycle stability, revealing a reversible capacity of 650.5 mAh g−1 at 2 A g−1 for 1200 cycles. Our DFT calculations revealed the pivotal role of oxygen defects in the ion transport process and in adjusting the electronic structure, leading to improved Li capture ability. Moreover, the electrode material uncovered a spectacular structural reservation capacity after cycling because of the entropy stabilization effect and the multi-cation synergistic effect, which is a vital stimulus for satisfactory cycle stability. This work presents positive results for the composition design and development of novel, spinel-structured, multi-component transition metal oxides with abundant oxygen vacancies. The as-fabricated materials are aimed to be applied as alternative LIB anode materials.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/batteries9010054/s1, S1: Experiments and Computation, Figure S1: SEM images and size statistics of products, Figure S2: EPR analysis and crystal structure model, Figure S3: EDS analysis, Figure S4: XRD of precursors and corresponding dealloyed products, Figure S5: CV curves of Fe3O4 and Fe3O4/Mn3O4, Figure S6: Charge/discharge profiles of experimental materials, Table S1: Comparison of lithium storage properties, Table S2: List of Li-ion diffusion coefficients of experimental materials [34,38,42,43,44,45,55].

Author Contributions

Conceptualization, Y.L., C.Q. and Z.W. (Zhifeng Wang); methodology, Y.L., W.Z. and Z.W. (Zhifeng Wang); investigation, L.D., Z.W. (Zigang Wang), C.J. and F.D.; data curation, L.D., C.J. and F.D.; writing—original draft preparation, L.D. and Z.W. (Zigang Wang); writing—review and editing, Y.L., W.Z. and Z.W. (Zhifeng Wang); visualization, Z.W. (Zigang Wang) and C.Q.; supervision, Y.L., W.Z. and C.Q.; project administration, Z.W. (Zhifeng Wang); funding acquisition, Y.L. and Z.W. (Zhifeng Wang). All authors have read and agreed to the published version of the manuscript.

Funding

The authors would like to acknowledge the financial support from Natural Science Foundation of Hebei Province, China (E2020202071), Hebei Higher Education Teaching Reform Reasearch and Practice Project, China (2021GJJG050), and Science and Technology Project of Hebei Education Department, China (ZD2020177).

Informed Consent Statement

Not applicable.

Data Availability Statement

The data presented in this study are available upon request from the corresponding author.

Acknowledgments

The numerical calculations in this paper were performed using TianHe-2 at LvLiang Cloud Computing Center of China. C.J. and F.D. acknowledge the support from Innovative Top-Notch Student Training Program and Innovation and Entrepreneurship Training Program (202210080001) of Hebei University of Technology.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Schematic revealing the preparation process of (Ni,Co,Mn)Fe2O4−x.
Figure 1. Schematic revealing the preparation process of (Ni,Co,Mn)Fe2O4−x.
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Figure 2. (a) SEM image, (b) TEM image, (c) SAED patterns, (d) HRTEM image and (e–j) EDS elemental mappings of as-prepared (Ni,Co,Mn)Fe2O4−x material.
Figure 2. (a) SEM image, (b) TEM image, (c) SAED patterns, (d) HRTEM image and (e–j) EDS elemental mappings of as-prepared (Ni,Co,Mn)Fe2O4−x material.
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Figure 3. (a) XRD patterns of pristine NiCoMnFe2 and dealloyed (Ni,Co,Mn)Fe2O4−x oxides. (b–g) XPS spectra of (Ni,Co,Mn)Fe2O4−x: (b) XPS survey spectra; (c–g) high-resolution core-level spectra of Fe 2p, Mn 2p, Ni 2p, Co 2p and O 1s, respectively.
Figure 3. (a) XRD patterns of pristine NiCoMnFe2 and dealloyed (Ni,Co,Mn)Fe2O4−x oxides. (b–g) XPS spectra of (Ni,Co,Mn)Fe2O4−x: (b) XPS survey spectra; (c–g) high-resolution core-level spectra of Fe 2p, Mn 2p, Ni 2p, Co 2p and O 1s, respectively.
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Figure 4. N2 adsorption–desorption isotherm of (Ni,Co,Mn)Fe2O4−x (a) and corresponding pore-size distribution (b).
Figure 4. N2 adsorption–desorption isotherm of (Ni,Co,Mn)Fe2O4−x (a) and corresponding pore-size distribution (b).
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Figure 5. Electrochemical performance of the as-prepared (Ni,Co,Mn)Fe2O4−x. (a) Cyclic voltammetry tested at 0.01–3 V at a scan rate of 0.1 mV/s. (b,c) Long cycle performance at different current densities: (b) 100 mA g−1 for 200 cycles and 300 mAg−1 for the following 300 cycles and (c) 2 Ag−1 for 1200 cycles. (d) Rate performance at varied current densities ranging 100–1500 mA g−1. (e) Nyquist plots of fresh cells (inset) and cells after cycling.
Figure 5. Electrochemical performance of the as-prepared (Ni,Co,Mn)Fe2O4−x. (a) Cyclic voltammetry tested at 0.01–3 V at a scan rate of 0.1 mV/s. (b,c) Long cycle performance at different current densities: (b) 100 mA g−1 for 200 cycles and 300 mAg−1 for the following 300 cycles and (c) 2 Ag−1 for 1200 cycles. (d) Rate performance at varied current densities ranging 100–1500 mA g−1. (e) Nyquist plots of fresh cells (inset) and cells after cycling.
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Figure 6. SEM images of (a,b) (Ni,Co,Mn)Fe2O4, (c,d) Fe3O4/Mn3O4 and (e,f) Fe3O4 electrodes before (a,c,e) and after (b,d,f) cycling at 100 mA g−1 for 200 cycles. (g) Schematic diagram of the structural changes in the corresponding electrodes before and after cycling.
Figure 6. SEM images of (a,b) (Ni,Co,Mn)Fe2O4, (c,d) Fe3O4/Mn3O4 and (e,f) Fe3O4 electrodes before (a,c,e) and after (b,d,f) cycling at 100 mA g−1 for 200 cycles. (g) Schematic diagram of the structural changes in the corresponding electrodes before and after cycling.
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Figure 7. Crystal structures of (a) (Ni,Co,Mn)Fe2O4 and (b) (Ni,Co,Mn)Fe2O4−x. (c) Calculated adsorption energy of Li on the surface of (Ni,Co,Mn)Fe2O4 and (Ni,Co,Mn)Fe2O4−x (insert: optimized Li adsorption configuration). Density of states of (d) (Ni,Co,Mn)Fe2O4 and (e) (Ni,Co,Mn)Fe2O4−x.
Figure 7. Crystal structures of (a) (Ni,Co,Mn)Fe2O4 and (b) (Ni,Co,Mn)Fe2O4−x. (c) Calculated adsorption energy of Li on the surface of (Ni,Co,Mn)Fe2O4 and (Ni,Co,Mn)Fe2O4−x (insert: optimized Li adsorption configuration). Density of states of (d) (Ni,Co,Mn)Fe2O4 and (e) (Ni,Co,Mn)Fe2O4−x.
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MDPI and ACS Style

Dong, L.; Wang, Z.; Li, Y.; Jin, C.; Dong, F.; Zhao, W.; Qin, C.; Wang, Z. Spinel-Structured, Multi-Component Transition Metal Oxide (Ni,Co,Mn)Fe2O4−x as Long-Life Lithium-Ion Battery Anode Material. Batteries 2023, 9, 54. https://doi.org/10.3390/batteries9010054

AMA Style

Dong L, Wang Z, Li Y, Jin C, Dong F, Zhao W, Qin C, Wang Z. Spinel-Structured, Multi-Component Transition Metal Oxide (Ni,Co,Mn)Fe2O4−x as Long-Life Lithium-Ion Battery Anode Material. Batteries. 2023; 9(1):54. https://doi.org/10.3390/batteries9010054

Chicago/Turabian Style

Dong, Lishan, Zigang Wang, Yongyan Li, Chao Jin, Fangbing Dong, Weimin Zhao, Chunling Qin, and Zhifeng Wang. 2023. "Spinel-Structured, Multi-Component Transition Metal Oxide (Ni,Co,Mn)Fe2O4−x as Long-Life Lithium-Ion Battery Anode Material" Batteries 9, no. 1: 54. https://doi.org/10.3390/batteries9010054

APA Style

Dong, L., Wang, Z., Li, Y., Jin, C., Dong, F., Zhao, W., Qin, C., & Wang, Z. (2023). Spinel-Structured, Multi-Component Transition Metal Oxide (Ni,Co,Mn)Fe2O4−x as Long-Life Lithium-Ion Battery Anode Material. Batteries, 9(1), 54. https://doi.org/10.3390/batteries9010054

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