Xiaohong Wu’s research while affiliated with Xiamen University of Technology and other places

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Publications (47)


(a) Ex/in situ ATR‐FTIR spectroscopy reveals the essence of concentration changes in both the bulk and interface. a) Ex situ ATR‐FTIR spectra of EC/EMC electrolytes with different concentrations. The upper part displays the original infrared absorption spectra, while the lower part shows the subtracted spectrum of the three electrolytes, and the 1.0 M as the background to be deducted. b) Schematic diagram of the ATR‐FTIR spectroscopy. c) (I) In situ ATR‐FTIR spectra of the LFP/electrolyte interface collected during the first cycle with the colors of the spectra varying from red in charge to blue in discharge. The in situ cell was cycled at a current density of 25 mA g⁻¹, with infrared spectra collected every 5 minutes. To highlight the detailed changes in the spectra, one spectrum was selected out of every four for plotting. There are no obvious changes in the original spectra because the main signals originate from the thin‐layer bulk. (II) The A(n)‐A(OCV) relative absorbance evolution during charging and discharging, and the spectrum collected at OCV as background to be deducted. (III) The A(n+1)‐A(n) relative absorbance evolution during charging, in which each spectrum has subtracted its corresponding preceding spectrum. d) Schematic illustration of the electrolyte solvation configuration at the LFP‐electrolyte interface during Li⁺‐(de)solvation (i. e., charging/discharging) process. The interface transitions from a solvent‐rich state to a Li⁺‐solvent/anion‐rich state during charging, while the reverse applies in the discharging process.
In situ ATR‐FTIR spectroscopy reveals the inflection point of interfacial Li⁺‐solvent/anion concentration caused by the anti‐synergy effect. a) A snapshot of the LiCoO2‐electrolyte interface in the simulation system. b). The potential of mean force (PMF) of interfacial solvated‐Li⁺ as a function of distance from the electrode under different voltages. c) In situ ATR‐FTIR spectra of the LCO/electrolyte interface collected during initial charging. The current density is 25 mA g⁻¹. The spectrum collected at inflection voltage is colored in red. d) Schematic illustration of the electrolyte solvation configuration at the LCO/electrolyte interface during the Li⁺‐solvation (charging) process at different voltages.
CEI architecture analysis from the influence of inflection point and protocol optimization method. (a) TOF‐SIMS characterization of the 4.1 V and 4.2 V‐cycled LCO cathodes (below/above the inflection voltage) retrieved from the coin cells after 5 cycles. Normalized depth profiles of representative inorganic and organic fragments illustrate the CEI architecture. (b) Schematic illustration of CEI structure formed at charge cut‐off voltages below/above inflection voltage. (c) The ToF‐SIMS chemical mapping (size: 150×150 μm²) of CHO2⁻ corresponding to different sputtering times in Figure 3a. (d) Charge curves of typical CC‐cycled and special CV‐holding mode. (f) Comparison of cycling performance of Li||LCO cells with different pre‐cycle modes.
Electrolyte engineering in regulating the CEI architecture. a) Schematic diagram illustrating the electrolyte design principle of reducing electropositivity of solvated‐Li⁺. b) ¹⁹F NMR of EC/EMC37 and EC/EMC11 electrolyte. c) The A(n+1)‐A(n) relative absorbance evolution on LCO surfaces upon charging to 4.5 V in EC/EMC37 and EC/EMC11 electrolyte. The spectrum collected at inflection voltage is colored in red. The middle part represents the corresponding voltage profile (red for EC/EMC37 and blue for EC/EMC11). d) ATR‐FTIR absorbance evolution of the O−C−O bands of EC and P−F band of CIP during the charging in the first cycle. e) Normalized depth profiles of CH2⁻ fragment of LCO surfaces upon charging to 4.5 V in EC/EMC37 and EC/EMC11 electrolyte. f) Cycling performance of LCO cathode in two electrolytes.
Revealing the Dynamic Evolution of Electrolyte Configuration on the Cathode‐Electrolyte Interface by Visualizing (De) Solvation Processes
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December 2024

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103 Reads

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2 Citations

Haiyan Luo

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Shi‐Gang Sun

Electrolyte engineering is crucial for improving cathode electrolyte interphase (CEI) to enhance the performance of lithium‐ion batteries, especially at high charging cut‐off voltages. However, typical electrolyte modification strategies always focus on the solvation structure in the bulk region, but consistently neglect the dynamic evolution of electrolyte solvation configuration at the cathode‐electrolyte interface, which directly influences the CEI construction. Herein, we reveal an anti‐synergy effect between Li⁺‐solvation and interfacial electric field by visualizing the dynamic evolution of electrolyte solvation configuration at the cathode‐electrolyte interface, which determines the concentration of interfacial solvated‐Li⁺. The Li⁺ solvation in the charging process facilitates the construction of a concentrated (Li⁺‐solvent/anion‐rich) interface and anion‐derived CEI, while the repulsive force derived from interfacial electric field induces the formation of a diluted (solvent‐rich) interface and solvent‐derived CEI. Modifying the electrochemical protocols and electrolyte formulation, we regulate the “inflection voltage” arising from the anti‐synergy effect and prolong the lifetime of the concentrated interface, which further improves the functionality of CEI architecture.

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Decoupling the Failure Mechanism of Li‐Rich Layered Oxide Cathode During High‐Temperature Storage in Pouch‐Type Full‐Cell: A Practical Concern on Anionic Redox Reaction

In addressing the global climate crisis, the energy storage performance of Li‐ion batteries (LIBs) under extreme conditions, particularly for high‐energy‐density Li‐rich layered oxide (LRLO) cathode, is of the essence. Despite numerous researches into the mechanisms and optimization of LRLO cathodes under ideal moderate environment, there is a dearth of case studies on their practical/harsh working environments (e.g., pouch‐type full‐cell, high‐temperature storage), which is a critical aspect for the safety and commercial application. In this study, using pouch‐type full‐cells as prototype investigation target, the study finds the cell assembled with LRLO cathode present severer voltage decay than typical NCM layered cathode after high‐temperature storage. Further decoupling elucidates the primary failure mechanism is the over‐activation of lattice oxidized oxygen (aggravate by high‐temperature storage) and subsequent escape of oxidized oxygen species (Oⁿ⁻), which disrupts transition metal (TM) coordination and exacerbates electrolyte decomposition, leading to severe TM dissolution, interfacial film reconstruction, and harmful shuttle effects. These chain behaviors upon high‐temperature storage significantly influence the stability of both electrodes, causing substantial voltage decay and lithium loss, which accelerates full‐cell failure. Although the anionic redox reaction can bring additional energy, but the escape of metastable Oⁿ⁻ species would introduce new concerns in practical cell working conditions.




Revealing the Dynamic Evolution of Electrolyte Configuration on the Cathode‐Electrolyte Interface by Visualizing (De)Solvation Processes

August 2024

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35 Reads

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1 Citation

Angewandte Chemie

Electrolyte engineering is crucial for improving cathode electrolyte interphase (CEI) to enhance the performance of lithium‐ion batteries, especially at high charging cut‐off voltages. However, typical electrolyte modification strategies always focus on the solvation structure in the bulk region, but consistently neglect the dynamic evolution of electrolyte solvation configuration at the cathode‐electrolyte interface, which directly influences the CEI construction. Herein, we reveal an anti‐synergy effect between Li+‐solvation and interfacial electric field by visualizing the dynamic evolution of electrolyte solvation configuration at the cathode‐electrolyte interface, which determines the concentration of interfacial solvated‐Li+. The Li+ solvation in the charging process facilitates the construction of a concentrated (Li+‐solvent/anion‐rich) interface and anion‐derived CEI, while the repulsive force derived from interfacial electric field induces the formation of a diluted (solvent‐rich) interface and solvent‐derived CEI. Modifying the electrochemical protocols and electrolyte formulation, we regulate the “inflection voltage” arising from the anti‐synergy effect and prolong the lifetime of the concentrated interface, which further improves the functionality of CEI architecture.


Full‐Dimensional Analysis of Gaseous Products Within Li‐Ion Batteries by On‐Line GC‐BID/MS

April 2024

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91 Reads

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3 Citations

The gas release within Li‐ion batteries, particularly during cycling and storage, can result in rapid performance degradation and potential safety hazards. However, this area has not garnered sufficient attention until now, primarily because the gassing information collected by typical OEMS/DEMS is quite limited and even inaccurate. Herein, for the first time, a state‐of‐the‐art on‐line GC‐BID/MS to full‐dimensionally analyze the gassing behavior within both lab‐scale coin‐type cell (in situ mode) and industry‐scale pouch‐type cell (operando mode) is originally designed/constructed. Not limited to common permanent gases (e.g. H2, CO, etc.) detected by online GC‐BID, but also complicated/various (semi‐)volatile products are identified/quantified by online GC‐MS. Based on the real‐time evolution information of water, alcohols, aldehydes, ethers, esters, and hydrocarbons, the decomposition mechanisms of electrolyte on both graphite anode and/or LCO cathode sides is further supplemented/perfected. Moreover, at the level of the device, series derivative/crosstalk reactions induced by trapped/accumulated gaseous species are unveiled in practical pouch‐cell.


Capturing the variation of interfacial electrolyte configuration during (de−)solvation process via IR spectroscopy. (a) Ex situ FTIR spectra of EC: DMC (volume ratio=1 : 1) with different LiPF6 concentrations of 0 M, 1 M, and 3 M, respectively. The differential spectrum between 1 M and 3 M reveals the amount of conversion of free solvents and coordinated solvents when changing salt concentration, demonstrating a bipolar “peak‐dip” pattern. (b) The schematic of the ATR‐IR that in situ monitoring electrolyte configuration at electrode/electrolyte interface. (c) In situ raw FTIR spectra and corresponding differential spectrum of electrolyte during potentiostatic plating and stripping processes. The bipolar “peak‐dip” pattern in differential spectra reveals the dynamic variation of interfacial electrolyte configuration. Schematic diagram of (d) the anion‐lean solvent‐rich interface and (e) the anion‐rich solvent‐lean interface involving the interfacial evolution of Li⁺‐solvent species and anions during the de‐solvation/solvation process.
Visualizing anion distribution during plating/stripping processes via in situ MRI. The schematic of (a) in situ MRI that in situ monitoring ¹⁹F to present concentration distribution of PF6⁻ anion and (b) the symmetric sealed cell for In situ MRI. (c) Original 2D‐MRI sagittal plane image. (d) In situ subtractive 2D‐MRI images (image acquisition every 30 minutes (I–IX)).
A pulse cycling protocol for regulating interfacial electrolyte configuration to modify SEI architecture. (a) The schematic of interfacial electrolyte configuration variation from typical galvanostatic and pulse protocol. For both protocols, the anion‐lean solvent‐rich interface is formed as the anodic current passes. For typical galvanostatic protocol, the anion is repelled when a cathodic current is applied. For pulse protocol, the gradient of concentration promotes anion diffusion towards the electrode in Toff. Thus, the concentration of anion in the interfacial region is restored leading to forming anion‐derived SEI. (b) Cycle performances of Li/Li symmetric cells with typical galvanostatic protocol (gray) and pulse protocol (blue) at a fixed capacity of 1 mAh cm⁻² at the current density of 3 mA cm⁻². Note: Ton=1 s; Ton: Toff=1 : 5. The rest time (Toff) has been subtracted.
Characterizations of SEIs formation in the 1 M LiPF6/EC: DMC (volume ratio=1 : 1) on the cycled Lithium foils with different protocols. (a) XPS spectra of SEIs formation with a pulse (upper) protocol and galvanostatic protocol (lower). (b) The atomic ratio of F, C, O, and P elements as a function of Ar⁺ etching depth. (c) 3D‐rendering images of LiF2⁻ (I and II) (indicating LiF component generated from anion decomposition), C2HO⁻ (III and IV), and LiCO3⁻ (V and VI) (indicating organic species especially carboxylates generated from carbonate decomposition). (d) The intuitive XZ‐2D plane reconstructed images of the relevant ion fragments.
Visualizing and Regulating Dynamic Evolution of Interfacial Electrolyte Configuration during De‐solvation Process on Lithium‐Metal Anode

March 2024

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70 Reads

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27 Citations

Acting as a passive protective layer, solid‐electrolyte interphase (SEI) plays a crucial role in maintaining the stability of the Li‐metal anode. Derived from the reductive decomposition of electrolytes (e.g., anion and solvent), the SEI construction presents as an interfacial process accompanied by the dynamic de‐solvation process during Li‐metal plating. However, typical electrolyte engineering and related SEI modification strategies always ignore the dynamic evolution of electrolyte configuration at the Li/electrolyte interface, which essentially determines the SEI architecture. Herein, by employing advanced electrochemical in situ FT‐IR and MRI technologies, we directly visualize the dynamic variations of solvation environments involving Li⁺‐solvent/anion. Remarkably, a weakened Li⁺‐solvent interaction and anion‐lean interfacial electrolyte configuration have been synchronously revealed, which is difficult for the fabrication of anion‐derived SEI layer. Moreover, as a simple electrochemical regulation strategy, pulse protocol was introduced to effectively restore the interfacial anion concentration, resulting in an enhanced LiF‐rich SEI layer and improved Li‐metal plating/stripping reversibility.


Visualizing and Regulating Dynamic Evolution of Interfacial Electrolyte Configuration during De‐solvation Process on Lithium‐Metal Anode

March 2024

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17 Reads

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4 Citations

Angewandte Chemie

Acting as a passive protective layer, solid‐electrolyte interphase (SEI) plays a crucial role in maintaining the stability of the Li‐metal anode. Derived from the reductive decomposition of electrolytes (e.g., anion and solvent), the SEI construction presents as an interfacial process accompanied by the dynamic de‐solvation process during Li‐metal plating. However, typical electrolyte engineering and related SEI modification strategies always ignore the dynamic evolution of electrolyte configuration at the Li/electrolyte interface, which essentially determines the SEI architecture. Herein, by employing advanced electrochemical in‐situ FT‐IR and MRI technologies, we directly visualize the dynamic variations of solvation environments involving Li+‐solvent/anion. Remarkably, a weakened Li+‐solvent interaction and anion‐lean interfacial electrolyte configuration have been synchronously revealed, which is difficult for the fabrication of anion‐derived SEI layer. Moreover, as a simple electrochemical regulation strategy, pulse protocol was introduced to effectively restore the interfacial anion concentration, resulting in an enhanced LiF‐rich SEI layer and improved Li‐metal plating/stripping reversibility.



[a] Typical initial galvanostatic charge/discharge curves of LRLO (2.0–4.8 V) cathode. Current density: 10 mA/g. [b] Potential/Time‐dependent in situ SERS spectra of LRLO recorded during first charging. The black traces present the Raman signal collected at open circuit voltage (OCV) for comparing. The newly‐produced Raman peaks have been assigned to superoxo, peroxo and Li2CO3 species, respectively. [c] ¹⁹F and ¹H NMR spectra of electrolytes after 30 cycles (extracted by D2O solvent, benzene as internal standard for fair normalization) of LRLO in different electrolytes, asterisks represented products unknown. [d] Possible reaction Schemes of HFE under nucleophilic attack on LRLO consistent with experimental and calculated results displayed. (e Schematic illustration of HFE intrinsic mechanism on LRLO interface for CEI fabrication.
[a] EIS‐GITT voltage profiles and corresponding logarithm of DLi+ of LRLO in EE and EEF electrolytes during first charge. [b] Picked Nyquist plots at 5th, 10th and 15th charging points from Figure 2 (a). [c,d] The variation of RCEI and Rct of LRLO during first charging in EE and EEF electrolytes. [e,f] Nyquist plots for LRLO in EE and EEF at different cycles. Corresponding fit results for the electrochemical impedance RCEI and Rct at the 3rd, 10th and 50th cycles. [g,h] TEM images of LRLO after 100 cycles using EE and EEF electrolytes. The IFFT results for the surface and bulk regions are also listed in Figure. The orange‐dashed ground state region is identified as a spinel structure, blue is defined as a distorted region, and red is assessed as a CEI morphology.
[a] Charge and discharge curve of LRLO by CCCV protocol. [b] The comparison of overall polarization ΔVcha‐dis (Vcha minus Vdis) on LRLO during cycling in different electrolytes. [c] The cycling performance (discharge capacity) of LRLO in EE and EEF electrolytes. [d] The variation of average voltage during charging and discharging along with cycling of LRLO in EE and EEF electrolytes. [e] The attribution of polarization. [f] The comparison of Rv and Lv changes during cycling in EE and EEF electrolytes. [g] The ratio of the charging capacity of the CV procedure to the total capacity of the current cycle at different cycle numbers in EE and EEF electrolytes. [h] The ratio of the irreversible capacity to the total capacity of the current cycle at different cycle numbers in EE and EEF electrolytes. [i] Floating current is obtained by holding 10 h at 4.8 V and the variation of floating current during cycling in EE and EEF electrolytes.
[a] O K‐edge sXAS spectra of discharged LRLO CEI with etching, fabricated by different electrolytes, including EEand EEF. [b] Characterization of the components of the CEI layer on LRLO after 50 cycles in different electrolytes via XPS F1s spectrums. [c] The concentration variation of elements C, O, F and P on LRLO in EE‐ and EEF‐CEI after different cycles with and without etching. [d] TOF‐SIMS characterization of the cycled cathode electrodes in EE and EEF after 100 cycles. The normalized depth profiles of the interface and bulk fragments illustrate the structure of the CEI. [e] 3D renderings of selected secondary ion fragments of different CEI. The sputtered volume is 100 μm (length) ×100 μm (width)×150 nm (height). [f] The CEI construction mechanism of HFE.
[a,b] Comparison of SEM morphologies on individual LRLO particles and electrode cracks after 300 cycles in EE and EEF. [c,d] The cross‐section images of electrodes after cycling in different electrolytes, local region is enlarged for comparing by‐products deposition from electrolyte decomposition. [e] Raman spectra of different LRLO samples after 100 cycles in EE and EEF compared with the pristine electrode (dark plots). [f] The comparison of structural rearrangement of LRLO cycled in EE and EEF via Raman intensity ratio of Ilayer/Ispinel and XRD intensity ratio of I(003)/I(104).
Manipulated Fluoro‐Ether Derived Nucleophilic Decomposition Products for Mitigating Polarization‐Induced Capacity Loss in Li‐Rich Layered Cathode

January 2024

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74 Reads

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15 Citations

Electrolyte engineering is a fascinating choice to improve the performance of Li‐rich layered oxide cathodes (LRLO) for high‐energy lithium‐ion batteries. However, many existing electrolyte designs and adjustment principles tend to overlook the unique challenges posed by LRLO, particularly the nucleophilic attack. Here, we introduce an electrolyte modification by locally replacing carbonate solvents in traditional electrolytes with a fluoro‐ether. By benefit of the decomposition of fluoro‐ether under nucleophilic O‐related attacks, which delivers an excellent passivation layer with LiF and polymers, possessing rigidity and flexibility on the LRLO surface. More importantly, the fluoro‐ether acts as “sutures”, ensuring the integrity and stability of both interfacial and bulk structures, which contributed to suppressing severe polarization and enhancing the cycling capacity retention from 39 % to 78 % after 300 cycles for the 4.8 V‐class LRLO. This key electrolyte strategy with comprehensive analysis, provides new insights into addressing nucleophilic challenge for high‐energy anionic redox related cathode systems.


Citations (28)


... Electrolyte from the cell with pristine carbon exhibits a distinct peak at~875 cm À 1 , attributed to the presence of peroxide. [37,38] This peak is absent in the cells with Ru active sites, signifying the absence of peroxide formation and suggesting a different mechanism for ORR and OER. With carbon only, hydrogen peroxide forms during discharge and is subsequently oxidized to water during charging via a twoelectron process. ...

Reference:

Ru‐Based Catalysts Deposited by Atomic Layer Deposition for Non‐Alkaline Zn‐Air Batteries
Concerns on the Peroxo-Based Reaction Process in Aqueous Zn–O 2 Battery
  • Citing Article
  • October 2024

The Journal of Physical Chemistry C

... In addition, co-solvents can be used to replace water and form an SEI layer [153,154], alleviating intensified corrosion and dendrite growth. Introducing suitable co-solvents [156]. Copyright 2024, The Royal Society of Chemistry to promote a balanced competitive interaction among the dissolution capabilities of various components is a promising approach, capable of generating variable dissolution conformations that respond to temperature changes. ...

Dual-Anion Chemistry Synchronously Regulating Solvation Structure and Electric Double Layer for Durable Zn Metal Anodes
  • Citing Article
  • January 2024

Energy & Environmental Science

... To further clarify the principles behind the discrepancy of fast charging performance, we then studied the solvation structures of electrolytes, which usually result from the competition between different interactions. [48][49][50][51][52] The solvation structure can be generally classied into three types according to the coordination number of Li + with TFSI − , namely AGGs (>1 Li + ), CIPs (contact ion pairs = 1 Li + ), and SSIPs (solvent-separated ion pairs, no Li + and free TFSI − ). Symmetric S-N-S stretching vibration in TFSI − , located at around 750 cm −1 in Raman and Fourier Transform Infrared (FTIR) spectra, is sensitive to the coordination of Li + . ...

Visualizing and Regulating Dynamic Evolution of Interfacial Electrolyte Configuration during De‐solvation Process on Lithium‐Metal Anode

... The repeated occurrence of CEI rupture and repair at local position on the cathode surface inevitably increases electrolyte consumption, causing CE to decrease and fluctuate significantly. 36,37 Therefore, the average CE of the baselinebattery within 100 cycles is only 90.5%, which is obviously lower than the 98.7% of TMS-battery (Fig. 5b). Further compared with the CE results over 100 cycles at 2-4.8 V in Fig. 2b, the CE of the baselinebattery decreases by 8.56% even though the upper cut-off voltage just increases by 0.2 V (4.8 to 5 V), while the TMS-battery only decreased by 0.48%. ...

Gradient Interphase Engineering Enabled by Anionic Redox for High-Voltage and Long-Life Li-Ion Batteries
  • Citing Article
  • February 2024

Journal of the American Chemical Society

... With the widespread adoption of new energy vehicles and large-scale energy storage devices, traditional Li + batteries are approaching their limits in the energy storage capacity. [1][2][3][4] Lithium-sulfur (Li-S) batteries, with their high theoretical energy density (2600 W h kg À 1 ) and low cost, are emerging as promising candidates for the next generation of energy storage system. [5] However, the real-world application of LiÀ S batteries has encountered significant obstacles, primarily due to limited practical energy density, low coulombic efficiency, and poor cycling stability. ...

Lattice Engineering on Li 2 CO 3 ‐Based Sacrificial Cathode Pre‐lithiation Agent for Improving The Energy Density of Li‐Ion Battery Full‐Cell

... In recent years, numerous approaches have been developed to stabilize the lattice, including introducing a more stable structure to act as a scaffold. 116,117 As shown in Fig. 13A, researchers have incorporated the perovskite variant phase La 4 [LiTM]O 8 (LLMO) as a "rivet" into the layered structure, forming a mechanically stable crystal structure. 114 HAADF-STEM images display the coherent growth of the LLMO phase along the [100] direction within the layered NCM (Fig. 13B). ...

One-Step Surface-to-Bulk Modification of High-Voltage and Long-Life LiCoO2 Cathode with Concentration Gradient Architecture

... [14] However, lithium salt additives, such as LiF, LiNO 3 , and LiDFOB, are costly and limited in variety. [15] Inorganic compound additives may lead to cycling instability due to subtle changes in size, morphology, and crystal phase. In contrast, ionic liquids (ILs), particularly pyrrole-and imidazolyl-based ones, have gained extensive attentions as organic additives due to their low cost, renewability, and self-repairing properties. ...

Protecting Li-metal in O2 atmosphere by sacrificial polymer additive for Li-O2 Battery
  • Citing Article
  • November 2023

Nanoscale

... [35] In contrast, large-sized single crystals avoid these defects, but at the same time face the problem of long diffusion distance of K + ions in the lattice and accumulation of internal stress. [36][37][38] Herein, we demonstrate a template-assisted regulation strategy to synthesize mesoporous single-crystal FeHCF (MCS-FeHCF) microspheres. On the one hand, the large-sized MCS-FeHCF has less grain boundaries, which enables fast charge transportation within FeHCF and diminish side reactions. ...

Does single-crystallization a feasible direction for designing Li-rich layered cathodes?
  • Citing Article
  • August 2023

Energy Storage Materials

... Subsequently, in 1991, Sony commercialized the first lithium-ion batteries (LIBs) product [9][10][11][12][13] . With the continued strong demand in the new energy market and the release of production capacity in the industry, new batteries such as zinc ions [14] , sodium ions [15] , and lithium-sulfur [16] have appeared dramatically. During this period, scientific researchers conducted continuous research on the battery efficiency and found that it largely depended on the characteristics of the cathode materials [17] . ...

Recognition and Application of Catalysis in Secondary Rechargeable Batteries
  • Citing Article
  • July 2023

ACS Catalysis

... In addition to adjusting the voltage window, the implementation of a pre-sodiation strategy has emerged as an effective approach to address the requirements for the practical applications. [41,42] In this work, we comprehensively explored the electrochemical performance of the high entropy Mn-based layered oxide cathode, focusing predominantly on the whole voltage window of 1.5 to 4.5 V. ...

Injecting Excess Na into a P2-Type Layered Oxide Cathode to Achieve Presodiation in a Na-Ion Full Cell
  • Citing Article
  • July 2023

Nano Letters