Melamine Foam-Derived Carbon Scaffold for Dendrite-Free and Stable Zinc Metal Anode

Aqueous Zn-ion batteries (AZIBs) are one of the most promising large-scale energy storage devices due to the excellent characteristics of zinc metal anode, including high theoretical capacity, high safety and low cost. Nevertheless, the large-scale applications of AZIBs are mainly limited by uncontrollable Zn deposition and notorious Zn dendritic growth, resulting in low plating/stripping coulombic efficiency and unsatisfactory cyclic stability. To address these issues, herein, a carbon foam (CF) was fabricated via melamine-foam carbonization as a scaffold for a dendrite-free and stable Zn anode. Results showed that the abundant zincophilicity functional groups and conductive three-dimensional network of this carbon foam could effectively regulate Zn deposition and alleviate the Zn anode’s volume expansion during cycling. Consequently, the symmetric cell with CF@Zn electrode exhibited lower voltage hysteresis (32.4 mV) and longer cycling performance (750 h) than the pure Zn symmetric cell at 1 mA cm−2 and 1 mAh cm−2. Furthermore, the full battery coupling CF@Zn anode with MnO2 cathode can exhibit a higher initial capacity and better cyclic performance than the one with the bare Zn anode. This work brings a new idea for the design of three-dimensional (3D) current collectors for stable zinc metal anode toward high-performance AZIBs.


Introduction
With the rapid developments of electric vehicles and smart grids, the ever-increasing demand for lithium-ion batteries (LIBs) and their further application would be hindered by the limited lithium resource. In this context, aqueous Zn-ion batteries (AZIBs) have been developed as alternatives to LIBs because of their low-cost, non-toxic, and high safety [1][2][3][4]. Nevertheless, during the charge-discharge process, the Zn metal anodes suffer from uncontrolled dendritic growth and harmful side reactions, leading to the unsatisfactory electrochemical performance of AZIBs [5,6]. In particular, the uncontrolled Zn dendritic growth may puncture the separator of the cell and cause an internal short circuit, which results in low Coulombic efficiency, poor reversibility and rapid capacity degradation of AZIBs, which severely limits their further application and development [7,8].
Until now, many efforts have been devoted to solving the aforementioned problems, including surface modification of Zn metal anodes [9][10][11][12][13][14][15][16], electrolyte optimization [17][18][19], novel separator design [20] and three-dimensional (3D) host design [21][22][23][24]. For example, He et al. [25] deposited an ultrathin Al 2 O 3 film on the Zn anode via the atomic layer deposition method, which effectively improved the interfacial wettability of the Zn anode and thus physically suppressed the formation of Zn dendrites. However, seen that MF exhibits a 3D porous skeleton structure providing a large specific surface area, which is favorable for Zn deposition. However, its conductivity is inferior and cannot be directly used as a zinc anode collector. In this study, a conductive 3D skeleton structure was formed by carbonizing the MF. As shown in Figure 1c, the CF still maintains the intact porous skeleton structure. In addition, energy dispersive spectroscopy (EDS) was carried out for element mapping of fabricated CF. the results of elemental mapping show that carbon, nitrogen, and oxygen elements are uniformly distributed on their surface ( Figure S1). This three-dimensional structure provides interconnected channels, facilitating rapid e − transport and excellent conductivity [28,33,35]. The porous 3D carbon foam framework can effectively alleviate the volume expansion of the electrode during repeated charge and discharge cycles, facilitating the integrity of the electrode structure and excellent cycling performance. Hence, a high-performance Zn metal anode could be anticipated by employing this carbon foam. After 10 mAh cm −2 amount of zinc deposition, CF@Zn with a relatively smooth surface was obtained (Figure 1d).
The fabrication procedure of CF@Zn is shown in Figure 1a. Firstly, the melamine foam was carbonized at 700 °C for 2 h under Ar2 to obtain CF, and then Zn was electrochemically deposited into the interior of CF to produce the CF@Zn electrode ( Figure 1a). Figure 1b depicts the SEM (scanning electron microscopy) image of melamine foam, and it can be seen that MF exhibits a 3D porous skeleton structure providing a large specific surface area, which is favorable for Zn deposition. However, its conductivity is inferior and cannot be directly used as a zinc anode collector. In this study, a conductive 3D skeleton structure was formed by carbonizing the MF. As shown in Figure 1c, the CF still maintains the intact porous skeleton structure. In addition, energy dispersive spectroscopy (EDS) was carried out for element mapping of fabricated CF. the results of elemental mapping show that carbon, nitrogen, and oxygen elements are uniformly distributed on their surface ( Figure S1). This three-dimensional structure provides interconnected channels, facilitating rapid e − transport and excellent conductivity [28,33,35]. The porous 3D carbon foam framework can effectively alleviate the volume expansion of the electrode during repeated charge and discharge cycles, facilitating the integrity of the electrode structure and excellent cycling performance. Hence, a high-performance Zn metal anode could be anticipated by employing this carbon foam. After 10 mAh cm −2 amount of zinc deposition, CF@Zn with a relatively smooth surface was obtained (Figure 1d).  Figure S2 shows the XRD (X-ray diffraction) patterns of pristine carbon foam and carbon foam after the pre-deposition of 10 mAh cm −2 zinc (CF@Zn). The XRD peaks of the CF@Zn sample could be Indexed to the peaks of standard zinc (PDF#04-0831), indicating the successful pre-deposition of Zn ions on the CF surface. Moreover, XPS (X-ray photoelectron spectroscopy) technique was carried out to investigate the surface chemical structures of the CF sample, and the binding energies were referenced to the C1s line at 284.8 eV from adventitious carbon. The results showed that the surface of CF contains carbon, nitrogen, and oxygen elements (Figure 2a), with the highest content of C elements, which is conducive to increase electrical conductivity. Figure 2b depicts the high-resolution C 1s spectra, and the presence of C=N and C-O peaks could be observed. Figure 2c displays the XPS energy spectrum of N 1s with zincophilicity pyrrole nitrogen and pyridine nitrogen peaks. The high-resolution XPS spectrum of O 1s is demonstrated in Figure 2d, where the spectrum consists of two characteristic peaks corresponding to the C=O and C-OH bonds, respectively. According to previous reports in the literature, the presence of pyridine nitrogen, pyrrole nitrogen, C=N [36] and C=O [34] could prove the high zincophilicity  Figure S2 shows the XRD (X-ray diffraction) patterns of pristine carbon foam and carbon foam after the pre-deposition of 10 mAh cm −2 zinc (CF@Zn). The XRD peaks of the CF@Zn sample could be Indexed to the peaks of standard zinc (PDF#04-0831), indicating the successful pre-deposition of Zn ions on the CF surface. Moreover, XPS (X-ray photoelectron spectroscopy) technique was carried out to investigate the surface chemical structures of the CF sample, and the binding energies were referenced to the C1s line at 284.8 eV from adventitious carbon. The results showed that the surface of CF contains carbon, nitrogen, and oxygen elements (Figure 2a), with the highest content of C elements, which is conducive to increase electrical conductivity. Figure 2b depicts the high-resolution C 1s spectra, and the presence of C=N and C-O peaks could be observed. Figure 2c displays the XPS energy spectrum of N 1s with zincophilicity pyrrole nitrogen and pyridine nitrogen peaks. The high-resolution XPS spectrum of O 1s is demonstrated in Figure 2d, where the spectrum consists of two characteristic peaks corresponding to the C=O and C-OH bonds, respectively. According to previous reports in the literature, the presence of pyridine nitrogen, pyrrole nitrogen, C=N [36] and C=O [34] could prove the high zincophilicity on the CF surface. These nitrogen and oxygen-containing functional groups endow the CF with excellent zincophilicity characteristics [14]. The large specific surface area and zincophilicity characteristic of the CF provides substantial plating sites for Zn ions and could effectively regulate uniform Zn deposition [26]. on the CF surface. These nitrogen and oxygen-containing functional groups endow the CF with excellent zincophilicity characteristics [14]. The large specific surface area and zincophilicity characteristic of the CF provides substantial plating sites for Zn ions and could effectively regulate uniform Zn deposition [26]. To explore the deposition behavior of zinc ions on CF sample and copper foil at different deposition amounts, scanning electron microscopy was utilized to investigate the electrode morphologies at deposition amounts of 1, 5 and 10 mAh cm −2 . When plated with a capacity of 1 mAh cm −2 , the metallic zinc was deposited preferentially on the skeleton, as shown in Figure 3a. As the plating capacity reached 5 mAh cm −2 , the voids of CF were gradually filled ( Figure 3b). When the zinc deposition capacity increased to 10 mAh cm −2 , the skeleton was fully filled, and the zinc deposition was relatively uniform without the generation of Zn dendrites (Figure 3c). In contrast, at a deposition capacity of only 1 mAh cm −2 , metallic zinc has spread over the entire Cu foil ( Figure 3d). As the deposition capacity continued to increase to 5 mAh cm −2 (Figure 3e), holes began to appear on the Cu foil surface. When further increased to 10 mAh cm −2 , the holes become more apparent ( Figure  3f). The different deposition behaviors of zinc on the two collectors indicate that CF can effectively promote the uniform deposition of zinc ions, and there is more space to accommodate zinc ions, thus alleviating the volume expansion during cycling. To explore the deposition behavior of zinc ions on CF sample and copper foil at different deposition amounts, scanning electron microscopy was utilized to investigate the electrode morphologies at deposition amounts of 1, 5 and 10 mAh cm −2 . When plated with a capacity of 1 mAh cm −2 , the metallic zinc was deposited preferentially on the skeleton, as shown in Figure 3a. As the plating capacity reached 5 mAh cm −2 , the voids of CF were gradually filled ( Figure 3b). When the zinc deposition capacity increased to 10 mAh cm −2 , the skeleton was fully filled, and the zinc deposition was relatively uniform without the generation of Zn dendrites ( Figure 3c). In contrast, at a deposition capacity of only 1 mAh cm −2 , metallic zinc has spread over the entire Cu foil ( Figure 3d). As the deposition capacity continued to increase to 5 mAh cm −2 (Figure 3e), holes began to appear on the Cu foil surface. When further increased to 10 mAh cm −2 , the holes become more apparent (Figure 3f). The different deposition behaviors of zinc on the two collectors indicate that CF can effectively promote the uniform deposition of zinc ions, and there is more space to accommodate zinc ions, thus alleviating the volume expansion during cycling.
To further demonstrate the advantage of the 3D CF for regulating uniform Zn deposition, Zn||Cu foil (or Zn||CF) cells were used to investigate the coulombic efficiency (CE) of Zn anodes. Figure 4a depicts the voltage profiles of the Zn||Cu foil cells at the 1st, 25th and 50th cycles at a current density of 5 mA cm −2 and a capacity of 2 mAh cm −2 . The copper foil electrode exhibited a high overpotential of 88.2 mV. Compared with the copper foil electrode, the CF electrode exhibited a low voltage hysteresis of 60 mV (Figure 4b). In addition, the Zn||CF half-cell is capable of 120 stable cycles, while the Cu foil electrode can only run about 80 cycles (Figure 4c). Compared with the previously reported literature, the average Coulomb efficiency of CF electrodes still has some advantages, especially at the large current density and large areal capacity (Table S2). In addition, we investigated the surface morphology of CF and Cu foil after cycling a different number of cycles. As shown in Figure S3, after 50 cycles, large Zn dendrites had already formed on the Cu foil electrode. With the cycle number of cycles, more and more Zn flakes could be found on the surface of Cu foil. In striking contrast, the surface of the CF electrode became flat after 50 cycles, and the uniform Zn plating layer, in turn, enabled smooth Zn plating/stripping reactions in the following cycles. When tested at 10 mA cm −2 and 10 mAh cm −2 , the CF electrode exhibited higher cycling stability and longer cycling stability compared to the Cu foil electrode (Figure 4d). The electrochemical performance of the half-cells indicates that the zinc ion plating/stripping process of the carbon foam electrode was more stable, which was closely related to the high specific surface area and porous conductive structure of the carbon foam electrode. To further demonstrate the advantage of the 3D CF for regulating uniform Zn deposition, Zn||Cu foil (or Zn||CF) cells were used to investigate the coulombic efficiency (CE) of Zn anodes. Figure 4a depicts the voltage profiles of the Zn||Cu foil cells at the 1st, 25th and 50th cycles at a current density of 5 mA cm −2 and a capacity of 2 mAh cm −2 . The copper foil electrode exhibited a high overpotential of 88.2 mV. Compared with the copper foil electrode, the CF electrode exhibited a low voltage hysteresis of 60 mV ( Figure  4b). In addition, the Zn||CF half-cell is capable of 120 stable cycles, while the Cu foil electrode can only run about 80 cycles (Figure 4c). Compared with the previously reported literature, the average Coulomb efficiency of CF electrodes still has some advantages, especially at the large current density and large areal capacity (Table S2). In addition, we investigated the surface morphology of CF and Cu foil after cycling a different number of cycles. As shown in Figure S3, after 50 cycles, large Zn dendrites had already formed on the Cu foil electrode. With the cycle number of cycles, more and more Zn flakes could be found on the surface of Cu foil. In striking contrast, the surface of the CF electrode became flat after 50 cycles, and the uniform Zn plating layer, in turn, enabled smooth Zn plating/stripping reactions in the following cycles. When tested at 10 mA cm −2 and 10 mAh cm −2 , the CF electrode exhibited higher cycling stability and longer cycling stability compared to the Cu foil electrode (Figure 4d). The electrochemical performance of the halfcells indicates that the zinc ion plating/stripping process of the carbon foam electrode was more stable, which was closely related to the high specific surface area and porous conductive structure of the carbon foam electrode.  To further investigate the electrochemical behavior of the CF electrode in a symmetric cell, a 10 mAh cm −2 capacity of zinc was pre-electrodeposited to the CF and Cu foil electrodes prior to cycling. At a current density of 1 mA cm −2 and a capacity of 1 mAh cm −2 , the symmetric cell with CF electrodes exhibited a low overpotential of about 32.4 To further investigate the electrochemical behavior of the CF electrode in a symmetric cell, a 10 mAh cm −2 capacity of zinc was pre-electrodeposited to the CF and Cu foil electrodes prior to cycling. At a current density of 1 mA cm −2 and a capacity of 1 mAh cm −2 , the symmetric cell with CF electrodes exhibited a low overpotential of about 32.4 mV and was able to cycle stably for nearly 800 h (Figure 5a), which is better than the cycle life of most of the reported zinc anodes with carbon-based hosts or modified by carbonbased materials (Table S1, Supporting Information). On the contrary, with Cu foil electrodes and pure zinc electrodes, the overpotential of the symmetric cells increased after a period of cycling until, finally, an internal short circuit was observed, which may be associated with the generation of zinc dendrites. Furthermore, the cycling stability of the symmetric cell with CF@Zn electrode was tested at a higher current density. Impressively, the symmetric cell with CF@Zn electrodes still exhibited stable cycling (650 h) and low overpotential (45.6 mV) at 2 mA cm −2 . By contrast, the symmetric cells with Cu foil electrodes and the pure Zn electrodes exhibited significant voltage oscillation and short cycle life (Figure 5b). When increased to 4 mA cm −2 and 2 mAh cm −2 , the symmetric cell with CF electrodes could cycle stably for 500 h with a low voltage polarization (54.1 mV). In contrast, the cell with Cu foil electrodes exhibited a larger overpotential (57.1 mV) and a large voltage drop at 100 h upon cycling, indicating an internal short circuit, followed by severe voltage fluctuations with continued cycling, indicating the generation of substantial zinc dendrites inside the Cu foil electrode. The cell with pure zinc electrodes exhibited a much higher overpotential (76.3 mV) (Figure 5c). Therefore, the above symmetric cell results showed that the CF electrode was able to effectively inhibit the generation of Zn dendrites, ensuring that the cell could be cycled stably for a longer lifetime.
The advantage of the carbon foam skeleton toward stable Zn metal anodes was also demonstrated in full cells by coupling with the MnO 2 cathode. The X-ray diffraction pattern of the as-prepared cathode material is depicted in Figure S4a, which could be indexed to α-MnO 2 . In addition, the scanning electron microscopy image of the as-prepared α-MnO 2 ( Figure S4b) depicts the morphology of nanorods. In order to explore the influence of different porosity of CF@Zn on electrochemical performance, we pre-deposited CF with different amounts of Zn (2 mAh cm −2 , 5 mAh cm −2 and 10 mAh cm −2 ) and conducted full-cell electrochemical performance tests of these CF@Zn electrodes. As shown in Figure S5, when the pre-deposition amount of Zn was 2 mAh cm −2 , the cell with this CF@Zn electrode could not run; when the Zn deposition amount was 5 mAh cm −2 , the capacity of the cell was relatively low and decreased rapidly; when the deposition amount was 10 mAh cm −2 , the battery capacity was much higher, and the cycling performance was better than the other two cells, so the deposition amount of 10 mAh cm −2 was used in the subsequent electrochemical tests. Figure 6a shows the cyclic voltammetry curves of Zn||α-MnO 2 and CF@Zn||α-MnO 2 full cells. Both exhibit essentially similar redox peak positions, indicating that the CF electrode does not change the reaction mechanism of α-MnO 2 . Moreover, the CF@Zn||α-MnO 2 cell exhibited a higher peak current density and area, indicating that the CF@Zn electrode could provide higher capacity and electrochemical reactivity. The rate performance of Zn||α-MnO 2 and CF@Zn||α-MnO 2 full cells were subsequently tested in the current density of 0.5 to 5.0 A g −1 . As shown in Figure 6b, the average discharge capacities of CF@Zn||α-MnO 2 full cells were 111.9, 119, 83.9, and 43.5 mAh g −1 at 0.5, 1, 2, and 5 A g −1 . All were higher than those of Zn||α-MnO 2 full cells. When the current density returned to 0.5 A g −1 , the CF@Zn||α-MnO 2 full cell (183.2 mAh g −1 ) remained much higher than the average discharge capacity of the Zn||α-MnO 2 full cell (128.9 mAh g −1 ). The charge and discharge curves of CF@Zn||α-MnO 2 and Zn||α-MnO 2 full cells at different current densities are shown in Figures 6c and 6d, respectively. Compared to the bare Zn||α-MnO 2 full battery, the CF@Zn||α-MnO 2 full cell has a lower charging voltage plateau and a higher discharge voltage plateau, indicating that the rate performance of the bare Zn anode is effectively improved. Figure 6e shows the Electrochemical Impedance Spectroscopy (EIS) spectra of the Zn||α-MnO 2 and CF@Zn||α-MnO 2 cells. The CF@Zn negative electrode exhibited lower charge transfer resistance (Rct) and zinc ion diffusion resistance, which indicated that the CF electrode had good interfacial wettability with the electrolyte. By fitting the EIS with the equivalent circuit (inset in Figures 6e and S6), the fitting curve matched well with the raw data, indicating the suitability of the employed equivalent circuit. The calculated impendence parameters are shown in Tables S3 and S4. The dramatic growth of the Rs and Rct of bare Zn||α-MnO 2 cell suggest a deteriorated electrode/electrolyte interface during the Zn stripping/plating cycling process. In comparison, for CF@Zn||α-MnO 2 cells, the Rs and Rct exhibited much slower growth, indicating that the CF could inhibit the formation of Zn dendrites and provide space for volume expansion during repeated charge-discharge cycles. Figure 6f shows the cycling performance of bare Zn||α-MnO 2 and CF@Zn||α-MnO 2 at 1 A g −1 . CF@Zn||α-MnO 2 exhibited a higher initial capacity (123.6 mAh g −1 ) and still had 66.1 mAh g −1 after 180 cycles. The advantage of the carbon foam skeleton toward stable Zn metal anodes was al demonstrated in full cells by coupling with the MnO2 cathode. The X-ray diffraction p tern of the as-prepared cathode material is depicted in Figure S4a, which could be index to α-MnO2. In addition, the scanning electron microscopy image of the as-prepared MnO2 ( Figure S4b) depicts the morphology of nanorods. In order to explore the influen of different porosity of CF@Zn on electrochemical performance, we pre-deposited CF w different amounts of Zn (2 mAh cm −2 , 5 mAh cm −2 and 10 mAh cm −2 ) and conducted fu cell electrochemical performance tests of these CF@Zn electrodes. As shown in Figure S when the pre-deposition amount of Zn was 2 mAh cm −2 , the cell with this CF@Zn electro After cycling, the cells were disassembled to check the state of the Zn anodes. As shown in Figure S7b, the bare Zn became tattered due to the formation of massive byproducts accompanied by dramatic Zn-mass redistribution. On the other hand, the CF@Zn electrode remains quite an integral structure with a relatively uniform surface morphology ( Figure S7a). Apart from that, the cross-sectional view SEM images of the CF@Zn before and after cycling are shown in Figure S8. The thickness of the CF@Zn electrode before cycling is around 125 µm. After 100 cycles in a full cell with the α-MnO2 cathode at 1 A g −1 , the thickness of the CF@Zn electrode increased a little bit to about 129 µm, which indicates that the abundant zincophilicity functional groups and conductive three-dimensional network of this carbon foam can effectively regulate Zn deposition and alleviate the Zn anode's volume expansion during cycling. The CF@Zn electrode exhibited a superior full-cell electrochemical performance, which can be attributed to its ability to effectively suppress zinc dendritic growth, thereby improving the cyclic stability of aqueous Zn-ion batteries. After cycling, the cells were disassembled to check the state of the Zn anodes. As shown in Figure S7b, the bare Zn became tattered due to the formation of massive byproducts accompanied by dramatic Zn-mass redistribution. On the other hand, the CF@Zn electrode remains quite an integral structure with a relatively uniform surface morphology ( Figure S7a). Apart from that, the cross-sectional view SEM images of the CF@Zn before and after cycling are shown in Figure S8. The thickness of the CF@Zn electrode before cycling is around 125 µm. After 100 cycles in a full cell with the α-MnO 2 cathode at 1 A g −1 , the thickness of the CF@Zn electrode increased a little bit to about 129 µm, which indicates that the abundant zincophilicity functional groups and conductive three-dimensional network of this carbon foam can effectively regulate Zn deposition and alleviate the Zn anode's volume expansion during cycling. The CF@Zn electrode exhibited a superior full-cell electrochemical performance, which can be attributed to its ability to effectively suppress zinc dendritic growth, thereby improving the cyclic stability of aqueous Zn-ion batteries.

Materials
All reagents were of analytical grade and used as received without further purification. The MA sponge was provided by SINOYQX Co., Ltd., Chengdu, China. KMnO 4 and MnSO 4 were purchased from Shanghai Aladdin Biochemical Technology Co., Ltd., Shanghai, China. Ethanol (C 2 H 5 OH, 99.7%) was purchased from Sinopharm Chemical. Reagent Co., Ltd. The Zn foil and CR2032 coin cells were from Guangdong Canrd New Energy Technology Co., Ltd., Dongguan, China.

Preparation of the Carbon Foam
The carbon foam was fabricated via the carbonization method as described elsewhere [33]. Carbon foam (CF) was prepared by calcining melamine foam at 700 • C for 2 h under an Ar 2 atmosphere (The heating rate was 5 • C min −1 ).

Preparation of the α-MnO 2 Cathode
For the α-MnO 2 cathode, 6 mmoL KMnO 4 was dissolved in 60 mL distilled H 2 O, then 20 mmoL concentrated HCl was slowly added under severe agitation. Afterward, transferred the resulting clear purple solution to a Teflon-lined stainless steel autoclave with a volume of 100 mL. The sealed autoclave was heated to 140 • C for 12 h. After cooling to room temperature, the precipitate was collected through centrifugation and cleaned several times with distilled water. After 12 h dried by vacuum oven at 60 • C, the α-MnO 2 was obtained.

Electrochemical Measurements
The cathode slurry was obtained by mixing the α-MnO 2 powder, acetylene black carbon, and polyvinylidene difluoride in a 7:2:1 weight ratio in an NMP solution. Then, the obtained slurry was painted onto the stainless steel mesh. After 12 h of vacuum drying at 60 • C, the stainless steel mesh was cut into 12 mm diameter discs. The obtained discs with a loading mass of 1.0-1.5 mg of active material were used as cathode electrodes for AZIBs. CR2032 coin cells assembled with working and counter electrodes separated via a glass fiber separator (Φ18) were used to assess electrochemical properties. CF pre-deposited 10 mAh cm −2 of zinc as the anode (CF@Zn). The performance of Zn plating/stripping was evaluated in symmetrical Zn||Zn (CF@Zn||CF@Zn) batteries with a 2 M ZnSO 4 (100 µL) solution as the electrolyte. Zn||Cu (or Zn||CF) cells were used to evaluate the CE of Zn anodes. The electrochemical performance of full cells (Zn||α-MnO 2 or CF@Zn|α-MnO 2 ) was investigated using a 2 M ZnSO 4 + 0.1 M MnSO 4 (100 µL) solution as the electrolyte at 1 A g −1 in the 0.8-1.8 V voltage range. All these tests were performed on a LANDCT2001A battery testing system. Electrochemical impedance spectroscopy (EIS) was evaluated on a CHI660E electrochemical workstation in the 0.01 Hz to 100 kHz frequency range. For full cells, cyclic voltammetry (CV) curves were tested by an electrochemical workstation system (CHI-660E type) with a scan rate of 0.1 mV s −1 .

Materials Characterizations
X-ray diffraction (XRD) (Bruker D8 ADVANCE, Cu Kα source, a scan speed of 5 • min −1 ) was used to determine the phase composition and crystal structure of the prepared samples. Scanning electron microscopy (SEM) was used to evaluate the morphology, energy dispersive spectroscopy (EDS), and element mapping of produced materials (JSM-7800F, JEOL, Akishima, Japan). The chemical structures of the samples were analyzed by X-ray photoelectron spectroscopy (XPS), which was carried out on a Thermo K-Alpha XPS spectrometer (Thermo Fisher Scientific, Waltham, MA, USA) with a monochromatic Al Ka X-ray source (1486.6 eV). The binding energies were referenced to the C1s line at 284.8 eV from adventitious carbon.

Conclusions
In summary, we have successfully demonstrated the effectiveness of an MF-derived carbon foam collector in the construction of a dendrite-free zinc metal anode. The large specific surface area of carbon foam reduces the local current density of the electrode and avoids the tip effect. Furthermore, the carbon foam surface containing a large number of active sites could promote uniform zinc deposition and inhibit Zn dendritic growth. Symmetric cells assembled with CF@Zn electrodes have superior electrochemical performance than pure Zn electrodes. At 1 mA cm −2 and 1 mAh cm −2 , the CF@Zn symmetric cell depicted a lower overpotential (32.4 mV) and better cycling performance (750 h) than the Zn symmetric cell. After being assembled with α-MnO 2 into a full cell, the CF@Zn anode exhibited superior rate performance and longer cycling performance than the pure Zn anode. Our further study will be focused on compositing other zincophilic materials (e.g., Ag, ZIF-8 and graphene) with CF to further increase the CF's electrochemical performance. The development of the CF@Zn anode would bring a new strategy for the realization of high-performance aqueous zinc-ion batteries.
Supplementary Materials: The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules28041742/s1. Figure S1: (a) SEM and (b) corresponding mapping images of CF; Figure S2: XRD patterns of pure CF and CF@Zn samples; Figure S3: Scanning electron microscopy images of (a,c,e) CF and (b,d,f) Cu foil electrodes at the deposition current density of 5 mA cm −2 and deposition capacities of 2 mAh cm −2 with different cycles: (a) and (b) 20 cycles; (c) and (d) 50 cycles; (e) and (f) 80 cycles; Figure S4: (a) XRD patterns and (b) SEM image of α-MnO 2 ; Figure S5: Cyclic performance of pre-deposited CF with different amounts of Zn (2 mAh cm −2 , 5 mAh cm −2 and 10 mAh cm −2 ) in full cells; Figure S6: Nyquist plots of bare Zn and CF@Zn full cells at 1 A g −1 after 100 cycles (inset is the equivalent circuit); Figure S7: SEM images of (a) CF@Zn and (b) bare Zn anodes in full cells with α-MnO 2 cathode after 100 cycles at 1 A g −1 ; Figure S8: Cross-sectional view SEM images of (a) CF@Zn and (b) bare Zn anodes in full cells with α-MnO 2 cathode after 100 cycles at 1 A g −1 ; Table S1: A survey of zinc anodes with carbon-based hosts or modified by carbon-based materials and corresponding electrochemical properties; Table S2: Different host materials for zinc metal anodes and the corresponding average CE value; Table S3: The impedance parameters for full cells with α-MnO 2 cathode before cycling; Table S4: The impedance parameters for full cells with α-MnO 2 cathode at 1 A g −1 after 100 cycles. References [37][38][39][40][41][42] are cited in supplementary materials.