Next Article in Journal
Prediction of Surface Treatment Effects on the Tribological Performance of Tool Steels Using Artificial Neural Networks
Next Article in Special Issue
Ablation and Patterning of Carbon Nanotube Film by Femtosecond Laser Irradiation
Previous Article in Journal
Review of Machining Equipment Reliability Analysis Methods based on Condition Monitoring Technology
Previous Article in Special Issue
Na2Ti7O15 Nanowires with an Oriented Tunnel Structure and High Mechanical Stability: A Potential Anode of Sodium-Ion Batteries and Gas Sensing Materials
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Applied Sciences
Volume 9
Issue 14
10.3390/app9142787
applsci-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Review

Recent Progress of Metal–Air Batteries—A Mini Review

by
Chunlian Wang
1,
Yongchao Yu
2,
Jiajia Niu
3,
Yaxuan Liu
2,
Denzel Bridges
2,
Xianqiang Liu
3,
Joshi Pooran
4,
Yuefei Zhang
3 and
Anming Hu
1,2,*
1
Institute of Laser Engineering, Beijing University of Technology, Beijing 100124, China
2
Department of Mechanical, Aerospace and Biomedical Engineering, University of Tennessee, Knoxville, TN 37996, USA
3
Institute of Microstructure and Properties of Advanced Materials, Beijing University of Technology, Beijing 100124, China
4
Oak Ridge National Lab, Oak Ridge, TN 37831, USA
*
Author to whom correspondence should be addressed.
Appl. Sci. 2019, 9(14), 2787; https://doi.org/10.3390/app9142787
Submission received: 3 June 2019 / Revised: 4 July 2019 / Accepted: 6 July 2019 / Published: 11 July 2019
(This article belongs to the Special Issue Laser Processing and Advanced Manufacturing of Microscale Energy Storage Devices)
Browse Figures
Review Reports Versions Notes

Abstract

:

Featured Application

This paper can provide the basic knowledge on metal-air batteries for beginners and relevant comprehensive review for researchers.

Abstract

With the ever-increasing demand for power sources of high energy density and stability for emergent electrical vehicles and portable electronic devices, rechargeable batteries (such as lithium-ion batteries, fuel batteries, and metal–air batteries) have attracted extensive interests. Among the emerging battery technologies, metal–air batteries (MABs) are under intense research and development focus due to their high theoretical energy density and high level of safety. Although significant progress has been achieved in improving battery performance in the past decade, there are still numerous technical challenges to overcome for commercialization. Herein, this mini-review summarizes major issues vital to MABs, including progress on packaging and crucial manufacturing technologies for cathode, anode, and electrolyte. Future trends and prospects of advanced MABs by additive manufacturing and nanoengineering are also discussed.

1. Introduction

1.1. Market Demand and Technical Tendencies

With the continued growth of the global economy, the demand for energy has significantly increased. Unfortunately, Earth’s conventional non-renewable energy resources, such as coal, oil, and natural gas, are limited. Hence, the development of new energy devices is important for a sustainable society. Innovative biofuel batteries, supercapacitors, and metal–air batteries are among the most suitable candidates to meet the energy storage demand [1,2,3,4,5,6]. Among the various power storage devices currently on the market, lithium-ion batteries (LIBs) have the best performance. However, it is still a challenge to achieve high capacity (>200 mA h g−1) in LIBs and to meet safe energy storage requirements for electric vehicles [7,8]. Recently, MABs attracted significant attention as they can operate in an open-air atmosphere. MABs consist of metal anodes and an air cathode. The MAB cathode uses oxygen from ambient air, which leads to significant battery weight reduction, which has unprecedented advantages for many applications. Compared to other batteries, especially Lithium-ion batteries, which currently dominate the market share, MABs are cheap, because the cathode source (oxygen from air) is abundant and the anode can be made using low-cost metals, such as, Al, Zn, Fe. Figure 1 shows the application of MABs as the energy storage system for various technologies. MABs are attractive not only as compact power sources for portable electronics and electric vehicles but also as compelling energy transfer stations or energy storage devices to manage energy flow among renewable energy generators, such as wind turbines and photovoltaic panels, electric grids and end-users.
Theoretical energy density is an important factor in evaluating the performance of various battery configurations. Figure 2 shows theoretical energy density, specific energy, and nominal cell voltage of different metal-air batteries (MABs) [9]. As oxygen, directly supplied from the surrounding environment, is involved in the cathode as an oxidant during the discharge period, MABs show considerably higher energy density. Although, theoretically, lithium–air batteries (LABs) offer the best combination of the highest theoretical energy density (5928 Wh kg−1) and high cell potential (nominally 2.96 V), iron–air batteries (FABs) possess the smallest theoretical energy density and cell voltage (nominally 1.28 V). Al-, Zn-, and Fe–air batteries are also the research hotspots because of economic and safety considerations.
In the present paper, aluminum–air batteries (AABs), zinc–air batteries (ZABs), iron–air batteries (FABs), and lithium–air batteries (LABs) have been reviewed with a focus on working principle and device configuration, and performance progress. In addition, major technology barriers have been identified, and possible solutions discussed. Emerging advanced manufacturing methods, such as 3D printing and laser processing techniques, for the development a high-performance rechargeable MABs, have also been discussed.

1.2. Working Principles

The working principle of MABs differs from that of traditional ionic batteries. The traditional ionic batteries involve the transformation of metallic ions from the anode to the cathode. In MABs, metals or alloys transform to metallic ions at anode and oxygen transforms to hydroxide ions at the cathode. Figure 3 shows the operation of a MAB in aqueous or non-aqueous electrolyte medium. In an aqueous electrolyte system, oxygen diffuses into batteries through the gas diffusion layer and transforms into receiving electrons forming oxygen anions. In a non-aqueous electrolyte system, oxygen receives electrons and transforms into oxygen anion. Metals release electrons, transform to metallic ions and dissolve into electrolytes. These processes will be reversible during a charging procedure of a rechargeable MAB.
For MABs, oxygen and metals participate in electrochemical reactions. Specific reaction formulas are as Equations (1) and (2):
Anode: M ⇌ Mn+ + ne−
Cathode: O2 + 2H2O + 4e− ⇌ 4OH−
The reaction kinetics of FABs in the alkaline aqueous electrolyte are shown in Equations (1) and (6) [10].
Anode: Fe + 2OH− ⇌ Fe(OH)2 + 2e−
3Fe(OH)2 + 2OH− ⇌ Fe3O4 + 4H2O + 2e−
Cathode: O2 + 2H2O + 4e− ⇌ 4OH−
Overall reaction: 2O2 + 3Fe ⇌ Fe3O4
The working principle of AABs in the alkaline aqueous electrolyte is shown in (9) [11].
Anode: Al + 4OH− ⇌ Al(OH)4− + 3e−
Cathode: O2 + 2H2O + 4e− ⇌ 4OH−
Overall reaction: 3O2 + 2Al ⇌ Al2O3
The working principle of ZABs in the alkaline aqueous electrolyte is shown in (13) [12].
Anode: Zn + 4OH− ⇌ Zn(OH)42− + 2e
Zn(OH)42− ⇌ ZnO + 2OH− + H2O
Cathode: O2 + 2H2O + 4e− ⇌ 4OH−
Overall reaction: O2 + Zn ⇌ ZnO
The working principle of LABs in the non-aqueous electrolyte is shown in (18) [1].
Anode: Li ⇌ Li+ + e−
Cathode: O2 + e− ⇌ O2−
O2− + Li+ ⇌ LiO2
LiO2 + Li+ + e− ⇌ Li2O2
Overall reaction: O2 + Li ⇌ Li2O2

1.3. Configuration of MABs

Based on packaging and practical application requirements, MABs can be classified as traditional static batteries, flow batteries, and novel flexible batteries [13]. In this part, three kinds of batteries will be discussed briefly. The latter part is based on the analysis of solid-state batteries.
Traditional static batteries: As shown in Figure 3, traditional static air batteries have four main parts: cathode, separator, electrolyte, and anode. Compared to the fast kinetics of the anode reaction, oxygen reaction on cathodes is kinetically sluggish in nature. A three-phase reaction boundary of solid (catalyst)–liquid (electrolyte)–gas (oxygen) contributes to the oxygen reduction reaction (ORR). Meanwhile, a reversed oxygen evolution reaction (OER) occurs on a two-phase boundary solid (catalyst)–liquid (electrolyte) at the cathode [14]. Highly efficient bifunctional catalysts are thus required to facilitate both OER and ORR. In addition, since an active electrolyte is employed in traditional static MABs, it is challenging to completely overcome the issue of insoluble deposition of by-products on the surface of both the metal anode and air cathode during the charge–discharge cycles. These deposited by-products consequently block the electrode pores limiting the diffusion of air that eventually results in a lower battery performance [15].
Flow batteries: This type of MAB consists of an electrode, separator, electrolyte, and an electrolyte bank installed as an additional part. Usually, a pump is also integrated to drive electrolyte flow, as shown in Figure 4b. Flowing-electrolyte configuration addresses some of the problems associated with the metal anode and an air cathode. For instance, in zinc–nickel batteries, a large volume of flowing electrolyte decreases the formation of dendrites and irregular shape changes of zinc and thereby, avoid passivation by improving current distribution and reducing concentration gradients [16]. However, the complicated flowing-configuration of MABs has some shortcomings, including decreased energy efficiency and volume density, and increased complications as additional pumps and tubes are needed to drive the flow of electrolyte during the discharge.
Flexible batteries: With the increasing demand for portable electronics in recent years, light and small form-factor flexible batteries have become a hot research topic [17,18]. The main components of a flexible battery include a cathode, anode, separator, and high conductivity electrolyte. Conventional electrolyte for a flexible battery system is a solid-state electrolyte. A thin metallic plate is used as a metal anode to reduce the battery weight. Various nano compounds and nanocomposites are being explored as a potential cathode material. Specific materials include carbon fibers, carbon nanotubes, and graphene. According to the current development trend, flexible batteries are undergoing an evolution, from polymer batteries, flexible alkaline batteries, lithium-based batteries to metal–air batteries. Currently, ZABs and AABs are the ideal flexible batteries due to low cost, safe operation, and high energy density [19].

1.4. Technical barriers

Although metal–air batteries have been studied for many years, there are still major technical issues to address for practical applications. Metallic anodes face many challenges, such as corrosion, hydrogen generation, forming passivation layers, dendritic formation, electrode deformation, and energy loss due to self-charging. The air anode has many obstacles, such as lack of efficient catalysts for both ORR and OER, affecting electrolyte stability due to impurity and dissolved gas, and gas diffusion blockage by side reaction products. Electrolyte selection, which is an important component for efficient electrochemical reaction, also poses some technical barriers due to side reaction with the anode, reaction with CO2 from air, and low conductivity. In the following sections, we will discuss these issues and potential solutions.

2. Cathodes

2.1. Components of the Cathodic Electrode

On the cathode, chemistry reactions are ORR and OER. The oxidant is oxygen from air atmosphere. The catalysts are required to lower overpotential of ORR and OER. For an aqueous electrolyte, water loss should be avoided to keep battery stability. Hence, the practical cathode is composed of a catalyst layer, gas diffusion layer, and current collector, as shown in Figure 5. The current collector can be metal and non-metal. Metal current collectors are a porous foam-like metal, for example, Ni, Cu. Non-metal current collectors are carbon-based material, for example, conductive carbon paper, graphitic fiber or carbon cloth. Gas diffusion layer (GDL) and the catalysts are also extremely crucial for cathode performance.
(1) Gas diffusion layer: In MABs, the GDL has multi-folded functions: supporting of catalyst layer; providing oxygen diffusion channels between air and catalyst layer; preventing water getting into battery and electrolyte getting out of battery. To better serve as a bridge between air and catalyst layer, the GDL should be thin, light, highly porous, and hydrophobic. Figure 4b indicates that the ORR in MABs occurs at the three phase boundaries (oxygen air, liquid electrolyte, and solid catalyst). The GDL can simultaneously provide hydrophilic micro-channels to the liquid electrolyte, and hydrophobic layers to prevent electrolyte leakage and good properties of gaseous oxygen diffusion [20].
(2) Catalyst layer: Since the kinetics for the oxygen reaction is naturally slow, bifunctional catalysis is required to improve ORR and OER to improve electrochemical performances of MABs. Based on previous researches, platinum (Pt) [21], ruthenium (Ru) oxides, and iridium oxides (Ir) [22] showed excellent performance in ORR and OER. Furthermore, nanostructures of the following materials also had good catalytic activity, (a) transition metal oxides, MnO, CoO, NiO, etc. [23]; (b) transition metal hydroxide and sulfide, NiCoFe-LDH (Layered double hydroxides) layered double hydroxides [24]; (c) spinel compounds, such as CuCo2O4 [25]; (d) carbon-based materials, such as nitrogen doping carbon [26]; (e) nanocomposite materials mixing ORR catalyst Fe-N-C and OER catalyst NiFe [27].

2.2. Improving ORR and OER

The appropriate catalyst should be designed and applied to maximize catalytic efficiency. Metal-based catalysts possess high catalytic efficiencies due to different crystal structures. Spinel-type oxide (AxB3−xO4) [28] and perovskite oxides (ABO3) [29] are widely used as bifunctional electrocatalysts in alkaline electrolytes. Maiyalagan et al. [30] synthesized a spinel-type lithium cobalt oxide LiCoO2 at high-temperature (800 °C, LiCoO2-HT) and low-temperature LiCoO2-LT at 400 °C. LiCoO2-LT adopts a lithiated spinel structure [Li2]16c[Co2]16dO4 in which the Co3+ ions occupy all the 16d octahedral sites (space group: Fd3m) [31]. As shown in Figure 6a, LiCoO2-HT has the α-NaFeO2 structure (space group: R3m) arrays. Li+ ions and Co3+ ion occupy on alternate (111) NaFeO2-style structure arrays, due to the large size and charge differences between the Li+ and Co3+ ions [32]. In Figure 6b, it is obvious that HT-LCoO2 has a better catalytic performance than LT-LiCoO2 and Co3O4.
Catalysts are preferred at nanoscale for better catalytic behavior. By using a vacuum DC arc method, Lang et al. [33] synthesized a novel Mn3O4/MnO nano spherical transition metal compound. The results showed that the size of Mn3O4/MnO particles was controlled at a range of 40 to 60 nm. The Mn3O4/MnO catalyst potential platform reaches to 2.7 V.
Nanoscale catalysts can also be fabricated with various other morphologies, such as nano-rod LaCoO3 [34], 3D ordered mesoporous structure Co3O4 [35], hollow cobalt oxide nanoparticles [36]. Different morphologies of catalysts are shown in Figure 7. Many low-cost and efficient catalysts have been developed, including transition metals and nitrogen co-doped carbons (M-N/C, M=Fe or Co) [25], metal oxides [37], transition metal carbides [38], nitrides [39], and metal-free heteroatom-doped carbon-based catalysts [40]. Compared to metal-contained catalysts, the heteroatom-doped carbon-based materials with N, S, B, and P, can promote oxygen adsorption on the carbon nanostructure since these hetero-atoms are more electronegative than carbon, and cause neighboring carbon atoms electron deficiency [41]. Among them, N-doped carbons are extensively studied due to their remarkable ORR catalytic activity. N-doped carbon materials are shown in four ways, graphitic N, Oxidized N, pyrrolic N, and pyridic N in Figure 8.
Although several materials have shown catalytic activity for oxygen reaction in MABs cathodes, the catalytic efficiency is not ideal when used alone. To improve comprehensive catalyst performance, composition materials have been synthesized and used as catalysts in both ORR and OER. MnO2 and RuO2 are single catalysts for ORR and OER, respectively. Combining MnO2 with RuO2 is used as a bifunctional catalyst. Sun et al. [42] synthesized RuO2 nanoparticles (np-RuO2/nr-MnO2) supported on MnO2 nanorods by a two-step hydrothermal reaction. Electrochemical characterizations are carried on nanocomposites np-RuO2/nr-MnO2 as catalysts for LABs. Charge–discharge tests showed a reversible discharge capacity of 500 mAh g−1 for 75 cycles at a current density of 50 mA g−1. LABs with the RuO2/MnO2 catalyst presented much lower overpotential of 0.58 V at 50 mA g−1 than that measured with a single catalyst. ORR and OER electrocatalytic activity were tested by using rotating disk electrodes. It was found that np-RuO2/nr-MnO2 ORR limitation diffusion current was 6.01 mA cm−2, and ORR half-wave potential (E1/2) was −0.158 V. These results demonstrated that an np-RuO2 and nr-MnO2 combination can work as an effective catalyst for LABs with high activity while maintaining batteries stability.

2.3. In Situ Characterization Using an Electron Microscope

An in situ electron microscope is a promising tool for scientific research due to real-time observation and plays a major role in many MAB studies, such as the catalytic mechanism, the oxidation–reduction mechanism, the growth of nanostructures, and the deformation of electrodes. Based on the distinctive features of the preceding, Katharine et al. [43] found that higher Coulombic efficiency and more homogeneous morphology of the Li deposits in a coin-cell contributed to the presence of a compressed lithium separator interface through in situ electrochemical-scanning transmission microscope (EC-STEM), compared with a macroscale cell. In addition, Yoon et al. [44] used in situ atomic force microscope (AFM) to measure the dominant wavelength of the wrinkled surface topography. The planes strain modulus of the SEI was determined from the measured wavelength. Li et al. [45] explored the reaction mechanism and unveiled that α-MoO3 converted to crystalline Li2MoO3 in the first stage of lithiation, and further converted to metallic Mo and amorphous Li2O in the next stage. As shown in Figure 9a, with a negative potential to the Au/MnO2 nanowires (NWs), bubble-like NaO2 nucleated on the contact where the Au/MnO2 NW and Na2O intersects, then grows along the NW, resulting in 18 times volume increase. Meanwhile, the discharge product shrinks as a result of the disproportionation of NaO2 to Na2O2 and O2, confirming the occurrence of ORR [46]. Similarly, Liu et al. [47] also reported the real-time observation of ORR in Figure 9b. In this research, CuO nanowires (NWs), as the air cathode, firstly converted to Cu2O and then to Cu, as a metal catalyst to accelerate the disproportionation of NaO2 to Na2O2 and O2. During the reaction process, the morphological changes were investigated by an electrochemical atomic force microscope. Liu et al. [48] used EC-AFM to observe the dynamic process of Li2O2 growth/decomposition during the ORR/OER on a gold electrode in Figure 9c and found that the Li2O2 decomposed at a lower potential due to electrochemically generated TTF+ through a homogeneous oxidation mechanism.

3. Anodes

The chemical activity of the metal anode determines the discharge capacity. Because of high metal activity, an unavoidable side reaction with various components in the electrolyte may occur. Depending on the purity of the metal, the battery performance and the incidence of side reactions can be different.

3.1. Anode Materials: High Purity Metal and Alloy

Fan et al. [49] took industrial 5 N Al (99.999% high purity) and aluminum alloy (1050, 2011, 3003, 4032, 5052, 6061, 7050, and 8011) as anodes for AABs in alkaline electrolytes, using the hydrogen collection method and electrochemical impedance spectroscopy (EIS) to determine the corrosion behaviors, electrochemical properties, and potentiodynamic polarization. Test results of corrosion and EIS showed the sample in 4 M KOH was more suitable than in 4 M NaOH. Al 8011 had a transfer resistance (Rt) of 1.247 Ω cm2 in 4 M NaOH and 1.108 Ω cm2 in 4 M KOH. 5 N Al had Rt of 2.29 Ω cm2 in 4 M NaOH and 15.3 Ω cm2 in 4 M KOH. 5 N Al had 1.699 V Ecorr in 4M NaOH and 1.821 V Ecorr in 4M KOH. All industrial Al alloy anodes had the hydrogen adsorption phenomenon of hydrogen evolution reaction, and 8011 had relatively better performance than the others. As shown in Table 1, Al 8011 had a lower corrosion potential (Ecorr) at −1.42 V, corrosion current (Icorr), of 135 mA cm−2, and polarization resistance (Rp) of 3.628 Ωcm2 among industrial Al alloys. Therefore, impurity elements had different roles in the corrosion behaviors. Mg, Mn, Cr, Ti, and Zn were helpful to improve the corrosion resistance of Al alloy anodes, while Fe, Cu, and Si formed cathodic sites and lowered overpotential for hydrogen evolution reaction (HER) [49,50,51]. Different components Al alloys (Zn-rich and Al-rich phases) worked as abode AABs anode. Test results showed Al-rich alloys were better performance, due to lower the anodic passivation. Zn-Al alloys are promising anode materials as primary and mechanical-rechargeable Zn-air batteries [52].

3.2. Metal Coating and Composite Electrodes

Different from previous research using Al alloy as anodes, Mutlu [53] investigated Cu coating on Al and 7075 Al alloy as anodes. Copper was deposited on the Al surface by chemical (Al or Alloy/Cu-CD) and electrochemical (Al or Alloy/Cu-ED) processes, SEM images are shown in the Figure 10a,b. Al has a lower resistance than Al-Cu alloy. EIS measurements showed that copper on the Al surface could decrease anodic potential and improve batteries performance as shown in Figure 10c,d. The solution–electrode interaction resistance (Rs) was increased by adding copper to aluminum because copper can form a protective layer against the corrosion on the aluminum–solution interface. Hang et al. [54] found that FeS can employ as an additive for the electrode to suppress hydrogen evolution and improve the cyclic performance of the Fe/C composite anode. FeS additive and the carbon component also strongly affected the redox behavior of iron. An electrode with FeS can promote the process (in the Figure 11) of Fe0 to Fe2++ and Fe2+ to Fe3+ at around −0.85 V (a1), −0.65 V (a2), respectively. Furthermore, there were also additional intermediate species which appeared around −0.97 V (a0). The discharge capacity of the electrode was significantly improved with adding 2 wt.% FeS, which was mainly because the incorporation of FeS in the electrode improved the adsorbed capability of S2− on the electrode surface, resulting in the easy breaking of the oxide layer. For HER at the anode in alkaline electrolyte, both molecular recombination and electrochemical desorption can be parallel steps in the overall process. The molecular recombination reaction will appreciably contribute to HER only when the current density is low, and the molecular hydrogen concentration at the liquid boundary layer is near to zero. Under these conditions, it has been indicated that the molecular recombination reaction is affected by S2− ion chemisorption.

3.3. Common Challenge of Metal Anode

The common issues with metallic anodes are corrosion, passivation, and dendrite formation. These mechanisms are displayed in Figure 12.
Corrosion: Corrosion is one of the major side reactions between metal and electrolyte, and its reaction can be expressed as follows:
M + (2 + x)H2O ⇌ 2M(OH) + H2
M + H2O ⇌ MOX + H2
Equations (19) and (20) evaluates the corrosion rate due to hydrogen evolution reaction (HER). For almost all MABs, the M/MO standard voltage was below that of the hydrogen revolution. Therefore, hydrogen evolution was spontaneously favored. The HER decreased metal anode Coulombic efficiency because it consumed electrons from the metal anode in the charge. Moreover, hydrogen diffusing into electrolyte leads to the increase of internal battery pressure and could result in an explosion.
Hydrogen evolution reaction: Hydrogen evolution reaction (HER) was a side reaction of metal electrodes during the charge–discharge of batteries. The specific working principle is shown in Equations (19) and (20). Metal releases electrons to the aqueous electrolyte system and hydrogen ions replace metal ions obtaining electron reduction in hydrogen. HER in MABs thus influences the rates of metal electrodes. Hydrogen overpotential decreases on the ZnO surface since the self-discharge rate reduced with increasing ZnO on the electrode surface [55]. Increasing overpotential of HER (decreased HER rate) can thus improve the charging efficiency. In addition, the corrosion and oxidation of Al in alkaline electrolytes depend on electrolyte properties, temperature, and purity [56]. Using ionic liquid or solid state electrolyte is an effective solution to reduce the HER rate, which has been confirmed in FABs [57]. An alloy as anodes replacing pure metal also reduced the corrosion rate, and additives, such as bismuth or sulfur, could minimize the corrosion of the iron electrode and the evolution of hydrogen [58].
Passivation layers: Passivation used to describe an electrode that could not be further discharged because an insulating film on its surface blocked migration of the discharge product. In MABs, LiOH, ZnO, and Al2O3 were passivation layers for corresponding systems. Soluble species formed at the air cathode will be reduced to a non-conductive layer on the metal surface. This a non-conductive layer increases the internal electrical resistance of the cell and prevents metal dissolution. The efficient method is to use porous electrodes to hinder the formation of passivation layers.
Dendritic formation and deformation: During the metal electrode cycling in an alkaline electrolyte, the metal anode releases ions during discharge and the metal ions re-deposit on the surface of the anode during charging. As a result, the metal electrode will gradually change shape, and its surface will become roughened with uneven thicknesses. Over several charge and discharge cycles, the uneven shape accumulates to form dendrites, causing the battery system to become unstable or short cut. Different approaches have been attempted to mitigate dendritic formation and deformation, such as coating the zinc metal and using non-reaction additives in the zinc electrode or electrolyte [59]. Lithium alloying with Na [60], Mg [61], Al [62] has been confirmed to effectively suppress the growth of dendritic Li.
In summary, passivation layers happen in AABs, ZABs, and LABs, dendritic structures form in ZABs, and LABs and FABs, and corrosion may occur in FABs, AABs, ZABs, and LABs. Different strategies are needed to address these issues.

4. Electrolytes

An electrolyte is a medium to transport ions and electrons to ensure the continued oxidation–reduction reaction. Electrolyte divided into four types: aqueous, non-aqueous, hybrid, and solid state, as shown in Figure 13.

4.1. Aqueous Electrolyte

Alkaline solutions (7 < pH ≤ 14): Alkaline electrolytes are the most applied electrolyte in aqueous-based MABs, because the ORR is more favorable with faster reaction kinetics and a lower overpotential, compared to acidic electrolytes. Alkaline electrolytes have a shortcoming that CO2 (from air atmosphere) reacts with electrolyte and forms a carbonate surrounding the cathode. The large amount of carbonate will block the porous structure of the positive electrode material and decrease cathode efficiency.
Neutral salt solution (pH = 7): Al alloy–air batteries can discharge in a neutral salt solution with a lower corrosion rate and higher activity than in an alkaline electrolyte.
Acidic solutions (2 ≤ pH < 7): Acidic electrolytes are rarely used in aqueous-based MABs because a large amount of H+ in solution could directly react with metal and reducing battery efficiency. Saidman et al. [63] reported Al-Zn alloy anode performance changed with various types of acids at the same concentration, pH, and operating temperature. Electrochemical test results indicted Al–Zn alloy in 0.5 M HCl was more negative than that in 0.5 M HAc: −1.02 V and −0.80 V, respectively.
Hybrid electrolyte: In Figure 14b,c, a novel type of aqueous FABs was equipped with an alkaline anode electrolyte (anolyte) and an acidic cathode electrolyte (catholyte). The anolyte and catholyte are separated by an alkali metallic ion (Li+ or Na+) solid-state electrolyte separator. The alkali metal ion serves as an ionic mediator to sustain the redox reactions at both the anode and cathode [64].

4.2. Non-Aqueous Electrolyte

Solid-state electrolyte: Solid-state electrolytes are different from aqueous electrolytes in dual characteristics of wettability and ion conduction. For MABs, aqueous electrolytes with an excellent wetting property at three-phase boundaries could be in full contact with the cathode. For a solid-based electrolyte, the three-phase interface reaction can be restricted by the poor wetting property of the “immobilized” electrolyte, thereby, interfacial transporting resistance of OH− may be remarkably higher than that of an aqueous system [65]. Alkaline gel electrolytes (AGEs), consisting of low molecular weight polymer and alkaline solutions have been developed to mitigate these issues for primary lithium–air batteries [66].
Ionic liquid electrolyte: Ionic liquids are non-aqueous liquid electrolytes, including two types of cations: large organic cations with organic/inorganic anions and alkali metal ions in an organic solvent, such as organic carbonates, ethers, and esters [67,68]. Lithium salt, such as LiPF6, LiAsF6, LiN(SO2CF3)2, and LiSO3CF3 are commonly used in LABs [69]. PYR14TFSI–TEGDME–LiCF3SO3 are also employed in LABs [70], consisting of LiCF3SO3 in tetraethylene glycol dimethyl ether (TEGDME) and pure PYR14TFSI. Ionic liquid electrolytes also face challenges because of the formation of carbonates, which consume the electrolyte and block the electrode pores. What is more, the understanding of the oxygen reaction in an ionic liquid is very limited. These hinder the practical application of ionic liquid electrolytes.
In summary, neutral salt solution, acidic solutions, and hybrid electrolyte are rarely used in industrial application. Alkaline solutions electrolytes and ionic liquid electrolyte are usually employed. Aqueous electrolytes do not match LABs. Furthermore, solid-state electrolytes can work in all MABs.

5. Advanced Manufacturing of MABs

Advanced manufacturing techniques for electrodes and batteries is composed of printing and laser processing. Printing technology has various advantages in microstructure controlling and large batch low-cost fabrication. Printing includes screen printing [71], spray printing [72], direct ink writing processing [73], and roll-to-roll fabrication, as shown in Figure 15. Figure 16 shows printed 1- to 4D structures. 3D and 4D printing are achieved by layer-to-layer printing of functional micro/nanomaterials in geometric and temporal complexes.
Screen printing is one popular and simple method among printing technologies. During screen printing, the ink is pressed through a patterned screen onto the substrate using a roller and forms a film with the structures defined by the patterned screen. Spray printing injects particles from a solution and can easily fabricate large area sheets with a non-contact mode. Meanwhile, direct ink writing using a nozzle can feasibly form a 2D–3D structure with a certain thickness on the substrate. Therefore, different printing technologies can be applied to various battery electrodes.

5.1. Spray Coating and 2D Printing

Spray coating is a traditional coating method to fabricate composites by depositing particles onto the substrate surface. According to the working mechanism, spray can be divided into two types, cold spray and thermal spray. Thermal spray delivers melted metal drops or non-metal particles at high temperatures and forms a coat on the substrate [74]. Thermal spray has relatively wide applications in metal or alloy materials processing, such as surface coating and corrosion resistance. In contrast to thermal spray, cold spray without heating is a coating process to accelerate particles using the supersonic driving gas passing through a convergent–divergent nozzle and subsequently ejected onto a substrate in high speed [75]. Cold spray enables the delivery of various materials, including high melting point metal materials, low melting point polymer materials, even biomaterials. Helfritch [76] reviewed 24 new applications of cold spray, such as medical devices, electronics, microdevices, and so on.
Printing is another advanced manufacturing method, including inkjet printing, lithography, 3D printing, 4D printing. In this section, we will first discuss lithography and inkjet 2D printing. Inkjet printing [77,78] is additive manufacturing and appears after screen-printing and spin coating. The principle of inkjet printing consists of five stages: drop ejection, drop flight, drop impact, drop spreading, and drop solidification. Inkjet printing has been used in depositing functional inks onto various substrates for numerical devices, to specific, sensors, micro-batteries, solar cell, and other conductive parts of cells [79,80,81,82]. Lim [83] thoroughly reviewed technology issues and influence on different substrates for printed capacitive sensors. Furthermore, since Mirkin [84] reported “Dip-pen nanolithography” (DPN) in science, lithography became the focus of contemporary microfabrication. A DPN system is composed of an atomic force microscope tip as a “nib”, solid-state substrate as “paper”, and molecules with a chemical affinity for the solid-state substrate “ink”. By controlling the AFM tip, the nib directly writes controlled patterns on the substrate materials. Lithography contributes to microfabrication in nanomaterials and micro-devices, such as micro-reactors and sensors, micro-optical system [85,86,87,88]. Shao [89] reported nanoimprint lithography in the processing of flexible electronics, conductive electrodes, optoelectronic devices, flexible microlens, and flexible sensors. Certainly, it is feasible to print electrodes with a thin-film structure for metal–air batteries.

5.2. Laser Processing

Laser processing has gained more and more attention in recent years. Laser ablation, laser cutting, laser welding, laser sintering, laser direct writing, and other laser-assisted synthesis process are powerful tools for precise manufacturing [90,91]. For microfabrication, laser ablation is used to fabricate porous graphene and graphene quantum dots. Laser power, spot size diameter, hatch distance, scanning speed, wavelength, had an influence on the formation of nanomaterials and nanostructures [92,93]. Lasers can be applied for sintering various materials including metals, ceramics, and polymers [94,95,96]. In recent years, laser processing has been employed in the fabrication of electrodes [97], supercapacitors [98,99], even full batteries [100]. Successful micromanufacturing includes laser-drilling of microholes in LiFePO4 cathode for Li-ion batteries [101] and laser carbonization anode (graphene) for an interdigital film battery [102]. Li [6] reported femtosecond laser-reduced nano joined graphene oxide/Au conductive network as micro-supercapacitors electrodes. Pröll [103] reported femtosecond-laser structuring of LiMn2O4 composite cathodes for Li-ion micro-batteries.
Yu [3] reported laser sintering of printed anodes for AABs. Results indicated that laser sintering can remove the organic solvent from the printed Al nanoparticle slurry and increase the conductivity of the printed anode. Electrochemical characterization demonstrated laser power of 10 W for sintering for better performance, and 3-layer printed anode with a bigger discharge capacity. A 3-layer battery cell can yield a 239 mAh g−1 discharge capacity at an operation voltage of 0.95 V, as shown in Figure 17.

5.3. 3D Printing

Traditional thin film 2D batteries have suffered from limited energy capacity. 3D printing of flexible micro-batteries with nanostructures can overcome this weakness. Currently, the printed parts of batteries can be electrodes, current collector, solid-state separator, and catalyst in metal–air batteries [104]. Zhou [105] reviewed 3D printing energy storage devices with a sandwich-type and in-plane architecture and demonstrated that the electrochemical energy storage systems can be greatly promoted with 3D printing. Lewis et al. [106,107] reported 3D fully printed electrodes for Li-ion batteries. Li4Ti5O12 (LTO) and LiFePO4 (LFP) were separately employed as anode and cathode materials. Electrode material inks were printed onto the substrate, forming multilayer electrodes and an anode and cathode in an interdigitated structure. The results showed that the charge and discharge of 8-layer full cell delivered 1.2 mAh cm−2 at a rate of 0.5 C. EIS test revealed the thicker electrode had higher resistance. Meanwhile, CV testing showed the thin wall displayed broader redox peaks. Furthermore, both thin and thick electrodes exhibit excellent Coulombic efficiencies. 3D printed LIBs had 4.45 mAh cm−2 at 0.14 mA cm−2, corresponding a full cell delivering 14.5 mAh cm−2 at 0.2 mA cm−2. The same printed technology can also be employed for MABs. For MABs, screen printing has been used in catalysts [108]. A remarkable shortcoming is the narrow choice of suitable materials for printing. In addition, expensive equipment also limits application. However, 3D printing is the destructive technology in MAB manufacturing due to unprecedented designing freedom, high precision, and cost-effective processing.

6. Summary and Outlook

In summary, this paper briefly reviewed the recent advances in the studies of the metal–air batteries. Better batteries should be an excellent combination of cathode, anode, and electrolyte., however, there are still some problems to be solved, such as anode side reaction, impure gas CO2 release, electrolyte instability, and so on.
Essentially, improving ORR and OER are quite important to the cathode. Crystallographic structure, materials size, materials morphology, carbon-based materials-doped, and composites can influence different activities of catalyst, which is required to improve both ORR and OER in the cathode.
Nanocomposites and doped-carbon materials are good choices for catalysts in ORR and OER. Research indicates that compared with traditional alloy as an anode, alloys with nanocomposites can reduce the side reaction and improve discharge capacity. While various electrolytes have different advantages more efficient solid-state electrolyte is required in rechargeable metal–air batteries.
Integration of advanced manufacturing, especially 3D printing and laser processing, opens new horizons for MABs. These manufacturing processes allow a better strategy for the systematic combination of the best performance of anodes, cathodes, and electrolyte for improved energy density, efficiency, and cycling stabilities. Although many issues still exist, the further development of MABs, as a compelling alternative to LIBs, holds great promise to address emergent needs of portable electronics, electrical vehicles, and IoTs.

Author Contributions

C.W. is responsible for the reference survey, analysis, figure preparation and manuscript drafting. Y.Y. contributes to the laser processing section. J.N., X.L., Y.Z. contribute to the section of “in situ characterization using an electron microscope”. Y.L., D.B., J.P. are responsible for the revision of the paper. A.H. advises the review structures, revises the logic order of the chapters and polishes the final manuscript.

Funding

This work is partially supported by the National Natural Science Foundation of China (51575016) and NSFC-DFG joint project (51761135129).

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Gür, T.M. Review of electrical energy storage technologies, materials and systems: Challenges and prospects for large-scale grid storage. Energy Environ. Sci. 2018, 11, 2696–2767. [Google Scholar] [CrossRef]
  2. Li, S.; Guo, Z.P.; Wang, C.Y.; Wallace, G.G.; Liu, H.K. Flexible cellulose based polypyrrole–multiwalled carbon nanotube films for bio-compatible zinc batteries activated by simulated body fluids. J. Mater. Chem. A 2013, 1, 14300–14305. [Google Scholar] [CrossRef]
  3. Yu, Y.; Chen, M.; Wang, S.; Hill, C.; Joshi, P.; Kuruganti, T.; Hu, A. Laser sintering of printed anodes for al-air batteries. J. Electrochem. Soc. 2018, 165, A584–A592. [Google Scholar] [CrossRef]
  4. Jeżowski, P.; Crosnier, O.; Deunf, E.; Poizot, P.; Béguin, F.; Brousse, T. Safe and recyclable lithium-ion capacitors using sacrificial organic lithium salt. Nat. Mater. 2018, 17, 167. [Google Scholar] [CrossRef] [PubMed]
  5. Jeżowski, P.; Fic, K.; Crosnier, O.; Broussebc, T.; Béguin, F. Lithium rhenium (vii) oxide as a novel material for graphite pre-lithiation in high performance lithium-ion capacitors. J. Mater. Chem. A 2016, 4, 12609–12615. [Google Scholar] [CrossRef]
  6. Li, R.-Z.; Peng, R.; Kihm, K.D.; Bai, S.; Bridges, D.; Tumuluri, U.; Wu, Z.; Zhang, T.; Compagnini, G.; Feng, Z. High-rate in-plane micro-supercapacitors scribed onto photo paper using in situ femtolaser-reduced graphene oxide/Au nanoparticle microelectrodes. Energy Environ. Sci. 2016, 9, 1458–1467. [Google Scholar]
  7. Jeżowski, P.; Fic, K.; Crosnier, O.; Brousse, T.; Béguin, F. Use of sacrificial lithium nickel oxide for loading graphitic anode in Li-ion capacitors. Electrochim. Acta 2016, 206, 440–445. [Google Scholar]
  8. Pellow, M.A.; Emmott CJ, M.; Barnhart, C.J.; Benson, S.M. Hydrogen or batteries for grid storage? A net energy analysis. Energy Environ. Sci. 2015, 8, 1938–1952. [Google Scholar] [CrossRef] [Green Version]
  9. Zhang, X.; Wang, X.G.; Xie, Z.; Zhou, Z. Recent progress in rechargeable alkali metal–air batteries. Green Energy Environ. 2016, 1, 4–17. [Google Scholar] [CrossRef]
  10. McKerracher, R.D.; Ponce de Leon, C.; Wills RG, A.; Shah, D.A.A.; Walsh, P.F.C. A review of the iron–air secondary battery for energy storage. ChemPlusChem 2015, 80, 323–335. [Google Scholar] [CrossRef]
  11. Zhang, Z.; Zuo, C.; Liu, Z.; Yu, Y.; Zuo, Y.; Song, Y. All-solid-state Al–air batteries with polymer alkaline gel electrolyte. J. Power Sources 2014, 251, 470–475. [Google Scholar] [CrossRef]
  12. Li, Y.; Dai, H. Recent advances in zinc–air batteries. Chem. Soc. Rev. 2014, 43, 5257–5275. [Google Scholar] [CrossRef] [PubMed]
  13. Wang, Y.; Kwok, H.; Pan, W.; Zhang, H.; Leung, D.Y.C. Innovative paper-based Al-air batteries as a low-cost and green energy technology for the miniwatt market. J. Power Sources 2019, 414, 278–282. [Google Scholar] [CrossRef]
  14. Wu, D.; Guo, Z.; Yin, X.; Pang, Q.; Tu, B.; Zhang, L.; Wang, Y.; Li, Q. Metal–organic frameworks as cathode materials for Li–O2 batteries. Adv. Mater. 2014, 26, 3258–3262. [Google Scholar] [CrossRef] [PubMed]
  15. Cheng, F.; Chen, J. Metal–air batteries: From oxygen reduction electrochemistry to cathode catalysts. Chem. Soc. Rev. 2012, 41, 2172–2192. [Google Scholar] [CrossRef] [PubMed]
  16. Cheng, J.; Zhang, L.; Yang, Y.S.; Wen, Y.-H.; Cao, G.-P.; Wang, X.-D. Preliminary study of single flow zinc–nickel battery. Electrochem. Commun. 2007, 9, 2639–2642. [Google Scholar] [CrossRef]
  17. Fu, J.; Zhang, J.; Song, X.; Zarrin, H.; Tian, X.; Qiao, J.; Rasen, L.; Li, K.; Chen, Z. A flexible solid-state electrolyte for wide-scale integration of rechargeable zinc–air batteries. Energy Environ. Sci. 2016, 9, 663–670. [Google Scholar] [CrossRef]
  18. Zhou, G.; Li, F.; Cheng, H.M. Progress in flexible lithium batteries and future prospects. Energy Environ. Sci. 2014, 7, 1307–1338. [Google Scholar] [CrossRef]
  19. Sumboja, A.; Ge, X.; Zong, Y.; Liu, Z.P. Rogress in development of flexible metal–air batteries. Funct. Mater. Lett. 2016, 9, 1630001. [Google Scholar] [CrossRef]
  20. Gu, P.; Zheng, M.; Zhao, Q.; Xiao, X.; Xuea, H.; Pang, H. Rechargeable zinc–air batteries: A promising way to green energy. J. Mater. Chem. A 2017, 5, 7651–7666. [Google Scholar] [CrossRef]
  21. Guo, S.; Zhang, S.; Sun, S. Tuning nanoparticle catalysis for the oxygen reduction reaction. Ang. Chem. Int. Edit. 2013, 52, 8526–8544. [Google Scholar] [CrossRef] [PubMed]
  22. Jörissen, L. Bifunctional oxygen/air electrodes. J. Power Sources 2006, 155, 23–32. [Google Scholar] [CrossRef]
  23. Cao, R.; Lee, J.S.; Liu, M.; Cho, J. Recent progress in non-precious catalysts for metal-air batteries. Adv. Energy Mater. 2012, 2, 816–829. [Google Scholar] [CrossRef]
  24. Qian, L.; Lu, Z.; Xu, T.; Wu, X.; Tian, Y.; Li, Y.; Huo, Z.; Sun, X.; Duan, X. Trinary layered double hydroxides as high-performance bifunctional materials for oxygen electrocatalysis. Adv. Energy Mater. 2015, 5, 1500245. [Google Scholar] [CrossRef]
  25. Liu, Y.; Cao, L.J.; Cao, C.W.; Wang, M.; Leung, K.-L.; Zeng, S.-S.; Hung, T.F.; Chung, C.Y.; Lu, Z.-G. Facile synthesis of spinel CuCo2O4 nanocrystals as high-performance cathode catalysts for rechargeable Li–air batteries. Chem. Commun. 2014, 50, 14635–14638. [Google Scholar] [CrossRef]
  26. Han, X.; Wu, X.; Zhong, C.; Deng, Y.; Zhao, N.; Hu, W. NiCo2S4 nanocrystals anchored on nitrogen-doped carbon nanotubes as a highly efficient bifunctional electrocatalyst for rechargeable zinc-air batteries. Nano Energy 2017, 31, 541–550. [Google Scholar] [CrossRef]
  27. Dresp, S.; Luo, F.; Schmack, R.; Kühl, S.; Gliecha, M.; Strasser, P. An efficient bifunctional two-component catalyst for oxygen reduction and oxygen evolution in reversible fuel cells, electrolyzers and rechargeable air electrodes. Energy Environ. Sci. 2016, 9, 2020–2024. [Google Scholar] [CrossRef] [Green Version]
  28. Indra, A.; Menezes, P.W.; Sahraie, N.R.; Bergmann, A.; Das, C.; Tallarida, M.; Schmeißer, D.; Strasser, P.; Driess, M. Unification of catalytic water oxidation and oxygen reduction reactions: Amorphous beat crystalline cobalt iron oxides. J. Am. Chem. Soc. 2014, 136, 17530–17536. [Google Scholar] [CrossRef]
  29. Yamada, I.; Fujii, H.; Takamatsu, A.; Ikeno, H.; Wada, K.; Tsukasaki, H.; Kawaguchi, S.; Mori, S.; Yagi, S. Bifunctional oxygen reaction catalysis of quadruple manganese Perovskites. Adv. Mater. 2017, 29, 1603004. [Google Scholar] [CrossRef]
  30. Maiyalagan, T.; Jarvis, K.A.; Therese, S.; Ferreira, P.J.; Manthiram, A. Spinel-type lithium cobalt oxide as a bifunctional electrocatalyst for the oxygen evolution and oxygen reduction reactions. Nat. Commun. 2014, 5, 3949. [Google Scholar] [CrossRef] [Green Version]
  31. Gummow, R.J.; Thackeray, M.M.; David, W.I.F.; Hull, S. Structure and electrochemistry of lithium cobalt oxide synthesised at 400 °C. Mater. Res. Bull. 1992, 27, 327–337. [Google Scholar] [CrossRef]
  32. Gummow, R.J.; Liles, D.C.; Thackeray, M.M. Spinel versus layered structures for lithium cobalt oxide synthesised at 400 °C. Mater. Res. Bull. 1993, 28, 235–246. [Google Scholar] [CrossRef]
  33. Lang, X.; Ge, F.; Cai, K.; Lan Li Wang, Q.; Zhang, Q. A novel Mn3O4/MnO nano spherical transition metal compound prepared by vacuum direct current arc method as bi-functional catalyst for lithium-oxygen battery with excellent electrochemical performances. J. Alloy. Compd. 2019, 770, 451–457. [Google Scholar] [CrossRef]
  34. Shin, B.; Choi, S.; Tak, Y. Electrocatalytic activity of Co-based perovskite oxides for oxygen reduction and evolution reactions]. Int. J. Electrochem. Sci. 2016, 11, 5900. [Google Scholar] [CrossRef]
  35. Park, M.G.; Lee, D.U.; Seo, M.H.; Cano, Z.P.; Chen, Z. 3D ordered mesoporous bifunctional oxygen catalyst for electrically rechargeable zinc–air batteries. Small 2016, 12, 2707–2714. [Google Scholar] [CrossRef] [PubMed]
  36. Tian, Y.; Xu, L.; Bao, J.; Qian, J.; Su, H.; Li, H.; Gu, H.; Yan, C.; Li, H. Hollow cobalt oxide nanoparticles embedded in nitrogen-doped carbon nanosheets as an efficient bifunctional catalyst for Zn–air battery. J. Energy Chem. 2019, 33, 59–66. [Google Scholar] [CrossRef]
  37. Osgood, H.; Devaguptapu, S.V.; Xu, H.; Cho, J.; Wu, G. Transition metal (Fe, Co, Ni, and Mn) oxides for oxygen reduction and evolution bifunctional catalysts in alkaline media. Nano Today 2016, 11, 601–625. [Google Scholar] [CrossRef]
  38. Zhang, Y.; Jiang, W.J.; Guo, L.; Zhang, X.; Hu, J.-S.; Wei, Z.; Wan, L.-J. Confining iron carbide nanocrystals inside CNx@ CNT toward an efficient electrocatalyst for oxygen reduction reaction. ACS Appl. Mater. Inter. 2015, 7, 11508–11515. [Google Scholar] [CrossRef]
  39. Wu, G.; Santandreu, A.; Kellogg, W.; Gupta, S.; Ogoke, O.; Zhang, H.; Wang, H.-L.; Dai, L. Carbon nanocomposite catalysts for oxygen reduction and evolution reactions: From nitrogen doping to transition-metal addition. Nano Energy 2016, 29, 83–110. [Google Scholar] [CrossRef] [Green Version]
  40. Wang, L.; Liang, K.; Deng, L.; Liu, Y.-N. Protein hydrogel networks: A unique approach to heteroatom self-doped hierarchically porous carbon structures as an efficient ORR electrocatalyst in both basic and acidic conditions. Appl. Catal. B Environ. 2019, 246, 89–99. [Google Scholar] [CrossRef]
  41. Zhou, N.; Wang, N.; Wu, Z.; Li, L. Probing Active Sites on Metal-Free, Nitrogen-Doped Carbons for Oxygen Electroreduction: A Review. Catalysts 2018, 8, 509. [Google Scholar] [CrossRef]
  42. Xu, Y.F.; Chen, Y.; Xu, G.L.; Zhang, X.-R.; Chen, Z.; Li, J.-T.; Huang, L.; Amine, K.; Sun, S.-G. RuO2 nanoparticles supported on MnO2 nanorods as high efficient bifunctional electrocatalyst of lithium-oxygen battery. Nano Energy 2016, 28, 63–70. [Google Scholar] [CrossRef]
  43. Harrison, K.L.; Zavadil, K.R.; Hahn, N.T.; Meng, X.; Elam, J.W.; Leenheer, A.; Zhang, J.-G.; Jungjohann, K.L. Lithium self-discharge and its prevention: Direct visualization through in situ electrochemical scanning transmission electron microscopy. ACS Nano 2017, 11, 11194–11205. [Google Scholar] [CrossRef] [PubMed]
  44. Yoon, I.; Jurng, S.; Abraham, D.P.; Lucht, B.L.; Guduru, P.R. In Situ Measurement of the Plane-Strain Modulus of the Solid Electrolyte Interphase on Lithium-Metal Anodes in Ionic Liquid Electrolytes. Nano Lett. 2018, 18, 5752–5759. [Google Scholar] [CrossRef] [PubMed]
  45. Li, Y.; Sun, H.; Cheng, X.; Zhang, Y.; Zhao, K. In-situ TEM experiments and first-principles studies on the electrochemical and mechanical behaviors of α-MoO3 in Li-ion batteries. Nano Energy 2016, 27, 95–102. [Google Scholar] [CrossRef]
  46. Liu, Q.; Geng, L.; Yang, T.; Tang, Y.; Jia, P.; Li, Y.; Li, H.; Shen, T.; Zhang, L.; Huang, J. In-situ imaging electrocatalysis in a Na-O2 battery with Au-coated MnO2 nanowires air cathode. Energy Storage Mater. 2019, 19, 48–55. [Google Scholar] [CrossRef]
  47. Liu, Q.; Yang, T.; Du, C.; Tang, Y.; Sun, Y.; Jia, P.; Chen, J.; Ye, H.; Shen, T.; Peng, Q.; et al. In Situ Imaging the Oxygen Reduction Reactions of Solid State Na–O2 Batteries with CuO Nanowires as the Air Cathode. Nano Lett. 2018, 18, 3723–3730. [Google Scholar] [CrossRef] [PubMed]
  48. Liu, C.; Ye, S. In situ atomic force microscopy (AFM) study of oxygen reduction reaction on a gold electrode surface in a dimethyl sulfoxide (DMSO)-Based electrolyte solution. J. Phys. Chem. C 2016, 120, 25246–25255. [Google Scholar] [CrossRef]
  49. Fan, L.; Lu, H.; Leng, J.; Sun, Z.; Chen, C. The study of industrial aluminum alloy as anodes for aluminum-air batteries in alkaline electrolytes. J. Electrochem. Soc. 2016, 163, A8–A12. [Google Scholar] [CrossRef]
  50. Cho, Y.J.; Park, I.J.; Lee, H.J.; Kim, J.-G. Aluminum anode for aluminum–air battery–Part I: Influence of aluminum purity. J. Power Sources 2015, 277, 370–378. [Google Scholar] [CrossRef]
  51. Park, I.J.; Choi, S.R.; Kim, J.G. Aluminum anode for aluminum-air battery–Part II: Influence of In addition on the electrochemical characteristics of Al-Zn alloy in alkaline solution. J. Power Sources 2017, 357, 47–55. [Google Scholar] [CrossRef]
  52. Lan, C.J.; Chin, T.S.; Lin, P.H.; Perng, T.P. Zn-Al alloy as a new anode-metal of a zinc-air battery. J. New Mater. Electrochem. Syst 2006, 9, 27–32. [Google Scholar]
  53. Mutlu, R.N. Copper-deposited aluminum anode for aluminum-air battery. J. Solid State Electrochem. 2019, 23, 529–541. [Google Scholar] [CrossRef]
  54. Hang, B.T.; Watanabe, T.; Egashira, M.; Watanabe, I.; Okada, S.; Yamaki, J.-I. The effect of additives on the electrochemical properties of Fe/C composite for Fe/air battery anode. J. Power Sources 2006, 155, 461–469. [Google Scholar] [CrossRef]
  55. Lee, C.W.; Eom, S.W.; Sathiyanarayanan, K.; SooYun, M. Preliminary comparative studies of zinc and zinc oxide electrodes on corrosion reaction and reversible reaction for zinc/air fuel cells. Electrochim. Acta 2006, 52, 1588–1591. [Google Scholar] [CrossRef]
  56. Zhao, Y.; VanderNoot, T.J. Electrodeposition of aluminium from room temperature AlCl3-TMPAC molten salts. Electrochim. Acta 1997, 42, 1639–1643. [Google Scholar] [CrossRef]
  57. Zhao, X.; Xu, N.; Li, X.; Huang, K. Energy storage characteristics of a new rechargeable solid oxide iron–air battery. RSC Adv. 2012, 2, 10163. [Google Scholar] [CrossRef]
  58. Ponrouch, A.; Frontera, C.; Bardé, F.; Palacín, M.R. Towards a calcium-based rechargeable battery. Nat. Mater. 2016, 15, 169. [Google Scholar] [CrossRef]
  59. Lee, S.M.; Kim, Y.J.; Eom, S.W.; Choi, N.-S.; Kim, K.-W.; Cho, S.-B. Improvement in self-discharge of Zn anode by applying surface modification for Zn–air batteries with high energy density. J. Power Sources 2013, 227, 177–184. [Google Scholar] [CrossRef]
  60. Stark, J.K.; Ding, Y.; Kohl, P.A. Dendrite-free electrodeposition and reoxidation of lithium-sodium alloy for metal-anode battery. J. Electrochem. Soc. 2011, 158, A1100–A1105. [Google Scholar] [CrossRef]
  61. Yoon, S.; Lee, J.; Kim, S.O.; Sohn, H.-J. Enhanced cyclability and surface characteristics of lithium batteries by Li–Mg co-deposition and addition of HF acid in electrolyte. Electrochim. Acta 2008, 53, 2501–2506. [Google Scholar] [CrossRef]
  62. Ishikawa, M.; Machino, S.; Morita, M. Electrochemical control of a Li metal anode interface: Improvement of Li cyclability by inorganic additives compatible with electrolytes. J. Electroanal. Chem. 1999, 473, 279–284. [Google Scholar] [CrossRef]
  63. Smoljko, I.; Gudić, S.; Kuzmanić, N.; Kliškić, M. Electrochemical properties of aluminium anodes for Al/air batteries with aqueous sodium chloride electrolyte. J. Appl. Electrochem. 2012, 42, 969–977. [Google Scholar] [CrossRef]
  64. Yu, X.; Manthiram, A. A Voltage-Enhanced, Low-Cost Aqueous Iron–Air Battery Enabled with a Mediator-Ion Solid Electrolyte. ACS Energy Lett. 2017, 2, 1050–1055. [Google Scholar] [CrossRef]
  65. Wang, Y.J.; Qiao, J.; Baker, R.; Zhang, J. Alkaline polymer electrolyte membranes for fuel cell applications. Chem. Soc. Rev. 2013, 42, 5768–5787. [Google Scholar] [CrossRef]
  66. Li, F.; Kitaura, H.; Zhou, H. The pursuit of rechargeable solid-state Li–air batteries. Energy Environ. Sci. 2013, 6, 2302–2311. [Google Scholar] [CrossRef]
  67. Xu, K. Nonaqueous liquid electrolytes for lithium-based rechargeable batteries. Chem. Rev. 2004, 104, 4303–4418. [Google Scholar] [CrossRef]
  68. Mokhtar, M.; MeorTalib, M.Z.; Majlan, E.H.; Tasirin, S.M.; Ramli, W.M.F.W.; Daud, W.R.W.; Sahari, J. Recent developments in materials for aluminum–air batteries: A review. J. Ind. Eng. Chem. 2015, 32, 1–20. [Google Scholar] [CrossRef]
  69. Daming, G.; Yu, W.; Shuo, G.; Zhang, C. Research Progress and Optimization of Non-aqueous Electrolyte for Lithium Air Batteries. ACTA Chim. Sin. 2013, 71, 1354–1364. [Google Scholar] [Green Version]
  70. Cecchetto, L.; Salomon, M.; Scrosati, B.; Croce, F. Study of a Li–air battery having an electrolyte solution formed by a mixture of an ether-based aprotic solvent and an ionic liquid. J. Power Sources 2012, 213, 233–238. [Google Scholar] [CrossRef]
  71. Shaheen, S.E.; Radspinner, R.; Peyghambarian, N.; Jabbour, G.E. Fabrication of bulk heterojunction plastic solar cells by screen printing. Appl. Phys. Lett. 2001, 79, 2996–2998. [Google Scholar] [CrossRef]
  72. Gan, J.A.; Berndt, C.C. Nanocomposite coatings: Thermal spray processing, microstructure and performance. Int. Mater. Rev. 2015, 60, 195–244. [Google Scholar] [CrossRef]
  73. Yin, S.; Chen, C.; Suo, X.; Lupoi, R. Cold-Sprayed Metal Coatings with Nanostructure. Adv. Mater. Sci. Eng. 2018, 2018, 2804576. [Google Scholar] [CrossRef]
  74. Champagne, V.K.; Helfritch, D.J. Mainstreaming cold spray–push for applications. Surf. Eng. 2014, 30, 396–403. [Google Scholar] [CrossRef]
  75. Cummins, G.; Desmulliez, M.P.Y. Inkjet printing of conductive materials: A review. Circuit World 2012, 38, 193–213. [Google Scholar] [CrossRef]
  76. Li, R.Z.; Hu, A.; Zhang, T.; Oakes, K.D. Direct writing on paper of foldable capacitive touch pads with silver nanowire inks. ACS Appl. Mater. Interfaces 2014, 6, 21721–21729. [Google Scholar] [CrossRef] [PubMed]
  77. Sousa, R.E.; Costa, C.M.; Lanceros-Méndez, S. Advances and Future Challenges in Printed Batteries. ChemSusChem 2015, 8, 3539–3555. [Google Scholar] [CrossRef]
  78. Kim, H.J.; Kim, J.J.; Lee, J.K. Enhancement of the Surface Roughness by Powder Spray Coating on Zirconia Substrate. J. Nanosci. Nanotechnol. 2019, 19, 6285–6290. [Google Scholar] [CrossRef]
  79. Bonetti, I.; da Costa, C.E.; Paredes, R.S.C.; Paredes, R.S.C.; Sucharski, G.B.; da Costa, E.M.; Franco, E.; Milan, J.C.G. Effect of flame spray deposition parameters on the microstructure, microhardness and corrosion resistance of FeNbC coatings on AISI 1020 steel. Mater. Res. Express 2019, 6, 086530. [Google Scholar] [CrossRef]
  80. Lotya, M.; Hernandez, Y.; King, P.J.; Smith, R.J.; Nicolosi, V.; Karlsson, L.S.; Blighe, F.M.; De, S.; Wang, Z.; McGovern, I.T. Liquid phase production of graphene by exfoliation of graphite in surfactant/water solutions. J. Am. Chem. Soc. 2009, 131, 3611–3620. [Google Scholar] [CrossRef]
  81. Salim, A.; Lim, S. Review of recent inkjet-printed capacitive tactile sensors. Sensors 2017, 17, 2593. [Google Scholar] [CrossRef] [PubMed]
  82. Piner, R.D.; Zhu, J.; Xu, F.; Hong, S.; Mirkin, C.A. “Dip-pen” nanolithography. Science 1999, 283, 661–663. [Google Scholar] [CrossRef] [PubMed]
  83. Kelly, K.L.; Coronado, E.; Zhao, L.L.; Schatz, G.C. The optical properties of metal nanoparticles: The influence of size, shape, and dielectric environment. J. Phys. Chem. B 2003, 107, 668–677. [Google Scholar] [CrossRef]
  84. Mottay, E.; Liu, X.; Zhang, H.; Mazur, E. Industrial applications of ultrafast laser processing. MRS Bull. 2016, 41, 984–992. [Google Scholar] [CrossRef]
  85. Yu, Y.; Bai, S.; Wang, S.; Hu, A. Ultra-Short Pulsed Laser Manufacturing and Surface Processing of Microdevices. Engineering 2018, 4, 779–786. [Google Scholar] [CrossRef]
  86. Yu, Y.; Wang, S.; Ma, D.; Joshi, P.; Hu, A. Recent Progress on Laser Manufacturing of Microsize Energy Devices on Flexible Substrates. JOM 2018, 70, 1816–1822. [Google Scholar] [CrossRef]
  87. Shao, J.Y.; Chen, X.L.; Li, X.M.; Tian, H. Nanoimprint lithography for the manufacturing of flexible electronics. Sci. China Technol. Sci. 2019, 62, 175–198. [Google Scholar] [CrossRef]
  88. Hu, A.; Rybachuk, M.; Lu, Q.B.; Duley, W. Direct synthesis of sp-bonded carbon chains on graphite surface by femtosecond laser irradiation. Appl. Phys. Lett. 2007, 91, 131906. [Google Scholar] [CrossRef] [Green Version]
  89. Hu, A.; Li, R.; Bridges, D.; Zhou, W. Photonic nanomanufacturing of high performance energy devices on flexible substrates. J. Laser Appl. 2016, 28, 022602. [Google Scholar] [CrossRef]
  90. Hu, A.; Lu, Q.B.; Duley, W.W.; Rybachuk, M. Spectroscopic characterization of carbon chains in nanostructured tetrahedral carbon films synthesized by femtosecond pulsed laser deposition. J. Chem. Phys. 2007, 126, 154705. [Google Scholar] [CrossRef]
  91. Wang, S.; Yu, Y.; Li, R.; Feng, G.; Wu, Z.; Compagnini, G.; Gulino, A.; Feng, Z.; Hu, A. High-performance stacked in-plane supercapacitors and supercapacitor array fabricated by femtosecond laser 3D direct writing on polyimide sheets. Electrochim. Acta 2017, 241, 153–161. [Google Scholar] [CrossRef]
  92. Li, R.-Z.; Hu, A.; Bridges, D.; Zhang, T.; Oakes, K.D.; Peng, R.; Tumuluri, U.; Wue, Z.; Feng, Z. Robust Ag nanoplate ink for flexible electronics packaging. Nanoscale 2015, 7, 7368–7377. [Google Scholar] [CrossRef] [PubMed]
  93. Peng, P.; Hu, A.; Zhou, Y. Laser sintering of silver nanoparticle thin films: Microstructure and optical properties. Appl. Phys. A 2012, 108, 685–691. [Google Scholar] [CrossRef]
  94. Ma, Y.; Li, H.; Bridges, D.; Peng, P.; Lawrie, B.; Feng, Z.; Hu, A. Zero-dimensional to three-dimensional nanojoining: Current status and potential applications. RSC Adv. 2016, 6, 75916–75936. [Google Scholar] [CrossRef]
  95. Pfleging, W. A review of laser electrode processing for development and manufacturing of lithium-ion batteries. Nanophotonics 2018, 7, 549–573. [Google Scholar] [CrossRef]
  96. Gao, W.; Singh, N.; Song, L.; Liu, Z.; Reddy, A.L.M.; Ci, L.; Vajtai, R.; Zhang, Q.; Wei, B.; Ajayan, P.M. Direct laser writing of micro-supercapacitors on hydrated graphite oxide films. Nat. Nanotechnol. 2011, 6, 496. [Google Scholar] [CrossRef]
  97. Ma, D.L.; Ma, Y.; Chen, Z.W.; Hu, A.M. A silk fabric derived carbon fibre net for transparent capacitive touch pads and all-solid supercapacitors. J. Mater. Chem. A 2017, 5, 20608–20614. [Google Scholar] [CrossRef]
  98. Ohta, S.; Komagata, S.; Seki, J.; Saeki, T.; Morishita, S.; Asaoka, T. All-solid-state lithium ion battery using garnet-type oxide and Li3BO3 solid electrolytes fabricated by screen-printing. J. Power Sources 2013, 238, 53–56. [Google Scholar] [CrossRef]
  99. Tsuda, T.; Ando, N.; Nakamura, S.; Ishihara, Y.; Hayashi, N.; Soma, N.; Gunji, T.; Tanabe, T.; Ohsaka, T.; Matsumoto, F. Improvement of high-rate discharging performance of LiFePO4 cathodes by forming micrometer-sized through-holed electrode structures with a pico-second pulsed laser. Electrochim. Acta 2019, 296, 27–38. [Google Scholar] [CrossRef]
  100. Fu, K.; Wang, Y.; Yan, C.; Yao, Y.; Chen, Y.; Dai, J.; Lacey, S.; Wang, Y.; Wan, J.; Li, T. Graphene oxide-based electrode inks for 3D-printed lithium-ion batteries. Adv. Mater. 2016, 28, 2587–2594. [Google Scholar] [CrossRef]
  101. Pröll, J.; Kim, H.; Piqué, A.; Seifert, H.J.; Pfleging, W. Laser-printing and femtosecond-laser structuring of LiMn2O4 composite cathodes for Li-ion microbatteries. J. Power Sources 2014, 255, 116–124. [Google Scholar] [CrossRef]
  102. Ferrari, S.; Loveridge, M.; Beattie, S.D.; Jahn, M.; Dashwood, R.J.; Bhagat, R. Latest advances in the manufacturing of 3D rechargeable lithium microbatteries. J. Power Sources 2015, 286, 25–46. [Google Scholar] [CrossRef] [Green Version]
  103. Tian, X.; Jin, J.; Yuan, S.; Chua, C.K.; Tor, S.B.; Zhou, K. Emerging 3D-printed electrochemical energy storage devices: A critical review. Adv. Energy Mater. 2017, 7, 1700127. [Google Scholar] [CrossRef]
  104. Sun, K.; Wei, T.S.; Ahn, B.Y.; Seo, J.Y.; Dillon, S.J.; Lewis, J.A. 3D printing of interdigitated Li-Ion microbattery architectures. Adv. Mater. 2013, 25, 4539–4543. [Google Scholar] [CrossRef]
  105. Wei, T.S.; Ahn, B.Y.; Grotto, J.; Lewis, J.A. 3D Printing of Customized Li-Ion Batteries with Thick Electrodes. Adv. Mater. 2018, 30, 1703027. [Google Scholar] [CrossRef]
  106. Jung, C.Y.; Zhao, T.S.; An, L.; Wei, Z.H. Screen printed cathode for non-aqueous lithium–oxygen batteries. J. Power Sources 2015, 297, 174–180. [Google Scholar] [CrossRef]
  107. Zhao, C.; Wang, C.; Gorkin Iii, R.; Beirne, S.; Shu, K.; Wallace, G.G. Three dimensional (3D) printed electrodes for interdigitated supercapacitors. Electrochem. Commun. 2014, 41, 20–23. [Google Scholar] [CrossRef] [Green Version]
  108. Yang, Y.; Shi, M.; Zhou, Q.F.; Li, Y.-S.; Fu, Z.-W. Platinum nanoparticle–graphene hybrids synthesized by liquid phase pulsed laser ablation as cathode catalysts for Li-air batteries. Electrochem. Commun. 2012, 20, 11–14. [Google Scholar] [CrossRef]
Applsci 09 02787 g001 550
Figure 1. Applications of metal–air batteries as energy source and storage systems.
Figure 1. Applications of metal–air batteries as energy source and storage systems.
Applsci 09 02787 g001
Applsci 09 02787 g002 550
Figure 2. Theoretical specific energies, volumetric energy densities, and nominal battery voltages of various metal–air batteries (MABs) [9].
Figure 2. Theoretical specific energies, volumetric energy densities, and nominal battery voltages of various metal–air batteries (MABs) [9].
Applsci 09 02787 g002
Applsci 09 02787 g003 550
Figure 3. Schematic diagrams of MABs working principles for (a) non-aqueous electrolyte, and (b) aqueous electrolyte.
Figure 3. Schematic diagrams of MABs working principles for (a) non-aqueous electrolyte, and (b) aqueous electrolyte.
Applsci 09 02787 g003
Applsci 09 02787 g004 550
Figure 4. Schematic diagram of different MAB configurations: (a) multi-cell static configuration, (b) flow battery, and (c) flexible battery.
Figure 4. Schematic diagram of different MAB configurations: (a) multi-cell static configuration, (b) flow battery, and (c) flexible battery.
Applsci 09 02787 g004
Applsci 09 02787 g005 550
Figure 5. Various cathodic electrode of MABs, (A) metal current collector with a gas diffusion layer and coated catalyst facing electrolyte, (B) carbon-base current collector and gas diffusion and catalyst, (C) carbon paper-current collector and gas diffusion and catalyst.
Figure 5. Various cathodic electrode of MABs, (A) metal current collector with a gas diffusion layer and coated catalyst facing electrolyte, (B) carbon-base current collector and gas diffusion and catalyst, (C) carbon paper-current collector and gas diffusion and catalyst.
Applsci 09 02787 g005
Applsci 09 02787 g006 550
Figure 6. (a) X-ray diffraction patterns and (b) electrochemical behaviors of Co3O4, low-temperature (LT)-LiCoO2, high-temperature (HT)-LiCoO2 catalysts [30] (Copyright © 2014, Springer Nature).
Figure 6. (a) X-ray diffraction patterns and (b) electrochemical behaviors of Co3O4, low-temperature (LT)-LiCoO2, high-temperature (HT)-LiCoO2 catalysts [30] (Copyright © 2014, Springer Nature).
Applsci 09 02787 g006
Applsci 09 02787 g007 550
Figure 7. (a) SEM images of Mn3O4/MnO nanoparticles [33] (Copyright © 2019, Elsevier), (b) TEM images of LaCoO3 catalysts [34], (c) TEM image of honeycomb-like 3D ordered mesoporous spinel Co3O4 [35] (Copyright © 2016, John Wiley and Sons), (d) TEM image of hollow cobalt oxide nanoparticles [36] (Copyright © 2019, Elsevier).
Figure 7. (a) SEM images of Mn3O4/MnO nanoparticles [33] (Copyright © 2019, Elsevier), (b) TEM images of LaCoO3 catalysts [34], (c) TEM image of honeycomb-like 3D ordered mesoporous spinel Co3O4 [35] (Copyright © 2016, John Wiley and Sons), (d) TEM image of hollow cobalt oxide nanoparticles [36] (Copyright © 2019, Elsevier).
Applsci 09 02787 g007
Applsci 09 02787 g008 550
Figure 8. Four nitrogen doping configurations of a graphene molecule [23].
Figure 8. Four nitrogen doping configurations of a graphene molecule [23].
Applsci 09 02787 g008
Applsci 09 02787 g009 550
Figure 9. (a) Structure evolution of the NaO2 discharge product during oxygen reduction reaction (ORR) [46] (Copyright © 2019, Elsevier); (b) Structural and phase characterization of a CuO nanowire (NW) during discharging and charging in an O2 environment [47] (Copyright © 2018, American Chemical Society); (c) Cyclic voltammetry performed in electrochemical-atomic force microscope cell and the resulting AFM image after CV reduction [48] (Copyright © 2016, American Chemical Society).
Figure 9. (a) Structure evolution of the NaO2 discharge product during oxygen reduction reaction (ORR) [46] (Copyright © 2019, Elsevier); (b) Structural and phase characterization of a CuO nanowire (NW) during discharging and charging in an O2 environment [47] (Copyright © 2018, American Chemical Society); (c) Cyclic voltammetry performed in electrochemical-atomic force microscope cell and the resulting AFM image after CV reduction [48] (Copyright © 2016, American Chemical Society).
Applsci 09 02787 g009
Applsci 09 02787 g010 550
Figure 10. SEM images and EDS maps of (a) Al/Cu-CD, (b) Al/Cu-ED, (c) The cyclic voltammogram in 1 M NaOH of Al (pure), Al/Cu-CD, and Al/Cu-ED, (d) EIS measurements of anodes in 1 M NaOH, The Nyquist a Al (pure), Al/Cu-CD, Al/Cu-ED [53] (Copyright © 2018, Springer Nature).
Figure 10. SEM images and EDS maps of (a) Al/Cu-CD, (b) Al/Cu-ED, (c) The cyclic voltammogram in 1 M NaOH of Al (pure), Al/Cu-CD, and Al/Cu-ED, (d) EIS measurements of anodes in 1 M NaOH, The Nyquist a Al (pure), Al/Cu-CD, Al/Cu-ED [53] (Copyright © 2018, Springer Nature).
Applsci 09 02787 g010
Applsci 09 02787 g011 550
Figure 11. Cyclic voltammetry for Fe/C composite electrodes composited carbon nano-fibers (a) without and (b) with FeS additive [54] (Copyright © 2006, Elsevier).
Figure 11. Cyclic voltammetry for Fe/C composite electrodes composited carbon nano-fibers (a) without and (b) with FeS additive [54] (Copyright © 2006, Elsevier).
Applsci 09 02787 g011
Applsci 09 02787 g012 550
Figure 12. Corrosion, passivation, and dendrite formation processes at a metal anode.
Figure 12. Corrosion, passivation, and dendrite formation processes at a metal anode.
Applsci 09 02787 g012
Applsci 09 02787 g013 550
Figure 13. Schematic diagrams of various electrolytes of MABs.
Figure 13. Schematic diagrams of various electrolytes of MABs.
Applsci 09 02787 g013
Applsci 09 02787 g014 550
Figure 14. (a) Schematic illustration of theoretical voltages of Fe−air batteries operated with an alkaline or an acidic cathode electrolyte. Two types of Fe−air batteries with a Na+- or a Li+-ion solid electrolyte, for (b) a Fe(LiOH)//Li-SSE//O2(H3PO4/LiH2PO4) cell, and (c) a Fe(NaOH)//Na-SS//O2(H3PO4/NaH2PO4) cell. SSE represents solid-state electrolyte [64] (Copyright © 2017, American Chemical Society).
Figure 14. (a) Schematic illustration of theoretical voltages of Fe−air batteries operated with an alkaline or an acidic cathode electrolyte. Two types of Fe−air batteries with a Na+- or a Li+-ion solid electrolyte, for (b) a Fe(LiOH)//Li-SSE//O2(H3PO4/LiH2PO4) cell, and (c) a Fe(NaOH)//Na-SS//O2(H3PO4/NaH2PO4) cell. SSE represents solid-state electrolyte [64] (Copyright © 2017, American Chemical Society).
Applsci 09 02787 g014
Applsci 09 02787 g015 550
Figure 15. Schematics of (a) a screen printing [71] (Copyright © 2017, RSC Pub), (b) spray printing [72] (Copyright © 2015, John Wiley and Sons), (c) direct ink writing processes [73] (Copyright © 2017, John Wiley and Sons).
Figure 15. Schematics of (a) a screen printing [71] (Copyright © 2017, RSC Pub), (b) spray printing [72] (Copyright © 2015, John Wiley and Sons), (c) direct ink writing processes [73] (Copyright © 2017, John Wiley and Sons).
Applsci 09 02787 g015
Applsci 09 02787 g016 550
Figure 16. Of 1-, 2-, 3-, and 4D concepts. A 4D structure is a structure (x, y, z) made by 3D changes over time (t). Arrows indicate the direction of change with respect to time.
Figure 16. Of 1-, 2-, 3-, and 4D concepts. A 4D structure is a structure (x, y, z) made by 3D changes over time (t). Arrows indicate the direction of change with respect to time.
Applsci 09 02787 g016
Applsci 09 02787 g017 550
Figure 17. (a) Schematic of aluminum–air batteries (AAB) working principle, (b) Photo of a packaged battery cell, (c) The first cycle discharge capacity with different laser sintering powers. (d) Discharge capacity for 3D printed anode and relationship between anode thickness and capacity [3] (Copyright © 2018, Electrochemical Society).
Figure 17. (a) Schematic of aluminum–air batteries (AAB) working principle, (b) Photo of a packaged battery cell, (c) The first cycle discharge capacity with different laser sintering powers. (d) Discharge capacity for 3D printed anode and relationship between anode thickness and capacity [3] (Copyright © 2018, Electrochemical Society).
Applsci 09 02787 g017
Table
Table 1. Parameters and electrochemical impedance spectroscopy (EIS) value of different grades of Al anodes [49].
Table 1. Parameters and electrochemical impedance spectroscopy (EIS) value of different grades of Al anodes [49].
GradeEcorr (V vs. Hg/HgO)Icorr (mA cm−2)Rp (Ω cm2)
4 M NaOH4 M KOH4 M NaOH4 M KOH4 M NaOH4 M KOH
10501.2901.2911861764.1085.683
20111.4101.4201351424.1246.674
30031.3151.3401811654.6075.892
40321.3901.3901451744.6532.572
50521.3101.3201911573.7662.539
60611.3701.3801611684.7662.655
70501.4201.4501891434.5162.848
80111.4201.4501351443.6282.670
5N1.6991.82124.34.79.66817.9
Grade
Equivalent elementssolution105020113003403250526061705080115N
Rt (Ω cm2)4 M NaOH0.700.750.570.840.740.490.761.2472.29
4 M KOH1.230.691.2080.33510.780.360.601.10815.3

Share and Cite

MDPI and ACS Style

Wang, C.; Yu, Y.; Niu, J.; Liu, Y.; Bridges, D.; Liu, X.; Pooran, J.; Zhang, Y.; Hu, A. Recent Progress of Metal–Air Batteries—A Mini Review. Appl. Sci. 2019, 9, 2787. https://doi.org/10.3390/app9142787

AMA Style

Wang C, Yu Y, Niu J, Liu Y, Bridges D, Liu X, Pooran J, Zhang Y, Hu A. Recent Progress of Metal–Air Batteries—A Mini Review. Applied Sciences. 2019; 9(14):2787. https://doi.org/10.3390/app9142787

Chicago/Turabian Style

Wang, Chunlian, Yongchao Yu, Jiajia Niu, Yaxuan Liu, Denzel Bridges, Xianqiang Liu, Joshi Pooran, Yuefei Zhang, and Anming Hu. 2019. "Recent Progress of Metal–Air Batteries—A Mini Review" Applied Sciences 9, no. 14: 2787. https://doi.org/10.3390/app9142787

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop