Journal Archive

Johnson Matthey Technol. Rev., 2015, 59, (1), 56
doi: 10.1595/205651315X685733

17th International Meeting on Lithium Batteries

Highlights of the latest research on post-lithium-ion battery chemistry

  • Reviewed by Mario Joost* and Sam Alexander
  • Johnson Matthey Technology Centre,
  • Sonning Common, Reading, RG4 9NH, UK
  • Email: *

1. Introduction

Within the last 20 years, publication numbers in the field of lithium battery research have increased from a few hundred in the mid 1990s to more than 4500 publications in 2013 (Figure 1). It has grown to a major research topic, with many universities, state laboratories and commercial research and development (R&D) facilities involved. The number of meetings dedicated to battery work has increased likewise. The International Meeting on Lithium Batteries (IMLB) has been held biannually since 1982 and is one of the top meetings in the Li battery community. It is organised by an international executive committee, currently comprising of 24 international scientists. Following Jeju, Korea, in 2012, this year’s meeting was held in Como, Italy. It was co-organised by the Electrochemical Society (ECS) which will also publish dedicated special issues in Journal of the Electrochemical Society and ECS Transactions. Around 1000 people attended the meeting with 40+ keynote speakers, presenting in nine plenary sessions and three large poster sessions with more than 500 contributions. Further details on the 17th IMLB meeting including details of the scientific programme and biographies of the invited speakers can be found on the conference website (1).

Fig. 1.

Numbers of scientific publications related to different types of battery. The search was run on keywords in the manuscript titles and abstracts. Note that the numbers for sodium batteries include the (high-temperature) molten salt and Na-sulfur systems

In recent years there has been increasing interest in next-generation, ‘beyond lithium-ion’ battery technologies, especially in Li-air, Li-sulfur and sodium based chemistries. A major theme of the meeting addressed recent advances in beyond Li-ion batteries, where novelty was a key requirement for paper acceptance. The main areas of interest were Li battery related science and technology such as, but not limited to: electrode materials, electrolytes, Li-air, Li-sulfur, sodium batteries, new analytical tools, computational work and safety.

Due to the huge amount of contributions during this conference, only a few highlights of each main topic are included in this review. For a detailed overview of the conference contents, the interested reader is referred to the conference homepage (1).

2. Lithium-Oxygen Batteries

No other battery system is the subject of such controversial discussion as Li-oxygen. The list of ‘unsolvable’ problems is long and small successes are contrasted by big setbacks. The many reports on stability issues of electrolyte solvents are just one example (24). Reaction mechanisms of the oxygen reduction reaction (ORR) and the oxygen evolution reaction (OER) are still not explained satisfactorily (5) and side reactions are omnipresent. Contamination originating from the cathode, which is open to the environment, cannot be blocked sufficiently (6).

From the start, the question of the preferred morphology of Li2O2 deposition was heavily discussed amongst the speakers. Together with her co-workers, Yang Shao-Horn (Massachusetts Institute of Technology (MIT), USA) studied the effect of solvation on Li-O2 redox reactions. The results revealed the formation of very small Li2O2 particles at high discharge rates and/or when using a solvent with low solvation power (here: dimethylether (DME)). At low rates and/or when using solvents with higher donor numbers (here: dimethyl sulfoxide (DMSO)), larger, disc-like particles (Figure 2) are formed (7). Lower overpotential (i.e. higher discharge voltage) was observed in the latter case. Increased solvation power due to high donor numbers lowers the energy levels of the Li/Li+ redox reaction and increases that of the O2/2*O2– reaction. Larger particles seemed to improve the kinetics and better fill the volume of carbon pores, whereas smaller particles have a reduced overpotential (5).

Fig. 2.

Li2O2 toroidal discs on a porous carbon electrode

Large, toroidal shaped discs in high donor number solvents were also found by Peter Bruce’s group (University of Oxford, UK). According to his theory, high solubility of the superoxide radical in the electrolyte leads to Li2O2 growth from the solution rather than from the electrode surface. The addition of redox mediators was discussed to aid the dissolution of Li2O2 on charge and therefore increase the rate capability (8). Also focused on the donor abilities of electrolyte solvents, K. M. Abraham’s (Northeastern University, USA) approach was based on the ‘hard and soft acids and bases’ (HSAB) concept. Ionic liquids (ILs) with soft cations (such as 1-methyl-1-butyl-pyrrolidinium bis(triflouromethanesulfonyl)imide (Pyr14TFSI) and 1-ethyl-3-methylimidazolium bis-(trifluoromethanesulfonyl)imide (EMITFSI)) reduce the Li+ acidity in organic electrolytes and therefore increase the lifetime of initially formed O2 (9). The potential of Pyr14TFSI was demonstrated by Jakub Reiter (BMW Group, Germany) when he presented results of an ionic liquid electrolyte (Pyr14TFSI/LiTFSI (9:1)), applied in a Li-air battery using a Super-P® cathode and a Li-metal anode (10).

Tailoring Li2O2 morphology by providing an optimised cathode structure was the idea of Xin-Bo Zhang and co-workers (Chinese Academy of Sciences, China). A free-standing honeycomb-like palladium modified hollow spherical carbon was applied as Li-air cathode, which led to organised, toroidal nanosheets of Li2O2. More than 100 cycles at a current density of 300 mA g–1 and a specific capacity limit of 1000 mAh g–1 were presented (11). In contrast to the results discussed before, Li2O2 was observed to form rapidly if the superoxide binds well on the cathode surface. Atomically dispersed Fe/N/C composite as bifunctional catalysts showed better performance, exhibiting fewer side reactions than a classic α-manganese(IV) oxide (MnO2) catalyst (12).

The possible instability of the carbon cathode and the related importance of the 2e per O2 ratio for the ORR and OER was a key message from Peter Bruce (1315). Arumugam Manthiram (University of Texas, USA) suggested hybrid Li-air batteries as a solution to the aforementioned problems. The benefits of an aqueous cathodic compartment and a non-aqueous anodic compartment can compensate for the increased complexity of the system (16, 17). Novel catalysts like iridium(IV) oxide (IrO2) (18), low-temperature Li1–xCoO2 or LiMn1.5Ni0.5O4 were successfully employed (19). Other workers used a cobalt phthalocyanine-derived catalyst to enable the full reduction of O2 to Li2O, thus utilising the full theoretical range of a Li-air cell (20). To reduce safety issues, replacing the Li metal anode with SnC, Fe0.1Zn0.9O or SiC was suggested (10).

3. Lithium-Sulfur Batteries

Lithium-sulfur (Li-S) batteries are expected to be closer to a marketable product than Li-air batteries. A major remaining challenge, addressed in many contributions, is the high solubility of polysulfide intermediates formed during the stepwise (but in no case straightforward) reduction from S8 to the final discharge product Li2S (21, 22). These polysulfides migrate to the anode, ending up as a self-discharge promoting redox shuttle or as a deposit blocking the anode surface (23, 24).

Yi Cui (Stanford University, USA) started with a quick overview of the recent evolution of Li-S cathodes (from sulfur/carbon mixtures to encapsulated hollow particles) and he summarised by stating that no satisfying solution to ‘capture’ the sulfur has been found yet. Tin-doped indium oxide was found to fix polysulfide to carbon (25). Core-shell material showed increased sulfur ‘trapping’ but still lost polysulfides during cycling (26, 27). Yu-Guo Guo (Chinese Academy of Sciences) tried to start from smaller sulfur homologues (S2–4) which could be successfully trapped inside microporous carbon or carbon nanotubes (CNTs) (28). The group of Linda F. Nazar (University of Waterloo, Canada) replaced the carbon support with titania (TiO2), alumina (Al2O3) and titanium oxide (Ti4O7) and successfully reduced the fade rate (29).

A second approach to stop polysulfide migration would be an electrolyte which would act as a polysulfide barrier. A polymer electrolyte made from poly ethylene(oxide) with 10 wt% ZrO2, LiCF3SO3 and Li2S was presented by Jusef Hassoun (Sapienza University of Rome, Italy). Cells had to be operated at 70°C to deliver 900 mAh g–1 (30). Doping the electrolyte (tetraglyme) with a polysulfide (Li2S8) proved to decrease the internal resistance and seemed to buffer further polysulfide dissolution (31). The incorporation of ionic liquids might also be a viable solution to the problem. Aleksandar Matic (Chalmers University, Sweden) presented imidazolium- and pyrrolidinium-based electrolytes (32), some of them mixed with 1,3-dioxolane or glymes (33). Linda F. Nazar could achieve decreased polysulfide dissolution in electrolyte systems based on 1,3-dioxolane, 1,2-dimethoxyethane and bis(trifluoromethylsulfonyl)imide (TFSI) salts (34). She also presented an in operando X-ray absorption spectroscopy technique to identify the different sulfur species (35). As an alternative approach, a membrane-free polysulfide flow battery was presented by Yi Cui (36).

4. Sodium Batteries

High-temperature Na batteries were developed as molten Na-S or Na-NiCl2 (ZEBRA) batteries in the 1980s. However, these systems were quickly pushed aside by the success of Li-ion batteries. Low-temperature sodium systems, like Li-ion technology, have now started to gain interest within the last few years (Figure 1). They can certainly benefit from experience in the Li-ion field but knowledge transfer will not be as straightforward as it may seem.

‘Walking on the sodium side’ was the slogan of Maria Rosa Palacín (Institut de Ciència de Materials de Barcelona-Consejo Superior de Investigaciones Científicas (ICMAB-CSIC), Spain) as she opened the Na-ion related talks. Major safety concerns come with the use of Na metal as anode, which reacts more fiercely with water than Li. Carbon would be one alterative (37), but Ti-based insertion materials, especially Na2Ti3O7, could also give reasonable performance, with Na insertion potentials as low as 0.3 V vs. Na+/Na (38, 39). Young-Jun Kim (Korea Electronics Technology Institute) would employ sodium metal in systems like Na-S, Na-NiCl2, Na-O2 and Na-ion when electrolytes like NaAlCl4*SO2 or organic liquids would prove suitable. However, side reactions with the electrolyte are an issue for sodium. Maria Rosa Palacín’s group found ethylene carbonate and/or propylene carbonate based solutions with sodium perchlorate (NaClO4) to be relatively stable (40). Laurence Croguennec (Institut de Chimie de la Matière Condensée de Bordeaux-Centre National de la Recherche Scientifique (ICMCB-CNRS), France) suggested fluorophosphates as high energy density positive electrodes for Na (and Li) batteries. In particular the compound Na3V2(PO4)2F3 was investigated, since vanadium offers a wide range of stable oxidation states and structures in Na (41, 42) and Li (43) containing compounds.

5. Layered Lithium-Ion Battery Cathode Materials

There is a large drive to increase the operating potential of Li-ion batteries in order to increase the gravimetric energy density. The gravimetric energy density is the product of capacity and the mean operating voltage and therefore can be altered by changing either of these material properties. Layered metal oxides have been used as Li-ion battery cathodes since the first commercial battery produced by Sony in the early 1990s. These materials are made up of slabs of edge sharing MO6 octahedra (where M is Ni, Co and/or Mn) separated by layers of Li cations (Figure 3). The elemental composition of these materials has changed significantly since Sony first used LiCoO2 as an intercalation cathode. Modern versions are doped with Ni and Mn (known as NMC) with the formula Li[NixMnyCoz]O2, where x + y + z = 1. The transition metal ratios can be altered to control properties such as capacity and operating potential.

Fig. 3.

Structure of LiMO2: green = lithium, purple = metal (M) and red = oxygen (O)

One major issue with NMC type compounds is structural instability caused by either collapse of the MO6 layers on Li removal or by migration of transition metals into the empty Li positions. Increasing the Ni content in Li[NixMnyCoz]O2 leads to increased capacity but also decreased capacity retention and concomitant decrease in structural stability. When x is as high as 0.85, the material has a higher initial capacity, but 90% of the structure collapses during cycling, leading to fast capacity loss. Therefore Yang-Kook Sun (Hangyang University, Korea) described a core-shell material with increased capacity in the core and good stability (and therefore high safety) on the surface (44). However, these materials do not perform well due to separation of the shell from the core during cycling, caused by different volume change ratios. Applying a gradient throughout the whole particle, using a slow concentration change in the core and a fast concentration change in the shell, led to mechanically stable particles while keeping the capacity and stability advantages (45, 46).

Al2O3 coatings as an alternative method for stabilising NMC particles were described by Kuniaki Tatsumi (National Institute of Advanced Industrial Science and Technology (AIST), Japan). Li[Ni1/3Mn1/3Co1/3]O2 was mechanochemically coated, the Al2O3 was uniformly distributed on the surface with no migration into the bulk particle. The material showed greatly improved cycling performance, even at elevated temperatures. The Al2O3 coating suppressed crack formation, reduced degradation of charge transfer sites and increased cycling stability at 1 C. Without coating, carbonates and LiF formed on the particle surfaces, concomitant with an increase in the detrimental cubic NMC phase at particle surfaces (47).

A third strategy to increase the stability of NMC based layered compounds is to make a composite of Li2MnO3 and LiNixMnyCozO2, also known as Li-rich NMC. Li2MnO3 is structurally related to LiNixMnyCozO2; however excess Li resides in the transition metal layers. This results in the presence of electrochemically inactive Mn4+ which acts as a structural scaffold and prevents collapse of the metal oxide layers. The resulting compound has a reversible capacity as high as 200 mAh g–1. However, transition metal cations migrate from the transition metal layers to the Li layers, leading to voltage fade over time. The cause of this migration is not fully understood, however, Jean-Marie Tarascon shed some light on the problem using simplified compounds like Li2Ru(IV)1–ySn(IV)yO3 (as opposed to Li2MnO3). This 3d-metal-free compound could be cycled over 100 times, delivering reasonably high capacity. X-ray diffraction (XRD) was used to show the onset of large disorder on charging which was recovered on discharge. High-angle annular dark-field-scanning transmission electron microscopy (HAADF-STEM) showed massive cationic migration to the Li layers on charging which returned to the completely ordered state when subsequently discharged. Despite this cationic migration the Li2Ru(IV)1–ySn(IV)yO3 structure shows no voltage fade over time. Testing the impact of ion size (Sn4+>Ti4+>Mn4+), the titanium compound Li2Ru0.75Ti0.25O3 was synthesised. It showed the worst voltage fade. A combination of X-ray photoelectron spectroscopy (XPS) and electron microscopy showed that upon cycling, Ti4+ accumulates in tetrahedral sites between the metal oxide and Li layers where it is no longer active. Preventing metals entering these tetrahedral sites will prevent voltage fade in layered-layered compounds. Sn4+ is therefore attractive to reduce voltage fade, however replacing Mn with Sn has not worked. Compounds with the stoichiometry Li4(Mn+,Mm+)O6 where m + n = 8 are considered best as an answer to the voltage fade issue in Li-rich NMCs (48, 49).

6. Anode Materials

Future anode materials are more likely to be conversion or alloying type materials rather than insertion materials like the state-of-the-art graphite anode. Complex reaction mechanisms and high volume changes present challenges for these materials. Nanostructuring and coating with polymers or carbons are two approaches to protect materials against side reactions and ensure good cycling, even at high rates.

Fe3O4 is a conversion material which reacts with Li+ to form Li2O and Fe metal. The Fe metal produced can also alloy with Li as the battery continues to discharge. Fe3O4 has in the past been doped with Zn to produce ZnFe2O4, however this material has poor coulombic efficiency. Stefano Passerini (Helmholtz Institute, Ulm, Germany) presented his group’s work in which ZnFe2O4 was coated with carbon using glucose as precursor. In addition to the particle coating, a carbon matrix was formed in which many particles were combined to form macroscopically sized particles. These ‘carbon coated matrix’ particles showed improved performance compared to micron sized particles (50, 51). In a separate piece of work TiO2 nanorods were carbon coated using polyacrylonitrile (PAN) as precursor. The block copolymer was anchored to the TiO2 surface before carbonising to create an even carbon layer. The performance of these new nanorods was greatly improved with respect to the uncoated sample (52).

Karim Zaghib (Hydro-Québec, Canada) described the latest advances in trying to stabilise reactive Li metal anodes with polymer coatings. The challenges and opportunities in developing thin Li metal with a stable solid electrolyte interphase (SEI) as the negative electrode were discussed in this presentation. In a unique process, Li metal was extruded to 20 μm thin films at a speed of 30 m min–1. The surface was treated with a special solution and pressed against a solid polymer electrolyte film (dry polymer and ionic liquid-polymer electrolytes). Due to the surface treatment, the very clean conditions and constant pressure on the stack, long term cycling (3000 cycles at C/3 and 80°C) without major fading and dendrite growth was possible.

Nanostructuring has become a key requirement for the utilisation of high capacity silicon anodes. Whilst these anodes have very high capacities they can be difficult to utilise, due to a large volume change of around 300% occurring on lithiation. Fei Luo (Chinese Academy of Sciences) described how the volume variation in Si/C composites is very anisotropic. Si/C particles were synthesised as nanorods attached to the substrate which allowed for the large volume expansion. There was a complex evolution of particle shape caused by amorphous to amorphous diffusion-controlled phase transitions; however porous films did not prevent cracking. Isolated Si column structures showed much less cracking than dense films (53).

7. Electrolytes

Increasing the operational potential of the cathodes brings new challenges for the electrolyte. Jeff Dahn and Laura Downie (Dalhousie University, Canada) described their approach to tackle increased side reactions originating from electrolyte oxidation on high voltage material surfaces. Commonly used carbonate based electrolyte solutions show increasing reaction rates above 4.2 V vs. Li+/Li. Additives such as vinylidene carbonate (VC), tris(trimethylsilyl)phosphite (TTSPi) and methylene methanedisulfonate (MMDS) (54) can be used to increase this maximum operating potential (55). NMC pouch cells were cycled at C/10 with low temperature impedance measurements made every 10 cycles. The results of this study showed that there was a very large increase in charge transfer resistance when cells are cycled above 4.4 V. Increased electrolyte oxidation is correlated to increased parasitic heat flow, detected via isothermal microcalorimetry. When more than 100 μV of heat is generated during cycling, the entire electrolyte of an A5 pouch cell would be consumed within one year (5658). Jeff Dahn carefully summarised that the electrolyte stability usually increases with the number of additives.

Ceramic solid state electrolytes as a safe high-voltage solution were presented by Chihiro Yada (Toyota Motor Europe). A main problem is the huge charge-transfer resistance at the interfaces due to fast Li-ion depletion upon load. Dielectric modification of these layers using BaTiO3 could decrease this resistance and increase the quantity of Li at the interface. Li1.1(Nb0.5Ta0.5)0.9O3–δ was identified as a promising material with high permeation and Li-ion mobility (59). Flexible solid state electrolytes which can be printed in any shape were presented as a key component for future electronic devices (wearable technology, flexible devices) by Sang-Young Lee (Ulsan National Institute of Science and Technology (UNIST), Korea). The plastic crystal electrolyte (PCE) consists of alumina/silica ceramic nanoparticles, ethylene carbonate, succinonitrile and an ultraviolet (UV) cross linker. The electrolyte ink has no additional processing solvents and shows thixotropic behaviour. Addition of ethoxylated trimethylolpropane triacrylate (ETPTA) successfully suppresses dendrite growth. Cells can be stretched and bent during operation (60, 61). Maria Forsyth (Deakin University, Australia) presented organic ionic plastic crystals (OIPCs, solidified ionic liquids), which show good electrochemical behaviour. Phosphonium based OIPCs incorporating Na salts show electrochemical properties similar to Li containing analogues (6264). However, the presence of multiple phases, high viscosity and high-temperature eutectics remain issues which can be altered by a careful choice of ion combination (65).

The fact that polymer electrolytes are still solid, after 30 years of research, was no cause for concern for Michel Armand (CIC EnergiGUNE, Spain). Poly(ethylene oxide) (PEO) suffers from increasing glass transition temperature (Tg) (and therefore decreased conductivity) with increasing salt concentration. In poly(ethylene carbonate) (PEC) it is the other way around and this might be an interesting solution for the problem of low conductivity at sub-ambient temperatures (66). Polyelectrolytes have the anion attached to the backbone and the Li transport number should therefore be 1, since Li+ is the only mobile species. However, the overall conductivity remains low for these systems so far. Armand’s group linked TFSI anions and PEO elements to a polystyrene backbone which could achieve conductivities around 10–5 S cm–1 at 60°C (67, 68). The question of whether PEO based systems can successfully suppress Li dendrite formation was investigated by the group of Noboyuki Imanishi (Mie University, Japan). A PEO18LiTFSI with 10 wt% BaTiO3 system was swollen with ionic liquid which reduced the bulk resistance of the battery and increased the cycle performance. In situ scanning electron microscopy investigations showed that dendrite growth could be retarded.

8. Conclusions

This conference was loaded with excellent talks and an enormous number of interesting poster contributions. It was a very well organised event and the beautiful weather underlined the lovely venue. It was obvious that the research on post Li-ion systems is a quickly growing field, which already generate dedicated conferences. One can happily look forward to the next IMLB meeting in 2016 which will be held in Chicago, USA.


  1.  The 17th International Meeting on Lithium Batteries, 10th–14th June, 2014, Como, Italy LINK
  2.  D. G. Kwabi, N. Ortiz-Vitoriano, S. A. Freunberger, Y. Chen, N. Imanishi, P. G. Bruce and Y. Shao-Horn, MRS Bull., 2014, 39, (5), 443 LINK
  3.  M. Balaish, A. Kraytsberg and Y. Ein-Eli, Phys. Chem. Chem. Phys., 2014, 16, (7), 2801 LINK
  4.  M. D. Bhatt, H. Geaney, M. Nolan and C. O’Dwyer, Phys. Chem. Chem. Phys., 2014, 16, (24), 12093 LINK
  5.  B. M. Gallant, D. G. Kwabi, R. R. Mitchell, J. Zhou, C. V. Thompson and Y. Shao-Horn, Energy Environ. Sci., 2013, 6, (8), 2518 LINK
  6.  M. H. Cho, J. Trottier, C. Gagnon, P. Hovington, D. Clément, A. Vijh, C.-S. Kim, A. Guerfi, R. Black, L. Nazar and K. Zaghib, J. Power Sources, 2014, 268, 565 LINK
  7.  B. Horstmann, B. Gallant, R. Mitchell, W. G. Bessler, Y. Shao-Horn and M. Z. Bazant, J. Phys. Chem. Lett., 2013, 4, (24), 4217 LINK
  8.  Y. Chen, S. A. Freunberger, Z. Peng, O. Fontaine and P. G. Bruce, Nature Chem., 2013, 5, (6), 489 LINK
  9.  C. J. Allen, J. Hwang, R. Kautz, S. Mukerjee, E. J. Plichta, M. A. Hendrickson and K. M. Abraham, J. Phys. Chem. C, 2012, 116, (39), 20755 LINK
  10.  G. A. Elia, J. Hassoun, W.-J. Kwak, Y.-K. Sun, B. Scrosati, F. Mueller, D. Bresser, S. Passerini, P. Oberhumer, N. Tsiouvaras and J. Reiter, Nano Lett., 2014, 14, (11), 6572 LINK
  11.  J.-J. Xu, Z.-L. Wang, D. Xu, L.-L. Zhang and X.-B. Zhang, Nature Commun., 2013, 4, 2438 LINK
  12.  J.-L. Shui, N. K. Karan, M. Balasubramanian, S.-Y. Li and D.-J. Liu, J. Am. Chem. Soc., 2012, 134, (40), 16654 LINK
  13.  M. M. Ottakam Thotiyl, S. A. Freunberger, Z. Peng and P. G. Bruce, J. Am. Chem. Soc., 2013, 135, (1), 494 LINK
  14.  M. M. Ottakam Thotiyl, S. A. Freunberger, Z. Peng, Y. Chen, Z. Liu and P. G. Bruce, Nature Mater., 2013, 12, (11), 1050 LINK
  15.  Z. Peng, S. A. Freunberger, Y. Chen and P. G. Bruce, Science, 2012, 337, (6094), 563 LINK
  16.  L. Li, X. Zhao, Y. Fu and A. Manthiram, Phys. Chem. Chem. Phys., 2012, 14, (37), 12737 LINK
  17.  L. Li, X. Zhao and A. Manthiram, Electrochem. Commun., 2012, 14, (1), 78 LINK
  18.  L. Li and A. Manthiram, J. Mater. Chem. A, 2013, 1, (16), 5121 LINK
  19.  T. Maiyalagan, K. A. Jarvis, S. Therese, P. J. Ferreira and A. Manthiram, Nature Commun., 2014, 5, 3949 LINK
  20.  M. J. Trahan, Q. Jia, S. Mukerjee, E. J. Plichta, M. A. Hendrickson and K. M. Abraham, J. Electrochem. Soc., 2013, 160, (9), A1577 LINK
  21.  D.-H. Han, B.-S. Kim, S.-J. Choi, Y. Jung, J. Kwak and S.-M. Park, J. Electrochem. Soc., 2004, 151, (9), E283 LINK
  22.  N. S. A. Manan, L. Aldous, Y. Alias, P. Murray, L. J. Yellowlees, M. C. Lagunas and C. Hardacre, J. Phys. Chem. B, 2011, 115, (47), 13873 LINK
  23.  L. Chen and L. L. Shaw, J. Power Sources, 2014, 267, 770 LINK
  24.  D. Bresser, S. Passerini and B. Scrosati, Chem. Commun., 2013, 49, (90), 10545 LINK
  25.  H. Yao, G. Zheng, P.-C. Hsu, D. Kong, J. J. Cha, W. Li, Z. W. Seh, M. T. McDowell, K. Yan, Z. Liang, V. K. Narasimhan and Y. Cui, Nature Commun., 2014, 5, 3943 LINK
  26.  Z. W. Seh, W. Li, J. J. Cha, G. Zheng, Y. Yang, M. T. McDowell, P.-C. Hsu and Y. Cui, Nature Commun., 2013, 4, 1331 LINK
  27.  G. Zheng, Y. Yang, J. J. Cha, S. S. Hong and Y. Cui, Nano Lett., 2011, 11, (10), 4462 LINK
  28.  S. Xin, L. Gu, N.-H. Zhao, Y.-X. Yin, L.-J. Zhou, Y.-G. Guo and L.-J. Wan, J. Am. Chem. Soc., 2012, 134, (45), 18510 LINK
  29.  Q. Pang, D. Kundu, M. Cuisinier and L. F. Nazar, Nature Commun., 2014, 5, 4759 LINK
  30.  J. Hassoun and B. Scrosati, Adv. Mater., 2010, 22, (45), 5198 LINK
  31.  D.-J. Lee, M. Agostini, J.-W. Park, Y.-K. Sun, J. Hassoun and B. Scrosati, ChemSusChem, 2013, 6, (12), 2245 LINK
  32.  S. Xiong, K. Xiea, E. Blomberg, P. Jacobsson and A. Matic, J. Power Sources, 2014, 252, 150 LINK
  33.  K .Ueno, K. Yoshida, M. Tsuchiya, N. Tachikawa, K. Dokko and M. Watanabe, J. Phys. Chem. B, 2012, 116, (36), 11323 LINK
  34.  J. Schuster, G. He, B. Mandlmeier, T. Yim, K. T. Lee, T. Bein and L. F. Nazar, Angew. Chem. Int. Ed., 2012, 51, (15), 3591 LINK
  35.  M. Cuisinier, P.-E. Cabelguen, S. Evers, G. He, M. Kolbeck, A. Garsuch, T. Bolin, M. Balasubramanian and L. F. Nazar, J. Phys. Chem. Lett., 2013, 4, (19), 3227 LINK
  36.  Y. Yang, G. Zheng and Y. Cui, Energy Environ. Sci., 2013, 6, (5), 1552 LINK
  37.  A. Ponrouch, A. R. Goñi and M. R. Palacín, Electrochem. Commun., 2013, 27, 85 LINK
  38.  P. Senguttuvan, G. Rousse, V. Seznec, J.-M. Tarascon and M. R. Palacín, Chem. Mater., 2011, 23, (18), 4109 LINK
  39.  G. Rousse, M. E. Arroyo-de Dompablo, P. Senguttuvan, A. Ponrouch, J.-M. Tarascon and M. R. Palacín, Chem. Mater., 2013, 25, (24), 4946 LINK
  40.  A. Ponrouch, R. Dedryvère, D. Monti, A. E. Demet, J. M. Ateba Mba, L. Croguennec, C. Masquelier, P. Johansson and M. R. Palacín, Energy Environ. Sci., 2013, 6, (8), 2361 LINK
  41.  M. Bianchini, N. Brisset, F. Fauth, F. Weill, E. Elkaim, E. Suard, C. Masquelier and L. Croguennec, Chem. Mater., 2014, 26, (14), 4238 LINK
  42.  K. Chihara, A. Kitajou, I. D. Gocheva, S. Okada and J.-i. Yamaki, J. Power Sources, 2013, 227, 80 LINK
  43.  M. Bianchini, J. M. Ateba-Mba, P. Dagault, E. Bogdan, D. Carlier, E. Suard, C. Masquelier and L. Croguennec, J. Mater. Chem. A, 2014, 2, (26), 10182 LINK
  44.  M.-H. Kim, H.-S. Shin, D. Shin and Y.-K. Sun, J. Power Sources, 2006, 159, (2), 1328 LINK
  45.  Y.-K. Sun, S.-T. Myung, B.-C. Park, J. Prakash, I. Belharouak and K. Amine, Nature Mater., 2009, 8, (4), 320 LINK
  46.  Y.-K. Sun, Z. Chen, H.-J. Noh, D.-J. Lee, H.-G. Jung, Y. Ren, S. Wang, C. S. Yoon, S.-T. Myung and K. Amine, Nature Mater., 2012, 11, (11), 942 LINK
  47.  K. Araki, N. Taguchi, H. Sakaebe, K. Tatsumi and Z. Ogumi, J. Power Sources, 2014, 269, 236 LINK
  48.  G. Rousse and J. M. Tarascon, Chem. Mater., 2014, 26, (1), 394 LINK
  49.  M. Sathiya, G. Rousse, K. Ramesha, C. P. Laisa, H. Vezin, M. T. Sougrati, M.-L. Doublet, D. Foix, D. Gonbeau, W. Walker, A. S. Prakash, M. Ben Hassine, L. Dupont and J.-M. Tarascon, Nature Mater., 2013, 12, (9), 827 LINK
  50.  F. Martinez-Julian, A. Guerrero, M. Haro, J. Bisquert, D. Bresser, E. Paillard, S. Passerini and G. Garcia-Belmonte, J. Phys. Chem. C, 2014, 118, (12), 6069 LINK
  51.  D. Bresser, F. Mueller, M. Fiedler, S. Krueger, R. Kloepsch, D. Baither, M. Winter, E. Paillard and S. Passerini, Chem. Mater., 2013, 25, (24), 4977 LINK
  52.  D. Bresser, E. Paillard, E. Binetti, S. Krueger, M. Striccoli, M. Winter and S. Passerini, J. Power Sources, 2012, 206, 301 LINK
  53.  Y. He, X. Yu, G. Li, R. Wang, H. Li, Y. Wang, H. Gao and X. Huang, J. Power Sources, 2012, 216, 131 LINK
  54.  J. Xia, N. N. Sinha, L. P. Chen, G. Y. Kim, D. J. Xiong and J. R. Dahn, J. Electrochem. Soc., 2014, 161, (1), A84 LINK
  55.  S. R. Li, N. N. Sinha, C. H. Chen, K. Xu and J. R. Dahn, J. Electrochem. Soc., 2013, 160, (11), A2014 LINK
  56.  A. J. Smith, J. C. Burns, D. Xiong and J. R. Dahn, J. Electrochem. Soc., 2011, 158, (10), A1136 LINK
  57.  L. E. Downie and J. R. Dahn, J. Electrochem. Soc., 2014, 161, (12), A1782 LINK
  58.  L. E. Downie, K. J. Nelson, R. Petibon, V. L. Chevrier and J. R. Dahn, ECS Electrochem. Lett., 2013, 2, (10), A106 LINK
  59.  C. Yada and C. Brasse, ATZelektronik, 2014, 9, (3), 20 LINK
  60.  K.-H. Choi, S.-J. Cho, S.-H. Kim, Y. H. Kwon, J. Y. Kim and S.-Y. Lee, Adv. Funct. Mater., 2014, 24, (1), 44 LINK
  61.  S.-Y. Lee, K.-H. Choi, W.-S. Choi, Y. H. Kwon, H.-R. Jung, H.-C. Shin and J. Y. Kim, Energy Environ. Sci., 2013, 6, (8), 2414 LINK
  62.  L. Jin, P. C. Howlett, J. M. Pringle, J. Janikowski, M. Armand, D. R. MacFarlane and M. Forsyth, Energy Environ. Sci., 2014, 7, (10), 3352 LINK
  63.  M. Forsyth, T. Chimdi, A. Seeber, D. Gunzelmann and P. C. Howlett, J. Mater. Chem. A, 2014, 2, (11), 3993 LINK
  64.  S. A. Mohd Noor, P. C. Howlett, D. R. MacFarlane and M. Forsyth, Electrochim. Acta, 2013, 114, 766 LINK
  65.  E. I. Izgorodina, D. Golze, R. Maganti, V. Armel, M. Taige, T. J. S. Schubert and D. R. MacFarlane, Phys. Chem. Chem. Phys., 2014, 16, (16), 7209 LINK
  66.  Y. Tominaga and K. Yamazaki, Chem. Commun., 2014, 50, (34), 4448 LINK
  67.  S. Feng, D Shi, F. Liu, L. Zheng, J. Nie, W. Feng, X. Huang, M. Armand and Z. Zhou, Electrochim. Acta, 2013, 93, 254 LINK
  68.  R. Bouchet, S. Maria, R. Meziane, A. Aboulaich, L. Lienafa, J.-P. Bonnet, T. N. T Phan, D. Bertin, D. Gigmes, D. Devaux, R. Denoyel and M. Armand, Nature Mater., 2013, 12, (5), 452 LINK

The Reviewers

Joost-59-1-Jan15-p1 Mario Joost obtained his Diploma and PhD in physical chemistry from the University of Münster, Germany. He spent a postdoctoral year at the Münster Electrochemical Energy Technology (MEET) battery research centre before joining the battery materials research team at the Johnson Matthey Technology Centre, Sonning Common, UK, in 2013. His current research is focused on the development of novel electrolytes for next generation battery systems, including Li-air and Li-sulfur.

Joost-59-1-Jan15-p2 Sam Alexander obtained a Masters degree in Chemistry from the University of Sheffield, UK, before completing a PhD in Materials Chemistry at University College London, UK, in 2012, focusing on solid state synthesis of complex metal oxides. Subsequently he joined the Johnson Matthey Technology Centre, Sonning Common, in 2012. His current research is focused on the development of high energy cathode materials for Li-ion batteries.

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