Research in lithium-ion batteries

Research in lithium-ion batteries has produced many proposed refinements of lithium-ion batteries. Areas on research interest have focused on improving energy density, safety, rate capability, cycle durability, flexibility, and cost.


Lithium-ion battery anodes have traditionally been made of graphite. At this time, significant other classes of lithium-ion battery anode materials have been proposed and evaluated as alternatives to graphite, especially in cases where niche applications require novel approaches.

Intercalation oxides

Several types of metal oxides and sulfides can reversibly intercalate lithium cations at voltages between 1 and 2V against lithium metal with little difference between the charge and discharge steps. Specifically the mechanism of insertion involves lithium cations filling crystallographic vacancies in the host lattice with minimal changes to the bonding within the host lattice. This differentiates intercalation anodes from conversion anodes that store lithium by complete disruption and formation of alternate phases, usually as lithia. Conversion systems typically disproportionate to lithia and a metal (or lower metal oxide) at low voltages, < 1V vs Li, and reform the metal oxide at voltage > 2V, for example, CoO + 2Li --> Co+Li2O.

Titanium dioxide

In 1984, researchers at Bell Labs reported the synthesis and evaluation of a series of lithiated titanates. Of specific interest were the anatase form of titanium dioxide and the lithium spinel LiTi2O4 [1] Anatase has been observed to have a maximum capacity of 150 mAh/g (0.5Li/Ti)with the capacity limited by the availability of crystallographic vacancies in the framework. The TiO2 polytype brookite has also been evaluated and found to be electrochemically active when produced as nanoparticles with a capacity approximately half that of anatase (0.25Li/Ti). In 2014, researchers at Nanyang Technological University used a materials derived from a titanium dioxide gel derived from naturally spherical titanium dioxide particles into nanotubes[2] In addition, a non-naturally occurring electrochemically active titanate referred to as TiO2(B) can be made by ion-exchange followed by dehydration of the potassium titanate K2Ti4O9.[3] This layered oxide can be produced in multiple forms including nanowires, nanotubes, or oblong particles with an observed capacity of 210 mAh/g in the voltage window 1.5-2.0V (vs Li).


In 2011, Lu et al., reported reversible electrochemical activity in the porous niobate KNb5O13.[4] This material inserted approximately 3.5Li per formula unit (about 125 mAh/g) at a voltage near 1.3V (vs Li). This lower voltage (compared to titantes) is useful in systems where higher energy density is desirable without significant SEI formation as it operates above the typical electrolyte breakdown voltage.

Transition-metal oxides

In 2000, researchers from the Université de Picardie Jules Verne examined the use of nano-sized transition-metal oxides as conversion anode materials. The metals used were cobalt, nickel, copper, and iron, which proved to have capacities of 700 mA h/g and maintain full capacity for 100 cycles. The materials operate by reduction of the metal cation to either metal nanoparticles or to a lower oxidation state oxide. These promising results show that transition-metal oxides may be useful in ensuring the integrity of the lithium-ion battery over many discharge-recharge cycles.[5]


Lithium anodes were used for the first lithium-ion batteries in the 1960s, based on the TiS
cell chemistry, but were eventually replaced due to dendrite formation which caused internal short-circuits and was a fire hazard.[6][7] Replaced in commercial cell designs in the late-1970s by graphite carbon, effort continued in areas that required lithium, including charged cathodes such as manganese dioxide, vanadium pentoxide, or molybdenum oxide and some polymer electrolyte based cell designs. The interest in lithium metal anodes was re-established with the increased interest in high capacity lithium-air battery and lithium-sulfur battery systems.

Research to inhibit dendrite formation has been an active area due in part to the need for a stable anode for these new beyond-lithium energy storage chemistries. Doron Aurbach and co-workers at Bar-Ilan University have extensively studied the role of solvent and salt in the formation of films on the lithium surface. Notable observations were the addition of LiNO3, dioxolane, and hexafluoroarsenate salts all appeared to create films that inhibit dendrite formation while incorporating reduced Li3As as a lithium-ion conductive component.[8][9]

Non-graphitic carbon

Various forms of carbon are used in lithium-ion battery cell configurations. Besides graphite poorly or non-electrochemically active types of carbon are used in cells such as CNTs, carbon black, graphene, graphene oxides, or MWCNTs.

Recent work includes efforts in 2014 by researchers at Northwestern University who found that metallic single-walled carbon nanotubes (SWCNTs) accommodate lithium much more efficiently than their semiconducting counterparts. If made denser, semiconducting SWCNT films take up lithium at levels comparable to metallic SWCNTs.[10]

In 2015 hydrogen-treated graphene nanofoam electrodes in LIBs showed higher capacity and faster transport. Chemical synthesis methods used in standard anode manufacture leave significant amounts of atomic hydrogen. Experiments and multiscale calculations revealed that low-temperature hydrogen treatment of defect-rich graphene can improve rate capacity. The hydrogen interacts with the graphene defects to open gaps to facilitate lithium penetration, improving transport. Additional reversible capacity is provided by enhanced lithium binding near edges, where hydrogen is most likely to bind.[11] Rate capacities increased by 17–43% at 200 mA/g.[12] In 2015, researchers in China used porous graphene as the material for a lithium ion battery anode in order to increase the specific capacity and binding energy between lithium atoms at the anode. The properties of the battery can be tuned by applying strain. The binding energy increases as biaxial strain is applied.[13]


Silicon is an earth abundant element, and is fairly inexpensive to refine to high purity. When alloyed with lithium it has a theoretical capacity of ~3,600 milliampere hours per gram (mAh/g), which is nearly 10 times the energy density of graphite electrodes (372 mAh/g).[14] One of silicon's inherent traits, unlike carbon, is the expansion of the lattice structure by as much as 400% upon full lithiation (charging). For bulk electrodes, this causes great structural stress gradients within the expanding material, inevitably leading to fractures and mechanical failure, which significantly limits the lifetime of the silicon anodes.[15][16] In 2011, a group of researchers assembled data tables that summarized the morphology, composition, and method of preparation of those nanoscale and nanostructured silicon anodes, along with their electrochemical performance.[17]

Porous silicon nanoparticles are more reactive than bulk silicon materials and tend to have a higher weight percentage of silica as a result of the smaller size. Porous materials allow for internal volume expansion to help control overall materials expansion. Methods include a silicon anode with an energy density above 1,100 mAh/g and a durability of 600 cycles that used porous silicon particles using ball-milling and stain-etching.[14] In 2013, researchers developed a battery made from porous silicon nanoparticles.[18][19] Below are various structural morphologies attempted to overcome issue with silicon's intrinsic properties.

Silicon encapsulation

As a method to control the ability of fully lithiated silicon to expand and become electronically isolated, a method for caging 3 nm-diameter silicon particles in a shell of graphene was reported in 2016. The particles were first coated with nickel. Graphene layers then coated the metal. Acid dissolved the nickel, leaving enough of a void within the cage for the silicon to expand. The particles broke into smaller pieces, but remained functional within the cages.[20][21]

In 2014 researchers encapsulated silicon nanoparticles inside carbon shells, and then encapsulated clusters of the shells with more carbon. The shells provide enough room inside to allow the nanoparticles to swell and shrink without damaging the shells, improving durability.[22]

Silicon nanowire

Porous-silicon inorganic-electrode design

In 2012, Vaughey, et al., reported a new all-inorganic electrode structure based on electrochemically active silicon particles bound to a copper substrate by a Cu3Si intermetallic.[23][24] Copper nanoparticles were deposited on silicon particles articles, dried, and laminated onto a copper foil. After annealing, the copper nanoparticles annealed to each other and to the copper current collector to produce a porous electrode with a copper binder once the initial polymeric binder burned out. The design had performance similar to conventional electrode polymer binders with exceptional rate capability owing to the metallic nature of the structure and current pathways.

Silicon nanofiber

In 2015 a prototype electrode was demonstrated that consists of sponge-like silicon nanofibers increases Coulombic efficiency and avoids the physical damage from silicon's expansion/contractions. The nanofibers were created by applying a high voltage between a rotating drum and a nozzle emitting a solution of tetraethyl orthosilicate (TEOS). The material was then exposed to magnesium vapors. The nanofibers contain 10 nm diameter nanopores on their surface. Along with additional gaps in the fiber network, these allow for silicon to expand without damaging the cell. Three other factors reduce expansion: a 1 nm shell of silicon dioxide; a second carbon coating that creates a buffer layer; and the 8-25 nm fiber size, which is below the size at which silicon tends to fracture.[25]

Conventional lithium-ion cells use binders to hold together the active material and keep it in contact with the current collectors. These inactive materials make the battery bigger and heavier. Experimental binderless batteries do not scale because their active materials can be produced only in small quantities. The prototype has no need for current collectors, polymer binders or conductive powder additives. Silicon comprises over 80 percent of the electrode by weight. The electrode delivered 802 mAh/g after more than 600 cycles, with a Coulombic efficiency of 99.9 percent.[25]


Lithium tin Zintl phases, discovered by Eduard Zintl,have been studied as anode materials in lithium-ion energy storage systems for several decades. First reported in 1981 by Robert Huggins,[26] the system has a multiphase discharge curve and stores approximately 1000 mAh/g (Li22Sn5). Tin and its compounds have been extensively studied but, similar to silicon or germanium anode systems, issues associated with volume expansion (associated with gradual filling of p-orbitals and essential cation insertion), unstable SEI formation, and electronic isolation have been studied in an attempt to commercialize these materials. In 2013, work on morphological variation by researchers at Washington State University used standard electroplating processes to create nanoscale tin needles that show 33% lower volume expansion during charging.[27][28]

Intermetallic insertion materials

As for oxide intercalation (or insertion) anode materials, similar classes of materials where the lithium cation is inserted into crystallographic vacancies within a metal host lattice have been discovered and studied since 1997. In general because of the metallic lattice, these types of materials, for example Cu6Sn5,[29] Mn2Sb,[30] lower voltages and higher capacities have been found when compared to their oxide counterparts.


Cu6Sn5 is an intermetallic alloy with a defect NiAs type structure. In NiAs type nomenclature it would have the stoichiometry Cu0.2CuSn, with 0.2 Cu atoms occupying a usually unoccupied crystallographic position in the lattice. These copper atoms are displaced to the grain boundaries when charged to form Li2CuSn. With retention of most of the metal-metal bonding down to 0.5V, Cu6Sn5 has become an attractive potential anode material due to its high theoretical specific capacity, resistance against Li metal plating especially when compared to carbon-based anodes, and ambient stability.[29][31][32] In this and related NiAs-type materials, lithium intercalation occurs through an insertion process to fill the two crystallographic vacancies in the lattice, at the same time as the 0.2 extra coppers are displaced to the grain boundaries. Efforts to charge compensate the main group metal lattice to remove the excess copper have had limited success.[33] Although significant retention of structure is noted down to the ternary lithium compound Li2CuSn, over discharging the material results in disproportionation with formation of Li22Sn5 and elemental copper. This complete lithiation is accompanied by volume expansion of approximately 250%. Current research focuses on investigating alloying and low dimensional geometries to mitigate mechanical stress during lithiation. Alloying tin with elements that do not react with lithium, such as copper, has been shown to reduce stress. As for low dimensional applications, thin films have been produced with discharge capacities of 1127 mAhg−1 with excess capacity assigned to lithium ion storage at grain boundaries and associated with defect sites.[34] Other approaches include making nanocomposites with Cu6Sn5 at its core with a nonreactive outer shell, SnO2-c hybrids have been shown to be effective,[35] to accommodate volume changes and overall stability over cycles.

Copper antimonide

The layered intermetallic materials derived from the Cu2Sb-type structure are attractive anode materials due to the open gallery space available and structural similarities to the discharge Li2CuSb product. First reported in 2001 [36] In 2011, researchers reported a method to create porous three dimensional electrodes materials based on electrodeposited antimony onto copper foams followed by a low temperature annealing step. It was noted to increase the rate capacity by lowering the lithium diffusion distances while increasing the surface area of the current collector.[24] In 2015 researchers announced a solid-state 3-D battery anode using the electroplated copper antimonide (copper foam). The anode is then layered with a solid polymer electrolyte that provides a physical barrier across which ions (but not electrons) can travel. The cathode is an inky slurry. The volumetric energy density was up to twice as much energy conventional batteries. The solid electrolyte prevents dendrite formation.[37]

Three-dimensional nanostructure

Nanoengineered porous electrodes have the advantage of short diffusion distances, room for expansion and contraction, and high activity. In 2006 an example of a three dimensional engineered ceramic oxide based on lithium titante was reported that had dramatic rate enhancement over the non-porous analogue.[38] Later work by Vaughey et al., highlighted the utility of electrodeposition of electroactive metals on copper foams to create thin film intermetallic anodes. These porous anodes have high power in addition to higher stability as the porous open nature of gthe electrode allows for space to absorb some of the volume expansion. In 2011, researchers at University of Illinois at Urbana-Champaign discovered that wrapping a thin film into a three-dimensional nanostructure can decrease charge time by a factor of 10 to 100. The technology is also capable of delivering a higher voltage output.[39] In 2013, the team improved the microbattery design, delivering 30 times the energy density 1,000x faster charging.[40] The technology also delivers better power density than supercapacitors. The device achieved a power density of 7.4 W/cm2/mm.[41]


In 2016 researchers announced an anode composed of a slurry of Lithium-iron phosphate and graphite with a liquid electrolyte. They claimed that the technique increased safety (the anode could be deformed without damage) and energy density.[42] A flow battery without carbon, called Solid Dispersion Redox Flow Battery, was reported, proposing increased energy density and high operating efficiencies.[43][44] A review of different semi-solid battery systems can be found here.[45]


Several varieties of cathode exist, but typically they can easily divided into two categories, namely charged and discharged. Charged cathodes are materials with pre-existing crystallographic vacancies. These materials, for instance spinels, vanadium pentoxide, molybdenum oxide or LiV3O8, typically are tested in cell configurations with a lithium metal anode as they need a source of lithium to function. While not as common in secondary cell designs, this class is commonly seen in primary batteries that do not require recharging, such as implantable medical device batteries. The second variety are discharged cathodes where the cathode typically in a discharged state (cation in a stable reduced oxidation state), has electrochemically active lithium, and when charged, crystallographic vacancies are created. Due to their increased manufacturing safety and without the need for a lithium source at the anode, this class is more commonly studied. Examples include lithium cobalt oxide, lithium nickel manganese cobalt oxide NMC, or lithium iron phosphate olivine which can be combined with most anodes such as graphite, lithium titanate spinel, titanium oxide, silicon, or intermetallic insertion materials to create a working electrochemical cell.

Vanadium oxides

Vanadium oxides have been a common class of cathodes to study due to their high capacity, ease of synthesis, and electrochemical window that matches well with common polymer electrolytes. Vanadium oxides cathodes, typically classed as charged cathodes, are found in many different structure types. These materials have been extensively studied by Stanley Whittingham among others.[46][47][48] In 2007, Subaru introduced a battery with double the energy density while only taking 15 minutes for an 80% charge. They used a nanostructured vanadium oxide, which is able to load two to three times more lithium ions onto the cathode than the layered lithium cobalt oxide.[49] In 2013 researchers announced a synthesis of hierarchical vanadium oxide nanoflowers (V10O24·nH2O) synthesized by an oxidation reaction of vanadium foil in a NaCl aqueous solution. Electrochemical tests demonstrate deliver high reversible specific capacities with 100% coulombic efficiency, especially at high C rates (e.g., 140 mAh g−1 at 10 C).[50] In 2014, researchers announced the use of vanadate-borate glasses (V2O5 – LiBO2 glass with reduced graphite oxide) as a cathode material. The cathode achieved around 1000 Wh/kg with high specific capacities in the range of ~ 300 mAh/g for the first 100 cycles.[51]

Disordered materials

In 2014, researchers at Massachusetts Institute of Technology found that creating high lithium content lithium-ion batteries materials with cation disorder among the electroactive metals could achieved 660 watt-hours per kilogram at 2.5 volts.[52] The materials of the stoichiometry Li2MO3-LiMO2 are similar to the lithium rich lithium nickel manganese cobalt oxide (NMC) materials but without the cation ordering. The extra lithium creates better diffusion pathways and eliminates high energy transition points in the structure that inhibit lithium diffusion.


In 2015 researchers blended powdered vanadium pentoxide with borate compounds at 900 C and quickly cooled the melt to form glass. The resulting paper-thin sheets were then crushed into a powder to increase their surface area. The powder was coated with reduced graphite oxide (RGO) to increase conductivity while protecting the electrode. The coated powder was used for the battery cathodes. Trials indicated that capacity was quite stable at high discharge rates and remained consistently over 100 charge/discharge cycles. Energy density reached around 1,000 watt-hours per kilogram and a discharge capacity that exceeded 300 mAh/g.[53]


Used as the cathode for a lithium-sulfur battery this system has high capacity on the formation of Li2S. In 2014, researchers at USC Viterbi School of Engineering used a graphite oxide coated sulfur cathode to create a battery with 800 mAh/g for 1,000 cycles of charge/discharge, over 5 times the energy density of commercial cathodes. Sulfur is abundant, low cost and has low toxicity. Sulfur has been a promising cathode candidate owing to its high theoretical energy density, over 10 times that of metal oxide or phosphate cathodes. However, sulfur's low cycle durability has prevented its commercialization. Graphene oxide coating over sulfur is claimed to solve the cycle durability problem. Graphene oxide high surface area, chemical stability, mechanical strength and flexibility.[14]


In 2012, researchers at Polyplus Corporation created a battery with an energy density more than triple that of traditional lithium-ion batteries using the halides or organic materials in seawater as the active cathode. Its energy density is 1,300 W·h/kg, which is a lot more than the traditional 400 W·h/kg. It has a solid lithium positive electrode and a solid electrolyte. It could be used in underwater applications.[54]

Lithium-based cathodes

Lithium nickel manganese cobalt oxide

In 1998, a team from Argonne National Laboratory reported on the discovery of lithium rich NMC cathodes.[55], [56] These high capacity high voltage materials consist of nanodomains of the two structurally similar but different materials. On first charge, noted by its long plateau around 4.5V (vs Li), the activation step creates a structure that gradually equilibrates to a more stable materials by cation re-positioning from high energy points to lower energy points in the lattice. The intellectual property surrounding these materials has been licensed to several manufacturers including BASF, General Motors for the Chevy Volt and Chevy Bolt, and Toda. The mechanism for the high capacity and the gradual voltage fade has been extensively examined. It is generally believed the high voltage activation step induces various cation defects that on cycling equilibrate through the lithium-layer sites to a lower energy state that exhibits a lower cell voltage but with a similar capacity [57], [58].

Lithium iron phosphate

LiFePO4 is a 3.6V lithium-ion battery cathode initially reported by John Goodenough and is structurally related to the mineral olivine and consists of a three dimensional lattice of an [FePO4] framework surrounding a lithium cation. The lithium cation sits in a one dimensional channel along the [010] axis of the crystal structure. This alignment yields anisotropic ionic conductivity that has implications for its usage as a battery cathode and makes morphological control an important variable in its electrochemical cell rate performance. Although the iron analogue is the most commercial owing to its stability, the same composition exists for nickel, manganese, and cobalt although the observed high cell charging voltages and synthetic challenges for these materials make them viable but more difficult to commercialize. While the material has good ionic conductivity it possesses poor intrinsic electronic conductivity. This combination makes nanophase compositions and composites or coatings (to increase electronic conductivity of the whole matrix) with materials such as carbon advantageous. Alternatives to nanoparticles include mesoscale structure such as nanoball batteries of the olivine LiFePO4 that can have rate capabilities two orders of magnitude higher than randomly ordered materials. The rapid charging is related to the nanoballs high surface area where electrons are transmitted to the surface of the cathode at a higher rate.

In 2012, researchers at A123 Systems developed a battery that operates in extreme temperatures without the need for thermal management material. It went through 2,000 full charge-discharge cycles at 45 C while maintaining over 90% energy density. It does this using a nanophosphate positive electrode.[59][60]

Lithium manganese silicon oxide

A “lithium orthosilicate-related” cathode compound,  Li
, was able to support a charging capacity of 335 mAh/g.[61] Li2MnSiO4@C porous nanoboxes were synthesized via a wet-chemistry solid-state reaction method. The material displayed a hollow nanostructure with a crystalline porous shell composed of phase-pure Li2MnSiO4 nanocrystals. Powder X-ray diffraction patterns and transmission electron microscopy images revealed that the high phase purity and porous nanobox architecture were achieved via monodispersed MnCO3@SiO2 core–shell nanocubes with controlled shell thickness.[62]


In 2009, researchers at the University of Dayton Research Institute announced a solid-state battery with higher energy density that uses air as its cathode. When fully developed, the energy density could exceed 1,000 Wh/kg.[63][64] In 2014, researchers at the School of Engineering at the University of Tokyo and Nippon Shokubai discovered that adding cobalt to the lithium oxide crystal structure gave it seven times the energy density.[65][66] In 2017, researchers at University of Virginia reported a scalable method to produce sub-micrometer scale lithium cobalt oxide.[67]

Iron fluoride

Iron fluoride, a potential intercalation-conversion cathode, presents a high theoretical energy density of 1922 Wh kg−1. This material displays poor electrochemical reversibility. When doped with cobalt and oxygen, reversibility improves to over 1000 cycles and capacity reaches 420 mAh g−1. Doping changes the reaction from less-reversible intercalation-conversion to a highly reversible intercalation-extrusion.[68]


Currently, electrolytes are typically made of lithium salts in a liquid organic solvent. Common solvents are organic carbonates (cyclic, straight chain), sulfones, imides, polymers (polyethylene oxide) and fluorinated derivatives. Common salts include LiPF6, LiBF4, LiTFSI, and LiFSI. Research centers on increased safety via reduced flammability and reducing shorts via preventing dendrites.


In 2014, researchers at University of North Carolina found a way to replace the electrolyte’s flammable organic solvent with nonflammable perfluoropolyether (PFPE). PFPE is usually used as an industrial lubricant, e.g., to prevent marine life from sticking to the ship bottoms. The material exhibited unprecedented high transference numbers and low electrochemical polarization, indicative of a higher cycle durability.[69]


While no solid-state batteries have reached the market, multiple groups are researching this alternative. The notion is that solid-state designs are safer because they prevent dendrites from causing short circuits. They also have the potential to substantially increase energy density because their solid nature prevents dendrite formation and allows the use of pure metallic lithium anodes. They may have other benefits such as lower temperature operation.

In 2015 researchers announced an electrolyte using superionic lithium-ion conductors, which are compounds of lithium, germanium, phosphorus and sulfur.[70]


In 2015, researchers worked with a lithium carbon fluoride battery. They incorporated a solid lithium thiophosphate electrolyte wherein the electrolyte and the cathode worked in cooperation, resulting in capacity 26 percent. Under discharge, the electrolyte generates a lithium fluoride salt that further catalyzes the electrochemical activity, converting an inactive component to an active one. More significantly, the technique was expected to substantially increase battery life.[71]

Glassy electrolytes

In March 2017, researchers announced a solid-state battery with a glassy ferroelectric electrolyte of lithium, oxygen, and chlorine ions doped with barium, a lithium metal anode, and a composite cathode in contact with a copper substrate. A spring behind the copper cathode substrate holds the layers together as the electrodes change thickness. The cathode comprises particles of sulfur "redox center", carbon, and electrolyte. During discharge, the lithium ions plate the cathode with lithium metal and the sulfur is not reduced unless irreversible deep discharge occurs. The thickened cathode is a compact way to store the used lithium. During recharge, this lithium moves back into the glassy electrolyte and eventually plates the anode, which thickens. No dendrites form.[72] The cell has 3 times the energy density of conventional lithium-ion batteries. An extended life of more than 1,200 cycles was demonstrated. The design also allows the substitution of sodium for lithium minimizing lithium environmental issues.[73]



Conventional electrolytes generally contain halogens, which are toxic. In 2015 researchers claimed that these materials could be replaced with non-toxic superhalogens with no compromise in performance. In superhalogens the vertical electron detachment energies of the moieties that make up the negative ions are larger than those of any halogen atom.[74] The researchers also found that the procedure outlined for Li-ion batteries is equally valid for other metal-ion batteries, such as sodium-ion or magnesium-ion batteries.[75]


In 2015, researchers at the University of Maryland and the Army Research Laboratory showed significantly increased stable potential windows for aqueous electrolytes with very high salt concentration.[76][77][78] By increasing the molality of Bis(trifluoromethane)sulfonimide lithium salt to 21 m, the potential window could be increased from 1.23 to 3 V due to the formation of SEI on the anode electrode, which has previously only been accomplished with non-aqueous electrolytes.[79] Using aqueous rather than organic electrolyte could significantly improve the safety of Li-ion batteries.[76]

Design and management


In 2014, researchers at MIT, Sandia National Laboratories, Samsung Advanced Institute of Technology America and Lawrence Berkeley National Laboratory discovered that uniform charging could be used with increased charge speed to speed up battery charging. This discovery could also increase cycle durability to ten years. Traditionally slower charging prevented overheating, which shortens cycle durability. The researchers used a particle accelerator to learn that in conventional devices each increment of charge is absorbed by a single or a small number of particles until they are charged, then moves on. By distributing charge/discharge circuitry throughout the electrode, heating and degradation could be reduced while allowing much greater power density.[80][81]

In 2014, researchers at Qnovo developed software for a smartphone and a computer chip capable of speeding up re-charge time by a factor of 3-6, while also increasing cycle durability. The technology is able to understand how the battery needs to be charged most effectively, while avoiding the formation of dendrites.[82]

In 2019, Chao-Yang Wang from Penn State University found that it is possible to recharge the (conventional) lithium-ion batteries of EV's in under 10 minutes. He did so by heating the battery to 60°C, recharging it and then cooling if quickly afterwards. This causes only very little damage to the batteries. Professor Wang used a thin nickel foil with one end attached to the negative terminal and the other end extending to outside the cell in order to create a third terminal. A temperature sensor attached to a switch completes the circuit.[83]



In 2014, independent researchers from Canada announced a battery management system that increased cycles four-fold, that with specific energy of 110 – 175 Wh/kg using a battery pack architecture and controlling algorithm that allows it to fully utilize the active materials in battery cells. The process maintains lithium-ion diffusion at optimal levels and eliminates concentration polarization, thus allowing the ions to be more uniformly attached/detached to the cathode. The SEI layer remains stable, preventing energy density losses.[84][85]


In 2016 researchers announced a reversible shutdown system for preventing thermal runaway. The system employed a thermoresponsive polymer switching material. This material consists of electrochemically stable, graphene-coated, spiky nickel nanoparticles in a polymer matrix with a high thermal expansion coefficient. Film electrical conductivity at ambient temperature was up to 50 S cm−1. Conductivity decreases within one second by 107-108 at the transition temperature and spontaneously recovers at room temperature. The system offers 103–104x greater sensitivity than previous devices.[86][87]


In 2014, multiple research teams and vendors demonstrated flexible battery technologies for potential use in textiles and other applications.

One technique made li-ion batteries flexible, bendable, twistable and crunchable using the Miura fold. This discovery uses conventional materials and could be commercialized for foldable smartphones and other applications.[88]

Another approached used carbon nanotube fiber yarns. The 1 mm diameter fibers were claimed to be lightweight enough to create weavable and wearable textile batteries. The yarn was capable of storing nearly 71 mAh/g. Lithium manganate (LMO) particles were deposited on a carbon nanotube (CNT) sheet to create a CNT-LMO composite yarn for the cathode. The anode composite yarns sandwiched a CNT sheet between two silicon-coated CNT sheets. When separately rolled up and then wound together separated by a gel electrolyte the two fibers form a battery. They can also be wound onto a polymer fiber, for adding to an existing textile. When silicon fibers charge and discharge, the silicon expands in volume up to 300 percent, damaging the fiber. The CNT layer between the silicon-coated sheet buffered the silicon's volume change and held it in place.[89]

A third approach produced rechargeable batteries that can be printed cheaply on commonly used industrial screen printers. The batteries used a zinc charge carrier with a solid polymer electrolyte that prevents dendrite formation and provides greater stability. The device survived 1,000 bending cycles without damage.[90]

A fourth group created a device that is one hundredth of an inch thick and doubles as a supercapacitor. The technique involved etching a 900 nanometer-thick layer of Nickel(II) fluoride with regularly spaced five nanometer holes to increase capacity. The device used an electrolyte made of potassium hydroxide in polyvinyl alcohol. The device can also be used as a supercapacitor. Rapid charging allows supercapacitor-like rapid discharge, while charging with a lower current rate provides slower discharge. It retained 76 percent of its original capacity after 10,000 charge-discharge cycles and 1,000 bending cycles. Energy density was measured at 384 Wh/kg, and power density at 112 kW/kg.[91]

Volume expansion

Current research has been primarily focused on finding new materials and characterising them by means of specific capacity (mAh/g), which provides a good metric to compare and contrast all electrode materials. Recently, some of the more promising materials are showing some large volume expansions which need to be considered when engineering devices. Lesser known to this realm of data is the volumetric capacity (mAh/cm3) of various materials to their design.


Researchers have taken various approaches to improving performance and other characteristics by using nanostructured materials. One strategy is to increase electrode surface area. Another strategy is to reduce the distance between electrodes to reduce transport distances. Yet another strategy is to allow the use of materials that exhibit unacceptable flaws when used in bulk forms, such as silicon.

Finally, adjusting the geometries of the electrodes, e.g., by interdigitating anode and cathode units variously as rows of anodes and cathodes, alternating anodes and cathodes, hexagonally packed 1:2 anodes:cathodes and alternating anodic and cathodic triangular poles. One electrode can be nested within another.

Carbon nanotubes and nanowires have been examined for various purposes, as have aerogels and other novel bulk materials.

Finally, various nanocoatings have been examined, to increase electrode stability and performance.

Nanosensors is now being integrated in to each cell of the battery. This will help to monitor the state of charge in real time which will be helpful not only for security reason but also be useful to maximize the use of the battery.[92]


In 2016, researchers from CMU found that prismatic cells are more likely to benefit from production scaling than cylindrical cells.[93][94]

See also


  1. Cava, Robert (1978). "The Crystal Structures of Lithium-Inserted Titanium Oxides LixTiO2 anatase, LiTi2O4 Spinel and Li2Ti2O4". Journal of Solid State Chemistry. 53: 64–75. doi:10.1016/0022-4596(84)90228-7.
  2. "Ultra-fast charging batteries that can be 70% recharged in just two minutes". Science Daily. 13 October 2014. Retrieved 7 January 2017.
  3. Fujishima, A; Honda, K (1972). "A New Layered Titanate Produced by Ion Exchange". Nature. 238 (5358): 37–40. doi:10.1038/238037a0. PMID 12635268.
  4. Lu, Yuhao (2011). "Behavior of Li Guest in KNb5O13 Host with One-Dimensional Tunnels and Multiple Interstitial Sites". Chemistry of Materials. 23 (13): 3210–3216. doi:10.1021/cm200958r.
  5. Poizot, P. (2000). "Nano-sized transition-metal oxides as negative-electrode materials for lithium-ion batteries". Nature. 407 (6803): 496–499. Bibcode:2000Natur.407..496P. doi:10.1038/35035045. PMID 11028997.
  6. Whittingham, M.Stanley (1978). "Chemistry of intercalation compounds: Metal guests in chalcogenide hosts". Progress in Solid State Chemistry. 12: 41–99. doi:10.1016/0079-6786(78)90003-1.
  7. Whittingham, M. S. (1976). "Electrical Energy Storage and Intercalation Chemistry". Science. 192 (4244): 1126–1127. Bibcode:1976Sci...192.1126W. doi:10.1126/science.192.4244.1126. PMID 17748676.
  8. Pan, B (1995). "Performance and Safety Behavior of Rechargeable AA Li/LiMnO2 Cell". Journal of Power Sources. 54: 143–47. doi:10.1016/0378-7753(94)02055-8.
  9. Lei, W (2015). "The synergetic effect of lithium polysulfide and lithium nitrate to prevent lithium dendrite growth". Nature Communications. 6: 7436–9. Bibcode:2015NatCo...6.7436L. doi:10.1038/ncomms8436. PMID 26081242.
  10. Nanotubes make for better lithium-ion batteries,, 3 March 2014.
  11. Ye, Jianchao; Ong, Mitchell T.; Heo, Tae Wook; Campbell, Patrick G.; Worsley, Marcus A.; Liu, Yuanyue; Shin, Swanee J.; Charnvanichborikarn, Supakit; Matthews, Manyalibo J. (5 November 2015). "Universal roles of hydrogen in electrochemical performance of graphene: high rate capacity and atomistic origins". Scientific Reports. 5: 16190. Bibcode:2015NatSR...516190Y. doi:10.1038/srep16190. PMC 4633639. PMID 26536830.
  12. Stark, Anne M. (5 November 2015). "Using hydrogen to enhance lithium-ion batteries". Research & Development. Retrieved 10 February 2016.
  13. Wang, Yusheng (2015). "Porous graphene for high capacity lithium ion battery anode material". Applied Surface Science. 363: 318–322. doi:10.1016/j.apsusc.2015.11.264.
  14. Researchers Developing Cheap, Better-Performing Lithium-Ion Batteries, Product Design & Development, 1 April 2014, Megan Hazle
  15. Aricò, Antonino Salvatore; Bruce, Peter; Scrosati, Bruno; Tarascon, Jean-Marie; van Schalkwijk, Walter (May 2005). "Nanostructured materials for advanced energy conversion and storage devices". Nature Materials. 4 (5): 366–377. Bibcode:2005NatMa...4..366A. doi:10.1038/nmat1368. PMID 15867920.
  16. Chan, Candace K.; Peng, Hailin; Liu, Gao; McIlwrath, Kevin; Zhang, Xiao Feng; Huggins, Robert A.; Cui, Yi (16 December 2007). "High-performance lithium battery anodes using silicon nanowires". Nature Nanotechnology. 3 (1): 31–35. doi:10.1038/nnano.2007.411. PMID 18654447.
  17. Szczech, Jeannine R.; Jin, Song (2011). "Nanostructured silicon for high capacity lithium battery anodes". Energy & Environmental Science. 4 (1): 56–72. doi:10.1039/C0EE00281J.
  18. Ben Coxworth (14 February 2013). "Silicon nanoparticles used to create a super-performing battery". New Atlas. Retrieved 7 January 2017.
  19. Ge, Mingyuan; Rong, Jiepeng; Fang, Xin; Zhang, Anyi; Lu, Yunhao; Zhou, Chongwu (12 February 2013). "USC team develops new porous silicon nanoparticle material for high-performance Li-ion anodes". Nano Research. 6 (3): 174–181. doi:10.1007/s12274-013-0293-y. Retrieved 4 June 2013.
  20. Mack, Eric (30 January 2016). "Lithium-ion battery boost could come from "caging" silicon in graphene". New Atlas. Retrieved 6 January 2017.
  21. Li, Yuzhang; Yan, Kai; Lee, Hyun-Wook; Lu, Zhenda; Liu, Nian; Cui, Yi (2016). "Growth of conformal graphene cages on micrometre-sized silicon particles as stable battery anodes". Nature Energy. 1 (2): 15029. Bibcode:2016NatEn...115029L. doi:10.1038/nenergy.2015.29.
  22. Nick Lavars (19 February 2014). "Pomegranate-inspired electrode could mean longer lithium-ion battery life". New Atlas. Retrieved 6 January 2017.
  23. Joyce, C.; Trahy, L; Bauer, Sara; Dogan, Fulya; Vaughey, John (2012). "Metallic Copper Binders for Lithium-Ion Battery Silicon Electrodes". Journal of the Electrochemical Society. 159 (6): A909–15. doi:10.1149/2.107206jes. ISSN 0013-4651.
  24. Trahey, L.; Kung, H; Thackeray, M.; Vaughey, John (2011). "Effect of Electrode Dimensionality and Morphology on the Performance of Cu2Sb Thin Film Electrodes for Lithium Batteries". European Journal of Inorganic Chemistry. 2011 (26): 3984–3988. doi:10.1002/ejic.201100329.
  25. Borghino, Dario (25 February 2015). "Going small with silicon potentially has big implications for lithium-ion battery capacity". New Atlas. Retrieved 6 January 2017.
  26. Boukamp, B.A.; Lesh, G. C.; Huggins, R.A (1981). "All Solid Lithium Electrodes with a Mixed Conductor Matrix". Journal of the Electrochemical Society. 128 (4): 725–29. doi:10.1149/1.2127495.
  27. WSU Researchers Create Super Lithium-ion Battery Retrieved 10 January 2013
  28. "Washington State University Gets Funding to Scale Up New Tin Batteries". MacroCurrent. 30 April 2013. Archived from the original on 28 April 2014. Retrieved 4 June 2013.
  29. Kepler, K.; Vaughey, John; Thackeray, M.M. (1999). "LixCu6Sn5 An Intermetallic Insertion Electrode for Rechargeable Lithium Batteries". Electrochemical and Solid State Letters. 2: 307–309. doi:10.1149/1.1390819.
  30. Fransson, L.; Vaughey, John; Thackeray, M.; Edstrom, K. (2003). "Structural Transformations in Intermetallic Electrode for Lithium Batteries". Journal of the Electrochemical Society. 150: A86–91. doi:10.1149/1.1524610.
  31. Tan, Xin Fu; McDonald, Stuart D.; Gu, Qinfen; Hu, Yuxiang; Wang, Lianzhou; Matsumura, Syo; Nishimura, Tetsuro; Nogita, Kazuhiro (2019). "Characterisation of lithium-ion battery anodes fabricated via in-situ Cu6Sn5 growth on a copper current collector". Journal of Power Sources. 415: 50–61. Bibcode:2019JPS...415...50T. doi:10.1016/j.jpowsour.2019.01.034. ISSN 0378-7753.
  32. Wang, Zhaodong; Shan, Zhongqiang; Tian, Jianhua; Huang, Wenlong; Luo, Didi; Zhu, Xi; Meng, Shuxian (2017). "Immersion-plated Cu6Sn5/Sn composite film anode for lithium ion battery". Journal of Materials Science. 52 (10): 6020–6033. Bibcode:2017JMatS..52.6020W. doi:10.1007/s10853-017-0841-z. ISSN 0022-2461.
  33. Jansen, A.; Clevenger, Jessica; Baebler, Anna; Vaughey, John (2011). "Variable Temperature Performance of Intermetallic Lithium Ion Battery Anode Materials". Journal of Alloys and Compounds. 509: 4457–61. doi:10.1016/j.jallcom.2011.01.0111 (inactive 14 October 2019). ISSN 0925-8388.
  34. Kim, Il Seok.; Vaughey, John; Auciello, Orlando (2008). "Thin Film Cu6Sn5 Electrodes: Synthesis< Properties, and Current Collector Interactions". Journal of the Electrochemical Society. 155: A448–51. doi:10.1149/1.2904525. ISSN 0013-4651.
  35. Hu, Renzong; Waller, Gordon Henry; Wang, Yukun; Chen, Yu; Yang, Chenghao; Zhou, Weijia; Zhu, Min; Liu, Meilin (2015). "Cu6Sn5@SnO2–C nanocomposite with stable core/shell structure as a high reversible anode for Li-ion batteries". Nano Energy. 18: 232–244. doi:10.1016/j.nanoen.2015.10.037. ISSN 2211-2855.
  36. Fransson, L.; Vaughey, J; Benedek, R.; Vaughey, John; Edstrom, K; Thomas, J.; Thackeray, M.M. (2001). "Phase Transition in Lithiated Cu2Sb Anodes for lithium Batteries: An In-Situ X-Ray Diffraction". Electrochemistry Communications. 3: 317–323. doi:10.1016/S1388-2481(01)00140-0. ISSN 1388-2481.
  37. Martin, Richard (25 October 2015). "New Foam Batteries Promise Fast Charging, Higher Capacity". MIT Technology Review. Retrieved 10 February 2016.
  38. Sorenson, E.; Barry, S; Jung, H.K.; Rondinelli, James; Vaughey, John; Poeppelmeier, Kenneth (2006). "Three Dimensionally Ordered Macroporous Li4Ti5O12:Effect of Wall Structure of Electrochemical Performance". Chemistry of Materials. 18: 482–489. doi:10.1021/cm052203y.
  39. Batteries charge very quickly and retain capacity, thanks to new structure, News Bureau Illinois, 21 March 2011, Liz Ahlberg
  40. Small in size, big on power: New microbatteries a boost for electronics, News Bureau Illinois, 16 April 2013, Liz Ahlberg
  41. Pikul, JH; Gang Zhang, H; Cho, J; Braun, PV; King, WP (2013). "High-power lithium ion microbatteries from interdigitated three-dimensional bicontinuous nanoporous electrodes". Nature Communications. 4: 1732. Bibcode:2013NatCo...4.1732P. doi:10.1038/ncomms2747. PMID 23591899.
  42. Woyke, Elizabeth. "A clever twist on the batteries in smartphones could help us better harness wind and solar power". MIT Technology Review. Retrieved 2 February 2017.
  43. Qi, Zhaoxiang; Koenig, Gary M. (15 August 2016). "A carbon-free lithium-ion solid dispersion redox couple with low viscosity for redox flow batteries". Journal of Power Sources. 323: 97–106. Bibcode:2016JPS...323...97Q. doi:10.1016/j.jpowsour.2016.05.033. ISSN 0378-7753.
  44. Qi, Zhaoxiang; Liu, Aaron L.; Koenig, Gary M. (20 February 2017). "Carbon-free Solid Dispersion LiCoO2 Redox Couple Characterization and Electrochemical Evaluation for All Solid Dispersion Redox Flow Batteries". Electrochimica Acta. 228: 91–99. doi:10.1016/j.electacta.2017.01.061. ISSN 0013-4686.
  45. Qi, Zhaoxiang; Koenig, Gary M. (July 2017). "Review Article: Flow battery systems with solid electroactive materials". Journal of Vacuum Science & Technology B, Nanotechnology and Microelectronics: Materials, Processing, Measurement, and Phenomena. 35 (4): 040801. doi:10.1116/1.4983210. ISSN 2166-2746.
  46. Chernova, N.; Roppolo, M; Dillon, Anne; Whittingham, Stanley (2009). "Layered vanadium and molybdenum oxides: batteries and electrochromics". Journal of Materials Chemistry. 19 (17): 2526–2552. doi:10.1039/b819629j.
  47. Zavalij, Peter; Whittingham, Stanley (1999). "Structural chemistry of vanadium oxides with open frameworks". Acta Crystallographica Section B. 55 (5): 627–663. doi:10.1107/S0108768199004000. PMID 10927405.
  48. Chirayil, Thomas; Zavalij, Peter; Whittingham, Stanley (1998). "Hydrothermal Synthesis of vanadium Oxides". Chemistry of Materials. 10 (10): 2629–2640. doi:10.1021/cm980242m.
  49. Loz Blain (2 November 2007). "Subaru doubles the battery range on its electric car concept". New Atlas. Retrieved 7 January 2017.
  50. Tang, Yuxin; Rui, Xianhong; Zhang, Yanyan; Lim, Tuti Mariana; Dong, Zhili; Hng, Huey Hoon; Chen, Xiaodong; Yan, Qingyu; Chen, Zhong (2013). "Vanadium pentoxide cathode materials for high-performance lithium-ion batteries enabled by a hierarchical nanoflower structure via an electrochemical process". J. Mater. Chem. A. 1 (1): 82–88. doi:10.1039/C2TA00351A. ISSN 2050-7488.
  51. Afyon, Semih; Krumeich, Frank; Mensing, Christian; Borgschulte, Andreas; Nesper, Reinhard (19 November 2014). "New High Capacity Cathode Materials for Rechargeable Li-ion Batteries: Vanadate-Borate Glasses". Scientific Reports. 4 (1): 7113. Bibcode:2014NatSR...4E7113A. doi:10.1038/srep07113. ISSN 2045-2322. PMC 5382707. PMID 25408200.
  52. Umair Irfan and ClimateWire (17 January 2014). "Messy Innards Make for a Better Lithium Ion Battery". Scientific American. Retrieved 7 January 2017.
  53. "Glass for battery electrodes". R&D. 13 January 2015. Retrieved 6 January 2017.
  54. "Seawater battery sparks sub dreams". New Scientist. 25 April 2012. Retrieved 22 June 2012.
  55. C. S. Johnson, J. T. Vaughey, M. M. Thackeray, T. E. Bofinger, and S. A. Hackney "Layered Lithium-Manganese Oxide Electrodes Derived from Rock-Salt LixMnyOz (x+y=z) Precursors" 194th Meeting of the Electrochemical Society, Boston, MA, Nov.1-6, (1998)
  56. Thackeray, M.; Kang, S.-H; Johnson, C.S.; Vaughey, John; Benedek, Roy; Hackney, S (2007). "Li2MnO3-Stabilized LiMO2 (M-Mn,Ni,Co)Electrodes for Lithium-Ion Batteries". Journal of Materials Chemistry. 17 (30): 31122–3125. doi:10.1039/b702425h.
  57. Dogan, F.; Croy, J.; Balasubramanian, M.; Slater, M.D.; Iddir, H.; Johnson, C.S.; Vaughey, J.; Key, B. (2015). "Solid State NMR Studies of Li2MnO3 and Li-Rich Cathode Materials: Proton Insertion, Local Structure, and Voltage Fade". Journal of the Electrochemical Society. 162: A235–A243. doi:10.1149/2.1041501jes.
  58. Croy, J.; Balasubramanian, M.; Gallagher, K.; Burrell, A.K. (2015). "Review of the U.S. Department of Energy's "Deep Dive" Effort to Understand Voltage Fade in Li- and Mn-Rich Cathodes". Accounts of Chemical Research. 48 (11): 2813–2821. doi:10.1021/acs.accounts.5b00277. PMID 26451674.
  59. A123 Systems introduces new Nanophosphate EXT Li-ion battery technology with optimized performance in extreme temperatures; OEM micro-hybrid program due next year, Green Car Congress, 12 June 2012
  60. A123's new battery tech goes to extremes, EE Times, 12 June 2012
  61. "A 'breakthrough' in rechargeable batteries for electronic devices and electric vehicles". KurzweilAI. 26 February 2015. Retrieved 6 January 2017.
  62. Yang, X. F.; Yang, J.-H.; Zaghib, K.; Trudeau and, M. L.; Ying, J. Y. (March 2015). "Synthesis of phase-pure Li2MnSiO4@C porous nanoboxes for high-capacity Li-ion battery cathodes". Nano Energy. 12: 305–313. doi:10.1016/j.nanoen.2014.12.021.
  63. Kumar, B.; Kumar, J.; Leese, R.; Fellner, J. P.; Rodrigues, S. J.; Abraham, K. M. (2010). "A Solid-State, Rechargeable, Long Cycle Life Lithium–Air Battery". Journal of the Electrochemical Society. 157: A50. doi:10.1149/1.3256129.
  64. "Researchers Develop Solid-State, Rechargeable Lithium-Air Battery; Potential to Exceed 1,000 Wh/kg". Green Car Congress. 21 November 2009. Retrieved 28 August 2013.
  65. Researchers hard at work to make the workhorse lithium ion battery better, Gigaom, 28 July 2014, Katie Fehrenbacher
  66. New Rechargeable Cell Has 7 Times Higher Energy Density Than Li-ion Cells, Nikkei Technology, 23 July 2014, Motohiko Hamada
  67. Qi, Zhaoxiang; Koenig, Gary M. (16 August 2016). "High-Performance LiCoO2Sub-Micrometer Materials from Scalable Microparticle Template Processing". ChemistrySelect. 1 (13): 3992–3999. doi:10.1002/slct.201600872. ISSN 2365-6549.
  68. Fan, Xiulin; Hu, Enyuan; Ji, Xiao; Zhu, Yizhou; Han, Fudong; Hwang, Sooyeon; Liu, Jue; Bak, Seongmin; Ma, Zhaohui (13 June 2018). "High energy-density and reversibility of iron fluoride cathode enabled via an intercalation-extrusion reaction". Nature Communications. 9 (1): 2324. Bibcode:2018NatCo...9.2324F. doi:10.1038/s41467-018-04476-2. ISSN 2041-1723. PMC 5998086. PMID 29899467.
  69. First nonflammable lithium-ion battery will stop your smartphone, car, and plane from exploding, Extreme Tech, 13 February 2014, Sebastian Anthony
  70. "Rechargeable batteries with almost infinite lifetimes coming, say MIT-Samsung engineers". 24 August 2015. Retrieved 10 February 2016.
  71. Lavars, Nick (4 May 2014). "Dual-functioning electrolyte improves capacity of long-life batteries". New Atlas. Retrieved 6 January 2017.
  72. Braga, M. H.; Grundish, N. S.; Murchison, A. J.; Goodenough, J. B. (2017). "Alternative strategy for a safe rechargeable battery". Energy & Environmental Science. 10: 331–336. doi:10.1039/c6ee02888h.
  73. Hislop, Martin (1 March 2017). "Solid-state EV battery breakthrough from Li-ion battery inventor John Goodenough". North American Energy News. The American Energy News. Retrieved 15 March 2017.
  74. Santanab Giri; Swayamprabha Behera; Puru Jena (14 October 2014). "Superhalogens as Building Blocks of Halogen-Free Electrolytes in Lithium-Ion Batteries". Angewandte Chemie. 126 (50): 14136–14139. doi:10.1002/ange.201408648.
  75. McNeill, Brian (24 October 2014). "Physicists find toxic halogens in Li-ion batteries".
  76. Suo, Liumin; Borodin, Oleg; Gao, Tao; Olguin, Marco; Ho, Janet; Fan, Xiulin; Luo, Chao; Wang, Chunsheng; Xu, Kang (20 November 2015). ""Water-in-salt" electrolyte enables high-voltage aqueous lithium-ion chemistries". Science. 350 (6263): 938–943. doi:10.1126/science.aab1595. ISSN 0036-8075. PMID 26586759.
  77. Suo, Liumin; Borodin, Oleg; Sun, Wei; Fan, Xiulin; Yang, Chongyin; Wang, Fei; Gao, Tao; Ma, Zhaohui; Schroeder, Marshall (13 June 2016). "Advanced High-Voltage Aqueous Lithium-Ion Battery Enabled by "Water-in-Bisalt" Electrolyte". Angewandte Chemie International Edition. 55 (25): 7136–7141. doi:10.1002/anie.201602397. ISSN 1521-3773. PMID 27120336.
  78. Smith, Leland; Dunn, Bruce (20 November 2015). "Opening the window for aqueous electrolytes". Science. 350 (6263): 918. doi:10.1126/science.aad5575. ISSN 0036-8075. PMID 26586752.
  79. Wang, Fei; Lin, Yuxiao; Suo, Liumin; Fan, Xiulin; Gao, Tao; Yang, Chongyin; Han, Fudong; Qi, Yue; Xu, Kang (29 November 2016). "Stabilizing high voltage LiCoO2 cathode in aqueous electrolyte with interphase-forming additive". Energy & Environmental Science. 9 (12): 3666–3673. doi:10.1039/c6ee02604d. ISSN 1754-5706.
  80. Want lithium-ion batteries to last? Slow charging may not be the answer, PC World
  81. Why Lithium Ion Batteries Go Bad, Product Design & Development, 15 September 2014
  82. Software on your smartphone can speed up lithium-ion battery charging by up to 6x, Extreme Tech, 14 August 2014, Sebastian Anthony
  83. "In and out with 10-minute electrical vehicle recharge | Penn State University".
  84. New battery management technology could boost Li-ion capacity by 40%, quadruple recharging cycles, TreeHugger, 5 February 2014, Derek Markham
  85. Long-life laptop battery the tech industry doesn’t want you to have, The Globe and Mail, 6 February 2014, Jordana Divon
  86. "Stanford researchers develop heat-sensitive batteries". ZME Science. 12 January 2016. Retrieved 7 February 2016.
  87. Chen, Zheng; Hsu, Po-Chun; Lopez, Jeffrey; Li, Yuzhang; To, John W. F.; Liu, Nan; Wang, Chao; Andrews, Sean C.; Liu, Jia (11 January 2016). "Fast and reversible thermoresponsive polymer switching materials for safer batteries". Nature Energy. 1 (1): 15009. Bibcode:2016NatEn...115009C. doi:10.1038/nenergy.2015.9.
  88. Origami: The surprisingly simple secret to creating flexible, high-power lithium-ion batteries, Extreme Tech, 5 February 2014, Sebastian Anthony
  89. Sandhana, Lakshmi (30 May 2014). "Scientists create weavable Li-ion fiber battery yarn". New Atlas. Retrieved 7 January 2017.
  90. Lovering, Daniel (18 July 2014). "Flexible, Printed Batteries for Wearable Devices". Technology Review. Retrieved 7 January 2017.
  91. Borghino, Dario (2 May 2014). "Flexible, high-performance battery could soon find its way to your smartwatch". New Atlas. Retrieved 7 January 2017.
  92. "Cooperation with AGM Batteries Ltd in full swing". 12 October 2016. Retrieved 7 January 2017.
  93. Cieza, Rebecca E.; Whitacrea, J.F. (2017). "Comparison between cylindrical and prismatic lithium-ion cell costs using a process based cost model". Journal of Power Sources. 340: 273–281. Bibcode:2017JPS...340..273C. doi:10.1016/j.jpowsour.2016.11.054. economies of scale have already been reached, and future cost reductions from increased production volumes are minimal. Prismatic cells, which are able to further capitalize on the cost reduction from larger formats, can offer further reductions than those possible for cylindrical cells.
  94. "Customized Lithium ion Battery Pack Supplier". LargePower. Retrieved 5 March 2016.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.