Lithium-ion battery

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Lithium-ion battery
Nokia Battery.jpg
Nokia Li-ion battery for powering a mobile phone
Specific energy

100–265 W·h/kg[1][2]

(0.36–0.95 MJ/kg)
Energy density

250–730 W·h/L[2]

(0.90–2.23 MJ/L)
Specific power~250-~340 W/kg[1]
Charge/discharge efficiency80–90%[3]
Energy/consumer-price2.5 W·h/US$
Self-discharge rate8% at 21 °C
15% at 40 °C
31% at 60 °C
(per month)[4]
Cycle durability

400–1200 cycles

Nominal cell voltageNMC 3.6 / 3.7 V, LiFePO4 3.2 V
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Lithium-ion battery
Nokia Battery.jpg
Nokia Li-ion battery for powering a mobile phone
Specific energy

100–265 W·h/kg[1][2]

(0.36–0.95 MJ/kg)
Energy density

250–730 W·h/L[2]

(0.90–2.23 MJ/L)
Specific power~250-~340 W/kg[1]
Charge/discharge efficiency80–90%[3]
Energy/consumer-price2.5 W·h/US$
Self-discharge rate8% at 21 °C
15% at 40 °C
31% at 60 °C
(per month)[4]
Cycle durability

400–1200 cycles

Nominal cell voltageNMC 3.6 / 3.7 V, LiFePO4 3.2 V

A lithium-ion battery (sometimes Li-ion battery or LIB) is a member of a family of rechargeable battery types in which lithium ions move from the negative electrode to the positive electrode during discharge and back when charging. Li-ion batteries use an intercalated lithium compound as the electrode material, compared to the metallic lithium used in non-rechargeable lithium battery.

Lithium-ion batteries are common in consumer electronics. They are one of the most popular types of rechargeable battery for portable electronics, with one of the best energy densities, no memory effect (note, however, that new studies have shown signs of memory effect in lithium-ion batteries[6]), and only a slow loss of charge when not in use. Beyond consumer electronics, LIBs are also growing in popularity for military, electric vehicle and aerospace applications.[7] For example, Lithium-ion batteries are becoming a common replacement for the lead acid batteries that have been used historically for golf carts and utility vehicles. Instead of heavy lead plates and acid electrolyte, the trend is to use a lightweight lithium/carbon negative electrodes and lithium iron phosphate positive electrodes. Lithium-ion batteries can provide the same voltage as lead-acid batteries, so no modification to the vehicle's drive system is required.[8]

Chemistry, performance, cost and safety characteristics vary across LIB types. Handheld electronics mostly use LIBs based on lithium cobalt oxide (LiCoO
), which offers high energy density, but presents safety risks, especially when damaged. Lithium iron phosphate (LFP), lithium manganese oxide (LMO) and lithium nickel manganese cobalt oxide (NMC) offer lower energy density, but longer lives and inherent safety. Such batteries are widely used for electric tools, medical equipment and other roles. NMC in particular is a leading contender for automotive applications. Lithium nickel cobalt aluminum oxide (NCA) and lithium titanate (LTO) are specialty designs aimed at particular niche roles.

Lithium-ion batteries can be dangerous under some conditions and can pose a safety hazard since they contain, unlike other rechargeable batteries, a flammable electrolyte and are also kept pressurized. Because of this the testing standards for these batteries are more stringent than those for acid-electrolyte batteries, requiring both a broader range of test conditions and additional battery-specific tests.[9] This is in response to reported accidents and failures, and there have been battery-related recalls by some companies.


Before commercial introduction[edit]

Varta lithium-ion battery, Museum Autovision, Altlussheim, Germany

Lithium batteries were first proposed by M. S. Whittingham, now at Binghamton University, while working for Exxon in the 1970s.[10] Whittingham used titanium(IV) sulfide and lithium metal as the electrodes.

Reversible intercalation in graphite[11][12] and intercalation into cathodic oxides[13][14] was discovered in the 1970s by J. O. Besenhard at TU Munich. Besenhard proposed its application in lithium cells.[15][16] Electrolyte decomposition and solvent co-intercalation into graphite were severe early drawbacks for battery life.

Primary lithium batteries with metallic lithium negative electrodes pose safety issues. As a result, lithium-ion batteries were developed in which both electrodes are made of a material containing lithium ions.[clarification needed][citation needed]

At Oxford University, England, in 1979, John Goodenough and Koichi Mizushima demonstrated a rechargeable cell with voltage in the 4 V range using lithium cobalt oxide (LiCoO
) as the positive electrode and lithium metal as the negative electrode.[17][clarification needed] This innovation provided the positive electrode material that made LIBs possible. LiCoO
is a stable positive electrode material which acts as a donor of lithium ions, which means that it can be used with a negative electrode material other than lithium metal. By enabling the use of stable and easy-to-handle negative electrode materials, LiCoO
opened a whole new range of possibilities for novel rechargeable battery systems.

In 1977, Samar Basu demonstrated electrochemical intercalation of lithium in graphite at the University of Pennsylvania.[18][19] This led to the development of a workable lithium intercalated graphite electrode at Bell Labs (LiC
)[20] to provide an alternative to the lithium metal electrode battery.

In 1980, Rachid Yazami demonstrated the reversible electrochemical intercalation of lithium in graphite.[21][22] The organic electrolytes available at the time would decompose during charging with a graphite negative electrode, slowing the development of a rechargeable lithium/graphite battery. Yazami used a solid electrolyte to demonstrate that lithium could be reversibly intercalated in graphite through an electrochemical mechanism. The graphite electrode discovered by Yazami is currently (2011-03-20) the most commonly used electrode in commercial lithium ion batteries.

In 1983, Michael M. Thackeray, Goodenough, and coworkers identified manganese spinel as a positive electrode material.[23] Spinel showed great promise, given its low-cost, good electronic and lithium ion conductivity, and three-dimensional structure, which gives it good structural stability. Although pure manganese spinel fades with cycling, this can be overcome with chemical modification of the material.[24] As of 2013 manganese spinel was used in commercial cells.[25]

In 1985, Akira Yoshino assembled a prototype cell using carbonaceous material into which lithium ions could be inserted as one electrode, and lithium cobalt oxide (LiCoO
), which is stable in air, as the other.[26] By using materials without metallic lithium, safety was dramatically improved. LiCoO
enabled industrial-scale production and represents the birth of the current lithium-ion battery.

In 1989, Goodenough and Arumugam Manthiram of the University of Texas at Austin showed that positive electrodes containing polyanions, e.g., sulfates, produce higher voltages than oxides due to the induction effect of the polyanion.[27]

From commercial introduction[edit]

The performance and capacity of lithium-ion batteries increases as development progresses.

In 1991 Sony and Asahi Kasei released the first commercial lithium-ion battery.

In 1996 Goodenough, Akshaya Padhi and coworkers proposed lithium iron phosphate (LiFePO
) and other phospho-olivines (lithium metal phosphates with the same structure as mineral olivine) as positive electrode materials.[28]

In 2002 Yet-Ming Chiang and his group at MIT showed a substantial improvement in the performance of lithium batteries by boosting the material's conductivity by doping it[citation needed] with aluminium, niobium and zirconium. The exact mechanism causing the increase became the subject of widespread debate.[29]

In 2004 Chiang again increased performance by utilizing iron phosphate particles of less than 100 nanometers in diameter. This decreased particle density almost one hundredfold, increased the positive electrode's surface area and improved capacity and performance. Commercialization led to a rapid growth in the market for higher capacity LIBs, as well as a patent infringement battle between Chiang and Goodenough.[29]

As of 2011, lithium-ion batteries accounted for 66% of all portable secondary (i.e., rechargeable) battery sales in Japan.[30]

In June 2012 John Goodenough, Rachid Yazami and Akira Yoshino received the 2012 IEEE Medal for Environmental and Safety Technologies for developing the lithium ion battery.

By 2013 the lithium rechargeable battery had progressed to a lithium vanadium phosphate battery to increase energy efficiency in the forward and reverse reaction.

In 2014 John Goodenough, Yoshio Nishi, Rachid Yazami and Akira Yoshino were rewarded by The National Academy of Engineering for pioneering and leading the groundwork for today’s lithium ion battery. The prize, which is in its 25th year, includes a $500,000 award.[31]

In 2014 batteries stated to have 20% higher capacity than those previously available, with a silicon anode rather than graphite (carbon) anode, were being delivered to smartphone manufacturers.[32]


Cylindrical 18650 lithium iron phosphate cell before closing

The three primary functional components of a lithium-ion battery are the positive and negative electrodes and electrolyte. Generally, the negative electrode of a conventional lithium-ion cell is made from carbon. The positive electrode is a metal oxide, and the electrolyte is a lithium salt in an organic solvent.[33] The electrochemical roles of the electrodes reverse between anode and cathode, depending on the direction of current flow through the cell.

The most commercially popular negative electrode is graphite. The positive electrode is generally one of three materials: a layered oxide (such as lithium cobalt oxide), a polyanion (such as lithium iron phosphate) or a spinel (such as lithium manganese oxide).[34]

The electrolyte is typically a mixture of organic carbonates such as ethylene carbonate or diethyl carbonate containing complexes of lithium ions.[35] These non-aqueous electrolytes generally use non-coordinating anion salts such as lithium hexafluorophosphate (LiPF
), lithium hexafluoroarsenate monohydrate (LiAsF
), lithium perchlorate (LiClO
), lithium tetrafluoroborate (LiBF
) and lithium triflate (LiCF

Depending on materials choices, the voltage, energy density, life and safety of a lithium-ion battery can change dramatically. Recently, novel architectures using nanotechnology have been employed to improve performance.

Pure lithium is highly reactive. It reacts vigorously with water to form lithium hydroxide and hydrogen gas. Thus, a non-aqueous electrolyte is typically used, and a sealed container rigidly excludes moisture from the battery pack.

Lithium ion batteries are more expensive than NiCd batteries but operate over a wider temperature range with higher energy densities. They require a protective circuit to limit peak voltage.

For notebooks or laptops, lithium-ion cells are supplied as part of a battery pack with temperature sensors, voltage converter/regulator circuit, voltage tap, battery charge state monitor and the main connector. These components monitor the state of charge and current in and out of each cell, capacities of each individual cell (drastic change can lead to reverse polarities which is dangerous),[36] temperature of each cell and minimize the risk of short circuits.[37]


Nissan Leaf's lithium-ion battery pack.

Li-ion cells (as distinct from entire batteries) are available in various shapes, which can generally be divided into four groups:[38][full citation needed]

The absence of a case gives pouch cells the highest energy density; however, batteries using pouch and prismatic cells require an external means of containment to prevent expansion when their state-of-charge (SOC) level is high.[39]

Since 2011 several research groups have announced demonstrations of lithium-ion flow batteries that suspend the cathode or anode material in an aqueous or organic solution.[40]


The participants in the electrochemical reactions in a lithium-ion battery are the negative and positive electrodes with the electrolyte providing a conductive medium for Lithium-ions to move between the electrodes.

Both electrodes allow lithium ions to move in and out of their interiors. During insertion (or intercalation) ions move into the electrode. During the reverse process, extraction (or deintercalation), ions move back out. When a lithium-ion based cell is discharging, the positive Lithium ion moves from the negative electrode (usually graphite) and enters the positive electrode (lithium containing compound). When the cell is charging, the reverse occurs.

Useful work is performed when electrons flow through a closed external circuit. The following equations show one example of the chemistry, in units of moles, making it possible to use coefficient x.

The positive electrode half-reaction is:[41]


The negative electrode half reaction is:

x\mathrm{Li^+} + x\mathrm{e^-} + x\mathrm{C_6} \leftrightarrows\ x\mathrm{LiC_6}

The overall reaction has its limits. Overdischarge supersaturates lithium cobalt oxide, leading to the production of lithium oxide,[42] possibly by the following irreversible reaction:

\mathrm{Li^+} + \mathrm{e^-} + \mathrm{LiCoO_2} \rightarrow \mathrm{Li_2O} + \mathrm{CoO}

Overcharge up to 5.2 volts leads to the synthesis of cobalt(IV) oxide, as evidenced by x-ray diffraction:[43]

 \mathrm{LiCoO_2} \rightarrow \mathrm{Li^+} + \mathrm{CoO_2} +\mathrm{e^-}

In a lithium-ion battery the lithium ions are transported to and from the positive or negative electrodes by oxidizing the transition metal, cobalt (Co), in Li
from Co3+
to Co4+
during charge, and reduced from Co4+
to Co3+
during discharge. The cobalt electrode reaction is only reversible for x < 0.5, limiting the depth of discharge allowable. This chemistry was used in the Li-ion cells developed by Sony in 1990.

The cell's energy is equal to the voltage times the charge. Each gram of lithium represents Faraday's constant/6.941 or 13,901 coulombs. At 3 V, this gives 41.7 kJ per gram of lithium, or 11.6 kWh per kg. This is a bit more than the heat of combustion of gasoline, but does not consider the other materials that go into a lithium battery and that make lithium batteries many times heavier per unit of energy.


The cell voltages given in the Electrochemistry section are larger than the potential at which aqueous solutions will electrolyze. Given lithium metal's high reactivity to water, nonaqueous or aprotic solutions are used.

Liquid electrolytes in lithium-ion batteries consist of lithium salts, such as LiPF
, LiBF
or LiClO
in an organic solvent, such as ethylene carbonate, dimethyl carbonate, and diethyl carbonate. A liquid electrolyte acts as a carrier between the positive and negative electrodes when current flows through an external circuit. Typical conductivities of liquid electrolyte at room temperature (20 °C (68 °F)) are in the range of 10 mS/cm (1 S/m), increasing by approximately 30–40% at 40 °C (104 °F) and decreasing slightly at 0 °C (32 °F).[44]

Organic solvents easily decompose on the negative electrodes during charge. When appropriate organic solvents are used as the electrolyte, the solvent decomposes on initial charging and forms a solid layer called the solid electrolyte interphase (SEI),[45] which is electrically insulating yet provides significant ionic conductivity. The interphase prevents further decomposition of the electrolyte after the second charge. For example, ethylene carbonate is decomposed at a relatively high voltage, 0.7 V vs. lithium, and forms a dense and stable interface.[46]

Composite electrolytes based on POE (poly(oxyethylene)) developed by Syzdek et al., provide a relatively stable interface.[47][48] It can be either solid (high molecular weight) and be applied in dry Li-polymer cells, or liquid (low molecular weight) and be applied in regular Li-ion cells.

Room temperature ionic liquids (RTILs) are another approach to limiting the flammability and volatility of organic electrolytes.[49]

Charge and discharge[edit]

During discharge, lithium ions Li+
carry the current from the negative to the positive electrode, through the non-aqueous electrolyte and separator diaphragm.[50]

During charging, an external electrical power source (the charging circuit) applies an over-voltage (a higher voltage but of the same polarity) than that produced by the battery, forcing the current to pass in the reverse direction. The lithium ions then migrate from the positive to the negative electrode, where they become embedded in the porous electrode material in a process known as intercalation.

Charging procedure[edit]

The charging procedures for single Li-ion cells, and complete Li-ion batteries, are slightly different.

  1. Constant current (CC)
  2. Voltage source (CV)
  1. Constant current
  2. Balance (not required once a battery is balanced)
  3. Voltage source

During the constant current phase, the charger applies a constant current to the battery at a steadily increasing voltage, until the voltage limit per cell is reached.

During the balance phase, the charger reduces the charging current (or cycle the charging on and off to reduce the average current) while the state of charge of individual cells is brought to the same level by a balancing circuit, until the battery is balanced. Some fast chargers skip this stage. Some chargers accomplish the balance by charging each cell independently.

During the constant voltage phase, the charger apply a voltage equal to the maximum cell voltage times the number of cells in series to the battery, as the current gradually declines towards 0, until the current is below a set threshold of about 3% of initial constant charge current.

Periodic topping charge about once per 500 hours. Top charging is recommended to be initiated when voltage goes below 4.05 V/cell.

Lithium-ion is charged at approximately 4.2 ± 0.05 V/cell except for "military long life" that uses 3.92 V to extend battery life. Most protection circuits cut off if voltage greater than 4.3 V or temperature greater than 90 °C is reached. Below 2.50 V/cell the battery protection circuit may render the battery unchargeable with regular charging equipment. Most battery circuits stop at 2.7–3.0 V/cell.

Failure to follow current and voltage limitations can result in an explosion.[51]

Charging at high and low temperatures[edit]

Charging temperature limits for Li-ion are stricter than operational limits. Lithium-ion performs well at elevated temperatures; however, prolonged exposure to heat reduces longevity.

Li‑ion batteries offer reasonably good charging performance at cooler temperatures and allow fast-charging in a temperature bandwidth of 5 to 45 °C[citation needed] (41 to 113 °F).[52] Charging should be performed within this temperature range. At temperatures from 0 to 5 °C charging is possible, but the charge current should be reduced. During low-temperature charge the slight temperature rise above ambient due to the internal cell resistance is beneficial. Higher temperatures during charging may lead to battery degradation while charging at temperatures above 45 °C will degrade battery performance, whereas at lower temperatures the internal resistance of the battery will increase, resulting in less charging and longer charging times.[52]

Consumer-grade lithium-ion batteries cannot be charged at temperatures below 0 °C (32 °F). Although the pack appears to be charging normally, permanent plating of metallic lithium can occur on the anode during a subfreezing charge, and cannot be removed with cycling. Batteries with lithium plating are known to be more vulnerable to failure if exposed to vibration or other stressful conditions.[53] Most devices equipped with Li-ion batteries do not allow charging outside of 0-45 °C for safety reasons, except for mobile phones that allow some degree of charging when they detect an emergency call in progress.[54]


Industry produced about 660 million cylindrical lithium-ion cells in 2012; the 18650 format is by far the most popular for cylindrical cells. If Tesla meets its goal of shipping 40,000 Model S electric cars in 2014 and if the 85-kWh battery, which uses 7,000 of these cells, proves as popular overseas as it was in the U.S., in 2014 the Model S alone would use almost 40 percent of global cylindrical battery production.[55] Production is gradually shifting to higher-capacity 3,000+ mAh cells. Annual flat polymer cell demand was expected to exceed 700 million in 2013.[56]


Because lithium-ion batteries can have a variety of positive and negative electrode materials, the energy density and voltage vary accordingly.

The open circuit voltage is higher than aqueous batteries (such as lead acid, nickel-metal hydride and nickel-cadmium).[58] The internal resistance of widely used LiCoO
batteries is higher than that of nickel-metal hydride, nickel-cadmium, LiFePO
and lithium-polymer cells.[59] Internal resistance increases with both cycling and age.[58][60] Rising internal resistance causes the voltage at the terminals to drop under load, which reduces the maximum current draw. Eventually increasing resistance means that the battery can no longer operate for an adequate period.

Batteries with a lithium iron phosphate positive and graphite negative electrodes have a nominal open-circuit voltage of 3.2 V and a typical charging voltage of 3.6 V. Lithium nickel manganese cobalt (NMC) oxide positives with graphite negatives have a 3.7 V nominal voltage with a 4.2 V maximum while charging. The charging procedure is performed at constant voltage with current-limiting circuitry (i.e., charging with constant current until a voltage of 4.2 V is reached in the cell and continuing with a constant voltage applied until the current drops close to zero). Typically, the charge is terminated at 3% of the initial charge current. In the past, lithium-ion batteries could not be fast-charged and needed at least two hours to fully charge. Current-generation cells can be fully charged in 45 minutes or less and some types can reach 90% of full charge in as little as 10 minutes.[61]

Materials used in construction[edit]

The increasing demand for batteries has led vendors and academics to focus on improving the energy density, operating temperature, safety, durability, charging time, output power, and cost of LIB solutions.

Positive electrode[edit]

Positive electrode
TechnologyResearchersTarget applicationDateBenefit
Manganese spinel (LMO)Lucky Goldstar Chemical,[62] NEC, Samsung,[25] Hitachi,[63] Nissan/AESC,[64] EnerDel[65]Hybrid electric vehicle, cell phone, laptop1996durability, cost
Lithium iron phosphateUniversity of Texas/Hydro-Québec,[66] Phostech Lithium Inc., Valence Technology, A123Systems/MIT[67][68]Segway Personal Transporter, power tools, aviation products, automotive hybrid systems, PHEV conversions1996moderate density (2 A·h outputs 70 amperes) operating temperature >60 °C (140 °F)
Lithium nickel manganese cobalt (NMC)Imara Corporation, Nissan Motor,[69][70] Microvast Inc.2008density, output, safety
Lithium Manganese Oxide/NMCSony, Sanyo[71]power, safety (although limited durability)
Lithium iron fluorophosphateUniversity of Waterloo[72]2007durability, cost (replace Li with Na or Na/Li)
5% Vanadium-doped lithium iron phosphate olivineBinghamton University[73]2008output
Lithium purpurinArava Leela Mohana Reddy Rice University[74]2012Organic material, low production cost
90 milliamp hours per gram after 50 charge/discharge cycles
Lithium manganese dioxide on porous tinUniversity of Illinois at Urbana-Champaign[75]automotive, electronics2013energy density, power, fast charge using microstructured porous tin
AirIBM, Polyplus[76]Automotive2012Energy density: up to 10,000 mA·h per gram of positive electrode material. Rechargeable.
AirUniversity of Dayton Research Institute[77][78]automotive2009density, safety
WaterPolyplus Corporation[79][80]Marine2012Energy density: 1300 w·h/kg Non-rechargeable. Solid lithium positive electrode. Solid electrolyte. Reduced self-discharge.

Negative electrode[edit]

Negative electrode
TechnologyDensityDurabilityResearchersTarget applicationDateBenefit
Lithium-titanate battery (LT)9,000Altairnano, Microvast Inc.automotive (Phoenix Motorcars), electrical grid (PJM Interconnection Regional Transmission Organization control area,[81] United States Department of Defense[82]), bus (Proterra)2008output, charging time, durability (safety, operating temperature −50–70 °C (−58–158 °F))[83][dead link]
Lithium vanadium oxide745W·h/lSamsung/Subaru.[84]automotive2007density[85]
Cobalt-oxide nanowires from genetically modified virusMIT2006density, thickness[86]
Three-dimensional (3D) porous particles composed of curved 2D nanolayersspecific energy >2000 mA·h/gGeorgia Institute of Technologyhigh energy batteries for electronics and electrical vehicles2011high efficiency, rapid low-cost synthesis[87]
Iron-phosphate nanowires from genetically modified virusMIT2009density, thickness, self-assembly[88][89][90]
Silicon/titanium dioxide composite nanowires from genetically modified tobacco virus2000mA·h/g150University of Marylandexplosive detection sensors, biomimetic structures, water-repellent surfaces, micro/nanoscale heat pipes2010density, low charge time[91]
Silicon whisker on carbon nanofiber composite800-1000mA·h/gJunqing Ma, Physical sciences, Inc.portable electronics, electrical vehicles, electrical grid2009high capacity, good cycle life, fast rate, low charge time[92]
Silicon nanowires on stainless steel4,200 mA·h/gStanford Universitywireless sensors networks2007circumvents swelling[93][94] (shift from negative to positive electrode limited) but safety issue remains (wire cracking)
Silicon oxide-coated double-walled silicon nanotubes6,000Yi Cui/Stanford University[95][96]Automotive and electronics2012
Silicon nanotubes (or silicon nanospheres) confined within rigid carbon outer shells2400 mA·h/gGeorgia Institute of Technology, MSE, NanoTech Yushin's group[97]stable high energy batteries for cell phones, laptops, netbooks, radios, sensors and electrical vehicles2010ultra-high Coulombic Efficiency and outstanding SEI stability[98]
Silicon nanopowder in a conductive polymer binder1400 mA·h/gLawrence Berkeley National Laboratory [99]Automotive and Electronics2011Compatible with commercial Si, good cycling characteristics
Silicon nanopowder in MgO/C matrix700 mA·h/gBinghamton University [100][101]Automotive and Electronics2011Si was reduced from SiO by Mg during ball-milling and thus simultaneously embedded in MgO. Carbon is incorporated to improve the conductivity. The Si has 99.5+% Charge/discharge efficiency and good cycling characteristics
Silicon oxycarbide-coated carbon nanotubes~225 mA·h/g at 1.6A/g; ~750 mA·h/g at 50 mA/gG Singh/Kansas State University[102]Automotive2013~99.6 % average coulombic efficiency; Negative electrode active weight (1.0 mg/cm2), Thickness (~125 micrometers)
Electro-plated tinWashington State University[96]Consumer electronics2012Reduced cost. 3x capacity vs conventional Li-ion
Solid-state plated copper antimonide nanowire750Prieto battery[96]Consumer electronics2012Reduced charging time from reduced positive/negative electrode gap. Increased energy density.
Boron-doped silicon nanoparticles1,400 mA·h/g at a current rate of 1 A/g, 1,000 mA·h/g at 2 A/g200University of Southern California Chongwu Zhou[103][104]Various2012Ten minute charging time. Scalable construction.
Hard carbonEnerg2[105]Consumer electronics2013greater storage capacity
Silicon/conducting polymer hydrogel2,500 mA·h/g to 1,100 mA·h/g at charge/discharge rate from 0.3 to 3.0 A g-1. Volumetric capacity: ~1,080 mA·h/cm5,000Stanford University[106][107]Various201310x energy density of carbon without destruction caused by 400% negative electrode expansion under charge
Nanomatrix structureVolumetric: 580 W·h/lAmprius[108]Smartphones, providing 1850 mA·h capacity2013Uses silicon and other electrochemicals. Energy density
Carbon-encased silicon nanoparticles2800 mA·h/g at C/101000 at 74% capacityStanford[109]Various2013Commercially available Si nanoparticles sealed inside conformal, self-supporting carbon shells, with rationally designed void space between particles and shell. The space allows Si particles to expand without breaking the outer carbon shell, stabilizing the SEI on the shell surface. Coulombic efficiency of 99.84%.
Lithium/titanium/oxideEner1/Delphi[65]2006durability, safety (limited density)
-plated copper nanorods
Université Paul Sabatier/Université Picardie Jules Verne[110][111]2006density
Nanophosphate2,000A123 Systems[112]


Automotive2012Operation at high and low ambient temperature
Nickel/Tin on porous nickelPower density: 7.4 mW cm−2 μm−1University of Illinois at Urbana-Champaign[115][116]Automotive, electronics2013energy density and power using microstructured metal as the substrate for thin film Nickel/Tin. These are assembled as three-dimensional bicontinuous interdigitated microelectrodes.
Manganese oxide nanowires produced by M13 virusEnergy density: 13,350 mAh g−1c (7,340 mAh g−1c+catalyst)MIT[117]2013Energy density from increased surface produced by genetically engineered M13 virus that produces a roughened surface.


TechnologyDurabilityResearchersTarget applicationDateBenefit
Lithium imide750-800 at 80%Leyden[96]Consumer electronics2012Reduced thermal expansion.
Wax/liquidWashington State[118]Consumer/vehicle electronics2014Reduced fire risk
Perfluoropolyether (PFPE)University of North CarolinaGrid storage, low temperature environments2014Reduced fired risk. Combines with lithium salts, and is nonflammable and thermally stable beyond 200 °C (392 °F). High transference number and electrochemical polarization, both of which relate to battery life and performance. PFPE carries most of its current in the cation (the positive ion), resulting in a transference value higher than most other solvents. Conductivity is relatively low, although high transference may compensate for low conductivity. High-voltage cathode tests confirmed stable operation.[119]


TechnologyDurabilityResearchersTarget applicationDateBenefit
CeramicAutomotive, grid stabilization2008Heat resistance up to 700 °C (1,292 °F)[120]


Li-ion batteries provide lightweight, high energy density power sources for a variety of devices. To power larger devices, such as electric cars, connecting many small batteries in a parallel circuit is more effective[121] and more efficient than connecting a single large battery.[citation needed] Such devices include:

Li-ion batteries are used in telecommunications applications. Secondary non-aqueous lithium batteries provide reliable backup power to load equipment located in a network environment of a typical telecommunications service provider. Li-ion batteries compliant with specific technical criteria are recommended for deployment in the Outside Plant (OSP) at locations such as Controlled Environmental Vaults (CEVs), Electronic Equipment Enclosures (EEEs), and huts, and in uncontrolled structures such as cabinets. In such applications, li-ion battery users require detailed, battery-specific hazardous material information, plus appropriate fire-fighting procedures, to meet regulatory requirements and to protect employees and surrounding equipment.[122]


A lithium-ion battery from a laptop computer (176 kJ)

Batteries gradually self-discharge even if not connected and delivering current. Li+ rechargeable batteries have a self-discharge rate typically stated by manufacturers to be 1.5-2% per month.[123][124] The rate increases with temperature and state of charge. A 2004 study found that for most cycling conditions self-discharge was primarily time-dependent; however, after several months of stand on open circuit or float charge, state-of-charge dependent losses became significant. The self-discharge rate did not increase monotonically with state-of-charge, but dropped somewhat at intermediate states of charge.[125] Self-discharge rates may increase as batteries age.[126]

For comparison, the self-discharge rate is over 30% per month for common nickel metal hydride (NiMH) batteries,[127] dropping to about 1.25% per month for low self-discharge NiMH batteries, and 10% per month in nickel-cadmium batteries.

Battery life[edit]

Rechargeable battery life is often stated in number of charge cycles, but depth of discharge is usually not explicitly stated. Apple Inc. clarify that a charge cycle means using all the battery's capacity, but not necessarily by full charge and discharge; e.g., using half the charge of a fully charged battery, charging it, and then using the same amount of charge again count as a single charge cycle.[128]

It is widely stated on Web sites and other sources, without citing any evidence or source, that "lithium-ion batteries deteriorate over time, whether they're being used or not. So a spare battery won't last much longer than the one in use."[129] However, manufacturers' information clearly indicates that the life of a battery that is not abused depends upon the number of charge cycles it undergoes, specifying typical battery capacity in terms of number of cycles (e.g., capacity dropping linearly to 80% over 500 cycles), with no mention of age of the battery.[130] Battery performance is rarely specified over more than 500 cycles. This means that batteries of mobile phones, or other hand-held devices in daily use, are not expected to last longer than three years. Electric car batteries are even worse, because they experience wide temperature changes. This seriously limits the use of Lithium-ion batteries in electric cars.[citation needed]

All rechargeable batteries degrade with use, the capacity decreasing until it is unusably small. Li+ batteries last longer[129][unreliable source?][dubious ] if not deeply discharged (depleted) before recharging.

Batteries may last longer if not stored fully discharged. As the battery self-discharges over time, its voltage gradually reduces. When depleted below the low-voltage threshold of the protection circuit (2.4 to 2.9 V/cell, depending on chemistry) it will be disabled and cannot be further discharged until recharged.[129] This because as the discharge progresses, the metallic contents of the cell are plated onto its internal structure creating an unwanted discharge path. It is recommended to store batteries at 40% charge level.[129][dubious ]

The rate of degradation of lithium-ion batteries is strongly temperature-dependent; they degrade much faster if stored or used at higher temperatures. The carbon negative electrode of the cell also generates heat. High charge levels and elevated temperatures (whether from charging or ambient air) hasten capacity loss.[58] Poor ventilation may increase temperatures, further shortening battery life. Loss rates vary by temperature: 6% loss at 0 °C (32 °F), 20% at 25 °C (77 °F), and 35% at 40 °C (104 °F). In contrast, the calendar life of LiFePO
cells is not affected by high charge states.[131] They may be stored in a refrigerator.[132][133]

Charging forms deposits inside the electrolyte that inhibit ion transport. The increase in internal resistance reduces the cell's ability to deliver current. This problem is more pronounced in high-current applications. Older batteries also do not charge as much as new ones (charging time required decreases).


The need to "condition" NiCd and NiMH batteries has incorrectly leaked into folklore surrounding Li-ion batteries. The recommendation for the older technologies is to leave the device plugged in for seven or eight hours, even if fully charged.[134] This may be a confusion of battery software calibration instructions with the "conditioning" instructions for NiCd and NiMH batteries.[135] The software of a typical smart phone, for example, learns how to accurately gauge the battery's life by watching it discharge and leaving it on the charger produces a series of "micro discharges" that the software can watch and learn from.[citation needed]

Multicell devices[edit]

Li-ion batteries require a battery management system to prevent operation outside each cell's safe operating area (over-charge, under-charge, safe temperature range) and to balance cells to eliminate state of charge mismatches, thereby significantly improving battery efficiency and increasing overall capacity. As the number of cells and load currents increase, the potential for mismatch increases. The two kinds of mismatch are state-of-charge (SOC) and capacity/energy ("C/E"). Though SOC is more common, each problem limits pack charge capacity (mA·h) to that of the weakest cell.


If overheated or overcharged, Li-ion batteries may suffer thermal runaway and cell rupture.[136] In extreme cases this can lead to combustion. To reduce these risks, lithium-ion battery packs contain fail-safe circuitry that shuts down the battery when its voltage is outside the safe range of 3–4.2 V per cell.[41][127] When stored for long periods the small current draw of the protection circuitry may drain the battery below its shutdown voltage; normal chargers are then ineffective. Many types of lithium-ion cells cannot be charged safely below 0 °C.[137]

Other safety features are required in each cell:[41]

These devices occupy useful space inside the cells, add additional points of failure and irreversibly disable the cell when activated. They are required because the negative electrode produces heat during use, while the positive electrode may produce oxygen. These devices and improved electrode designs reduce/eliminate the risk of fire or explosion. Further, these features increase costs compared to nickel metal hydride batteries, which require only a hydrogen/oxygen recombination device (preventing damage due to mild overcharging) and a back-up pressure valve.[138] Contaminants inside the cells can defeat these safety devices.[clarification needed]

Short-circuiting a battery will cause the cell to overheat and possibly to catch fire. Adjacent cells may then overheat and fail, possibly causing the entire battery to ignite or rupture. In the event of a fire, the device may emit dense irritating smoke.[139] The fire energy content (electrical + chemical) of cobalt-oxide cells is about 100 to 150 kJ per A·h, most of it chemical. Extinguishing this fire is dangerous as lithium burns violently when it comes in contact with water or moisture in the air; a suitable waterless fire extinguisher is recommended.[36][140]

Replacing the lithium cobalt oxide positive electrode material in lithium-ion batteries with a lithium metal phosphate such as lithium iron phosphate improves cycle counts, shelf life and safety, but lowers capacity. As of 2006 these 'safer' lithium-ion batteries were mainly used in electric cars and other large-capacity battery applications, where safety is critical.[141]

Lithium-ion batteries, unlike other rechargeable batteries, have a potentially hazardous pressurised flammable electrolyte, and require strict quality control during manufacture.[142] A faulty battery can cause a serious fire. Faulty chargers can affect the safety of the battery because they can destroy the battery's protection circuit. While charging at temperatures below 0 °C, the negative electrode of the cells gets plated with pure lithium, which can compromise the safety of the whole pack. Battery packs which are not branded by a reputable manufacturer may not be built to the same safety standard as branded ones.

While fire is often serious, it may be catastrophically so. In about 2010 large lithium-ion batteries were introduced in place of other chemistries to power systems on some aircraft; as of January 2014 there had been at least four serious lithium-ion battery fires, or smoke, on the Boeing 787 passenger aircraft, introduced in 2011, which did not cause crashes but had the potential to do so.[143][144]

Environmental concerns and recycling[edit]

Since Li-ion batteries contain no toxic metals (unlike other types of batteries which may contain lead or cadmium)[41] they are generally categorized as non-hazardous waste. Li-ion battery elements including iron, copper, nickel and cobalt are considered safe for incinerators and landfills. These metals can be recycled, but mining generally remains cheaper than recycling.[145] At present, not much is invested into recycling Li-ion batteries due to costs, complexities and low yield. The most expensive metal involved in the construction of the cell is cobalt. Lithium iron phosphate is cheaper but has other drawbacks. Lithium is less expensive than other metals used. The manufacturing processes of nickel and cobalt for the positive electrode and also the solvent, present potential environmental and health hazards.[146][147]


In October 2004 Kyocera Wireless recalled approximately 1 million mobile phone batteries to identify counterfeits.[148]

In December 2006 Dell recalled approximately 22,000 laptop computer batteries.[149] Approximately 10 million Sony batteries used in Dell, Sony, Apple, Lenovo, Panasonic, Toshiba, Hitachi, Fujitsu and Sharp laptops were recalled in 2006. The batteries were found to be susceptible to internal contamination by metal particles during manufacture. Under some circumstances, these particles could pierce the separator, causing a dangerous short-circuit.[150]

In March 2007 computer manufacturer Lenovo recalled approximately 205,000 batteries at risk of explosion. In August 2007 mobile phone manufacturer Nokia recalled over 46 million batteries at risk of overheating and exploding.[151] One such incident occurred in the Philippines involving a Nokia N91, which used the BL-5C battery.[152]

Transport restrictions[edit]

Japan Airlines Boeing 787 lithium cobalt oxide battery that caught fire in 2013

IATA estimates that over a billion lithium cells are flown each year.[140] The United States Department of Transportation has not allowed passengers on commercial aircraft to carry spare lithium batteries (i.e., not installed in a device) in their checked baggage since 1 January 2008. Types of batteries covered by this rule are those containing small amounts of lithium, including Li-ion, lithium polymer, and lithium cobalt oxide chemistries. Lithium-ion batteries containing more than 25 grams (0.88 oz) equivalent lithium content (ELC) are forbidden in US air travel.[153]

Replacement batteries may be transported in carry-on luggage. Tips are provided on safe packaging and carriage of batteries; e.g., such batteries should be in their original protective packaging or in individual containers or plastic bags.[153][154]

Some postal administrations restrict air shipping (including EMS) of lithium and lithium-ion batteries, either separately or installed in equipment. Such restrictions apply in Hong Kong,[155] Australia and Japan.[156]

On 16 May 2012 the United States Postal Service (USPS) banned shipping anything containing a lithium battery to an overseas address, after fires from transport of batteries.[157] This restriction made it difficult to send anything containing lithium batteries to military personnel overseas, as the USPS was the only method of shipment to these addresses; the ban was lifted on 15 November 2012.[158]

The Boeing 787 Dreamliner uses large lithium cobalt oxide[159] batteries, which are more reactive than newer types of batteries such as LiFePO


Researchers are working to improve the power density, safety, cycle durability, recharge time, cost, flexibility and other characteristics of these batteries.

Solid-state design (no electrolyte)[edit]

Solid-state lithium-ion batteries designs[161] have the potential to deliver three times the energy density of typical 2011 lithium-ion batteries at less than half the cost per kilowatt-hour. This approach eliminates binders, separators and liquid electrolytes. By eliminating these, "you can get around 95% of the theoretical energy density of the active materials."[162] Solid-state designs do not overheat or catch fire like traditional lithium-ion batteries can. They are much safer because they do not use liquid electrolyte. Plans are to have products ready for field testing as early as March 2015.[163] Solid-state lithium-ion batteries are probably going to become the standard for electronics that are capable of operating in multiples of 3.2, 3.6 and 3.7 volts, respectively.

Tin electrode[edit]

Washington State University researchers developed a tin negative electrode technology that they predicted would triple the energy capacity of lithium ion batteries. The technology involves using standard electroplating process to create tin nanoneedles that do not shortciruit when the tin expands by one third during charging.[164][165]

Microporous tin has been used as a substrate for negative and positive electrodes that exhibit high energy density, power and fast recharge. The substrate self-assembles. Small spheres are packed onto a surface, forming a lattice. The area between the spheres is coated with the substrate material (nickel). The spheres are dissolved/melted and the resulting surface is electro-polished to enlarge the pores. Finally the substrate is coated with a thin film of the active material (Ni/Sn for negative electrode, LiMnO
for positive).[75][115]

Higher lithium content electrode[edit]

Researchers at Nissan Arc are investigating lithium-rich batteries that may increase energy density by 150% and improve cycle durability.[166]

Silicon anode[edit]

Researchers at Amprius have created a lithium-ion battery that holds 20% more energy than the standard lithium-ion battery and they are in the process of producing higher levels of energy density. Theoretically, they can create a battery that can contain up to ten times as much energy density.[167] They are using a silicon anode, rather than standard graphite (carbon). These new batteries are being produced with all the same materials as the standard.[168]

Pomegranate style electrode for silicon anode[edit]

Researchers have discovered that using a pomegranate-inspired electrode with a silicon anode can reduce swelling while charging and reduce the gunk from the reaction with the electrolyte. This technique involves gathering yolk shells into clusters and then applying another coat of carbon around the cluster.

Researchers have previously overcome these problems by using silicon nanoparticles, which are already too small break. They place the silicon nanoparticles in yolk shells made from carbon, with enough spare room inside for them to swell and shrink without causing damage.[169]

Silicon-carbon anode[edit]

Researchers have developed a battery that blends silicon and carbon that has a dramatic energy density improvement and five times the life cycle improvement than regular silicon anode lithium-ion batteries. The new silicon-anode batteries will allow electric vehicles to go 200–300 miles on a single charge. They are also cost effective and can be produced large scale.[170]

Sticky liquid electrolyte[edit]

Researchers have developed a chewing gum like substance to replace liquid electrolytes. This new material contain liquid electrolyte but is sticky and thus eliminates the fire hazard. This material is also flexible so it can be used with bendable electronics in the future.[171]

Disorder in battery materials[edit]

Creating lithium-ion batteries with disorder in the materials they are composed of has achieved 660 watt-hours per kilogram at 2.5 volts, a result rarely observed even in perfectly structured devices. Lithium-ion batteries are most commonly made of meticulously arranged rigid patterns of materials.[172]


Researchers have discovered a way to make li-ion batteries flexible, bendable, twistable and crunchable using the Miura fold. This discovery comes on the heels of using all the same material of conventional lio-ion batteries and could be commercialized for foldable smartphones and other applications.[173]

Nonflammable perfluoropolyether electrolyte[edit]

Researchers found a way to replace the electrolyte’s flammable organic solvent with nonflammable perfluoropolyether (PFPE), which eliminate the fire hazard. PFPE is usually used as an industrial lubricant. Researchers had originally been looking at using PFPE on the bottom of ships to prevent marine life from sticking, which is a serious problem in the world of shipping. More testing to see if the nonflammable electrolyte can withstand the rigors of everyday use, but they also exhibit unprecedented high transference numbers and low electrochemical polarization, indicative of longer battery life.[174]

Germanium nanowire-based anode[edit]

Researchers have found that germanium nanowire-based anodes more than double the capacity of standard graphite anodes while still retaining high capacity even after being charged and discharged over 1,000 times.[175][176]

Uniformity of li-ions into and out of cathode[edit]

Researchers have discovered a way to raise the charge durability to last four times more than traditional lithium-ion batteries while still maintaining adequate capacity. The process used maintains the lithium-ion diffusion at optimal levels and eliminates concentration polarization and thus allows the Li-ions to be more uniformly extracted from or reinserted into the cathode materials. This maintains the SEI layer at a stable state and prevents battery capacity fading.

Some of the companies interested in this new technology are concerned that this would mean fewer products are sold because the batteries would last so long.[177] This lack of interest in bringing new technology is part of a corporate eco-system that holds technology back.

Architecture and controlling algorithm[edit]

Researchers have discovered a way to store 10-40% more capacity (specific energy of 110 – 175 Wh/kg) using their special battery pack architecture and controlling algorithm that allows it to fully utilize the active materials in battery cells.[178]

Lithium iron phosphate cathode[edit]

Scientists at Massachusetts Institute of Technology have created Nanoball batteries that are capable re-charging 100 times faster than traditional li-ion batteries. They are capable of a 10 second re-charge in the size of a cell phone battery and a 5 minute re-charge in the size of an electric car battery. The cathode portion of the battery is composed of nanosized balls of lithium iron phosphate and the batteries can be charged much faster because the li-ion nanoballs transmit electrons to the surface of the cathode at a much higher rate. The batteries have also shown higher energy density and cycle durability than traditional li-ions. The issue is that the batteries also discharge at the much faster rate.[179][180]

Single-walled carbon nanotubes[edit]

Researchers at Northwestern University have made discoveries about Single-walled carbon nanotubes (SWCNTs) that could help boost their energy density and cycle durability. They found that metallic SWCNTs accommodate lithium much more efficiently than their semiconducting counterparts. Another important discovery was that, if made denser, the semiconducting SWCNT films also begin to take up lithium at levels comparable to metallic SWCNTs. The team is also looking into other nanomaterials for research.[181]

See also[edit]


  1. ^ a b c "Rechargeable Li-Ion OEM Battery Products". Archived from the original on April 13, 2010. Retrieved 23 April 2010. 
  2. ^ a b c "Panasonic Develops New Higher-Capacity 18650 Li-Ion Cells; Application of Silicon-based Alloy in Anode". Retrieved 31 January 2011. 
  3. ^ Valøen, Lars Ole and Shoesmith, Mark I. (2007). The effect of PHEV and HEV duty cycles on battery and battery pack performance (PDF). 2007 Plug-in Highway Electric Vehicle Conference: Proceedings. Retrieved 11 June 2010.
  4. ^ Abe, H.; Murai, T.; Zaghib, K. (1999). "Vapor-grown carbon fiber anode for cylindrical lithium ion rechargeable batteries". Journal of Power Sources 77 (2): 110. doi:10.1016/S0378-7753(98)00158-X.  edit
  5. ^ Battery Types and Characteristics for HEV ThermoAnalytics, Inc., 2007. Retrieved 11 June 2010.
  6. ^ Tsuyoshi Sasaki, Yoshio Ukyo & Petr Novák (14 April 2013). "Memory effect in a lithium-ion battery". 
  7. ^ Ballon, Massie Santos (14 October 2008). "Electrovaya, Tata Motors to make electric Indica". Cleantech Group. Archived from the original on 2011-05-09. Retrieved 11 June 2010. 
  8. ^ "Explain how lithium batteries work in electric golf carts". LithiumBoost. Retrieved 2013-05-09. 
  9. ^ Millsaps, C. (2012, Jul 10). Second Edition of IEC 62133: The Standard for Secondary Cells and Batteries Containing Alkaline or Other Non-Acid Electrolytes is in its Final Review Cycle. Retrieved from Battery Power Online (2014, Jan 10)
  10. ^ Whittingham, M. S. (1976). "Electrical Energy Storage and Intercalation Chemistry". Science 192 (4244): 1126–1127. doi:10.1126/science.192.4244.1126. PMID 17748676.  edit
  11. ^ Besenhard, J.O. and Fritz, H.P. (1974). "Cathodic Reduction of Graphite in Organic Solutions of Alkali and NR4+ Salts". J. Electroanal. Chem. 53 (2): 329. doi:10.1016/S0022-0728(74)80146-4. 
  12. ^ Besenhard, J. O. (1976). "The electrochemical preparation and properties of ionic alkali metal-and NR4-graphite intercalation compounds in organic electrolytes". Carbon 14 (2): 111–115. doi:10.1016/0008-6223(76)90119-6.  edit
  13. ^ Schöllhorn, R.; Kuhlmann, R.; Besenhard, J. O. (1976). "Topotactic redox reactions and ion exchange of layered MoO3 bronzes". Materials Research Bulletin 11: 83. doi:10.1016/0025-5408(76)90218-X.  edit
  14. ^ Besenhard, J. O.; Schöllhorn, R. (1976). "The discharge reaction mechanism of the MoO3 electrode in organic electrolytes". Journal of Power Sources 1 (3): 267. doi:10.1016/0378-7753(76)81004-X.  edit
  15. ^ Besenhard, J. O.; Eichinger, G. (1976). "High energy density lithium cells". Journal of Electroanalytical Chemistry and Interfacial Electrochemistry 68: 1. doi:10.1016/S0022-0728(76)80298-7.  edit
  16. ^ Eichinger, G.; Besenhard, J. O. (1976). "High energy density lithium cells". Journal of Electroanalytical Chemistry and Interfacial Electrochemistry 72: 1. doi:10.1016/S0022-0728(76)80072-1.  edit
  17. ^ "USPTO search for inventions by "Goodenough, John"". Retrieved 8 October 2011. 
  18. ^ Zanini, M.; Basu, S.; Fischer, J. E. (1978). "Alternate synthesis and reflectivity spectrum of stage 1 lithium—graphite intercalation compound". Carbon 16 (3): 211. doi:10.1016/0008-6223(78)90026-X.  edit
  19. ^ Basu, S.; Zeller, C.; Flanders, P. J.; Fuerst, C. D.; Johnson, W. D.; Fischer, J. E. (1979). "Synthesis and properties of lithium-graphite intercalation compounds". Materials Science and Engineering 38 (3): 275. doi:10.1016/0025-5416(79)90132-0.  edit
  20. ^ US 4304825, Basu; Samar, "Rechargeable battery", issued 8 December 1981, assigned to Bell Telephone Laboratories 
  21. ^ International Meeting on Lithium Batteries, Rome, 27–29 April 1982, C.L.U.P. Ed. Milan, Abstract #23
  22. ^ Yazami, R.; Touzain, P. (1983). "A reversible graphite-lithium negative electrode for electrochemical generators". Journal of Power Sources 9 (3): 365. doi:10.1016/0378-7753(83)87040-2.  edit
  23. ^ Thackeray, M. M.; David, W. I. F.; Bruce, P. G.; Goodenough, J. B. (1983). "Lithium insertion into manganese spinels". Materials Research Bulletin 18 (4): 461. doi:10.1016/0025-5408(83)90138-1.  edit
  24. ^ Nazri, Gholamabbas and Pistoia, Gianfranco (2004). Lithium batteries: science and Technology. Springer. ISBN 1402076282. 
  25. ^ a b Voelcker, John (September 2007). Lithium Batteries Take to the Road. IEEE Spectrum. Retrieved 15 June 2010.
  26. ^ US 4668595, Yoshino; Akira, "Secondary Battery", issued 10 May 1985, assigned to Asahi Kasei 
  27. ^ Manthiram, A.; Goodenough, J. B. (1989). "Lithium insertion into Fe2(SO4)3 frameworks". Journal of Power Sources 26 (3–4): 403. doi:10.1016/0378-7753(89)80153-3.  edit
  28. ^ Padhi, A. K. (1997). "Phospho-olivines as Positive-Electrode Materials for Rechargeable Lithium Batteries". Journal of the Electrochemical Society 144 (4): 1188–1110. doi:10.1149/1.1837571.  edit
  29. ^ a b "In search of the perfect battery" (PDF). The Economist. 6 March 2008. Archived from the original on 25 September 2009. Retrieved 11 May 2010. 
  30. ^ Monthly battery sales statistics. Machinery statistics released by the Ministry of Economy, Trade and Industry, March 2011.
  31. ^ "Lithium Ion Battery Pioneers Receive Draper Prize, Engineering’s Top Honor", University of Texas, Jan. 6, 2014
  32. ^ "At long last, new lithium battery tech actually arrives on the market (and might already be in your smartphone)". ExtremeTech. Retrieved 2014-02-16. 
  33. ^ Silberberg, M. (2006). Chemistry: The Molecular Nature of Matter and Change, 4th Ed. New York (NY): McGraw-Hill Education. p. 935, ISBN 0077216504.
  34. ^ Thackeray, M. M.; Thomas, J. O.; Whittingham, M. S. (2011). "Science and Applications of Mixed Conductors for Lithium Batteries". MRS Bulletin 25 (3): 39. doi:10.1557/mrs2000.17.  edit
  35. ^ MSDS: National Power Corp Lithium Ion Batteries (PDF).; Tektronix Inc., 7 May 2004. Retrieved 11 June 2010.
  36. ^ a b c "How to rebuild a Li-Ion battery pack". Electronics Lab. Retrieved 6 June 2013. 
  37. ^ "Inside a notebook battery pack". ZDNet. Rupert Goodwins . August 17, 2006. Retrieved 6 June 2013. 
  38. ^ Andrea 2010, p. 2.
  39. ^ Andrea 2010, p. 234.
  40. ^ Wang, Y.; He, P.; Zhou, H. (2012). "Li-Redox Flow Batteries Based on Hybrid Electrolytes: At the Cross Road between Li-ion and Redox Flow Batteries". Advanced Energy Materials 2 (7): 770. doi:10.1002/aenm.201200100.  edit
  41. ^ a b c d Lithium Ion technical handbook (PDF). Gold Peak Industries Ltd. November 2003. Archived from the original on 2007-10-07. 
  42. ^ Choi, H. C.; Jung, Y. M.; Noda, I.; Kim, S. B. (2003). "A Study of the Mechanism of the Electrochemical Reaction of Lithium with CoO by Two-Dimensional Soft X-ray Absorption Spectroscopy (2D XAS), 2D Raman, and 2D Heterospectral XAS−Raman Correlation Analysis". The Journal of Physical Chemistry B 107 (24): 5806. doi:10.1021/jp030438w.  edit
  43. ^ Amatucci, G. G. (1996). "CoO2, the End Member of the LixCoO2 Solid Solution". Journal of the Electrochemical Society 143 (3): 1114–1110. doi:10.1149/1.1836594.  edit
  44. ^ Wenige, Niemann, et al. (30 May 1998). Liquid Electrolyte Systems for Advanced Lithium Batteries (PDF).; Chemical Engineering Research Information Center(KR). Retrieved 11 June 2010.
  45. ^ Balbuena, P.B., Wang, Y.X. (eds) (2004). Lithium Ion Batteries: Solid Electrolyte Interphase, Imperial College Press, London, ISBN 1860943624.
  46. ^ Fong, R. A. (1990). "Studies of Lithium Intercalation into Carbons Using Nonaqueous Electrochemical Cells". Journal of the Electrochemical Society 137 (7): 2009–2010. doi:10.1149/1.2086855.  edit
  47. ^ Syzdek, J. A.; Borkowska, R.; Perzyna, K.; Tarascon, J. M.; Wieczorek, W. A. A. (2007). "Novel composite polymeric electrolytes with surface-modified inorganic fillers". Journal of Power Sources 173 (2): 712. doi:10.1016/j.jpowsour.2007.05.061.  edit
  48. ^ Syzdek, J. A.; Armand, M.; Marcinek, M.; Zalewska, A.; Żukowska, G. Y.; Wieczorek, W. A. A. (2010). "Detailed studies on the fillers modification and their influence on composite, poly(oxyethylene)-based polymeric electrolytes". Electrochimica Acta 55 (4): 1314. doi:10.1016/j.electacta.2009.04.025.  edit
  49. ^ Reiter, J.; Nádherná, M.; Dominko, R. (2012). "Graphite and LiCo1/3Mn1/3Ni1/3O2 electrodes with piperidinium ionic liquid and lithium bis(fluorosulfonyl)imide for Li-ion batteries". Journal of Power Sources 205: 402. doi:10.1016/j.jpowsour.2012.01.003.  edit
  50. ^ David Linden, Thomas B. Reddy (ed) (2002 ). Handbook of Batteries 3rd Edition. McGraw-Hill, New York, chapter 35, ISBN 0-07-135978-8.
  51. ^ "Design Review For: Advanced Electric Vehicle Battery Charger, ECE 445 Senior Design Project".  090521
  52. ^ a b "Lithium Ion Rechargeable Batteries. Technical Handbook". 
  53. ^ "Safe Charge Rates for Lithium-Ion Cells Effects of Lithium Plating". NASA Aerospace Battery Workshop. National Aeronautics and Space Administration (NASA). Retrieved 16 December 2013.  |coauthors= requires |author= (help)
  54. ^ Siemens CL75 user manual. Siemens AG. 2005. p. 8. 
  55. ^ Fisher, Thomas. "Will Tesla Alone Double Global Demand For Its Battery Cells? (Page 2)". Retrieved 2014-02-16. 
  56. ^ "Reduced cell cost suggests the upcoming era of large capacity cells". EnergyTrend. 2013-05-06. Retrieved 2014-02-16. 
  57. ^ "Overview of lithium ion batteries". Panasonic. Jan 2007. Archived from the original on Nov 7, 2011. 
  58. ^ a b c Winter & Brodd 2004, p. 4258
  59. ^ "High Power Lithium Ion ANR26650M1A". Archived from the original on 2010-06-01. 
  60. ^ Andrea 2010, p. 12.
  61. ^ AeroVironment achieves electric vehicle fast-charge milestone; AeroVironment, 30 May 2007. (Press release). "Test rapidly recharges a battery pack designed for use in passenger vehicles. 10-minute recharge restores enough energy to run electric vehicle for two hours at 60 miles per hour."
  62. ^ Jost, Kevin [ed.] (October 2006). Tech Briefs: CPI takes new direction on Li-ion batteries (PDF).; Automotive Engineering Online.
  63. ^ Loveday, Eric (23 April 2010). "Hitachi develops new manganese cathode, could double life of li-ion batteries". Retrieved 11 June 2010. 
  64. ^ Nikkei (29 November 2009). Report: Nissan On Track with Nickel Manganese Cobalt Li-ion Cell for Deployment in 2015 Green Car Congress (blog). Retrieved 11 June 2010.
  65. ^ a b EnerDel Technical Presentation (PDF). EnerDel Corporation. 29 October 2007..
  66. ^ Elder, Robert and Zehr, Dan (16 February 2006). Valence sued over UT patent Austin American-Statesman (courtesy Bickle & Brewer Law Firm)..
  67. ^ Bulkeley, William M. (26 November 2005). "New Type of Battery Offers Voltage Aplenty, at a Premium". The Day. p. E6. 
  68. ^ A123Systems (2 November 2005). A123Systems Launches New Higher-Power, Faster Recharging Li-Ion Battery Systems Green Car Congress; A123Systems (Press release). Retrieved 11 May 2010.
  69. ^ "Imara Corporation website". Retrieved 8 October 2011. 
  70. ^ O'Dell, John (17 December 2008). Fledgling Battery Company Says Its Technology Boosts Hybrid Battery Performance Green Car Advisor; Edmunds Inc. Retrieved 11 June 2010.
  71. ^ "Comparison of Different Lithium Anode: LCO, LMO, LFP and NMC". 2011-12-12. Retrieved 2013-08-28. 
  72. ^ Ellis, B. L.; Makahnouk, W. R. M.; Makimura, Y.; Toghill, K.; Nazar, L. F. (2007). "A multifunctional 3.5 V iron-based phosphate cathode for rechargeable batteries". Nature Materials 6 (10): 749–753. Bibcode:2007NatMa...6..749E. doi:10.1038/nmat2007. PMID 17828278.  edit
  73. ^ Hong, J.; Wang, C. S.; Chen, X.; Upreti, S.; Whittingham, M. S. (2009). "Vanadium Modified LiFePO4 Cathode for Li-Ion Batteries". Electrochemical and Solid-State Letters 12 (2): A33. doi:10.1149/1.3039795.  edit
  74. ^ Quick, Darren (11 December 2012). "Plant root used to create eco-friendly lithium-ion battery". 
  75. ^ a b "Batteries charge very quickly and retain capacity, thanks to new structure | News Bureau | University of Illinois". 2011-03-21. Retrieved 2013-04-20. 
  76. ^ Garling, Caleb (20 April 2012). "IBM Demos Uber Battery That 'Breathes' | Wired Enterprise". Retrieved 22 June 2012. 
  77. ^ 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.  edit
  78. ^ "Researchers Develop Solid-State, Rechargeable Lithium-Air Battery; Potential to Exceed 1,000 Wh/kg". Green Car Congress. 2009-11-21. Retrieved 2013-08-28. 
  79. ^ "Seawater battery sparks sub dreams". New Scientist. 25 April 2012. Retrieved 22 June 2012. 
  80. ^ "PolyPlus Lithium-Water". Retrieved 22 June 2012. 
  81. ^ "... Acceptance of the First Grid-Scale, Battery Energy Storage System" (Press release). Altair Nanotechnologies. 21 November 2008. Retrieved 8 October 2009. 
  82. ^ Ozols, Marty (11 November 2009). Altair Nanotechnologies Power Partner – The Military. Systemagicmotives (personal webpage)[dubious ]. Retrieved 11 June 2010.
  83. ^ Gotcher, Alan J. (29 November 2006). "Altair EDTA Presentation". Archived from the original on 2007-06-16. 
  84. ^ Blain, Loz (2 November 2007). "Subaru doubles the battery range on its electric car concept". gizmag. Retrieved 8 October 2009. 
  85. ^ "Li-Ion Rechargeable Batteries Made Safer". Nikkei Electronics Asia. 29 January 2008. Retrieved 8 October 2009. 
  86. ^ Nam, K. T.; Kim, D. W.; Yoo, P. J.; Chiang, C. Y.; Meethong, N.; Hammond, P. T.; Chiang, Y. M.; Belcher, A. M. (2006). "Virus-Enabled Synthesis and Assembly of Nanowires for Lithium Ion Battery Electrodes". Science 312 (5775): 885–888. doi:10.1126/science.1122716. PMID 16601154.  edit
  87. ^ Evanoff, K.; Magasinski, A.; Yang, J.; Yushin, G. (2011). "Nanosilicon-Coated Graphene Granules as Anodes for Li-Ion Batteries". Advanced Energy Materials 1 (4): 495. doi:10.1002/aenm.201100071.  edit
  88. ^ Palca, Joe (6 April 2009). Hidden Ingredient In New, Greener Battery: A Virus.; National Public Radio. Retrieved 11 June 2010.
  89. ^ Zandonella, Catherine (11 April 2009). "Battery grown from "armour plated" viruses". New Scientist (Tribune media Services International) 202 (2703): 1. 
  90. ^ Bullis, Kevin (28 September 2006). "Powerful Batteries That Assemble Themselves". Technology Review. Retrieved 15 June 2010. 
  91. ^ "Bad Virus Put to Good Use". Clark School of Engineering, University of Maryland. 6 December 2010. Retrieved December 2010. 
  92. ^ "Silicon Whisker and Carbon Nanofiber Composite Anode". NASA BAttery Workshop 2009. 17 November 2009. Retrieved November 2009. 
  93. ^ "New Nanowire Battery Holds 10 Times The Charge of Existing Ones". Science Daily. 20 December 2007. 
  94. ^ Dennis, Lyle (21 December 2007). "Interview with Dr. Cui, Inventor of Silicon Nanowire Lithium-ion Battery Breakthrough". GM-Volt. Retrieved 8 October 2009. 
  95. ^ "the Foresight Institute » Blog Archive » Novel silicon nanostructure extends battery life". 15 May 2012. Retrieved 24 May 2012. 
  96. ^ a b c d Dolcourt, Jessica. (3 September 2012)battery life: 2 problems, 4 fixes (Smartphones Unlocked) | Dialed In – CNET Blogs. Retrieved on 16 April 2013.
  97. ^ "Laboratory of the Prof. Gleb Yushin". 31 August 2011. Retrieved 8 October 2011. 
  98. ^ Hertzberg, B.; Alexeev, A.; Yushin, G. (2010). "Deformations in Si−Li Anodes Upon Electrochemical Alloying in Nano-Confined Space". Journal of the American Chemical Society 132 (25): 8548–8549. doi:10.1021/ja1031997. PMID 20527882.  edit
  99. ^ Preuss, Paul (23 September 2011). "Better Lithium-Ion Batteries Are On The Way From Berkeley Lab". Lawrence Berkeley National Laboratory. 
  100. ^ Millikin, Mike (14 August 2011). "SUNY Binghamton researchers show Si/MgO/graphite composite as high-performance Li-ion anode material". 
  101. ^ "High performance Si/MgO/graphite composite as the anode for lithium-ion batteries". 2011-10-31. Retrieved 2014-02-16. 
  102. ^ Bhandavat, R.; Singh, G. (2013). "Stable and Efficient Li-Ion Battery Anodes Prepared from Polymer-Derived Silicon Oxycarbide–Carbon Nanotube Shell/Core Composites". The Journal of Physical Chemistry C: 130531122619008. doi:10.1021/jp310733b.  edit
  103. ^ Coxworth, Ben (14 February 2013). Silicon nanoparticles used to create a super-performing battery. Retrieved on 16 April 2013.
  104. ^ "USC team develops new porous silicon nanoparticle material for high-performance Li-ion anodes". Green Car Congress. 2013-02-12. doi:10.1007/s12274-013-0293-y. Retrieved 2013-06-04. 
  105. ^ Synthetic Carbon Negative electrode Boosts Battery Capacity 30 Percent | MIT Technology Review. (2 April 2013). Retrieved on 16 April 2013.
  106. ^ "Silicon-hydrogel electrodes improve lithium-ion battery performance". KurzweilAI. doi:10.1038/ncomms2941. Retrieved 2013-06-04. 
  107. ^ Wu, H.; Yu, G.; Pan, L.; Liu, N.; McDowell, M. T.; Bao, Z.; Cui, Y. (2013). "Stable Li-ion battery anodes by in-situ polymerization of conducting hydrogel to conformally coat silicon nanoparticles". Nature Communications 4. doi:10.1038/ncomms2941.  edit
  108. ^ Newman, Jared (2013-05-23). "Amprius Begins Shipping a Better Smartphone Battery |". Retrieved 2013-06-04. 
  109. ^ Liu, N.; Wu, H.; McDowell, M. T.; Yao, Y.; Wang, C.; Cui, Y. (2012). "A Yolk-Shell Design for Stabilized and Scalable Li-Ion Battery Alloy Anodes". Nano Letters 12 (6): 3315–3321. doi:10.1021/nl3014814. PMID 22551164.  edit
  110. ^ Bullis, Kevin (22 June 2006).Higher-Capacity Lithium-Ion BatteriesTechnology Review. Retrieved 11 June 2010.
  111. ^ Taberna, P. L.; Mitra, S.; Poizot, P.; Simon, P.; Tarascon, J. -M. (2006). "High rate capabilities Fe3O4-based Cu nano-architectured electrodes for lithium-ion battery applications". Nature Materials 5 (7): 567–573. Bibcode:2006NatMa...5..567T. doi:10.1038/nmat1672. PMID 16783360.  edit
  112. ^ Vlasic, Bill; Wald, Matthew L. (12 June 2012). "A123, U.S.-Backed Battery Maker, Claims Breakthrough". The New York Times. 
  113. ^ "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. Retrieved 13 June 2012. 
  114. ^ "A123's new battery tech goes to extremes". Retrieved 13 June 2012. 
  115. ^ a b "Small in size, big on power: New microbatteries a boost for electronics | News Bureau | University of Illinois". 2013-04-16. Retrieved 2013-04-20. 
  116. ^ Pikul, J. H.; Gang Zhang, H.; Cho, J.; Braun, P. V.; King, W. P. (2013). "High-power lithium ion microbatteries from interdigitated three-dimensional bicontinuous nanoporous electrodes". Nature Communications 4: 1732. doi:10.1038/ncomms2747. PMID 23591899.  edit
  117. ^ "Better batteries through biology". KurzweilAI. 2013-11-16. doi:10.1038/ncomms3756. Retrieved 2014-02-16. 
  118. ^ "Lithium batteries could soon be safer, thanks to a material inspired by gum". 2014-02-06. Retrieved 2014-02-16. 
  119. ^ [1]
  120. ^ "Evonik Industries - Specialty chemicals - Energy source of the future - Evonik Industries - Specialty Chemicals". Retrieved 2013-08-28. 
  121. ^ Andrea 2010, p. 229.
  122. ^ GR-3150-CORE, Generic Requirements for Secondary Non-Aqueous Lithium Batteries.
  123. ^ Sanyo: Overview of Lithium Ion Batteries, listing self-discharge rate of 2%/mo
  124. ^ Sanyo: Harding energy specification, listing self-discharge rate of 0.3%/mo
  125. ^ Zimmerman, A. H. (2004). "Self-discharge losses in lithium-ion cells". IEEE Aerospace and Electronic Systems Magazine 19 (2): 19. doi:10.1109/MAES.2004.1269687.  edit
  126. ^ Phil Weicker (1 November 2013). A Systems Approach to Lithium-Ion Battery Management. Artech House. p. 214. ISBN 978-1-60807-659-8. 
  127. ^ a b Winter & Brodd 2004, p. 4259
  128. ^ Apple: Lithium-ion Batteries
  129. ^ a b c d "Five tips for extending lithium-ion battery life". TechRepublic. Retrieved 14 February 2013. 
  130. ^ Specification sheet for typical lithium-ion battery
  131. ^ Andrea 2010, p. 9.
  132. ^ Cristo, L.M. and Atwater, T. B. Characteristics and Behavior of 1M LiPF6 1EC:1DMC Electrolyte at Low Temperatures. Fort Monmouth, NJ: U.S. Army Research. 
  133. ^ "Modelling capacity fade in Lithium-ion cells, Bor Yann Liaw, Jungst, Nagasubramanian, and Doughty, Sandia National Laborator – Analysis of Lithium-Ion Battery Degradation during Thermal Aging" (PDF). Retrieved 8 October 2011. 
  134. ^ Tip: Condition your new cell phone’s battery to make it last longer (but be sure to condition it properly). (24 December 2011). Retrieved on 16 April 2013.
  135. ^ Yadav, Antriksh. (31 December 2010) Top 5 lithium-ion battery myths. Retrieved on 16 April 2013.
  136. ^ Spotnitz, R.; Franklin, J. (2003). "Abuse behavior of high-power, lithium-ion cells". Journal of Power Sources 113: 81. doi:10.1016/S0378-7753(02)00488-3.  edit
  137. ^ "Lithium-ion Battery Charging Basics". PowerStream Technologies. Retrieved 4 December 2010. 
  138. ^ Winter & Brodd 2004, p. 4259.
  139. ^ Electrochem Commercial Power (9 September 2006). "Safety and handling guidelines for Electrochem Lithium Batteries" (PDF). Rutgers University. Retrieved 21 May 2009. 
  140. ^ a b Mikolajczak, Celina; Kahn, Michael; White, Kevin and Long, Richard Thomas (July 2011). "Lithium-Ion Batteries Hazard and Use Assessment". Fire Protection Research Foundation. pp. 76, 90, 102. Retrieved 27 January 2013. 
  141. ^ Cringely, Robert X. (1 September 2006). "Safety Last". The New York Times. Retrieved 14 April 2010. 
  142. ^ "Can anything tame the battery flames?". Cnet . Michael Kanellos. August 15, 2006. Retrieved 14 June 2013. 
  143. ^ Guardian newspaper: Heathrow fire on Boeing Dreamliner 'started in battery component', 18 July 2013
  144. ^ "Boeing 787 aircraft grounded after battery problem in Japan". BBC News. January 14, 2014. Retrieved January 16, 2014. 
  145. ^ "Are lithium batteries sustainable to the environment?". Alternative Energy Resources. Vaishnovi Kamyamkhane. Retrieved 3 June 2013. 
  146. ^ "Study Identifies Environmental and Health Impacts of Lithium-ion Batteries for EVs". May 28, 2013. Greenfleet Magazine. Retrieved 3 June 2013. 
  147. ^ "Can Nanotech Improve Li-ion Battery Performance". May 30, 2013. Environmental Leader. Retrieved 3 June 2013. 
  148. ^ "Kyocera Launches Precautionary Battery Recall, Pursues Supplier of Counterfeit Batteries" (Press release). Kyocera Wireless. 28 October 2004. Archived from the original on 7 January 2006. Retrieved 15 June 2010. 
  149. ^ Tullo, Alex (21 August 2006). "Dell Recalls Lithium Batteries". Chemical and Engineering News 84 (34): 11. doi:10.1021/cen-v084n034.p011a. 
  150. ^ Hales, Paul (21 June 2006). Dell laptop explodes at Japanese conference. The Inquirer. Retrieved 15 June 2010.
  151. ^ Nokia issues BL-5C battery warning, offers replacement. Wikinews. 14 August 2007. Retrieved 8 October 2009. 
  152. ^ Nokia N91 cell phone explodes, Mukamo – Filipino News (27 July 2007). Retrieved 15 June 2010.
  153. ^ a b "Safe Travel". U.S. Department of Transportation. 1 January 2008. Retrieved 8 October 2009. 
  154. ^ Galbraith, Rob (3 January 2008). "U.S. Department of Transportation revises lithium battery rules press release". Little Guy Media. Retrieved 11 May 2009. 
  155. ^ Prohibitions – 6.3.12 – Dangerous, offensive and indecent articles (PDF). Hong Kong Post Office Guide. December 2009. Retrieved 15 June 2010.
  156. ^ International Mail > FAQs > Goods/Services: Shipping a Laptop. Japan Post Service Co. Ltd. Retrieved 15 June 2010.
  157. ^ USPS To Stop Delivering iPads And Kindles To Troops And Overseas Consumers On 16 May. USPS. Retrieved 27 June 2012.
  158. ^ Just in Time for the Holidays, U.S. Postal Service to Begin Global Shipping of Packages with Lithium Batteries USPS. Retrieved 6 December 2012.
  159. ^ "Lithium ion cells for Aerospace applications: LVP series". GS UASA. Retrieved 17 January 2013. 
  160. ^ Dalløkken, Per Erlien (17 January 2013). "Her er Dreamliner-problemet" (in Norway). Teknisk Ukeblad. Retrieved 17 January 2013. 
  161. ^ Timmer, John. (2 August 2011) Retrieved 3 November 2011. Retrieved on 16 April 2013.
  162. ^ Melody Voth (6 December 2010). "Battery Booster". Chemical & Engineering News 88 (49). Retrieved 9 February 2011.  (subscription required)
  163. ^ Solid-state battery developed at CU-Boulder could double the range of electric cars, University of Boulder Colorado News, 18 September 2013
  164. ^ WSU Researchers Create Super Lithium-ion Battery Retrieved 2013 January 10
  165. ^ "Washington State University Gets Funding to Scale Up New Tin Batteries". MacroCurrent. 2013-04-30. Retrieved 2013-06-04. 
  166. ^ Nissan develops world first analysis technique for better lithium ion battery durability, Automotive World, 13 March 2014
  167. ^ Amprius Gets $30M Boost for Silicon-Based Lithium-Ion Batteries, Greentech Efficiency, 6 January 2014, Jeff St. John
  168. ^ At long last, new lithium battery tech actually arrives on the market (and might already be in your smartphone), Extreme Tech, 10 January 2014, Sebastian Anthony
  169. ^ Pomegranate-inspired electrode could mean longer lithium-ion battery life, Gizmag, 19 February 2014, Nick Lavars
  170. ^ EnerG2 Announces Major Breakthrough in Lithium-Ion Battery Capacity and Performance, PRWeb, 23 January 2014
  171. ^ Chewing gum-like material makes lithium ion batteries safer, Tree Hugger, 5 February 2014, Megan Treacy
  172. ^ Messy Innards Make for a Better Lithium Ion Battery, Scientific American, 17 January 2014, Umair Irfan and ClimateWire
  173. ^ Origami: The surprisingly simple secret to creating flexible, high-power lithium-ion batteries, Extreme Tech, 5 February 2014, Sebastian Anthony
  174. ^ First nonflammable lithium-ion battery will stop your smartphone, car, and plane from exploding, Extreme Tech, 13 February 2014, Sebastian Anthony
  175. ^ Researchers Make Breakthrough in Battery Technology with New Tin-Seeded Germanium Nanowire Anode, World Industrial Reporter, 11 February 2014
  176. ^ New tin-seeded germanium nanowire array anodes for Li-ion batteries show high capacity and lifetime, Green Car Congress, 10 February 2014
  177. ^ New battery management technology could boost Li-ion capacity by 40%, quadruple recharging cycles, TreeHugger, 5 February 2014, Derek Markham
  178. ^ New battery management technology could boost Li-ion capacity by 40%, quadruple recharging cycles, TreeHugger, 5 February 2014, Derek Markham
  179. ^ Re-engineered battery material could lead to rapid recharging of many devices, MIT News, 11 March 2009, Elizabeth A. Thomson
  180. ^ Zyga, Lisa (12 March 2009). "Nanoball Batteries Could Charge Electric Cars in 5 Minutes". PhysOrg. Retrieved 21 March 2012. 
  181. ^ Nanotubes make for better lithium-ion batteries,, 3 March 2014


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