Lithium-ion battery

Not to be confused with lithium battery or lithium polymer battery.

"Lithium-ion" redirects here. For the metal element, see Lithium.

Lithium-ion battery

Nokia Li-ion battery for powering a mobile phone
Specific energy	100–265 W·h/kg (0.36–0.95 MJ/kg)
Energy density	250–730 W·h/L (0.90–2.23 MJ/L)
Specific power	~250-~340 W/kg
Charge/discharge efficiency	80–90%
Energy/consumer-price	2.5 W·h/US$
Self-discharge rate	8% at 21 °C 15% at 40 °C 31% at 60 °C (per month)
Cycle durability	400–1200 cycles
Nominal cell voltage	NMC 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 the 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 ), 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. For example, Lithium-ion batteries are becoming a common replacement for the lead acid batteries that have been used historically for golf carts or utility vehicles. Instead of using heavy lead plates and acid electrolyte, the trend is to use a light weight Lithium/Carbon anode and Lithium Iron Phosphate cathode. Lithium-ion batteries can provide the same voltage as lead acid batteries and therefore no modifications of the cart's electrical drive system are required.

Research is yielding a stream of improvements to traditional LIB technology, focusing on energy density, durability, cost, and intrinsic safety.

Chemistry, performance, cost, and safety characteristics vary across LIB types. Handheld electronics mostly use LIBs based on lithium cobalt oxide (LiCoO₂), which offers high energy density, but have well-known safety concerns, 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. These chemistries are being 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.

Charge and discharge

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

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.

Construction

Cylindrical 18650 lithium iron phosphate cell before closing

The three primary functional components of a lithium-ion battery are the negative electrode, positive electrode, and the electrolyte. 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. The electrochemical roles of the electrodes change between anode and cathode, depending on the direction of current flow through the cell.

The most commercially popular negative electrode material 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).

The electrolyte is typically a mixture of organic carbonates such as ethylene carbonate or diethyl carbonate containing complexes of lithium ions. These non-aqueous electrolytes generally use non-coordinating anion salts such as lithium hexafluorophosphate (LiPF₆), lithium hexafluoroarsenate monohydrate (LiAsF₆), lithium perchlorate (LiClO₄), lithium tetrafluoroborate (LiBF₄), and lithium triflate (LiCF₃SO₃).

Depending on materials choices, the voltage, capacity, 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 very 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 water from the battery pack.

Lithium ion batteries are more expensive than NiCd batteries but operate over a wider temperature range with higher energy densities, while being smaller and lighter. They are fragile and so need a protective circuit to limit peak voltages.

Formats

Nissan Leaf's lithium-ion battery pack.

Li-ion cells are available in various formats, which can generally be divided into four groups:

• Small cylindrical (solid body without terminals, such as those used in laptop batteries)
• Large cylindrical (solid body with large threaded terminals)
• Pouch (soft, flat body, such as those used in cell phones)
• Prismatic (semi-hard plastic case with large threaded terminals, often used in vehicles' traction packs)

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

History

See also: History of the battery

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. Whittingham used titanium(IV) sulfide and lithium metal as the electrodes.

The reversible intercalation in graphite and intercalation into cathodic oxides was also discovered in the 1970s by J. O. Besenhard at TU Munich. Besenhard also proposed the application as high energy density lithium cells. Electrolyte decomposition and solvent co-intercalation into graphite were severe drawbacks for long battery cycle life.

Primary lithium batteries in which the negative electrode is made from metallic lithium pose safety issues. As a result, lithium-ion batteries were developed in which both electrodes are made of a material containing lithium ions.

At Oxford University, England, in 1979, John Goodenough and Koichi Mizushima demonstrated a rechargeable cell with high cell voltage in the 4 V range using lithium cobalt oxide (LiCoO₂) as the positive electrode and lithium metal as the negative electrode. This innovation provided the positive electrode material which made LIBs possible. LiCoO₂ 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, LiCoO₂ 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. This led to the development of a workable lithium intercalated graphite electrode at Bell Labs (LiC6) to provide an alternative to the lithium metal electrode battery.

In 1980, Rachid Yazami also demonstrated the reversible electrochemical intercalation of lithium in graphite. The organic electrolytes available at the time would decompose during charging if used with a graphite negative electrode, preventing the early development of a rechargeable battery which employed the lithium/graphite system. 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 the most commonly used electrode in commercial lithium ion batteries.

In 1983, Michael M. Thackeray, Goodenough, and coworkers identified manganese spinel as a cathode material. 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. Manganese spinel is currently used in commercial cells.

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 (LiCoO₂), which is stable in air, as the other. By using materials without metallic lithium, safety was dramatically improved over batteries which used lithium metal. The use of lithium cobalt oxide (LiCoO₂) enabled industrial-scale production to be achieved easily.

This was the birth of the current lithium-ion battery.

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.

Modern batteries

In 1989, Goodenough and Arumugam Manthiram of the University of Texas at Austin showed that cathodes containing polyanions, e.g., sulfates, produce higher voltages than oxides due to the inductive effect of the polyanion.

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

In 1996, Goodenough, Akshaya Padhi and coworkers identified lithium iron phosphate (LiFePO₄) and other phospho-olivines (lithium metal phosphates with the same structure as mineral olivine) as cathode materials.

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 with aluminium, niobium and zirconium. The exact mechanism causing the increase became the subject of widespread debate.

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 cathode'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.

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

Uses

Li-ion batteries provide light weight, high energy density power sources for a variety of devices, where nickel-cadmium or nickel-metal hydride batteries would be too heavy or large. Such devices include:

• Portable devices: these include mobile phones and smartphones, laptops and tablets, digital cameras and camcorders, handheld game consoles and torches.
• Power tools: Li-ion batteries are used in tools such as cordless drills, sanders, saws and a variety of garden equipment including whipper-snippers and hedge trimmers.
• Electric vehicles: Because of their light weight Li-ion batteries are used for energy storage for many electric vehicles for everything from electric cars to Pedelecs, from hybrid vehicles to advanced electric wheelchairs, from radio-controlled models and model aircraft to the Mars Curiosity rover.

Electrochemistry

The three participants in the electrochemical reactions in a lithium-ion battery are the positive and negative electrodes and the electrolyte.

Both electrodes are materials into which, and from which, lithium ions can migrate. During insertion (or intercalation) lithium ions move into the electrode. During the reverse process, extraction (or deintercalation), lithium ions move back out. When a lithium-based cell is discharging, the positive lithium ion is extracted from the negative electrode (usually graphite) and inserted into the positive electrode (lithium containing compound). When the cell is charging, the reverse occurs.

Useful work can only be extracted if 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 the coefficient $n$.

The positive electrode half-reaction (with charging being forwards) is:

$\mathrm{LiCoO_2} \leftrightarrows \mathrm{Li}_{1-n}\mathrm{CoO_2} + n\mathrm{Li^+} + n\mathrm{e^-}$

The negative electrode half-reaction is:

$n\mathrm{Li^+} + n\mathrm{e^-} + \mathrm{C} \leftrightarrows \mathrm{Li_nC}$

The overall reaction has its limits. Overdischarge supersaturates lithium cobalt oxide, leading to the production of lithium oxide, 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

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

In a lithium-ion battery the lithium ions are transported to and from the cathode or anode, with the transition metal, cobalt (Co), in $\mathrm{Li}_x \mathrm{Co} \mathrm{O}_2$ being oxidized from Co³⁺ to Co⁴⁺ during charging, and reduced from Co⁴⁺ to Co³⁺ during discharge.

The energy provided by the cell is equal to the voltage times the charge. Each gram of lithium represents Faraday's constant/6.941 or 13 901 coulombs. For a voltage of 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 take into account all the other materials that go into a lithium battery and which make lithium batteries many times heavier per unit of energy.

Electrolytes

The cell voltages given in the Electrochemistry section are larger than the potential at which aqueous solutions can electrolyze, in addition lithium is highly reactive to water, therefore, nonaqueous or aprotic solutions are used.

Liquid electrolytes in lithium-ion batteries consist of lithium salts, such as LiPF₆, LiBF₄ or LiClO₄ in an organic solvent, such as ethylene carbonate, dimethyl carbonate, and diethyl carbonate. A liquid electrolyte conducts lithium ions, acting as a carrier between the cathode and the anode when a battery passes an electric current 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 by a slightly smaller amount at 0 °C (32 °F)

Unfortunately, organic solvents easily decompose on anodes during charging. However, 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), which is electrically insulating yet provides sufficient ionic conductivity. The interphase prevents 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.

A good solution for the interface instability is the application of a new class of composite electrolytes based on POE (poly(oxyethylene)) developed by Syzdek et al. 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.

Concerning the flammability and volatility of the organic solvents present in the electrolyte, another option, how to improve the overall safety of the battery, is in using room temperature ionic liquids (RTILs) as the main component of the electrolyte.

Advantages and disadvantages

Note that both advantages and disadvantages depend on the materials and design that make up the battery. This summary reflects older designs that use carbon anode, metal oxide cathodes, and lithium salt in an organic solvent for the electrolyte.

Advantages

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

• Wide variety of shapes and sizes efficiently fitting the devices they power.
• Much lighter than other energy-equivalent secondary batteries.
• High open circuit voltage in comparison to aqueous batteries (such as lead acid, nickel-metal hydride and nickel-cadmium). This is beneficial because it increases the amount of power that can be transferred at a lower current.
• No memory effect.
• Self-discharge rate of approximately 5–10% per month, compared to over 30% per month in common nickel metal hydride batteries, approximately 1.25% per month for Low Self-Discharge NiMH batteries and 10% per month in nickel-cadmium batteries. According to one manufacturer, lithium-ion cells (and, accordingly, "dumb" lithium-ion batteries) do not have any self-discharge in the usual meaning of this word. What looks like a self-discharge in these batteries is a permanent loss of capacity (see Disadvantages). On the other hand, "smart" lithium-ion batteries do self-discharge, due to the drain of the built-in voltage monitoring circuit.
• Components are environmentally safe as there is no free lithium metal.^{[citation needed]}

Disadvantages

Cell life

• Charging forms deposits inside the electrolyte that inhibit ion transport. Over time, the cell's capacity diminishes. The increase in internal resistance reduces the cell's ability to deliver current. This problem is more pronounced in high-current applications. The decrease means that older batteries do not charge as much as new ones (charging time required decreases proportionally).
• High charge levels and elevated temperatures (whether from charging or ambient air) hasten capacity loss. Charging heat is caused by the carbon anode.
• A Standard (Cobalt) Li-ion cell that is full most of the time at 25 °C (77 °F) irreversibly loses approximately 20% capacity per year.^{[citation needed]} 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). When stored at 40%–60% charge level, the capacity loss is reduced to 2%, 4%, and 15%, respectively.^{[citation needed]} In contrast, the calendar life of LiFePO₄ cells is not affected by being kept at a high state of charge.

Internal resistance

• The internal resistance of standard (Cobalt) lithium-ion batteries is high compared to both other rechargeable chemistries such as nickel-metal hydride and nickel-cadmium, and LiFePO4 and lithium-polymer cells. Internal resistance increases with both cycling and age. 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.

• To power larger devices, such as electric cars, connecting many small batteries in a parallel circuit is more effective and more efficient than connecting a single large battery.^{[citation needed]}

Safety requirements

If overheated or overcharged, Li-ion batteries may suffer thermal runaway and cell rupture. In extreme cases this can lead to combustion. Deep discharge may short-circuit the cell, in which case recharging would be unsafe.^{[citation needed]} 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. When stored for long periods the small current draw of the protection circuitry itself may drain the battery below its shut down voltage; normal chargers are then ineffective. Many types of lithium-ion cell cannot be charged safely below 0 °C.

Other safety features are required in each cell:

• Shut-down separator (for overheating)
• Tear-away tab (for internal pressure)
• Vent (pressure relief)
• Thermal interrupt (overcurrent/overcharging)

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 anode produces heat during use, while the cathode 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.

These safety issues present a problem for large scale application of such cells in Electric Vehicles; A dramatic decrease in the failure rate is necessary.

Market

• Costs more per watt-hour than other chemistries
• Not suitable for AAA, AA, C or D form factors due to voltage per cell being more than 2 volts (i.e. 3.7 volts), though most devices designed for a voltage that is a multiple of 1.5 can run safely on a voltage that is 30% higher.^{[citation needed]}

Specifications and design

• Specific energy density: 150 to 250 W·h/kg (540 to 900 kJ/kg)
• Volumetric energy density: 250 to 620 W·h/l (900 to 1900 J/cm³)
• Specific power density: 300 to 1500 W/kg (@ 20 seconds and 285 W·h/l)

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

Lithium-ion batteries with a lithium iron phosphate cathode and graphite anode 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 cathode with graphite anodes have a 3.7 V nominal voltage with a 4.2 V max charge. 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. Some lithium-ion varieties can reach 90% in as little as 10 minutes.

Battery charging procedure

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

• A single Li-ion cell is charged in 2 stages:^{[citation needed]}

1. CC
2. CV

• A Li-ion battery (a set of Li-ion cells in series) is charged in 3 stages:

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

Stage 1: CC: Apply charging current to the battery, until the voltage limit per cell is reached.

Stage 2: Balance: Reduce the charging current (or cycle the charging on and off to reduce the average current) while the state of charge of individual cells is balanced by a balancing circuit, until the battery is balanced. Some fast chargers skip stage 2.

Stage 3: CV: Apply a voltage equal to the maximum cell voltage times the number of cells in series to the battery, as the current gradually declines asymptotically 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 with approximate 4.2 ± 0.05 V/cell except for military long life that uses 3.92 V to extend battery life. Most protection circuits cuts off if either >4.3 V or 90 °C is reached. Also if threshold of below 2.50 V/cell is reached the battery protection circuit may render it 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 explosion.

Materials and construction

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.

LIB types

Area	Technology	Researchers	Target application	Date	Benefit
Cathode	Manganese spinel (LMO)	Lucky Goldstar Chemical, NEC, Samsung, Hitachi, Nissan/AESC	Hybrid electric vehicle, cell phone, laptop	1996	durability, cost
	Lithium iron phosphate	University of Texas/Hydro-Québec,/Phostech Lithium Inc., Valence Technology, A123Systems/MIT	Segway Personal Transporter, power tools, aviation products, automotive hybrid systems, PHEV conversions	1996	moderate density (2 A·h outputs 70 amperes) operating temperature >60 °C (140 °F)
	Lithium nickel manganese cobalt (NMC)	Imara Corporation, Nissan Motor, Microvast Inc.		2008	density, output, safety
	LMO/NMC	Sony, Sanyo			power, safety (although limited durability)
	Lithium iron fluorophosphate	University of Waterloo		2007	durability, cost (replace Li with Na or Na/Li)
	Lithium air	University of Dayton Research Institute	automotive	2009	density, safety
	5% Vanadium-doped Lithium iron phosphate olivine	Binghamton University		2008	output
	Lithium purpurin	Arava Leela Mohana Reddy Rice University		2012	Organic material, low production cost 90 milliamp hours per gram after 50 charge/discharge cycles
	Lithium manganese dioxide on porous tin	University of Illinois at Urbana-Champaign	automotive, electronics	2013	energy density, power, fast charge using microstructured porous tin
Anode	Lithium-titanate battery (LT)	Altairnano, Microvast Inc.	automotive (Phoenix Motorcars), electrical grid (PJM Interconnection Regional Transmission Organization control area, United States Department of Defense), bus (Proterra)	2008	output, charging time, durability (20 years, 9,000 cycles), safety, operating temperature (-50–70 °C (-58–158 °F)
	Lithium vanadium oxide	Samsung/Subaru.	automotive	2007	density (745Wh/l)
	Cobalt-oxide nanowires from genetically modified virus	MIT		2006	density, thickness
	Three-dimensional (3D) porous particles composed of curved 2D nanolayers	Georgia Institute of Technology	high energy batteries for electronics and electrical vehicles	2011	specific capacity > 2000 mA·h/g, high efficiency, rapid low-cost synthesis
	Iron-phosphate nanowires from genetically modified virus	MIT		2009	density, thickness
	Silicon/titanium dioxide composite nanowires from genetically modified tobacco virus	University of Maryland	explosive detection sensors, biomimetic structures, water-repellent surfaces, micro/nanoscale heat pipes	2010	density, low charge time
	Silicon whisker on carbon nanofiber composite	Junqing Ma, Physical sciences, Inc.	portable electronics, electrical vehicles, electrical grid	2009	high capacity, good cycle life, fast rate, low charge time
	nanosized wires on stainless steel	Stanford University	wireless sensors networks,	2007	density (shift from anode- to cathode-limited), durability issue remains (wire cracking)
	Metal hydrides	Laboratoire de Réactivité et de Chimie des Solides, General Motors		2008	density (1480 mA·h/g)
	Silicon nanotubes (or silicon nanospheres) confined within rigid carbon outer shells	Georgia Institute of Technology, MSE, NanoTech Yushin's group	stable high energy batteries for cell phones, laptops, netbooks, radios, sensors and electrical vehicles	2010	specific capacity 2400 mA·h/g, ultra-high Coulombic Efficiency and outstanding SEI stability
	Silicon nanopowder in a conductive polymer binder	Lawrence Berkeley National Laboratory	Automotive and Electronics	2011	Compatible with commercial Si, high capacity anodes (1400 mA·h/g) with good cycling characteristics
	Silicon oxide-coated double-walled silicon nanotubes	Yi Cui/Stanford University	Automotive and electronics	2012	Durability (6,000 charge cycles)
	Water	Polyplus Corporation	Marine	2012	Energy density: 1500 watt-hours/kg. Non-rechargeable.
	Air	IBM, Polyplus	Automotive	2012	Energy density: up to 10,000 mA·h per gram of cathode material. Rechargeable.
	Electro-plated tin	Washington State University	Consumer electronics	2012	Reduced cost. 3x capacity vs conventional Li-ion
	Solid-state plated copper antimonide nanowire	Prieto battery	Consumer electronics	2012	Reduced charging time from reduced cathode/anode gap. Increased energy density. 750 charging cycles.
	Boron-doped silicon nanospheres	University of Southern California Chongwu Zhou	Various	2012	Reduced charging time. Increased density.
	Hard carbon	Energ2	Consumer electronics	2013	30% greater storage capacity than graphite
Electrode	LT/LMO	Ener1/Delphi,		2006	durability, safety (limited density)
	Nanostructure	Université Paul Sabatier/Université Picardie Jules Verne		2006	density
	Nanophosphate	A123 Systems	Automotive	2012	Operation at high and low ambient temperature
	Nickel/Tin on porous nickel	University of Illinois at Urbana-Champaign	Automative, electronics	2013	energy density and power using microstructured metal as the substrate for thin film Nickel/Tin.
Electrolyte	Lithium imide	Leyden	Consumer electronics	2012	750 and 800 charging cycles with greater than 80% of original capacity. Reduced thermal expansion.

Battery pack life

Li+ batteries last longer if not deeply discharged (depleted) before recharging. The smaller the depth of discharge, the longer the battery will last.^{[citation needed]}

Batteries may last longer if not stored fully discharged. As the battery will self-discharge over time, its voltage will gradually reduce, and when it is 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 discharged any further until recharged. It is frequently recommended to store batteries at 40% charge level.

The rate of degradation of lithium-ion batteries is strongly temperature-dependent; they degrade much faster if stored or used at higher temperatures. They may be stored in a refrigerator.

Conditioning controversy

There is a belief that Li+ batteries need to be "conditioned" before first use. One is told to plug the battery/device into a charger and leave it there for seven or eight hours, even if fully charged. But this may simply be a confusion of the battery software calibration instructions with the "conditioning" instructions for NiCd and NiMH batteries. 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.

Lithium ion batteries do not need the "conditioning" of being fully discharged and charged the way NiCd and NiMH batteries do.

Multicell devices

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, significantly improving battery efficiency and increasing overall capacity. As the number of cells and load currents increase, the potential for mismatch increases. There are two kinds of mismatch in the pack: state-of-charge (SOC) and capacity/energy ("C/E") mismatch. Though SOC is more common, each problem limits pack current capacity (mA·h) to that of the weakest cell.

Safety

See also: Plug-in electric vehicle fire incidents

Lithium-ion batteries can rupture, ignite, or explode when exposed to high temperature. 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. The fire energy content (electrical + chemical) of cobalt-oxide cells is about 100 to 150 kJ per A·h, most of it chemical. Authorities and handlers lack knowledge on how to treat Li-Ion battery fire.

Replacing the lithium cobalt oxide cathode 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. Currently, these 'safer' lithium-ion batteries are mainly used in electric cars and other large-capacity battery applications, where safety issues are critical.

Lithium-ion batteries normally contain safety devices to protect the cells from disturbance. However, contaminants inside the cells can defeat these safety devices.

Recalls

In March 2007, Lenovo recalled approximately 205,000 batteries at risk of explosion. In August 2007, Nokia recalled over 46 million batteries at risk of overheating and exploding. One such incident occurred in the Philippines involving a Nokia N91, which uses the BL-5C battery.

In December 2006, Dell recalled approximately 22,000 laptop batteries from the US market. Approximately 10 million Sony batteries used in Dell, Sony, Apple, Lenovo/IBM, 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 short-circuit.

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

Transport restrictions

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. In January 2008, the United States Department of Transportation ruled that passengers on commercial aircraft could carry lithium batteries in their checked baggage if the batteries were installed in a device. 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 air travel. This restriction is due to the possibility of batteries short-circuiting and causing a fire.^{[citation needed]}

Additionally, a limited number of replacement batteries may be transported in carry-on luggage. Such batteries must be sealed in their original protective packaging or in individual containers or plastic bags.

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, Australia and Japan.

On 16 May 2012, United States Postal Service (USPS) banned shipping anything containing a lithium battery to an overseas address due to fires resulting from transport of batteries. Because of this restriction, it became 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.

The Boeing 787 Dreamliner contains lithium cobalt oxide batteries which are more reactive than newer types of batteries such as LiFePo.

Research

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

Solid-state designs 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."

Earlier trials of this technology encountered cost barriers, because the semiconductor industry's vacuum deposition technology cost 20–30 times too much. The new process deposits semiconductor-quality films from a solution. The nanostructured films grow directly on a substrate and then sequentially on top of each other. The process allows the firm to "spray-paint a cathode, then a separator/electrolyte, then the anode. It can be cut and stacked in various form factors."

Washington State University researchers expect to bring to market before June 2013 a tin anode technology that will triple the energy capacity of lithium ion batteries. The technology involves using standard electroplating process to create tin nanoneedles.

Sandia has studied ways to improve safety and robustness of lithium ion batteries by using different electrolytes and separators.

Microporous Tin has been used as a substrate for anode and cathodes 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 anode, LiMnO₂ for cathode.)

Extrusion

PARC’s Hardware Systems Laboratory designed a cathode that contains more lithium by using one dense material optimised for storage and a second, porous one to enable the speedy transfer of charge. Wide storage regions alternate with narrow conductive regions. The storage region is 100 microns across, compared with ten for the conductor.

The two materials are mixed with an organic material to form pastes and fed into an additive manufacturing device that extrudes the pastes adjacent to each other on a metal foil. Drying the substrate removes most of the organic material, leaving a solid cathode. In tests against otherwise identical batteries with monolithic cathodes, the new battery could store twenty percent more energy.

The researchers envision extruding entire batteries using five pastes—two each for the cathode and the anode, plus a separator.

See also

• Potassium-ion battery
• Nanowire battery
• List of battery sizes
• List of battery types

Bibliography

• Winter, M.; Brodd, J. (2004). "What Are Batteries, Fuel Cells, and Supercapacitors?". Chemical Review (PDF) 104 (104): 4245. doi:10.1021/cr020730k. 

External links

• Lithium batteries at the Open Directory Project