Lithium-ion battery

A 3.6 V Li-ion battery from a Nokia 3310 mobile phone
Specific energy	100–265 W⋅h/kg (360–950 kJ/kg)[1][2]
Energy density	250–693 W⋅h/L (900–2,490 J/cm3)[3][4]
Specific power	c. 250–340 W/kg[1]
Charge/discharge efficiency	80–90%[5]
Energy/consumer-price	7.6 Wh/US$ (US$132/kWh)[6]
Self-discharge rate	0.35% to 2.5% per month depending on state of charge[7]
Cycle durability	400–1,200 cycles [8]
Nominal cell voltage	3.6 / 3.7 / 3.8 / 3.85 V, LiFePO4 3.2 V, Li4Ti5O12 2.3 V

A lithium-ion or Li-ion battery is a type of rechargeable battery that uses the reversible intercalation of Li⁺ ions into electronically conducting solids to store energy. In comparison with other commercial rechargeable batteries, Li-ion batteries are characterized by higher specific energy, higher energy density, higher energy efficiency, a longer cycle life, and a longer calendar life. Also noteworthy is a dramatic improvement in lithium-ion battery properties after their market introduction in 1991: within the next 30 years, their volumetric energy density increased threefold while their cost dropped tenfold.^[9]

There are at least 12 different chemistries of Li-ion batteries, see List of battery types

The invention and commercialization of Li-ion batteries may have had one of the greatest impacts of all technologies in human history,^[10] as recognized by the 2019 Nobel Prize in Chemistry. More specifically, Li-ion batteries enabled portable consumer electronics, laptop computers, cellular phones, and electric cars, or what has been called the e-mobility revolution.^[11] It also sees significant use for grid-scale energy storage as well as military and aerospace applications.

Lithium-ion cells can be manufactured to optimize energy or power density.^[12] Handheld electronics mostly use lithium polymer batteries (with a polymer gel as an electrolyte), a lithium cobalt oxide (LiCoO
₂) cathode material, and a graphite anode, which together offer high energy density.^[13][14] Lithium iron phosphate (LiFePO
₄), lithium manganese oxide (LiMn
₂O
₄ spinel, or Li
₂MnO
₃-based lithium-rich layered materials, LMR-NMC), and lithium nickel manganese cobalt oxide (LiNiMnCoO
₂ or NMC) may offer longer life and a higher discharge rate. NMC and its derivatives are widely used in the electrification of transport, one of the main technologies (combined with renewable energy) for reducing greenhouse gas emissions from vehicles.^[15]

M. Stanley Whittingham conceived intercalation electrodes in the 1970s and created the first rechargeable lithium-ion battery, based on a titanium disulfide cathode and a lithium-aluminum anode, although it suffered from safety problems and was never commercialized.^[16] John Goodenough expanded on this work in 1980 by using lithium cobalt oxide as a cathode.^[17] The first prototype of the modern Li-ion battery, which uses a carbonaceous anode rather than lithium metal, was developed by Akira Yoshino in 1985 and commercialized by a Sony and Asahi Kasei team led by Yoshio Nishi in 1991.^[18] M. Stanley Whittingham, John Goodenough, and Akira Yoshino were awarded the 2019 Nobel Prize in Chemistry for their contributions to the development of lithium-ion batteries.

Lithium-ion batteries can be a safety hazard if not properly engineered and manufactured because they have flammable electrolytes that, if damaged or incorrectly charged, can lead to explosions and fires. Much progress has been made in the development and manufacturing of safe lithium-ion batteries.^[19] Lithium-ion solid-state batteries are being developed to eliminate the flammable electrolyte. Improperly recycled batteries can create toxic waste, especially from toxic metals, and are at risk of fire. Moreover, both lithium and other key strategic minerals used in batteries have significant issues at extraction, with lithium being water intensive in often arid regions and other minerals used in some Li-ion chemistries potentially being conflict minerals such as cobalt.^{[not verified in body]} Both environmental issues have encouraged some researchers to improve mineral efficiency and find alternatives such as Lithium iron phosphate lithium-ion chemistries or non-lithium-based battery chemistries like iron-air batteries.

Research areas for lithium-ion batteries include extending lifetime, increasing energy density, improving safety, reducing cost, and increasing charging speed,^[20][21] among others. Research has been under way in the area of non-flammable electrolytes as a pathway to increased safety based on the flammability and volatility of the organic solvents used in the typical electrolyte. Strategies include aqueous lithium-ion batteries, ceramic solid electrolytes, polymer electrolytes, ionic liquids, and heavily fluorinated systems.^{[22][23][24][25]}

History

Research on rechargeable Li-ion batteries dates to the 1960s; one of the earliest examples is a CuF
₂/Li battery developed by NASA in 1965. The breakthrough that produced the earliest form of the modern Li-ion battery was made by British chemist M. Stanley Whittingham in 1974, who first used titanium disulfide (TiS
₂) as a cathode material, which has a layered structure that can take in lithium ions without significant changes to its crystal structure. Exxon tried to commercialize this battery in the late 1970s, but found the synthesis expensive and complex, as TiS
₂ is sensitive to moisture and releases toxic H
₂S gas on contact with water. More prohibitively, the batteries were also prone to spontaneously catch fire due to the presence of metallic lithium in the cells. For this, and other reasons, Exxon discontinued the development of Whittingham's lithium-titanium disulfide battery.^[26]

In 1980, working in separate groups Ned A. Godshall et al.,^[27][28][29] and, shortly thereafter, Koichi Mizushima and John B. Goodenough, after testing a range of alternative materials, replaced TiS
₂ with lithium cobalt oxide (LiCoO
₂, or LCO), which has a similar layered structure but offers a higher voltage and is much more stable in air. This material would later be used in the first commercial Li-ion battery, although it did not, on its own, resolve the persistent issue of flammability.^[26]

These early attempts to develop rechargeable Li-ion batteries used lithium metal anodes, which were ultimately abandoned due to safety concerns, as lithium metal is unstable and prone to dendrite formation, which can cause short-circuiting. The eventual solution was to use an intercalation anode, similar to that used for the cathode, which prevents the formation of lithium metal during battery charging. A variety of anode materials were studied. In 1980, Rachid Yazami demonstrated reversible electrochemical intercalation of lithium in graphite,^[30][31] a concept originally proposed by Jürgen Otto Besenhard in 1974 but considered unfeasible due to unresolved incompatibilities with the electrolytes then in use.^[26][32][33] In fact, Yazami's work was itself limited to a solid electrolyte (polyethylene oxide), because liquid solvents tested by him and before co-intercalated with Li⁺ ions into graphite, causing the graphite to crumble.

In 1985, Akira Yoshino at Asahi Kasei Corporation discovered that petroleum coke, a less graphitized form of carbon, can reversibly intercalate Li-ions at a low potential of ~0.5 V relative to Li+ /Li without structural degradation.^[34] Its structural stability originates from the amorphous carbon regions in petroleum coke serving as covalent joints to pin the layers together. Although the amorphous nature of petroleum coke limits capacity compared to graphite (~Li0.5C6, 0.186 Ah g–1), it became the first commercial intercalation anode for Li-ion batteries owing to its cycling stability.

in 1987, Akira Yoshino patented what would become the first commercial lithium-ion battery using an anode of "soft carbon" (a charcoal-like material) along with Goodenough's previously reported LiCoO₂ cathode and a carbonate ester-based electrolyte. This battery is assembled in a discharged state, which makes its manufacturing safer and cheaper. In 1991, using Yoshino's design, Sony began producing and selling the world's first rechargeable lithium-ion batteries. The following year, a joint venture between Toshiba and Asashi Kasei Co. also released their lithium-ion battery.^[26]

Significant improvements in energy density were achieved in the 1990s by replacing the soft carbon anode first with hard carbon and later with graphite. In 1990, Jeff Dahn and two colleagues at Dalhousie University (Canada) reported reversible intercalation of lithium ions into graphite in the presence of ethylene carbonate solvent (which is solid at room temperature and is mixed with other solvents to make a liquid), thus finding the final piece of the puzzle leading to the modern lithium-ion battery.^[35]

In 2010, global lithium-ion battery production capacity was 20 gigawatt-hours.^[36] By 2016, it was 28 GWh, with 16.4 GWh in China.^[37] Global production capacity was 767 GWh in 2020, with China accounting for 75%.^[38] Production in 2021 is estimated by various sources to be between 200 and 600 GWh, and predictions for 2023 range from 400 to 1,100 GWh.^[39]

In 2012, John B. Goodenough, Rachid Yazami and Akira Yoshino received the 2012 IEEE Medal for Environmental and Safety Technologies for developing the lithium-ion battery; Goodenough, Whittingham, and Yoshino were awarded the 2019 Nobel Prize in Chemistry "for the development of lithium-ion batteries".^[40] Jeff Dahn received the ECS Battery Division Technology Award (2011) and the Yeager award from the International Battery Materials Association (2016).

In April 2023, CATL announced that it would begin scaled-up production of its semi-solid condensed matter battery that produces a then record 500 Wh/kg. They use electrodes made from a gelled material, requiring fewer binding agents. This in turn shortens the manufacturing cycle. One potential application is in battery-powered airplanes.^[41][42][43] Another new development of lithium-ion batteries are flow batteries with redox-targeted solids,that use no binders or electron-conducting additives, and allow for completely independent scaling of energy and power.^[44]

Design

Generally, the negative electrode of a conventional lithium-ion cell is graphite made from carbon. The positive electrode is typically a metal oxide or phosphate. The electrolyte is a lithium salt in an organic solvent.^[45] The negative electrode (which is the anode when the cell is discharging) and the positive electrode (which is the cathode when discharging) are prevented from shorting by a separator.^[46] The electrodes are separated from external electronics with a piece of metal called a current collector.^[47]

The negative and positive electrodes swap their electrochemical roles (anode and cathode) when the cell is charged. Despite this, in discussions of battery design the negative electrode of a rechargeable cell is often just called "the anode" and the positive electrode "the cathode".

In its fully lithiated state of LiC₆, graphite correlates to a theoretical capacity of 1339 coulombs per gram (372 mAh/g).^[48] 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).^[49] More experimental materials include graphene-containing electrodes, although these remain far from commercially viable due to their high cost.^[50]

Lithium reacts vigorously with water to form lithium hydroxide (LiOH) and hydrogen gas. Thus, a non-aqueous electrolyte is typically used, and a sealed container rigidly excludes moisture from the battery pack. The non-aqueous electrolyte is typically a mixture of organic carbonates such as ethylene carbonate and propylene carbonate containing complexes of lithium ions.^[51] Ethylene carbonate is essential for making solid electrolyte interphase on the carbon anode,^[52] but since it is solid at room temperature, a liquid solvent (such as propylene carbonate or diethyl carbonate) is added.

The electrolyte salt is almost always^{[citation needed]} lithium hexafluorophosphate (LiPF
₆), which combines good ionic conductivity with chemical and electrochemical stability. The hexafluorophosphate anion is essential for passivating the aluminum current collector used for the positive electrode. A titanium tab is ultrasonically welded to the aluminum current collector. Other salts like lithium perchlorate (LiClO
₄), lithium tetrafluoroborate (LiBF
₄), and lithium bis(trifluoromethanesulfonyl)imide (LiC
₂F
₆NO
₄S
₂) are frequently used in research in tab-less coin cells, but are not usable in larger format cells,^[53] often because they are not compatible with the aluminum current collector. Copper (with a spot-welded nickel tab) is used as the current collector at the negative electrode.

Current collector design and surface treatments may take various forms: foil, mesh, foam (dealloyed), etched (wholly or selectively), and coated (with various materials) to improve electrical characteristics.^[47]

Depending on materials choices, the voltage, energy density, life, and safety of a lithium-ion cell can change dramatically. Current effort has been exploring the use of novel architectures using nanotechnology to improve performance. Areas of interest include nano-scale electrode materials and alternative electrode structures.^[54]

Electrochemistry

The reactants in the electrochemical reactions in a lithium-ion cell are the materials of the electrodes, both of which are compounds containing lithium atoms. Although many thousands of different materials have been investigated for use in lithium-ion batteries, only a very small number are commercially usable. All commercial Li-ion cells use intercalation compounds as active materials.^[55] The negative electrode is usually graphite, although silicon is often mixed in to increase the capacity. The solvent is usually lithium hexafluorophosphate, dissolved in a mixture of organic carbonates. A number of different materials are used for the positive electrode, such as LiCoO₂, LiFePO₄, and lithium nickel manganese cobalt oxides.

During cell discharge the negative electrode is the anode and the positive electrode the cathode: electrons flow from the anode to the cathode through the external circuit. An oxidation half-reaction at the anode produces positively charged lithium ions and negatively charged electrons. The oxidation half-reaction may also produce uncharged material that remains at the anode. Lithium ions move through the electrolyte; electrons move through the external circuit toward the cathode where they recombine with the cathode material in a reduction half-reaction. The electrolyte provides a conductive medium for lithium ions but does not partake in the electrochemical reaction. The reactions during discharge lower the chemical potential of the cell, so discharging transfers energy from the cell to wherever the electric current dissipates its energy, mostly in the external circuit.

During charging these reactions and transports go in the opposite direction: electrons move from the positive electrode to the negative electrode through the external circuit. To charge the cell the external circuit has to provide electrical energy. This energy is then stored as chemical energy in the cell (with some loss, e. g., due to coulombic efficiency lower than 1).

Both electrodes allow lithium ions to move in and out of their structures with a process called insertion (intercalation) or extraction (deintercalation), respectively.

As the lithium ions "rock" back and forth between the two electrodes, these batteries are also known as "rocking-chair batteries" or "swing batteries" (a term given by some European industries).^[56][57]

The following equations exemplify the chemistry (left to right: discharging, right to left: charging).

The negative electrode half-reaction for the graphite is^[58][59]

${\displaystyle {\ce {LiC6 <=> C6 + Li+ + e^-}}}$

The positive electrode half-reaction in the lithium-doped cobalt oxide substrate is

${\displaystyle {\ce {CoO2 + Li+ + e- <=> LiCoO2}}}$

The full reaction being

${\displaystyle {\ce {LiC6 + CoO2 <=> C6 + LiCoO2}}}$

The overall reaction has its limits. Overdischarging supersaturates lithium cobalt oxide, leading to the production of lithium oxide,^[60] possibly by the following irreversible reaction:

${\displaystyle {\ce {Li+ + e^- + LiCoO2 -> Li2O + CoO}}}$

Overcharging up to 5.2 volts leads to the synthesis of cobalt (IV) oxide, as evidenced by x-ray diffraction:^[61]

${\displaystyle {\ce {LiCoO2 -> Li+ + CoO2 + e^-}}}$

The transition metal in the positive electrode, cobalt (Co), is reduced from Co⁴⁺
to Co³⁺
during discharge, and oxidized from Co³⁺
to Co⁴⁺
during charge.

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 kilogram of lithium. 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.

Note that the cell voltages involved in these reactions are larger than the potential at which an aqueous solutions would electrolyze.

Discharging and charging

During discharge, lithium ions (Li⁺
) carry the current within the battery cell from the negative to the positive electrode, through the non-aqueous electrolyte and separator diaphragm.^[62]

During charging, an external electrical power source applies an over-voltage (a voltage greater than the cell's own voltage) to the cell, forcing electrons to flow from the positive to the negative electrode. The lithium ions also migrate (through the electrolyte) from the positive to the negative electrode where they become embedded in the porous electrode material in a process known as intercalation.

Energy losses arising from electrical contact resistance at interfaces between electrode layers and at contacts with current collectors can be as high as 20% of the entire energy flow of batteries under typical operating conditions.^[63]

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

• A single Li-ion cell is charged in two stages:^[64][65]

1. Constant current (CC)
2. Constant voltage (CV)

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

1. Constant current
2. Balance (only required when cell groups become unbalanced during use)
3. Constant voltage

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

During the balance phase, the charger/battery reduces the charging current (or cycles 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. Balancing typically occurs whenever one or more cells reach their top-of-charge voltage before the other(s), as it is generally inaccurate to do so at other stages of the charge cycle. This is most commonly done by passive balancing, which dissipates excess charge via resistors connected momentarily across the cell(s) to be balanced. Active balancing is less common, more expensive, but more efficient, returning excess energy to other cells (or the entire pack) through the means of a DC-DC converter or other circuitry. Some fast chargers skip this stage. Some chargers accomplish the balance by charging each cell independently. This is often performed by the battery protection circuit/battery management system (BPC or BMS) and not the charger (which typically provides only the bulk charge current, and does not interact with the pack at the cell-group level), e.g., e-bike and hoverboard chargers. In this method, the BPC/BMS will request a lower charge current (such as EV batteries), or will shut-off the charging input (typical in portable electronics) through the use of transistor circuitry while balancing is in effect (to prevent over-charging cells). Balancing most often occurs during the constant voltage stage of charging, switching between charge modes until complete. The pack is usually fully charged only when balancing is complete, as even a single cell group lower in charge than the rest will limit the entire battery's usable capacity to that of its own. Balancing can last hours or even days, depending on the magnitude of the imbalance in the battery.

During the constant voltage phase, the charger applies 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. ^{[dubious – discuss]}

Failure to follow current and voltage limitations can result in an explosion.^[66][67]

Charging temperature limits for Li-ion are stricter than the operating limits. Lithium-ion chemistry performs well at elevated temperatures but prolonged exposure to heat reduces battery life. Li‑ion batteries offer good charging performance at cooler temperatures and may even allow "fast-charging" within a temperature range of 5 to 45 °C (41 to 113 °F).^{[68][better source needed]} 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 a low-temperature (under 0 °C) charge, the slight temperature rise above ambient due to the internal cell resistance is beneficial. High temperatures during charging may lead to battery degradation and charging at temperatures above 45 °C will degrade battery performance, whereas at lower temperatures the internal resistance of the battery may increase, resulting in slower charging and thus longer charging times.^{[68][better source needed]}

Batteries gradually self-discharge even if not connected and delivering current. Li-ion rechargeable batteries have a self-discharge rate typically stated by manufacturers to be 1.5–2% per month.^[69][70]

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.^[71] Self-discharge rates may increase as batteries age.^[72] In 1999, self-discharge per month was measured at 8% at 21 °C, 15% at 40 °C, 31% at 60 °C.^[73] By 2007, monthly self-discharge rate was estimated at 2% to 3%, and 2^[7]–3% by 2016.^[74]

By comparison, the self-discharge rate for NiMH batteries dropped, as of 2017, from up to 30% per month for previously common cells^[75] to about 0.08–0.33% per month for low self-discharge NiMH batteries, and is about 10% per month in NiCd batteries.^{[citation needed]}

Cathode

There are three classes of commercial cathode materials in lithium-ion batteries: (1) layered oxides, (2) spinel oxides and (3) oxoanion complexes. All of them were discovered by John Goodenough and his collaborators.^[76]

(a) Layered Oxides

LiCoO₂ was used in the first commercial lithium-ion battery made by Sony in 1991. The layered oxides have a pseudo-tetrahedral structure comprising layers made of MO₆ octahedra separated by interlayer spaces that allow for two-dimensional lithium-ion diffusion.^{[citation needed]} The band structure of Li_xCoO₂ allows for true electronic (rather than polaronic) conductivity. However, due to an overlap between the Co⁴⁺ t_2g d-band with the O^2- 2p-band, the x must be >0.5, otherwise O₂ evolution occurs. This limits the charge capacity of this material to ~140 mA h g^-1.^[76]

Several other first-row (3d) transition metals form layered LiMO₂ salts. Some of them can be directly prepared from lithium oxide and M₂O₃ (e.g. for M=Ti, V, Cr, Co, Ni), while others (M= Mn or Fe) can be prepared by ion exchange from NaMO₂. LiVO₂, LiMnO₂ and LiFeO₂ suffer from structural instabilities (including mixing between M and Li sites) due to a low energy difference between octahedral and tetrahedral environments for the metal ion M. For this reason, they are not used in lithium-ion batteries.^[76] However, Na⁺ and Fe³⁺ have sufficiently different sizes that NaFeO₂ can be used in sodium-ion batteries.^[77]

Similarly, LiCrO₂ shows reversible lithium (de)intercalation around 3.2 V with 170-270 mAh/g.^[78] However, its cycle life is short, because of disproportionation of Cr⁴⁺ followed by translocation of Cr⁶⁺ into tetrahedral sites.^[79] On the other hand, NaCrO₂ shows a much better cycling stability.^[80] LiTiO₂ shows Li+ (de)intercalation at a voltage of ~1.5 V, which is too low for a cathode material.

These problems leave LiCoO
₂ and LiNiO
₂ as the only practical layered oxide materials for lithium-ion battery cathodes. The cobalt-based cathodes show high theoretical specific (per-mass) charge capacity, high volumetric capacity, low self-discharge, high discharge voltage, and good cycling performance. Unfortunately, they suffer from a high cost of the material.^[81] For this reason, the current trend among lithium-ion battery manufacturers is to switch to cathodes with higher Ni content and lower Co content.^[82]

In addition to a lower (than cobalt) cost, nickel-oxide based materials benefit from the two-electron redox chemistry of Ni: in layered oxides comprising nickel (such as nickel-cobalt-manganese NCM and nickel-cobalt-aluminium oxides NCA), Ni cycles between the oxidation states +2 and +4 (in one step between +3.5 and +4.3 V),^[83][76] cobalt- between +2 and +3, while Mn (usually >20%) and Al (typically, only 5% is needed)^[84] remain in +4 and 3+, respectively. Thus increasing the Ni content increases the cyclable charge. For example, NCM111 shows 160 mAh/g, while LiNi0.8Co0.1Mn0.1O2 (NCM811) and LiNi0.8Co0.15Al0.05O2 (NCA) deliver a higher capacity of ~200 mAh/g.^[85]

It is worth mentioning so-called "lithium-rich" cathodes, that can be produced from traditional NCM (LiMO2, where M=Ni, Co, Mn) layered cathode materials upon cycling them to voltages/charges corresponding to Li:M<0.5. Under such conditions a new semi-reversible redox transition at a higher voltage with ca. 0.4-0.8 electrons/metal site charge appears. This transition involves non-binding electron orbitals centered mostly on O atoms. Despite significant initial interest, this phenomenon did not result in marketable products because of the fast structural degradation (O2 evolution and lattice rearrangements) of such "lithium-rich" phases.^[86]

(b) Cubic oxides (spinels)

LiMn2O4 adopts a cubic lattice, which allows for three-dimensional lithium-ion diffusion.^[87] Manganese cathodes are attractive because manganese is less expensive than cobalt or nickel. The operating voltage of Li-LiMn2O4 battery is 4 V, and ca. one lithium per two Mn ions can be reversibly extracted from the tetrahedral sites, resulting in a practical capacity of <130 mA h g–1. However, Mn³⁺ is not a stable oxidation state, as it tends to disporportionate into insoluble Mn⁴⁺ and soluble Mn²⁺.^[81][88] LiMn2O4 can also intercalate more than 0.5 Li per Mn at a lower voltage around +3.0 V. However, this results in an irreversible phase transition due to Jahn-Teller distortion in Mn3+:t2g3eg1, as well as disproportionation and dissolution of Mn³⁺.

An important improvement of Mn spinel are related cubic structures of the LiMn1.5Ni0.5O4 type, where Mn exists as Mn4+ and Ni cycles reversibly between the oxidation states +2 and +4.^[76] This materials show a reversible Li-ion capacity of ca. 135 mAh/g around 4.7 V. Although such high voltage is beneficial for increasing the specific energy of batteries, the adoption of such materials is currently hindered by the lack of suitable high-voltage electrolytes.^[89] In general, materials with a high nickel content are favored in 2023, because of the possibility of a 2-electron cycling of Ni between the oxidation states +2 and +4.

LiV2O4 operates as a lower (ca. +3.0V) voltage than LiMn2O4, suffers from similar durability issues, is more expensive, and thus is not considered of practical interest.^[90]

(c) Oxoanionic/olivins

Around 1980 Manthiram discovered, that oxoanions (molybdates and tungstates in that particular case) cause a substantial positive shift in the redox potential of the metal-ion compared to oxides.^[91] In addition, these oxoanionic cathode materials offer better stability/safety than the corresponding oxides. On the other hand, unlike the aforementioned oxides, oxoanionic cathodes suffer from poor electronic conductivity, which stems primarily from a long distance between redox-active metal centers, which slows down the electron transport. This necessitates the use of small (<200 nm) cathode particles and coatng each particle with a layer of electroncally-conducting carbon to overcome its low electrical conductivity.^[92] This further reduces the packing density of these materials.

Although numerous oxoanions (sulfate, phosphate, silicate) / metal (Mn, Fe, Co, Ni) cation combinations have been studied since, LiFePO4 is the only one, that reached the market. As of 2023^[update], LiFePO
₄ is the primary candidate for large-scale use of lithium-ion batteries for stationary energy storage (rather than electric vehicles) due to its low cost, excellent safety, and high cycle durability. For example, Sony Fortelion batteries have retained 74% of their capacity after 8000 cycles with 100% discharge.^[93]

Positive electrode

Technology	Company	Target application	Benefit
Lithium nickel manganese cobalt oxide NMC, LiNixMnyCozO2	Imara Corporation, Nissan Motor,[94][95] Microvast Inc., LG Chem,[96] Northvolt[97]	Electric vehicles, power tools, grid energy storage	Good specific energy and specific power density
Lithium nickel cobalt aluminium oxide NCA, LiNiCoAlO2	Panasonic,[96] Saft Groupe S.A.[98] Samsung[99]	Electric vehicles, power tools, grid energy storage	High specific energy, good life span
Lithium nickel cobalt manganese aluminum oxide NCMA, LiNi 0.89Co 0.05Mn 0.05Al 0.01O 2	LG Chem,[100] Hanyang University[101]	Electric vehicles, grid energy storage	Good specific energy, improved long-term cycling stability, faster charging
Lithium manganese oxide LMO, LiMn2O4	LG Chem,[102] NEC, Samsung,[103] Hitachi,[104] Nissan/AESC,[105] EnerDel[106]	Hybrid electric vehicle, cell phone, laptop
Lithium iron phosphate LFP, LiFePO4	University of Texas/Hydro-Québec,[107] Phostech Lithium Inc., Valence Technology, A123Systems/MIT[108][109]	Electric vehicles, Segway Personal Transporter, power tools, aviation products, automotive hybrid systems, PHEV conversions	moderate density (2 A·h outputs 70 amperes) High safety compared to Cobalt / Manganese systems. Operating temperature >60 °C (140 °F)
Lithium cobalt oxide LCO, LiCoO2	Sony first commercial production[110][111]	Broad use, laptop	High specific energy

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