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A '''lithium-ion''' or '''Li-ion battery''' is a type of [[rechargeable battery]] that uses the reversible [[Intercalation (chemistry)|intercalation]] of Li<sup>+</sup> ions into [[electronically]] [[Electrical conductor|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 (physics)|energy efficiency]], a longer [[cycle life]], and a longer [[durability|calendar life]]. Also noteworthy is a dramatic improvement in lithium-ion battery properties after their market introduction in 1991:
There are at least 12 different chemistries of Li-ion batteries; see "[[List of battery types]]."
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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.<ref>{{cite web | url=https://www.evolute.in/e-mobility-revolution-lithium-ion-batteries-powering-the-transportation-industry/#:~:text=While%20lithium%2Dion%20batteries%20have,extending%20the%20range%20of%20EVs | title=E-Mobility Revolution : Lithium-Ion Batteries Powering the Transportation Industry - Evolute | date=29 September 2023 | access-date=27 October 2023 | archive-date=27 October 2023 | archive-url=https://web.archive.org/web/20231027221649/https://www.evolute.in/e-mobility-revolution-lithium-ion-batteries-powering-the-transportation-industry/#:~:text=While%20lithium%2Dion%20batteries%20have,extending%20the%20range%20of%20EVs | url-status=live }}</ref> It also sees significant use for [[Battery storage power station|grid-scale energy storage]] as well as military and [[aerospace]] applications.
Lithium-ion cells can be manufactured to optimize energy or power density.<ref>{{Cite journal|last1=Lain|first1=Michael J.|last2=Brandon |first2=James|last3=Kendrick|first3=Emma |date=December 2019|title=Design Strategies for High Power vs. High Energy Lithium Ion Cells|journal=Batteries|language=en|volume=5|issue=4|pages=64 |doi=10.3390/batteries5040064|quote=Commercial lithium ion cells are now optimized for either high energy density or high power density. There is a trade-off in cell design between power and energy requirements.|doi-access=free}}</ref> Handheld electronics mostly use [[Lithium polymer battery|lithium polymer batteries]] (with a polymer gel as an electrolyte), a [[lithium cobalt oxide]] ({{chem|LiCoO|2}}) cathode material, and a [[graphite]] anode, which together offer high energy density.<ref>{{cite journal |last1=Mauger |first1=A |last2=Julien |first2=C.M. |date=28 June 2017 |title=Critical review on lithium-ion batteries: are they safe? Sustainable? |journal=Ionics |volume=23 |issue=8 |pages=1933–1947 |doi=10.1007/s11581-017-2177-8 |s2cid=103350576 |url=https://hal.sorbonne-universite.fr/hal-01558209/file/Mauger_2017_Critical_review_on.pdf |access-date=26 July 2019 |archive-date=2 March 2023 |archive-url=https://web.archive.org/web/20230302135828/https://hal.sorbonne-universite.fr/hal-01558209/file/Mauger_2017_Critical_review_on.pdf |url-status=live }}</ref><ref name="E-electric20200604" /> [[Lithium iron phosphate]] ({{chem|LiFePO|4}}), [[lithium ion manganese oxide battery|lithium manganese oxide]] ({{chem|LiMn|2|O|4}} [[spinel]], or {{chem|Li|2|MnO|3}}-based lithium-rich layered materials, LMR-NMC), and [[lithium nickel manganese cobalt oxide]] ({{chem|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|greenhouse gas emissions from vehicles]].<ref>{{Cite journal |last1=Zhang |first1=Runsen |last2=Fujimori |first2=Shinichiro |date=2020-02-19 |title=The role of transport electrification in global climate change mitigation scenarios |journal=Environmental Research Letters |language=en |volume=15 |issue=3 |pages=034019 |doi=10.1088/1748-9326/ab6658 |bibcode=2020ERL....15c4019Z |s2cid=212866886 |issn=1748-9326|doi-access=free |hdl=2433/245921 |hdl-access=free }}</ref>
[[M. Stanley Whittingham]] conceived [[intercalation (chemistry)|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.<ref name="rfsuny">{{cite web |title=Binghamton professor recognized for energy research |url=https://www.rfsuny.org/rf-news/binghamton-energy/binghamton---energy.html |website=The Research Foundation for the State University of New York |access-date=10 October 2019 |archive-date=30 October 2017 |archive-url=https://web.archive.org/web/20171030175258/https://www.rfsuny.org/rf-news/binghamton-energy/binghamton---energy.html |url-status=live }}</ref> [[John Goodenough]] expanded on this work in 1980 by using [[lithium cobalt oxide]] as a cathode.<ref name="nobel">{{cite web |title=The Nobel Prize in Chemistry 2019 |url=https://www.nobelprize.org/prizes/chemistry/2019/summary/ |website=[[Nobel Prize]] |publisher=[[Nobel Foundation]] |year=2019 |access-date=1 January 2020 |archive-date=21 May 2020 |archive-url=https://web.archive.org/web/20200521195355/https://www.nobelprize.org/prizes/chemistry/2019/summary/ |url-status=live }}</ref> 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.<ref name="NAE">{{cite web | title = Yoshio Nishi | url = https://www.nae.edu/105800/Yoshio-Nishi | website = [[National Academy of Engineering]] | access-date = 12 October 2019 | archive-date = 11 April 2019 | archive-url = https://web.archive.org/web/20190411130013/https://www.nae.edu/105800/Yoshio-Nishi | url-status = live }}</ref> [[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.<ref>{{cite journal | doi=10.1016/j.jechem.2020.10.017 | title=A review of lithium-ion battery safety concerns: The issues, strategies, and testing standards | year=2021 | last1=Chen | first1=Yuqing | last2=Kang | first2=Yuqiong | last3=Zhao | first3=Yun | last4=Wang | first4=Li | last5=Liu | first5=Jilei | last6=Li | first6=Yanxi | last7=Liang | first7=Zheng | last8=He | first8=Xiangming | last9=Li | first9=Xing | last10=Tavajohi | first10=Naser | last11=Li | first11=Baohua | journal=Journal of Energy Chemistry | volume=59 | pages=83–99 | s2cid=228845089 | doi-access=free | bibcode=2021JEnCh..59...83C }}</ref> Lithium-ion [[Solid-state battery|solid-state batteries]] are being developed to eliminate the flammable electrolyte. Improperly [[Battery recycling|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 resource|conflict minerals]] such as [[cobalt]].{{not verified in body|date=April 2024}} Both [[Environmental impacts of lithium-ion batteries|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 battery|iron-air batteries]].
Research areas for lithium-ion batteries include extending lifetime, increasing energy density, improving safety, reducing cost, and increasing charging speed,<ref>{{cite journal | doi = 10.1021/acssuschemeng.7b00046 | title = Lithium-Ion Batteries with High Rate Capabilities |last= Eftekhari| first= Ali| year=2017| journal=ACS Sustainable Chemistry & Engineering| volume=5|issue=3|pages=2799–2816 }}</ref><ref>{{Cite web |title=Rising Lithium Costs Threaten Grid-Scale Energy Storage - News |url=https://eepower.com/news/rising-lithium-costs-threaten-grid-scale-energy-storage/ |access-date=2022-11-02 |website=eepower.com |language=en |archive-date=9 June 2022 |archive-url=https://web.archive.org/web/20220609180453/https://eepower.com/news/rising-lithium-costs-threaten-grid-scale-energy-storage/ |url-status=live }}</ref> 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 battery|aqueous lithium-ion batteries]], ceramic solid electrolytes, polymer electrolytes, ionic liquids, and heavily fluorinated systems.<ref>{{Cite news|url=https://www.futurity.org/lithium-ion-batteries-1606992-2/|title=Watch: Cuts and dunks don't stop new lithium-ion battery - Futurity|last=Hopkins|first=Gina|date=16 November 2017|work=Futurity|access-date=10 July 2018|archive-date=10 July 2018|archive-url=https://web.archive.org/web/20180710195029/https://www.futurity.org/lithium-ion-batteries-1606992-2/|url-status=live}}</ref><ref>{{Cite journal | last1 = Chawla | first1 = N. | last2 = Bharti | first2 = N. | last3 = Singh | first3 = S. |doi = 10.3390/batteries5010019 | title = Recent Advances in Non-Flammable Electrolytes for Safer Lithium-Ion Batteries| journal = Batteries| volume = 5 | page = 19 | year = 2019 | doi-access = free }}</ref><ref>{{Cite journal | last1 = Yao | first1 = X.L. | last2 = Xie | first2 = S. | last3 = Chen | first3 = C. | last4 = Wang | first4 = Q.S. |last5 = Sun | first5 = J. |last6 = Wang | first6 = Q.S. |last7 = Sun | first7 = J. |doi = 10.1016/j.jpowsour.2004.11.042| title = Comparative study of trimethyl phosphite and trimethyl phosphate as electrolyte additives in lithium ion batteries| journal = Journal of Power Sources| volume = 144 | pages = 170–175 |year = 2004 }}</ref><ref>{{Cite journal | last1 = Fergus | first1 = J.W. | doi = 10.1016/j.jpowsour.2010.01.076| title = Ceramic and polymeric solid electrolytes for lithium-ion batteries| journal = Journal of Power Sources| volume = 195 | issue = 15 | pages = 4554–4569 |year = 2010 | bibcode = 2010JPS...195.4554F }}</ref>
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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 (crystal)|dendrite]] formation, which can cause [[Short circuit|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,<ref>International Meeting on Lithium Batteries, Rome, 27–29 April 1982, C.L.U.P. Ed. Milan, Abstract #23</ref><ref>{{Cite journal | last1 = Yazami | first1 = R. | last2 = Touzain | first2 = P. | doi = 10.1016/0378-7753(83)87040-2 | title = A reversible graphite-lithium negative electrode for electrochemical generators | journal = Journal of Power Sources | volume = 9 | issue = 3 | pages = 365–371 | year = 1983 | bibcode = 1983JPS.....9..365Y }}</ref> a concept originally proposed by Jürgen Otto Besenhard in 1974 but considered unfeasible due to unresolved incompatibilities with the electrolytes then in use.<ref name="Li-2018" /><ref>{{Cite journal |last1=Besenhard |first1=J. O. |last2=Eichinger |first2=G. |year=1976 |title=High energy density lithium cells |journal=Journal of Electroanalytical Chemistry and Interfacial Electrochemistry |volume=68 |pages=1–18 |doi=10.1016/S0022-0728(76)80298-7}}</ref><ref>{{Cite journal |last1=Eichinger |first1=G. |last2=Besenhard |first2=J. O. |year=1976 |title=High energy density lithium cells |journal=Journal of Electroanalytical Chemistry and Interfacial Electrochemistry |volume=72 |pages=1–31 |doi=10.1016/S0022-0728(76)80072-1}}</ref> 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<sup>+</sup> 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.<ref>Yoshino, A., Sanechika, K. & Nakajima, T. Secondary battery. JP patent 1989293 (1985)</ref> 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
in 1987, [[Akira Yoshino]] patented what would become the first commercial lithium-ion battery using an anode of "[[Hard carbon|soft carbon]]" (a charcoal-like material) along with Goodenough's previously reported [[LiCoO2|LiCoO<sub>2</sub>]] 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 [[Asahi Kasei|Asashi Kasei]] Co. also released their lithium-ion battery.<ref name="Li-2018" />
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[[File:Liion-18650-AA-battery.jpg|thumb|upright|Left: AA alkaline battery. Right: 18650 lithium ion battery]]
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 (chemistry)|salt]] in an [[organic compound|organic]] [[solvent]].<ref name="auto">Silberberg, M. (2006). ''Chemistry: The Molecular Nature of Matter and Change'', 4th Ed. New York (NY): McGraw-Hill Education. p. 935, {{ISBN|0077216504}}.</ref> 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.<ref name="auto1">{{Cite journal |last1=Li |first1=Ao |last2=Yuen |first2=Anthony Chun Yin |last3=Wang |first3=Wei |last4=De Cachinho Cordeiro |first4=Ivan Miguel |last5=Wang |first5=Cheng |last6=Chen |first6=Timothy Bo Yuan |last7=Zhang |first7=Jin |last8=Chan |first8=Qing Nian |last9=Yeoh |first9=Guan Heng |date=January 2021 |title=A Review on Lithium-Ion Battery Separators towards Enhanced Safety Performances and Modelling Approaches |journal=Molecules |language=en |volume=26 |issue=2 |pages=478 |doi=10.3390/molecules26020478 |issn=1420-3049 |pmc=7831081 |pmid=33477513 |doi-access=free}}</ref> The electrodes are
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".
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Other salts like [[lithium perchlorate]] ({{chem|LiClO|4}}), [[lithium tetrafluoroborate]] ({{chem|LiBF|4}}), and [[lithium bis(trifluoromethanesulfonyl)imide]] ({{chem|LiC|2|F|6|NO|4|S|2}}) are frequently used in research in tab-less [[Button cell|coin cells]], but are not usable in larger format cells,<ref>{{cite journal |last1=Xu |first1=Kang |title=Nonaqueous Liquid Electrolytes for Lithium-Based Rechargeable Batteries |journal=Chemical Reviews |date=1 October 2004 |volume=104 |issue=10 |pages=4303–4418 |doi=10.1021/cr030203g|pmid=15669157 }}</ref> often because they are not compatible with the aluminum current collector. Copper (with a [[Spot welding|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.<ref name="Zhu-2020">{{Cite web|url=https://www.researchgate.net/publication/346987573|title=
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 [[Nanoarchitectures for lithium-ion batteries|novel architectures]] using [[nanotechnology]] to improve performance. Areas of interest include nano-scale electrode materials and alternative electrode structures.<ref>{{Cite journal |last1=Joyce |first1=C. |last2=Trahy |first2=L. |last3=Bauer |first3=S.| last4=Dogan |first4=F. |last5=Vaughey |first5=J. |doi=10.1149/2.107206jes |title=Metallic Copper Binders for Lithium-Ion Battery Silicon Electrodes| journal=Journal of the Electrochemical Society| volume=159 |issue=6 |pages=909–914| year=2012|doi-access=free }}</ref>
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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 (chemistry)|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.<ref>{{cite journal| last1=Zhai| first1=C| display-authors=etal| title=Interfacial electro-mechanical behaviour at rough surfaces| journal=Extreme Mechanics Letters| year=2016| volume=9| pages=422–429| doi=10.1016/j.eml.2016.03.021| bibcode=2016ExML....9..422Z| hdl=1959.4/unsworks_60452| url=https://hal.archives-ouvertes.fr/hal-02307660/file/Interfacial%20electromechanical%20EML%20authors%20version.pdf| access-date=31 August 2020| archive-date=19 April 2021| archive-url=https://web.archive.org/web/20210419021929/https://hal.archives-ouvertes.fr/hal-02307660/file/Interfacial%20electromechanical%20EML%20authors%20version.pdf| url-status=live}}</ref>
The charging procedures for single Li-ion cells, and complete Li-ion batteries, are slightly different:
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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.<ref name=":1" />
====
[[LiCoO2|LiCoO<sub>2</sub>]] was used in the first commercial lithium-ion battery made by Sony in 1991. The layered oxides have a pseudo-[[Tetrahedron|tetrahedral]] structure comprising layers made of MO<sub>6</sub> [[Octahedron|octahedra]] separated by interlayer spaces that allow for two-dimensional lithium-ion [[diffusion]].{{Citation needed|date=January 2024}} The [[Electronic band structure|band structure]] of Li<sub>x</sub>CoO<sub>2</sub> allows for true [[Electrical resistivity and conductivity|electronic]] (rather than [[polaron]]ic) conductivity. However, due to an overlap between the Co<sup>4+</sup> t<sub>2g</sub> d-band with the O<sup>2-</sup> 2p-band, the x must be >0.5, otherwise O<sub>2</sub> evolution occurs. This limits the charge capacity of this material to ~140 mA h g<sup>−1</sup>.<ref name=":1">{{Cite journal |last=Manthiram |first=Arumugam |date=2020-03-25 |title=A reflection on lithium-ion battery cathode chemistry |journal=Nature Communications |language=en |volume=11 |issue=1 |page=1550 |doi=10.1038/s41467-020-15355-0 |issn=2041-1723 |pmc=7096394 |pmid=32214093|bibcode=2020NatCo..11.1550M }}</ref>
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https://onlinelibrary.wiley.com/doi/10.1002/9783527629022.ch4 {{Webarchive|url=https://web.archive.org/web/20231005154711/https://onlinelibrary.wiley.com/doi/10.1002/9783527629022.ch4 |date=5 October 2023 }}</ref>
Similarly, LiCrO<sub>2</sub> shows reversible lithium (de)intercalation around 3.2
1703415</ref> LiTiO<sub>2</sub> shows Li+ (de)intercalation at a voltage of ~1.5 V, which is too low for a cathode material.
These problems leave {{chem|LiCoO|2}} and {{chem|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.<ref name="ReferenceB">{{cite journal|last1=Nitta|first1=Naoki|last2=Wu|first2=Feixiang|last3=Lee|first3=Jung Tae|last4=Yushin|first4=Gleb|author4-link=Gleb Yushin| title = Li-ion battery materials: present and future|journal=Materials Today | date = 2015|volume=18|issue=5 | doi = 10.1016/j.mattod.2014.10.040|pages=252–264|doi-access=free}}</ref> For this reason, the current trend among lithium-ion battery manufacturers is to switch to cathodes with higher Ni content and lower Co content.<ref>{{cite journal|last1=Fergus|first1=Jeffrey | title = Recent developments in cathode materials for lithium ion batteries|journal=Journal of Power Sources | date = 2010|volume=195|issue=4 | doi = 10.1016/j.jpowsour.2009.08.089|pages=939–954|bibcode=2010JPS...195..939F}}</ref>
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 [[Lithium nickel manganese cobalt oxides|NCM]] and nickel-cobalt-aluminium oxides [[Lithium nickel cobalt aluminium oxides|NCA]]), Ni cycles between the oxidation states +2 and +4 (in one step between +3.5 and +4.3 V),<ref>Ohzuku, T., Ueda, A. & Nagayama, M. Electrochemistry and structural chemistry of {{chem2|LiNiO2}} (R3m) for 4 volt secondary lithium cells. J. Electrochem. Soc. 140, 1862–1870 (1993).</ref><ref name=":1" /> cobalt- between +2 and +3, while Mn (usually >20%) and Al (typically, only 5% is needed)<ref>W. Li, E.M. Erickson, A. Manthiram, Nat. Energy 5 (2020) 26–34</ref> remain in +4 and 3+, respectively. Thus increasing the Ni content increases the cyclable charge. For example, NCM111 shows 160
It is worth mentioning so-called "lithium-rich" cathodes, that can be produced from traditional NCM ({{chem2|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.<ref>{{cite journal|last1=Xies|first1=Ying | title = Li-rich layered oxides: Structure, capacity and voltage fading mechanisms and solving strategies|journal=Particuology | date = 2022|volume=61|issue=4 |doi = 10.1016/j.partic.2021.05.011|pages=1–10|s2cid=237933219 |doi-access=free}}</ref>
====
[[Lithium ion manganese oxide battery|
An important improvement of Mn spinel are related cubic structures of the
lithium with LiV2O4. Mater. Res. Bull. 20, 1409–1420 (1985)</ref>
====
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.<ref>Gopalakrishnan, J. & Manthiram, A. Topochemically controlled hydrogen reduction of scheelite-related rare-earth metal molybdates. Dalton Trans. 3, 668–672 (1981) due to the [[inductive effect]]</ref> 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-[[conductive agent|conducting carbon]] to overcome its low electrical conductivity.<ref>{{cite journal|last1=Eftekhari|first1=Ali | title = LiFePO<sub>4</sub>/C Nanocomposites for Lithium-Ion Batteries|journal=Journal of Power Sources | date = 2017|volume=343 | doi = 10.1016/j.jpowsour.2017.01.080|pages=395–411|bibcode=2017JPS...343..395E}}</ref> This further reduces the [[packing density]] of these materials.
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| Graphite
| 260 Wh/kg || || [[Tesla, Inc.|Tesla]]
| style="max-width:0;" | The dominant negative electrode material used in lithium
| style="max-width:0;" | Low cost and good energy density. Graphite anodes can accommodate one lithium atom for every six carbon atoms. Charging rate is governed by the shape of the long, thin graphene sheets that constitute graphite. While charging, the lithium ions must travel to the outer edges of the graphene sheet before coming to rest (intercalating) between the sheets. The circuitous route takes so long that they encounter congestion around those edges.<ref name="nwu1404">{{cite web | url = http://electroiq.com/blog/2011/11/northwestern-researchers-advance-li-ion-battery-with-graphene-silicon-sandwich/ | title = Northwestern researchers advance Li-ion batteries with graphene-silicon sandwich {{pipe}} Solid State Technology |publisher=Electroiq.com | date = November 2011 |access-date=3 January 2019 |archive-url=https://web.archive.org/web/20180315064945/http://electroiq.com/blog/2011/11/northwestern-researchers-advance-li-ion-battery-with-graphene-silicon-sandwich/ |archive-date=15 March 2018 |url-status=dead}}<br />{{Cite journal | doi = 10.1002/aenm.201100426| title = In-Plane Vacancy-Enabled High-Power Si-Graphene Composite Electrode for Lithium-Ion Batteries| journal = Advanced Energy Materials| volume = 1| issue = 6| pages = 1079–1084| year = 2011| last1 = Zhao | first1 = X. | last2 = Hayner | first2 = C. M. | last3 = Kung | first3 = M. C. | last4 = Kung | first4 = H. H. | s2cid = 98312522| doi-access = free| bibcode = 2011AdEnM...1.1079Z}}</ref>
|-
| Lithium titanate<br />'''LTO''', Li{{sub|4}}Ti{{sub|5}}O{{sub|12}} || || || style="max-width:0;" | Toshiba, [[Altairnano]] || style="max-width:0;" | Automotive ([[Phoenix Motorcars]]), electrical grid (PJM Interconnection Regional Transmission Organization control area,<ref>{{cite press release | url = http://www.b2i.us/profiles/investor/ResLibraryView.asp?ResLibraryID=27574&GoTopage=1&BzID=546&Category=1183&a= | title = ... Acceptance of the First Grid-Scale, Battery Energy Storage System |publisher=Altair Nanotechnologies | date = 21 November 2008 |access-date=8 October 2009 |archive-date=3 August 2020 |archive-url=https://web.archive.org/web/20200803203141/http://www.b2i.us/profiles/investor/ResLibraryView.asp?ResLibraryID=27574&GoTopage=1&BzID=546&Category=1183&a= |url-status=dead }}</ref> [[United States Department of Defense]]<ref>Ozols, Marty (11 November 2009). [http://systemagicmotives.com/Altairnative%20Site/Power/Power%20Partners/The%20DOD.htm Altair Nanotechnologies Power Partner – The Military] {{Webarchive|url=https://web.archive.org/web/20110716181133/http://systemagicmotives.com/Altairnative%20Site/Power/Power%20Partners/The%20DOD.htm |date=16 July 2011 }}. Systemagicmotives (personal webpage){{Dubious | date = June 2010}}. Retrieved 11 June 2010.</ref>), bus (Proterra) || Improved output, charging time, durability (safety, operating temperature {{convert|-50|-|70|C|F}}).<ref>{{cite web | url = http://www.altairnano.com/documents/AltairnanoEDTAPresentation.pdf |archive-url=https://web.archive.org/web/20070616083647/http://www.altairnano.com/documents/AltairnanoEDTAPresentation.pdf |archive-date=16 June 2007 | title = Altair EDTA Presentation |publisher=Altairnano.com | date = 29 November 2006|author=Gotcher, Alan J. }}</ref>
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As graphite is limited to a maximum capacity of 372 mAh/g<ref name="SiOC" /> much research has been dedicated to the development of materials that exhibit higher theoretical capacities and overcoming the technical challenges that presently encumber their implementation. The extensive 2007 Review Article by Kasavajjula et al.<ref name="Journal of Power Sources">{{Cite journal|last1=Kasavajjula|first1=U.|last2=Wang|first2=C.|last3=Appleby|first3=A.J. C.. | title = Nano- and bulk-silicon-based insertion anodes for lithium-ion secondary cells|journal=Journal of Power Sources |volume=163|issue=2|pages=1003–1039 | doi = 10.1016/j.jpowsour.2006.09.084|year=2007|bibcode=2007JPS...163.1003K}}</ref>
summarizes early research on silicon-based anodes for lithium-ion secondary cells. In particular, Hong Li et al.<ref name="Solid State Ionics">{{Cite journal|last1=Li|first1=H.|last2=Huang|first2=X.|last3=Chenz|first3=L. C.|last4=Zhou|first4=G.|last5=Zhang|first5=Z. | title = The crystal structural evolution of nano-Si anode caused by lithium insertion and extraction at room temperature|journal=Solid State Ionics |volume=135|issue=1–4|pages=181–191 | doi = 10.1016/S0167-2738(00)00362-3|year=2000}}</ref> showed in 2000 that the electrochemical insertion of lithium ions in silicon [[nanoparticle]]s and silicon nanowires leads to the formation of an amorphous Li-Si alloy. The same year, Bo Gao and his doctoral advisor, Professor Otto Zhou described the cycling of electrochemical cells with anodes comprising silicon nanowires, with a reversible capacity ranging from at least approximately 900 to 1500
doi = 10.1002/1521-4095(200106)13:11<816::AID-ADMA816>3.0.CO;2-P|year=2001|bibcode=2001AdM....13..816G }}</ref>
Diamond-like carbon coatings can increase retention capacity by 40% and cycle life by 400% for lithium based batteries.<ref>{{cite journal |last1=Zia |first1=Abdul Wasy |last2=Hussain |first2=Syed Asad |last3=Rasul |first3=Shahid |last4=Bae |first4=Dowon |last5=Pitchaimuthu |first5=Sudhagar |title=Progress in diamond-like carbon coatings for lithium-based batteries |journal=Journal of Energy Storage |date=November 2023 |volume=72 |pages=108803 |doi=10.1016/j.est.2023.108803|s2cid=261197954 |doi-access=free |bibcode=2023JEnSt..7208803Z }}</ref>
To improve the stability of the lithium anode, several approaches to installing a protective layer have been suggested.<ref name="Girishkumar-2010">{{Cite journal|last1=Girishkumar|first1=G.|last2=McCloskey|first2=B.|last3=Luntz|first3=A. C.|last4=Swanson|first4=S.|last5=Wilcke|first5=W. | date = 2 July 2010 | title = Lithium−Air Battery: Promise and Challenges|journal=The Journal of Physical Chemistry Letters|volume=1|issue=14|pages=2193–2203 | doi = 10.1021/jz1005384|issn=1948-7185}}</ref> Silicon is beginning to be looked at as an anode material because it can accommodate significantly more lithium ions, storing up to 10 times the electric charge, however this alloying between lithium and silicon results in significant volume expansion (ca. 400%),<ref name="Hayner-2012" /> which causes catastrophic failure for the cell.<ref>{{cite web | title = A Better Anode Design to Improve Lithium-Ion Batteries | url = https://www-als.lbl.gov/index.php/holding/650-a-better-anode-design-to-improve-lithium-ion-batteries-.html|website=Berkeley Lab: Lawrence Berkeley National Laboratory|url-status=dead|archive-url=https://web.archive.org/web/20160304072942/https://www-als.lbl.gov/index.php/holding/650-a-better-anode-design-to-improve-lithium-ion-batteries-.html|archive-date=4 March 2016}}</ref> Silicon has been used as an anode material but the insertion and extraction of <chem>\scriptstyle Li+</chem> can create cracks in the material. These cracks expose the Si surface to an electrolyte, causing decomposition and the formation of a solid electrolyte interphase (SEI) on the new Si surface (crumpled graphene encapsulated Si nanoparticles). This SEI will continue to grow thicker, deplete the available <chem>\scriptstyle Li+</chem>, and degrade the capacity and cycling stability of the anode.
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The absence of a case gives pouch cells the highest gravimetric energy density; however, many applications require containment<!-- compression --> to prevent expansion when their [[state of charge]] (SOC) level is high,{{sfn|Andrea|2010|p=234}} and for general structural stability. Both rigid plastic and pouch-style cells are sometimes referred to as [[Prism (geometry)|prismatic]] cells due to their rectangular shapes.<ref>{{cite web | title = Prismatic cell winder | url = https://www.youtube.com/watch?v=Zzx6LbcRidg | publisher = [[University of Michigan]] | date = 25 June 2015 | access-date = 1 February 2020 | archive-date = 17 May 2020 | archive-url = https://web.archive.org/web/20200517093341/https://www.youtube.com/watch?v=Zzx6LbcRidg&gl=US&hl=en | url-status = live }}</ref> Three basic battery types are used in 2020s-era electric vehicles: cylindrical cells (e.g., Tesla), prismatic pouch (e.g., from [[LG Corporation|LG]]), and prismatic can cells (e.g., from LG, [[Samsung]], [[Panasonic]], and others).<!-- cylindrical cells are the least expensive to manufacture, and have been made for decades; prismatic pouches and prismatic can cells require additional infrastructure in battery pack manufacture: both prismatic types have to be compressed, need to have structure in the battery pack to hold compression so they don't delaminate in charge and discharge cycles. Cylindrical cells ("jelly roll") hold compression within each cell and are much easier to manufacture. --><ref name="E-electric20200604">{{cite AV media |url=https://www.youtube.com/watch?v=WigjD2CZAJE&t=233s |title=Sandy Munro on Tesla's Battery Tech Domination |date=4 June 2020 |medium=video |publisher=E for Electric |time=3:53–5:50 |access-date=29 June 2020 |via=YouTube |people=Mark Ellis, Sandy Munro |archive-date=7 July 2022 |archive-url=https://web.archive.org/web/20220707172944/https://www.youtube.com/watch?v=WigjD2CZAJE&t=233s |url-status=live }}</ref>
[[lithium-ion flow battery|Lithium-ion flow batteries]] have been demonstrated that suspend the cathode or anode material in an aqueous or organic solution.<ref>{{Cite journal |last1=Wang |first1=Y. |last2=He |first2=P. |last3=Zhou |first3=H. |doi=10.1002/aenm.201200100 |title=Li-Redox Flow Batteries Based on Hybrid Electrolytes: At the Cross Road between Li-ion and Redox Flow Batteries |journal=Advanced Energy Materials |volume=2 |issue=7 |pages=770–779 |year=2012 |bibcode=2012AdEnM...2..770W |s2cid=96707630}}</ref><ref>{{Cite journal |date=15 August 2016 |title=A carbon-free lithium-ion solid dispersion redox couple with low viscosity for redox flow batteries |journal=Journal of Power Sources|volume=323|pages=97–106|doi=10.1016/j.jpowsour.2016.05.033|last1=Qi |first1=Zhaoxiang|last2=Koenig|first2=Gary M.|bibcode=2016JPS...323...97Q|doi-access=free}}</ref>
As of 2014, the smallest Li-ion cell was [[pin]]
Batteries may be equipped with temperature sensors, heating/cooling systems, [[voltage regulator]] circuits, [[Tap changer|voltage taps]], and charge-state monitors. These components address safety risks like overheating and [[short circuit]]ing.<ref name="Znet:inside a battery pack">{{cite news|author=Goodwins, Rupert|date=17 August 2006|title=Inside a notebook battery pack|url=
== Uses ==
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The [[open-circuit voltage]] is higher than in [[aqueous battery|aqueous batteries]] (such as [[lead–acid battery|lead–acid]], [[nickel–metal hydride battery|nickel–metal hydride]] and [[nickel–cadmium battery|nickel–cadmium]]).<ref name="J. Brodd, Chem 2004">{{harvnb|Winter|Brodd|2004|p=4258}}</ref>{{Failed verification | date = February 2018}} [[Internal resistance]] increases with both cycling and age,{{sfn|Andrea|2010|p=12}} although this depends strongly on the voltage and temperature the batteries are stored at.<ref>{{Cite journal|last1=Stroe|first1=Daniel-Ioan|last2=Swierczynski|first2=Maciej|last3=Kar|first3=Soren Knudsen|last4=Teodorescu|first4=Remus|date=2017-09-22|title=Degradation Behavior of Lithium-Ion Batteries During Calendar Ageing—The Case of the Internal Resistance Increase|url=https://ieeexplore.ieee.org/document/8048537|journal=IEEE Transactions on Industry Applications|volume=54|issue=1|pages=517–525|doi=10.1109/TIA.2017.2756026|s2cid=34944228|issn=0093-9994|access-date=10 February 2022|archive-date=26 January 2022|archive-url=https://web.archive.org/web/20220126210620/https://ieeexplore.ieee.org/document/8048537/|url-status=live}}</ref> Rising internal resistance causes the voltage at the terminals to drop under load, which reduces the maximum current draw. Eventually, increasing resistance will leave the battery in a state such that it can no longer support the normal discharge currents requested of it without unacceptable voltage drop or overheating.
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. In 2015 researchers demonstrated a small 600
Performance of manufactured batteries has improved over time. For example, from 1991 to 2005 the energy capacity per price of lithium
Overall, between 1991 and 2018, prices for all types of lithium-ion cells (in dollars per kWh) fell approximately 97%.<ref name=Ziegler(2021)>{{Cite journal |last1=Ziegler |first1=Micah S. |last2=Trancik |first2=Jessika E. |date=2021-04-21 |title=Re-examining rates of lithium-ion battery technology improvement and cost decline |journal=Energy & Environmental Science |language=en |volume=14 |issue=4 |pages=1635–1651 |doi=10.1039/D0EE02681F |s2cid=220830992 |issn=1754-5706|doi-access=free |arxiv=2007.13920 }}</ref> Over the same time period, energy density more than tripled.<ref name="Ziegler(2021)" />
Efforts to increase energy density contributed significantly to cost reduction.<ref>{{Cite journal |last1=Ziegler |first1=Micah S. |last2=Song |first2=Juhyun |last3=Trancik |first3=Jessika E. |date=2021-12-09 |title=Determinants of lithium-ion battery technology cost decline |journal=Energy & Environmental Science |language=en |volume=14 |issue=12 |pages=6074–6098 |doi=10.1039/D1EE01313K |s2cid=244514877 |issn=1754-5706|doi-access=free |hdl=1721.1/145588 |hdl-access=free }}</ref> Energy density can also be increased by improvements in the chemistry if the cell, for instance, by full or partial replacement of graphite with silicon. Silicon anodes enhanced with graphene nanotubes to eliminate the premature degradation of silicon open the door to reaching record-breaking battery energy density of up to 350
Differently sized cells with similar chemistry can also have different energy densities. The [[21700 battery|21700 cell]] has 50% more energy than the [[18650 battery|18650 cell]], and the bigger size reduces heat transfer to its surroundings.<ref name=quinn2018>{{cite journal |last1=Quinn |first1=Jason B. |last2=Waldmann |first2=Thomas |last3=Richter |first3=Karsten |last4=Kasper |first4=Michael |last5=Wohlfahrt-Mehrens |first5=Margret | title = Energy Density of Cylindrical Li-Ion Cells: A Comparison of Commercial 18650 to the 21700 Cells |journal=Journal of the Electrochemical Society | date = 19 October 2018 |volume=165 |issue=14 |pages=A3284–A3291 | doi = 10.1149/2.0281814jes |s2cid=105193083 |doi-access=free }}</ref>
=== Round-trip efficiency ===
The table below shows the result of an experimental evaluation of a "high-energy" type 3.
{| class="wikitable"
|+
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== Lifespan ==
{{See also|Electronic waste|Technology-critical element}}
The lifespan of a lithium-ion battery is typically defined as the number of full charge-discharge cycles to reach a failure threshold in terms of capacity loss or impedance rise. Manufacturers' datasheet typically uses the word "cycle life" to specify lifespan in terms of the number of cycles to reach 80% of the rated battery capacity.<ref>{{Cite web | url = https://www.ineltro.ch/media/downloads/SAAItem/45/45958/36e3e7f3-2049-4adb-a2a7-79c654d92915.pdf | title = Lithium-ion Battery DATA SHEET Battery Model : LIR18650 2600 mAh | access-date = 3 May 2019 | archive-date = 3 May 2019 | archive-url = https://web.archive.org/web/20190503022927/https://www.ineltro.ch/media/downloads/SAAItem/45/45958/36e3e7f3-2049-4adb-a2a7-79c654d92915.pdf | url-status = live }}</ref> Simply storing lithium-ion batteries in the charged state also reduces their capacity (the amount of cyclable {{chem2|Li+}}) and increases the cell resistance (primarily due to the continuous growth of the solid electrolyte interface on the [[anode]]). Calendar life is used to represent the whole life cycle of battery involving both the cycle and inactive storage operations. Battery cycle life is affected by many different stress factors including temperature, discharge current, charge current, and state of charge ranges (depth of discharge).<ref name="Cycle-life">{{Cite journal | doi = 10.1016/j.jpowsour.2010.11.134| title = Cycle-life model for graphite-LiFePO4 cells| journal = Journal of Power Sources| volume = 196| issue = 8| pages = 3942–3948| year = 2011| last1 = Wang | first1 = J.| last2 = Liu | first2 = P.| last3 = Hicks-Garner | first3 = J.| last4 = Sherman | first4 = E.| last5 = Soukiazian | first5 = S.| last6 = Verbrugge | first6 = M.| last7 = Tataria | first7 = H.| last8 = Musser | first8 = J.| last9 = Finamore | first9 = P.| bibcode = 2011JPS...196.3942W}}</ref><ref name="Saxena-2016">{{Cite journal | doi = 10.1016/j.jpowsour.2016.07.057| title = Cycle life testing and modeling of graphite/LiCoO2 cells under different state of charge ranges| journal = Journal of Power Sources| volume = 327| pages = 394–400| year = 2016| last1 = Saxena | first1 = S.| last2 = Hendricks | first2 = C.| last3 = Pecht | first3 = M.| bibcode = 2016JPS...327..394S}}</ref> Batteries are not fully charged and discharged in real applications such as smartphones, laptops and electric cars and hence defining battery life via full discharge cycles can be misleading. To avoid this confusion, researchers sometimes use cumulative discharge<ref name="Cycle-life"/> defined as the total amount of charge (Ah) delivered by the battery during its entire life or equivalent full cycles,<ref name="Saxena-2016" /> which represents the summation of the partial cycles as fractions of a full charge-discharge cycle. Battery degradation during storage is affected by temperature and battery state of charge (SOC) and a combination of full charge (100% SOC) and high temperature (usually > 50 °C) can result in a sharp capacity drop and gas generation.<ref>{{Cite journal | doi = 10.3390/en11123295| title = Derating Guidelines for Lithium-Ion Batteries| journal = Energies| volume = 11| issue = 12| page = 3295| year = 2018| last1 = Sun | first1 = Y.|last2 = Saxena | first2 = S.| last3 = Pecht | first3 = M.| doi-access = free| hdl = 1903/31442| hdl-access = free}}</ref> Multiplying the battery cumulative discharge by the rated nominal voltage gives the total energy delivered over the life of the battery. From this one can calculate the cost per kWh of the energy (including the cost of charging).
Over their lifespan batteries degrade gradually leading to reduced capacity (and, in some cases, lower operating cell voltage) due to a variety of chemical and mechanical changes to the electrodes.<ref name="ReferenceA">{{Cite journal | doi = 10.1016/j.jpowsour.2015.07.100| title = A failure modes, mechanisms, and effects analysis (FMMEA) of lithium-ion batteries| journal = Journal of Power Sources| volume = 327| pages = 113–120| year = 2016| last1 = Hendricks | first1 = C.| last2 = Williard | first2 = N.| last3 = Mathew | first3 = S.| last4 = Pecht | first4 = M.| doi-access = free}}.</ref>
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The most common degradation mechanisms in lithium-ion batteries include:<ref name=WHOKNOWS1>{{Cite journal |vauthors=Attia PM, Bills A, Planella FB, Dechent P, dos Reis G, Dubarry M, Gasper P, Gilchrist R, Greenbank S, Howey D, Liu O, Khoo E, Preger Y, Soni A, Sripad S, Stefanopoulou AG, Sulzer V |date=10 June 2022 |title=Review-"Knees" in Lithium-Ion Battery Aging Trajectories |journal=Journal of the Electrochemical Society |volume=169 |issue=6 |page=28 |doi=10.1149/1945-7111/ac6d13|arxiv=2201.02891 |bibcode=2022JElS..169f0517A |s2cid=245836782 }}.</ref>
# Reduction of the organic carbonate electrolyte at the anode, which results in the growth of Solid Electrolyte Interface (SEI), where {{chem2|Li+}} ions get irreversibly trapped, i.e. loss of lithium inventory. This shows as increased ohmic impedance and reduced Ah charge. At constant temperature, the SEI film thickness (and therefore, the SEI resistance and the loss in cyclable {{chem2|Li+}}) increases as a square root of the time spent in the charged state. The number of cycles is not a useful metric in characterizing this degradation pathway. Under high temperatures or in the presence of a mechanical damage the electrolyte reduction can proceed explosively.
# Lithium metal plating also results in the loss of lithium inventory (cyclable Ah charge), as well as internal short-circuiting and ignition of a battery. Once Li plating commences during cycling, it results in larger slopes of capacity loss per cycle and resistance increase per cycle. This degradation mechanism become more prominent during fast charging and low temperatures.
# Loss of the (negative or positive) electroactive materials due to dissolution (e.g. of {{chem2|Mn(3+)}} species), cracking, exfoliation, detachment or even simple regular volume change during cycling. It shows up as both charge and power fade (increased resistance). Both positive and negative electrode materials are subject to fracturing due to the volumetric strain of repeated (de)lithiation cycles.
# Structural degradation of cathode materials, such as {{chem2|Li+/
# Other material degradations. Negative copper current collector is particularly prone to corrosion/dissolution at low cell voltages. PVDF binder also degrades, causing the detachment of the electroactive materials, and the loss of cyclable Ah charge.
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These are shown in the figure on the right. A change from one main degradation mechanism to another appears as a knee (slope change) in the capacity vs. cycle number plot.<ref name=WHOKNOWS1/>
Most studies of lithium-ion battery aging have been done at elevated (50–60 °C) temperatures in order to complete the experiments sooner. Under these storage conditions, fully charged nickel-cobalt-aluminum and lithium-iron phosphate cells lose ca. 20% of their cyclable charge in 1–2 years. It is believed that the aforementioned anode aging is the most important degradation pathway in these cases. On the other hand, manganese-based cathodes show a (ca. 20–50%) faster degradation under these conditions, probably due to the additional mechanism of Mn ion dissolution.<ref name=Vermeer/> At 25 °C the degradation of lithium-ion batteries seems to follow the same pathway(s) as the degradation at 50 °C, but with half the speed.<ref name=Vermeer/> In other words, based on the limited extrapolated experimental data, lithium-ion batteries are expected to lose irreversibly ca. 20% of their cyclable charge in 3–5 years or 1000–2000 cycles at 25 °C.<ref name=WHOKNOWS1/> Lithium-ion batteries with titanate anodes do not suffer from SEI growth, and last longer (>5000 cycles) than graphite anodes. However, in complete cells other degradation mechanisms (i.e. the dissolution of
===Detailed degradation description===
A more detailed description of some of these mechanisms is provided below:
{{olist
Depending on the electrolyte and additives,<ref>{{Cite journal | doi = 10.1149/1945-7111/ac1e55| title = A Systematic Study of Electrolyte Additives in Single Crystal and Bimodal LiNi0.8Mn0.1 Co0.1O2/Graphite Pouch Cells| journal = Journal of the Electrochemical Society| volume = 168| issue = 9| page = 090503| year = 2021| last1 = Song | first1 = Wentao| last2 = Harlow | first2 = J.| last3 = Logan | first3 = E. | last4 = Hebecker | first4 = H.| last5 = Coon | first5 = M| last6 = Molino | first6 = L.| last7 = Johnson | first7 = M.| last8 = Dahn | first8 = J.| last9 = Metzger | first9 = M.| bibcode = 2021JElS..168i0503S| doi-access = free}}.</ref> common components of the SEI layer that forms on the anode include a mixture of lithium oxide, [[lithium fluoride]] and semicarbonates (e.g., lithium alkyl carbonates). At elevated temperatures, alkyl carbonates in the electrolyte decompose into insoluble species such as {{chem|link=Li2CO3|Li|2|CO|3}} that increases the film thickness. This increases cell impedance and reduces cycling capacity.<ref name="2014JPS...262..129W" /> Gases formed by electrolyte decomposition can increase the cell's internal pressure and are a potential safety issue in demanding environments such as mobile devices.<ref name="Voelker-2014" /> Below 25 °C, plating of metallic Lithium on the anodes and subsequent reaction with the electrolyte is leading to loss of cyclable Lithium.<ref name="2014JPS...262..129W" /> Extended storage can trigger an incremental increase in film thickness and capacity loss.<ref name="Voelker-2014" /> Charging at greater than 4.2 V can initiate Li<sup>+</sup> plating on the anode, producing irreversible capacity loss.
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Electrolyte degradation mechanisms include hydrolysis and thermal decomposition.<ref name="Voelker-2014" /> At concentrations as low as 10 ppm, water begins catalyzing a number of degradation products that can affect the electrolyte, anode and cathode.<ref name="Voelker-2014" /> {{chem|LiPF|6}} participates in an [[Chemical equilibrium|equilibrium]] reaction with LiF and {{chem|PF|5}}. Under typical conditions, the equilibrium lies far to the left. However the presence of water generates substantial LiF, an insoluble, electrically insulating product. LiF binds to the anode surface, increasing film thickness.<ref name="Voelker-2014" /> {{chem|LiPF|6}} hydrolysis yields {{chem|PF|5}}, a strong [[Lewis acid]] that reacts with electron-rich species, such as water. {{chem|PF|5}} reacts with water to form [[hydrofluoric acid]] (HF) and [[phosphorus oxyfluoride]]. Phosphorus oxyfluoride in turn reacts to form additional HF and difluorohydroxy [[phosphoric acid]]. HF converts the rigid SEI film into a fragile one. On the cathode, the carbonate solvent can then diffuse onto the cathode oxide over time, releasing heat and potentially causing thermal runaway.<ref name="Voelker-2014" /> Decomposition of electrolyte salts and interactions between the salts and solvent start at as low as 70 °C. Significant decomposition occurs at higher temperatures. At 85 °C [[transesterification]] products, such as dimethyl-2,5-dioxahexane carboxylate (DMDOHC) are formed from EC reacting with DMC.<ref name="Voelker-2014" />
Batteries generate heat when being charged or discharged, especially at high currents. Large battery packs, such as those used in electric vehicles, are generally equipped with thermal management systems that maintain a temperature between {{convert|15|C|F}} and {{convert|35|C|F}}.<ref>{{Cite journal|last1=Jaguemont|first1=Joris|last2=Van Mierlo|first2=Joeri|date=October 2020|title=A comprehensive review of future thermal management systems for battery-electrified vehicles|url=https://linkinghub.elsevier.com/retrieve/pii/S2352152X20301754|journal=Journal of Energy Storage|language=en|volume=31|pages=101551|doi=10.1016/j.est.2020.101551|bibcode=2020JEnSt..3101551J |s2cid=219934100|access-date=28 November 2021|archive-date=24 February 2022|archive-url=https://web.archive.org/web/20220224221518/https://linkinghub.elsevier.com/retrieve/pii/S2352152X20301754|url-status=live}}</ref> Pouch and cylindrical cell temperatures depend linearly on the discharge current.<ref>{{Cite journal |doi=10.1149/2.0561506jes| title=Influence of Cell Design on Temperatures and Temperature Gradients in Lithium-Ion Cells: An in Operando Study| journal=Journal of the Electrochemical Society| volume=162| issue=6| page=A921| year=2015| last1=Waldmann| first1=T.| last2=Bisle| first2=G.| last3=Hogg| first3=B.-I.| last4=Stumpp |first4=S.| last5=Danzer |first5=M. A.| last6=Kasper| first6=M.| last7=Axmann| first7=P.| last8=Wohlfahrt-Mehrens| first8=M.| doi-access=free}}.</ref> Poor internal ventilation may increase temperatures. For large batteries consisting of multiple cells, non-uniform temperatures can lead to non-uniform and accelerated degradation.<ref>{{Cite journal |last=Malabet |first=Hernando |date=2021 |title=Electrochemical and Post-Mortem Degradation Analysis of Parallel-Connected Lithium-Ion Cells with Non-Uniform Temperature Distribution |journal=Journal of the Electrochemical Society |volume=168 |issue=10 |page=100507 |doi=10.1149/1945-7111/ac2a7c |bibcode=2021JElS..168j0507G |s2cid=244186025 |doi-access=free }}</ref> In contrast, the calendar life of [[Lithium iron phosphate battery|{{chem|LiFePO|4}}]] cells is not affected by high charge states.{{sfn|Andrea|2010|p=9}}<ref>{{Cite journal| doi=10.1016/j.jpowsour.2004.08.017| title=Modeling capacity fade in lithium-ion cells| journal=Journal of Power Sources| volume=140| issue=1| pages=157–161| year=2005| last1=Liaw| first1=B. Y.| last2=Jungst| first2=R. G.| last3=Nagasubramanian| first3=G.| last4=Case| first4=H. L.| last5=Doughty| first5=D. H.| bibcode=2005JPS...140..157L}}</ref>
Positive SEI layer in lithium-ion batteries is much less understood than the negative SEI. It is believed to have a low-ionic conductivity and shows up as an increased interfacial resistance of the cathode during cycling and calendar aging.<ref name="Voelker-2014"/><ref name=Vermeer/><ref name="ReferenceA"/>
: 2Mn<sup>3+</sup> → Mn<sup>2+</sup>+ Mn<sup>4+</sup>
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Material loss of the spinel results in capacity fade. Temperatures as low as 50 °C initiate Mn<sup>2+ </sup>deposition on the anode as metallic manganese with the same effects as lithium and copper plating.<ref name="2014JPS...262..129W" /> Cycling over the theoretical max and min voltage plateaus destroys the [[crystal lattice]] via [[Jahn-Teller distortion]], which occurs when Mn<sup>4+</sup> is reduced to Mn<sup>3+</sup> during discharge.<ref name="Voelker-2014" /> Storage of a battery charged to greater than 3.6 V initiates electrolyte oxidation by the cathode and induces SEI layer formation on the cathode. As with the anode, excessive SEI formation forms an insulator resulting in capacity fade and uneven current distribution.<ref name="Voelker-2014" /> Storage at less than 2 V results in the slow degradation of {{chem|LiCoO|2}} and {{chem|LiMn|2|O|4}} cathodes, the release of oxygen and irreversible capacity loss.<ref name="Voelker-2014" />
}}
===Recommendations===
The [[IEEE]] standard 1188–1996 recommends replacing
== Safety ==
The problem of lithium-ion battery safety has been recognized even before these batteries were first commercially released in 1991. The two main reasons for lithium-ion battery fires and explosions are related to processes on the negative electrode (cathode). During a normal battery charge lithium ions intercalate into graphite. However, if the charge is forced to go too fast (or at a too low temperature) lithium metal starts plating on the anode, and the resulting dendrites can penetrate the battery separator, internally short-circuit the cell, resulting in high electric current, heating and ignition. In other mechanism, an explosive reaction between the charge anode material (
Nowadays, all reputable manufacturers employ at least two safety devices in all their lithium-ion batteries of an 18650 format or larger: a current interrupt (CID) device and a positive temperature coefficient (PTC) device. The CID comprises two metal disks, that make an electric contact with each other. When pressure inside the cell increases, the distance between the two disks increases too and they lose the electric contact with each other, thus terminating the flow of electric current through the battery. The PTC device is made of an electrically conducting polymer. When the current going through the PTC device increases, the polymer gets hot, and its electric resistance rises sharply, thus reducing the current through the battery.<ref>Safety and Quality Issues of Counterfeit Lithium-Ion Cells. 2023. ACS Energy Lett. 8/6, 2831-9. T. Joshi, S. Azam, D. Juarez-Robles, J.A. Jeevarajan. doi: 10.1021/acsenergylett.3c00724.</ref>
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If a lithium-ion battery is damaged, crushed, or is subjected to a higher electrical load without having overcharge protection, then problems may arise. External short circuit can trigger a battery explosion.<ref>{{Cite journal|last1=Chen|first1=Mingyi|last2=Liu|first2=Jiahao|last3=He|first3=Yaping|last4=Yuen|first4=Richard|last5=Wang|first5=Jian | date = October 2017 | title = Study of the fire hazards of lithium-ion batteries at different pressures|journal=Applied Thermal Engineering|volume=125|pages=1061–1074 | doi = 10.1016/j.applthermaleng.2017.06.131|bibcode=2017AppTE.125.1061C |issn=1359-4311}}</ref>
Such incidents can occur when lithium-ion batteries are not disposed of through the appropriate channels, but are thrown away with other waste. The way they are treated by recycling companies can damage them and cause fires, which in turn can lead to large-scale conflagrations. Twelve such fires were recorded in Swiss recycling facilities in 2023. <ref name=" ">
{{cite news|author=[[Pierre Cormon]]| url = https://www.entrepriseromande.ch/web/er/w/batteries-lithium-ion-un-grave-danger-pour-les-recycleurs | title = Les batteries lithium-ion, un grave danger pour les recycleurs | last1 = | first1 = | publisher = [[Fédération des Entreprises Romandes Genève]] | newspaper = Entreprise romande | date = 20 June 2024 | accessdate = 30 June 2024}}</ref>
If overheated or overcharged, Li-ion batteries may suffer [[thermal runaway]] and cell rupture.<ref name="Spotnitz:2003a">{{Cite journal | last1 = Spotnitz | first1 = R. | last2 = Franklin | first2 = J. | doi = 10.1016/S0378-7753(02)00488-3 | title = Abuse behavior of high-power, lithium-ion cells | journal = Journal of Power Sources | volume = 113 | issue = 1 | pages = 81–100 | year = 2003 | bibcode = 2003JPS...113...81S }}</ref><ref name="Finegan:2015">{{Cite journal | doi = 10.1038/ncomms7924| title = In-operando high-speed tomography of lithium-ion batteries during thermal runaway| journal = Nature Communications| volume = 6| page = 6924| year = 2015| last1 = Finegan | first1 = D. P. | last2 = Scheel | first2 = M. | last3 = Robinson | first3 = J. B. | last4 = Tjaden | first4 = B. | last5 = Hunt | first5 = I. | last6 = Mason | first6 = T. J. | last7 = Millichamp | first7 = J. | last8 = Di Michiel | first8 = M. | last9 = Offer | first9 = G. J. | last10 = Hinds | first10 = G. | last11 = Brett | first11 = D. J. L. | last12 = Shearing | first12 = P. R. | pmid=25919582 | pmc=4423228| bibcode = 2015NatCo...6.6924F }}</ref> During thermal runaway, internal degradation and [[Oxidisation|oxidization]] processes can keep cell temperatures above 500 °C, with the possibility of igniting secondary combustibles, as well as leading to leakage, explosion or fire in extreme cases.<ref>{{Cite book |last1=Loznen |first1=Steli |title=Electrical product compliance and safety engineering |last2=Bolintineanu |first2=Constantin |last3=Swart |first3=Jan |publisher=Artech House |year=2017 |isbn=978-1-63081-011-5 |location=Boston |pages=192–196}}</ref> To reduce these risks, many lithium-ion cells (and battery packs) contain fail-safe circuitry that disconnects the battery when its voltage is outside the safe range of 3–4.2 V per cell,<ref name="Gold Peak"/><ref name="WinterBrodd2004">{{harvnb|Winter|Brodd|2004|p=4259}}</ref> or when overcharged or discharged. Lithium battery packs, whether constructed by a vendor or the end-user, without effective battery management circuits are susceptible to these issues. Poorly designed or implemented battery management circuits also may cause problems; it is difficult to be certain that any particular battery management circuitry is properly implemented.
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=== Voltage limits ===
Lithium-ion cells are susceptible to stress by voltage ranges outside of safe ones between 2.5 and 3.65/4.1/4.2 or 4.
Other safety features are required{{by whom | date = July 2020}} in each cell:<ref name="Gold Peak"/>
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* Thermal interrupt (overcurrent/overcharging/environmental exposure)
These features are required because the negative electrode produces heat during use, while the positive electrode may produce oxygen. However, these additional devices occupy space inside the cells, add points of failure, and may irreversibly disable the cell when activated. Further, these features increase costs compared to [[Nickel–metal hydride battery|nickel metal hydride batteries]], which require only a hydrogen/oxygen recombination device and a back-up pressure valve.<ref name="WinterBrodd2004"/> Contaminants inside the cells can defeat these safety devices. Also, these features can not be applied to all kinds of cells, e.g., prismatic high current cells cannot be equipped with a vent or thermal interrupt. High current cells must not produce excessive heat or oxygen, lest there be a failure, possibly violent. Instead, they must be equipped with internal thermal fuses which act before the anode and cathode reach their thermal limits.<ref>{{
Replacing the [[lithium cobalt oxide]] positive electrode material in lithium-ion batteries with a lithium metal phosphate such as lithium iron phosphate (LFP) improves cycle counts, shelf life and safety, but lowers capacity. As of 2006, these safer lithium-ion batteries were mainly used in [[electric car]]s and other large-capacity battery applications, where safety is critical.<ref>{{Cite news | url=https://www.nytimes.com/2006/09/01/opinion/01cringely.html | work=The New York Times | title=Safety Last | first=Robert X. | last=Cringely | date=1 September 2006 | access-date=14 April 2010 | archive-date=4 July 2012 | archive-url=https://web.archive.org/web/20120704053530/http://www.nytimes.com/2006/09/01/opinion/01cringely.html? | url-status=live }}</ref> In 2016, an LFP-based energy storage system was chosen to be installed in [[Paiyun Lodge]] on [[Yu Shan|Mt.Jade (Yushan)]] (the highest lodge in [[Taiwan]]). As of June 2024, the system was still operating safely.<ref name="Batteries10(2024)202">{{cite journal |last1=Chung |first1=Hsien-Ching |title=The Long-Term Usage of an Off-Grid Photovoltaic System with a Lithium-Ion Battery-Based Energy Storage System on High Mountains: A Case Study in Paiyun Lodge on Mt. Jade in Taiwan |journal=Batteries |date=13 June 2024 |volume=10 |issue=6 |pages=202 |doi=10.3390/batteries10060202|doi-access=free |arxiv=2405.04225 }}</ref>
=== Recalls ===
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=== Solid waste and recycling ===
{{Main|Battery recycling}}
Li-ion battery elements including iron, copper, nickel and cobalt are considered safe for [[incinerators]] and [[landfills]].<ref>{{Cite web |last=Mitchell |first=Robert L. |date=2006-08-22 |title=Lithium ion batteries: High-tech's latest mountain of waste |url=https://www.computerworld.com/article/2482910/lithium-ion-batteries--high-tech-s-latest-mountain-of-waste.html |access-date=2022-04-22 |website=Computerworld |language=en |archive-date=22 April 2022 |archive-url=https://web.archive.org/web/20220422205547/https://www.computerworld.com/article/2482910/lithium-ion-batteries--high-tech-s-latest-mountain-of-waste.html |url-status=live }}</ref>{{Citation needed|date=October 2021}} These metals can be [[recycle]]d,<ref name="Recycling of Lithium-Ion Batteries">{{cite book|last1=Hanisch|first1=Christian|title=Handbook of Clean Energy Systems – Recycling of Lithium-Ion Batteries|last2=Diekmann|first2=Jan|last3=Stieger|first3=Alexander|last4=Haselrieder |first4=Wolfgang|last5=Kwade|first5=Arno|date=2015|publisher=John Wiley & Sons, Ltd|isbn=9781118991978 |editor1-last=Yan|editor1-first=Jinyue|edition=5 Energy Storage|pages=2865–2888|chapter=27 |doi=10.1002/9781118991978.hces221|editor2-last=Cabeza|editor2-first=Luisa F.|editor3-last=Sioshansi |editor3-first=Ramteen}}</ref><ref>{{cite web|last1=Hanisch|first1=Christian|title=Recycling of Lithium-Ion Batteries|url=http://www.lion-eng.de/images/pdf/Recycling-of-Lithium-Ion-Batteries-LionEngineering.pdf|access-date=22 July 2015|website=Presentation on Recycling of Lithium-Ion Batteries|publisher=Lion Engineering GmbH|archive-date=26 February 2017|archive-url=https://web.archive.org/web/20170226171944/http://www.lion-eng.de/images/pdf/Recycling-of-Lithium-Ion-Batteries-LionEngineering.pdf|url-status=dead}}</ref> usually by burning away the other materials,<ref name="Morris">{{cite web|last1=Morris|first1=Charles|date=27 August 2020|title=Li-Cycle recovers usable battery-grade materials from shredded Li-ion batteries|url=https://chargedevs.com/features/li-cycle-recovers-usable-battery-grade-materials-from-shredded-li-ion-batteries/|url-status=live|archive-url=https://web.archive.org/web/20200916100246/https://chargedevs.com/features/li-cycle-recovers-usable-battery-grade-materials-from-shredded-li-ion-batteries/|archive-date=16 September 2020|access-date=31 October 2020 |website=chargedevs.com|quote=thermally treat them—they're burning off plastic and electrolyte in the batteries and are not really focused on the material recovery. It's mainly the cobalt, the nickel and the copper that they can get via that method. Lithium-ion is quite a bit more complex, than lead–acid}}</ref> but mining generally remains cheaper than recycling;<ref name="Alternative Energy Resources">{{cite web|author=Kamyamkhane, Vaishnovi |title=Are lithium batteries sustainable to the environment?|url=http://www.alternative-energy-resources.net/are-lithium-ion-batteries-sustainable-to-the-environment-i.html?|url-status=dead|archive-url=https://web.archive.org/web/20110917012206/http://www.alternative-energy-resources.net/are-lithium-ion-batteries-sustainable-to-the-environment-i.html|archive-date=17 September 2011|access-date=3 June 2013 |publisher=Alternative Energy Resources}}</ref> recycling may cost $3/kg,<ref>{{cite web|date=27–28 August 2019|title=R&D Insights for Extreme Fast Charging of Medium- and Heavy-Duty Vehicles|url=https://afdc.energy.gov/files/u/publication/extreme_fast_charging.pdf|publisher=[[NREL]]|page=6|quote=Some participants paid $3/kg to recycle batteries at end of life|access-date=23 October 2020|archive-date=18 October 2020|archive-url=https://web.archive.org/web/20201018040107/https://afdc.energy.gov/files/u/publication/extreme_fast_charging.pdf|url-status=live}}</ref> and in 2019 less than 5% of lithium
Accumulation of battery waste presents technical challenges and health hazards.<ref name="Jacoby-2019-1">{{Cite news|last=Jacoby|first=Mitch|date=July 14, 2019|title=It's time to get serious about recycling lithium-ion batteries|work=Chemical & Engineering News|url=https://cen.acs.org/materials/energy-storage/time-serious-recycling-lithium/97/i28|quote=The enormousness of the impending spent-battery situation is driving researchers to search for cost-effective, environmentally sustainable strategies for dealing with the vast stockpile of Li-ion batteries looming on the horizon.; Cobalt, nickel, manganese, and other metals found in batteries can readily leak from the casing of buried batteries and contaminate soil and groundwater, threatening ecosystems and human health...The same is true of the solution of lithium fluoride salts (LiPF6 is common) in organic solvents that are used in a battery's electrolyte|access-date=29 October 2021|archive-date=29 October 2021|archive-url=https://web.archive.org/web/20211029214517/https://cen.acs.org/materials/energy-storage/time-serious-recycling-lithium/97/i28|url-status=live}}</ref> Since the environmental impact of electric cars is heavily affected by the production of lithium-ion batteries, the development of efficient ways to repurpose waste is crucial.<ref name="Jacoby-2019" /> Recycling is a multi-step process, starting with the storage of batteries before disposal, followed by manual testing, disassembling, and finally the chemical separation of battery components. Re-use of the battery is preferred over complete recycling as there is less [[embodied energy]] in the process. As these batteries are a lot more reactive than classical vehicle waste like tire rubber, there are significant risks to stockpiling used batteries.<ref>{{Cite journal |date=2012 |title=A General Discussion of Li Ion Battery Safety |journal=Electrochemical Society Interface |doi=10.1149/2.f03122if |bibcode=2012ECSIn..21b..37D |issn=1944-8783 |last1=Doughty|first1=Daniel H.|last2=Roth|first2=E. Peter|volume=21|issue=2|page=37}}</ref>
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=== Human rights impact ===
Extraction of raw materials for lithium
Cobalt sourced from the Democratic Republic of the Congo is often mined by workers using hand tools with few safety precautions, resulting in frequent injuries and deaths.<ref>{{Cite news|last1=Mucha|first1=Lena|last2=Sadof|first2=Karly Domb|last3=Frankel|first3=Todd C.|date=2018-02-28|title=Perspective - The hidden costs of cobalt mining|language=en-US|newspaper=The Washington Post|url=https://www.washingtonpost.com/news/in-sight/wp/2018/02/28/the-cost-of-cobalt/|access-date=2018-03-07|issn=0190-8286|archive-date=10 April 2019|archive-url=https://web.archive.org/web/20190410171546/https://www.washingtonpost.com/news/in-sight/wp/2018/02/28/the-cost-of-cobalt/|url-status=live}}</ref> Pollution from these mines has exposed people to toxic chemicals that health officials believe to cause birth defects and breathing difficulties.<ref>{{cite news|author=Todd C. Frankel|date=September 30, 2016|title=THE COBALT PIPELINE: Tracing the path from deadly hand-dug mines in Congo to consumers' phones and laptops|newspaper=The Washington Post|url=https://www.washingtonpost.com/graphics/business/batteries/congo-cobalt-mining-for-lithium-ion-battery/|access-date=29 October 2021|archive-date=17 April 2019|archive-url=https://web.archive.org/web/20190417134443/https://www.washingtonpost.com/graphics/business/batteries/congo-cobalt-mining-for-lithium-ion-battery/|url-status=live}}</ref> Human rights activists have alleged, and [[investigative journalism]] reported confirmation,<ref>Crawford, Alex. [http://news.sky.com/story/meet-dorsen-8-who-mines-cobalt-to-make-your-smartphone-work-10784120 Meet Dorsen, 8, who mines cobalt to make your smartphone work] {{Webarchive|url=https://web.archive.org/web/20180907130830/https://news.sky.com/story/meet-dorsen-8-who-mines-cobalt-to-make-your-smartphone-work-10784120 |date=7 September 2018 }}. ''Sky News UK''. Retrieved on 2018-01-07.</ref><ref>[http://news.sky.com/video/are-you-holding-a-product-of-child-labour-right-now-10785338 Are you holding a product of child labour right now? (Video)] {{Webarchive|url=https://web.archive.org/web/20180701194026/https://news.sky.com/video/are-you-holding-a-product-of-child-labour-right-now-10785338 |date=1 July 2018 }}. ''Sky News UK'' (2017-02-28). Retrieved on 2018-01-07.</ref> that [[child labor]] is used in these mines.<ref name="wpDRC1">{{cite news|last1=Frankel|first1=Todd C.|date=2016-09-30|title=Cobalt mining for lithium ion batteries has a high human cost|url=https://www.washingtonpost.com/graphics/business/batteries/congo-cobalt-mining-for-lithium-ion-battery/|access-date=2016-10-18|newspaper=[[The Washington Post]]|archive-date=17 April 2019|archive-url=https://web.archive.org/web/20190417134443/https://www.washingtonpost.com/graphics/business/batteries/congo-cobalt-mining-for-lithium-ion-battery/|url-status=live}}</ref>
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