Témbongkeun sumber pikeun Litium

<!--{{Infobox litium}}-->[[Gambar:Wie funktioniert eine Lithium-Schwefel-Batterie?.webm|jmpl|Litium]]
'''Litium''' nyaéta [[unsur kimia]] nu lambangna '''Li''' sarta boga [[nomer atom]] 3, [[logam alkali]] lemes nu kelirna bodas pérak. Dina [[hawa jeung tekenan baku|kaayaan baku]], ieu unsur téh minangka [[logam]] panghampangna sarta unsur padet anu dénsitasna handap pisan. Sakumaha galibna logam alkali, litium téh réaktif pisan, gancang [[tai hiang]]an dina udara lembab. Ku kituna, litium diteundeunna sok dibulen ku [[minyak]].

Ceuk téori, litium (utamana <sup>7</sup>Li) téh salah sahiji nu kabentuk dina kajadian ''[[Big Bang]]'', najan dina éta kajadian, litium nu kabentuk gancang udar deui. Pudar sarta prosés-prosés kabentukna litium dianggap penting dina ulikan [[astronomi]]. Litium téh unsur ka-33 panglobana di [[Marcapada]]<ref name=krebs>{{cite book | last = Krebs | first = Robert E. | year = 2006 | title = The History and Use of Our Earth's Chemical Elements : A Reference Guide | publisher = Greenwood Press | location = Westport, Conn. | isbn = 0-313-33438-2 | pages = 47-50}}</ref>, ngan ku sabab [[réaktivitas|réaktif pisan]], di alam ieu unsur ukur aya dina bentuk [[sanyawa kimia|sanyawaan]]. Litium aya dina sababaraha [[mineral]] [[pegmatit]], tapi ogé biasa diala tina [[taneuh liat]]; dina skala komérsil, logam litium diala tina [[éléktrolisis]] campuran [[litium klorida]] jeung [[kalium klorida]].

Litium aya di [[sagara]] jeung sababaraha [[organismeu]] dina jumlah renik. Litium teu boga pancen biologis dina awak manusa, pangaruh ion litium (Li<sup>+</sup>) kana saraf dimangpaatkeun pikeun ngastabilkeun ''mood''. Litium jeung sanyawaanana dipaké pikeun rupa-rupa pangabutuh, di antarana [[gelas]] jeung [[keramik]] tahan panas, [[alloy]] liat-hampang pikeun [[wahana wiyati]], jeung [[batré litium]]. Litium  ogé penting dina dunya [[fisika inti]]: [[fisi inti]] atom litium mangrupa [[réaksi inti]] munggaran jieunan manusa, sedengkeun [[litium deuterida]] dipaké [[suluh]] dina [[fusi inti|fusi]] [[rarancang Teller-Ulam|pakarang térmonuklir]].

== Sajarah jeung étimologi ==
[[Petalit]] (silikat litium aluminum) munggaran didadarkeun taun [[1800]] ku élmuwan Brazil [[José Bonifácio de Andrade e Silva]], nu manggihan éta mineral di hiji tempat [[nambang beusi]] di pulo [[Utö, Swédia|Utö]], [[Swédia]]. Unsur litiumna sorangan kakara [[papanggihan unsur kimia|kapanggih]] taun [[1817]] ku [[Johan August Arfwedson]], lajeng ku nu magang di laboratorium [[Jöns Jakob Berzelius]], nalika nalungtik bijih petalit. Ieu unsur ngabentuk sanyawaan nu sarupa jeung sanyawaan [[natrium]] jeung [[kalium]], najan karbonat jeung hidroksidana kurang [[kelarutan|gampang leyur]] sarta bisa nganétralkeun [[asam]] leuwih loba. Ku Berzelius, ieu unsur dingaranan "lithion", tina [[basa Yunani]] ''λιθoς'' (''lithos'', "batu"), pikeun ngagambarkeun kapanggihna dina mineral, béda jeung natrium jeung kalium nu kapanggihna tina jaringan [[tutuwuhan]]; ieu ngaran terus dibakukeun jadi "lithium". Arfwedson lajeng nunjukkeun yén unsur nu sarua aya ogé dina bijih mineral [[spodumen]] jeung [[lepidolit]]. Taun [[1818]], [[Christian Gmelin]] nunjukkeun yén garam litium ngahasilkeun warna beureum burahay dina seuneu, tapi boh Arfwedson atawa Gmelin gagal ngisolasi ieu unsur tina garamna.<ref name="we-hist">{{cite web |last= Winter |first= Mark J|url=http://www.webelements.com/webelements/elements/text/Li/hist.html |title=Chemistry : Periodic Table : lithium : historical information |accessmonthday=19 Ags. |accessyear=2007 | publisher=Web Elements}}</ref><ref name=eote>{{cite book | year = 2004 | title = Encyclopedia of the Elements: Technical Data - History - Processing - Applications | publisher = Wiley | isbn = 978-3527306664 | pages = 287-300}}</ref><ref>[http://www.vanderkrogt.net/elements/elem/li.html 03 Lithium]</ref>

Unsur litium kakara diisolasi taun [[1821]] ku [[William Thomas Brande]] ku cara [[éléktrolisis]] [[litium oksida]], cara nu saméméhna geus dipaké ku [[Sir Humphry Davy]] pikeun ngisolasi kalium jeung natrium<ref name=eote/><ref>[http://www.diracdelta.co.uk/science/source/t/i/timeline/source.html Timeline - DiracDelta Science & Engineering Encyclopedia] {{Webarchive|url=https://web.archive.org/web/20181012054730/http://www.diracdelta.co.uk/science/source/t/i/timeline/source.html |date=2018-10-12 }}</ref>. Brande ogé medarkeun garam-garam litium, kayaning klorida, sarta nyoba ngitung beurat atomna. Taun [[1855]], [[Robert Bunsen]] jeung Augustus Matthiessen ngahasilkeun loba pisan logam tina éléktrolisis [[litium klorida]]. Logam kalium mimiti dijieun sacara komérsil taun [[1923]] ku hiji [[Metallgesellschaft AG]] maké téhnik éléktrolisis campuran litium klorida jeung [[kalium klorida]]<ref name=we-hist/><ref>[http://www.echeat.com/essay.php?t=29195 Free Essay Analysis of the Element Lithium] {{Webarchive|url=https://web.archive.org/web/20100201162023/http://echeat.com/essay.php?t=29195 |date=2010-02-01 }}</ref>.

== Pasipatan ==
[[Gambar:LithiumPelletsUSGOV.jpg|thumb|left|Pélét litium (dibungkus ku litium hidroksida bodas)]]
Kawas [[logam alkali]] lianna, litium boga hiji [[éléktron valénsi]] nu siap leupas antukna jadi [[kation]]; dicirikeun ku [[éléktronégativitas]]na nu leutik. Hasilna, litium gampang pisan robah, réaktif pisan, sarta mibanda [[titik lééh]] jeung [[titik golak]] nu panghandapna batan logam lianna. Lemahna logam alkali dina meungkeut éléktron valénsi katébong pisan di litium, ku sabab ieu unsur téh nu [[radius atom|pangleutikna]], antukna paling éléktronégatifdina golongan alkali. Litium ogé boga [[hubungan diagonal]] jeung [[magnésium]], unsur nu mibanda radius atom jeung [[radius ionik|ionik]] anu sarupa. Duanana sarupa dina ngabentuk [[nitrida]] dina N<sub>2</sub>, [[oksida]] mun kaduruk dina O<sub>2</sub>, [[garam (kimia)|garam]] nu [[kelarutan]]ana sarua, sarta [[karbonat]] jeung [[nitrida]]na anu teu stabil mun kapanasan<ref name=kamienski>Kamienski et al. "Lithium and lithium compounds". ''Kirk-Othmer Encyclopedia of Chemical Technology''. John Wiley & Sons, Inc. Publikasi online '''2004'''. {{doi|10.1002/0471238961.1209200811011309.a01.pub2}}</ref>.<!--

Litium hipu pisan nepi ka bisa dikeureut ku péso, najan leuwih hésé batan ngeureut natrium. The fresh metal has a silvery-white color which only remains untarnished in dry air.<ref name=kamienski/> Lithium has about half the density of water, giving solid sticks of lithium metal the odd heft of a light-to-medium wood like [[pine]]. The metal floats highly in [[hydrocarbon]]s; in the laboratory, jars of lithium are typically composed of black-coated sticks held down in hydrocarbon mechanically by the jar's lid and other sticks.

Lithium is greatly heat-resistant, possessing a low [[coefficient of thermal expansion]] and the highest [[specific heat capacity]] of any solid element. Lithium has also been found to be [[superconductive]] below 400 [[microkelvin|μK]]. This finding paves the way for further study of superconductivity, as lithium's [[atomic lattice]] is the simplest of all metals.
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== Kimia ==
Dina hawa nu lembab, logam litium gampang rumeuk kabulen ku [[litium hidroksida]] (LiOH jeung LiOH·H<sub>2</sub>O), [[litium nitrida]] (Li<sub>3</sub>N), jeung  [[litium karbonat]] (Li<sub>2</sub>CO<sub>3</sub> anu hideung, hasil [[rékasi kimia|réaksi]] sékundér antara LiOH jeung [[karbon dioksida|CO<sub>2</sub>]])<ref name=kamienski/>.

Mun dideukeutkeun kana seuneu, litium mencarkeun cahya burahay semu bungur, tapi mun diduruk seuneuna bodas caang. Litium bakal hurung sarta kaduruk dina oksigén mun keuna kana cai atawa saab. Ieu unsur téh hiji-hijina logam anu bisa ngalaman réaksi jeung nitrogén dina hawa rohangan.<!--

== Isotopes ==
{{main|Isotopes of lithium}}

Naturally occurring lithium is composed of two stable [[isotope]]s <sup>6</sup>Li and <sup>7</sup>Li, the latter being the more abundant (92.5% [[natural abundance]]). Seven [[radioisotope]]s have been characterized, the most stable being <sup>8</sup>Li with a [[half-life]] of 838 [[millisecond|ms]] and <sup>9</sup>Li with a half-life of 178.3&nbsp;ms. All of the remaining [[radioactive]] isotopes have half-lives that are shorter than 8.6&nbsp;ms. The shortest-lived isotope of lithium is <sup>4</sup>Li which decays through [[proton emission]] and has a half-life of 7.58043x10<sup>-23</sup> s.

<sup>7</sup>Li is one of the [[primordial elements]] or, more properly, primordial isotopes, produced in [[Big Bang nucleosynthesis]] (a small amount of <sup>6</sup>Li is also produced in stars). Lithium isotopes fractionate substantially during a wide variety of natural processes, including mineral formation (chemical precipitation), [[metabolism]], and [[ion exchange]]. Lithium ion substitutes for [[magnesium]] and [[iron]] in octahedral sites in [[clay]] minerals, where <sup>6</sup>Li is preferred to <sup>7</sup>Li, resulting in enrichment of the light isotope in processes of hyperfiltration and rock alteration.

The exotic <sup>11</sup>Li is known to exhibit a [[nuclear halo]].

== Natural occurrence ==
''See also [[:category:Lithium minerals|Lithium minerals]].''

Lithium is widely distributed on Earth and is the 33rd most abundant element;<ref name=krebs/> however, it does not naturally occur in elemental form due to its high reactivity. Estimates for [[crust (geology)|crustal]] content range from 20 to 70 ppm by weight.<ref name=kamienski/> In keeping with its name, lithium forms a minor part of [[igneous]] rocks, with the largest concentrations in [[granite]]s. Granitic [[pegmatite]]s also provide the greatest abundance of lithium-containing minerals, with [[spodumene]] and [[petalite]] being the most commercially-viable mineral sources for the element.<ref name=kamienski/>

== Applications ==
Because of its [[specific heat]] capacity, the highest of all [[solid]]s, lithium is often used in heat transfer applications.

It is an important ingredient in [[cathode]] materials, used in rechargeable and single-use [[Lithium battery|batteries]] because of its high [[electrochemical potential]], light weight, and high current density.

Large quantities of lithium are also used in the manufacture of [[organolithium reagent]]s, especially [[n-butyllithium|''n''-butyllithium]] which has many uses in fine chemical and [[polymer]] synthesis.

=== Medical use ===
{{main|Lithium pharmacology}}

Lithium salts were used during the 19th century to treat [[gout]].  Lithium salts such as [[lithium carbonate]] (Li<sub>2</sub>CO<sub>3</sub>), [[lithium citrate]], and [[lithium orotate]] are mood stabilizers. They are used in the treatment of [[bipolar disorder]], since unlike most other mood altering drugs, they counteract both [[mania]] and [[depression (mood)|depression]]. Lithium can also be used to augment other [[antidepressant]] drugs. It is also sometimes prescribed as a preventive treatment for [[migraine]] disease and [[cluster headache]]s.

The active principle in these salts is the lithium ion Li<sup>+</sup>, which having a smaller diameter, can easily displace K<sup>+</sup> and Na<sup>+</sup> and even Ca<sup>+2</sup>, in spite of its greater charge, occupying their sites in several critical neuronal enzymes and neurotransmitter receptors. Although Li<sup>+</sup> cannot displace Mg<sup>2+</sup> and Zn<sup>2+</sup>, because of these ions small size and greater charge (higher charge density, hence stronger bonding), when Mg<sup>+2</sup> or Zn<sup>+2</sup> are present in low concentrations, and Li<sup>+</sup> is present in high concentrations, the latter can occupy sites normally occupied by Mg<sup>+2</sup> or Zn<sup>+2</sup> in various enzymes. Therapeutically useful amounts of lithium (0.6 to 1.2 mmol/l) are only slightly lower than toxic amounts (>1.5 mmol/l), so the blood levels of lithium must be carefully monitored during treatment to avoid toxicity. Therefore, in theory, coadministration of 400 IU vitamin D, 1 g magnesium citrate (not the insoluble oxide or carbonate), 15 mg Zn (as gluconate or piccolinate, not the insoluble oxide) and 1 pill of [[vitamin B]] complex a day, should potentiate the effect of Li, {{Fact|date=December 2007}} in some cases allowing for the reduction of the therapeutic range to 0.5 to 0.9 mmol/l, of the daily dose of lithium carbonate and of the risk of toxicity.

Common side effects include muscle tremors, twitching, [[ataxia]], hyperparathyroidism (bone loss, hypercalcemia, hypertension, etc,), kidney damage, [[nephrogenic diabetes insipidus]] (polyuria and polydipsia) and seizures. Many of the side-effects are a result caused by the increased elimination of potassium.

=== Other uses ===
* [[Lithium chloride]] and [[lithium bromide]] are extremely [[hygroscopic]] and frequently used as [[desiccant]]s.
* [[stearic acid|Lithium stearate]] is a common all-purpose high-temperature [[lubricant]].
* Lithium is an [[alloy]]ing agent used to synthesize [[organic compound]]s.
* Lithium is used as a [[flux (metallurgy)|flux]] to promote the fusing of metals during [[welding]] and [[soldering]]. It also eliminates the forming of oxides during welding by absorbing impurities. This fusing quality is also important as a flux for producing [[ceramic]]s, [[Vitreous enamel|enamels]], and [[glass]].
* Lithium is sometimes used in glasses and ceramics including the glass for the 200-inch (5.08&nbsp;m) [[telescope]] at [[Mt. Palomar]].
* [[Alloy]]s of the metal with [[aluminium]], [[cadmium]], [[copper]], and [[manganese]] are used to make high performance [[aircraft]] parts.
* [[Lithium niobate]] is used extensively in telecommunication products, such as [[mobile phone]]s and [[optical modulator]]s, for such components as resonant crystals. Lithium products are currently used in more than 60 percent of mobile phones.<ref>{{cite news |author=Spring, Martin |title=Two ways to play the lithium boom |url=http://www.moneyweek.com/file/32991/two-ways-to-play-the-lithium-boom.html |publisher=[[MoneyWeek]] |date=2007-01-08 |accessdate=2007-08-19}}</ref>
* The high non-linearity of lithium niobate also makes a good choice for [[nonlinear optics|non-linear optics applications]].
* [[Lithium deuteride]] was the [[nuclear fusion|fusion fuel]] of choice in early versions of the [[Nuclear weapon|hydrogen bomb]]. When bombarded by [[neutron]]s, both <sup>6</sup>Li and <sup>7</sup>Li produce [[tritium]]—this reaction, which was not fully understood when hydrogen bombs were first tested, was responsible for the runaway yield of the [[Castle Bravo]] nuclear test. Tritium fuses with [[deuterium]] in a [[Nuclear fusion|fusion]] reaction that is relatively easy to achieve. Although details remain secret, lithium-6 deuteride still apparently plays a role in modern [[nuclear weapons]], as a fusion material.
* Metallic lithium and its complex [[hydride]]s such as e.g. Li[AlH<sub>4</sub>] are considered as high energy additives to [[rocket propellant]]s<sup>[3]</sup>. 
* [[Lithium peroxide]], [[lithium nitrate]], lithium chlorate and [[lithium perchlorate]] are used and thought of as oxidizers in both rocket propellants and [[oxygen candle]]s to supply submarines and space capsules with oxygen.<ref>{{cite journal | author = K. Ernst-Christian | title = Special Materials in Pyrotechnics: III. Application of Lithium and its Compounds in Energetic Systems | year = 2004 | journal = [[Propellants, Explosives, Pyrotechnics]] | volume = 29 | issue = 2 | pages = 67-80 | doi = 10.1002/prep.200400032}}</ref> 
* Lithium will be used to produce tritium in magnetically confined nuclear fusion reactors using deuterium and tritium as the fuel. Tritium does not occur naturally and will be produced by surrounding the reacting plasma with a 'blanket' containing lithium where neutrons from the deuterium-tritium reaction in the plasma will react with the lithium to produce more tritium. <sup>6</sup>Li + n → <sup>4</sup>He + <sup>3</sup>H. Various means of doing this will be tested at the [[ITER]] reactor being built at Cadarache, France.
* Lithium is used as a source for [[alpha particle]]s, or [[helium]] nuclei. When <sup>7</sup>Li is bombarded by accelerated [[proton]]s, <sup>8</sup>[[beryllium|Be]] is formed, which undergoes spontaneous fission to form two alpha particles. This was the first man-made [[nuclear reaction]], produced by Cockroft and Walton in [[1929]].
* [[Lithium hydroxide]] (LiOH) is an important compound of lithium obtained from lithium carbonate (Li<sub>2</sub>CO<sub>3</sub>). It is a strong base, and when heated with a fat, it produces a lithium soap. Lithium soap has the ability to thicken oils and so is used commercially to manufacture lubricating greases. 
* It is also an efficient and lightweight purifier of air. In confined areas, such as aboard [[spacecraft]] and [[submarine]]s, the concentration of carbon dioxide can approach unhealthy or toxic levels. Lithium hydroxide absorbs the carbon dioxide from the air by reacting with it to form lithium carbonate. Any alkali hydroxide will absorb CO<sub>2</sub>, but lithium hydroxide is preferred, especially in spacecraft applications, because of the low formula weight conferred by the lithium. Even better materials for this purpose include lithium peroxide (Li<sub>2</sub>O<sub>2</sub>) that, in presence of moisture, not only absorb carbon dioxide to form lithium carbonate, but also release oxygen. E.g. 2 Li<sub>2</sub>O<sub>2</sub> + 2 CO<sub>2</sub> → 2 Li<sub>2</sub>CO<sub>3</sub> + O<sub>2</sub>.
* Lithium metal is used as a [[reducing agent]] in some types of [[methamphetamine]] production, particularly in illegal amateur “meth labs.”

== Production ==
Since the end of [[World War II]], lithium metal production has greatly increased. The metal is separated from other elements in igneous mineral such as those above, and is also extracted from the water of [[mineral springs]].

The metal is produced [[electrolysis|electrolytically]] from a mixture of fused lithium and [[potassium chloride]]. In [[1998]] it was about [[US dollar|US$]] 43 per [[Pound (mass)|pound]] ($95 per [[kilogram|kg]]).<ref name=ober>{{cite web |url=http://minerals.usgs.gov/minerals/pubs/commodity/lithium/450798.pdf |title=Lithium |accessmonthday=August 19 |accessyear=2007 |last=Ober |first=Joyce A |format=pdf |pages = 77-78| publisher=[[United States Geological Survey]]}}</ref>

[[Chile]] is currently the leading lithium metal producer in the world, with [[Argentina]] next. Both countries recover the lithium from brine pools. In the [[United States]] lithium is similarly recovered from brine pools in [[Nevada]].<ref name=lanl>{{cite web |url=http://periodic.lanl.gov/elements/3.html |title=Lithium |accessmonthday= August 19 |accessyear= 2007|date= December 15, 2003|publisher= [[Los Alamos National Laboratory]]}}</ref>

China may emerge as a significant producer of brine-based lithium carbonate towards the end of this decade. Potential capacity of up to 45,000 tonnes per year could come on-stream if projects in Qinghai province and Tibet proceed.{{Fact|date=August 2007}}

== Precautions ==
Lithium metal, due to its alkaline tarnish, is corrosive and requires special handling to avoid skin contact. Breathing lithium dust or lithium compounds (which are often alkaline) can irritate the nose and throat; higher exposure to lithium can cause a build-up of fluid in the lungs, leading to [[pulmonary edema]]. The metal itself is usually a handling hazard because of the caustic hydroxide produced when it is in contact with moisture causing an explosion. Lithium should be stored in a non-reactive compound such as [[naphtha]] or a hydrocarbon.

=== Regulation ===
Some jurisdictions limit the sale of [[lithium battery|lithium batteries]], which are the most readily available source of lithium metal for ordinary consumers. Lithium can be used to reduce pseudoephedrine and ephedrine to [[methamphetamine]] in the [[Birch reduction]] method, which employs solutions of alkali metals dissolved in anhydrous ammonia. However, the effectiveness of such restrictions in controlling illegal production of methamphetamine remains indeterminate and controversial.

Carriage and shipment of some kinds of lithium batteries may be prohibited aboard certain types of transportation (particularly aircraft), because of the ability of most types of lithium batteries to fully discharge very rapidly when [[short circuit|short-circuited]], leading to overheating and possible [[explosion]]. However, most consumer lithium batteries have thermal overload protection built-in to prevent this type of incident, or their design inherently limits short-circuit currents.
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== Rujukan ==
<references />

== Tumbu kaluar ==
{{Commons|Lithium}}
* [http://minerals.usgs.gov/minerals/pubs/commodity/lithium/ USGS: Lithium Statistics and Information]
* [http://www.webelements.com/webelements/elements/text/Li/index.html WebElements.com – Lithium]
* [http://education.jlab.org/itselemental/ele003.html It's Elemental – Lithium]
* [http://www.state.nj.us/health/eoh/rtkweb/1119.pdf Safety information on Lithium]
* [http://www.bipolar-lives.com/lithium.html Information on Lithium and Bipolar Disorder]
* [http://www.mcis.soton.ac.uk/Site_Files/pdf/nuclear_history/Working_Paper_No_5.pdf University of Southampton, Mountbatten Centre for International Studies, Nuclear History Working Paper No5.]

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