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リチウム

リチウム 化学構造式
7439-93-2
CAS番号.
7439-93-2
化学名:
リチウム
别名:
リチウム;金属リチウム;リチウム(ワイヤー);リチウム(塊状);リチウムディスパージョン;金属「リチウム」;リチウム(粒状);リチウム (棒) 10Φ×30MM;リチウム(棒状);リチウム、粒状;リチウム granules (99+%);リチウム ribbon (99.8%);リチウム rod (99.8%)
英語化学名:
Lithium
英語别名:
Li;Litium;LITHIUM;LITHIUM;LI000260;LI000205;LI000220;rolledfoil;lithium(1+);Lithium rod
CBNumber:
CB9495849
化学式:
Li
分子量:
6.94
MOL File:
7439-93-2.mol

リチウム 物理性質

融点 :
180 °C(lit.)
沸点 :
1342 °C(lit.)
比重(密度) :
0.534 g/mL at 25 °C(lit.)
蒸気圧:
1 hPa (723 °C)
貯蔵温度 :
water-free area
外見 :
wire
比重:
0.534
色:
Silvery
電気抵抗率 (resistivity):
9.446 μΩ-cm, 20°C
水溶解度 :
REACTS
Sensitive :
air sensitive, moisture sensitive
Merck :
13,5542
安定性::
Stability Stable, but reacts violently with water. Store under oil.
CAS データベース:
7439-93-2(CAS DataBase Reference)
NISTの化学物質情報:
Lithium(7439-93-2)
EPAの化学物質情報:
Lithium(7439-93-2)
安全性情報
  • リスクと安全性に関する声明
  • 危険有害性情報のコード(GHS)
主な危険性  Xi,C,F
Rフレーズ  36/38-34-14/15-23
Sフレーズ  8-43-45-43C-36/37/39-26
RIDADR  UN 3264 8/PG 3
WGK Germany  2
RTECS 番号 OJ5540000
10
TSCA  Yes
HSコード  2805 19 90
国連危険物分類  4.3
容器等級  I
有毒物質データの 7439-93-2(Hazardous Substances Data)
消防法 危険物第3類
絵表示(GHS)
注意喚起語 Danger
危険有害性情報
コード 危険有害性情報 危険有害性クラス 区分 注意喚起語 シンボル P コード
H260 水に触れると自然発火するおそれのある可燃性 /引火性ガスを発生 水反応可燃性化学品 1 危険 P223, P231+P232, P280, P335+ P334,P370+P378, P402+P404, P501
H314 重篤な皮膚の薬傷?眼の損傷 皮膚腐食性/刺激性 1A, B, C 危険 P260,P264, P280, P301+P330+ P331,P303+P361+P353, P363, P304+P340,P310, P321, P305+ P351+P338, P405,P501
注意書き
P223 激しい反応と火災の発生の危険があるため、水と接 触させないこと。
P231+P232 湿気を遮断し、不活性ガス下で取り扱うこと。
P260 粉じん/煙/ガス/ミスト/蒸気/スプレーを吸入しないこ と。
P280 保護手袋/保護衣/保護眼鏡/保護面を着用するこ と。
P303+P361+P353 皮膚(または髪)に付着した場合:直ちに汚染された衣 類をすべて脱ぐこと/取り除くこと。皮膚を流水/シャワー で洗うこと。
P305+P351+P338 眼に入った場合:水で数分間注意深く洗うこと。次にコ ンタクトレンズを着用していて容易に外せる場合は外す こと。その後も洗浄を続けること。
P370+P378 火災の場合:消火に...を使用すること。
P402+P404 乾燥した場所または密閉容器に保管するこ と。
P405 施錠して保管すること。
P422 内容物を...中で保管すること。

リチウム 価格 もっと(57)

メーカー 製品番号 製品説明 CAS番号 包装 価格 更新時間 購入
富士フイルム和光純薬株式会社(wako) W01SRM03-0375
Lithium granules (99+%)
7439-93-2 50g ¥42100 2018-12-26 購入
富士フイルム和光純薬株式会社(wako) W01SRM03-0375
Lithium granules (99+%)
7439-93-2 250g ¥166300 2018-12-26 購入
関東化学株式会社(KANTO) 21144-2A リチウム(粒状)
Lithium, granular
7439-93-2 250g ¥61000 2018-12-13 購入
関東化学株式会社(KANTO) 21144-1A リチウム(粒状)
Lithium, granular
7439-93-2 25g ¥7800 2018-12-13 購入
Sigma-Aldrich Japan 220914 リチウム wire (in mineral oil), diam. 3.2?mm, 99.9% trace metals basis
Lithium wire (in mineral oil), diam. 3.2?mm, 99.9% trace metals basis
7439-93-2 25g ¥21000 2018-12-25 購入

リチウム 化学特性,用途語,生産方法

外観

銀白色~灰褐色、粒状

溶解性

水及び希塩酸に溶ける。水と激しく反応して、水素を発生し水酸化リチウムになるが、その反応性はアルカリ金属の中では最も穏やかである。

主な性質

  1. 全ての金属の中で一番軽く、水に浮く銀白色の金属(大気中では黒色の錆びを生成する)
  2. リチウムは液体で存在する温度領域が極めて広い。融点と沸点が1,200℃近くも離れている
  3. イオン化傾向が最も大きく、電気化学的に最も卑な金属である
  4. 常温での反応性には、アルカリ金属に属するにもかかわらず?窒素と反応する ?水と穏やかに反応する ?炭化物を作る ?化合物の水への溶解度はマグネシウムに類似する、など特異な性質である
  5. 溶融状態の金属リチウムは極めて活性であり、水とは爆発的に反応し、多くの金属や耐火物を激しく侵す
  6. リチウムは中性子吸収断面積が大きく、遅い中性子の放射を受けるとトリウムを発生する
  7. アルミニウムーリチウム合金は、低比重、高剛性が特徴で、高速回転や航空機材に使われる

用途

金属還元剤?合金添加?リチウム電池

効能

躁病薬

主な用途

  1. 航空機部材(Al-Li合金)
  2. ブラウン管(テレビ、パソコンモニター)
  3. 弾性表面フィルター(テレビ、携帯電話など)
  4. リチウムイオン電池正極材(2次電池)
  5. 水冷媒吸収剤(吸収式冷凍機)
  6. 溶接用フラックス(溶接棒)
  7. 除湿材(空調機)
  8. 耐熱ガラス、陶磁器うわぐすり(耐熱ガラス製品)
  9. 合成ゴム重合触媒(合成ゴム製造用)
  10. グリース(潤滑材)
  11. 電解質(リチウム?イオン電池など、1次、2次電池)

使用上の注意

不活性ガス封入

化学的特性

soft silver metal

化学的特性

Lithium is a silvery to grayish-white metal that turns yellow on exposure to air and/or moisture.

物理的性質

In the metallic state, lithium is a very soft metal with a density of 0.534 g/cm3. When asmall piece is placed on water, it will float as it reacts with the water, releasing hydrogen gas.Lithium’s melting point is 179°C, and it has about the same heat capacity as water, with aboiling point of 1,342°C. It is electropositive with an oxidation state of +1, and it is an excellent conductor of heat and electricity. Its atom is the smallest of the alkali earth metals andthus is the least reactive because its valence electron is in the K shell, which is held closest toits nuclei.

同位体

There are two stable lithium isotopes: Li-6.015, which makes up 7.5% of all lithium atoms, and Li-7.016, which makes up 92.5% of lithium atoms found in the Earth’scrust. Less prevalent isotopes of lithium are Li-4, Li-5, Li-8, Li-9, Li-10, and Li-11. Theyare unstable with short half-lives and make up only a very small fraction of Lithium’stotal averaged atomic weight.

名前の由来

The name lithium comes from the Greek word lithos, meaning “stone” because it was found in rocks on Earth.

天然物の起源

Lithium ranks 33rd among the most abundant elements found on Earth. It does not existin pure metallic form in nature because it reacts with water and air. It is always combinedwith other elements in compound forms. These lithium mineral ores make up only about0.0007%, or about 65 ppm, of the Earth’s crust.Lithium is contained in minute amounts in the mineral ores of spodumene, lepidolite, andamblygonite, which are found in the United States and several countries in Europe, Africa, andSouth America. High temperatures are required to extract lithium from its compounds and byelectrolysis of lithium chloride. It is also concentrated by solar evaporation of salt brine in lakes.Metallic lithium is produced on a commercial scale by electrolysis of molten lithium chloride (LiCl) that is heated as a mixture with potassium chloride (KCl). Both have a rather highmelting point, but when mixed, the temperature required to melt them (400°C) is severalhundred degrees lower than their individual melting points. This liquid mixture of LiCl andKCl becomes the electrolyte. The anode is graphite (carbon) and the cathode is steel. Themolten liquid positive lithium cations collect at the cathode while negative chlorine anionscollect at the anode, and the potassium chloride remains in the electrolyte. Each positive ion oflithium that collects at the cathode gains an electron, thus producing neutral atoms of moltenlithium metal, which is then further purified.

来歴

Discovered by Arfvedson in 1817. Lithium is the lightest of all metals, with a density only about half that of water. It does not occur free in nature; combined it is found in small amounts in nearly all igneous rocks and in the waters of many mineral springs. Lepidolite, spodumene, petalite, and amblygonite are the more important minerals containing it. Lithium is presently being recovered from brines of Searles Lake, in California, and from Nevada, Chile, and Argentina. Large deposits of spodumene are found in North Carolina. The metal is produced electrolytically from the fused chloride. Lithium is silvery in appearance, much like Na and K, other members of the alkali metal series. It reacts with water, but not as vigorously as sodium. Lithium imparts a beautiful crimson color to a flame, but when the metal burns strongly the flame is a dazzling white. Since World War II, the production of lithium metal and its compounds has increased greatly. Because the metal has the highest specific heat of any solid element, it has found use in heat transfer applications; however, it is corrosive and requires special handling. The metal has been used as an alloying agent, is of interest in synthesis of organic compounds, and has nuclear applications. It ranks as a leading contender as a battery anode material because it has a high electrochemical potential. Lithium is used in special glasses and ceramics. The glass for the 200-inch telescope at Mt. Palomar contains lithium as a minor ingredient. Lithium chloride is one of the most hygroscopic materials known, and it, as well as lithium bromide, is used in air conditioning and industrial drying systems. Lithium stearate is used as an all-purpose and hightemperature lubricant. Other lithium compounds are used in dry cells and storage batteries. Seven isotopes of lithium are recognized. Natural lithium contains two isotopes. The metal is priced at about $1.50/g (99.9%).

特性

While classified as an alkali metal, lithium also exhibits some properties of the alkali earthmetals found in group 2 (IIA). Lithium is the lightest in weight and softest of all the metalsand is the third lightest of all substances listed on the periodic table, with an average atomicweight of about 7. (The other two are hydrogen and helium.) Although it will float on water,it reacts with water, liberating explosive hydrogen gas and lithium hydroxide (2Li + 2H2O →2LiOH + H2?). It will also ignite when exposed to oxygen in moist air (4Li + O2 → 2Li2O).It is electropositive and thus an excellent reducing agent because it readily gives up electrons inchemical reactions. Lithium is the only metal that reacts with nitrogen at room temperature.When a small piece of the metal, which is usually stored in oil or kerosene, is cut, the newsurface has a bright, shiny, silvery surface that soon turns gray from oxidation.

使用

Lithium has many uses in today’s industrial society. It is used as a flux to promote the fusing of metals during welding and soldering. It also eliminates the formation of oxides duringwelding by absorbing impurities. This fusing quality is also important as a flux for producingceramics, enamels, and glass.A major use is as lithium stearate for lubricating greases. It makes a solid grease that canwithstand hard use and high temperatures.Lithium is used to manufacture electric storage cells (batteries) that have a long shelf lifefor use in heart pacemakers, cameras, and so forth.Some lithium compounds are used as rocket propellants, nuclear reactor coolants, alloyhardeners, and deoxidizers and to make special ceramics.Lithium is a source of alpha particles when bombarded in a nuclear accelerator. The following occurs: lithium nuclei (3 protons + 4 neutrons) are targeted by high-speed protons(hydrogen nuclei), resulting in lithium absorbing a proton to form 4 protons + 4 neutrons,which become two alpha particles (helium nuclei). For example, see the following equation:1H + 3Li = 2He + 2He. This is an example of the first man-made nuclear reaction produced bySir John Cockcroft (1897–1967) and Ernest Walton (1903–1995) in 1929.Several compounds of lithium are used as pharmaceuticals to treat severe psychoticdepression (as antidepressant agents). And lithium carbonate is also used as a sedative ormild tranquilizer to treat less severe anxiety, which is a general feeling of uneasiness or distressabout present condition or future uncertainties. Lithium is also used in the production ofvitamin A.

使用

Lithium is used in making alloys, in themanufacture of lithium salts, and in vacuumtubes.

使用

In production of organometallic alkyl and aryl lithium compounds; in production of high-strength, low-density aluminum alloys for the aircraft industry; extremely tough, low-density alloys with aluminum and magnesium used for armour plate and aerospace components. In polymerization catalysts for the polyolefin plastics industry; manufacture of high-strength glass and glass-ceramics. As anode in electrochemical cells and batteries; as chemical intermediate in organic syntheses. Lithium stearate as thickener and gelling agent to transform oils into lubricating greases.

定義

A light silvery moderately reactive metal; the first member of the alkali metals (group 1 of the periodic table). It occurs in a number of complex silicates, such as spodumene, lepidolite, and petalite, and a mixed phosphate, tryphilite. It is a rare element accounting for 0.0065% of the Earth’s crust. Lithium ores are treated with concentrated sulfuric acid and lithium sulfate subsequently separated by crystallization. The element can be obtained by conversion to the chloride and electrolysis of the fused chloride or of solutions of LiCl in pyridine.
Lithium has the electronic configuration 1s22s1 and is entirely monovalent in its chemistry. The lithium ion is, however, much smaller than the ions of the other alkali metals; consequently it is polarizing and a certain degree of covalence occurs in its bonds. Lithium also has the highest ionization potential of the alkali metals.
The element reacts with hydrogen to form lithium hydride, LiH, a colorless high-melting solid, which releases hydrogen at the anode during electrolysis (confirming the ionic nature Li+H). The compound reacts with water to release hydrogen and is also frequently used as a reducing agent in organometallic synthesis. Lithium reacts with oxygen to give Li2O (sodium gives the peroxide) and with nitrogen to form Li3N on fairly gentle warming. The metal itself reacts only slowly with water, giving the hydroxide (LiOH) but lithium oxide reacts much more vigorously to give again the hydroxide; the nitride is hydrolyzed to ammonia. The metal reacts with halogens to form halides (LiX).
Apart from the fluoride the halides are readily soluble both in water and in oxygen- containing organic solvents. In this property lithium partly resembles magnesium which has a similar charge/size ratio. Compared to the other carbonates of group 1, lithium carbonate is thermally unstable decomposing to Li2O and CO2. This is because the small Li+ ion leads to particularly high lattice energies favouring the formation of Li2O.
Lithium also forms a wide range of alkyl- and aryl-compounds with organic compounds, which are particularly useful in organic synthesis. Lithium compounds impart a characteristic purple color to flames. Symbol: Li; m.p. 180.54°C; b.p. 1347°C; r.d. 0.534 (20°C); p.n. 3; r.a.m. 6.941.

定義

Symbol Li. A soft silverymetal, the first member of group 1(formerly IA) of the periodic table(see alkali metals); a.n. 3; r.a.m.6.939; r.d. 0.534; m.p. 180.54°C; b.p.1347°C. It is a rare element found inspodumene (LiAlSi2O6), petalite(LiAlSi4O10), the mica lepidolite, andcertain brines. It is usually extractedby treatment with sulphuric acid togive the sulphate, which is convertedto the chloride. This is mixed with asmall amount of potassium chloride,melted, and electrolysed. The stableisotopes are lithium–6 and lithium–7.Lithium–5 and lithium–8 are shortlivedradioisotopes. The metal is usedto remove oxygen in metallurgy andas a constituent of some Al and Mgalloys. It is also used in batteries andis a potential tritium source for fusionresearch. Lithium salts are usedin psychomedicine. The element reactswith oxygen and water; on heating it also reacts with nitrogen andhydrogen. Its chemistry differs somewhatfrom that of the other group 1elements because of the small size ofthe Li+ ion.

生物学の機能

For more than 40 years, Li+ has been used to treat mania. While it is relatively inert in individuals without a mood disorder, lithium carbonate is effective in 60 to 80% of all acute manic episodes within 5 to 21 days of beginning treatment. Because of its delayed onset of action in the manic patient, Li+ is often used in conjunction with low doses of high-potency anxiolytics (e.g., lorazepam) and antipsychotics (e.g. haloperidol) to stabilize the behavior of the patient. Over time, increased therapeutic responses to Li+ allow for a gradual reduction in the amount of anxiolytic or neuroleptic required, so that eventually Li+ is the sole agent used to maintain control of the mood disturbance.
In addition to its acute actions, Li+ can reduce the frequency of manic or depressive episodes in the bipolar patient and therefore is considered a mood-stabilizing agent. Accordingly, patients with bipolar disorder are often maintained on low stabilizing doses of Li+ indefinitely as a prophylaxis to future mood disturbances. Antidepressant medications are required in addition to Li+ for the treatment of breakthrough depression.

一般的な説明

A soft silvery metal that is normally grayish white due to oxide formation. Spontaneous ignition is likely if heated to melting point.

空気と水の反応

Highly flammable. Is readily ignited by and reacts with most extinguishing agents such as water, carbon dioxide, and carbon tetrachloride [Mellor 2, Supp 2:71. 1961]. Reacts with water to form caustic Litium hydroxide and hydrogen gas (H2). Litium is spontaneously flammable in air if heated to 180°C if the surface of the metal is clean.

反応プロフィール

Burns in air, oxygen, nitrogen, hydrogen, and carbon dioxide. The reactions can become extremely violent at higher temperatures. The disposition to ignite of surfaces of molten Litium exposed to any of these gases is increased by the presence of Litium oxides and nitrides. Litium reacts avidly with water to generate gaseous hydrogen and a solution of Litium hydroxide (a caustic). Contact with halogenated hydrocarbons can produce extremely violent reactions, especially on impact [Haz. Chem. Data 1966]. Boron trifluoride reacts with incandescence when heated with Litium [Merck 11th ed. 1989]. Maleic anhydride decomposes explosively in the presence of Litium [Chemical Safety Data Sheet SD-88. 1962, Chem. Haz. Info. Series C-71. 1960]. Chlorine vapors and Litium react producing a luminous flame [Mellor 2, Supp. 1:380. 1956]. The product of the reaction between Litium and carbon monoxide, Litium carbonyl, detonates violently with water, igniting the gaseous products [Mellor 2, Supp. 2:84. 1961]. The reaction of Litium and ferrous sulfide starts around 260°C with subsequent rise in temperature to 950° C [Mellor 2, Supp. 2:80. 1961]. A truck, which was carrying Litium batteries, sodium dithionite and derivatives of cyanide, caught fire; multiple explosions occurred as the cargo was exposed to the air.

危険性

Lithium metal is highly flammable, explosive, and toxic. It will ignite when exposed towater, acids, and even damp air. Metallic lithium is a reducing agent that readily gives up anelectron to active oxidizing agents that require an electron to complete their outer valenceshell—thus the violent chemical reaction that follows. Lithium will even burn in nitrogengas, which is relatively stable. In addition, many of its compounds also react violently whenexposed to water.
As an element (metal), it must be stored in oil or in some type of air and moisture-free container,given that many of its compounds will also burn when exposed to air or water. Lithiumfires are difficult to extinguish. If water is poured on the fire, lithium will just burn faster orexplode. A supply of special chemicals or even dry sand is required to extinguish such fires.
Solutions and powders of several lithium salts are very toxic to the human nervous system,thus requiring close observation by a physician when used as antidepressant drugs.

健康ハザード

Lithium can react with moisture on the skinto produce corrosive hydroxide. Thus, contactof this metal with the skin or eyes can causeburn. The fumes are irritating to the skin,eyes, and mucous membranes. Ingestion of lithium can cause kidney injury, especiallywhen sodium intake is limited (Merck 1996).

健康ハザード

Contact with eyes causes caustic irritation or burn. Incontact with skin Litium reacts with body moisture to cause chemical burns: foil, ribbon, and wire react relatively slowly.

火災危険

Lithium is less active than sodium or potassium. Finely divided metal ignites spontaneously in air. The ignition of the bulk metal occurs when heated to its melting point. It burns with a carmine-red flame. Burning evolves dense white and opaque fumes. Vigorous reaction occurs when the metal is mixed with water. The heat of reaction, if not dissipated, can ignite or explode hydrogen that is liberated.
Violent explosive reactions occur with carbon tetrachloride; carbon tetrabromide; chloroform, bromoform, or iodoform (on heating); carbon monoxide in the presence of water; phosphorus (on heating); arsenic (on heating); and sulfur (molten). Among the substances that constitute high explosion hazards, the halogenated hydrocarbons are most significant. A number of compounds of this class in addition to those mentioned above form impact-sensitive products that can detonate on heating or impact.
Heating with nitric acid can cause fires. Lithium reacts with nitrogen at elevated temperatures to form lithium nitride, which can ignite on heating.
.

応用例(製薬)

Lithium inhibits GSK-3 and InsP, and both pathways have therefore been suggested to be involved in the treatment of BD and schizophrenia. The theory behind this hypothesis is that overactive InsP signalling in the brain of these patients potentially causes BD and this may be reduced by the inhibitory effect of lithium on such signalling.
It is believed that lithium potentially can protect against disease-induced cell death. GSK-3 has been implicated in the origins of schizophrenia, but with the availability of many antipsychotic drugs on the market, lithium ions are not in common use for the treatment of schizophrenia. There are also several direct roles of lithium in the treatment of Alzheimer’s disease. Alzheimer’s disease is a neurodegenerative brain disorder causing neuronal dysfunction and ultimately cell death.
Onset occurs with the accumulation of extracellular senile plaques composed of amyloid-β peptides and with the accumulation of intercellular neurofibrillary tangles.

工業用途

This lightest of all metals is found in more than 40 minerals, but is obtained chiefly from lepidolite, spodumene, and salt brines.
It is unstable chemically and burns in the air with a dazzling white flame when heated to just above its melting point. The metal is silvery white but tarnishes quickly in the air. The metal is kept submerged in kerosene. Lithium resembles sodium, barium, and potassium, but has a wider reactive power than the other alkali metals. It combines easily with oxygen, nitrogen, and sulfur to form low melting-point compounds that pass off as gases, and is thus useful as a deoxidizer and degasifier of metals.

作用機序

Lithium is a monovalent cation that can replace Na+ in some biological processes. It can be argued that competition by Li+ for active Na+ sites may lead to altered neuronal functions that may account for its antimanic and mood-stabilizing actions. In this regard, the failure of Li+ to maintain a normal membrane potential because of its lower affinity for the Na+ pump has been demonstrated. However, this action of Li+ would not explain its relatively selective effects on the CNS, sparing comparable excitable tissues (e.g. cardiac muscle) in the periphery.Moreover, an action on membrane polarity would be so general that the entire pool of brain neurons would be affected by Li+. It seems more reasonable that Li+ produces its psychotropic actions by perturbation of molecular events common to a few CNS synapses that might have been disturbed during the course of the manic-depressive illness.
Recently, attention has focused on the actions of Li+ on receptor-mediated second-messenger signaling systems of the brain. In this regard, interactions between Li+ and guanine nucleotide (GTP) binding proteins (G proteins) have been the target of many studies, since G proteins play a pivotal role in the function of many second- messenger signaling systems. Lithium is capable of altering G-protein function. It can diminish the coupling between the receptor recognition site and the G protein.The molecular mechanism involves the competition for Mg++ sites on the G protein, which are essential for GTP binding. Guanine nucleotide activates the G protein. Accordingly, in the presence of Li+, receptormediated activation of these G proteins is attenuated. This action of Li+ has been selectively demonstrated for G proteins associated with β-adrenoceptors and M1 muscarinic receptors of the CNS.
While it is not possible at present to assign a therapeutic role to this action of Li+, it is a step toward explaining the stabilizing actions of this drug. Since several neurotransmitter receptors share common G protein–regulated second-messenger signaling systems, Li+ could simultaneously correct the alterations at individual synapses associated with depression and mania by a single action on the function of specific G proteins. An additional action of Li+ is interruption of the phosphatidylinositide cycle through an inhibitory action on inositol phosphate metabolism. By this mechanism, depletion of membrane inositol and the phosphoinositide- derived second-messenger products diacylglycerol and inositol triphosphate ultimately reduces signaling through receptor systems dependent on the formation of these products. It is presently unclear to what extent inhibition of inositol phosphate metabolism contributes to the therapeutic properties of Li+ in bipolar patients.

副作用

The frequency and severity of adverse reactions associated with Li+ therapy are directly related to serum levels Since Li+ has a low therapeutic index (approximately 3) and a narrow therapeutic window (0.5–1.5 mEq/L), the frequent measurement of serum steadystate concentrations is standard practice in the treatment of bipolar patients.
Adverse reactions occurring at serum trough levels (12 hours after the last dose) below 1.5 mEq/L are generally mild, whereas those seen above 2.5 mEq/L are usually quite severe. Mild toxicity is usually expressed as nausea, vomiting, abdominal pain, diarrhea, polyuria, sedation, and fine tremor. If the serum concentration of Li+ progressively rises above 2 mEq/L, frank neurological toxicity appears, beginning with mental confusion and progressing to hyperreflexia, gross tremor, dysarthria, focal neurological signs, seizures, progressive coma, and even death.
Adverse effects sometimes seen during chronic maintenance of bipolar patients with Li+ include hypothyroidism (approximately 5%) and nephrogenic dia-betes insipidus.Both conditions are readily reversible by discontinuation of Li+. Routine laboratory monitoring includes TSH (thyroid-stimulating hormone) and serum creatinine measurements to detect hypothyroidism and any change in renal capacity to clear the drug.

職業ばく露

Lithium is used in inorganic syntheses; the manufacture of storage batteries; heat transfer liquids; and metal alloys.

輸送方法

UN1415 Lithium, Hazard Class: 4.3; Labels: 4.3-Dangerous when wet material. UN3089 Metal powders, flammable, n.o.s., Hazard Class: 4.1; Labels: 4.1- Flammable solid

純化方法

After washing with pet ether to remove storage oil, lithium is fused at 400o and then forced through a 10-micron stainless-steel filter with argon pressure. It is again melted in a dry-box, skimmed, and poured into an iron distillation pot. After heating under a vacuum to 500o, cooling and returning it to the dry-box for a further cleaning of its surface, the lithium is distilled at 600o using an all-iron distillation apparatus [Gunn & Green J Am Chem Soc 80 4782 1958].

不和合性

Violent reaction with water, forming flammable hydrogen gas and corrosive lithium hydroxide, a strong caustic solution. Heating may cause violent combustion or explosion. Finely divided particles or powdered form may ignite spontaneously in air. Contact with air forms corrosive fumes of lithium hydroxide. Violent reaction with oxidizers, acetonitrile, nitric acid; arsenic, bromobenzene, carbon tetrachloride; hydrocarbons, halogens, halons, sulfur, and many other substances. Forms impactand friction-sensitive mixtures with bromobenzene, carbon tetrabromide, chloroform (weak explosion), iodoform, halogens, halocarbons, methyl dichloride; methyl diiodide and other substances. Attacks plastics, rubber, ceramic materials; concrete, sand, and metal alloys: cobalt, iron, manganese, nickel

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(1R)-2,2-ジメチル-3-(2-メチル-1-プロペニル)シクロプロパンカルボン酸1-エチニル-2-メチル-2-ペンテニル 2-(6-メチル-2-ピリジル)エタノール 2-ジフェニルホスフィノ-6-メチルピリジン ジ(p-トリル)ホスフィンオキシド クロロジメチルフェニルシラン ジフェニルホスフィン ジフェニル-2-ピリジルホスフィン ペルオキシジリチウム (1S,2S)-(-)-1,2-ジフェニルエチレンジアミン (2S,3S)-(+)-1,4-ビス(ジフェニルホスフィノ)-2,3-O-イソプロピリデン-2,3-ブタンジオール ジフェニルホスフィンオキシド 2-(2-(ジフェニルホスフィノ)エチル)ピリジン ビス(ジフェニルホスフィノ)メタン β-エストラジオール ビス(3,5-ジメチルフェニル)ホスフィンオキシド rac-2β*-(2-メチルベンジルオキシ)-4α*-イソプロピル-1α*-メチル-7-オキサビシクロ[2.2.1]ヘプタン ジフェニル[2-(トリエトキシシリル)エチル]ホスフィン 2-(ジフェニルホスフィノ)エチルアミン トリス(トリフェニルホスフィン)ルテニウム(II) ジクロリド (2R,3R)-(-)-1,4-ビス(ジフェニルホスフィノ)-2,3-O-イソプロピリデン-2,3-ブタンジオール [1,3-ビス(ジフェニルホスフィノ)プロパン]ニッケル(II)ジクロリド 1,3-ビス(ジフェニルホスフィノ)プロパン (+)-N-ベンジル-(3R,4R)-ビス(ジフェニルホスフィノ)ピロリジン [1,2-ビス(ジフェニルホスフィノ)エタン]ニッケル(II)ジクロリド (1R,2R)-(+)-1,2-ジフェニルエチレンジアミン トリス(トリメチルシリル)シラン (S)-(-)-2,2'-ビス(ジフェニルホスフィノ)-1,1'-ビナフチル 3-メトキシ-13β-エチルゴナ-2,5(10)-ジエン-17-オン 2-(p-トリル)ピリジン [1,2-ビス(ジフェニルホスフィノ)エタン]パラジウム(II)ジクロリド シクロペンタノール 3-メトキシ-13β-エチルゴナ-2,5(10)-ジエン-17β-オール 塩化2,6-ジクロロ-5-フルオロニコチノイル デフラザコート cis-3-ヘキセン-1-オール ゲムフィブロジル

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