WordNet

a silvery soft waxy metallic element of the alkali metal group; occurs abundantly in natural compounds (especially in salt water); burns with a yellow flame and reacts violently in water; occurs in sea water and in the mineral halite (rock salt) (同)Na, atomic number 11

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ソジウム,ナトリウム(金属元素;化学記号はNa)

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2017/01/17 15:58:09」(JST)

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ナトリウム（独: Natrium [ˈnaːtriʊm]、羅: Natrium）は原子番号 11、原子量 22.99 の元素、またその単体金属である。元素記号は Na。アルカリ金属元素の一つで、典型元素である。医薬学や栄養学などの分野ではソジウム（ソディウム、英: sodium [ˈsoʊdiəm]）とも言い、日本の工業分野では（特に化合物中において）曹達（ソーダ）と呼ばれる^{[※ 1]}。毒物及び劇物取締法により劇物に指定されている^[2]。

歴史

1807年、ハンフリー・デービーが水酸化ナトリウム（苛性ソーダ）を電気分解することにより発見した。ナトリウムという名称は天然炭酸ソーダを意味するギリシャ語の νίτρον^[3]、あるいはラテン語の natron（ナトロン）^[4]に由来するといわれる。

ドイツ語では Natrium、英語では sodium と呼ばれ、いずれも近代にラテン語として造語された単語である（現代ラテン語では natrium が使われる）。日本にはドイツ語から輸入され、ナトリウムという名称が定着した。元素記号はドイツ語から Na になった一方、IUPAC名は英語から sodium とされている。

単体

性質

常温、常圧での結晶構造は、BCC 構造（体心立方構造）。融点は98 ℃で、沸点は883℃（他に883 ℃、881 ℃という実験値あり）。比重は0.97で、わずかに水より軽い。

非常に反応性の高い金属で、酸、塩基に侵され、水と激しく反応する。下記に示される化学反応過程を経て水酸化ナトリウムとなるため、素手で触れると手の表面にある水分と化合し水酸化ナトリウムとなって皮膚を侵す。さらに空気中で容易に酸化されるため、保存する時は灯油に浸ける。後述化学反応に示すようにアルコール等のプロトン溶媒とも反応するがエーテルや灯油とは反応しないため、灯油等を保存液体として使用する。イオン化する時は一価の陽イオンになりやすい。炎色反応で黄色を呈する。

消防法第2条第7項及び別表第一第3類1号により第3類危険物に指定されている。

200 GPa（約200万気圧）の高圧下では、結晶構造が変化し、金属光沢を失い透明になる^[5]。

生産

水酸化物や塩化物を融解塩電解することによって単体を得られる。カストナー法（原料 NaOH）、ダウンズ法（原料 NaCl）が知られる。2006年まで、新潟県に立地する日本曹達二本木工場が、国内で唯一工業的規模の金属ナトリウム製造を行っていたが、現在は操業を停止している。海外ではフランスのMAAS社とアメリカのDuPont社がダウンズ法で生産している^[6]。日本の輸入量は2007年で3055トンであった^[7]。またカストナー法は工業生産としては使用されていない。

用途

熱伝導率がよく、高温でも液体で存在するため、単体としては高速増殖炉の冷却材として用いられる。高性能自動車エンジンの排気バルブのステム内部に封入し熱伝導を向上させる用途にも使われる。そのほかに、負極にナトリウム、正極に硫黄を使った、NaS電池がある。これは大型の非常用電源や、風力発電のエネルギー貯蔵に利用される。トンネルの中などに使われている発光（ナトリウムのD線、D1: 589.6 nmとD2: 589.0 nm）はナトリウムランプである。

生体にとっては重要な電解質の一つであり、ヒトではその大部分が細胞外液に分布している。神経細胞や心筋細胞などの電気的興奮性細胞の興奮には、細胞内外のナトリウムイオン濃度差が不可欠である。細胞外濃度は 135–145 mmol/l程度に保たれており、細胞外液の陽イオンの大半を占める。そのため、ナトリウムイオンの過剰摂取は濃度維持のための水分貯留により、高血圧の大きな原因となる。

主な化学反応

水と反応して水素を発生させながら水酸化ナトリウム (NaOH) になる。

2 Na + 2 H₂O → 2 NaOH + H₂
- 発熱反応・低融点のため水に固体ナトリウムを投げ込むとナトリウムが反応熱で溶融し細粒化して反応面積が激増して爆発する

アルコール、カルボン酸、フェノール類などのヒドロキシ基と反応して水素を発生させながらアルコキシドなどを与える。

2 Na + 2 ROH → 2 RONa + H₂（アルコール：R = アルキル基、フェノール類：R = 芳香族置換基）

2 Na + 2 RCOOH → 2 RCOONa + H₂
ハロゲンの単体と結合（反応）して、塩になる。

2 Na + Cl₂ → 2 NaCl

化合物

記事カテゴリ Category:ナトリウムの化合物も参照。

オキソ酸の塩

炭酸水素ナトリウム（重曹）(NaHCO₃)
炭酸ナトリウム（炭酸ソーダ）(Na₂CO₃)
過炭酸ナトリウム (2Na₂CO₃･3H₂O₂)
亜二チオン酸ナトリウム（亜ジチオン酸ナトリウム、ナトリウムハイドロサルファイト）(Na₂S₂O₄)
亜硫酸ナトリウム (Na₂SO₃)
亜硫酸水素ナトリウム (NaHSO₃)
硫酸ナトリウム（芒硝）(Na₂SO₄)
チオ硫酸ナトリウム（ハイポ）(Na₂S₂O₃)
亜硝酸ナトリウム (NaNO₂)
硝酸ナトリウム (NaNO₃)

ハロゲン化物

フッ化ナトリウム (NaF)
塩化ナトリウム（食塩）(NaCl)
臭化ナトリウム (NaBr)
ヨウ化ナトリウム (NaI)

酸化物・水酸化物

酸化ナトリウム (Na₂O)
過酸化ナトリウム (Na₂O₂)
水酸化ナトリウム（苛性ソーダ）(NaOH)

その他の無機塩

水素化ナトリウム (NaH)
硫化ナトリウム (Na₂S)
硫化水素ナトリウム（水硫化ナトリウム）(NaHS)
珪酸ナトリウム (Na₂SiO₃)
リン酸三ナトリウム (Na₃PO₄)
ホウ酸ナトリウム (Na₃BO₃)
水素化ホウ素ナトリウム (NaBH₄)
シアン化ナトリウム（青酸ナトリウム）(NaCN)
シアン酸ナトリウム (NaOCN)
テトラクロロ金酸ナトリウム (Na[AuCl₄])

有機酸塩

酢酸ナトリウム (CH₃COONa)
クエン酸ナトリウム

同位体

詳細は「ナトリウムの同位体」を参照

脚注

[ヘルプ]

注釈

^ 炭酸水素ナトリウムを重炭酸ソーダ（重曹）と呼んだり、水酸化ナトリウムを苛性ソーダと呼ぶ。また、ナトリウム化合物を作ることから日本曹達や東洋曹達（現東ソー）などの名前の由来となっている。

出典

^ Endt, P. M. ENDT, ,1 (1990) (12/1990). “Energy levels of A = 21-44 nuclei (VII)”. Nuclear Physics A 521: 1. doi:10.1016/0375-9474(90)90598-G.
^ 毒物及び劇物取締法昭和二十五年十二月二十八日法律三百三号第二条別表第二
^ 近角、木越、田沼「最新元素知識」東京書籍、1976年
^ 桜井「元素111の新知識」BLUE BACKS、講談社、1997年。 ISBN 4-06-257192-7
^ Yanming Ma et al., "Transparent dense sodium", Nature 458, 182-185 (2009). doi:10.1038/nature07786
^ “Sodium Metal from France”. U.S. International Trade Commission. 2012年8月4日閲覧。
^ 『15509の化学商品』化学工業日報社、2009年2月。ISBN 978-4-87326-544-5。

外部リンク

ナトリウムの特性（原子力百科事典　ATOMICA）
ナトリウム冷却システム（原子力百科事典　ATOMICA）
ナトリウム取扱い技術（原子力百科事典　ATOMICA）
ナトリウムの安全性（1次系ナトリウム）（原子力百科事典　ATOMICA）
ナトリウムの安全性（蒸気発生器および2次系ナトリウム）　（原子力百科事典　ATOMICA）
ナトリウム - 「健康食品」の安全性・有効性情報（国立健康・栄養研究所）
ナトリウムと水の反応動画
DuPount社Reactive Metals部門HP

wiki en

[Wiki en表示]

Sodium is a chemical element with symbol Na (from Latin natrium) and atomic number 11. It is a soft, silvery-white, highly reactive metal. Sodium is an alkali metal, being in group 1 of the periodic table, because it has a single electron in its outer shell that it readily donates, creating a positively charged atom—the Na⁺ cation. Its only stable isotope is ²³Na. The free metal does not occur in nature, but must be prepared from compounds. Sodium is the sixth most abundant element in the Earth's crust, and exists in numerous minerals such as feldspars, sodalite and rock salt (NaCl). Many salts of sodium are highly water-soluble: sodium ions have been leached by the action of water from the Earth's minerals over eons, and thus sodium and chlorine are the most common dissolved elements by weight in the oceans.

Sodium was first isolated by Humphry Davy in 1807 by the electrolysis of sodium hydroxide. Among many other useful sodium compounds, sodium hydroxide (lye) is used in soap manufacture, and sodium chloride (edible salt) is a de-icing agent and a nutrient for animals including humans.

Sodium is an essential element for all animals and some plants. Sodium ions are the major cation in the extracellular fluid (ECF) and as such are the major contributor to the ECF osmotic pressure and ECF compartment volume. Loss of water from the ECF compartment increases the sodium concentration, a condition called hypernatremia. Isotonic loss of water and sodium from the ECF compartment decreases the size of that compartment in a condition called ECF hypovolemia.

By means of the sodium-potassium pump, living human cells pump three sodium ions out of the cell in exchange for two potassium ions pumped in; comparing ion concentrations across the cell membrane, inside to outside, potassium measures about 40:1, and sodium, about 1:10. In nerve cells, the electrical charge across the cell membrane enables transmission of the nerve impulse—an action potential—when the charge is dissipated; sodium plays a key role in that activity.

1 Characteristics
- 1.1 Physical
- 1.2 Isotopes
2 Chemistry
- 2.1 Salts and oxides
- 2.2 Aqueous solutions
- 2.3 Electrides and sodides
- 2.4 Organosodium compounds
- 2.5 Intermetallic compounds
3 History
4 Occurrence
5 Commercial production
6 Applications
- 6.1 Free element
  - 6.1.1 Heat transfer
7 Biological role
8 Safety and precautions
9 See also
10 References
11 Bibliography
12 External links

Characteristics

Physical

Emission spectrum for sodium, showing the D line.

Sodium at standard temperature and pressure is a soft silvery metal that combines with oxygen in air and forms grayish white sodium oxide unless immersed in oil or inert gas, which are the conditions it is usually stored in. Sodium metal can be easily cut with a knife and is a good conductor of electricity and heat because it has only one electron in its valence shell, resulting in weak metallic bonding and free electrons, which carry energy. Due to having low atomic weight and large atomic radius, sodium is third-least dense of all elemental metals and is one of only three metals that can float on water, the other two being lithium and potassium.^[5] The melting (98 °C) and boiling (883 °C) points of sodium are lower than those of lithium but higher than those of the heavier alkali metals potassium, rubidium, and caesium, following periodic trends down the group.^[6] These properties change dramatically at elevated pressures: at 1.5 Mbar, the color changes from silvery metallic to black; at 1.9 Mbar the material becomes transparent with a red color; and at 3 Mbar, sodium is a clear and transparent solid. All of these high-pressure allotropes are insulators and electrides.^[7]

A positive flame test for sodium has a bright yellow color.

In a flame test, sodium and its compounds glow yellow^[8] because the excited 3s electrons of sodium emit a photon when they fall from 3p to 3s; the wavelength of this photon corresponds to the D line at about 589.3 nm. Spin-orbit interactions involving the electron in the 3p orbital split the D line into two, at 589.0 and 589.6 nm; hyperfine structures involving both orbitals cause many more lines.^[9]

Isotopes

Twenty isotopes of sodium are known, but only ²³Na is stable. ²³Na is created in the carbon-burning process in stars by fusing two carbon atoms together; this requires temperatures above 600 megakelvins and a star of at least three solar masses.^[10] Two radioactive, cosmogenic isotopes are the byproduct of cosmic ray spallation: ²²Na has a half-life of 2.6 years and ²⁴Na, a half-life of 15 hours; all other isotopes have a half-life of less than one minute.^[11] Two nuclear isomers have been discovered, the longer-lived one being ^24mNa with a half-life of around 20.2 milliseconds. Acute neutron radiation, as from a nuclear criticality accident, converts some of the stable ²³Na in human blood to ²⁴Na; the neutron radiation dosage of a victim can be calculated by measuring the concentration of ²⁴Na relative to ²³Na.^[12]

Chemistry

Sodium atoms have 11 electrons, one more than the extremely stable configuration of the noble gas neon. Because of this and its low first ionization energy of 495.8 kJ/mol, the sodium atom is much more likely to lose the last electron and acquire a positive charge than to gain one and acquire a negative charge.^[13] This process requires so little energy that sodium is readily oxidized by giving up its 11th electron. In contrast, the second ionization energy is very high (4562 kJ/mol), because the 10th electron is closer to the nucleus than the 11th electron. As a result, sodium usually forms ionic compounds involving the Na⁺ cation.^[14]

The most common oxidation state for sodium is +1. It is generally less reactive than potassium and more reactive than lithium.^[15] Sodium metal is highly reducing, with the reduction of sodium ions requiring −2.71 volts,^[16] though potassium and lithium have even more negative potentials.^[17]

Salts and oxides

Structure of sodium chloride, showing octahedral coordination around Na⁺ and Cl⁻ centres. This framework disintegrates when dissolved in water and reassembles when the water evaporates.

Sodium compounds are of immense commercial importance, being particularly central to industries producing glass, paper, soap, and textiles.^[18] The most important sodium compounds are table salt (NaCl), soda ash (Na₂CO₃), baking soda (NaHCO₃), caustic soda (NaOH), sodium nitrate (NaNO₃), di- and tri-sodium phosphates, sodium thiosulfate (Na₂S₂O₃·5H₂O), and borax (Na₂B₄O₇·10H₂O).^[19] In compounds, sodium is usually ionically bonded to water and anions, and is viewed as a hard Lewis acid.^[20]

Two equivalent images of the chemical structure of sodium stearate, a typical soap.

Most soaps are sodium salts of fatty acids. Sodium soaps have a higher melting temperature (and seem "harder") than potassium soaps.^[19]

Like all the alkali metals, sodium reacts exothermically with water, and sufficiently large pieces melt to a sphere and may explode. The reaction produces caustic soda (sodium hydroxide) and flammable hydrogen gas. When burned in air, it forms primarily sodium peroxide with some sodium oxide.^[21]

Aqueous solutions

Sodium tends to form water-soluble compounds, such as halides, sulfates, nitrates, carboxylates and carbonates. The main aqueous species are the aquo complexes [Na(H₂O)_n]⁺, where n = 4–8; with n = 6 indicated from X-ray diffraction data and computer simulations.^[22]

Direct precipitation of sodium salts from aqueous solutions is rare because sodium salts typically have a high affinity for water; an exception is sodium bismuthate (NaBiO₃).^[23] Because of this, sodium salts are usually isolated as solids by evaporation or by precipitation with an organic solvent, such as ethanol; for example, only 0.35 g/L of sodium chloride will dissolve in ethanol.^[24] Crown ethers, like 15-crown-5, may be used as a phase-transfer catalyst.^[25]

Sodium content in bulk may be determined by treating with a large excess of uranyl zinc acetate; the hexahydrate (UO₂)₂ZnNa(CH₃CO₂)·6H₂O precipitates and can be weighed. Caesium and rubidium do not interfere with this reaction, but potassium and lithium do.^[26] Lower concentrations of sodium may be determined by atomic absorption spectrophotometry^[27] or by potentiometry using ion-selective electrodes.^[28]

Electrides and sodides

Like the other alkali metals, sodium dissolves in ammonia and some amines to give deeply colored solutions; evaporation of these solutions leaves a shiny film of metallic sodium. The solutions contain the coordination complex (Na(NH₃)₆)⁺, with the positive charge counterbalanced by electrons as anions; cryptands permit the isolation of these complexes as crystalline solids. Sodium forms complexes with crown ethers, cryptands and other ligands.^[29] For example, 15-crown-5 has high affinity for sodium because the cavity size of 15-crown-5 is 1.7–2.2 Å, which is enough to fit sodium ion (1.9 Å).^[30]^[31] Cryptands, like crown ethers and other ionophores, also have a high affinity for the sodium ion; derivatives of the alkalide Na⁻ are obtainable^[32] by the addition of cryptands to solutions of sodium in ammonia via disproportionation.^[33]

Organosodium compounds

The structure of the complex of sodium (Na⁺, shown in yellow) and the antibiotic monensin-A.

Many organosodium compounds have been prepared. Because of the high polarity of the C-Na bonds, they behave like sources of carbanions (salts with organic anions). Some well known derivatives include sodium cyclopentadienide (NaC₅H₅) and trityl sodium ((C₆H₅)₃CNa).^[34] Because of the large size and very low polarising power of the Na⁺ cation, it can stabilize large, aromatic, polarisable radical anions, such as in sodium naphthalenide, Na⁺[C₁₀H₈•]⁻, a strong reducing agent.^[35]

Intermetallic compounds

Sodium forms alloys with many metals, such as potassium, calcium, lead, and the group 11 and 12 elements. Sodium and potassium form KNa₂ and NaK. NaK is 40–90% potassium and it is liquid at ambient temperature. It is excellent thermal and electrical conductor. Sodium-calcium alloys are by-products of electrolytic production of sodium from binary salt mixture of NaCl-CaCl₂ and ternary mixture NaCl-CaCl₂-BaCl₂. Calcium is only partially miscible with sodium. In liquid state, sodium is completely miscible with lead. There are several methods to make sodium-lead alloys. One is to melt them together and another is to deposit sodium electrolycally on molten lead cathodes. NaPb₃, NaPb, Na₉Pb₄, Na₅Pb₂, and Na₁₅Pb₄ are some of the known sodium-lead alloys. Sodium also forms alloys with gold (NaAu₂) and silver (NaAg₂). Group 12 metals (zinc, cadmium and mercury) are known to make alloys with sodium. NaZn₁₃ and NaCd₂ are alloys of zinc and cadmium. Sodium and mercury form NaHg, NaHg₄, NaHg₂, Na₃Hg₂, and Na₃Hg.^[36]

History

Because of its importance in human metabolism, salt has long been an important commodity as shown by the English word salary, which derives from salarium, the wafers of salt sometimes given to Roman soldiers along with their other wages. In medieval Europe, a compound of sodium with the Latin name of sodanum was used as a headache remedy. The name sodium is thought to originate from the Arabic suda, meaning headache, as the headache-alleviating properties of sodium carbonate or soda were well known in early times.^[37] Although sodium, sometimes called soda, had long been recognized in compounds, the metal itself was not isolated until 1807 by Sir Humphry Davy through the electrolysis of sodium hydroxide.^[38]^[39] In 1809, the German physicist and chemist Ludwig Wilhelm Gilbert proposed the names Natronium for Humphry Davy's "sodium" and Kalium for Davy's "potassium".^[40] The chemical abbreviation for sodium was first published in 1814 by Jöns Jakob Berzelius in his system of atomic symbols,^[41]^[42] and is an abbreviation of the element's New Latin name natrium, which refers to the Egyptian natron,^[37] a natural mineral salt mainly consisting of hydrated sodium carbonate. Natron historically had several important industrial and household uses, later eclipsed by other sodium compounds.^[43]

Sodium imparts an intense yellow color to flames. As early as 1860, Kirchhoff and Bunsen noted the high sensitivity of a sodium flame test, and stated in Annalen der Physik und Chemie:^[44]

In a corner of our 60 m³ room farthest away from the apparatus, we exploded 3 mg. of sodium chlorate with milk sugar while observing the nonluminous flame before the slit. After a while, it glowed a bright yellow and showed a strong sodium line that disappeared only after 10 minutes. From the weight of the sodium salt and the volume of air in the room, we easily calculate that one part by weight of air could not contain more than 1/20 millionth weight of sodium.

Occurrence

The Earth's crust contains 2.27% sodium, making it the seventh most abundant element on Earth and the fifth most abundant metal, behind aluminium, iron, calcium, and magnesium and ahead of potassium.^[45] Sodium's estimated oceanic abundance is 1.08×10⁴ milligrams per liter.^[46] Because of its high reactivity, it is never found as a pure element. It is found in many different minerals, some very soluble, such as halite and natron, others much less soluble, such as amphibole and zeolite. The insolubility of certain sodium minerals such as cryolite and feldspar arises from their polymeric anions, which in the case of feldspar is a polysilicate. In the interstellar medium, sodium is identified by the D spectral line; though it has a high vaporization temperature, its abundance in Mercury's atmosphere enabled its detection by Potter and Morgan using ground-based high resolution spectroscopy. Sodium has been detected in at least one comet; astronomers watching Comet Hale-Bopp in 1997 observed a sodium tail consisting of neutral atoms (not ions) and extending to some 50 million kilometres behind the head.^[47]

Commercial production

Employed only in rather specialized applications, only about 100,000 tonnes of metallic sodium are produced annually.^[18] Metallic sodium was first produced commercially in the late 19th century^[48] by carbothermal reduction of sodium carbonate at 1100 °C, as the first step of the Deville process for the production of aluminium:^[49]^[50]^[51]

Na₂CO₃ + 2 C → 2 Na + 3 CO

The high demand of aluminium created the need for the production of sodium. After the introduction of the Hall–Héroult process for the production of aluminium in by electrolysing a molten salt bath ended the need for large quantities of sodium. A related process based on the reduction of sodium hydroxide was developed in 1886.^[49]

Sodium is now produced commercially through the electrolysis of molten sodium chloride, based on a process patented in 1924.^[52]^[53] This is done in a Downs cell in which the NaCl is mixed with calcium chloride to lower the melting point below 700 °C. As calcium is less electropositive than sodium, no calcium will be deposited at the cathode.^[54] This method is less expensive than the previous Castner process (the electrolysis of sodium hydroxide).^[55]

The market for sodium is volatile due to the difficulty in its storage and shipping; it must be stored under a dry inert gas atmosphere or anhydrous mineral oil to prevent the formation of a surface layer of sodium oxide or sodium superoxide.^[56]

Applications

Though metallic sodium has some important uses, the major applications for sodium use compounds; millions of tons of sodium chloride, hydroxide, and carbonate are produced annually. Sodium chloride is extensively used for anti-icing and de-icing and as a preservative; sodium bicarbonate is mainly used for cooking. Along with potassium, many important medicines have sodium added to improve their bioavailability; though potassium is the better ion in most cases, sodium is chosen for its lower price and atomic weight.^[57] Sodium hydride is used as a base for various reactions (such as the aldol reaction) in organic chemistry, and as a reducing agent in inorganic chemistry.^[58]

Free element

Metallic sodium is used mainly for the production of sodium borohydride, sodium azide, indigo, and triphenylphosphine. Previous uses were for the making of tetraethyllead and titanium metal; because applications for these chemicals were discontinued, the production of sodium declined after 1970.^[18] Sodium is also used as an alloying metal, an anti-scaling agent,^[59] and as a reducing agent for metals when other materials are ineffective. Note the free element is not used as a scaling agent, ions in the water are exchanged for sodium ions. Sodium plasma ("vapor") lamps are often used for street lighting in cities, shedding light that ranges from yellow-orange to peach as the pressure increases.^[60] By itself or with potassium, sodium is a desiccant; it gives an intense blue coloration with benzophenone when the desiccate is dry.^[61] In organic synthesis, sodium is used in various reactions such as the Birch reduction, and the sodium fusion test is conducted to qualitatively analyse compounds.^[62] Sodium reacts with alcohol and gives alkoxides, and when sodium is dissolved in ammonia solution, it can be used to reduce alkynes to trans-alkenes.^[63]^[64] Sodium lasers emitting light at the D line are used to create artificial laser guide stars that assist in the adaptive optics for land-based visible light telescopes.^[65]

Heat transfer

NaK phase diagram, showing the melting point of sodium as a function of potassium concentration. NaK with 77% potassium is eutectic and has the lowest melting point of the NaK alloys at −12.6 °C.^[66]

Liquid sodium is used as a heat transfer fluid in some fast reactors^[67] because it has the high thermal conductivity and low neutron absorption cross section required to achieve a high neutron flux in the reactor.^[68] The high boiling point of sodium allows the reactor to operate at ambient (normal) pressure,^[68] but the drawbacks include its opacity, which hinders visual maintenance, and its explosive properties.^[69] Radioactive sodium-24 may be produced by neutron bombardment during operation, posing a slight radiation hazard; the radioactivity stops within a few days after removal from the reactor.^[70] If a reactor needs to be shut down frequently, NaK is used; because NaK is a liquid at room temperature, the coolant does not solidify in the pipes.^[71] In this case, the pyrophoricity of potassium requires extra precautions to prevent and detect leaks.^[72] Another heat transfer application is poppet valves in high-performance internal combustion engines; the valve stems are partially filled with sodium and work as a heat pipe to cool the valves.^[73]

Biological role

In humans, sodium is an essential mineral that regulates blood volume, blood pressure, osmotic equilibrium and pH; the minimum physiological requirement for sodium is 500 milligrams per day.^[74] Sodium chloride is the principal source of sodium in the diet, and is used as seasoning and preservative in such commodities as pickled preserves and jerky; for Americans, most sodium chloride comes from processed foods.^[75] Other sources of sodium are its natural occurrence in food and such food additives as monosodium glutamate (MSG), sodium nitrite, sodium saccharin, baking soda (sodium bicarbonate), and sodium benzoate.^[76] The US Institute of Medicine set its Tolerable Upper Intake Level for sodium at 2.3 grams per day,^[77] but the average person in the United States consumes 3.4 grams per day.^[78] Studies have found that lowering sodium intake by 2 g per day tends to lower systolic blood pressure by about two to four mm Hg.^[79] It has been estimated that such a decrease in sodium intake would lead to between 9 and 17% fewer cases of hypertension.^[79]

Hypertension causes 7.6 million premature deaths worldwide each year.^[80] (Note that salt contains about 39.3% sodium^[81]—the rest being chlorine and trace chemicals; thus, 2.3 g sodium is about 5.9 g, or 2.7 ml of salt—about half a US teaspoon.^[82]^[83]) The American Heart Association recommends no more than 1.5 g of sodium per day.^[84]

One study found that people with or without hypertension who excreted less than 3 grams of sodium per day in their urine (and therefore were taking in less than 3 g/d) had a higher risk of death, stroke, or heart attack than those excreting 4 to 5 grams per day. Levels of 7 g per day or more in people with hypertension were associated with higher mortality and cardiovascular events, but this was not found to be true for people without hypertension.^[85] The US FDA states that adults with hypertension and prehypertension should reduce daily intake to 1.5 g.^[83]

The renin-angiotensin system regulates the amount of fluid and sodium concentration in the body. Reduction of blood pressure and sodium concentration in the kidney result in the production of renin, which in turn produces aldosterone and angiotensin, retaining sodium in the urine. When the concentration of sodium increases, the production of renin decreases, and the sodium concentration returns to normal.^[86] The sodium ion (Na⁺) is an important electrolyte in neuron function, and in osmoregulation between cells and the extracellular fluid. This is accomplished in all animals by Na⁺/K⁺-ATPase, an active transporter pumping ions against the gradient, and sodium/potassium channels.^[87] Sodium is the most prevalent metallic ion in extracellular fluid.^[88]

Unusually low or high sodium levels in humans are recognized in medicine as hyponatremia and hypernatremia. These conditions may be caused by genetic factors, ageing, or prolonged vomiting or diarrhea.^[89]

In C4 plants, sodium is a micronutrient that aids in metabolism, specifically in regeneration of phosphoenolpyruvate and synthesis of chlorophyll.^[90] In others, it substitutes for potassium in several roles, such as maintaining turgor pressure and aiding in the opening and closing of stomata.^[91] Excess sodium in the soil limits the uptake of water by decreasing the water potential, which may result in plant wilting; excess concentrations in the cytoplasm can lead to enzyme inhibition, which in turn causes necrosis and chlorosis.^[92] In response, some plants developed mechanisms to limit sodium uptake in the roots, to store it in cell vacuoles, and restriction of salt transport from roots to leaves;^[93] excess sodium may also be stored in old plant tissue, limiting the damage to new growth.

Safety and precautions

Sodium forms flammable hydrogen and caustic sodium hydroxide on contact with water;^[95] ingestion and contact with moisture on skin, eyes or mucous membranes can cause severe burns.^[96]^[97] Sodium spontaneously explodes in the presence of an oxidizer such as water.^[98] Fire extinguishers based on water accelerate sodium fires; those based on carbon dioxide and bromochlorodifluoromethane should not be used on sodium fire.^[97] Metal fires are Class D, but not all Class D extinguishers are workable with sodium. An effective extinguishing agent for sodium fires is Met-L-X.^[97] Other effective agents include Lith-X, which has graphite powder and an organophosphate flame retardant, and dry sand.^[99] Sodium fires are prevented in nuclear reactors by isolating sodium from oxygen by surrounding sodium pipes with inert gas.^[100] Pool-type sodium fires are prevented using different design measures called catch pan systems. They collect leaking sodium into a leak-recovery tank where it is isolated from oxygen.^[100]

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Bibliography

Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.

External links

Sodium at The Periodic Table of Videos (University of Nottingham)
Etymology of "natrium" – source of symbol Na
The Wooden Periodic Table Table's Entry on Sodium
Sodium isotopes data from The Berkeley Laboratory Isotopes Project's

UpToDate Contents

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1. 低ナトリウム血症を有する成人の評価 evaluation of adults with hyponatremia
2. 水分バランス異常（低ナトリウム血症および高ナトリウム血症）およびナトリウムバランス異常（循環血液量減少および浮腫）の一般原則 general principles of disorders of water balance hyponatremia and hypernatremia and sodium balance hypovolemia and edema
3. 塩分摂取量および塩分摂取量制限と原発性（本態性）高血圧 salt intake salt restriction and primary essential hypertension
4. 高ナトリウム血症の病因および評価 etiology and evaluation of hypernatremia
5. 小児における低ナトリウム血症 hyponatremia in children

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NAID 110009982514

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★リンクテーブル★

リンク元	「100Cases 34」「ナトリウム」
拡張検索	「flavin-adenine dinucleotide sodium」「isotonic sodium chloride solution」「sodium-phosphate cotransporter protein」「fluorescein sodium」「ceftiofur sodium」

「100Cases 34」

NFPA 704; "fire diamond"
	1 3 2 W
	The fire diamond hazard sign for sodium metal

Sodium, ₁₁Na
	Spectral lines of sodium
General properties
Name, symbol	sodium, Na
Pronunciation	/ˈsoʊdiəm/; SOH-dee-əm
Appearance	silvery white metallic
Sodium in the periodic table
	neon ← sodium → magnesium
Atomic number (Z)	11
Group, block	group 1 (alkali metals), s-block
Period	period 3
Element category	alkali metal
Standard atomic weight (±) (Ar)	22.98976928(2)
Electron configuration	[Ne] 3s1
per shell	2, 8, 1
Physical properties
Phase	solid
Melting point	370.944 K (97.794 °C, 208.029 °F)
Boiling point	1156.090 K (882.940 °C, 1621.292 °F)
Density near r.t.	0.968 g/cm3
when liquid, at m.p.	0.927 g/cm3
Critical point	2573 K, 35 MPa (extrapolated)
Heat of fusion	2.60 kJ/mol
Heat of vaporization	97.42 kJ/mol
Molar heat capacity	28.230 J/(mol·K)
Atomic properties
Oxidation states	+1, −1 (a strongly basic oxide)
Electronegativity	Pauling scale: 0.93
Ionization energies	1st: 495.8 kJ/mol; 2nd: 4562 kJ/mol; 3rd: 6910.3 kJ/mol; (more)
Atomic radius	empirical: 186 pm
Covalent radius	166±9 pm
Van der Waals radius	227 pm
Miscellanea
Crystal structure	body-centered cubic (bcc)
Speed of sound thin rod	3200 m/s (at 20 °C)
Thermal expansion	71 µm/(m·K) (at 25 °C)
Thermal conductivity	142 W/(m·K)
Electrical resistivity	47.7 nΩ·m (at 20 °C)
Magnetic ordering	paramagnetic
Magnetic susceptibility (χmol)	+16.0·10−6 cm3/mol (298 K)
Young's modulus	10 GPa
Shear modulus	3.3 GPa
Bulk modulus	6.3 GPa
Mohs hardness	0.5
Brinell hardness	0.69 MPa
CAS Number	7440-23-5
History
Discovery and first isolation	Humphry Davy (1807)
Most stable isotopes of sodium
1.27453(2)	22Ne
1.27453(2)	22Ne
	* = excited state
	view; talk; edit; \| references \| in Wikidata

外見
	銀白色; ; ; ナトリウムのスペクトル線
一般特性
名称, 記号, 番号	ナトリウム, Na, 11
分類	アルカリ金属
族, 周期, ブロック	1, 3, s
原子量	22.98976928(2)
電子配置	[Ne] 3s1
電子殻	2,8,1（画像）
物理特性
相	固体
密度（室温付近）	0.968 g/cm3
融点での液体密度	0.927 g/cm3
融点	370.87 K, 97.72 °C, 207.9 °F
沸点	1156 K, 883 °C, 1621 °F
臨界点	（推定）2573 K, 35 MPa
融解熱	2.60 kJ/mol
蒸発熱	97.42 kJ/mol
熱容量	(25 °C) 28.230 J/(mol·K)
蒸気圧
原子特性
酸化数	+1, 0, -1; (強塩基性酸化物)
電気陰性度	0.93（ポーリングの値）
イオン化エネルギー	第1： 495.8 kJ/mol
	第2： 4562 kJ/mol
	第3： 6910.3 kJ/mol
原子半径	186 pm
共有結合半径	166±9 pm
ファンデルワールス半径	227 pm
その他
結晶構造	体心立方構造
磁性	常磁性
電気抵抗率	(20 °C) 47.7 nΩ·m
熱伝導率	(300 K) 142 W/(m·K)
熱膨張率	(25 °C) 71 µm/(m·K)
音の伝わる速さ; （微細ロッド）	(20 °C) 3200 m/s
ヤング率	10 GPa
剛性率	3.3 GPa
体積弾性率	6.3 GPa
モース硬度	0.5
ブリネル硬度	0.69 MPa
CAS登録番号	7440-23-5
最安定同位体
	詳細はナトリウムの同位体を参照
1.27453(2)	22Ne
1.27453(2)	22Ne
	表示

　　[★]

☆case34　てんかん発作

■症例

23歳　アフリカ-カリブ系　女性　銀行の店員

主訴：てんかん発作

現病歴：強直間代発作を2回起こしたところを母親が目撃していた。娘の行動は次第におかしくなり、また娘は自分のことを話している声が聞こえていた(幻聴)。最近、頭痛を訴えていた。体重が減少し、脱毛があった。盗汗と主に足と手の小関節に及ぶflitting 関節痛を訴えていた。服用薬なし。タバコ1日5-10本、アルコール10 unit/week(缶ビール(350ml)6本弱)

既往歴：特記なし(medical or psychiatric history)

家族歴：

生活歴：

・身体診断

意識：眠そうだが痛みに反応。頚部硬直：なし。頭髪：薄く斑状。体温38.5℃。リンパ節：たくさんの部位で触知。

心拍：104/分、整。血圧：164/102 mmHg。心血管系、呼吸器系、腹部：異常なし。

神経所見：focal anormalityなし(局所性異常)。乳頭浮腫：認めず。

・検査

(血液生化学)

上昇：erythrocyte sedimentation rate、urea、creatinine

低下：hemoglobin、white cell count、platelet

正常：mean corpuscular volume、sodium、potassium、glucose

(腰椎穿刺)

上昇：leukocytes、CSF protein

正常：CSF glucose

(尿検査)

蛋白：＋＋＋。血尿：＋＋＋。赤血球：＋＋。赤血球円柱：あり。

(その他)

胸部X線：異常なし。ECG：洞性頻脈。頭部 CT：正常。CSF グラム染色：陰性(光顕レベルで細菌なし)

■glossary

fall out　(毛髪などが)抜ける

night sweat 盗汗、寝汗

tonic-clonic generalized seizure 全般性強直間代発作

flit　vi (鳥・蝶など)すいすい/ひらひら飛ぶ、飛び回る、飛翔する。(人が)軽やかに通る、行き交う。(時が)(飛ぶように)すぎる。(幻想など)去来する、よぎる、(表情が)かすめる

drowsy　adj. 眠い。眠そうな。眠気を誘う。ものうい。眠ったような

stiffness　n. 堅いこと、堅ぐるしさ、がんこさ

delirium tremens 振戦譫妄

hypertensive encephalopathy 高血圧性脳症

alopecia　脱毛症

African-Caribbean アフリカ-カリブ系

fit n.　(病気の)発作。引きつけ、痙攣。(感情の)激発、一時的興奮、気まぐれ

chorea n. 舞踏病

recreational drug 耽溺性があり乱用される脱法薬物

urgent adj. (物・事が)急を要する、緊急の、背拍質(pressing)。(～を)緊急に必要とする(in)。(S is ～ (with O1) for [in] O2)(人が)(O1(人)に)O2(物・事)をしつこく求める。(人に/～するように)催促する(for/to do)。(要求などが)執拗な。

□てんかん発作

・新規発生したてんかん発作の原因(ICU.805-806)

・薬物中毒(テオフィリンなど)

・薬物からの離脱(アルコールなど)

・感染症(髄膜炎、膿瘍など)

・頭部外傷

・虚血障害(虚血あるいはびまん性)

・占拠性病変(腫瘍あるいは血腫)

・代謝性障害(肝性脳症、尿毒症性脳症、敗血症、低血糖、低ナトリウム血症、低カルシウム血症など)

・合併症(ICU.805-806)

・全身性てんかん発作の場合：高血圧、乳酸アシドーシス、高体温、呼吸障害、誤嚥、肺水腫、横紋筋融解、自傷、不可逆性の神経学的障害(30分間以上てんかん発作が持続した場合)

■可能性の高い診断

　全身性エリテマトーデス systemic lupus erythematosus(SLE)

■鑑別診断のポイント

　自己免疫疾患は多彩な症状を示す。そのため、個々の症状に着目して鑑別診断をあげるのではなく、症状や検査値の異常を総合的に見て判断する必要がある。

■解答

　(第1パラグラフ)SLEの病態

精神症状：(SLEは脳で血管炎を呈することで生じる)うつ(depression)、統合失調症様の精神病、痙攣(fits)、舞踏病(chorea)、脳梗塞/脊髄梗塞

脳脊髄液：白血球増多(leukopenia)、蛋白増加

血液：自己免疫性溶血貧血(Coombs'-positive hemolytic anemia)がありうる。白血球減少と血小板減少症は普通にみられる。

腎症状：ループス腎炎は普通に見られ、顕微鏡的血尿・タンパク尿、ネフローゼ、あるいは腎不全が現れるかもしれない。

関節症状：変形を伴わない関節痛(PIP 関節(近位指節間関節)、MP 関節(中手指節関節)、手関節)

　(第2パラグラフ)SLEの確定診断のための検査・治療

　・すぐにすべきことは降圧薬、抗痙攣薬の投与

　・確定診断のために次の検査を行っていく(もっとも、症例の提示された所見で(日本の？)SLEの診断基準を満たすけど)

　　・検疫血清検査：抗DNA 抗体、C3、C4

　　・腎生検：ループス腎炎の程度を把握

　・治療：活動性の感染がないことを確認　←　薬物療法ではステロイドや免疫抑制薬を使うため

　　・ステロイド静脈内投与、あるいはシクロホスファミドなどの細胞毒性薬(cytotoxic agents)の投与

　　・重症、治療抵抗性だったら血漿交換を行う。

■鑑別診断　頭痛/精神病的様態(psychiatric features)/痙攣

・髄膜炎、脳炎

・レクリエーショナルドラッグの中毒(例えばコカイン)

・脳腫瘍

・急性のアルコール禁断症状：振戦譫妄

・高血圧脳症

■KEYPOINT

・SLEは特に若いアフリカ系-カリブ系に普通に一般的

・SLEでは主に神経症状と精神症状をを伴って現れることがある

・白血球低下と血小板の低下はしばしばSLEを示唆する

□tonic-clonic seizure 強直間代発作

　意識消失とともに全身の随意筋に強直痙攣が生じ(強直痙攣期tonic convulsion)、次いで全身の筋の強直と弛緩とが律動的に繰り返される時期(間代痙攣期clonic convulsion)を経て、発作後もうろう状態を呈する一連の発作。

□350ml アルコール5%

350x0.05/10=1.75 unit

□細胞毒性薬

　免疫抑制薬や抗腫瘍薬として用いられる。

antimetabolites

アザチオプリン azathioprine

メトトレキセート methotrexate

ミコフェノール酸 mycophenolic acid, ミコフェノール酸モフェチル mycophenolate mofetil

レフルノミド leflunomide

alkylating agents

シクロホスファミド cyclophosphamide

「ナトリウム」

　　[★]

英: sodium, natrium, Na
関: Na+

血液(血清)中のナトリウム (臨床検査法提要第32版)

136-145 mEq/l

尿中のナトリウム

<20 mEq/l (正常と判断できる範囲)
>40 mEq/l (腎性腎不全を示唆)

Na排泄率

≦1% (臨床検査法提要第32版)

尿Na,Kと血清Naによる血清Naの予測

経口摂取と輸液による自由水の摂取がなければ

尿([Na⁺]+[K⁺])　＜　血清[Na⁺]　→　血清[Na⁺]上昇

尿([Na⁺]+[K⁺])　＝　血清[Na⁺]　→　血清[Na⁺]普遍

尿([Na⁺]+[K⁺])　＞　血清[Na⁺]　→　血清[Na⁺]低下

食品中の食塩量

ほとんどの製品ラベルに記載されている、ナトリウム[g]はそのまま食塩量[g]と考えることができないので、指導する債には注意を促す。
分子量から考えるとNa(23), Cl(35.5)なので、ナトリウムx[g]は食塩 x /23 * (23 + 35.5)、つまり2.54 * x [g]となる。

例えば、小生が常食している某社のインスタントラーメンにはナトリウム2[g]との記載があるが、これは5.08gの食塩が含まれているということになる。もちろんスープは全部飲む。1日3袋食べたことがあるのだが、、、

臨床関連

高ナトリウム血症：急激なNa補正→脳浮腫
低ナトリウム血症：急激なNa補正→橋中心髄鞘崩壊症

「flavin-adenine dinucleotide sodium」

　　[★]

フラビンアデニンジヌクレオチドナトリウム

関: FAD、flavin-adenine dinucleotide

「isotonic sodium chloride solution」

　　[★]

等張食塩水、生理食塩水

関: physiological saline、saline、saline solution

「sodium-phosphate cotransporter protein」

　　[★]

ナトリウム・リン酸共輸送体

関: sodium-phosphate cotransporter

「fluorescein sodium」

　　[★] フルオレセイン。フルオレセインナトリウム

「ceftiofur sodium」

　　[★]

セフチオフルナトリウム

[2] 炭酸水素ナトリウムを重炭酸ソーダ（重曹）と呼んだり、水酸化ナトリウムを苛性ソーダと呼ぶ。また、ナトリウム化合物を作ることから日本曹達や東洋曹達（現東ソー）などの名前の由来となっている。

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[3] 毒物及び劇物取締法昭和二十五年十二月二十八日法律三百三号第二条別表第二

[4] 近角、木越、田沼「最新元素知識」東京書籍、1976年

[5] 桜井「元素111の新知識」BLUE BACKS、講談社、1997年。 ISBN 4-06-257192-7

[6] Yanming Ma et al., "Transparent dense sodium", Nature 458, 182-185 (2009). doi:10.1038/nature07786

[7] “Sodium Metal from France”. U.S. International Trade Commission. 2012年8月4日閲覧。

[kagaku-8] 『15509の化学商品』化学工業日報社、2009年2月。ISBN 978-4-87326-544-5。

[IUPAC-1] Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights

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[Greenwood75-5] Greenwood and Earnshaw, p. 75

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v t e Sodium compounds

NaAlO₂ NaBH₄ NaBH₃(CN) NaBO₂ NaBiO₃ NaBr NaBrO NaBrO₃ NaCH₃COO NaC₆H₅CO₂ NaC₆H₄(OH)CO₂ NaCN NaCl NaClO NaClO₂ NaClO₃ NaClO₄ NaF Na₂FeO₄ NaH NaHCO₃ NaH₂PO₄ NaHSO₃ NaHSO₄ NaI NaIO₃ NaIO₄ Na₅IO₆ NaMnO₄ NaN₃ NaNH₂ NaNO₂ NaNO₃ NaOCN NaO₂ NaO₃ NaOH NaPO₂H₂ NaReO₄ NaSCN NaSH NaTcO₄ NaVO₃ Na₂CO₃ Na₂C₂O₄ Na₂CrO₄ Na₂Cr₂O₇ Na₂GeO₃ Na₂MnO₄ Na₃MnO₄ Na₂MoO₄ Na₂MoS₄ Na₂N₂O₂ Na₂O Na₂O₂ Na₂O(UO₃)₂ Na₂PO₃F Na₂S Na₂SO₃ Na₂SO₄ Na₂S₂O₃ Na₂S₂O₄ Na₂S₂O₅ Na₂S₂O₆ Na₂S₂O₇ Na₂S₂O₈ Na₂S₄O₆ Na₂Se Na₂SeO₃ Na₂SeO₄ Na₂SiO₃ Na₂Si₂O₅ Na₄SiO₄ Na₂Te Na₂TeO₃ Na₂TeO₄ Na₂Po Na₂Ti₃O₇ Na₂U₂O₇ NaWO₄ Na₂Zn(OH)₄ Na₃N Na₃P Na₃PO₄ Na₃VO₄ Na₄Fe(CN)₆ Na₄P₃O₇ Na₅P₃O₁₀

Chemical formulas

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sodium