関: Ar

WordNet

a colorless and odorless inert gas; one of the six inert gases; comprises approximately 1% of the earths atmosphere (同)Ar, atomic number 18
a pidgin incorporating Chinook and French and English words; formerly used as a lingua franca in northwestern North America (同)Oregon Jargon
geraniums native chiefly to South Africa; widely cultivated (同)genus Pelargonium
geological dating that relies on the proportions of radioactive potassium in a rock sample and its decay product, argon

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アルゴン(気体元素;化学記号は『Ar』)
argonの化学記号

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2015/07/09 15:57:10」(JST)

wiki ja

[Wiki ja表示]

アルゴン（英: argon）は原子番号18の元素で、元素記号はArである。周期表において第18族元素（希ガス）かつ第3周期元素に属す。アルゴンは地球大気中に3番目に多く含まれている気体で、その容量パーセント濃度は0.93%であり、二酸化炭素 (0.039%) より多く存在している。地球上のアルゴンのほとんどは質量数40のもの（アルゴン40）であり、これは地殻中のカリウム40の崩壊により生成した。一方、宇宙においてはアルゴン36が最も多量に存在し、超新星爆発による元素合成によりつくられた。

「アルゴン」という名はギリシャ語で「怠惰な」「不活発な」を意味する「αργον」という単語に由来する。事実、アルゴンは化学反応をほとんど起こさない元素である。最外殻電子数が8でありオクテット則を満たしているので、アルゴンは安定でほかの元素と結合しにくい。三重点は83.8058 Kであり、これは1990年国際温度目盛 (ITS-90) の定義定点に採用された。

特徴

凍結させたアルゴン

希ガスの一つ。常温、常圧で無色、無臭の気体。希ガスのため不活性である。比重は、1.65（-233 ℃: 固体）、1.39（-186 ℃: 液体）、空気に対する比重は、1.38。固体での安定構造は、面心立方構造 (FCC)。

空気中（地表）に 0.93% 含まれているのでアルゴンは空気を液化、分留して得ることができる（酸素の沸点が近いので、これとの分離が少々面倒）。

希ガスの中では最も空気中での存在比が大きく、乾燥空気を構成する物質では第2位の酸素の 20.93% についで第3位の 0.93% である。空気中のアルゴンの存在比が希ガス中最も大きいのは、自然界すなわち岩石中に存在していたカリウム40の一部 (11%) が電子捕獲によってアルゴン40となったためである。このため地球および火星など岩石惑星大気中ではアルゴン40の同位体比が圧倒的に大きいのに対し、太陽大気中ではアルゴン36の同位体が大部分を占める^[2]。第4位は二酸化炭素だが、2008年現在得られる資料では 0.038% であり3位との差は大きい。

電気を通すとスカイブルーの光を放つ。

用途

アルゴンは、水銀灯、蛍光灯、電球、真空管等の封入ガス、アルゴンレーザー、アーク溶接時の保護ガス、チタン精練、チタン入りろう材による加工、食品の酸化防止のための充填ガスなどに利用される。
分析化学の分野ではICP（誘導結合プラズマ）のプラズマ用ガスや、ガスクロマトグラフィーを行う際の移動相として利用する。
テクニカルダイビングにおいて、ドライスーツ用ガスや混合ガスとして使用される。
岩石の年代測定にカリウム・アルゴン (K-Ar) 法として用いられ、岩石が最後の加熱を受けてからの年代を求める事が出来る。数千万年前から数十億年前という幅広い年代の推定が可能。

アルゴンの2004年度日本国内生産量は219,461 km³、工業消費量は38,348 km³である。近年の需要に対応して、2005年に日本工業規格 (JIS K 1105) が改正され、純度が高められた。

歴史

1892年にレイリー卿（ジョン・ウィリアム・ストラット）が大気分析の過程で未知の気体に気づき、1894年にウィリアム・ラムゼーと共にその正体がアルゴンであることを突き止めた^[3]。しかし、その100年も前に、ヘンリー・キャヴェンディッシュが存在に気がついていたと言われている。なお、1904年にレイリー卿は「気体の密度に関する研究、およびこの研究により成されたアルゴンの発見」によりノーベル物理学賞を、ウィリアム・ラムゼーは「空気中の希ガス元素の発見と周期律におけるその位置の決定」によりノーベル化学賞を、それぞれ授与された。

アルゴンという名称はギリシャ語で「不活発、不活性」という意味の「αργόν」に由来する。「働く」という意味の「εργον」に「αν」をつけた「αν εργον」（働かない）が語源とする説もある。また、ギリシャ語で「怠け者」という意味の「αργος」が語源とする説もある。

化合物

アルゴンは単原子でオクテット則を満たしていることから、他の原子と結合した化合物は長い間知られていなかった。2000年、フィンランドの研究者により初のアルゴン化合物、アルゴンフッ素水素化物 (HArF) の合成が発表された。これは、アルゴンとフッ化水素、ヨウ化セシウムを混合して 7.5 K で紫外線照射することにより合成された^[4]。

同位体

詳細は「アルゴンの同位体」を参照

出典

^ Magnetic susceptibility of the elements and inorganic compounds, in Handbook of Chemistry and Physics 81st edition, CRC press.
^ 小嶋稔　『地球物理概論』　東京大学出版会、1990年
^ 桜井弘『元素111の新知識』講談社、1998年、109頁。ISBN 4-06-257192-7。
^ Khriachtchev, L.; Pettersson, M.; Runeberg, N.; Lundell, J.; Räsänen, M. Nature, 2000, 406, 874-876. DOI: 10.1038/35022551

外部リンク

岩石の年代測定カリウム・アルゴン法 40Ar/39Arの解析

ウィキメディア・コモンズには、アルゴンに関連するメディアがあります。

wiki en

[Wiki en表示]

Argon is a chemical element with symbol Ar and atomic number 18. It is in group 18 of the periodic table and is a noble gas.^[5] Argon is the third most common gas in the Earth's atmosphere, at 0.93% (9,300 ppm), making it approximately 23.7 times as abundant as the next most common atmospheric gas, carbon dioxide (390 ppm), and more than 500 times as abundant as the next most common noble gas, neon (18 ppm). Nearly all of this argon is radiogenic argon-40 derived from the decay of potassium-40 in the Earth's crust. In the universe, argon-36 is by far the most common argon isotope, being the preferred argon isotope produced by stellar nucleosynthesis in supernovas. In addition, argon is the most prevalent of the noble gases in Earth's crust, with the element composing 0.00015% of this crust.^[6]

The name "argon" is derived from the Greek word αργον, neuter singular form of αργος meaning "lazy" or "inactive", as a reference to the fact that the element undergoes almost no chemical reactions. The complete octet (eight electrons) in the outer atomic shell makes argon stable and resistant to bonding with other elements. Its triple point temperature of 83.8058 K is a defining fixed point in the International Temperature Scale of 1990.

Argon is produced industrially by the fractional distillation of liquid air. Argon is mostly used as an inert shielding gas in welding and other high-temperature industrial processes where ordinarily non-reactive substances become reactive; for example, an argon atmosphere is used in graphite electric furnaces to prevent the graphite from burning. Argon gas also has uses in incandescent and fluorescent lighting, and other types of gas discharge tubes. Argon makes a distinctive blue-green gas laser. Argon is also used in fluorescent glow starters.

1 Characteristics
2 History
3 Occurrence
4 Isotopes
5 Compounds
6 Production
- 6.1 Industrial
- 6.2 In radioactive decays
7 Applications
- 7.1 Industrial processes
- 7.2 Scientific research
- 7.3 Preservative
- 7.4 Laboratory equipment
- 7.5 Medical use
- 7.6 Lighting
- 7.7 Miscellaneous uses
8 Safety
9 See also
10 References
11 Further reading
12 External links

Characteristics

A small piece of rapidly melting solid argon.

Argon has approximately the same solubility in water as oxygen, and is 2.5 times more soluble in water than nitrogen. Argon is colorless, odorless, nonflammable and nontoxic as a solid, liquid, and gas.^[7] Argon is chemically inert under most conditions and forms no confirmed stable compounds at room temperature.

Although argon is a noble gas, it has been found to have the capability of forming some compounds. For example, the creation of argon fluorohydride (HArF), a compound of argon with fluorine and hydrogen which is stable below 17 K, was reported by researchers at the University of Helsinki in 2000.^[8]^[9] Although the neutral ground-state chemical compounds of argon are presently limited to HArF, argon can form clathrates with water when atoms of it are trapped in a lattice of the water molecules.^[10] Argon-containing ions and excited state complexes, such as ArH+
and ArF, respectively, are known to exist. Theoretical calculations have predicted several argon compounds that should be stable,^[11] but for which no synthesis routes are currently known.

History

Lord Rayleigh's method for the isolation of argon, based on an experiment of Henry Cavendish's. The gases are contained in a test-tube (A) standing over a large quantity of weak alkali (B), and the current is conveyed in wires insulated by U-shaped glass tubes (CC) passing through the liquid and round the mouth of the test-tube. The inner platinum ends (DD) of the wire receive a current from a battery of five Grove cells and a Ruhmkorff coil of medium size.

Argon (’αργόν, neuter singular form of ’αργός, Greek meaning "inactive", in reference to its chemical inactivity)^[12]^[13] was suspected to be present in air by Henry Cavendish in 1785 but was not isolated until 1894 by Lord Rayleigh and Sir William Ramsay at University College London in an experiment in which they removed all of the oxygen, carbon dioxide, water and nitrogen from a sample of clean air.^[14]^[15]^[16] They had determined that nitrogen produced from chemical compounds was one-half percent lighter than nitrogen from the atmosphere. The difference seemed insignificant, but it was important enough to attract their attention for many months. They concluded that there was another gas in the air mixed in with the nitrogen.^[17] Argon was also encountered in 1882 through independent research of H. F. Newall and W. N. Hartley. Each observed new lines in the color spectrum of air but were unable to identify the element responsible for the lines. Argon became the first member of the noble gases to be discovered. The symbol for argon is now "Ar", but up until 1957 it was "A".^[18]

Occurrence

Argon constitutes 0.934% by volume and 1.288% by mass of the Earth's atmosphere,^[19] and air is the primary raw material used by industry to produce purified argon products. Argon is isolated from air by fractionation, most commonly by cryogenic fractional distillation, a process that also produces purified nitrogen, oxygen, neon, krypton and xenon.^[20] The Earth's crust and seawater contain 1.2 ppm and 0.45 ppm of argon, respectively.^[21]

Isotopes

The main isotopes of argon found on Earth are 40
Ar (99.6%), 36
Ar (0.34%), and 38
Ar (0.06%). Naturally occurring 40
K, with a half-life of 1.25×10⁹ years, decays to stable 40
Ar (11.2%) by electron capture or positron emission, and also to stable 40
Ca (88.8%) via beta decay. These properties and ratios are used to determine the age of rocks by the method of K-Ar dating.^[21]^[22]

In the Earth's atmosphere, 39
Ar is made by cosmic ray activity, primarily with 40
Ar. In the subsurface environment, it is also produced through neutron capture by 39
K or alpha emission by calcium. 37
Ar is created from the neutron spallation of 40
Ca as a result of subsurface nuclear explosions. It has a half-life of 35 days.^[22]

Argon is notable in that its isotopic composition varies greatly between different locations in the Solar System. Where the major source of argon is the decay of 40
K in rocks, 40
Ar will be the dominant isotope, as it is on Earth. Argon produced directly by stellar nucleosynthesis, in contrast, is dominated by the alpha process nuclide, 36
Ar. Correspondingly, solar argon contains 84.6% 36
Ar based on solar wind measurements,^[23] and the ratio of the three isotopes ³⁶Ar : ³⁸Ar : ⁴⁰Ar in the atmospheres of the outer planets is measured to be 8400 : 1600 : 1.^[24] This contrasts with the abundance of primordial 36
Ar in Earth's atmosphere: only 31.5 ppmv (= 9340 ppmv × 0.337%), comparable to that of neon (18.18 ppmv); and with measurements by interplanetary probes.

The Martian atmosphere contains 1.6% of 40
Ar and 5 ppm of 36
Ar. The Mariner probe fly-by of the planet Mercury in 1973 found that Mercury has a very thin atmosphere with 70% argon, believed to result from releases of the gas as a decay product from radioactive materials on the planet. In 2005, the Huygens probe discovered the presence of exclusively 40
Ar on Titan, the largest moon of Saturn.^[21]^[25]

The predominance of radiogenic 40
Ar is responsible for the standard atomic weight of terrestrial argon being greater than that of the next element, potassium, which was puzzling at the time when argon was discovered. Mendeleev had placed the elements in his periodic table in order of atomic weight, but the inertness of argon suggested a placement before the reactive alkali metal. Henry Moseley later solved this problem by showing that the periodic table is actually arranged in order of atomic number. (See History of the periodic table).

Compounds

Space-filling model of argon fluorohydride.

Argon's complete octet of electrons indicates full s and p subshells. This full outer energy level makes argon very stable and extremely resistant to bonding with other elements. Before 1962, argon and the other noble gases were considered to be chemically inert and unable to form compounds; however, compounds of the heavier noble gases have since been synthesized. In August 2000, the first argon compound was formed by researchers at the University of Helsinki. By shining ultraviolet light onto frozen argon containing a small amount of hydrogen fluoride with caesium iodide,^[26] argon fluorohydride (HArF) was formed.^[9]^[27] It is stable up to 40 kelvin (−233 °C). The metastable ArCF2+
2 dication, which is valence isoelectronic with carbonyl fluoride, was observed in 2010.^[28] Argon-36, in the form of argon hydride ions, has been detected in cosmic dust associated with the Crab Nebula supernova; this was the first noble-gas molecule detected in outer space.^[29]^[30]

Production

Industrial

Argon is produced industrially by the fractional distillation of liquid air in a cryogenic air separation unit; a process that separates liquid nitrogen, which boils at 77.3 K, from argon, which boils at 87.3 K, and liquid oxygen, which boils at 90.2 K. About 700,000 tonnes of argon are produced worldwide every year.^[21]^[31]

In radioactive decays

⁴⁰Ar, the most abundant isotope of argon, is produced by the decay of ⁴⁰K with a half-life of 1.25×10⁹ years by electron capture or positron emission. Because of this, it is used in potassium-argon dating to determine the age of rocks.

Applications

Cylinders containing argon gas for use in extinguishing fire without damaging server equipment

There are several different reasons argon is used in particular applications:

An inert gas is needed. In particular, argon is the cheapest alternative when nitrogen is not sufficiently inert.
Low thermal conductivity is required.
The electronic properties (ionization and/or the emission spectrum) are necessary.

Other noble gases would probably work as well in most of these applications, but argon is by far the cheapest. Argon is inexpensive since it occurs naturally in air, and is readily obtained as a byproduct of cryogenic air separation in the production of liquid oxygen and liquid nitrogen: the primary constituents of air are used on a large industrial scale. The other noble gases (except helium) are produced this way as well, but argon is the most plentiful by far. The bulk of argon applications arise simply because it is inert and relatively cheap.

Industrial processes

Argon is used in some high-temperature industrial processes, where ordinarily non-reactive substances become reactive. For example, an argon atmosphere is used in graphite electric furnaces to prevent the graphite from burning.

For some of these processes, the presence of nitrogen or oxygen gases might cause defects within the material. Argon is used in various types of arc welding such as gas metal arc welding and gas tungsten arc welding, as well as in the processing of titanium and other reactive elements. An argon atmosphere is also used for growing crystals of silicon and germanium.

Argon is used in the poultry industry to asphyxiate birds, either for mass culling following disease outbreaks, or as a means of slaughter more humane than the electric bath. Argon's relatively high density causes it to remain close to the ground during gassing. Its non-reactive nature makes it suitable in a food product, and since it replaces oxygen within the dead bird, argon also enhances shelf life.^{[citation needed]}^[32]

Argon is sometimes used for extinguishing fires where damage to equipment is to be avoided.

Scientific research

Liquid argon is used as the target for neutrino experiments and direct dark matter searches. The interaction of a hypothetical WIMP particle with the argon nucleus produces scintillation light that is detected by photomultiplier tubes. Two-phase detectors also use argon gas to detect the ionized electrons produced during the WIMP-nucleus scattering. As with most other liquefied noble gases, argon has a high scintillation lightyield (~ 51 photons/keV^[33]), is transparent to its own scintillation light, and is relatively easy to purify. Compared to xenon, argon is cheaper and has a distinct scintillation time profile which allows the separation of electronic recoils from nuclear recoils. On the other hand, its intrinsic beta-ray background is larger due to 39
Ar contamination, unless one uses underground argon sources which has much less 39
Ar contamination. Most of the argon in the Earth’s atmosphere was produced by electron capture of long-lived 40
K (40
K + e− → 40
Ar + ν) present in natural potassium within the earth. The 39
Ar activity in the atmosphere is maintained by cosmogenic production through 40
Ar(n,2n)39
Ar and similar reactions. The half-life of 39
Ar is only 269 yr. As a result, the underground Ar, shielded by rock and water, has much less 39
Ar contamination.^[34] Dark matter detectors currently operating with liquid argon include DarkSide, WArP, ArDM, microCLEAN and DEAP-I. Neutrino experiments include Icarus and MicroBooNE both of which use high purity liquid argon in a time projection chamber for fine grained three-dimensional imaging of neutrino interactions.

Preservative

A sample of caesium is packed under argon to avoid reactions with air

Argon is used to displace oxygen- and moisture-containing air in packaging material to extend the shelf-lives of the contents (argon has the European food additive code of E938). Aerial oxidation, hydrolysis, and other chemical reactions which degrade the products are retarded or prevented entirely. Bottles of high-purity chemicals and certain pharmaceutical products are available in sealed bottles or ampoules packed in argon.

In winemaking, argon is used in a variety of activities to provide a barrier against oxygen at the liquid's surface, which can spoil wine by fueling both microbial metabolism (such as with acetic acid bacteria) and standard redox chemistry.

Argon is also available in aerosol-type cans, which may be used to preserve compounds such as varnish, polyurethane, paint, etc. for storage after opening.^[35]

Since 2002, the American National Archives stores important national documents such as the Declaration of Independence and the Constitution within argon-filled cases to retard their degradation. Using argon reduces gas leakage, compared with the helium used in the preceding five decades.^[36]

Laboratory equipment

Gloveboxes are often filled with argon, which recirculates over scrubbers to maintain an oxygen-, nitrogen-, and moisture-free atmosphere

Argon may be used as the inert gas within Schlenk lines and gloveboxes. The use of argon over comparatively less expensive nitrogen is preferred where nitrogen may react with the experimental reagents or apparatus.

Argon may be used as the carrier gas in gas chromatography and in electrospray ionization mass spectrometry; it is the gas of choice for the plasma used in ICP spectroscopy. Argon is preferred for the sputter coating of specimens for scanning electron microscopy. Argon gas is also commonly used for sputter deposition of thin films as in microelectronics and for wafer cleaning in microfabrication.

Medical use

Cryosurgery procedures such as cryoablation use liquefied argon to destroy tissue such as cancer cells. In surgery it is used in a procedure called "argon enhanced coagulation" which is a form of argon plasma beam electrosurgery. The procedure carries a risk of producing gas embolism in the patient and has resulted in the death of one person via this type of accident.^[37]

Blue argon lasers are used in surgery to weld arteries, destroy tumors, and to correct eye defects.^[21]

Argon has also been used experimentally to replace nitrogen in the breathing or decompression mix known as Argox, to speed the elimination of dissolved nitrogen from the blood.^[38]

Lighting

Argon gas-discharge lamp forming the symbol for argon "Ar".

Incandescent lights are filled with argon, to preserve the filaments at high temperature from oxidation. It is used for the specific way it ionizes and emits light, such as in plasma globes and calorimetry in experimental particle physics. Gas-discharge lamps filled with pure argon provide lilac/violet light, filled with argon and some mercury blue light. Argon is also used for the creation of blue and green laser light.

Miscellaneous uses

Argon is used for thermal insulation in energy efficient windows.^[39] Argon is also used in technical scuba diving to inflate a dry suit, because it is inert and has low thermal conductivity.^[40] Argon is being used as a propellant in the development of the Variable Specific Impulse Magnetoplasma Rocket (VASIMR). Compressed argon gas is allowed to expand, to cool the seeker heads of the AIM-9 Sidewinder missile, and other missiles that use cooled thermal seeker heads. The gas is stored at high pressure.^[41]

Argon-39, with a half-life of 269 years, has been used for a number of applications, primarily ice core and ground water dating. Also, potassium-argon dating is used in dating igneous rocks.^[21]

Argon has been used by athletes as a doping agent to simulate hypoxic conditions. On August 31, 2014 the World Anti Doping Agency (WADA) added argon and xenon to the list of prohibited substances and methods, although at this time there is no reliable test for abuse.^[42]

Safety

Although argon is non-toxic, it is 38% denser than air and is therefore considered a dangerous asphyxiant in closed areas. It is also difficult to detect because it is colorless, odorless, and tasteless. A 1994 incident in which a man was asphyxiated after entering an argon-filled section of oil pipe under construction in Alaska highlights the dangers of argon tank leakage in confined spaces, and emphasizes the need for proper use, storage and handling.^[43]

References

^ Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights
^ ^a ^b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.121. ISBN 1439855110.
^ Shuen-Chen Hwang, Robert D. Lein, Daniel A. Morgan (2005). "Noble Gases". Kirk Othmer Encyclopedia of Chemical Technology. Wiley. pp. 343–383. doi:10.1002/0471238961.0701190508230114.a01.
^ Magnetic susceptibility of the elements and inorganic compounds, in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
^ In older versions of the periodic table, the noble gases were identified as Group VIIIA or as Group 0. See Group (periodic table).
^ http://www.ptable.com/#Property/Abundance/Crust
^ Material Safety Data Sheet Gaseous Argon, Universal Industrial Gases, Inc. Retrieved 14 October 2013.
^ Leonid Khriachtchev; Mika Pettersson; Nino Runeberg; Jan Lundell et al. (2000). "A stable argon compound". Nature 406: 874–876. doi:10.1038/35022551. PMID 10972285.
^ ^a ^b Perkins, S. (26 August 2000). "HArF! Argon's not so noble after all – researchers make argon fluorohydride". Science News.
^ Belosludov, V. R.; Subbotin, O. S.; Krupskii, D. S.; Prokuda, O. V. et al. (2006). "Microscopic model of clathrate compounds". Journal of Physics: Conference Series 29: 1. Bibcode:2006JPhCS..29....1B. doi:10.1088/1742-6596/29/1/001.
^ Cohen, A.; Lundell, J.; Gerber, R. B. (2003). "First compounds with argon–carbon and argon–silicon chemical bonds". Journal of Chemical Physics 119 (13): 6415. Bibcode:2003JChPh.119.6415C. doi:10.1063/1.1613631.
^ Hiebert, E. N. (1963). "In Noble-Gas Compounds". In Hyman, H. H. Historical Remarks on the Discovery of Argon: The First Noble Gas. University of Chicago Press. pp. 3–20.
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^ Lord Rayleigh; Ramsay, William (1894–1895). "Argon, a New Constituent of the Atmosphere". Proceedings of the Royal Society 57 (1): 265–287. doi:10.1098/rspl.1894.0149. JSTOR 115394.
^ Lord Rayleigh; Ramsay, William (1895). "VI. Argon: A New Constituent of the Atmosphere". Philosophical Transactions of the Royal Society A 186: 187. Bibcode:1895RSPTA.186..187R. doi:10.1098/rsta.1895.0006. JSTOR 90645.
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^ "Encyclopædia Britannica Online, s.v. "argon (Ar)"". Retrieved 14 January 2014.
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^ ^a ^b ^c ^d ^e ^f Emsley, J. (2001). Nature's Building Blocks. Oxford University Press. pp. 44–45. ISBN 978-0-19-960563-7.
^ ^a ^b "⁴⁰Ar/³⁹Ar dating and errors". Archived from the original on 9 May 2007. Retrieved 7 March 2007.
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^ Barlow, M. J. et al. (2013). "Detection of a Noble Gas Molecular Ion, ³⁶ArH⁺, in the Crab Nebula". Science 342 (6164): 1343–1345. arXiv:1312.4843. Bibcode:2013Sci...342.1343B. doi:10.1126/science.1243582.
^ Quenqua, Douglas (13 December 2013). "Noble Molecules Found in Space". New York Times. Retrieved 13 December 2013.
^ "Periodic Table of Elements: Argon – Ar". Environmentalchemistry.com. Retrieved 12 September 2008.
^ Fletcher, D. L. "Slaughter Technology" (PDF). Symposium: Recent Advances in Poultry Slaughter Technology. Retrieved 1 January 2010.
^ Gastler, Dan; Kearns, Ed; Hime, Andrew; Stonehill, Laura C. et al. (2012). "Measurement of scintillation efficiency for nuclear recoils in liquid argon". Physical Review C 85 (6). arXiv:1004.0373. Bibcode:2012PhRvC..85f5811G. doi:10.1103/PhysRevC.85.065811.
^ Xu, J.; Calaprice, F.; Galbiati, C.; Goretti, A.; Guray, G. et al. (2012). "A Study of the Residual 39Ar Content in Argon from Underground Sources". arXiv:1204.6011v1.
^ Zawalick, Steven Scott "Method for preserving an oxygen sensitive liquid product" U.S. Patent 6,629,402 Issue date: 7 October 2003
^ "Schedule for Renovation of the National Archives Building". Retrieved 7 July 2009.
^ "Fatal Gas Embolism Caused by Overpressurization during Laparoscopic Use of Argon Enhanced Coagulation". MDSR. 24 June 1994.
^ Pilmanis Andrew A; Balldin UI; Webb James T; Krause KM (2003). "Staged decompression to 3.5 psi using argon-oxygen and 100% oxygen breathing mixtures". Aviation, Space, Environmental Medicine 74 (12): 1243–50. PMID 14692466.
^ "Energy-Efficient Windows". FineHomebuilding.com. Retrieved 1 August 2009.
^ Nuckols ML; Giblo J; Wood-Putnam JL (15–18 September 2008). "Thermal Characteristics of Diving Garments When Using Argon as a Suit Inflation Gas". Proceedings of the Oceans 08 MTS/IEEE Quebec, Canada Meeting (MTS/IEEE). Retrieved 2 March 2009.
^ "Description of Aim-9 Operation". planken.org. Archived from the original on 22 December 2008. Retrieved 1 February 2009.
^ "WADA amends Section S.2.1 of 2014 Prohibited List". 31 August 2014.
^ Alaska FACE Investigation 94AK012 (23 June 1994). "Welder's Helper Asphyxiated in Argon-Inerted Pipe – Alaska (FACE AK-94-012)". State of Alaska Department of Public Health. Retrieved 29 January 2011.

External links

Silicon at The Periodic Table of Videos (University of Nottingham)
USGS Periodic Table – Argon
Diving applications: Why Argon?

UpToDate Contents

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1. Bronchoscopic argon plasma coagulation in the management of airway disease in adults
2. 消化管出血のマネージメントにおけるアルゴンプラズマ凝固法 argon plasma coagulation in the management of gastrointestinal hemorrhage
3. 食道表在癌のマネージメント management of superficial esophageal cancer
4. Clinical presentation, diagnostic evaluation, and management of central airway obstruction in adults
5. 消化管の血管異形成 angiodysplasia of the gastrointestinal tract

English Journal

Influence of dissolved gases on sonochemistry and sonoluminescence in a flow reactor.

Gielen B1, Marchal S2, Jordens J1, Thomassen LC1, Braeken L1, Van Gerven T3.
Ultrasonics sonochemistry.Ultrason Sonochem.2016 Jul;31:463-72. doi: 10.1016/j.ultsonch.2016.02.001. Epub 2016 Feb 2.
In the present work, the influence of gas addition is investigated on both sonoluminescence (SL) and radical formation at 47 and 248kHz. The frequencies chosen in this study generate two distinct bubble types, allowing to generalize the conclusions for other ultrasonic reactors. In this case, 47kHz
PMID 26964973

Structural analysis of the outermost hair surface using TOF-SIMS with gas cluster ion beam sputtering.

Lshikawa K1, Okamoto M1, Aoyagi S2.
Biointerphases.Biointerphases.2016 Jun 28;11(2):02A315. doi: 10.1116/1.4940770.
A hair cuticle, which consists of flat overlapping scales that surround the hair fiber, protects inner tissues against external stimuli. The outermost surface of the cuticle is covered with a thin membrane containing proteins and lipids called the epicuticle. In a previous study, the authors conduct
PMID 26822506

Improved mass resolution and mass accuracy in TOF-SIMS spectra and images using argon gas cluster ion beams.

Shon HK1, Yoon S1, Moon JH2, Lee TG3.
Biointerphases.Biointerphases.2016 Jun 9;11(2):02A321. doi: 10.1116/1.4941447.
The popularity of argon gas cluster ion beams (Ar-GCIB) as primary ion beams in time-of-flight secondary ion mass spectrometry (TOF-SIMS) has increased because the molecular ions of large organic- and biomolecules can be detected with less damage to the sample surfaces. However, Ar-GCIB is limited b
PMID 26861497

Correlation between porous texture and cell seeding efficiency of gas foaming and microfluidic foaming scaffolds.

Costantini M1, Colosi C2, Mozetic P3, Jaroszewicz J4, Tosato A2, Rainer A3, Trombetta M3, Święszkowski W4, Dentini M2, Barbetta A5.
Materials science & engineering. C, Materials for biological applications.Mater Sci Eng C Mater Biol Appl.2016 May 1;62:668-77. doi: 10.1016/j.msec.2016.02.010. Epub 2016 Feb 5.
In the design of scaffolds for tissue engineering applications, morphological parameters such as pore size, shape, and interconnectivity, as well as transport properties, should always be tailored in view of their clinical application. In this work, we demonstrate that a regular and ordered porous t
PMID 26952471

Japanese Journal

Perturber Dependence of Disalignment Cross Sections of the Argon 2p Atoms Measured at Temperatures between 77 and 295K

MATSUKUMA Hiraku,TANAKA Hirotaka,TAKAIE Yukihiro [他]
Journal of the Physical Society of Japan 81(11), 114302-1-7, 2012-11
NAID 40019484212

Effect of capacitive coupling in a miniature inductively coupled plasma source

Takao Yoshinori,Eriguchi Koji,Ono Kouichi
Journal of Applied Physics 112(9), 2012-11
… The mICP is 3 mm in radius and 6 mm in height with a three-turn planar coil, where argon plasma is sustained. …
NAID 120004920433

症例アルゴンプラズマ凝固療法に耐性であった幽門輪発赤を伴うびまん性胃前庭部毛細血管拡張症の1例

久保秀文,西山光郎,多田耕輔 [他]
外科 74(9), 1000-1002, 2012-09
NAID 40019418757

Fuel hydrogen retention of tungsten and the reduction by inert gas glow discharges

Hino T.,Yamauchi Y.,Kimura Y.,Nishimura K.,Ueda Y.
Fusion Engineering and Design 87(5-6), 876-879, 2012-08
Polycrystalline tungsten was exposed to deuterium glow discharge followed by He, Ne or Ar glow discharge. The amount of retained deuterium in the tungsten was measured using residual gas analysis. The …
NAID 120004979567

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拡張検索	「Pelargonium属」「Pelargonium」

「Pelargonium属」

Argon, ₁₈Ar
	Spectral lines of argon
General properties
Name, symbol	argon, Ar
Pronunciation	/ˈɑrɡɒn/; AR-gon
Appearance	colorless gas exhibiting a lilac/violet glow when placed in a high voltage electric field
Argon in the periodic table
	chlorine ← argon → potassium
Atomic number	18
Standard atomic weight (±) (Ar)	39.948(1)
Element category	noble gas
Group, block	group 18 (noble gases), p-block
Period	period 3
Electron configuration	[Ne] 3s2 3p6
per shell	2, 8, 8
Physical properties
Phase	gas
Melting point	83.81 K (−189.34 °C, −308.81 °F)
Boiling point	87.302 K (−185.848 °C, −302.526 °F)
Density at stp (0 °C and 101.325 kPa)	1.784 g·L−1
when liquid, at b.p.	1.3954 g·cm−3
Triple point	83.8058 K, 68.89 kPa
Critical point	150.687 K, 4.863 MPa
Heat of fusion	1.18 kJ·mol−1
Heat of vaporization	6.53 kJ·mol−1
Molar heat capacity	20.85 J·mol−1·K−1
Atomic properties
Oxidation states	0
Electronegativity	Pauling scale: no data
Ionization energies	1st: 1520.6 kJ·mol−1; 2nd: 2665.8 kJ·mol−1; 3rd: 3931 kJ·mol−1; (more)
Covalent radius	106±10 pm
Van der Waals radius	188 pm
Miscellanea
Crystal structure	face-centered cubic (fcc)
Speed of sound	323 m·s−1 (gas, at 27 °C)
Thermal conductivity	17.72×10−3 W·m−1·K−1
Magnetic ordering	diamagnetic
CAS Registry Number	7440–37–1
History
Discovery and first isolation	Lord Rayleigh and William Ramsay (1894)
Most stable isotopes
	Main article: Isotopes of argon
	Decay modes in parentheses are predicted, but have not yet been observed
	view; talk; edit; · references

外見
	無色の気体。高圧電場下に置かれるとライラック（紫）色の光を発する。; ; ; アルゴンのスペクトル線
一般特性
名称, 記号, 番号	アルゴン, Ar, 18
分類	希ガス
族, 周期, ブロック	18, 3, p
原子量	39.948(1)
電子配置	[Ne] 3s2 3p6
電子殻	2, 8, 8（画像）
物理特性
相	気体
密度	(0 °C, 101.325 kPa); 1.784 g/L
融点	83.80 K, −189.35 °C, −308.83 °F
沸点	87.30 K, −185.85 °C, −302.53 °F
三重点	83.8058 K (-189°C), 69 kPa
臨界点	150.87 K, 4.898 MPa
融解熱	1.18 kJ·mol-1
蒸発熱	6.43 kJ·mol-1
熱容量	(25 °C) 5R/2=20.786 J·mol-1·K-1
蒸気圧
原子特性
酸化数	0
電気陰性度	no data（ポーリングの値）
イオン化エネルギー; （詳細）	第1： 1520.6 kJ·mol-1
	第2： 2665.8 kJ·mol-1
	第3： 3931 kJ·mol-1
共有結合半径	106±10 pm
ファンデルワールス半径	188 pm
その他
結晶構造	面心立方構造
磁性	反磁性
熱伝導率	(300 K) 17.72x10-3 W·m-1·K-1
音の伝わる速さ	(気体, 27 °C) 323 m/s
CAS登録番号	7440–37–1
最安定同位体
	詳細はアルゴンの同位体を参照
	表示

　　[★]

ラ: Pelargonium
関: ペラルゴニウム属

「Pelargonium」

　　[★]

ペラルゴニウム属、Pelargonium属　

[1] Magnetic susceptibility of the elements and inorganic compounds, in Handbook of Chemistry and Physics 81st edition, CRC press.

[kojima-2] 小嶋稔　『地球物理概論』　東京大学出版会、1990年

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

[b92-2] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.121. ISBN 1439855110.

[3] Shuen-Chen Hwang, Robert D. Lein, Daniel A. Morgan (2005). "Noble Gases". Kirk Othmer Encyclopedia of Chemical Technology. Wiley. pp. 343–383. doi:10.1002/0471238961.0701190508230114.a01.

[4] Magnetic susceptibility of the elements and inorganic compounds, in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.

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[findarticles-harf-9] Perkins, S. (26 August 2000). "HArF! Argon's not so noble after all – researchers make argon fluorohydride". Science News.

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[lazyone1-12] Hiebert, E. N. (1963). "In Noble-Gas Compounds". In Hyman, H. H. Historical Remarks on the Discovery of Argon: The First Noble Gas. University of Chicago Press. pp. 3–20.

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[lazyone3-15] Lord Rayleigh; Ramsay, William (1895). "VI. Argon: A New Constituent of the Atmosphere". Philosophical Transactions of the Royal Society A 186: 187. Bibcode:1895RSPTA.186..187R. doi:10.1098/rsta.1895.0006. JSTOR 90645.

[16] Ramsay, W. (1904). "Nobel Lecture". The Nobel Foundation.

[17] "About Argon, the Inert; The New Element Supposedly Found in the Atmosphere". The New York Times. 3 March 1895. Retrieved 1 February 2009.

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[emsley-21] ^ ^a ^b ^c ^d ^e ^f Emsley, J. (2001). Nature's Building Blocks. Oxford University Press. pp. 44–45. ISBN 978-0-19-960563-7.

[iso-22] "⁴⁰Ar/³⁹Ar dating and errors". Archived from the original on 9 May 2007. Retrieved 7 March 2007.

[23] Lodders, K. (2008). "The solar argon abundance". Astrophysical Journal 674: 607. arXiv:0710.4523. Bibcode:2008ApJ...674..607L. doi:10.1086/524725.

[24] Cameron, A. G. W. (1973). "Elemental and isotopic abundances of the volatile elements in the outer planets". Space Science Reviews 14 (3–4): 392–400. doi:10.1007/BF00214750. edit

[25] "Seeing, touching and smelling the extraordinarily Earth-like world of Titan". European Space Agency. 21 January 2005.

[26] Kean, Sam (2011). "Chemistry Way, Way Below Zero". The Disappearing Spoon. Black Bay Books.

[27] Bartlett, Neil (8 September 2003). "The Noble Gases". Chemical & Engineering News 81 (36).

[28] Lockyear, JF; Douglas, K; Price, SD; Karwowska, M et al. (2010). "Generation of the ArCF₂²⁺ Dication". Journal of Physical Chemistry Letters 1: 358. doi:10.1021/jz900274p.

[29] Barlow, M. J. et al. (2013). "Detection of a Noble Gas Molecular Ion, ³⁶ArH⁺, in the Crab Nebula". Science 342 (6164): 1343–1345. arXiv:1312.4843. Bibcode:2013Sci...342.1343B. doi:10.1126/science.1243582.

[NYT-20131213-30] Quenqua, Douglas (13 December 2013). "Noble Molecules Found in Space". New York Times. Retrieved 13 December 2013.

[31] "Periodic Table of Elements: Argon – Ar". Environmentalchemistry.com. Retrieved 12 September 2008.

[32] Fletcher, D. L. "Slaughter Technology" (PDF). Symposium: Recent Advances in Poultry Slaughter Technology. Retrieved 1 January 2010.

[33] Gastler, Dan; Kearns, Ed; Hime, Andrew; Stonehill, Laura C. et al. (2012). "Measurement of scintillation efficiency for nuclear recoils in liquid argon". Physical Review C 85 (6). arXiv:1004.0373. Bibcode:2012PhRvC..85f5811G. doi:10.1103/PhysRevC.85.065811.

[34] Xu, J.; Calaprice, F.; Galbiati, C.; Goretti, A.; Guray, G. et al. (2012). "A Study of the Residual 39Ar Content in Argon from Underground Sources". arXiv:1204.6011v1.

[35] Zawalick, Steven Scott "Method for preserving an oxygen sensitive liquid product" U.S. Patent 6,629,402 Issue date: 7 October 2003

[36] "Schedule for Renovation of the National Archives Building". Retrieved 7 July 2009.

[37] "Fatal Gas Embolism Caused by Overpressurization during Laparoscopic Use of Argon Enhanced Coagulation". MDSR. 24 June 1994.

[38] Pilmanis Andrew A; Balldin UI; Webb James T; Krause KM (2003). "Staged decompression to 3.5 psi using argon-oxygen and 100% oxygen breathing mixtures". Aviation, Space, Environmental Medicine 74 (12): 1243–50. PMID 14692466.

[39] "Energy-Efficient Windows". FineHomebuilding.com. Retrieved 1 August 2009.

[IEEE2008-40] Nuckols ML; Giblo J; Wood-Putnam JL (15–18 September 2008). "Thermal Characteristics of Diving Garments When Using Argon as a Suit Inflation Gas". Proceedings of the Oceans 08 MTS/IEEE Quebec, Canada Meeting (MTS/IEEE). Retrieved 2 March 2009.

[41] "Description of Aim-9 Operation". planken.org. Archived from the original on 22 December 2008. Retrieved 1 February 2009.

[42] "WADA amends Section S.2.1 of 2014 Prohibited List". 31 August 2014.

[43] Alaska FACE Investigation 94AK012 (23 June 1994). "Welder's Helper Asphyxiated in Argon-Inerted Pipe – Alaska (FACE AK-94-012)". State of Alaska Department of Public Health. Retrieved 29 January 2011.

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