Magnesium (Mg)
alkaline-earth-metalSolid
標準原子量
24.305 u [24.304, 24.307]電子配置
[Ne] 3s2融点
649.85 °C沸点
1089.85 °C密度
1740 kg/m³酸化数
0, +1, +2電気陰性度（Pauling）
1.31第1イオン化エネルギー
7.646236 eV発見年
1755原子半径
150 pm詳細
Magnesium is a light alkaline earth metal and a major rock-forming element. It occurs in silicate minerals, carbonates, evaporites, seawater, and brines, almost entirely as Mg²⁺ rather than as native metal. Its low density, ready formation of stable salts, and high affinity for oxygen shape both its metallurgy and its geochemistry. Magnesium is also essential in biology, where it stabilizes phosphate chemistry and is central to chlorophyll.
Magnesium is a light, silvery-white, and fairly tough metal. It tarnishes slightly in air, and finely divided magnesium readily ignites upon heating in air and burns with a dazzling white flame.
The name derives from Magnesia, a district in the north-eastern region of Greece called Thessalia. The Scottish chemist Joseph Black recognized it as a separate element in 1755. In 1808, the English chemist Humphry Davy obtained the impure metal, and in 1831 the French pharmacist and chemist Antoine- Alexandre Brutus Bussy isolated the metal in the pure state.
Although it is the eighth most abundant element in the universe and the seventh most abundant element in the earth's crust, magnesium is never found free in nature. Magnesium was first isolated by Sir Humphry Davy, an English chemist, through the electrolysis of a mixture of magnesium oxide (MgO) and mercuric oxide (HgO) in 1808. Today, magnesium can be extracted from the minerals dolomite (CaCO3·MgCO3) and carnallite (KCl·MgCl2·6H2O), but is most often obtained from seawater. Every cubic kilometer of seawater contains about 1.3 billion kilograms of magnesium (12 billion pounds per cubic mile).
From Magnesia, district in Thessaly. Compounds of magnesium have long been known. Black recognized magnesium as an element in 1755. Davy isolated it in 1808 and Bussy prepared it in coherent form in 1831. Magnesium is the eighth most abundant element in the earth's crust. It does not occur uncombined, but is found in large deposits in the form of magnesite, dolomite, and other minerals.
Pure magnesium is a silvery-white metal with a bright metallic luster when freshly cut. In air it slowly dulls as a thin oxide and hydroxide film develops. It is light, machinable, and solid at ordinary conditions, but finely divided metal can burn with an intense white flame.
Magnesium metal is used mainly where low mass is valuable, especially in aluminum alloys, die-cast automotive and electronic parts, and some aerospace components. It serves as a reducing agent in the production of metals such as titanium from titanium tetrachloride (TiCl₄). Magnesium is used in sacrificial anodes for corrosion protection, in pyrotechnic compositions and flares, and in specialty batteries. Magnesium compounds are widely used in refractories, fertilizers, animal feed, pharmaceuticals, and water treatment.
Magnesium burns with a brilliant white light and is used in pyrotechnics, flares and photographic flashbulbs. Magnesium is the lightest metal that can be used to build things, although its use as a structural material is limited since it burns at relatively low temperatures. Magnesium is frequently alloyed with aluminum, which makes aluminum easier to roll, extrude and weld. Magnesium-aluminum alloys are used where strong, lightweight materials are required, such as in airplanes, missiles and rockets. Cameras, horseshoes, baseball catchers' masks and snowshoes are other items that are made from magnesium alloys.
Magnesium oxide (MgO), also known as magnesia, is the second most abundant compound in the earth's crust. Magnesium oxide is used in some antacids, in making crucibles and insulating materials, in refining some metals from their ores and in some types of cements. When combined with water (H2O), magnesia forms magnesium hydroxide (Mg(OH)2), better known as milk of magnesia, which is commonly used as an antacid and as a laxative.
Hydrated magnesium sulphate (MgSO4·7H2O), better known as Epsom salt, was discovered in 1618 by a farmer in Epsom, England, when his cows refused to drink the water from a certain mineral well. He tasted the water and found that it tasted very bitter. He also noticed that it helped heal scratches and rashes on his skin. Epsom salt is still used today to treat minor skin abrasions.
Other magnesium compounds include magnesium carbonate (MgCO3) and magnesium fluoride (MgF2). Magnesium carbonate is used to make some types of paints and inks and is added to table salt to prevent caking. A thin film of magnesium fluoride is applied to optical lenses to help reduce glare and reflections.
Uses include flashlight photography, flares, and pyrotechnics, including incendiary bombs. It is one third lighter than aluminum, and in alloys is essential for airplane and missile construction. The metal improves the mechanical, fabrication, and welding characteristics of aluminum when used as an alloying agent. Magnesium is used in producing nodular graphite in cast iron, and is used as an additive to conventional propellants.
It is also used as a reducing agent in the production of pure uranium and other metals from their salts. The hydroxide (milk of magnesia), chloride, sulfate (Epsom salts), and citrate are used in medicine. Dead-burned magnesite is employed for refractory purposes such as brick and liners in furnaces and converters.
Isotopes in Biology
Natural magnesium enriched in the stable isotopes 25Mg and 26Mg has been used as tracers in human studies to assess absorption, excretion, distribution, and utilization of magnesium in basic and applied research [108] World Nuclear Association. Radioisotopes in Industry: Industrial Uses of Radioisotopes, World Nuclear Association (2014), Feb. 24; http://www.world-nuclear.org/info/inf56.html., [113] M. Sabatier, W. R. Keyes, F. Pont, M. J. Arnaud, J. R. Turnlund. Am. J. Clin. Nutr.77, 1206 (2003)., [114] M. Sabatier, F. Pont, M. J. Arnaud, J. R. Turnlund. Am. J. Physiol.285, R656 (2003)..
Isotopes in Earth/Planetary Science
Molecules, atoms, and ions of the stable isotopes of magnesium possess slightly different physical and chemical properties, and they commonly will be fractionated during physical, chemical, and biological processes, giving rise to variations in isotopic abundances and in atomic weights. There are substantial variations in the isotopic abundances of magnesium in natural terrestrial materials (Fig. IUPAC.12.1). These variations are useful in investigating the origin of substances and studying environmental, hydrological, and geological processes [13] M. W. Wieser, T. B. Coplen. Pure Appl Chem.83, 359 (2011)., [17] T. B. Coplen, J. A. Hopple, J. K. Böhlke, H. S. Peiser, S. E. Rieder, H. R. Krouse, K. J. R. Rosman, T. Ding, R. D. Vocke, K. Revesz, A. Lamberty, P. D. P. Taylor, P. D. Bièvre. United States Geological Survey Water-Resources Investigations Report, 01-4222, (2002)., [115] J. G. Montes, R. A. Sjodin, A. L. Yergey, N. E. Vieira. Biophys. J.56, 437 (1989)..
Isotopes in Geochronology
26Mg is a stable isotope and is the radiogenic product of 26Al decay. 26Al is produced by cosmic rays in space and in the atmosphere, and it was present in the primordial solar nebula. The anomalous abundance of 26Mg in meteorite inclusions indicate that this material must have been formed early in the development of the Solar System before all primordial 26Al (with half-life of 7.1×105 years) had decayed [116] S. Sahijpal, J. N. Goswami. Astrophys. J.509, L137 (1998)..
Magnesium chemistry is dominated by the +2 oxidation state and by ionic or strongly polar compounds. Magnesium oxide (MgO) is a refractory basic oxide, while magnesium hydroxide (Mg(OH)₂) is sparingly soluble and used where mild alkalinity is needed. Important salts include magnesium chloride (MgCl₂), magnesium sulfate (MgSO₄), and magnesium carbonate (MgCO₃). Magnesium silicates are major constituents of rocks. Organomagnesium halides, known as Grignard reagents, are central synthetic intermediates in organic chemistry.
Organic magnesium is important in both plant and animal life. Chlorophylls are magnesium-centered perphyrins.
The adult daily nutritional requirement, which is affected by various factors include weight and size, is about 300 mg/day.
See more information at the Magnesium compound page.
Bulk magnesium metal is not highly toxic, and magnesium ions are essential nutrients. The main elemental hazard is fire: shavings, powder, and molten metal can ignite, and burning magnesium is difficult to extinguish with water because hydrogen and heat may be produced. Intense ultraviolet and visible light from burning magnesium can injure eyes. Excess intake of soluble magnesium salts can cause physiological effects, especially when renal clearance is impaired, and industrial dusts require exposure control.
Because serious fires can occur, great care should be taken in handling magnesium metal, especially when finely divided. Water should not be used on burning magnesium or on magnesium fires.
Magnesium is abundant in the crust and hydrosphere and cycles through weathering, river transport, seawater chemistry, carbonate deposition, and biological uptake. It is a common nutrient for plants and animals, and its availability affects soil fertility and water hardness. In the ocean, Mg²⁺ is one of the major dissolved cations. Magnesium minerals also participate in long-term carbon cycling through carbonate formation and alteration of silicate rocks.
Magnesium is produced from mineral sources and brines, chiefly by electrolysis of magnesium chloride (MgCl₂) or by thermal reduction of magnesium oxide (MgO)-bearing feedstocks such as dolomite-derived material. Energy cost, process emissions, and control of oxidation during melting are important industrial factors. Demand is tied to lightweight alloys, aluminum alloying, die casting, desulfurization and chemical uses. Recycling is significant for clean alloy scrap, although mixed or oxidized scrap is harder to recover efficiently. Substitution is possible in many structural applications, but magnesium remains attractive where low density outweighs cost and handling constraints.
The metal is now principally obtained in the U.S. by electrolysis of fused magnesium chloride derived from brines, wells, and sea water.
Magnesium is a relatively abundant cosmic element formed mainly by fusion processes in massive stars and dispersed by supernovae and stellar winds. It is common in silicate dust and rocky planetary material, where it combines with oxygen and silicon. In meteorites and terrestrial planets it is concentrated in minerals such as olivine and pyroxene rather than in metallic form.
- Magnesium burns in carbon dioxide (CO₂) as well as in air, forming magnesium oxide and carbon.
- Chlorophyll contains a magnesium ion held in a porphyrin ring.
- Seawater is an important practical source of magnesium, although the metal itself is not present there.
- Grignard reagents made from magnesium helped transform carbon-carbon bond formation in synthesis.
- Magnesium alloys often need protective atmospheres or fluxes during melting to limit oxidation.
画像
性質
物理的性質
- 原子半径（経験値）
- 150 pm 全元素の原子半径（経験値）を比較 →
- 共有結合半径
- 141 pm 全元素の共有結合半径を比較 →
- ファンデルワールス半径
- 173 pm 全元素のファンデルワールス半径を比較 →
- 金属半径
- 136 pm 全元素の金属半径を比較 →
- 密度
- 1740 kg/m³ 全元素の密度を比較 →
- モル体積
- 0.014 L/mol
- 標準温度・圧力（STP）での相
- 固体 全元素の標準温度・圧力（STP）での相を比較 →
- 融点
- 649.85 °C 全元素の融点を比較 →
- 沸点
- 1089.85 °C 全元素の沸点を比較 →
- 熱伝導率
- 156 W/(m·K) 全元素の熱伝導率を比較 →
- 比熱容量
- 1.023 J/(g·K) 全元素の比熱容量を比較 →
- モル熱容量
- 24.869 J/(mol·K) 全元素のモル熱容量を比較 →
- 結晶構造
- 六方最密充填構造 全元素の結晶構造を比較 →
化学的性質
- 電気陰性度（Pauling）
- 1.31 全元素の電気陰性度（Pauling）を比較 →
- 電気陰性度（Allen）
- 1.293
- 電子親和力
- -0.4 eV (負の値—この原子は電子を取り込まないと予測される)
- 第1イオン化エネルギー
- 7.646236 eV 全元素の第1イオン化エネルギーを比較 →
- 第2イオン化エネルギー
- 15.035323 eV 全元素の第2イオン化エネルギーを比較 →
- 第3イオン化エネルギー
- 80.143876 eV 全元素の第3イオン化エネルギーを比較 →
- 第4イオン化エネルギー
- 109.265776 eV 全元素の第4イオン化エネルギーを比較 →
- 第5イオン化エネルギー
- 141.330486 eV 全元素の第5イオン化エネルギーを比較 →
- 酸化数
- 0, +1, +2 全元素の酸化数を比較 →
- 価電子
- 2 全元素の価電子を比較 →
- 電子配置
- [Ne] 3s2
熱力学的性質
- 融解熱
- 0.08788931 eV 全元素の融解熱を比較 →
- 蒸発熱
- 1.326631 eV 全元素の蒸発熱を比較 →
- 昇華熱
- 1.524589 eV
- 原子化熱
- 1.524589 eV
- 原子化エンタルピー
- 1.524589 eV
原子核
- 陽子数
- 12 全元素の陽子数を比較 →
- 中性子数
- 12 全元素の中性子数を比較 →
- 既知の同位体
- 23 全元素の既知の同位体を比較 →
- 安定同位体
- 3 全元素の安定同位体を比較 →
- 最も安定な同位体
- Mg-24
- 発見年
- 1755
存在度
- 存在度（地殻）
- 2.33e+4 mg/kg 全元素の存在度（地殻）を比較 →
- 存在度（海洋）
- 1290 mg/L 全元素の存在度（海洋）を比較 →
結晶構造
- 格子定数a
- 321 pm
電子構造
- 各電子殻の電子数
- 2, 8, 2 全元素の各電子殻の電子数を比較 →
識別子
- CAS登録番号
- 7439-95-4 全元素のCAS登録番号を比較 →
- 項記号
- 1S0
- InChI
- InChI=1S/Mg
- InChI Key
- FYYHWMGAXLPEAU-UHFFFAOYSA-N
電子配置 測定値
Mg: 3s²[Ne] 3s²1s² 2s² 2p⁶ 3s²原子モデル
同位体によって中性子数、質量、安定性は変わりますが、中性原子の電子配置は変わりません。
模式的な原子モデルです。実際の縮尺とは異なります。
原子の指紋
発光／吸収スペクトル
同位体分布
| 質量数 | 原子質量（u） | 天然存在比 | 半減期 |
|---|---|---|---|
| 24 安定 | 23.985041697 ± 0.000000014 | 78.9900% | 安定 |
| 25 安定 | 24.985836976 ± 0.00000005 | 10.0000% | 安定 |
| 26 安定 | 25.982592968 ± 0.000000031 | 11.0100% | 安定 |
相／状態
理由: 融点（649.85 °C）より624.9 °C低い
模式図、実際の縮尺とは異なります
相転移点
相転移エネルギー
融点で1 molを融解させるのに必要なエネルギー
沸点で1 molを蒸発させるのに必要なエネルギー
昇華点で1 molを昇華させるのに必要なエネルギー
密度
標準条件下
標準条件下
原子スペクトル
全12件中10件を表示しています。 イオンの電荷の昇順で並べています。
スペクトル線データの収録状況 ?
| イオン | 電荷 | スペクトル線の総数 | 遷移確率 | 準位の表記 |
|---|---|---|---|---|
| Mg I | 0 | 1342 | 1090 | 1342 |
| Mg II | +1 | 601 | 482 | 601 |
| Mg III | +2 | 452 | 149 | 452 |
| Mg IV | +3 | 821 | 625 | 821 |
| Mg V | +4 | 518 | 513 | 515 |
| Mg VI | +5 | 890 | 883 | 890 |
| Mg VII | +6 | 379 | 344 | 379 |
| Mg VIII | +7 | 944 | 941 | 944 |
| Mg IX | +8 | 461 | 444 | 461 |
| Mg X | +9 | 223 | 184 | 223 |
準位データの収録状況 ?
| イオン | 電荷 | 準位 |
|---|---|---|
| Mg I | 0 | 323 |
| Mg II | +1 | 149 |
| Mg III | +2 | 114 |
| Mg IV | +3 | 173 |
| Mg V | +4 | 104 |
| Mg VI | +5 | 120 |
| Mg VII | +6 | 104 |
| Mg VIII | +7 | 113 |
| Mg IX | +8 | 94 |
| Mg X | +9 | 60 |
イオン半径
| 電荷 | 配位 | スピン | 半径 |
|---|---|---|---|
| +2 | 4 | データなし | 56.99999999999999 pm |
| +2 | 5 | データなし | 66 pm |
| +2 | 6 | データなし | 72 pm |
| +2 | 8 | データなし | 89 pm |
化合物
同位体 (3)
| 質量数 | 原子質量（u） | 天然存在比 | 半減期 | 崩壊形式 | |
|---|---|---|---|---|---|
| 24 安定 | 23.985041697 ± 0.000000014 | 78.9900% ± 0.0400% | 安定 | stable | |
| 25 安定 | 24.985836976 ± 0.00000005 | 10.0000% ± 0.0100% | 安定 | stable | |
| 26 安定 | 25.982592968 ± 0.000000031 | 11.0100% ± 0.0300% | 安定 | stable |
スペクトル線
全399件中50件を表示しています。 初期設定では、強度の測定値があるスペクトル線のみを表示します。
| 波長（nm） | 強度 | 電離段階 | 種類 | 遷移 | 精度 | 出典 | |
|---|---|---|---|---|---|---|---|
| 518.36043 nm | 45 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | 測定値 | NIST | |
| 517.26844 nm | 44 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | 測定値 | NIST | |
| 516.73213 nm | 42 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | 測定値 | NIST | |
| 383.82919 nm | 40 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | 測定値 | NIST | |
| 552.84047 nm | 40 | Mg I | emission | 3s.3p 1P* → 3s.4d 1D | 測定値 | NIST | |
| 383.23039 nm | 38 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | 測定値 | NIST | |
| 382.93547 nm | 36 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | 測定値 | NIST | |
| 470.29908 nm | 30 | Mg I | emission | 3s.3p 1P* → 3s.5d 1D | 測定値 | NIST | |
| 571.1088 nm | 30 | Mg I | emission | 3s.3p 1P* → 3s.5s 1S | 測定値 | NIST | |
| 435.19057 nm | 20 | Mg I | emission | 3s.3p 1P* → 3s.6d 1D | 測定値 | NIST | |
| 416.72713 nm | 15 | Mg I | emission | 3s.3p 1P* → 3s.7d 1D | 測定値 | NIST | |
| 625.6757 nm | 15 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4p 2[5/2] | 測定値 | NIST | |
| 448.1126 nm | 14 | Mg II | emission | 2p6.3d 2D → 2p6.4f 2F* | 測定値 | NIST | |
| 448.1325 nm | 13 | Mg II | emission | 2p6.3d 2D → 2p6.4f 2F* | 測定値 | NIST | |
| 738.7689 nm | 12 | Mg I | emission | 3s.3d 1D → 3s.8f 1F* | 測定値 | NIST | |
| 405.75052 nm | 10 | Mg I | emission | 3s.3p 1P* → 3s.8d 1D | 測定値 | NIST | |
| 439.0572 nm | 10 | Mg II | emission | 2p6.4p 2P* → 2p6.5d 2D | 測定値 | NIST | |
| 473.00286 nm | 10 | Mg I | emission | 3s.3p 1P* → 3s.6s 1S | 測定値 | NIST | |
| 491.5991 nm | 10 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[5/2] → 2s2.2p5.(2P*<3/2>).4d 2[7/2]* | 測定値 | NIST | |
| 583.981 nm | 10 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4p 2[3/2] | 測定値 | NIST | |
| 631.8717 nm | 10 | Mg I | emission | 3s.4s 3S → 3s.6p 3P* | 測定値 | NIST | |
| 634.6742 nm | 10 | Mg II | emission | 2p6.4d 2D → 2p6.6f 2F* | 測定値 | NIST | |
| 719.3184 nm | 10 | Mg I | emission | 3s.3d 1D → 3s.9f 1F* | 測定値 | NIST | |
| 729.1055 nm | 10 | Mg I | emission | 3s.4s 1S → 3s.6p 1P* | 測定値 | NIST | |
| 438.4637 nm | 9 | Mg II | emission | 2p6.4p 2P* → 2p6.5d 2D | 測定値 | NIST | |
| 443.3988 nm | 9 | Mg II | emission | 2p6.4p 2P* → 2p6.6s 2S | 測定値 | NIST | |
| 452.6219 nm | 9 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[1/2] → 2s2.2p5.(2P*<3/2>).4d 2[3/2]* | 測定値 | NIST | |
| 459.6921 nm | 9 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[1/2] → 2s2.2p5.(2P*<3/2>).4d 2[1/2]* | 測定値 | NIST | |
| 496.041 nm | 9 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[5/2] → 2s2.2p5.(2P*<3/2>).4d 2[7/2]* | 測定値 | NIST | |
| 631.9237 nm | 9 | Mg I | emission | 3s.4s 3S → 3s.6p 3P* | 測定値 | NIST | |
| 634.6964 nm | 9 | Mg II | emission | 2p6.4d 2D → 2p6.6f 2F* | 測定値 | NIST | |
| 384.8211 nm | 8 | Mg II | emission | 2p6.3d 2D → 2p6.5p 2P* | 測定値 | NIST | |
| 398.67533 nm | 8 | Mg I | emission | 3s.3p 1P* → 3s.9d 1D | 測定値 | NIST | |
| 442.7994 nm | 8 | Mg II | emission | 2p6.4p 2P* → 2p6.6s 2S | 測定値 | NIST | |
| 467.3315 nm | 8 | Mg III | emission | 2s2.2p5.(2P*<1/2>).4s 2[1/2]* → 2s2.2p5.(2P*<1/2>).4p 2[1/2] | 測定値 | NIST | |
| 498.1469 nm | 8 | Mg III | emission | 2s2.2p5.(2P*<1/2>).4p 2[3/2] → 2s2.2p5.(2P*<1/2>).4d 2[5/2]* | 測定値 | NIST | |
| 526.422 nm | 8 | Mg II | emission | 2p6.4d 2D → 2p6.7f 2F* | 測定値 | NIST | |
| 640.6637 nm | 8 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4p 2[5/2] | 測定値 | NIST | |
| 678.7855 nm | 8 | Mg II | emission | 2p6.5p 2P* → 2p6.7d 2D | 測定値 | NIST | |
| 681.927 nm | 8 | Mg II | emission | 2p6.5p 2P* → 2p6.8s 2S | 測定値 | NIST | |
| 706.0414 nm | 8 | Mg I | emission | 3s.3d 1D → 3s.10f 1F* | 測定値 | NIST | |
| 385.0386 nm | 7 | Mg II | emission | 2p6.3d 2D → 2p6.5p 2P* | 測定値 | NIST | |
| 423.9473 nm | 7 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<1/2>).4p 2[1/2] | 測定値 | NIST | |
| 463.2537 nm | 7 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[1/2] → 2s2.2p5.(2P*<3/2>).4d 2[1/2]* | 測定値 | NIST | |
| 480.2585 nm | 7 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[3/2] → 2s2.2p5.(2P*<3/2>).4d 2[3/2]* | 測定値 | NIST | |
| 491.5363 nm | 7 | Mg III | emission | 2s2.2p5.(2P*<1/2>).4p 2[3/2] → 2s2.2p5.(2P*<1/2>).4d 2[5/2]* | 測定値 | NIST | |
| 497.0497 nm | 7 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[3/2] → 2s2.2p5.(2P*<3/2>).4d 2[5/2]* | 測定値 | NIST | |
| 502.3674 nm | 7 | Mg III | emission | 2s2.2p5.(2P*<3/2>).4p 2[3/2] → 2s2.2p5.(2P*<3/2>).4d 2[5/2]* | 測定値 | NIST | |
| 526.4364 nm | 7 | Mg II | emission | 2p6.4d 2D → 2p6.7f 2F* | 測定値 | NIST | |
| 591.6431 nm | 7 | Mg II | emission | 2p6.4d 2D → 2p6.7p 2P* | 測定値 | NIST |
詳細な性質
共有結合半径（詳細）
- 共有結合半径（Pyykkö）
- 139 pm
- 共有結合半径（Pyykkö、二重結合）
- 132 pm
- 共有結合半径（Pyykkö、三重結合）
- 127 pm
- 共有結合半径（Bragg）
- 142 pm
ファンデルワールス半径
- Bondi
- 173 pm
- Batsanov
- 220 pm
- Alvarez
- 251 pm
- UFF
- 302.1 pm
- MM3
- 243 pm
原子半径と金属半径
- 原子半径（Rahm）
- 240 pm
- 金属半径（C12）
- 160 pm
番号付けの尺度
- Mendeleev
- 76
- Pettifor
- 73
- Glawe
- 73
電気陰性度の尺度
- Ghosh
- 0
- Miedema
- 3
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 3
分極率と分散
- 双極子分極率
- 71.2 a.u.
- 双極子分極率（不確かさ）
- 0.4 a.u.
- C₆
- 626 Ha·Bohr6
- C₆ (Gould–Bučko)
- 629 Ha·Bohr6
化学親和力
- プロトン親和力
- 819.6 kJ/mol
- 気相塩基性
- 797.3 kJ/mol
ミーデマパラメータ
- ミーデマモル体積
- 14 cm3/mol
- ミーデマ電子密度
- 2
供給リスクと経済性
- 生産集中度
- 64
- 相対供給リスク
- 7
- 埋蔵量の分布
- 26
- 政治的安定性（最大生産国）
- 24
- 政治的安定性（最大埋蔵国）
- 18
相転移と同素体
| 融点 | 923.15 K |
| 沸点 | 1363.15 K |
酸化数の分類
専門参考データ
遮蔽定数 (4)
| n | 軌道 | σ |
|---|---|---|
| 1 | s | 0.3911 |
| 2 | p | 4.1742 |
| 2 | s | 4.608 |
| 3 | s | 8.6925 |
結晶半径の詳細 (4)
| 電荷 | CN | スピン | rcrystal (pm) | 由来 |
|---|---|---|---|---|
| 2 | IV | 71 | ||
| 2 | V | 80 | ||
| 2 | VI | 86 | ||
| 2 | VIII | 103 | calculated, |
同位体の崩壊形式 (43)
| 同位体 | モード | 強度 |
|---|---|---|
| 19 | 2p | 100% |
| 20 | B+ | 100% |
| 20 | B+p | 30.3% |
| 21 | B+ | 100% |
| 21 | B+p | 20.1% |
| 21 | B+A | 0.1% |
| 21 | B+pA | 0% |
| 22 | B+ | 100% |
| 23 | B+ | 100% |
| 27 | B- | 100% |
X線散乱因子 (755)
| エネルギー (eV) | f₁ | f₂ |
|---|---|---|
| 0.5 | 0.117 | 0.14592 |
| 0.5079 | 0.1168 | 0.14896 |
| 0.516 | 0.1165 | 0.15206 |
| 0.5242 | 0.1165 | 0.15522 |
| 0.5325 | 0.1162 | 0.15845 |
| 0.5409 | 0.1162 | 0.16175 |
| 0.5495 | 0.1162 | 0.16511 |
| 0.5582 | 0.1161 | 0.16855 |
| 0.5671 | 0.1163 | 0.17205 |
| 0.5761 | 0.1167 | 0.17558 |
追加データ
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.33×104 milligrams per kilogram
参考文献 (1)
- [5] Magnesium https://education.jlab.org/itselemental/ele012.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
1.29×103 milligrams per liter
参考文献 (1)
- [5] Magnesium https://education.jlab.org/itselemental/ele012.html
Sources
Sources of this element.
The metal is now principally obtained in the U.S. by electrolysis of fused magnesium chloride derived from brines, wells, and sea water.
参考文献 (1)
- [6] Magnesium https://periodic.lanl.gov/12.shtml
参考文献
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Magnesium.
The element property data was retrieved from publications.