Magnesium (Mg)
alkaline-earth-metalSolid
표준 원자량
24.305 u [24.304, 24.307]전자 배치
[Ne] 3s2녹는점
649.85 °C끓는점
1089.85 °C밀도
1740 kg/m³산화 상태
0, +1, +2전기 음성도(Pauling)
1.31제1 이온화 에너지
7.646236 eV발견 연도
1755원자 반지름
150 pm상세 정보
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.
이미지
특성
물리적 특성
- 원자 반지름(경험값)
- 150 pm 모든 원소의 원자 반지름(경험값) 비교 →
- 공유 결합 반지름
- 141 pm 모든 원소의 공유 결합 반지름 비교 →
- 반데르발스 반지름
- 173 pm 모든 원소의 반데르발스 반지름 비교 →
- 금속 반지름
- 136 pm 모든 원소의 금속 반지름 비교 →
- 밀도
- 1740 kg/m³ 모든 원소의 밀도 비교 →
- 몰 부피
- 0.014 L/mol
- STP에서의 상
- 고체 모든 원소의 STP에서의 상 비교 →
- 녹는점
- 649.85 °C 모든 원소의 녹는점 비교 →
- 끓는점
- 1089.85 °C 모든 원소의 끓는점 비교 →
- 열전도율
- 156 W/(m·K) 모든 원소의 열전도율 비교 →
- 비열
- 1.023 J/(g·K) 모든 원소의 비열 비교 →
- 몰 열용량
- 24.869 J/(mol·K) 모든 원소의 몰 열용량 비교 →
- 결정 구조
- 육방 조밀 충전 모든 원소의 결정 구조 비교 →
화학적 특성
- 전기 음성도(Pauling)
- 1.31 모든 원소의 전기 음성도(Pauling) 비교 →
- 전기 음성도(Allen)
- 1.293
- 전자 친화도
- -0.4 eV (음수 값 — 추가 전자를 결합하지 않을 것으로 예측됨)
- 제1 이온화 에너지
- 7.646236 eV 모든 원소의 제1 이온화 에너지 비교 →
- 제2 이온화 에너지
- 15.035323 eV 모든 원소의 제2 이온화 에너지 비교 →
- 제3 이온화 에너지
- 80.143876 eV 모든 원소의 제3 이온화 에너지 비교 →
- 제4 이온화 에너지
- 109.265776 eV 모든 원소의 제4 이온화 에너지 비교 →
- 제5 이온화 에너지
- 141.330486 eV 모든 원소의 제5 이온화 에너지 비교 →
- 산화 상태
- 0, +1, +2 모든 원소의 산화 상태 비교 →
- 원자가 전자
- 2 모든 원소의 원자가 전자 비교 →
- 전자 배치
- [Ne] 3s2
열역학적 특성
- 융해열
- 0.08788931 eV 모든 원소의 융해열 비교 →
- 기화열
- 1.326631 eV 모든 원소의 기화열 비교 →
- 승화열
- 1.524589 eV
- 원자화열
- 1.524589 eV
- 원자화 엔탈피
- 1.524589 eV
핵 특성
- 양성자 수
- 12 모든 원소의 양성자 수 비교 →
- 중성자 수
- 12 모든 원소의 중성자 수 비교 →
- 알려진 동위원소 수
- 23 모든 원소의 알려진 동위원소 수 비교 →
- 안정 동위원소 수
- 3 모든 원소의 안정 동위원소 수 비교 →
- 가장 안정한 동위원소
- Mg-24
- 발견 연도
- 1755
존재비
- 존재비(지각)
- 2.33e+4 mg/kg 모든 원소의 존재비(지각) 비교 →
- 존재비(해양)
- 1290 mg/L 모든 원소의 존재비(해양) 비교 →
결정 구조
- 격자 상수 a
- 321 pm
전자 구조
- 전자껍질별 전자 수
- 2, 8, 2 모든 원소의 전자껍질별 전자 수 비교 →
식별자
- CAS 등록 번호
- 7439-95-4 모든 원소의 CAS 등록 번호 비교 →
- 항 기호
- 1S0
- InChI
- InChI=1S/Mg
- InChI 키
- FYYHWMGAXLPEAU-UHFFFAOYSA-N
전자 배치 측정값
Mg: 3s²[Ne] 3s²1s² 2s² 2p⁶ 3s²원자 모형
동위원소에 따라 중성자 수, 질량, 안정성은 달라지지만, 중성 원자의 전자 배치는 달라지지 않습니다.
개략적인 원자 모형이며 실제 비율과 다릅니다.
원자 지문
방출 / 흡수 스펙트럼
동위원소 분포
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 |
|---|---|---|---|
| 24 안정 | 23.985041697 ± 0.000000014 | 78.9900% | 안정 |
| 25 안정 | 24.985836976 ± 0.00000005 | 10.0000% | 안정 |
| 26 안정 | 25.982592968 ± 0.000000031 | 11.0100% | 안정 |
상 / 상태
이유: 녹는점(649.85 °C)보다 624.9 °C 낮음
개략도이며 실제 비율과 다름
상전이점
전이 에너지
녹는점에서 1 mol을 녹이는 데 필요한 에너지
끓는점에서 1 mol을 기화시키는 데 필요한 에너지
승화점에서 1 mol을 승화시키는 데 필요한 에너지
밀도
표준 조건에서
표준 조건에서
원자 스펙트럼
전체 12개 중 10개를 표시합니다. 이온 전하순으로 정렬되었습니다(오름차순).
보유 스펙트럼선 데이터 ?
| 이온 | 전하 | 총 스펙트럼선 수 | 전이 확률 | 준위 표기 |
|---|---|---|---|---|
| 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 |
보유 에너지 준위 데이터 ?
| 이온 | 전하 | 준위 |
|---|---|---|
| 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 |
이온 반지름
| 전하 | 배위 | 스핀 | 반지름 |
|---|---|---|---|
| +2 | 4 | 해당 없음 | 56.99999999999999 pm |
| +2 | 5 | 해당 없음 | 66 pm |
| +2 | 6 | 해당 없음 | 72 pm |
| +2 | 8 | 해당 없음 | 89 pm |
화합물
동위원소 (3)
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 | 붕괴 방식 | |
|---|---|---|---|---|---|
| 24 안정 | 23.985041697 ± 0.000000014 | 78.9900% ± 0.0400% | 안정 | stable | |
| 25 안정 | 24.985836976 ± 0.00000005 | 10.0000% ± 0.0100% | 안정 | stable | |
| 26 안정 | 25.982592968 ± 0.000000031 | 11.0100% ± 0.0300% | 안정 | stable |
스펙트럼선
전체 399개 중 50개를 표시합니다. 기본적으로 세기가 측정된 스펙트럼선만 표시됩니다.
| 파장(nm) | 세기 | 이온화 단계 | 유형 | 전이 | 정확도 | 출처 | |
|---|---|---|---|---|---|---|---|
| 518.36043 nm | 45 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | 측정값 | NIST | |
| 517.26844 nm | 44 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | 측정값 | NIST | |
| 516.73213 nm | 42 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | 측정값 | NIST | |
| 383.82919 nm | 40 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | 측정값 | NIST | |
| 552.84047 nm | 40 | Mg I | emission | 3s.3p 1P* → 3s.4d 1D | 측정값 | NIST | |
| 383.23039 nm | 38 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | 측정값 | NIST | |
| 382.93547 nm | 36 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | 측정값 | NIST | |
| 470.29908 nm | 30 | Mg I | emission | 3s.3p 1P* → 3s.5d 1D | 측정값 | NIST | |
| 571.1088 nm | 30 | Mg I | emission | 3s.3p 1P* → 3s.5s 1S | 측정값 | NIST | |
| 435.19057 nm | 20 | Mg I | emission | 3s.3p 1P* → 3s.6d 1D | 측정값 | NIST | |
| 416.72713 nm | 15 | Mg I | emission | 3s.3p 1P* → 3s.7d 1D | 측정값 | 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] | 측정값 | NIST | |
| 448.1126 nm | 14 | Mg II | emission | 2p6.3d 2D → 2p6.4f 2F* | 측정값 | NIST | |
| 448.1325 nm | 13 | Mg II | emission | 2p6.3d 2D → 2p6.4f 2F* | 측정값 | NIST | |
| 738.7689 nm | 12 | Mg I | emission | 3s.3d 1D → 3s.8f 1F* | 측정값 | NIST | |
| 405.75052 nm | 10 | Mg I | emission | 3s.3p 1P* → 3s.8d 1D | 측정값 | NIST | |
| 439.0572 nm | 10 | Mg II | emission | 2p6.4p 2P* → 2p6.5d 2D | 측정값 | NIST | |
| 473.00286 nm | 10 | Mg I | emission | 3s.3p 1P* → 3s.6s 1S | 측정값 | 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]* | 측정값 | 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] | 측정값 | NIST | |
| 631.8717 nm | 10 | Mg I | emission | 3s.4s 3S → 3s.6p 3P* | 측정값 | NIST | |
| 634.6742 nm | 10 | Mg II | emission | 2p6.4d 2D → 2p6.6f 2F* | 측정값 | NIST | |
| 719.3184 nm | 10 | Mg I | emission | 3s.3d 1D → 3s.9f 1F* | 측정값 | NIST | |
| 729.1055 nm | 10 | Mg I | emission | 3s.4s 1S → 3s.6p 1P* | 측정값 | NIST | |
| 438.4637 nm | 9 | Mg II | emission | 2p6.4p 2P* → 2p6.5d 2D | 측정값 | NIST | |
| 443.3988 nm | 9 | Mg II | emission | 2p6.4p 2P* → 2p6.6s 2S | 측정값 | 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]* | 측정값 | 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]* | 측정값 | 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]* | 측정값 | NIST | |
| 631.9237 nm | 9 | Mg I | emission | 3s.4s 3S → 3s.6p 3P* | 측정값 | NIST | |
| 634.6964 nm | 9 | Mg II | emission | 2p6.4d 2D → 2p6.6f 2F* | 측정값 | NIST | |
| 384.8211 nm | 8 | Mg II | emission | 2p6.3d 2D → 2p6.5p 2P* | 측정값 | NIST | |
| 398.67533 nm | 8 | Mg I | emission | 3s.3p 1P* → 3s.9d 1D | 측정값 | NIST | |
| 442.7994 nm | 8 | Mg II | emission | 2p6.4p 2P* → 2p6.6s 2S | 측정값 | 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] | 측정값 | 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]* | 측정값 | NIST | |
| 526.422 nm | 8 | Mg II | emission | 2p6.4d 2D → 2p6.7f 2F* | 측정값 | 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] | 측정값 | NIST | |
| 678.7855 nm | 8 | Mg II | emission | 2p6.5p 2P* → 2p6.7d 2D | 측정값 | NIST | |
| 681.927 nm | 8 | Mg II | emission | 2p6.5p 2P* → 2p6.8s 2S | 측정값 | NIST | |
| 706.0414 nm | 8 | Mg I | emission | 3s.3d 1D → 3s.10f 1F* | 측정값 | NIST | |
| 385.0386 nm | 7 | Mg II | emission | 2p6.3d 2D → 2p6.5p 2P* | 측정값 | 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] | 측정값 | 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]* | 측정값 | 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]* | 측정값 | 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]* | 측정값 | 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]* | 측정값 | 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]* | 측정값 | NIST | |
| 526.4364 nm | 7 | Mg II | emission | 2p6.4d 2D → 2p6.7f 2F* | 측정값 | NIST | |
| 591.6431 nm | 7 | Mg II | emission | 2p6.4d 2D → 2p6.7p 2P* | 측정값 | NIST |
확장 특성
공유 결합 반지름(확장)
- 공유 결합 반지름(Pyykkö)
- 139 pm
- 공유 결합 반지름(Pyykkö, 이중 결합)
- 132 pm
- 공유 결합 반지름(Pyykkö, 삼중 결합)
- 127 pm
- 공유 결합 반지름(Bragg)
- 142 pm
반데르발스 반지름
- Bondi
- 173 pm
- Batsanov
- 220 pm
- Alvarez
- 251 pm
- UFF
- 302.1 pm
- MM3
- 243 pm
원자 및 금속 반지름
- 원자 반지름(Rahm)
- 240 pm
- 금속 반지름(C12)
- 160 pm
번호 척도
- Mendeleev
- 76
- Pettifor
- 73
- Glawe
- 73
전기 음성도 척도
- Ghosh
- 0
- Miedema
- 3
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 3
분극률 및 분산
- 쌍극자 분극률
- 71.2 a.u.
- 쌍극자 분극률(불확도)
- 0.4 a.u.
- C₆
- 626 Ha·Bohr6
- C₆ (Gould–Bučko)
- 629 Ha·Bohr6
화학 친화력
- 양성자 친화도
- 819.6 kJ/mol
- 기체상 염기성
- 797.3 kJ/mol
미데마 매개변수
- 미데마 몰 부피
- 14 cm3/mol
- 미데마 전자 밀도
- 2
공급 위험 및 경제성
- 생산 집중도
- 64
- 상대적 공급 위험
- 7
- 매장량 분포
- 26
- 정치적 안정성(최대 생산국)
- 24
- 정치적 안정성(최대 매장국)
- 18
상전이 및 동소체
| 녹는점 | 923.15 K |
| 끓는점 | 1363.15 K |
산화 상태 분류
심화 참고 데이터
차폐 상수 (4)
| n | 오비탈 | σ |
|---|---|---|
| 1 | s | 0.3911 |
| 2 | p | 4.1742 |
| 2 | s | 4.608 |
| 3 | s | 8.6925 |
결정 반지름 상세 정보 (4)
| 전하 | CN | 스핀 | rcrystal (pm) | 기원 |
|---|---|---|---|---|
| 2 | IV | 71 | ||
| 2 | V | 80 | ||
| 2 | VI | 86 | ||
| 2 | VIII | 103 | calculated, |
동위원소 붕괴 방식 (43)
| 동위원소 | 모드 | 세기 |
|---|---|---|
| 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% |
X선 산란 인자 (755)
| 에너지 (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 |
추가 데이터
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.33×104 milligrams per kilogram
참고 문헌 (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
참고 문헌 (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.
참고 문헌 (1)
- [6] Magnesium https://periodic.lanl.gov/12.shtml
참고 문헌
(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.