Magnesium (Mg)
alkaline-earth-metalSolid
Standard Atomic Weight
24.305 u [24.304, 24.307]Electron configuration
[Ne] 3s2Melting point
649.85 °CBoiling point
1089.85 °CDensity
1740 kg/m³Oxidation states
0, +1, +2Electronegativity (Pauling)
1.31Ionization energy (1st)
7.646236 eVDiscovery year
1755Atomic radius
150 pmDetails
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.
Images
Properties
Physical
- Atomic radius (empirical)
- 150 pm Compare Atomic radius (empirical) of all elements →
- Covalent radius
- 141 pm Compare Covalent radius of all elements →
- Van der Waals radius
- 173 pm Compare Van der Waals radius of all elements →
- Metallic radius
- 136 pm Compare Metallic radius of all elements →
- Density
- 1740 kg/m³ Compare Density of all elements →
- Molar volume
- 0.014 L/mol
- Phase at STP
- Solid Compare Phase at STP of all elements →
- Melting point
- 649.85 °C Compare Melting point of all elements →
- Boiling point
- 1089.85 °C Compare Boiling point of all elements →
- Thermal conductivity
- 156 W/(m·K) Compare Thermal conductivity of all elements →
- Specific heat capacity
- 1.023 J/(g·K) Compare Specific heat capacity of all elements →
- Molar heat capacity
- 24.869 J/(mol·K) Compare Molar heat capacity of all elements →
- Crystal structure
- Hexagonal close-packed Compare Crystal structure of all elements →
Chemical
- Electronegativity (Pauling)
- 1.31 Compare Electronegativity (Pauling) of all elements →
- Electronegativity (Allen)
- 1.293
- Electron affinity
- -0.4 eV (negative value — the atom is not predicted to bind an extra electron)
- Ionization energy (1st)
- 7.646236 eV Compare Ionization energy (1st) of all elements →
- Ionization energy (2nd)
- 15.035323 eV Compare Ionization energy (2nd) of all elements →
- Ionization energy (3rd)
- 80.143876 eV Compare Ionization energy (3rd) of all elements →
- Ionization energy (4th)
- 109.265776 eV Compare Ionization energy (4th) of all elements →
- Ionization energy (5th)
- 141.330486 eV Compare Ionization energy (5th) of all elements →
- Oxidation states
- 0, +1, +2 Compare Oxidation states of all elements →
- Valence electrons
- 2 Compare Valence electrons of all elements →
- Electron configuration
- [Ne] 3s2
Thermodynamic
- Heat of fusion
- 0.08788931 eV Compare Heat of fusion of all elements →
- Heat of vaporization
- 1.326631 eV Compare Heat of vaporization of all elements →
- Heat of sublimation
- 1.524589 eV
- Heat of atomization
- 1.524589 eV
- Atomization enthalpy
- 1.524589 eV
Nuclear
- Protons
- 12 Compare Protons of all elements →
- Neutrons
- 12 Compare Neutrons of all elements →
- Known isotopes
- 23 Compare Known isotopes of all elements →
- Stable isotopes
- 3 Compare Stable isotopes of all elements →
- Most stable isotope
- Mg-24
- Discovery year
- 1755
Abundance
- Abundance (Earth's crust)
- 2.33e+4 mg/kg Compare Abundance (Earth's crust) of all elements →
- Abundance (ocean)
- 1290 mg/L Compare Abundance (ocean) of all elements →
Crystal Structure
- Lattice constant a
- 321 pm
Electronic Structure
- Electrons per shell
- 2, 8, 2 Compare Electrons per shell of all elements →
Identifiers
- CAS number
- 7439-95-4 Compare CAS number of all elements →
- Term symbol
- 1S0
- InChI
- InChI=1S/Mg
- InChI Key
- FYYHWMGAXLPEAU-UHFFFAOYSA-N
Electron Configuration Measured
Mg: 3s²[Ne] 3s²1s² 2s² 2p⁶ 3s²Atomic model
Isotopes change neutron count, mass, and stability — not the electron configuration of a neutral atom.
Schematic atomic model, not to scale.
Atomic Fingerprint
Emission / Absorption Spectrum
Isotope Distribution
| Mass number | Atomic mass (u) | Natural abundance | Half-life |
|---|---|---|---|
| 24 Stable | 23.985041697 ± 0.000000014 | 78.9900% | Stable |
| 25 Stable | 24.985836976 ± 0.00000005 | 10.0000% | Stable |
| 26 Stable | 25.982592968 ± 0.000000031 | 11.0100% | Stable |
Phase / State
Reason: 624.9 °C below melting point (649.85 °C)
Schematic, not to scale
Phase transition points
Transition energies
Energy required to melt 1 mol at melting point
Energy required to vaporize 1 mol at boiling point
Energy required to sublime 1 mol at sublimation point
Density
At standard conditions
At standard conditions
Atomic Spectra
Showing 10 of 12. Sorted by ion charge (ascending).
Lines Holdings ?
| Ion | Charge | Total lines | Transition probabilities | Level designations |
|---|---|---|---|---|
| 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 |
Levels Holdings ?
| Ion | Charge | Levels |
|---|---|---|
| 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 |
Ionic Radii
| Charge | Coordination | Spin | Radius |
|---|---|---|---|
| +2 | 4 | N/A | 56.99999999999999 pm |
| +2 | 5 | N/A | 66 pm |
| +2 | 6 | N/A | 72 pm |
| +2 | 8 | N/A | 89 pm |
Compounds
Isotopes (3)
| Mass number | Atomic mass (u) | Natural abundance | Half-life | Decay mode | |
|---|---|---|---|---|---|
| 24 Stable | 23.985041697 ± 0.000000014 | 78.9900% ± 0.0400% | Stable | stable | |
| 25 Stable | 24.985836976 ± 0.00000005 | 10.0000% ± 0.0100% | Stable | stable | |
| 26 Stable | 25.982592968 ± 0.000000031 | 11.0100% ± 0.0300% | Stable | stable |
Spectral Lines
Showing 50 of 399. Only spectral lines with measured intensity are shown by default.
| Wavelength (nm) | Intensity | Ion stage | Type | Transition | Accuracy | Source | |
|---|---|---|---|---|---|---|---|
| 518.36043 nm | 45 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | Measured | NIST | |
| 517.26844 nm | 44 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | Measured | NIST | |
| 516.73213 nm | 42 | Mg I | emission | 3s.3p 3P* → 3s.4s 3S | Measured | NIST | |
| 383.82919 nm | 40 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | Measured | NIST | |
| 552.84047 nm | 40 | Mg I | emission | 3s.3p 1P* → 3s.4d 1D | Measured | NIST | |
| 383.23039 nm | 38 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | Measured | NIST | |
| 382.93547 nm | 36 | Mg I | emission | 3s.3p 3P* → 3s.3d 3D | Measured | NIST | |
| 470.29908 nm | 30 | Mg I | emission | 3s.3p 1P* → 3s.5d 1D | Measured | NIST | |
| 571.1088 nm | 30 | Mg I | emission | 3s.3p 1P* → 3s.5s 1S | Measured | NIST | |
| 435.19057 nm | 20 | Mg I | emission | 3s.3p 1P* → 3s.6d 1D | Measured | NIST | |
| 416.72713 nm | 15 | Mg I | emission | 3s.3p 1P* → 3s.7d 1D | Measured | 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] | Measured | NIST | |
| 448.1126 nm | 14 | Mg II | emission | 2p6.3d 2D → 2p6.4f 2F* | Measured | NIST | |
| 448.1325 nm | 13 | Mg II | emission | 2p6.3d 2D → 2p6.4f 2F* | Measured | NIST | |
| 738.7689 nm | 12 | Mg I | emission | 3s.3d 1D → 3s.8f 1F* | Measured | NIST | |
| 405.75052 nm | 10 | Mg I | emission | 3s.3p 1P* → 3s.8d 1D | Measured | NIST | |
| 439.0572 nm | 10 | Mg II | emission | 2p6.4p 2P* → 2p6.5d 2D | Measured | NIST | |
| 473.00286 nm | 10 | Mg I | emission | 3s.3p 1P* → 3s.6s 1S | Measured | 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]* | Measured | 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] | Measured | NIST | |
| 631.8717 nm | 10 | Mg I | emission | 3s.4s 3S → 3s.6p 3P* | Measured | NIST | |
| 634.6742 nm | 10 | Mg II | emission | 2p6.4d 2D → 2p6.6f 2F* | Measured | NIST | |
| 719.3184 nm | 10 | Mg I | emission | 3s.3d 1D → 3s.9f 1F* | Measured | NIST | |
| 729.1055 nm | 10 | Mg I | emission | 3s.4s 1S → 3s.6p 1P* | Measured | NIST | |
| 438.4637 nm | 9 | Mg II | emission | 2p6.4p 2P* → 2p6.5d 2D | Measured | NIST | |
| 443.3988 nm | 9 | Mg II | emission | 2p6.4p 2P* → 2p6.6s 2S | Measured | 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]* | Measured | 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]* | Measured | 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]* | Measured | NIST | |
| 631.9237 nm | 9 | Mg I | emission | 3s.4s 3S → 3s.6p 3P* | Measured | NIST | |
| 634.6964 nm | 9 | Mg II | emission | 2p6.4d 2D → 2p6.6f 2F* | Measured | NIST | |
| 384.8211 nm | 8 | Mg II | emission | 2p6.3d 2D → 2p6.5p 2P* | Measured | NIST | |
| 398.67533 nm | 8 | Mg I | emission | 3s.3p 1P* → 3s.9d 1D | Measured | NIST | |
| 442.7994 nm | 8 | Mg II | emission | 2p6.4p 2P* → 2p6.6s 2S | Measured | 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] | Measured | 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]* | Measured | NIST | |
| 526.422 nm | 8 | Mg II | emission | 2p6.4d 2D → 2p6.7f 2F* | Measured | 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] | Measured | NIST | |
| 678.7855 nm | 8 | Mg II | emission | 2p6.5p 2P* → 2p6.7d 2D | Measured | NIST | |
| 681.927 nm | 8 | Mg II | emission | 2p6.5p 2P* → 2p6.8s 2S | Measured | NIST | |
| 706.0414 nm | 8 | Mg I | emission | 3s.3d 1D → 3s.10f 1F* | Measured | NIST | |
| 385.0386 nm | 7 | Mg II | emission | 2p6.3d 2D → 2p6.5p 2P* | Measured | 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] | Measured | 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]* | Measured | 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]* | Measured | 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]* | Measured | 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]* | Measured | 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]* | Measured | NIST | |
| 526.4364 nm | 7 | Mg II | emission | 2p6.4d 2D → 2p6.7f 2F* | Measured | NIST | |
| 591.6431 nm | 7 | Mg II | emission | 2p6.4d 2D → 2p6.7p 2P* | Measured | NIST |
Extended Properties
Covalent Radii (Extended)
- Covalent radius (Pyykkö)
- 139 pm
- Covalent radius (Pyykkö, double)
- 132 pm
- Covalent radius (Pyykkö, triple)
- 127 pm
- Covalent radius (Bragg)
- 142 pm
Van der Waals Radii
- Bondi
- 173 pm
- Batsanov
- 220 pm
- Alvarez
- 251 pm
- UFF
- 302.1 pm
- MM3
- 243 pm
Atomic & Metallic Radii
- Atomic radius (Rahm)
- 240 pm
- Metallic radius (C12)
- 160 pm
Numbering Scales
- Mendeleev
- 76
- Pettifor
- 73
- Glawe
- 73
Electronegativity Scales
- Ghosh
- 0
- Miedema
- 3
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 3
Polarizability & Dispersion
- Dipole polarizability
- 71.2 a.u.
- Dipole polarizability (unc.)
- 0.4 a.u.
- C₆
- 626 Ha·Bohr6
- C₆ (Gould–Bučko)
- 629 Ha·Bohr6
Chemical Affinity
- Proton affinity
- 819.6 kJ/mol
- Gas basicity
- 797.3 kJ/mol
Miedema Parameters
- Miedema molar volume
- 14 cm3/mol
- Miedema electron density
- 2
Supply Risk & Economics
- Production concentration
- 64
- Relative supply risk
- 7
- Reserve distribution
- 26
- Political stability (top producer)
- 24
- Political stability (top reserve)
- 18
Phase Transitions & Allotropes
| Melting point | 923.15 K |
| Boiling point | 1363.15 K |
Oxidation State Categories
Advanced Reference Data
Screening Constants (4)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0.3911 |
| 2 | p | 4.1742 |
| 2 | s | 4.608 |
| 3 | s | 8.6925 |
Crystal Radii Detail (4)
| Charge | CN | Spin | rcrystal (pm) | Origin |
|---|---|---|---|---|
| 2 | IV | 71 | ||
| 2 | V | 80 | ||
| 2 | VI | 86 | ||
| 2 | VIII | 103 | calculated, |
Isotope Decay Modes (43)
| Isotope | Mode | Intensity |
|---|---|---|
| 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‑ray Scattering Factors (755)
| Energy (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 |
Additional Data
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.33×104 milligrams per kilogram
References (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
References (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.
References (1)
- [6] Magnesium https://periodic.lanl.gov/12.shtml
References
(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.