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Magnesium
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Not to be confused with manganese (Mn).
Magnesium, 12Mg
General properties
Pronunciation
/mæɡˈniːziəm/ (mag-NEE-zee-əm)
Appearance
shiny grey solid
Standard atomic weight (Ar, standard)
[7001243040000000000♠24.304, 7001243070000000000♠24.307] conventional: 7001243050000000000♠24.305[1]
Magnesium in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
Be
↑
Mg
↓
Ca
sodium ← magnesium → aluminium
Atomic number (Z)
12
Group, period
group 2 (alkaline earth metals), period 3
Block
s-block
Element category
alkaline earth metal
Electron configuration
[Ne] 3s2
Electrons per shell
2, 8, 2
Physical properties
Phase (at STP)
solid
Melting point
923 K (650 °C, 1202 °F)
Boiling point
1363 K (1091 °C, 1994 °F)
Density (near r.t.)
1.738 g/cm3
when liquid (at m.p.)
1.584 g/cm3
Heat of fusion
8.48 kJ/mol
Heat of vaporization
128 kJ/mol
Molar heat capacity
24.869 J/(mol·K)
Vapor pressure
P (Pa)
1
10
100
1 k
10 k
100 k
at T (K)
701 773 861 971 1132 1361
Atomic properties
Oxidation states
+2, +1[2] (a strongly basic oxide)
Electronegativity
Pauling scale: 1.31
Ionization energies
1st: 737.7 kJ/mol
2nd: 1450.7 kJ/mol
3rd: 7732.7 kJ/mol
(more)
Atomic radius
empirical: 160 pm
Covalent radius
141±7 pm
Van der Waals radius
173 pm
Spectral lines
Miscellanea
Crystal structure
hexagonal close-packed (hcp)
Speed of sound thin rod
4940 m/s (at r.t.) (annealed)
Thermal expansion
24.8 µm/(m·K) (at 25 °C)
Thermal conductivity
156 W/(m·K)
Electrical resistivity
43.9 nΩ·m (at 20 °C)
Magnetic ordering
paramagnetic
Magnetic susceptibility
+13.1·10−6 cm3/mol (298 K)[3]
Young's modulus
45 GPa
Shear modulus
17 GPa
Bulk modulus
35.4[4] GPa
Poisson ratio
0.290
Mohs hardness
1–2.5
Brinell hardness
44–260 MPa
CAS Number
7439-95-4
History
Naming
after Magnesia, Greece
Discovery
Joseph Black (1755)
First isolation
Humphry Davy (1808)
Main isotopes of magnesium
Isotope
Abundance
Half-life (t1/2)
Decay mode
Product
24Mg
79.0% stable
25Mg
10.0% stable
26Mg
11.0% stable
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Magnesium is a chemical element with symbol Mg and atomic number 12. It is a shiny gray solid which bears a close physical resemblance to the other five elements in the second column (group 2, or alkaline earth metals) of the periodic table: all group 2 elements have the same electron configuration in the outer electron shell and a similar crystal structure.
Magnesium is the ninth most abundant element in the universe.[5][6] It is produced in large, aging stars from the sequential addition of three helium nuclei to a carbon nucleus. When such stars explode as supernovas, much of the magnesium is expelled into the interstellar medium where it may recycle into new star systems. Magnesium is the eighth most abundant element in the Earth's crust[7] and the fourth most common element in the Earth (after iron, oxygen and silicon), making up 13% of the planet's mass and a large fraction of the planet's mantle. It is the third most abundant element dissolved in seawater, after sodium and chlorine.[8]
Magnesium occurs naturally only in combination with other elements, where it invariably has a +2 oxidation state. The free element (metal) can be produced artificially, and is highly reactive (though in the atmosphere, it is soon coated in a thin layer of oxide that partly inhibits reactivity — see passivation). The free metal burns with a characteristic brilliant-white light. The metal is now obtained mainly by electrolysis of magnesium salts obtained from brine, and is used primarily as a component in aluminium-magnesium alloys, sometimes called magnalium or magnelium. Magnesium is less dense than aluminium, and the alloy is prized for its combination of lightness and strength.
Magnesium is the eleventh most abundant element by mass in the human body and is essential to all cells and some 300 enzymes.[9] Magnesium ions interact with polyphosphate compounds such as ATP, DNA, and RNA. Hundreds of enzymes require magnesium ions to function. Magnesium compounds are used medicinally as common laxatives, antacids (e.g., milk of magnesia), and to stabilize abnormal nerve excitation or blood vessel spasm in such conditions as eclampsia.[9]
Contents
[hide]
1 Characteristics
1.1 Physical properties
1.2 Chemical properties
1.2.1 Flammability
1.2.2 Source of light
1.3 Occurrence
2 Forms
2.1 Alloy
2.1.1 Corrosion
2.1.2 High-temperature creep and flammability
2.2 Compounds
2.3 Isotopes
3 Production
4 History
5 Uses as a metal
5.1 Aircraft
5.2 Automotive
5.3 Electronics
5.4 Other
5.5 Safety precautions
6 Useful compounds
7 Biological roles
7.1 Mechanism of action
7.2 Dietary sources, recommended intake, and supplementation
7.3 Metabolism
7.4 Detection in serum and plasma
7.5 Deficiency
7.6 Therapy
7.7 Overdose
7.8 Function in plants
8 See also
9 Notes
10 References
11 External links
Characteristics
Physical properties
Elemental magnesium is a gray-white lightweight metal, two-thirds the density of aluminium. It tarnishes slightly when exposed to air, although, unlike the other alkaline earth metals, an oxygen-free environment is unnecessary for storage because magnesium is protected by a thin layer of oxide that is fairly impermeable and difficult to remove. Magnesium has the lowest melting (923 K (1,202 °F)) and the lowest boiling point 1,363 K (1,994 °F) of all the alkaline earth metals.
Magnesium reacts with water at room temperature, though it reacts much more slowly than calcium, a similar group 2 metal. When submerged in water, hydrogen bubbles form slowly on the surface of the metal—though, if powdered, it reacts much more rapidly. The reaction occurs faster with higher temperatures (see #Precautions). Magnesium's reversible reaction with water can be harnessed to store energy and run a magnesium-based engine.
Magnesium also reacts exothermically with most acids such as hydrochloric acid (HCl), producing the metal chloride and hydrogen gas, similar to the HCl reaction with aluminium, zinc, and many other metals.
Chemical properties
Flammability
Magnesium is highly flammable, especially when powdered or shaved into thin strips, though it is difficult to ignite in mass or bulk. Flame temperatures of magnesium and magnesium alloys can reach 3,100 °C (5,610 °F),[10] although flame height above the burning metal is usually less than 300 mm (12 in).[11] Once ignited, such fires are difficult to extinguish, with combustion continuing in nitrogen (forming magnesium nitride), carbon dioxide (forming magnesium oxide and carbon), and water (forming magnesium oxide and hydrogen). This property was used in incendiary weapons during the firebombing of cities in World War II, where the only practical civil defense was to smother a burning flare under dry sand to exclude atmosphere from the combustion.
Magnesium may also be used as an igniter for thermite, a mixture of aluminium and iron oxide powder that ignites only at a very high temperature.
Source of light
When burning in air, magnesium produces a brilliant-white light that includes strong ultraviolet wavelengths. Magnesium powder (flash powder) was used for subject illumination in the early days of photography.[12][13] Later, magnesium filament was used in electrically ignited single-use photography flashbulbs. Magnesium powder is used in fireworks and marine flares where a brilliant white light is required. It was also used for various theatrical effects,[14] such as lightning,[15] pistol flashes,[16] and supernatural appearances.[17]
Occurrence
See also: Category:Magnesium minerals.
Magnesium is the eighth-most-abundant element in the Earth's crust by mass and tied in seventh place with iron in molarity.[7] It is found in large deposits of magnesite, dolomite, and other minerals, and in mineral waters, where magnesium ion is soluble.
Although magnesium is found in more than 60 minerals, only dolomite, magnesite, brucite, carnallite, talc, and olivine are of commercial importance.
The Mg2+
cation is the second-most-abundant cation in seawater (about ⅛ the mass of sodium ions in a given sample), which makes seawater and sea salt attractive commercial sources for Mg. To extract the magnesium, calcium hydroxide is added to seawater to form magnesium hydroxide precipitate.
MgCl
2 + Ca(OH)
2 → Mg(OH)
2 + CaCl
2
Magnesium hydroxide (brucite) is insoluble in water and can be filtered out and reacted with hydrochloric acid to produced concentrated magnesium chloride.
Mg(OH)
2 + 2 HCl → MgCl
2 + 2 H
2O
From magnesium chloride, electrolysis produces magnesium.
Forms
Alloy
As of 2013, magnesium alloy consumption was less than one million tons per year, compared with 50 million tons of aluminum alloys. Its use has been historically limited by its tendency to corrode, creep at high temperatures, and combust.[18]
Corrosion
The presence of iron, nickel, copper, and cobalt strongly activates corrosion. Greater than a very small percentage, these metals precipitate as intermetallic compounds, and the precipitate locales function as active cathodic sites that reduce water, causing the loss of magnesium.[18] Controlling the quantity of these metals improves corrosion resistance. Sufficient manganese overcomes the corrosive effects of iron. This requires precise control over composition, increasing costs.[18] Adding a cathodic poison captures atomic hydrogen within the structure of a metal. This prevents the formation of free hydrogen gas, an essential factor of corrosive chemical processes. The addition of about one in three hundred parts arsenic reduces its corrosion rate in a salt solution by a factor of nearly ten.[18][19]
High-temperature creep and flammability
Research showed that magnesium's tendency to creep at high-temperatures is eliminated by the addition of scandium and gadolinium. Flammability is greatly reduced by a small amount of calcium in the alloy.[18]
Compounds
Magnesium forms a variety of compounds important to industry and biology, including magnesium carbonate, magnesium chloride, magnesium citrate, magnesium hydroxide (milk of magnesia), magnesium oxide, magnesium sulfate, and magnesium sulfate heptahydrate (Epsom salts).
Isotopes
Main article: Isotopes of magnesium
Magnesium has three stable isotopes: 24
Mg, 25
Mg and 26
Mg. All are present in significant amounts (see table of isotopes above). About 79% of Mg is 24
Mg. The isotope 28
Mg is radioactive and in the 1950s to 1970s was produced by several nuclear power plants for use in scientific experiments. This isotope has a relatively short half-life (21 hours) and its use was limited by shipping times.
The nuclide 26
Mg has found application in isotopic geology, similar to that of aluminium. 26
Mg is a radiogenic daughter product of 26
Al, which has a half-life of 717,000 years. Excessive quantities of stable 26
Mg have been observed in the Ca-Al-rich inclusions of some carbonaceous chondrite meteorites. This anomalous abundance is attributed to the decay of its parent 26
Al in the inclusions, and researchers conclude that such meteorites were formed in the solar nebula before the 26
Al had decayed. These are among the oldest objects in the solar system and contain preserved information about its early history.
It is conventional to plot 26
Mg/24
Mg against an Al/Mg ratio. In an isochron dating plot, the Al/Mg ratio plotted is27
Al/24
Mg. The slope of the isochron has no age significance, but indicates the initial 26
Al/27
Al ratio in the sample at the time when the systems were separated from a common reservoir.
Production
Country
2011 production
(tonnes)[20]
China 661,000
U.S.[note 1] 63,500
Russia 37,000
Israel 30,000
Kazakhstan 21,000
Brazil 16,000
Ukraine 2,000
Serbia 1,500
Total 832,000
Magnesium sheets and ingots
China is the dominant supplier of magnesium, with approximately 80% of the world market share. China is almost completely reliant on the silicothermic Pidgeon process (the reduction of the oxide at high temperatures with silicon, often provided by a ferrosilicon alloy in which the iron is but a spectator in the reactions) to obtain the metal.[21] The process can also be carried out with carbon at approx 2300 °C:
2MgO
(s) + Si
(s) + 2CaO
(s) → 2Mg
(g) + Ca
2SiO
4(s)
MgO
(s) + C
(s) → Mg
(g) + CO
(g)
In the United States, magnesium is obtained principally with the Dow process, by electrolysis of fused magnesium chloride from brine and sea water. A saline solution containing Mg2+
ions is first treated with lime (calcium oxide) and the precipitated magnesium hydroxide is collected:
Mg2+
(aq) + CaO
(s) + H
2O → Ca2+
(aq) + Mg(OH)
2(s)
The hydroxide is then converted to a partial hydrate of magnesium chloride by treating the hydroxide with hydrochloric acid and heating of the product:
Mg(OH)
2(s) + 2 HCl → MgCl
2(aq) + 2H
2O
(l)
The salt is then electrolyzed in the molten state. At the cathode, the Mg2+
ion is reduced by two electrons to magnesium metal:
Mg2+
+ 2
e−
→ Mg
At the anode, each pair of Cl−
ions is oxidized to chlorine gas, releasing two electrons to complete the circuit:
2 Cl−
→ Cl
2 (g) + 2
e−
A new process, solid oxide membrane technology, involves the electrolytic reduction of MgO. At the cathode, Mg2+
ion is reduced by two electrons to magnesium metal. The electrolyte is Yttria-stabilized zirconia (YSZ). The anode is a liquid metal. At the YSZ/liquid metal anode O2−
is oxidized. A layer of graphite borders the liquid metal anode, and at this interface carbon and oxygen react to form carbon monoxide. When silver is used as the liquid metal anode, there is no reductant carbon or hydrogen needed, and only oxygen gas is evolved at the anode.[22] It has been reported that this method provides a 40% reduction in cost per pound over the electrolytic reduction method.[23] This method is more environmentally sound than others because there is much less carbon dioxide emitted.
The United States has traditionally been the major world supplier of this metal, supplying 45% of world production even as recently as 1995. Today, the US market share is at 7%, with a single domestic producer left, US Magnesium, a Renco Group company in Utah born from now-defunct Magcorp.[24]
History
The name magnesium originates from the Greek word for a district in Thessaly called Magnesia.[25] It is related to magnetite and manganese, which also originated from this area, and required differentiation as separate substances. See manganese for this history.
In 1618, a farmer at Epsom in England attempted to give his cows water from a well there. The cows refused to drink because of the water's bitter taste, but the farmer noticed that the water seemed to heal scratches and rashes. The substance became known as Epsom salts and its fame spread.[citation needed] It was eventually recognized as hydrated magnesium sulfate, MgSO
4·7 H
2O.
The metal itself was first isolated by Sir Humphry Davy in England in 1808. He used electrolysis on a mixture of magnesia and mercuric oxide.[26] Antoine Bussy prepared it in coherent form in 1831. Davy's first suggestion for a name was magnium,[26] but the name magnesium is now used.
Uses as a metal
An unusual application of magnesium as an illumination source while wakeskating in 1931
Magnesium is the third-most-commonly-used structural metal, following iron and aluminium.[27]
The main applications of magnesium are, in order: aluminium alloys, die-casting (alloyed with zinc),[28] removing sulfur in the production of iron and steel, and the production of titanium in the Kroll process.[29]
Magnesium is used in super-strong, lightweight materials and alloys. For example, when infused with silicon carbide nanoparticles, it has extremely high specific strength.[30]
Historically, magnesium was one of the main aerospace construction metals and was used for German military aircraft as early as World War I and extensively for German aircraft in World War II.
The Germans coined the name "Elektron" for magnesium alloy, a term which is still used today. In the commercial aerospace industry, magnesium was generally restricted to engine-related components, due fire and corrosion hazards. Currently, magnesium alloy use in aerospace is increasing, driven by the importance of fuel economy.[31] Development and testing of new magnesium alloys continues, notably Elektron 21, which (in test) has proved suitable for aerospace engine, internal, and airframe components.[32] The European Community runs three R&D magnesium projects in the Aerospace priority of Six Framework Program.
In the form of thin ribbons, magnesium is used to purify solvents; for example, preparing super-dry ethanol.
Aircraft
Wright Aeronautical used a magnesium crankcase in the WWII-era Wright Duplex Cyclone aviation engine. This presented a serious problem for the earliest models of the Boeing B-29 heavy bomber when an in-flight engine fire ignited the engine crankcase. The resulting combustion was as hot as 5,600 °F (3,100 °C) and could sever the wing spar from the fuselage.[33][34][35]
Automotive
Mg alloy motorcycle engine blocks
Mercedes-Benz used the alloy Elektron in the body of an early model Mercedes-Benz 300 SLR; these cars ran (with successes) at Le Mans, the Mille Miglia, and other world-class race events in 1955.
Porsche used magnesium alloy frames in the 917/053 that won Le Mans in 1971, and continues to use magnesium alloys for its engine blocks due to the weight advantage.
Volkswagen Group has used magnesium in its engine components for many years.[citation needed]
Mitsubishi Motors uses magnesium for its paddle shifters.
BMW used magnesium alloy blocks in their N52 engine, including an aluminium alloy insert for the cylinder walls and cooling jackets surrounded by a high-temperature magnesium alloy AJ62A. The engine was used worldwide between 2005 and 2011 in various 1, 3, 5, 6, and 7 series models; as well as the Z4, X1, X3, and X5.
Chevrolet used the magnesium alloy AE44 in the 2006 Corvette Z06.
Both AJ62A and AE44 are recent developments in high-temperature low-creep magnesium alloys. The general strategy for such alloys is to form intermetallic precipitates at the grain boundaries, for example by adding mischmetal or calcium.[36] New alloy development and lower costs that make magnesium competitive with aluminium will increase the number of automotive applications.
Electronics
Because of low weight and good mechanical and electrical properties, magnesium is widely used for manufacturing of mobile phones, laptop and tablet computers, cameras, and other electronic components.
Products made of magnesium: firestarter and shavings, sharpener, magnesium ribbon
Other
Magnesium, being readily available and relatively nontoxic, has a variety of uses:
Magnesium is flammable, burning at a temperature of approximately 3,100 °C (3,370 K; 5,610 °F),[10] and the autoignition temperature of magnesium ribbon is approximately 473 °C (746 K; 883 °F).[37] It produces intense, bright, white light when it burns. Magnesium's high combustion temperature makes it a useful tool for starting emergency fires. Other uses include flash photography, flares, pyrotechnics, and fireworks sparklers. Magnesium is also often used to ignite thermite or other materials that require a high ignition temperature.
Magnesium firestarter (in left hand), used with a pocket knife and flint to create sparks that ignite the shavings
In the form of turnings or ribbons, to prepare Grignard reagents, which are useful in organic synthesis.
As an additive agent in conventional propellants and the production of nodular graphite in cast iron.
As a reducing agent to separate uranium and other metals from their salts.
As a sacrificial (galvanic) anode to protect boats, underground tanks, pipelines, buried structures, and water heaters.
Alloyed with zinc to produce the zinc sheet used in photoengraving plates in the printing industry, dry-cell battery walls, and roofing.[28]
As a metal, this element's principal use is as an alloying additive to aluminium with these aluminium-magnesium alloys being used mainly for beverage cans, sports equipment such as golf clubs, fishing reels, and archery bows and arrows.
Specialty, high-grade car wheels of magnesium alloy are called "mag wheels", although the term is often misapplied to aluminium wheels. Many car and aircraft manufacturers have made engine and body parts from magnesium.
Magnesium batteries have been commercialized as primary batteries, and are an active topic of research for rechargeable secondary batteries.
Safety precautions
Play media
Magnesium block heated with blowtorch to self-combustion, emitting intense white light
Magnesium metal and its alloys can be explosive hazards; they are highly flammable in their pure form when molten or in powder or ribbon form. Burning or molten magnesium reacts violently with water. When working with powdered magnesium, safety glasses with eye protection and UV filters (such as welders use) are employed because burning magnesium produces ultraviolet light that can permanently damage the retina of a human eye.[38]
Magnesium is capable of reducing water and releasing highly flammable hydrogen gas:[39]
Mg (s) + 2 H
2O (l) → Mg(OH)
2 (s) + H
2 (g)
Therefore, water cannot extinguish magnesium fires. The hydrogen gas produced intensifies the fire. Dry sand is an effective smothering agent, but only on relatively level and flat surfaces.
Magnesium reacts with carbon dioxide exothermically to form magnesium oxide and carbon:[40]
2 Mg + CO
2 → 2 MgO + C (s)
Hence, carbon dioxide fuels rather than extinguishes magnesium fires.
Burning magnesium can be quenched by using a Class D dry chemical fire extinguisher, or by covering the fire with sand or magnesium foundry flux[citation needed] to remove its air source.
Useful compounds
Magnesium compounds, primarily magnesium oxide (MgO), are used as a refractory material in furnace linings for producing iron, steel, nonferrous metals, glass, and cement. Magnesium oxide and other magnesium compounds are also used in the agricultural, chemical, and construction industries. Magnesium oxide from calcination is used as an electrical insulator in fire-resistant cables.[41]
Magnesium reacted with an alkyl halide gives a Grignard reagent, which is a very useful tool for preparing alcohols.
Magnesium salts are included in various foods, fertilizers (magnesium is a component of chlorophyll), and microbe culture media.
Magnesium sulfite is used in the manufacture of paper (sulfite process).
Magnesium phosphate is used to fireproof wood used in construction.
Magnesium hexafluorosilicate is used for moth-proofing textiles.
Biological roles
Main article: Magnesium in biology
Mechanism of action
The important interaction between phosphate and magnesium ions makes magnesium essential to the basic nucleic acid chemistry of all cells of all known living organisms. More than 300 enzymes require magnesium ions for their catalytic action, including all enzymes using or synthesizing ATP and those that use other nucleotides to synthesize DNA and RNA. The ATP molecule is normally found in a chelate with a magnesium ion.[42]
Dietary sources, recommended intake, and supplementation
Examples of food sources of magnesium
Spices, nuts, cereals, cocoa and vegetables are rich sources of magnesium.[9] Green leafy vegetables such as spinach are also rich in magnesium.[43]
In the UK, the recommended daily values for magnesium is 300 mg for men and 270 mg for women.[44] In the U.S. the Recommended Dietary Allowances (RDAs) are 400 mg for men ages 19–30 and 420 mg for older; for women 310 mg for ages 19–30 and 320 mg for older.[45]
Numerous pharmaceutical preparations of magnesium and dietary supplements are available. In two human trials magnesium oxide, one of the most common forms in magnesium dietary supplements because of its high magnesium content per weight, was less bioavailable than magnesium citrate, chloride, lactate or aspartate.[46][47]
Metabolism
An adult has 22–26 grams of magnesium,[9][48] with 60% in the skeleton, 39% intracellular (20% in skeletal muscle), and 1% extracellular.[9] Serum levels are typically 0.7–1.0 mmol/L or 1.8–2.4 mEq/L. Serum magnesium levels may be normal even when intracellular magnesium is deficient. The mechanisms for maintaining the magnesium level in the serum are varying gastrointestinal absorption and renal excretion. Intracellular magnesium is correlated with intracellular potassium. Increased magnesium lowers calcium[49] and can either prevent hypercalcemia or cause hypocalcemia depending on the initial level.[49] Both low and high protein intake conditions inhibit magnesium absorption, as does the amount of phosphate, phytate, and fat in the gut. Unabsorbed dietary magnesium is excreted in feces; absorbed magnesium is excreted in urine and sweat.[50]
Detection in serum and plasma
Magnesium status may be assessed by measuring serum and erythrocyte magnesium concentrations coupled with urinary and fecal magnesium content, but intravenous magnesium loading tests are more accurate and practical.[51] A retention of 20% or more of the injected amount indicates deficiency.[52] No biomarker has been established for magnesium.[53]
Magnesium concentrations in plasma or serum may be monitored for efficacy and safety in those receiving the drug therapeutically, to confirm the diagnosis in potential poisoning victims, or to assist in the forensic investigation in a case of fatal overdose. The newborn children of mothers who received parenteral magnesium sulfate during labor may exhibit toxicity with normal serum magnesium levels.[54]
Deficiency
Low plasma magnesium (hypomagnesemia) is common: it is found in 2.5–15% of the general population.[55] The primary cause of deficiency is low dietary intake: fewer than 10% of people in the United States meet the recommended dietary allowance. Other causes are increased renal or gastrointestinal loss, an increased intracellular shift, and proton-pump inhibitor antacid therapy. Most are asymptomatic, but symptoms referable to neuromuscular, cardiovascular, and metabolic dysfunction may occur.[55] Alcoholism is often associated with magnesium deficiency. Chronically low serum magnesium levels are associated with metabolic syndrome, diabetes mellitus type 2, fasciculation, and hypertension.[56]
Therapy
Intravenous magnesium is recommended by the ACC/AHA/ESC 2006 Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death for patients with ventricular arrhythmia associated with torsades de pointes who present with long QT syndrome; and for the treatment of patients with digoxin induced arrhythmias.[57]
Magnesium sulfate - intravenous - is used for the management of pre-eclampsia and eclampsia.[58][59]
Hypomagnesemia, including that caused by alcoholism, is reversible by oral or parenteral magnesium administration depending on the degree of deficiency.[60]
There is limited evidence that magnesium supplementation may play a role in the prevention and treatment of migraine.[61]
Sorted by type of magnesium salt, other therapeutic applications include:
Magnesium sulfate, as the heptahydrate called Epsom salts, is used as bath salts, a laxative, and a highly soluble fertilizer.[62]
Magnesium hydroxide, suspended in water, is used in milk of magnesia antacids and laxatives.
Magnesium chloride, oxide, gluconate, malate, orotate, glycinate, ascorbate and citrate are all used as oral magnesium supplements.
Magnesium borate, magnesium salicylate, and magnesium sulfate are used as antiseptics.
Magnesium bromide is used as a mild sedative (this action is due to the bromide, not the magnesium).
Magnesium stearate is a slightly flammable white powder with lubricating properties. In pharmaceutical technology, it is used in pharmacological manufacture to prevent tablets from sticking to the equipment while compressing the ingredients into tablet form.
Magnesium carbonate powder is used by athletes such as gymnasts, weightlifters, and climbers to eliminate palm sweat, prevent sticking, and improve the grip on gymnastic apparatus, lifting bars, and climbing rocks.
Overdose
Overdose from dietary sources alone is unlikely because excess magnesium in the blood is promptly filtered by the kidneys,[55] and overdose is more likely in the presence of impaired renal function. In spite of this, megadose therapy has caused death in a young child,[63] and severe hypermagnesemia in a woman[64] and a young girl[65] who had healthy kidneys. The most common symptoms of overdose are nausea, vomiting, and diarrhea; other symptoms include hypotension, confusion, slowed heart and respiratory rate, deficiencies of other minerals, coma, cardiac arrhythmia, and death from cardiac arrest.[49]
Function in plants
Plants require magnesium to synthesize chlorophyll, essential for photosynthesis. Magnesium in the center of the porphyrin ring in chlorophyll functions in a manner similar to the iron in the center of the porphyrin ring in heme. Magnesium deficiency in plants causes late-season yellowing between leaf veins, especially in older leaves, and can be corrected by either applying epsom salts (which is rapidly leached), or crushed dolomitic limestone, to the soil.
See also
List of countries by magnesium production
Magnesium oil
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Notes
Jump up ^ Capacity. Production figures withheld to avoid disclosing company proprietary data.
References
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Jump up ^ Bernath, P. F.; Black, J. H. & Brault, J. W. (1985). "The spectrum of magnesium hydride" (PDF). Astrophysical Journal. 298: 375. Bibcode:1985ApJ...298..375B. doi:10.1086/163620.
Jump up ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
Jump up ^ K. A. Gschneider, Solid State Phys. 16, 308 (1964)
Jump up ^ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. pp. 305–306. ISBN 978-0131755536.
Jump up ^ Ash, Russell (2005). The Top 10 of Everything 2006: The Ultimate Book of Lists. Dk Pub. ISBN 0-7566-1321-3. Archived from the original on 2006-10-05.
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^ Jump up to: a b c d e "Dietary Supplement Fact Sheet: Magnesium". Office of Dietary Supplements, US National Institutes of Health. 11 February 2016. Retrieved 13 October 2016.
^ Jump up to: a b Dreizin, Edward L.; Berman, Charles H. & Vicenzi, Edward P. (2000). et al Combustion%26Flame2000.pdf "Condensed-phase modifications in magnesium particle combustion in air" Check |url= value (help) (PDF). Scripta Materialia. 122: 30–42. doi:10.1016/S0010-2180(00)00101-2.
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^ Jump up to: a b Baker, Hugh D. R.; Avedesian, Michael (1999). Magnesium and magnesium alloys. Materials Park, OH: Materials Information Society. p. 4. ISBN 0-87170-657-1.
Jump up ^ Ketil Amundsen; Terje Kr. Aune; Per Bakke; Hans R. Eklund; Johanna Ö. Haagensen; Carlos Nicolas; et al. (2002). "Magnesium". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a15_559. ISBN 3527306730.
Jump up ^ "UCLA researchers create super-strong magnesium metal". ucla.edu.
Jump up ^ Aghion, E.; Bronfin, B. (2000). "Magnesium Alloys Development towards the 21st Century". Materials Science Forum. 350–351: 19–30. doi:10.4028/www.scientific.net/MSF.350-351.19.
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Jump up ^ Dreizin, Edward L.; Berman, Charles H.; Vicenzi, Edward P. (2000). "Condensed-phase modifications in magnesium particle combustion in air". Scripta Materialia. 122: 30–42. doi:10.1016/S0010-2180(00)00101-2.
Jump up ^ Dorr, Robert F. (15 September 2012). Mission to Tokyo: The American Airmen Who Took the War to the Heart of Japan. pp. 40–41. ISBN 9781610586634.
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Jump up ^ Luo, Alan A. & Powell, Bob R. (2001). "Tensile and Compressive Creep of Magnesium-Aluminum-Calcium Based Alloys" (PDF). Materials & Processes Laboratory, General Motors Research & Development Center. Archived from the original (PDF) on 28 September 2007. Retrieved 21 August 2007.
Jump up ^ "Magnesium (Powder)". International Programme on Chemical Safety (IPCS). IPCS INCHEM. April 2000. Retrieved 21 December 2011.
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Jump up ^ Linsley, Trevor (2011). "Properties of conductors and insulators". Basic Electrical Installation Work. p. 362. ISBN 978-0-08-096628-1.
Jump up ^ Romani, Andrea, M.P. (2013). "Chapter 3. Magnesium in Health and Disease". In Astrid Sigel; Helmut Sigel; Roland K. O. Sigel. Interrelations between Essential Metal Ions and Human Diseases. Metal Ions in Life Sciences. 13. Springer. pp. 49–79. doi:10.1007/978-94-007-7500-8_3.
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Jump up ^ Firoz M; Graber M (2001). "Bioavailability of US commercial magnesium preparations". Magnes Res. 14 (4): 257–62. PMID 11794633.
Jump up ^ Lindberg JS; Zobitz MM; Poindexter JR; Pak CY (1990). "Magnesium bioavailability from magnesium citrate and magnesium oxide". J Am Coll Nutr. 9 (1): 48–55. doi:10.1080/07315724.1990.10720349. PMID 2407766.
Jump up ^ Saris NE, Mervaala E, Karppanen H, Khawaja JA, Lewenstam A (April 2000). "Magnesium. An update on physiological, clinical and analytical aspects". Clin Chim Acta. 294 (1-2): 1–26. PMID 10727669.
^ Jump up to: a b c "Magnesium | University of Maryland Medical Center". Umm.edu. 7 May 2013. Retrieved 19 September 2013.
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Jump up ^ Arnaud MJ (2008). "Update on the assessment of magnesium status". Br. J. Nutr. 99 Suppl 3: S24–36. doi:10.1017/S000711450800682X. PMID 18598586.
Jump up ^ Rob PM; Dick K; Bley N; Seyfert T; Brinckmann C; Höllriegel V; et al. (1999). "Can one really measure magnesium deficiency using the short-term magnesium loading test?". J. Intern. Med. 246 (4): 373–378. doi:10.1046/j.1365-2796.1999.00580.x. PMID 10583708.
Jump up ^ Franz KB (2004). "A functional biological marker is needed for diagnosing magnesium deficiency". J Am Coll Nutr. 23 (6): 738S–41S. doi:10.1080/07315724.2004.10719418. PMID 15637224.
Jump up ^ Baselt, R. (2008). Disposition of Toxic Drugs and Chemicals in Man (8th ed.). Biomedical Publications. pp. 875–7. ISBN 0-9626523-7-7.
^ Jump up to: a b c Ayuk J.; Gittoes N.J. (Mar 2014). "Contemporary view of the clinical relevance of magnesium homeostasis". Annals of Clinical Biochemistry. 51 (2): 179–88. doi:10.1177/0004563213517628.
Jump up ^ Geiger H; Wanner C (2012). "Magnesium in disease" (PDF). Clin Kidney J. 5 (Suppl 1): i25–i38. doi:10.1093/ndtplus/sfr165.
Jump up ^ Zipes DP; Camm AJ; Borggrefe M; et al. (2012). "ACC/AHA/ESC 2006 Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death: a report of the American College of Cardiology/American Heart Association Task Force and the European Society of Cardiology Committee for Practice Guidelines (writing committee to develop Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death): developed in collaboration with the European Heart Rhythm Association and the Heart Rhythm Society" (PDF). Circulation. 114 (10): e385–e484. doi:10.1161/CIRCULATIONAHA.106.178233. PMID 16935995.
Jump up ^ James MF (2010). "Magnesium in obstetrics". Best Pract Res Clin Obstet Gynaecol. 24 (3): 327–337. doi:10.1016/j.bpobgyn.2009.11.004. PMID 20005782.
Jump up ^ Euser, A. G.; Cipolla, M. J. (2009). "Magnesium Sulfate for the Treatment of Eclampsia: A Brief Review". Stroke. 40 (4): 1169–1175. doi:10.1161/STROKEAHA.108.527788. PMC 2663594  . PMID 19211496.
Jump up ^ Giannini, A. J. (1997). Drugs of Abuse (Second ed.). Los Angeles: Physicians Management Information Co. ISBN 0-87489-499-9.
Jump up ^ Teigen L, Boes CJ (2014). "An evidence-based review of oral magnesium supplementation in the preventive treatment of migraine". Cephalalgia (Review). doi:10.1177/0333102414564891. PMID 25533715. There is a strong body of evidence demonstrating a relationship between magnesium status and migraine. Magnesium likely plays a role in migraine development at a biochemical level, but the role of oral magnesium supplementation in migraine prophylaxis and treatment remains to be fully elucidated. The strength of evidence supporting oral magnesium supplementation is limited at this time.
Jump up ^ Gowariker, Vasant; Krishnamurthy, V. P.; Gowariker, Sudha; Dhanorkar, Manik; Paranjape, Kalyani (8 April 2009). The Fertilizer Encyclopedia. p. 224. ISBN 9780470431764.
Jump up ^ McGuire, John; Kulkarni, Mona Shah; Baden, Harris (February 2000). "Fatal Hypermagnesemia in a Child Treated With Megavitamin/Megamineral Therapy". Pediatrics. 105 (2). PMID 10654978. Retrieved 1 February 2017.
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Jump up ^ Kutsal, Ebru; Aydemir, Cumhur; Eldes, Nilufer; Demirel, Fatma; Polat, Recep; Taspınar, Ozan; Kulah, Eyup (February 2000). "Severe Hypermagnesemia as a Result of Excessive Cathartic Ingestion in a Child Without Renal Failure". Pediatrics. 205 (2): 570–572. doi:10.1097/PEC.0b013e31812eef1c. PMID 17726419.
External links
Magnesium at The Periodic Table of Videos (University of Nottingham)
Chemistry in its element podcast (MP3) from the Royal Society of Chemistry's Chemistry World: Magnesium
"Magnesium – a versatile and often overlooked element: new perspectives with a focus on chronic kidney disease". Clin Kidney J. 5 (Suppl 1). February 2012.
[hide]
v
t
e
Periodic table
(Large cells)
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
1
H He
2
Li Be B C N O F Ne
3
Na Mg Al Si P S Cl Ar
4
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6
Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7
Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
Alkali metal Alkaline earth metal Lanthanide Actinide Transition metal Post-transition metal Metalloid Polyatomic nonmetal Diatomic nonmetal Noble gas Unknown
chemical
properties
[show]
v
t
e
Magnesium compounds
MgB2
MgBr2
MgCO3
MgC2O4
MgC6H6O7
MgC14H10O4
MgCl2
Mg(ClO4)2
MgF2
MgH2
Mg(HCO3)2
MgI2
Mg(NO3)2
MgO
MgO2
Mg(OH)2
MgPo
MgS
MgSO3
MgSO4
MgU2O7
Mg2Al3
Mg2Si
Mg2SiO4
Mg2Si3O8
Mg3N2
Mg3(PO4)2
Mg2(CrO4)2
[show]
v
t
e
Ionotropic glutamate receptor modulators
AMPAR
Agonists: Main site agonists: 5-Fluorowillardiine
Acromelic acid (acromelate)
AMPA
BOAA
Domoic acid
Glutamate
Ibotenic acid
Proline
Quisqualic acid
Willardiine; Positive allosteric modulators: Aniracetam
Cyclothiazide
CX-516
CX-546
CX-614
Farampator (CX-691, ORG-24448)
CX-717
CX-1739
CX-1942
Diazoxide
Hydrochlorothiazide (HCTZ)
IDRA-21
LY-392098
LY-395153
LY-404187
LY-451646
LY-503430
Mibampator (LY-451395)
Nooglutyl
ORG-26576
Oxiracetam
PEPA
PF-04958242
Piracetam
Pramiracetam
S-18986
Tulrampator (S-47445, CX-1632)
Antagonists: ACEA-1011
ATPO
Becampanel
Caroverine
CNQX
Dasolampanel
DNQX
Fanapanel (MPQX)
GAMS
Kaitocephalin
Kynurenic acid
Kynurenine
Licostinel (ACEA-1021)
NBQX
PNQX
Selurampanel
Tezampanel
Theanine
Topiramate
YM90K
Zonampanel; Negative allosteric modulators: Barbiturates (e.g., pentobarbital, sodium thiopental)
Cyclopropane
Enflurane
Ethanol (alcohol)
Evans blue
GYKI-52466
GYKI-53655
Halothane
Irampanel
Isoflurane
Perampanel
Pregnenolone sulfate
Sevoflurane
Talampanel; Unknown/unsorted antagonists: Minocycline
KAR
Agonists: Main site agonists: 5-Bromowillardiine
5-Iodowillardiine
Acromelic acid (acromelate)
AMPA
ATPA
Domoic acid
Glutamate
Ibotenic acid
Kainic acid
LY-339434
Proline
Quisqualic acid
SYM-2081; Positive allosteric modulators: Cyclothiazide
Diazoxide
Enflurane
Halothane
Isoflurane
Antagonists: ACEA-1011
CNQX
Dasolampanel
DNQX
GAMS
Kaitocephalin
Kynurenic acid
Licostinel (ACEA-1021)
LY-382884
NBQX
NS102
Selurampanel
Tezampanel
Theanine
Topiramate
UBP-302; Negative allosteric modulators: Barbiturates (e.g., pentobarbital, sodium thiopental)
Enflurane
Ethanol (alcohol)
Evans blue
NS-3763
Pregnenolone sulfate
NMDAR
Agonists: Main site agonists: AMAA
Aspartate
Glutamate
Homocysteic acid (L-HCA)
Homoquinolinic acid
Ibotenic acid
NMDA
Proline
Quinolinic acid
Tetrazolylglycine
Theanine; Glycine site agonists: β-Fluoro-D-alanine
ACBD
ACC (ACPC)
ACPD
AK-51
Apimostinel (NRX-1074)
B6B21
CCG
D-Alanine
D-Cycloserine
D-Serine
DHPG
Dimethylglycine
Glycine
HA-966
L-687414
L-Alanine
L-Serine
Milacemide
Neboglamine (nebostinel)
Rapastinel (GLYX-13)
Sarcosine; Polyamine site agonists: Neomycin
Spermidine
Spermine; Other positive allosteric modulators: 24S-Hydroxycholesterol
DHEA (prasterone)
DHEA sulfate (prasterone sulfate)
Epipregnanolone sulfate
Pregnenolone sulfate
SAGE-718
Antagonists: Competitive antagonists: AP5 (APV)
AP7
CGP-37849
CGP-39551
CGP-39653
CGP-40116
CGS-19755
CPP
Kaitocephalin
LY-233053
LY-235959
LY-274614
MDL-100453
Midafotel (d-CPPene)
NPC-12626
NPC-17742
PBPD
PEAQX
Perzinfotel
PPDA
SDZ-220581
Selfotel; Glycine site antagonists: 4-Cl-KYN (AV-101)
5,7-DCKA
7-CKA
ACC
ACEA-1011
ACEA-1328
Apimostinel (NRX-1074)
AV-101
Carisoprodol
CGP-39653
CNQX
D-Cycloserine
DNQX
Felbamate
Gavestinel
GV-196771
Harkoseride
Kynurenic acid
Kynurenine
L-689560
L-701324
Licostinel (ACEA-1021)
LU-73068
MDL-105519
Meprobamate
MRZ 2/576
PNQX
Rapastinel (GLYX-13)
ZD-9379; Polyamine site antagonists: Arcaine
Co 101676
Diaminopropane
Diethylenetriamine
Huperzine A
Putrescine; Uncompetitive pore blockers (mostly dizocilpine site): 2-MDP
3-HO-PCP
3-MeO-PCE
3-MeO-PCMo
3-MeO-PCP
4-MeO-PCP
8A-PDHQ
18-MC
α-Endopsychosin
Alaproclate
Alazocine (SKF-10047)
Amantadine
Aptiganel
Argiotoxin-636
Arketamine
ARL-12495
ARL-15896-AR
ARL-16247
Budipine
Coronaridine
Delucemine (NPS-1506)
Dexoxadrol
Dextrallorphan
Dextromethadone
Dextromethorphan
Dextrorphan
Dieticyclidine
Diphenidine
Dizocilpine
Ephenidine
Esketamine
Etoxadrol
Eticyclidine
Fluorolintane
Gacyclidine
Ibogaine
Ibogamine
Indantadol
Ketamine
Ketobemidone
Lanicemine
Levomethadone
Levomethorphan
Levomilnacipran
Levorphanol
Loperamide
Memantine
Methadone
Methorphan
Methoxetamine
Methoxphenidine
Milnacipran
Morphanol
NEFA
Neramexane
Nitromemantine
Noribogaine
Norketamine
Orphenadrine
PCPr
PD-137889
Pethidine (meperidine)
Phencyclamine
Phencyclidine
Propoxyphene
Remacemide
Rhynchophylline
Rimantadine
Rolicyclidine
Sabeluzole
Tabernanthine
Tenocyclidine
Tiletamine
Tramadol; Ifenprodil (NR2B) site antagonists:
Besonprodil
Buphenine (nylidrin)
CO-101244 (PD-174494)
Eliprodil
Haloperidol
Isoxsuprine
Radiprodil (RGH-896)
Rislenemdaz (CERC-301, MK-0657)
Ro 8-4304
Ro 25-6981
Safaprodil
Traxoprodil (CP-101606); NR2A-selective antagonists: MPX-004
MPX-007
TCN-201
TCN-213; Cations: Hydrogen
Magnesium
Zinc; Alcohols/volatile anesthetics/related: Benzene
Butane
Chloroform
Cyclopropane
Desflurane
Diethyl ether
Enflurane
Ethanol (alcohol)
Halothane
Hexanol
Isoflurane
Methoxyflurane
Nitrous oxide
Octanol
Sevoflurane
Toluene
Trichloroethane
Trichloroethanol
Trichloroethylene
Urethane
Xenon
Xylene; Unknown/unsorted antagonists: ARR-15896
Bumetanide
Caroverine
D-αAA
Dexanabinol
Flufenamic acid
Flupirtine
FPL-12495
FR-115427
Furosemide
Hodgkinsine
Ipenoxazone (MLV-6976)
MDL-27266
Metaphit
Minocycline
MPEP
Niflumic acid
Pentamidine
Pentamidine isethionate
Piretanide
Psychotridine
Transcrocetin (saffron)
See also: Receptor/signaling modulators
Metabotropic glutamate receptor modulators
Glutamate metabolism/transport modulators
Authority control
LCCN: sh85079651
GND: 4128915-8
BNF: cb119771902 (data)
NDL: 00567385
BNE: XX530348
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values: Standard conditions for temperature and pressure

values: STP: standard temperature and pressure: 0 °C and 101.325 kPa

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Kilojoule per mole

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values: Hexagonal close packed crystal structure for magnesium

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Coefficient of thermal expansion

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values: List of data references for chemical elements

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Sacrificial anode

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Magnesium alloy wheel

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Primary battery

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Secondary battery

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Nonferrous metal

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Alkyl halide

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Culture medium

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Milk of magnesia

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Cardiac arrhythmia/bradycardia

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Porphyrin ring

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Leaching (chemical science)

values: List of countries by magnesium production

values: Book:Chemical elements (sorted alphabetically)

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values: Meitnerium, 109 (unknown chemical properties)

values: Darmstadtium, 110 (unknown chemical properties)

values: Roentgenium, 111 (unknown chemical properties)

values: Copernicium, 112 (post-transition metal)

values: Nihonium, 113 (unknown chemical properties)

values: Flerovium, 114 (unknown chemical properties)

values: Moscovium, 115 (unknown chemical properties)

values: Livermorium, 116 (unknown chemical properties)

values: Tennessine, 117 (unknown chemical properties)

values: Oganesson, 118 (unknown chemical properties)

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Polyatomic nonmetal

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Diatomic nonmetal

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/wiki/N-Methyl-D-aspartate_receptor
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N-Methyl-D-aspartate receptor

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/wiki/DHEA_sulfate
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DHEA sulfate

values: Epipregnanolone sulfate (page does not exist)

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values: Cis-1-(phenanthrene-2-carbonyl)piperazine-2,3-dicarboxylic acid (page does not exist)

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Pentamidine isethionate

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Magnesium – Afrikaans
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af
interlanguage-link-target

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https://an.wikipedia.org/wiki/Magnesio
Magnesio – Aragonese
an
an
interlanguage-link-target

values:
https://ast.wikipedia.org/wiki/Magnesiu
Magnesiu – Asturian
ast
ast
interlanguage-link-target

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https://az.wikipedia.org/wiki/Maqnezium
Maqnezium – Azerbaijani
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az
interlanguage-link-target

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https://bs.wikipedia.org/wiki/Magnezij
Magnezij – Bosnian
bs
bs
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https://br.wikipedia.org/wiki/Magneziom
Magneziom – Breton
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br
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values:
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Magnesi – Catalan
ca
ca
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https://ceb.wikipedia.org/wiki/Magnesyo
Magnesyo – Cebuano
ceb
ceb
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values:
https://co.wikipedia.org/wiki/Magnesiu
Magnesiu – Corsican
co
co
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values:
https://cy.wikipedia.org/wiki/Magnesiwm
Magnesiwm – Welsh
cy
cy
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values:
https://da.wikipedia.org/wiki/Magnesium
Magnesium – Danish
da
da
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values:
https://de.wikipedia.org/wiki/Magnesium
Magnesium – German
de
de
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values: މެގްނީޒިއަމް – Divehi

values: Μαγνήσιο – Greek

values:
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Magnesio – Spanish
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es
interlanguage-link-target

values:
https://eo.wikipedia.org/wiki/Magnezio
Magnezio – Esperanto
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eo
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Magnesio – Basque
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eu
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values:
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Magnesium – Faroese
fo
fo
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values:
https://fy.wikipedia.org/wiki/Magnesium
Magnesium – Western Frisian
fy
fy
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values:
https://fur.wikipedia.org/wiki/Magnesi
Magnesi – Friulian
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fur
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values:
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Magnesium – Scottish Gaelic
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gd
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values:
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Magnesio – Galician
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gl
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values:
https://ki.wikipedia.org/wiki/Magnesium
Magnesium – Kikuyu
ki
ki
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values: મેગ્નેશિયમ – Gujarati

values: Маңһанис – Kalmyk

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values: मैग्नीसियम – Hindi

values:
https://hr.wikipedia.org/wiki/Magnezij
Magnezij – Croatian
hr
hr
interlanguage-link-target

values:
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Magnezo – Ido
io
io
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values:
https://id.wikipedia.org/wiki/Magnesium
Magnesium – Indonesian
id
id
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values:
https://ia.wikipedia.org/wiki/Magnesium
Magnesium – Interlingua
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ia
interlanguage-link-target

values:
https://it.wikipedia.org/wiki/Magnesio
Magnesio – Italian
it
it
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values:
https://jv.wikipedia.org/wiki/Magnesium
Magnesium – Javanese
jv
jv
interlanguage-link-target

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values:
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Magnez – Kashubian
csb
csb
interlanguage-link-target

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values:
https://sw.wikipedia.org/wiki/Magnesi
Magnesi – Swahili
sw
sw
interlanguage-link-target

values: Магний – Komi

values: Магний – Kyrgyz

values:
https://la.wikipedia.org/wiki/Magnesium
Magnesium – Latin
la
la
interlanguage-link-target

values:
https://lv.wikipedia.org/wiki/Magnijs
Magnijs – Latvian
lv
lv
interlanguage-link-target

values:
https://lb.wikipedia.org/wiki/Magnesium
Magnesium – Luxembourgish
lb
lb
interlanguage-link-target

values:
https://lt.wikipedia.org/wiki/Magnis
Magnis – Lithuanian
lt
lt
interlanguage-link-target

values:
https://lij.wikipedia.org/wiki/Magnesio
Magnesio – Ligurian
lij
lij
interlanguage-link-target

values:
https://li.wikipedia.org/wiki/Magnesium
Magnesium – Limburgish
li
li
interlanguage-link-target

values:
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Manezu – Lingala
ln
ln
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values:
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Magnii – Livvi-Karelian
olo
olo
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values:
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Magnesio – Lombard
lmo
lmo
interlanguage-link-target

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values:
https://mi.wikipedia.org/wiki/Konupora
Konupora – Maori
mi
mi
interlanguage-link-target

values: मॅग्नेशियम – Marathi

values:
https://ms.wikipedia.org/wiki/Magnesium
Magnesium – Malay
ms
ms
interlanguage-link-target

values: Магнезь – Moksha

values: မဂ္ဂနီစီယမ် – Burmese

values:
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Magnesium – Dutch
nl
nl
interlanguage-link-target

values: म्याग्नेसियम – Nepali

values: म्याग्नेजियम – Newari

values:
https://no.wikipedia.org/wiki/Magnesium
Magnesium – Norwegian
no
no
interlanguage-link-target

values:
https://nn.wikipedia.org/wiki/Magnesium
Magnesium – Norwegian Nynorsk
nn
nn
interlanguage-link-target

values: ମାଗ୍ନେସିଅମ – Odia

values:
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Magniy – Uzbek
uz
uz
interlanguage-link-target

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Magnesi – Piedmontese
pms
pms
interlanguage-link-target

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Magnez – Polish
pl
pl
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values:
https://ro.wikipedia.org/wiki/Magneziu
Magneziu – Romanian
ro
ro
interlanguage-link-target

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values:
https://scn.wikipedia.org/wiki/Magnesiu
Magnesiu – Sicilian
scn
scn
interlanguage-link-target

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values:
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Magnezij – Slovenian
sl
sl
interlanguage-link-target

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values:
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Magnezij – Serbo-Croatian
sh
sh
interlanguage-link-target

values:
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Magnesium – Finnish
fi
fi
interlanguage-link-target

values:
https://sv.wikipedia.org/wiki/Magnesium
Magnesium – Swedish
sv
sv
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values:
https://tl.wikipedia.org/wiki/Magnesyo
Magnesyo – Tagalog
tl
tl
interlanguage-link-target

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Magnezyum – Turkish
tr
tr
interlanguage-link-target

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values:
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Magnii – Veps
vep
vep
interlanguage-link-target

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Magie – Vietnamese
vi
vi
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Magnesyo – Waray
war
war
interlanguage-link-target

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镁 – Chinese
zh
zh
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