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Magnesium, 12Mg
Magnesium crystals.jpg
Magnesium
Pronunciation /mæɡˈnziəm/ (mag-NEE-zee-əm)
Appearance shiny grey solid
Standard atomic weight Ar, std(Mg) [24.30424.307] conventional: 24.305
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
sodiummagnesiumaluminium
Atomic number (Z) 12
Group group 2 (alkaline earth metals)
Period period 3
Block   s
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 +1, +2 (a strongly basic oxide)
Electronegativity Pauling scale: 1.31
Ionization energies
  • (more)
Atomic radius empirical: 160 pm
Covalent radius 141±7 pm
Van der Waals radius 173 pm
Color lines in a spectral range
Spectral lines of magnesium
Other properties
Natural occurrence primordial
Crystal structure ​hexagonal close-packed (hcp)
Hexagonal close packed crystal structure for magnesium
Speed of sound thin rod (annealed)
4940 m/s (at r.t.)
Thermal expansion 24.8 µm/(m⋅K) (at 25 °C)
Thermal conductivity 156 W/(m⋅K)
Electrical resistivity 43.9 n Ω⋅m (at 20 °C)
Magnetic ordering paramagnetic
Young's modulus 45 GPa
Shear modulus 17 GPa
Bulk modulus 45 GPa
Poisson ratio 0.290
Mohs hardness 2.5
Brinell hardness 260 MPa
CAS Number 7439-95-4
History
Discovery Joseph Black (1755)
First isolation Humphry Davy (1808)
Main isotopes of magnesium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
24Mg 78.99% 24Mg is stable with 12 neutrons
25Mg 10.00% 25Mg is stable with 13 neutrons
26Mg 11.01% 26Mg is stable with 14 neutrons
Magnesium
Magnesium metal

Magnesium (pronounced mag-NEE-zee-əm) is a chemical element. Its symbol is Mg and its atomic number is 12. It is a type of metal called an alkaline earth metal.

Magnesium is very common. It is the eighth most abundant element in the Earth's crust, making up about 2% of its weight. It is also the ninth most common element in the entire universe. This is because magnesium is easily formed inside giant stars that explode, known as supernovas.

Magnesium ions (which are atoms with an electrical charge) dissolve very well in water. This makes magnesium the third most common element found dissolved in seawater.

Why is Magnesium Important for Life?

Magnesium is the 11th most common element by weight in the human body. Its ions are vital for all living cells to work properly. These ions help manage important biological compounds like ATP (which gives cells energy), DNA, and RNA.

Many enzymes (special proteins that help chemical reactions happen) need magnesium ions to do their job. Magnesium is also the metal found at the center of chlorophyll, which is the green pigment that helps plants make their own food using sunlight. Because of this, magnesium is often added to fertilizers to help plants grow.

Magnesium ions can taste a bit sour. In small amounts, they give a natural tartness to fresh mineral waters.

How Do We Get Magnesium?

You won't find pure magnesium metal naturally on Earth. This is because it is very reactive, meaning it easily combines with other elements. However, once the metal is made, it gets covered with a thin layer of oxide. This layer helps protect it and makes it less reactive.

Pure magnesium metal burns with a very bright white light. This makes it useful in things like flares and fireworks. Today, most magnesium metal is made by a process called electrolysis. This involves using electricity to separate magnesium from its salts, which are often taken from salty water (brine).

What is Magnesium Used For?

Magnesium is a very useful metal. Its main use is to be mixed with other metals to create strong, lightweight materials.

Strong and Light Alloys

One of the most common uses for magnesium is mixing it with aluminium. These mixtures are called "magnalium" or "magnelium." Since magnesium is lighter than aluminium, these alloys are valued for being both light and strong. They are used to make parts for things like bicycle frames and car engines.

Everyday Uses

Magnesium is used in fireworks to create a brilliant white light when it burns. It can also be found in many electronic devices.

Magnesium in Electronics

Because it is light and has good electrical properties, magnesium is used in:

Magnesium in Medicine

Magnesium compounds are also used in medicine. They can be found in common laxatives (to help with digestion) and antacids (like milk of magnesia, which helps with stomach upset). Magnesium is also used in situations where doctors need to calm overactive nerves or relax blood vessels.

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