Magnesium is an element with the symbol Mg. Its atomic number is 12. It is an alkaline earth metal and is the eighth most abundant element in the Earth’s crust. Below is an overview of the chemical and physical properties of magnesium, its valency, electronic configuration, uses, reactions with other elements, and industrial and medical applications.
Chemical Properties of magnesium:
- Magnesium is a highly reactive metal that reacts with many substances, including oxygen, water, acids, and bases.
- It can form a wide range of compounds with other elements, including oxides, chlorides, and carbonates.
- Magnesium has a relatively low electronegativity and can easily donate its valence electrons to form ionic compounds.
Physical Properties of magnesium:
- Magnesium is a silvery-white metal at room temperature and pressure.
- It has a melting point of 650°C and a boiling point of 1,090°C.
- Magnesium is relatively light, with a density of 1.74 g/cm³.
Valency of magnesium:
- Magnesium has a valency of +2.
- It readily donates its two valence electrons to form ionic compounds.
Electronic Configuration of magnesium:
- Magnesium has its electron configuration as of [Ne] 3s2.
- It has two valence electrons that are easily donated to form ionic compounds.
Uses of magnesium:
- Magnesium is used in the production of lightweight alloys for use in the automotive and aerospace industries.
- It is used in the production of fireworks, flares, and other pyrotechnics.
- Magnesium is used as a reducing agent in the production of metals such as titanium and zirconium.
Reactions of magnesium with Other Elements:
- Magnesium reacts with oxygen to form magnesium oxide, a common component of many minerals and rocks.
- It reacts with water to produce magnesium hydroxide and hydrogen gas.
- Magnesium can also react with acids to produce hydrogen gas and a magnesium salt.
Chemical and Physical Properties of Magnesium in a table
|Electron Configuration||[Ne] 3s2|
|Solubility||Insoluble in water|