Natriums

Natrium, known in modern chemistry as sodium, is a chemical element with the symbol Na and atomic number 11. It is a soft, silvery-white alkali metal that is highly reactive, particularly with water. In pure form it is too reactive for practical use and is usually encountered in compounds such as sodium chloride.

Discovered in the early 19th century by Humphry Davy through the electrolysis of molten sodium hydroxide, natrium was given its Latin-derived name, from Natrium, the ancient name for sodium. The symbol Na also derives from this name.

Natrium occurs in the Earth's crust only in compounds and, as a free element, is rare due to its reactivity. It is abundant in seawater and in many minerals. Commercial natrium is produced mainly by electrolysis of concentrated sodium chloride solutions (the Downs process) or by the electrolysis of molten NaCl.

Key properties include a melting point of 97.72 °C and a boiling point of 883 °C. It forms a wide range of compounds, including sodium chloride (table salt), sodium hydroxide, and sodium carbonate. The sodium ion (Na+) is essential in many biological processes, such as nerve impulse transmission and fluid balance.

Uses of natrium include the chlor-alkali process for producing chlorine and sodium hydroxide, as a reducing agent in metallurgical processes, and in specialized lighting (sodium-vapor lamps). In medicine, saline solutions provide isotonic electrolytes.

Safety: Natrium is highly reactive with water and air, generating hydrogen gas and heat and posing fire or explosion hazards. It is stored under oil or in inert atmospheres and handled with appropriate precautions to avoid contact with moisture.