|Group||2||Melting point||727°C, 1341°F, 1000 K|
|Period||6||Boiling point||1845°C, 3353°F, 2118 K|
|Block||s||Density (g cm−3)||3.62|
|Atomic number||56||Relative atomic mass||137.327|
|State at 20°C||Solid||Key isotopes||138 Ba|
|Electron configuration||[Xe] 6s2||CAS number||7440-39-3|
|ChemSpider ID||4511436||ChemSpider is a free chemical structure database|
- Represented by the symbol ‘Ba’, Barium is a group 2 element in the periodic table with atomic number 56.
- Barium is a dense alkaline earth metal that occurs naturally in ore deposits and makes up 0.05% of the Earth’s crust (Genter 2001). Barium and its compounds may be found in nature or produced industrially for various uses.
- It is a silvery-white metal that can be found in the environment, where it exists naturally. It occurs combined with other chemicals, such as carbon, oxygen, and sulfur.
- It is very light and its density is half of that of iron.
- Barium oxidizes in air, reacts vigorously with water to form the hydroxide, liberating hydrogen. It reacts with almost all the non-metals, forming often poisoning compounds.
- Barium is often used for spark-plug electrodes and in vacuum tubes as a drying and oxygen-removing agent. As well as fluorescent lamps: impure barium sulfide phosphorescence after exposure to light.
- Its compounds are used by oil and gas industries to make drilling mud. Drilling mud simplifies drilling through rocks by lubricating the drill.
- Barium compounds are also used to make paint, bricks, tiles, glass, and rubber.
- Barium nitrate and chlorate give fireworks a green color.
Practise This Question