|Name, symbol||Barium, Ba|
|Barium in the periodic table|
|Standard atomic weight (Ar)||137.327(7)|
|Group, block||(alkaline earth metals); s-block|
|Electron configuration||[Xe] 6s2|
|2, 8, 18, 18, 8, 2|
|Melting point||1000 K (727 °C, 1341 °F)|
|Boiling point||2118 K (1845 °C, 3353 °F)|
|Density near r.t.||3.51 g/cm3|
|when liquid, at||3.338 g/cm3|
|Heat of fusion||7.12 kJ/mol|
|Heat of||142 kJ/mol|
|Molar heat capacity||28.07 J/(mol·K)|
|Oxidation states||+2, +1 (a strongly basic oxide)|
|Electronegativity||Pauling scale: 0.89|
1st: 502.9 kJ/mol |
2nd: 965.2 kJ/mol
3rd: 3600 kJ/mol
|Atomic radius||empirical: 222 pm|
|Covalent radius||215±11 pm|
|Van der Waals radius||268 pm|
|Crystal structure||body-centered cubic|
|Speed of sound thin rod||1620 m/s (at 20 °C)|
|Thermal expansion||20.6 µm/(m·K) (at 25 °C)|
|Thermal conductivity||18.4 W/(m·K)|
|Electrical resistivity||332 Ω·m (at 20 °C)|
|Young's modulus||13 GPa|
|Shear modulus||4.9 GPa|
|Bulk modulus||9.6 GPa|
|CAS Registry Number||7440-39-3|
|Discovery||Carl Wilhelm Scheele (1772)|
|First isolation||Humphry Davy (1808)|
Barium is a chemical element with symbol Ba and atomic number 56. It is the heaviest non-radioactive s-block element.
Barium slowly oxidizes in air to form a dark layer of barium oxide and barium nitride. Barium and its compounds burn with a green flame.
- Ba + 2 H2O → Ba(OH)2 + H2
The same reaction also happens with alcohols, giving barium alkoxide.
Barium reacts with ammonia to form complexes such as Ba(NH3)6.
Barium is a silvery white metal, that rapidly turns black on exposure with air. Barium melts at 730 °C, intermediate between those of the lighter strontium (780 °C) and heavier radium (700 °C). Its boiling point of 1,900 °C is higher than that of strontium (1,382 °C) and radium (~1737 °C). Barium has a density of 3.62 g/cm3
Barium metal is sold by various chemical suppliers, either under oil or ampouled. GalliumSource sells 50 g of barium at a price of $92.00.
Barium can be extracted through the aluminothermic reduction of barium oxide:
- 4 BaO + 2 Al → 3 Ba↑ + BaAl2O4
Due to the high temperatures released during this reaction, the resulting barium metal turns to vapors, which are condensed under argon.
Silicon can also be used as a reducing agent.
- Make barium peroxide
- Make soluble barium salts
- Green flame
- Ellement collecting
Barium readily reacts with water releasing hydrogen gas, which is flammable and its build-up may cause explosions. However, unlike alkali metals, it can be safely handled with bare hand.
Soluble barium salts and other compounds are very toxic to organisms and should be handled with proper protection. Insoluble barium compounds however, are pretty much non-toxic .
Barium metal is best converted to barium sulfate, which is non-toxic.