BARIUM - Ba

Properties of Barium:

Alkaline earth metal. Silvery-white, malleable, ductile. In the air is covered with a dark oxide-nitride film. Colors the flame of a gas burner in a yellow-green color. High reactivity. Reacts with oxygen, nitrogen, hydrogen, halogens and other non-metals. Strong reducing agent. Reacts with water, acids, hydrogen sulfide, ammonia.


Molar mass g/mol 137.327
Density g/cm3 3.60
Melting point °C 727
Boiling point °C 1860

Methods for preparation of Barium:

BaH2 = Ba + H2 (over 675°C).

3BaO + Si = BaSiO3 + 2Ba (1200°C),

3BaO + 2Al = 2Ba + (BaAl2)O4 (1100-1200°C).


Сhemical reactions with metal Barium:

Ba + 2H2O = Ba(OH)2 + H2↑ (normal temp.).

Ba + 2HCl(diluted) = BaCl2 + H2↑.

4Ba + 10HNO3(diluted) = 4Ba(NO3)2 + N2O↑ + 5H2O,

4Ba + 10HNO3(highly diluted) = 4Ba(NO3)2 + NH4NO3 + 3H2O.

Ba + H2 = BaH2 (150-300°C).

3Ba + 2O2 = 2BaO + BaO2 (until 500°C, burning on air),

2Ba + O2 = 2BaO (over 800°C).

Ba + E2 = BaE2 (100-150◦ C; E = F, Cl, Br, I).

Ba + S = BaS (150°C).

3Ba + N2 = Ba3N2 (200-460°C, burning on air).

Ba + 2C(graphite) = BaC2 (500°C).

Ba + H2S = BaS+H2 (over 350°C).

6Ba + 2NH3(gas) = Ba3N2 + 3BaH2 (600-650°C).

Ba + 6NH3(liquid) = [Ba(NH3)6](blue) [-40°C, in the atm. of Ar],

Ba + 2NH3(liquid) = Ba(NH2)2 + H2 (catalyst Pt).

2Ba + 3CO2 = 2BaCO3 + C(graphite) [normal temp.].
 

Did you know?

A pure element can take many forms. For example, diamond and graphite both are forms of pure carbon.