BARIUM - BaProperties 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.
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.]. |
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Empirical formulas show the simplest whole number ratio of atoms in a formula.