STRONTIUM NITRIDE is obtained by heating elemental Sr in nitrogen at 460 °C for an extended period until the reaction is complete. Alternatively, if the rate of ammonia absorption is slow during the aforementioned reaction, the temperature may be raised to 700–750 °C.
Strontium nitride should have the molecular formula
of Sr3N2 and the molecular weight of 290.8752 g/mol.
However, according to some sources, Strontium does
not form the ionic compound Sr3N2 and Sr2N is the
only compound that has been properly characterized
to date. The reaction of Sr metal in a pure stream of
nitrogen gas produces the “subnitride”:
4Sr +N2 2Sr2N
A second method would be the decomposition of an
amide:
2Sr(NH2)2 + Heat 2Sr2N+ 2NH3 +H2
In air, it strontium metal burns and produces strontium
oxide and strontium nitride. But, since it does not
react with nitrogen below 380 °C, it will only form the
oxide spontaneously at room temperature. To produce
the pure nitride, it is necessary to maintain the temperature
above 380 °C in air or to heat the metal in pure
nitrogen gas. In air, the molten mass, as it cools from
380 °C, tends to convert some of the nitride to oxide.
Strontium nitride is described as Sr3N2,produced by burning strontium metal in air (resulting in a mixture with strontium oxide) or in nitrogen. Like other alkaline earth metal nitrides, it reacts with water to give strontium hydroxide and ammonia: Sr3N2 + 6H2O 3Sr(OH)2 + 2NH3
Strontium nitride (Sr3N2) can be used in the synthesis of ternary nitride oxide with molybdenum nitride under a low partial pressure of oxygen. It can also be used in the synthesis of barium-strontium silicate-based hollow structures for potential usage in drug delivery, catalysis, and sensors.
