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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.