![]() Unit cell containing 31 nitride ions (red) and 48 calcium ions (white). Each nitride is surrounded by six calcium, and each calcium by four nitride ions. | |
Names | |
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IUPAC name
Calcium nitride | |
Other names
tricalcium dinitride | |
Identifiers | |
3D model (JSmol) |
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ECHA InfoCard | 100.031.435 ![]() |
EC Number |
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PubChem CID |
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CompTox Dashboard (EPA) |
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Properties | |
Ca3N2 | |
Molar mass | 148.248 g·mol−1 |
Appearance | red-brown crystalline solid |
Density | 2.670 g/cm3 2.63 g/cm3 (17 °C) |
Melting point | 1,195 °C (2,183 °F; 1,468 K) |
decomposes | |
Structure | |
Cubic, cI80 | |
Ia-3, No. 206 | |
Related compounds | |
Other anions |
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Other cations |
Beryllium nitride Magnesium nitride Strontium nitride Barium nitride Radium nitride Zinc nitride Aluminium nitride Lithium nitride Sodium nitride Potassium nitride |
Related compounds |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). |
Calcium nitride is the inorganic compound with the chemical formula Ca3N2.[1] It exists in various forms (isomorphs), α-calcium nitride being more commonly encountered.
α-Calcium nitride adopts an anti-bixbyite structure, similar to Mn2O3, except that the positions of the ions are reversed: calcium (Ca2+) take the oxide (O2−) positions and nitride ions (N3−) the manganese (Mn3+). In this structure, Ca2+ occupies tetrahedral sites, and the nitride centres occupy two different types of octahedral sites.[2]
Calcium nitride is formed along with the oxide, CaO, when calcium burns in air. It can be produced by direct reaction of the elements:[3]
It reacts with water or even the moisture in air to give ammonia and calcium hydroxide:[4]
Like sodium oxide, calcium nitride absorbs hydrogen above 350 °C:
Calcium nitride.
Salts and covalent derivatives of the nitride ion
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