Contents

Sodium nitride

Not to be confused with sodium nitrate, sodium nitrite, or sodium azide.

Sodium nitride

Names
IUPAC name Sodium nitride
Identifiers
CAS Number	12136-83-3 Y
3D model (JSmol)	Interactive image Interactive image Interactive image
ECHA InfoCard	100.032.017
EC Number	235-232-3
InChI InChI=1/3Na.N Key: ZOULLXMSYSKRPG-UHFFFAOYNA-N
SMILES [Na]N([Na])[Na] [Na+].[Na+].[Na+].[N-3] [Na+].[Na][N-][Na]
Properties
Chemical formula	Na3N
Molar mass	82.976 g/mol
Appearance	reddish brown or dark blue solid
Melting point	87 °C (189 °F; 360 K)[1] (decomposes)
Solubility in water	reacts
Structure
Crystal structure	Cubic, cP4[2]
Space group	Pm3m[2]
Thermochemistry
Std enthalpy of formation (ΔfH⦵298)	-151 J/mol[2]
Related compounds
Other anions	Sodium amide Sodium imide
Other cations	Lithium nitride Potassium nitride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

Sodium nitride is the inorganic compound with the chemical formulaNa₃N. In contrast to lithium nitride and some other nitrides, sodium nitride is an extremely unstable alkali metal nitride. It can be generated by combining atomic beams of sodium and nitrogen deposited onto a low-temperature sapphire substrate.^[1] It readily decomposes into its elements:

${\displaystyle {\ce {2 Na3N -> 6 Na + N2}}}$

Synthesis[edit]

Sodium nitride can be synthesized in two different ways: by the thermal decompositionofNaNH₂ or by the direct reaction of the elements.^[2] The most common way to successfully synthesize sodium nitride has been done by Dieter Fischer & Martin Jansen and Grigori Vajenine using the latter method. The first way is to introduce desired ratios of Na and N₂ in gas phase separately and depositing them in a vacuum chamber on a cooled substrate, which is then heated to room temperate (298 K) to crystallize.^[1] The second method is to react elemental sodium with plasma activated nitrogen on a metal surface. This synthesis can be further facilitated by introducing liquid Na-K alloy to the compound with the excess liquid removed and washed with fresh alloy. The solid is then separated from the liquid using a centrifuge. However Vajenine’s method is very air-sensitive and can decompose and combust rapidly, unless exposed to a pure oxygen (O₂) environment.^[3]

Characteristics[edit]

Sodium nitride can be of reddish brown or dark blue color depending on the synthesis of the compound due to intrinsic properties.^[1][3] It shows no signs of decomposition after several weeks when at room temperature.^[3] The compound does not have a melting point as it decomposes back into its elemental forms as demonstrated using mass spectrometry around 360 K.^[1][2] The estimated enthalpy of formation for the compound is +64 kJ/mol.^[3]

Structure[edit]

Sodium nitride seems to be about 90% ionic at room temperature, but has the band gap typical for a semiconductor.^[2][3] It adopts the anti-ReO₃ structure with a simple lattice made up of NNa₆ octahedra.^[1][2][3][4] The compound has N­−Na bond lengths of 236.6 pm.^[1][3] This structure has been confirmed through X-ray diffraction and more recently neutron diffraction on powder and single crystals.^[1][2][3][4]

References[edit]