Magnesium nitride

Magnesium nitride

Names
IUPAC name Magnesium nitride
Other names trimagnesium dinitride
Identifiers
CAS Number	12057-71-5 Y
3D model ( JSmol )	Interactive image
ECHA InfoCard	100.031.826
EC Number	235-022-1
PubChem CID	3673438
UNII	7941Y31SR6 Y
CompTox Dashboard (EPA)	DTXSID701014275
InChI InChI=1S/3Mg.2N InChI=1S/3Mg.2N/q3*+2;2*-3 InChI=1S/3Mg.2N/q;;+2;2*-1
SMILES [Mg+2].[Mg+2].[Mg+2].[N-3].[N-3]
Properties
Chemical formula	Mg3N2
Molar mass	100.9494 g/mol
Appearance	greenish yellow powder
Density	2.712 g/cm3
Melting point	approx. 1500°C
Hazards[1]
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H228, H315, H319, H335
Precautionary statements	P210, P261, P280, P305+P351+P338, P405, P501
Safety data sheet (SDS)	External MSDS
Related compounds
Other cations	Beryllium nitride Calcium 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

Magnesium nitride, which possesses the chemical formula Mg₃N₂, is an inorganic compound of magnesium and nitrogen. At room temperature and pressure it is a greenish yellow powder.

Preparation

• By passing dry nitrogen over heated magnesium:

${\displaystyle {\begin{matrix}{}\\{\ce {{3Mg}+N2->[{\ce {800^{\circ }C}}]Mg3N2}}\\{}\end{matrix}}}$

• or ammonia:

${\displaystyle {\begin{matrix}{}\\{\ce {{3Mg}+2NH3->[{\ce {700^{\circ }C}}]{Mg3N2}+3H2}}\\{}\end{matrix}}}$

Chemistry

Magnesium nitride reacts with water to produce magnesium hydroxide and ammonia gas, as do many metal nitrides.

Mg₃N_2(s) + 6 H₂O_(l) → 3 Mg(OH)_2(aq) + 2 NH_3(g)

In fact, when magnesium is burned in air, some magnesium nitride is formed in addition to the principal product, magnesium oxide.

Thermal decomposition of magnesium nitride gives magnesium and nitrogen gas (at 700-1500 °C).

At high pressures, the stability and formation of new nitrogen-rich nitrides (N/Mg ratio equal or greater to one) were suggested and later discovered.^[2][3][4] These include the Mg₂N₄ and MgN₄ solids which both become thermodynamically stable near 50 GPa.^[5] The Mg₂N₄ is composed of exotic cis-tetranitrogen N₄⁴⁻ species with N-N bond orders close to one. This Mg₂N₄ compound was recovered to ambient conditions, along with the N₄⁴⁻ units, marking only the fourth polynitrogen entity bulk stabilized at ambient conditions.

Uses and history

When isolating argon, William Ramsay passed dry air over copper to remove oxygen and over magnesium to remove the nitrogen, forming magnesium nitride.

Magnesium nitride was the

Out of desperation and curiosity (he called it the "make the maximum number of mistakes" approach[7]), he added some magnesium wire to the hexagonal boron nitride and gave it the same pressure and heat treatment. When he examined the wire under a microscope, he found tiny dark lumps clinging to it. These lumps could scratch a polished block of boron carbide, something only diamond was known to do.

From the smell of ammonia, caused by the reaction of magnesium nitride with the moisture in the air, he deduced that the magnesium metal had reacted with the boron nitride to form magnesium nitride, which was the true catalyst.

Magnesium nitride has also been applied to synthesize aluminum nitride nanocrystals, cubic boron nitride and nitrides of aluminum and Group 3 ^[8] It has also been proposed as an intermediate in a fossil-fuel-free nitrogen fixation process.^[9]

References