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{{chembox |
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{{chembox |
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| verifiedrevid = 403294454 |
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| verifiedrevid = 420366204 |
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| Name = Magnesium nitride |
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| Name = Magnesium nitride |
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| ImageFile = |
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| ImageFile = Magnesium nitride.jpg |
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| ImageName = Magnesium nitride |
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| ImageFile1 = File:Mg3P2.png |
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| ImageName = |
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| IUPACName = Magnesium nitride |
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| ImageName1 = structure of magnesium nitride |
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| IUPACName = Magnesium nitride |
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| OtherNames = |
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| OtherNames = trimagnesium dinitride |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| SMILES = |
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| SMILES = .... |
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| CASNo = 12057-71-5 |
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| InChI = InChI=1S/3Mg.2N |
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| PubChem = 16212682 |
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| InChI2 = InChI=1S/3Mg.2N/q3*+2;2*-3 |
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| RTECS = |
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| InChI3 = InChI=1S/3Mg.2N/q;;+2;2*-1 |
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| CASNo_Ref = {{cascite|correct|??}} |
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| Section2 = {{Chembox Properties |
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| CASNo = 12057-71-5 |
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| Formula = Mg<sub>3</sub>N<sub>2</sub> |
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| EINECS = 235-022-1 |
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| MolarMass = 100.9494 g/mol |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| Appearance = greenish yellow powder |
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| UNII = 7941Y31SR6 |
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| Density = 2.712 g/cm<sup>3</sup> |
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| PubChem = 3673438 |
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| Solubility = |
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| RTECS = |
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| MeltingPt = approx. 1500°C |
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| BoilingPt = |
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|Section2={{Chembox Properties |
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| pKa = |
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| Formula = {{chem2|Mg3N2}} |
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| pKb = |
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| MolarMass = 100.9494 g/mol |
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| Viscosity = |
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| Appearance = greenish yellow powder |
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}} |
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| Density = 2.712 g/cm<sup>3</sup> |
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| Section3 = {{Chembox Structure |
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| MolShape = |
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| Solubility = |
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| MeltingPt = approx. 1500°C |
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| Coordination = |
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| CrystalStruct = |
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| BoilingPt = |
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| Dipole = |
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| pKa = |
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| pKb = |
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| Viscosity = |
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| Section7 = {{Chembox Hazards |
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| ExternalMSDS = |
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|Section3={{Chembox Structure |
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| MainHazards = |
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| FlashPt = |
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| MolShape = |
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| Coordination = |
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| RPhrases = {{R36}}, {{R37}}, {{R38}} |
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| CrystalStruct = |
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| SPhrases = {{S26}}, {{S36}} |
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| Dipole = |
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| Section8 = {{Chembox Related |
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|Section7={{Chembox Hazards |
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| OtherAnions = |
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| OtherCpds = |
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| MainHazards = |
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| FlashPt = |
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| Hazards_ref=<ref>{{cite web |title=Summary of Classification and Labelling |url=https://echa.europa.eu/information-on-chemicals/cl-inventory-database/-/discli/details/68017 |access-date=4 December 2021}}</ref> |
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| GHSPictograms = {{GHS02}}{{GHS07}} |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|228|315|319|335}} |
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| PPhrases = {{P-phrases|210|261|280|305+351+338|405|501}} |
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|Section8={{Chembox Related |
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| OtherAnions = |
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| OtherCations = {{ubl|]|]|]}} |
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'''Magnesium nitride''', which has the ] Mg<sub>3</sub>N<sub>2</sub>, is an ] of ] and ]. At room temperature and pressure it is a greenish yellow powder. |
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'''Magnesium nitride''', which possesses the ] {{chem2|Mg3N2|auto=1}}, is an ] of ] and ]. At room temperature and pressure it is a greenish yellow powder. |
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==Chemistry== |
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== History == |
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When measuring the boiling point of magnesium, ] and Henri Caron identified that molten magnesium they distilled covered itself by "small colorless and transparent needles which are destroyed fairly quickly by transforming into ammonia and magnesia". In their 1857 publication the chemists interpreted it as a likely nitride similar to those discovered by ] and ].<ref>]</ref> |
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Magnesium nitride reacts with water to produce ] gas, as do many metal ]s. |
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It was indeed confirmed in 1862 when Friedrich Briegleb and ] synthesized the compound on purpose and first studied it.<ref>{{Cite journal |last=Briegleb |first=Fr. |last2=Geuther |first2=A. |date=1862 |title=Ueber das Stickstoffmagnesium und die Affinitäten des Stickgases zu Metallen |url=https://books.google.com/books?id=netSAAAAcAAJ&pg=PA228 |journal=Justus Liebigs Annalen der Chemie |language=de |volume=123 |issue=2 |pages=228–241 |doi=10.1002/jlac.18621230212 |issn=1099-0690}}</ref> |
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:Mg<sub>3</sub>N<sub>2</sub> + 6 H<sub>2</sub>O → 3 Mg(OH)<sub>2</sub> + 2 NH<sub>3</sub> |
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==Synthesis== |
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== Preparation == |
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Magnesium nitride can be produced by heating magnesium metal in a pure nitrogen atmosphere. |
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* By passing dry nitrogen over heated magnesium at 800 °C: |
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:3 Mg + N<sub>2</sub> → Mg<sub>3</sub>N<sub>2</sub> |
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:{{chem2|3 Mg + N2 → Mg3N2}} |
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* or ammonia at 700 °C: |
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:{{chem2|3 Mg + 2 NH3 → Mg3N2 + 3 H2}} |
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==Chemistry== |
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Magnesium nitride reacts with water to produce ] and ] gas, as do many metal ]s. |
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:{{chem2|Mg3N2(s) + 6 H2O(l) → 3 Mg(OH)2(aq) + 2 NH3(g)}} |
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In fact, when magnesium is burned in air, some magnesium nitride is formed in addition to the principal product, ]. |
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In fact, when magnesium is burned in air, some magnesium nitride is formed in addition to the principal product, ]. |
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Thermal decomposition of magnesium nitride gives magnesium and nitrogen gas (at 700-1500 °C). |
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==Uses== |
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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.<ref>{{Cite journal|last1=Yu|first1=Shuyin|last2=Huang|first2=Bowen|last3=Zeng|first3=Qingfeng|last4=Oganov|first4=Artem R.|last5=Zhang|first5=Litong|last6=Frapper|first6=Gilles|date=June 2017|title=Emergence of Novel Polynitrogen Molecule-like Species, Covalent Chains, and Layers in Magnesium–Nitrogen Mg x N y Phases under High Pressure|journal=The Journal of Physical Chemistry C|volume=121|issue=21|pages=11037–11046|doi=10.1021/acs.jpcc.7b00474|issn=1932-7447}}</ref><ref>{{Cite journal|last1=Wei|first1=Shuli|last2=Li|first2=Da|last3=Liu|first3=Zhao|last4=Li|first4=Xin|last5=Tian|first5=Fubo|last6=Duan|first6=Defang|last7=Liu|first7=Bingbing|last8=Cui|first8=Tian|date=2017|title=Alkaline-earth metal (Mg) polynitrides at high pressure as possible high-energy materials|journal=Physical Chemistry Chemical Physics|volume=19|issue=13|pages=9246–9252|doi=10.1039/C6CP08771J|pmid=28322368|bibcode=2017PCCP...19.9246W|issn=1463-9076}}</ref><ref>{{Cite journal|last1=Xia|first1=Kang|last2=Zheng|first2=Xianxu|last3=Yuan|first3=Jianan|last4=Liu|first4=Cong|last5=Gao|first5=Hao|last6=Wu|first6=Qiang|last7=Sun|first7=Jian|date=2019-04-25|title=Pressure-Stabilized High-Energy-Density Alkaline-Earth-Metal Pentazolate Salts|journal=The Journal of Physical Chemistry C|volume=123|issue=16|pages=10205–10211|doi=10.1021/acs.jpcc.8b12527|s2cid=132258000|issn=1932-7447}}</ref> These include the {{chem2|Mg2N4}} and {{chem2|MgN4}} solids which both become thermodynamically stable near 50 GPa.<ref>{{Cite journal|last1=Laniel|first1=Dominique|last2=Winkler|first2=Bjoern|last3=Koemets|first3=Egor|last4=Fedotenko|first4=Timofey|last5=Bykov|first5=Maxim|last6=Bykova|first6=Elena|last7=Dubrovinsky|first7=Leonid|last8=Dubrovinskaia|first8=Natalia|date=December 2019|title=Synthesis of magnesium-nitrogen salts of polynitrogen anions|journal=Nature Communications|volume=10|issue=1|pages=4515|doi=10.1038/s41467-019-12530-w|issn=2041-1723|pmc=6778147|pmid=31586062|bibcode=2019NatCo..10.4515L}}</ref> The {{chem2|Mg2N4}} is composed of exotic ''cis''-tetranitrogen {{chem2|N4(4−)}} species with N-N bond orders close to one. This {{chem2|Mg2N4}} compound was recovered to ambient conditions, along with the {{chem2|N4(4−)}} units, marking only the fourth polynitrogen entity bulk stabilized at ambient conditions. |
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==Uses and history== |
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When isolating ], ] passed dry air over ] to remove ] and over ] to remove the ], forming magnesium nitride. |
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Magnesium nitride was the ] in the first practical synthesis of ] (cubic ]).<ref>{{cite journal |
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Magnesium nitride was the ] in the first practical synthesis of ] (cubic ]).<ref>{{cite journal |
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| author = R. H. Wentorf, Jr. |
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| author = R. H. Wentorf, Jr. |
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| authorlink = Robert H. Wentorf, Jr. |
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| authorlink = Robert H. Wentorf, Jr. |
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| year = 1961 |
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| date=March 1961 |
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| title = Synthesis of the Cubic Form of Boron Nitride |
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| month = March |
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| journal = Journal of Chemical Physics |
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| title = Synthesis of the Cubic Form of Boron Nitride |
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| volume = 34 |
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| journal = Journal of Chemical Physics |
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| volume = 34 |
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| issue = 3 |
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| issue = 3 |
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| pages = 809–812 |
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| doi = 10.1063/1.1731679 |
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| pages = 809–812 |
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| doi = 10.1063/1.1731679 |
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| bibcode = 1961JChPh..34..809W |
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}}</ref> |
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}}</ref> |
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] was trying to convert the hexagonal form of boron nitride into the cubic form by a combination of heat, pressure, and a catalyst. He had already tried all the logical catalysts (for instance, those that catalyze the synthesis of ]), but with no success. |
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] was trying to convert the hexagonal form of boron nitride into the cubic form by a combination of heat, pressure, and a catalyst. He had already tried all the logical catalysts (for instance, those that catalyze the synthesis of ]), but with no success. |
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| accessdate = June 28, 2006 |
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| accessdate = June 28, 2006 |
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| author = Robert H. Wentorf, Jr. |
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| author = Robert H. Wentorf, Jr. |
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| year = 1993 |
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| date=October 1993 |
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| month = October |
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| work = R&D Innovator |
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| work = R&D Innovator |
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}}</ref>), 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 ], something only diamond was known to do. |
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}}</ref>), 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 ], something only diamond was known to do. |
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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. |
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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. |
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Magnesium nitride has also been applied to synthesize aluminum nitride nanocrystals, cubic boron nitride and nitrides of aluminum and Group 3 <ref>{{Cite journal|last1=Zong|first1=Fujian|last2=Meng|first2=Chunzhan|last3=Guo|first3=Zhiming|last4=Ji|first4=Feng|last5=Xiao|first5=Hongdi|last6=Zhang|first6=Xijian|last7=Ma|first7=Jin|last8=Ma|first8=Honglei|title=Synthesis and characterization of magnesium nitride powder formed by Mg direct reaction with N2|journal=_Journal of Alloys and Compounds|year=2010 |volume=508|issue=1|pages=172–176|doi=10.1016/j.jallcom.2010.07.224}}</ref> It has also been proposed as an intermediate in a fossil-fuel-free nitrogen fixation process.<ref>{{Cite journal|last1=Hu|first1=Yang|last2=Chen|first2=George Z.|last3=Zhuang|first3=Lin|last4=Wang|first4=Zhivong|last5=Jin|first5=Xianbo|title=Indirect electrosynthesis of ammonia from nitrogen and water by a magnesium chloride cycle at atmospheric pressure|journal=Cell Reports Physical Science|year=2021 |volume=2|issue=5|page=100425|issn=2666-3864|doi=10.1016/j.xcrp.2021.100425|bibcode=2021CRPS....200425H |s2cid=235555007 |doi-access=free}}</ref> |
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==References== |
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==References== |
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{{reflist}} |
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{{reflist}} |
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==Further reading== |
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* {{cite journal |author1=Wu, P. |author2=Tiedje, T. | year = 2018| title = Molecular beam epitaxy growth and optical properties of Mg<sub>3</sub>N<sub>2</sub> films | journal = Applied Physics Letters | volume = 113 | issue = 8 | pages = 082101 | publisher = ] | doi = 10.1063/1.5035560 |bibcode=2018ApPhL.113h2101W |s2cid=125356057}} |
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{{Magnesium compounds}} |
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{{Magnesium compounds}} |
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{{Nitrides}} |
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{{DEFAULTSORT:Magnesium Nitride}} |
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{{DEFAULTSORT:Magnesium Nitride}} |
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