Zinc nitride
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| Identifiers | |
|---|---|
1313-49-1  |
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| Properties | |
| Zn3N2 | |
| Molar mass | 224.154 g/mol |
| Appearance | blue-gray cubic crystals[1] |
| Density | 6.22 g/cm³, solid[1] |
| Melting point | decomposes 700°C[1] |
| insoluble (decomposes) | |
| Structure | |
| Cubic, cI80 | |
| Ia-3, No. 206[2] | |
| Vapor pressure | {{{value}}} |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
Zinc nitride (Zn3N2) is an inorganic compound of zinc and nitrogen, usually obtained as (blue)grey crystals. It is a semiconductor. In pure form, it has the anti-bixbyite structure.
Chemical properties
Zinc nitride can be obtained by thermally decomposing zincamide (zinc diamine)[3] in an anaerobic environment, at temperatures in excess of 200 °C. The by-product of the reaction is ammonia.[4]
It can also be formed by heating zinc to 600 °C in a current of ammonia; the by-product is hydrogen gas.[3][5]
The decomposition of Zinc Nitride into the elements at the same temperature is a competing reaction.[6] At 700°C Zinc Nitride decomposes.[1] It has also been made by producing an electric discharge between zinc electrodes in a nitrogen atmosphere.[6][7] Thins films have been produced by chemical vapour deposition of Bis(bis(trimethylsilyl)amido]zinc with ammonia gas onto silica or ZnO coated alumina at 275 to 410°C.[8]
The crystal structure is anti-isomorphous with Manganese(III) oxide. (bixbyite).[2][7] The heat of formation is c. 24 kilocalories (100 kJ) per mol.[7] It is a semiconductor with a reported bandgap of c. 3.2eV,[9] however , a thin zinc nitride film prepared by electrolysis of molten salt mixture containing Li3N with a zinc electrode showed a band-gap of 1.01 eV.[10]
Zinc nitride reacts violently with water to form ammonia and zinc oxide.[3][4]
Zinc nitride reacts with lithium (produced in an electrochemical cell) by insertion. The initial reaction is the irreversible conversion into LiZn in a matrix of beta-Li3N. These products then can be converted reversibly and electrochemicalically into LiZnN and metallic Zn.[11][12]
See also
References
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Further reading
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External links
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