Zinc nitride

Zinc nitride
Identifiers
1313-49-1 YesY
ECHA InfoCard 100.013.826
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]
Hazards
not listed
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
0
1
1
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]

3Zn(NH2)2 → Zn3N2 + 4NH3

It can also be formed by heating zinc to 600 °C in a current of ammonia; the by-product is hydrogen gas.[3][5]

3Zn + 2NH3 → Zn3N2 + 3H2

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]

Zn3N2 + 3H2O → 3ZnO + 2NH3

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

  1. 1 2 3 4 CRC Handbook of Chemistry and Physics (96 ed.), §4-100 Physical Constants of Inorganic Compounds
  2. 1 2 Partin, D. E.; Williams, D. J.; O'Keeffe, M. (1997). "The Crystal Structures of Mg3N2 and Zn3N2". Journal of Solid State Chemistry. 132 (1): 56–59. Bibcode:1997JSSCh.132...56P. doi:10.1006/jssc.1997.7407.
  3. 1 2 3 Roscoe, H. E.; Schorlemmer, C. (1907) [1878]. A Treatise on Chemistry: Volume II, The Metals (4th ed.). London: Macmillan. pp. 650–651. Retrieved 2007-11-01.
  4. 1 2 Bloxam, C. L. (1903). Chemistry, Inorganic and Organic (9th ed.). Philadelphia: P. Blakiston's Son & Co. p. 380. Retrieved 2007-10-31.
  5. ↑ Lowry, M. T. (1922). Inorganic Chemistry. Macmillan. p. 872. Retrieved 2007-11-01.
  6. 1 2 Maxtead, E.B. (1921), Ammonia and the Nitrides, pp. =69–20
  7. 1 2 3 Mellor, J.W. (1964), A Comprehensive Treatise on Inorganic and Theoretical Chemistry, 8, Part 1, pp. 160–161
  8. ↑ Maile, E.; Fischer, R. A. (Oct 2005), "MOCVD of the Cubic Zinc Nitride Phase, Zn3N2, Using Zn[N(SiMe3)2]2 and Ammonia as Precursors", Chemical Vapour Deposition, 11 (10): 409–414, doi:10.1002/cvde.200506383
  9. ↑ Ebru, S.T.; Ramazan, E.; Hamide, K. (2007), "Structural and Optical Properties of Zinc Nitride Films Prepared by Pulsed Filtered Cathodic Vacuum Arc Deposition" (PDF), CHIN.PHYS.LETT., 24 (12): 3477, doi:10.1088/0256-307x/24/12/051
  10. ↑ Toyoura, Kazuaki; Tsujimura, Hiroyuki; Goto, Takuya; Hachiya, Kan; Hagiwara, Rika; Ito, Yasuhiko (2005), "Optical properties of zinc nitride formed by molten salt electrochemical process", Thin Solid Films (492): 88–92
  11. ↑ Amatucci, G. G.; Pereira, N. (2004). "Nitride and Silicide Negative Electrodes". In Nazri, G.-A.; Pistoia, G. Lithium Batteries: Science and Technology. Kluwer Academic Publishers. p. 256. ISBN 978-1-4020-7628-2. Retrieved 2007-11-01.
  12. ↑ Pereiraa, N.; Klein, L.C.; Amatuccia, G.G. (2002), "The Electrochemistry of Zn3 N 2 and LiZnN - A Lithium Reaction Mechanism for Metal Nitride Electrodes", Journal of the Electrochemical Society, 149 (3), doi:10.1149/1.1446079

Further reading

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