Zinc nitride

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Zinc nitride
1313-49-1 YesY
Molar mass 224.15 g/mol[1]
Appearance gray powder[1]
Density 6.22 g/cm³, solid[1]
insoluble (decomposes)
Crystal structure Cubic, cI80
Space group Ia-3, No. 206[1][2]
EU classification 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
Except where noted otherwise, data is 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. In pure form, it is cubic in structure.[1][2]

Chemical properties[edit]

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

Zinc nitride reacts violently with water to form ammonia and zinc oxide.[3][4]

Zn3N2 + 3H2O → 3ZnO + 2NH3

It is soluble in hydrochloric acid[6] and "reversibly reacts with lithium electrochemically".[7] Like magnesium nitride (Mg3N2) and lithium nitride (Li3N), it has a high melting point.[8]

See also[edit]


  1. ^ a b c d e Sangeeta, D. (1997). Inorganic Materials Chemistry Desk Reference. CRC Press. p. 278. ISBN 978-0-8493-8900-9. Retrieved 2007-09-30. 
  2. ^ a b 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. ^ a b c 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. ^ a b 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. ^ Comey, A. M.; Hahn, D. A. (1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: Macmillan. p. 1124. Retrieved 2007-11-01. 
  7. ^ 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. 
  8. ^ Grolier Incorporated (1994). Academic American Encyclopedia. Danbury, CT: Grolier Inc. p. 202. ISBN 978-0-7172-2053-3. Retrieved 2007-11-01. 

Further reading[edit]

External links[edit]