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Zinc nitride
Identifiers
3D model ( JSmol)
ECHA InfoCard 100.013.826 Edit this at Wikidata
EC Number
  • 215-207-3
PubChem CID
UNII
  • InChI=1S/2N.3Zn/q2*-1;;;+2
    Key: AKJVMGQSGCSQBU-UHFFFAOYSA-N
  • [N-]=[Zn].[N-]=[Zn].[Zn+2]
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, reacts
Structure
Cubic, cI80
Ia-3, No. 206 [2]
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H315, H319
P264, P280, P302+P352, P305+P351+P338, P321, P332+P313, P337+P313, P362
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond Health 1: Exposure would cause irritation but only minor residual injury. E.g. turpentine Flammability 0: Will not burn. E.g. water Instability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorus Special hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
1
0
2
W
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY  verify ( what is checkY☒N ?)

Zinc nitride ( Zn3 N2) 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 + 4 NH3

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

3 Zn + 2 NH3 → Zn3N2 + 3 H2

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] Thin 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 + 3 H2O → 3 ZnO + 2 NH3

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 electrochemically into LiZnN and metallic Zn. [11] [12]

See also

References

  1. ^ a b c d CRC Handbook of Chemistry and Physics (96 ed.), §4-100 Physical Constants of Inorganic Compounds
  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. ^ a b Maxtead, E.B. (1921), Ammonia and the Nitrides, pp. 69–20
  7. ^ a b c Mellor, J.W. (1964), A Comprehensive Treatise on Inorganic and Theoretical Chemistry, vol. 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 Vapor 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, Bibcode: 2007ChPhL..24.3477S, doi: 10.1088/0256-307x/24/12/051, S2CID  123496085
  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 (1–2): 88–92, Bibcode: 2005TSF...492...88T, doi: 10.1016/j.tsf.2005.06.057
  11. ^ Amatucci, G. G.; Pereira, N. (2004). "Nitride and Silicide Negative Electrodes". In Nazri, G.-A.; Pistoia, G. (eds.). 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): A262, Bibcode: 2002JElS..149A.262P, doi: 10.1149/1.1446079

Further reading

External links

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