Amide anion
Names
Pronunciation /ˈæzənaɪd/
IUPAC name
Azanide
Other names
monoamide, amide ion, ammonia ion, amide, ammonide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
  • InChI=1S/H2N/h1H2/q-1
    Key: HYGWNUKOUCZBND-UHFFFAOYSA-N
  • [NH2-]
  • [N-]
Properties
NH−2
Molar mass 16.023 g·mol−1
Conjugate acid Ammonia
Structure
Bent
Related compounds
Other anions
 Phosphanide
Arsinide
Imide
Nitride
Nitridohydride
water, fluoronium
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Azanide is the IUPAC-sanctioned name for the anion NH−2. The term is obscure; derivatives of NH−2 are almost invariably referred to as amides,[1][2][3] despite the fact that amide also refers to the organic functional group –C(=O)−NR2. The anion NH−2 is the conjugate base of ammonia, so it is formed by the self-ionization of ammonia. It is produced by deprotonation of ammonia, usually with strong bases or an alkali metal. Azanide has a H–N–H bond angle of 104.5°.

Alkali metal derivatives

The alkali metal derivatives are best known, although usually referred to as alkali metal amides. Examples include lithium amide, sodium amide, and potassium amide. These salt-like solids are produced by treating liquid ammonia with strong bases or directly with the alkali metals (blue liquid ammonia solutions due to the solvated electron):[1][2][4]

2 M + 2 NH3 → 2 MNH2 + H2, where M = Li, Na, K

Silver(I) amide (AgNH2) is prepared similarly.[3]

Transition metal complexes of the amido ligand are often produced by salt metathesis reaction or by deprotonation of metal ammine complexes.

References

  1. 1 2 Bergstrom, F. W. (1940). "Sodium Amide". Organic Syntheses. 20: 86. doi:10.15227/orgsyn.020.0086.
  2. 1 2 P. W. Schenk (1963). "Lithium amide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1. New York, NY: Academic Press. p. 454.
  3. 1 2 O. Glemser, H. Sauer (1963). "Silver Amide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry. Vol. 1 (2nd ed.). New York, NY: Academic Press. p. 1043.
  4. ↑ Greenlee, K. W.; Henne, A. L. (1946). "Sodium Amide". Inorganic Syntheses. Inorganic Syntheses. Vol. 2. pp. 128–135. doi:10.1002/9780470132333.ch38. ISBN 9780470132333.
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