Azanide

Azanide is the IUPAC-sanctioned name for the anion NH2−. The term is obscure: derivatives of NH2− are almost invariably referred to as amides,[1][2][3] despite the fact that amide also refers to the functional group -C(O)NR2. The anion NH2− 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.

This article is about the negative anion. For other compounds with the formula NH2 but different charges, see amino radical and nitrenium ion.
Amide anion
Names
IUPAC name
Azanide
Other names
monoamide, amide ion, ammonia ion, amide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
Properties
H2N−
Molar mass 16.024 g·mol−1
Conjugate acid Ammonia
Structure
Bent
Related compounds
water, fluoronium
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

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 ammonia with strong bases or the alkali metals:.[1][4][2]

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

Potassium amide is prepared similarly.[3]

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

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