Azanide

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Amide anion
Azanide-ion-3D-vdW.png
Names
Pronunciation /ˈæzənd/
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
NH2
Molar mass 16.023 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).

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 organic functional groupC(=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. Azanide has a H–N–H bond angle of 104.5°.

Alkali metal derivatives[edit]

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 → 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[edit]

  1. ^ a b Bergstrom, F. W. (1940). "Sodium Amide". Organic Syntheses. 20: 86. doi:10.15227/orgsyn.020.0086.
  2. ^ a b 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. ^ a b 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.