Azanide
![]() | |
Names | |
---|---|
Pronunciation | A-za-nayd |
IUPAC name
Azanide
| |
Other names
monoamide, amide ion, ammonia ion, amide
| |
Identifiers | |
3D model (JSmol)
|
|
ChEBI | |
ChemSpider | |
PubChem CID
|
|
CompTox Dashboard (EPA)
|
|
| |
| |
Properties | |
H2N− | |
Molar mass | 16.024 g·mol−1 |
Conjugate acid | Ammonia |
Structure | |
Bent | |
Related compounds | |
Related isoelectronic
|
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 (M = Li, Na, K)
(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[]
- ^ a b Bergstrom, F. W. (1940). "Sodium Amide". Organic Syntheses. 20: 86. doi:10.15227/orgsyn.020.0086.
- ^ a b P. W. Schenk (1963). "Lithium amide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. 1. New York, NY: Academic Press. p. 454.
- ^ a b O. Glemser, H. Sauer (1963). "Silver Amide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry. 1 (2nd ed.). New York, NY: Academic Press. p. 1043.
- ^ Greenlee, K. W.; Henne, A. L. (1946). "Sodium Amide". Inorganic Syntheses. Inorganic Syntheses. 2. pp. 128–135. doi:10.1002/9780470132333.ch38. ISBN 9780470132333.
- Anions
- Nitrogen hydrides