Azanide
| Names | |
|---|---|
| Pronunciation | /ˈæzənaɪd/ |
| IUPAC name
Azanide | |
Other names
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| Identifiers | |
3D model (JSmol) |
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| ChEBI | |
| ChemSpider | |
PubChem CID |
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CompTox Dashboard (EPA) |
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| Properties | |
| NH−2 | |
| Molar mass | 16.023 g·mol−1 |
| Conjugate acid | Ammonia |
| Structure | |
| Bent | |
| Related compounds | |
Other anions |
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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, 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 2 Bergstrom, F. W. (1940). "Sodium Amide". Organic Syntheses. 20: 86. doi:10.15227/orgsyn.020.0086.
- 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.
- 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.
- ↑ Greenlee, K. W.; Henne, A. L. (1946). "Sodium Amide". Inorganic Syntheses. Vol. 2. pp. 128–135. doi:10.1002/9780470132333.ch38. ISBN 9780470132333.
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