Names | |
---|---|
Other names
Silver(I) hyponitrite,
Argentous hyponitrite
| |
Identifiers | |
3D model (
JSmol)
|
|
ChemSpider | |
PubChem
CID
|
|
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties | |
Ag2N2O2 | |
Molar mass | 275.75 |
Appearance | bright canary yellow solid [1] |
Density | 5.75 g/cm3 (at 30 °C) |
slightly soluble | |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Silver hyponitrite is an
ionic compound with formula Ag2N2O2 or (Ag+
)2[ON=NO]2−, containing
monovalent
silver
cations and
hyponitrite
anions. It is a bright yellow solid practically insoluble in water and most organic solvents, including
DMF and
DMSO.
[1]
[2]
[3]
The compound was described in 1848. [4]
The salt can be precipitated from a solution of sodium hyponitrite in water by the addition of silver nitrate: [2]
Excess silver nitrate yields a brown or black precipitate. [1] [2]
Silver hyponitrite can also be prepared by reacting silver nitrate with sodium amalgam. [5]
Silver hyponitrite is sparingly soluble in concentrated
alkali hyponitrite solutions, but quite soluble in aqueous
ammonia due to the formation of the complex cation [(NH
3)2Ag]+.
[6] The compound is slowly decomposed by light.
[5]
The anhydrous compound decomposes in vacuum at 158 °C. The primary decomposition products are
silver(I) oxide Ag
2O and
nitrous oxide N
2O. However, these then react to form a variable mixture of
nitrogen, metallic
silver, and various
oxides of the two elements and silver salts.
[1]
Reaction of silver hyponitrite with anhydrous hydrogen chloride in ether is the standard way to prepare hyponitrous acid:
Spectroscopic data indicate a trans configuration for the resulting acid. [7]
Silver hyponitrite reacts with alkyl halides, to form alkyl hyponitrites. For example, reaction with methyl bromide yields the spontaneously explosive dimethyl hyponitrite: [2]
Other alkyl hyponitrites reported in the literature include those of ethyl, [8] benzyl, [9] [10] [11] and tert-butyl. [12] [13] [14]
Names | |
---|---|
Other names
Silver(I) hyponitrite,
Argentous hyponitrite
| |
Identifiers | |
3D model (
JSmol)
|
|
ChemSpider | |
PubChem
CID
|
|
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties | |
Ag2N2O2 | |
Molar mass | 275.75 |
Appearance | bright canary yellow solid [1] |
Density | 5.75 g/cm3 (at 30 °C) |
slightly soluble | |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Silver hyponitrite is an
ionic compound with formula Ag2N2O2 or (Ag+
)2[ON=NO]2−, containing
monovalent
silver
cations and
hyponitrite
anions. It is a bright yellow solid practically insoluble in water and most organic solvents, including
DMF and
DMSO.
[1]
[2]
[3]
The compound was described in 1848. [4]
The salt can be precipitated from a solution of sodium hyponitrite in water by the addition of silver nitrate: [2]
Excess silver nitrate yields a brown or black precipitate. [1] [2]
Silver hyponitrite can also be prepared by reacting silver nitrate with sodium amalgam. [5]
Silver hyponitrite is sparingly soluble in concentrated
alkali hyponitrite solutions, but quite soluble in aqueous
ammonia due to the formation of the complex cation [(NH
3)2Ag]+.
[6] The compound is slowly decomposed by light.
[5]
The anhydrous compound decomposes in vacuum at 158 °C. The primary decomposition products are
silver(I) oxide Ag
2O and
nitrous oxide N
2O. However, these then react to form a variable mixture of
nitrogen, metallic
silver, and various
oxides of the two elements and silver salts.
[1]
Reaction of silver hyponitrite with anhydrous hydrogen chloride in ether is the standard way to prepare hyponitrous acid:
Spectroscopic data indicate a trans configuration for the resulting acid. [7]
Silver hyponitrite reacts with alkyl halides, to form alkyl hyponitrites. For example, reaction with methyl bromide yields the spontaneously explosive dimethyl hyponitrite: [2]
Other alkyl hyponitrites reported in the literature include those of ethyl, [8] benzyl, [9] [10] [11] and tert-butyl. [12] [13] [14]