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Names | |
---|---|
IUPAC name
Lithium amide
| |
Other names
Lithium azanide
Lithamide | |
Identifiers | |
3D model (
JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.029.062 |
PubChem
CID
|
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
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Properties | |
LiNH2 | |
Molar mass | 22.96 g·mol−1 |
Appearance | white solid |
Density | 1.178 g/cm3 |
Melting point | 375 °C (707 °F; 648 K) |
Boiling point | 430 °C (806 °F; 703 K) decomposes |
reacts | |
Solubility | slightly soluble in
ethanol insoluble in ammonia |
Thermochemistry | |
Std enthalpy of
formation (ΔfH⦵298) |
-182 kJ/mol |
Hazards | |
NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Lithium amide or lithium azanide is an inorganic compound with the chemical formula LiNH2. It is a white solid with a tetragonal crystal structure. [1] Lithium amide can be made by treating lithium metal with liquid ammonia: [2]
The conjugate bases of amines are known as amides. Thus, a lithium amide may also refer to any compound in the class of the lithium salt of an amine. These compounds have the general form LiNR2, with the chemical lithium amide itself as the parent structure. Common lithium amides include lithium diisopropylamide (LDA), lithium tetramethylpiperidide (LiTMP), and lithium hexamethyldisilazide (LiHMDS). They are produced by the reaction of Li metal with the appropriate amine:
Lithium amides are very reactive compounds. Specifically, they are strong bases.
Lithium tetramethylpiperidide has been crystallised as a tetramer. [3] On the other hand, the lithium derivative of bis(1-phenylethyl)amine crystallises as a trimer: [4]
It is also possible to make mixed oligomers of metal alkoxides and amides. [5] These are related to the superbases, which are mixtures of metal alkoxides and alkyls. The cyclic oligomers form when the nitrogen of the amide forms a sigma bond to a lithium, while the nitrogen lone pair binds to another metal centre.
Other organolithium compounds (such as BuLi) are generally considered to exist in and function via high-order, aggregated species.
| |
Names | |
---|---|
IUPAC name
Lithium amide
| |
Other names
Lithium azanide
Lithamide | |
Identifiers | |
3D model (
JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.029.062 |
PubChem
CID
|
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties | |
LiNH2 | |
Molar mass | 22.96 g·mol−1 |
Appearance | white solid |
Density | 1.178 g/cm3 |
Melting point | 375 °C (707 °F; 648 K) |
Boiling point | 430 °C (806 °F; 703 K) decomposes |
reacts | |
Solubility | slightly soluble in
ethanol insoluble in ammonia |
Thermochemistry | |
Std enthalpy of
formation (ΔfH⦵298) |
-182 kJ/mol |
Hazards | |
NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Lithium amide or lithium azanide is an inorganic compound with the chemical formula LiNH2. It is a white solid with a tetragonal crystal structure. [1] Lithium amide can be made by treating lithium metal with liquid ammonia: [2]
The conjugate bases of amines are known as amides. Thus, a lithium amide may also refer to any compound in the class of the lithium salt of an amine. These compounds have the general form LiNR2, with the chemical lithium amide itself as the parent structure. Common lithium amides include lithium diisopropylamide (LDA), lithium tetramethylpiperidide (LiTMP), and lithium hexamethyldisilazide (LiHMDS). They are produced by the reaction of Li metal with the appropriate amine:
Lithium amides are very reactive compounds. Specifically, they are strong bases.
Lithium tetramethylpiperidide has been crystallised as a tetramer. [3] On the other hand, the lithium derivative of bis(1-phenylethyl)amine crystallises as a trimer: [4]
It is also possible to make mixed oligomers of metal alkoxides and amides. [5] These are related to the superbases, which are mixtures of metal alkoxides and alkyls. The cyclic oligomers form when the nitrogen of the amide forms a sigma bond to a lithium, while the nitrogen lone pair binds to another metal centre.
Other organolithium compounds (such as BuLi) are generally considered to exist in and function via high-order, aggregated species.