Sodium amide

Sodium amide

Names
IUPAC name Sodium amide, sodium azanide[1]
Other names Sodamide
Identifiers
CAS Number	7782-92-5 Y
3D model (JSmol)	Interactive image Interactive image
ChEBI	CHEBI:176791
ChemSpider	22940 N
ECHA InfoCard	100.029.064
EC Number	231-971-0
PubChem CID	24533
UNII	5DB3G6PX9D Y
UN number	1390
CompTox Dashboard (EPA)	DTXSID2064816
InChI InChI=1S/H2N.Na/h1H2;/q-1;+1 N Key: ODZPKZBBUMBTMG-UHFFFAOYSA-N N
SMILES [Na]N [NH2-].[Na+]
Properties
Chemical formula	NaNH2
Molar mass	39.013 g·mol−1
Appearance	Colourless crystals
Odor	Ammonia-like
Density	1.39 g/cm3
Melting point	210 °C (410 °F; 483 K)
Boiling point	400 °C (752 °F; 673 K)
Solubility in water	Reacts
Solubility	40 mg/L (liquid ammonia), reacts with ethanol
Acidity (pKa)	38 (conjugate acid)[2]
Structure
Crystal structure	orthorhombic
Thermochemistry
Heat capacity (C)	66.15 J/(mol·K)
Std molar entropy (S⦵298)	76.9 J/(mol·K)
Std enthalpy of formation (ΔfH⦵298)	-118.8 kJ/mol
Gibbs free energy (ΔfG⦵)	-59 kJ/mol
Hazards
NFPA 704 (fire diamond)	3 2 3 W
Flash point	4.44 °C (39.99 °F; 277.59 K)
Autoignition temperature	450 °C (842 °F; 723 K)
Related compounds
Other anions	Sodium bis(trimethylsilyl)amide
Other cations	Lithium amide Potassium amide
Related compounds	Ammonia
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Sodium amide, commonly called sodamide (systematic name sodium azanide), is the inorganic compound with the formula NaNH₂. It is a salt composed of the sodium cation and the azanide anion. This solid, which is dangerously reactive toward water, is white, but commercial samples are typically gray due to the presence of small quantities of metallic iron from the manufacturing process. Such impurities do not usually affect the utility of the reagent.^{[citation needed]} NaNH₂ conducts electricity in the fused state, its conductance being similar to that of NaOH in a similar state. NaNH₂ has been widely employed as a strong base in organic synthesis.

Sodium amide can be prepared by the reaction of sodium with ammonia gas,^[3] but it is usually prepared by the reaction in liquid ammonia using iron(III) nitrate as a catalyst. The reaction is fastest at the boiling point of the ammonia, c. −33 °C. An electride, [Na(NH₃)₆]⁺e⁻, is formed as a reaction intermediate.^[4]

2 Na + 2 NH₃ → 2 NaNH₂ + H₂

NaNH₂ is a salt-like material and as such, crystallizes as an infinite polymer.^[5] The geometry about sodium is tetrahedral.^[6] In ammonia, NaNH₂ forms conductive solutions, consistent with the presence of [Na(NH₃)₆]⁺ and NH−2 ions.

Sodium amide is mainly used as a strong base in organic chemistry, often suspended (it is insoluble^[7]) in liquid ammonia solution. One of the main advantages to the use of sodium amide is its relatively low nucleophilicity. In the industrial production of indigo, sodium amide is a component of the highly basic mixture that induces cyclisation of N-phenylglycine. The reaction produces ammonia, which is recycled typically.^[8]

Sodium amide is a standard base for dehydrohalogenations.^[9] It induces the loss of two equivalents of hydrogen bromide from a vicinal dibromoalkane to give a carbon–carbon triple bond, as in a preparation of phenylacetylene.^[10] Usually two equivalents of sodium amide yields the desired alkyne. Three equivalents are necessary in the preparation of a terminal alkynes because the terminal CH of the resulting alkyne protonates an equivalent amount of base.

Hydrogen chloride and ethanol can also be eliminated in this way,^[11] as in the preparation of 1-ethoxy-1-butyne.^[12]

Where there is no β-hydrogen to be eliminated, cyclic compounds may be formed, as in the preparation of methylenecyclopropane below.^[13]

Cyclopropenes,^[14] aziridines^[15] and cyclobutanes^[16] may be formed in a similar manner.

Carbon acids which can be deprotonated by sodium amide in liquid ammonia include terminal alkynes,^[17] methyl ketones,^[18] cyclohexanone,^[19] phenylacetic acid and its derivatives^[20] and diphenylmethane.^[21] Acetylacetone loses two protons to form a dianion.^[22] Sodium amide will also deprotonate indole^[23] and piperidine.^[24]

It is however poorly soluble in solvents other than ammonia. Its use has been superseded by the related reagents sodium hydride, sodium bis(trimethylsilyl)amide (NaHMDS), and lithium diisopropylamide (LDA).

• Rearrangement with orthodeprotonation^[25]
• Oxirane synthesis^[26]
• Indole synthesis^[27]
• Chichibabin reaction

Sodium amide is a common reagent with a long history of laboratory use.^[9] It can decompose violently on contact with water, producing ammonia and sodium hydroxide:

NaNH₂ + H₂O → NH₃ + NaOH

When burned in oxygen, it will give oxides of sodium (which react with the produced water, giving sodium hydroxide) along with nitrogen oxides:

4 NaNH₂ + 5 O₂ → 4 NaOH + 4 NO + 2 H₂O

4 NaNH₂ + 7 O₂ → 4 NaOH + 4 NO₂ + 2 H₂O

In the presence of limited quantities of air and moisture, such as in a poorly closed container, explosive mixtures of peroxides may form.^[28] This is accompanied by a yellowing or browning of the solid. As such, sodium amide is to be stored in a tightly closed container, under an atmosphere of an inert gas. Sodium amide samples which are yellow or brown in color represent explosion risks.^[29]