Zinc amide

Crystal structure
__ Zn 2+      __ N 3−      __ H +
General
Surname	Zinc amide
other names	Diamino zinc Zinc diazanide
Ratio formula	Zn (NH 2 ) 2
Brief description	colorless solid
External identifiers / databases
CAS number 13470-41-2 PubChem 23629652 Wikidata Q4064287
properties
Molar mass	97.4 g mol −1
Physical state	firmly
density	2.13 g cm −3
solubility	almost insoluble in ammonia
safety instructions
GHS hazard labeling no classification available
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Zinc amide is an inorganic chemical compound of zinc from the group of amides .

Extraction and presentation

Amorphous zinc amide can be obtained by reacting zinc diethyl with ammonia at 150 ° C.

${\displaystyle \mathrm {Zn(C_{2}H_{5})_{2}+2\ NH_{3}\longrightarrow Zn(NH_{2})_{2}+2\ C_{2}H_{6}} }$

Zinc amide can also be obtained by reacting zinc nitrate with potassium amide in ammonia, with an excess of potassium amide also forming the complex compound potassium ammonium zincate .

${\displaystyle \mathrm {Zn(NO_{3})_{2}+2\ KNH_{2}\longrightarrow Zn(NH_{2})_{2}+2\ KNO_{3}} }$

${\displaystyle \mathrm {Zn(NH_{2})_{2}+2\ KNH_{2}\longrightarrow K_{2}[Zn(NH_{2})_{4}]} }$

properties

Zinc amide is a colorless solid that slowly decomposes in air. Crystalline zinc amide is formed from the amorphous product by heating under ammonothermal conditions in an autoclave. The crystalline form has a crystal structure with the space group I 4 ₁ / acd (space group no. 142) and is isotype to that of magnesium amide and beryllium amide . The compound is amphoteric in ammonia . At 350 ° C it decomposes with the formation of zinc nitride .

${\displaystyle \mathrm {3\ Zn(NH_{2})_{2}\ {\xrightarrow {350\ ^{\circ }C}}\ Zn_{3}N_{2}+4\ NH_{3}} }$

Individual evidence

1. ↑ ^{a b c d e} Georg Brauer , with the collaboration of Marianne Baudler u. a. (Ed.): Handbook of Preparative Inorganic Chemistry . 3rd, revised edition. tape I . Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , pp. 1030 .
2. ^ ^{A b} A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 653.
3. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
4. ↑ Gopalan, R .: Inorganic Chemistry for Undergraduates . Universities Press, 2009, ISBN 81-7371-660-9 , pp. 139 ( limited preview in Google Book search).
5. ↑ B. Fröhling, G. Kreiner, H. Jacobs: Synthesis and crystal structure of manganese (II) - and zinc amide, Mn (NH2) 2 and Zn (NH2) 2. In: Journal of Inorganic and General Chemistry. 625, 1999, pp. 211-216, doi : 10.1002 / (SICI) 1521-3749 (199902) 625: 2 <211 :: AID-ZAAC211> 3.0.CO; 2-1 .
6. ^ Mary Eagleson: Concise Encyclopedia Chemistry . Walter de Gruyter, 1994, ISBN 3-11-011451-8 , p. 1197 ( limited preview in Google Book Search).