Chemistry:Zinc nitrate

Zinc nitrate
Names
	IUPAC name Zinc nitrate
	Other names Zinc dinitrate
Identifiers
CAS Number	7779-88-6 ; 19154-63-3 (tetrahydrate) ; 10196-18-6 (hexahydrate) ;
3D model (JSmol)	Interactive image;
ChemSpider	22926 ;
EC Number	231-943-8;
PubChem CID	24518;
RTECS number	ZH4772000;
UNII	EDO66F5U49 ;
UN number	1514
	InChI InChI=1S/2NO3.Zn/c22-1(3)4;/q2-1;+2 Key: ONDPHDOFVYQSGI-UHFFFAOYSA-N ; InChI=1/2NO3.Zn/c22-1(3)4;/q2-1;+2 Key: ONDPHDOFVYQSGI-UHFFFAOYAQ;
	SMILES [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Zn+2];
Properties
Chemical formula	Zn(NO; 3); 2
Molar mass	189.36 g/mol (anhydrous); 297.49 g/mol (hexahydrate)
Appearance	colorless, deliquescent crystals
Density	2.065 g/cm3 (hexahydrate)
Melting point	110 °C (230 °F; 383 K) (anhydrous); 45.5 °C (trihydrate); 36.4 °C (hexahydrate)
Boiling point	~ 125 °C (257 °F; 398 K) decomposes (hexahydrate)
Solubility in water	327 g/(100 mL), 40 °C (trihydrate); 184.3 g/(100 mL), 20 °C (hexahydrate)
Solubility	very soluble in alcohol
Magnetic susceptibility (χ)	−63.0·10−6 cm3/mol
Hazards
Main hazards	Oxidant, may explode on heating
Safety data sheet	ICSC 1206
GHS pictograms
Flash point	Non-flammable
Related compounds
Other anions	Zinc sulfate; Zinc chloride
Other cations	Cadmium nitrate; Mercury(II) nitrate
Related compounds	Copper(II) nitrate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Zinc nitrate is an inorganic chemical compound with the formula Zn(NO
3)
2. This colorless, crystalline salt is highly deliquescent. It is typically encountered as a hexahydrate Zn(NO
3)
2 · 6H₂O. It is soluble in both water and alcohol.

Synthesis

Zinc nitrate is usually prepared by dissolving zinc metal, zinc oxide, or related materials in nitric acid:

Zn + 2 HNO
3 → Zn(NO
3)
2 + H
2

ZnO + 2 HNO
3 → Zn(NO
3)
2 + H
2O

These reactions are accompanied by the hydration of the zinc nitrate.

The anhydrous salt arises by the reaction of anhydrous zinc chloride with nitrogen dioxide:^[1]

ZnCl
2 + 4 NO
2 → Zn(NO
3)
2 + 2 NOCl

Reactions

Treatment of zinc nitrate with acetic anhydride gives zinc acetate.^[2]

On heating, zinc nitrate undergoes thermal decomposition to form zinc oxide, nitrogen dioxide and oxygen:

2 Zn(NO
3)
2 → 2 ZnO + 4 NO
2 + 1 O
2

Applications

Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers.^[3] Its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires.^[4]

It can be used as a mordant in dyeing. An example reaction gives a precipitate of zinc carbonate:

Zn(NO
3)
2 + Na
2CO
3 → ZnCO
3 + 2 NaNO
3

References

↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 455. ISBN 978-0-08-037941-8.
↑ O. F. Wagenknecht; R. Juza (1963). "Zinc Acetate". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 2. NY, NY: Academic Press. p. 1087.
↑ Barnett, Sarah A; Champness, Neil R (November 2003). "Structural diversity of building-blocks in coordination framework synthesis—combining M(NO3)2 junctions and bipyridyl ligands". Coordination Chemistry Reviews 246 (1–2): 145–168. doi:10.1016/S0010-8545(03)00121-8.
↑ Greene, Lori E.; Yuhas, Benjamin D.; Law, Matt; Zitoun, David; Yang, Peidong (September 2006). "Solution-Grown Zinc Oxide Nanowires". Inorganic Chemistry 45 (19): 7535–7543. doi:10.1021/ic0601900. PMID 16961338.