Zinc nitrate

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;
ChEBI	CHEBI:231504;
ChemSpider	22926 ;
ECHA InfoCard	100.029.038
EC Number	231-943-8;
PubChem CID	24518;
RTECS number	ZH4772000;
UNII	EDO66F5U49 ;
UN number	1514
CompTox Dashboard (EPA)	DTXSID10890636 ;
	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(NO3)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
	Occupational safety and health (OHS/OSH):
Main hazards	Oxidant, may explode on heating
	GHS labelling:
Pictograms
Flash point	Non-flammable
Safety data sheet (SDS)	ICSC 1206
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). verify (what is ?) Infobox references

Zinc nitrate is an inorganic chemical compound with the formula Zn(NO₃)₂. This colorless, crystalline salt is highly deliquescent. It is typically encountered as a hexahydrate Zn(NO₃)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 HNO₃ → Zn(NO₃)₂ + H₂

ZnO + 2 HNO₃ → Zn(NO₃)₂ + H₂O

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]

ZnCl₂ + 4 NO₂ → Zn(NO₃)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(NO₃)₂ → 2 ZnO + 4 NO₂ + 1 O₂

Aqueous zinc nitrate contains aquo complexes [Zn(H₂O)₆]²⁺ and [Zn(H₂O)₄]²⁺.^[3] and, thus, this reaction may be better written as the reaction of the aquated ion with hydroxide through donation of a proton, as follows.

Applications

Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers.^[4] Its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires.^[5]

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

Zn(NO₃)₂ + Na₂CO₃ → ZnCO₃ + 2 NaNO₃

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 (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1087.
^ Sze, Yu-Keung, and Donald E. Irish. "Vibrational spectral studies of ion-ion and ion-solvent interactions. I. Zinc nitrate in water." Journal of Solution Chemistry 7.6 (1978): 395-415.
^ 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.

[G&E-1] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 455. ISBN 978-0-08-037941-8.

[2] O. F. Wagenknecht; R. Juza (1963). "Zinc Acetate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1087.

[3] Sze, Yu-Keung, and Donald E. Irish. "Vibrational spectral studies of ion-ion and ion-solvent interactions. I. Zinc nitrate in water." Journal of Solution Chemistry 7.6 (1978): 395-415.

[4] 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.

[5] 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.

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Zinc nitrate

Synthesis

Reactions

Applications

References

Information related to Zinc nitrate

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