Copper(II) nitrate
| Copper(II) nitrate | |
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Copper(II) nitrate
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Other names
Cupric nitrate
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| Identifiers | |
| CAS number | 3251-23-8  |
| PubChem | 18616 |
| ChemSpider | 17582 |
| UNII | 9TC879S2ZV |
| RTECS number | GL7875000 |
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[Cu+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
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InChI=1S/Cu.2NO3/c;2*2-1(3)4/q+2;2*-1
Key: XTVVROIMIGLXTD-UHFFFAOYSA-N
InChI=1/Cu.2NO3/c;2*2-1(3)4/q+2;2*-1 Key: XTVVROIMIGLXTD-UHFFFAOYAG |
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| Properties | |
| Molecular formula | Cu(NO3)2 |
| Molar mass | 187.56 g/mol ( |
| Appearance | blue crystals hygroscopic |
| Density | 3.05 g/cm3 (anhydrous) 2.32 g/cm3 (trihydrate) 2.07 g/cm3 (hexahydrate) |
| Melting point |
256 °C (anhydrous, decomp) |
| Boiling point |
170 °C (trihydrate, decomposes) |
| Solubility in water | 137.8 g/100 mL (0 °C) (trihydrate) |
| Solubility | hydrates very soluble in ethanol, water |
| Structure | |
| Crystal structure | orthorhombic (anhydrous) rhombohedral (hydrates) |
| Hazards | |
| MSDS | Cu(NO3)2·3H2O |
| EU Index | Not listed |
| Main hazards | Toxic, irritant |
| Related compounds | |
| Other anions | Copper(II) sulfate Copper(II) chloride |
| Other cations | Nickel(II) nitrate Zinc nitrate |
 (what is this?) (verify)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references |
Copper(II) nitrate is the chemical compound with the formula Cu(NO3)2. Commonly referred to simply as copper nitrate, the anhydrous form is a blue, crystalline solid. Hydrated forms of copper nitrate, also blue, are commonly used in school laboratories to demonstrate chemical voltaic cell reactions.
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[edit] Synthesis and reactions
Cu(NO3)2 forms when copper metal is treated with N2O4:[1]
- Cu + 2 N2O4 → Cu(NO3)2 + 2 NO
Hydrated copper nitrate can be prepared by hydrolysis of the anhydrous material or by treating copper metal with an aqueous solution of silver nitrate or concentrated nitric acid:
- Cu + 4 HNO3 → Cu(NO3)2 + 2 H2O + 2 NO2
Copper nitrate can be used to generate nitric acid by heating it until decomposition and passing the fumes directly into water. This method is similar to the last step in the Ostwald process. The equations are as follows:
- 2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
- 3NO2 + H2O → 2HNO3 + NO
[edit] Use in organic synthesis
Copper nitrate, in combination with acetic anhydride, is an effective reagent for nitration of aromatic compounds, under what are known as "Menke conditions", in honor of the Dutch chemist who discovered that metal nitrates are effective reagents for nitration.[2] Hydrated copper nitrate absorbed onto clay affords a reagent called "Claycop". The resulting blue-colored clay is used as a slurry, for example for the oxidation of thiols to disulfides. Claycop is also used to convert dithioacetals to carbonyls.[3] A related reagent based on Montmorillonite has proven useful for the nitration of aromatic compounds.[4]
[edit] References
- ^ Jolly, W. L. "The Synthesis and Characterization of Inorganic Compounds" Prentice Hall, London, 1970
- ^ Menke J.B. (1925). "Nitration with nitrates". Recueil des Travaux Chimiques des Payes-Bas 44: 141.
- ^ Balogh, M. "Copper(II) Nitrate–K10 Bentonite Clay" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.
- ^ Collet, C.; Delville, A.; Laszlo, P. “Clays Direct Aromatic Nitration” Angewandte Chemie International Edition in English, 2003, Volume 29, Issue 5 , Pages 535 - 536. doi:10.1002/anie.199005351.
[edit] External links
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