Copper(II) nitrate Identifiers Properties Hazards
IUPAC name Copper(II) nitrate
other names Cupric nitrate
CAS number 3251-23-8
RTECS number GL7875000
molecular formula Cu(NO3)2
Molar mass 187.57 g/mol, 241.60 (Cu(NO3)2.3H2O),232.59 (Cu(NO3)2.2.5H2O
Appearance blue crystals
Density 2.32 g/cm3 (anhydrous)
melt point

114.5°C (trihydrate)210°C sublimation (anhydrous)

boil point

170°C (decomposition)

Solubility in water 138 g/100 mL (0 °C) trihydrate
MSDS Cu(NO3)2.3H2O
main hazards Toxic, irritant
NFPA 704
0
3
0

Copper(II) nitrate is the chemical compound v the formula Cu(NO3)2. Generally referred to merely as copper nitrate, the anhydrous form is a blue, crystalline solid. Hydrated creates of copper nitrate, likewise blue, are generally used in college laboratories to demonstrate chemical voltaic cabinet reactions. The hydrated and anhydrous varieties have remarkably different properties, showing the result of water that crystallization.

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The Roman character sign is come specify that the copper has an oxidation state of +2.


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Contents


1 Properties

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Properties

Hydrated and anhydrous copper nitrates act differently.

Anhydrous form

The bright blue anhydrous material, Cu(NO3)2, is a volatile solid, subliming in a vacuum. In the gas-phase, Cu(NO3)2 is square planar, each Cu center being surrounded by 4 oxygen atoms. ~ above condensation, this monomer polymerizes.<1>

character language copper nitrate

Crystalline Cu(NO3)2(H2O)2.5 attributes octahedral Cu centers surrounded by water and also the nitrate anions.<1>This hydrate decomposes in ~ ca. 170 °C into copper(II) oxide, nitrogen dioxide and oxygen:

2Cu(NO3)2(s) → 2CuO(s) + 4NO2(g) + O2(g)

Copper nitrate have the right to be used to create nitric acid by heater it until decomposition and also passing the fumes directly into water. This an approach is comparable to the last step in the Ostwald process. The equations room as follows:

2Cu(NO3)2 → 2CuO + 4NO2 + O23NO2 + H2O → 2 HNO3 + NO

Copper nitrate wet splints of wood burn with an emerald green flame. Enhancement of Magnesium nitrate gives a lime eco-friendly color.

Synthesis

Cu(NO3)2 develops when copper metal is treated with N2O4:<2>

Cu + 2 N2O4 → Cu(NO3)2 + 2 NO

It can additionally be formed by reacting copper steel with an aqueous solution of silver- nitrate, view this page for more info.

usage in essential synthesis

Copper nitrate, in combination with acetic anhydride, is an effective reagent because that nitration of aromatic compounds, under what are well-known as "Menke conditions", in respect of the dutch chemist who discovered that steel nitrates are efficient reagents for nitration.<3>Hydrated copper nitrate took in onto clay affords a reagent dubbed "claycop". The resulting blue clay is used as a slurry, for example for the oxidation of thiols to disulfides. Claycop is likewise used to convert dithioacetals to carbonyls.<4> A associated reagent based upon Montmorillonite has actually proven beneficial for the nitration of fragrant compounds.

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References


Categories: Copper link | Nitrates


This write-up is license is granted under the GNU complimentary Documentation License. It uses material from the Wikipedia article "Copper(II)_nitrate". A list of authors is available in Wikipedia.