Copper ( II ) nitrate - wikipedia Copper ( II ) nitrate Not to be confused with Copper ( I ) nitrate. Copper ( II ) nitrate Names IUPAC name Copper ( II ) nitrate Other names Cupric nitrate Identifiers CAS Number 3251 - 23 - 8 10031 - 43 - 3 ( trihydrate ) 13478 - 38 - 1 ( hexahydrate ) 19004 - 19 - 4 ( hemipentahydrate ) 3D model ( JSmol ) Interactive image ChEBI CHEBI : 78036 ChemSpider 17582 ECHA InfoCard 100.019. 853 PubChem CID 18616 RTECS number GL7875000 UNII 9TC879S2ZV InChI 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 SMILES ( Cu + 2 ). ( O - ) ( N+ ) ( ( O - ) ) = O. ( O - ) ( N+ ) ( ( O - ) ) = O Properties Chemical formula Cu ( NO ) Molar mass 187.5558 g / mol ( anhydrous ) 241.60 g / mol ( trihydrate ) 232.591 g / mol ( hemipentahydrate ) Appearance blue crystals hygroscopic Density 3.05 g / cm ( anhydrous ) 2.32 g / cm ( trihydrate ) 2.07 g / cm ( hexahydrate ) Melting point 256 ° C ( 493 ° F ; 529 K ) ( anhydrous, decomposes ) 114.5 ° C ( trihydrate ) 26.4 ° C ( hexahydrate, decomposes ) Boiling point 170 ° C ( 338 ° F ; 443 K ) ( trihydrate, decomposes ) Solubility in water trihydrate : 381 g / 100 mL ( 40 ° C ) 666 g / 100 mL ( 80 ° C ) hexahydrate : 243.7 g / 100 mL ( 80 ° C ) Solubility hydrates very soluble in ethanol, ammonia, water ; insoluble in ethyl acetate Magnetic susceptibility ( χ ) + 1570.0 10 cm / mol ( ~ 3H O ) Structure Crystal structure orthorhombic ( anhydrous ) rhombohedral ( hydrates ) Hazards Main hazards Irritant, Oxidizer Safety data sheet Cu ( NO ) 3H O NFPA 704 0 OX US health exposure limits ( NIOSH ) : PEL ( Permissible ) TWA 1 mg / m ( as Cu ) REL ( Recommended ) TWA 1 mg / m ( as Cu ) IDLH ( Immediate danger ) TWA 100 mg / m ( as Cu ) Related compounds Other anions Copper ( II ) sulfate Copper ( II ) chloride Other cations Nickel ( II ) nitrate Zinc nitrate Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). N verify ( what is ? ) Infobox references Copper ( II ) nitrate, Cu ( N O ), is an inorganic compound that forms a blue crystalline solid. Anhydrous copper nitrate forms deep blue - green crystals and sublimes in a vacuum at 150 - 200 ° C. Copper nitrate also occurs as five different hydrates, the most common ones being the trihydrate and hexahydrate. These materials are more commonly encountered in commerce than in the laboratory. Contents 1 Synthesis and reactions for copper nitrate 2 Structure 2.1 Anhydrous copper ( II ) nitrate 2.2 Hydrated copper ( II ) nitrate 3 Applications 3.1 Organic Synthesis 4 References 5 External links Synthesis and reactions for copper nitrate Aqueous solution of copper ( II ) nitrate. Hydrated copper nitrate can be prepared by hydration of the anhydrous material or by treating copper metal with an aqueous solution of silver nitrate or concentrated nitric acid : Cu + 4 HNO → Cu ( NO ) + 2 H O + 2 NO Anhydrous Cu ( NO ) forms when copper metal is treated with N O : Cu + 2 N O → Cu ( NO ) + 2 NO Attempted dehydration of any of the hydrated copper ( II ) nitrates by heating instead affords the oxides, not Cu ( NO ). At 80 ° C, the hydrates convert to `` basic copper nitrate '' ( Cu ( NO ) ( OH ) ), which converts to CuO at 180 ° C. Exploiting this reactivity, 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 ( NO ) → 2 CuO + 4 NO + O 3NO + H O → 2HNO + NO Natural basic copper nitrates include the rare minerals gerhardtite and rouaite, both being polymorphs of Cu ( NO ) ( OH ) substance. Structure Anhydrous copper ( II ) nitrate Anhydrous copper ( II ) nitrate has been crystallized in two solvate - free polymorphs. α - and β - Cu ( NO ) are fully 3D coordination polymer networks. The alpha form has only one Cu environment, with ( 4 + 1 ) coordination, but the beta form has two different copper centers, one with ( 4 + 1 ) and one that is square planar. The nitromethane solvate also features `` ( 4 + 1 ) coordination '', with four short Cu - O bonds of approximately 200 pm and one longer bond at 240 pm. They are coordination polymers, with infinite chains of copper ( II ) centers and nitrate groups. In the gas phase, copper ( II ) nitrate features two bidentate nitrate ligands ( see image at upper right ). Thus, evaporation of the solid entails `` cracking '' to give the copper ( II ) nitrate molecule. Hydrated copper ( II ) nitrate Five hydrates have been reported : the monohydrate ( Cu ( NO ) H O ), the sesquihydrate ( Cu ( NO ) 1.5 H O ), the hemipentahydrate ( Cu ( NO ) 2.5 H O ), a trihydrate ( Cu ( NO ) 3H O ), and a hexahydrate ( Cu ( H O ) ) ( NO ) ). The hexahydrate is interesting because the Cu - O distances are all equal, not revealing the usual effect of Jahn - Teller distortion that is otherwise characteristic of octahedral Cu ( II ) complexes. This non-effect is attributed to the strong hydrogen bonding that limits the elasticity of the Cu - O bonds. Applications Copper ( II ) nitrate finds a variety of applications, the main one being its conversion to copper ( II ) oxide, which is used as catalyst for a variety of processes in organic chemistry. Its solutions are used in textiles and polishing agents for other metals. Copper nitrates are found in some pyrotechnics. It is often used in school laboratories to demonstrate chemical voltaic cell reactions. 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. Hydrated copper nitrate adsorbed 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. A related reagent based on montmorillonite has proven useful for the nitration of aromatic compounds. Wikimedia Commons has media related to Copper ( II ) nitrate. References ^ Jump up to : Perrys ' Chem Eng Handbook, 7th Ed ^ Jump up to : `` NIOSH Pocket Guide to Chemical Hazards # 0150 ''. National Institute for Occupational Safety and Health ( NIOSH ). Jump up ^ Pass and Sutcliffe ( 1968 ). Practical Inorganic Chemistry. London : Chapman and Hall. ^ Jump up to : H. Wayne Richardson `` Copper Compounds '' Ullmann 's Encyclopedia of Industrial Chemistry 2005, Wiley - VCH, Weinheim. doi : 10.1002 / 14356007. a07 567. Jump up ^ Mindat, http://www.mindat.org/min-10588.html Jump up ^ α - Cu ( NO ) S.C. Wallwork, W.E. Addison, `` The crystal structures of anhydrous nitrates and their complexes. Part I. The α form of copper ( II ) nitrate '' J. Chem. Soc. ( 1965 ) 2925 - 2933. doi : 10.1039 / JR9650002925. ^ Jump up to : β - Cu ( NO ) : S.I. Troyanov, I.V. Morozov, K.O. Znamenkov, Yu. M. Korenev, `` Synthesis and X-Ray Structure of New Copper ( II ) Nitrates : Cu ( NO ) H O and β - modification of Cu ( NO ) '' Z. Anorg. Allg. Chem. ( 1995 ) vol. 621, pp. 1261 -- 1265. doi : 10.1002 / zaac. 19956210727 Jump up ^ B. Duffin and S.C. Wallwork `` The crystal structure of anhydrous nitrates and their complexes. II. The 1 : 1 copper ( II ) nitrate - nitromethane complex '' Acta Crystallographica 1966. volume 20, pp. 210 - 213. doi : 10.1107 / S0365110X66000434 Jump up ^ R.E. LaVilla, S.H. Bauer `` The Structure of Gaseous Copper ( II ) Nitrate as Determined by Electron Diffraction '' J. Am. Chem. Soc., 1963, volume 85, pp 3597 -- 3600. doi : 10.1021 / ja00905a015 Jump up ^ K. Dornberger - Schiff, J. Leciejewicz, `` Zur Struktur des Kupfernitrates Cu ( NO ) 1.5 H O '' Acta Crystallogr. 1958, volume 11, pp. 825 -- 826. doi : 10.1107 / S0365110X58002322 Jump up ^ B. Morosin, `` The crystal structure of Cu ( NO ). 2.5 H O '' Acta Crystallogr. 1970, volume B26, pp. 1203 -- 1208. doi : 10.1107 / S0567740870003898 Jump up ^ J. Garaj, Sbornik Prac. Chem. - Technol. Fak. Svst., Cskosl. 1966, pp. 35 -- 39. Jump up ^ R. Zibaseresht, R.M. Hartshorn, `` Hexaaquacopper ( II ) dinitrate : absence of Jahn - Teller distortion '' Acta Crystallogr. 2006, volume E62, pp. i19 -- i22. doi : 10.1107 / S1600536805041851 Jump up ^ Menke J.B. ( 1925 ). `` Nitration with nitrates ''. Recueil des Travaux Chimiques des Pays - Bas. 44 : 141. doi : 10.1002 / recl. 19250440209. Jump up ^ 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. Jump up ^ 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. External links National Pollutant Inventory -- Copper and compounds fact sheet ICSC Copper and compounds fact sheet Copper compounds Cu ( 0, I ) Cu Si Cu ( I ) CuBr CuCN CuCl CuF CuH CuI Cu C Cu Cr O Cu O CuOH CuNO Cu P Cu S CuSCN Cu ( II ) Cu ( BF ) CuBr CuC Cu ( CN ) CuCO CuCl CuF Cu ( NO ) Cu ( PO ) CuN CuO CuO Cu ( OH ) CuI CuS CuSO Cu ( AsO ) Cu ( III ) K CuF Cu O Cu ( IV ) Cs CuF Rb CuF Salts and covalent derivatives of the Nitrate ion HNO He LiNO Be ( NO ) B ( NO ) O FNO Ne NaNO Mg ( NO ) Al ( NO ) Si ClONO Ar KNO Ca ( NO ) Sc ( NO ) Ti ( NO ) VO ( NO ) Cr ( NO ) Mn ( NO ) Fe ( NO ), Fe ( NO ) Co ( NO ), Co ( NO ) Ni ( NO ) Cu ( NO ) Zn ( NO ) Ga ( NO ) Ge As Se Br Kr RbNO Sr ( NO ) Y Zr ( NO ) Nb Mo Tc Ru Rh Pd ( NO ) AgNO Cd ( NO ) In Sn Sb ( NO ) Te Xe ( NO ) CsNO Ba ( NO ) Hf Ta Re Os Ir Pt Au Hg ( NO ), Hg ( NO ) Tl ( NO ), TlNO Pb ( NO ) Bi ( NO ) BiO ( NO ) Po At Rn FrNO Ra ( NO ) Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og ↓ La ( NO ) Ce ( NO ), Ce ( NO ) Pr Nd Pm Sm Eu ( NO ) Gd ( NO ) Tb Dy Ho Er Tm Yb Lu Ac ( NO ) Th ( NO ) Pa UO ( NO ) Np Pu Am Cm Bk Cf Es Fm Md No Lr Retrieved from `` https://en.wikipedia.org/w/index.php?title=Copper(II)_nitrate&oldid=812546180 '' Categories : Copper compounds Nitrates Pyrotechnic oxidizers Pyrotechnic colorants Oxidizing agents Hidden categories : Chemical articles with multiple compound IDs Multiple chemicals in an infobox that need indexing Chemical articles with multiple CAS registry numbers Articles without KEGG source Articles with changed CASNo identifier Articles with changed EBI identifier ECHA InfoCard ID from Wikidata Articles containing unverified chemical infoboxes Talk Contents About Wikipedia تۆرکجه Català Čeština Deutsch فارسی Français 한국어 Italiano ქართული Magyar Nederlands 日本 語 Polski Português Română Русский Simple English Slovenčina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska తెలుగు Tiếng Việt 中文 Edit links This page was last edited on 28 November 2017, at 13 : 09. 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Question: is copper ii nitrate a compound or element
Answer: compound