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Copper(II) sulfate is an inorganic compound with the chemical formula Cu SO 4.It forms hydrates CuSO 4 ·nH 2 O, where n can range from 1 to 7. The pentahydrate (n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper(II) sulfate, [10] while its anhydrous form is white. [11]
Copper is a chemical element with the symbol Cu (from Latin: cuprum) and the atomic number of 29. It is easily recognisable, due to its distinct red-orange color.Copper also has a range of different organic and inorganic salts, having varying oxidation states ranging from (0,I) to (III).
Many other oxyanions form complexes; these include copper(II) acetate, copper(II) nitrate, and copper(II) carbonate. Copper(II) sulfate forms a blue crystalline pentahydrate, the most familiar copper compound in the laboratory. It is used in a fungicide called the Bordeaux mixture. [3]
Tetraamminecopper(II) sulfate monohydrate, or more precisely tetraammineaquacopper(II) sulfate, is the salt with the formula [Cu(N H 3) 4]S O 4 ·H 2 O, or more precisely [Cu(NH 3) 4 (H 2 O)]SO 4. This dark blue to purple solid is a sulfuric acid salt of the metal complex [Cu(NH 3) 4 (H 2 O)] 2+ (tetraammineaquacopper(II) cation).
Basic copper carbonate is a chemical compound, more properly called copper(II) carbonate hydroxide. It can be classified as a coordination polymer or a salt. It consists of copper(II) bonded to carbonate and hydroxide with formula Cu 2 (CO 3)(OH) 2. It is a green solid that occurs in nature as the mineral malachite.
Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO 3) 2 (H 2 O) x. The hydrates are hygroscopic blue solids . Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C.
Copper does not react with hydrogen even on heating, [13] thus copper hydrides are made indirectly from copper(I) and copper(II) precursors. Examples include the reduction of copper(II) sulfate with sodium hypophosphite in the presence of sulfuric acid, [1] or more simply with just hypophosphorous acid. [14]
The formulation of copper sulfide as Cu II S (i.e. containing no sulfur-sulfur bond) is clearly incompatible with the crystal structure, and also at variance with the observed diamagnetism [15] as a Cu(II) compound would have a d 9 configuration and be expected to be paramagnetic. [6]
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