Cu(s) + 2 H2SO4(l) + 3 H2O(l) CuSO4·5 H2O(s) + SO2(g)The compound also occurs naturally as the mineral chalcanthite- one of the few soluble sulfate minerals. It is also called "bluestone", "copper vitriol", and "flower of copper".
The beautiful blue color arises from water molecules attached directly to the copper(II) ion. The water/copper ion complex absorbs photons of yellow or red light. Absorption of a photon promotes an electron from the water to the copper(II) ion. Since only yellow or red light is absorbed, blue light is transmitted, and the crystals appear blue.
If blue crystalline CuSO4·5 H2O is heated strongly, the hydration water is driven off, leaving white powdery CuSO4 ("anhydrous" copper(II) sulfate). The blue will reappear if the anhydrous copper sulfate is exposed to even small amounts of moisture, making it sometimes useful as a spot test for water.
Four waters are directly bound to the copper to form a Cu(H2O)42+ ion, with the copper at the center of a square formed by the oxygens of the waters. The crystal structure of copper(II) sulfate pentahydrate can be pictured as an array of these Cu(H2O)42+ ions bridged by sulfate ions (SO42-) and water molecules, with one sulfate and one water per Cu(H2O)4+2 ion.
Copper(II) sulfate is used in:
Copper sulfate's toxicity has curtailed its use as an algaecide and fungicide. (In the 19th century it was actually used as a blue food coloring!)
Author: Fred Senese email@example.com
Copyright © 1997-2010 by Fred Senese
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Last Revised 08/17/15.URL: http://antoine.frostburg.edu/chem/senese/101/inorganic/faq/print-blue-vitriol.shtml