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CuO + 2 HCl → CuCl 2 + H 2 O CuO + H 2 SO 4 → CuSO 4 + H 2 O. In presence of water it reacts with concentrated alkali to form the corresponding cuprate salts: 2 NaOH + CuO + H 2 O → Na 2 [Cu(OH) 4] It can also be reduced to copper metal using hydrogen, carbon monoxide, and carbon: CuO + H 2 → Cu + H 2 O CuO + CO → Cu + CO 2 2 CuO + C ...
Copper(II) oxide (cupric oxide, CuO) Copper peroxide (CuO 2), a hypothetical compound; Paramelaconite (copper(I,II) oxide, Cu 4 O 3) Copper(III) oxide (Cu 2 O 3) does not exist although Cu(III) is a component of cuprate superconductors; Copper(IV) oxide (CuO 2) has been proposed to exist in the gas phase [2]
Copper(I) oxide or cuprous oxide is the inorganic compound with the formula Cu 2 O. It is one of the principal oxides of copper, the other being copper(II) oxide or cupric oxide (CuO).The compound can appear either yellow or red, depending on the size of the particles. [2]
Copper compounds, whether organic complexes or organometallics, promote or catalyse numerous chemical and biological processes. [2] Binary compounds
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).
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]
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Copper(II) oxide – CuO; Copper(II) sulfate – CuSO 4; Copper(II) sulfide – CuS; ... Protonated molecular hydrogen – H + 3; Trioxidane – H 2 O 3; Water - H 2 ...
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