Copper (II) oxide

Copper (II) oxide. It is a metallic oxide, black gray in color, found in nature contained in the mineral Tenorite. It is the copper oxide with the highest oxidation number. Its chemical formula is CuO.

Summary

[ hide ]

• 1 Historical Review
  • 1 Physical properties
  • 2 Chemical Properties
  • 3 Obtaining copper oxide II
• 2 Applications
• 3 Health effects
• 4 Sources

Historical review

Copper oxide II is the main content of the mineral Tenorite , it was named by the Italian botanist Michele Tenore ( 1780 – 1861 ), its name comes in honor of the discoverer’s last name. According to the IUPAC the simple formula is CuO.

It occurs in the open or in rusty areas related to the deepest primary deposits of copper sulfide , that is, with chrysocolla and copper, azurite and malachite carbonates. The opaque gray-black color of the tenorite contrasts sharply with the blue veining of the chrysocolla.

Physical properties

Color:

• Black gray

– Density :

6,515

Molar mass :

• 79,545 g / mol

Solubility in water :

• Insoluble

Solubility in Ethanol :

• Insoluble

Ammoniacal aqueous solution:

• Soluble

Melting temperature:

• 1201 ° C

Boiling temperature:

• 2000 ° C

Crystal structure:

• monoclinic

Chemical formula:

• CuO

Chemical properties

The copper oxide (II) is a basic oxide and dissolved in mineral acids such as hydrochloric acid , the sulfuric acid or nitric acid to give the corresponding salts of copper (II):

• CuO + 2 HNO ₃= Cu (NO ₃ ) ₂ + H ₂ O
• CuO + 2 HCl = CuCl ₂+ H ₂ O
• CuO + H ₂SO ₄ = CuSO ₄ + H ₂ O

Reacts with concentrated alkali to form corresponding cuprate salts.

• 3 XOH + CuO + H2O → X3 [Cu (OH) 6]

It can be reduced to metallic copper using hydrogen or carbon monoxide:

• CuO (s) + H ₂(g) = Cu + H ₂ O (g)
• CuO (s) + CO (g) = Cu + CO ₂(g)

Obtaining copper oxide II

Copper oxide II can be obtained by direct combustion of copper in the presence of air:

2 Cu (s) + O ₂ (g) = 2 CuO (s)

During this process, copper (I) oxide is also obtained as a side product, so it is better to prepare it by heating copper (II) nitrate, copper (II) hydroxide or copper (II) carbonate:

• 2 Cu (NO ₃) 2 (s) = 2 CuO (s) + 4 NO ₂ + O ₂
• Cu (OH) ₂(s) = C _or O (s) + H ₂ O (l)
• CuCO ₃(s) = CuO (s) + CO ₂

In the laboratory it can be obtained from the electrolysis of water containing sodium bicarbonate at a moderate voltage with a copper anode, and then collect the mixture of copper hydroxide, basic copper carbonate, and produced copper carbonate, and heat it.

Applications

1. It is used in consumer products such as pillowcases and socks, due to its cosmetic and antimicrobial properties. The risk of skin sensitivity to copper is considered extremely small.
2. Cupric oxide is used as a pigment in ceramicsto produce blue, red, and green (and sometimes gray, pink, or black) enamels.
3. It is occasionally used as a dietary supplement in copper deficient animals.
4. It is used as a p-type semiconductorbecause it has a narrow band gap of 1.2 eV. It is an abrasive used to polish optical equipment.
5. It can be used to produce dry cells. And in wet cells as a cathode , with lithium as the anode , and dioxalane mixed with lithium perchlorate as the electrolyte.
6. Copper (II) oxide can be used to produce other copper salts. Another use is as a substitute for iron (II) oxide in termite. This can change the termite from incendiary to a low explosive.

Health effects

• Contact with the eyes can cause irritation and significant damage to the cornea, which can cause conjunctivitis. On the skin it causes irritation and discoloration. Ingestion of copper (II) oxide powder can result in a metallic taste, nausea, vomiting, and stomach pain.
• Inhalation can cause damage to the lungsand the diaphragm and its vapors during the fusion of cupric oxide powder can lead to a disease called metallic smoke fever, which can cause flu-like symptoms and can also cause damage to the endocrine system and  central nervous .
• Handling of copper (II) oxide powder should be done in a well-ventilated area, as copper is a trace mineral essential for the normal function of many tissues, including the nervous system, immune system, heart, skin and for the formation of capillaries, being extremely well metabolized by humans.

Use in substance removal:

Cupric oxide can be used to safely remove hazardous materials such as cyanide , hydrocarbons , halogenated hydrocarbons , and dioxins, through oxidation .