Metal Oxides (basic oxides)

Content

• Nomenclature of metal oxides
• Examples of basic or metallic oxides

The metal oxides (also known as basic oxides) are compounds that originate from the combination of a metal and oxygen, with the particularity of being linked by a link called ionic.

They generally have the characteristic of being solid and have a point of fusion relatively high (precisely this is what is typical of them, differing from the non-metallic oxides which have a much lower one).

The metal oxides they are usually crystalline and at least moderately soluble in water. Metal oxides are good drivers heat and electricity, and that is why they are commonly used for these purposes.

In its composition, metallic oxides are binary combinations of a metal with oxygen, with the latter acting with an oxidation number -2.Therefore, it is necessary to take into account the valences of the metal that intervenes in the reaction together with oxygen, to have a notion of how many atoms of the element it will be necessary to exchange for every atom of oxygen.

• See also: Examples of Oxidation

Nomenclature of metal oxides

Oxides of this type have a particularity with regard to their denomination, since it is not easy to name each one since the same substances sometimes have different oxidation numbers. In the event that the element complementary to oxygen has a single oxidation number, the traditional way of naming it will be 'oxide of (and the corresponding element)'.

When the element has two oxidation numbers, it will be named oxide (and the corresponding element, with the ending ‘bear’If the oxidation number used is lower, and‘ico'When the number is greater). Finally, if the element has more than two oxidation numbers (it can have up to four), the amount of valences is observed and the ending -ico, -oso, hypo-bear, or per-ico is added accordingly. This is the traditional nomenclature, however there are alternatives such as the stock numeral or atomicity.

Examples of basic or metallic oxides

1. Cuprous oxide (Cu₂OR). This copper oxide is insoluble in water and organic solvents.
2. Cupric oxide (CuO). It is the copper oxide with the highest oxidation number. As a mineral it is known as tenorite.
3. Cobaltous oxide(CoO). It is an inorganic monoxide with an olive green or reddish appearance in its crystalline form.
4. Auric oxide (Au₂OR₃). It is the most stable oxide of gold. It has a reddish-brown color, and is insoluble in water.
5. Titanium oxide (Uncle₂₎. It is naturally found in some minerals, in a spherical shape. It is inexpensive, safe, and abundant.
6. Zinc oxide (Z_nOR). It is a white compound, also known as the white zinc compound. It is slightly soluble in water but very soluble in acids.
7. Nickel oxide (Neither₂OR₃). It is a compound of nickel (it has 77% nickel in its composition). It is also known as black nickel oxide.
8. Silver oxide (Ag₂OR). This compound is a fine black or brown powder that is used to prepare other silver compounds.
9. Mercuric oxide (HgO). Mercury (II) oxide is also a compound that has an orange or red color, it occurs in a solid state at room temperature.
10. Chromic oxide (CrO). It is an inorganic compound of chromium and oxygen.
11. Barium oxide (Beam).
12. Chromic oxide (Cr₂OR₃). It is an inorganic compound that is used as a pigment, chromium green.
13. Plumb rust (PbO). With an orange color it is frequently used in ceramics and in the chemical industry.
14. Permanganic oxide.
15. Ferrous oxide (Ugly)
16. Ferric oxide (Faith₂OR₃)
17. Calcium oxide (CaO)
18. Lithium oxide (Li₂OR). 
19. Stannous oxide (SnO).
20. Stannic oxide (SnO2).

They can serve you:

• Examples of Oxides
• Examples of Basic Oxides
• Examples of Acidic Oxides
  
• Examples of Non-Metallic Oxides