Chemistry

Examples of Metallic Oxides

We explain that what are examples of metallic oxides? In chemistry, metal oxides are the compounds that result from the combination of metals with oxygen . In this formation process called oxidation , each oxygen atom receives two electrons to complete its Octet Rule and thus achieve stability. Due to the variety of valences in the atoms of metals, these will join in different numbers to oxygen to complete the two electrons mentioned.

During oxidation, metals oxidize by giving up the negative charges of their electrons. On the other hand, oxygen atoms are reduced , since they receive those electrons. This process is called the REDOX reaction , or oxidation-reduction reaction, and both oxidation and reduction occur simultaneously. There is no one without the other . This union occurs by ionic bonding.
The general formula that describes this chemical change is:

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Metal + oxygen = metal oxide

Rust on a metal forms when it is exposed to high humidity and outdoors for a period of time. This creates a layer of its oxide on its surface. This causes the metallic material to weaken and disintegrate. This phenomenon of wear of the metal is called corrosion , and it reduces its usefulness when performing its functions. For this reason, anti-corrosion products are marketed to protect the surface and prevent moisture from leaving the metal susceptible to rusting.

Formation of metal oxides

Molecules of metal oxides are naturally formed by the action of oxygen in atmospheric air on the surface of metals . This process becomes easier when there is a high percentage of humidity (water vapor) in the environment. The water intervenes by providing a means for the external structure of the metal to weaken and tend to react more. Thus, the metal atoms will deliver their valence electrons to those of oxygen.

When rust forms, it appears as a powdery substance that dulls the shine of the metal. Depending on the element it comes from, it will take different colors. For example, iron oxide (Fe 2 O 3 ) is red-orange and copper oxide (CuO) is blue-green. As can be seen in the subscripts of their formulas, two iron atoms are needed to combine with three oxygen atoms (Fe 2 O 3 ), and one copper atom to join one oxygen atom (CuO).

 

Nomenclature of metal oxides

Metal oxides can be named in two ways based on the valence of the metal :

  • With the endings bear and ico .
  • With the valence in Roman numeral.

Nomenclature with bear and ico endings

To name the oxides with the endings bear and ico , follow these steps:

  1. The word “rust” is written
  2. The valence of the metal is observed
  3. If it is the lowest valence, the name of the metal is written with a “bear” ending. If it is the greatest valence, the name of the metal is written with the ending “ico”.
  4. If the metal only has one valence , it is written “oxide + of + metal name”.

For example:

  • Iron Valences: +2, +3. Its oxides are FeO ferrous oxide; Fe 2 O 3 , ferric oxide.
  • Copper Valences: +1, +2. Its oxides are Cu 2 O cuprous oxide; CuO, cupric oxide.
  • Mercury Valences: +1, +2. Its oxides are Hg 2 O mercurous oxide; HgO mercuric oxide.
  • Zinc Valencia: +2. Its oxide is ZnO, zinc oxide.
  • Sodium Valencia: +1. Its oxide is Na 2 O, sodium oxide.
  • Calcium Valencia: +2. Its oxide is CaO, calcium oxide.

Nomenclature with valence in Roman numeral

To name the metal oxides with their valence in Roman numerals, just follow these steps:

  1. The word oxide is written , followed by de .
  2. The name of the element is written.
  3. The valence of the element is written in Roman numerals.
  4. If the element has only one valence, the Roman numeral is omitted.

For example:

  • FeO: iron oxide II
  • Fe 2 O 3 : iron oxide III
  • Cu 2 O: copper oxide I
  • CuO: copper oxide II
  • Hg 2 O: mercury oxide I
  • HgO: mercury oxide II
  • ZnO: zinc oxide
  • Na 2 O: sodium oxide
  • CaO: calcium oxide

40 examples of metal oxides

  1. Li 2 O: lithium oxide
  2. Na 2 O: sodium oxide
  3. K 2 O: potassium oxide
  4. Rb 2 O: rubidium oxide
  5. Cs 2 O: cesium oxide
  6. MgO: magnesium oxide
  7. CaO: calcium oxide
  8. SrO: strontium oxide
  9. BaO: barium oxide
  10. ZnO: zinc oxide
  11. FeO: ferrous oxide or iron oxide II
  12. Fe 2 O 3 : ferric oxide or iron oxide III
  13. Hg 2 O: mercurous oxide or mercury oxide I
  14. HgO: mercuric oxide or mercury oxide II
  15. TiO 2 : titanium dioxide
  16. SnO: stannous oxide or tin oxide II
  17. Sn 2 O 4 : stannic oxide or tin oxide IV
  18. MnO 2 : manganese dioxide or manganese oxide IV
  19. Mn 2 O 7 : manganese heptoxide or manganese oxide VII
  20. PbO: plumb oxide or lead oxide II
  21. Pb 2 O 4 : lead oxide or lead oxide IV
  22. Cu 2 O: cuprous oxide or copper oxide I
  23. CuO: cupric oxide or copper oxide II
  24. CrO: chromium oxide or chromium II oxide
  25. Cr 2 O 3 : chromic oxide or chromium III oxide
  26. CrO 3 : chromium trioxide or chromium VI oxide
  27. Au 2 O: aurous oxide or gold oxide I
  28. Au 2 O 3 : auric oxide or gold oxide II
  29. Ag 2 O: silver oxide
  30. CoO: cobalt oxide or cobalt II oxide
  31. Co 2 O 3 : cobalt oxide or cobalt III oxide
  32. WO: tungsten oxide or tungsten oxide II
  33. W 2 O 3 : tungsten oxide or tungsten oxide III
  34. W 2 O 4 : tungsten oxide IV
  35. W 2 O 6 : tungsten oxide VI
  36. PtO: platinous oxide or platinum oxide II
  37. Pt 2 O 3 : platinum oxide or platinum oxide III
  38. Cd 2 O: cadmium oxide or cadmium oxide I
  39. CdO: Cadmic Oxide or Cadmium Oxide II
  40. PdO: palladium oxide II

 

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