Examples of Oxides

In chemistry, oxides are the compounds that result from combining an element , either metal or nonmetal, and oxygen . They are present in the earth’s crust and in the atmosphere due to the action of physical and chemical phenomena on the planet. Oxides are classified into two large groups: metallic oxides and non-metallic oxides, which, in addition to being distinguished by the element that accompanies oxygen, does so by the conditions required to form.examples of oxides

 

Examples of OxidesMetal oxides examples of oxides

Metal oxides carry a metal , which can be alkaline, alkaline earth, transitional or part of the rare earth. In order for them to form, there must be abundant humidity in the environment; This will weaken the bonds between the atoms on its surface and oxygen will have access to them to begin to combine and create the oxide, which will appear as a powder of a different color from that of pure metal. examples of oxides

If too much rust is generated, the metal will gradually weaken and become useless for mechanical purposes, for example. It will become brittle. This process is called corrosion , and it is so damaging that the industry manufactures oils and lubricants with anti-corrosion agents, to prevent parts of a mechanism from becoming unusable or breaking during operation. They are also called basic oxides, because when they combine with water they produce hydroxides.

Non-metallic oxides

Non-metallic oxides have a non-metal , which can be Group IIIA in front of the periodic table of elements. For them to form, there must be a sufficient temperature so that the atoms have enough kinetic energy and also their bonds can be broken. This is the case of nitrogen (N 2 ) , which at different temperatures the triple bond of its diatomic molecule will break to form a great variety of oxides: N 2 O, NO, N 2 O 3 , NO 2 , N 2 O 5 , NO 3 , N 2 O 7 .

It is the same case with sulfur oxides (S) , which are generally expressed SOx. Sulfur dioxide SO 2 comes from the roasting (burning at high temperatures) of sulfides, and through further heating and catalytic oxidation, sulfur trioxide SO 3 can be obtained . Non-metallic oxides are also called acid oxides, because when combined with water they produce acids. For example, water is added to sulfur trioxide SO 3 and sulfuric acid H 2 SO 4 is produced. examples of oxides

Another name they receive is anhydrides (etymology: an-hydro “without water”), because they are the molecules that remain from releasing a molecule of water from acids. To explain it more clearly: If a molecule of water H 2 O is removed from sulfuric acid H 2 SO 4 , sulfur trioxide SO 3 remains .

Oxides

 

Examples of Oxides50 examples of oxides

  1. Ag 2 O: Silver oxide
  2. MgO: Magnesium oxide
  3. CaO: Calcium oxide
  4. Na 2 O: Sodium oxide
  5. 2 O: Potassium oxide
  6. SO 2 : Sulfur dioxide
  7. SO 3 : Sulfur trioxide
  8. Al 2 O 3 : Aluminum oxide
  9. PbO: Lead oxide II
  10. Pb 2 O 4 : Lead oxide IV
  11. ZnO: Zinc oxide
  12. TiO 2 : Titanium dioxide
  13. OsO 4 : Osmium Tetroxide
  14. Hg 2 O: Mercury oxide I
  15. HgO: Mercury oxide II
  16. FeO: Iron oxide II
  17. Fe 2 O 3 : Iron oxide III
  18. Cl 2 O: Chlorine oxide I
  19. ClO: Chlorine oxide II
  20. Cl 2 O 3 : Dichloro trioxide
  21. ClO 2 : Chlorine dioxide
  22. Cl 2 O 5 : Dichloro pentoxide
  23. Cl 2 O 7 : Dichloro heptaoxide
  24. CO: Carbon monoxide
  25. CO 2 : Carbon dioxide
  26. SiO 2 : Silicon dioxide
  27. TeO: Tellurium oxide II
  28. TeO 2 : Tellurium oxide IV
  29. SeO: Selenium oxide II
  30. SeO 2 : Selenium oxide IV
  31. Cr 2 O 3 : Chromium III oxide
  32. CrO 3 : Chromium oxide VI
  33. Br 2 O: Bromine oxide I
  34. BrO: Bromine II oxide
  35. Br 2 O 3 : Bromine III oxide
  36. BrO 2 : Bromine oxide IV
  37. Br 2 O 5 : Bromine oxide V
  38. N2O: Nitrous oxide
  39. NO: Nitric oxide
  40. 2 O 3 : Dinitrogen trioxide
  41. NO 2 : Nitrogen dioxide
  42. 2 O 5 : Dinitrogen pentoxide
  43. 2 O 7 : Dinitrogen heptaoxide
  44. MnO 2 : Manganese dioxide
  45. Mn 2 O 7 : Manganese oxide VII
  46. 2 O 3 : Diphosphorous trioxide
  47. 2 O 5 : Diphosphorous pentoxide
  48. Cu 2 O: Cuprous oxide
  49. CuO: Cupric oxide
  50. Mo 2 O 5 : Molybdenum oxide V

 

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