Examples of Oxides
Metal 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 .
50 examples of oxides
- Ag 2 O: Silver oxide
- MgO: Magnesium oxide
- CaO: Calcium oxide
- Na 2 O: Sodium oxide
- K 2 O: Potassium oxide
- SO 2 : Sulfur dioxide
- SO 3 : Sulfur trioxide
- Al 2 O 3 : Aluminum oxide
- PbO: Lead oxide II
- Pb 2 O 4 : Lead oxide IV
- ZnO: Zinc oxide
- TiO 2 : Titanium dioxide
- OsO 4 : Osmium Tetroxide
- Hg 2 O: Mercury oxide I
- HgO: Mercury oxide II
- FeO: Iron oxide II
- Fe 2 O 3 : Iron oxide III
- Cl 2 O: Chlorine oxide I
- ClO: Chlorine oxide II
- Cl 2 O 3 : Dichloro trioxide
- ClO 2 : Chlorine dioxide
- Cl 2 O 5 : Dichloro pentoxide
- Cl 2 O 7 : Dichloro heptaoxide
- CO: Carbon monoxide
- CO 2 : Carbon dioxide
- SiO 2 : Silicon dioxide
- TeO: Tellurium oxide II
- TeO 2 : Tellurium oxide IV
- SeO: Selenium oxide II
- SeO 2 : Selenium oxide IV
- Cr 2 O 3 : Chromium III oxide
- CrO 3 : Chromium oxide VI
- Br 2 O: Bromine oxide I
- BrO: Bromine II oxide
- Br 2 O 3 : Bromine III oxide
- BrO 2 : Bromine oxide IV
- Br 2 O 5 : Bromine oxide V
- N2O: Nitrous oxide
- NO: Nitric oxide
- N 2 O 3 : Dinitrogen trioxide
- NO 2 : Nitrogen dioxide
- N 2 O 5 : Dinitrogen pentoxide
- N 2 O 7 : Dinitrogen heptaoxide
- MnO 2 : Manganese dioxide
- Mn 2 O 7 : Manganese oxide VII
- P 2 O 3 : Diphosphorous trioxide
- P 2 O 5 : Diphosphorous pentoxide
- Cu 2 O: Cuprous oxide
- CuO: Cupric oxide
- Mo 2 O 5 : Molybdenum oxide V
