Oxides
Dioxide (in English: Oxide) oxide is a chemical compound of oxygen with another chemical element. Most of the earth's crust consists of oxides. Oxides of interaction with the elements of air is composed.
Ion oxide cathode 2-O, is the conjugate base of the hydroxide ion -OH, and marks meet him in ionic oxides such as calcium oxide.
2-O is unstable in aqueous solution
It produces oxygen union with another element. Oxides formed when elements combine with oxygen. For example, the carbon in coal or wood, producing carbon dioxide CO2 and the carbon dioxide CO combustion. . Burning is a quick oxidation process.
Carbon dioxide in the animal cells composed by the slow oxidation process, and out of the lungs by exhaling.
Iron and steel process slow oxidation process also. It contains rust to ferric oxide Fe2O3.
Metallic oxides combine with water consisting hydroxides base, while when non-metallic oxides combine with water they are Oksgenih acids.
And oxides of sulfur and nitrogen is particularly important; because it can be used for the production of acids. But sulfur dioxide and nitrogen oxides, air pollution when emitted by cars, factories, power plants and coal-fired and oil. They combine with moisture in the air and be different sulphurous acid and nitrogen acid. These acids and hit the ground in the form of acid rain. Acid. This acid and damage plants and wildlife.
When mixing calcium oxide CaO or the so-called neighborhood with lime, hydrated lime is made with water which is used in the coating process in a solution of lime plaster work.
The sand, which is of great importance in the glass industry, it is one of the types of silicon dioxide which is named silica (SiO2). Other types of second silicon oxide quartz, agate, opal.
Types of oxides
Metallic oxides
P oxide (P replaced by the name of the metallic element)
Examples:
Na2O: sodium oxide and MgO: magnesium oxide.
Non-metallic oxides
To find out the name should be the relationship between the number of oxygen atoms and the number of atoms of the element Allamadena account and add the appropriate prefix of the relationship: oxygen atoms to atoms element Allavlz
Uses
As materials
Two examples of the use of oxides: glass (mostly SiO 2 </ sub>), and the silence on the part of the blue and cobalt oxide in addition to some oxides which have many features such as:
Semi-conductors: FeO
Superconductors: the third copper oxide YBa2Cu3O7
Resistors: CeO2 (above the melting point of 3000 ° C), alumina, MgO
Stimulating: alumina (Al2O3), zeolite-based SiO2, and platinum oxides.
Of composite materials in: ceramic, cement, glasses: private and SiO2 in the silica glass and limestone CaCO3 in the cement.
Dyes: TiO2 coating white and various oxides Alkrrom glass.
Nuclear energy: fuel used in the form of oxides as they are more manageable in this form (uranium interacts automatically with air at a given temperature)
In chemical reactions
Iron oxide
Preparation metals (metals):
Iron by Fe2O3 et Fe3O4 (see Steel)
Aluminum from alumina
Hydrogen from water
And many metals such as uranium, tungsten, molybdenum, tin, titanium (traffic from TiCl4), and silicon.
Reactions in organic chemistry:
Reactions to add organic matter to CO2 or metal Keaton
Interaction with SO3 to produce PFOS.
B oxidation MnO4-, CrO3
B drought P2O5
Stimulate, especially alumina and zeolite
Mineral chemistry:
With water to produce oxygen acids such as SO3 + H2O → H2SO4
Strong production bases Na2O
Oxidizing / carrier of oxygen: nitrogen oxides nitric acid factors Albermnganat sugary compound, perchlorate (see explosives)
Dyes, fireworks (metal oxides)
