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Oxygen is reknown for its ability to combust or combine with other elements and form compounds known as oxides. Two of the most famously known compounds that fall into this category are carbon dioxide (CO2) and carbon monoxide (CO). These provide good example of the first two types of oxide valences, which are oxide (O2, -4), where each oxygen has room for two electrons, and peroxide (O2, -2), where each oxygen provides room for one electron and leaves room for another electron charge. There is a third oxide called a superoxide (O2,-1), that uses half an electron vacancy for each oxygen atom. Other examples of common oxides are phosphorous pentoxide, (P4O10), and iron oxide, or rust (FeO, Fe2O3, Fe3O4). There are even some examples where oxygen will combine to form a cation, where there is an excess of positive charge, as with nitrosonin (NO+).
There are four different types of oxides:
1. Normal Oxides (-2) Valencies
2. Per oxides (-1) Valencies
3. Super oxides (-1/2) Valencies
4. Sub oxides Valencies is not defined
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