Oxide



An oxide is a corrosion.

Most oxides are insoluble in water

The oxide proton from a solvent H2O molecule:

O2− + H2O → 2 OH−

Although many anions are stable in aqueous solution, ionic oxides are not. For example, hydroxide:

CaO + H2O → Ca2+ + 2 OH-

In fact, no monoatomic dianion is known to dissolve in water - all are so basic that they undergo hydrolysis. Concentrations of oxide ion in water are too low to be detectable with current technology.

Authentic soluble oxides do exist, but they release oxyanions, not O2−. Well known soluble salts of oxyanions include potassium permanganate (KMnO4), and sodium nitrate (NaNO3).

Nomenclature

In the 18th century, oxides were named calxes or calces after the calcination process used to produce oxides. Calx was later replaced by oxyd.

Oxides are usually named after the number of oxygen atoms in the oxide. Oxides containing only one oxygen are called oxides or monoxides, those containing two oxygen atoms are dioxides, three oxygen atoms makes it a trioxide, four oxygen atoms are tetroxides, and so on following the Greek numerical prefixes.

Two other types of oxide are oxidation states than oxide.

Types of oxides

Oxides of more electropositive elements tend to be basic. They are called basic anhydrides; adding water, they may form basic sodium hydroxide.

Oxides of more perchloric acid is a more hydrated form.

Some oxides can act as both acid and base at different times. They are aluminium oxide. Some oxides do not show behavior as either acid or base.

The oxides of the O10

List of all known oxides sorted by oxidation state

  • Element in −1 oxidation state
    • F2)
  • Element in +1 oxidation state
    • O)
    • Dicarbon monoxide (O)
    • Dichlorine monoxide (O)
    • Lithium oxide (O)
    • O)
    • O)
    • O)
    • Thallium oxide (O)
    • Sodium oxide (O)
    • O)
  • Element in +2 oxidation state
    • O)
    • Barium oxide (O)
    • O)
    • Cadmium oxide (O)
    • O)
    • O)
    • Cobalt(II) oxide (O)
    • O)
    • Iron(II) oxide (O)
    • Lead(II) oxide (O)
    • O)
    • Mercury(II) oxide (O)
    • Nickel(II) oxide (O)
    • Nitrogen oxide (O)
    • Palladium(II) oxide (PdO)
    • Silver(II) oxide (O)
    • Strontium oxide (O)
    • O)
    • Tin(II) oxide (O)
    • Titanium(II) oxide (O)
    • Vanadium(II) oxide (O)
    • O)
  • Element in +3 oxidation state
    • O3)
    • O3)
    • O3)
    • O3)
    • O3)
    • O3)
    • O3)
    • Erbium(III) oxide (O3)
    • Gadolinium(III) oxide (O3)
    • Gallium(III) oxide (O3)
    • Holmium(III) oxide (O3)
    • Indium(III) oxide (O3)
    • O3)
    • O3)
    • Lutetium(III) oxide (O3)
    • O3)
    • Phosphorus trioxide (O6)
    • Promethium(III) oxide (O3)
    • Rhodium(III) oxide (O3)
    • Samarium(III) oxide (O3)
    • Scandium(III) oxide (O3)
    • Terbium(III) oxide (O3)
    • Thallium(III) oxide (O3)
    • Thulium(III) oxide (O3)
    • Titanium(III) oxide (O3)
    • Tungsten(III) oxide (O3)
    • Vanadium(III) oxide (O3)
    • Ytterbium(III) oxide (O3)
    • Yttrium(III) oxide (O3)
  • Element in +4 oxidation state
    • O2)
    • O3)
    • O2)
    • O2)
    • O2)
    • O4)
    • O2)
    • Hafnium(IV) oxide (O2)
    • Lead(I) peroxide (O2)
    • O2)
    • O2)
    • O2)
    • Ruthenium(IV) oxide (O2)
    • O2)
    • O2)
    • O2)
    • O2)
    • O2)
    • Tin dioxide (O2)
    • O2)
    • Tungsten(IV) oxide (O2)
    • O2)
    • Vanadium(IV) oxide (O2)
    • O2)
  • Element in +5 oxidation state
    • Antimony pentoxide (O5)
    • O5)
    • O5)
    • Niobium pentoxide
    • O5)
    • O5)
    • O5)
  • Element in +6 oxidation state
    • O3)
    • O3)
    • Rhenium trioxide (O3)
    • Selenium trioxide (O3)
    • O3)
    • Tellurium trioxide (O3)
    • O4)
    • O3)
    • O3)
    • Xenon trioxide (O3)
  • Element in +8 oxidation state

See also

References

  1. ^ Fully Exploiting the Potential of the Periodic Table through Pattern Recognition Schultz, Emeric. J. Chem. Educ. 2005 82 1649.
 
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