why are the Highest Oxidation states of the transition metals is stabilized in the oxide and fluoride compounds
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The number of electrons that an atom gains, loses or uses to bond with
other atoms influences its oxidation state. This also determines whether
the atom can lose electrons (oxidize) or gain electrons (reduce) other
atoms.
Reduction usually results in decrease in oxidation state while oxidation leads to increase of oxidation state. This therefore means that an atom has a higher number of vallence shell if it is reduced which also means a higher oxidation state making it a strong oxidant.
The best examples of strong oxidants are oxygen and flourine. Both oxide ion and flouride ion are highly electronegative and are very small in size.
As a result of these properties oxide and flouride are able to oxidize metals to the highest oxidation state.
Reduction usually results in decrease in oxidation state while oxidation leads to increase of oxidation state. This therefore means that an atom has a higher number of vallence shell if it is reduced which also means a higher oxidation state making it a strong oxidant.
The best examples of strong oxidants are oxygen and flourine. Both oxide ion and flouride ion are highly electronegative and are very small in size.
As a result of these properties oxide and flouride are able to oxidize metals to the highest oxidation state.
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