Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?

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Solution

$Highest oxidation state of a metal$

Oxygen and fluorine are strong oxidizing agents, and both of their oxides and fluorides are highly electronegative in nature and also small in size. Because of these properties, they can oxidize the metal to its highest oxidation states.

This is the reason why the highest oxidation state of a metal exhibited in its oxide or fluoride only.

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Q. The highest oxidation state of a transition metal is usually exhibited in its oxide and fluoride.

Give examples and suggest reasons for the following features of the transition metal chemistry:

(i)The lowest oxide of transition metal is basic, and the highest is amphoteric/acidic.

(ii) A transition metal exhibits the highest oxidation state in oxides and fluorides.

(iii) The highest oxidation state is exhibited in the oxoanions of a metal.

Why does Mn in oxide exhibit higher oxidation state than fluoride?

Highest oxidation state of manganese in fluoride is $+ 4 (M n F_{4}),$ but the highest oxidation state in oxides is $+ 7 (M n_{2} O_{7})$ because ____________.

Q. Copper exhibits only

+ 2

oxidation state in its stable compounds. Why?

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