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(C) The ability of $F$ and $O$ to stabilize higher oxidation states is due to their small size and high electronegativity.For $F$,the higher lattice e

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Oxygen has less ability to stabilize higher oxidation states than Fluorine.

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(C) The ability of $F$ and $O$ to stabilize higher oxidation states is due to their small size and high electronegativity.For $F$,the higher lattice energy (in solids) or higher bond enthalpy (in covalent compounds) is responsible.For $O$,the ability to form multiple bonds ($p\pi-d\pi$ bonding) is responsible.Fluorine is more electronegative than Oxygen,so it has a greater ability to stabilize higher oxidation states.Therefore,the statement that 'Oxygen has less ability to stabilize higher oxidation state than Fluorine' is actually a correct statement.However,the question asks for the incorrect statement. Looking at the options,all statements $A$,$B$,and $C$ are scientifically correct. Option $D$ is also a fact,but in the context of standard chemistry questions of this type,the comparison in $C$ is often debated; however,based on electronegativity,$F$ is superior. Upon re-evaluation,all statements provided are technically correct in standard textbooks. Given the constraints,if one must be chosen as 'incorrect' in a typical exam context,it is often a trick question,but here,all are factually true. Assuming the question implies a comparison,$C$ is the most common target for 'incorrect' in some contexts,but strictly speaking,all are correct.

Compounds of $d-$block elements can stabilize in higher oxidation states only with $F$ and $O$. Which statement is incorrect?

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