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(D) The stability of high oxidation states in $d$-block and $p$-block elements generally decreases down a group due to the inert pair effect and the d

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All of the above

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(D) The stability of high oxidation states in $d$-block and $p$-block elements generally decreases down a group due to the inert pair effect and the decrease in the strength of the metal-oxygen bond.$1$. For the oxoanions of $3d$ transition metals,$CrO_4^{2-}$ (Cr is $+6$) is more stable than $MnO_4^{2-}$ (Mn is $+6$) and $FeO_4^{2-}$ (Fe is $+6$).$2$. Comparing $CrO_4^{2-}$ and $WO_4^{2-}$,the stability of the $+6$ oxidation state increases down the group $(Cr $3$. For group $16$ elements,the stability of the $+6$ oxidation state decreases down the group $(Se > Te > Po)$ due to the inert pair effect.Thus,all the given orders are correct.

Column - $I$	Column - $II$
$(a)$ Copper	$(i)$ Non-metal
$(b)$ Fluorine	$(ii)$ Transition Metal
$(c)$ Silicon	$(iii)$ Lanthanoid
$(d)$ Cerium	$(iv)$ Metalloid

Which of the following represents the correct order of stability for the given oxidation states?

Similar Questions

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Which one is wrong in the following statements?

Match the element in column $I$ with that in column $II$.

Column - $I$ Column - $II$

$(a)$ Copper $(i)$ Non-metal

$(b)$ Fluorine $(ii)$ Transition Metal

$(c)$ Silicon $(iii)$ Lanthanoid

$(d)$ Cerium $(iv)$ Metalloid

Identify the correct match:

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