The main reason for the actinoids exhibiting | vedclass

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(B) The electronic configuration of lanthanoids is $[Xe] 4f^{1-14} 5d^{0-1} 6s^2$,while for actinoids it is $[Rn] 5f^{1-14} 6d^{0-1} 7s^2$. In actinoi

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The energy difference between $5f$ and $6d$ orbitals is less than that between $4f$ and $5d$ orbitals.

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(B) The electronic configuration of lanthanoids is $[Xe] 4f^{1-14} 5d^{0-1} 6s^2$,while for actinoids it is $[Rn] 5f^{1-14} 6d^{0-1} 7s^2$. In actinoids,the energy difference between the $5f$ and $6d$ orbitals is much smaller than the energy difference between the $4f$ and $5d$ orbitals in lanthanoids. Additionally,because the $5f$ orbitals are further from the nucleus,they are less tightly held,allowing for greater participation in bonding and the exhibition of a wider range of oxidation states.

List-$I$ (Property)	List-$II$ (Element)
$(A)$ Lanthanoid showing $+4$ oxidation state	$(i)$ $Pm$
$(B)$ Lanthanoid showing $+2$ oxidation state	$(ii)$ $Ce$
$(C)$ Radioactive lanthanoid	$(iii)$ $Lu$
$(D)$ Lanthanoid with $4f^7$ configuration in $+3$ state	$(iv)$ $Eu$
$(E)$ Lanthanoid with $4f^{14}$ configuration in $+3$ state	$(v)$ $Gd$
-	$(vi)$ $Dy$

The main reason for the actinoids exhibiting a larger number of oxidation states than the lanthanoids is:

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