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(C) The electronic configuration of $Tb$ $(Z=65)$ is $[Xe] 4f^9 6s^2$. Therefore,$Tb^{4+}$ has the configuration $[Xe] 4f^7$,which is half-filled. The

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$Tb^{4+}$ and $Yb^{2+}$

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(C) The electronic configuration of $Tb$ $(Z=65)$ is $[Xe] 4f^9 6s^2$. Therefore,$Tb^{4+}$ has the configuration $[Xe] 4f^7$,which is half-filled. The electronic configuration of $Yb$ $(Z=70)$ is $[Xe] 4f^{14} 6s^2$. Therefore,$Yb^{2+}$ has the configuration $[Xe] 4f^{14}$,which is completely filled. Thus,$Tb^{4+}$ and $Yb^{2+}$ correspond to half-filled and completely filled $f$ orbitals,respectively.

The $f$ orbitals are half-filled and completely filled,respectively,in which of the following lanthanide ions?
(Given: Atomic numbers: $Eu=63, Sm=62, Tm=69, Tb=65, Yb=70, Dy=66$)

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The $f$ orbitals are half-filled and completely filled,respectively,in which of the following lanthanide ions? (Given: Atomic numbers: $Eu=63, Sm=62, Tm=69, Tb=65, Yb=70, Dy=66$)