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(C) Isoelectronic species are those that have the same number of electrons.$(A)$ $Pr^{3+}$: Number of electrons $= 59 - 3 = 56$. $Nd^{3+}$: Number of

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$Eu^{2+}, Gd^{3+}$

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(C) Isoelectronic species are those that have the same number of electrons.$(A)$ $Pr^{3+}$: Number of electrons $= 59 - 3 = 56$. $Nd^{3+}$: Number of electrons $= 60 - 3 = 57$. Thus,they are not isoelectronic.$(B)$ $Tb^{3+}$: Number of electrons $= 65 - 3 = 62$. $Dy^{2+}$: Number of electrons $= 66 - 2 = 64$. Thus,they are not isoelectronic.$(C)$ $Eu^{2+}$: Number of electrons $= 63 - 2 = 61$. $Gd^{3+}$: Number of electrons $= 64 - 3 = 61$. Since both have $61$ electrons,they are isoelectronic.$(D)$ $Pr^{3+}$: Number of electrons $= 59 - 3 = 56$. $Ce^{4+}$: Number of electrons $= 58 - 4 = 54$. Thus,they are not isoelectronic.

Identify the isoelectronic pair of ions from the following.

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