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(C) Statement $I$: The electronic configuration of the ions after the first ionization are $B^+ (2s^2)$, $Al^+ (3s^2)$, and $Ga^+ (4s^2)$. As the prin

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Statement $I$ is true but Statement $II$ is false

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(C) Statement $I$: The electronic configuration of the ions after the first ionization are $B^+ (2s^2)$, $Al^+ (3s^2)$, and $Ga^+ (4s^2)$. As the principal quantum number increases from $B$ to $Ga$, the size of the ion increases, leading to a decrease in the ionization enthalpy. Thus, the order $B > Al > Ga$ is correct.Statement $II$: The general trend for the first ionization enthalpy in group $14$ is $C > Si > Ge > Sn < Pb$. Due to the poor shielding effect of $d$ and $f$ electrons in $Pb$, the effective nuclear charge increases, making the first ionization enthalpy of $Pb$ higher than that of $Sn$. The given order $Si < Ge < Pb < Sn$ is incorrect.

Given below are two statements:
Statement $I$: The second ionization enthalpy of $B$, $Al$ and $Ga$ is in the order of $B > Al > Ga$.
Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.

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Given below are two statements:Statement $I$: The second ionization enthalpy of $B$, $Al$ and $Ga$ is in the order of $B > Al > Ga$.Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.