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(A) The first ionization energy $(IE_1)$ trend for group $14$ elements is $C > Si > Ge > Sn < Pb$.Statement $I$: The $IE_1$ of $Pb$ $(715 \ kJ/mol)$ i

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

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(A) The first ionization energy $(IE_1)$ trend for group $14$ elements is $C > Si > Ge > Sn Statement $I$: The $IE_1$ of $Pb$ $(715 \ kJ/mol)$ is greater than that of $Sn$ $(708 \ kJ/mol)$ due to the poor shielding effect of $4f$ and $5d$ electrons (lanthanoid contraction),which increases the effective nuclear charge. Thus,Statement $I$ is true.Statement $II$: The $IE_1$ of $Ge$ $(761 \ kJ/mol)$ is less than that of $Si$ $(786 \ kJ/mol)$ because $Si$ is smaller than $Ge$. Thus,Statement $II$ is false.Therefore,Statement $I$ is true but Statement $II$ is false.

Given below are two statements:
Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.
Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.
In the light of the above statements,choose the correct answer from the options given below:

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Given below are two statements:Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.In the light of the above statements,choose the correct answer from the options given below: