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(D) The first ionization energy decreases as we move down a group in the periodic table due to an increase in atomic size and shielding effect. Carbon

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Tin

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(D) The first ionization energy decreases as we move down a group in the periodic table due to an increase in atomic size and shielding effect. Carbon $(C)$,Silicon $(Si)$,Tin $(Sn)$,and Lead $(Pb)$ belong to Group $14$. Among these,$Sn$ and $Pb$ are lower in the group than $C$ and $Si$. However,due to the poor shielding effect of $d$ and $f$ orbitals in $Pb$,the effective nuclear charge increases,which makes the ionization energy of $Pb$ higher than that of $Sn$. Therefore,$Sn$ $(Tin)$ has the lowest first ionization energy among the given options.

The first ionization energy is the lowest for which of the following elements?

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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:

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