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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.

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$)	List-$II$ (Element)
$A$. $1510$	$1$. $H$
$B$. $495, 6500, 10200$	$2$. $Li$
$C$. $840, 1630, 13100$	$3$. $Be$
$D$. $600, 2050, 3100$	$4$. $B$

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:

Similar Questions

The successive ionization energies of an element $(A)$ are given as $IE_1 = 20 \ eV, IE_2 = 45 \ eV, IE_3 = 150 \ eV, IE_4 = 900 \ eV, IE_5 = 1800 \ eV$. What is the formula of the halide of $(A)$?

The correct trend in the first ionization enthalpies of the elements in the $3^{rd}$ period of periodic table is:

The first ionization energy of boron is less than that of beryllium because

Match List-$I$ with List-$II$ with correct code:

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$) List-$II$ (Element)

$A$. $1510$ $1$. $H$

$B$. $495, 6500, 10200$ $2$. $Li$

$C$. $840, 1630, 13100$ $3$. $Be$

$D$. $600, 2050, 3100$ $4$. $B$

In which of the following arrangements is the order not correct according to the property indicated against it?

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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: