JEE MAIN - Chemistry (2025 - 3rd April Morning Shift - No. 2)
Which of the following statements are correct?
A. The process of adding an electron to a neutral gaseous atom is always exothermic.
B. The process of removing an electron from an isolated gaseous atom is always endothermic.
C. The $1^{\text {st }}$ ionization energy of boron is less than that of beryllium.
D. The electronegativity of C is 2.5 in $\mathrm{CH}_4$ and $\mathrm{CCl}_4$
E. Li is the most electropositive among elements of group I.
Choose the correct answer from the options given below:
Explanation
(A) The process of adding an $\mathrm{e}^{-}$to a neutral gaseous atom is not always exothermic it may be exothermic or endothermic.
$\begin{array}{cc}\text { (C) } \mathrm{Be} & \mathrm{B} \\ 1 \mathrm{~s}^2 2 s^2 & 1 s^2 2 s^2 2 p^1\end{array}$
In Be 2s subshell in fully filled
So, need high energy to remove $\mathrm{e}^{-}$as compared to B .
_3rd_April_Morning_Shift_en_2_1.png)
due to partially positive charge $z_{\text {eff }} \uparrow, \mathrm{EN} \uparrow$
So, EN of $\mathrm{C} \Rightarrow \mathrm{CCl}_4>\mathrm{CH}_4$
(E) Cs is most electropositive.
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