(A) The electron affinity of $Cl$ $(349 \ kJ \ mol^{-1})$ is higher than that of $F$ $(322 \ kJ \ mol^{-1})$. This is because the $2p$ subshell of $F$

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Weaker electron-electron repulsion in $Cl$

(A) The electron affinity of $Cl$ $(349 \ kJ \ mol^{-1})$ is higher than that of $F$ $(322 \ kJ \ mol^{-1})$. This is because the $2p$ subshell of $F$ is very small,leading to significant inter-electronic repulsion when an incoming electron is added. In contrast,the $3p$ subshell of $Cl$ is larger,which results in weaker electron-electron repulsion,making it easier for $Cl$ to accept an electron.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Electron affinity

Medium

The electron affinities of halogens are $F = 322, Cl = 349, Br = 324, I = 295 \ kJ \ mol^{-1}$. The higher value for $Cl$ as compared to that of $F$ is due to :-

A
Weaker electron-electron repulsion in $Cl$
B
Higher atomic radius of $F$
C
Smaller electronegativity of $F$
D
More vacant $p$-subshell in $Cl$

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Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Electron affinity

Discuss the factors affecting electron gain enthalpy and the trend in its variation in the periodic table.

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Column-$I$ shows the electronic configuration of some elements and Column-$II$ shows the values of electron gain enthalpy. Match these values correctly. Match the electronic configuration with the electron gain enthalpy.

Column-$I$ Electronic Configuration Column-$II$ Electron Gain Enthalpy / $kJ \ mol^{-1}$

$(A) \ 1s^2 2s^2 2p^6$ $(1) -53$

$(B) \ 1s^2 2s^2 2p^6 3s^1$ $(2) -328$

$(C) \ 1s^2 2s^2 2p^5$ $(3) -141$

$(D) \ 1s^2 2s^2 2p^4$ $(4) +53$

Medium

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The amount of energy released on the addition of an electron in the outermost shell of an atom is called:

Easy

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Which of the following has the highest electron affinity $(EA)$?

Medium

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The electron gain enthalpy $\Delta_{eg}H$ of $Cl_{(g)}$ is $-349 \ kJ \ mol^{-1}$. If the ground state energy of $Cl_{(g)}$ is $x \ kJ \ mol^{-1}$,the ground state energy (in $kJ \ mol^{-1}$) of $Cl^{-}_{(g)}$ is

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Column-$I$ Electronic Configuration	Column-$II$ Electron Gain Enthalpy / $kJ \ mol^{-1}$
$(A) \ 1s^2 2s^2 2p^6$	$(1) -53$
$(B) \ 1s^2 2s^2 2p^6 3s^1$	$(2) -328$
$(C) \ 1s^2 2s^2 2p^5$	$(3) -141$
$(D) \ 1s^2 2s^2 2p^4$	$(4) +53$

The electron affinities of halogens are $F = 322, Cl = 349, Br = 324, I = 295 \ kJ \ mol^{-1}$. The higher value for $Cl$ as compared to that of $F$ is due to :-

Similar Questions

Discuss the factors affecting electron gain enthalpy and the trend in its variation in the periodic table.

The amount of energy released on the addition of an electron in the outermost shell of an atom is called:

Which of the following has the highest electron affinity $(EA)$?

The electron gain enthalpy $\Delta_{eg}H$ of $Cl_{(g)}$ is $-349 \ kJ \ mol^{-1}$. If the ground state energy of $Cl_{(g)}$ is $x \ kJ \ mol^{-1}$,the ground state energy (in $kJ \ mol^{-1}$) of $Cl^{-}_{(g)}$ is

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