Within each pair of elements of F and Cl,S an | vedclass

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(C) $(i)$ The electron gain enthalpy (or electron affinity) of the second period $p$-block elements is less negative than that of the corresponding th

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$Cl, S$ and $Li$

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(C) $(i)$ The electron gain enthalpy (or electron affinity) of the second period $p$-block elements is less negative than that of the corresponding third period $p$-block elements due to the small size and high inter-electronic repulsion in the $2p$ subshell. Thus,for the pair $F$ and $Cl$,$Cl$ releases more energy.$(ii)$ Down a group,the electron gain enthalpy generally becomes less negative as the atomic size increases. Thus,for the pair $S$ and $Se$,$S$ releases more energy,and for the pair $Li$ and $Na$,$Li$ releases more energy.Therefore,the correct elements are $Cl, S$,and $Li$.

Within each pair of elements of $F$ and $Cl$,$S$ and $Se$,and $Li$ and $Na$,respectively,the elements that release more energy upon an electron gain are

Similar Questions

Which of the following statements is correct?

Which of the following pairs of elements would have a more negative electron gain enthalpy?
$(i)$ $O$ or $F$
$(ii)$ $F$ or $Cl$

Which one of the following statements is incorrect?

The electron affinity of chlorine is $3.7 \ eV$. $1 \ g$ of chlorine is completely converted to $Cl^-$ ion in a gaseous state. $(1 \ eV = 23.06 \ kcal \ mol^{-1})$. Energy released in the process is $...... \ kcal$.

Explain the periodicity of electron gain enthalpy of elements in the periodic table.

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