In which of the following options are the ele | vedclass

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(C) The electron gain enthalpy becomes more negative as we move across a period,but there are exceptions due to electronic configuration and atomic si

Vedclass · Accepted Answer

$Cl > F > S > P$

Vedclass · Answer

(C) The electron gain enthalpy becomes more negative as we move across a period,but there are exceptions due to electronic configuration and atomic size.$Cl$ has the highest negative electron gain enthalpy among these elements because of its relatively larger size compared to $F$,which reduces inter-electronic repulsion.$F$ has a lower negative electron gain enthalpy than $Cl$ due to its very small size,which causes significant inter-electronic repulsion.Between $S$ and $P$,$S$ has a higher negative electron gain enthalpy than $P$ because $P$ has a stable half-filled $3p^3$ electronic configuration.Therefore,the correct order of negative electron gain enthalpy is: $Cl > F > S > P$.

In which of the following options are the elements correctly arranged with respect to their negative electron gain enthalpies?

Similar Questions

Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of the given atomic species?

Identify the correct order of electron gain enthalpy (electron affinity) for the elements $Be, B, C, N$.

The electron affinity values are negative for:
$A$. $Be \rightarrow Be^{-}$
$B$. $N \rightarrow N^{-}$
$C$. $O^{-} \rightarrow O^{2-}$
$D$. $Na \rightarrow Na^{-}$
$E$. $Al \rightarrow Al^{-}$
Choose the most appropriate answer from the options given below:

The correct order of increasing electron affinity of the following elements is

Which of the following statements is incorrect?

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