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

$Cl > F > S > P$

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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 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

The formation of the oxide ion $O_{(g)}^{2-}$ requires first an exothermic and then an endothermic step as shown below. This is because
$O_{(g)} + e^{-} \rightarrow O_{(g)}^{-}; \Delta H^{o} = -142 \ kJ \ mol^{-1}$
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Which of the following will have the most negative electron gain enthalpy and which the least negative?
$P, S, Cl, F$
Explain your answer.

Which of the following elements has a positive electron gain enthalpy?

If the electron affinity of an element $M$ is $x \ kJ/mol$,then the ionisation potential of this element is:

Which of the following elements have the highest and lowest electron gain enthalpy,respectively?

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