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(D) The electron gain enthalpy $(\Delta_{eg}H)$ generally becomes more negative as we move from left to right across a period due to an increase in ef

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$Ca < Al < C < O < F$

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(D) The electron gain enthalpy $(\Delta_{eg}H)$ generally becomes more negative as we move from left to right across a period due to an increase in effective nuclear charge.It becomes less negative as we move down a group due to an increase in atomic size.Comparing the elements:$1$. $Ca$ (Group $2$,Period $4$): It has a very low electron affinity,often positive or slightly negative.$2$. $Al$ (Group $13$,Period $3$): It has a small negative value.$3$. $C$ (Group $14$,Period $2$): It has a more negative value than $Al$.$4$. $O$ (Group $16$,Period $2$): It has a more negative value than $C$.$5$. $F$ (Group $17$,Period $2$): It has the most negative electron gain enthalpy among these elements.Therefore,the correct order from least negative to most negative is: $Ca < Al < C < O < F$.

Which one of the following arrangements represents the correct order of least negative to most negative electron gain enthalpy for $C, Ca, Al, F$ and $O$?

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