Which of the following will have the most negative electron gain enthalpy and which the least negative?
$P, S, Cl, F$
Explain your answer.
$P, S, Cl, F$
Explain your answer.
(A) Electron gain enthalpy generally becomes more negative across a period as we move from left to right.
Within a group,electron gain enthalpy becomes less negative down a group.
However,adding an electron to the $2p$-orbital (as in $F$) leads to greater inter-electronic repulsion than adding an electron to the larger $3p$-orbital (as in $Cl$).
Therefore,$Cl$ has the most negative electron gain enthalpy.
Among the given elements,$P$ has the least negative electron gain enthalpy due to its stable half-filled $3p^3$ electronic configuration.
Within a group,electron gain enthalpy becomes less negative down a group.
However,adding an electron to the $2p$-orbital (as in $F$) leads to greater inter-electronic repulsion than adding an electron to the larger $3p$-orbital (as in $Cl$).
Therefore,$Cl$ has the most negative electron gain enthalpy.
Among the given elements,$P$ has the least negative electron gain enthalpy due to its stable half-filled $3p^3$ electronic configuration.
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Similar Questions
Which element has maximum electron affinity?
Easy
View SolutionMatch the following elements in List-$I$ with their respective electron gain enthalpy values in List-$II$:
List-$I$ (Element) List-$II$ (Electron gain enthalpy in $kJ \ mol^{-1}$) $(A)$ $F$ $(I)$ $-141$ $(B)$ $Cl$ $(II)$ $-328$ $(C)$ $O$ $(III)$ $-200$ $(D)$ $S$ $(IV)$ $-349$
| List-$I$ (Element) | List-$II$ (Electron gain enthalpy in $kJ \ mol^{-1}$) |
|---|---|
| $(A)$ $F$ | $(I)$ $-141$ |
| $(B)$ $Cl$ | $(II)$ $-328$ |
| $(C)$ $O$ | $(III)$ $-200$ |
| $(D)$ $S$ | $(IV)$ $-349$ |
Choose the correct order of $\Delta H_{eg}$ ?
$(\Delta H_{eg} = \text{electron gain enthalpy})$
$(\Delta H_{eg} = \text{electron gain enthalpy})$
Medium
View SolutionThe set containing the elements with positive electron gain enthalpies is
The correct electron affinity order is $(EA = -\Delta H_{EG})$
Medium
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