The electron affinities of halogens are $F = 322$,$Cl = 349$,$Br = 324$,$I = 295 \ kJ \ mol^{-1}$. The higher value for $Cl$ as compared to that of $F$ is due to
- AWeaker electron-electron repulsion in $Cl$
- BHigher atomic radius of $F$
- CSmaller electronegativity of $F$
- DMore vacant $p-$subshell in $Cl$
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Which one of the elements has the maximum electron affinity?
DifficultAIPMT 1996
View SolutionThe 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:
$A$. $Be \rightarrow Be^{-}$
$B$. $N \rightarrow N^{-}$
$C$. $O^{-} \rightarrow O^{2-}$
$D$. $Na \rightarrow Na^{-}$
$E$. $Al \rightarrow Al^{-}$
Choose the most appropriate answer from the options given below:
The set containing the elements with positive electron gain enthalpies is
Assertion $(A)$: Fluorine has a smaller negative electron gain enthalpy than chlorine.
Reason $(R)$: The electron-electron repulsion is higher in chlorine than in fluorine.
Reason $(R)$: The electron-electron repulsion is higher in chlorine than in fluorine.
Among the following configurations,the element which has the highest electron affinity is
Medium
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