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(B) The ionization energy of an anion depends on the effective nuclear charge and the inter-electronic repulsions. As we move down the group from $O^{

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$S^{-}$

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(B) The ionization energy of an anion depends on the effective nuclear charge and the inter-electronic repulsions. As we move down the group from $O^{-}$ to $Te^{-}$,the size of the atom increases,which decreases the ionization energy. However,for $O^{-}$,the electron density is concentrated in a smaller $2p$ orbital,leading to significant inter-electronic repulsion. This makes the removal of an electron from $O^{-}$ easier compared to $S^{-}$. Thus,$S^{-}$ has a higher ionization energy than $O^{-}$. Therefore,the trend for ionization energy among these species is $S^{-} > Se^{-} > Te^{-} > O^{-}$.

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

Which of the following atomic species has maximum ionisation energy?

Similar Questions

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$ $801$

$Al$ $577$

$Ga$ $579$

$In$ $558$

$Tl$ $589$

How would you explain this deviation from the general trend?

Given below are two statements:
Statement $I$: The second ionization enthalpy of $B$, $Al$ and $Ga$ is in the order of $B > Al > Ga$.
Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.

Suppose a gaseous mixture of $He$, $Ne$, $Ar$ and $Kr$ is treated with photons of the frequency appropriate to ionize $Ar$. What ion$(s)$ will be present in the mixture?

The correct order of ionisation energy for comparing carbon,nitrogen,and oxygen atoms is:

Which of the following elements has the lowest ionisation potential?

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