Which of the following atoms has the highest | vedclass

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(B) The first ionization energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.$K$ $(Z=19)$ and $Na$ $

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$Sc$

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(B) The first ionization energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.$K$ $(Z=19)$ and $Na$ $(Z=11)$ are alkali metals (Group $1$),which have the lowest ionization energies in their respective periods.$Rb$ $(Z=37)$ is also an alkali metal with an even lower ionization energy than $K$ due to its larger atomic size.$Sc$ $(Z=21)$ is a $d$-block transition metal.Transition metals generally have higher first ionization energies compared to alkali metals in the same or adjacent periods because of their smaller atomic radii and higher effective nuclear charge,which holds the valence electrons more tightly.

Which of the following atoms has the highest first ionization energy?

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