Which of the following atoms has the lowest i | vedclass

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(B) Ionization potential is the energy required to remove the most loosely bound electron from an isolated gaseous atom.As we move down a group in the

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$_{55}^{133}Cs$

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(B) Ionization potential is the energy required to remove the most loosely bound electron from an isolated gaseous atom.As we move down a group in the periodic table,the atomic size increases due to the addition of new shells.As the atomic size increases,the distance between the nucleus and the valence electron increases,resulting in a weaker electrostatic force of attraction.Therefore,it becomes easier to remove the valence electron,leading to a decrease in ionization potential.Among the given elements,$_7^{14}N$ (Nitrogen),$_8^{16}O$ (Oxygen),and $_{18}^{40}Ar$ (Argon) are non-metals or noble gases with relatively small atomic radii.$_{55}^{133}Cs$ (Cesium) is an alkali metal located at the bottom of the periodic table (Group $1$,Period $6$),which has the largest atomic radius among the options.Thus,$_{55}^{133}Cs$ has the lowest ionization potential.

Which of the following atoms has the lowest ionization potential?

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