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Explain in terms of atomic structure, why cesium has a lower first ionization energy than rubidium. Determine the family/group in which each element is located

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Answer:

Explain in terms of atomic structure, why Cesium (Cs) has a LOWER first ionization energy than Rubidium (Rb). Cesium is further down on the periodic table. ... The ion K+1 has one more electron than the atom K. K+1 has lost one electron from its valence shell, and therefore has one less electron shell than K.

Explanation:

Cricetus

Radium contains the most electron shells, which creates a shielding effect that reduces the ionization energy.

Radium:

  • [tex][Rn]7 S^2[/tex] Layer atomic radius

Calcium:

  • [tex][Ar]4S^2[/tex] Smaller atomic radius

A higher proportion of electron shells creates a shielding effect, resulting throughout a decreased zeff as well as easier ionization of the outermost election.

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