In each of the following sets, which atom or ion has the...

In each of the following sets, which atom or ion has the smallest ionization energy?
a. $\mathrm{Ca}, \mathrm{Sr}, \mathrm{Ba}$
b. $\mathrm{K}, \mathrm{Mn}, \mathrm{Ga}$
c. $\mathrm{N}, \mathrm{O}, \mathrm{F}$
d. $\mathrm{S}^{2-}, \mathrm{S}, \mathrm{S}^{2+}$
e. $\mathrm{Cs}$, Ge, Ar

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Key Concepts

Ionization Energy

Ionization energy is the amount of energy required to remove an electron from a neutral atom or ion. This concept is central in understanding how tightly an electron is bound to an atom, which in turn helps predict chemical reactivity and trends in the periodic table.

Periodic Trends

Periodic trends, such as the increase in ionization energy across a period and the decrease down a group, are essential for predicting differences in electron removal energies among elements. These trends arise from variations in effective nuclear charge and atomic radius.

Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by electrons after accounting for shielding by inner electrons. A higher effective nuclear charge generally results in a stronger pull on the electrons, thus increasing the ionization energy.

Atomic and Ionic Radii

Atomic and ionic radii play a crucial role in determining ionization energy. Larger radii typically mean that outer electrons are farther from the nucleus and experience greater shielding, which lowers the ionization energy, while smaller radii lead to higher ionization energies.

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