Which of the following elements would typically have the highest ionization energy?

Fluorine typically has the highest ionization energy among the elements listed because it is located further to the right in the periodic table, within the same period as sodium, lithium, and potassium. Ionization energy generally increases across a period due to the increasing nuclear charge, which enhances the attraction between the nucleus and the valence electrons, making them more difficult to remove.

Fluorine, being in Group 17, has a high effective nuclear charge and only needs to remove one valence electron to achieve a stable electronic configuration, akin to noble gases. This stability desired by achieving a full outer electron shell contributes to its high ionization energy.

In contrast, lithium, sodium, and potassium are alkali metals found in Group 1. As you move down the group, ionization energy decreases due to the increasing electron shielding from inner electron layers and the larger atomic radius, which makes the outermost electron easier to remove. Therefore, the ionization energies of lithium, sodium, and potassium are significantly lower than that of fluorine. This trend reflects the principles governing atomic structure and periodic trends.