Which elements tend to exhibit higher ionization energies?

Nonmetals tend to exhibit higher ionization energies due to their position on the periodic table and their electron configurations. Ionization energy is the energy required to remove an electron from an atom in the gas phase. Nonmetals, which are found on the right side of the periodic table, have a nearly full valence shell, making it more energetically favorable for them to gain electrons rather than lose them. As a result, they hold onto their electrons tightly, requiring more energy to remove one.

In contrast, metals, which are located on the left side of the periodic table, typically have lower ionization energies. This is because they possess fewer valence electrons and a more significant tendency to lose electrons to achieve a stable electron configuration. Metalloids display properties intermediate between metals and nonmetals, resulting in ionization energies that are also intermediate. Noble gases, although they have high ionization energies due to their complete valence shells, are typically not the focus in this context since they are already stable and unlikely to lose electrons in chemical reactions.

Thus, nonmetals are characterized by their higher ionization energies because of their electron affinity and effective nuclear charge, making the removal of electrons more challenging compared to other categories of elements.