Ionization Energy Among Alkali Metals

The periodic table organizes elements based on their atomic structure, including their atomic numbers and electron configurations. Elements typically display periodic trends in properties such as atomic radius, ionization energy, and electronegativity. For instance, as one moves across a period from left to right, the ionization energy generally increases due to the increased nuclear charge and greater attraction between the nucleus and the valence electrons. Conversely, moving down a group often leads to an increase in atomic radius due to the addition of electron shells. Consider the following elements: lithium (Li), sodium (Na), and potassium (K). Each of these elements is an alkali metal with one valence electron. Which of these elements would you expect to have the highest ionization energy?