(b) Which element in the periodic table has the largest ionization energy? Which has the smallest?

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of how strongly an atom holds onto its electrons. Generally, ionization energy increases across a period from left to right due to increasing nuclear charge and decreases down a group as the distance between the nucleus and the outermost electrons increases.

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Key trends include ionization energy, electronegativity, and atomic radius. Understanding these trends helps in predicting the behavior of elements, including which will have the highest or lowest ionization energies.

Noble gases, located in Group 18 of the periodic table, typically have the highest ionization energies due to their stable electron configurations. In contrast, alkali metals in Group 1 have the lowest ionization energies because they have a single electron in their outermost shell, which is easily removed. This distinction is crucial for identifying the elements with the largest and smallest ionization energies.