Chemistry

Question Analysis
This question evaluates the understanding of the periodic trend in ionization energy and the factors that influence it as you move down a group in the periodic table.

Key Concept Explanation
Ionization energy generally decreases down a group due to the increasing atomic radius. As you move down a group, additional electron shells are added, increasing the distance between the nucleus and the outermost electrons. This increased distance reduces the attraction between the nucleus and the outermost electrons, making it easier to remove an electron.

Step-by-step Solution
1. Identify the trend: Ionization energy decreases down a group.
2. Consider the factors that influence ionization energy:
Nuclear charge (positive correlation)
Atomic radius (negative correlation)
E...