Final answer:
Rubidium (Rb) has the largest atomic radius among the given elements because it is positioned further down the group in the periodic table, indicating more electron shells and greater atomic radius.
Step-by-step explanation:
The atomic radius of an element is the distance from the center of the nucleus to the boundary of the surrounding cloud of electrons. According to the trends in the periodic table, atomic radius increases as you move down a group and decreases as you move from left to right across a period. Hence, among Li (lithium), Rb (rubidium), N (nitrogen), F (fluorine), and I (iodine), Rb (rubidium) has the largest atomic radius because it is located further down the group compared to the other elements listed. Specifically, rubidium is in the fifth period of the alkali metals, indicating a larger number of electron shells which increases the atomic radius.
The atomic radius is a measure of the size of an atom. As you move from left to right across a period in the periodic table, the atomic radius generally decreases. This is because the number of protons and electrons increases, resulting in a stronger attractive force that pulls the electrons closer to the nucleus.
The largest atomic radius among the given elements is Rb (Rubidium). It is located below Li (Lithium) in Group 1 of the periodic table. As you move down a group, the atomic radius generally increases. This is because each successive element has an additional electron shell, which leads to an increase in size.