To compare the atomic radii of different atoms, we can use a general inequality statement. However, atomic radii can vary significantly between different elements based on their positions in the periodic table. Generally, atomic radii increase as you move down a group and decrease as you move from left to right across a period.
For example, let's compare a few common elements: hydrogen (H), lithium (Li), and fluorine (F). A possible inequality statement representing their atomic radii could be:
\[ \text{radii}(H) < \text{radii}(F) < \text{radii}(Li) \]
However, if we select a specific group of elements (like noble gases, alkali metals, or halogens) or a specific subgroup, the inequality might differ. Therefore, here's a more generalized representation for a few groups:
For alkali metals:
\[ \text{radii}(Li) < \text{radii}(Na) < \text{radii}(K) < \text{radii}(Rb) < \text{radii}(Cs) \]
For halogens:
\[ \text{radii}(F) < \text{radii}(Cl) < \text{radii}(Br) < \text{radii}(I) \]
To create a more precise inequality statement, you would need to specify which atoms you are comparing.