In the periodic table, atomic radius tends to increase as you move from the top to the bottom of a group (column) and from the right to the left across a period (row). As such, the atoms with the largest atomic radius are found in the bottom left corner of the periodic table.
Here’s a detailed explanation of the trends:
1. Down a Group (Column): As you move down a group, each successive element has an additional electron shell compared to the element above it. This increases the distance between the nucleus and the outermost electrons, resulting in a larger atomic radius.
2. Across a Period (Row): As you move from left to right across a period, the number of protons in the nucleus increases, which would attract the electrons more strongly and pull them closer to the nucleus. However, this effect is somewhat countered by the increase in electron-electron repulsion. Nonetheless, the overall effect is a decrease in atomic radius across a period.
Therefore, the largest atomic radii are found among the elements that are located in the bottom left corner of the periodic table, where the atomic radius is maximized due to the combined effect of having the most electron shells and the least attraction exerted by the nucleus on the outermost electrons.
