In general, elements that are located towards the bottom-left corner of the periodic table tend to have larger atomic radii. This trend is known as the atomic radius trend.

Here are some key points regarding elements with larger atomic radii:

  1. Down a Group: As you move down a group (a column) in the periodic table, the atomic radius generally increases. This is because each subsequent element in a group has an additional electron shell, which increases the distance between the nucleus and the outermost electrons.

  1. Across a Period: As you move from left to right across a period (a row) in the periodic table, the atomic radius generally decreases. This is because although each subsequent element in a period has one more proton in the nucleus, which tends to pull the electrons closer, the added electron is also being added to the same electron shell, thus not significantly increasing the distance between the nucleus and the outermost electrons.

So, to summarize, elements in the bottom-left corner of the periodic table (such as the alkali metals and alkaline earth metals) generally have larger atomic radii compared to those in the top-right corner (such as the halogens and noble gases).