Which of the following describes the trend in metallic character in the periodic table?

The trend in metallic character throughout the periodic table is that it increases from top to bottom within a group (column). This occurs because as you move down a group, the atomic size increases due to the addition of electron shells. The larger atomic radius makes it easier for the outer electrons to be lost, which is a characteristic of metals that exhibit metallic behavior. Consequently, elements towards the bottom of a group, such as alkali metals, are much more metallic in nature compared to the elements at the top of the same group, like lithium or sodium.

In contrast, as you move from left to right across a period, the metallic character decreases. More positively charged nuclear protons in the nucleus exert a stronger attraction on the electrons, making it harder for the outer electrons to be removed. Thus, while the lower elements in a group exhibit more metallic properties, those on the right side of the periodic table are typically nonmetals or metalloids and possess less metallic character.