What does the octet rule explain about atomic bonding?

The correct choice is grounded in the concept of the octet rule, which states that atoms tend to bond in such a way that they have eight electrons in their outermost shell, or valence shell. This configuration is particularly stable and is akin to the electron configuration of noble gases, which are known for their lack of reactivity.

Atoms will either share, lose, or gain electrons through chemical bonding—whether ionic or covalent—to satisfy this rule and achieve a full valence shell. For example, in covalent bonds, atoms share electrons to fill their valence shells, while in ionic bonds, one atom transfers electrons to another, resulting in the stabilization of both atoms through the formation of full valence shells.

In contrast to this concept, the other options do not accurately represent the fundamental ideas behind atomic bonding. The formation of positive charges and increase in atomic mass are not primary goals of atomic interactions. Additionally, while atoms may exchange electrons or ions during the bonding process, the exchange of particles is a broader concept that doesn’t specifically address the motivation behind bonding as succinctly as the octet rule does.