What does the octet rule state regarding atomic bonding?

The octet rule is a fundamental principle in chemistry that describes the tendency of atoms to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration akin to that of the noble gases. This stability is sought because atoms with full valence shells (usually consisting of eight electrons) are less reactive and more stable than those with partially filled valence shells.

When atoms bond—whether by sharing (covalent bonding) or transferring (ionic bonding) electrons—they do so to attain this octet configuration. For example, a sodium atom (which has one electron in its outer shell) tends to lose that electron to achieve a stable configuration, while a chlorine atom (with seven electrons in its outer shell) will gain an electron. This transfer of electrons allows both atoms to satisfy the octet rule.

This understanding helps to explain why many common compounds, such as sodium chloride (table salt), form: the sodium atom loses an electron to become a positively charged ion, and the chlorine atom gains that electron to become a negatively charged ion, resulting in an overall neutral compound with both atoms having achieved octet stability.

The other choices do not accurately reflect the concept of atomic bonding as described by the octet rule