Final answer:
Most metals achieve the octet rule by losing their valence electrons, becoming positively charged ions or cations with stable electron configurations similar to the nearest noble gas. In contrast, nonmetals gain electrons forming anions, and both types of ions can form ionic bonds to satisfy the octet rule.
Step-by-step explanation:
In order to reach stability and achieve the octet rule, most metals will lose their valence electrons.
This loss of electrons results in a positive ion or cation, with a stable electron configuration that typically mirrors that of the nearest noble gas.
Since metals have relatively few electrons in their outermost shell, it is easier for them to donate these electrons than to gain enough to complete their octet.
For example, a sodium (Na) atom, which has one valence electron, will lose that electron to form a Na+ ion.
This cation will have a stable electron configuration like that of neon, with a complete octet in the next lowest principal energy level.
In contrast, nonmetals tend to gain electrons to complete their valence shell octet, leading to the formation of anions.
The principle that underlies the formation of these ions is the drive of elements to attain electron configurations like those of the noble gases, which have full energy levels and are highly stable.
The ionic bond is formed through the attraction between the positively charged metal ion and a negatively charged nonmetal ion, fulfilling the octet rule for both atoms involved.