What is the relationship between Gilbert N. Lewis's bonding model and the octet rule?

Gilbert N. Lewis’s bonding model and the octet rule are fundamentally linked through the concept of electronic stability. Lewis proposed that atoms form chemical bonds by sharing pairs of electrons to achieve the stable electronic structure of a noble gas.12

The relationship between these concepts is defined by the following points:

• Attaining Stability: Lewis described bond formation as a tendency for atoms to combine so that each atom attains a "closed-shell" configuration, which typically involves eight outer electrons—the octet rule.32
• Lewis Structures: In the Lewis structure method, electrons are distributed around atoms to ensure each atom has a share in an octet, representing a state of lower total energy.12
• Energy Minimization: Lewis viewed the octet rule as a means of achieving lower energy rather than an absolute goal. Sharing electrons allows atoms to reach this configuration, resulting in a more stable state than that of widely separated atoms.2
• Terminology: While Lewis developed the bonding model, the specific term "octet rule" was popularized by the American chemist Irving Langmuir.1

While the octet rule is a useful guide for many elements, Lewis’s model also accounts for exceptions, such as hypervalent compounds, where atoms may accommodate more than eight electrons.2