Undergrad Electron configuration vs. Lewis dot structure?

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Electron configurations and Lewis dot structures both represent electron distribution in atoms, but they focus on different aspects. Electron configurations detail the arrangement of all electrons in an atom, while Lewis dot structures emphasize the valence electrons involved in bonding. The octet rule, which states that atoms tend to form bonds to achieve eight valence electrons, primarily applies to main-group elements, particularly in their s and p orbitals. This rule explains why Lewis diagrams typically show eight electrons as a full shell, despite electron configurations allowing for varying numbers of electrons in outer orbitals. Understanding these differences clarifies how each model contributes to the study of chemical bonding.
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I am trying to make a connection between the two in terms of the electron configuration for an atom relative to the octet rule for Lewis Dot diagrams. Maybe I just don't understand what the electron configuration represents. Why is it that Lewis Dot diagrams utilize 8 valence electrons as a full 'shell', whereas electron configurations have varying degrees of allowable electrons per orbitals as in the outermost orbital?
 
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The octet rule is applicable to main-group elements, where it is the s and p orbitals that participate in bonding.
 

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