How do Lewis structures show lone pairs and bonding pairs of electrons?

In Lewis structures, electrons are represented to show how atoms achieve stable configurations, typically following the octet rule. These diagrams distinguish between two types of electron pairs:

• Bonding pairs: These are shared between two atoms to form a covalent bond. In a Lewis structure, a bonding pair is represented by a solid line (dash) connecting the two atoms.12
• Lone pairs: These are pairs of valence electrons that remain on a single atom and do not participate in bonding. They are typically represented as pairs of dots placed around the atom.12

By counting the total valence electrons and arranging them, chemists use these structures to illustrate the topological pattern of bonds within a molecule, ensuring that atoms attain a stable electron shell through sharing. While these diagrams are essential for understanding chemical bonding, they do not necessarily depict the actual three-dimensional shape of the molecule.12