Lewis Structures: The Basics
Lewis Structures are like molecular blueprints that show how valence electrons arrange themselves around atoms in covalently bonded molecules. They reveal which electrons are being shared between atoms and which ones remain as lone pairs. Remember though - these structures don't show the actual 3D shape of molecules!
In these diagrams, we represent single bonds with one line (sharing 2 electrons), double bonds with two lines (sharing 4 electrons), and triple bonds with three lines (sharing 6 electrons). For example, methane (CH₄) shows carbon with four single bonds to hydrogen atoms, while nitrogen gas (N₂) shows a triple bond between nitrogen atoms.
When drawing atoms, we can show lone pairs (unshared electrons) as dots. Sulfur might have dots representing its lone pairs, while oxygen in a double bond would share 4 electrons with another atom while keeping some electrons to itself.
Quick Tip: Valence electrons come from the outermost s and p orbitals, which is why most atoms can have up to 8 valence electrons (octet).
