NaCl: The Ionic Bond
A sodium atom transfers one electron to a chlorine atom, forming Na+ and Cl- ions held together by electrostatic attraction in a cubic crystal lattice; real melting point, 6:6 ion coordination, and dissociation in water.
A sodium atom carries one electron loose Sitting alone in its outer shell, restless A chlorine atom needs one electron to complete Its outer shell missing a single spot They meet, and sodium lets the electron go Chlorine catches it, pulls it fully in Sodium becomes a positive ion now Neon's electron count, though sodium keeps eleven protons Chlorine becomes a negative ion now Argon's electron count, seventeen protons still inside Opposite charges pull, electrostatic and strong Millions of ions stack into a cube Each sodium ion ringed by six chlorines around it Each chlorine ion ringed by six sodiums the same A crystal lattice, ordered, hard to break Melts only past eight hundred one degrees Celsius Drop it in water, the lattice falls apart Ions scatter, free to carry a current Sodium chloride, table salt, born from a transfer
Key Concepts: Sodium transfers one electron to chlorine (not shared, an ionic transfer) | Na+ (10 electrons, like neon) and Cl- (18 electrons, like argon) attract electrostatically | Real cubic crystal lattice with 6:6 ion coordination and a real melting point (801°C) | Dissolving in water breaks the lattice and frees ions to conduct electricity | Companion to "Sodio and Chlora Make Salt"
Key Words: ionic bond, electron transfer, cation, anion, crystal lattice, coordination, NaCl