University:
Felician University
Course:
CHEM-001 | Basic Chemistry
Academic year:

2019
Views:

428

Pages:

18
Author:

StellarStrategist

Metallic bonding METALLIC BONDING Chemical bonding in METALS is different because of their valence e-s. METALLIC BONDING Metals are great electrical conductors in their solid state because their valence e-s move a lot METALLIC BONDING Why doesn’t this happen in an ionic or covalent bond? In an ionic or covalent bond, e-s are held more tightly due to stronger nuclear force of attraction of the atoms in these bonds. The highest E-level of metals are occupied by few e-s, leaving many vacant orbitals. Within a metal, these vacant orbitals overlap. This overlapping allows e-s to roam around ALL of the orbitals of ALL of the atoms. es These are delocalized: they do not belong to any one atom. These “delocalized” electrons form a sea of electrons around the metal atoms. The chemical bonding that results from the attraction between metal atoms and the surrounding sea of e-s is called metallic bonding. Metallic Bonds: Mellow dogs with plenty of bones to go around. A Sea of Electrons The sea of es causes High electrical conductivity Conductor of heat and electricity. The sea of es causes High thermal conductivity The sea of Luster es causes Shiny because metals reflect light The sea of es causes METALLIC PROPERTIES The sea of e-s causes - High electrical conductivity - high thermal conductivity - luster - malleability - ductility