chem
Sea of Electrons Model
- Metal atoms form cations for stable electron configurations, sharing valence electrons freely in metals.
- Metallic bonds: electrostatic attraction between free-moving valence electrons and positive metal cations.
- Metallic bonding modeled as a "sea of electrons."
Extended Structures
- Metals have regular structures, not discrete molecules, held by the sea of electrons.
- Specific properties derived from the sea of electrons are conductivity, malleability, and ductility.
Malleability and Ductility
- Metals change shape without breaking; cations slide past each other while electrons move.
- Metals can be drawn into wires due to flexible atomic structure that prevents breaking.
Melting and Boiling Points
- Metals generally have high melting and boiling points due to strong electrostatic forces.
- Examples: Iron - 1535°C, Sodium - 98°C, Magnesium - 649°C.
- Higher nuclear charge & valence electrons increase melting point through stronger attraction.
- Sodium ions (1+) vs. Magnesium ions (2+); more electrons from magnesium lead to stronger bonds.
Conductive Properties
- Metals like copper, aluminum, and iron are used for cooking.
- Delocalized electrons rapidly transfer kinetic energy, enhancing heat conductivity.
- High melting points make them suitable for cookware.