Furthermore, sodium is an excellent conductor of both heat and electricity, a property explained by the mobility of the free electrons throughout the lattice. The single electron in the outermost 3s orbital is only weakly held by the nucleus due to shielding by the inner electron layers.
How Sodium's Delocalized Electrons Enable Conductivity and Metallic Bonding
The type of bonding holding elemental sodium together is a classic example of metallic interaction. This electron is easily lost, resulting in a stable Na⁺ ion.
The answer lies not in discrete molecules but in a collective sea of electrons, a defining feature of metallic bonding. Covalent bonding, which involves the sharing of electron pairs between specific atoms, is also absent in pure sodium.
How Sodium's Delocalized Electrons Enable Conductivity and Define Metallic Bonding
These electrons are not bound to any specific atom; instead, they are free to move throughout the entire structure. This sea of delocalized electrons defines the physical and chemical identity of the metal, explaining its reactivity in water and its utility in electrical wiring.
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