In a metallic bond, the attraction between metallic ions and valence electrons is a result of electrostatic forces. Metallic bonding occurs between metal atoms, which have a tendency to lose electrons and form positive ions (cations). When metal atoms lose electrons, they form cations with a positive charge.
The valence electrons in a metallic bond are delocalized, meaning they are not associated with any specific atom but are free to move throughout the entire structure of the metal. These mobile valence electrons are often referred to as a "sea of electrons." They are not tightly bound to any particular metal ion and can move relatively freely throughout the metal lattice.
The attraction between the positively charged metal ions and the negatively charged valence electrons creates a force of attraction. This attraction is due to the opposite charges of the ions and electrons. The positive metal ions attract the negatively charged valence electrons, and the electrons are distributed and shared among the metal ions.
The mobility of the valence electrons in a metallic bond is crucial in determining the unique properties of metals. Because the valence electrons are not strongly localized, metals are excellent conductors of heat and electricity. The delocalized electrons can move easily in response to an electric field or heat, allowing for efficient transfer of energy.
It's important to note that in a metallic bond, the octet rule is not necessarily followed because metals often have fewer than eight valence electrons in their outermost energy level. Instead, metallic bonding occurs through the sharing and pooling of valence electrons among a large number of atoms in the metal lattice.