Metallic bonding: attraction between cations and delocalized electrons

Steps:

• Recall that metals consist of a lattice of positive ions (cations) formed by losing valence electrons.
• Note that valence electrons are delocalized, forming a "sea" of mobile electrons around the lattice.
• Identify the bonding force as electrostatic attraction between the positively charged ions and the negatively charged electron sea.
• Eliminate options that misidentify charges or particles involved.

Why B is correct:

• It matches the definition of metallic bonding as the electrostatic force between a lattice of positive metal ions and delocalized valence electrons, enabling properties like conductivity.

Why the others are wrong:

• A: Negative ions do not form in metals; it's positive ions, and the sea is electrons, not protons.
• C: Describes ionic bonding, not metallic, as metals lack distinct negative ions.
• D: Protons are fixed in nuclei, not a mobile "sea"; the sea consists of electrons.

Final answer: B