Metallic Bonding Explains Copper's High Melting Point

Steps:

• Identify copper as a metal, so its structure involves metallic bonding.
• In metals, atoms form positive ions by losing valence electrons, creating a "sea" of delocalized electrons.
• These delocalized electrons attract the positive ions, forming strong electrostatic forces throughout the lattice.
• High energy is required to overcome these forces, resulting in a high melting point.

Why B is correct:

• Metallic bonding is defined by electrostatic attractions between positive metal ions and delocalized electrons, which are strong in copper due to its many valence electrons.

Why the others are wrong:

• A: Copper atoms do not bond covalently; metallic bonding involves ions, not neutral atoms.
• C: Attractions involve ions, not neutral atoms, with delocalized electrons.
• D: Ion-ion repulsions would destabilize the lattice without balancing electron attractions.

Final answer: B