Metallic Bonding in Copper

Steps:

• Copper is a transition metal that forms a giant metallic lattice.
• In this lattice, copper atoms donate valence electrons to create positive ions and a sea of delocalized electrons.
• The strong electrostatic attraction between these ions and delocalized electrons holds the structure together.
• Overcoming this attraction requires significant energy, resulting in a high melting point.

Why B is correct:

• Metallic bonding is defined by the electrostatic forces between positively charged metal ions and freely moving delocalized electrons, which provide strength and explain copper's high melting point (around 1085°C).

Why the others are wrong:

• A: Copper does not form covalent bonds between neutral atoms; metallic bonding involves ions, not atoms alone.
• C: Attractions occur between ions, not neutral atoms, which would imply incorrect covalent character.
• D: Lacks "only," failing to emphasize that ion-electron forces are the sole key attractive interaction in pure metallic copper.

Final answer: B