What holds the positively charged metal ions together within a metallic bond?

• A. Electrostatic attraction between ions and polar molecules
• B. Covalent sharing of electrons between metal atoms
• C. A sea of delocalized electrons
• D. Ionic attraction between metal ions and nonmetal ions

Answer: (C)

Verified step by step guidance

1. Understand that metallic bonding involves metal atoms arranged in a lattice structure where the valence electrons are not bound to any specific atom.
2. Recognize that these valence electrons become delocalized, meaning they move freely throughout the entire metal structure, forming what is called a 'sea of electrons'.
3. Identify that the positively charged metal ions (cations) are held together by the electrostatic attraction to this sea of delocalized electrons, which acts as a glue keeping the metal ions in place.
4. Note that this type of bonding is different from ionic bonding (which involves attraction between metal and nonmetal ions) and covalent bonding (which involves sharing electrons between specific atoms).
5. Conclude that the key feature holding metal ions together in a metallic bond is the electrostatic attraction between the metal cations and the surrounding sea of delocalized electrons.