Which of the following best describes metallic bonding?

• A. Atoms are held together by hydrogen bonds between molecules.
• B. Electrons are shared equally between two nonmetal atoms.
• C. Electrons are transferred from one atom to another, resulting in oppositely charged ions.
• D. Valence electrons are delocalized and move freely throughout a lattice of metal cations.

Answer: (D)

Verified step by step guidance

1. Understand that metallic bonding is a type of chemical bonding unique to metals, where atoms are arranged in a lattice structure.
2. Recall that in metallic bonding, valence electrons are not localized between individual atoms but are free to move throughout the entire metal lattice.
3. Recognize that this 'sea of delocalized electrons' allows metal atoms (cations) to be held together by the electrostatic attraction between the positively charged metal ions and the negatively charged electrons.
4. Compare this to other types of bonding: hydrogen bonding involves attraction between molecules, covalent bonding involves sharing electrons between specific atoms, and ionic bonding involves transfer of electrons creating ions.
5. Conclude that the best description of metallic bonding is that valence electrons are delocalized and move freely throughout a lattice of metal cations.