Metallic Bonding in Metals

Steps:

• Recall metallic structure: lattice of positive metal cations surrounded by delocalized electrons.
• For malleability, layers of cations slide over each other while electrons maintain bonding.
• For electrical conductivity, delocalized electrons move freely to carry charge.
• Evaluate options: match properties to accurate structural features, eliminating those with anions or mobile cations.

Why C is correct:

• Malleability arises because layers of metal cations (positive ions) can slide past each other in the lattice, with delocalized electrons providing flexible bonding.

Why the others are wrong:

• A: Metals contain cations, not anions; anion layers do not exist in metallic structure.
• B: Conduction occurs via mobile electrons, not anions, which are absent in metals.
• D: Cations form a fixed lattice and do not move to conduct electricity; electrons do.

Final answer: C