Metallic Bonding Explains Metal Properties

Steps:

• Identify metallic structure: positive ions in lattice with delocalized electrons.
• Test A: Layers slide due to weak inter-layer forces, enabling malleability.
• Test B: Conduction involves electron flow, not layer vibration.
• Test C: Bond strength determines melting point, not intermolecular forces.
• Test D: Alloys require similar atomic radii for substitution, not ionic.

Why A is correct:

• In metallic bonding, delocalized electrons hold ions together, allowing planes of atoms to slide over each other without disrupting the lattice, per the sea of electrons model.

Why the others are wrong:

• B: Metals conduct electricity via mobile delocalized electrons, not vibrating atomic layers.
• C: Metallic lattices use metallic bonds, not intermolecular forces like in molecular solids.
• D: Alloy compatibility depends on atomic radii for lattice fit, not ionic radii relevant to ionic compounds.

Final answer: A