Which property of metals can be inferred from their ability to conduct electricity well?

• A. Metals have delocalized electrons that can move freely throughout the structure.
• B. Metals are composed of ionic bonds between atoms.
• C. Metals have tightly bound electrons that do not move.
• D. Metals are poor conductors of heat.

Answer: (A)

Verified step by step guidance

1. Understand that electrical conductivity in metals is related to the movement of electrons within the metal structure.
2. Recall that metals have a unique bonding called metallic bonding, where electrons are not bound to any specific atom but are free to move throughout the metal lattice.
3. Recognize that these free-moving electrons are called delocalized electrons, and their mobility allows metals to conduct electricity efficiently.
4. Contrast this with ionic bonds, where electrons are localized between ions, and tightly bound electrons, which do not contribute to conductivity.
5. Conclude that the property responsible for good electrical conductivity in metals is the presence of delocalized electrons that can move freely throughout the structure.