Why are metals good conductors of both heat and electricity?

• A. Because metals have large atomic radii that allow for easy energy transfer.
• B. Because metals have free-moving valence electrons that can transfer energy efficiently.
• C. Because metals are always in a liquid state at room temperature.
• D. Because metals have tightly bound electrons that prevent energy loss.

Answer: (B)

Verified step by step guidance

1. Understand that electrical and thermal conductivity in metals is primarily due to the behavior of electrons within the metal structure.
2. Recall that metals have a lattice of positively charged ions surrounded by a 'sea' of free-moving valence electrons, often called delocalized electrons.
3. Recognize that these free electrons can move easily throughout the metal, allowing them to carry electrical charge efficiently, which explains electrical conductivity.
4. Similarly, these free electrons can transfer kinetic energy rapidly from one part of the metal to another, facilitating efficient heat conduction.
5. Conclude that the presence of free-moving valence electrons is the key reason metals are good conductors of both heat and electricity, rather than factors like atomic radius or physical state.