Which of the following metal atoms would have the highest electrical conductivity?

• A. Ag
• B. Na
• C. Fe
• D. Cu

Answer: (A)

Verified step by step guidance

1. Understand that electrical conductivity in metals depends primarily on the number of free electrons available to move through the metal lattice and the ease with which these electrons can flow.
2. Recall that metals with a higher number of valence electrons that are loosely held tend to have better electrical conductivity because these electrons can move more freely.
3. Consider the electron configurations of the given metals: Sodium (Na), Iron (Fe), Copper (Cu), and Silver (Ag), focusing on their valence electrons and how these contribute to conductivity.
4. Recognize that silver (Ag) has a single valence electron in its outermost shell that is very free to move, and it has the least resistance to electron flow compared to the others, which is why it exhibits the highest electrical conductivity.
5. Compare the conductivity trends of these metals, noting that although copper (Cu) is also highly conductive, silver (Ag) surpasses it due to its atomic structure and electron mobility.