Which of the following best describes the relationship between the atomic radius of a metal and its melting point?

• A. There is no relationship between atomic radius and melting point in metals.
• B. Metals with smaller atomic radii generally have lower melting points because their atoms are closer together.
• C. Metals with smaller atomic radii generally have higher melting points due to stronger metallic bonding.
• D. Metals with larger atomic radii always have higher melting points because their atoms are more massive.

Answer: (C)

Verified step by step guidance

1. Understand that the melting point of a metal is largely influenced by the strength of the metallic bonds holding the atoms together in the solid state.
2. Recall that metallic bonding strength depends on how closely the metal atoms are packed and how strongly the delocalized electrons hold the atoms together.
3. Recognize that a smaller atomic radius means atoms are closer together, which allows the metallic bonds to be stronger because the positive nuclei can attract the delocalized electrons more effectively.
4. Conclude that stronger metallic bonding generally leads to a higher melting point, so metals with smaller atomic radii tend to have higher melting points.
5. Therefore, the best description is that metals with smaller atomic radii generally have higher melting points due to stronger metallic bonding.