Which statement best describes the relationship between metallic bond strength and the enthalpy of vaporization of a metal?

• A. A stronger metallic bond results in a lower enthalpy of vaporization.
• B. A stronger metallic bond results in a higher enthalpy of vaporization.
• C. A weaker metallic bond results in a higher enthalpy of vaporization.
• D. Metallic bond strength and enthalpy of vaporization are unrelated.

Answer: (B)

Verified step by step guidance

1. Understand that metallic bonds are the forces holding metal atoms together in a solid lattice, involving the attraction between positively charged metal ions and delocalized electrons.
2. Recognize that the enthalpy of vaporization (\( \Delta H_{vap} \)) is the amount of energy required to convert one mole of a substance from liquid to gas, which involves breaking intermolecular or interatomic forces.
3. Realize that stronger metallic bonds mean more energy is needed to overcome these bonds to vaporize the metal, so the enthalpy of vaporization increases with bond strength.
4. Therefore, the relationship is direct: as metallic bond strength increases, the enthalpy of vaporization also increases.
5. Conclude that the correct statement is: 'A stronger metallic bond results in a higher enthalpy of vaporization.'