Which of the following best explains why most metals have high boiling and melting points?

• A. Metals have weak van der Waals forces between their atoms.
• B. Metals have strong metallic bonds due to the attraction between delocalized electrons and positive metal ions.
• C. Metals have high ionization energies that prevent them from melting easily.
• D. Metals have covalent bonds between their atoms.

Answer: (B)

Verified step by step guidance

1. Understand that melting and boiling points are related to the strength of the forces holding atoms or molecules together in a substance.
2. Recall that in metals, atoms are arranged in a lattice structure where positive metal ions are surrounded by a 'sea' of delocalized electrons.
3. Recognize that the attraction between these delocalized electrons and the positive metal ions is called metallic bonding, which is generally very strong.
4. Compare this to other types of forces: van der Waals forces are weak, covalent bonds are directional and not typical in metals, and ionization energy relates to removing electrons rather than bonding strength.
5. Conclude that the high melting and boiling points of metals are best explained by the strong metallic bonds formed by the attraction between delocalized electrons and positive metal ions.