Metallic Bonding in Element X

Steps:

• Identify the lattice of positive ions and sea of electrons as the structure of metallic bonding in metals.
• Recall that metallic bonds are strong electrostatic attractions between ions and delocalized electrons.
• List key metal properties: high melting points, electrical conductivity via electrons, malleability, and stability under current.
• Match properties to options, selecting the one that fits high melting point due to bond strength.

Why B is correct:

• Strong metallic bonds require significant energy to overcome for melting, leading to high melting points as defined in metallic bonding theory.

Why the others are wrong:

• A: Metals conduct via delocalized electrons only, not ion movement.
• C: Metals are not decomposed by electric current; this applies to electrolytes in electrolysis.
• D: Metals are malleable due to layers of ions sliding past each other.

Final answer: B