Which property of metallic bonding explains why metals are malleable?

• A. Strong ionic bonds hold the metal atoms rigidly in place.
• B. The presence of delocalized electrons allows metal atoms to slide past each other without breaking bonds.
• C. Covalent bonds between metal atoms allow for easy reshaping.
• D. Hydrogen bonding between metal atoms provides flexibility.

Answer: (B)

Verified step by step guidance

1. Understand that metallic bonding involves metal atoms surrounded by a 'sea' of delocalized electrons, which are not fixed to any particular atom.
2. Recognize that these delocalized electrons act as a glue, holding the metal atoms together while allowing them to move relative to each other.
3. Realize that when a force is applied to a metal, the metal atoms can slide past one another without breaking the metallic bonds because the electron sea adjusts to maintain bonding.
4. This ability for atoms to slide without breaking bonds explains the malleability of metals, meaning they can be hammered or rolled into sheets without shattering.
5. Therefore, the key property of metallic bonding responsible for malleability is the presence of delocalized electrons that allow metal atoms to move while maintaining the bond.