Which of the following best describes the arrangement of electrons in a metallic bond?

• A. Electrons are localized between two atoms, forming a directional bond.
• B. Electrons are transferred from one atom to another, creating positive and negative ions.
• C. Electrons are delocalized and move freely throughout a lattice of metal cations.
• D. Electrons are shared equally between two nonmetal atoms.

Answer: (C)

Verified step by step guidance

1. Understand the nature of metallic bonding: In metallic bonds, atoms in a metal lattice release some of their electrons, which are not bound to any specific atom.
2. Recognize that these released electrons become delocalized, meaning they are free to move throughout the entire metal structure rather than being confined between two atoms.
3. Contrast this with other types of bonding: covalent bonds involve electrons shared between specific atoms, ionic bonds involve transfer of electrons creating ions, and directional bonds localize electrons between atoms.
4. Identify that the delocalized electrons in metallic bonds create a 'sea of electrons' that surrounds positively charged metal ions, allowing for properties like electrical conductivity and malleability.
5. Conclude that the best description of electron arrangement in metallic bonding is that electrons are delocalized and move freely throughout a lattice of metal cations.