Which of the following best describes how a metallic bond differs from an ionic bond?

• A. In a metallic bond, electrons are delocalized and shared among many atoms, while in an ionic bond, electrons are transferred from one atom to another.
• B. In a metallic bond, atoms share electron pairs between two specific atoms, while in an ionic bond, electrons are equally shared.
• C. In a metallic bond, only nonmetals are involved, while in an ionic bond, only metals are involved.
• D. In a metallic bond, positive and negative ions are held together by electrostatic forces, while in an ionic bond, atoms are held together by a sea of electrons.

Answer: (A)

Verified step by step guidance

1. Understand the nature of metallic bonds: In metallic bonding, atoms (usually metals) release some of their electrons to form a 'sea of electrons' that are free to move throughout the entire structure. These electrons are delocalized and shared among many atoms, which gives metals their characteristic properties like conductivity and malleability.
2. Understand the nature of ionic bonds: Ionic bonding occurs between metals and nonmetals, where electrons are transferred from one atom (usually a metal) to another (usually a nonmetal). This transfer creates positively charged ions (cations) and negatively charged ions (anions) that are held together by strong electrostatic forces.
3. Compare electron behavior: In metallic bonds, electrons are not localized between two atoms but are shared collectively across many atoms, whereas in ionic bonds, electrons are fully transferred from one atom to another, resulting in discrete ions.
4. Analyze the options given: Identify which description correctly contrasts the delocalized electron sharing in metallic bonds with the electron transfer and electrostatic attraction in ionic bonds.
5. Conclude that the best description is the one stating that metallic bonds involve delocalized electrons shared among many atoms, while ionic bonds involve electron transfer from one atom to another, leading to electrostatic attraction between ions.