Which of the following best describes how metallic bonds differ from ionic and covalent bonds?

• A. Metallic bonds involve a 'sea of electrons' that are delocalized and shared among many metal atoms.
• B. Metallic bonds result from the electrostatic attraction between oppositely charged ions.
• C. Metallic bonds occur only in compounds containing both metals and nonmetals.
• D. Metallic bonds form between nonmetal atoms by sharing electron pairs.

Answer: (A)

Verified step by step guidance

1. Step 1: Understand the nature of metallic bonds. Metallic bonds occur between metal atoms where valence electrons are not localized between two atoms but are free to move throughout the entire metal structure. This creates a 'sea of electrons' that are delocalized and shared among many metal atoms.
2. Step 2: Compare metallic bonds to ionic bonds. Ionic bonds form due to the electrostatic attraction between positively and negatively charged ions, typically between metals and nonmetals, where electrons are transferred from one atom to another.
3. Step 3: Compare metallic bonds to covalent bonds. Covalent bonds involve the sharing of electron pairs between specific nonmetal atoms, where electrons are localized between the bonded atoms.
4. Step 4: Recognize that metallic bonds do not require the presence of nonmetals and are not formed by sharing electron pairs localized between two atoms, unlike covalent bonds.
5. Step 5: Conclude that the best description of metallic bonds is that they involve a 'sea of electrons' that are delocalized and shared among many metal atoms, distinguishing them from ionic and covalent bonds.