Which of the following is necessary for a metallic bond to form?

• A. The overlap of atomic orbitals to form sigma and pi bonds
• B. A lattice of positive metal ions surrounded by a sea of delocalized electrons
• C. The sharing of electron pairs between two nonmetal atoms
• D. The transfer of electrons from a metal to a nonmetal

Answer: (B)

Verified step by step guidance

1. Understand that a metallic bond is a type of chemical bond found in metals, characterized by a lattice of positive metal ions surrounded by a 'sea' of delocalized electrons.
2. Recognize that unlike covalent bonds (which involve sharing electron pairs between specific atoms) or ionic bonds (which involve transfer of electrons from metal to nonmetal), metallic bonds involve electrons that are not localized between atoms but are free to move throughout the metal lattice.
3. Note that the overlap of atomic orbitals to form sigma and pi bonds is typical of covalent bonding, not metallic bonding.
4. Identify that the key feature necessary for metallic bonding is the presence of a lattice of positive metal ions immersed in a sea of delocalized electrons, which allows metals to conduct electricity and be malleable.
5. Conclude that the correct description of what is necessary for a metallic bond to form is the lattice of positive metal ions surrounded by delocalized electrons.