Which type of bond is characterized by electrostatic attraction between delocalized electrons and positive ions in a lattice?

The correct answer is the metallic bond. This bond is defined by the presence of a lattice structure where positive metal ions are surrounded by a "sea" of delocalized electrons. These delocalized electrons are free to move throughout the metal lattice, allowing for conductivity, malleability, and ductility—key properties of metals.

In a metallic bond, the electrostatic attraction between the positively charged ions and the negatively charged delocalized electrons holds the structure together. This is distinctly different from other types of bonds, such as ionic or covalent bonds, where the bonding characteristics rely on the transfer or sharing of electrons, rather than the delocalized nature observed in metals.

Understanding this concept is crucial in differentiating between bonding types based on their electronic structures and behaviors in materials.