What describes the structure of metals?

Metals are characterized by a giant regular structure, often referred to as a metallic lattice, which consists of a three-dimensional arrangement of positively charged metal ions surrounded by a 'sea' of delocalized electrons. This structure allows metals to exhibit unique properties such as electrical conductivity, malleability, and ductility.

The arrangement of the positive ions in a regular pattern contributes to the strength and stability of the metal, while the delocalized electrons facilitate the conduction of electricity and heat. This combination of atomic structure and electron behavior is crucial in understanding metallic bonding and the distinctive properties of metals.

In contrast, the other options describe different types of structures. Molecular structures refer to covalent compounds that consist of discrete molecules. Individual atoms held together by covalent bonds are typical of covalent networks or simple molecular compounds, not metals. Weak intermolecular forces are characteristics of molecular substances rather than metals, which rely on strong metallic bonds for their structural integrity.