What best describes the structure of metals?

The structure of metals is best described as a giant regular structure of positive ions surrounded by a sea of electrons. This model is often referred to as the "metallic bond" theory. In this arrangement, metal atoms lose some of their electrons, which are not bound to any specific atom and are free to move throughout the structure. This delocalization of electrons creates a "sea" that helps to hold the positively charged metal ions together, providing metals with their characteristic properties such as electrical conductivity, malleability, and ductility.

The regular arrangement of the positive ions in the metallic lattice contributes to the overall stability of the metal. As the electrons are mobile, they can carry charge, which is why metals are good conductors of electricity. Additionally, the ability of the positive ions to slide past each other without breaking the metallic bond allows metals to be shaped and deformed without fracturing.

In contrast, other structures listed do not account for the unique properties and arrangement found in metals. A random arrangement of atoms does not apply to metals, as they have a well-defined lattice structure. Isolated atoms in a crystalline lattice describe non-metallic elements or ionic compounds, which do not behave like metals. A grid of non-mobile positive ions would imply