Final answer:
The cations in a metallic bond surrounded by a sea of electrons explain the structure and properties of metals, including their strength, electrical conductivity, and flexibility. This metallic bond is a strong attraction that helps dictate specific metal attributes.
Step-by-step explanation:
The lattice of cations in metallic bonds being surrounded by a sea of electrons explains one of the quintessential characteristics of metallic bonding in solids. This description pertains to how metals are structured at the atomic level. The metal atoms exist as positively charged ions (cations) arranged in a well-defined three-dimensional structure known as a crystal lattice. These positively charged ions are surrounded by a sea of delocalized electrons that are free to move throughout the metal. This 'sea' allows for flexibility and conductivity within the metal, as the electrons can easily flow and carry electrical current.
The metallic bond itself is the force of attraction between these positive metal ions and the surrounding valence electrons. This bond is particularly strong and is responsible for many of the characteristic properties of metals such as strength, malleability, ductility, and high electrical and thermal conductivity. The number of valence electrons participating in this 'sea' also influences the melting points and hardness of different metals.