Metallic Bonding Practice Quiz

The 'sea of electrons' refers to the concept in metallic bonding where the valence electrons of metal atoms are delocalized and free to move throughout the entire metal lattice. This means that all the electrons in the outer shell of that metal are part of this 'sea of electrons'.

Metals are able to conduct electricity because they have a "sea of electrons" that is free to move throughout the metal lattice. These delocalized electrons are not bound to any particular atom and are able to flow freely, carrying electric charges with them. When a potential difference is applied across a metal, the electrons can easily move from atom to atom, allowing the electric current to flow. This is why metals are excellent conductors of electricity.

True. Metallic bonds are strong and the atoms are often tightly packed together. Therefore, it will take a higher temperature for them to melt.

The structure for Metallic Bonding is called a Giant lattice. In metallic bonding, the metal atoms are arranged in a regular pattern, forming a three-dimensional lattice structure. This structure allows the metal atoms to share their outer electrons with neighboring atoms, creating a sea of delocalized electrons that are free to move throughout the lattice. This delocalization of electrons gives metals their characteristic properties such as high electrical and thermal conductivity, malleability, and ductility. Therefore, the correct answer is Giant lattice.