As a materials science expert, I have a deep understanding of the atomic and molecular structures that constitute various materials, including metals. The bonding in metals is a fascinating subject that involves quantum mechanics to fully comprehend. Let's delve into the nature of metallic bonds and how they are held together.

Metallic bonds are a type of chemical bond that occurs between the atoms of a metal. Unlike covalent or ionic bonds, metallic bonds do not involve the sharing or transfer of electrons between atoms in a fixed manner. Instead, they are characterized by a 'sea' of delocalized electrons that are free to move throughout the metal lattice.

The electrons in a metallic bond are not associated with a single atom but are shared among all the atoms present. This is due to the fact that the atomic orbitals of the metal atoms overlap significantly, creating a network of molecular orbitals that span the entire structure. These molecular orbitals are known as delocalized orbitals, and the electrons within them are referred to as delocalized electrons.

The delocalization of electrons is a key feature of metallic bonding. It means that the electrons are not bound to any particular atom but are free to move throughout the metal. This delocalization is what gives metals many of their characteristic properties, such as high electrical and thermal conductivity. The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom.

The metal atoms themselves are positively charged ions, as they have lost their valence electrons to the sea of delocalized electrons. These positive ions are arranged in a regular, repeating pattern known as a crystal lattice. The crystal lattice provides the structural framework for the metal.

The bond that holds the metal together is the electrostatic attraction between the positively charged metal ions and the delocalized electrons. This force is incredibly strong and is what gives metals their strength and durability. The delocalized electrons are attracted to the positive nuclei of the metal atoms, creating a cohesive force that holds the metal together.

In addition to the electrostatic attraction, there is also a quantum mechanical effect known as exchange interaction that contributes to the stability of the metallic bond. This is a complex phenomenon that arises from the wave-like nature of electrons and their indistinguishability from one another.

In summary, metallic bonds are held together by the strong forces of attraction between the positive nuclei of the metal atoms and the delocalized electrons. This unique bonding arrangement is responsible for the wide range of properties that metals exhibit, such as malleability, ductility, and high electrical and thermal conductivity.

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The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom. The electrons are said to be delocalised. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalised electrons. ... It is made of atoms.read more >>