As a specialist in the field of electrical engineering and physics, I can provide a comprehensive answer to your question about the conduction of electricity by electrons.

Electricity is the flow of electric charge, and in most cases, this charge is carried by electrons. The ability of electrons to conduct electricity is a fundamental aspect of electrical systems and is the basis for various applications, from simple household appliances to complex electronic devices.

In a metal, the atoms have outer electrons that are not tightly bound to any single atom. These are known as free electrons. The structure of a metal allows these electrons to move freely within the material. When an electric field is applied, these free electrons can move in a directed manner, creating an electric current. This is why metals are considered good conductors of electricity.

The movement of free electrons in a metal is facilitated by the metallic bonding that occurs between atoms. In metallic bonding, the valence electrons of the atoms are delocalized and form a "sea" of electrons that can move freely throughout the structure. This delocalization of electrons is what gives metals their characteristic properties, such as high thermal and electrical conductivity.

In contrast, in covalent or ionic solids, the electrons are not free to move. In covalent solids, electrons are shared between atoms to form strong covalent bonds. These bonds are directional and localized, meaning the electrons are tied to specific atoms and cannot move freely. As a result, covalent solids do not conduct electricity well.

In ionic solids, the electrons are transferred from one atom to another, resulting in the formation of ions. These ions are held together by strong electrostatic forces known as ionic bonds. The electrons are localized around the ions and cannot move freely to conduct electricity.

It's important to note that while metals are good conductors, their conductivity can be influenced by factors such as temperature, impurities, and the presence of defects in the metal's crystal structure. As temperature increases, the movement of free electrons can be impeded by increased lattice vibrations, which can reduce conductivity. Similarly, impurities or defects can disrupt the flow of electrons, affecting the metal's ability to conduct electricity.

Furthermore, the concept of conduction is not limited to metals. There are other materials, such as semiconductors and superconductors, that also exhibit interesting electrical properties.
Semiconductors, for example, have a unique ability to conduct electricity under certain conditions. They have a band structure that allows electrons to move more freely when energy is supplied, such as through heat or light.
Superconductors, on the other hand, are materials that can conduct electricity with zero electrical resistance below a certain critical temperature. This is a fascinating area of study with many potential applications.

In summary, electrons do conduct electricity, and their ability to do so is a key factor in the functioning of electrical devices and systems. The movement of electrons is facilitated by the properties of the material they are in, with metals being particularly effective conductors due to their structure and the presence of free electrons. Understanding the principles of electrical conduction is crucial for the design and operation of various electrical and electronic systems.

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Metal atoms have outer electrons which are not tied to any one atom. These electrons can move freely within the structure of a metal when an electric current is applied. There are no such free electrons in covalent or ionic solids, so electrons can't flow through them - they are non-conductors.read more >>