The valence band is the highest range of electron energies in a solid where electrons are normally present at absolute zero temperature.

These electrons are bound to atoms and participate in chemical bonding, such as covalent or metallic bonds.

In crystalline solids, the valence band is formed by the overlap of atomic orbitals, creating a continuous range of energy levels.

Electrons in this band are not free to move throughout the material because they are tightly held by their parent atoms.

As a result, they do not contribute to electrical conductivity under normal conditions.

However, when external energy—such as heat, light, or an electric field—is applied, some electrons may gain enough energy to transition from the valence band to the conduction band.

This transition is critical in semiconductors and insulators, where the ability to excite electrons from the valence band determines the material’s conductivity.

The valence band is typically fully occupied in insulators and semiconductors, and its position relative to the conduction band defines the material’s electronic properties.

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