Which orbitals contribute to the formation of the s/p band?

The s/p band in solid-state chemistry refers to the range of energy levels formed by the overlapping of s and p orbitals. In particular, when s orbitals from one atom and p orbitals from adjacent atoms combine, they generate bonding and antibonding states that make up the band structure in metals and semiconductors.

In this context, both s and p orbitals have distinct shapes and energy levels: s orbitals are spherical, while p orbitals are oriented in three-dimensional space along the x, y, and z axes. When these orbitals mix, they contribute to the formation of a band that encompasses a range of energies. The result is a cohesive band structure that influences the electrical and optical properties of materials.

The inclusion of s and p orbitals in this band structure is significant because it is the combination of these orbitals that allows for the delocalization of electrons, which is a crucial feature for conductivity in metals. Other orbitals, such as d or f, may participate in more complex band structures in other contexts, but they do not contribute to the s/p band, which is fundamentally defined by these two types of orbitals. Therefore, recognizing that the s and p orbitals are the key contributors to this