High school chemistry, hybridization ~ Who can tell me about it?

hybridization is a theoretical explanation in the process of atoms forming molecules, including sp (such as BeCl2), sp2 (such as BF3), sp3 (such as CH4), sp3d (such as PCl5), sp3d2 (such as SF6) hybridization, etc.

orbital hybridization theory refers to the atomic orbital hybridization theory. We know that the extranuclear electrons of atoms are arranged on the atomic orbits of different energy levels. When atoms form molecules, in order to enhance the bonding ability (the lowest energy is the most stable after bonding), different types of atomic orbits with similar energy in the same atom are recombined to form new atomic orbits with different energy, shape and direction (the energy of such orbits is lower than that before hybridization). For example, sp hybridization, sp2 hybridization and so on. This process of atomic orbital recombination is called atomic orbital hybridization, and the new atomic orbitals formed are called hybrid orbitals. After the hybrid orbitals are formed, they combine with other atoms to reduce the energy of the whole molecule and reach a stable state.

Key points

Key points of hybrid orbital theory:

In the bonding process, due to the interaction between atoms, several different types of atomic orbitals (i.e. wave functions) with similar energy in the same atom can be linearly combined, redistributed energy and determined space direction to form new atomic orbitals with the same number. This process of orbital recombination is called hybridization, and the new orbitals formed after hybridization are called hybrid orbitals.

Types of hybridization:

Isotropic hybridization: The hybridization in which all the orbitals of single electrons participate is called isotropic hybridization.

unequal hybridization: the hybridization involving lone pair orbitals is called unequal hybridization.

the types of hybrid orbitals depend on the types and numbers of valence orbitals and the number of bonds formed by atoms. Common ones are:

sp hybridization: sp hybridization refers to two sp hybrid orbitals formed by hybridizing an ns and an np orbital of an atom, and each sp hybrid orbital contains a 1/2s component and a 1/2p component, and the two orbitals extend in opposite directions, forming a σ bond with an included angle of 18 degrees. Linear type.

sp2 hybridization: atoms hybridize with one ns and two np orbitals to form three sp2 hybrid orbitals with the same energy, each of which contains 1/3s component and 2/3p component. The included angle between the three hybrid orbitals is 12 degrees.

sp3 hybridization: four sp3 hybridization orbitals with the same energy are formed by hybridization of one ns and three np orbitals. Each sp3 orbit contains 1/4s component and 3/4p component. The configuration is regular tetrahedron.

sp3d hybridization: five sp3d hybrid orbitals with the same energy are formed by hybridization of one ns, three np orbitals and one nd orbital. Each sp3d orbit contains 1/5 S, 3/5 P and 1/5 D components. The configuration is triangular bipyramid.

sp3d2 hybridization: Six sp3d2 hybrid orbitals with the same energy are formed by hybridizing one ns, three np orbitals and two nd orbitals. Each sp3d2 orbit contains 1/6 S, 1/2 P and 1/3 D components. The configuration is octahedron.