Hybridization

Atomic orbitals: The basic building blocks of hybridization theory are the atomic orbitals of an atom. Different atomic orbitals have different shapes and sizes, and they are used to build hybrid orbitals.

Valence electrons: Valence electrons are the electrons in the outermost shell of an atom. They are involved in chemical bonding and are the electrons that are affected during hybridization.

Hybrid orbitals: Hybrid orbitals are made by combining atomic orbitals from different subshells to form new orbitals that can be used for bonding. They have characteristics of both the parent orbitals.

Hybridization types: There are different types of hybridizations, such as sp, sp2, and sp3 hybridizations. Each type depends on the number of electron groups surrounding the atom of interest.

Sigma and pi bonds: In hybridization, the bonds are formed by either sigma or pi bonds. Sigma bonds are formed by the overlapping of orbitals directly between the bonding atoms, while pi bonds are formed by the overlapping of orbitals of non-hybridized p-orbitals.

Molecular geometry: The molecular geometry is determined by the arrangement of the atoms in space, which is influenced by the hybridization of the central atom.

Resonance: Resonance is the phenomenon where a molecule has multiple valid Lewis structures, but the actual molecule cannot be represented by any one of these structures alone. Hybridization theory can help explain this phenomenon.

Chemical reactions: Understanding hybridization can help predict and explain chemical reactions that involve bonding and electron movement.

Hybridization in organic chemistry: Organic chemistry involves the study of carbon-based compounds, which often involve hybridization to form covalent bonds.

Hybridization in inorganic chemistry: Inorganic chemistry involves the study of non-carbon based compounds, which also involve hybridization in the formation of bonds.

sp Hybridization: In sp hybridization, one s orbital and one p orbital bond together to create two hybrid orbitals that are linearly aligned.

sp2 Hybridization: In sp2 hybridization, one s orbital and two p orbitals bond together to create three hybrid orbitals that are coplanar and form a 120-degree bond angle.

sp3 Hybridization: In sp3 hybridization, one s orbital and three p orbitals bond together to create four hybrid orbitals that are tetrahedral and form a 109.5-degree bond angle.

sp3d Hybridization: In sp3d hybridization, one s orbital, three p orbitals, and one d orbital bond together to form five hybrid orbitals that are trigonal bipyramidal.

sp3d2 Hybridization: In sp3d2 hybridization, one s orbital, three p orbitals, and two d orbitals bond together to form six hybrid orbitals that are octahedral.

dsp2 Hybridization: In dsp2 hybridization, one s orbital, two p orbitals, and two d orbitals bond together to form five hybrid orbitals that are trigonal bipyramidal, with one of the hybrid orbitals being nonbonding.

d2sp3 Hybridization: In d2sp3 hybridization, two d orbitals, one s orbital, and three p orbitals bond together to form six hybrid orbitals that are octahedral, with two of the hybrid orbitals being nonbonding.

sp3d3 Hybridization: In sp3d3 hybridization, one s orbital, three p orbitals, and three d orbitals bond together to form seven hybrid orbitals that are pentagonal bipyramidal.

sp3d4 Hybridization: In sp3d4 hybridization, one s orbital, three p orbitals, and four d orbitals bond together to form eight hybrid orbitals that are capped square antiprismatic.

sp3d5 Hybridization: In sp3d5 hybridization, one s orbital, three p orbitals, and five d orbitals bond together to form nine hybrid orbitals that are tricapped trigonal prism.