Hybridized orbitals are very useful in explaining of the shape of molecular orbitals for molecules, and are an integral part of valence bond theory. The hybrids are named for the atomic orbitals involved in the hybridization. In methane CH 4 for example, a set of sp 3 orbitals forms by mixing one s- and three p-orbitals on the carbon atom. The orbitals are directed toward the four hydrogen atoms, which are located at the vertices of a regular tetrahedron.
Ethene C 2 H 4 has a double bond between the carbons. For this molecule, carbon will sp 2 hybridize. In sp 2 hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of 3 sp 2 orbitals with one p-orbital remaining.
The pi bond between the carbon atoms forms by a 2p-2p overlap. The two remaining p orbitals p y and p z do not hybridize and remain unoccupied see Figure 6 below.
The geometry of the sp hybrid orbitals is linear, with the lobes of the orbitals pointing in opposite directions along one axis, arbitrarily defined as the x-axis see Figure 7. Each can bond with a 1s orbital from a hydrogen atom to form the linear BeH 2 molecule. Figure 7. The process of sp hybridization is the mixing of an s orbital with a single p orbital the pxorbital by convention , to form a set of two sp hybrids. The two lobes of the sp hybrids point opposite one another to produce a linear molecule.
Other molecules whose electron domain geometry is linear and for whom hybridization is necessary also form sp hybrid orbitals.
Examples include CO 2 and C 2 H 2 , which will be discussed in further detail later. First a paired 2s electron is promoted to the empty 2p y orbital see Figure 8. This is followed by hybridization of the three occupied orbitals to form a set of three sp 2 hybrids, leaving the 2p z orbital unhybridized see Figure 9.
The geometry of the sp 2 hybrid orbitals is trigonal planar, with the lobes of the orbitals pointing towards the corners of a triangle see Figure 9. Each can bond with a 2 p orbital from a fluorine atom to form the trigonal planar BF 3 molecule.
The process of sp 2 hybridization is the mixing of an s orbital with a set of two p orbitals p x and p y to form a set of three sp 2 hybrid orbitals. Each large lobe of the hybrid orbitals points to one corner of a planar triangle. Other molecules with a trigonal planar electron domain geometry form sp 2 hybrid orbitals. Ozone O 3 is an example of a molecule whose electron domain geometry is trigonal planar, though the presence of a lone pair on the central oxygen makes the molecular geometry bent.
The hybridization of the central O atom of ozone is sp 2. Only read the boron section. Skip to main content.
Covalent Bonding. Search for:. Hybrid Orbitals Learning Objectives Define hybridization. Describe sp 3 hybridization and covalent bond formation. Do you recognize this plant? Figure 1. Orbital configuration for carbon atom. Figure 2. Promotion of carbon s electron to empty p orbital. Figure 3. Carbon sp 3 hybrid orbitals. Figure 4.
Summary Electrons hybridize in order to form covalent bonds. Nonequivalent orbitals mix to form hybrid orbitals. For oxygen, assume at least one unhybridised p-orbital. This is the nitrogen inversion. Sign up to join this community. The best answers are voted up and rise to the top. Stack Overflow for Teams — Collaborate and share knowledge with a private group.
Create a free Team What is Teams? Learn more. Ask Question. Asked 5 years, 10 months ago. Active 5 years, 10 months ago. Viewed 9k times. Improve this question. Hybridization is not a physical phenomenon, really. Add a comment. Active Oldest Votes. Once you have taken that for granted, the question may remain: But when do I need to take hybridisation into account for orbital considerations?
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