are delocalized electron pairs counted in hybrid orbital?
No, delocalized electron pairs, also known as pi (π) electrons, are not included in the hybrid orbital count. Hybrid orbitals are formed by the combination of atomic orbitals and are involved in sigma (σ) bonding. Pi (π) bonding, which involves the overlap of p orbitals, is not considered in the formation of hybrid orbitals.
Delocalized electron pairs are not directly counted in hybrid orbitals. Hybrid orbitals are formed by the mixing of atomic orbitals to account for the observed shape and bonding properties of molecules. They are often used to describe the bonding in organic compounds.
When determining the hybridization of an atom, only the localized electron pairs (also called lone pairs) and the sigma bonds are considered. These electron pairs and bonds are involved in the formation of hybrid orbitals. Delocalized electrons, such as those found in pi bonds or in resonance structures, are not directly accounted for in the hybridization.
However, delocalized electrons can influence the overall bonding and reactivity of a molecule, and the presence of pi bonds or resonance can affect the molecular geometry and hybridization indirectly. It is important to note that hybridization is a simplification, and in certain cases, the actual electronic structure of a molecule may require a more complex description using molecular orbital theory.
When determining the hybridization of an atom, only the localized electron pairs are typically considered. Delocalized electron pairs, such as those found in pi bonds or resonance structures, do not contribute to the hybrid orbitals.
To determine the hybridization of an atom, follow these steps:
1. Determine the number of valence electrons for the atom.
2. Count the number of electron pairs around the atom, including both lone pairs and bonds.
3. Use the concept of hybridization to determine the type of hybrid orbitals that will form.
4. Assign the appropriate number of hybrid orbitals to accommodate all the electron pairs.
For example, let's consider the central atom in carbon monoxide (CO). Carbon has 4 valence electrons, and oxygen has 6 valence electrons. Oxygen forms a double bond with carbon, resulting in a total of 8 electrons around carbon.
Since there are two electron pairs, carbon will undergo hybridization to form two hybrid orbitals. In this case, carbon hybridizes to form two sp hybrid orbitals.
Note that the delocalized electrons in the pi bond between carbon and oxygen are not considered when determining the hybridization. They are accounted for separately in the molecular orbital theory, which explains the electronic structure of molecules more accurately.