Why is hybridization in chemistry necessary?

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The term “hybridization” refers to the production of something new from a combination or mixture of other components. The classic use of the term “hybrid” is to describe plants that have been blended together. A hybrid plant is one made from two different plants blended together. The hybrid has characteristics of the two composite plants. The hybridization process is necessary to produce an improved or healthier plant.

In the world of chemistry, “hybridization” refers to the mixing of atomic orbitals. Hybridization in chemistry is the process by which orbitals within the same atom but of slightly different energies mix or rearrange to redistribute their energies. A new set of atomic orbitals with the same total electron capacity is formed. The energies of this new set of orbitals are equivalent and between those of the original orbitals before the hybridization process. The new orbitals are called hybridized orbitals or hybrids. There is the same number of the newly formed hybridized orbitals as the number of atomic orbitals that were hybridized. In the context of chemistry, hybridization of atomic orbitals explains the apparent change between the orbitals in an uncombined atom and the orbitals that that same atom uses during bonding.

Hybridization, then, is a theory to explain the rearranging of orbitals where it would appear that such rearrangement or blending might not otherwise be possible. The concept of hybridization was developed (and was actively promoted by Nobel Prize-winning chemist Linus Pauling) for a simple chemical system. It was subsequently applied more broadly until it was deemed to be an accepted explanation for processes involving organic compounds.

By way of example, electronics of the lowest energy will be found around the atomic nucleus. This sphere-shaped region is the orbital that would contain no more than two electrons. It is known as an ‘s’ orbital. The lowest energy level is called “1s.” The “p” orbitals are similar to two rubber balls fused together. Their region in space follows a straight line.

What is significant is the orientation and the angles of the bonds produced within the molecules. Methane CH4 molecule is frequently used to demonstrate the principle. The bond angles are found to be approximately 109 degrees. The orbitals used for bonding are arranged in such a manner as to suggest that they have the same energy although they do not. The three “2p” orbitals have greater energy than the “2s” orbital. One of the electrons must move from the “2s” orbital to the “2pz” orbital for hybridization to take place. The hybridization process is critical as it permits the combination of the atomic orbitals and the production of four hybridized orbitals. Because the four hybrids came from one “s” and three “p” orbitals, the hybridized orbitals are identified as “sp3″ orbitals. These hybrids are then used for bonding.

Hybridization is a normal process. All elements undergo hybridization, or something similar to it, when bonding. Atoms need to rearrange their atomic orbitals so as to form rearranged orbitals with shapes more conducive for bonding. The hybridization process is necessary so that there is better and more effective bonding than if unhybridized orbitals blended together.

Resource by Will

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