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In chemistry, orbital hybridisation (or hybridization) is the concept of mixing atomic orbitals to form new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory.
The chart of orbitals (left) is arranged by increasing energy (see Madelung rule). Atomic orbits are functions of three variables (two angles, and the distance r from the nucleus). These images are faithful to the angular component of the orbital, but not entirely representative of the orbital as a whole.
In chemistry, isovalent or second order hybridization is an extension of orbital hybridization, the mixing of atomic orbitals into hybrid orbitals which can form chemical bonds, to include fractional numbers of atomic orbitals of each type (s, p, d). It allows for a quantitative depiction of bond formation when the molecular geometry deviates ...
Hybridization (or hybridisation) may refer to: Hybridization (biology) , the process of combining different varieties of organisms to create a hybrid Orbital hybridization , in chemistry, the mixing of atomic orbitals into new hybrid orbitals
In chemistry, Bent's rule describes and explains the relationship between the orbital hybridization and the electronegativities of substituents. [1] [2] The rule was stated by Henry A. Bent as follows: [2] Atomic s character concentrates in orbitals directed toward electropositive substituents.
Hybridization is a model that describes how atomic orbitals combine to form new orbitals that better match the geometry of molecules. Atomic orbitals that are similar in energy combine to make hybrid orbitals. For example, the carbon in methane (CH 4) undergoes sp 3 hybridization to form four equivalent orbitals, resulting in a tetrahedral shape.
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In chemical bonds, an orbital overlap is the concentration of orbitals on adjacent atoms in the same regions of space. Orbital overlap can lead to bond formation. Linus Pauling explained the importance of orbital overlap in the molecular bond angles observed through experimentation; it is the basis for orbital hybridization.