Table of Contents
Orbital overlap in a chemical bond is the merging of orbitals on neighbouring atoms in the same areas of space. The bond formation can result from orbital overlap. When two atoms approach close together during the orbital process, they pierce each other’s orbital, establishing a new hybridized orbital in which the bonding pair of electrons dwell. Because it has less energy than the atomic orbital, this hybridized orbital is more stable. It is in a low-energy condition. Orbital overlap refers to the partial penetration of an orbital to generate a new hybridized orbital. The orbitals have two sorts of overlapping areas: sigma (σ) and pi (π). Orbital overlap refers to this partial penetration of the orbital.
The extent of overlap is determined by the two participating atoms, their size, and the number of valence electrons. In general, the stronger the link created between the two atoms, the bigger the overlap. According to the orbital overlap notion, atoms interact by overlapping their orbitals, generating a lower energy state in which their valence electrons with opposing spin couple up to create a covalent bond.
Linus Pauling stressed the relevance of orbital overlap in explaining the chemical bond angles seen through experiments, which is the foundation for the notion of orbital hybridization.
Bond Directional Properties
The directional features of the bond were used to explain the molecular bond angles. The hydrogen molecule is created by the overlap of 1s orbitals in a head-on collision.
Atomic Orbital Overlap
When two atoms make contact to create a bond, their overlap can be positive, negative, or even zero, depending on the phase and sign of the two interacting orbitals.
- Positive Atomic Orbital Overlap – When the phases of two interacting orbitals match, the overlap is positive and the bond is formed. The phase of the two interacting orbitals (+ or -) is governed by the sign of the orbital wave function and has nothing to do with the charge.
- Negative Atomic Orbital Overlap – When two interacting atomic orbitals have opposing phases, the overlap is negative and no link is created.
- Zero Overlapping of Atomic Orbital- When the orientation of two interacting atomic orbitals is such that there is no overlapping of the orbitals, this is known as zero overlapping.
FAQs
Why do orbitals intersect?
Atomic orbitals overlap because they take up space. An atomic orbital is a location in space where an electron is most likely to be discovered. The increasing electron density attracts the two nuclei and reduces their repulsions. As a result, a covalent link between H and Cl is created.
What exactly are orbital phases?
Orbitals are mathematical functions that define complicated patterns of standing waves that can be graphed but have no physical substance. The wave-like features of electrons cause an orbital process.
What exactly is meant by hybridization?
In chemistry, orbital hybridization (or hybridization) is the process of mixing atomic orbitals to generate new hybrid orbitals (with varied energies, sizes, and so on) appropriate for matching electrons in valence bond theory to form chemical bonds.
