What is Orbital Overlap?
The atoms combine by colliding with each other. But what does this mean on atomic level. This situation refers to the process in which the two atoms comes so close to each other that they penetrate each other’s orbital and form a new hybridized orbital where the bonding pair of electrons reside. This hybridized orbital has lower energy than the atomic orbital and hence are stable. It is in the minimum energy state. This partial penetration of the orbital is known as orbital overlap.
The extent of overlap depends on the two participating atoms, their size and the valence electrons. In general, the greater the overlap, the stronger the bond formed between the two atoms. Thus, according to the orbital overlap concept, atoms combine by overlapping their orbital and thus forming a lower energy state where their valence electrons with opposite spin, pair up to form covalent bonds.
The importance of orbital overlap was emphasized by Linus Pauling while explaining the molecular bond angles observed through experimentation and is the basis for the concept of orbital hybridization.
Table of Contents
Directional Properties of bond
The molecular bond angles were explained through the directional properties of the bond. The molecule of hydrogen is formed by the overlap of 1s orbital in head-on collision.
Overlapping of Atomic Orbital
When two atoms come in contact with each other to form a bond, their overlap can be positive, negative or even zero depending upon the phase and sign of the two interacting orbitals.
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- Positive Overlapping of Atomic Orbitals – When the phase of two interacting orbitals is the same, then the overlap is positive and in this case, the bond is formed. The phase of the two interacting orbital (+ or -) comes from the sign of orbital wave function and is not related to the charge in any sense.
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- Negative Overlapping of Atomic Orbitals – When the phase of two interacting atomic orbitals is opposite, then the overlap is negative and in this case, the bond is not formed.
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- Zero Overlapping of Atomic Orbitals – When the orientation of two interacting atomic orbital is such that there is no overlapping of the orbitals, that is known as zero overlapping.
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Frequently Asked Questions – FAQs
Why do orbitals overlap?
Orbital is a space around the nucleus where there is a maximum probability of finding the electrons. Orbital overlap leads to bond formation resulting in the stability of the combining atoms.
What is the positive overlap?
If the two interacting orbitals have the same phase, then the overlap is positive and a bond is formed. The phase of the two interacting orbitals (+ or -) is the sign of orbital wave function and is not related to the charge.
What do you mean by zero overlaps?
A zero overlap is a result of orbitals do not overlap at all or do not overlap efficiently. A zero overlap does not lead to bond formation between the atomic orbitals.
What are orbital phases?
Orbitals are essentially mathematical functions that define complex patterns of standing waves that can be graphed on a graph but do not have any physical reality. An orbital process is a direct result of electrons’ wave-like properties.
What is meant by hybridization?
Orbital hybridization (or hybridization) in chemistry is the process of combining atomic orbitals into new hybrid orbitals (with different energies, sizes, etc., than atomic orbitals) suitable for pairing electrons in valence bond theory to form chemical bonds.
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