Back Bonding in Chemistry | Inorganic and Organic Chemistry | IIT Jee Mains, Advance, NEET & AIIMS - Videos

Hello Guys,
Back-Bonding is one of the most important topic for Jee Mains, Advance, NEET & AIIMS.
Sigma bond: A covalent bond resulting from the formation of a molecular orbital by the end-to-end overlap of atomic orbitals, denoted by the symbol σ.

Pi bond: A covalent bond resulting from the formation of a molecular orbital by side-to-side overlap of atomic orbitals along a plane perpendicular to a line connecting the nuclei of the atoms, denoted by the symbol π.

now, coming to the explanation part:

If there is bonding between two atoms where one atom is having one vacant orbital and another is having one lone pair of electrons, then this electron pair is donated to that respective vacant orbital ..then this bonding is called p-p or p-d depending upon the orbital to which the pair is donated and from which the electron pair is donated. if both the orbitals are d, then its called d(pi)-d(pi) bonding. these bonding are also called back-bonding bonds.

Eg.

in BF3, B has incomplete octet so a fully filled p(pi) orbital of F donates a lone pair of e to the vacant orbital of B. so here pp(pi)-p(pi) bonding occurs and is known as back-bonding also.

dπ-pπ bonding is the formation of a π molecular orbital by the overlap of a d orbital on one atom with a
p or p* orbital on another atom.
An example is the orbital overlap in a metal carbonyl such as Ni(CO)₄.
Usually, one atom supplies both electrons to the new bond. If the
d-orbital supplies the electrons, the process is called backbonding.

Phosphorus does not form dπ-pπ bonds, because the d-orbitals on P are too high in energy.
However, the lone-pair electrons in phosphines (R₃P) make good
σ donors to the d orbitals of transition metals.
Electron withdrawing groups lower the energies of the
σ*orbitals. These antibonding orbitals can then act as backbonding
π acceptors. PF₃ is almost as good an acceptor as CO. Phosphites [(RO)₃P] are about half as good as CO.
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