Banana Bond in Chemistry | Explained by IITian | IIT Jee Mains, Advance, BITSAT, NEET and AIIMS Video
A banana bond is also known as a bent bond. It is a type of chemical bonding where the ordinary hybridization state of two atoms making up a chemical bond are modified with increased or decreased s-orbital character in order to accommodate a particular molecular geometry (that of 3 bananas in a ring shape).
Technically, the banana bonds can be said to be made up of orbitals similar to sp3sp3 but not exactly (like two sp 3.1 and two sp 2.9 orbitals--since hybridization is just addition of wave functions, we can always change the coefficients to give proper geometry).
You see this type of bond in small-ring compounds like cyclopropane (C₃H₆) and cyclobutane (C₄H₈) and in 3- and 4-membered heterocyclic rings.
Looking at this in a little more detail, we can see that the C-C bonds of cyclopropane are "bent" and not pure sigma bonds. Recall that overlap is greatest when orbitals overlap "end-on", i.e., via sigma bonding. Pi bonds overlap laterally. The overlap in cyclopropane is neither end-on or lateral, but in between. So it is intermediate between sigma and pi bonding. These bonds are also sometimes called "banana bonds".
The cause of the bent overlap is that the internuclear angle ( the angle between the bond lines connecting the nuclei) is forced to be much smaller (60 degrees) than the interorbital angle (the angle between the axis of the two AO's on a given carbon), which is 109.5 degrees.
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