Question

Does pz orbital overlap laterally(pie bond formation)?

Answer 1

Many of us are already aware of the definition of a sigma bond from our teachers, text books or from many of the websites online. However, if you are still not aware of what these two bonds are, then here is a basic definition of the two:

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.

Now have a look at this illustration to see how this end-to-end overlapping occures:

Fig 1: Formation of a Sigma bond

Misconception: many students in the Pacific may have this worng notion that a sigma

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.

Here's another illustration showing how the side-to-side overlapping occurs:

Fig 2: Formation of a Pi bond

It is important to note that different sources use different terms to define what a sigma and pi bond is. However, once examined carefully, it will be evident that they all try to explain the same thing.