what is a pi bond?
A pi bond is the sideways overlap of two p orbitals. The sigma bond is a head to head overlap of and s and p or two p orbitals
When the electron orbitals overlap laterally, the bond is called the pi () bond. In pi bonds the resulting overlap is not maximum and these bonds are relatively weak. A molecule of ethylene or ethene (C2H4) has 4 bonds and 2 bonds. In pi bonds the resulting overlap is not maximum and these bonds are relatively weak. A molecule of ethylene or ethene (C2H4) has 4 bonds and 2 bonds.
A pi bond is a type of chemical bond that forms when two atomic orbitals, which are not in the line of the internuclear axis, overlap side-by-side. Pi bonds are commonly seen in molecules containing double or triple bonds.
To understand pi bonds, it is important to know the concept of molecular orbitals. Molecular orbitals are regions where electron density is concentrated in a molecule. There are two types of molecular orbitals: sigma (σ) and pi (π) orbitals.
First, two atoms form a sigma bond by overlapping their atomic orbitals along the internuclear axis. This type of bond allows for free rotation around the internuclear axis.
When atoms have unhybridized p orbitals, they can overlap sideways above and below the internuclear axis. This overlapping results in the formation of a pi bond. Pi bonds are characterized by the electron density above and below the plane formed by the bonded atoms. Importantly, unlike sigma bonds, pi bonds prevent free rotation around the internuclear axis.
Overall, pi bonds are essential in forming multiple bonds in organic molecules and greatly influence the reactivity and shape of molecules.