Explain how \({\rm{\sigma }}\) and \({\rm{\pi }}\) bonds are similar and how they are different.

The axial overlap of atomic orbitals forms a sigma bond, while the side-to-side overlap of p-orbitals forms pi bonds.

Both the sigma and pi bonds are covalent bonds that are formed by sharing an electron pair. When two orbitals overlap axially along the internuclear axis, the sigma bond is formed; it is a strong bond that requires a lot of energy to break. According to the VSEPR model, the shape of a molecule is determined by its sigma bonds. The sigma bonds can rotate, but the pi bonds cannot because they will break if they are rotated.

Therefore, the similarities between sigma and pi bonds are that they are both formed by orbital overlap and that they are both covalent bonds, meaning they involve a bond pair. The difference between sigma and pi bonds is that sigma bonds are the strongest, whereas pi bonds are weaker than sigma bonds. The sigma bond is formed by linear atomic orbital overlap, whereas the pi bond is formed by side-to-side atomic orbital overlap. The shape of a molecule is determined by the sigma bond, while the length is determined by the pi bond. The sigma bond can rotate freely around its axis, whereas the pi bond can't because it's locked.