Final answer:
σ (sigma) and π (pi) bonds are distinguished by their form of orbital overlap, with σ bonds involving end-to-end overlap and being present in all single bonds, whereas π bonds result from side-to-side orbital overlap and are found in double and triple bonds. Option a
Step-by-step explanation:
σ (sigma) and π (pi) bonds are types of covalent bonds that differ in the way atomic orbitals overlap. σ bonds involve head-on (or end-to-end) overlap of atomic orbitals and are found in every single bond. These bonds allow for the free rotation of bonded atoms because the electron density is symmetrically distributed along the internuclear axis.
On the other hand, π bonds result from the side-by-side overlap of atomic orbitals, particularly p orbitals, leading to electron density above and below the internuclear axis. Pi bonds restrict rotation and are found in double and triple bonds, accompanying a sigma bond.
σ and π bonds share the similarity that both are results of the overlap of atomic orbitals on adjacent atoms, and they each can contain a maximum of two electrons. However, σ bonds are generally stronger due to the direct overlap, making them more effective at holding the two atoms together compared to the parallel overlap of π bonds.
It's also worth noting that multiple bonds (double or triple) are made up of one σ bond and one or two π bonds respectively.
Given the information provided, the correct answer to the question would be: a) Similar: Both involve the overlap of atomic orbitals; Different: σ bonds involve head-on overlap, while π bonds involve side-to-side overlap. Option a