From your drawing, describe the difference in sigma and pi orbitals based on the interaction of different atomic orbitals in valence bond theory.

Question: From your drawing, describe the difference in sigma and pi orbitals based on the interaction of different atomic orbitals in valence bond theory.

Sigma and pi orbitals are different ways of describing the overlapping of atomic orbitals in covalent bonds. Sigma orbitals are formed by the head-to-head or axial overlap of two orbitals, such as s-s, s-p, or p-p. Pi orbitals are formed by the side-by-side or lateral overlap of two p orbitals. Sigma bonds are stronger and more stable than pi bonds, because the overlap is more effective and the electrons are closer to the nuclei. Pi bonds are weaker and more reactive than sigma bonds, because the overlap is less effective and the electrons are farther from the nuclei. Sigma bonds also allow free rotation around the bond axis, while pi bonds restrict the rotation and create a rigid structure.

Here is a diagram that illustrates the difference between sigma and pi orbitals for some common bond types:

!sigma and pi orbitals

The diagram shows that a single bond is always a sigma bond, while a double bond consists of one sigma bond and one pi bond, and a triple bond consists of one sigma bond and two pi bonds. The diagram also shows the orientation of the overlapping orbitals and the shape of the resulting molecular orbitals.

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