Which of the following molecule does not possess a permanent dipole moment? (a) H2 S (b) SO2 (c

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Which of the following molecule does not possess a permanent...

Key Concepts

Molecular Geometry

Molecular geometry refers to the three?dimensional arrangement of atoms in a molecule, which is determined by the VSEPR (Valence Shell Electron Pair Repulsion) theory. The geometry affects how individual bond dipoles, which arise from differences in electronegativity, are oriented. In symmetric geometries, these dipoles may cancel each other out, leading to a nonpolar molecule, whereas in asymmetrical geometries, they do not, resulting in a net dipole moment.

Dipole Moment

A dipole moment is a measure of the separation of positive and negative charges in a molecule. For a molecule to possess a permanent dipole moment, it must have an uneven distribution of electrons due to differences in electronegativity and an asymmetric molecular geometry. If the molecular structure is symmetric, the individual bond dipoles can cancel, leaving no overall dipole moment.

Symmetry

Symmetry in a molecule plays a critical role in determining its polarity. When a molecule is highly symmetric, the symmetry leads to a cancellation of individual bond dipoles—even if the bonds are polar—which results in a molecule with no permanent dipole moment. Hence, recognizing patterns such as linear, trigonal planar, or tetrahedral symmetry is essential in predicting molecular polarity.

Electronegativity

Electronegativity is the tendency of an atom to attract shared electrons in a chemical bond. The difference in electronegativity between atoms creates polar bonds, where electrons are unevenly distributed. However, the overall molecular polarity also depends on the molecular geometry; in symmetric molecules, even bonds with significant electronegativity differences can cancel each other out, resulting in no permanent dipole moment.

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