Final answer:
Sulfur dioxide (SO₂) is a polar molecule due to its bent shape and the difference in electronegativity between sulfur and oxygen, which creates a net dipole moment. The bent geometry means that the dipole moments do not cancel out, confirming its polarity. Consequently, SO₂ has properties characteristic of polar molecules, such as solubility in water.
Explanation:
Sulfur Dioxide (SO₂) Molecular Structure
Sulfur dioxide (SO₂) is a molecule that has a bent shape due to the presence of a lone pair of electrons on the sulfur atom. This bent geometry is represented accurately in the Lewis structure, which helps us visualize the distribution of electron pairs around the central sulfur atom.
Polarity of SO₂
To determine if a molecule is polar or nonpolar, we need to consider both its shape and the electronegativity of its atoms. In the case of SO₂:
- The sulfur atom is less electronegative than the oxygen atoms, leading to a dipole moment where the electron density is drawn more towards the oxygen atoms.
- Because of the bent shape of the molecule, these dipole moments do not cancel out, meaning that there is a net dipole moment in the direction of the oxygen atoms.
As a result, sulfur dioxide is a polar molecule. This polarity contributes to various physical properties such as its solubility in water.
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