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Correct Answer: 119.5
the correct bond angle for the sulfur dioxide (so2) molecule is 119.5 degrees. this value is crucial in understanding the molecular geometry and behavior of so2 in various chemical environments.
typically, if a molecule like so2, which consists of a central sulfur atom bonded to two oxygen atoms, did not possess any lone pairs of electrons on the central atom, it would exhibit a trigonal planar shape with a bond angle of 120 degrees. however, the actual structure of so2 is not trigonal planar but rather bent or v-shaped.
this deviation from the expected trigonal planar shape is due to the presence of a lone pair of electrons on the sulfur atom. in molecular geometry, lone pairs are significant because they occupy more space around the central atom compared to bonding pairs. this is because lone pairs are solely located on the central atom and not shared between atoms, which allows them more room to spread out.
in the case of so2, the lone pair on the sulfur atom exerts repulsion forces on the bonding pairs (the sulfur-oxygen bonds). according to the vsepr (valence shell electron pair repulsion) theory, these repulsion forces between the lone pair and bond pairs are greater than the repulsions between bond pairs themselves. as a result, the lone pair pushes the two sulfur-oxygen bonds closer together, reducing the bond angle from the ideal 120 degrees to approximately 119.5 degrees.
understanding this behavior is important for predicting the physical and chemical properties of the molecule, including its reactivity and interaction with other molecules. this knowledge plays a critical role in fields like environmental science, where so2 is known as a significant pollutant, and in industrial applications where so2 is used or produced.
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