Final answer:
The correct Lewis dot structure for SO2 involves a central sulfur atom doubly bonded to two oxygen atoms, each with two lone pairs, in an OSO arrangement. This structure is supported by formal charge considerations and resonance theory, which posits that the actual molecule is a blend of the drawn resonance forms.
Step-by-step explanation:
The Lewis dot structure for sulfur dioxide (SO2) consists of a central sulfur atom with six valence electrons and two oxygen atoms, each with six valence electrons as well. With a total of 18 valence electrons to consider, the Lewis structure will depict sulfur doubly bonded to each oxygen atom, with each oxygen atom also having two lone pairs of electrons. Formal charge considerations suggest the most stable structure is OSO, with the sulfur in the center.
In the context of resonance structures, these various forms are all correct and portray the molecule's delocalized electrons. It's important to remember that, while we may draw different resonance forms, the actual molecule is a blend of these forms, known as a resonance hybrid. For SO2, the structure that minimizes formal charges is often used to represent the molecule.