Draw three resonance structures for sulfur tetroxide, SO4, whose connections are shown below. (This is a neutral mol-ecule; it is not a sulfate ion.) Assign formal charges to the atoms in each structure.

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In resonance, the actual structure of the molecule is a hybrid of these forms, which helps to represent the distribution of electrons more accurately. For sulfur tetroxide (SO4), multiple resonance structures can be drawn to show how the double bonds and lone pairs can be arranged differently while maintaining the same connectivity.

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps in determining the most stable resonance structure, as the best structure typically has the lowest formal charges on the atoms. In the case of SO4, calculating formal charges for each atom in the resonance structures is essential to assess their stability.

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They provide a visual representation of the molecule's structure, including how atoms are connected and the distribution of electrons. For sulfur tetroxide, drawing the correct Lewis structure is the first step in identifying possible resonance forms and understanding the molecule's overall geometry and electron distribution.