Which of the following compounds have resonance structures? a. H2O b. SO3 c. CCl4 d. none of the compounds have resonance structures.
The Correct Answer and Explanation is:
The correct answer is b. SO3.
Explanation:
- H2O (Water): Water has a simple structure where the oxygen atom forms two single bonds with two hydrogen atoms. There is no possibility for the shifting of electrons or multiple bonding between atoms that would create resonance structures. Thus, H2O does not have resonance structures.
- SO3 (Sulfur Trioxide): Sulfur trioxide is an example of a molecule with resonance structures. In SO3, sulfur is centrally bonded to three oxygen atoms, each via a double bond. However, these bonds are not fixed; rather, they delocalize across the molecule. The actual structure of SO3 is a hybrid of multiple resonance forms, where the double bonds between sulfur and oxygen are not fixed but rather spread out over the three oxygen atoms. This delocalization of electrons is a key characteristic of resonance structures.
- CCl4 (Carbon Tetrachloride): In carbon tetrachloride, carbon forms four single bonds with chlorine atoms, and there are no multiple bonds or lone pairs that could be involved in electron delocalization. The bonding is quite straightforward, and the molecule does not exhibit resonance structures.
Thus, the only compound among the options with resonance structures is SO3, as it has delocalized electrons and multiple valid Lewis structures that contribute to the overall bonding of the molecule.
