Question

For the following reaction, write a reasonable mechanism, using curved arrow notation to show the flow of electrons, for the formation of all three products. Your answer should include all important resonance structures.

a) True
b) False

Answer 1

Writing resonance forms involves depicting different Lewis structures to represent the distribution and delocalization of electrons in a molecule or ion. The double-headed arrow symbolizes that the true form is a hybrid of these structures.

Step-by-step explanation:

The question asks to write resonance forms that describe the distribution of electrons in specific molecules or ions, such as sulfur dioxide (SO2) and the carbonate ion (CO32-). Resonance forms are multiple Lewis structures that collectively describe the delocalization of electrons in a molecule or ion. The structures show the same arrangement of atoms but differ in the placement of electrons, especially in terms of pi bonds and nonbonding electrons.

In the case of sulfur dioxide (SO2), two resonance structures can be drawn to show the delocalization of electrons between the sulfur atom and the oxygen atoms. For the carbonate ion (CO32-), three resonance structures are typically drawn to show the electrons being shared between the carbon and three oxygen atoms evenly, with each oxygen atom forming a double bond with carbon in at least one structure.

To indicate resonance, a double-headed arrow (↔) is used between the structures, representing that the actual molecular structure is a hybrid of these resonance forms. Every resonance form should maintain the overall charge of the molecule or ion and should follow the octet rule where applicable.