Final answer:
To add missing nonbonding electrons and formal charges to a resonance structure can be a true statement if the existing structure is incomplete or incorrectly represented. It helps in identifying the most stable structure by aiming for charges close to zero. However, in cases like benzene, where formal charges are already zero, it is not applicable. Option d is correct.
Step-by-step explanation:
When asked to add missing nonbonding electrons and formal charges to resonance structure 1, the answer could be true or false depending on the specific context and the resonance structure provided. In general, to achieve a more accurate representation of a molecule, you indeed should add all nonbonding (lone pair) electrons and calculate the formal charges for each atom within a resonance structure. Formal charge calculations are based on the idea that electrons in bonds are shared equally between the two bonded atoms, and it helps chemists to determine the most plausible Lewis structure for a molecule. When comparing different possible structures (resonance forms), those with formal charges closest to zero are usually considered more stable and therefore preferable.
Using benzene as an example, each carbon atom in the resonance structures of benzene contributes to bonds using sp2 hybridized orbitals and has no nonbonding electrons, resulting in a formal charge of zero for each carbon atom. This makes both resonance forms equally preferable and their superposition accurately represents benzene's delocalized pi bonding. In this case, adding nonbonding electrons and calculating formal charges is not applicable because the structure is already optimized as all carbons are neutral.
It is important to understand that formal charges do not reflect the actual charge but serve as a tool for determining the most stable electronic structure by balancing the counts of electrons around atoms.