Final answer:
The formal charges for each resonance contributor of the fulminate ion can be determined by assigning formal charges to each atom in the Lewis structure. The actual distribution of electrons in the fulminate ion is an average of these resonance contributors, resulting in a formal charge of -1 on the nitrogen atom and a formal charge of 0 on the carbon and oxygen atoms.
Step-by-step explanation:
The formal charges for each resonance contributor of the fulminate ion can be determined by assigning formal charges to each atom in the Lewis structure. The fulminate ion, CNO-, has a resonance structure with a triple bond between the carbon and nitrogen atoms, and a single bond between the nitrogen and oxygen atoms. The formal charges for each atom in this resonance contributor are as follows:
- Carbon atom (-1)
- Nitrogen atom (0)
- Oxygen atom (0)
In another resonance contributor, the double bond is between the carbon and oxygen atoms, while the nitrogen atom maintains a single bond with the oxygen atom. The formal charges for each atom in this resonance contributor are as follows:
- Carbon atom (0)
- Nitrogen atom (-1)
- Oxygen atom (+1)
These resonance forms show different distributions of electrons, while keeping the same arrangement of atoms. The actual distribution of electrons in the fulminate ion is an average of these resonance contributors, resulting in a formal charge of -1 on the nitrogen atom and a formal charge of 0 on the carbon and oxygen atoms.