b. Draw the resonance forms for ozone (bonded O–O–O)
c. Sulfur dioxide has one more resonance form than ozone. Explain why this structure is not possible for ozone.

For each pair of ions, determine which ion is more stable. Use resonance forms to explain your answers.

(e)

(f)

In the following sets of resonance forms, label the major and minor contributors and state which structures would be of equal energy. Add any missing important resonance forms.

(d)

(e)

Use resonance structures to identify the areas of high and low electron density in the following compounds:

(a)

(b)

(c)

Draw the important resonance forms to show the delocalization of charges in the following ions. In each case, indicate the major resonance form(s).

(j)

(k)

a. Draw the resonance forms for SO₂ (bonded O–S–O).

Draw the important resonance forms of the following cations and anions:

(c)

(d)

Draw the important resonance forms for the following molecules and ions.

(d) NO₃^–

(e) NO₂^–

(f)

Draw the important resonance forms for the following molecules and ions.

(a) CO₃^2–

(b)

(c)