Final answer:
Resonance structures involve shifting double bonds and lone pairs within a molecule without changing its overall connectivity. To find the formal charges, the electrons around each atom are counted and compared to the typical valence electron count. Ozone, sulfate, nitrite, and carbonate ions have different resonance structures, each affecting the formal charge differently.
Step-by-step explanation:
Drawing all possible resonance structures for compounds and determining the formal charge on each atom can be done using Lewis structures. Let's go through each compound:
Ozone (O₃)
Ozone has three resonance structures with a double bond shifting among the three oxygen atoms. Each resonance structure has one oxygen with a formal charge of +1, one with a formal charge of -1, and one neutral oxygen.
Sulfate ion (SO4²⁻)
The sulfate ion has four resonance structures because the double bonds can rotate among the four oxygen atoms. Each oxygen in double bond has a formal charge of 0, while the oxygens with single bonds have a formal charge of -1. The sulfur has a formal charge of +2.
Nitrite ion (NO²⁻)
Nitrite ion has two resonance structures with the double bond switching between the two oxygen atoms. One oxygen has a formal charge of 0 in each structure, while the other has a formal charge of -1, and the nitrogen has a formal charge of +1.
Carbonate ion (CO3²⁻)
The carbonate ion has three equivalent resonance structures, each with a different oxygen double-bonded to carbon. In each structure, the double-bonded oxygen has a formal charge of 0, while the singly bonded oxygens have a formal charge of -1. The central carbon has a formal charge of +1.