Draw the resonatin structure of
(i) Ozone molecule (ii) Nitrate ion

Explanation

To draw the resonating structures of ozone (O₃) and the nitrate ion (NO₃⁻), we will follow these steps:

### Step 1: Draw the Lewis Structure of Ozone (O₃)
1. **Count the total valence electrons**: Oxygen has 6 valence electrons, and there are 3 oxygen atoms, so the total is 6 x 3 = 18 valence electrons.
2. **Arrange the atoms**: The central atom is usually the least electronegative, which in this case is one of the oxygen atoms. So, we have O-O-O.
3. **Distribute the electrons**: Start by forming single bonds between the central oxygen and the other two oxygens. This uses 4 electrons (2 bonds).
4. **Place remaining electrons**: Distribute the remaining 14 electrons to satisfy the octet rule. You will end up with one oxygen having a double bond with the central oxygen and one oxygen with a single bond.

### Step 2: Identify Resonating Structures of Ozone
1. **First Resonating Structure**:
- One oxygen has a double bond with the central oxygen, while the other has a single bond.
- Assign formal charges: The oxygen with a double bond has no charge, the central oxygen has a positive charge (+1), and the oxygen with a single bond has a negative charge (-1).

2. **Second Resonating Structure**:
- Shift the double bond to the other oxygen.
- Now, the first oxygen has a single bond and a negative charge, the central oxygen has a positive charge, and the second oxygen has a double bond with the central oxygen.

### Step 3: Draw the Resonance Hybrid for Ozone
- The resonance hybrid shows that the bonds are not purely single or double but rather have partial double bond character.
- Each oxygen will have a partial charge, with the central oxygen having a +1 charge and the terminal oxygens having a -1/2 charge.

### Step 4: Draw the Lewis Structure of Nitrate Ion (NO₃⁻)
1. **Count the total valence electrons**: Nitrogen has 5 valence electrons and each oxygen has 6. For NO₃⁻, we have 5 + (6 x 3) + 1 (for the negative charge) = 24 valence electrons.
2. **Arrange the atoms**: Place nitrogen in the center with three oxygens around it.
3. **Distribute the electrons**: Form single bonds between nitrogen and each oxygen. This uses 6 electrons. Distribute the remaining 18 electrons to satisfy the octet rule.

### Step 5: Identify Resonating Structures of Nitrate Ion
1. **First Resonating Structure**:
- One oxygen has a double bond with nitrogen, while the other two have single bonds.
- Assign formal charges: The nitrogen has a +1 charge, and one oxygen with a double bond has no charge, while the other two oxygens have a -1 charge each.

2. **Second Resonating Structure**:
- Shift the double bond to one of the other oxygens.
- The nitrogen still has a +1 charge, and the other two oxygens will have a -1 charge each.

3. **Third Resonating Structure**:
- Shift the double bond to the third oxygen.
- The nitrogen remains with a +1 charge, and the two oxygens with single bonds have a -1 charge each.

### Step 6: Draw the Resonance Hybrid for Nitrate Ion
- The resonance hybrid shows that all N-O bonds are equivalent and have partial double bond character.
- Each oxygen will have a charge of -2/3, and nitrogen will have a +1 charge.

### Summary
- The resonating structures of ozone (O₃) involve two forms where the double bond shifts between the terminal oxygens.
- The nitrate ion (NO₃⁻) has three resonating structures where the double bond shifts among the three oxygen atoms.