Find the number of species in which `dpi-ppi` bonds are present?
`ClO_(3)^(-),PO_(4)^(3-),SO_(3),NO_(3)^(-)`

Explanation

To find the number of species in which d-π-p-π bonds are present among the given species: ClO₃⁻, PO₄³⁻, SO₃, and NO₃⁻, we will analyze each species one by one.

### Step 1: Analyze ClO₃⁻ (Chlorate Ion)
- **Central Atom**: Chlorine (Cl)
- **Electronic Configuration**: Cl has the configuration of 3s² 3p⁵. It has vacant 3d orbitals.
- **Bonding**: In ClO₃⁻, Cl forms double bonds with two oxygen atoms and a single bond with one oxygen atom (which carries a negative charge).
- **Covalency**: To achieve a covalency of 5, Cl must promote electrons from the 3s and 3p orbitals into the 3d orbital.
- **Bond Types**: The double bonds formed with oxygen involve d-π interactions. Therefore, ClO₃⁻ has d-π-p-π bonds.

### Step 2: Analyze PO₄³⁻ (Phosphate Ion)
- **Central Atom**: Phosphorus (P)
- **Electronic Configuration**: P has the configuration of 3s² 3p³. It also has vacant 3d orbitals.
- **Bonding**: In PO₄³⁻, P forms four sigma bonds with four oxygen atoms, and some of these bonds can involve double bonding.
- **Covalency**: To achieve a covalency of 5, P can promote electrons to the 3d orbital.
- **Bond Types**: The pi bonds formed with oxygen involve d-π interactions. Thus, PO₄³⁻ also has d-π-p-π bonds.

### Step 3: Analyze SO₃ (Sulfur Trioxide)
- **Central Atom**: Sulfur (S)
- **Electronic Configuration**: S has the configuration of 3s² 3p⁴. It has vacant 3d orbitals.
- **Bonding**: In SO₃, S forms double bonds with three oxygen atoms.
- **Covalency**: To achieve a covalency of 6, S can promote electrons from the 3s and 3p orbitals into the 3d orbital.
- **Bond Types**: The double bonds formed with oxygen involve d-π interactions. Therefore, SO₃ has d-π-p-π bonds.

### Step 4: Analyze NO₃⁻ (Nitrate Ion)
- **Central Atom**: Nitrogen (N)
- **Electronic Configuration**: N has the configuration of 2s² 2p³. It does not have vacant d orbitals.
- **Bonding**: In NO₃⁻, N forms double bonds with one oxygen and a single bond with another oxygen (which carries a negative charge).
- **Covalency**: The maximum covalency of N is 4, and it cannot form d-π bonds as it lacks d orbitals.
- **Bond Types**: Therefore, NO₃⁻ does not have d-π-p-π bonds.

### Conclusion
The species that contain d-π-p-π bonds are ClO₃⁻, PO₄³⁻, and SO₃.

Thus, the total number of species with d-π-p-π bonds is **3**.

### Final Answer
**The number of species in which d-π-p-π bonds are present is 3.**

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