The species having no `ppi-ppi` bond but its bond order equal to that of `O_(2)^(-)`

Options

A. `ClO_(3)^(-)`
B. `PO_(4)^(3-)`
C. `SO_(4)^(2-)`
D. `XeO_(3)`

Explanation

To solve the problem of finding a species that has no Pπ-Pπ bond but a bond order equal to that of O2^(-), we can follow these steps:

### Step 1: Determine the bond order of O2^(-)
- O2^(-) has a total of 6 bonding electrons and 3 antibonding electrons.
- The bond order is calculated using the formula:
\[ \text{Bond Order} = \frac{\text{Number of bonding electrons} - \text{Number of antibonding electrons}}{2} \]
- Substituting the values:
\[ \text{Bond Order} = \frac{6 - 3}{2} = \frac{3}{2} = 1.5 \]

### Step 2: Identify species with bond order of 1.5
- We need to find other species that also have a bond order of 1.5 but do not exhibit Pπ-Pπ bonding.
- One such species is SO4^(2-).

### Step 3: Calculate the bond order of SO4^(2-)
- In SO4^(2-), we can calculate the bond order similarly:
- The charge on the sulfur atom can be calculated as follows:
\[ x - 4 \times (-2) = -2 \implies x + 8 = -2 \implies x = -10 \]
- This means the effective charge on the sulfur is +6.
- The bond order is calculated as:
\[ \text{Bond Order} = \frac{6}{4} = 1.5 \]

### Step 4: Confirm absence of Pπ-Pπ bonds in SO4^(2-)
- In SO4^(2-), the bonding between sulfur and oxygen does not involve Pπ-Pπ bonding but rather Dπ-Pπ bonding due to the involvement of d-orbitals from sulfur.

### Conclusion
- The species that has no Pπ-Pπ bond but a bond order equal to that of O2^(-) is SO4^(2-).

### Final Answer
**SO4^(2-)**