Chemistry - CHEMICAL BONDING Question with Solution | TestHub

To determine the number of $p_{\pi }-d_{\pi }$ bonds, we analyze the central atom's hybridization and bonding.

1. SO₃: S is sp² hybridized, forming three $\sigma$ bonds and two $p_{\pi }-d_{\pi }$ bonds.

2. XeO₂F₂: Xe is sp³d hybridized, forming four $\sigma$ bonds and two $p_{\pi }-d_{\pi }$ bonds.

3. SOF₄: S is sp³d hybridized, forming five $\sigma$ bonds and one $p_{\pi }-d_{\pi }$ bond.

4. XeO₃: Xe is sp³ hybridized, forming three $\sigma$ bonds and three $p_{\pi }-d_{\pi }$ bonds.

5. XeO₄: Xe is sp³ hybridized, forming four $\sigma$ bonds and four $p_{\pi }-d_{\pi }$ bonds.

6. SO₂: S is sp² hybridized, forming two $\sigma$ bonds and one $p_{\pi }-d_{\pi }$ bonds.

7. SO₂Cl₂: S is sp³ hybridized, forming four $\sigma$ bonds and two $p_{\pi }-d_{\pi }$ bonds.

CO₂ does not have "d" orbital to form any $p_{\pi }-d_{\pi }$ bonds.