The incorrect statement regarding `O(SiH_(3))_(2) and OCl_(2)` molecule is/are

Options

A. The strength of back bonding is more in `O(SiH_(3))_(2)` molecule than `Ocl_(2)` molecule
B. `Si-O-Si` bond angle in `O(SiH_(3))_(2)` is greater than `Cl-O-Cl` bond angle in `OCl_(2)`
C. The nature of back in both molecules is `2p_(x)-3d_(pi)`
D. Hybridisation of central O-atom in both molecules is same

Explanation

To determine the incorrect statement regarding the molecules OSiH₃₂ and OCl₂, we will analyze each option step by step.

### Step 1: Analyze Back Bonding Strength
- **Statement**: The strength of back bonding is more in OSiH₃₂ than in OCl₂.
- **Analysis**: In OSiH₃₂, the back bonding involves the 2P orbitals of oxygen and the 3D orbitals of silicon, which allows for effective overlap and stronger back bonding. In contrast, OCl₂ has less effective back bonding due to the larger size of chlorine atoms, which do not allow for effective overlap with the oxygen's orbitals.
- **Conclusion**: This statement is **correct**.

### Step 2: Compare Bond Angles
- **Statement**: The Si-O-Si bond angle in OSiH₃₂ is greater than the Cl-O-Cl bond angle in OCl₂.
- **Analysis**: The bond angle in OSiH₃₂ is approximately 144 degrees due to the presence of lone pairs and the hybridization of sp². In OCl₂, the bond angle is around 111 degrees due to sp³ hybridization and the repulsion between lone pairs.
- **Conclusion**: This statement is **correct**.

### Step 3: Nature of Back Bonding
- **Statement**: The nature of back bonding in both molecules is 2Pₓ 3D π.
- **Analysis**: In OSiH₃₂, the back bonding is indeed characterized by 2P and 3D orbitals. However, in OCl₂, the back bonding is less effective and does not involve significant 3D orbital participation.
- **Conclusion**: This statement is **correct**.

### Step 4: Hybridization of Central Oxygen Atoms
- **Statement**: The hybridization of central O atoms in both molecules is the same.
- **Analysis**: In OSiH₃₂, the oxygen atom undergoes sp² hybridization due to the presence of one lone pair and the formation of sigma bonds with silicon. In OCl₂, the oxygen atom is sp³ hybridized due to two lone pairs and two sigma bonds with chlorine.
- **Conclusion**: This statement is **incorrect**.

### Final Conclusion
The incorrect statement regarding OSiH₃₂ and OCl₂ is the fourth statement: "The hybridization of central O atoms in both molecules is the same."

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