Which of the folowing set of molecules have same shape but different hybridisation ?

Options

A. `XeO_(4), SF_(4)`
B. `XeO_(3), BrF_(3)`
C. `H_(2)O, SnCl_(2)`
D. `I_(3)^(-), I_(3)^(+)`

Answer

To determine which of the following sets of molecules have the same shape but different hybridization, we will analyze the hybridization and molecular geometry of each molecule step by step.

### Step 1: Analyze the first set of molecules (XeF4 and SF4)
1. **XeF4 (Xenon Tetrafluoride)**
- Central atom: Xenon (Xe)
- Valence electrons of Xe: 8
- Number of monovalent atoms (F): 4
- Total: 8 (valence electrons) + 0 (monovalent atoms) = 8
- Hybridization: \( \text{sp}^3\text{d}^2 \) (since we have 6 regions of electron density)
- Lone pairs: 2 (8 - 4 bond pairs = 4)
- Shape: Square planar

2. **SF4 (Sulfur Tetrafluoride)**
- Central atom: Sulfur (S)
- Valence electrons of S: 6
- Number of monovalent atoms (F): 4
- Total: 6 + 4 = 10
- Hybridization: \( \text{sp}^3\text{d} \) (5 regions of electron density)
- Lone pairs: 1 (5 - 4 bond pairs = 1)
- Shape: Seesaw

**Conclusion**: Different shapes, so this set does not qualify.

### Step 2: Analyze the second set of molecules (XeO3 and BrF3)
1. **XeO3 (Xenon Trioxide)**
- Central atom: Xenon (Xe)
- Valence electrons of Xe: 8
- Number of monovalent atoms (O): 3
- Total: 8 + 0 = 8
- Hybridization: \( \text{sp}^3 \) (4 regions of electron density)
- Lone pairs: 1 (4 - 3 bond pairs = 1)
- Shape: Pyramidal

2. **BrF3 (Bromine Trifluoride)**
- Central atom: Bromine (Br)
- Valence electrons of Br: 7
- Number of monovalent atoms (F): 3
- Total: 7 + 3 = 10
- Hybridization: \( \text{sp}^3\text{d} \) (5 regions of electron density)
- Lone pairs: 2 (5 - 3 bond pairs = 2)
- Shape: T-shaped

**Conclusion**: Different shapes, so this set does not qualify.

### Step 3: Analyze the third set of molecules (H2O and SnCl2)
1. **H2O (Water)**
- Central atom: Oxygen (O)
- Valence electrons of O: 6
- Number of monovalent atoms (H): 2
- Total: 6 + 0 = 6
- Hybridization: \( \text{sp}^3 \) (4 regions of electron density)
- Lone pairs: 2 (4 - 2 bond pairs = 2)
- Shape: Bent

2. **SnCl2 (Tin(II) Chloride)**
- Central atom: Tin (Sn)
- Valence electrons of Sn: 4
- Number of monovalent atoms (Cl): 2
- Total: 4 + 0 = 4
- Hybridization: \( \text{sp}^2 \) (3 regions of electron density)
- Lone pairs: 1 (3 - 2 bond pairs = 1)
- Shape: Bent

**Conclusion**: Both have the same shape (bent) but different hybridization (sp3 for H2O and sp2 for SnCl2).

### Final Answer:
The set of molecules that have the same shape but different hybridization is **H2O and SnCl2**.