In which of the following both are nonpolar -

Options

A. `XeF_(4),O_(3)`
B. `XeF_(5)^(-),I_(2)Cl_(6)`
C. `SF_(4),XeF_(2)`
D. `BrF_(3),SCl_(2)`

Answer

To determine which of the given molecules are nonpolar, we need to analyze the molecular geometry and the dipole moments of each molecule. A molecule is considered nonpolar if the dipole moments cancel out, resulting in a net dipole moment of zero. Here’s a step-by-step solution:

### Step 1: Analyze XeF4
- **Molecular Geometry**: Xenon tetrafluoride (XeF4) has a square planar structure.
- **Dipole Moments**: The individual dipole moments from the Xe-F bonds will point towards the fluorine atoms. However, due to the symmetry of the square planar shape, these dipole moments cancel each other out.
- **Conclusion**: The dipole moment of XeF4 is zero, making it nonpolar.

### Step 2: Analyze O3 (Ozone)
- **Molecular Geometry**: Ozone has a bent shape.
- **Dipole Moments**: The dipole moments do not cancel out due to the bent geometry and the difference in electronegativity between the oxygen atoms.
- **Conclusion**: O3 has a net dipole moment, making it polar.

### Step 3: Analyze XeF5^-
- **Molecular Geometry**: Xenon pentafluoride ion (XeF5^-) has a square pyramidal structure.
- **Dipole Moments**: The dipole moments from the Xe-F bonds and the lone pairs do not cancel out due to the asymmetry of the structure.
- **Conclusion**: XeF5^- is polar.

### Step 4: Analyze I2Cl6
- **Molecular Geometry**: I2Cl6 is a dimer of ICl3 and has a non-planar structure.
- **Dipole Moments**: The molecule is symmetric and the dipole moments from the I-Cl bonds cancel out.
- **Conclusion**: I2Cl6 has a net dipole moment of zero, making it nonpolar.

### Step 5: Analyze SF4
- **Molecular Geometry**: Sulfur tetrafluoride (SF4) has a see-saw shape.
- **Dipole Moments**: The dipole moments do not cancel out due to the asymmetry of the molecule.
- **Conclusion**: SF4 is polar.

### Step 6: Analyze XeF2
- **Molecular Geometry**: Xenon difluoride (XeF2) has a linear structure.
- **Dipole Moments**: The dipole moments from the Xe-F bonds cancel out due to the linear geometry.
- **Conclusion**: XeF2 is nonpolar.

### Step 7: Analyze BrF3
- **Molecular Geometry**: Bromine trifluoride (BrF3) has a T-shaped structure.
- **Dipole Moments**: The dipole moments do not cancel out due to the asymmetry of the molecule.
- **Conclusion**: BrF3 is polar.

### Step 8: Analyze SCl2
- **Molecular Geometry**: Sulfur dichloride (SCl2) has a bent shape.
- **Dipole Moments**: The dipole moments do not cancel out due to the bent geometry.
- **Conclusion**: SCl2 is polar.

### Final Answer
The molecules that are nonpolar from the given options are **XeF4** and **I2Cl6**.

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