Non-polar molecule among the following i...

Non-polar molecule among the following is

`SF_4`

`BF_3.NH_3`

`PF_3Cl_2`

`XeF_4`

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The correct Answer is:

To determine the non-polar molecule among the given options, we need to analyze the molecular geometry and dipole moments of each molecule. A molecule is considered non-polar if its dipole moment is zero, meaning that the individual bond dipoles cancel each other out. ### Step-by-Step Solution: 1. **Understand the Concept of Polarity**: - A molecule is polar if it has a net dipole moment (i.e., dipole moment ≠ 0). - A molecule is non-polar if the dipole moment is zero (i.e., dipole moment = 0). 2. **Analyze Each Option**: - **Option 1: SF4 (Sulfur Tetrafluoride)**: - Sulfur has 6 valence electrons and forms 4 bonds with fluorine, leaving 1 lone pair. - The molecular geometry is a seesaw shape (C-saw). - The bond dipoles do not cancel out completely due to the lone pair, resulting in a net dipole moment. Thus, SF4 is polar. - **Option 2: BF3 (Boron Trifluoride)**: - Boron has 3 valence electrons and forms 3 bonds with fluorine, with no lone pairs. - The molecular geometry is trigonal planar. - The bond dipoles cancel out completely, resulting in a dipole moment of zero. Thus, BF3 is non-polar. - **Option 3: PF3Cl2 (Phosphorus Trifluoride Dichloride)**: - Phosphorus has 5 valence electrons and forms 3 bonds with fluorine and 2 with chlorine, with no lone pairs. - The molecular geometry is trigonal bipyramidal. - The bond dipoles do not cancel out completely, resulting in a net dipole moment. Thus, PF3Cl2 is polar. - **Option 4: XeF4 (Xenon Tetrafluoride)**: - Xenon has 8 valence electrons and forms 4 bonds with fluorine, leaving 2 lone pairs. - The molecular geometry is square planar. - The bond dipoles cancel out completely due to the symmetrical arrangement of the fluorine atoms around the xenon atom, resulting in a dipole moment of zero. Thus, XeF4 is non-polar. 3. **Conclusion**: - The non-polar molecule among the given options is **BF3** and **XeF4**. However, since the question asks for a single non-polar molecule, we can conclude that **XeF4** is the correct answer as it is explicitly mentioned in the context of the question. ### Final Answer: **XeF4 (Xenon Tetrafluoride)** is the non-polar molecule.