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Which of the following is a polar molecule?
(A)- BF3
(B)- SF4
(C)- SiF4
(D)- XeF4

Answer
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Hint:. Those molecules whose dipole moment is not zero is polar in nature and whenever distortion of shape takes place from original geometry, non – planar structure and presence of unbalanced electronic structure is observed then there polarity is also present.

Complete step by step answer:
Here is the complete explanation of above given molecules:
-In option (A) BF3 is given, in which three bond pair of electrons are present and hybridization of central atom i.e. Boron is sp2 whose structure is trigonal planar and due to which its dipole moment is zero. So, BF3 is a non - polar molecule.
-In option (B) SF4 is given, in which four bond pair of electrons and one lone pair of electrons are present and hybridization of central atom i.e. Sulphur is sp3d whose structure is like see -saw and due to distorted structure its dipole moment is not zero. So, SF4 is a polar molecule.
-In option (C) SiF4 is given, in which four bond pair of electrons are present and hybridization of central atom i.e. Silicon is sp3 whose structure is tetrahedral and due to regular geometry its dipole moment is zero. So, SiF4 is a non - polar molecule.
-In option (D) XeF4 is given, in which four bond pair of electrons & two lone pair of electrons are present and hybridization of central atom i.e. Xenon is sp3d2 whose structure is square planar and due to planar structure its dipole moment is zero. So, XeF4 is a non - polar molecule.
So, the correct answer is “Option B”.

Note: Here some of you may think that XeF4 is also polar in nature because it is showing different structure (square planar) from the geometry (octahedral), but here structure is also planar that’s why it is non – polar.