Solved: CHEMISTRY Question for NEET

NEET CHEMISTRYMedium

Which of the following is a polar molecule?

SF₄

SiF₄

XeF₄

BF₃

Analyze $BF_3$ : Boron has 3 valence electrons and forms 3 bonds. The molecule is Trigonal Planar and symmetrical. The bond dipoles cancel out ( $\\mu = 0$ ). Non-polar.
Analyze $SiF_4$ : Silicon has 4 valence electrons and forms 4 bonds. The molecule is Tetrahedral and symmetrical. The bond dipoles cancel out ( $\\mu = 0$ ). Non-polar.
Analyze $XeF_4$ : Xenon has 8 valence electrons. It forms 4 bonds and has 2 lone pairs. The geometry is Square Planar (lone pairs are at $180^\\circ$ ). The symmetry causes bond dipoles to cancel ( $\\mu = 0$ ). Non-polar.
Analyze $SF_4$ : Sulfur has 6 valence electrons. It forms 4 bonds with Fluorine, leaving 1 lone pair. The electron geometry is trigonal bipyramidal, and the molecular shape is See-Saw (asymmetrical). The dipole moments do not cancel ( $\\mu \\neq 0$ ). It is polar.

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