JEE Main · ChemistryHard

$Consider the molecule ClF_{3} . Which of the following statements correctly describes its geometry and the nature of its bonding according to VSEPR theory and hybridization?$

A. $The molecule is T-shaped with sp^{3} d hybridization and two lone pairs in the equatorial positions.$
B. $The molecule is trigonal planar with sp^{2} hybridization and one lone pair.$
C. $The molecule is T-shaped with sp^{3} d hybridization and two lone pairs in the axial positions.$
D. $The molecule is pyramidal with sp^{3} hybridization and one lone pair.$

Show correct answer & step-by-step solution

Correct answer: A — $The molecule is T-shaped with sp^{3} d hybridization and two lone pairs in the equatorial positions.$

Solution

$The central atom Cl has 7 valence electrons and forms 3 bonds with F atoms, leaving 2 lone pairs.$
$The steric number is $3 + 2 = 5$, corresponding to sp^{3} d hybridization.$
$According to Bent's rule and VSEPR, lone pairs occupy equatorial positions in a trigonal bipyramidal arrangement to minimize 9 0^{\circ} repulsions.$
$This results in aT-shaped molecular geometry.$
$Hence the answer is (A).$

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