The bond angles in SF₅⁺ are expected to be A) 90^$\circ$. B) 120^$\circ$. C) 90^$\circ$ and 120^$\circ$. D) 90^$\circ$ and 180^$\circ$. E) 90^$\circ$, 120^$\circ$, and 180^$\circ$.

Question

Quizplus · Accepted Answer

The molecule SF₅⁺ has a trigonal bipyramidal geometry. The central sulfur atom (S1) is bonded to three fluorine atoms (F1) in a plane with 120° bond angles (equatorial position) and two axial positions (U1), one of which is occupied by a sulfur atom (S2) and the other by a phosphorus atom (P1) and a lone pair of electrons (S1). The lone pair on sulfur (S1) occupies an equatorial position in a plane perpendicular to the plane of the three fluorine atoms. Therefore, the expected bond angles are as follows: - F1-S1-F1: 90° (lone pair on S1 repels the bonding pairs) - F1-S1-S2: 120° (trigonal planar arrangement of F-S-F at equatorial positions) - F1-S1-P1: 120° (trigonal planar arrangement of F-S-F at equatorial positions) - S2-S1-P1: 180° (linear arrangement of axial atoms)

The Bond Angles in SF5+ Are Expected to Be A) ∘\circ∘

The Bond Angles in SF₅⁺ Are Expected to Be
A) $\circ$