Question

question 6 (5 points)
listen
the compound f₂o has two lone pairs on the central oxygen atom. whats the structure of an f₂o molecule? is this compound polar or non - polar?
a) trigonal planar, polar
b) bent or angular, non - polar
c) trigonal planar, non - polar
d) bent or angular, polar

Explanation:

1. Determine Molecular Geometry: For \( \ce{F2O} \), the central atom (O) has 2 bonding pairs (with F atoms) and 2 lone pairs. Using VSEPR theory, the electron - pair geometry is tetrahedral, but the molecular geometry (considering only bonding pairs and lone pairs' effect on shape) is bent (angular). Trigonal planar geometry would require 3 bonding pairs (or a combination that gives a planar, triangular arrangement), which is not the case here.
2. Determine Polarity: The \( \ce{O - F} \) bonds are polar (since F is more electronegative than O). The bent molecular geometry means that the dipole moments of the two \( \ce{O - F} \) bonds do not cancel each other out. In a non - polar molecule, the symmetry of the molecule causes the dipole moments of the bonds to cancel. Since the \( \ce{F2O} \) molecule is bent, the overall molecule has a net dipole moment, so it is polar.

Answer:

D) Bent or angular, polar