Final answer:
FCIO₂ has a bent molecular geometry due to lone pair repulsion, and its dipole points towards the oxygen atoms. F₂ClO₂⁻ has a T-shaped molecular geometry with a dipole pointing towards the unbonded oxygen atom. Both have polar bonds, but the overall dipole moment depends on the geometry and bond dipoles. The correct answer is option a) | FCIO₂ | Tetrahedral, Bent
| F₂ClO₂⁻ | Trigonal Bipyramidal, Linear
Step-by-step explanation:
The molecular geometry of FCIO₂ can be predicted as tetrahedral due to the presence of four areas of electron density around the central chlorine atom (two oxygen atoms, one fluorine atom, and one lone pair). However, the lone pair's repulsion causes the shape to distort into a bent or angular geometry. On the other hand, the molecular geometry of F₂ClO₂⁻ is based on a trigonal bipyramidal electron pair geometry, but the presence of a lone pair of electrons on the central chlorine atom distorts it into a T-shaped molecular geometry.
Sketches for these molecules would show FCIO₂ with an overall dipole moment pointing from chlorine towards the more electronegative oxygen atoms, while in F₂ClO₂⁻, the dipole moment would point from the chlorine atom towards the single unbonded oxygen atom, as it is more electronegative than fluorine atoms. It's crucial to note that although all the mentioned compounds contain polar bonds, not all of them will have a net dipole moment; this will depend on the geometry and the distribution of the individual bond dipoles.