A molecule can be polar or nonpolar depending upon the nature of the bonds and t

Question

A molecule can be polar or nonpolar depending upon the nature of the bonds and the shape of the molecule For a molecule that has different outer atoms the molecular symmetry will decide the polarity. If the molecular geometry is such that the dipole moments of each polar bond cancel each other then the molecule is nonpolar. However, if the the molecular geometry is such that the dipole moments of each polar bond don't cancel each other then the molecule is polar. PF_3I_2 is a nonpolar molecule. Based on this information, determine the F-P-F bond angle, the I-P-I bond angle, and the F-P-I bond angle. Enter the number of degrees of the F-P-F, I-P-I, and F-P-I bond angles, separated by commas (e.g., 30, 45, 90) Which statement best describes the polarity of CH_2CI_2? The molecule is always polar. The molecule is always nonpolar. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar. Which statement best describes the polanty of SCI_4 F_2? The molecule is always polar. The molecule is always nonpolar. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.

Explanation / Answer

A)
It must be trigonal bipyramidal is shape with all 3 Fluorine in equatorial plane and 2 I in axial position

So,
FPF = 120 degree
IPI = 180 degree
FPI = 90 degree

B)
This will be having tetrahedral shape.
It will never attain symmetry and will always have dipole moment
So, the molecule is always polar

C)
It will have octahedral shape.
Dipole moment will be changing depending on position of atoms.
If symmetry is not there for particular arrangement, dipole moment can be non zero as well .
If atoms are rranged maintaining symmetry, dipole moment = 0
So,
depending on the arrangement of outer atoms, this molecule could be polar or non polar

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