Question

In a polar nitrogen trifluoride, NF3 molecule, nitrogen and fluorine atoms share electrons. The fluorine atoms have a stronger attraction for electrons than the nitrogen atom has. What can be determined from the molecule's polarity?

A. It has polar bonds and is symmetric.
B. It has ionic bonds and is symmetric.
C. It has polar bonds and is asymmetric.
D. It has nonpolar bonds and is asymmetric.

Answer 1

Option C

In
`NF_(3)` molecule, nitrogen has 5 valence electrons and F has 7 valence electron, 3 electrons of nitrogen are shared with 3 Fluorine atoms and 2 electrons are left on nitrogen atom as lone-pair.

The structure of
`NF_(3)` will be pyramidal.

Fluorine is more electronegative than nitrogen, due to this high electronegativity difference the N-F bond is polar in nature. There is net dipole moment in
`NF_(3)` molecule thus, it is asymmetric in nature.

The structure of
`NF_(3)` is in the attached file.

Therefore, it has polar bonds and it is asymmetric.