Question

Which of the following molecules has a non-dipole moment?

• A. ${\mathrm{NH}}_4^{+}$
• B. ${\mathrm{PCl}}_5$
• C. ${\mathrm{BrF}}_3$
• D. ${\mathrm{XeO}}_3{\mathrm{F}}_2$

Answer 1

The correct option is C

${\mathrm{BrF}}_3$

The explanation for the Correct option

(C) Bromine trifluoride (${\mathrm{BrF}}_3$) possesses a non-dipole moment .

The electronegativity gap between bromine and fluorine atoms assures polarity across the Br-F bond in this molecule, which comprises three fluorine atoms encircling one bromine atom. The polar bond's dipole moment is never zero.

The explanation for the incorrect options

${\mathrm{NH}}_4^{+}$, ${\mathrm{PCl}}_5$, ${\mathrm{XeO}}_3{\mathrm{F}}_2$all are showing zero dipole moment.