Question

Which molecule has zero dipole moment in the following:

• A. ${\mathrm{CH}}_2{\mathrm{CI}}_2$
• B. ${\mathrm{BF}}_3$
• C. ${\mathrm{NF}}_3$
• D. ${\mathrm{CIO}}_2$

Answer 1

The correct option is B

${\mathrm{BF}}_3$

The explanation for the correct option:

(B) ${\mathrm{BF}}_3$

• Boron trifluoride has zero dipole moment although it has three polar $\mathrm{B}—\mathrm{F}$ bonds.
• ${\mathrm{BF}}_3$ has ${\mathrm{sp}}^2$ hybridization and regular trigonal planar geometry.
• When there is a charge separation in a system, a dipole moment develops.
• Dipole moments are produced by the disparity in electronegativity between two atoms that are bonded chemically.

The explanation for the incorrect options:

(A) ${\mathrm{CH}}_2{\mathrm{CI}}_2$

• With the chemical formula${\mathrm{CH}}_2{\mathrm{CI}}_2$, dichloromethane is an organochlorine compound.
• This colorless, flammable liquid, which has a pleasant, chloroform-like aroma, is frequently employed as a solvent.
• It is polar and miscible with a variety of organic solvents despite not being miscible with water.
• The dipole moment of ${\mathrm{CH}}_2{\mathrm{CI}}_2$ is $1.62\mathrm{D}$.

(C) ${\mathrm{NF}}_3$

• Nitrogen trifluoride $\left({\mathrm{NF}}_3\right)$ is an inorganic gas that has a faint musty smell and is colorless, nonflammable, and poisonous.
• It is increasingly used in the production of LEDs, photovoltaics, flat-panel displays, and other microelectronics.
• The dipole moment of ${\mathrm{NF}}_3$ is $0.24\mathrm{D}$.

(D) ${\mathrm{CIO}}_2$

• Chlorine dioxide $\left({\mathrm{CIO}}_2\right)$may be found as a brilliant orange crystal below$-59°C$.
• It exists as a reddish-brown liquid between $11°C$ and $-59°C$ and a yellowish-green gas above$11°C$.
• The Dipole moment of ${\mathrm{CIO}}_2$ is $1.792\mathrm{D}$.

Hence, the correct option is (B) ${\mathrm{BF}}_3$.