The dipole moment of chlorobenzene is 1.5 D. | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) The dipole moment of a molecule is the vector sum of the individual bond dipoles. For chlorobenzene, the dipole moment is $1.5 \ D$. Let the dipol

Vedclass · Accepted Answer

$2.54$

Vedclass · Answer

(C) The dipole moment of a molecule is the vector sum of the individual bond dipoles. For chlorobenzene, the dipole moment is $1.5 \ D$. Let the dipole moment of a $C-Cl$ bond be $\mu$. For $o-$dichlorobenzene, the two $C-Cl$ bonds are at an angle of $60^{\circ}$ to each other. The resultant dipole moment is given by $\mu_{net} = \sqrt{\mu^2 + \mu^2 + 2\mu^2 \cos(60^{\circ})}$. Since $\cos(60^{\circ}) = 0.5$, we have $\mu_{net} = \sqrt{2\mu^2 + 2\mu^2(0.5)} = \sqrt{3\mu^2} = \mu \sqrt{3}$. Given $\mu = 1.5 \ D$, the dipole moment of $o-$dichlorobenzene is $1.5 	imes 1.732 \approx 2.54 \ D$.

The dipole moment of chlorobenzene is $1.5 \ D$. The dipole moment of $o-$dichlorobenzene is (in $D$)

Similar Questions

Which molecule does not show zero dipole moment?

Which of the following statements is correct?

Which molecule has a zero dipole moment?

The cyanide ion $(CN^{-})$ and $N_2$ are isoelectronic. However,in contrast to $CN^{-}$,the $N_2$ molecule is chemically inert due to:

Which of the following diagrams shows the correct change in the polarity of the bond?

Vedclass Test Series

Exam Paper Generator

Online Exam Module