Which of the following molecules has a zero d | vedclass

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(B) The dipole moment of a molecule is zero if the vector sum of the individual bond dipoles is zero. This typically occurs in symmetric molecules whe

Vedclass · Accepted Answer

$1,4-$dichlorobenzene

Vedclass · Answer

(B) The dipole moment of a molecule is zero if the vector sum of the individual bond dipoles is zero. This typically occurs in symmetric molecules where the bond dipoles cancel each other out.$1.$ In $1,4$-dihydroxybenzene,the two $-OH$ groups are at the para positions. Due to the rotation of the $-OH$ groups,the bond dipoles do not perfectly cancel out,resulting in a non-zero dipole moment.$2.$ In $1,4$-dichlorobenzene,the two $C-Cl$ bonds are at $180^{\circ}$ to each other. Since the $C-Cl$ bond dipoles are equal in magnitude and opposite in direction,they cancel each other out,resulting in a net dipole moment of zero.$3.$ In $4$-nitrophenol,the $-OH$ and $-NO_2$ groups are at the para positions. Since these groups have different electronic effects and different bond dipole magnitudes,they do not cancel out,resulting in a non-zero dipole moment.Therefore,only $1,4$-dichlorobenzene has a zero dipole moment.

Which of the following molecules has a zero dipole moment?

Similar Questions

The correct set of species with zero dipole moment is:
$(i) \, CO_2, \, (ii) \, COCl_2, \, (iii) \, CH_2Cl_2, \, (iv) \, BCl_3$

Dipole moment of $HCl = 1.03 \ D$,$HI = 0.38 \ D$. Bond length of $HCl = 1.3 \ \mathring{A}$ and $HI = 1.6 \ \mathring{A}$. The ratio of the fraction of electric charge,$\delta$,existing on each atom in $HCl$ and $HI$ is

$(a)$ Discuss the significance/applications of dipole moment.
$(b)$ Represent diagrammatically the bond moments and the resultant dipole moment in $CO_2, NF_3$ and $CHCl_3$.

Which molecule is polar?

Which one of the following arrangements of molecules is correct on the basis of their dipole moments?

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