The electric potential on the axis of an electric dipole at a distance'r from it's centre is V. Then the potential at a point at the samedistance on its equa.

On the other hand, in case of CH2Cl2, the resultant of the dipole moments of two C-Cl bonds is strengthened by the resultant of the dipole moments of two C-H bonds. As a result, CH2Cl2 has a higher dipole moment of 1.60 D than CHCl3 i.e., CH2Cl2 has the highest dipole moment. Hence, the given compounds can be arranged in the increasing order of.

In molecular geometries that are highly symmetrical (most notably tetrahedral and square planar, trigonal bipyramidal, and octahedral), individual bond dipole moments completely cancel, and there is no net dipole moment. Although a molecule like CHCl 3 is best described as tetrahedral, the atoms bonded to carbon are not identical.

Best answer CCl4 is a symmetrical molecule. Therefore, the dipole moments of all four C-Cl bonds cancel each other. Hence its resultant dipole moment is zero. As shown in the above figure, in CHCl3, the resultant dipole moments of two C-Cl bonds is opposed by the resultant dipole moments of one C-H and one C-Cl bond.

The dipole moment of a molecule is therefore the vector sum of the dipole moments of the individual bonds in the molecule. If the individual bond dipole moments cancel one another, there is no net dipole moment. Such is the case for CO 2, a linear molecule (Figure 1.7.1a ).

Updated on: 26/04/2023 Give reasons : The dipole moment of chlorobenzene is lower than that of cyclohexyl chloride. ADVERTISEMENT Text Solution Verified by Experts Chlorine is more electronegative than carbon. This creates a positive charge on carbon linked to Cl in cyclohexyl chloride.

∈ 0 = Absolute electric permittivity of free space. In the given case, cube encloses an electric dipole. Therefore, the total charge enclosed by the cube is zero, i.e. Q = 0. Therefore, from (i), we have `phi_E=ointvecE.vec(ds)=0/epsilon_0=0`