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Q.
The correct sequence of dipole moments among the chlorides of methane is
Chemical Bonding and Molecular Structure
Solution:
$\mu_{CCl_4} = 0$
The resultant dipole moment of three $C -H$ bonds $= 0.4\,D$.
Net dipole moment $= 1.9 \,D$
The resultant of two $C -H$ bonds
$=\sqrt{\left(0.4\right)^{2}+\left(0.4\right)^{2}+2 \times\left(0.4\right)^{2} \times cos \,109.5^{\circ}} $
$=\sqrt{0.16 + 0.16 -0.2873} = 0.18 D$
The resultant of two $C - Cl$ bonds
$=\sqrt{\left(1.5\right)^{2}+\left(1.5\right)^{2}+2\times\left(1.5\right)^{2} cos \,109.5^{\circ}} $
$=\sqrt{2.25+2.25 + 2\times2.25 \times cos \,109.5^{\circ}} $
$=\sqrt{4.5 - 4.04} $
$ =\sqrt{0.46} = 0.678$
$\therefore \mu_{cal} = 0.858\,D$ but experimentally for
$CH_2Cl_2, \mu = 1.59\, D$.
The resultant of three $C - Cl$ bonds $= 1.5 \,D$
Experimental dipole moment of $CHCl_3 = 1.15 \,D$
