Question

Which of the following has zero dipole moment ?
A. $B{F_3}$
B. $BeClBr$
C. $C{H_2}C{l_2}$
D. $COS$

Answer 1

Dipole moment is defined as the product of the magnitude of the charge and the distance between the centre of positive and negative charges. Dipole moment is a measure of the polarity of a molecule .

Complete step by step answer:
Dipole moments arise from electronegativity differences .
it is denoted by $\mu$
$\mu = q \times r$
where , q=magnitude of charge
and r= distance between charges
In the case of polyatomic molecules, $\mu$ not only depends upon the individual dipole moments of the bonds but also on the spatial arrangement of various bonds in the molecule.
When all the bonds in a molecule are oriented in such a way that they totally cancel each other's effects then the dipole moment is said to be zero.
In case of BF3,

As we can see , the molecule has a trigonal planar shape
That is, the bonds are oriented at an angle of ${120^ \circ }$ such that the resultant dipole due to two $B - F$ bonds cancel the third bond dipole and so the net dipole moment becomes zero.
In all the other molecules given in the options , the bonds are so arranged that the net dipole moment is not equal to zero

So, the correct answer is Option A .

Note:
Dipole moment is used to calculate the polarity of the bonds . The dipole moment of a molecule depends on two things: the individual dipole moment of each bond and the arrangement of the molecules .