Question

Which of the following arrangements of molecules is correct on the basis of their dipole moments?
(A) $B{F_3} > N{F_3} > N{H_3}$
(B) $N{F_3} > B{F_3} > N{H_3}$
(C) $N{H_3} > B{F_3} > N{F_3}$
(D) $N{H_3} > N{F_3} > B{F_3}$

Answer 1

Hint: How far away two electrical charges are from one another is measured in terms of a dipole moment. Dipole moments are a type of vector. The direction is from negative charge to positive charge, and the magnitude is equal to the charge times the distance between the charges. The formula of the dipole moment is $p = qd$ .
Complete step by step solution:
As we discussed above some characteristics of Dipole moment, let we consider the correct arrangement for the molecules on the basis of their dipole moment,
We know that, In $N{H_3}$ , the charge from three bonds was delocalised in the direction of lone pairs, towards nitrogen.




 $N{F_3}$ has a greater dipole moment than $B{F_3}$ as a result of its pyramidal and trigonal planar structures. For $B{F_3}$ , there is no resulting dipole.

Therefore, from the above conclusion we get the correct sequence is $N{H_3} > N{F_3} > B{F_3}$ .
Hence, the correct option is (D).
Note: The dipole moment is helpful in determining how polar the chemical connection is: The bond becomes more polar as the size of the dipole moment grows. Non-polar molecules are those that have no dipole moment.