Question

The resultant dipole moment $\mu$ of two compound of NOF and $N{O}_{2}F$ is 1.81 D and 0.47 D respectively.Which dipole moment do you predict?

• A. 1.81 D for $N{O}_{2}F$ and 0.47 D for NOF
• B. 0.47 D for $N{O}_{2}F$ and 1.81 D for NOF
• C. For both $N{O}_{2}F$ and NOF, dipole moment $\left(\mu \right)$ is 1.81D
• D. For both $N{O}_{2}F$ and NOF. Dipole moment $\left(\mu \right)$ is 0.47 D

Answer 1

The correct option is B 0.47 D for $N{O}_{2}F$ and 1.81 D for NOF

$NOF$ has bent shape and $N{O}_{2}F$ has trigonal planar shape with asymmetrical distribution of charge on central atom. The dipole moment in case of $N{O}_{2}F$ is less than $NOF$ due to its symmetrical shape. Hence, dipole moment of $N{O}_{2}F$ should be 0.47 D and that of $NOF$ should be 1.81 D.