If $Q$ is the magnitude of charge and $r$ is the distance between the centres of positive and negative charges,then the dipole moment $(\mu)$ is given by:

Consider the following:
Assertion $(A)$: Dipole moment of $NF_3$ is lesser than $NH_3$.
Reason $(R)$: In $NF_3$,the orbital dipole due to lone pair of electrons is in the opposite direction to the resultant dipole moment of the three $N-F$ bonds.
The correct answer is:

The bond length of $HCl$ molecule is $1.275 \ \text{Å}$ and its dipole moment is $1.03 \ \text{D}$. The ionic character of the molecule (in percent) (charge of the electron $= 4.8 \times 10^{-10} \ \text{esu}$) is

Among the following,the molecule with the highest dipole moment is

Give the correct order of initials $T$ or $F$ for the following statements. Use $T$ if the statement is true and $F$ if it is false.
$I. \, (CH_3)_2P(CF_3)_3$ is non-polar and $(CH_3)_3P(CF_3)_2$ is a polar molecule.
$II. \, CH_3 \widehat{P} CH_3$ bond angles are equal in the $(CH_3)_3P(CF_3)_2$ molecule.
$III. \, PF_3$ will be more soluble in a polar solvent than $SiF_4$.

For which of the following molecules is the dipole moment $\mu \ne 0$?