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:

Choose the correct option for the following molecule in view of chemical bonding:
$Cl-CH=C=C=CH-Cl$

If the $HCl$ molecule were completely polar,the expected dipole moment would be $6.12 \ D$,but the experimental value of the dipole moment is $1.03 \ D$. What is the percentage of ionic character (in $\%$)?

For which molecules among the following,the resultant dipole moment $(\mu) \neq 0?$

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:

If $HCl$ were purely ionic,its expected dipole moment would be $6.12 \, D$. However,the experimental dipole moment is $1.03 \, D$. Calculate the percentage ionic character. (in $\%$)