What is the dipole moment $(\mu)$ of a bond? Explain with an example.

(N/A) Polar bonding: As a result of polarization,a molecule possesses a dipole moment.
Definition: The dipole moment is defined as the product of the magnitude of the charge $(Q)$ and the distance $(r)$ between the centers of positive and negative charge.
Mathematical expression: $\mu = Q \times r$
Where:
$Q = \text{magnitude of charge on the atom in Coulomb (C)}$
$r = \text{distance between the centers in meters (m)}$
$\mu = \text{dipole moment in Debye (D) units}$
Conversion factor: $1 \ D = 3.33564 \times 10^{-30} \ C \ m$
Representation: Dipole moment is a vector quantity. By convention,it is depicted by an arrow $(\rightarrow)$ pointing from the positive center to the negative center. In chemistry,it is represented by a crossed arrow $(\mapsto)$ placed on the Lewis structure of the molecule,where the cross is on the positive end and the arrowhead is on the negative end.
Example: For the $HF$ molecule,the dipole moment is represented as:
$H^{\delta+} - F^{\delta-} \quad \text{or} \quad H \xrightarrow{\quad} \ddot{F}:$