Answer to Question #69898 in Physical Chemistry for Puneet

Question

Explain the term dipole moment and describe briefly its experimental determination.

Answer 1

The dipole moment is an intermolecular force between atoms in the same or another kind of molecule. This helps us understand the interaction between the atoms of molecules.
The dipole moment is a measure of the total molecular polarity, which is the magnitude of the charge q at both ends of the dipole molecule and the distance between these charges, represented by d. The dipole moment is denoted by μ.
Thus: μ = q ∙ d
A dipole moment is a force that explains the separation of a charge in an atom or molecule.
A dipole moment can be defined as the product of the charge value and the distance between the centers of positive and negative charges, usually by means of a cross-sectional arrow, imposed on the Lewis structure of the molecules transverse to the positive end, the arrow head is on and the negative end. this arrow symbolizes the direction of the displacement of the electron density in the molecule, we note that the direction of the crossed arrow is opposite to the traditional direction of the vector of the dipole moment.
In the case of polyatomic molecules, the dipole moment depends not only on the individual dipole moment of the bonds, but also on the spatial arrangement of various bonds in the molecule; in this case, the dipole moment of the molecule is the vector amount of various dipole moments.