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What is Dipole Moment?, Application, Important Factor Of Dipole Moment

Dipole Moment Introduction  : Dipole moment, a crucial concept in chemistry, serves as a key indicator of the polarity of a molecule. It provides valuable insights into the distribution of charge within a molecular structure, influencing various physical and chemical properties. This article delves into the fundamental aspects of dipole moment and explores its wide-ranging applications in different scientific domains.
authorImageShrivastav 20 Dec, 2023
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Dipole Moment

What is Dipole Moment?

A dipole moment is a measure of the separation of positive and negative charges within a molecule. It arises when there is an asymmetrical distribution of electron density. And it leads to a permanent electric dipole.

In other words, it is the measure of overall polarity of a molecule. dipole moment-1 q = Charge on any one of the atom which is in order of 10 –10 esu or 10 –19 coloumb and d = Distance between charged atoms is in the order of 10 –8 cm.

10 –18 esu cm = 1 debye (unit of dipole moment)

In S. I. system 1 esu = dipole moment-2 1 cm = 10 –2 m 1D = 10 –18 × 3.33 × 10 –10 × 10 –2 cm 1D = 3.33 × 10 –30 cm
  • The degree of polarity of covalent bond is given by the dipole moment (μ)
  • It is the product of the either charge and the distance between them.
dipole moment-3 Electronegativity of A < Electronegativity of B
  • Dipole moment is a vector quantity.
  • The direction of dipole moment is represented by ↦

Important Factors Affecting Dipole Moment

  • Electronegativity difference between bonded atoms
  • Direction of bond dipole moment
  • Angle between various bonds
  • Influence of unshared e – pairs
  • Magnitude of polarity of the molecule
  • Symmetrical / Unsymmetrical shape.

Examples :

Dipole moment of H 2 O is 1.84 D which is resultant μ of two O–H bonds. μ of H 2 O > μ of H 2 S because electronegativity of oxygen is higher than sulphur.

Applications of Dipole Moment :

1. Determining the polarity and geometry of molecules.

  • If μ = 0 compound is nonpolar and symmetrical

Eg. CO 2 , BF 3 , CCl 4 , CH 4 , BeF 2 etc.

  • If μ ≠ 0 compound will be polar and unsymmetrical H 2 O, SO 2 , NH 3 , Cl 2 O, CH 3 Cl, CHCl 3 etc.
dipole moment-7

2. Calculation of ionic character

Percentage of ionic character dipole moment-8

Solved Example: Calculate the μ of HCl ? If bond distance is 1.34 Å, charge = 4.8 × 10 –10 esu and calculate % ionic character if experiment value of μ = 1.08 D ?

μ = q × d = 4.8 × 10 –10 × 1.34 × 10 –8 M = 6.432 × 10 –18 esu cm. % Ionic character = dipole moment-9

Some important orders of Dipole Moments:

H 2 O > HF > NH 3 > NF 3 (value based) H 2 O > H 2 S. CH 3 Cl > CH 3 F > CH 3 Br > CH 3 I BF 3 < NF 3 < NH 3 NO 2 – > NO 2 > NO 2 + H 2 O < H 2 O 2

Dipole Moment FAQs

1. Write the order of the dipole moment of following compounds? CH3Cl, CH2Cl2, CHCl3, CCl4

Sol. Right order is → CCl4 < CHCl3 < CH2Cl2 < CH3Cl μ = 0 1.021.55 1.93

Q.2. What is a dipole moment, and how is it defined in chemistry?

Ans. In chemistry, a dipole moment is a quantitative measure of the separation of positive and negative charges within a molecule. It is defined as the product of the charge and the distance between these charges, expressed as 

Q.3:  How does a dipole moment assist in determining the polarity of a molecule?

Ans. A molecule is considered polar if it possesses a dipole moment. The direction of the dipole moment indicates the orientation of charge separation. If there is an uneven distribution of electron density, the molecule is polar.

Q.4.  Can you provide an example of a polar molecule and elaborate on its dipole moment?

Ans. Water (H2O) is an exemplary polar molecule. The oxygen atom's higher electronegativity compared to the hydrogen atoms leads to an asymmetric distribution of electron density, resulting in a significant dipole moment.

Q.5:  How does the dipole moment contribute to the physical properties of substances, such as boiling points and melting points?

Ans. Dipole-dipole interactions, influenced by dipole moments, contribute to the strength of intermolecular forces. Substances with higher dipole moments generally have stronger intermolecular forces, impacting properties like boiling points,melting points, and solubility.
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