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Dipole Moment - Overview, Definition, Formula, FAQs

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Dipole Moment - Overview, Definition, Formula, FAQs

Edited By Team Careers360 | Updated on Jun 27, 2022 03:30 PM IST

What is a Dipole?

In chemistry, a dipole is the separation of charges between two covalently linked atoms or atoms that share an ionic connection inside a molecule. A water molecule (H2O) is an example of a dipole.

What is Dipole Moment?

A dipole moment is the turning force a fixed charge has on a dipole in a molecule. The moment depends on the charge at the end of the dipole and its distance from the charge at the other end of the dipole.

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Bond Dipole Moment

Bond dipole moment can be used to measure the polarity of a chemical bond that present between 2 atoms in a molecule of a compound. It makes use of the concept of electric dipole moment, which is a measurement of the distance between negative and positive charges in a system. It has both magnitude and direction i.e., bond dipole moment can be used to say that it is a vector quantity. So, what is dipole moment in case of HCl? The answer can be seen from the figure below i.e., the dipole moment that occurs in an HCl (hydrochloric acid) molecule is, The letters ẟ+ and ẟ denote the two electric charges that originate in a molecule, which are equal in magnitude but have opposing signs. They are separated by a set distance, which is commonly symbolised by the letter 'd.'

From the points given below we can easily understand what is dipole moment.

  • The bond dipole moment is the dipole moment of a single bond in a polyatomic molecule, which is distinct from the molecule's overall dipole moment.

  • It's a vector quantity, which means it has both magnitude and defined directions.

  • It can also be 0 because the two oppositely acting bond dipoles can cancel each other out as a vector quantity.

  • A tiny arrow with its tail on the negative centre and its head on the positive centre is used to represent it.

  • The dipole moment is represented by a modified arrow sign. On the positive centre, there is a cross, and on the negative centre, there is an arrowhead. The change in electron density of the molecule is shown by this arrow.

Dipole moment formula

By the dipole moment definition, the dipole moment formula is the product of magnitude of charge and the distance between the positive and negative charge centres. The Greek letter “µ” stands for it.

Mathematically, dipole moment formula can be written as,

Dipole Moment=ChargeQ*Distance of separation(d)

-It is measured in Debye units, which are represented by the letter ‘D.'

1 D = 3.3356*10-30 Cm,

Where, C stands for Coulomb and m for metre.

In a chemical bond between two atoms with differing electronegativities, the bond dipole moment formula can be written as,

μ=δd

Where: μ → bond dipole moment,

? → magnitude of the partial charges ?+ and ?,

d → distance between ?+ and ?.

The bond dipole moment (µ) is a vector quantity with the same direction as the bond axis. The arrows used to illustrate dipole moments in chemistry start at the positive charge and stop at the negative charge.

When two atoms with different electronegativities collide, the electrons tend to migrate away from their original locations in order to approach the more electronegative atom. The bond dipole moment in chemistry can be used to depict the movement of electrons.

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Dipole Moment in Chemistry

  1. BeF2

The bond angle between the two beryllium-fluorine bonds in a beryllium fluoride molecule is 180o. Fluorine pushes the electron density towards itself since it is the more electronegative atom. Below is a diagram of the individual bond dipole moments of a BeF2 molecule.


Beryllium-Fluorine bonds

Because the two individual bond dipole moments in a BeF2 molecule are identical in magnitude but opposite in direction, they cancel each other out, as seen in the picture

  1. Dipole Moment of H2O

Because the oxygen atom is significantly more electronegative than the hydrogen atom, the electrons in a water molecule cluster around it. The existence of a lone pair of electrons in the oxygen atom, on the other hand, causes the water molecule to bend (as per the VSEPR theory). As a result, unlike in the BeF2 molecule, the individual bond dipole moments do not cancel each other out. The dipole moment of a H2O molecule is seen in the diagram below.


Dipole Water

A water molecule's bond angle is 104.5o. An oxygen-hydrogen bond has a 1.5 D individual bond moment. Therefore, the dipole moment of H2O is determined to be 1.84D.

  1. HCl

The dipole moment of the HCl molecule in the diatomic molecule is the same as the dipole moment of the HCl link, which is 1.03D.

HCL Molecule

  1. Carbon dioxide

The dipole moment of the triatomic CO2 (carbon dioxide) molecule is zero. The dipole moment of the C=O bond (2.3D) on one side of the molecule is negated by that on the opposite side of the molecule due to the linear structure of the molecule, resulting in net zero dipole moment.

CO2 (Carbon Dioxide)

  1. Boron Trihydride

The dipole moment of boron trihydride (BH3) is zero, whereas that of ammonia (NH3) is 1.49D. This is due to the fact that BH3 has a symmetrical structure, with the three B-H bonds arranged at a 120-degree angle to one another. Dipole moments cancel each other out in a single plane, resulting in a net dipole moment of zero.

Boron Trihydride

NCERT Chemistry Notes :

  1. Ammonia

The molecule ammonia (NH3) is polar. One nitrogen atom is covalently linked to three hydrogen atoms in ammonia. Because nitrogen attracts electrons more strongly than hydrogen, the electrons they share are attracted to nitrogen rather than hydrogen. This provides nitrogen a partial negative charge (shown by a minus sign on N) and hydrogen a partial positive charge (represented by a plus sign on H) (which is denoted by a plus sign on each H). Ammonia is polar due to the existence of both positive and negative charges on the molecule, and so has a net dipole moment. With three N-H bonds and a lone pair on the nitrogen atom, NH3 has a pyramidal structure. This yields a dipole moment of 1.49D as a consequence.

Ammonia

  1. BeF3 Dipole Moment

A molecule's dipole moment definition is a phrase that defines the two opposing charges within the molecule that are separated by a distance. The structure of the molecule BF3 can be drawn to get a sense of the BF3 dipole moment value contained in the molecule.


BF3 Dipole Moment

To begin, let's review the notion of dipole moment, which is a number that is measured in a molecule to determine the partial charges present between the two atoms or groups present in that molecule. The net dipole moment of a molecule is zero when two equal and opposing charges are present in the molecule. Therefore, the BF3 dipole moment is zero.

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Frequently Asked Question (FAQs)

1. What is the best method for determining the greatest dipole moment?

A dipole moment occurs when the electronegativity of two atoms engaged in a bond is different. The bond's dipole moment and polarity increase as the electronegativity gap between the two atoms grows.

2. What is the dipole moment's symbol and dipole moment definition?

The dipole moment (µ) is the result of multiplying the magnitude of the charge Q by the distance r between the charges to get the net molecular polarity at each end of the molecular dipole. The partition of charges in a molecule is represented by dipolar moments. As a result, this article briefly discusses the definition and formula of dipole moments.

3. Arrange the following compounds in the correct order of dipole moment.

H2O > NH3 > NF3 > BeF2 = CH4

i.e., the dipole moment of the compounds is H2O = 1084D, NH3 = 1.49D, 

NF3 =0.24D, BeF2 = CH4 = 0

4. What is permanent dipole moment?

Permanent Dipole Moments arise when the electronegativity of two atoms in a molecule differs significantly. The atom with the higher electronegativity will attract more electrons, resulting in a partial negative charge surrounding it and a partial positive charge around the atom with the lower electronegativity. Molecules possessing persistent dipole moments, as opposed to dipole moments generated by other molecules, are simply polar molecules. They're significant because a molecule's polarity influences many of its characteristics and interactions with other molecules.

5. Why BF3 dipole moment is zero?

Despite having three polar B—F bonds, BF3dipole moment is zero. Because BF3 has sp2 hybridisation and a regular trigonal planal shape, this is the case. As a result, the individual dipole moments of polar bonds cancel out, resulting in a zero overall dipole moment.

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