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Can anyone share some quality theory of dipole moment? need it asap. ty :)?
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In a polar molecule, there are two poles present in the molecule.Hence, the molecule is said to possess an electric dipole.Since the molecule as a whole is electrically neutral ,the negative charges is always equal in magnitude to the positive charge.

The product of magnitude of negative or positive charge(q) and the distance between the centres of the positive and negative charges is called dipole moment.

It is usually donated by µ.

It can be expressed as µ = q × d

The charge q is of the order of 10-10 esu and the internuclear distance d is of the order of 10-8 cm.

Therefore ,the dipole moment is of order 10 -18 esu cm.


In S.I. units, 1 D = 3.335 × 10 -30 C m

Dipole moment and molecular structure

Diatomic molecules

Dipole moment is a vector quantity i.e. it has magnitude as well as direction.

As a polar diatomic molecule possesses only one polar bond, the dipole moment of that molecule is equal to the dipole moment of the polar Bond.

In HCl, the molecular dipole moment is equal to the dipole moment of H-Cl bond i.e 1.07 D.

Greater the electronegativity difference between the bonded atom, greater if the dipole moment. Dipole moment of hydrogen halides are in the order :

H-F > H-Cl > H-Br > H-I

Polyatomic molecules

As a polyatomic molecule has more than one polar bond ,the dipole moment is equal to the resultant dipole moment of all the individual bonds.

The magnitude of resultant dipole moment not only depends upon the values of the individual dipole moment of the bonds but also on their arrangement in space.


Dipole moment of water is 1.84 D which is equal to the resultant dipole moment of two O-H bonds.

Dipole Moments - Class 11

In case of ammonia ,the dipole moment of molecule i.e. 1.47 D is the resultant of the dipole moment of the individual dipole moments of N-H bonds.

In carbon dioxide molecule, there are two polar bonds. These polar bonds possesses the same value of dipole moment but the overall dipole moment of molecule is found to be zero. Individual dipole moment in this molecule are of equal magnitude but their directions are opposite to each and hence cancel out.

Dipole Moments - Class 11

In symmetrical molecules like Boron trifluoride ( BF3)  Methane ( CH4)  and carbon tetrachloride (CCl4),  the molecular dipole moment is found to be zero. Individual dipole moments cancel out on account of the symmetry of the molecule. In BF3 ,the resultant of two bond moments being equal and opposite to that of the third cancel out.

Dipole Moments - Class 11

 

Dipole Moments - Class 11


CHCl3 is also tetrahedral but has a dipole moment of 1.04.

Dipole moment of NH3 and NF3

Dipole Moments - Class 11

Both NH3 and NF3 molecules have pyramidal shape with one lone pair of electrons on N atom. As fluorine is highly electronegative, it appears that N-F bond should be more polar and the net dipole moment of NF3 should be much greater than that of NH3.

The dipole formed between the lone pair and nitrogen atom has to be taken into consideration which is in the direction of the lone pair.
F is more electronegative than nitrogen ,therefore direction of bond is from nitrogen to fluorine whereas nitrogen is more electronegative than hydrogen, the direction of bond is from hydrogen to nitrogen.

Resultant moment of N-H bond adds up to the bone moment of the lone pair, that of 3 N-F bonds partly cancel the resultant of the lone pair.Hence the net dipole moment of NF3 is less than that of NH3.

Application of dipole moment

1) In determining the polarity of bonds : Greater is the magnitude of dipole moment, higher will be the polarity of the bond.This is applicable to molecules containing only one polar bond.In case of non-polar molecules like H2 , O2, N2 etc, the dipole moment is found to be zero .This is because there is no charge separation in these molecules.

2)In the calculation of percentage ionic character

Dipole Moments - Class 11


3)In determining the symmetry of the molecules

If any molecule possesses two or more polar bonds ,it will not be symmetrical if it possesses some molecular dipole moment.

Water µ= 1.84 D

H2S µ = 0.95 D

NH3 µ=1.47 D

If a molecule contains a number of similar atoms linked to the central atom and the overall dipole moment of the molecule is found to be zero ,this will imply that the molecule is symmetrical.

For Ex: BF3 , CH4 , CCl4

4) To distinguish between cis and trans isomers

Cis isomer usually has higher dipole moment than trans isomer.

5)To distinguish between Ortho, meta and para isomers


The dipole moment of para isomer is zero and that of ortho is greater than that of meta.

Dipole Moments - Class 11

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FAQs on Dipole Moments - Class 11

1. What is a dipole moment?
Ans. A dipole moment is a measure of the polarity of a molecule. It represents the separation of positive and negative charges within a molecule. It is defined as the product of the magnitude of the charge and the distance between the charges.
2. How is a dipole moment calculated?
Ans. The dipole moment of a molecule is calculated by multiplying the magnitude of the charge on each atom by the distance between them. The charges are determined by the difference in electronegativity between the atoms, and the distance is measured between the centers of positive and negative charges.
3. What does a dipole moment indicate about a molecule?
Ans. A dipole moment indicates the polarity of a molecule. If a molecule has a dipole moment, it means that the charge distribution within the molecule is not symmetric, and it has a positive and negative end. A larger dipole moment signifies a more polar molecule.
4. How does the dipole moment affect the physical properties of a molecule?
Ans. The dipole moment affects the physical properties of a molecule in several ways. It influences the molecule's boiling point, melting point, and solubility in polar solvents. A higher dipole moment generally leads to stronger intermolecular forces and higher melting and boiling points.
5. Can a molecule have a zero dipole moment?
Ans. Yes, a molecule can have a zero dipole moment if the charge distribution within the molecule is symmetrical. This means that the positive and negative charges are evenly distributed, resulting in a cancellation of the dipole moments. Examples of molecules with zero dipole moments are carbon dioxide (CO2) and methane (CH4).
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