Question

Question 4.16 Write the significance/applications of dipole moment.

Class XI Chemical Bonding and Molecular Structure Page 130

Answer 1

The significance or applications of dipole moment are :

1. dipole moment is the scalar product of charge and displacement between two pole.
e.g., μ = Q × d
It means dipole moment helps to predict whether a molecule is polar or non- polar . e.g., if the magnitude of dipole moment is directly proportional to polarity of molecule.for non - polar molecule dipole moment is always zero.

2. The percentage of ionic character is calculated with help of dipole moment.
e.g., % of ionic character = μ(observed) /μ(ionic) × 100


3. symmetrical molecules have zero dipole moment. For example : - BF3 , CH4 , etc has zero dipole moment because these molecules are symmetry and number of lone pairs is zero in central atom.


4.it helps to distinguish between Ortho,meta and para isomers. Dipole moment of para molecule is zero. D.P of Ortho is greater than that of meta isomer.

Answer 2

Answer:

Here you go...

Application sod dipole moment are as follows-

(i) Distinction between polar and non polar molecules:

Non polar molecules such has nitrogen, oxygen and hydrogen have zero dipole moment whereas polar molecules have non zero dipole moment. For example, the dipole moment of water, HF, HCl and H2S are 1.85D, 1.78D, 1.07D and 0.95 D respectively.

(ii) Degree of polarity in a molecule: Greater is the value of dipole moment, greater is the degree of polarity. This relationship specially holds true for diatomic molecules.  HF (1.78D) is more polar than HCl (1.07D).

(iii) Shapes of molecules:

Water and carbon dioxide have dipole moments 1.85 D and 0 respectively.

Thus, water has angular shape whereas carbon dioxide has linear shape.

(iv) Ionic character in a molecule.

The percentage ionic character is the ratio of observed dipole moment to dipole moment for complete ionic character multiplied by 100.

Explanation: