Ncert Exercises & Solutions

1. Discuss the significance/applications of dipole moment.

2. Represent diagrammatically the bond moments and the resultant dipole moment in CO₂, NF₃ and CHCl₃.

(a) The applications of dipole moment are

(i) The dipole moment helps to predict whether a molecule is polar or non-polar. As

μ = q \times d

, greater is the magnitude of dipole moment, higher will be the polarity of the bond. For non-polar molecules, the dipole moment is zero.

(ii) The percentage of ionic character can be calculated as

Percentage of ionic character

= \frac{μ_{observed}}{μ_{ionic}} \times 100

(iii) Symmetrical molecules have zero dipole moment although they have two or more polar bonds (in determination of symmetry).

(iv) It helps to distinguish between cis and trans isomers. Usually cis-isomer has higher dipole moment than trans isomer.

(v) It helps to distinguish between ortho, meta and para isomers. Dipole moment of para isomer is zero. Dipole moment of ortho isomer is greater than that of meta isomer.

(b)

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