Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length d for the bond. Unit of dipole moment is Debye. One Debye is equal to 10–18 esu cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be used to distinguish between cis- and trans-isomers; ortho-, meta- and para-forms of a substance, etc.

Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length d for the bond. Unit of dipole moment is Debye. One Debye is equal to 10^–18 esu cm.
Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be used to distinguish between cis- and trans-isomers; ortho-, meta- and para-forms of a substance, etc.

Linked Question 1

μ of the AX₄ type of molecule is zero. The geometry of it can be

None

Tetrahedral

Sq. planar

A or B

No solution

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Linked Question 2

Which of the following statement is correct regarding C₂H₂F₂ molecule.

Two isomers are only possible and planar

Two isomers are planar, one is non planar

One isomer is polar, one is non polar

Two isomers are polar, one is non polar

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Linked Question 3

Arrange the following compounds in increasing order of dipole moments, toluene (I), o-dichlorobenzene (II), m-dichlorobenzene (III) and p-dichlorobenzene (IV)

IV < I < II < III

IV < I < III < II

I < IV < II < III

IV < II < I < III

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Linked Question 4

A diatomic molecule has a dipole moment of 1.2 D. If the bond length is 1.0 × 10^–8 cm, what fraction of charge does exist on each atom?

0.25

0.3

0.1

0.2

Fraction of charge = $\frac{1 .2 \times 10^{- 18}}{4 .8 \times 10^{- 10} \times 10^{- 8}}$ = 0.25

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Linked Question 5

Which is a polar molecule?

XeF₄

I₂Cl₆

PCl₂F₃

BF₃

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