# Which of the following molecules has the maximum dipole moment ? Option 1) CO2 Option 2) CH4 Option 3) NH3 Option 4) NF3

As we learnt in

Resultant dipole moment -

Let XY and XZ are two polar bonds inclined at an angle $\theta$ their dipole moments are

$\mu _{1}\: and\: \mu _{2}$

- wherein

$Resultant\:\mu_{R}=\sqrt{\mu_{1}^{2}+\mu_{2}^{2}+2\mu_{1}\mu_{2}cos\theta}$

Zero dipole moment -

A molecule having two or more polar bonds may have zero net  $\mu$ when the molecule has regular structure

- wherein

Example:-

$CCl_{4},\:PCl_{5},\:SF_{6},\:IF_{7}$

In NH3, H is less electronegative than N and hence dipole moment of each N—H bond is towards N and create high net dipole moment, where as in NF3, F is more electronegative than N, the dipole moment of each N—F bond is opposite to that of lone pair hence reducing the net dipole moment.

Option 1)

CO2

This option is incorrect

Option 2)

CH4

This option is incorrect

Option 3)

NH3

This option is correct

Option 4)

NF3

This option is incorrect

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