The resultant dipole moment (μ) of two compounds NOF and NO2F is 1.81 D and 0.47 D respectively. Which dipole moment do you predict?

For both NO 2 F and NOF, dipole moment ( μ ) is 0.47 D

For both NO 2 F and NOF, dipole moment ( μ ) is 0.47 D

0.47 D for NO 2 F and 1.81 D for NOF

For both NO 2 F and NOF, dipole moment ( μ ) is 0.47 D

1.81 D for NO 2 F and 0.47 D for NOF

For both NO 2 F and NOF, dipole moment ( μ ) is 1.81 D

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The resultant dipole moment ( $μ$ ) of two compounds NOF and NO₂F is 1.81 D and 0.47 D respectively. Which dipole moment do you predict?

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0.47 D for NO₂F and 1.81 D for NOF

For both NO₂F and NOF, dipole moment ( $μ$ ) is 0.47 D

1.81 D for NO₂F and 0.47 D for NOF

For both NO₂F and NOF, dipole moment ( $μ$ ) is 1.81 D

answer is B.

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NOF has bent shape and NO₂F has trigonal planar shape with asymmetrical distribution of charge on central atom.
The dipole moment in case of NO₂F is less than NOF due to its symmetrical shape.
Hence, dipole moment of NO₂F should be 0.47 D and that of NOF should be 1.81 D.

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