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?

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.

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?

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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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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Detailed Solution

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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