One of the two compounds in NOF and NO2F has a resultant dipole moment of μ=1.81D and the other has a resultant dipole moment of μ=0.47D. Regarding these compounds, which of the following is correct?
A
1.81D for NO2F and 0.47 D for NOF
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B
0.47D for NO2F and 1.81D for NOF
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C
For both NO2F and NOF dipole moment, μ=1.81D
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D
For both NO2F and NOF dipole moment, μ=0.47D
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Solution
The correct option is B0.47D for NO2F and 1.81D for NOF Fluorine is the most electronegative and oxygen is more electronegative than nitrogen.
In NOF, the bond dipole moments will add up while the lone pair are in the opposite direction. Since the lone pair has a less impact on the net dipole moment, we see significant dipole moment in NOF.
The dipole moment in NOF will be more than in NO2F since the former has a bent shape and the latter has a trigonal planar shape. The trigonal planar shape is more symmetrical which decreases its dipole moment.