Of the two compounds NOF and $\mathrm{NO}_{2} \mathrm{~F}$, one has $\mu=$ $1.81 \mathrm{D}$ and the other has $\mu=0.47 \mathrm{D}$. Which dipole moment do you predict for each compound? Explain

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∻Solution∻ ‖ 1 ⋮ **Analyze Molecular Geometry**: The molecular geometry of a compound affects its dipole moment. Linear molecules or symmetrical shapes generally have a smaller dipole moment because the individual bond dipoles cancel out. ‖ ‖ 2 ⋮ **Predict Geometry for NOF**: The molecule NOF has a bent geometry due to the presence of a lone pair on the nitrogen atom, which leads to a significant dipole moment as the bond dipoles do not cancel out completely. ‖ ‖ 3 ⋮ **Predict Geometry for $\mathrm{NO_2F}$**: The molecule $\mathrm{NO_2F}$ is trigonal planar with respect to the nitrogen atom. The bond dipoles from the two $\mathrm{N-O}$ bonds are in opposite directions and of equal magnitude, thus they partially cancel each other out. The bond dipole from the $\mathrm{N-F}$ bond does not completely cancel out the remaining dipole, resulting in a smaller dipole moment than NOF. ‖ ‖ 4 ⋮ **Assign Dipole Moments**: Based on the predicted geometries, NOF, with its bent geometry, should have the larger dipole moment of $1.81 \mathrm{D}$, and $\mathrm{NO_2F}$, with a more symmetrical geometry, should have the smaller dipole moment of $0.47 \mathrm{D}$. ‖ ∻Answer∻ ⚹ NOF has a dipole moment of $1.81 \mathrm{D}$ and $\mathrm{NO_2F}$ has a dipole moment of $0.47 \mathrm{D}$. ⚹ ∻Key Concept∻ ⚹ Molecular geometry and symmetry determine the dipole moment of a molecule. ⚹ ∻Explanation∻ ⚹ NOF has a bent geometry leading to a larger dipole moment, while $\mathrm{NO_2F}$ has a more symmetrical geometry resulting in a smaller dipole moment. ⚹◊What is the relationship between molecular structure and dipole moment in chemical compounds such as NOF and $NO_{2}F$?⍭ Generate me a similar question◊

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