Of the two compounds NOF and NO2F, one has m $=$ $1.81 \mathrm{D}$ and the other has $\mathrm{m}=0.47 \mathrm{D}$. Which dipole moment do you predict for each compound? Explain

Question

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Analyze Molecular Geometry**: The molecular geometry of a compound affects its dipole moment. Linear molecules tend to have smaller dipole moments than bent molecules because the vector sum of the individual bond dipoles can cancel out more in linear geometries. ‖ ‖ 2 ⋮ **Predict Geometry for NOF**: Nitrogen monoxide fluoride (NOF) is expected to have a bent molecular geometry due to the presence of a lone pair on the nitrogen atom, which leads to a larger dipole moment. ‖ ‖ 3 ⋮ **Predict Geometry for NO2F**: Nitryl fluoride (NO2F) has a trigonal planar geometry around the nitrogen atom with one of the positions occupied by a lone pair, resulting in a bent shape for the NO2 group. This geometry also leads to a significant dipole moment, but the presence of the additional oxygen atom in NO2F compared to NOF may lead to a more effective cancellation of bond dipoles. ‖ ‖ 4 ⋮ **Compare Dipole Moments**: Given the geometries, NOF is expected to have a larger dipole moment than NO2F because the bond dipoles in NOF are less effectively canceled out than in NO2F. ‖ ∻Answer∻ ⚹ NOF has a dipole moment of $1.81 \mathrm{D}$ and NO2F 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 NO2F, although also bent, has more effective cancellation of bond dipoles due to its additional oxygen atom, resulting in a smaller dipole moment. ⚹◊Which compound, NOF or NO2F, is likely to have the dipole moment of $1.81 \mathrm{D}$?⍭ Generate me a similar question◊

Sia