Identify the correct order of average molecul | vedclass

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(A) $1$. For $PCl_3F_2$: It has a trigonal bipyramidal geometry. The more electronegative $F$ atoms occupy the axial positions, while $Cl$ atoms occup

Vedclass · Accepted Answer

$PCl_3F_2 > N_2O_{4(g)} > N_2O_{4(s)}$

Vedclass · Answer

(A) $1$. For $PCl_3F_2$: It has a trigonal bipyramidal geometry. The more electronegative $F$ atoms occupy the axial positions, while $Cl$ atoms occupy the equatorial positions. Due to the difference in electronegativity between $P-F$ and $P-Cl$ bonds, the dipole moments do not cancel out completely, resulting in a non-zero dipole moment.$2$. For $N_2O_{4(g)}$: $N_2O_{4}$ in the gas phase exists as a planar molecule with $D_{2h}$ symmetry. The two $NO_2$ groups are connected, and due to rotation and symmetry, the net dipole moment is zero.$3$. For $N_2O_{4(s)}$: In the solid state, $N_2O_{4}$ exists as a planar molecule, but due to crystal packing and intermolecular interactions, it maintains a zero dipole moment similar to the gas phase, or effectively zero due to symmetry.$4$. However, comparing the specific molecular structures: $PCl_3F_2$ has a permanent dipole moment $(\mu 
eq 0)$, whereas $N_2O_{4}$ is non-polar $(\mu = 0)$ in both gas and solid states due to its centrosymmetric structure.$5$. Therefore, the correct order is $N_2O_{4(g)} = N_2O_{4(s)}  N_2O_{4(g)} = N_2O_{4(s)}$. Since this is not explicitly listed, we re-evaluate: $N_2O_{4}$ is non-polar, so $\mu = 0$. $PCl_3F_2$ is polar. Thus, $PCl_3F_2 > N_2O_{4(g)} = N_2O_{4(s)}$.

Identify the correct order of average molecular dipole moment for the following species: $PCl_3F_2$, $N_2O_{4(g)}$, and $N_2O_{4(s)}$.

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