Identify the incorrect statemens

1.	Identify the incorrect statemens
Answer» All the five P-Cl bonds are identical in `PCl_(5)` `/_H-P-H` bonds angles in `PH_(3)` are smaller than `/_H-N-H` bonds angles in `NH_(3)`. `CO_(2)` is non polar, while `SO_(2)` is polar. The dipole moment of `NF_(3)` is much higher than `NH_(3)` Solution :In `PCl_(5)`, the phosphorus atom is `sp^(3)d-` hybridised givig five hybrid orbitals. These hybrid orbitals are directd towards the five corners of a trigonal bipyramid. However these five hybrid orbitals are not equivalent. Two axial bondshave large dp character and EQUATORIAL bonds have more `sp^(2)` character. Both `NF_(3)` and `NH_(3)` molecules have trigonal pyramidal shape, but hte former has lower dipole moment than latter. In `NF_(3)` molecule, F being more electronegative than N the electron pairs are ATTRACTED more towards the FLUORINE atom. Hence themoment of the lone pair electrons on N atom and N-F bond moment act in opposite direction. As a result the resultant dipole moment is lowered. On the other hand in `NH_(3)` molecule N being more electronegative than H the bond pair electrons are attracted more towards nitrogen atom. Hence the moment due ot lone pair electrons on N-atom and the N-H bond moments act in the same direction. As a result the resultant dipole moment of `NH_(3)` is much highr than `NF_(3)`

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