Which of following statements are incorrect? 

In contrast to P-Nitrophenol, which forms an intermolecular H bond, O-Nitrophenol forms an intramolecular H bond. The boiling point rises during boiling due to the strong intermolecular H bonds, whereas intramolecular H bonds are unable to do the same. As a result, P-Nitrophenol is less volatile in steam than O-Nitrophenol.

Hence, this is incorrect.

Due to its lack of symmetry, ${\mathrm{H}}_2\mathrm{O}$ is a polar molecule. It is a bent or V-shaped molecule. The oxygen molecule has two lone pairs at the top and two hydrogen atoms at the bottom. Flourine is more electronegative than O in the molecular structure ${\mathrm{OF}}_2$. However, O was more electronegative in ${\mathrm{H}}_2\mathrm{O}$, which is why in ${\mathrm{OF}}_2$ the lone pair and OF bond have the opposite dipole direction. However, in ${\mathrm{H}}_2\mathrm{O}$, both the bond dipole moment and the single paid dipole moment point in the same direction. ${\mathrm{H}}_2\mathrm{O}$ hence has a greater dipole moment than ${\mathrm{OF}}_2$.

Hence, this is incorrect.

Because there won't be any attraction of electron pairs to any of the atoms in an $A{X}_4$ if A and X have zero OR nearly zero electronegativity difference, the dipole moment of $A{X}_4$ will be zero if it is perfectly square planar. By resolving the vectors of the dipole moment, we can say that every dipole moment will be cancelled by another dipole moment, resulting in a net dipole moment of zero.

Hence, this is incorrect.