Consider the following statements :

(P) The hybridization found in cation of solid ${\mathrm{PCI}}_5$ is ${\mathrm{sp}}^3$

Q) In${\mathrm{AB}}_2{\mathrm{L}}_2$ type the BAB bond angle is always greater than the normal tetrahedral bond angle. 

(R) In ${\mathrm{ClO}}_3^{-},{\mathrm{NH}}_3$ and ${\mathrm{XeO}}_3$, the hybridization and  the number of lone pairs on the central atoms are same. 

(S) In ${\mathrm{P}}_4$ molecule, there are six $\mathrm{P}-\mathrm{P}$ bonds four lone pairs of electrons.

Of these statements :

Statement Q is incorrect. Because the bond angle of ${\mathrm{OF}}_2$​ and ${\mathrm{OBr}}_2$​ is less than $109.5^{\mathrm{o}}$.

It is due to the bond pairs of electrons being drawn to fluorine due to its higher electronegative state, there is greater lp-lp repulsion, which reduces the bond angle.

The bond pairs are repelled by the more electronegative oxygen atoms nearby, which causes the bond angle to increase. Steric repulsion is also produced by the larger Br atoms, which raises the bond angle