Consider the following statements and select the correct set of codes using T (True) and F (False) in the given sequence.

(p) ${\mathrm{PI}}_5\left(s\right)$ does not exist due to steric crowding.

(Q) All possible angles in ${\mathrm{BF}}_2\mathrm{Cl}$ are ${120}^{\circ }$

(R) In $\mathrm{N}{\left({\mathrm{SiH}}_3\right)}_3$ lone pair of N is present in $s{p}^3$ hybrid orbital.

(S) d-orbital used in hybridization of P in ${\mathrm{PBr}}_5\left(s\right)$ is $d_{z^2}$

Due to the size of iodine, which is quite enormous, five iodine atoms cannot fit around the P atom to form phosphorus pentaiodide.

All possible angle in ${\mathrm{BF}}_2\mathrm{Cl}$ is not equal to120 degree.

Since Si possesses empty d-orbitals, $\mathrm{N}{\left({\mathrm{SiH}}_3\right)}_3$ has a planar structure because the lone pair N-atom is moved to the silicon's empty d-orbitals ($\mathrm{p}\pi -\mathrm{d}\pi$ overlap).

All the options are false.

Hence, the option C is correct.