Match the following columns :

${\mathrm{SO}}_3$ (gas)	(P) Polar molecule
${\mathrm{OSF}}_4$	(Q) p$\mathrm{\pi }$-d$\mathrm{\pi }$ bond
${\mathrm{SO}}_3{\mathrm{F}}^{-}$	(R) Non-polar molecule
${\mathrm{ClOF}}_3$	(S) One lone pair on central at.om

In Sulphur, there are one pure p orbital and two pure d orbitals. Two $\mathrm{p\pi }‐\mathrm{p\pi }$ bonds and one pp bond each contain these three orbitals. Its polarity is non-polar.
The trigonal bipyramidal molecular structure of ${\mathrm{SOF}}_4$ has an asymmetric charge distribution all around the core atom.${\mathrm{SOF}}_4$ is hence polar.
The lone pair electrons at the "top" of the structure, which cause electron-electron repulsion and a region of partial negative charge, make ${{\mathrm{SO}}^{2-}}_3$ a polar molecule.
Because of its asymmetrical form and the existence of two lone pair electrons, which causes an uneven distribution of charge, ${\mathrm{ClF}}_3$ is a polar molecule.