The number of molecule(s) or ion(s) from the following having...

The species which have ${sp}^{2}$ hybridisation with no lone pairs, ${sp}^{3}{d}^{2}$ hybridisation with two lone pairs are planar molecules.

The number of hybrid orbitals can be calculated as follows,

No.of hybrid orbitals = 1/2(V+M-C+A)

V = number of valence electrons

M = number of monovalent atoms attached to central atom.

C = Number of positive charges on the molecule

A = Number of negative charges on the molecule

${SO}_{3}$	${sp}^{2}$	Planar
${BF}_{3}$	${sp}^{2}$	Planar
${NO}_{3}^{-}$	${sp}^{2}$	Planar
${SF}_{4}$	${sp}^{3}d$	Non-Planar
${H}_{2}{O}_{2}$	${sp}^{3}$	Non-Planar
${PCl}_{3}$	${sp}^{3}$	Non-Planar
${\left[Al{\left(OH\right)}_{4}\right]}^{-}$	${sp}^{3}$	Non-Planar
${XeF}_{4}$	${sp}^{3}{d}^{2}$	Planar
${XeO}_{3}$	${sp}^{3}$	Non-Planar
${PH}_{4}^{+}$	${sp}^{3}$	Non-Planar