The total number of lone pairs of electrons present on the central atoms of the species XeF2, XeF4, XeO3, XeOF4 and ICl4^- taken together is ____ .

For each central atom, lone pairs $=\tfrac12$(valence electrons of the atom, adjusted for charge, minus the electrons it commits to bonds with the surrounding atoms; a double bond commits two electrons). $\mathrm{XeF_2}$: Xe has $8$ valence electrons and commits $2$ to two Xe-F bonds, leaving $6$, i.e. $3$ lone pairs (linear). $\mathrm{XeF_4}$: $8-4=4$ electrons, $2$ lone pairs (square planar). $\mathrm{XeO_3}$: three Xe=O bonds commit $6$ electrons, leaving $2$, i.e. $1$ lone pair (trigonal pyramidal). $\mathrm{XeOF_4}$: four Xe-F single bonds and one Xe=O bond commit $4+2=6$ electrons, leaving $1$ lone pair (square pyramidal). $\mathrm{ICl_4^-}$: $7+1=8$ valence electrons, $4$ committed to I-Cl bonds, so $2$ lone pairs (square planar). The total number of lone pairs on the central atoms is $3+2+1+1+2=9$.