Among [ I _ 3 ] ^ + , [ SiO _ 4 ] ^ 4 - , SO _ 2 Cl _ 2 , XeF _ 2 ,...

${I}^{3 +}$ ion has ${sp}^{3}$ hybridisation and bent shape containing two bond pairs and two lone pairs. Structure of ${{SiO}_{4}}^{4 -}$ is tetrahedral structure and $Si$ is ${sp}^{3}$ hybridised. The molecular geometry of ${SOCl}_{2}$ is trigonal pyramidal and its electron geometry is tetrahedral. In this molecule sulphur undergo ${sp}^{3}$ hbridisation,

${XeF}_{2}$ molecule is linear molecule but it is ${sp}^{3}d$ hybridised. In ${SF}_{4}$, sulphur undergo ${sp}^{3}d$ hybridisation and molecule has see-saw shape. In ${ClF}_{3}$, chlorine undergo ${sp}^{3}d$ hybridisation and shape of the molecule is T-shape.

The nickel tetracarbonyl is a tetrahedral complex in which nickel metal undergo ${sp}^{3}$ hybridisation. In the molecule ${XeO}_{2}{F}_{2}$, $Xe$ undergo ${sp}^{3}d$ hybridisation and molecular shape is see-saw. Tetrachloroplatinate(II) is a square planar complex in which platinum undergoes ${dsp}^{2}$ hbridisation.

${XeF}_{4}$ is square planar compound in which xenon undergoes ${sp}^{3}{d}^{2}$ hybridisation. In the tetrahedral molecule ${SO}_{2}{Cl}_{2}$, sulphur undergoes ${sp}^{3}$ hybridisation.

Hence, the total number of ${sp}^{3}$ hybridised central atom molecules are 5.