Indicate the hybridization of the central atom in (a) $\mathrm{H}_{2} \mathrm{~S}$, (d) \(\mathrm{AlI}_{3}\). (b) \(\mathrm{SeF}_{6},(\mathbf{c}) \mathrm{P}(\mathrm{OH})_{3}\)

First, we need to identify the central atom and electron domains for each molecule mentioned above to estimate the geometry of these molecules. We can do this by counting the number of lone electron pairs and the number of covalent bonding groups around the central atom. For molecule (a) \(H_2S\): Central atom: S Lone pair of electrons: 2 Number of bonded atoms: 2 For molecule (b) \(SeF_6\): Central atom: Se Lone pair of electrons: 0 Number of bonded atoms: 6 For molecule (c) \(P(OH)_3\): Central atom: P Lone pair of electrons: 0 Number of bonded atoms: 3 For molecule (d) \(AlI_3\): Central atom: Al Lone pair of electrons: 0 Number of bonded atoms: 3

We will now use the electron domain geometry for each molecule to determine the hybridization of the central atom. For molecule (a) \(H_2S\): Total electron domains: 2 (lone pair) + 2 (bonded) = 4 Geometry: Tetrahedral Hybridization: sp^3 For molecule (b) \(SeF_6\): Total electron domains: 0 (lone pair) + 6 (bonded) = 6 Geometry: Octahedral Hybridization: sp^3d^2 For molecule (c) \(P(OH)_3\): Total electron domains: 0 (lone pair) + 3 (bonded) = 3 Geometry: Trigonal planar Hybridization: sp^2 For molecule (d) \(AlI_3\): Total electron domains: 0 (lone pair) + 3 (bonded) = 3 Geometry: Trigonal planar Hybridization: sp^2 So, the hybridization of the central atoms for each molecule is: a) \(H_2S\): sp^3 b) \(SeF_6\): sp^3d^2 c) \(P(OH)_3\): sp^2 d) \(AlI_3\): sp^2