Answer
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Work Step by Step
i. Trigonal Bipyramidal Geometry:
The central atom in a trigonal bipyramidal geometry exhibits sp3d hybridization. This means that the central atom uses a combination of one s orbital, three p orbitals, and one d orbital to form the five bonding regions.
Octahedral Geometry:
The central atom in an octahedral geometry exhibits sp3d2 hybridization. This means that the central atom uses a combination of one s orbital, three p orbitals, and two d orbitals to form the six bonding regions.
Bonding in PF5, SF4, SF6, and IF5:
PF5 (Phosphorus Pentafluoride):
The central atom, phosphorus, exhibits sp3d hybridization. The five fluorine atoms form covalent bonds with the phosphorus atom, resulting in a trigonal bipyramidal geometry. The bonding can be described using the localized electron model, where the five bonding pairs of electrons are localized between the phosphorus and fluorine atoms.
SF4 (Sulfur Tetrafluoride):
The central atom, sulfur, exhibits sp3 hybridization. The four fluorine atoms form covalent bonds with the sulfur atom, resulting in a see-saw (or trigonal bipyramidal) geometry. The bonding can be described using the localized electron model, where the four bonding pairs of electrons are localized between the sulfur and fluorine atoms.
SF6 (Sulfur Hexafluoride):
The central atom, sulfur, exhibits sp3d2 hybridization. The six fluorine atoms form covalent bonds with the sulfur atom, resulting in an octahedral geometry. The bonding can be described using the localized electron model, where the six bonding pairs of electrons are localized between the sulfur and fluorine atoms.
IF5 (Iodine Pentafluoride):
The central atom, iodine, exhibits sp3d hybridization. The five fluorine atoms form covalent bonds with the iodine atom, resulting in a trigonal bipyramidal geometry. The bonding can be described using the localized electron model, where the five bonding pairs of electrons are localized between the iodine and fluorine atoms.
