answerTo describe the five bonding orbitals in a trigonal bipyramidal arrangement, we must use five of the valence shell atomic orbitals(the s orbital, the three p orbitals, and one of the d orbitals), which gives us five sp3d hybrid orbitals, With an octahedral arrangement of six hybrid orbitals, we must use six valence shell atomic orbitals(the s orbital, the three p orbitals, and two of the d orbitals in its valence shell), which gives us six sp3d2 hybrid orbitals, These hybridizations are only possible for atoms that have d orbitals in their valence subshells(that is, not those in the first or second period)
-In a molecule of phosphorus pentachloride, PCl5, there are five P-Cl bonds(thus five pairs of valence electrons around the phosphorus atom) directed toward the corners of a trigonal bipyramid, We use the 3s orbital, the three 3p orbitals, and one of the 3d orbitals to form the set of five sp3d2 hybrid orbitals that are involved in the P-Cl bonds
-The sulfur atom in sulfur hexafluoride, SF6, exhibits sp3d2 hybridization, A molecule of sulfur hexafluoride has six bonding pairs of electrons connecting six fluorine atoms to a single sulfur atom, There are no lone pairs of electrons on the central atom, To bond six fluorine atoms, the 3s orbital, the three 3p orbitals, and the two of the 3d orbitals form six equivalent sp3d2 hybrid orbitals, each directed toward a different corner of an octahedron