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Introduction to sp3d2 hybridization Hybridization: sp3d2:- According to the valance bond theory (VBT) by Pauling and Slater, during chemical reactions, valance shell electrons in an atom get excited by absorbing energy from the environment and become unpaired by promoting themselves to the orbitals possessing higher energies. The orbitals containing unpaired electrons then combine each other to form degenerated, similar and more stable hybridized orbitals. This process is known as “hybridization”. There are several types of such combinations like sp, sp2, sp3 etc. When one “s” orbital, three “p” orbitals and two “d” orbitals containing unpaired electrons combine together, a sp3d2 hybridized system is formed. There are many examples of compounds in which the central atoms are in sp3d2-hybridized state. One common example is sulfur hexafluoride or SF6 in which the central atom sulfur has formed six covalent bonds with six different fluorine atoms violating octet rule: hybridization Valance bond theory (VBT) : sp3d2 hybridization Valance bond theory (VBT) explains this violation in terms of sp3d2 hybridization. The ground state electronic configuration of sulfur is: 1s2 2s2 2p6 3s2 3p4 with the 3d orbital remaining vacant. Box representation of the valance shell electronic configuration is: Valance bond theory (VBT) explains this violation in terms of sp3d2 hybridization. The ground state electronic configuration of sulfur is: 1s2 2s2 2p6 3s2 3p4 with the 3d orbital remaining vacant. Box representation of the valance shell electronic configuration is: Fluorine atoms having electronic configuration 1s2 2s2 2p5, form six single covalent bonds sharing its unpaired electron with each of the unpaired electron of sulfur. This leads to the formation of SF6 or sulfur hexafluoride molecule. The SF6 molecules has an octahedral geometry: It may be noted that the maximum covalency exhibited by an element is equal to the number of unpaired electrons available after impairing all the “s” and “p” electrons in its valance shell. The variable valency is exhibited by those elements whose atoms have vacant “d” orbitals in their valance shell so that the impairing of ‘‘s’’ and ‘‘p’’ orbital electrons by promoting them to the vacant “d” orbitals may be possible. This explains why the elements belonging to the 2nd period of the periodic table like oxygen, nitrogen etc. don’t exhibit variable covalency. It also explains why compounds like OF6 or NCl5 do not exist. In all compounds of hexavalent sulfur like sulfuric acid, hybrid state of sulfur is sp3d2. There are several other examples of such hybrid state in non sulfur compounds also. There are outer orbital complexes in which the central metal atom is in sp3d2 hybrid state. Some examples are: [Cr(CN)6]4-, [Fe(CN)6]4-, [FeF6]3-, [Co(H2O)6]2+, [Cu(NH3)6]2+, [Mn(CN)6]3+, [Ni(H2O)6]2+ etc. In those cases, the central metal atom or central metal ion makes available a number of empty s, p or d atomic orbitals equal to its coordination number. These vacant orbitals become degenerated and equivalent due after getting hybridised. sp3d2 hybridization Fluorine atoms having electronic configuration 1s2 2s2 2p5, form six single covalent bonds sharing its unpaired electron with each of the unpaired electron of sulfur. This leads to the formation of SF6 or sulfur hexafluoride molecule. The SF6 molecules has an octahedral geometry: sp3d2 hybridization It may be noted that the maximum covalency exhibited by an element is equal to the number of unpaired electrons available after impairing all the “s” and “p” electrons in its valance shell. The variable valency is exhibited by those elements whose atoms have vacant “d” orbitals in their valance shell so that the impairing of ‘‘s’’ and ‘‘p’’ orbital electrons by promoting them to the vacant “d” orbitals may be possible. This explains why the elements belonging to the 2nd period of the periodic table like oxygen, nitrogen etc. don’t exhibit variable covalency. It also explains why compounds like OF6 or NCl5 do not exist. In all compounds of hexavalent sulfur like sulfuric acid, hybrid state of sulfur is sp3d2. There are several other examples of such hybrid state in non sulfur compounds also. There are outer orbital complexes in which the central metal atom is in sp3d2 hybrid state. Some examples are: [Cr(CN)6]4-, [Fe(CN)6]4-, [FeF6]3-, [Co(H2O)6]2+, [Cu(NH3)6]2+, [Mn(CN)6]3+, [Ni(H2O)6]2+ etc. In those cases, the central metal atom or central metal ion makes available a number of empty s, p or d atomic orbitals equal to its coordination number. These vacant orbitals become degenerated and equivalent due after getting hybridised. Learn more on about Brownian Movement and its Examples. Between, if you have problem on these topics Ionic Strength, please browse expert math related websites. Please share your comments
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