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Hybridization A Blending of Orbitals Methane CH4 Sometimes called “natural gas, ” methane is used to heat homes. Shape of Methane Tetrahedral geometry 109.5o angle between bonds Carbon’s atomic orbitals 4 valence electrons Outermost orbitals: 2s, 2px, 2py, 2pz How can this happen? 2 possibilities Maybe our quantum mechanical model of atomic orbitals is totally wrong. OR Maybe carbon is doing something else with its orbitals to form this compound. Hybridization occurs A mathematical blending of orbitals Number of atomic orbitals blended = number of hybrid orbitals produced Result: Identical orbitals – New shape – New orientation in space sp3 hybridization s + px + Py + pz = 4 sp3 orbitals Sp3 hybridization on carbon 4 identical sp3 orbitals 109.5o between orbitals Tetrahedral orientation Bonds form when orbitals overlap Sigma bonds: end to end overlap of orbitals What happens in ethene? C2H4 Properties Double bond between carbons Trigonal planar geometry around C 120o bond angles Sp2 hybridization occurs S + px + py = 3 sp2 orbitals 1 unused p orbital left over Bonding in ethene Sigma bond: end to end overlap Pi bond: side to side overlap Putting ethene together Carbon-carbon double bond = 1 sigma bond and 1 Pi bond 4 C-H sigma bonds Trigonal planar geometry results What happens in ethyne? C2H2 Linear geometry What type of hybridization is involved? What hybrid and atomic orbitals can it use? What types and numbers of bonds are present in the molecule?